The $K_{sp}$ expression for $Ca_3(PO_4)_2$ is:

Which substance precipitates when $HCl$ is added to a solution of $SnS$ in yellow ammonium sulfide?

Solubility of $Th_3(PO_4)_4$ $(M_w = m)$ is $w \ g / 100 \ mL$ at $25 \ ^oC$. The $K_{sp}$ is:

The solubility of salt $BA_2$ is $4 \times 10^{-4} \ mol \ dm^{-3}$. What is the solubility product of the salt?

Equal volumes of $0.02 \ M$ $CaCl_2$ and $0.00004 \ M$ $Na_2SO_4$ solutions are mixed. Will a precipitation of $CaSO_4$ occur? $(K_{sp} = 2.4 \times 10^{-5})$

The solubility product constant $K_{sp}$ of $Mg(OH)_2$ is $9.0 \times 10^{-12}.$ If a solution is $0.010 \ M$ with respect to $Mg^{2+}$ ion,what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $Mg(OH)_2$?