Question

The $K_{s p}$ of $Ag_{2}CrO_{4}$ is $1.1\times 10^{- 12}$ at $0.1 K$ . The solubility (in $mol/L$ ) of $Ag_{2}CrO_{4}$ in a $0.1 M \, AgNO_{3}$ solution is

• A. $1.1\times 10^{- 11}$
• B. $1.1\times 10^{- 10}$
• C. $1.1\times 10^{- 12}$
• D. $1.1\times 10^{- 9}$

Answer 1

Answer: (B)

$\left(\text{Ag}\right)_{2} \left(\text{CrO}\right)_{4} \left(\text{s}\right) \rightleftharpoons \underset{2 \text{s} + 0.1}{2 \left(\text{Ag}\right)^{+} \left(\text{aq}\right)} + \underset{\text{s}}{\text{CrO}_{4}^{2 -} \left(\text{aq}\right)}$
$K_{s p}=\left(\right.0.1\left(\left.\right)^{2}s=1.1\times 10^{- 12}$
$s=1.1\times 10^{- 10}M$