Question

Sketch cyclic voltammograms for the silver oxidation and reduction in different electrolytes. Assume electrochemical reversibility and a concentration of 50 mM of either one of the respective salt in the solutions. The solubility products of the different silver salts in are: Ksp(AgBr)=5.4⋅10−13, Ksp(AgCl)=1.6⋅10−10, sp(AgI)=8.5⋅10−17, Ksp(AgSCN)=1.0⋅10−12. Sketch for (a) bromide solution, (b) chloride solution, (c) iodide solution, (d) thiocyanate solution. Hint: The concentration of silver ions in the Nernst equation can be substituted with the rearranged equation of the solubility product.

Answer 1

Cyclic voltammograms can be used to study the oxidation and reduction of silver in different electrolytes. The shape of the voltammogram depends on the electrolyte used and the concentration of the silver salts.

Step-by-step explanation:

Cyclic voltammograms can be used to study the oxidation and reduction of silver in different electrolytes. The shape of the voltammogram will depend on the electrolyte used. The concentration of the silver salts can affect the height of the peaks in the voltammogram.

In the case of (a) bromide solution, the silver oxidation peak will be observed at a higher potential compared to the reduction peak. This is because the reduction of silver occurs at a more negative potential than the oxidation of silver.

The shape of the voltammogram will be similar for (b) chloride solution, (c) iodide solution, and (d) thiocyanate solution.

It is important to note that the solubility products of the different silver salts mentioned are not directly related to the voltammograms.

The solubility products provide information about the solubility of the salts in water, whereas the voltammograms show how the silver ion is oxidized and reduced in the presence of different electrolytes.