Question

The concentration of $ A{{g}^{+}} $ ion in a given saturated solution of $ AgCl $ at $ 25{}^\circ C $ is $ 1.06\times {{10}^{-5}}g- $ ion per litre. Thus, 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

Answer: (C)

$[Ag^+] = 1.06 \times 10^{-5} \,g - ion/L$
$ = 1.06 \times 10^{-5} \,mol/L = [Cl^-]$
$AgCl(s) \rightleftharpoons Ag^+ + Cl^-$
$K_{sp} = [Ag^+][Cl^-]$
$= (1.06 \times 10^{-5})^2$
$ = 1.12 \times 10^{-10}$