The solubility product of $AgI$ at $25^{\circ} C$ is $1.0 \times 10^{-16} \ mol^2 \ L^{-2}$. What is the solubility of $AgI$ in $10^{-4} \ N \ KI$ at $25^{\circ} C$?

The $pH$ of a saturated solution of $Ca(OH)_2$ is $12.25$. Calculate its solubility product $(K_{sp})$.

If $0.001435 \ g$ of $AgCl$ is present in $100 \ mL$ of water,calculate the $K_{sp}$.

The solubility product of $PbCl_2$ at $298 \ K$ is $1 \times 10^{-6}$. Its solubility in $mol/L$ is:

Consider two Group $IV$ metal ions $X^{2+}$ and $Y^{2+}$. $A$ solution containing $0.01 \ M$ $X^{2+}$ and $0.01 \ M$ $Y^{2+}$ is saturated with $H_2S$. The pH at which the metal sulphide $YS$ will form as a precipitate is . . . . . . (Nearest integer). (Given: $K_{sp}(XS)=1 \times 10^{-22}$ at $25^{\circ} C$, $K_{sp}(YS)=4 \times 10^{-16}$ at $25^{\circ} C$, $[H_2S]=0.1 \ M$ in solution, $K_{a1} \times K_{a2}(H_2S)=1.0 \times 10^{-21}$, $\log 2=0.30, \log 3=0.48, \log 5=0.70$)

The molar solubility (in $mol \cdot L^{-1}$) of a sparingly soluble salt $MX_4$ is $S$. The corresponding solubility product is $K_{sp}$. $S$ in terms of $K_{sp}$ is given by the relation: