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?

Which of the following is a sparingly soluble salt?

The minimum volume of water required to dissolve $0.1 \ g$ of lead $(II)$ chloride to get a saturated solution ($K_{sp}$ of $PbCl_2 = 3.2 \times 10^{-8}$; atomic mass of $Pb = 207 \ u$,$Cl = 35.5 \ u$) is......$L$

The solubility of calcium carbonate $(CaCO_3)$ at $298 \ K$ is $6.4 \times 10^{-5} \ mol \ dm^{-3}$. Calculate the value of solubility product $(K_{sp})$ at the same temperature.

$M_{3}A_{2}$ is a sparingly soluble salt of molar mass $y \text{ g mol}^{-1}$ and solubility $x \text{ g L}^{-1}$. The ratio of the molar concentration of the anion $(A^{3-})$ to the solubility product of the salt is

Zinc carbonate is precipitated from zinc sulphate solution by the addition of