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		<updated>2026-10-19T08:31:05Z</updated>
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	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4808</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4808"/>
				<updated>2018-03-14T10:57:01Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an [https://www.edaq.com/ER175 ER175 Waveform Generator] can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. To create a traditional votammogram, current (and ∆f) versus potential use the XY View option in the Chart Software (see manual).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication–ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as [https://www.originlab.com Origin] or [https://www.wavemetrics.com Igor Pro], or even Microsoft Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4804</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4804"/>
				<updated>2018-03-09T10:09:51Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Techniques */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an [https://www.edaq.com/ER175 ER175 Waveform Generator] can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication–ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as [https://www.originlab.com Origin] or [https://www.wavemetrics.com Igor Pro], or even Microsoft Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4803</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4803"/>
				<updated>2018-03-09T10:05:54Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Techniques */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication–ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as [https://www.originlab.com Origin] or [https://www.wavemetrics.com Igor Pro], or even Microsoft Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4802</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4802"/>
				<updated>2018-03-09T10:02:00Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Techniques */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as [https://www.originlab.com Origin] or [https://www.wavemetrics.com Igor Pro], or even Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4801</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4801"/>
				<updated>2018-03-09T10:01:37Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Techniques */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as [https://www.originlab.com Origin] or [https://www.waavemetrics.com Igor Pro], or even Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4800</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4800"/>
				<updated>2018-03-09T10:00:25Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as [https://www.originlab.com Origin] or Igor Pro, or even Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4799</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4799"/>
				<updated>2018-03-09T09:58:42Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Techniques */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to estimate the amount of charge transferred. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited, or removed, from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral Channel command, and the integral functions in the Data Pad.&lt;br /&gt;
&lt;br /&gt;
To get publication ready diagrams it is usually best to copy and paste selected parts of the signal to specialist graphing software such as OriginLab or Igor Pro, or even Excel.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4798</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4798"/>
				<updated>2018-03-09T09:53:12Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* QCM Techniques */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.  You will need to consult the Chart Software Manual for more details.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current and ∆f versus potential).&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to prove an estimate of transferred charge. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited or removed from the QCM electrode. See the Chart Software Manual for methods for reporting an integrated quantity, such as Computed function: Integral, Integral, Channel command, and the integral function in the Data Pad.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4797</id>
		<title>Using the SRS QCM200 Quartz Crystal Microbalance with an e-corder</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Using_the_SRS_QCM200_Quartz_Crystal_Microbalance_with_an_e-corder&amp;diff=4797"/>
				<updated>2018-03-09T09:42:27Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;[[File:Figure 1. SRS QCM200 Quartz Crystal Microbalance.jpg|300px|thumb|'''Figure 1.''' SRS QCM200 Quartz Crystal Microbalance]]&lt;br /&gt;
&lt;br /&gt;
''Use a Stanford Research Systems QCM200 Quartz Crystal Microbalance with an e-corder to perform QCM experiments, including Electrochemical Quartz Crystal Microbalance (EQCM) experiments.''&lt;br /&gt;
&lt;br /&gt;
== Introduction ==&lt;br /&gt;
The [http://www.thinksrs.com/products/QCM200.htm QCM200 System] is a [http://en.wikipedia.org/wiki/Quartz_crystal_microbalance Quartz Crystal Microbalance] (QCM) manufactured by [http://www.thinksrs.com Stanford Research Systems Inc.] It measures the resonant frequency and series resistance of a 5 MHz, AT-cut quartz crystal. Resonant frequency changes as a linear function of the mass of material deposited on the crystal surface.&lt;br /&gt;
&lt;br /&gt;
The instrument outputs an analog signal proportional to relative frequency (Δf) and a signal proportional to conductance (Vc). The Vc signal is related to the series resistance of the crystal and solution viscosity.&lt;br /&gt;
&lt;br /&gt;
This application note describes the procedure to monitor relative frequency (Δf) and mass displacement (Δm) on an e-corder. It also describes the setup to perform Electrochemical Quartz Crystal Microbalance (EQCM) techniques with an eDAQ [http://www.edaq.com/EA163 EA163 Potentiostat] and e-corder, or an eDAQ [http://www.edaq.com/ER466 ER466 Potentiostat].&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 2. Rear of QCM200 unit.jpg|300px|thumb|right|'''Figure 2.''' Rear of QCM200 unit]]&lt;br /&gt;
[[File:Figure 3. Front of QCM200 unit.jpg|300px|thumb|right|'''Figure 3.''' Front of QCM200 unit]]&lt;br /&gt;
&lt;br /&gt;
== QCM Experiments ==&lt;br /&gt;
Set up the QCM200 and QCM Probe as per instructions in the Operation and Service Manual supplied with the system.&lt;br /&gt;
&lt;br /&gt;
For immersion experiments, secure the QCM Probe to a retort stand and insure that the reaction vessel is big enough and has enough solution to immerse the head of the QCM Probe.&lt;br /&gt;
&lt;br /&gt;
To monitor the Δf signal, connect a BNC to BNC cable from Frequency Analog Out on the rear of the QCM200 to an e-corder input (See Figure 2), or to ER466 Potentiostat Input 1.&lt;br /&gt;
&lt;br /&gt;
If you also wish to monitor Vc, connect a BNC to BNC cable from the Conductance Output on the front of the QCM200 to a spare e-corder input (See Figure 3), or to ER466 Potentiostat Input 2.&lt;br /&gt;
&lt;br /&gt;
[[File:Table 1. delta f ranges and suitable Scale Factors.jpg|300px|thumb|'''Table 1.''' Δf ranges and suitable Scale Factors]]&lt;br /&gt;
[[File:Figure 4. Units Conversion Window.jpg|300px|thumb|right|'''Figure 4.''' Units Conversion Window]]&lt;br /&gt;
&lt;br /&gt;
== Chart Settings and Calibration ==&lt;br /&gt;
In Chart’s rate pop-up menu, select a suitable sampling speed for monitoring the processes that will be occurring at the face of the crystal oscillator.&lt;br /&gt;
&lt;br /&gt;
With the head of the QCM probe out of the solution, set the C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; Compensation switch on the front of the QCM200 to HOLD and the ten-turn dial to 8.0 (Dry Operation Setting). See Operation and Service Manual for how to set the optimal C&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; for different media. &lt;br /&gt;
&lt;br /&gt;
Press on the PARAMETER Key on the QCM200 to scroll through the LED display menus.&lt;br /&gt;
&lt;br /&gt;
Hold down the VALUE key for 2 seconds whilst in any display menu to (1) set the Frequency Offset to the current Absolute Frequency value (2) Zero the Relative Frequency readings (3) zero the Mass Displacement display and (4) zero the Frequency Analog Out voltage output.&lt;br /&gt;
&lt;br /&gt;
Press PARAMETER until Scale is displayed. The Voltage Scale Factors are displayed in either Hz/V or kHz/V. Press on VALUE to change the Scale Factor. The Scale Factor to choose depends on the largest Δf value expected, noting the QCM200 has a maximum analog output of ±10 V.&lt;br /&gt;
&lt;br /&gt;
          Analog Frequency Out [V] = Δf/Scale Factor&lt;br /&gt;
&lt;br /&gt;
Double the expected maximum Δf and use the values in Table 1 to determine the best Scale Factor to use. Using the narrowest range possible, increases the digital resolution of the measurements.&lt;br /&gt;
&lt;br /&gt;
For a simple immersion test in water, the expected Δf is approximately 715 Hz, so the 200 Hz Scale Factor is the best.&lt;br /&gt;
&lt;br /&gt;
For very small frequency fluctuations, the sensitivity can be further increased by using a narrower e-corder gain range than the default ±10 V range.&lt;br /&gt;
&lt;br /&gt;
Select the Input Amplifier for the Channel connected to the QCM200 Frequency Analog Out. With the Crystal Oscillator in air, the signal should be already zeroed. If not, press the VALUE Key on the front of the QCM200 for 2 seconds. If the signal is noisy, experiment with the various low pass filters.&lt;br /&gt;
&lt;br /&gt;
Click on Units... in the Input Amplifier window, to open the Units Conversion window (Figure 4).&lt;br /&gt;
 &lt;br /&gt;
For Point 1, enter 0 in the left hand cell, and zero in the right hand cell. For Point 2, enter 1 in the left hand cell, and the Scale Factor selected (200 for the immersion test) in the right hand cell.  Define the units as either Hz or kHz, depending on the Scale Factor selected.&lt;br /&gt;
&lt;br /&gt;
Click OK. The channel is now calibrated to read the relative frequency output in either Hz or kHz.&lt;br /&gt;
&lt;br /&gt;
To configure another Channel to directly display mass displacement, select Arithmetic... on the Channel. &lt;br /&gt;
&lt;br /&gt;
The general mass sensitivity equation is &lt;br /&gt;
&lt;br /&gt;
          Δf = −Cf × Δm&lt;br /&gt;
&lt;br /&gt;
Where Cf = the sensitivity factor for the crystal (56.6 Hz.µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; for a 5 MHz crystal at room temperature).&lt;br /&gt;
&lt;br /&gt;
If using the standard 5 MHz quartz crystal supplied with the QCM200 system, enter the expression in either Figure 5 or 6 into the Arithmetic window.&lt;br /&gt;
&lt;br /&gt;
{|&lt;br /&gt;
| [[File:Figure 5. Use this expression if using 200 and 500 Hz Scale Factor.jpg|300px|thumb|right|'''Figure 5.''' Use this expression if using 200 and 500 Hz Scale Factor]]&lt;br /&gt;
| [[File:Figure 6. Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor.jpg|300px|thumb|right|'''Figure 6.''' Use this expression if using 1, 2, 5, 10, 20 kHz Scale Factor]]&lt;br /&gt;
| [[File:Figure 7. Series Resistance expression, assuming Vc is monitored.jpg|300px|thumb|right|'''Figure 7.''' Series Resistance expression, assuming Vc is monitored]]&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Enter µg/cm&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt; as the unit name.&lt;br /&gt;
&lt;br /&gt;
The Conductance Output signal (Vc) in related to the series resistance of the QCM crystal by:&lt;br /&gt;
&lt;br /&gt;
          R = 10000 × (10 − Vc/5) − 75&lt;br /&gt;
&lt;br /&gt;
[[File:Figure 8. e-corder and Potentiostat setup for EQCM work.jpg|600px|thumb|right|'''Figure 8.''' e-corder and Potentiostat setup for EQCM work]]&lt;br /&gt;
&lt;br /&gt;
Enter this expression in into the Arithmetic window of a spare channel to record series resistance directly (See Figure 7). Define the unit name as Ω (Ohms).&lt;br /&gt;
&lt;br /&gt;
The e-corder system is now set up to record relative frequency, mass displacement and series resistance of the QCM simultaneously. Click on start to begin recording data and perform your experiments.&lt;br /&gt;
&lt;br /&gt;
Note, other parameters such as temperature an pH can be monitored on other channels with suitable amplifiers and transducers.&lt;br /&gt;
&lt;br /&gt;
== EQCM Experiments ==&lt;br /&gt;
&lt;br /&gt;
In EQCM experiments, a potential is applied to the gold surface of the quartz crystal oscillator, and the change in mass near the surface and current from electrochemical processes are monitored simultaneously.&lt;br /&gt;
&lt;br /&gt;
To perform EQCM techniques, set up the [http://www.edaq.com/ER466 ER466 Potentiostat], or the [http://www.edaq.com/EA163 EA163 Potentiostat] and [http://www.edaq.com/e-corder-units e-corder with four or more channels], as per instructions in their respective hardware manuals. Reference and auxiliary electrodes are also required, as found in the [http://www.edaq.com/ET014 ET014 EChem Electrode Kit].&lt;br /&gt;
&lt;br /&gt;
Connect the green working electrode cable from the Potentiostat to the Crystal Face Bias connector on the QCM25 Crystal Controller, using a banana plug adapter. Connect the yellow cable to your reference electrode, and the red cable to your auxiliary electrode.&lt;br /&gt;
&lt;br /&gt;
Figure 8 shows a typical setup for EQCM work.&lt;br /&gt;
&lt;br /&gt;
=== QCM Techniques ===&lt;br /&gt;
&lt;br /&gt;
Chart software is used for EQCM experiments.&lt;br /&gt;
&lt;br /&gt;
For amperometric  (current versus time) techniques, a fixed potential can be set in the Chart software Stimulator menu.&lt;br /&gt;
&lt;br /&gt;
For cyclic voltammetry techniques a potential ramp can be defined in the Chart software Stimulator menu (Up &amp;amp; Down, and Triangle items). If greater versatility of the applied potential is required (eg arbitrary start and end potentials, manual ramp interrupt or ramp reversal) an ER175 Waveform Generator can be used.&lt;br /&gt;
&lt;br /&gt;
Chart typically displays signals (current, potential and QCM ∆f) all versus time. Use the Chart Software XY window to show the more useful votammogram (current ∆f versus potential). See the Chart Software Manual for more detailed instructions.&lt;br /&gt;
&lt;br /&gt;
Sections of the current signal can be integrated (wth respect to time) to prove an estimate of transferred charge. This should correspond to the amount of electrolysed sample which in turn should be proportional to to the amount of material deposited or removed from the QCM electrode. See the various Chart software methods for reporting an integrated quantity&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Main_Page&amp;diff=4300</id>
		<title>Main Page</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Main_Page&amp;diff=4300"/>
				<updated>2017-03-20T00:38:15Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;This Wiki site was created for discussion about eDAQ products and their uses.&lt;br /&gt;
&lt;br /&gt;
== [[Application Notes]] ==&lt;br /&gt;
# [[Application_Notes#Electrochemistry|Electrochemistry]]&lt;br /&gt;
# [[Application_Notes#Chromatography_PowerChrom|PowerChrom]]&lt;br /&gt;
# [[Application_Notes#Data_Recording_in_Chart|Data Recording in Chart]]&lt;br /&gt;
# [[Application_Notes#C4D_Conductivity_Detector|C4D Conductivity Detector]]&lt;br /&gt;
# [[Application_Notes#SDx_Tethered_Membranes|SDx Tethered Membranes]]&lt;br /&gt;
# [[Application_Notes#Technical_Notes|Technical Notes]]&lt;br /&gt;
&lt;br /&gt;
== [[Teaching Notes]] ==&lt;br /&gt;
# [[Teaching_Notes#EXP001_Anodic_Stripping_Voltammetry|Anodic Stripping Voltammetry]]&lt;br /&gt;
# [[Teaching_Notes#EXP002_Cyclic_Voltammetry_of_Ferrocene_Carboxylic_Acid|Cyclic Voltammetry]]&lt;br /&gt;
# [[Teaching_Notes#EXP004a_Measurement_of_Iron_Corrosion_Exchange_Current|Corrosion of Iron]]&lt;br /&gt;
# [[Teaching_Notes#EXP006_Fluoride_Ion_Selective_Electrodes|Ion Selective Electrodes]]&lt;br /&gt;
# [[Teaching_Notes#EXP009_Heat_of_Neutralisation|Heat of Neutralisation]]&lt;br /&gt;
# [[Teaching_Notes#EXP011_The_pH_Electrode_and_Potentiometric_Titrations|Potentiometric Titration]]&lt;br /&gt;
# [[Teaching_Notes#Phospholipid_Membrane_Conductivity|Conductivity of a Phospholipid Membrane]]&lt;br /&gt;
&lt;br /&gt;
== [[Screencast Training Videos]] ==&lt;br /&gt;
# [[Screencast_Training_Videos#Electrochemistry|Electrochemistry]]&lt;br /&gt;
# [[Screencast_Training_Videos#Electrochemical_Impedance_Spectroscopy_.28EIS.29|Electrochemical Impedance Spectroscopy]]&lt;br /&gt;
# [[Screencast_Training_Videos#Chart|Chart]]&lt;br /&gt;
# [[Screencast_Training_Videos#PowerChrom|PowerChrom]]&lt;br /&gt;
# [[Screencast_Training_Videos#C4D_Conductivity_Detector|C4D Conductivity Detector]]&lt;br /&gt;
# [[Screencast_Training_Videos#SDx_Tethered_Membranes|SDx Tethered Membranes]]&lt;br /&gt;
# [[Screencast_Training_Videos#FIA_Flow_Injection_Analysis|Flow Injection Analysis]]&lt;br /&gt;
# [[Screencast_Training_Videos#Pod-Vu_for_isoPods|Pod-Vu Software]]&lt;br /&gt;
&lt;br /&gt;
== [[Manuals]] ==&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Main_Page&amp;diff=4299</id>
		<title>Main Page</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Main_Page&amp;diff=4299"/>
				<updated>2017-03-20T00:38:05Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;This Wiki site was created for discussion about eDAQ products and their uses.&lt;br /&gt;
&lt;br /&gt;
== [[Application Notes]] ==&lt;br /&gt;
# [[Application_Notes#Electrochemistry|Electrochemistry]]&lt;br /&gt;
# [[Application_Notes#Chromatography_PowerChrom|PowerChrom]]&lt;br /&gt;
# [[Application_Notes#Data_Recording_in_Chart|Data Recording in Chart]]&lt;br /&gt;
# [[Application_Notes#C4D_Conductivity_Detector|C4D Conductivity Detector]]&lt;br /&gt;
# [[Application_Notes#SDx_Tethered_Membranes|SDx Tethered Membranes]]&lt;br /&gt;
# [[Application_Notes#Technical_Notes|Technical Notes]]&lt;br /&gt;
&lt;br /&gt;
== [[Teaching Notes]] ==&lt;br /&gt;
# [[Teaching_Notes#EXP001_Anodic_Stripping_Voltammetry|Anodic Stripping Voltammetry]]&lt;br /&gt;
# [[Teaching_Notes#EXP002_Cyclic_Voltammetry_of_Ferrocene_Carboxylic_Acid|Cyclic Voltammetry]]&lt;br /&gt;
# [[Teaching_Notes#EXP004a_Measurement_of_Iron_Corrosion_Exchange_Current|Corrosion of Iron]]&lt;br /&gt;
# [[Teaching_Notes#EXP006_Fluoride_Ion_Selective_Electrodes|Ion Selective Electrodes]]&lt;br /&gt;
# [[Teaching_Notes#EXP009_Heat_of_Neutralisation|Heat of Neutralisation]]&lt;br /&gt;
# [[Teaching_Notes#EXP011_The_pH_Electrode_and_Potentiometric_Titrations|Potentiometric Titration]]&lt;br /&gt;
# [[Teaching_Notes#Phospholipid_Membrane_Conductivity|Conductivity of a Phospholipid Membrane]]&lt;br /&gt;
&lt;br /&gt;
== [[Screencast Training Videos]] ==&lt;br /&gt;
# [[Screencast_Training_Videos#Electrochemistry|Electrochemistry]]&lt;br /&gt;
# [[Screencast_Training_Videos#Electrochemical_Impedance_Spectroscopy_.28EIS.29|Electrochemical Impedance Spectroscopy]]&lt;br /&gt;
# [[Screencast_Training_Videos#Chart|Chart]]&lt;br /&gt;
# [[Screencast_Training_Videos#PowerChrom|PowerChrom]]&lt;br /&gt;
# [[Screencast_Training_Videos#C4D_Conductivity_Detector|C4D Conductivity Detector]]&lt;br /&gt;
# [[Screencast_Training_Videos#SDx_Tethered_Membranes|SDx Tethered Membranes]]&lt;br /&gt;
# [[Screencast_Training_Videos#FIA_Flow_Injection_Analysis|Flow Injection Analysis]]&lt;br /&gt;
# [[Screencast_Training_Videos#Pod-Vu_for_isoPods|Pod-Vu Software]]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== [[Manuals]] ==&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Test&amp;diff=4298</id>
		<title>Test</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Test&amp;diff=4298"/>
				<updated>2017-03-20T00:37:16Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;Testing, 1...2...3..4...5...6...7...&lt;br /&gt;
&lt;br /&gt;
abc&lt;br /&gt;
&lt;br /&gt;
xyz&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Ionophores_in_Society&amp;diff=4225</id>
		<title>Ionophores in Society</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Ionophores_in_Society&amp;diff=4225"/>
				<updated>2016-08-24T08:06:57Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&amp;lt;big&amp;gt;'''Medicines, Toxins, Pollutants, Growth Promoters, Sensors'''&amp;lt;/Big&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Ionophore Ionophores] are lipophilic molecules produced, and often excreted, by microorganisms and animals that are characterised by their ability to transport ions (especially Na&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;, K&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;, Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;, and Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;) across cell membranes. They are not only chemically interesting in their own right but many have important medical and economic roles in our society.&lt;br /&gt;
&lt;br /&gt;
A selection of ionophores is presented below for study in mainstream chemistry courses as well as courses for pre-med, vet, pharma, biochemistry, and soil and agricultural science students.  The demonstration of ion movement across membranes is also relevant to courses on neurophysiology, and biophysics.&lt;br /&gt;
&lt;br /&gt;
The use of ionophore 'growth promoters' in the animal feedstock industry is not only of interest to agricultural scientists, but also of concern to environmental chemists because of their presence in manure and sewerage sludges that may be used as fertiliser for human or animal crops.&lt;br /&gt;
&lt;br /&gt;
The ability of these materials to transport ions across phospholipid bilayer cell membranes, which is usually the key to understanding their mode of action, can be easily studied using [http://wiki.edaq.com/index.php/Tethered_Membranes tethered membrane technology]. A suitable method is outlined in Application Note: [http://wiki.edaq.com/index.php/SDx_Protocol_1 SDx Protocol 1].&lt;br /&gt;
&lt;br /&gt;
Most of these ionophores can be obtained from [http://www.edaq.com/chemicals eDAQ].&lt;br /&gt;
&lt;br /&gt;
=== Amphotericin B ===&lt;br /&gt;
[[File:AmphotericinB_1.jpg|200px|thumb|right|Amphotericin B. MW 923.5. Compare this structure with that of Nystatin, below.]]&lt;br /&gt;
[http://en.wikipedia.org/wiki/Amphotericin_B Amphotericin B] is an antibiotic ([http://www.accessdata.fda.gov/drugsatfda_docs/label/2012/050740s021lbl.pdf AmBisome&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], ) used to treat serious fungal infections. It forms ion channels in the fungal cell membrane with the assistance of [http://en.wikipedia.org/wiki/Ergosterol ergosterol] which is a naturally occurring lipid in fungal membranes. As a [http://www.nlm.nih.gov/medlineplus/druginfo/meds/a682643.html medicine] it is administered intravenously as a [http://www.accessdata.fda.gov/drugsatfda_docs/label/2008/050740s016lbl.pdf liposomal preparation].&lt;br /&gt;
&lt;br /&gt;
While its affinity for [http://en.wikipedia.org/wiki/Ergosterol ergosterol] makes it target fungal cells, Amphotericin can also interact with the [http://en.wikipedia.org/wiki/Cholesterol cholesterol] in mammalian cells. This limits its therapeutic dosage because of toxicity.&lt;br /&gt;
&lt;br /&gt;
Amphotericin B is similar both in structure and in action to Nystatin.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 27.0 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Novel, unifying mechanism for amphotericin B and other polyene drugs: electron affinity, radicals, electron transfer, autoxidation, toxicity, and antifungal action. Peter Kovacic and    Andrew Cooksy, Medicinal Chemical Communications, 3, 274-280, 2012. [http://dx.doi.org/10.1039/C2MD00267A DOI: 10.1039/C2MD00267A]&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Amphotericin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-A1441-25mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Beauvericin.jpg|200px|thumb|right|Beauvericin. MW 784.0. Compare this structure with that of the Enniatin Complex, below.]]&lt;br /&gt;
&lt;br /&gt;
=== Beauvericin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Beauvericin Beauvericin] is closely related to the macrocyclic enniatins, having three benzyl groups in place of the aliphatic chains of the enniatins. It is a potentially toxic agent found in grain crops affected by [http://en.wikipedia.org/wiki/Fusarium ''Fusarium''] fungi. The selectivity for monovalent cations is reported as K&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; &amp;gt; Na&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ~ Rb&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; &amp;gt; Cs&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ~ Li&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; &amp;gt; NH&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;, and for divalent cations as  Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;. The antibiotic properties of Beauvericin are being investigated.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 31.9 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Occurrence of Beauvericin and Enniatins in Wheat Affected by ''Fusarium avenaceum'' Head Blight. A Logrieco, A Rizzo, R Ferracane, and A Ritieni, Applied Environmental Microbiology, 68, 82-85, 2002. [http://dx.doi.org/10.1128/AEM.68.1.82-85.2002 DOI: 10.1128/AEM.68.1.82-85.2002]&lt;br /&gt;
# Selective Binding of Alkali and Alakaline Earth Ions to Beauvericin Investigated by Electrospray Mass Spectrometry. Tara-Lynn Baratz, Courtney N. Richardson, J. Brett Kimbrell, Joshua Hite, (Dr. Farooq A. Khan). [https://ncurdb.cur.org/ncur/archive/Display_NCUR.aspx?id=41814 Poster presentation], 2010.&lt;br /&gt;
# Beauvericin and enniatins H, I and MK1688 are new potent inhibitors of human immunodeficiency virus type-1 integrase. CG Shin, DG An, HH Song, C Lee, The Journal of antibiotics, 62, 687-690, 2009. [http://dx.doi.org/10.1038/ja.2009.102 DOI: 10.1038/ja.2009.102]&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-B1238-25mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Calcimycin.jpg|200px|thumb|right|Calcimycin. MW 523.6]]&lt;br /&gt;
&lt;br /&gt;
=== Calcimycin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Calcimycin Calcimycin] is also widely known as Ionophore A23187. The most notable feature of calcimycin  is the ability to transport divalent cation across cell membranes. Its in vitro affinity for cations is Ni&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Co&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Zn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; ~ Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;, however transport rates across lipsomal membranes are reported as Cd&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt;  Zn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;. Calcimycin has antibiotic properties, and is also being used in [http://www.gynemed.de/fileadmin/downloads/Medien/Produktfolien/Backgroundinformation_GM508_Cult-Active_Rev01_00.pdf IVF treatments]. &lt;br /&gt;
&lt;br /&gt;
Dissolve 5 mg in 9.55 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
# Structures and Properties of Naturally Occurring Polyether Antibiotics. Jacek Rutkowski and Bogumil Brzezinski, BioMed Research International, Article ID 162513, 2013. [http://dx.doi.org/10.1155/2013/162513 DOI: 10.1155/2013/162513]&lt;br /&gt;
# Equilibria between ionophore A23187 and divalent cations: stability of 1:1 complexes in solutions of 80% methanol/water. CJ Chapman, AK Puri, RW Taylor, DR Pfeiffer, Biochemistry, 26, 5009-5018, 1987. [http://dx.doi.org/10.1021/bi00390a019 DOI: 10.1021/bi00390a019]&lt;br /&gt;
# The specificity of ionophore A23187 in cation transport across lipid membranes. Studies with lecithin vesicles. WG Pohl, R Kreikenbohm, K. Seuwen, Z Naturforsch C, 35, 562-568, 1980.&lt;br /&gt;
#Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; transport properties of ionophores A23187, ionomycin, and 4-BrA23187 in a well defined model system. W.L. Erdahl, C.J. Chapman, R.W. Taylor and D.R. Pfeiffer, Biophysical Journal,  66, 1678-1693, 1994. [http://dx.doi.org/DOI:10.1016/S0006-3495(94)80959-2 10.1016/S0006-3495(94)80959-2]&lt;br /&gt;
# Application of a ready-to-use calcium ionophore increases rates of fertilization and pregnancy in severe male factor infertility. Thomas Ebner, Maria Köster, Omar Shebl, Marianne Moser, Hans Van der Ven, Gernot Tews, Markus Montag, Fertility and Sterility, 98, 1432–1437, 2012. [http://dx.doi.org/10.1016/j.fertnstert.2012.07.1134 DOI: 10.1016/j.fertnstert.2012.07.1134]. Free [http://www.utd.org.tr/download/kasim_2012/Kasim-MAKALE2ORJINAL.pdf download].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-C1236-5mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:EnniatinComplex.jpg|200px|thumb|right|Enniatin Complex. Approximate MW 640. Beauvericin is a related molecule with R&amp;lt;sub&amp;gt;1&amp;lt;/sub&amp;gt; = R&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; = R&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt; = benzyl.]]&lt;br /&gt;
&lt;br /&gt;
===  Enniatin complex ===&lt;br /&gt;
[http://en.wikipedia.org/wiki/Enniatin Enniatins] are produced by [http://en.wikipedia.org/wiki/Fusarium ''Fusarium''] fungi that commonly infect wheat and other grains. High levels are potentially toxic.&lt;br /&gt;
&lt;br /&gt;
A mixture of related macrocylic molecules, with different peripheral alkyl substituents, is commonly encountered and this is refried to as a 'complex'. There are at least 28 naturally occurring enniatins.&lt;br /&gt;
&lt;br /&gt;
Enniantins also have promise as antibiotics and anti-cancer drugs.&lt;br /&gt;
&lt;br /&gt;
Dissolve 50 mg in 78.1 mL, or 10 mg in 15.6 mL, of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Occurrence of Beauvericin and Enniatins in Wheat Affected by ''Fusarium avenaceum'' Head Blight. A Logrieco, A Rizzo, R Ferracane, and A Ritieni, Applied Environmental Microbiology, 68, 82-85, 2002. [http://dx.doi.org/10.1128/AEM.68.1.82-85.2002 DOI: 10.1128/AEM.68.1.82-85.2002]&lt;br /&gt;
# Beauvericin and enniatins H, I and MK1688 are new potent inhibitors of human immunodeficiency virus type-1 integrase. CG Shin, DG An, HH Song, C Lee, The Journal of antibiotics, 62, 687-690, 2009. [http://dx.doi.org/10.1038/ja.2009.102 DOI: 10.1038/ja.2009.102]&lt;br /&gt;
# [http://toxinology.nilu.no/Researchareas/Fungaltoxins/Factsheets/Enniatins/tabid/4536/Default.aspx Toxicology Portal at Toxicology.no].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-E1071-50mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:GramicidinA.jpg|200px|thumb|right|Gramicidin A. MW 1882]]&lt;br /&gt;
&lt;br /&gt;
=== Gramicidin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Gramicidin Gramicidin] is often regarded as the archetypal ion channel for monovalent cations, despite its unusual dimer arrangement that forms across the cell membrane. It was one of the first commercially available antibiotics and is used today in several topical medications ([http://www.drugs.com/ingredient/gramicidin.html Neosporin, Neocidin, Neoptic, Ocu-Spore-G]).&lt;br /&gt;
&lt;br /&gt;
Gramicidin is usually sold as a mixture of related linear polypeptides (principally A, B and C) but the main component is Gramicidin A.&lt;br /&gt;
&lt;br /&gt;
Dissolve 100 mg in 53.1 mL of solvent to make a 1.00 mM stock solution. &lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Gramicidin_S Gramicidin S] is an unusual macrocyclic variant.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# The gramicidin ion channel: A model membrane protein. Devaki A. Kelkar, Amitabha Chattopadhyay, Biochimica et Biophysica Acta 1768, 2011–2025, 2007. [http://dx.doi.org/10.1016/j.bbamem.2007.05.011 DOI: 10.1016/j.bbamem.2007.05.011]&lt;br /&gt;
# Structure of gramicidin A. B A Wallace, Biophysics Journal, 49, 295–306, 1986. Free access at PubMed Central: [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1329637/ PMC1329637]&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Gramicidin Drug Information Online].&lt;br /&gt;
# Available from [http://www.sigmaaldrich.com/catalog/product/sigma/g5002?lang=en&amp;amp;region=US Sigma-Aldrich] or [http://www.scbt.com/datasheet-252865-gramicidin-from-bacillus-aneurinolyticus-bacillus-brevis.html Santa Cruz Biotechnology]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Ionomycin.jpg|350px|thumb|right|Ionomycin. MW 747.1]]&lt;br /&gt;
&lt;br /&gt;
=== Ionomycin ===&lt;br /&gt;
[http://en.wikipedia.org/wiki/Ionomycin Ionomycin] is a noted calcium ionophore with a selectivity of Pb&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Cd&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Zn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt;&amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; ~ Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;. There is almost no binding to Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; or Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; or to  monovalent alkali metal cations.&lt;br /&gt;
&lt;br /&gt;
Dissolve 5 mg in 6.69 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# [http://www.jbc.org/content/253/17/5892 Characterization of ionomycin as a calcium ionophore.] C Liu and T E Hermann, Journal of Biological Chemistry, 253, 5892-5894, 1978.&lt;br /&gt;
# Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; transport properties of ionophores A23187, ionomycin, and 4-BrA23187 in a well defined model system. W.L. Erdahl, C.J. Chapman, R.W. Taylor and D.R. Pfeiffer, Biophysical Journal,  66, 1678-1693, 1994. [http://dx.doi.org/10.1016/S0006-3495(94)80959-2 DOI:10.1016/S0006-3495(94)80959-2]&lt;br /&gt;
# Ionomycin, a Carboxylic Acid Ionophore, Transports Pb&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; with High Selectivity. Warren L. Erdahl, Clifford J. Chapman, Richard W. Taylor and Douglas R. Pfeiffer, Journal of Biological Chemistry, 275, 7071-7079, 2000. [http://dx.doi.org/10.1074/jbc.275.10.7071 DOI: 10.1074/jbc.275.10.7071]&lt;br /&gt;
# Ion-selective electrodes based on natural carboxylic polyether antibiotics. Koji Suzuki, Koji Tohda, Hiroshi Aruga, Misako Matsuzoe, Hidenari Inoue, Tsuneo Shirai, Analytical Chemistry, 60, 1714–1721, 1988. [http://dx.doi.org/10.1021/ac00168a016 DOI: 10.1021/ac00168a016]&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-I1261-5mg eDAQ], [http://www.hoelzel-biotech.com/en/products/detail/nr/lc-laboratories--inhibitors--other--i-5700-25mg--ionomycin-free-acid.html Hölzel Diagnostica], or [http://www.lclabs.com/PRODFILE/G-K/I-5700.php4 LC Labs].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Lasalocid.jpg|200px|thumb|right|Lasalocid. MW 590.8]]&lt;br /&gt;
&lt;br /&gt;
=== Lasalocid ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Lasalocid Lasalocid] is used as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=096-298 Avatec&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;, Bovatec&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;])  for control of coccidiosis, a protozoan parasite of poultry and livestock.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 42.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC243437/pdf/aem00200-0082.pdf, Effect of Monensin and Lasalocid-Sodium on the Growth of Methanogenic and Rumen Saccharolytic Bacteria]. Min Chen and MJ Wolin, Applied and Environmental Microbiology, 72-77, 1979.&lt;br /&gt;
# Ionophores for Dairy Cattle: Current Status and Future Outlook. R.K. McGuffey, L.F. Richardson, J.I.D. Wilkinson, Journal of Dairy Science 84, E194–E203, 2001. [http://dx.doi.org/10.3168/jds.S0022-0302(01)70218-4 DOI: 10.3168/jds.S0022-0302(01)70218-4]&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Ion-selective electrodes based on natural carboxylic polyether antibiotics. Koji Suzuki, Koji Tohda, Hiroshi Aruga, Misako Matsuzoe, Hidenari Inoue, Tsuneo Shirai, Analytical Chemistry, 60, 1714–1721, 1988. [http://dx.doi.org/10.1021/ac00168a016 DOI: 10.1021/ac00168a016]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Lasalocid Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-L1533-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Maduramicin.jpg|200px|thumb|right|Maduramicin. MW 917.1]]&lt;br /&gt;
&lt;br /&gt;
=== Maduramicin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Maduramicin Maduramicin] is used as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=139-075 Cygro&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;]) for control of coccidiosis, a protozoan parasite of poultry and livestock.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 27.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Maduramicin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-M1542-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
=== Magainins and PGLa===&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Magainin magainins] are linear polypeptides of 23 amino acids first discovered in the skin of the African clawed frog, [http://en.wikipedia.org/wiki/Xenopus ''Xenopus laevis''], and are believed to be responsible for the resistance of the frog to many of the pathogens that would otherwise cause disease in their moist habitat. Magainins and similar compounds are now known to be present in the skin of many amphibians and are have been shown to be active against  viruses, both gram-positive and gram-negative bacteria, protozoa, yeasts and fungi, and may also be hemolytic and cytotoxic to cancer cells. Their mode of action is believed to be by 4 − 7 magainin molecules forming a pore in the phospholipid bilayer membrane of their target. Magainin 2 also has a synergistic effect with the linear polypeptide PGLa (also from ''Xenopus'') suggesting the formation of a hybrid pore.&lt;br /&gt;
&lt;br /&gt;
Magainins 1 and 2 differ in two amino acid locations where a positively charged lysine residue (&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;) is replaced by a neutral amino acid. &lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;0&amp;quot; style=&amp;quot;width:1000px; height:40px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |'''Magainin 1:'''&lt;br /&gt;
|   &amp;lt;small&amp;gt;&amp;lt;tt&amp;gt;H-Gly-Ile-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Leu-His-Ser-Ala-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Phe-Val-Gly-Glu-Ile-Met-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ser-OH&amp;lt;/tt&amp;gt;&amp;lt;/small&amp;gt;&lt;br /&gt;
|MW 2410&lt;br /&gt;
|  1 mg in 415 µL = 1 mM&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |'''Magainin 2:'''&lt;br /&gt;
|   &amp;lt;small&amp;gt;&amp;lt;tt&amp;gt;H-Gly-Ile-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Leu-His-Ser-Ala-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Phe-Val-Gly-Glu-Ile-Met-Asn-Ser-OH&amp;lt;/tt&amp;gt;&amp;lt;/small&amp;gt;&lt;br /&gt;
|MW 2467&lt;br /&gt;
|  1 mg in 405 µL = 1 mM&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |'''PGLa:'''&lt;br /&gt;
|   &amp;lt;small&amp;gt;&amp;lt;tt&amp;gt;H-Gly-Met-Ala-Ser-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Gly-Ala-Ile-Ala-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ile-Ala-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Val-Ala-Leu-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Leu-NH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;/tt&amp;gt;&amp;lt;/small&amp;gt;&lt;br /&gt;
|MW 1969&lt;br /&gt;
|  1 mg in 508 µL = 1 mM&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Nonetheless at physiological pH each magainin still contains four positively charged lysine residues which are believed to help target the negatively charged cell membranes of bacteria while ignoring relatively uncharged vertebrate cell membranes. PGLa is a slightly smaller polypeptide but also has four positively charged lysine residues.&lt;br /&gt;
&lt;br /&gt;
At least one derivative of magainin, [http://dx.doi.org/10.2165/00003495-199856060-00011 Pexiganan], has been in clinical trials for use in antibiotic medications such as [http://dipexiumpharmaceuticals.com Locilex™]. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Magainins, a class of antimicrobial peptides from Xenopus skin: Isolation, characterization of two active forms, and partial cDNA sequence of a precursor. Michael Zasloff, Proceedings of the  National Academy of Sciences, [http://www.pnas.org/content/84/15/5449.full.pdf 84, 5449-5453, 1987.]&lt;br /&gt;
# Membrane Pores Induced by Magainin. Steve J. Ludtke, Ke He, William T. Heller, Thad A. Harroun, Lin Yang, and Huey W. Huang, Biochemistry, 35, 13723-13728, 1996. [http://dx.doi.org/10.1021/bi9620621 DOI: 10.1021/bi9620621] Free [http://dipexiumpharmaceuticals.com/files/Ludtke1996.pdf download].&lt;br /&gt;
# Interaction of a Magainin−PGLa Hybrid Peptide with Membranes:  Insight into the Mechanism of Synergism. Minoru Nishida , Yuichi Imura, Megumi Yamamoto, Satoe Kobayashi, Yoshiaki Yano, and Katsumi Matsuzaki, Biochemistry, 46, 14284–14290 2007. [http://dx.doi.org/10.1021/bi701850m DOI: 10.1021/bi701850m]&lt;br /&gt;
# In Vitro Antibacterial Properties of Pexiganan, an Analog of Magainin. Yigong Ge, Dorothy L. MacDonald, Kenneth J. Holroyd, Clyde Thornsberry, Hannah Wexler, and Michael Zasloff, Antimicrobial Agents and Chemotherapy, 43, 782-788, 1999. [http://aac.asm.org/content/43/4/782.full.pdf+html Free download.]&lt;br /&gt;
# [http://www.anaspec.com/products/product.asp?id=30706 Magainin 1] and [http://www.anaspec.com/products/product.asp?id=30708 Magainin 2] available from AnaSpec, as well as [http://www.abbiotec.com/peptides?populate=Antimicrobial&amp;amp;field_protein_family_tid=All Abbiotec] and [http://www.genscript.com/ GenScript] who also supply PGLa.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:MonensinA.jpg|200px|thumb|right|Monensin A. MW 670.9]]&lt;br /&gt;
&lt;br /&gt;
=== Monensin A ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Monensin Monensin] is used in the livestock industry as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=095-735 Rumensin&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=038-878 Coban&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], Elancoban&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;, Coxidin&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;), where it can alter the gut flora (bacteria populations) of the animal so that animal growth rates are improved. However some species have a low tolerance and it is particularly toxic to horses.&lt;br /&gt;
&lt;br /&gt;
It has been reported to have anti-tumor properties, and has also been investigated as a chelation agent for the treatment of lead toxicity.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 37.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Structure and Antimicrobial Properties of Monensin A and Its Derivatives: Summary of the Achievements Daniel Łowicki and Adam Huczyński, BioMed Research International, Article ID 742149, 2013. [http://dx.doi.org/10.1155/2013/742149 DOI: 10.1155/2013/742149]&lt;br /&gt;
# Effect of Monensin and Lasalocid-Sodium on the Growth of Methanogenic and Rumen Saccharolytic Bacteria. Min Chen and MJ Wolin, Applied and Environmental Microbiology, 72-77, 1979. Free Access at PubMed Central: [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC243437 PMC243437]&lt;br /&gt;
# Ionophores for Dairy Cattle: Current Status and Future Outlook. R.K. McGuffey, L.F. Richardson, J.I.D. Wilkinson, Journal of Dairy Science 84, E194–E203, 2001. [http://dx.doi.org/10.3168/jds.S0022-0302(01)70218-4 DOI: 10.3168/jds.S0022-0302(01)70218-4]&lt;br /&gt;
#Polyether ionophores — promising bioactive molecules for cancer therapy. Adam Huczyński, Bioorganic &amp;amp; Medicinal Chemistry Letters, 22, 7002–7010, 2012. [http://dx.doi.org/10.1016/j.bmcl.2012.09.046 DOI: 10.1016/j.bmcl.2012.09.046]&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Monensin Improves the Effectiveness of meso-Dimercaptosuccinate when Used to Treat Lead Intoxication in Rats. Shawn A. Hamidinia, Warren L. Erdahl, Clifford J. Chapman, Gregory E. Steinbaugh, Richard W. Taylor, and Douglas R. Pfeiffer, Environmental Health Perspectives, 114, 484–493, 2006. [http://dx.doi.org/10.1289/ehp.8279 DOI: 10.1289/ehp.8279]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.bioagrimix.com/haccp/html/ionophores.html Hazard Analysis Critical Control Point (HACCP) Manual], Bio Agri Mix LP.&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Monensin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-M1303-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Narasin.jpg|200px|thumb|right|Narasin. MW 765.0. Compare this structure with that of Salinomycin, below. Note the methyl group in the lower left hand corner.]]&lt;br /&gt;
&lt;br /&gt;
=== Narasin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Narasin Narasin] is a methylated derivative of [http://en.wikipedia.org/wiki/Salinomycin salinomycin], and has similar properties. It is used as a food additive ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=118-980 Monteban&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;]) in the poultry industry where it acts as a [http://en.wikipedia.org/wiki/Coccidiostat coccidiostat].&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 32.7 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''Reference'''&lt;br /&gt;
&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=narasin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-N1363-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:NystatinA1.jpg|200px|thumb|right|Nystatin A1. MW 926.1. Compare this structure with that of Amphotericin B, above.]]&lt;br /&gt;
&lt;br /&gt;
=== Nystatin A===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Nystatin Nystatin] is an antifungal antibiotic often prescribed for the treatment of [http://en.wikipedia.org/wiki/Candida_(fungus) ''Candida''] infections. It forms ion channels in the fungal cell membrane with the assistance of [http://en.wikipedia.org/wiki/Ergosterol ergosterol] which is a naturally occurring lipid in fungal membranes. As a [http://www.nlm.nih.gov/medlineplus/druginfo/meds/a682758.html medicine] Nystatin is taken orally or topically.&lt;br /&gt;
&lt;br /&gt;
It is also used as an ingredient in several topical veterinary medications ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=012-258 Panolog&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=140-847 Animax], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=140-810 Derma-Vet™, Panavet] and [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=141-003 Derm-Otic]) for cats and dogs, and as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=012-680 Pharmastatin&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;-20]) for [http://en.wikipedia.org/wiki/Candida_(fungus) ''Candida''] infections in turkeys.&lt;br /&gt;
&lt;br /&gt;
While its affinity for [http://en.wikipedia.org/wiki/Ergosterol ergosterol] makes it target fungal cells, it can also interact, with the [http://en.wikipedia.org/wiki/Cholesterol cholesterol] in mammalian cells. This can limit its therapeutic dosage because of toxicity.&lt;br /&gt;
&lt;br /&gt;
It is similar both in structure and in action to Amphotericin B.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Leafcutter_ant Leafcutter ants] use nystatin-like antibiotics to selectively raise the fungus they produce in their leaf-mulch gardens.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 27.0 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=nystatin Drug Information Online].&lt;br /&gt;
#A mixed community of [http://en.wikipedia.org/wiki/Actinobacteria actinomycetes] produce multiple antibiotics for the fungus farming ant [http://en.wikipedia.org/wiki/Acromyrmex_octospinosus ''Acromyrmex octospinosus''].  Jörg Barke, Ryan F. Seipke, Sabine Grüschow, Darren Heavens, Nizar Drou, Mervyn J. Bibb,Rebecca J.M. Goss, Douglas W. Yu, Matthew I. Hutchings, BMC Biology, 8, 109, 2010. [http://dx.doi.org/doi:10.1186/1741-7007-8-109 DOI: 10.1186/1741-7007-8-109]&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-N1416-25mg eDAQ].&lt;br /&gt;
# Australian veterinary [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Salinomycin.jpg|200px|thumb|right|Salinomycin. MW 751.0. Compare this structure with that of Narasin, above.]]&lt;br /&gt;
&lt;br /&gt;
=== Salinomycin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Salinomycin Salinomycin] is used in the poultry industry as a food supplement ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=128-686 Bio-Cox&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=200-075 Sacox&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;] ), where it acts as a [http://en.wikipedia.org/wiki/Coccidiostat coccidiostat].&lt;br /&gt;
&lt;br /&gt;
It is also being investigated as an anti-cancer agent.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 33.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Persistence of antibiotics such as macrolides, tiamulin and salinomycin in soil. Michael P. Schlüsener, Kai Bester, Environmental Pollution, 143, 565–571, 2006. [http://dx.doi.org/10.1016/j.envpol.2005.10.049 DOI: 10.1016/j.envpol.2005.10.049]&lt;br /&gt;
# Effects of the veterinary pharmaceutical salinomycin and its formulation on the plant ''Brassica rapa''. V. Furtula, G. L. Stephenson, K. M. Olaveson, P. A. Chambers, Archives of  Environmental Contamination and Toxicology,  63, 513-522, 2012. [http://dx.doi.org/10.1007/s00244-012-9807-y DOI: 10.1007/s00244-012-9807-y]&lt;br /&gt;
#Polyether ionophores—promising bioactive molecules for cancer therapy. Adam Huczyński, Bioorganic &amp;amp; Medicinal Chemistry Letters, 22, 7002–7010, 2012. [http://dx.doi.org/10.1016/j.bmcl.2012.09.046 DOI: 10.1016/j.bmcl.2012.09.046]&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# A case of human poisoning by salinomycin, an agricultural antibiotic. Phillipa Story and Alan Doube, The New Zealand Medical Journal, [http://journal.nzma.org.nz/journal/117-1190/799/content.pdf 117, 1190, 2004.]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf 15, 7-9, 2007.]&lt;br /&gt;
# [http://www.bioagrimix.com/haccp/html/ionophores.html Hazard Analysis Critical Control Point (HACCP) Manual], Bio Agri Mix LP.&lt;br /&gt;
# [http://www.merck-animal-health-usa.com/binaries/intp1069_SACOX_tcm96-86731.pdf SACOX Product Information Sheet], Invert Inc.&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=salinomycin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-S1540-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Valinomycin.jpg|200px|thumb|right|Valinomycin. MW 1111.3]]&lt;br /&gt;
&lt;br /&gt;
=== Valinomycin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Valinomycin Valinomycin] is a macrocylic polypeptide and is historically one of the best known ionophores, especially for its 10&amp;lt;sup&amp;gt;4&amp;lt;/sup&amp;gt; fold selectivity for potassium over sodium ions. It is being investigated for use as an antibiotic, as well as being used in the manufacture of [http://en.wikipedia.org/wiki/Potassium_selective_electrode potassium ion selective electrodes].&lt;br /&gt;
&lt;br /&gt;
Dissolve 100 mg in 90.0 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# K&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Na&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; Selectivity in K-Channels and Valinomycin: Over-coordination Versus Cavity-size constraints. Sameer Varma, Dubravko Sabo, Susan B. Rempe, Journal of Molecular Biology, 376 13–22, 2008. [http://dx.doi.org/10.1016/j.jmb.2007.11.059 DOI: 10.1016/j.jmb.2007.11.059]. Free Access at PubMed Central: [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC2390915 PMC2390915]&lt;br /&gt;
#Design principles for K+ selectivity in membrane transport. Sameer Varma, David M. Rogers, Lawrence R. Pratt, and Susan B. Rempe, Journal of General Physiology, 137, 479-488, 2011. [http://dx.doi.org/10.1085/jgp.201010579 DOI: 10.1085/jgp.201010579]&lt;br /&gt;
#Ion-Selective Electrodes With Ionophore-Doped Sensing Membranes, Philippe Bühlmann and Li D. Chen, 2539-2579 in &amp;quot;Supramolecular Chemistry: From Molecules to Nanomaterials&amp;quot;, Philip A. Gale and Jonathan W. Steed (Eds), John Wiley &amp;amp; Sons Ltd. 2012. ISBN: 978-0-470-74640-0. Free [http://www.chem.umn.edu/groups/buhlmann/Ion-Selective%20Electrodes%20With%20Ionophore-Doped.pdf download].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-V1114-100mg eDAQ].&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Ionophores_in_Society&amp;diff=4224</id>
		<title>Ionophores in Society</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Ionophores_in_Society&amp;diff=4224"/>
				<updated>2016-08-24T07:59:37Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&amp;lt;big&amp;gt;'''Medicines, Toxins, Pollutants, Growth Promoters, Sensors'''&amp;lt;/Big&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Ionophore Ionophores] are lipophilic molecules produced, and often excreted, by microorganisms and animals that are characterised by their ability to transport ions (especially Na&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;, K&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;, Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;, and Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;) across cell membranes. They are not only chemically interesting in their own right but many have important medical and economic roles in our society.&lt;br /&gt;
&lt;br /&gt;
A selection of ionophores is presented below for study in mainstream chemistry courses as well as courses for pre-med, vet, pharma, biochemistry, and soil and agricultural science students.  The demonstration of ion movement across membranes is also relevant to courses on neurophysiology, and biophysics.&lt;br /&gt;
&lt;br /&gt;
The use of ionophore 'growth promoters' in the animal feedstock industry is not only of interest to agricultural scientists, but also of concern to environmental chemists because of their presence in manure and sewerage sludges than are used as fertiliser for human and animal crops.&lt;br /&gt;
&lt;br /&gt;
The ability of these materials to transport ions across phospholipid bilayer cell membranes, which is usually the key to understanding their mode of action, can be easily studied using [http://wiki.edaq.com/index.php/Tethered_Membranes tethered membrane technology]. A suitable method is outlined in Application Note: [http://wiki.edaq.com/index.php/SDx_Protocol_1 SDx Protocol 1].&lt;br /&gt;
&lt;br /&gt;
Most of these ionophores can be obtained from [http://www.edaq.com/chemicals eDAQ].&lt;br /&gt;
&lt;br /&gt;
=== Amphotericin B ===&lt;br /&gt;
[[File:AmphotericinB_1.jpg|200px|thumb|right|Amphotericin B. MW 923.5. Compare this structure with that of Nystatin, below.]]&lt;br /&gt;
[http://en.wikipedia.org/wiki/Amphotericin_B Amphotericin B] is an antibiotic ([http://www.accessdata.fda.gov/drugsatfda_docs/label/2012/050740s021lbl.pdf AmBisome&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], ) used to treat serious fungal infections. It forms ion channels in the fungal cell membrane with the assistance of [http://en.wikipedia.org/wiki/Ergosterol ergosterol] which is a naturally occurring lipid in fungal membranes. As a [http://www.nlm.nih.gov/medlineplus/druginfo/meds/a682643.html medicine] it is administered intravenously as a [http://www.accessdata.fda.gov/drugsatfda_docs/label/2008/050740s016lbl.pdf liposomal preparation].&lt;br /&gt;
&lt;br /&gt;
While its affinity for [http://en.wikipedia.org/wiki/Ergosterol ergosterol] makes it target fungal cells, Amphotericin can also interact with the [http://en.wikipedia.org/wiki/Cholesterol cholesterol] in mammalian cells. This limits its therapeutic dosage because of toxicity.&lt;br /&gt;
&lt;br /&gt;
Amphotericin B is similar both in structure and in action to Nystatin.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 27.0 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Novel, unifying mechanism for amphotericin B and other polyene drugs: electron affinity, radicals, electron transfer, autoxidation, toxicity, and antifungal action. Peter Kovacic and    Andrew Cooksy, Medicinal Chemical Communications, 3, 274-280, 2012. [http://dx.doi.org/10.1039/C2MD00267A DOI: 10.1039/C2MD00267A]&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Amphotericin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-A1441-25mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Beauvericin.jpg|200px|thumb|right|Beauvericin. MW 784.0. Compare this structure with that of the Enniatin Complex, below.]]&lt;br /&gt;
&lt;br /&gt;
=== Beauvericin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Beauvericin Beauvericin] is closely related to the macrocyclic enniatins, having three benzyl groups in place of the aliphatic chains of the enniatins. It is a potentially toxic agent found in grain crops affected by [http://en.wikipedia.org/wiki/Fusarium ''Fusarium''] fungi. The selectivity for monovalent cations is reported as K&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; &amp;gt; Na&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ~ Rb&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; &amp;gt; Cs&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ~ Li&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; &amp;gt; NH&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;, and for divalent cations as  Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;. The antibiotic properties of Beauvericin are being investigated.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 31.9 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Occurrence of Beauvericin and Enniatins in Wheat Affected by ''Fusarium avenaceum'' Head Blight. A Logrieco, A Rizzo, R Ferracane, and A Ritieni, Applied Environmental Microbiology, 68, 82-85, 2002. [http://dx.doi.org/10.1128/AEM.68.1.82-85.2002 DOI: 10.1128/AEM.68.1.82-85.2002]&lt;br /&gt;
# Selective Binding of Alkali and Alakaline Earth Ions to Beauvericin Investigated by Electrospray Mass Spectrometry. Tara-Lynn Baratz, Courtney N. Richardson, J. Brett Kimbrell, Joshua Hite, (Dr. Farooq A. Khan). [https://ncurdb.cur.org/ncur/archive/Display_NCUR.aspx?id=41814 Poster presentation], 2010.&lt;br /&gt;
# Beauvericin and enniatins H, I and MK1688 are new potent inhibitors of human immunodeficiency virus type-1 integrase. CG Shin, DG An, HH Song, C Lee, The Journal of antibiotics, 62, 687-690, 2009. [http://dx.doi.org/10.1038/ja.2009.102 DOI: 10.1038/ja.2009.102]&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-B1238-25mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Calcimycin.jpg|200px|thumb|right|Calcimycin. MW 523.6]]&lt;br /&gt;
&lt;br /&gt;
=== Calcimycin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Calcimycin Calcimycin] is also widely known as Ionophore A23187. The most notable feature of calcimycin  is the ability to transport divalent cation across cell membranes. Its in vitro affinity for cations is Ni&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Co&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Zn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; ~ Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;, however transport rates across lipsomal membranes are reported as Cd&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt;  Zn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;. Calcimycin has antibiotic properties, and is also being used in [http://www.gynemed.de/fileadmin/downloads/Medien/Produktfolien/Backgroundinformation_GM508_Cult-Active_Rev01_00.pdf IVF treatments]. &lt;br /&gt;
&lt;br /&gt;
Dissolve 5 mg in 9.55 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
# Structures and Properties of Naturally Occurring Polyether Antibiotics. Jacek Rutkowski and Bogumil Brzezinski, BioMed Research International, Article ID 162513, 2013. [http://dx.doi.org/10.1155/2013/162513 DOI: 10.1155/2013/162513]&lt;br /&gt;
# Equilibria between ionophore A23187 and divalent cations: stability of 1:1 complexes in solutions of 80% methanol/water. CJ Chapman, AK Puri, RW Taylor, DR Pfeiffer, Biochemistry, 26, 5009-5018, 1987. [http://dx.doi.org/10.1021/bi00390a019 DOI: 10.1021/bi00390a019]&lt;br /&gt;
# The specificity of ionophore A23187 in cation transport across lipid membranes. Studies with lecithin vesicles. WG Pohl, R Kreikenbohm, K. Seuwen, Z Naturforsch C, 35, 562-568, 1980.&lt;br /&gt;
#Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; transport properties of ionophores A23187, ionomycin, and 4-BrA23187 in a well defined model system. W.L. Erdahl, C.J. Chapman, R.W. Taylor and D.R. Pfeiffer, Biophysical Journal,  66, 1678-1693, 1994. [http://dx.doi.org/DOI:10.1016/S0006-3495(94)80959-2 10.1016/S0006-3495(94)80959-2]&lt;br /&gt;
# Application of a ready-to-use calcium ionophore increases rates of fertilization and pregnancy in severe male factor infertility. Thomas Ebner, Maria Köster, Omar Shebl, Marianne Moser, Hans Van der Ven, Gernot Tews, Markus Montag, Fertility and Sterility, 98, 1432–1437, 2012. [http://dx.doi.org/10.1016/j.fertnstert.2012.07.1134 DOI: 10.1016/j.fertnstert.2012.07.1134]. Free [http://www.utd.org.tr/download/kasim_2012/Kasim-MAKALE2ORJINAL.pdf download].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-C1236-5mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:EnniatinComplex.jpg|200px|thumb|right|Enniatin Complex. Approximate MW 640. Beauvericin is a related molecule with R&amp;lt;sub&amp;gt;1&amp;lt;/sub&amp;gt; = R&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; = R&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt; = benzyl.]]&lt;br /&gt;
&lt;br /&gt;
===  Enniatin complex ===&lt;br /&gt;
[http://en.wikipedia.org/wiki/Enniatin Enniatins] are produced by [http://en.wikipedia.org/wiki/Fusarium ''Fusarium''] fungi that commonly infect wheat and other grains. High levels are potentially toxic.&lt;br /&gt;
&lt;br /&gt;
A mixture of related macrocylic molecules, with different peripheral alkyl substituents, is commonly encountered and this is refried to as a 'complex'. There are at least 28 naturally occurring enniatins.&lt;br /&gt;
&lt;br /&gt;
Enniantins also have promise as antibiotics and anti-cancer drugs.&lt;br /&gt;
&lt;br /&gt;
Dissolve 50 mg in 78.1 mL, or 10 mg in 15.6 mL, of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Occurrence of Beauvericin and Enniatins in Wheat Affected by ''Fusarium avenaceum'' Head Blight. A Logrieco, A Rizzo, R Ferracane, and A Ritieni, Applied Environmental Microbiology, 68, 82-85, 2002. [http://dx.doi.org/10.1128/AEM.68.1.82-85.2002 DOI: 10.1128/AEM.68.1.82-85.2002]&lt;br /&gt;
# Beauvericin and enniatins H, I and MK1688 are new potent inhibitors of human immunodeficiency virus type-1 integrase. CG Shin, DG An, HH Song, C Lee, The Journal of antibiotics, 62, 687-690, 2009. [http://dx.doi.org/10.1038/ja.2009.102 DOI: 10.1038/ja.2009.102]&lt;br /&gt;
# [http://toxinology.nilu.no/Researchareas/Fungaltoxins/Factsheets/Enniatins/tabid/4536/Default.aspx Toxicology Portal at Toxicology.no].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-E1071-50mg eDAQ].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:GramicidinA.jpg|200px|thumb|right|Gramicidin A. MW 1882]]&lt;br /&gt;
&lt;br /&gt;
=== Gramicidin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Gramicidin Gramicidin] is often regarded as the archetypal ion channel for monovalent cations, despite its unusual dimer arrangement that forms across the cell membrane. It was one of the first commercially available antibiotics and is used today in several topical medications ([http://www.drugs.com/ingredient/gramicidin.html Neosporin, Neocidin, Neoptic, Ocu-Spore-G]).&lt;br /&gt;
&lt;br /&gt;
Gramicidin is usually sold as a mixture of related linear polypeptides (principally A, B and C) but the main component is Gramicidin A.&lt;br /&gt;
&lt;br /&gt;
Dissolve 100 mg in 53.1 mL of solvent to make a 1.00 mM stock solution. &lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Gramicidin_S Gramicidin S] is an unusual macrocyclic variant.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# The gramicidin ion channel: A model membrane protein. Devaki A. Kelkar, Amitabha Chattopadhyay, Biochimica et Biophysica Acta 1768, 2011–2025, 2007. [http://dx.doi.org/10.1016/j.bbamem.2007.05.011 DOI: 10.1016/j.bbamem.2007.05.011]&lt;br /&gt;
# Structure of gramicidin A. B A Wallace, Biophysics Journal, 49, 295–306, 1986. Free access at PubMed Central: [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC1329637/ PMC1329637]&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Gramicidin Drug Information Online].&lt;br /&gt;
# Available from [http://www.sigmaaldrich.com/catalog/product/sigma/g5002?lang=en&amp;amp;region=US Sigma-Aldrich] or [http://www.scbt.com/datasheet-252865-gramicidin-from-bacillus-aneurinolyticus-bacillus-brevis.html Santa Cruz Biotechnology]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Ionomycin.jpg|350px|thumb|right|Ionomycin. MW 747.1]]&lt;br /&gt;
&lt;br /&gt;
=== Ionomycin ===&lt;br /&gt;
[http://en.wikipedia.org/wiki/Ionomycin Ionomycin] is a noted calcium ionophore with a selectivity of Pb&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Cd&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Zn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mn&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt; Mg&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; &amp;gt;&amp;gt; Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; ~ Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt;. There is almost no binding to Sr&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; or Ba&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; or to  monovalent alkali metal cations.&lt;br /&gt;
&lt;br /&gt;
Dissolve 5 mg in 6.69 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# [http://www.jbc.org/content/253/17/5892 Characterization of ionomycin as a calcium ionophore.] C Liu and T E Hermann, Journal of Biological Chemistry, 253, 5892-5894, 1978.&lt;br /&gt;
# Ca&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; transport properties of ionophores A23187, ionomycin, and 4-BrA23187 in a well defined model system. W.L. Erdahl, C.J. Chapman, R.W. Taylor and D.R. Pfeiffer, Biophysical Journal,  66, 1678-1693, 1994. [http://dx.doi.org/10.1016/S0006-3495(94)80959-2 DOI:10.1016/S0006-3495(94)80959-2]&lt;br /&gt;
# Ionomycin, a Carboxylic Acid Ionophore, Transports Pb&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; with High Selectivity. Warren L. Erdahl, Clifford J. Chapman, Richard W. Taylor and Douglas R. Pfeiffer, Journal of Biological Chemistry, 275, 7071-7079, 2000. [http://dx.doi.org/10.1074/jbc.275.10.7071 DOI: 10.1074/jbc.275.10.7071]&lt;br /&gt;
# Ion-selective electrodes based on natural carboxylic polyether antibiotics. Koji Suzuki, Koji Tohda, Hiroshi Aruga, Misako Matsuzoe, Hidenari Inoue, Tsuneo Shirai, Analytical Chemistry, 60, 1714–1721, 1988. [http://dx.doi.org/10.1021/ac00168a016 DOI: 10.1021/ac00168a016]&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-I1261-5mg eDAQ], [http://www.hoelzel-biotech.com/en/products/detail/nr/lc-laboratories--inhibitors--other--i-5700-25mg--ionomycin-free-acid.html Hölzel Diagnostica], or [http://www.lclabs.com/PRODFILE/G-K/I-5700.php4 LC Labs].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Lasalocid.jpg|200px|thumb|right|Lasalocid. MW 590.8]]&lt;br /&gt;
&lt;br /&gt;
=== Lasalocid ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Lasalocid Lasalocid] is used as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=096-298 Avatec&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;, Bovatec&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;])  for control of coccidiosis, a protozoan parasite of poultry and livestock.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 42.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC243437/pdf/aem00200-0082.pdf, Effect of Monensin and Lasalocid-Sodium on the Growth of Methanogenic and Rumen Saccharolytic Bacteria]. Min Chen and MJ Wolin, Applied and Environmental Microbiology, 72-77, 1979.&lt;br /&gt;
# Ionophores for Dairy Cattle: Current Status and Future Outlook. R.K. McGuffey, L.F. Richardson, J.I.D. Wilkinson, Journal of Dairy Science 84, E194–E203, 2001. [http://dx.doi.org/10.3168/jds.S0022-0302(01)70218-4 DOI: 10.3168/jds.S0022-0302(01)70218-4]&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Ion-selective electrodes based on natural carboxylic polyether antibiotics. Koji Suzuki, Koji Tohda, Hiroshi Aruga, Misako Matsuzoe, Hidenari Inoue, Tsuneo Shirai, Analytical Chemistry, 60, 1714–1721, 1988. [http://dx.doi.org/10.1021/ac00168a016 DOI: 10.1021/ac00168a016]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Lasalocid Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-L1533-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Maduramicin.jpg|200px|thumb|right|Maduramicin. MW 917.1]]&lt;br /&gt;
&lt;br /&gt;
=== Maduramicin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Maduramicin Maduramicin] is used as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=139-075 Cygro&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;]) for control of coccidiosis, a protozoan parasite of poultry and livestock.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 27.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Maduramicin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-M1542-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
=== Magainins and PGLa===&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Magainin magainins] are linear polypeptides of 23 amino acids first discovered in the skin of the African clawed frog, [http://en.wikipedia.org/wiki/Xenopus ''Xenopus laevis''], and are believed to be responsible for the resistance of the frog to many of the pathogens that would otherwise cause disease in their moist habitat. Magainins and similar compounds are now known to be present in the skin of many amphibians and are have been shown to be active against  viruses, both gram-positive and gram-negative bacteria, protozoa, yeasts and fungi, and may also be hemolytic and cytotoxic to cancer cells. Their mode of action is believed to be by 4 − 7 magainin molecules forming a pore in the phospholipid bilayer membrane of their target. Magainin 2 also has a synergistic effect with the linear polypeptide PGLa (also from ''Xenopus'') suggesting the formation of a hybrid pore.&lt;br /&gt;
&lt;br /&gt;
Magainins 1 and 2 differ in two amino acid locations where a positively charged lysine residue (&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;) is replaced by a neutral amino acid. &lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;0&amp;quot; style=&amp;quot;width:1000px; height:40px;&amp;quot;&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |'''Magainin 1:'''&lt;br /&gt;
|   &amp;lt;small&amp;gt;&amp;lt;tt&amp;gt;H-Gly-Ile-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Leu-His-Ser-Ala-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Phe-Val-Gly-Glu-Ile-Met-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ser-OH&amp;lt;/tt&amp;gt;&amp;lt;/small&amp;gt;&lt;br /&gt;
|MW 2410&lt;br /&gt;
|  1 mg in 415 µL = 1 mM&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |'''Magainin 2:'''&lt;br /&gt;
|   &amp;lt;small&amp;gt;&amp;lt;tt&amp;gt;H-Gly-Ile-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Leu-His-Ser-Ala-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Phe-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Phe-Val-Gly-Glu-Ile-Met-Asn-Ser-OH&amp;lt;/tt&amp;gt;&amp;lt;/small&amp;gt;&lt;br /&gt;
|MW 2467&lt;br /&gt;
|  1 mg in 405 µL = 1 mM&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |'''PGLa:'''&lt;br /&gt;
|   &amp;lt;small&amp;gt;&amp;lt;tt&amp;gt;H-Gly-Met-Ala-Ser-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Gly-Ala-Ile-Ala-Gly-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ile-Ala-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Val-Ala-Leu-&amp;lt;span style=&amp;quot;color:#00BFFF&amp;quot;&amp;gt;Lys&amp;lt;/span&amp;gt;-Ala-Leu-NH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;/tt&amp;gt;&amp;lt;/small&amp;gt;&lt;br /&gt;
|MW 1969&lt;br /&gt;
|  1 mg in 508 µL = 1 mM&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
Nonetheless at physiological pH each magainin still contains four positively charged lysine residues which are believed to help target the negatively charged cell membranes of bacteria while ignoring relatively uncharged vertebrate cell membranes. PGLa is a slightly smaller polypeptide but also has four positively charged lysine residues.&lt;br /&gt;
&lt;br /&gt;
At least one derivative of magainin, [http://dx.doi.org/10.2165/00003495-199856060-00011 Pexiganan], has been in clinical trials for use in antibiotic medications such as [http://dipexiumpharmaceuticals.com Locilex™]. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Magainins, a class of antimicrobial peptides from Xenopus skin: Isolation, characterization of two active forms, and partial cDNA sequence of a precursor. Michael Zasloff, Proceedings of the  National Academy of Sciences, [http://www.pnas.org/content/84/15/5449.full.pdf 84, 5449-5453, 1987.]&lt;br /&gt;
# Membrane Pores Induced by Magainin. Steve J. Ludtke, Ke He, William T. Heller, Thad A. Harroun, Lin Yang, and Huey W. Huang, Biochemistry, 35, 13723-13728, 1996. [http://dx.doi.org/10.1021/bi9620621 DOI: 10.1021/bi9620621] Free [http://dipexiumpharmaceuticals.com/files/Ludtke1996.pdf download].&lt;br /&gt;
# Interaction of a Magainin−PGLa Hybrid Peptide with Membranes:  Insight into the Mechanism of Synergism. Minoru Nishida , Yuichi Imura, Megumi Yamamoto, Satoe Kobayashi, Yoshiaki Yano, and Katsumi Matsuzaki, Biochemistry, 46, 14284–14290 2007. [http://dx.doi.org/10.1021/bi701850m DOI: 10.1021/bi701850m]&lt;br /&gt;
# In Vitro Antibacterial Properties of Pexiganan, an Analog of Magainin. Yigong Ge, Dorothy L. MacDonald, Kenneth J. Holroyd, Clyde Thornsberry, Hannah Wexler, and Michael Zasloff, Antimicrobial Agents and Chemotherapy, 43, 782-788, 1999. [http://aac.asm.org/content/43/4/782.full.pdf+html Free download.]&lt;br /&gt;
# [http://www.anaspec.com/products/product.asp?id=30706 Magainin 1] and [http://www.anaspec.com/products/product.asp?id=30708 Magainin 2] available from AnaSpec, as well as [http://www.abbiotec.com/peptides?populate=Antimicrobial&amp;amp;field_protein_family_tid=All Abbiotec] and [http://www.genscript.com/ GenScript] who also supply PGLa.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:MonensinA.jpg|200px|thumb|right|Monensin A. MW 670.9]]&lt;br /&gt;
&lt;br /&gt;
=== Monensin A ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Monensin Monensin] is used in the livestock industry as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=095-735 Rumensin&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=038-878 Coban&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], Elancoban&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;, Coxidin&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;), where it can alter the gut flora (bacteria populations) of the animal so that animal growth rates are improved. However some species have a low tolerance and it is particularly toxic to horses.&lt;br /&gt;
&lt;br /&gt;
It has been reported to have anti-tumor properties, and has also been investigated as a chelation agent for the treatment of lead toxicity.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 37.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Structure and Antimicrobial Properties of Monensin A and Its Derivatives: Summary of the Achievements Daniel Łowicki and Adam Huczyński, BioMed Research International, Article ID 742149, 2013. [http://dx.doi.org/10.1155/2013/742149 DOI: 10.1155/2013/742149]&lt;br /&gt;
# Effect of Monensin and Lasalocid-Sodium on the Growth of Methanogenic and Rumen Saccharolytic Bacteria. Min Chen and MJ Wolin, Applied and Environmental Microbiology, 72-77, 1979. Free Access at PubMed Central: [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC243437 PMC243437]&lt;br /&gt;
# Ionophores for Dairy Cattle: Current Status and Future Outlook. R.K. McGuffey, L.F. Richardson, J.I.D. Wilkinson, Journal of Dairy Science 84, E194–E203, 2001. [http://dx.doi.org/10.3168/jds.S0022-0302(01)70218-4 DOI: 10.3168/jds.S0022-0302(01)70218-4]&lt;br /&gt;
#Polyether ionophores — promising bioactive molecules for cancer therapy. Adam Huczyński, Bioorganic &amp;amp; Medicinal Chemistry Letters, 22, 7002–7010, 2012. [http://dx.doi.org/10.1016/j.bmcl.2012.09.046 DOI: 10.1016/j.bmcl.2012.09.046]&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Monensin Improves the Effectiveness of meso-Dimercaptosuccinate when Used to Treat Lead Intoxication in Rats. Shawn A. Hamidinia, Warren L. Erdahl, Clifford J. Chapman, Gregory E. Steinbaugh, Richard W. Taylor, and Douglas R. Pfeiffer, Environmental Health Perspectives, 114, 484–493, 2006. [http://dx.doi.org/10.1289/ehp.8279 DOI: 10.1289/ehp.8279]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.bioagrimix.com/haccp/html/ionophores.html Hazard Analysis Critical Control Point (HACCP) Manual], Bio Agri Mix LP.&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=Monensin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-M1303-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Narasin.jpg|200px|thumb|right|Narasin. MW 765.0. Compare this structure with that of Salinomycin, below. Note the methyl group in the lower left hand corner.]]&lt;br /&gt;
&lt;br /&gt;
=== Narasin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Narasin Narasin] is a methylated derivative of [http://en.wikipedia.org/wiki/Salinomycin salinomycin], and has similar properties. It is used as a food additive ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=118-980 Monteban&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;]) in the poultry industry where it acts as a [http://en.wikipedia.org/wiki/Coccidiostat coccidiostat].&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 32.7 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''Reference'''&lt;br /&gt;
&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, 15, 7-9, 2007. Free [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf download].&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=narasin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-N1363-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:NystatinA1.jpg|200px|thumb|right|Nystatin A1. MW 926.1. Compare this structure with that of Amphotericin B, above.]]&lt;br /&gt;
&lt;br /&gt;
=== Nystatin A===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Nystatin Nystatin] is an antifungal antibiotic often prescribed for the treatment of [http://en.wikipedia.org/wiki/Candida_(fungus) ''Candida''] infections. It forms ion channels in the fungal cell membrane with the assistance of [http://en.wikipedia.org/wiki/Ergosterol ergosterol] which is a naturally occurring lipid in fungal membranes. As a [http://www.nlm.nih.gov/medlineplus/druginfo/meds/a682758.html medicine] Nystatin is taken orally or topically.&lt;br /&gt;
&lt;br /&gt;
It is also used as an ingredient in several topical veterinary medications ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=012-258 Panolog&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=140-847 Animax], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=140-810 Derma-Vet™, Panavet] and [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=141-003 Derm-Otic]) for cats and dogs, and as a food supplement antibiotic ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=012-680 Pharmastatin&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;-20]) for [http://en.wikipedia.org/wiki/Candida_(fungus) ''Candida''] infections in turkeys.&lt;br /&gt;
&lt;br /&gt;
While its affinity for [http://en.wikipedia.org/wiki/Ergosterol ergosterol] makes it target fungal cells, it can also interact, with the [http://en.wikipedia.org/wiki/Cholesterol cholesterol] in mammalian cells. This can limit its therapeutic dosage because of toxicity.&lt;br /&gt;
&lt;br /&gt;
It is similar both in structure and in action to Amphotericin B.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Leafcutter_ant Leafcutter ants] use nystatin-like antibiotics to selectively raise the fungus they produce in their leaf-mulch gardens.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 27.0 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=nystatin Drug Information Online].&lt;br /&gt;
#A mixed community of [http://en.wikipedia.org/wiki/Actinobacteria actinomycetes] produce multiple antibiotics for the fungus farming ant [http://en.wikipedia.org/wiki/Acromyrmex_octospinosus ''Acromyrmex octospinosus''].  Jörg Barke, Ryan F. Seipke, Sabine Grüschow, Darren Heavens, Nizar Drou, Mervyn J. Bibb,Rebecca J.M. Goss, Douglas W. Yu, Matthew I. Hutchings, BMC Biology, 8, 109, 2010. [http://dx.doi.org/doi:10.1186/1741-7007-8-109 DOI: 10.1186/1741-7007-8-109]&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-N1416-25mg eDAQ].&lt;br /&gt;
# Australian veterinary [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Salinomycin.jpg|200px|thumb|right|Salinomycin. MW 751.0. Compare this structure with that of Narasin, above.]]&lt;br /&gt;
&lt;br /&gt;
=== Salinomycin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Salinomycin Salinomycin] is used in the poultry industry as a food supplement ([http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=128-686 Bio-Cox&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;], [http://www.accessdata.fda.gov/scripts/animaldrugsatfda/details.cfm?dn=200-075 Sacox&amp;lt;sup&amp;gt;®&amp;lt;/sup&amp;gt;] ), where it acts as a [http://en.wikipedia.org/wiki/Coccidiostat coccidiostat].&lt;br /&gt;
&lt;br /&gt;
It is also being investigated as an anti-cancer agent.&lt;br /&gt;
&lt;br /&gt;
Dissolve 25 mg in 33.3 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# Persistence of antibiotics such as macrolides, tiamulin and salinomycin in soil. Michael P. Schlüsener, Kai Bester, Environmental Pollution, 143, 565–571, 2006. [http://dx.doi.org/10.1016/j.envpol.2005.10.049 DOI: 10.1016/j.envpol.2005.10.049]&lt;br /&gt;
# Effects of the veterinary pharmaceutical salinomycin and its formulation on the plant ''Brassica rapa''. V. Furtula, G. L. Stephenson, K. M. Olaveson, P. A. Chambers, Archives of  Environmental Contamination and Toxicology,  63, 513-522, 2012. [http://dx.doi.org/10.1007/s00244-012-9807-y DOI: 10.1007/s00244-012-9807-y]&lt;br /&gt;
#Polyether ionophores—promising bioactive molecules for cancer therapy. Adam Huczyński, Bioorganic &amp;amp; Medicinal Chemistry Letters, 22, 7002–7010, 2012. [http://dx.doi.org/10.1016/j.bmcl.2012.09.046 DOI: 10.1016/j.bmcl.2012.09.046]&lt;br /&gt;
# Trace Level Determination of Polyether Ionophores in Feed. BioMed Research International, 2013, Article ID 151363. Mervi Rokka, Marika Jestoi, and Kimmo Peltonen, [http://dx.doi.org/10.1155/2013/151363 DOI: 10.1155/2013/151363]&lt;br /&gt;
# A case of human poisoning by salinomycin, an agricultural antibiotic. Phillipa Story and Alan Doube, The New Zealand Medical Journal, [http://journal.nzma.org.nz/journal/117-1190/799/content.pdf 117, 1190, 2004.]&lt;br /&gt;
# Rotation programmes for coccidiosis control. Dr H. D. Chapman, International Poultry Production, [http://www.positiveaction.info/pdfs/articles/pp15.1p7.pdf 15, 7-9, 2007.]&lt;br /&gt;
# [http://www.bioagrimix.com/haccp/html/ionophores.html Hazard Analysis Critical Control Point (HACCP) Manual], Bio Agri Mix LP.&lt;br /&gt;
# [http://www.merck-animal-health-usa.com/binaries/intp1069_SACOX_tcm96-86731.pdf SACOX Product Information Sheet], Invert Inc.&lt;br /&gt;
# [http://www.drugs.com/search.php?searchterm=salinomycin Drug Information Online].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-S1540-25mg eDAQ].&lt;br /&gt;
# Australian [http://www.apvma.gov.au regulatory details].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
[[File:Valinomycin.jpg|200px|thumb|right|Valinomycin. MW 1111.3]]&lt;br /&gt;
&lt;br /&gt;
=== Valinomycin ===&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Valinomycin Valinomycin] is a macrocylic polypeptide and is historically one of the best known ionophores, especially for its 10&amp;lt;sup&amp;gt;4&amp;lt;/sup&amp;gt; fold selectivity for potassium over sodium ions. It is being investigated for use as an antibiotic, as well as being used in the manufacture of [http://en.wikipedia.org/wiki/Potassium_selective_electrode potassium ion selective electrodes].&lt;br /&gt;
&lt;br /&gt;
Dissolve 100 mg in 90.0 mL of solvent to make a 1.00 mM stock solution.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
# K&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Na&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; Selectivity in K-Channels and Valinomycin: Over-coordination Versus Cavity-size constraints. Sameer Varma, Dubravko Sabo, Susan B. Rempe, Journal of Molecular Biology, 376 13–22, 2008. [http://dx.doi.org/10.1016/j.jmb.2007.11.059 DOI: 10.1016/j.jmb.2007.11.059]. Free Access at PubMed Central: [http://www.ncbi.nlm.nih.gov/pmc/articles/PMC2390915 PMC2390915]&lt;br /&gt;
#Design principles for K+ selectivity in membrane transport. Sameer Varma, David M. Rogers, Lawrence R. Pratt, and Susan B. Rempe, Journal of General Physiology, 137, 479-488, 2011. [http://dx.doi.org/10.1085/jgp.201010579 DOI: 10.1085/jgp.201010579]&lt;br /&gt;
#Ion-Selective Electrodes With Ionophore-Doped Sensing Membranes, Philippe Bühlmann and Li D. Chen, 2539-2579 in &amp;quot;Supramolecular Chemistry: From Molecules to Nanomaterials&amp;quot;, Philip A. Gale and Jonathan W. Steed (Eds), John Wiley &amp;amp; Sons Ltd. 2012. ISBN: 978-0-470-74640-0. Free [http://www.chem.umn.edu/groups/buhlmann/Ion-Selective%20Electrodes%20With%20Ionophore-Doped.pdf download].&lt;br /&gt;
# Available from [http://www.edaq.com/BIA-V1114-100mg eDAQ].&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4154</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4154"/>
				<updated>2015-09-02T04:57:11Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; +  2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment. See the [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells-Copper.htm Corrosion Doctors'] website for a recipe.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4150</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4150"/>
				<updated>2015-08-18T09:24:06Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; +  2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment. See the [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells-Copper.htm Corrosion Doctors'] website for a recipe.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4149</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4149"/>
				<updated>2015-08-18T09:21:56Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; +  2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment. See the [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells-Copper.htm Corrosion Doctors] website for a recipe.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4148</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4148"/>
				<updated>2015-08-18T09:21:30Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; +  2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment. See the [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells-Copper.htm Corrosion Doctors] website for a recipe.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4147</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4147"/>
				<updated>2015-08-18T09:20:35Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
&lt;br /&gt;
:: Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; +  2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment. See the [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells-Copper.htm Corrosion Doctors] website for a recipe.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4146</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4146"/>
				<updated>2015-08-18T09:17:46Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment. See the [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells-Copper.htm Corrosion Doctors] website for a recipe.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4145</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4145"/>
				<updated>2015-08-18T09:14:19Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example:&lt;br /&gt;
&lt;br /&gt;
:• [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
:• [http://www.mcmiller.com MC Miller]&lt;br /&gt;
:• [http://www.matcor.com/cathodic-protection-reference-electrodes/ Matcor]&lt;br /&gt;
&lt;br /&gt;
If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4144</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4144"/>
				<updated>2015-08-18T08:33:06Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example see reference 1. If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4143</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4143"/>
				<updated>2015-08-18T08:32:50Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example see reference 1. If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
.&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4142</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4142"/>
				<updated>2015-08-18T08:32:32Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example see reference 1. If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4141</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4141"/>
				<updated>2015-08-18T08:31:25Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent of acid concentration. However basic samples should be avoided as hydroxide leaching into the electrolyte compartment will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrodes are available, for example see reference 1. If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 V with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4140</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4140"/>
				<updated>2015-08-18T08:28:48Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO4) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The saturated [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Cu&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is independent on acid concentration but basic samples should be avoided as hydroxide leaching into the electrode will cause formation of insoluble copper hydroxide and copper oxide.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
Many commercial electrode are available, for example see reference 1. If you are attempting to make your own electrode then you need to saturate the solution with copper sulfate and have excess crystalline material in the electrolyte compartment.&lt;br /&gt;
&lt;br /&gt;
The potential of the Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode is +0.314 volt with respect to the standard hydrogen electrode (SHE).&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. [http://tinker-rasor.com/products/reference-electrodes/cu/ Tinker &amp;amp; Rasor]&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4139</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4139"/>
				<updated>2015-08-18T08:13:01Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* The Copper/Copper Sulfate (Cu/CuSO44) Electrode */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode=&lt;br /&gt;
&lt;br /&gt;
The [https://en.wikipedia.org/wiki/Copper–copper(II)_sulfate_electrode (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) electrode] is often used as a reference in the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4138</id>
		<title>Reference Electrode Potentials</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Reference_Electrode_Potentials&amp;diff=4138"/>
				<updated>2015-08-18T08:11:19Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: &lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;The inspiration and source for much of the information on this page was the web site [http://www.consultrsr.net  Research Solutions and Sources] created by the late Dr Bob Rodgers.&lt;br /&gt;
&lt;br /&gt;
Do you need to convert potentials obtained with one reference electrode to the equivalent values versus another reference electrode? Then try this [http://www.consultrsr.net/resources/ref/refpotls3.htm calculator]&lt;br /&gt;
&lt;br /&gt;
Two of the important general texts for reference electrodes are:&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). Available at [http://www.amazon.com/ Amazon]&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
&lt;br /&gt;
= The Hydrogen (H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;/H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is based on the half cell equation  2H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As can be seen from this equation, the reaction is affected by the pH (hydrogen ion concentration) of the system, and in fact a hydrogen electrode can also be used an a pH electrode!&lt;br /&gt;
&lt;br /&gt;
Hydrogen electrodes are usually more fully described as the:&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:1. [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode Standard Hydrogen Electrode (SHE)], which is the basis against which other [http://en.wikipedia.org/wiki/Standard_electrode_potential_(data_page) reduction/oxidation (redox) couples] are reported. These days, the SHE is more of a theoretical ideal electrode. In days gone by, the electrode was known as the [http://en.wikipedia.org/wiki/Normal_hydrogen_electrode Normal Hydrogen Electrode {NHE)] which used conditions of 1 atm pressure of H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;, 25 °C, and 1 N HCl. Corrections had to be made for barometric pressure and the partial pressure of water vapour in H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; gas for the most accurate work. The SHE concept took this a step further by redefining the electrode only in terms of H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; ions without any interaction with other ions present (such as Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;) and this means that it is not actually physically possible to construct a SHE!&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
:2. [http://en.wikipedia.org/wiki/Reversible_hydrogen_electrode Reversible Hydrogen Electrode (RHE)], which usually refers to a real physical electrode that may or may not be operating under 'standard conditions'.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://www.consultrsr.net/resources/ref/hydrogen.htm hydrogen electrode] is traditionally constructed by having a platinum plate or coiled wire in a vessel containing 1 N HCl. A tube through which hydrogen gas was being blown was arranged so that the gas was bubbled over the surface of the platinum. Adequate ventilation is required to avoid possible build up of hydrogen gas which is an explosion/fire hazard. These safety concerns mean that students can often pass through an entire chemistry course without ever having used, or even seen a real hydrogen electrode.&lt;br /&gt;
&lt;br /&gt;
A clever way of making a modern RHE is to use a small cartridge that contains substances that produce a slow release of hydrogen gas that can be passed through a diffusion membrane containing small particles of platinum catalyst. See the [http://www.edaq.com/ET070 Hydroflex™] electrode. This dispenses with the need to rent expensive hydrogen gas cylinders and overcomes the fire safety issues of using hydrogen gas.&lt;br /&gt;
&lt;br /&gt;
The potential provided by an RHE is given by the equation  &lt;br /&gt;
&lt;br /&gt;
: E  =  E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; – (RT/nF)ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]  &lt;br /&gt;
: E  =  –ln(10)(RT/nF)log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]     note that ln[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;] = ln(10) × log[H&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;]&lt;br /&gt;
: E  =  2.303(RT/nF)pH      note that ln(10) ≅ 2.303&lt;br /&gt;
: E  =  0.0591pH      at 25 °C and 1 atm, see Table 1.  Note that E  =  0.0615pH at 37 °C (body temperature, often used for biological experiments).&lt;br /&gt;
&lt;br /&gt;
where:&lt;br /&gt;
: E is the [http://en.wikipedia.org/wiki/Electrode_potential electrode potential] expressed in volts&lt;br /&gt;
: E&amp;lt;sub&amp;gt;0&amp;lt;/sub&amp;gt; is the standard [http://www.wikipedia.org/wiki/Reduction_potential reduction potential] (zero for the hydrogen electrode)&lt;br /&gt;
: R is the [http://en.wikipedia.org/wiki/Universal_gas_constant Gas Constant], 8.314 J/mol/K&lt;br /&gt;
: T is the temperature, K&lt;br /&gt;
: n is +1 for hydrogen ion&lt;br /&gt;
: F is the [http://www.wikipedia.org/wiki/Faraday_constant Faraday constant], 96485 C/mol&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:500px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Potential, E (versus SHE), of the reversible hydrogen electrode, RHE, at 25°C and 1 atm. E = 0.0591pH'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | pH&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E /V&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 0 || 0 || 8 || 0.473  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 1 || 0.059 || 9 || 0.532&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 2 || 0.118 || 10 || 0.591 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 3 || 0.177 || 11 || 0.650&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 4 || 0.236 || 12 || 0.709 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 5 || 0.296 || 13 || 0.768 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 6 || 0.355 || 14 || 0.827 &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | 7 || 0.414 || 15 || 0.887 &lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
If you are planning to use a RHE as a reference electrode directly in contact with your sample solution then they tend to work best under acidic (&amp;lt; pH 4) or basic conditions (&amp;gt; pH 10) where the sample is naturally buffered. If you are working at intermediate pH conditions then you will need to make sure that the sample has added pH buffer salts to ensure there is no appreciable change in pH during the experiment.&lt;br /&gt;
&lt;br /&gt;
Often a better idea is to use the RHE with a salt bridge, or other double junction arrangement, linking to the test solution.  Hydrogen around the RHE will be prevented from acting as a reductant in the test solution, and materials in the test solution will be prevented from contacting (and possibly poisoning) the platinum used in the RHE.  You can also match the pH and ionic content of the solution around the RHE to be the same as the test solution in order to eliminate junction potential.&lt;br /&gt;
&lt;br /&gt;
If you are using the RHE as a pH electrode then connect it to a pH meter using a Ag/AgCl,  calomel, or other external reference electrode. Unlike glass pH electrodes the RHE is not affected by strongly basic solutions and can also be used in hydrofluoric acid solutions. You can calibrate the RHE in the usual manner of using two standard solutions of known pH.&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Chloride (Ag/AgCl) Electrode =&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Silver_chloride_electrode Ag/AgCl electrode] is by far the most popular type of laboratory reference electrode in use today.&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). There are several ways to do this (see reference 7). The most popular method in industry is to dip a silver wire into molten silver chloride, while in the laboratory it is more common to electrodeposit AgCl onto a silver wire that is made the anode in an electrochemical cell containing dilute HCl (0.1 – 1.0 M) as the electrolyte solution. The chloridized end of the wire is then inserted into an electrolyte solution of KCl or NaCl. &lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
AgCl&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_chloride Silver chloride] is quite insoluble in water (~0.2 mg/100 mL), but is slightly more soluble in concentrated chloride solutions owing to the formation of the complex ion [AgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;. Though electrode potential is actually dependent on silver ion concentration (as with any metal/metal ion electrode), this is limited by the low solubility of AgCl, and thus the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration, and so is not directly pH dependent. However when used with samples of high pH, hydroxide ion can contaminate the electrode causing the formation of AgOH and brown/black Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O in place of the white/grey AgCl coating and noticeable potential drift will occur. Thus long term use with alkaline samples is normally avoided.&lt;br /&gt;
&lt;br /&gt;
Ag/AgCl electrodes can be used up to 100°C (depending on the materials used to make the electrode), and are commercially available from many companies. The potential does vary with temperature, but between 10 – 40°C, can be estimated by the equations (see reference 2):&lt;br /&gt;
&lt;br /&gt;
:E = 205 – 0.73 × (T – 25)     for an electrolyte of 3.5 M KCl&lt;br /&gt;
:E = 199 – 1.01 × (T – 25)     for an electrolyte of saturated KCl&lt;br /&gt;
&lt;br /&gt;
where T is the temperature (°C), and E is the electrode potential (mV).&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Potential, E (in volts), of the Ag/AgCl Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.2881 || 0.047 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3 M) || 0.210 || -0.032 || - || 4&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5 M) || 0.205 || -0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.197 || -0.045 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.199 || -0.045 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (sat'd) || 0.1988 || -0.042 || - || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (3 M) || 0.209 || -0.035 || Yes || 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaCl (sat'd) || 0.197 || -0.047 || Yes || 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://en.wikipedia.org/wiki/Seawater Seawater] (~0.47 M NaCl) || 0.25 || 0.01 || Yes || 6&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
:NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
:SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963). ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. [http://www.dx.doi.org/10.1016/S0013-4686(98)99006-5 DOI: 10.1016/S0013-4686(98)99006-5]&lt;br /&gt;
&lt;br /&gt;
:5. [http://www.bioanalytical.com/products/ec/faqele.html#Ref_Type www.bioanalytical.com/products/ec/faqele.html#Ref_Type]&lt;br /&gt;
&lt;br /&gt;
:6. [http://www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm www.corrosion-doctors.org/Corrosion-Thermodynamics/Reference-Half-Cells.htm]&lt;br /&gt;
&lt;br /&gt;
:7. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961). See pages 203 – 213.&lt;br /&gt;
&lt;br /&gt;
:8. Standard Potential of the Silver-Silver Chloride Electrode. R G  Bates and J B  MacAskill, Pure &amp;amp; Applied Chemistry, 50, 1701—1706, 1978. [http://www.iupac.org/publications/pac/1978/pdf/5011x1701.pdf IUPAC]&lt;br /&gt;
&lt;br /&gt;
:9. An inexpensive, commercial-type, reference electrode. T H Randle and P J Kelly, Journal of Chemical Education, 61, 721, 1984. [http://dx.doi.org/10.1021/ed061p721 DOI: 10.1021/ed061p721]&lt;br /&gt;
&lt;br /&gt;
:10. Easy-to-Make Ag/AgCl Reference Electrode. Gaston A. East , M. A. del Valle, Journal of Chemical Education, 77, 97, 2000. [http://dx.doi.org/10.1021/ed077p97 DOI: 10.1021/ed077p97]&lt;br /&gt;
&lt;br /&gt;
= The Silver/Silver Sulfate (Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
The Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is enjoying increasing popularity as a replacement for the Hg/HgSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode, and where a mercury– and chloride–free electrode is required. It is especially useful in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
It is constructed from a silver wire, part of which is covered with finely divided silver sulfate, usually prepared electrochemically using the silver wire as an anode in a sulfuric acid electrolyte solution, see reference 7. If making your own electrode be careful to exclude even trace amounts of halide in the starting reagents as silver halide salts around the silver wire will affect the reference potential.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:  Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Ag&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Silver_sulfate Silver sulfate] is sparingly soluble in water (~0.83 g/100 mL). Thus the electrolyte must be high in sulfate ion concentration to ensure that it is saturated in silver ion.&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 3. Potential, E (in volts), of the Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.72 || 0.48 || - || 1, 3, 5  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.71 || 0.47 || Yes || 4, 5&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.68 || 0.44 || - || 2, 5&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
: See [http://www.consultrsr.net/resources/ref/ag2so4.htm  more information] about how these numbers were calculated.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Reference 7 suggests that the electrolyte filling solution should have sulfate concentrations higher than 0.01 M and silver ion concentrations between 0.001 – 1 mM, for best performance.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000).  ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Table 5.3&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Electrochemical Deposition of Co under the Influence of High Magnetic Fields, M. Uhlemann, A. Krause, J. P. Chopart, and A. Gebert, Journal of the  Electrochemical Society, 152, C817-C826, 2005. [http://dx.doi.org DOI: 10.1149/1.2073167]&lt;br /&gt;
&lt;br /&gt;
:5. Calculated by adding 40 mV to the corresponding mercury-mercurous sulfate electrode, see the section on these electrodes, below.&lt;br /&gt;
&lt;br /&gt;
:7. On the stability of the silver/silver sulfate reference electrode, Matěj Velický, Kin Y. Tamb, and Robert A. W. Dryfe, Analytical Methods, 4, 1207-1211, 2012.&lt;br /&gt;
[http://dx.doi.org//10.1039/C2AY00011C DOI: 10.1039/C2AY00011C]&lt;br /&gt;
&lt;br /&gt;
:8. Silver–silver sulfate reference electrodes for lead-acid batteries, Paul Ruetschi, Journal of Power Sources, 113, 363–370, 2003. [http://dx.doi.org/10.1016/S0378-7753(02)00549-9 DOI: 10.1016/S0378-7753(02)00549-9]&lt;br /&gt;
&lt;br /&gt;
= The Calomel (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The [http://en.wikipedia.org/wiki/Saturated_calomel_electrode calomel electrode] (more accurately described as the 'mercury/calomel electrode') is usually constructed from a platinum wire inserted into a mixture of [http://en.wikipedia.org/wiki/Mercury%28I%29_chloride calomel] (mercurous chloride, Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;) and liquid mercury, with an electrolyte solution of KCl or NaCl. &lt;br /&gt;
Calomel is insoluble in water (~0.4 mg/100 mL) to about the same extent as silver chloride, see reference 5.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub &amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2Cl&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration. &lt;br /&gt;
&lt;br /&gt;
Calomel electrodes are unstable much above 50°C owing to the [http://en.wikipedia.org/wiki/Disproportionation disproportionation] reaction: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;Cl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + HgCl&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;&lt;br /&gt;
&lt;br /&gt;
Commercial calomel electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
: [http://www.ionode.com Ionode Pty Ltd] (Australia)&lt;br /&gt;
&lt;br /&gt;
and some other companies that make pH electrodes (though many such companies have stopped production because of falling demand). In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.&lt;br /&gt;
  	&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 4. Potential, E (in volts), of the Calomel Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.3337 || 0.0925 || - || 1, 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (0.1 M) || 0.336 || 0.092 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.2801 || 0.0389 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NCE, KCl (1 M) || 0.283 || 0.039 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KCl (3.5M) || 0.250 || 0.006 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.2412 || 0 || - || 1, 3&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SCE, KCl (sat'd) || 0.244 || 0 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | SSCE, NaCl (sat'd) || 0.2360 || -0.0052 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NCE, normal calomel electrode&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode] &lt;br /&gt;
: SSCE, saturated salt calomel electrode&lt;br /&gt;
: For values at other temperatures use this [http://www.consultrsr.net/resources/ref/calomelpotl.htm calculator].&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. &amp;quot;Electrochemistry for Chemists, Second Edition&amp;quot;, D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley &amp;amp; Sons, NY (1995). ISBN 0471594687. See Section 5.2.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:4. Standard E.m.f. of the hydrogen-calomel cell from 0 to 45°C. S R Gupta,   G J Hills and  D J G Ives. Transactions of the Faraday Society, 59, 1874-1885, 1963. [http://dx.doi.org/10.1039/TF9635901874 DOI: 10.1039/TF9635901874]&lt;br /&gt;
&lt;br /&gt;
:5. Compilation and Evaluation of Solubility Data in the Mercury(I) Chloride–Water System. Y Marcus, Journal of Physical Chemistry Reference Data, 9, 1307–1329, 1980. [http://www.nist.gov/data/PDFfiles/jpcrd173.pdf www.nist.gov/data/PDFfiles/jpcrd173.pdf]&lt;br /&gt;
&lt;br /&gt;
:6. A versatile compact reference electrode. Kousuke Kusuda, J.]ournal of Chemical Education, 66, 531, 1989. [http://dx.doi.org/10.1021/ed066p531 DOI: 10.1021/ed066p531]&lt;br /&gt;
&lt;br /&gt;
= The Mercury/Mercurous Sulfate (Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;) Electrode =&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; electrode is used where a chloride free electrode is required. It is especially used in experiments to do with lead–acid batteries (reference 8).&lt;br /&gt;
&lt;br /&gt;
The electrode is usually constructed from a platinum wire inserted into a mixture of Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; and liquid mercury, with an electrolyte solution of K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; or H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt;  + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt; 2Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;2–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(I)_sulfate Mercurous sulfate] is slightly soluble in water (51 mg/100 mL).&lt;br /&gt;
&lt;br /&gt;
Commercial electrodes are available from:&lt;br /&gt;
&lt;br /&gt;
: [http://www.koslow.com Koslow Scientific] (USA)&lt;br /&gt;
: [http://www.als-japan.com/1390.html ALS Co. Ltd] (Japan)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 5. Potential, E (in volts), of the Hg/Hg&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.68 || 0.44 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (0.5 M) || 0.682 || 0.441 || - || 3  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (1.0 M)  || 0.674 || 0.430 || Yes || 2&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.64 || 0.40 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | K&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt; (sat'd)  || 0.65 || 0.41 || - || 3&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Electrochemical Methods: Fundamentals and Applications&amp;quot;, A J Bard and L R Faulkner, John Wiley &amp;amp; Sons, NY (2000). ISBN 0471405213. See the table on inside back cover.&lt;br /&gt;
&lt;br /&gt;
:2. M Uhlemann, A Krause, JP Chopart, A Gebert, J. Electrochem. Soc., 152 (2005), C817-C826.&lt;br /&gt;
&lt;br /&gt;
:3. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
=The Mercury/Mercury Oxide (Hg/HgO) Electrode=&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''WARNING.''' Mercury and its salts are highly toxic. Only suitably qualified persons should attempt to make mercury containing electrodes.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=The Copper/Copper Sulfate (Cu/CuSO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;4) Electrode=&lt;br /&gt;
&lt;br /&gt;
This electrode is often used as a reference the field for commercial applications of cathodic protection.&lt;br /&gt;
&lt;br /&gt;
Many conventional reference electrodes (Ag/AgCl, Ag/Ag&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, calomel) will have limited life times in very alkaline solutions. This is caused by hydroxide diffusing into the electrode filling solution, and forming silver hydroxy/oxide species on the silver wire (which becomes brown/blackened) and which then causes a shift in the electrode potential. This can be ameliorated, to some extent, by the use of a double junction to slow the hydroxide diffusion, but an electrode that is stable under alkaline conditions is often a better answer.&lt;br /&gt;
&lt;br /&gt;
The Hg/HgO electrode is ideal for use in alkaline solutions. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is:&lt;br /&gt;
HgO&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(s)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2e&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;  + H&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O  &amp;lt;math&amp;gt;\rightarrow&amp;lt;/math&amp;gt;  Hg&amp;lt;sub&amp;gt;&amp;lt;i&amp;gt;(liq)&amp;lt;/i&amp;gt;&amp;lt;/sub&amp;gt; + 2OH&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
&lt;br /&gt;
As the half cell equation suggests the potential is dependent on the hydroxide ion concentration used in the electrolyte solution. It is usual to match the hydroxide concentration of the filling solution to that of the sample to minimise the junction potential.&lt;br /&gt;
&lt;br /&gt;
[http://en.wikipedia.org/wiki/Mercury(II)_oxide Mercuric oxide] is sparingly soluble in water (~5.3 mg/100 mL), and alkaline solutions. &lt;br /&gt;
&lt;br /&gt;
A commercial electrode is available (see reference 2). If you are attempting to make your own electrode then you should be aware of the information in reference 3. A simple procedure for making an electrode is given in reference 4, although you may want to try substituting carbon fiber for the toxic asbestos fibre.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;2&amp;quot; style=&amp;quot;width:600px; height:100px;&amp;quot;&lt;br /&gt;
|+ '''Table 6. Potential, E (in volts), of the Hg/HgO Electrode at 25°C'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Electrolyte Solution&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs NHE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | E vs SCE&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | LJ&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Reference&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (0.1 M) || 0.165 || -0.076 || - || 1  &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | NaOH (1 M) || 0.140 || -0.101 || - || 1&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | KOH (20%) || 0.098 || - || ? || 2&lt;br /&gt;
|-&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
'''Notes'''&lt;br /&gt;
: LJ, [http://en.wikipedia.org/wiki/Liquid_junction_potential liquid junction]. Value obtained using a cell which included a liquid junction potential.&lt;br /&gt;
: NHE, [http://en.wikipedia.org/wiki/Standard_hydrogen_electrode normal hydrogen electrode]&lt;br /&gt;
: SCE, [http://en.wikipedia.org/wiki/Saturated_calomel_electrode saturated calomel electrode]&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
&lt;br /&gt;
:1. &amp;quot;Handbook of Analytical Chemistry&amp;quot;, L Meites (ed.), McGraw Hill, NY (1963).  ISBN 0070413363. See Section 5.&lt;br /&gt;
&lt;br /&gt;
:2. [http://www.koslow.com/reference_electrodes/5088/ Koslow Scientific Testing Instruments]&lt;br /&gt;
&lt;br /&gt;
:3. [http://www.consultrsr.net/resources/ref/hgopotl.htm  Research Solution and Sources].&lt;br /&gt;
&lt;br /&gt;
:4.  A simple procedure for making Hg\HgO reference electrodes. Raymond Thacker, Journal of Chemical Education, 45, 180, 1968. [http://dx.doi.org/10.1021/ed045p180 DOI: 10.1021/ed045p180]&lt;br /&gt;
&lt;br /&gt;
:5. Behaviour of the mercury, mercuric oxide electrode in alkaline solutions in the temperature range 298–363 K. H Corti, R Fernández-Prini,  Journal of the Chemical Society, Faraday Transactions 1, 78, 545-554, 1982. [http://dx.doi.org/10.1039/F19827800545 DOI: 10.1039/F19827800545]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=Other Reference Electrodes=&lt;br /&gt;
&lt;br /&gt;
It is possible to construct many other types of reference electrodes, many of which are used to cope with special conditions peculiar to the experiment being undertaken, for example see references 1 - 3. For teaching, a Cu&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;/Cu&amp;lt;sup&amp;gt;2+&amp;lt;/sup&amp;gt; has being described, reference 4, while for alkaline conditions an electrode using manganese dioxide has been proposed, reference 5. &lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. &amp;quot;Handbook of Reference Electrodes&amp;quot;. György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. DOI:10.1007/978-3-642-36188-3&lt;br /&gt;
:3. Preparation and characterization of palladium-hydride-coated titanium as a reference electrode for the supercritical carbon dioxide emulsion electrochemical system. Yung-Yi Wua, Chun-Tsung Hsua, Tso-Fu Mark Changb, Masato Soneb, Chi-Chang Hu, Electrochimica Acta 155, 209–216, 2015.  [http://dx.doi.org/10.1016/j.electacta.2014.12.141 DOI: 10.1016/j.electacta.2014.12.141]&lt;br /&gt;
:4. Low-Cost Reference Electrode for Potentiotitrimetry. P. Riyazuddin, Journal of Chemical Education, 71, 167, 1994. [http://dx.doi.org/10.1021/ed071p167 DOI: 10.1021/ed071p167]&lt;br /&gt;
:5. Assembly of a Robust and Economical MnO2-Based Reference Electrode. Robert C. Massé and James B. Gerken, Journal of Chemical Education, 92, 110–115, 2015 [http://dx.doi.org/10.1021/ed500587a DOI: 10.1021/ed500587a]&lt;br /&gt;
&lt;br /&gt;
=The Salt Bridge=&lt;br /&gt;
&lt;br /&gt;
These reference electrodes, above, all need a [http://en.wikipedia.org/wiki/Salt_bridge salt bridge] which is a junction or portal that connects the internal electrolyte solution of the electrode to the external sample solution. To limit the diffusion of ions across the junction (which would contaminate both the internal and external solution with foreign ions) some semipermeable material is usually inserted into the portal. This is often a plug of mineral fibers (asbestos was often used in the past until its toxicity was discovered), or porous ceramic, glass, or plastic.  Obviously this plug is selected to be as chemically inert as possible. In some cases the junction is left completely open (just a pinhole opening is used) or the electrode is constructed so that a sleeve of electrolyte solution is constructed between two close fitting pieces of glass. If the plug is too impermeable then it increases the electrical resistance between the reference electrode and the sample, and if too permeable it allows too much exchange of the ionic materials. There is always a trade off between these two extremes. Electrode manufacturers will have optimised permeability for what they perceive to be applications for which the electrode is designed but occasionally their choice of material may became a source of problems, for example see reference 2. Similarly, if you want to make your own reference electrode then do not neglect to consider the choice of material for the junction.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. &amp;quot;Reference Electrodes. Theory and Practice&amp;quot; David J G Ives, and George J Janz, (eds) Academic Press (1961).&lt;br /&gt;
:2. Reference Electrodes with Salt Bridges Contained in Nanoporous Glass: An Underappreciated Source of Error. Maral P. S. Mousavi and Philippe Bühlmann, Analytical Chemistry, 85, 8895−8901, 2013. [http://dx.doi.org/10.1021/ac402170u DOI: 10.1021/ac402170u]&lt;br /&gt;
&lt;br /&gt;
=Organic solvents=&lt;br /&gt;
&lt;br /&gt;
If your experiments require the use of an organic solvent the use of classical aqueous reference electrode may be impracticable. &lt;br /&gt;
&lt;br /&gt;
Cyclic voltammetry of organics, organometallics, or of complex ions, often requires the use of organic solvents such as dichloromethane, acetonitrile, tetrahydrofuran, propylene carbonate, or dimethylsulfoxide. In these cases the International Union of Pure and Applied Chemistry (IUPAC) recommends the use of the ferrocenium ion/ferrocene or bis(biphenyl)chromium(I)/bis(biphenyl)chromium(0) couple, reference 1. However a wider range of materials are considered in reference 2.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion (Fc/Fc&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;) couple has also been studied as to providing an estimate for the uncompensated resistance encountered when doing cyclic voltammetry in organic solvents, reference 3.&lt;br /&gt;
&lt;br /&gt;
'''References'''&lt;br /&gt;
:1. Recommendations on reporting electrode potentials in nonaqueous solvents. G Gritzner, J Kuta, Pure and Applied Chemistry 56, 461-466, 1984. [http://dx.doi.org/10.1351/pac198456040461 DOI 10.1351/pac198456040461]&lt;br /&gt;
:2. Reference Redox Systems in Nonaqueous Systems and the Relation of Electrode Potentials in Nonaqueous and Mixed Solvents to Standard Potentials in Water. Gerhard Gritzner, [http://www.springer.com/978-3-642-36187-6, Chapter 2] in &amp;quot;Handbook of Reference Electrodes&amp;quot;.  György Inzelt, Andrzej Lewenstam, and Fritz Scholz (eds). Springer-Verlag (2013). ISBN 3642361870. [http://dx.doi.org/10.1007/978-3-642-36188-3 DOI:10.1007/978-3-642-36188-3]&lt;br /&gt;
:3. Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
=Disclaimer=&lt;br /&gt;
Any products mentioned on this page are for informational purposes only and constitute neither an endorsement nor a recommendation.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4067</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4067"/>
				<updated>2015-08-10T08:20:57Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
Manuals for capacitively coupled contactless conductivity detection (C4D) and related equipment can be found here. Also see sections on PowerChrom and e-corder systems for signal recording.&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
: Potentiostats manual for:&lt;br /&gt;
:::• EA163 Potentiostat&lt;br /&gt;
:::• EA164 QuadStat&lt;br /&gt;
:::• EA362 Dual Picostat&lt;br /&gt;
:: [[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
: ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
: EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
: ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: [http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4066</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4066"/>
				<updated>2015-08-10T08:20:23Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
Manuals for capacitively coupled contactless conductivity detection (C4D) and related equipment can be found here. Also see sections on PowerChrom and e-corder systems for signal recording.&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
: Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
: [[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
: ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
: EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
: ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: [http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4065</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4065"/>
				<updated>2015-08-10T08:19:45Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Contactless Conductivity */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
Manuals for capacitively coupled contactless conductivity detection (C4D) and related equipment can be found here. Also see sections on PowerChrom and e-corder systems for signal recording.&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
: [[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
: ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: [http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4064</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4064"/>
				<updated>2015-08-10T08:16:20Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
: [[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
: ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: [http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4063</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4063"/>
				<updated>2015-08-10T08:16:02Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* isoPods */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
: ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
: [[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
: ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: [http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4062</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4062"/>
				<updated>2015-08-10T08:15:25Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
: ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
: [[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
: EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4061</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4061"/>
				<updated>2015-08-10T08:14:38Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4060</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4060"/>
				<updated>2015-08-10T08:14:05Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator: [[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor: [[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4059</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4059"/>
				<updated>2015-08-10T08:12:44Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[Media:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4058</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4058"/>
				<updated>2015-08-10T08:12:25Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[[Media:EA167 Manual 0414.pdf]]xxxxxxx] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4057</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4057"/>
				<updated>2015-08-10T08:11:58Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[Media:EA167 Manual 0414.pdf]xxxxxx] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4056</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4056"/>
				<updated>2015-08-10T08:11:33Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[Media:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[Media:EA167 Manual 0414.pdf xxxxxx]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4055</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4055"/>
				<updated>2015-08-10T08:10:00Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[File:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[Media:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[File:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4054</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4054"/>
				<updated>2015-08-10T08:08:58Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[File:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[File:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[File:EA167 Manual 0414.pdf]] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4053</id>
		<title>Manuals</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Manuals&amp;diff=4053"/>
				<updated>2015-08-10T08:08:10Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Potentiostats and related equipment */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;'''NOTE:''' This page is under construction and is not yet complete!&lt;br /&gt;
Manuals can also be found at [http://www.edaq.com/edaq-product-manuals www.edaq.com/edaq-product-manuals]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
eDAQ User Manuals can be found here.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
== e-corder units ==&lt;br /&gt;
&lt;br /&gt;
== Chromatography ==&lt;br /&gt;
&lt;br /&gt;
== Contactless Conductivity ==&lt;br /&gt;
&lt;br /&gt;
== Potentiostats and related equipment ==&lt;br /&gt;
&lt;br /&gt;
ER466 Potentiostat&lt;br /&gt;
&lt;br /&gt;
Potentiostats manual for:&lt;br /&gt;
::• EA163 Potentiostat&lt;br /&gt;
::• EA164 QuadStat&lt;br /&gt;
::• EA362 Dual Picostat&lt;br /&gt;
[[File:Potentiostats.pdf]] ‎(file size: 2.55 MB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
ER175 Waveform Generator &lt;br /&gt;
&lt;br /&gt;
[[File:ER175 Waveform Generator.pdf]] (file size: 389 KB)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
EA167 Dual Reference Adaptor&lt;br /&gt;
&lt;br /&gt;
[[File:EA167 Manual 0414.pdf]] EA167 Dual Reference Adaptor] (file size: 557 KB)&lt;br /&gt;
&lt;br /&gt;
== isoPods ==&lt;br /&gt;
&lt;br /&gt;
ER454 Quad MF isoPod with USB&lt;br /&gt;
&lt;br /&gt;
[http://wiki.edaq.com/index.php/EPU452_Manual EPU452 Manual]&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=Cyclic_Voltammetry:_Hints_and_Tips&amp;diff=4041</id>
		<title>Cyclic Voltammetry: Hints and Tips</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=Cyclic_Voltammetry:_Hints_and_Tips&amp;diff=4041"/>
				<updated>2015-08-10T07:17:04Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Tetraethylammonium perchlorate, [(CH3CH2)4N]ClO4, Mr = 229.7 */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;{{#ev:youtube|mbeCoCaTd-Q|300|right|Video 1. How to Setup the EChem Software for Cyclic Voltammetry}}&lt;br /&gt;
== Safety ==&lt;br /&gt;
Purification and distillation of solvents should only be undertaken by an experienced chemist or laboratory technician. Incorrect procedures could lead to explosion or fire.&lt;br /&gt;
&lt;br /&gt;
*All organic solvents, to a lesser or greater degree, are toxic, and most are flammable. General safety procedures include working in a well-ventilated area (a fume hood is usually necessary), with protective clothing including rubber gloves and safety glasses. Adequate ventilation must be ensured about the distillation apparatus to prevent the buildup of flammable and toxic solvent vapours.&lt;br /&gt;
&lt;br /&gt;
*Even if the solvent is relatively harmless, most organic solvents can penetrate the skin easily carrying potentially toxic solutes with them. Similarly most electrolytes used with organic solvents are toxic and/or skin irritants. Always familiarize yourself with the potential hazards by reading the MSDS (Materials Safety Data Sheets) available from the suppliers of solvents and electrolytes. Always assume that new compounds (for which no safety data may be available) are toxic and handle them with due care.&lt;br /&gt;
&lt;br /&gt;
*Only use the drying agent indicated for that particular solvent. Do NOT mix drying agents.&lt;br /&gt;
&lt;br /&gt;
*Solvents may be grossly wet and require pre-drying with a mild reagent (eg anhydrous sodium sulfate) before drying with highly reactive drying agents such as sodium wire or phosphorous pentoxide.&lt;br /&gt;
&lt;br /&gt;
*Appropriate care should be exercised in the handling and disposal of reactive agents such as metal hydrides, phosphorous pentoxide, and sodium wire&lt;br /&gt;
&lt;br /&gt;
*The constituent ions (both cations and anions) of electrolytes may be toxic and when dissolved in organic solvents they can be carried across the skin. In cases of accidental spillage, where a specific treatment is unknown, contaminated skin areas should be continuously flushed with water for at least several minutes.&lt;br /&gt;
&lt;br /&gt;
Also be aware of the capabilities of your potentiostat. Some potentiostats have large current and/or voltage capability and are capable of causing electrical shock. Always operate the potentiostat in accordance with the manufacturer's instructions.&lt;br /&gt;
&lt;br /&gt;
== Solvents ==&lt;br /&gt;
A suitable solvent must be chosen that meets several criteria. Obviously the analyte molecule of interest must have sufficient solubility (usually more than 0.1 mM) to provide an adequate current signal. Also the solvent should not react with the analyte or its electrolysis products. It must also provide a potential window (the range between the cathodic to anodic potentials at which the solvent itself electrolyses) wide enough to see the redox processes of the analyte.&lt;br /&gt;
&lt;br /&gt;
Unfortunately most organic solvents are poor electrical conductors and need relatively high concentrations (typically 0.1 M) of an inert electrolyte added to facilitate the cyclic voltammetry experiment. In general the less polar the solvent, the fewer electrolytes there are that will dissolve to large enough concentrations.&lt;br /&gt;
&lt;br /&gt;
==== Water ====&lt;br /&gt;
Water is obviously a low toxicity, non-flammable solvent capable of dissolving many ionic and polar compounds. It also has the advantage of being a moderately good electrical conductor especially when used with an inert electrolyte added (often 0.1 mol/L KCl). If the analyte has acidic or basic functional groups then pH control of the solution is essential if repeatable results are to be obtained. Its main disadvantage, however, is the vast number of organic compounds that insoluble in it, and which must therefore be studied using an organic solvent.&lt;br /&gt;
&lt;br /&gt;
====Organic Solvents ====&lt;br /&gt;
While it is almost always possible to find a solvent for any given organic compound one must also be aware that the solvent must be relatively inert under the oxidizing and reducing conditions to be used in a cyclic voltammetry experiment. It must be possible to purify the solvent to a high degree, as even a small percentage of an electroactive impurity would produce peaks in a cyclic voltammogram larger than those of the analyte (which is typically present in a concentration of between 0.1 and 1 mM). &lt;br /&gt;
&lt;br /&gt;
For guidelines on the purification of many solvents see “Purification of Laboratory Chemicals”, 4th edition, W. L. F. Armarego and D. D. Perrin, Butterworth-Heinemann, 1997, ISBN 0750637617.&lt;br /&gt;
&lt;br /&gt;
Often anhydrous organic solvents are required because water sensitive compounds are being employed, or because the solvent itself may react with water at an electrode, or because water causes a reduction of the potential window of the system (the difference between the maximum anodic and cathodic potentials that can be applied).&lt;br /&gt;
&lt;br /&gt;
Solvents should be of at least AR (analytical reagent) grade otherwise they may be grossly wet, or otherwise need a preliminary purification. Further drying and purification is then usually necessary before the solvent can be used for cyclic voltammetry or other electroanalytical techniques.&lt;br /&gt;
&lt;br /&gt;
Distillation of solvents should always take place using a short fractionating column filled with glass rings to prevent an aerosol of the boiling solvent being carried through the condenser. A dedicated still for each solvent is ideal.&lt;br /&gt;
&lt;br /&gt;
Ethers (including tetrahydrofuran, diethyl ether, 1,4-dioxan, and 1,2-dimethoxyethane), as well as aromatic hydrocarbons (benzene, toluene, xylenes) can be first dried over sodium wire then distilled from freshly drawn sodium wire with a little [http://wikipedia.org/wiki/Benzophenone benzophenone] added to the distillation pot. A dark blue or purple color should develop and persist during reflux, for at least 10 minutes, which signals the presence of sodium benzophenone [http://wikipedia.org/wiki/Ketyl ketyl] (a radical anion). The ketyl can only exist in the absence of water and oxygen. The anhydrous solvent can then be distilled. Excess sodium wire is destroyed by allowing the distillation pot to cool and cautiously adding absolute ethanol.&lt;br /&gt;
&lt;br /&gt;
Dichloromethane, 1,2-dichloroethane, cyclohexane, or hexane, can be dried by distillation from either  [http://wikipedia.org/wiki/Phosphorus_pentoxide phosphorus pentoxide], P&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;, or from [http://wikipedia.org/wiki/Calcium_hydride calcium hydride], CaH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;.&lt;br /&gt;
&lt;br /&gt;
Dimethyl sulfoxide or dimethylformamide should be predried using a [http://wikipedia.org/wiki/Molecular_sieve molecular sieve] with a pore size less than 4 Å, followed by distillation at reduced pressure (10 – 20 mmHg).&lt;br /&gt;
&lt;br /&gt;
Pre-dry acetonitrile with a molecular sieve, pore size less than 4 Å. Distil after reflux with a small amount of P&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;, (about 0.5% w/v) to remove the residual water. Avoid using too much P&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;O&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt; to prevent excessive formation of an orange polymeric material.&lt;br /&gt;
&lt;br /&gt;
==== Supercritical Fluids ====&lt;br /&gt;
[http://wikipedia.org/wiki/Supercritical_fluid Supercritical fluids] have been used as solvents for cyclic voltammetry. For an example see ‘Electrochemical investigations in liquid and supercritical 1,1,1,2-tetrafluoroethane (HFC 134a) and difluoromethane (HFC 32)’, Andrew P. Abbott, Christopher A. Eardley, John C. Harper, and Eric G. Hope, Journal of Electroanalytical Chemistry, 457, 1–4, 1998. In particular HFC 134a, with tetra-n-butyl ammonium tetrafluoroborate as electrolyte, was shown to be have an extraordinarily wide redox stability window of 9 V.&lt;br /&gt;
&lt;br /&gt;
==== Liquid Electrolytes ====&lt;br /&gt;
The use of electrolytes that are liquid at ambient temperatures, often referred to as [http://wikipedia.org/wiki/Ionic_liquid ionic liquids], has become more common in recent years, especially for use in battery technology. These materials can also be used as solvents for cyclic and other voltammetric techniques.&lt;br /&gt;
&lt;br /&gt;
==== Inorganic Liquids ====&lt;br /&gt;
Cyclic voltammetry can also be performed in liquid ammonia, sulfur dioxide, hydrogen fluoride, etc, although obviously special reaction vessels must be constructed to withstand the high pressure and corrosive conditions employed.&lt;br /&gt;
&lt;br /&gt;
== Electrolytes ==&lt;br /&gt;
Some empirical rules for solubility of electrolytes in organic solvents are:&lt;br /&gt;
* chlorides, nitrates, tosylates and perchlorates (care! explosion hazard), are usually most soluble in alcohols;&lt;br /&gt;
* perchlorate, in the presence of potassium (or rubidium or cesium) ions, will give a precipitate of the metal perchlorate salt;&lt;br /&gt;
* electrolytes comprising large cations and anions will be relatively more soluble in non-polar solvents and less soluble in polar solvents;&lt;br /&gt;
* dimethylsulfoxide is often a good solvent for most electrolytes;&lt;br /&gt;
* fluoroborate and hexafluorophosphate salts exhibit particularly good solubility in acetone and acetonitrile;&lt;br /&gt;
* dichloromethane and similar solvents usually require tetra-n-butylammonium hexafluorophosphate, or other large anion/cation salt as an electrolyte;&lt;br /&gt;
* electrochemistry in toluene an be performed using liquid tetrabutylammonium tetrafluoroborate toluene solvate. See ''A simple hydrocarbon electrolyte: completing the electron-transfer series [Fe4S4(SPh)4]&amp;lt;sup&amp;gt;1–/2–/3–/4–&amp;lt;/sup&amp;gt;'', C. J. Pickett , Journal of the Chemical Society, Chemical Communications, 323-326, 1985. [http://dx.doi.org/10.1039/C39850000323 DOI: 10.1039/C39850000323].&lt;br /&gt;
&lt;br /&gt;
===== Use of Large Ions as Electrolytes =====&lt;br /&gt;
In general, larger cations and anions (with lower charge densities) produce salts that are more soluble in organic solvents, and so it is nearly always possible to find an electrolyte that will be suitable for a specific solvent. Common electrolytes are commercially available, but others will need to be prepared by the user. Purity of both commercial and home made electrolytes should be checked by performing a ‘blank’ voltammetric run at the same sensitivity setting of the potentiostat that is used when the analyte is present. Remember that ‘purity’ is a relative term — electrolyte and solvent that have been used satisfactorily with high concentrations of analyte at low potentiostat sensitivity settings, may prove to be hopelessly contaminated when used with much lower analyte concentrations at very high potentiostat sensitivity settings.&lt;br /&gt;
&lt;br /&gt;
===== Cations =====&lt;br /&gt;
Complex cations are typically subject to reduction at sufficiently large potential, oxidation is usually less of a problem. Remember that only a small proportion of the electrolyte needs to be electrolyzed to produce a signal that can interfere with the signal of the analyte.&lt;br /&gt;
Some large cations that can be employed are shown in Table 1. Tetraalkylammonium salts are the most commonly used for organic solvent work because of their relatively low cost and because they are fairly resistant to reduction.&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;1&amp;quot; style=&amp;quot;width:900px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 1. Complex cations'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Cation&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Formula&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt;&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Comments&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Tetramethylammonium tetramethylammonium] &lt;br /&gt;
| [N(CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt; || 74.15 ||   &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://wikipedia.org/wiki/Tetraethylammonium tetraethylammonium] &lt;br /&gt;
| [N(CH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 130.3&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  tetra-n-butylammonium	 &lt;br /&gt;
| [N(CH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 242.5&lt;br /&gt;
| PF&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; salt used in dichloromethane&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://wikipedia.org/wiki/Tetraphenylphosphonium_chloride tetraphenylphosphonium]&lt;br /&gt;
| [P(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 339.4&lt;br /&gt;
| Easily reduced. Hydrolyzed by hydroxide.&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://wikipedia.org/wiki/Bis(triphenylphosphine)iminium_chloride bis(triphenylphosphino)imminium] &lt;br /&gt;
| [(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;P=N=P(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 538.6&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | tetraphenylarsonium&lt;br /&gt;
| [As(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 383.3&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/18-Crown-6 (18-crown-6)potassium]&lt;br /&gt;
| [K(C&amp;lt;sub&amp;gt;12&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;24&amp;lt;/sub&amp;gt;O&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;)]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 303.4&lt;br /&gt;
| Can be prepared in situ from potassium salts.&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Dibenzo-18-crown-6 (dibenzo-18-crown-6)potassium]&lt;br /&gt;
| [K(C&amp;lt;sub&amp;gt;20&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;24&amp;lt;/sub&amp;gt;O&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;)]&amp;lt;sup&amp;gt;+&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 399.5&lt;br /&gt;
| Can be prepared in situ from potassium salts. Soluble in benzene, toluene etc.&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
===== Anions =====&lt;br /&gt;
Large anions may be subject to reduction or oxidation. Some anions that can be employed as shown in Table 2 below. Perchlorate salts are a known explosion hazard and should be avoided wherever possible. &lt;br /&gt;
&lt;br /&gt;
Note that while nitrate is often considered safe to use, it is still an oxidizing agent and should be handled with due caution. Its use as an electrolyte (at relatively high concentrations) in organic solvents is a potential explosion/fire hazard, especially if traces of acid are present, or if the solution is left to evaporate.&lt;br /&gt;
&lt;br /&gt;
{| border=&amp;quot;1&amp;quot; style=&amp;quot;width:900px; height:200px;&amp;quot;&lt;br /&gt;
|+ '''Table 2. Complex anions'''&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Anion&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Formula&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt;&lt;br /&gt;
! scope=&amp;quot;col&amp;quot; | Comments&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Nitrate nitrate]&lt;br /&gt;
| NO&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt; || 62.00 ||  Potential explosion/fire hazard &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Perchlorate perchlorate] &lt;br /&gt;
| ClO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 99.45&lt;br /&gt;
| Explosion hazard&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://wikipedia.org/wiki/Trifluoromethanesulfonate trifluoromethanesulfonate (triflate)] &lt;br /&gt;
| CF&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 149.1&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://en.wikipedia.org/wiki/Mesylate methanesulfonate (mesylate)]&lt;br /&gt;
| CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 95.09&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://wikipedia.org/wiki/P-Toluenesulfonic_acid toluenesulfonate (tosylate)] &lt;br /&gt;
| CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 171.2&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; |  [http://en.wikipedia.org/wiki/Trifluoroacetic_acid trifluoroacetate]&lt;br /&gt;
| CF&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;COO&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 113.0&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Tetrafluoroborate tetrafluoroborate]&lt;br /&gt;
| BF&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 86.80&lt;br /&gt;
| May hydrolyze to HF&lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Tetraphenylborate tetraphenylborate]&lt;br /&gt;
| B(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 312.9&lt;br /&gt;
| &lt;br /&gt;
|-&lt;br /&gt;
! scope=&amp;quot;row&amp;quot; | [http://wikipedia.org/wiki/Hexafluorophosphate hexafluorophosphate]&lt;br /&gt;
| PF&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;&amp;lt;sup&amp;gt;–&amp;lt;/sup&amp;gt;&lt;br /&gt;
| 145.0&lt;br /&gt;
| May hydrolyze to HF&lt;br /&gt;
|}&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
==== Synthesis of Some Tetraalkylammonium Electrolytes  ====&lt;br /&gt;
While many of these salts are commercially available it is still often much cheaper to make them when larger quantities are required (as is often the case when a lab has several workers using them as electrolytes). The commercially available salts often need recrystallisation to increase their purity to an acceptable level for cyclic voltammetry, which further increases their effective cost.&lt;br /&gt;
===== Tetraethylammonium perchlorate, [(CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;2&amp;lt;/sub&amp;gt;)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;N]ClO&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt; = 229.7  =====&lt;br /&gt;
This compound is not recognised as spontaneously explosive but large quantities should not be heated or stored close to organic compounds. &lt;br /&gt;
&lt;br /&gt;
'''Acid–Bromide method''': Tetraethylammonium bromide, M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt; = 210.2, (100 g, 0.48 mol) is dissolved in water (100 mL) with slight warming, then 1.0 M perchloric acid (600 mL, 0.60 mol) is added. White crystals form immediately and are filtered off after cooling the mixture to below 5 °C. The crude product is washed with ice cold 1.0 M perchloric acid (100  mL) then recrystallised from 1.0 M perchloric acid (300 mL). The product is filtered off, washed first with ice cold 1.0 M perchloric acid (100 mL), then ice cold ethanol (200 mL). Recrystallisation from boiling ethanol (300 mL) with sufficient water to ensure complete dissolution (about 30 mL) gives the final product, which is washed with ice cold ethanol (200 mL). The product can be checked for purity by dissolving about 0.5 g in warm water (2 mL) and testing the pH of the solution (should be about 7), and for any reaction with silver nitrate (no precipitate of AgBr should be visible). A further recrystallisation from ethanol may be necessary. The product is dried under vacuum (0.1 mm Hg), to yield 70.3 g (64%) of white needles. The solid compound should be treated as an oxidising agent and stored away from reducing (organic) materials.&lt;br /&gt;
&lt;br /&gt;
'''Acid–Base method''': Aqueous 1 M perchloric acid (250 mL, 0.25 mol) is added to a solution of 1 M tetraethylammonium hydroxide (250 mL, 0.25 mol). The mixture is adjusted to pH 7 (use a narrow range pH indicator paper, not litmus paper) by the addition of more acid or base solution as required, and stirred while cooling in an ice bath. The resulting precipitate is removed from the cold suspension by suction filtration and washed with cold water. The crude product can be recrystallised from water and dried at 100°C for 24 h in vacuum. M.p. 351 – 352.5 °C with decomposition. The solid compound should be treated as an oxidising agent and stored away from reducing (organic) materials.&lt;br /&gt;
&lt;br /&gt;
The purity of the product should be checked by cyclic voltammetry.&lt;br /&gt;
&lt;br /&gt;
=====Tetra-n-butylammonium hexafluorophosphate,  [n–Bu&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;N]PF&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;, M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt; = 387.4  =====&lt;br /&gt;
'''Acid–Bromide method''': A solution of tetra-n-butylammonium bromide (100 g, 0.31 mol) in acetone (250 mL) is mixed with a solution of ammonium hexafluoro-phosphate (50 g, 0.4 mol) in acetone (350 mL). The resulting precipitate of ammonium bromide is removed by suction filtration. The filtrate is concentrated, with a rotary evaporator, to approximately 200 mL. Water is added to the acetone solution to precipitate tetra-n-butylammonium hexafluorophosphate (final volume approximately 2 L). The precipitate is removed by suction filtration, washed with water, and then redissolved in a solution of ammonium hexafluorophosphate (5 g, 0.04 mol) in acetone (200 mL) — more acetone can be added to complete dissolution if required. Addition of water (final volume approximately 2 L) causes the precipitation of the crude product which is removed by suction filtration and washed with water.&lt;br /&gt;
&lt;br /&gt;
'''Acid–base method''': An aqueous solution of 0.5 M hexafluorophosphoric acid (600 mL, 0.3 mol) is added to an aqueous 0.5 M solution of [http://wikipedia.org/wiki/Tetrabutylammonium_hydroxide tetra-n-butyl-ammonium hydroxide] (600 mL, 0.3 mol). The mixture is adjusted to pH 7 (use a narrow range pH indicator paper, not litmus paper) by the addition of more acid or base solution as required. The crude product is removed from the cooled mixture by suction filtration and washed with water.&lt;br /&gt;
&lt;br /&gt;
'''Recrystallisation''': The crude product, produced by either the acid–bromide or acid–base method, is recrystallized three or four times from a 3:1 mixture of ethanol/water and then dried for at least 24 h at 100°C in a vacuum oven. The yield is usually about 95 g. The purity of the product should be checked by cyclic voltammetry.&lt;br /&gt;
&lt;br /&gt;
===== Tetra-n-butylammonium tetrafluoroborate,  [n–Bu&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;N]BF&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;, M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt; = 329.3  =====&lt;br /&gt;
'''Acid–Bromide method''': Aqueous fluoroboric acid (48%, 36 mL) is added to a solution of tetra-n-butylammonium bromide (84 g, 0.25 mol) in water (180 mL) and the mixture stirred for 1 minute. The resulting precipitate is removed by suction filtration and washed with water until the washings are no longer acid (use a narrow range pH paper). The crude product can be recrystallised from ethyl acetate/cyclohexane. M.p. 162–162.5°C. The purity of the product should be checked by cyclic voltammetry.&lt;br /&gt;
&lt;br /&gt;
===== Tetra-n-butylammonium fluoroborate toluene solvate,  [n–Bu&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;N]BF&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.3(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;) =====&lt;br /&gt;
Tetrabutylammonium fluoroborate is stirred in toluene between 22 – 25°C. A two phase mixture results. The lower layer has an approximate formula of [n-Bu&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;N]BF&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;.3(C&amp;lt;sub&amp;gt;6&amp;lt;/sub&amp;gt;H&amp;lt;sub&amp;gt;5&amp;lt;/sub&amp;gt;CH&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;). (Below 22°C the solvent-free fluoroborate salt crystallises.) This layer an be separated and used, without further purification, for electrochemical work. &lt;br /&gt;
&lt;br /&gt;
Reference: A Simple Hydrocarbon Electrolyte: Completing the Electron-Transfer Series [Fe&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;S&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;(SPh)&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;]&amp;lt;sup&amp;gt;1–/2–/3–/4–&amp;lt;/sup&amp;gt;. C. J. Pickett,  Journal of the Chemical Society Chemical Communications, 323-326, 1985. [http://dx.doi.org/10.1039/C39850000323 DOI: 10.1039/C3985000032]&lt;br /&gt;
&lt;br /&gt;
===== Tetra-n-butylammonium triflate [n–Bu&amp;lt;sub&amp;gt;4&amp;lt;/sub&amp;gt;N]CF&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;SO&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt;, M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt; = 391.5 =====&lt;br /&gt;
Triflic acid (trifluoromethanesulfonic acid), M&amp;lt;sub&amp;gt;r&amp;lt;/sub&amp;gt; = 150.1, (600 mL, 0.15 mol) is slowly added, with stirring, and cooling, to a commercially available 40% solution of  [http://wikipedia.org/wiki/Tetrabutylammonium_hydroxide tetra-n-butyl-ammonium hydroxide] (Mr = 259.5) (100 mL 0.15 mol) until the pH drops to 6.5 (use a narrow range indicator paper). Water is added if necessary to allow adequate stirring. The crude product is suspended in ice cold water and filtered 5 times to wash it, then dried and recrystallised from a mixture of dichloromethane and diethyl ether. The purity of the product should be checked by cyclic voltammetry.&lt;br /&gt;
&lt;br /&gt;
Reference: Tetraalkylammonium trifluoromethanesulfonates as supporting electrolytes.&lt;br /&gt;
K. Rousseau, G. C. Farrington, D. Dolphin, Journal of Organic Chemistry, 37, 3968–3971, 1972. [http://dx.doi.org/10.1021/jo00797a054 DOI: 10.1021/jo00797a054]&lt;br /&gt;
&lt;br /&gt;
== Electrodes ==&lt;br /&gt;
==== Working Electrode ====&lt;br /&gt;
The working electrode is where the chemical reaction of interest takes place. Most commonly a disk electrode of 1 - 3 mm diameter is used that is embedded in a glass, [http://wikipedia.org/wiki/Teflon Teflon], or [http://wikipedia.org/wiki/PEEK PEEK] (polyetheretherketone) body.&lt;br /&gt;
&lt;br /&gt;
The disk material is usually made of an inert material, platinum, [http://wikipedia.org/wiki/Glassy_carbon glassy carbon], and to a lesser extent gold, being the most commonly encountered materials which are [http://wiki.edaq.com/index.php/Cleaning_and_Polishing_Voltammetric_Electrodes polished] to a mirror finish.&lt;br /&gt;
&lt;br /&gt;
For glass body platinum or gold electrodes a soda glass is preferred to borosilicate glass as the thermal coefficient expansion more closely matches that of the metal (so that the disk material does not separate from the glass after repeated temperature changes). While the use of glass body electrode may be required for some experiments in difficult environments the greater robustness of Teflon or PEEK body electrodes make them usually preferred. Teflon offers only slightly better chemical inertness than PEEK, but suffers from 'cold flow' or [http://wikipedia.org/wiki/Creep_(deformation) 'creep']. That is the disk material can separate from a Teflon body more easily than a PEEK body. PEEK body working electrodes with a 1 mm diameter disk are offered by eDAQ:&lt;br /&gt;
*[http://www.edaq.com/ET074-1 ET074 Glassy Carbon Disk Electrode]&lt;br /&gt;
*[http://www.edaq.com/ET075-1 ET075 Platinum Disk Electrode]&lt;br /&gt;
*[http://www.edaq.com/ET076-1 ET076 Gold Disk Electrode]&lt;br /&gt;
&lt;br /&gt;
Microelectrodes (sometimes referred to as [http://wikipedia.org/wiki/Ultramicroelectrode ultramicroelectrodes]) are usually considered to have disk diameters less than 25 microns. Thin platinum or gold wire electrodes have been made down to micron diameters. Carbon fiber (similar to glassy carbon) electrodes down to about 5 micron diameter have also been described..&lt;br /&gt;
&lt;br /&gt;
===== The Mercury Electrode =====&lt;br /&gt;
At times it may be of use to perform cyclic voltammetry experiments in organic solvents using a mercury working electrode. [http://en.wikipedia.org/wiki/Hanging_mercury_drop_electrode Hanging mercury drop electrodes] (HMDE’s) can be used but typically commercial models are expensive and all are cumbersome to set up, require periodic cleaning and maintenance, and require the use of relatively large amounts of elemental mercury. However they do have the advantage of being able to provide a clean mercury electrode by dislodgment of the old mercury drop and allowing a new drop to form, all at the press of a button, in any solvent you require.&lt;br /&gt;
Alternatively mercury film electrodes (MFE’s) use much less mercury (often much less than 1%) than a HMDE, and are relatively low cost. The mercury is usually electrodeposited as a thin film on a glassy carbon, platinum, or carbon–fiber, support electrode. However, the mercury film must be removed and replated if it is fouled or oxidised. Some workers prepare the MFE by electrodeposition from aqueous mercuric ion solutions and then wash the electrode to replace the solvent. However it is also possible to electrodeposit mercury directly in suitable organic solvents: G. Alarnes-Varela, A.L. Suárez-Fernández, A. Costa-García, Electrochimica Acta, 44, 763–772, 1998.&lt;br /&gt;
&lt;br /&gt;
==== Reference Electrode ====&lt;br /&gt;
Three-electrode potentiostats are designed so that no current passes through the [http://wikipedia.org/wiki/Reference_electrode reference electrode], thus it is not subject to any electrolysis reaction and maintains its integrity (and provides a constant potential) throughout the experiment. Unfortunately most reference electrodes are based on aqueous chemistry and are somewhat incompatible with the anhydrous immiscible organic solvents that are often used for cyclic voltammetry. &lt;br /&gt;
With some organic solvents (eg acetonitrile) a silver wire/silver ion reference electrode can be constructed from a standard refillable electrode:&lt;br /&gt;
*[http://www.edaq.com/ET073 Ag/AgCl miniature refillable electrode]&lt;br /&gt;
&lt;br /&gt;
At other times a simple platinum (or platinum coated wire) can be used as a pseudo-reference electrode and  after the experiment [http://wikipedia.org/wiki/Ferrocene ferrocene] (which has a known E&amp;lt;sub&amp;gt;1/2&amp;lt;/sub&amp;gt;) is added to the reaction mixture to calibrate the system.&lt;br /&gt;
A modern innovation is the leakless reference electrode which uses a solid polymer junction to separate the inner aqueous filling solution of the electrode from the other reaction mixture, see&lt;br /&gt;
*[http://www.edaq.com/ET069 ET069 5 mm diameter Leakless Ag/AgCl electrode]&lt;br /&gt;
*[http://www.edaq.com/ET072 ET072 2 mm diameter Leakless Ag/AgCl electrode]&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
In a two electrode system (almost never used these days for cyclic voltammetry experiments) the reference and auxiliary electrode leads of three electrode potentiostat are connected to a single 'counter' electrode. In this case significant current can pass through the counter electrode which must be constructed to maintain a constant chemical environment for the lifetime of the experiment.&lt;br /&gt;
&lt;br /&gt;
==== Auxiliary Electrode ====&lt;br /&gt;
&lt;br /&gt;
The [http://wikipedia.org/wiki/Auxiliary_electrode auxiliary electrode] is often the 'forgotten' electrode in a cyclic voltammetry experiment. If an oxidation event is occurring at the working electrode then a reduction event must be occurring at the auxiliary electrode (and vice versa). Often the reaction at the auxiliary electrode is the electrolysis of the solvent or of an electrolyte component. Thus the auxiliary electrode is required to be made of an inert material, and historically platinum wire has been used. While most metals can be used as electrodes for reduction processes relatively few are stable under oxidizing conditions, platinum being an obvious example. However several other metals are very oxidation resistant (often because they form a protective oxide coating). Molybdenum, tungsten, and titanium are in this category and make excellent auxiliary electrodes (and are much lower cost than platinum). In addition, platinum-coated titanium wire offers similar catalytic reactivity as pure platinum and these auxiliary electrodes are available from eDAQ:&lt;br /&gt;
*[http://www.edaq.com/ET078-1 ET078-1 70 mm Auxiliary Electrode]&lt;br /&gt;
&lt;br /&gt;
== Electrode Position ==&lt;br /&gt;
Electrode position is more critical in resistive organic solvents. Always position the electrodes so that the reference electrode tip is as close a possible to the working electrode tip. In particular avoid placing the auxiliary electrode between the working and reference electrodes.&lt;br /&gt;
&lt;br /&gt;
== iR Compensation ==&lt;br /&gt;
While the cyclic voltammogram of a perfectly reversible one-electron redox process ( for example the ferrocene/ferrocinium couple, or the hexacyano-Fe II/III couple) should exhibit a theoretical peak-to-peak separation of 57 mV at 25°C it is common to find that the experimentally observed separation can be in the order of 80, 100 mV, or even more. Resistive organic solvents show greater deviations than aqueous solutions. This separation can be minimised by using a high background electrolyte concentration and make sure that the reference electrode is close to the working electrode. The effect is due to the so called 'uncompensated resistance' or 'iR drop' between the reference and working electrodes. Some users like to employ iR compensation when performing cyclic voltammetry. In many cases 'positive feedback' compensation is used - but this is only an approximate correction at best, as the exact iR drop will vary with applied potential and with the relatively large currents flowing during the charge transfer process. 'Current interrupt' iR compensation will give better results as the iR drop is actually calculated at each potential in the potential staircase ramp, however many potentiostats do not provide this type of compensation, it is somewhat tricky for a non-specialist to set correctly, and it cannot be used for fast scan rates.&lt;br /&gt;
&lt;br /&gt;
One alternative is simply to do without iR compensation! Perform cyclic voltammetry, under the same conditions you propose for your experiment, on ferrocene (organic solvents), or ferrocene carboxylic acid or hexacyanoferrate (aqueous solutions). The peak-to-peak separations you observe for these one electrode redox couples can be considered to the minimum achievable with the solution and electrode arrangement that you are using. Thus if your analyte exhibits a redox couple with the same peak-to-peak separation you can safely assume it is also a one electron reversible couple.&lt;br /&gt;
&lt;br /&gt;
The use of the ferrocene/ferrocenium ion couple has alo been studied to providing an estimate for the uncompensated resistance: 'Use of the Ferrocene Oxidation Process To Provide Both Reference Electrode Potential Calibration and a Simple Measurement (via Semiintegration) of the Uncompensated Resistance in Cyclic Voltammetric Studies in High-Resistance Organic Solvents.'  Alan M. Bond, Keith B. Oldham, and Graeme A. Snook, Analytical Chemistry, 72, 3492-3496, 2000. [http://dx.doi.org/10.1021/ac000020j DOI: 10.1021/ac000020j]&lt;br /&gt;
&lt;br /&gt;
== Reaction Vessel ==&lt;br /&gt;
The vessel chosen in which to perform the cyclic voltammetry experiment must be designed to hold the electrodes and also to allow nitrogen purging for oxygen-sensitive compounds or their electrolysis  products. If you are characterising new compounds, which are often available only in milligram quantities, then a small volume vessel is also desirable. Even for routine or teaching experiments a small volume vessel cuts down on the amount of organic solvent and valuable electrolyte salts being used. Using 1 mm disk electrodes it is possible to perform cyclic voltammetry in vessels with only 1 - 3 mL of solvent. See&lt;br /&gt;
*[http://www.edaq.com/ET080-12 ET080 3 mL Reaction vessel]&lt;br /&gt;
*[http://www.edaq.com/ET014 ET014 EChem Electrode Kit]&lt;br /&gt;
It is often useful to have the reaction vessel equipped with a magnetic spin bar so that the solution can be stirred between scans.&lt;br /&gt;
&lt;br /&gt;
== Troubleshooting ==&lt;br /&gt;
{{#ev:youtube|rgHZq671adU|300|right|Video 2. Check the Performance of the Potentiostat with Potentiostat Maintenance Check}}&lt;br /&gt;
When unexpected results occur it may not be obvious as to the cause of the problem. However a few simple tests (shown in Video 2.) can cave an indication as to the location of the fault. &lt;br /&gt;
&lt;br /&gt;
Many potentiostats are fitted with a 'dummy cell', often an internal resistor with a value of a few kohm to several megohm. If this is the case, use the dummy cell mode and apply an appropriate potential. If the resulting current signal obeys Ohm's Law, i = E/R, then it is likely that the potentiostat itself is functioning correctly.&lt;br /&gt;
&lt;br /&gt;
Next, attach a resistor of appropriate value (usually a few kohm to several megohm) to the electrode leads if the potentiostat: working electrode lead to one end of the resistor, and reference and auxiliary leads to the other end. Apply a potential and check the current signal. If the current signal obeys Ohm's Law, i = E/R, (for example 1 V applied across a 1 megohm resistor would produce 1 microamp) then it is likely that the electrode leads are in good condition, and the problem may be with the electrodes or the chemistry in the reaction vessel.&lt;br /&gt;
&lt;br /&gt;
A variant on this latter procedure is to replace the resistor with a voltmeter. Most voltmeters have an internal resistance of 1 or 10 megohm, and so would produce a current of 1 or 0.1 µA if a 1 V potential were applied to them. Connect the working electrode lead of the potentiostat to red voltmeter input, and the reference and auxiliary leads to the black (reference) voltmeter input. The voltmeter will display the actual applied potential so that you can check that the potentiostat is actually applying the correct value. If a negative value is seen instead of a positive value (or vice versa) the you need to switch the polarity of your potentiostat.&lt;br /&gt;
&lt;br /&gt;
==== Noise ====&lt;br /&gt;
The current signal is susceptible to electrical interference. Usually noise levels on the current signal should be less than 1 µA peak-to-peak. Levels much above this indicate a potential problem or a large noise source nearby. Often the noise is picked up by a relatively high impedance from the reaction mixture or the electrodes themselves. A faulty broken reference electrode can give rise to excessive noise.&lt;br /&gt;
&lt;br /&gt;
Nearby equipment (especially equipment that has a heavy current requirement) may cause interference. Try turning nearby equipment off and see if the signal noise disappears.&lt;br /&gt;
&lt;br /&gt;
Mains powered equipment usually relies on the earthing of the power socket to also provide good grounding to the potentiostat (and its shielding). However what constitutes a safe electrical earthing does not always provide good instrumental grounding and noise may actually be picked up on the earthing. Power sockets also grouped in various power circuits distributed throughout the laboratory building and each circuit usually has its own earthing that goes to a common ground. This means that moving the apparatus to a different power socket on a different circuit may improve your signal.&lt;br /&gt;
&lt;br /&gt;
In most cases, currents signals of a microampere or greater can be measured without use of a Faraday cage, or other special shielding. It is usual to find that 90% or more of 'noise' is due to the pick up of mains hum (50 or 60 Hz) so that a 10 Hz filter is very effective at reducing most noise. However remember that a low pass filter can also distort you peak shapes. As a rough rule of thumb you can use a 10 Hz filter with scan rates up to 100 mV/s with no discernible peak shape distortion. In fact it is usually recommended to use a 10 Hz filter setting for all cyclic voltammetry experiments using a scan rate of 100 mV/s or less.&lt;br /&gt;
&lt;br /&gt;
If the current signal is sub-microampere, or if you are employing fast scan rates then you may have no choice but to place your reaction vessel inside a [http://wikipedia.org/wiki/Faraday_cage Faraday cage] (a cage or box of a conductive material electrically connected to earth). A home-made Faraday cage using an old biscuit tin, or a wooden frame covered with copper mesh, will often work just as well as an expensive commercial product, but remember that the cage must be earthed. All AC powered devices (including an AC powered potentiostat) should stay outside the Faraday cage. Many potentiostats employ shielded lead wires which are passed through a small hole in the wall of the Faraday cage. If your potentiostat has unshielded lead wires consider shortening them as much as possible to avoid unnecessary noise pickup. Note that [http://www.edaq.com/potentiostats.php eDAQ Potentiostats] have a conveniently placed 4 mm binding post on their back panel for the grounding of a Faraday cage. &lt;br /&gt;
&lt;br /&gt;
Desktop computers, and old CRT (cathode ray tube) monitors are often sources of high frequency noise. Laptop computers and LCD displays are usually much quieter. It is normally good practice to position the computer and monitor away from the reaction vessel.&lt;br /&gt;
&lt;br /&gt;
To check for noise emanating from nearby equipment, connect a high value resistor (1 megohm or more) to the potentiostat lead wires,  working electrode lead to one end of the resistor, and reference and auxiliary leads to the other end. This is shown in [[Check_the_Performance_of_the_Potentiostat_with_Potentiostat_Maintenance_Check|this video]]. Examine the current signal  (any potential even zero volts can be used) on a ranges of 10 microampere or less, so that you can see the signal noise. Make sure all low pass filters are turned off. As you move the resistor about, for example near power leads and computers, you may find noisy 'hot spots'.&lt;br /&gt;
&lt;br /&gt;
==== Hum/Sinusoidal noise====&lt;br /&gt;
Sometimes a sinusoidal interference is seen on the current signal. This is almost always due to an aliasing of mains interference (at 50 or 60 Hz) against the sampling frequency and sampling period. If the scan rate is less than 100 mV/s then use a 10 Hz low pass filter setting on the current signal. This will remove almost all the mains interference without distorting the peak shapes in the voltammogram. A similar effect can be achieved by making the sampling period an integral number of mains cycles (i.e. a multiple of 20 ms at 50 Hz, and 16&amp;lt;sup&amp;gt;2&amp;lt;/sup&amp;gt;/&amp;lt;sub&amp;gt;3&amp;lt;/sub&amp;gt; ms at 60 Hz, while a multiple of 100 ms works for both 50 and 60 Hz), however this also requires a relatively slow scan rate.&lt;br /&gt;
&lt;br /&gt;
==== Drift ====&lt;br /&gt;
Excessive current signal drift can indicate a faulty connection to the electrodes, or a faulty reference electrode. Also check the surface of the working electrode in case there has been some sort of by-product being electrodeposited.&lt;br /&gt;
&lt;br /&gt;
==== Decreasing peak intensity ====&lt;br /&gt;
The peak height might be seen to be slowly decreasing scan after scan. Even if the scanning is stopped and the solution stirred, and the scanning restarted, the peaks are still seen to be small. In this case check the working electrode for the buildup of an electrodeposited material which may be acting as an insulating layer.&lt;br /&gt;
&lt;br /&gt;
==== Zero Signal ====&lt;br /&gt;
A zero current signal usually indicates an incomplete circuit. Check that the working electrode is connected. Also check the working electrode with a multimeter/ohmmeter making sure that there are at most only a few ohms between the electrical contact at the top of the electrode and its tip.&lt;br /&gt;
&lt;br /&gt;
==== Peaks in Strange Positions ====&lt;br /&gt;
If the peaks you see are drifting to or have moved to potentials that seem to be wrong then the reference electrode is probably faulty. Try a new electrode, or cleaning the old electrode.&lt;br /&gt;
&lt;br /&gt;
==== Peaks at Opposite Polarity ====&lt;br /&gt;
If you find your redox couples appearing with a negative E&amp;lt;sub&amp;gt;1/2&amp;lt;/sub&amp;gt; instead of a positive value (or vice versa) then your potentiostat is probably operating with the wrong polarity. Most people doing a cyclic voltammetry experiment want a more negative potential to indicate more reducing conditions at the working electrode. However the potentiostat design may use the reverse convention where a negative potential means that the working electrode is more positive (ie oxidising) than the reference. Some older style potentiostats have a polarity reversal switch to invert the polarity. Read you potentiostat manual carefully to determine its polarity convention. You can also use a voltmeter to check the applied potential.  Connect the working electrode lead of the potentiostat to red voltmeter input, and the reference and auxiliary leads to the black (reference) voltmeter input. The voltmeter will display the actual applied potential so that you can check that the potentiostat is actually applying the correct value.&lt;br /&gt;
&lt;br /&gt;
==== Current Signal Overload ====&lt;br /&gt;
If the current signal goes off scale check that the electrodes (and their contacts and clips) are not touching one another. If the potentiostat dummy cell behaves well, but when the lead wires are connected to a external resistor a current overload occurs then suspect a short circuit in the lead wire connector, or an electrical short to a cable shield.&lt;br /&gt;
&lt;br /&gt;
==== Potential Overload ====&lt;br /&gt;
If the potentiostat indicates a potential overload (or 'out of compliance' situation) then check that the auxiliary electrode it still connected. If you are using particularly resistive organic solvents and the auxiliary electrode is distant from the working electrode, it is possible that your potentiostat does not have sufficient compliance potential (ie the potential between the working and auxiliary electrodes) to achieve the requested applied potential (i.e. the  potential between the working and reference electrodes). Consider bringing the auxiliary electrode closer to the working electrode, increasing the background electrolyte concentration, or changing the solvent.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3992</id>
		<title>ER430 Manual</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3992"/>
				<updated>2015-08-06T07:49:47Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* System Indicators */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;br /&gt;
== Introduction ==&lt;br /&gt;
[[File:ER430SmallPanels.jpg|thumb|upright=2|right|'''Figure 1.''' ER430 HV Sequencer front and back panels]]&lt;br /&gt;
This manual is intended to allow the user to install, check and run the ER430 HV Sequencer. It provides detailed information on the system and its operation. Please read this manual carefully prior to beginning operation.&lt;br /&gt;
&lt;br /&gt;
The ER430 High Voltage Sequencer provides the following functions:&lt;br /&gt;
::• Four independent programmable metered high voltage (HV) supplies.&lt;br /&gt;
::• Safety Interlock system&lt;br /&gt;
::• Software that allows arbitrary sequences of voltages to be generated&lt;br /&gt;
&lt;br /&gt;
== Checking the Instrument ==&lt;br /&gt;
Before you begin working with the device, you should check:&lt;br /&gt;
:• that the contents of the package you received match the packing list&lt;br /&gt;
:• for any sign of physical damage that might have occurred during transit.&lt;br /&gt;
If you find a problem, please contact your [http://www.edaq.com/edaq-distributors eDAQ distributor] or agent immediately.&lt;br /&gt;
&lt;br /&gt;
== Safety First ==&lt;br /&gt;
&lt;br /&gt;
This equipment generates high voltages of up to 3000 V DC at currents of up to 200 µA. Making contact with such voltages can be extremely dangerous.&lt;br /&gt;
&lt;br /&gt;
Ensure that the high voltage (HV) circuits are housed in an insulated enclosure fitted with an Interlock safety circuit and with no manual access to HV circuits while circuits are alive.&lt;br /&gt;
&lt;br /&gt;
Safety precautions:&lt;br /&gt;
::• Ensure that the safety interlock circuit is connected to the HV Sequencer and is only active and enabled when no accidental access to High Voltage circuits can be made.&lt;br /&gt;
::• Wear rubber soled footwear&lt;br /&gt;
::• Ensure the floor and bench top are dry&lt;br /&gt;
::• Stand on a rubber mat when in the vicinity of high voltages&lt;br /&gt;
&lt;br /&gt;
The ER430 features design precautions to ensure that there is no accidental application of high voltages. These include automatic shutdown in the event of voltage or current overloads . This will in some circumstances prevent the unit from operating. In these cases check all settings and safety interlocks carefully before resuming the experiment.&lt;br /&gt;
&lt;br /&gt;
=== What is an Interlock ===&lt;br /&gt;
&lt;br /&gt;
An interlock is a mechanical or electrical system that prevents the inadvertent operation of of an instrument.&lt;br /&gt;
&lt;br /&gt;
In the case of the  ER430 HV Sequencer this is achieved by using a switch located in the enclosure in which high voltages are active.  This switch is connected via a cable to the front panel INTERLOCK BNC in such a way that the switch is only closed when no access is available to the High voltages inside the enclosure.&lt;br /&gt;
&lt;br /&gt;
For example with the eDAQ supplied ET225 Micronit Chip Electrophoresis Platform, high voltages can only be applied when the top cover is in place.  This is detected and the interlock switch enabled to allow the application of high voltages.&lt;br /&gt;
&lt;br /&gt;
If the user is providing the MicroChip enclosure then it is the user’s responsibility to provide the required interlock function.&lt;br /&gt;
&lt;br /&gt;
To test the Interlock function it is sufficient to apply a short circuit across the INTERLOCK BNC input pins.  This should only be done with no connections to the High Voltage input connectors.&lt;br /&gt;
ER430 &lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
System indicators as shown in the preceding diagram provide a direct indication of system operation that reflects the state of the internal hardware.  These indicators will assist you in monitoring system operation and in diagnosing problems – study them carefully:  &lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED (Amber LED)&lt;br /&gt;
::• FLASHING = Interlock open, unit disarmed, arming not enabled.&lt;br /&gt;
::• OFF = Interlock in place and enabled, unit can be ARMED.&lt;br /&gt;
::• ON = Interlock in place, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
SYSTEM STATUS LED (RGB LED)&lt;br /&gt;
::• GREEN when “on line” and ready as a Master&lt;br /&gt;
&lt;br /&gt;
METER FUNCTION LED (RGB LED)&lt;br /&gt;
::• GREEN:  Safe (disconnected) &lt;br /&gt;
::• YELLOW:  Current Mode&lt;br /&gt;
::• BLUE:  Voltage mode&lt;br /&gt;
&lt;br /&gt;
HV STATUS (RED LED)&lt;br /&gt;
::• OFF: supply disconnected&lt;br /&gt;
::• ON: supply connected and active.&lt;br /&gt;
&lt;br /&gt;
Notes: &lt;br /&gt;
#On power up the system performs a startup test and flashes the front panel LEDs through the various colors available for display.&lt;br /&gt;
# In some cases where the HV supply needs to be used in proximity to light sensitive detectors it is possible to optionally turn off all the LEDs to maintain low background illumination.&lt;br /&gt;
&lt;br /&gt;
== Hardware Installation ==&lt;br /&gt;
'''ATTENTION:''' When installing the system for the first time ALWAYS perform software installation before connecting the hardware units.  This ensures that the correct drivers are installed &lt;br /&gt;
 &lt;br /&gt;
After carrying out the software installation described in the next section, perform the following Hardware installation procedure. It will confirm that:&lt;br /&gt;
::• That safety interlocks are in place and functioning correctly&lt;br /&gt;
::• The unit can be armed and disarmed&lt;br /&gt;
&lt;br /&gt;
Operation:&lt;br /&gt;
::• '''Safety first''' Connect the unit to a good ground using the terminal post on the rear of the unit.&lt;br /&gt;
::• Connect the unit to the 12V DC mains power pack.&lt;br /&gt;
::• Connect the unit to the PC using the USB cable provided.&lt;br /&gt;
::• Turn Power on.&lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED will flash if interlock is not enabled.&lt;br /&gt;
&lt;br /&gt;
HV Status LEDs: Off (no high voltage output)&lt;br /&gt;
&lt;br /&gt;
STATUS LEDs: Green&lt;br /&gt;
&lt;br /&gt;
=== TEST INTERLOCK Function ===&lt;br /&gt;
&lt;br /&gt;
This function can be tested without any software running:&lt;br /&gt;
::• The INTERLOCK LED will initially be flashing.&lt;br /&gt;
::• Connect a short circuit to the INTERLOCK BNC.&lt;br /&gt;
::• INTERLOCK LED will turn OFF.&lt;br /&gt;
::• Press the ARM Push Button for approximately 1 to 2 seconds.  You should hear a beep, warning you that the HV outputs have been armed (enabled) and the INTERLOCK LED will turn ON.&lt;br /&gt;
::• At this point all HV supplies are still inactive but are in a state where they can be set and controlled by the Sequencer Application software.&lt;br /&gt;
::• Pressing the Arm button again will DISARM the HV Sequencer, and the INTEROCK LED will turn off.&lt;br /&gt;
&lt;br /&gt;
A momentary push on  the Arm button will disable all the HV outputs of the Sequencer.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== INTERLOCK features ===&lt;br /&gt;
The system is provided with a number of safety features or Interlocks:&lt;br /&gt;
::• Chip adapter interlock:  The chip adapter used should provide a safety contact interlock to indicate that the microchip adapter is safe for use.  This interlock is a contact closure switch, which is closed when the HV circuit is fully enclosed and protected from user access. This interlock is connected to the front panel Interlock BNC and indicates to the ER430 that it is safe to arm the system.&lt;br /&gt;
::• USB Present:  The system cannot be ARMED without an active USB connection&lt;br /&gt;
::• Software Control: Once the system is ARMED High Voltages can only be applied under software control.&lt;br /&gt;
::• ARM circuit: prior to applying HV to an external circuit the system must be armed by the user by depressing the front panel ARM push button for approximately 2 seconds.&lt;br /&gt;
::• DISARM: The system can be disarmed by a momentary push of the ARM button.&lt;br /&gt;
::• Power Overloads:  the circuit detects power overloads and situations that lead to the generation of arcs (sparks).  The system will switch itself off in such circumstances and in such circumstances may require to be reinitiated with power being turned on Off and On.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION:'''  Do not disconnect HV leads by hand while High voltages are present – this is extremely dangerous and can cause harmful arcs to be generated. To disable power use the ARM/DISARM front panel button or the software’s Disarm or Disconnect menu items&lt;br /&gt;
&lt;br /&gt;
You are now ready to operate the Sequencer software which will allow you to generate and output a series of high voltage pulses and ramps.&lt;br /&gt;
&lt;br /&gt;
== Software Installation &amp;amp; Operation ==&lt;br /&gt;
&lt;br /&gt;
=== Installing the HV Sequencer software ===&lt;br /&gt;
Insert the HV Sequencer installation USB stick into your computer.  It is recommended to install the software before plugging in the hardware, as it ensures the drivers are correctly installed.&lt;br /&gt;
&lt;br /&gt;
The eDAQ Sequencer Setup Wizard will display a start-up screen; follow the prompts to install the software.&lt;br /&gt;
      Start up screen&lt;br /&gt;
			    Final Start up screen&lt;br /&gt;
&lt;br /&gt;
=== eDAQ Sequencer Overview ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Sequencer is a Windows application that provides the means to setup a series of steps that are executed under computer control.  The following functions are provided:&lt;br /&gt;
&lt;br /&gt;
System setup and sequence entry: The software identifies system configuration on startup and allows the operating parameters to be set immediately.&lt;br /&gt;
&lt;br /&gt;
Table driven Sequence: A time based table is filled out, specifying that the operations to be performed in sequence.  This includes setting of HV supplies to new voltages, trigger and digital I/O line functions. The following sequence operations are implemented: &lt;br /&gt;
&lt;br /&gt;
Time: set to xxxx seconds&lt;br /&gt;
Meter 1&amp;amp;2: Disconnect, Read V, Read I&lt;br /&gt;
Output1&amp;amp;2: Set V=xxxx (V and I monitored), Read V, Read I&lt;br /&gt;
Digital Out: Low/Open, High/Closed, Short Pulse, Long Pulse&lt;br /&gt;
Special commands: Wait for trigger, Wait for Arming, Go Safe&lt;br /&gt;
New functions can be readily added to meet customer requirements&lt;br /&gt;
&lt;br /&gt;
Digital outputs can be used to control external devices or the recording of data in an ecorder.&lt;br /&gt;
&lt;br /&gt;
Monitoring: Once a sequence is started the user is able to observe the progress of the sequence on the sequence table.  Values of HV supply voltages and currents are displayed during operation.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
 === HV Sequencer Main Window ===&lt;br /&gt;
&lt;br /&gt;
  &lt;br /&gt;
=== Communication ===&lt;br /&gt;
&lt;br /&gt;
The HV sequencer uses a virtual USB serial communications (COM) port.  When the ER430 hardware is first attached to USB, a free COM port number is automatically assigned by Windows.  That COM port will be then used every time that unit is plugged in again.&lt;br /&gt;
&lt;br /&gt;
Note:  the first time you connect the system to the computer it may take some time for the system to identify the HV sequencer device driver and install it.  You will be notified when the device is ready.&lt;br /&gt;
&lt;br /&gt;
The first time you use the sequencer software, you need to specify the COM port that the hardware has been assigned.  Select the Preferences option in the File menu, then choose your HV Sequencer in the list at the top – see screen shot below. This preference is automatically saved for future use&lt;br /&gt;
&lt;br /&gt;
  Preferences panel&lt;br /&gt;
&lt;br /&gt;
If you are uncertain about which COM port to assign use, the Serial Port Monitor application can help identify the COM port assigned to the HV sequencer. This small application is included on the HV Sequencer installer USB stick, and can also be downloaded from the eDAQ Utilities and Tools download webpage [http://www.edaq.com/utilities_tools.php www.edaq.com/utilities_tools.php]&lt;br /&gt;
&lt;br /&gt;
The serial port monitor runs as an icon in the notification area.  Clicking on it will show a list of eDAQ COM port devices attached to your computer.&lt;br /&gt;
&lt;br /&gt;
The other Preference options set the digital output type, and provide control over front panel lights in situations where light pollution needs to be kept to a minimum.&lt;br /&gt;
&lt;br /&gt;
Check if you have installed an interlock as described previously.  The INTERLOCK LED should be OFF indicating that the INTERLOCK is in place.&lt;br /&gt;
    &lt;br /&gt;
&lt;br /&gt;
Click the Online in the menu bar to attach the selected ER430 unit to the Sequencer application. &lt;br /&gt;
&lt;br /&gt;
Click the Offline in the menu bar to disconnect the selected ER430 unit from the Sequencer application.&lt;br /&gt;
&lt;br /&gt;
=== Disarming and Interlock Test ===&lt;br /&gt;
&lt;br /&gt;
Press and hold the red ARM button to arm the unit.  As before, the unit will beep and arm itself.  This will also be shown in the software’s display.&lt;br /&gt;
&lt;br /&gt;
You can now disarm the unit by either:&lt;br /&gt;
::• Pressing the red ARM button again&lt;br /&gt;
::• Clicking “Disarm” in the top-right of the software window.&lt;br /&gt;
&lt;br /&gt;
While the unit is armed, you can test the safety interlock by removing the short-circuit from the BNC connector.  The unit should immediately disarm itself, disconnecting the outputs, and turning off any applied voltages.&lt;br /&gt;
&lt;br /&gt;
=== Manual Settings ===&lt;br /&gt;
After arming the unit, click on the More… button to display the controls for making immediate changes to the unit.&lt;br /&gt;
&lt;br /&gt;
The right hand side of the HV Sequencer setup panel provides the means to manually set meter functions, output voltages, and the digital outputs’ states.  Make some selections, and then click on Set.  The ER430 hardware will immediately apply the settings you have chosen, and the software will display your choices, along with readings of current and/or voltage.&lt;br /&gt;
&lt;br /&gt;
At this point  the system will indicate the voltages set and currents measured.  Since no loads are yet connected, the currents will be very near zero. &lt;br /&gt;
&lt;br /&gt;
=== Setup panel ===&lt;br /&gt;
&lt;br /&gt;
At any time, pressing the Disarm button in the top-right hand corner of the Main Window or the red button on the front panel of the ER430 will disarm the unit and make it safe.  &lt;br /&gt;
&lt;br /&gt;
After disarming, you must press and hold the red button (as before) to re-arm it.  The software can not re-arm the device.&lt;br /&gt;
&lt;br /&gt;
Outputs let you control the digital outputs of the unit.  In the preference you can set Output configuration as contact closure, or TTL.&lt;br /&gt;
HV Sequences&lt;br /&gt;
The lower area of the Setup panel provides the means to define a “program” or “sequence” to run. This consists of a number of timed steps, each of which can update the state of one or more of the individual functions or outputs.  There are also some “special” commands that can be carried out. Unused connections can have the width of their columns reduced by dragging their column separator.&lt;br /&gt;
&lt;br /&gt;
All changes on a step happen simultaneously (within 2 milliseconds).&lt;br /&gt;
   Setup screen with an example&lt;br /&gt;
&lt;br /&gt;
Here is another example program:&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
If a step doesn’t have anything entered in its box, the output will remain unchanged from its previous setting.&lt;br /&gt;
&lt;br /&gt;
A time of “0” means “immediately upon starting”, and the times are cumulative, measured from when the sequence was started,  i.e.: the delay between the first four of the lines above is 5, 3, and 4 seconds respectively.&lt;br /&gt;
&lt;br /&gt;
It is recommended to have the first row setting every output to a known state, in case the previous run was stopped part-way through, leaving the unit in an unknown state.&lt;br /&gt;
&lt;br /&gt;
When the program finishes, the unit will be left in whatever state it was at the end.  It will not automatically disconnect or disarm the outputs, unless explicitly told to do so.&lt;br /&gt;
The Meter channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal (LED GREEN)&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE)&lt;br /&gt;
Read I:  Current Meter connection (LED YELLOW)&lt;br /&gt;
The Output channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal.&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE).&lt;br /&gt;
Read I: Current meter connection (LED YELLOW)&lt;br /&gt;
Set V: Set the voltage to the value entered in the second column – In this mode the Voltage indicated will be the actual voltage produced within 1%. (LED RED)&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
Digital outputs can be set to:&lt;br /&gt;
Low/Open: Output goes low or open, as per the “digital output mode” setting in Preferences. &lt;br /&gt;
High/Closed: Output goes high or closed.&lt;br /&gt;
&lt;br /&gt;
The type of digital output, TTL or Contact Closure, is set from the Preferences dialog in the File menu.&lt;br /&gt;
&lt;br /&gt;
Special is a special function to be performed.  You can either:&lt;br /&gt;
::• Disarm: Disconnect HV supplies, and stop the program, or&lt;br /&gt;
::• Wait for trigger: Pause, and wait for a high/close on the rear panel’s green connector “Trigger” pins.&lt;br /&gt;
&lt;br /&gt;
Simple editing commands are available on the Edit menu.  The option to Always show the slave will force the display of the second control panel and additional program columns, even if a second unit is not attached.&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
Programs can be saved and loaded using the menu options in the File menu. &lt;br /&gt;
&lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
Once you are satisfied with your program, click the Run button in the menu bar.  The software will step through the program, executing each step at the given time after starting.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Pause button can be used to pause running of the program.  The Run button changes to a Resume button, which you can click to continue execution.&lt;br /&gt;
Stop will stop execution, but it will leave the unit in the current state, with whatever voltages selected still being output.&lt;br /&gt;
The Disarm button will stop any running program and put the ER430 hardware into a safe state.&lt;br /&gt;
Various fault and safety switch conditions will also force a disarming (and termination of program), including:&lt;br /&gt;
•	USB cable being removed&lt;br /&gt;
•	Front panel safety interlock opened/removed&lt;br /&gt;
•	Front panel red button being pressed&lt;br /&gt;
•	When operating with a slave unit, disconnection from the slave unit&lt;br /&gt;
&lt;br /&gt;
=== Modes of Operation ===&lt;br /&gt;
&lt;br /&gt;
==== General ====&lt;br /&gt;
::• Disarmed/Safe – High voltages and meters disconnected  &lt;br /&gt;
::• Armed- High voltages are active and available for connection to external circuit.&lt;br /&gt;
&lt;br /&gt;
==== Programmable HV power supplies ====&lt;br /&gt;
Output Voltage:  Adjustable from ±200V to ±3000V at up to 200µA. &lt;br /&gt;
Output Polarity:  Positive or Negative with respect to the common ground potential&lt;br /&gt;
&lt;br /&gt;
==== Operating Modes ====&lt;br /&gt;
::• O/C mode: Open Circuit by disconnection with high voltage relay.&lt;br /&gt;
::• Voltage Mode: High voltage output mode with current and voltage monitoring&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 10 Meohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring&lt;br /&gt;
&lt;br /&gt;
==== Meters ====&lt;br /&gt;
::• O/C mode: Open Circuit achieved by disconnection with high voltage relay&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 100 Mohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring &lt;br /&gt;
&lt;br /&gt;
By combining the HV power supplies and meters it is possible to setup the conditions which load the sample into the separation channel and then apply the appropriate voltages to cause separation and detection of the sample components as shown in the example.&lt;br /&gt;
&lt;br /&gt;
=== Typical Installation ===&lt;br /&gt;
 &lt;br /&gt;
 &lt;br /&gt;
== ER430 HV Hardware ==&lt;br /&gt;
&lt;br /&gt;
=== ER430 HV Channel Block Diagram ===&lt;br /&gt;
A Block diagram of a HV supply channel is shown below; there are four identical HV channels in each ER430unit:&lt;br /&gt;
 &lt;br /&gt;
=== ER430 Meter Channel block diagram ===&lt;br /&gt;
&lt;br /&gt;
=== Green Connector Pin Numbers ===&lt;br /&gt;
&lt;br /&gt;
ER430 HV Sequencer “green” connector Pin functions&lt;br /&gt;
&lt;br /&gt;
:: 1	TRIG +	TTL  IN	11	HV 1 E	HV VOLTAGE  MONITOR 1&lt;br /&gt;
:: 2	TRIG -	TTL COM	12	HV 1 I	HV CURRENT MONITOR 1&lt;br /&gt;
:: 3	HV4  E	HV VOLTAGE  MONITOR 4	13	CTL1 +	DIGITAL  IN/OUT 1&lt;br /&gt;
:: 4	HV4  I	HV CURRENT MONITOR 4	14	CTL1 -	DIGITAL COM&lt;br /&gt;
:: 5	COM	COMMON	15	CTL2 +	DIGITAL  IN/OUT 2&lt;br /&gt;
:: 6	HV3 E	HV VOLTAGE  MONITOR 3	16	CTL2 -	DIGITAL COM&lt;br /&gt;
:: 7	HV3  I	HV CURRENT MONITOR 3	17	CTL3+	DIGITAL  IN/OUT 3&lt;br /&gt;
:: 8	HV 2 E	HV VOLTAGE  MONITOR 2	18	CTL3 -	DIGITAL COM&lt;br /&gt;
:: 9	HV 2  I	HV CURRENT MONITOR 2	19	CTL4 +	DIGITAL  IN/OUT 4&lt;br /&gt;
:: 10	COM	COMMON	20	CTL4 -	DIGITAL COM&lt;br /&gt;
&lt;br /&gt;
Notes:&lt;br /&gt;
# Digital I/O pins are implemented as contact closure or TTL outputs, software selectable&lt;br /&gt;
# Trigger input can be a contact closure or TTL input&lt;br /&gt;
# HV VOLTAGE  MONITOR scale factor: 500mV/kV&lt;br /&gt;
# HV Current Monitor Scale factor: 100mV/mA&lt;br /&gt;
&lt;br /&gt;
== Specifications==&lt;br /&gt;
&lt;br /&gt;
=== High Voltage Output and Mode Options ===&lt;br /&gt;
&lt;br /&gt;
::• Channels: 4&lt;br /&gt;
::• Model: UR3*&lt;br /&gt;
::• Maximum Voltage Setting: ±3000 V&lt;br /&gt;
::• Minimum Voltage Setting: ±200 V&lt;br /&gt;
::• Current: ±200 µA max&lt;br /&gt;
::• Ripple: 0.1%		&lt;br /&gt;
::• Operating Modes: Applied voltage, Open Circuit (O/C), and Short Circuit (S/C)		&lt;br /&gt;
::• Load regulation: &amp;lt;2% specified for 20-90% full load: &lt;br /&gt;
::• Rise and Fall times: &amp;lt;5 ms specified for changes within the same polarity regime&lt;br /&gt;
::• Mode Change: &amp;lt;100ms due to relay operations, safety and software latency&lt;br /&gt;
	&lt;br /&gt;
Note: Output is referred to system common (Case Ground)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Safety Features ===&lt;br /&gt;
An interlock is provided on&lt;br /&gt;
::• the mechanical case to ensure that no voltages are present with the case open unless authorized maintenance is in progress.  &lt;br /&gt;
::• the microchip environment to ensure that accidental contact is not made with the high voltages.&lt;br /&gt;
&lt;br /&gt;
The Arm/disarm switch needs to be held for 2 seconds to arm the system and allow high voltages to become active.  Any short contact on the ARM switch will disarm the system.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION''': It is the responsibility of the user to ensure that adequate protection is provided on the equipment provided by the user. eDAQ provides microfluidic chip adaptors with appropriate interlock features.&lt;br /&gt;
&lt;br /&gt;
=== Meter Functions ===&lt;br /&gt;
&lt;br /&gt;
::• Voltage Range:	±3000 V&lt;br /&gt;
::• Voltage Resolution: 1 V&lt;br /&gt;
::• Current Range: ±200 µA&lt;br /&gt;
::• Current resolution: 1 µA&lt;br /&gt;
::• Displayed resolution limited to 1 unit&lt;br /&gt;
&lt;br /&gt;
=== Communications and Inputs and outputs terminals ===&lt;br /&gt;
&lt;br /&gt;
::• Daisy Chain connectors: Twin DB9 connectors allow two (2) ER430 units to be daisy chained together.&lt;br /&gt;
::• USB Port:  Compatible with USB1 &amp;amp; USB 2 and provides, communications facility to PC’s&lt;br /&gt;
::• Output and Meters front panel connectors:  SHV (Safe High Voltage)  type &lt;br /&gt;
::• 20 Way 3.5mm Green screw terminal: &lt;br /&gt;
:::: - Four Digital I/O lines&lt;br /&gt;
:::: - Trigger TTL or CC&lt;br /&gt;
:::: - Four Voltage Monitor signals&lt;br /&gt;
:::: - FourCurrent  Monitor signals.&lt;br /&gt;
::• System/Chassis Earth terminal: 4 mm screw terminal.&lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
&lt;br /&gt;
The following LED front panel displays are available:&lt;br /&gt;
&lt;br /&gt;
::•  System Status (RGB LED)&lt;br /&gt;
::: GREEN when “on line” &lt;br /&gt;
&lt;br /&gt;
::• Interlock (amber LED)&lt;br /&gt;
::: FLASHING = Interlock open, unit disarmed, arming not allowed.&lt;br /&gt;
::: OFF = Interlock OK, unit disarmed&lt;br /&gt;
::: ON = Interlock OK, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
::• Meter Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (disconnected) &lt;br /&gt;
:::: YELLOW = Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (supply disconnected) &lt;br /&gt;
:::: YELLOW =  Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Status  (RGB LED)&lt;br /&gt;
:::: OFF = supply disconnected&lt;br /&gt;
:::: ON = supply connected and active.&lt;br /&gt;
&lt;br /&gt;
=== Physical ===&lt;br /&gt;
::• Dimensions (w x h x d): 200 x 65 x 250 mm (7.9 x 2.6 x 9.8 inch)&lt;br /&gt;
::• Weight: 3.00 kg packed&lt;br /&gt;
::• Operating temperature: 0 - 35ºC&lt;br /&gt;
::• Humidity: 10 to 80% non condensing &lt;br /&gt;
::• Power:  9 - 16 V @ 2 A maximum supplied by mains powered AC/DC converter (supplied)&lt;br /&gt;
&lt;br /&gt;
== Legal and Warranty ==&lt;br /&gt;
&lt;br /&gt;
=== Trademarks and Copyright ===&lt;br /&gt;
Sequencer, HV Sequencer, and Chart are trademarks of eDAQ Pty Ltd.&lt;br /&gt;
Windows XP, Vista, and Windows 7, Windows 8 and Windows 10 are trademarks of Microsoft Corporation.&lt;br /&gt;
This document is Copyright © July 2015. This document, or sections thereof, may be copied by the owners or users of an eDAQ Quad MF isoPod for their private use. Otherwise no part of this document may be&lt;br /&gt;
reproduced by any means without the prior written permission of eDAQ Pty Ltd.&lt;br /&gt;
&lt;br /&gt;
=== Responsibilities ===&lt;br /&gt;
&lt;br /&gt;
You and any others using any eDAQ product agree to use it in a sensible manner for purposes for which it is suited, and agree to take responsibility for their actions and the results of their actions. If problems arise with an eDAQ product, eDAQ will make all reasonable efforts to fix them. This service may incur a charge, depending on the nature of the problems, and is subject to the other conditions in this Agreement.&lt;br /&gt;
&lt;br /&gt;
=== Hardware Warranty ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd warrants this device, to be free of defects in material and workmanship for three years from the date of purchase. Note that this does NOT include external cables and electrodes that are subject to 'wear and tear' and manufacturing defects should be reported within 90 days of purchase. eDAQ Pty Ltd will repair or replace defective equipment as appropriate. To obtain a warranty repair/replacement you must first notify us before return of the instrument and we will issue you with a RAN (return authorisation number). You must ship the defective product at your expense. We will pay return shipping. The product should be packed safely (preferably in its original packaging) and have the RAN on the shipping label. Returns sent without a RAN may be refused delivery.&lt;br /&gt;
&lt;br /&gt;
This warranty does not cover hardware that has:&lt;br /&gt;
:• been modified by the user in any way;&lt;br /&gt;
:• been subjected to unusual physical, electrical, or environmental stress. This includes damage due to faulty power sockets, inadequate earthing, or power spikes or surges;&lt;br /&gt;
:• been damaged because of incorrect wiring to ancillary equipment, or because of substandard, connectors or cables; or&lt;br /&gt;
:• had the original identification marks removed or altered.&lt;br /&gt;
&lt;br /&gt;
=== Software License ===&lt;br /&gt;
&lt;br /&gt;
You have the non-exclusive right to use the supplied eDAQ software (Sequencer, Chart etc). Your employees or students, for example, are entitled to use it, provided they adhere to this agreement. &lt;br /&gt;
Each separate purchase of the eDAQ software licenses it to be used on two computers, more than two copies must not be used simultaneously. Departmental/company licences are available if you wish to run more than two copies simultaneously.&lt;br /&gt;
&lt;br /&gt;
=== Technical Support ===&lt;br /&gt;
&lt;br /&gt;
Please register your unit to receive technical support.&lt;br /&gt;
&lt;br /&gt;
Technical assistance is available via email. Please describe the problem with as much detail as possible. Include a small example data file, if appropriate. Please also state:&lt;br /&gt;
: • the model and serial number of your EDAQ system.&lt;br /&gt;
: • the type of computer and operating system being used (for example Windows XP, Vista, Windows 7, 8, or 10)&lt;br /&gt;
: • the software version you are using (for example Chart v5.5.2)&lt;br /&gt;
&lt;br /&gt;
We endeavor to answer all your questions, but in some cases, for example where the problem relates to the other equipment that you are using, a nominal fee may be charged.&lt;br /&gt;
&lt;br /&gt;
=== Jurisdiction ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd is bound by the laws of New South Wales in Australia, and any proceedings shall be heard by the Supreme Court of New South Wales in Australia.&lt;br /&gt;
&lt;br /&gt;
=== Disclaimer ===&lt;br /&gt;
&lt;br /&gt;
eDAQ reserves the right to alter specifications of hardware and software without notice. No liability can be accepted for consequential damages resulting from use of eDAQ products.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3991</id>
		<title>ER430 Manual</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3991"/>
				<updated>2015-08-06T07:46:08Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Communication */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;br /&gt;
== Introduction ==&lt;br /&gt;
[[File:ER430SmallPanels.jpg|thumb|upright=2|right|'''Figure 1.''' ER430 HV Sequencer front and back panels]]&lt;br /&gt;
This manual is intended to allow the user to install, check and run the ER430 HV Sequencer. It provides detailed information on the system and its operation. Please read this manual carefully prior to beginning operation.&lt;br /&gt;
&lt;br /&gt;
The ER430 High Voltage Sequencer provides the following functions:&lt;br /&gt;
::• Four independent programmable metered high voltage (HV) supplies.&lt;br /&gt;
::• Safety Interlock system&lt;br /&gt;
::• Software that allows arbitrary sequences of voltages to be generated&lt;br /&gt;
&lt;br /&gt;
== Checking the Instrument ==&lt;br /&gt;
Before you begin working with the device, you should check:&lt;br /&gt;
:• that the contents of the package you received match the packing list&lt;br /&gt;
:• for any sign of physical damage that might have occurred during transit.&lt;br /&gt;
If you find a problem, please contact your [http://www.edaq.com/edaq-distributors eDAQ distributor] or agent immediately.&lt;br /&gt;
&lt;br /&gt;
== Safety First ==&lt;br /&gt;
&lt;br /&gt;
This equipment generates high voltages of up to 3000 V DC at currents of up to 200 µA. Making contact with such voltages can be extremely dangerous.&lt;br /&gt;
&lt;br /&gt;
Ensure that the high voltage (HV) circuits are housed in an insulated enclosure fitted with an Interlock safety circuit and with no manual access to HV circuits while circuits are alive.&lt;br /&gt;
&lt;br /&gt;
Safety precautions:&lt;br /&gt;
::• Ensure that the safety interlock circuit is connected to the HV Sequencer and is only active and enabled when no accidental access to High Voltage circuits can be made.&lt;br /&gt;
::• Wear rubber soled footwear&lt;br /&gt;
::• Ensure the floor and bench top are dry&lt;br /&gt;
::• Stand on a rubber mat when in the vicinity of high voltages&lt;br /&gt;
&lt;br /&gt;
The ER430 features design precautions to ensure that there is no accidental application of high voltages. These include automatic shutdown in the event of voltage or current overloads . This will in some circumstances prevent the unit from operating. In these cases check all settings and safety interlocks carefully before resuming the experiment.&lt;br /&gt;
&lt;br /&gt;
=== What is an Interlock ===&lt;br /&gt;
&lt;br /&gt;
An interlock is a mechanical or electrical system that prevents the inadvertent operation of of an instrument.&lt;br /&gt;
&lt;br /&gt;
In the case of the  ER430 HV Sequencer this is achieved by using a switch located in the enclosure in which high voltages are active.  This switch is connected via a cable to the front panel INTERLOCK BNC in such a way that the switch is only closed when no access is available to the High voltages inside the enclosure.&lt;br /&gt;
&lt;br /&gt;
For example with the eDAQ supplied ET225 Micronit Chip Electrophoresis Platform, high voltages can only be applied when the top cover is in place.  This is detected and the interlock switch enabled to allow the application of high voltages.&lt;br /&gt;
&lt;br /&gt;
If the user is providing the MicroChip enclosure then it is the user’s responsibility to provide the required interlock function.&lt;br /&gt;
&lt;br /&gt;
To test the Interlock function it is sufficient to apply a short circuit across the INTERLOCK BNC input pins.  This should only be done with no connections to the High Voltage input connectors.&lt;br /&gt;
ER430 &lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
System indicators as shown in the preceding diagram provide a direct indication of system operation that reflects the state of the internal hardware.  These indicators will assist you in monitoring system operation and in diagnosing problems – study them carefully:  &lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED: Amber LED&lt;br /&gt;
	FLASHING = Interlock open, unit disarmed, arming not enabled.&lt;br /&gt;
	OFF = Interlock in place and enabled, unit can be ARMED.&lt;br /&gt;
	ON = Interlock in place, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
SYSTEM STATUS LED: RGB LED (Multicoloured)&lt;br /&gt;
GREEN when “on line” and ready as a Master&lt;br /&gt;
BLUE when ready as a Slave&lt;br /&gt;
&lt;br /&gt;
METER FUNCTION LED: RGB LED&lt;br /&gt;
GREEN:  Safe (disconnected) &lt;br /&gt;
YELLOW:  Current Mode&lt;br /&gt;
BLUE:  Voltage mode&lt;br /&gt;
&lt;br /&gt;
HV STATUS: RED LED&lt;br /&gt;
OFF: supply disconnected&lt;br /&gt;
ON: supply connected and active.&lt;br /&gt;
&lt;br /&gt;
Notes: &lt;br /&gt;
#On power up the system performs a startup test and flashes the front panel LEDs through the various colors available for display.&lt;br /&gt;
# In some cases where the HV supply needs to be used in proximity to light sensitive detectors it is possible to optionally turn off all the LEDs to maintain low background illumination.&lt;br /&gt;
 &lt;br /&gt;
== Hardware Installation ==&lt;br /&gt;
'''ATTENTION:''' When installing the system for the first time ALWAYS perform software installation before connecting the hardware units.  This ensures that the correct drivers are installed &lt;br /&gt;
 &lt;br /&gt;
After carrying out the software installation described in the next section, perform the following Hardware installation procedure. It will confirm that:&lt;br /&gt;
::• That safety interlocks are in place and functioning correctly&lt;br /&gt;
::• The unit can be armed and disarmed&lt;br /&gt;
&lt;br /&gt;
Operation:&lt;br /&gt;
::• '''Safety first''' Connect the unit to a good ground using the terminal post on the rear of the unit.&lt;br /&gt;
::• Connect the unit to the 12V DC mains power pack.&lt;br /&gt;
::• Connect the unit to the PC using the USB cable provided.&lt;br /&gt;
::• Turn Power on.&lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED will flash if interlock is not enabled.&lt;br /&gt;
&lt;br /&gt;
HV Status LEDs: Off (no high voltage output)&lt;br /&gt;
&lt;br /&gt;
STATUS LEDs: Green&lt;br /&gt;
&lt;br /&gt;
=== TEST INTERLOCK Function ===&lt;br /&gt;
&lt;br /&gt;
This function can be tested without any software running:&lt;br /&gt;
::• The INTERLOCK LED will initially be flashing.&lt;br /&gt;
::• Connect a short circuit to the INTERLOCK BNC.&lt;br /&gt;
::• INTERLOCK LED will turn OFF.&lt;br /&gt;
::• Press the ARM Push Button for approximately 1 to 2 seconds.  You should hear a beep, warning you that the HV outputs have been armed (enabled) and the INTERLOCK LED will turn ON.&lt;br /&gt;
::• At this point all HV supplies are still inactive but are in a state where they can be set and controlled by the Sequencer Application software.&lt;br /&gt;
::• Pressing the Arm button again will DISARM the HV Sequencer, and the INTEROCK LED will turn off.&lt;br /&gt;
&lt;br /&gt;
A momentary push on  the Arm button will disable all the HV outputs of the Sequencer.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== INTERLOCK features ===&lt;br /&gt;
The system is provided with a number of safety features or Interlocks:&lt;br /&gt;
::• Chip adapter interlock:  The chip adapter used should provide a safety contact interlock to indicate that the microchip adapter is safe for use.  This interlock is a contact closure switch, which is closed when the HV circuit is fully enclosed and protected from user access. This interlock is connected to the front panel Interlock BNC and indicates to the ER430 that it is safe to arm the system.&lt;br /&gt;
::• USB Present:  The system cannot be ARMED without an active USB connection&lt;br /&gt;
::• Software Control: Once the system is ARMED High Voltages can only be applied under software control.&lt;br /&gt;
::• ARM circuit: prior to applying HV to an external circuit the system must be armed by the user by depressing the front panel ARM push button for approximately 2 seconds.&lt;br /&gt;
::• DISARM: The system can be disarmed by a momentary push of the ARM button.&lt;br /&gt;
::• Power Overloads:  the circuit detects power overloads and situations that lead to the generation of arcs (sparks).  The system will switch itself off in such circumstances and in such circumstances may require to be reinitiated with power being turned on Off and On.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION:'''  Do not disconnect HV leads by hand while High voltages are present – this is extremely dangerous and can cause harmful arcs to be generated. To disable power use the ARM/DISARM front panel button or the software’s Disarm or Disconnect menu items&lt;br /&gt;
&lt;br /&gt;
You are now ready to operate the Sequencer software which will allow you to generate and output a series of high voltage pulses and ramps.&lt;br /&gt;
&lt;br /&gt;
== Software Installation &amp;amp; Operation ==&lt;br /&gt;
&lt;br /&gt;
=== Installing the HV Sequencer software ===&lt;br /&gt;
Insert the HV Sequencer installation USB stick into your computer.  It is recommended to install the software before plugging in the hardware, as it ensures the drivers are correctly installed.&lt;br /&gt;
&lt;br /&gt;
The eDAQ Sequencer Setup Wizard will display a start-up screen; follow the prompts to install the software.&lt;br /&gt;
      Start up screen&lt;br /&gt;
			    Final Start up screen&lt;br /&gt;
&lt;br /&gt;
=== eDAQ Sequencer Overview ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Sequencer is a Windows application that provides the means to setup a series of steps that are executed under computer control.  The following functions are provided:&lt;br /&gt;
&lt;br /&gt;
System setup and sequence entry: The software identifies system configuration on startup and allows the operating parameters to be set immediately.&lt;br /&gt;
&lt;br /&gt;
Table driven Sequence: A time based table is filled out, specifying that the operations to be performed in sequence.  This includes setting of HV supplies to new voltages, trigger and digital I/O line functions. The following sequence operations are implemented: &lt;br /&gt;
&lt;br /&gt;
Time: set to xxxx seconds&lt;br /&gt;
Meter 1&amp;amp;2: Disconnect, Read V, Read I&lt;br /&gt;
Output1&amp;amp;2: Set V=xxxx (V and I monitored), Read V, Read I&lt;br /&gt;
Digital Out: Low/Open, High/Closed, Short Pulse, Long Pulse&lt;br /&gt;
Special commands: Wait for trigger, Wait for Arming, Go Safe&lt;br /&gt;
New functions can be readily added to meet customer requirements&lt;br /&gt;
&lt;br /&gt;
Digital outputs can be used to control external devices or the recording of data in an ecorder.&lt;br /&gt;
&lt;br /&gt;
Monitoring: Once a sequence is started the user is able to observe the progress of the sequence on the sequence table.  Values of HV supply voltages and currents are displayed during operation.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
 === HV Sequencer Main Window ===&lt;br /&gt;
&lt;br /&gt;
  &lt;br /&gt;
=== Communication ===&lt;br /&gt;
&lt;br /&gt;
The HV sequencer uses a virtual USB serial communications (COM) port.  When the ER430 hardware is first attached to USB, a free COM port number is automatically assigned by Windows.  That COM port will be then used every time that unit is plugged in again.&lt;br /&gt;
&lt;br /&gt;
Note:  the first time you connect the system to the computer it may take some time for the system to identify the HV sequencer device driver and install it.  You will be notified when the device is ready.&lt;br /&gt;
&lt;br /&gt;
The first time you use the sequencer software, you need to specify the COM port that the hardware has been assigned.  Select the Preferences option in the File menu, then choose your HV Sequencer in the list at the top – see screen shot below. This preference is automatically saved for future use&lt;br /&gt;
&lt;br /&gt;
  Preferences panel&lt;br /&gt;
&lt;br /&gt;
If you are uncertain about which COM port to assign use, the Serial Port Monitor application can help identify the COM port assigned to the HV sequencer. This small application is included on the HV Sequencer installer USB stick, and can also be downloaded from the eDAQ Utilities and Tools download webpage [http://www.edaq.com/utilities_tools.php www.edaq.com/utilities_tools.php]&lt;br /&gt;
&lt;br /&gt;
The serial port monitor runs as an icon in the notification area.  Clicking on it will show a list of eDAQ COM port devices attached to your computer.&lt;br /&gt;
&lt;br /&gt;
The other Preference options set the digital output type, and provide control over front panel lights in situations where light pollution needs to be kept to a minimum.&lt;br /&gt;
&lt;br /&gt;
Check if you have installed an interlock as described previously.  The INTERLOCK LED should be OFF indicating that the INTERLOCK is in place.&lt;br /&gt;
    &lt;br /&gt;
&lt;br /&gt;
Click the Online in the menu bar to attach the selected ER430 unit to the Sequencer application. &lt;br /&gt;
&lt;br /&gt;
Click the Offline in the menu bar to disconnect the selected ER430 unit from the Sequencer application.&lt;br /&gt;
&lt;br /&gt;
=== Disarming and Interlock Test ===&lt;br /&gt;
&lt;br /&gt;
Press and hold the red ARM button to arm the unit.  As before, the unit will beep and arm itself.  This will also be shown in the software’s display.&lt;br /&gt;
&lt;br /&gt;
You can now disarm the unit by either:&lt;br /&gt;
::• Pressing the red ARM button again&lt;br /&gt;
::• Clicking “Disarm” in the top-right of the software window.&lt;br /&gt;
&lt;br /&gt;
While the unit is armed, you can test the safety interlock by removing the short-circuit from the BNC connector.  The unit should immediately disarm itself, disconnecting the outputs, and turning off any applied voltages.&lt;br /&gt;
&lt;br /&gt;
=== Manual Settings ===&lt;br /&gt;
After arming the unit, click on the More… button to display the controls for making immediate changes to the unit.&lt;br /&gt;
&lt;br /&gt;
The right hand side of the HV Sequencer setup panel provides the means to manually set meter functions, output voltages, and the digital outputs’ states.  Make some selections, and then click on Set.  The ER430 hardware will immediately apply the settings you have chosen, and the software will display your choices, along with readings of current and/or voltage.&lt;br /&gt;
&lt;br /&gt;
At this point  the system will indicate the voltages set and currents measured.  Since no loads are yet connected, the currents will be very near zero. &lt;br /&gt;
&lt;br /&gt;
=== Setup panel ===&lt;br /&gt;
&lt;br /&gt;
At any time, pressing the Disarm button in the top-right hand corner of the Main Window or the red button on the front panel of the ER430 will disarm the unit and make it safe.  &lt;br /&gt;
&lt;br /&gt;
After disarming, you must press and hold the red button (as before) to re-arm it.  The software can not re-arm the device.&lt;br /&gt;
&lt;br /&gt;
Outputs let you control the digital outputs of the unit.  In the preference you can set Output configuration as contact closure, or TTL.&lt;br /&gt;
HV Sequences&lt;br /&gt;
The lower area of the Setup panel provides the means to define a “program” or “sequence” to run. This consists of a number of timed steps, each of which can update the state of one or more of the individual functions or outputs.  There are also some “special” commands that can be carried out. Unused connections can have the width of their columns reduced by dragging their column separator.&lt;br /&gt;
&lt;br /&gt;
All changes on a step happen simultaneously (within 2 milliseconds).&lt;br /&gt;
   Setup screen with an example&lt;br /&gt;
&lt;br /&gt;
Here is another example program:&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
If a step doesn’t have anything entered in its box, the output will remain unchanged from its previous setting.&lt;br /&gt;
&lt;br /&gt;
A time of “0” means “immediately upon starting”, and the times are cumulative, measured from when the sequence was started,  i.e.: the delay between the first four of the lines above is 5, 3, and 4 seconds respectively.&lt;br /&gt;
&lt;br /&gt;
It is recommended to have the first row setting every output to a known state, in case the previous run was stopped part-way through, leaving the unit in an unknown state.&lt;br /&gt;
&lt;br /&gt;
When the program finishes, the unit will be left in whatever state it was at the end.  It will not automatically disconnect or disarm the outputs, unless explicitly told to do so.&lt;br /&gt;
The Meter channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal (LED GREEN)&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE)&lt;br /&gt;
Read I:  Current Meter connection (LED YELLOW)&lt;br /&gt;
The Output channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal.&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE).&lt;br /&gt;
Read I: Current meter connection (LED YELLOW)&lt;br /&gt;
Set V: Set the voltage to the value entered in the second column – In this mode the Voltage indicated will be the actual voltage produced within 1%. (LED RED)&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
Digital outputs can be set to:&lt;br /&gt;
Low/Open: Output goes low or open, as per the “digital output mode” setting in Preferences. &lt;br /&gt;
High/Closed: Output goes high or closed.&lt;br /&gt;
&lt;br /&gt;
The type of digital output, TTL or Contact Closure, is set from the Preferences dialog in the File menu.&lt;br /&gt;
&lt;br /&gt;
Special is a special function to be performed.  You can either:&lt;br /&gt;
::• Disarm: Disconnect HV supplies, and stop the program, or&lt;br /&gt;
::• Wait for trigger: Pause, and wait for a high/close on the rear panel’s green connector “Trigger” pins.&lt;br /&gt;
&lt;br /&gt;
Simple editing commands are available on the Edit menu.  The option to Always show the slave will force the display of the second control panel and additional program columns, even if a second unit is not attached.&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
Programs can be saved and loaded using the menu options in the File menu. &lt;br /&gt;
&lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
Once you are satisfied with your program, click the Run button in the menu bar.  The software will step through the program, executing each step at the given time after starting.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Pause button can be used to pause running of the program.  The Run button changes to a Resume button, which you can click to continue execution.&lt;br /&gt;
Stop will stop execution, but it will leave the unit in the current state, with whatever voltages selected still being output.&lt;br /&gt;
The Disarm button will stop any running program and put the ER430 hardware into a safe state.&lt;br /&gt;
Various fault and safety switch conditions will also force a disarming (and termination of program), including:&lt;br /&gt;
•	USB cable being removed&lt;br /&gt;
•	Front panel safety interlock opened/removed&lt;br /&gt;
•	Front panel red button being pressed&lt;br /&gt;
•	When operating with a slave unit, disconnection from the slave unit&lt;br /&gt;
&lt;br /&gt;
=== Modes of Operation ===&lt;br /&gt;
&lt;br /&gt;
==== General ====&lt;br /&gt;
::• Disarmed/Safe – High voltages and meters disconnected  &lt;br /&gt;
::• Armed- High voltages are active and available for connection to external circuit.&lt;br /&gt;
&lt;br /&gt;
==== Programmable HV power supplies ====&lt;br /&gt;
Output Voltage:  Adjustable from ±200V to ±3000V at up to 200µA. &lt;br /&gt;
Output Polarity:  Positive or Negative with respect to the common ground potential&lt;br /&gt;
&lt;br /&gt;
==== Operating Modes ====&lt;br /&gt;
::• O/C mode: Open Circuit by disconnection with high voltage relay.&lt;br /&gt;
::• Voltage Mode: High voltage output mode with current and voltage monitoring&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 10 Meohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring&lt;br /&gt;
&lt;br /&gt;
==== Meters ====&lt;br /&gt;
::• O/C mode: Open Circuit achieved by disconnection with high voltage relay&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 100 Mohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring &lt;br /&gt;
&lt;br /&gt;
By combining the HV power supplies and meters it is possible to setup the conditions which load the sample into the separation channel and then apply the appropriate voltages to cause separation and detection of the sample components as shown in the example.&lt;br /&gt;
&lt;br /&gt;
=== Typical Installation ===&lt;br /&gt;
 &lt;br /&gt;
 &lt;br /&gt;
== ER430 HV Hardware ==&lt;br /&gt;
&lt;br /&gt;
=== ER430 HV Channel Block Diagram ===&lt;br /&gt;
A Block diagram of a HV supply channel is shown below; there are four identical HV channels in each ER430unit:&lt;br /&gt;
 &lt;br /&gt;
=== ER430 Meter Channel block diagram ===&lt;br /&gt;
&lt;br /&gt;
=== Green Connector Pin Numbers ===&lt;br /&gt;
&lt;br /&gt;
ER430 HV Sequencer “green” connector Pin functions&lt;br /&gt;
&lt;br /&gt;
:: 1	TRIG +	TTL  IN	11	HV 1 E	HV VOLTAGE  MONITOR 1&lt;br /&gt;
:: 2	TRIG -	TTL COM	12	HV 1 I	HV CURRENT MONITOR 1&lt;br /&gt;
:: 3	HV4  E	HV VOLTAGE  MONITOR 4	13	CTL1 +	DIGITAL  IN/OUT 1&lt;br /&gt;
:: 4	HV4  I	HV CURRENT MONITOR 4	14	CTL1 -	DIGITAL COM&lt;br /&gt;
:: 5	COM	COMMON	15	CTL2 +	DIGITAL  IN/OUT 2&lt;br /&gt;
:: 6	HV3 E	HV VOLTAGE  MONITOR 3	16	CTL2 -	DIGITAL COM&lt;br /&gt;
:: 7	HV3  I	HV CURRENT MONITOR 3	17	CTL3+	DIGITAL  IN/OUT 3&lt;br /&gt;
:: 8	HV 2 E	HV VOLTAGE  MONITOR 2	18	CTL3 -	DIGITAL COM&lt;br /&gt;
:: 9	HV 2  I	HV CURRENT MONITOR 2	19	CTL4 +	DIGITAL  IN/OUT 4&lt;br /&gt;
:: 10	COM	COMMON	20	CTL4 -	DIGITAL COM&lt;br /&gt;
&lt;br /&gt;
Notes:&lt;br /&gt;
# Digital I/O pins are implemented as contact closure or TTL outputs, software selectable&lt;br /&gt;
# Trigger input can be a contact closure or TTL input&lt;br /&gt;
# HV VOLTAGE  MONITOR scale factor: 500mV/kV&lt;br /&gt;
# HV Current Monitor Scale factor: 100mV/mA&lt;br /&gt;
&lt;br /&gt;
== Specifications==&lt;br /&gt;
&lt;br /&gt;
=== High Voltage Output and Mode Options ===&lt;br /&gt;
&lt;br /&gt;
::• Channels: 4&lt;br /&gt;
::• Model: UR3*&lt;br /&gt;
::• Maximum Voltage Setting: ±3000 V&lt;br /&gt;
::• Minimum Voltage Setting: ±200 V&lt;br /&gt;
::• Current: ±200 µA max&lt;br /&gt;
::• Ripple: 0.1%		&lt;br /&gt;
::• Operating Modes: Applied voltage, Open Circuit (O/C), and Short Circuit (S/C)		&lt;br /&gt;
::• Load regulation: &amp;lt;2% specified for 20-90% full load: &lt;br /&gt;
::• Rise and Fall times: &amp;lt;5 ms specified for changes within the same polarity regime&lt;br /&gt;
::• Mode Change: &amp;lt;100ms due to relay operations, safety and software latency&lt;br /&gt;
	&lt;br /&gt;
Note: Output is referred to system common (Case Ground)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Safety Features ===&lt;br /&gt;
An interlock is provided on&lt;br /&gt;
::• the mechanical case to ensure that no voltages are present with the case open unless authorized maintenance is in progress.  &lt;br /&gt;
::• the microchip environment to ensure that accidental contact is not made with the high voltages.&lt;br /&gt;
&lt;br /&gt;
The Arm/disarm switch needs to be held for 2 seconds to arm the system and allow high voltages to become active.  Any short contact on the ARM switch will disarm the system.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION''': It is the responsibility of the user to ensure that adequate protection is provided on the equipment provided by the user. eDAQ provides microfluidic chip adaptors with appropriate interlock features.&lt;br /&gt;
&lt;br /&gt;
=== Meter Functions ===&lt;br /&gt;
&lt;br /&gt;
::• Voltage Range:	±3000 V&lt;br /&gt;
::• Voltage Resolution: 1 V&lt;br /&gt;
::• Current Range: ±200 µA&lt;br /&gt;
::• Current resolution: 1 µA&lt;br /&gt;
::• Displayed resolution limited to 1 unit&lt;br /&gt;
&lt;br /&gt;
=== Communications and Inputs and outputs terminals ===&lt;br /&gt;
&lt;br /&gt;
::• Daisy Chain connectors: Twin DB9 connectors allow two (2) ER430 units to be daisy chained together.&lt;br /&gt;
::• USB Port:  Compatible with USB1 &amp;amp; USB 2 and provides, communications facility to PC’s&lt;br /&gt;
::• Output and Meters front panel connectors:  SHV (Safe High Voltage)  type &lt;br /&gt;
::• 20 Way 3.5mm Green screw terminal: &lt;br /&gt;
:::: - Four Digital I/O lines&lt;br /&gt;
:::: - Trigger TTL or CC&lt;br /&gt;
:::: - Four Voltage Monitor signals&lt;br /&gt;
:::: - FourCurrent  Monitor signals.&lt;br /&gt;
::• System/Chassis Earth terminal: 4 mm screw terminal.&lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
&lt;br /&gt;
The following LED front panel displays are available:&lt;br /&gt;
&lt;br /&gt;
::•  System Status (RGB LED)&lt;br /&gt;
::: GREEN when “on line” &lt;br /&gt;
&lt;br /&gt;
::• Interlock (amber LED)&lt;br /&gt;
::: FLASHING = Interlock open, unit disarmed, arming not allowed.&lt;br /&gt;
::: OFF = Interlock OK, unit disarmed&lt;br /&gt;
::: ON = Interlock OK, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
::• Meter Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (disconnected) &lt;br /&gt;
:::: YELLOW = Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (supply disconnected) &lt;br /&gt;
:::: YELLOW =  Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Status  (RGB LED)&lt;br /&gt;
:::: OFF = supply disconnected&lt;br /&gt;
:::: ON = supply connected and active.&lt;br /&gt;
&lt;br /&gt;
=== Physical ===&lt;br /&gt;
::• Dimensions (w x h x d): 200 x 65 x 250 mm (7.9 x 2.6 x 9.8 inch)&lt;br /&gt;
::• Weight: 3.00 kg packed&lt;br /&gt;
::• Operating temperature: 0 - 35ºC&lt;br /&gt;
::• Humidity: 10 to 80% non condensing &lt;br /&gt;
::• Power:  9 - 16 V @ 2 A maximum supplied by mains powered AC/DC converter (supplied)&lt;br /&gt;
&lt;br /&gt;
== Legal and Warranty ==&lt;br /&gt;
&lt;br /&gt;
=== Trademarks and Copyright ===&lt;br /&gt;
Sequencer, HV Sequencer, and Chart are trademarks of eDAQ Pty Ltd.&lt;br /&gt;
Windows XP, Vista, and Windows 7, Windows 8 and Windows 10 are trademarks of Microsoft Corporation.&lt;br /&gt;
This document is Copyright © July 2015. This document, or sections thereof, may be copied by the owners or users of an eDAQ Quad MF isoPod for their private use. Otherwise no part of this document may be&lt;br /&gt;
reproduced by any means without the prior written permission of eDAQ Pty Ltd.&lt;br /&gt;
&lt;br /&gt;
=== Responsibilities ===&lt;br /&gt;
&lt;br /&gt;
You and any others using any eDAQ product agree to use it in a sensible manner for purposes for which it is suited, and agree to take responsibility for their actions and the results of their actions. If problems arise with an eDAQ product, eDAQ will make all reasonable efforts to fix them. This service may incur a charge, depending on the nature of the problems, and is subject to the other conditions in this Agreement.&lt;br /&gt;
&lt;br /&gt;
=== Hardware Warranty ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd warrants this device, to be free of defects in material and workmanship for three years from the date of purchase. Note that this does NOT include external cables and electrodes that are subject to 'wear and tear' and manufacturing defects should be reported within 90 days of purchase. eDAQ Pty Ltd will repair or replace defective equipment as appropriate. To obtain a warranty repair/replacement you must first notify us before return of the instrument and we will issue you with a RAN (return authorisation number). You must ship the defective product at your expense. We will pay return shipping. The product should be packed safely (preferably in its original packaging) and have the RAN on the shipping label. Returns sent without a RAN may be refused delivery.&lt;br /&gt;
&lt;br /&gt;
This warranty does not cover hardware that has:&lt;br /&gt;
:• been modified by the user in any way;&lt;br /&gt;
:• been subjected to unusual physical, electrical, or environmental stress. This includes damage due to faulty power sockets, inadequate earthing, or power spikes or surges;&lt;br /&gt;
:• been damaged because of incorrect wiring to ancillary equipment, or because of substandard, connectors or cables; or&lt;br /&gt;
:• had the original identification marks removed or altered.&lt;br /&gt;
&lt;br /&gt;
=== Software License ===&lt;br /&gt;
&lt;br /&gt;
You have the non-exclusive right to use the supplied eDAQ software (Sequencer, Chart etc). Your employees or students, for example, are entitled to use it, provided they adhere to this agreement. &lt;br /&gt;
Each separate purchase of the eDAQ software licenses it to be used on two computers, more than two copies must not be used simultaneously. Departmental/company licences are available if you wish to run more than two copies simultaneously.&lt;br /&gt;
&lt;br /&gt;
=== Technical Support ===&lt;br /&gt;
&lt;br /&gt;
Please register your unit to receive technical support.&lt;br /&gt;
&lt;br /&gt;
Technical assistance is available via email. Please describe the problem with as much detail as possible. Include a small example data file, if appropriate. Please also state:&lt;br /&gt;
: • the model and serial number of your EDAQ system.&lt;br /&gt;
: • the type of computer and operating system being used (for example Windows XP, Vista, Windows 7, 8, or 10)&lt;br /&gt;
: • the software version you are using (for example Chart v5.5.2)&lt;br /&gt;
&lt;br /&gt;
We endeavor to answer all your questions, but in some cases, for example where the problem relates to the other equipment that you are using, a nominal fee may be charged.&lt;br /&gt;
&lt;br /&gt;
=== Jurisdiction ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd is bound by the laws of New South Wales in Australia, and any proceedings shall be heard by the Supreme Court of New South Wales in Australia.&lt;br /&gt;
&lt;br /&gt;
=== Disclaimer ===&lt;br /&gt;
&lt;br /&gt;
eDAQ reserves the right to alter specifications of hardware and software without notice. No liability can be accepted for consequential damages resulting from use of eDAQ products.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3990</id>
		<title>ER430 Manual</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3990"/>
				<updated>2015-08-06T07:44:31Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Green Connector Pin Numbers */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;br /&gt;
== Introduction ==&lt;br /&gt;
[[File:ER430SmallPanels.jpg|thumb|upright=2|right|'''Figure 1.''' ER430 HV Sequencer front and back panels]]&lt;br /&gt;
This manual is intended to allow the user to install, check and run the ER430 HV Sequencer. It provides detailed information on the system and its operation. Please read this manual carefully prior to beginning operation.&lt;br /&gt;
&lt;br /&gt;
The ER430 High Voltage Sequencer provides the following functions:&lt;br /&gt;
::• Four independent programmable metered high voltage (HV) supplies.&lt;br /&gt;
::• Safety Interlock system&lt;br /&gt;
::• Software that allows arbitrary sequences of voltages to be generated&lt;br /&gt;
&lt;br /&gt;
== Checking the Instrument ==&lt;br /&gt;
Before you begin working with the device, you should check:&lt;br /&gt;
:• that the contents of the package you received match the packing list&lt;br /&gt;
:• for any sign of physical damage that might have occurred during transit.&lt;br /&gt;
If you find a problem, please contact your [http://www.edaq.com/edaq-distributors eDAQ distributor] or agent immediately.&lt;br /&gt;
&lt;br /&gt;
== Safety First ==&lt;br /&gt;
&lt;br /&gt;
This equipment generates high voltages of up to 3000 V DC at currents of up to 200 µA. Making contact with such voltages can be extremely dangerous.&lt;br /&gt;
&lt;br /&gt;
Ensure that the high voltage (HV) circuits are housed in an insulated enclosure fitted with an Interlock safety circuit and with no manual access to HV circuits while circuits are alive.&lt;br /&gt;
&lt;br /&gt;
Safety precautions:&lt;br /&gt;
::• Ensure that the safety interlock circuit is connected to the HV Sequencer and is only active and enabled when no accidental access to High Voltage circuits can be made.&lt;br /&gt;
::• Wear rubber soled footwear&lt;br /&gt;
::• Ensure the floor and bench top are dry&lt;br /&gt;
::• Stand on a rubber mat when in the vicinity of high voltages&lt;br /&gt;
&lt;br /&gt;
The ER430 features design precautions to ensure that there is no accidental application of high voltages. These include automatic shutdown in the event of voltage or current overloads . This will in some circumstances prevent the unit from operating. In these cases check all settings and safety interlocks carefully before resuming the experiment.&lt;br /&gt;
&lt;br /&gt;
=== What is an Interlock ===&lt;br /&gt;
&lt;br /&gt;
An interlock is a mechanical or electrical system that prevents the inadvertent operation of of an instrument.&lt;br /&gt;
&lt;br /&gt;
In the case of the  ER430 HV Sequencer this is achieved by using a switch located in the enclosure in which high voltages are active.  This switch is connected via a cable to the front panel INTERLOCK BNC in such a way that the switch is only closed when no access is available to the High voltages inside the enclosure.&lt;br /&gt;
&lt;br /&gt;
For example with the eDAQ supplied ET225 Micronit Chip Electrophoresis Platform, high voltages can only be applied when the top cover is in place.  This is detected and the interlock switch enabled to allow the application of high voltages.&lt;br /&gt;
&lt;br /&gt;
If the user is providing the MicroChip enclosure then it is the user’s responsibility to provide the required interlock function.&lt;br /&gt;
&lt;br /&gt;
To test the Interlock function it is sufficient to apply a short circuit across the INTERLOCK BNC input pins.  This should only be done with no connections to the High Voltage input connectors.&lt;br /&gt;
ER430 &lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
System indicators as shown in the preceding diagram provide a direct indication of system operation that reflects the state of the internal hardware.  These indicators will assist you in monitoring system operation and in diagnosing problems – study them carefully:  &lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED: Amber LED&lt;br /&gt;
	FLASHING = Interlock open, unit disarmed, arming not enabled.&lt;br /&gt;
	OFF = Interlock in place and enabled, unit can be ARMED.&lt;br /&gt;
	ON = Interlock in place, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
SYSTEM STATUS LED: RGB LED (Multicoloured)&lt;br /&gt;
GREEN when “on line” and ready as a Master&lt;br /&gt;
BLUE when ready as a Slave&lt;br /&gt;
&lt;br /&gt;
METER FUNCTION LED: RGB LED&lt;br /&gt;
GREEN:  Safe (disconnected) &lt;br /&gt;
YELLOW:  Current Mode&lt;br /&gt;
BLUE:  Voltage mode&lt;br /&gt;
&lt;br /&gt;
HV STATUS: RED LED&lt;br /&gt;
OFF: supply disconnected&lt;br /&gt;
ON: supply connected and active.&lt;br /&gt;
&lt;br /&gt;
Notes: &lt;br /&gt;
#On power up the system performs a startup test and flashes the front panel LEDs through the various colors available for display.&lt;br /&gt;
# In some cases where the HV supply needs to be used in proximity to light sensitive detectors it is possible to optionally turn off all the LEDs to maintain low background illumination.&lt;br /&gt;
 &lt;br /&gt;
== Hardware Installation ==&lt;br /&gt;
'''ATTENTION:''' When installing the system for the first time ALWAYS perform software installation before connecting the hardware units.  This ensures that the correct drivers are installed &lt;br /&gt;
 &lt;br /&gt;
After carrying out the software installation described in the next section, perform the following Hardware installation procedure. It will confirm that:&lt;br /&gt;
::• That safety interlocks are in place and functioning correctly&lt;br /&gt;
::• The unit can be armed and disarmed&lt;br /&gt;
&lt;br /&gt;
Operation:&lt;br /&gt;
::• '''Safety first''' Connect the unit to a good ground using the terminal post on the rear of the unit.&lt;br /&gt;
::• Connect the unit to the 12V DC mains power pack.&lt;br /&gt;
::• Connect the unit to the PC using the USB cable provided.&lt;br /&gt;
::• Turn Power on.&lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED will flash if interlock is not enabled.&lt;br /&gt;
&lt;br /&gt;
HV Status LEDs: Off (no high voltage output)&lt;br /&gt;
&lt;br /&gt;
STATUS LEDs: Green&lt;br /&gt;
&lt;br /&gt;
=== TEST INTERLOCK Function ===&lt;br /&gt;
&lt;br /&gt;
This function can be tested without any software running:&lt;br /&gt;
::• The INTERLOCK LED will initially be flashing.&lt;br /&gt;
::• Connect a short circuit to the INTERLOCK BNC.&lt;br /&gt;
::• INTERLOCK LED will turn OFF.&lt;br /&gt;
::• Press the ARM Push Button for approximately 1 to 2 seconds.  You should hear a beep, warning you that the HV outputs have been armed (enabled) and the INTERLOCK LED will turn ON.&lt;br /&gt;
::• At this point all HV supplies are still inactive but are in a state where they can be set and controlled by the Sequencer Application software.&lt;br /&gt;
::• Pressing the Arm button again will DISARM the HV Sequencer, and the INTEROCK LED will turn off.&lt;br /&gt;
&lt;br /&gt;
A momentary push on  the Arm button will disable all the HV outputs of the Sequencer.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== INTERLOCK features ===&lt;br /&gt;
The system is provided with a number of safety features or Interlocks:&lt;br /&gt;
::• Chip adapter interlock:  The chip adapter used should provide a safety contact interlock to indicate that the microchip adapter is safe for use.  This interlock is a contact closure switch, which is closed when the HV circuit is fully enclosed and protected from user access. This interlock is connected to the front panel Interlock BNC and indicates to the ER430 that it is safe to arm the system.&lt;br /&gt;
::• USB Present:  The system cannot be ARMED without an active USB connection&lt;br /&gt;
::• Software Control: Once the system is ARMED High Voltages can only be applied under software control.&lt;br /&gt;
::• ARM circuit: prior to applying HV to an external circuit the system must be armed by the user by depressing the front panel ARM push button for approximately 2 seconds.&lt;br /&gt;
::• DISARM: The system can be disarmed by a momentary push of the ARM button.&lt;br /&gt;
::• Power Overloads:  the circuit detects power overloads and situations that lead to the generation of arcs (sparks).  The system will switch itself off in such circumstances and in such circumstances may require to be reinitiated with power being turned on Off and On.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION:'''  Do not disconnect HV leads by hand while High voltages are present – this is extremely dangerous and can cause harmful arcs to be generated. To disable power use the ARM/DISARM front panel button or the software’s Disarm or Disconnect menu items&lt;br /&gt;
&lt;br /&gt;
You are now ready to operate the Sequencer software which will allow you to generate and output a series of high voltage pulses and ramps.&lt;br /&gt;
&lt;br /&gt;
== Software Installation &amp;amp; Operation ==&lt;br /&gt;
&lt;br /&gt;
=== Installing the HV Sequencer software ===&lt;br /&gt;
Insert the HV Sequencer installation USB stick into your computer.  It is recommended to install the software before plugging in the hardware, as it ensures the drivers are correctly installed.&lt;br /&gt;
&lt;br /&gt;
The eDAQ Sequencer Setup Wizard will display a start-up screen; follow the prompts to install the software.&lt;br /&gt;
      Start up screen&lt;br /&gt;
			    Final Start up screen&lt;br /&gt;
&lt;br /&gt;
=== eDAQ Sequencer Overview ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Sequencer is a Windows application that provides the means to setup a series of steps that are executed under computer control.  The following functions are provided:&lt;br /&gt;
&lt;br /&gt;
System setup and sequence entry: The software identifies system configuration on startup and allows the operating parameters to be set immediately.&lt;br /&gt;
&lt;br /&gt;
Table driven Sequence: A time based table is filled out, specifying that the operations to be performed in sequence.  This includes setting of HV supplies to new voltages, trigger and digital I/O line functions. The following sequence operations are implemented: &lt;br /&gt;
&lt;br /&gt;
Time: set to xxxx seconds&lt;br /&gt;
Meter 1&amp;amp;2: Disconnect, Read V, Read I&lt;br /&gt;
Output1&amp;amp;2: Set V=xxxx (V and I monitored), Read V, Read I&lt;br /&gt;
Digital Out: Low/Open, High/Closed, Short Pulse, Long Pulse&lt;br /&gt;
Special commands: Wait for trigger, Wait for Arming, Go Safe&lt;br /&gt;
New functions can be readily added to meet customer requirements&lt;br /&gt;
&lt;br /&gt;
Digital outputs can be used to control external devices or the recording of data in an ecorder.&lt;br /&gt;
&lt;br /&gt;
Monitoring: Once a sequence is started the user is able to observe the progress of the sequence on the sequence table.  Values of HV supply voltages and currents are displayed during operation.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
 === HV Sequencer Main Window ===&lt;br /&gt;
&lt;br /&gt;
  &lt;br /&gt;
=== Communication ===&lt;br /&gt;
&lt;br /&gt;
The HV sequencer uses a virtual USB serial communications (COM) port.  When the ER430 hardware is first attached to USB, a free COM port number is automatically assigned by Windows.  That COM port will be then used every time that unit is plugged in again.&lt;br /&gt;
&lt;br /&gt;
Note:  the first time you connect the system to the computer it may take some time for the system to identify the HV sequencer device driver and install it.  You will be notified when the device is ready.&lt;br /&gt;
&lt;br /&gt;
The first time you use the sequencer software, you need to specify the COM port that the hardware has been assigned.  Select the Preferences option in the File menu, then choose your HV Sequencer in the list at the top – see screen shot below. This preference is automatically saved for future use&lt;br /&gt;
&lt;br /&gt;
  Preferences panel&lt;br /&gt;
&lt;br /&gt;
If you are uncertain about which COM port to assign use, the Serial Port Monitor application can help identify the COM port assigned to the HV sequencer. This small application is included on the HV Sequencer installer USB stick, and can also be downloaded from the eDAQ Utilities and Tools download webpage:&lt;br /&gt;
&lt;br /&gt;
	[[http://www.edaq.com/utilities_tools.php www.edaq.com/utilities_tools.php]]&lt;br /&gt;
&lt;br /&gt;
The serial port monitor runs as an icon in the notification area.  Clicking on it will show a list of eDAQ COM port devices attached to your computer.&lt;br /&gt;
&lt;br /&gt;
The other Preference options set the digital output type, and provide control over front panel lights in situations where light pollution needs to be kept to a minimum.&lt;br /&gt;
&lt;br /&gt;
Check if you have installed an interlock as described previously.  The INTERLOCK LED should be OFF indicating that the INTERLOCK is in place.&lt;br /&gt;
    &lt;br /&gt;
&lt;br /&gt;
Click the Online in the menu bar to attach the selected ER430 unit to the Sequencer application. &lt;br /&gt;
&lt;br /&gt;
Click the Offline in the menu bar to disconnect the selected ER430 unit from the Sequencer application.&lt;br /&gt;
 &lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
=== Disarming and Interlock Test ===&lt;br /&gt;
&lt;br /&gt;
Press and hold the red ARM button to arm the unit.  As before, the unit will beep and arm itself.  This will also be shown in the software’s display.&lt;br /&gt;
&lt;br /&gt;
You can now disarm the unit by either:&lt;br /&gt;
::• Pressing the red ARM button again&lt;br /&gt;
::• Clicking “Disarm” in the top-right of the software window.&lt;br /&gt;
&lt;br /&gt;
While the unit is armed, you can test the safety interlock by removing the short-circuit from the BNC connector.  The unit should immediately disarm itself, disconnecting the outputs, and turning off any applied voltages.&lt;br /&gt;
&lt;br /&gt;
=== Manual Settings ===&lt;br /&gt;
After arming the unit, click on the More… button to display the controls for making immediate changes to the unit.&lt;br /&gt;
&lt;br /&gt;
The right hand side of the HV Sequencer setup panel provides the means to manually set meter functions, output voltages, and the digital outputs’ states.  Make some selections, and then click on Set.  The ER430 hardware will immediately apply the settings you have chosen, and the software will display your choices, along with readings of current and/or voltage.&lt;br /&gt;
&lt;br /&gt;
At this point  the system will indicate the voltages set and currents measured.  Since no loads are yet connected, the currents will be very near zero. &lt;br /&gt;
&lt;br /&gt;
=== Setup panel ===&lt;br /&gt;
&lt;br /&gt;
At any time, pressing the Disarm button in the top-right hand corner of the Main Window or the red button on the front panel of the ER430 will disarm the unit and make it safe.  &lt;br /&gt;
&lt;br /&gt;
After disarming, you must press and hold the red button (as before) to re-arm it.  The software can not re-arm the device.&lt;br /&gt;
&lt;br /&gt;
Outputs let you control the digital outputs of the unit.  In the preference you can set Output configuration as contact closure, or TTL.&lt;br /&gt;
HV Sequences&lt;br /&gt;
The lower area of the Setup panel provides the means to define a “program” or “sequence” to run. This consists of a number of timed steps, each of which can update the state of one or more of the individual functions or outputs.  There are also some “special” commands that can be carried out. Unused connections can have the width of their columns reduced by dragging their column separator.&lt;br /&gt;
&lt;br /&gt;
All changes on a step happen simultaneously (within 2 milliseconds).&lt;br /&gt;
   Setup screen with an example&lt;br /&gt;
&lt;br /&gt;
Here is another example program:&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
If a step doesn’t have anything entered in its box, the output will remain unchanged from its previous setting.&lt;br /&gt;
&lt;br /&gt;
A time of “0” means “immediately upon starting”, and the times are cumulative, measured from when the sequence was started,  i.e.: the delay between the first four of the lines above is 5, 3, and 4 seconds respectively.&lt;br /&gt;
&lt;br /&gt;
It is recommended to have the first row setting every output to a known state, in case the previous run was stopped part-way through, leaving the unit in an unknown state.&lt;br /&gt;
&lt;br /&gt;
When the program finishes, the unit will be left in whatever state it was at the end.  It will not automatically disconnect or disarm the outputs, unless explicitly told to do so.&lt;br /&gt;
The Meter channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal (LED GREEN)&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE)&lt;br /&gt;
Read I:  Current Meter connection (LED YELLOW)&lt;br /&gt;
The Output channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal.&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE).&lt;br /&gt;
Read I: Current meter connection (LED YELLOW)&lt;br /&gt;
Set V: Set the voltage to the value entered in the second column – In this mode the Voltage indicated will be the actual voltage produced within 1%. (LED RED)&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
Digital outputs can be set to:&lt;br /&gt;
Low/Open: Output goes low or open, as per the “digital output mode” setting in Preferences. &lt;br /&gt;
High/Closed: Output goes high or closed.&lt;br /&gt;
&lt;br /&gt;
The type of digital output, TTL or Contact Closure, is set from the Preferences dialog in the File menu.&lt;br /&gt;
&lt;br /&gt;
Special is a special function to be performed.  You can either:&lt;br /&gt;
::• Disarm: Disconnect HV supplies, and stop the program, or&lt;br /&gt;
::• Wait for trigger: Pause, and wait for a high/close on the rear panel’s green connector “Trigger” pins.&lt;br /&gt;
&lt;br /&gt;
Simple editing commands are available on the Edit menu.  The option to Always show the slave will force the display of the second control panel and additional program columns, even if a second unit is not attached.&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
Programs can be saved and loaded using the menu options in the File menu. &lt;br /&gt;
&lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
Once you are satisfied with your program, click the Run button in the menu bar.  The software will step through the program, executing each step at the given time after starting.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Pause button can be used to pause running of the program.  The Run button changes to a Resume button, which you can click to continue execution.&lt;br /&gt;
Stop will stop execution, but it will leave the unit in the current state, with whatever voltages selected still being output.&lt;br /&gt;
The Disarm button will stop any running program and put the ER430 hardware into a safe state.&lt;br /&gt;
Various fault and safety switch conditions will also force a disarming (and termination of program), including:&lt;br /&gt;
•	USB cable being removed&lt;br /&gt;
•	Front panel safety interlock opened/removed&lt;br /&gt;
•	Front panel red button being pressed&lt;br /&gt;
•	When operating with a slave unit, disconnection from the slave unit&lt;br /&gt;
&lt;br /&gt;
=== Modes of Operation ===&lt;br /&gt;
&lt;br /&gt;
==== General ====&lt;br /&gt;
::• Disarmed/Safe – High voltages and meters disconnected  &lt;br /&gt;
::• Armed- High voltages are active and available for connection to external circuit.&lt;br /&gt;
&lt;br /&gt;
==== Programmable HV power supplies ====&lt;br /&gt;
Output Voltage:  Adjustable from ±200V to ±3000V at up to 200µA. &lt;br /&gt;
Output Polarity:  Positive or Negative with respect to the common ground potential&lt;br /&gt;
&lt;br /&gt;
==== Operating Modes ====&lt;br /&gt;
::• O/C mode: Open Circuit by disconnection with high voltage relay.&lt;br /&gt;
::• Voltage Mode: High voltage output mode with current and voltage monitoring&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 10 Meohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring&lt;br /&gt;
&lt;br /&gt;
==== Meters ====&lt;br /&gt;
::• O/C mode: Open Circuit achieved by disconnection with high voltage relay&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 100 Mohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring &lt;br /&gt;
&lt;br /&gt;
By combining the HV power supplies and meters it is possible to setup the conditions which load the sample into the separation channel and then apply the appropriate voltages to cause separation and detection of the sample components as shown in the example.&lt;br /&gt;
&lt;br /&gt;
=== Typical Installation ===&lt;br /&gt;
 &lt;br /&gt;
 &lt;br /&gt;
== ER430 HV Hardware ==&lt;br /&gt;
&lt;br /&gt;
=== ER430 HV Channel Block Diagram ===&lt;br /&gt;
A Block diagram of a HV supply channel is shown below; there are four identical HV channels in each ER430unit:&lt;br /&gt;
 &lt;br /&gt;
=== ER430 Meter Channel block diagram ===&lt;br /&gt;
&lt;br /&gt;
=== Green Connector Pin Numbers ===&lt;br /&gt;
&lt;br /&gt;
ER430 HV Sequencer “green” connector Pin functions&lt;br /&gt;
&lt;br /&gt;
:: 1	TRIG +	TTL  IN	11	HV 1 E	HV VOLTAGE  MONITOR 1&lt;br /&gt;
:: 2	TRIG -	TTL COM	12	HV 1 I	HV CURRENT MONITOR 1&lt;br /&gt;
:: 3	HV4  E	HV VOLTAGE  MONITOR 4	13	CTL1 +	DIGITAL  IN/OUT 1&lt;br /&gt;
:: 4	HV4  I	HV CURRENT MONITOR 4	14	CTL1 -	DIGITAL COM&lt;br /&gt;
:: 5	COM	COMMON	15	CTL2 +	DIGITAL  IN/OUT 2&lt;br /&gt;
:: 6	HV3 E	HV VOLTAGE  MONITOR 3	16	CTL2 -	DIGITAL COM&lt;br /&gt;
:: 7	HV3  I	HV CURRENT MONITOR 3	17	CTL3+	DIGITAL  IN/OUT 3&lt;br /&gt;
:: 8	HV 2 E	HV VOLTAGE  MONITOR 2	18	CTL3 -	DIGITAL COM&lt;br /&gt;
:: 9	HV 2  I	HV CURRENT MONITOR 2	19	CTL4 +	DIGITAL  IN/OUT 4&lt;br /&gt;
:: 10	COM	COMMON	20	CTL4 -	DIGITAL COM&lt;br /&gt;
&lt;br /&gt;
Notes:&lt;br /&gt;
# Digital I/O pins are implemented as contact closure or TTL outputs, software selectable&lt;br /&gt;
# Trigger input can be a contact closure or TTL input&lt;br /&gt;
# HV VOLTAGE  MONITOR scale factor: 500mV/kV&lt;br /&gt;
# HV Current Monitor Scale factor: 100mV/mA&lt;br /&gt;
&lt;br /&gt;
== Specifications==&lt;br /&gt;
&lt;br /&gt;
=== High Voltage Output and Mode Options ===&lt;br /&gt;
&lt;br /&gt;
::• Channels: 4&lt;br /&gt;
::• Model: UR3*&lt;br /&gt;
::• Maximum Voltage Setting: ±3000 V&lt;br /&gt;
::• Minimum Voltage Setting: ±200 V&lt;br /&gt;
::• Current: ±200 µA max&lt;br /&gt;
::• Ripple: 0.1%		&lt;br /&gt;
::• Operating Modes: Applied voltage, Open Circuit (O/C), and Short Circuit (S/C)		&lt;br /&gt;
::• Load regulation: &amp;lt;2% specified for 20-90% full load: &lt;br /&gt;
::• Rise and Fall times: &amp;lt;5 ms specified for changes within the same polarity regime&lt;br /&gt;
::• Mode Change: &amp;lt;100ms due to relay operations, safety and software latency&lt;br /&gt;
	&lt;br /&gt;
Note: Output is referred to system common (Case Ground)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Safety Features ===&lt;br /&gt;
An interlock is provided on&lt;br /&gt;
::• the mechanical case to ensure that no voltages are present with the case open unless authorized maintenance is in progress.  &lt;br /&gt;
::• the microchip environment to ensure that accidental contact is not made with the high voltages.&lt;br /&gt;
&lt;br /&gt;
The Arm/disarm switch needs to be held for 2 seconds to arm the system and allow high voltages to become active.  Any short contact on the ARM switch will disarm the system.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION''': It is the responsibility of the user to ensure that adequate protection is provided on the equipment provided by the user. eDAQ provides microfluidic chip adaptors with appropriate interlock features.&lt;br /&gt;
&lt;br /&gt;
=== Meter Functions ===&lt;br /&gt;
&lt;br /&gt;
::• Voltage Range:	±3000 V&lt;br /&gt;
::• Voltage Resolution: 1 V&lt;br /&gt;
::• Current Range: ±200 µA&lt;br /&gt;
::• Current resolution: 1 µA&lt;br /&gt;
::• Displayed resolution limited to 1 unit&lt;br /&gt;
&lt;br /&gt;
=== Communications and Inputs and outputs terminals ===&lt;br /&gt;
&lt;br /&gt;
::• Daisy Chain connectors: Twin DB9 connectors allow two (2) ER430 units to be daisy chained together.&lt;br /&gt;
::• USB Port:  Compatible with USB1 &amp;amp; USB 2 and provides, communications facility to PC’s&lt;br /&gt;
::• Output and Meters front panel connectors:  SHV (Safe High Voltage)  type &lt;br /&gt;
::• 20 Way 3.5mm Green screw terminal: &lt;br /&gt;
:::: - Four Digital I/O lines&lt;br /&gt;
:::: - Trigger TTL or CC&lt;br /&gt;
:::: - Four Voltage Monitor signals&lt;br /&gt;
:::: - FourCurrent  Monitor signals.&lt;br /&gt;
::• System/Chassis Earth terminal: 4 mm screw terminal.&lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
&lt;br /&gt;
The following LED front panel displays are available:&lt;br /&gt;
&lt;br /&gt;
::•  System Status (RGB LED)&lt;br /&gt;
::: GREEN when “on line” &lt;br /&gt;
&lt;br /&gt;
::• Interlock (amber LED)&lt;br /&gt;
::: FLASHING = Interlock open, unit disarmed, arming not allowed.&lt;br /&gt;
::: OFF = Interlock OK, unit disarmed&lt;br /&gt;
::: ON = Interlock OK, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
::• Meter Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (disconnected) &lt;br /&gt;
:::: YELLOW = Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (supply disconnected) &lt;br /&gt;
:::: YELLOW =  Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Status  (RGB LED)&lt;br /&gt;
:::: OFF = supply disconnected&lt;br /&gt;
:::: ON = supply connected and active.&lt;br /&gt;
&lt;br /&gt;
=== Physical ===&lt;br /&gt;
::• Dimensions (w x h x d): 200 x 65 x 250 mm (7.9 x 2.6 x 9.8 inch)&lt;br /&gt;
::• Weight: 3.00 kg packed&lt;br /&gt;
::• Operating temperature: 0 - 35ºC&lt;br /&gt;
::• Humidity: 10 to 80% non condensing &lt;br /&gt;
::• Power:  9 - 16 V @ 2 A maximum supplied by mains powered AC/DC converter (supplied)&lt;br /&gt;
&lt;br /&gt;
== Legal and Warranty ==&lt;br /&gt;
&lt;br /&gt;
=== Trademarks and Copyright ===&lt;br /&gt;
Sequencer, HV Sequencer, and Chart are trademarks of eDAQ Pty Ltd.&lt;br /&gt;
Windows XP, Vista, and Windows 7, Windows 8 and Windows 10 are trademarks of Microsoft Corporation.&lt;br /&gt;
This document is Copyright © July 2015. This document, or sections thereof, may be copied by the owners or users of an eDAQ Quad MF isoPod for their private use. Otherwise no part of this document may be&lt;br /&gt;
reproduced by any means without the prior written permission of eDAQ Pty Ltd.&lt;br /&gt;
&lt;br /&gt;
=== Responsibilities ===&lt;br /&gt;
&lt;br /&gt;
You and any others using any eDAQ product agree to use it in a sensible manner for purposes for which it is suited, and agree to take responsibility for their actions and the results of their actions. If problems arise with an eDAQ product, eDAQ will make all reasonable efforts to fix them. This service may incur a charge, depending on the nature of the problems, and is subject to the other conditions in this Agreement.&lt;br /&gt;
&lt;br /&gt;
=== Hardware Warranty ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd warrants this device, to be free of defects in material and workmanship for three years from the date of purchase. Note that this does NOT include external cables and electrodes that are subject to 'wear and tear' and manufacturing defects should be reported within 90 days of purchase. eDAQ Pty Ltd will repair or replace defective equipment as appropriate. To obtain a warranty repair/replacement you must first notify us before return of the instrument and we will issue you with a RAN (return authorisation number). You must ship the defective product at your expense. We will pay return shipping. The product should be packed safely (preferably in its original packaging) and have the RAN on the shipping label. Returns sent without a RAN may be refused delivery.&lt;br /&gt;
&lt;br /&gt;
This warranty does not cover hardware that has:&lt;br /&gt;
:• been modified by the user in any way;&lt;br /&gt;
:• been subjected to unusual physical, electrical, or environmental stress. This includes damage due to faulty power sockets, inadequate earthing, or power spikes or surges;&lt;br /&gt;
:• been damaged because of incorrect wiring to ancillary equipment, or because of substandard, connectors or cables; or&lt;br /&gt;
:• had the original identification marks removed or altered.&lt;br /&gt;
&lt;br /&gt;
=== Software License ===&lt;br /&gt;
&lt;br /&gt;
You have the non-exclusive right to use the supplied eDAQ software (Sequencer, Chart etc). Your employees or students, for example, are entitled to use it, provided they adhere to this agreement. &lt;br /&gt;
Each separate purchase of the eDAQ software licenses it to be used on two computers, more than two copies must not be used simultaneously. Departmental/company licences are available if you wish to run more than two copies simultaneously.&lt;br /&gt;
&lt;br /&gt;
=== Technical Support ===&lt;br /&gt;
&lt;br /&gt;
Please register your unit to receive technical support.&lt;br /&gt;
&lt;br /&gt;
Technical assistance is available via email. Please describe the problem with as much detail as possible. Include a small example data file, if appropriate. Please also state:&lt;br /&gt;
: • the model and serial number of your EDAQ system.&lt;br /&gt;
: • the type of computer and operating system being used (for example Windows XP, Vista, Windows 7, 8, or 10)&lt;br /&gt;
: • the software version you are using (for example Chart v5.5.2)&lt;br /&gt;
&lt;br /&gt;
We endeavor to answer all your questions, but in some cases, for example where the problem relates to the other equipment that you are using, a nominal fee may be charged.&lt;br /&gt;
&lt;br /&gt;
=== Jurisdiction ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd is bound by the laws of New South Wales in Australia, and any proceedings shall be heard by the Supreme Court of New South Wales in Australia.&lt;br /&gt;
&lt;br /&gt;
=== Disclaimer ===&lt;br /&gt;
&lt;br /&gt;
eDAQ reserves the right to alter specifications of hardware and software without notice. No liability can be accepted for consequential damages resulting from use of eDAQ products.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3989</id>
		<title>ER430 Manual</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3989"/>
				<updated>2015-08-06T07:43:04Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Meters */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;br /&gt;
== Introduction ==&lt;br /&gt;
[[File:ER430SmallPanels.jpg|thumb|upright=2|right|'''Figure 1.''' ER430 HV Sequencer front and back panels]]&lt;br /&gt;
This manual is intended to allow the user to install, check and run the ER430 HV Sequencer. It provides detailed information on the system and its operation. Please read this manual carefully prior to beginning operation.&lt;br /&gt;
&lt;br /&gt;
The ER430 High Voltage Sequencer provides the following functions:&lt;br /&gt;
::• Four independent programmable metered high voltage (HV) supplies.&lt;br /&gt;
::• Safety Interlock system&lt;br /&gt;
::• Software that allows arbitrary sequences of voltages to be generated&lt;br /&gt;
&lt;br /&gt;
== Checking the Instrument ==&lt;br /&gt;
Before you begin working with the device, you should check:&lt;br /&gt;
:• that the contents of the package you received match the packing list&lt;br /&gt;
:• for any sign of physical damage that might have occurred during transit.&lt;br /&gt;
If you find a problem, please contact your [http://www.edaq.com/edaq-distributors eDAQ distributor] or agent immediately.&lt;br /&gt;
&lt;br /&gt;
== Safety First ==&lt;br /&gt;
&lt;br /&gt;
This equipment generates high voltages of up to 3000 V DC at currents of up to 200 µA. Making contact with such voltages can be extremely dangerous.&lt;br /&gt;
&lt;br /&gt;
Ensure that the high voltage (HV) circuits are housed in an insulated enclosure fitted with an Interlock safety circuit and with no manual access to HV circuits while circuits are alive.&lt;br /&gt;
&lt;br /&gt;
Safety precautions:&lt;br /&gt;
::• Ensure that the safety interlock circuit is connected to the HV Sequencer and is only active and enabled when no accidental access to High Voltage circuits can be made.&lt;br /&gt;
::• Wear rubber soled footwear&lt;br /&gt;
::• Ensure the floor and bench top are dry&lt;br /&gt;
::• Stand on a rubber mat when in the vicinity of high voltages&lt;br /&gt;
&lt;br /&gt;
The ER430 features design precautions to ensure that there is no accidental application of high voltages. These include automatic shutdown in the event of voltage or current overloads . This will in some circumstances prevent the unit from operating. In these cases check all settings and safety interlocks carefully before resuming the experiment.&lt;br /&gt;
&lt;br /&gt;
=== What is an Interlock ===&lt;br /&gt;
&lt;br /&gt;
An interlock is a mechanical or electrical system that prevents the inadvertent operation of of an instrument.&lt;br /&gt;
&lt;br /&gt;
In the case of the  ER430 HV Sequencer this is achieved by using a switch located in the enclosure in which high voltages are active.  This switch is connected via a cable to the front panel INTERLOCK BNC in such a way that the switch is only closed when no access is available to the High voltages inside the enclosure.&lt;br /&gt;
&lt;br /&gt;
For example with the eDAQ supplied ET225 Micronit Chip Electrophoresis Platform, high voltages can only be applied when the top cover is in place.  This is detected and the interlock switch enabled to allow the application of high voltages.&lt;br /&gt;
&lt;br /&gt;
If the user is providing the MicroChip enclosure then it is the user’s responsibility to provide the required interlock function.&lt;br /&gt;
&lt;br /&gt;
To test the Interlock function it is sufficient to apply a short circuit across the INTERLOCK BNC input pins.  This should only be done with no connections to the High Voltage input connectors.&lt;br /&gt;
ER430 &lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
System indicators as shown in the preceding diagram provide a direct indication of system operation that reflects the state of the internal hardware.  These indicators will assist you in monitoring system operation and in diagnosing problems – study them carefully:  &lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED: Amber LED&lt;br /&gt;
	FLASHING = Interlock open, unit disarmed, arming not enabled.&lt;br /&gt;
	OFF = Interlock in place and enabled, unit can be ARMED.&lt;br /&gt;
	ON = Interlock in place, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
SYSTEM STATUS LED: RGB LED (Multicoloured)&lt;br /&gt;
GREEN when “on line” and ready as a Master&lt;br /&gt;
BLUE when ready as a Slave&lt;br /&gt;
&lt;br /&gt;
METER FUNCTION LED: RGB LED&lt;br /&gt;
GREEN:  Safe (disconnected) &lt;br /&gt;
YELLOW:  Current Mode&lt;br /&gt;
BLUE:  Voltage mode&lt;br /&gt;
&lt;br /&gt;
HV STATUS: RED LED&lt;br /&gt;
OFF: supply disconnected&lt;br /&gt;
ON: supply connected and active.&lt;br /&gt;
&lt;br /&gt;
Notes: &lt;br /&gt;
#On power up the system performs a startup test and flashes the front panel LEDs through the various colors available for display.&lt;br /&gt;
# In some cases where the HV supply needs to be used in proximity to light sensitive detectors it is possible to optionally turn off all the LEDs to maintain low background illumination.&lt;br /&gt;
 &lt;br /&gt;
== Hardware Installation ==&lt;br /&gt;
'''ATTENTION:''' When installing the system for the first time ALWAYS perform software installation before connecting the hardware units.  This ensures that the correct drivers are installed &lt;br /&gt;
 &lt;br /&gt;
After carrying out the software installation described in the next section, perform the following Hardware installation procedure. It will confirm that:&lt;br /&gt;
::• That safety interlocks are in place and functioning correctly&lt;br /&gt;
::• The unit can be armed and disarmed&lt;br /&gt;
&lt;br /&gt;
Operation:&lt;br /&gt;
::• '''Safety first''' Connect the unit to a good ground using the terminal post on the rear of the unit.&lt;br /&gt;
::• Connect the unit to the 12V DC mains power pack.&lt;br /&gt;
::• Connect the unit to the PC using the USB cable provided.&lt;br /&gt;
::• Turn Power on.&lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED will flash if interlock is not enabled.&lt;br /&gt;
&lt;br /&gt;
HV Status LEDs: Off (no high voltage output)&lt;br /&gt;
&lt;br /&gt;
STATUS LEDs: Green&lt;br /&gt;
&lt;br /&gt;
=== TEST INTERLOCK Function ===&lt;br /&gt;
&lt;br /&gt;
This function can be tested without any software running:&lt;br /&gt;
::• The INTERLOCK LED will initially be flashing.&lt;br /&gt;
::• Connect a short circuit to the INTERLOCK BNC.&lt;br /&gt;
::• INTERLOCK LED will turn OFF.&lt;br /&gt;
::• Press the ARM Push Button for approximately 1 to 2 seconds.  You should hear a beep, warning you that the HV outputs have been armed (enabled) and the INTERLOCK LED will turn ON.&lt;br /&gt;
::• At this point all HV supplies are still inactive but are in a state where they can be set and controlled by the Sequencer Application software.&lt;br /&gt;
::• Pressing the Arm button again will DISARM the HV Sequencer, and the INTEROCK LED will turn off.&lt;br /&gt;
&lt;br /&gt;
A momentary push on  the Arm button will disable all the HV outputs of the Sequencer.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== INTERLOCK features ===&lt;br /&gt;
The system is provided with a number of safety features or Interlocks:&lt;br /&gt;
::• Chip adapter interlock:  The chip adapter used should provide a safety contact interlock to indicate that the microchip adapter is safe for use.  This interlock is a contact closure switch, which is closed when the HV circuit is fully enclosed and protected from user access. This interlock is connected to the front panel Interlock BNC and indicates to the ER430 that it is safe to arm the system.&lt;br /&gt;
::• USB Present:  The system cannot be ARMED without an active USB connection&lt;br /&gt;
::• Software Control: Once the system is ARMED High Voltages can only be applied under software control.&lt;br /&gt;
::• ARM circuit: prior to applying HV to an external circuit the system must be armed by the user by depressing the front panel ARM push button for approximately 2 seconds.&lt;br /&gt;
::• DISARM: The system can be disarmed by a momentary push of the ARM button.&lt;br /&gt;
::• Power Overloads:  the circuit detects power overloads and situations that lead to the generation of arcs (sparks).  The system will switch itself off in such circumstances and in such circumstances may require to be reinitiated with power being turned on Off and On.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION:'''  Do not disconnect HV leads by hand while High voltages are present – this is extremely dangerous and can cause harmful arcs to be generated. To disable power use the ARM/DISARM front panel button or the software’s Disarm or Disconnect menu items&lt;br /&gt;
&lt;br /&gt;
You are now ready to operate the Sequencer software which will allow you to generate and output a series of high voltage pulses and ramps.&lt;br /&gt;
&lt;br /&gt;
== Software Installation &amp;amp; Operation ==&lt;br /&gt;
&lt;br /&gt;
=== Installing the HV Sequencer software ===&lt;br /&gt;
Insert the HV Sequencer installation USB stick into your computer.  It is recommended to install the software before plugging in the hardware, as it ensures the drivers are correctly installed.&lt;br /&gt;
&lt;br /&gt;
The eDAQ Sequencer Setup Wizard will display a start-up screen; follow the prompts to install the software.&lt;br /&gt;
      Start up screen&lt;br /&gt;
			    Final Start up screen&lt;br /&gt;
&lt;br /&gt;
=== eDAQ Sequencer Overview ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Sequencer is a Windows application that provides the means to setup a series of steps that are executed under computer control.  The following functions are provided:&lt;br /&gt;
&lt;br /&gt;
System setup and sequence entry: The software identifies system configuration on startup and allows the operating parameters to be set immediately.&lt;br /&gt;
&lt;br /&gt;
Table driven Sequence: A time based table is filled out, specifying that the operations to be performed in sequence.  This includes setting of HV supplies to new voltages, trigger and digital I/O line functions. The following sequence operations are implemented: &lt;br /&gt;
&lt;br /&gt;
Time: set to xxxx seconds&lt;br /&gt;
Meter 1&amp;amp;2: Disconnect, Read V, Read I&lt;br /&gt;
Output1&amp;amp;2: Set V=xxxx (V and I monitored), Read V, Read I&lt;br /&gt;
Digital Out: Low/Open, High/Closed, Short Pulse, Long Pulse&lt;br /&gt;
Special commands: Wait for trigger, Wait for Arming, Go Safe&lt;br /&gt;
New functions can be readily added to meet customer requirements&lt;br /&gt;
&lt;br /&gt;
Digital outputs can be used to control external devices or the recording of data in an ecorder.&lt;br /&gt;
&lt;br /&gt;
Monitoring: Once a sequence is started the user is able to observe the progress of the sequence on the sequence table.  Values of HV supply voltages and currents are displayed during operation.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
 === HV Sequencer Main Window ===&lt;br /&gt;
&lt;br /&gt;
  &lt;br /&gt;
=== Communication ===&lt;br /&gt;
&lt;br /&gt;
The HV sequencer uses a virtual USB serial communications (COM) port.  When the ER430 hardware is first attached to USB, a free COM port number is automatically assigned by Windows.  That COM port will be then used every time that unit is plugged in again.&lt;br /&gt;
&lt;br /&gt;
Note:  the first time you connect the system to the computer it may take some time for the system to identify the HV sequencer device driver and install it.  You will be notified when the device is ready.&lt;br /&gt;
&lt;br /&gt;
The first time you use the sequencer software, you need to specify the COM port that the hardware has been assigned.  Select the Preferences option in the File menu, then choose your HV Sequencer in the list at the top – see screen shot below. This preference is automatically saved for future use&lt;br /&gt;
&lt;br /&gt;
  Preferences panel&lt;br /&gt;
&lt;br /&gt;
If you are uncertain about which COM port to assign use, the Serial Port Monitor application can help identify the COM port assigned to the HV sequencer. This small application is included on the HV Sequencer installer USB stick, and can also be downloaded from the eDAQ Utilities and Tools download webpage:&lt;br /&gt;
&lt;br /&gt;
	[[http://www.edaq.com/utilities_tools.php www.edaq.com/utilities_tools.php]]&lt;br /&gt;
&lt;br /&gt;
The serial port monitor runs as an icon in the notification area.  Clicking on it will show a list of eDAQ COM port devices attached to your computer.&lt;br /&gt;
&lt;br /&gt;
The other Preference options set the digital output type, and provide control over front panel lights in situations where light pollution needs to be kept to a minimum.&lt;br /&gt;
&lt;br /&gt;
Check if you have installed an interlock as described previously.  The INTERLOCK LED should be OFF indicating that the INTERLOCK is in place.&lt;br /&gt;
    &lt;br /&gt;
&lt;br /&gt;
Click the Online in the menu bar to attach the selected ER430 unit to the Sequencer application. &lt;br /&gt;
&lt;br /&gt;
Click the Offline in the menu bar to disconnect the selected ER430 unit from the Sequencer application.&lt;br /&gt;
 &lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
=== Disarming and Interlock Test ===&lt;br /&gt;
&lt;br /&gt;
Press and hold the red ARM button to arm the unit.  As before, the unit will beep and arm itself.  This will also be shown in the software’s display.&lt;br /&gt;
&lt;br /&gt;
You can now disarm the unit by either:&lt;br /&gt;
::• Pressing the red ARM button again&lt;br /&gt;
::• Clicking “Disarm” in the top-right of the software window.&lt;br /&gt;
&lt;br /&gt;
While the unit is armed, you can test the safety interlock by removing the short-circuit from the BNC connector.  The unit should immediately disarm itself, disconnecting the outputs, and turning off any applied voltages.&lt;br /&gt;
&lt;br /&gt;
=== Manual Settings ===&lt;br /&gt;
After arming the unit, click on the More… button to display the controls for making immediate changes to the unit.&lt;br /&gt;
&lt;br /&gt;
The right hand side of the HV Sequencer setup panel provides the means to manually set meter functions, output voltages, and the digital outputs’ states.  Make some selections, and then click on Set.  The ER430 hardware will immediately apply the settings you have chosen, and the software will display your choices, along with readings of current and/or voltage.&lt;br /&gt;
&lt;br /&gt;
At this point  the system will indicate the voltages set and currents measured.  Since no loads are yet connected, the currents will be very near zero. &lt;br /&gt;
&lt;br /&gt;
=== Setup panel ===&lt;br /&gt;
&lt;br /&gt;
At any time, pressing the Disarm button in the top-right hand corner of the Main Window or the red button on the front panel of the ER430 will disarm the unit and make it safe.  &lt;br /&gt;
&lt;br /&gt;
After disarming, you must press and hold the red button (as before) to re-arm it.  The software can not re-arm the device.&lt;br /&gt;
&lt;br /&gt;
Outputs let you control the digital outputs of the unit.  In the preference you can set Output configuration as contact closure, or TTL.&lt;br /&gt;
HV Sequences&lt;br /&gt;
The lower area of the Setup panel provides the means to define a “program” or “sequence” to run. This consists of a number of timed steps, each of which can update the state of one or more of the individual functions or outputs.  There are also some “special” commands that can be carried out. Unused connections can have the width of their columns reduced by dragging their column separator.&lt;br /&gt;
&lt;br /&gt;
All changes on a step happen simultaneously (within 2 milliseconds).&lt;br /&gt;
   Setup screen with an example&lt;br /&gt;
&lt;br /&gt;
Here is another example program:&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
If a step doesn’t have anything entered in its box, the output will remain unchanged from its previous setting.&lt;br /&gt;
&lt;br /&gt;
A time of “0” means “immediately upon starting”, and the times are cumulative, measured from when the sequence was started,  i.e.: the delay between the first four of the lines above is 5, 3, and 4 seconds respectively.&lt;br /&gt;
&lt;br /&gt;
It is recommended to have the first row setting every output to a known state, in case the previous run was stopped part-way through, leaving the unit in an unknown state.&lt;br /&gt;
&lt;br /&gt;
When the program finishes, the unit will be left in whatever state it was at the end.  It will not automatically disconnect or disarm the outputs, unless explicitly told to do so.&lt;br /&gt;
The Meter channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal (LED GREEN)&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE)&lt;br /&gt;
Read I:  Current Meter connection (LED YELLOW)&lt;br /&gt;
The Output channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal.&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE).&lt;br /&gt;
Read I: Current meter connection (LED YELLOW)&lt;br /&gt;
Set V: Set the voltage to the value entered in the second column – In this mode the Voltage indicated will be the actual voltage produced within 1%. (LED RED)&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
Digital outputs can be set to:&lt;br /&gt;
Low/Open: Output goes low or open, as per the “digital output mode” setting in Preferences. &lt;br /&gt;
High/Closed: Output goes high or closed.&lt;br /&gt;
&lt;br /&gt;
The type of digital output, TTL or Contact Closure, is set from the Preferences dialog in the File menu.&lt;br /&gt;
&lt;br /&gt;
Special is a special function to be performed.  You can either:&lt;br /&gt;
::• Disarm: Disconnect HV supplies, and stop the program, or&lt;br /&gt;
::• Wait for trigger: Pause, and wait for a high/close on the rear panel’s green connector “Trigger” pins.&lt;br /&gt;
&lt;br /&gt;
Simple editing commands are available on the Edit menu.  The option to Always show the slave will force the display of the second control panel and additional program columns, even if a second unit is not attached.&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
Programs can be saved and loaded using the menu options in the File menu. &lt;br /&gt;
&lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
Once you are satisfied with your program, click the Run button in the menu bar.  The software will step through the program, executing each step at the given time after starting.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Pause button can be used to pause running of the program.  The Run button changes to a Resume button, which you can click to continue execution.&lt;br /&gt;
Stop will stop execution, but it will leave the unit in the current state, with whatever voltages selected still being output.&lt;br /&gt;
The Disarm button will stop any running program and put the ER430 hardware into a safe state.&lt;br /&gt;
Various fault and safety switch conditions will also force a disarming (and termination of program), including:&lt;br /&gt;
•	USB cable being removed&lt;br /&gt;
•	Front panel safety interlock opened/removed&lt;br /&gt;
•	Front panel red button being pressed&lt;br /&gt;
•	When operating with a slave unit, disconnection from the slave unit&lt;br /&gt;
&lt;br /&gt;
=== Modes of Operation ===&lt;br /&gt;
&lt;br /&gt;
==== General ====&lt;br /&gt;
::• Disarmed/Safe – High voltages and meters disconnected  &lt;br /&gt;
::• Armed- High voltages are active and available for connection to external circuit.&lt;br /&gt;
&lt;br /&gt;
==== Programmable HV power supplies ====&lt;br /&gt;
Output Voltage:  Adjustable from ±200V to ±3000V at up to 200µA. &lt;br /&gt;
Output Polarity:  Positive or Negative with respect to the common ground potential&lt;br /&gt;
&lt;br /&gt;
==== Operating Modes ====&lt;br /&gt;
::• O/C mode: Open Circuit by disconnection with high voltage relay.&lt;br /&gt;
::• Voltage Mode: High voltage output mode with current and voltage monitoring&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 10 Meohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring&lt;br /&gt;
&lt;br /&gt;
==== Meters ====&lt;br /&gt;
::• O/C mode: Open Circuit achieved by disconnection with high voltage relay&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 100 Mohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring &lt;br /&gt;
&lt;br /&gt;
By combining the HV power supplies and meters it is possible to setup the conditions which load the sample into the separation channel and then apply the appropriate voltages to cause separation and detection of the sample components as shown in the example.&lt;br /&gt;
&lt;br /&gt;
=== Typical Installation ===&lt;br /&gt;
 &lt;br /&gt;
 &lt;br /&gt;
== ER430 HV Hardware ==&lt;br /&gt;
&lt;br /&gt;
=== ER430 HV Channel Block Diagram ===&lt;br /&gt;
A Block diagram of a HV supply channel is shown below; there are four identical HV channels in each ER430unit:&lt;br /&gt;
 &lt;br /&gt;
=== ER430 Meter Channel block diagram ===&lt;br /&gt;
&lt;br /&gt;
=== Green Connector Pin Numbers ===&lt;br /&gt;
&lt;br /&gt;
ER430 HV Sequencer “green” connector Pin functions&lt;br /&gt;
&lt;br /&gt;
1	TRIG +	TTL  IN	11	HV 1 E	HV VOLTAGE  MONITOR 1&lt;br /&gt;
2	TRIG -	TTL COM	12	HV 1 I	HV CURRENT MONITOR 1&lt;br /&gt;
3	HV4  E	HV VOLTAGE  MONITOR 4	13	CTL1 +	DIGITAL  IN/OUT 1&lt;br /&gt;
4	HV4  I	HV CURRENT MONITOR 4	14	CTL1 -	DIGITAL COM&lt;br /&gt;
5	COM	COMMON	15	CTL2 +	DIGITAL  IN/OUT 2&lt;br /&gt;
6	HV3 E	HV VOLTAGE  MONITOR 3	16	CTL2 -	DIGITAL COM&lt;br /&gt;
7	HV3  I	HV CURRENT MONITOR 3	17	CTL3+	DIGITAL  IN/OUT 3&lt;br /&gt;
8	HV 2 E	HV VOLTAGE  MONITOR 2	18	CTL3 -	DIGITAL COM&lt;br /&gt;
9	HV 2  I	HV CURRENT MONITOR 2	19	CTL4 +	DIGITAL  IN/OUT 4&lt;br /&gt;
10	COM	COMMON	20	CTL4 -	DIGITAL COM&lt;br /&gt;
&lt;br /&gt;
Notes:&lt;br /&gt;
# Digital I/O pins are implemented as contact closure or TTL outputs, software selectable&lt;br /&gt;
# Trigger input can be a contact closure or TTL input&lt;br /&gt;
# HV VOLTAGE  MONITOR scale factor: 500mV/kV&lt;br /&gt;
# HV Current Monitor Scale factor: 100mV/mA&lt;br /&gt;
&lt;br /&gt;
== Specifications==&lt;br /&gt;
&lt;br /&gt;
=== High Voltage Output and Mode Options ===&lt;br /&gt;
&lt;br /&gt;
::• Channels: 4&lt;br /&gt;
::• Model: UR3*&lt;br /&gt;
::• Maximum Voltage Setting: ±3000 V&lt;br /&gt;
::• Minimum Voltage Setting: ±200 V&lt;br /&gt;
::• Current: ±200 µA max&lt;br /&gt;
::• Ripple: 0.1%		&lt;br /&gt;
::• Operating Modes: Applied voltage, Open Circuit (O/C), and Short Circuit (S/C)		&lt;br /&gt;
::• Load regulation: &amp;lt;2% specified for 20-90% full load: &lt;br /&gt;
::• Rise and Fall times: &amp;lt;5 ms specified for changes within the same polarity regime&lt;br /&gt;
::• Mode Change: &amp;lt;100ms due to relay operations, safety and software latency&lt;br /&gt;
	&lt;br /&gt;
Note: Output is referred to system common (Case Ground)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Safety Features ===&lt;br /&gt;
An interlock is provided on&lt;br /&gt;
::• the mechanical case to ensure that no voltages are present with the case open unless authorized maintenance is in progress.  &lt;br /&gt;
::• the microchip environment to ensure that accidental contact is not made with the high voltages.&lt;br /&gt;
&lt;br /&gt;
The Arm/disarm switch needs to be held for 2 seconds to arm the system and allow high voltages to become active.  Any short contact on the ARM switch will disarm the system.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION''': It is the responsibility of the user to ensure that adequate protection is provided on the equipment provided by the user. eDAQ provides microfluidic chip adaptors with appropriate interlock features.&lt;br /&gt;
&lt;br /&gt;
=== Meter Functions ===&lt;br /&gt;
&lt;br /&gt;
::• Voltage Range:	±3000 V&lt;br /&gt;
::• Voltage Resolution: 1 V&lt;br /&gt;
::• Current Range: ±200 µA&lt;br /&gt;
::• Current resolution: 1 µA&lt;br /&gt;
::• Displayed resolution limited to 1 unit&lt;br /&gt;
&lt;br /&gt;
=== Communications and Inputs and outputs terminals ===&lt;br /&gt;
&lt;br /&gt;
::• Daisy Chain connectors: Twin DB9 connectors allow two (2) ER430 units to be daisy chained together.&lt;br /&gt;
::• USB Port:  Compatible with USB1 &amp;amp; USB 2 and provides, communications facility to PC’s&lt;br /&gt;
::• Output and Meters front panel connectors:  SHV (Safe High Voltage)  type &lt;br /&gt;
::• 20 Way 3.5mm Green screw terminal: &lt;br /&gt;
:::: - Four Digital I/O lines&lt;br /&gt;
:::: - Trigger TTL or CC&lt;br /&gt;
:::: - Four Voltage Monitor signals&lt;br /&gt;
:::: - FourCurrent  Monitor signals.&lt;br /&gt;
::• System/Chassis Earth terminal: 4 mm screw terminal.&lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
&lt;br /&gt;
The following LED front panel displays are available:&lt;br /&gt;
&lt;br /&gt;
::•  System Status (RGB LED)&lt;br /&gt;
::: GREEN when “on line” &lt;br /&gt;
&lt;br /&gt;
::• Interlock (amber LED)&lt;br /&gt;
::: FLASHING = Interlock open, unit disarmed, arming not allowed.&lt;br /&gt;
::: OFF = Interlock OK, unit disarmed&lt;br /&gt;
::: ON = Interlock OK, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
::• Meter Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (disconnected) &lt;br /&gt;
:::: YELLOW = Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (supply disconnected) &lt;br /&gt;
:::: YELLOW =  Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Status  (RGB LED)&lt;br /&gt;
:::: OFF = supply disconnected&lt;br /&gt;
:::: ON = supply connected and active.&lt;br /&gt;
&lt;br /&gt;
=== Physical ===&lt;br /&gt;
::• Dimensions (w x h x d): 200 x 65 x 250 mm (7.9 x 2.6 x 9.8 inch)&lt;br /&gt;
::• Weight: 3.00 kg packed&lt;br /&gt;
::• Operating temperature: 0 - 35ºC&lt;br /&gt;
::• Humidity: 10 to 80% non condensing &lt;br /&gt;
::• Power:  9 - 16 V @ 2 A maximum supplied by mains powered AC/DC converter (supplied)&lt;br /&gt;
&lt;br /&gt;
== Legal and Warranty ==&lt;br /&gt;
&lt;br /&gt;
=== Trademarks and Copyright ===&lt;br /&gt;
Sequencer, HV Sequencer, and Chart are trademarks of eDAQ Pty Ltd.&lt;br /&gt;
Windows XP, Vista, and Windows 7, Windows 8 and Windows 10 are trademarks of Microsoft Corporation.&lt;br /&gt;
This document is Copyright © July 2015. This document, or sections thereof, may be copied by the owners or users of an eDAQ Quad MF isoPod for their private use. Otherwise no part of this document may be&lt;br /&gt;
reproduced by any means without the prior written permission of eDAQ Pty Ltd.&lt;br /&gt;
&lt;br /&gt;
=== Responsibilities ===&lt;br /&gt;
&lt;br /&gt;
You and any others using any eDAQ product agree to use it in a sensible manner for purposes for which it is suited, and agree to take responsibility for their actions and the results of their actions. If problems arise with an eDAQ product, eDAQ will make all reasonable efforts to fix them. This service may incur a charge, depending on the nature of the problems, and is subject to the other conditions in this Agreement.&lt;br /&gt;
&lt;br /&gt;
=== Hardware Warranty ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd warrants this device, to be free of defects in material and workmanship for three years from the date of purchase. Note that this does NOT include external cables and electrodes that are subject to 'wear and tear' and manufacturing defects should be reported within 90 days of purchase. eDAQ Pty Ltd will repair or replace defective equipment as appropriate. To obtain a warranty repair/replacement you must first notify us before return of the instrument and we will issue you with a RAN (return authorisation number). You must ship the defective product at your expense. We will pay return shipping. The product should be packed safely (preferably in its original packaging) and have the RAN on the shipping label. Returns sent without a RAN may be refused delivery.&lt;br /&gt;
&lt;br /&gt;
This warranty does not cover hardware that has:&lt;br /&gt;
:• been modified by the user in any way;&lt;br /&gt;
:• been subjected to unusual physical, electrical, or environmental stress. This includes damage due to faulty power sockets, inadequate earthing, or power spikes or surges;&lt;br /&gt;
:• been damaged because of incorrect wiring to ancillary equipment, or because of substandard, connectors or cables; or&lt;br /&gt;
:• had the original identification marks removed or altered.&lt;br /&gt;
&lt;br /&gt;
=== Software License ===&lt;br /&gt;
&lt;br /&gt;
You have the non-exclusive right to use the supplied eDAQ software (Sequencer, Chart etc). Your employees or students, for example, are entitled to use it, provided they adhere to this agreement. &lt;br /&gt;
Each separate purchase of the eDAQ software licenses it to be used on two computers, more than two copies must not be used simultaneously. Departmental/company licences are available if you wish to run more than two copies simultaneously.&lt;br /&gt;
&lt;br /&gt;
=== Technical Support ===&lt;br /&gt;
&lt;br /&gt;
Please register your unit to receive technical support.&lt;br /&gt;
&lt;br /&gt;
Technical assistance is available via email. Please describe the problem with as much detail as possible. Include a small example data file, if appropriate. Please also state:&lt;br /&gt;
: • the model and serial number of your EDAQ system.&lt;br /&gt;
: • the type of computer and operating system being used (for example Windows XP, Vista, Windows 7, 8, or 10)&lt;br /&gt;
: • the software version you are using (for example Chart v5.5.2)&lt;br /&gt;
&lt;br /&gt;
We endeavor to answer all your questions, but in some cases, for example where the problem relates to the other equipment that you are using, a nominal fee may be charged.&lt;br /&gt;
&lt;br /&gt;
=== Jurisdiction ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd is bound by the laws of New South Wales in Australia, and any proceedings shall be heard by the Supreme Court of New South Wales in Australia.&lt;br /&gt;
&lt;br /&gt;
=== Disclaimer ===&lt;br /&gt;
&lt;br /&gt;
eDAQ reserves the right to alter specifications of hardware and software without notice. No liability can be accepted for consequential damages resulting from use of eDAQ products.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3988</id>
		<title>ER430 Manual</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3988"/>
				<updated>2015-08-06T07:41:34Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Operating Modes */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;br /&gt;
== Introduction ==&lt;br /&gt;
[[File:ER430SmallPanels.jpg|thumb|upright=2|right|'''Figure 1.''' ER430 HV Sequencer front and back panels]]&lt;br /&gt;
This manual is intended to allow the user to install, check and run the ER430 HV Sequencer. It provides detailed information on the system and its operation. Please read this manual carefully prior to beginning operation.&lt;br /&gt;
&lt;br /&gt;
The ER430 High Voltage Sequencer provides the following functions:&lt;br /&gt;
::• Four independent programmable metered high voltage (HV) supplies.&lt;br /&gt;
::• Safety Interlock system&lt;br /&gt;
::• Software that allows arbitrary sequences of voltages to be generated&lt;br /&gt;
&lt;br /&gt;
== Checking the Instrument ==&lt;br /&gt;
Before you begin working with the device, you should check:&lt;br /&gt;
:• that the contents of the package you received match the packing list&lt;br /&gt;
:• for any sign of physical damage that might have occurred during transit.&lt;br /&gt;
If you find a problem, please contact your [http://www.edaq.com/edaq-distributors eDAQ distributor] or agent immediately.&lt;br /&gt;
&lt;br /&gt;
== Safety First ==&lt;br /&gt;
&lt;br /&gt;
This equipment generates high voltages of up to 3000 V DC at currents of up to 200 µA. Making contact with such voltages can be extremely dangerous.&lt;br /&gt;
&lt;br /&gt;
Ensure that the high voltage (HV) circuits are housed in an insulated enclosure fitted with an Interlock safety circuit and with no manual access to HV circuits while circuits are alive.&lt;br /&gt;
&lt;br /&gt;
Safety precautions:&lt;br /&gt;
::• Ensure that the safety interlock circuit is connected to the HV Sequencer and is only active and enabled when no accidental access to High Voltage circuits can be made.&lt;br /&gt;
::• Wear rubber soled footwear&lt;br /&gt;
::• Ensure the floor and bench top are dry&lt;br /&gt;
::• Stand on a rubber mat when in the vicinity of high voltages&lt;br /&gt;
&lt;br /&gt;
The ER430 features design precautions to ensure that there is no accidental application of high voltages. These include automatic shutdown in the event of voltage or current overloads . This will in some circumstances prevent the unit from operating. In these cases check all settings and safety interlocks carefully before resuming the experiment.&lt;br /&gt;
&lt;br /&gt;
=== What is an Interlock ===&lt;br /&gt;
&lt;br /&gt;
An interlock is a mechanical or electrical system that prevents the inadvertent operation of of an instrument.&lt;br /&gt;
&lt;br /&gt;
In the case of the  ER430 HV Sequencer this is achieved by using a switch located in the enclosure in which high voltages are active.  This switch is connected via a cable to the front panel INTERLOCK BNC in such a way that the switch is only closed when no access is available to the High voltages inside the enclosure.&lt;br /&gt;
&lt;br /&gt;
For example with the eDAQ supplied ET225 Micronit Chip Electrophoresis Platform, high voltages can only be applied when the top cover is in place.  This is detected and the interlock switch enabled to allow the application of high voltages.&lt;br /&gt;
&lt;br /&gt;
If the user is providing the MicroChip enclosure then it is the user’s responsibility to provide the required interlock function.&lt;br /&gt;
&lt;br /&gt;
To test the Interlock function it is sufficient to apply a short circuit across the INTERLOCK BNC input pins.  This should only be done with no connections to the High Voltage input connectors.&lt;br /&gt;
ER430 &lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
System indicators as shown in the preceding diagram provide a direct indication of system operation that reflects the state of the internal hardware.  These indicators will assist you in monitoring system operation and in diagnosing problems – study them carefully:  &lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED: Amber LED&lt;br /&gt;
	FLASHING = Interlock open, unit disarmed, arming not enabled.&lt;br /&gt;
	OFF = Interlock in place and enabled, unit can be ARMED.&lt;br /&gt;
	ON = Interlock in place, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
SYSTEM STATUS LED: RGB LED (Multicoloured)&lt;br /&gt;
GREEN when “on line” and ready as a Master&lt;br /&gt;
BLUE when ready as a Slave&lt;br /&gt;
&lt;br /&gt;
METER FUNCTION LED: RGB LED&lt;br /&gt;
GREEN:  Safe (disconnected) &lt;br /&gt;
YELLOW:  Current Mode&lt;br /&gt;
BLUE:  Voltage mode&lt;br /&gt;
&lt;br /&gt;
HV STATUS: RED LED&lt;br /&gt;
OFF: supply disconnected&lt;br /&gt;
ON: supply connected and active.&lt;br /&gt;
&lt;br /&gt;
Notes: &lt;br /&gt;
#On power up the system performs a startup test and flashes the front panel LEDs through the various colors available for display.&lt;br /&gt;
# In some cases where the HV supply needs to be used in proximity to light sensitive detectors it is possible to optionally turn off all the LEDs to maintain low background illumination.&lt;br /&gt;
 &lt;br /&gt;
== Hardware Installation ==&lt;br /&gt;
'''ATTENTION:''' When installing the system for the first time ALWAYS perform software installation before connecting the hardware units.  This ensures that the correct drivers are installed &lt;br /&gt;
 &lt;br /&gt;
After carrying out the software installation described in the next section, perform the following Hardware installation procedure. It will confirm that:&lt;br /&gt;
::• That safety interlocks are in place and functioning correctly&lt;br /&gt;
::• The unit can be armed and disarmed&lt;br /&gt;
&lt;br /&gt;
Operation:&lt;br /&gt;
::• '''Safety first''' Connect the unit to a good ground using the terminal post on the rear of the unit.&lt;br /&gt;
::• Connect the unit to the 12V DC mains power pack.&lt;br /&gt;
::• Connect the unit to the PC using the USB cable provided.&lt;br /&gt;
::• Turn Power on.&lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED will flash if interlock is not enabled.&lt;br /&gt;
&lt;br /&gt;
HV Status LEDs: Off (no high voltage output)&lt;br /&gt;
&lt;br /&gt;
STATUS LEDs: Green&lt;br /&gt;
&lt;br /&gt;
=== TEST INTERLOCK Function ===&lt;br /&gt;
&lt;br /&gt;
This function can be tested without any software running:&lt;br /&gt;
::• The INTERLOCK LED will initially be flashing.&lt;br /&gt;
::• Connect a short circuit to the INTERLOCK BNC.&lt;br /&gt;
::• INTERLOCK LED will turn OFF.&lt;br /&gt;
::• Press the ARM Push Button for approximately 1 to 2 seconds.  You should hear a beep, warning you that the HV outputs have been armed (enabled) and the INTERLOCK LED will turn ON.&lt;br /&gt;
::• At this point all HV supplies are still inactive but are in a state where they can be set and controlled by the Sequencer Application software.&lt;br /&gt;
::• Pressing the Arm button again will DISARM the HV Sequencer, and the INTEROCK LED will turn off.&lt;br /&gt;
&lt;br /&gt;
A momentary push on  the Arm button will disable all the HV outputs of the Sequencer.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== INTERLOCK features ===&lt;br /&gt;
The system is provided with a number of safety features or Interlocks:&lt;br /&gt;
::• Chip adapter interlock:  The chip adapter used should provide a safety contact interlock to indicate that the microchip adapter is safe for use.  This interlock is a contact closure switch, which is closed when the HV circuit is fully enclosed and protected from user access. This interlock is connected to the front panel Interlock BNC and indicates to the ER430 that it is safe to arm the system.&lt;br /&gt;
::• USB Present:  The system cannot be ARMED without an active USB connection&lt;br /&gt;
::• Software Control: Once the system is ARMED High Voltages can only be applied under software control.&lt;br /&gt;
::• ARM circuit: prior to applying HV to an external circuit the system must be armed by the user by depressing the front panel ARM push button for approximately 2 seconds.&lt;br /&gt;
::• DISARM: The system can be disarmed by a momentary push of the ARM button.&lt;br /&gt;
::• Power Overloads:  the circuit detects power overloads and situations that lead to the generation of arcs (sparks).  The system will switch itself off in such circumstances and in such circumstances may require to be reinitiated with power being turned on Off and On.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION:'''  Do not disconnect HV leads by hand while High voltages are present – this is extremely dangerous and can cause harmful arcs to be generated. To disable power use the ARM/DISARM front panel button or the software’s Disarm or Disconnect menu items&lt;br /&gt;
&lt;br /&gt;
You are now ready to operate the Sequencer software which will allow you to generate and output a series of high voltage pulses and ramps.&lt;br /&gt;
&lt;br /&gt;
== Software Installation &amp;amp; Operation ==&lt;br /&gt;
&lt;br /&gt;
=== Installing the HV Sequencer software ===&lt;br /&gt;
Insert the HV Sequencer installation USB stick into your computer.  It is recommended to install the software before plugging in the hardware, as it ensures the drivers are correctly installed.&lt;br /&gt;
&lt;br /&gt;
The eDAQ Sequencer Setup Wizard will display a start-up screen; follow the prompts to install the software.&lt;br /&gt;
      Start up screen&lt;br /&gt;
			    Final Start up screen&lt;br /&gt;
&lt;br /&gt;
=== eDAQ Sequencer Overview ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Sequencer is a Windows application that provides the means to setup a series of steps that are executed under computer control.  The following functions are provided:&lt;br /&gt;
&lt;br /&gt;
System setup and sequence entry: The software identifies system configuration on startup and allows the operating parameters to be set immediately.&lt;br /&gt;
&lt;br /&gt;
Table driven Sequence: A time based table is filled out, specifying that the operations to be performed in sequence.  This includes setting of HV supplies to new voltages, trigger and digital I/O line functions. The following sequence operations are implemented: &lt;br /&gt;
&lt;br /&gt;
Time: set to xxxx seconds&lt;br /&gt;
Meter 1&amp;amp;2: Disconnect, Read V, Read I&lt;br /&gt;
Output1&amp;amp;2: Set V=xxxx (V and I monitored), Read V, Read I&lt;br /&gt;
Digital Out: Low/Open, High/Closed, Short Pulse, Long Pulse&lt;br /&gt;
Special commands: Wait for trigger, Wait for Arming, Go Safe&lt;br /&gt;
New functions can be readily added to meet customer requirements&lt;br /&gt;
&lt;br /&gt;
Digital outputs can be used to control external devices or the recording of data in an ecorder.&lt;br /&gt;
&lt;br /&gt;
Monitoring: Once a sequence is started the user is able to observe the progress of the sequence on the sequence table.  Values of HV supply voltages and currents are displayed during operation.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
 === HV Sequencer Main Window ===&lt;br /&gt;
&lt;br /&gt;
  &lt;br /&gt;
=== Communication ===&lt;br /&gt;
&lt;br /&gt;
The HV sequencer uses a virtual USB serial communications (COM) port.  When the ER430 hardware is first attached to USB, a free COM port number is automatically assigned by Windows.  That COM port will be then used every time that unit is plugged in again.&lt;br /&gt;
&lt;br /&gt;
Note:  the first time you connect the system to the computer it may take some time for the system to identify the HV sequencer device driver and install it.  You will be notified when the device is ready.&lt;br /&gt;
&lt;br /&gt;
The first time you use the sequencer software, you need to specify the COM port that the hardware has been assigned.  Select the Preferences option in the File menu, then choose your HV Sequencer in the list at the top – see screen shot below. This preference is automatically saved for future use&lt;br /&gt;
&lt;br /&gt;
  Preferences panel&lt;br /&gt;
&lt;br /&gt;
If you are uncertain about which COM port to assign use, the Serial Port Monitor application can help identify the COM port assigned to the HV sequencer. This small application is included on the HV Sequencer installer USB stick, and can also be downloaded from the eDAQ Utilities and Tools download webpage:&lt;br /&gt;
&lt;br /&gt;
	[[http://www.edaq.com/utilities_tools.php www.edaq.com/utilities_tools.php]]&lt;br /&gt;
&lt;br /&gt;
The serial port monitor runs as an icon in the notification area.  Clicking on it will show a list of eDAQ COM port devices attached to your computer.&lt;br /&gt;
&lt;br /&gt;
The other Preference options set the digital output type, and provide control over front panel lights in situations where light pollution needs to be kept to a minimum.&lt;br /&gt;
&lt;br /&gt;
Check if you have installed an interlock as described previously.  The INTERLOCK LED should be OFF indicating that the INTERLOCK is in place.&lt;br /&gt;
    &lt;br /&gt;
&lt;br /&gt;
Click the Online in the menu bar to attach the selected ER430 unit to the Sequencer application. &lt;br /&gt;
&lt;br /&gt;
Click the Offline in the menu bar to disconnect the selected ER430 unit from the Sequencer application.&lt;br /&gt;
 &lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
=== Disarming and Interlock Test ===&lt;br /&gt;
&lt;br /&gt;
Press and hold the red ARM button to arm the unit.  As before, the unit will beep and arm itself.  This will also be shown in the software’s display.&lt;br /&gt;
&lt;br /&gt;
You can now disarm the unit by either:&lt;br /&gt;
::• Pressing the red ARM button again&lt;br /&gt;
::• Clicking “Disarm” in the top-right of the software window.&lt;br /&gt;
&lt;br /&gt;
While the unit is armed, you can test the safety interlock by removing the short-circuit from the BNC connector.  The unit should immediately disarm itself, disconnecting the outputs, and turning off any applied voltages.&lt;br /&gt;
&lt;br /&gt;
=== Manual Settings ===&lt;br /&gt;
After arming the unit, click on the More… button to display the controls for making immediate changes to the unit.&lt;br /&gt;
&lt;br /&gt;
The right hand side of the HV Sequencer setup panel provides the means to manually set meter functions, output voltages, and the digital outputs’ states.  Make some selections, and then click on Set.  The ER430 hardware will immediately apply the settings you have chosen, and the software will display your choices, along with readings of current and/or voltage.&lt;br /&gt;
&lt;br /&gt;
At this point  the system will indicate the voltages set and currents measured.  Since no loads are yet connected, the currents will be very near zero. &lt;br /&gt;
&lt;br /&gt;
=== Setup panel ===&lt;br /&gt;
&lt;br /&gt;
At any time, pressing the Disarm button in the top-right hand corner of the Main Window or the red button on the front panel of the ER430 will disarm the unit and make it safe.  &lt;br /&gt;
&lt;br /&gt;
After disarming, you must press and hold the red button (as before) to re-arm it.  The software can not re-arm the device.&lt;br /&gt;
&lt;br /&gt;
Outputs let you control the digital outputs of the unit.  In the preference you can set Output configuration as contact closure, or TTL.&lt;br /&gt;
HV Sequences&lt;br /&gt;
The lower area of the Setup panel provides the means to define a “program” or “sequence” to run. This consists of a number of timed steps, each of which can update the state of one or more of the individual functions or outputs.  There are also some “special” commands that can be carried out. Unused connections can have the width of their columns reduced by dragging their column separator.&lt;br /&gt;
&lt;br /&gt;
All changes on a step happen simultaneously (within 2 milliseconds).&lt;br /&gt;
   Setup screen with an example&lt;br /&gt;
&lt;br /&gt;
Here is another example program:&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
If a step doesn’t have anything entered in its box, the output will remain unchanged from its previous setting.&lt;br /&gt;
&lt;br /&gt;
A time of “0” means “immediately upon starting”, and the times are cumulative, measured from when the sequence was started,  i.e.: the delay between the first four of the lines above is 5, 3, and 4 seconds respectively.&lt;br /&gt;
&lt;br /&gt;
It is recommended to have the first row setting every output to a known state, in case the previous run was stopped part-way through, leaving the unit in an unknown state.&lt;br /&gt;
&lt;br /&gt;
When the program finishes, the unit will be left in whatever state it was at the end.  It will not automatically disconnect or disarm the outputs, unless explicitly told to do so.&lt;br /&gt;
The Meter channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal (LED GREEN)&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE)&lt;br /&gt;
Read I:  Current Meter connection (LED YELLOW)&lt;br /&gt;
The Output channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal.&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE).&lt;br /&gt;
Read I: Current meter connection (LED YELLOW)&lt;br /&gt;
Set V: Set the voltage to the value entered in the second column – In this mode the Voltage indicated will be the actual voltage produced within 1%. (LED RED)&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
Digital outputs can be set to:&lt;br /&gt;
Low/Open: Output goes low or open, as per the “digital output mode” setting in Preferences. &lt;br /&gt;
High/Closed: Output goes high or closed.&lt;br /&gt;
&lt;br /&gt;
The type of digital output, TTL or Contact Closure, is set from the Preferences dialog in the File menu.&lt;br /&gt;
&lt;br /&gt;
Special is a special function to be performed.  You can either:&lt;br /&gt;
::• Disarm: Disconnect HV supplies, and stop the program, or&lt;br /&gt;
::• Wait for trigger: Pause, and wait for a high/close on the rear panel’s green connector “Trigger” pins.&lt;br /&gt;
&lt;br /&gt;
Simple editing commands are available on the Edit menu.  The option to Always show the slave will force the display of the second control panel and additional program columns, even if a second unit is not attached.&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
Programs can be saved and loaded using the menu options in the File menu. &lt;br /&gt;
&lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
Once you are satisfied with your program, click the Run button in the menu bar.  The software will step through the program, executing each step at the given time after starting.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Pause button can be used to pause running of the program.  The Run button changes to a Resume button, which you can click to continue execution.&lt;br /&gt;
Stop will stop execution, but it will leave the unit in the current state, with whatever voltages selected still being output.&lt;br /&gt;
The Disarm button will stop any running program and put the ER430 hardware into a safe state.&lt;br /&gt;
Various fault and safety switch conditions will also force a disarming (and termination of program), including:&lt;br /&gt;
•	USB cable being removed&lt;br /&gt;
•	Front panel safety interlock opened/removed&lt;br /&gt;
•	Front panel red button being pressed&lt;br /&gt;
•	When operating with a slave unit, disconnection from the slave unit&lt;br /&gt;
&lt;br /&gt;
=== Modes of Operation ===&lt;br /&gt;
&lt;br /&gt;
==== General ====&lt;br /&gt;
::• Disarmed/Safe – High voltages and meters disconnected  &lt;br /&gt;
::• Armed- High voltages are active and available for connection to external circuit.&lt;br /&gt;
&lt;br /&gt;
==== Programmable HV power supplies ====&lt;br /&gt;
Output Voltage:  Adjustable from ±200V to ±3000V at up to 200µA. &lt;br /&gt;
Output Polarity:  Positive or Negative with respect to the common ground potential&lt;br /&gt;
&lt;br /&gt;
==== Operating Modes ====&lt;br /&gt;
::• O/C mode: Open Circuit by disconnection with high voltage relay.&lt;br /&gt;
::• Voltage Mode: High voltage output mode with current and voltage monitoring&lt;br /&gt;
::• HiZ Mode: Voltage monitoring – 10 Meohm impedance&lt;br /&gt;
::• S/C Mode: Short circuit to ground with current monitoring&lt;br /&gt;
&lt;br /&gt;
==== Meters ====&lt;br /&gt;
Operating Modes&lt;br /&gt;
O/C mode: Circuit disconnected by high voltage relay&lt;br /&gt;
HiZ Mode: Voltage monitoring – 100Meg impedance&lt;br /&gt;
S/C Mode: Short circuit to ground with current monitoring &lt;br /&gt;
&lt;br /&gt;
By combining the HV power supplies and meters it is possible to setup the conditions which load the sample into the separation channel and then apply the appropriate voltages to cause separation and detection of the sample components as shown in the example.&lt;br /&gt;
&lt;br /&gt;
=== Typical Installation ===&lt;br /&gt;
 &lt;br /&gt;
 &lt;br /&gt;
== ER430 HV Hardware ==&lt;br /&gt;
&lt;br /&gt;
=== ER430 HV Channel Block Diagram ===&lt;br /&gt;
A Block diagram of a HV supply channel is shown below; there are four identical HV channels in each ER430unit:&lt;br /&gt;
 &lt;br /&gt;
=== ER430 Meter Channel block diagram ===&lt;br /&gt;
&lt;br /&gt;
=== Green Connector Pin Numbers ===&lt;br /&gt;
&lt;br /&gt;
ER430 HV Sequencer “green” connector Pin functions&lt;br /&gt;
&lt;br /&gt;
1	TRIG +	TTL  IN	11	HV 1 E	HV VOLTAGE  MONITOR 1&lt;br /&gt;
2	TRIG -	TTL COM	12	HV 1 I	HV CURRENT MONITOR 1&lt;br /&gt;
3	HV4  E	HV VOLTAGE  MONITOR 4	13	CTL1 +	DIGITAL  IN/OUT 1&lt;br /&gt;
4	HV4  I	HV CURRENT MONITOR 4	14	CTL1 -	DIGITAL COM&lt;br /&gt;
5	COM	COMMON	15	CTL2 +	DIGITAL  IN/OUT 2&lt;br /&gt;
6	HV3 E	HV VOLTAGE  MONITOR 3	16	CTL2 -	DIGITAL COM&lt;br /&gt;
7	HV3  I	HV CURRENT MONITOR 3	17	CTL3+	DIGITAL  IN/OUT 3&lt;br /&gt;
8	HV 2 E	HV VOLTAGE  MONITOR 2	18	CTL3 -	DIGITAL COM&lt;br /&gt;
9	HV 2  I	HV CURRENT MONITOR 2	19	CTL4 +	DIGITAL  IN/OUT 4&lt;br /&gt;
10	COM	COMMON	20	CTL4 -	DIGITAL COM&lt;br /&gt;
&lt;br /&gt;
Notes:&lt;br /&gt;
# Digital I/O pins are implemented as contact closure or TTL outputs, software selectable&lt;br /&gt;
# Trigger input can be a contact closure or TTL input&lt;br /&gt;
# HV VOLTAGE  MONITOR scale factor: 500mV/kV&lt;br /&gt;
# HV Current Monitor Scale factor: 100mV/mA&lt;br /&gt;
&lt;br /&gt;
== Specifications==&lt;br /&gt;
&lt;br /&gt;
=== High Voltage Output and Mode Options ===&lt;br /&gt;
&lt;br /&gt;
::• Channels: 4&lt;br /&gt;
::• Model: UR3*&lt;br /&gt;
::• Maximum Voltage Setting: ±3000 V&lt;br /&gt;
::• Minimum Voltage Setting: ±200 V&lt;br /&gt;
::• Current: ±200 µA max&lt;br /&gt;
::• Ripple: 0.1%		&lt;br /&gt;
::• Operating Modes: Applied voltage, Open Circuit (O/C), and Short Circuit (S/C)		&lt;br /&gt;
::• Load regulation: &amp;lt;2% specified for 20-90% full load: &lt;br /&gt;
::• Rise and Fall times: &amp;lt;5 ms specified for changes within the same polarity regime&lt;br /&gt;
::• Mode Change: &amp;lt;100ms due to relay operations, safety and software latency&lt;br /&gt;
	&lt;br /&gt;
Note: Output is referred to system common (Case Ground)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Safety Features ===&lt;br /&gt;
An interlock is provided on&lt;br /&gt;
::• the mechanical case to ensure that no voltages are present with the case open unless authorized maintenance is in progress.  &lt;br /&gt;
::• the microchip environment to ensure that accidental contact is not made with the high voltages.&lt;br /&gt;
&lt;br /&gt;
The Arm/disarm switch needs to be held for 2 seconds to arm the system and allow high voltages to become active.  Any short contact on the ARM switch will disarm the system.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION''': It is the responsibility of the user to ensure that adequate protection is provided on the equipment provided by the user. eDAQ provides microfluidic chip adaptors with appropriate interlock features.&lt;br /&gt;
&lt;br /&gt;
=== Meter Functions ===&lt;br /&gt;
&lt;br /&gt;
::• Voltage Range:	±3000 V&lt;br /&gt;
::• Voltage Resolution: 1 V&lt;br /&gt;
::• Current Range: ±200 µA&lt;br /&gt;
::• Current resolution: 1 µA&lt;br /&gt;
::• Displayed resolution limited to 1 unit&lt;br /&gt;
&lt;br /&gt;
=== Communications and Inputs and outputs terminals ===&lt;br /&gt;
&lt;br /&gt;
::• Daisy Chain connectors: Twin DB9 connectors allow two (2) ER430 units to be daisy chained together.&lt;br /&gt;
::• USB Port:  Compatible with USB1 &amp;amp; USB 2 and provides, communications facility to PC’s&lt;br /&gt;
::• Output and Meters front panel connectors:  SHV (Safe High Voltage)  type &lt;br /&gt;
::• 20 Way 3.5mm Green screw terminal: &lt;br /&gt;
:::: - Four Digital I/O lines&lt;br /&gt;
:::: - Trigger TTL or CC&lt;br /&gt;
:::: - Four Voltage Monitor signals&lt;br /&gt;
:::: - FourCurrent  Monitor signals.&lt;br /&gt;
::• System/Chassis Earth terminal: 4 mm screw terminal.&lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
&lt;br /&gt;
The following LED front panel displays are available:&lt;br /&gt;
&lt;br /&gt;
::•  System Status (RGB LED)&lt;br /&gt;
::: GREEN when “on line” &lt;br /&gt;
&lt;br /&gt;
::• Interlock (amber LED)&lt;br /&gt;
::: FLASHING = Interlock open, unit disarmed, arming not allowed.&lt;br /&gt;
::: OFF = Interlock OK, unit disarmed&lt;br /&gt;
::: ON = Interlock OK, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
::• Meter Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (disconnected) &lt;br /&gt;
:::: YELLOW = Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (supply disconnected) &lt;br /&gt;
:::: YELLOW =  Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Status  (RGB LED)&lt;br /&gt;
:::: OFF = supply disconnected&lt;br /&gt;
:::: ON = supply connected and active.&lt;br /&gt;
&lt;br /&gt;
=== Physical ===&lt;br /&gt;
::• Dimensions (w x h x d): 200 x 65 x 250 mm (7.9 x 2.6 x 9.8 inch)&lt;br /&gt;
::• Weight: 3.00 kg packed&lt;br /&gt;
::• Operating temperature: 0 - 35ºC&lt;br /&gt;
::• Humidity: 10 to 80% non condensing &lt;br /&gt;
::• Power:  9 - 16 V @ 2 A maximum supplied by mains powered AC/DC converter (supplied)&lt;br /&gt;
&lt;br /&gt;
== Legal and Warranty ==&lt;br /&gt;
&lt;br /&gt;
=== Trademarks and Copyright ===&lt;br /&gt;
Sequencer, HV Sequencer, and Chart are trademarks of eDAQ Pty Ltd.&lt;br /&gt;
Windows XP, Vista, and Windows 7, Windows 8 and Windows 10 are trademarks of Microsoft Corporation.&lt;br /&gt;
This document is Copyright © July 2015. This document, or sections thereof, may be copied by the owners or users of an eDAQ Quad MF isoPod for their private use. Otherwise no part of this document may be&lt;br /&gt;
reproduced by any means without the prior written permission of eDAQ Pty Ltd.&lt;br /&gt;
&lt;br /&gt;
=== Responsibilities ===&lt;br /&gt;
&lt;br /&gt;
You and any others using any eDAQ product agree to use it in a sensible manner for purposes for which it is suited, and agree to take responsibility for their actions and the results of their actions. If problems arise with an eDAQ product, eDAQ will make all reasonable efforts to fix them. This service may incur a charge, depending on the nature of the problems, and is subject to the other conditions in this Agreement.&lt;br /&gt;
&lt;br /&gt;
=== Hardware Warranty ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd warrants this device, to be free of defects in material and workmanship for three years from the date of purchase. Note that this does NOT include external cables and electrodes that are subject to 'wear and tear' and manufacturing defects should be reported within 90 days of purchase. eDAQ Pty Ltd will repair or replace defective equipment as appropriate. To obtain a warranty repair/replacement you must first notify us before return of the instrument and we will issue you with a RAN (return authorisation number). You must ship the defective product at your expense. We will pay return shipping. The product should be packed safely (preferably in its original packaging) and have the RAN on the shipping label. Returns sent without a RAN may be refused delivery.&lt;br /&gt;
&lt;br /&gt;
This warranty does not cover hardware that has:&lt;br /&gt;
:• been modified by the user in any way;&lt;br /&gt;
:• been subjected to unusual physical, electrical, or environmental stress. This includes damage due to faulty power sockets, inadequate earthing, or power spikes or surges;&lt;br /&gt;
:• been damaged because of incorrect wiring to ancillary equipment, or because of substandard, connectors or cables; or&lt;br /&gt;
:• had the original identification marks removed or altered.&lt;br /&gt;
&lt;br /&gt;
=== Software License ===&lt;br /&gt;
&lt;br /&gt;
You have the non-exclusive right to use the supplied eDAQ software (Sequencer, Chart etc). Your employees or students, for example, are entitled to use it, provided they adhere to this agreement. &lt;br /&gt;
Each separate purchase of the eDAQ software licenses it to be used on two computers, more than two copies must not be used simultaneously. Departmental/company licences are available if you wish to run more than two copies simultaneously.&lt;br /&gt;
&lt;br /&gt;
=== Technical Support ===&lt;br /&gt;
&lt;br /&gt;
Please register your unit to receive technical support.&lt;br /&gt;
&lt;br /&gt;
Technical assistance is available via email. Please describe the problem with as much detail as possible. Include a small example data file, if appropriate. Please also state:&lt;br /&gt;
: • the model and serial number of your EDAQ system.&lt;br /&gt;
: • the type of computer and operating system being used (for example Windows XP, Vista, Windows 7, 8, or 10)&lt;br /&gt;
: • the software version you are using (for example Chart v5.5.2)&lt;br /&gt;
&lt;br /&gt;
We endeavor to answer all your questions, but in some cases, for example where the problem relates to the other equipment that you are using, a nominal fee may be charged.&lt;br /&gt;
&lt;br /&gt;
=== Jurisdiction ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd is bound by the laws of New South Wales in Australia, and any proceedings shall be heard by the Supreme Court of New South Wales in Australia.&lt;br /&gt;
&lt;br /&gt;
=== Disclaimer ===&lt;br /&gt;
&lt;br /&gt;
eDAQ reserves the right to alter specifications of hardware and software without notice. No liability can be accepted for consequential damages resulting from use of eDAQ products.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

	<entry>
		<id>https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3987</id>
		<title>ER430 Manual</title>
		<link rel="alternate" type="text/html" href="https://www.edaq.com/w/index.php?title=ER430_Manual&amp;diff=3987"/>
				<updated>2015-08-06T07:39:37Z</updated>
		
		<summary type="html">&lt;p&gt;PaulDuckworth: /* Programmable HV power supplies */&lt;/p&gt;
&lt;hr /&gt;
&lt;div&gt;&lt;br /&gt;
== Introduction ==&lt;br /&gt;
[[File:ER430SmallPanels.jpg|thumb|upright=2|right|'''Figure 1.''' ER430 HV Sequencer front and back panels]]&lt;br /&gt;
This manual is intended to allow the user to install, check and run the ER430 HV Sequencer. It provides detailed information on the system and its operation. Please read this manual carefully prior to beginning operation.&lt;br /&gt;
&lt;br /&gt;
The ER430 High Voltage Sequencer provides the following functions:&lt;br /&gt;
::• Four independent programmable metered high voltage (HV) supplies.&lt;br /&gt;
::• Safety Interlock system&lt;br /&gt;
::• Software that allows arbitrary sequences of voltages to be generated&lt;br /&gt;
&lt;br /&gt;
== Checking the Instrument ==&lt;br /&gt;
Before you begin working with the device, you should check:&lt;br /&gt;
:• that the contents of the package you received match the packing list&lt;br /&gt;
:• for any sign of physical damage that might have occurred during transit.&lt;br /&gt;
If you find a problem, please contact your [http://www.edaq.com/edaq-distributors eDAQ distributor] or agent immediately.&lt;br /&gt;
&lt;br /&gt;
== Safety First ==&lt;br /&gt;
&lt;br /&gt;
This equipment generates high voltages of up to 3000 V DC at currents of up to 200 µA. Making contact with such voltages can be extremely dangerous.&lt;br /&gt;
&lt;br /&gt;
Ensure that the high voltage (HV) circuits are housed in an insulated enclosure fitted with an Interlock safety circuit and with no manual access to HV circuits while circuits are alive.&lt;br /&gt;
&lt;br /&gt;
Safety precautions:&lt;br /&gt;
::• Ensure that the safety interlock circuit is connected to the HV Sequencer and is only active and enabled when no accidental access to High Voltage circuits can be made.&lt;br /&gt;
::• Wear rubber soled footwear&lt;br /&gt;
::• Ensure the floor and bench top are dry&lt;br /&gt;
::• Stand on a rubber mat when in the vicinity of high voltages&lt;br /&gt;
&lt;br /&gt;
The ER430 features design precautions to ensure that there is no accidental application of high voltages. These include automatic shutdown in the event of voltage or current overloads . This will in some circumstances prevent the unit from operating. In these cases check all settings and safety interlocks carefully before resuming the experiment.&lt;br /&gt;
&lt;br /&gt;
=== What is an Interlock ===&lt;br /&gt;
&lt;br /&gt;
An interlock is a mechanical or electrical system that prevents the inadvertent operation of of an instrument.&lt;br /&gt;
&lt;br /&gt;
In the case of the  ER430 HV Sequencer this is achieved by using a switch located in the enclosure in which high voltages are active.  This switch is connected via a cable to the front panel INTERLOCK BNC in such a way that the switch is only closed when no access is available to the High voltages inside the enclosure.&lt;br /&gt;
&lt;br /&gt;
For example with the eDAQ supplied ET225 Micronit Chip Electrophoresis Platform, high voltages can only be applied when the top cover is in place.  This is detected and the interlock switch enabled to allow the application of high voltages.&lt;br /&gt;
&lt;br /&gt;
If the user is providing the MicroChip enclosure then it is the user’s responsibility to provide the required interlock function.&lt;br /&gt;
&lt;br /&gt;
To test the Interlock function it is sufficient to apply a short circuit across the INTERLOCK BNC input pins.  This should only be done with no connections to the High Voltage input connectors.&lt;br /&gt;
ER430 &lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
System indicators as shown in the preceding diagram provide a direct indication of system operation that reflects the state of the internal hardware.  These indicators will assist you in monitoring system operation and in diagnosing problems – study them carefully:  &lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED: Amber LED&lt;br /&gt;
	FLASHING = Interlock open, unit disarmed, arming not enabled.&lt;br /&gt;
	OFF = Interlock in place and enabled, unit can be ARMED.&lt;br /&gt;
	ON = Interlock in place, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
SYSTEM STATUS LED: RGB LED (Multicoloured)&lt;br /&gt;
GREEN when “on line” and ready as a Master&lt;br /&gt;
BLUE when ready as a Slave&lt;br /&gt;
&lt;br /&gt;
METER FUNCTION LED: RGB LED&lt;br /&gt;
GREEN:  Safe (disconnected) &lt;br /&gt;
YELLOW:  Current Mode&lt;br /&gt;
BLUE:  Voltage mode&lt;br /&gt;
&lt;br /&gt;
HV STATUS: RED LED&lt;br /&gt;
OFF: supply disconnected&lt;br /&gt;
ON: supply connected and active.&lt;br /&gt;
&lt;br /&gt;
Notes: &lt;br /&gt;
#On power up the system performs a startup test and flashes the front panel LEDs through the various colors available for display.&lt;br /&gt;
# In some cases where the HV supply needs to be used in proximity to light sensitive detectors it is possible to optionally turn off all the LEDs to maintain low background illumination.&lt;br /&gt;
 &lt;br /&gt;
== Hardware Installation ==&lt;br /&gt;
'''ATTENTION:''' When installing the system for the first time ALWAYS perform software installation before connecting the hardware units.  This ensures that the correct drivers are installed &lt;br /&gt;
 &lt;br /&gt;
After carrying out the software installation described in the next section, perform the following Hardware installation procedure. It will confirm that:&lt;br /&gt;
::• That safety interlocks are in place and functioning correctly&lt;br /&gt;
::• The unit can be armed and disarmed&lt;br /&gt;
&lt;br /&gt;
Operation:&lt;br /&gt;
::• '''Safety first''' Connect the unit to a good ground using the terminal post on the rear of the unit.&lt;br /&gt;
::• Connect the unit to the 12V DC mains power pack.&lt;br /&gt;
::• Connect the unit to the PC using the USB cable provided.&lt;br /&gt;
::• Turn Power on.&lt;br /&gt;
&lt;br /&gt;
INTERLOCK LED will flash if interlock is not enabled.&lt;br /&gt;
&lt;br /&gt;
HV Status LEDs: Off (no high voltage output)&lt;br /&gt;
&lt;br /&gt;
STATUS LEDs: Green&lt;br /&gt;
&lt;br /&gt;
=== TEST INTERLOCK Function ===&lt;br /&gt;
&lt;br /&gt;
This function can be tested without any software running:&lt;br /&gt;
::• The INTERLOCK LED will initially be flashing.&lt;br /&gt;
::• Connect a short circuit to the INTERLOCK BNC.&lt;br /&gt;
::• INTERLOCK LED will turn OFF.&lt;br /&gt;
::• Press the ARM Push Button for approximately 1 to 2 seconds.  You should hear a beep, warning you that the HV outputs have been armed (enabled) and the INTERLOCK LED will turn ON.&lt;br /&gt;
::• At this point all HV supplies are still inactive but are in a state where they can be set and controlled by the Sequencer Application software.&lt;br /&gt;
::• Pressing the Arm button again will DISARM the HV Sequencer, and the INTEROCK LED will turn off.&lt;br /&gt;
&lt;br /&gt;
A momentary push on  the Arm button will disable all the HV outputs of the Sequencer.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== INTERLOCK features ===&lt;br /&gt;
The system is provided with a number of safety features or Interlocks:&lt;br /&gt;
::• Chip adapter interlock:  The chip adapter used should provide a safety contact interlock to indicate that the microchip adapter is safe for use.  This interlock is a contact closure switch, which is closed when the HV circuit is fully enclosed and protected from user access. This interlock is connected to the front panel Interlock BNC and indicates to the ER430 that it is safe to arm the system.&lt;br /&gt;
::• USB Present:  The system cannot be ARMED without an active USB connection&lt;br /&gt;
::• Software Control: Once the system is ARMED High Voltages can only be applied under software control.&lt;br /&gt;
::• ARM circuit: prior to applying HV to an external circuit the system must be armed by the user by depressing the front panel ARM push button for approximately 2 seconds.&lt;br /&gt;
::• DISARM: The system can be disarmed by a momentary push of the ARM button.&lt;br /&gt;
::• Power Overloads:  the circuit detects power overloads and situations that lead to the generation of arcs (sparks).  The system will switch itself off in such circumstances and in such circumstances may require to be reinitiated with power being turned on Off and On.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION:'''  Do not disconnect HV leads by hand while High voltages are present – this is extremely dangerous and can cause harmful arcs to be generated. To disable power use the ARM/DISARM front panel button or the software’s Disarm or Disconnect menu items&lt;br /&gt;
&lt;br /&gt;
You are now ready to operate the Sequencer software which will allow you to generate and output a series of high voltage pulses and ramps.&lt;br /&gt;
&lt;br /&gt;
== Software Installation &amp;amp; Operation ==&lt;br /&gt;
&lt;br /&gt;
=== Installing the HV Sequencer software ===&lt;br /&gt;
Insert the HV Sequencer installation USB stick into your computer.  It is recommended to install the software before plugging in the hardware, as it ensures the drivers are correctly installed.&lt;br /&gt;
&lt;br /&gt;
The eDAQ Sequencer Setup Wizard will display a start-up screen; follow the prompts to install the software.&lt;br /&gt;
      Start up screen&lt;br /&gt;
			    Final Start up screen&lt;br /&gt;
&lt;br /&gt;
=== eDAQ Sequencer Overview ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Sequencer is a Windows application that provides the means to setup a series of steps that are executed under computer control.  The following functions are provided:&lt;br /&gt;
&lt;br /&gt;
System setup and sequence entry: The software identifies system configuration on startup and allows the operating parameters to be set immediately.&lt;br /&gt;
&lt;br /&gt;
Table driven Sequence: A time based table is filled out, specifying that the operations to be performed in sequence.  This includes setting of HV supplies to new voltages, trigger and digital I/O line functions. The following sequence operations are implemented: &lt;br /&gt;
&lt;br /&gt;
Time: set to xxxx seconds&lt;br /&gt;
Meter 1&amp;amp;2: Disconnect, Read V, Read I&lt;br /&gt;
Output1&amp;amp;2: Set V=xxxx (V and I monitored), Read V, Read I&lt;br /&gt;
Digital Out: Low/Open, High/Closed, Short Pulse, Long Pulse&lt;br /&gt;
Special commands: Wait for trigger, Wait for Arming, Go Safe&lt;br /&gt;
New functions can be readily added to meet customer requirements&lt;br /&gt;
&lt;br /&gt;
Digital outputs can be used to control external devices or the recording of data in an ecorder.&lt;br /&gt;
&lt;br /&gt;
Monitoring: Once a sequence is started the user is able to observe the progress of the sequence on the sequence table.  Values of HV supply voltages and currents are displayed during operation.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
 === HV Sequencer Main Window ===&lt;br /&gt;
&lt;br /&gt;
  &lt;br /&gt;
=== Communication ===&lt;br /&gt;
&lt;br /&gt;
The HV sequencer uses a virtual USB serial communications (COM) port.  When the ER430 hardware is first attached to USB, a free COM port number is automatically assigned by Windows.  That COM port will be then used every time that unit is plugged in again.&lt;br /&gt;
&lt;br /&gt;
Note:  the first time you connect the system to the computer it may take some time for the system to identify the HV sequencer device driver and install it.  You will be notified when the device is ready.&lt;br /&gt;
&lt;br /&gt;
The first time you use the sequencer software, you need to specify the COM port that the hardware has been assigned.  Select the Preferences option in the File menu, then choose your HV Sequencer in the list at the top – see screen shot below. This preference is automatically saved for future use&lt;br /&gt;
&lt;br /&gt;
  Preferences panel&lt;br /&gt;
&lt;br /&gt;
If you are uncertain about which COM port to assign use, the Serial Port Monitor application can help identify the COM port assigned to the HV sequencer. This small application is included on the HV Sequencer installer USB stick, and can also be downloaded from the eDAQ Utilities and Tools download webpage:&lt;br /&gt;
&lt;br /&gt;
	[[http://www.edaq.com/utilities_tools.php www.edaq.com/utilities_tools.php]]&lt;br /&gt;
&lt;br /&gt;
The serial port monitor runs as an icon in the notification area.  Clicking on it will show a list of eDAQ COM port devices attached to your computer.&lt;br /&gt;
&lt;br /&gt;
The other Preference options set the digital output type, and provide control over front panel lights in situations where light pollution needs to be kept to a minimum.&lt;br /&gt;
&lt;br /&gt;
Check if you have installed an interlock as described previously.  The INTERLOCK LED should be OFF indicating that the INTERLOCK is in place.&lt;br /&gt;
    &lt;br /&gt;
&lt;br /&gt;
Click the Online in the menu bar to attach the selected ER430 unit to the Sequencer application. &lt;br /&gt;
&lt;br /&gt;
Click the Offline in the menu bar to disconnect the selected ER430 unit from the Sequencer application.&lt;br /&gt;
 &lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
=== Disarming and Interlock Test ===&lt;br /&gt;
&lt;br /&gt;
Press and hold the red ARM button to arm the unit.  As before, the unit will beep and arm itself.  This will also be shown in the software’s display.&lt;br /&gt;
&lt;br /&gt;
You can now disarm the unit by either:&lt;br /&gt;
::• Pressing the red ARM button again&lt;br /&gt;
::• Clicking “Disarm” in the top-right of the software window.&lt;br /&gt;
&lt;br /&gt;
While the unit is armed, you can test the safety interlock by removing the short-circuit from the BNC connector.  The unit should immediately disarm itself, disconnecting the outputs, and turning off any applied voltages.&lt;br /&gt;
&lt;br /&gt;
=== Manual Settings ===&lt;br /&gt;
After arming the unit, click on the More… button to display the controls for making immediate changes to the unit.&lt;br /&gt;
&lt;br /&gt;
The right hand side of the HV Sequencer setup panel provides the means to manually set meter functions, output voltages, and the digital outputs’ states.  Make some selections, and then click on Set.  The ER430 hardware will immediately apply the settings you have chosen, and the software will display your choices, along with readings of current and/or voltage.&lt;br /&gt;
&lt;br /&gt;
At this point  the system will indicate the voltages set and currents measured.  Since no loads are yet connected, the currents will be very near zero. &lt;br /&gt;
&lt;br /&gt;
=== Setup panel ===&lt;br /&gt;
&lt;br /&gt;
At any time, pressing the Disarm button in the top-right hand corner of the Main Window or the red button on the front panel of the ER430 will disarm the unit and make it safe.  &lt;br /&gt;
&lt;br /&gt;
After disarming, you must press and hold the red button (as before) to re-arm it.  The software can not re-arm the device.&lt;br /&gt;
&lt;br /&gt;
Outputs let you control the digital outputs of the unit.  In the preference you can set Output configuration as contact closure, or TTL.&lt;br /&gt;
HV Sequences&lt;br /&gt;
The lower area of the Setup panel provides the means to define a “program” or “sequence” to run. This consists of a number of timed steps, each of which can update the state of one or more of the individual functions or outputs.  There are also some “special” commands that can be carried out. Unused connections can have the width of their columns reduced by dragging their column separator.&lt;br /&gt;
&lt;br /&gt;
All changes on a step happen simultaneously (within 2 milliseconds).&lt;br /&gt;
   Setup screen with an example&lt;br /&gt;
&lt;br /&gt;
Here is another example program:&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
If a step doesn’t have anything entered in its box, the output will remain unchanged from its previous setting.&lt;br /&gt;
&lt;br /&gt;
A time of “0” means “immediately upon starting”, and the times are cumulative, measured from when the sequence was started,  i.e.: the delay between the first four of the lines above is 5, 3, and 4 seconds respectively.&lt;br /&gt;
&lt;br /&gt;
It is recommended to have the first row setting every output to a known state, in case the previous run was stopped part-way through, leaving the unit in an unknown state.&lt;br /&gt;
&lt;br /&gt;
When the program finishes, the unit will be left in whatever state it was at the end.  It will not automatically disconnect or disarm the outputs, unless explicitly told to do so.&lt;br /&gt;
The Meter channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal (LED GREEN)&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE)&lt;br /&gt;
Read I:  Current Meter connection (LED YELLOW)&lt;br /&gt;
The Output channel functions are:&lt;br /&gt;
Disconnected: Disconnected from the front panel terminal.&lt;br /&gt;
Read V: Voltmeter connection (LED BLUE).&lt;br /&gt;
Read I: Current meter connection (LED YELLOW)&lt;br /&gt;
Set V: Set the voltage to the value entered in the second column – In this mode the Voltage indicated will be the actual voltage produced within 1%. (LED RED)&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
Digital outputs can be set to:&lt;br /&gt;
Low/Open: Output goes low or open, as per the “digital output mode” setting in Preferences. &lt;br /&gt;
High/Closed: Output goes high or closed.&lt;br /&gt;
&lt;br /&gt;
The type of digital output, TTL or Contact Closure, is set from the Preferences dialog in the File menu.&lt;br /&gt;
&lt;br /&gt;
Special is a special function to be performed.  You can either:&lt;br /&gt;
::• Disarm: Disconnect HV supplies, and stop the program, or&lt;br /&gt;
::• Wait for trigger: Pause, and wait for a high/close on the rear panel’s green connector “Trigger” pins.&lt;br /&gt;
&lt;br /&gt;
Simple editing commands are available on the Edit menu.  The option to Always show the slave will force the display of the second control panel and additional program columns, even if a second unit is not attached.&lt;br /&gt;
&lt;br /&gt;
 &lt;br /&gt;
&lt;br /&gt;
Programs can be saved and loaded using the menu options in the File menu. &lt;br /&gt;
&lt;br /&gt;
   &lt;br /&gt;
&lt;br /&gt;
Once you are satisfied with your program, click the Run button in the menu bar.  The software will step through the program, executing each step at the given time after starting.&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
The Pause button can be used to pause running of the program.  The Run button changes to a Resume button, which you can click to continue execution.&lt;br /&gt;
Stop will stop execution, but it will leave the unit in the current state, with whatever voltages selected still being output.&lt;br /&gt;
The Disarm button will stop any running program and put the ER430 hardware into a safe state.&lt;br /&gt;
Various fault and safety switch conditions will also force a disarming (and termination of program), including:&lt;br /&gt;
•	USB cable being removed&lt;br /&gt;
•	Front panel safety interlock opened/removed&lt;br /&gt;
•	Front panel red button being pressed&lt;br /&gt;
•	When operating with a slave unit, disconnection from the slave unit&lt;br /&gt;
&lt;br /&gt;
=== Modes of Operation ===&lt;br /&gt;
&lt;br /&gt;
==== General ====&lt;br /&gt;
::• Disarmed/Safe – High voltages and meters disconnected  &lt;br /&gt;
::• Armed- High voltages are active and available for connection to external circuit.&lt;br /&gt;
&lt;br /&gt;
==== Programmable HV power supplies ====&lt;br /&gt;
Output Voltage:  Adjustable from ±200V to ±3000V at up to 200µA. &lt;br /&gt;
Output Polarity:  Positive or Negative with respect to the common ground potential&lt;br /&gt;
&lt;br /&gt;
==== Operating Modes ====&lt;br /&gt;
O/C mode: Circuit disconnected by high voltage relay.&lt;br /&gt;
Voltage Mode: Voltage mode with current and voltage monitoring&lt;br /&gt;
HiZ Mode: Voltage monitoring – 10Meg impedance&lt;br /&gt;
S/C Mode: Short circuit to ground with current monitoring&lt;br /&gt;
&lt;br /&gt;
==== Meters ====&lt;br /&gt;
Operating Modes&lt;br /&gt;
O/C mode: Circuit disconnected by high voltage relay&lt;br /&gt;
HiZ Mode: Voltage monitoring – 100Meg impedance&lt;br /&gt;
S/C Mode: Short circuit to ground with current monitoring &lt;br /&gt;
&lt;br /&gt;
By combining the HV power supplies and meters it is possible to setup the conditions which load the sample into the separation channel and then apply the appropriate voltages to cause separation and detection of the sample components as shown in the example.&lt;br /&gt;
&lt;br /&gt;
=== Typical Installation ===&lt;br /&gt;
 &lt;br /&gt;
 &lt;br /&gt;
== ER430 HV Hardware ==&lt;br /&gt;
&lt;br /&gt;
=== ER430 HV Channel Block Diagram ===&lt;br /&gt;
A Block diagram of a HV supply channel is shown below; there are four identical HV channels in each ER430unit:&lt;br /&gt;
 &lt;br /&gt;
=== ER430 Meter Channel block diagram ===&lt;br /&gt;
&lt;br /&gt;
=== Green Connector Pin Numbers ===&lt;br /&gt;
&lt;br /&gt;
ER430 HV Sequencer “green” connector Pin functions&lt;br /&gt;
&lt;br /&gt;
1	TRIG +	TTL  IN	11	HV 1 E	HV VOLTAGE  MONITOR 1&lt;br /&gt;
2	TRIG -	TTL COM	12	HV 1 I	HV CURRENT MONITOR 1&lt;br /&gt;
3	HV4  E	HV VOLTAGE  MONITOR 4	13	CTL1 +	DIGITAL  IN/OUT 1&lt;br /&gt;
4	HV4  I	HV CURRENT MONITOR 4	14	CTL1 -	DIGITAL COM&lt;br /&gt;
5	COM	COMMON	15	CTL2 +	DIGITAL  IN/OUT 2&lt;br /&gt;
6	HV3 E	HV VOLTAGE  MONITOR 3	16	CTL2 -	DIGITAL COM&lt;br /&gt;
7	HV3  I	HV CURRENT MONITOR 3	17	CTL3+	DIGITAL  IN/OUT 3&lt;br /&gt;
8	HV 2 E	HV VOLTAGE  MONITOR 2	18	CTL3 -	DIGITAL COM&lt;br /&gt;
9	HV 2  I	HV CURRENT MONITOR 2	19	CTL4 +	DIGITAL  IN/OUT 4&lt;br /&gt;
10	COM	COMMON	20	CTL4 -	DIGITAL COM&lt;br /&gt;
&lt;br /&gt;
Notes:&lt;br /&gt;
# Digital I/O pins are implemented as contact closure or TTL outputs, software selectable&lt;br /&gt;
# Trigger input can be a contact closure or TTL input&lt;br /&gt;
# HV VOLTAGE  MONITOR scale factor: 500mV/kV&lt;br /&gt;
# HV Current Monitor Scale factor: 100mV/mA&lt;br /&gt;
&lt;br /&gt;
== Specifications==&lt;br /&gt;
&lt;br /&gt;
=== High Voltage Output and Mode Options ===&lt;br /&gt;
&lt;br /&gt;
::• Channels: 4&lt;br /&gt;
::• Model: UR3*&lt;br /&gt;
::• Maximum Voltage Setting: ±3000 V&lt;br /&gt;
::• Minimum Voltage Setting: ±200 V&lt;br /&gt;
::• Current: ±200 µA max&lt;br /&gt;
::• Ripple: 0.1%		&lt;br /&gt;
::• Operating Modes: Applied voltage, Open Circuit (O/C), and Short Circuit (S/C)		&lt;br /&gt;
::• Load regulation: &amp;lt;2% specified for 20-90% full load: &lt;br /&gt;
::• Rise and Fall times: &amp;lt;5 ms specified for changes within the same polarity regime&lt;br /&gt;
::• Mode Change: &amp;lt;100ms due to relay operations, safety and software latency&lt;br /&gt;
	&lt;br /&gt;
Note: Output is referred to system common (Case Ground)&lt;br /&gt;
&lt;br /&gt;
&lt;br /&gt;
=== Safety Features ===&lt;br /&gt;
An interlock is provided on&lt;br /&gt;
::• the mechanical case to ensure that no voltages are present with the case open unless authorized maintenance is in progress.  &lt;br /&gt;
::• the microchip environment to ensure that accidental contact is not made with the high voltages.&lt;br /&gt;
&lt;br /&gt;
The Arm/disarm switch needs to be held for 2 seconds to arm the system and allow high voltages to become active.  Any short contact on the ARM switch will disarm the system.&lt;br /&gt;
&lt;br /&gt;
'''CAUTION''': It is the responsibility of the user to ensure that adequate protection is provided on the equipment provided by the user. eDAQ provides microfluidic chip adaptors with appropriate interlock features.&lt;br /&gt;
&lt;br /&gt;
=== Meter Functions ===&lt;br /&gt;
&lt;br /&gt;
::• Voltage Range:	±3000 V&lt;br /&gt;
::• Voltage Resolution: 1 V&lt;br /&gt;
::• Current Range: ±200 µA&lt;br /&gt;
::• Current resolution: 1 µA&lt;br /&gt;
::• Displayed resolution limited to 1 unit&lt;br /&gt;
&lt;br /&gt;
=== Communications and Inputs and outputs terminals ===&lt;br /&gt;
&lt;br /&gt;
::• Daisy Chain connectors: Twin DB9 connectors allow two (2) ER430 units to be daisy chained together.&lt;br /&gt;
::• USB Port:  Compatible with USB1 &amp;amp; USB 2 and provides, communications facility to PC’s&lt;br /&gt;
::• Output and Meters front panel connectors:  SHV (Safe High Voltage)  type &lt;br /&gt;
::• 20 Way 3.5mm Green screw terminal: &lt;br /&gt;
:::: - Four Digital I/O lines&lt;br /&gt;
:::: - Trigger TTL or CC&lt;br /&gt;
:::: - Four Voltage Monitor signals&lt;br /&gt;
:::: - FourCurrent  Monitor signals.&lt;br /&gt;
::• System/Chassis Earth terminal: 4 mm screw terminal.&lt;br /&gt;
&lt;br /&gt;
=== System Indicators ===&lt;br /&gt;
&lt;br /&gt;
The following LED front panel displays are available:&lt;br /&gt;
&lt;br /&gt;
::•  System Status (RGB LED)&lt;br /&gt;
::: GREEN when “on line” &lt;br /&gt;
&lt;br /&gt;
::• Interlock (amber LED)&lt;br /&gt;
::: FLASHING = Interlock open, unit disarmed, arming not allowed.&lt;br /&gt;
::: OFF = Interlock OK, unit disarmed&lt;br /&gt;
::: ON = Interlock OK, unit armed and ready for operation.&lt;br /&gt;
&lt;br /&gt;
::• Meter Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (disconnected) &lt;br /&gt;
:::: YELLOW = Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Function (RGB LED)&lt;br /&gt;
:::: GREEN = Safe (supply disconnected) &lt;br /&gt;
:::: YELLOW =  Current Mode&lt;br /&gt;
:::: BLUE = Voltage Mode&lt;br /&gt;
&lt;br /&gt;
::• HV Supply Status  (RGB LED)&lt;br /&gt;
:::: OFF = supply disconnected&lt;br /&gt;
:::: ON = supply connected and active.&lt;br /&gt;
&lt;br /&gt;
=== Physical ===&lt;br /&gt;
::• Dimensions (w x h x d): 200 x 65 x 250 mm (7.9 x 2.6 x 9.8 inch)&lt;br /&gt;
::• Weight: 3.00 kg packed&lt;br /&gt;
::• Operating temperature: 0 - 35ºC&lt;br /&gt;
::• Humidity: 10 to 80% non condensing &lt;br /&gt;
::• Power:  9 - 16 V @ 2 A maximum supplied by mains powered AC/DC converter (supplied)&lt;br /&gt;
&lt;br /&gt;
== Legal and Warranty ==&lt;br /&gt;
&lt;br /&gt;
=== Trademarks and Copyright ===&lt;br /&gt;
Sequencer, HV Sequencer, and Chart are trademarks of eDAQ Pty Ltd.&lt;br /&gt;
Windows XP, Vista, and Windows 7, Windows 8 and Windows 10 are trademarks of Microsoft Corporation.&lt;br /&gt;
This document is Copyright © July 2015. This document, or sections thereof, may be copied by the owners or users of an eDAQ Quad MF isoPod for their private use. Otherwise no part of this document may be&lt;br /&gt;
reproduced by any means without the prior written permission of eDAQ Pty Ltd.&lt;br /&gt;
&lt;br /&gt;
=== Responsibilities ===&lt;br /&gt;
&lt;br /&gt;
You and any others using any eDAQ product agree to use it in a sensible manner for purposes for which it is suited, and agree to take responsibility for their actions and the results of their actions. If problems arise with an eDAQ product, eDAQ will make all reasonable efforts to fix them. This service may incur a charge, depending on the nature of the problems, and is subject to the other conditions in this Agreement.&lt;br /&gt;
&lt;br /&gt;
=== Hardware Warranty ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd warrants this device, to be free of defects in material and workmanship for three years from the date of purchase. Note that this does NOT include external cables and electrodes that are subject to 'wear and tear' and manufacturing defects should be reported within 90 days of purchase. eDAQ Pty Ltd will repair or replace defective equipment as appropriate. To obtain a warranty repair/replacement you must first notify us before return of the instrument and we will issue you with a RAN (return authorisation number). You must ship the defective product at your expense. We will pay return shipping. The product should be packed safely (preferably in its original packaging) and have the RAN on the shipping label. Returns sent without a RAN may be refused delivery.&lt;br /&gt;
&lt;br /&gt;
This warranty does not cover hardware that has:&lt;br /&gt;
:• been modified by the user in any way;&lt;br /&gt;
:• been subjected to unusual physical, electrical, or environmental stress. This includes damage due to faulty power sockets, inadequate earthing, or power spikes or surges;&lt;br /&gt;
:• been damaged because of incorrect wiring to ancillary equipment, or because of substandard, connectors or cables; or&lt;br /&gt;
:• had the original identification marks removed or altered.&lt;br /&gt;
&lt;br /&gt;
=== Software License ===&lt;br /&gt;
&lt;br /&gt;
You have the non-exclusive right to use the supplied eDAQ software (Sequencer, Chart etc). Your employees or students, for example, are entitled to use it, provided they adhere to this agreement. &lt;br /&gt;
Each separate purchase of the eDAQ software licenses it to be used on two computers, more than two copies must not be used simultaneously. Departmental/company licences are available if you wish to run more than two copies simultaneously.&lt;br /&gt;
&lt;br /&gt;
=== Technical Support ===&lt;br /&gt;
&lt;br /&gt;
Please register your unit to receive technical support.&lt;br /&gt;
&lt;br /&gt;
Technical assistance is available via email. Please describe the problem with as much detail as possible. Include a small example data file, if appropriate. Please also state:&lt;br /&gt;
: • the model and serial number of your EDAQ system.&lt;br /&gt;
: • the type of computer and operating system being used (for example Windows XP, Vista, Windows 7, 8, or 10)&lt;br /&gt;
: • the software version you are using (for example Chart v5.5.2)&lt;br /&gt;
&lt;br /&gt;
We endeavor to answer all your questions, but in some cases, for example where the problem relates to the other equipment that you are using, a nominal fee may be charged.&lt;br /&gt;
&lt;br /&gt;
=== Jurisdiction ===&lt;br /&gt;
&lt;br /&gt;
eDAQ Pty Ltd is bound by the laws of New South Wales in Australia, and any proceedings shall be heard by the Supreme Court of New South Wales in Australia.&lt;br /&gt;
&lt;br /&gt;
=== Disclaimer ===&lt;br /&gt;
&lt;br /&gt;
eDAQ reserves the right to alter specifications of hardware and software without notice. No liability can be accepted for consequential damages resulting from use of eDAQ products.&lt;/div&gt;</summary>
		<author><name>PaulDuckworth</name></author>	</entry>

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