Given the cell reactions \[ \begin{array}{l} \mathrm{AgCl}(\mathrm{s})+\mathrm{e} \longrightarro...
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0Given the cell reactions
\[
\begin{array}{l}
\mathrm{AgCl}(\mathrm{s})+\mathrm{e} \longrightarrow \mathrm{Ag}(\mathrm{s})+\mathrm{Cl}^{-}(\mathrm{aq}) ; \quad E^{0}=+0.22 \mathrm{~V} \\
\mathrm{Ag}(\mathrm{s}) ; \quad E^{0}=+0.80 \mathrm{~V}
\end{array}
\]
the solubility product of \( \mathrm{AgCl}(\mathrm{s}) \) at \( 298 \mathrm{~K} \) is
(A) \( 1.6 \times 10^{-18} \)
(B) \( 1.6 \times 10^{-5} \)
(C) \( 1.6 \times 10^{-10} \)
(D) \( 1.6 \times 10^{-12} \)
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