Question

The solubility product of $AgCl$ is $1.8\times {10}^{-10}$. Precipitation of $AgCl$ will occur only when equal volumes of solutions of:

• A. ${10}^{-4}MA{g}^{+}$ and ${10}^{-4}MC{l}^{-}$ are mixed
• B. ${10}^{-7}MA{g}^{+}$ and ${10}^{-7}MC{l}^{-}$ are mixed
• C. ${10}^{-5}MA{g}^{+}$ and ${10}^{-5}MC{l}^{-}$ are mixed
• D. $2\times {10}^{-5}MA{g}^{+}$ and ${10}^{-5}MC{l}^{-}$ are mixed

Answer 1

The correct option is A ${10}^{-4}MA{g}^{+}$ and ${10}^{-4}MC{l}^{-}$ are mixed

$Ksp\left[AgCl\right]=1.8\times {10}^{-10}$

Percipitation Occurs $⟶$ Ionic Product $>Ksp$

$K_{sp}\left[AgCl\right]=\left({10}^{-4}\right)\left({10}^{-4}\right)={10}^{-8}>1.8\times {10}^{-10}$

$⟹$ For ${10}^{-4}MA{g}^{+}$ and ${10}^{-4}MC{l}^{-},$ precipitation occurs.