Question

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

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

Answer 1

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

Precipitation will occur when $Q>K_{sp}$.
$Q={10}^{-4}\times {10}^{-4}={10}^{-8}>K_{sp}(1.8\times {10}^{-10})$