Question

When equal volumes of the following solutions are mixed, the precipitation of $AgCl(K_{sp}=1.8\times {10}^{-10})$ will occur only with

• A. ${10}^{-4}M\left(A{g}^{\oplus }\right)$ and ${10}^{-4}M\left(C{l}^{⊝}\right)$
• B. ${10}^{-5}M\left(A{g}^{\oplus }\right)$ and ${10}^{-5}M\left(C{l}^{⊝}\right)$
• C. ${10}^{-6}M\left(A{g}^{\oplus }\right)$ and ${10}^{-6}M\left(C{l}^{⊝}\right)$
• D. ${10}^{-10}M\left(A{g}^{\oplus }\right)$ and ${10}^{-10}M\left(C{l}^{⊝}\right)$

Answer 1

The correct option is A ${10}^{-4}M\left(A{g}^{\oplus }\right)$ and ${10}^{-4}M\left(C{l}^{⊝}\right)$

Precipitation will occur when

ionic product of $AgCl>$ solubility product of $AgCl$

${10}^{-4}M\left(A{g}^{\oplus }\right)$ and ${10}^{-4}M\left(C{l}^{⊝}\right)$ present.

Here, $\left[A{g}^{+}\right]\left[C{l}^{-}\right]=\frac{{10}^{-4}}{2}\times \frac{{10}^{-4}}{2}=2.5\times {10}^{-9}>K_{sp}$

So precipitation will occur.