The $K_{sp}$ values of $Al(OH)_3$ and $Zn(OH)_2$ are $8.5 \times 10^{-23}$ and $1.8 \times 10^{-14}$ respectively. If $NH_4OH$ is added to a solution containing $Al^{3+}$ and $Zn^{2+}$ ions,which will precipitate earlier?

Which of the following is the correct formula for the ionic product $(K_{sp})$ of $SnS_2$ (stannic sulfide)?

In a qualitative analysis, $Bi^{3+}$ is detected by the appearance of a precipitate of $BiO(OH)(s)$. Calculate the $pH$ when the following equilibrium exists at $298 \text{ K}$:
$BiO(OH)(s) \rightleftharpoons BiO^{+}(aq) + OH^{-}(aq)$,
$K = 4 \times 10^{-10}$
(Given: $\log 2 = 0.3010$)

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 $25^{\circ} C$?

At $298 \ K$,the solubility product of $PbCl_2$ is $1.0 \times 10^{-6}$. What will be the solubility of $PbCl_2$ in $mol \ L^{-1}$?

What is the concentration of $Ba^{2+}$ when $BaF_2$ $(K_{sp} = 1.0 \times 10^{-6})$ begins to precipitate from a solution that is $0.30 \, M \ F^{-}$?