Suppose that the concentrations of NaF and KCl were each 0.10 M in the cell (a) Using

Chapter 13, Problem 13-19

(choose chapter or problem)

Suppose that the concentrations of NaF and KCl were each 0.10 M in the cell

\(\mathrm{Pb}(s)\left|\mathrm{PbF}_{2}(s)\right| \mathrm{F}^{-}(a q) \| \mathrm{Cl}^{-}(a q)|\mathrm{AgCl}(s)| \mathrm{Ag}(s)\)

(a) Using the half-reactions \(2 \mathrm{AgCl}(s)+2 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{Ag}(s)+2 \mathrm{Cl}^{-}\) and \(\mathrm{PbF}_{2}(s)+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Pb}(s)+2 \mathrm{~F}^{-}\), calculate the cell voltage.

(b) By the reasoning in Figure 13-8, in which direction do electrons flow?

(c) Now calculate the cell voltage by using the reactions \(2 \mathrm{Ag}^{+}+2 \mathrm{e}^{-} \rightleftharpoons 2 \mathrm{Ag}(s)\) and \(\mathrm{Pb}^{2+}+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{Pb}(s)\). For this part, you will need the solubility products for \(\mathrm{PbF}_{2}\) and AgCl.