Chemistry - Ionic Equilibrium Question with Solution | TestHub

$\mathrm{Mg}(\mathrm{OH}{)}_2$ gives ${\mathrm{Mg}}^{2+}+2{\mathrm{OH}}^{-}$: $K_{sp}=s(2s{)}^2=4s^3=3.2\times 10^{-11}$.

$s^3=8\times 10^{-12}$, so $s=2\times 10^{-4}\mathrm{M}$.

Molar mass $=24+2\times 17=58g/mol$.

Solubility $=58\times 2\times 10^{-4}=0.0116g/L$.

Answer: 0.0116.