If the solubility of $Mg(OH)_2$ is $x \ mol/L$,then its solubility product $(K_{sp})$ is equal to .....

The solubility of $CaCO_3$ is $7 \times 10^{-5} \ mol \ dm^{-3}$ at $25^{\circ} C$. What is its solubility product at same temperature?

The solubility product of $Mg(OH)_2$ is $1 \times 10^{-11}$. At what $pH$ will $Mg(OH)_2$ start to precipitate from a $0.1 \, M \, Mg^{2+}$ solution?

The solubility of an $MX_2$ type electrolyte is $0.5 \times 10^{-4} \ mol/L$. The value of $K_{sp}$ of the electrolyte is:

When $150 \ mL$ of $0.0008 \ M$ ammonium sulfate solution is mixed with $50 \ mL$ of $0.04 \ M$ calcium nitrate solution,given $K_{sp} = 2.4 \times 10^{-5}$ for $CaSO_4$,what is the ionic product of $CaSO_4$?

Why only $As^{3+}$ gets precipitated as $As_2S_3$ and not $Zn^{2+}$ as $ZnS$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$?