Cyclic Voltammetry: Ferro/Ferricyanide, fact and fiction - Revision history

PaulDuckworth at 02:21, 19 November 2014

2014-11-19T02:21:17Z

PaulDuckworth at 02:16, 19 November 2014

2014-11-19T02:16:56Z

PaulDuckworth at 02:16, 19 November 2014

2014-11-19T02:16:15Z

PaulDuckworth at 02:11, 19 November 2014

2014-11-19T02:11:17Z

PaulDuckworth at 02:08, 19 November 2014

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PaulDuckworth at 02:03, 19 November 2014

2014-11-19T02:03:16Z

PaulDuckworth at 02:02, 19 November 2014

2014-11-19T02:02:16Z

PaulDuckworth at 02:01, 19 November 2014

2014-11-19T02:01:33Z

PaulDuckworth at 01:53, 19 November 2014

2014-11-19T01:53:10Z

PaulDuckworth at 01:50, 19 November 2014

2014-11-19T01:50:32Z

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-While is is true that a one electrode reversible reversible reaction will
+While is is true that a one electrode reversible reversible reaction will exhibit a a peak separation of 0.59 V at 25 deg C you should consider this
-exhibit a a peak separation of 0.59 V at 25 deg C you should consider this
+more of an 'ideal' at which to aim, rather than something you ever get to see in reality (unless you are very careful in setting up the experiment).
 more of an 'ideal' at which to aim, rather than something you ever get to
 see in reality (unless you are very careful in setting up the experiment).
 For example see
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 impacts on the observed CV.  Ferri/ferrocyanide is notorious for this, and hexachloroiridate has been proposed as a replacement:
-Cyclic Voltammetry of Hexachloroiridate(IV): An Alternative to the Electrochemical Study of the Ferricyanide Ion, Steven Petrovic, Chemical Educator 5, 231-235, 2000. [http://dx.doi.org/10.1007/s00897000416a DOI:10.1007/s00897000416a]
+Cyclic Voltammetry of Hexachloroiridate(IV): An Alternative to the Electrochemical Study of the Ferricyanide Ion, Steven Petrovic, Chemical Educator 5, 231-235, 2000. [http://dx.doi.org/10.1007/s00897000416a DOI:10.1007/s00897000416a] or [http://www.researchgate.net/publication/226317493_Cyclic_Voltammetry_of_Hexachloroiridate(IV)_An_Alternative_to_the_Electrochemical_Study_of_the_Ferricyanide_Ion/file/32bfe51010257121c9.pdf Research Gate]
 Other materials that are used for undergaduate experiments that are more

← Older revision		Revision as of 02:16, 19 November 2014
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	[https://www.pineinst.com/echem/files/LMECSPEXPT.pdf Hexammineruthenium II/III salts]		[https://www.pineinst.com/echem/files/LMECSPEXPT.pdf Hexammineruthenium II/III salts]

−	~~Inorganic~~ solvents the [http://en.wikipedia.org/wiki/Ferrocenium_tetrafluoroborate ferrocene/ferrocimium ion] is the nearly universal choice to demonstrate reversible cyclic voltammetry.	+	In organic solvents the [http://en.wikipedia.org/wiki/Ferrocenium_tetrafluoroborate ferrocene/ferrocimium ion] is the nearly universal choice to demonstrate reversible cyclic voltammetry.

← Older revision		Revision as of 02:16, 19 November 2014
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	[https://www.pineinst.com/echem/files/LMECSPEXPT.pdf Hexammineruthenium II/III salts]		[https://www.pineinst.com/echem/files/LMECSPEXPT.pdf Hexammineruthenium II/III salts]
		+
		+	Inorganic solvents the [http://en.wikipedia.org/wiki/Ferrocenium_tetrafluoroborate ferrocene/ferrocimium ion] is the nearly universal choice to demonstrate reversible cyclic voltammetry.

@@ Line 35: / Line 35: @@
 Uncompensated Resistance. 1. The Effect of Cell Geometry Jan C. Myland and
 Keith B. Oldham, Anal. Chem. 2000, 72, 3972-3980
-http://dx.doi.org/10.1021/ac0001535
+[http://dx.doi.org/10.1021/ac0001535 DOI:10.1021/ac0001535]
 Uncompensated Resistance. 2. The Effect of Reference Electrode Nonideality
 Keith B. Oldham and Nicholas P. C. Stevens, Anal. Chem. 2000, 72, 3981-3988.
-http://dx.doi.org/10.1021/ac000154x
+[http://dx.doi.org/10.1021/ac000154x DOI:10.1021/ac000154x]
 To reduce this iR drop (and uncompensated resistance) to a minimum you can
@@ Line 45: / Line 45: @@
 . Keep the reference electrode close to the working electrode (use of a
-'Luggin probe' style electrode is recommended for the most exacting
+[http://www.corrosion-doctors.org/References/Luggin.htm 'Luggin probe'] style electrode is recommended for the most exacting
-experiments). See
+experiments).
-   http://www.corrosion-doctors.org/References/Luggin.htm
 . Do not obscure the working electrode by placing a large reference

@@ Line 78: / Line 78: @@
 impacts on the observed CV.  Ferri/ferrocyanide is notorious for this, and hexachloroiridate has been proposed as a replacement:
-Cyclic Voltammetry of Hexachloroiridate(IV): An Alternative to the Electrochemical Study of the Ferricyanide Ion, Steven Petrovic, Chemical Educator 5, 231-235, 2000.
+Cyclic Voltammetry of Hexachloroiridate(IV): An Alternative to the Electrochemical Study of the Ferricyanide Ion, Steven Petrovic, Chemical Educator 5, 231-235, 2000. [http://dx.doi.org/10.1007/s00897000416a DOI:10.1007/s00897000416a]
 Other materials that are used for undergaduate experiments that are more

@@ Line 86: / Line 86: @@
 [http://wiki.edaq.com/index.php/File:EXP002_Cyclic_Voltammetry_of_Ferrocene_Carboxylic_Acid_PDF.pdf Water soluble ferrocene derivatives]
-   Hexammineruthenium II/III salts
+[https://www.pineinst.com/echem/files/LMECSPEXPT.pdf Hexammineruthenium II/III salts]
-   see https://www.pineinst.com/echem/files/LMECSPEXPT.pdf

@@ Line 1: / Line 1: @@
 [http://www.wikipedia.org/wiki/Potassium_ferricyanide Potassium ferricyanide] is a favourite choice in the laboratory to introduce students to cyclic voltammetry. This is largely due to a
-Cyclic Voltammetry of Hexachloroiridate(IV): An Alternative to the Electrochemical Study of the Ferricyanide Ion, Steven Petrovic, Chemical Educator 5, 231-235, 2000.
 describes an alternative to the use of ferri/ferrocyanide for educational cyclic voltammetry experiments in aqeuous solution..
@@ Line 10: / Line 10: @@
 Ferricyanide Redox Couple, Christine M. Pharr and Peter R. Griffith, Analytical Chemistry, 69, 4673-4679, 1997.
-The ferro/ferrcyanide couple is has a standard reduction potential of E<sub>0</sub> =  ~436 mV.  E<sub>1/2</sub> = . While it is true that this value would be obtained as the
+The ferro/ferrcyanide couple is has a standard reduction potential of E<sub>0</sub> =  ~436 mV however this is dependent on solution pH and

← Older revision		Revision as of 01:53, 19 November 2014
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	Ferricyanide Redox Couple, Christine M. Pharr and Peter R. Griffith, Analytical Chemistry, 69, 4673-4679, 1997.		Ferricyanide Redox Couple, Christine M. Pharr and Peter R. Griffith, Analytical Chemistry, 69, 4673-4679, 1997.

−	The ferro/ferrcyanide couple is has a standard reduction potential of E<sub>0</sub> E<sub>1/2</sub> = . While it is true that this value would be obtained as the	+	The ferro/ferrcyanide couple is has a standard reduction potential of E<sub>0</sub> = ~436 mV. E<sub>1/2</sub> = . While it is true that this value would be obtained as the