I am working on electrochemical reduction of CO2, using Pt as a counter electrode (area of the counter is always 10 times higher than the area of the working electrode) and electrolyte we are using is bicarbonate solution of 0.1 M (pH 6.8 after saturating with CO2) and 0.5 M (pH 7.2 after saturating with CO2). Potential we are applying at cathode is varying from -1.2 to -1.6 V vs Ag/ AgCl. For electrolysis we are using two compartment cell separated by Nafion-117 membrane. My doubt is during electrolysis whether Pt ( counter electrode ) can dissolve (as platinum oxide ) from the electrode surface and deposit over cathode after passing trough the membrane?
I would greatly appreciate if you could clear my doubt.
Dear colleague!
The chemically dissolved only on the platinum electrode in mixtures of concentrated solutions of strong acids and oxidizers, such as royal vodka (HNO3- 3HCI), a mixture of hydrogen peroxide and sulfuric acid. The electrochemically dissolvedon the platinum electrode, if you can by the subjecting it to anadic dissolution at current densities greater than 0.2 A/h and potentials greater than 3.0 V.
However, if in you do not reach such potentials and current density, then the electrochemical process of dissolving platinum can be ruled out. Maybe you should consider whether the platinum electrode forms complexes with the organic compound CO2RR. In secret, I say that platinum forms strong complexes with some organic compounds. Especially, on the platinum is very likes to form such complexes in solutions of organic compounds in the presence of their peroxides
I hope my answer will help your scientific work!
Best Regards, AMA
Actually, the following paper might help you to find a suitable answer to your question. Besides that, why you have to use Pt as counter electrode? Try to use carbon instead.
Article Influence of the Working and Counter Electrode Surface Areas...
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