Question

Now, construct the following cell and use it to determine the solubility product constant (= Ksp) for silver chloride. In order to prepare the solution for the left half-cell, mix appropriate volumes of the 0.1 M silver nitrate and 0.2 M potassium chloride stock solutions.

Ag│AgCl(s), Cl− (0.05 M)║Ag+ (0.1 M)│Ag (17)

For the determination of Ksp section: You can assume that Ag+ and Cl− will react quantitatively to form AgCl, which precipitates out of the solution (i.e. all consider that all available Ag+ in solution will react). Carefully consider what should be the limiting reagent in this reaction if you want to have “unreacted” [Cl−] = 0.05 M remaining in solution after this reaction is complete and you are ready to begin the electrochemical reaction. Show your work and describe how you will achieve this.

Answer 1