Question

Calculate the Ksp of AgI with the help of following cell

$Ag_{(s)}|AgI_{(s)}|I_{(aq)}^{-}(0.05M)||Ag_{(aq)}^{+}(0.05M)|Ag_{(s)};E_{cell}=0.7884V$

Answer 1

$K_{sp} = 1.1 \times 10^{-16}$

Answer 2

The given cell's potential ($E_{cell}$) is related to the standard potentials of the half-reactions and the concentrations of the ions by the Nernst equation. The standard cell potential ($E_{cell}^o$) for this cell, which involves the formation of AgI from its ions, is directly related to the solubility product ($K_{sp}$) of AgI. By substituting the given concentrations and measured cell potential into the derived Nernst equation, the $K_{sp}$ value for AgI can be calculated.