Question

The concentration of ${Ag}^{+}$ ions in a given saturated solution of $AgCl$ at ${25}^{o}C$ is $1.06\times {10}^{-5}g$ ion per litre. The solubility product of $AgCl$ is:

• A. $0.353\times {10}^{-10}$
• B. $0.530\times {10}^{-10}$
• C. $1.12\times {10}^{-10}$
• D. $2.12\times {10}^{-10}$

Answer 1

The correct option is C $1.12\times {10}^{-10}$

In a saturated solution of $AgCl$ the concentration of both ${Ag}^{+}$ and ${Cl}^{-}$ will be equal.

i.e, $\left[{Ag}^{+}\right]=\left[{Cl}^{-}\right]=1.06\times {10}^{-5}$

$\therefore$ The solubility product $=K_{sp}=\left[{Ag}^{+}\right]\left[{Cl}^{-}\right]$

$={(1.06\times {10}^{-5})}^2$

$=1.1236\times {10}^{-10}$

$\therefore$ Answer will be C.