Solubility of $Ca_{3}(PO_{4})_{2}$ is $S \ mol \ dm^{-3}$. Find the solubility product $(K_{sp})$.

Calculate the molar solubility of calcium hydroxide $Ca(OH)_2$ in $0.10 \ M \ NaOH$ solution. The solubility product constant $(K_{sp})$ of calcium hydroxide is $5.5 \times 10^{-6}$.

Using the Gibbs energy change,$\Delta G^{o} = +63.3 \ kJ \ mol^{-1}$,for the following reaction in water at $25 \ ^{\circ}C$,calculate the solubility product constant $(K_{sp})$:
$Ag_{2}CO_{3(s)} \rightleftharpoons 2Ag^{+}_{(aq)} + C{O_{3}}^{2-}_{(aq)}$
$(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

Which compound does not dissolve in acetic acid?

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:

At $298 \, K$,the solubility product $(K_{sp})$ of $M_2SO_4$ (where $M^+$ is a monovalent metal ion) is $1.2 \times 10^{-5}$. What is the maximum concentration of $M^+$ ions in a saturated solution of this salt at $298 \, K$?