Difference between revisions of "Reference Electrode Potentials"
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The Ag/AgCl electrode is by far the most popular type of reference electrode in use today. | The Ag/AgCl electrode is by far the most popular type of reference electrode in use today. | ||
− | It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). Silver chloride is qute incoble in water, though slimly more so in concentrated chord solutions owing to the formation of the complex ion [ | + | It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). Silver chloride is qute incoble in water, though slimly more so in concentrated chord solutions owing to the formation of the complex ion [AgCl<sub>2</sub>]<sup>–</sup>. The chloridized end of the wire is inserted into an electrolyte solution of KCl or NaCl. The relevant [http://en.wikipedia.org/wiki/Half-cell half cell] equation is: |
AgCl<sub><i>(s)</i></sub> + e<sup>–</sup> → Ag<sub><i>(s)</i></sub> + Cl<sup>–</sup> | AgCl<sub><i>(s)</i></sub> + e<sup>–</sup> → Ag<sub><i>(s)</i></sub> + Cl<sup>–</sup> | ||
Revision as of 15:44, 5 August 2014
The Silver/Silver Chloride (Ag/AgCl) Electrode
The Ag/AgCl electrode is by far the most popular type of reference electrode in use today.
It is constructed from a silver wire, part of which is 'chloridized' (covered with finely divided silver chloride). Silver chloride is qute incoble in water, though slimly more so in concentrated chord solutions owing to the formation of the complex ion [AgCl2]–. The chloridized end of the wire is inserted into an electrolyte solution of KCl or NaCl. The relevant half cell equation is: AgCl(s) + e– → Ag(s) + Cl–
The electrode potential is actually dependent on silver ion and chloride concentration, but as the silver ion concentration is limited by the low solubility of AgCl, the actual potential is effectively controlled by the chloride concentration alone. Note also that the potential is independent of hydrogen ion (acid) concentration.
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):
- E = 205 – 0.73 × (T – 25) for an electrolyte of 3.5 M KCl
- E = 199 – 1.01 × (T – 25) for an electrolyte of saturated KCl
where T is the temperature (°C), and E is the electrode potential (mV).
Electrolyte Solution | vs NHE | vs SCE | LJ | Reference |
---|---|---|---|---|
KCl (0.1 M) | 0.2881 | 0.047 | - | 1, 3 |
KCl (3 M) | 0.210 | -0.032 | - | 4 |
KCl (3.5 M) | 0.205 | -0.039 | Yes | 2 |
KCl (sat'd) | 0.197 | -0.045 | - | 1 |
KCl (sat'd) | 0.199 | -0.045 | Yes | 2 |
KCl (sat'd) | 0.1988 | -0.042 | - | 2 |
NaCl (3 M) | 0.209 | -0.035 | Yes | 5 |
NaCl (sat'd) | 0.197 | -0.047 | Yes | 3 |
Seawater | 0.25 | 0.01 | Yes | 6 |
Notes
- LJ, liquid junction. Value obtained using a cell which included a liquid junction potential.
- NHE, normal hydrogen electrode
- SCE, saturated calomel electrode
- Seawater has approximately 0.47 M NaCl.
References
- 1. "Electrochemical Methods: Fundamentals and Applications", A J Bard and L R Faulkner, John Wiley & Sons, NY (2000). See the table on inside back cover.
- 2. "Electrochemistry for Chemists, Second Edition", D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley & Sons, NY (1995). See Table 5.3
- 3. "Handbook of Analytical Chemistry", L Meites (ed.), McGraw Hill, NY (1963). See Section 5.
- 4. E P Friis, J E T Anderson, L L Madsen, N Bonander, Per Moller, J Ulstrup, Electrochimica Acta, 43, 1114-1122, 1998. DOI: 10.1016/S0013-4686(98)99006-5
The Calomel Electrode
The calomel electrode is usually constructed from a platinum wire inserted into a mixture of calomel (mercurous chloride, Hg2Cl2) and liquid mercury, with an electrolyte solution of KCl or NaCl. Calomel is reasonably insoluble in water (0.2 mg/100 mL). The relevant half cell equation is: Hg2Cl2 + 2e– → 2Hgliq + 2Cl–
As this equation implies, the electrode potential is dependent on chloride concentration, but independent of hydrogen ion (acid) concentration.
Calomel electrodes are unstable much above 50°C owing to the disproportionation reaction: Hg2Cl2 → Hgliq + HgCl2
Commercial calomel electrodes are available from:
- Koslow Scientific (USA)
- Ionode Pty Ltd (Australia)
In Europe the use of calomel electrodes is increasingly problematic because many countries no longer permit the use of mercury-containing devices.
Electrolyte Solution | vs NHE | vs SCE | LJ | Reference |
---|---|---|---|---|
KCl (0.1 M) | 0.3337 | 0.0925 | - | 1, 3 |
KCl (0.1 M) | 0.336 | 0.092 | Yes | 2 |
NCE, KCl (1 M) | 0.2801 | 0.0389 | - | 1, 3 |
NCE, KCl (1 M) | 0.283 | 0.039 | Yes | 2 |
KCl (3.5M) | 0.250 | 0.006 | Yes | 2 |
SCE, KCl (sat'd) | 0.2412 | 0 | - | 1, 3 |
SCE, KCl (sat'd) | 0.244 | 0 | Yes | 2 |
SSCE, NaCl (sat'd) | 0.2360 | -0.0052 | - | 1 |
Notes
- LJ, liquid junction. Value obtained using a cell which included a liquid junction potential.
- NCE, normal calomel electrode
- NHE, normal hydrogen electrode
- SCE, saturated calomel electrode
- SSCE, saturated salt calomel electrode
- For values at other temperatures see a calculator here.
References
- 1. "Electrochemical Methods: Fundamentals and Applications", A J Bard and L R Faulkner, John Wiley & Sons, NY (2000). See the table on inside back cover.
- 2. "Electrochemistry for Chemists, Second Edition", D T Sawyer, A J Sobkowiak, J Roberts, Jr., John Wiley & Sons, NY (1995). See Section 5.2.
- 3. "Handbook of Analytical Chemistry", L Meites (ed.), McGraw Hill, NY (1963). See Section 5.
- 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. DOI: 10.1039/TF9635901874