If the solubility product of lead iodide $(PbI_2)$ is $3.2 \times 10^{-8}$,then its solubility in $moles/litre$ will be

$A$ solution is $0.1 \ M$ in $Cl^{-}$ and $0.001 \ M$ in $CrO_{4}^{2-}$. Solid $AgNO_{3}$ is gradually added to it. Assuming that the addition does not change in volume and $K_{sp}(AgCl) = 1.7 \times 10^{-10} \ M^{2}$ and $K_{sp}(Ag_{2}CrO_{4}) = 1.9 \times 10^{-12} \ M^{3}$. Select the correct statement from the following:

The $K_{sp}$ of $Mg(OH)_2$ is $1.0 \times 10^{-12}$. At which $pH$ does $0.01 \ M$ $Mg^{2+}$ solution begin to precipitate? Calculate the solubility of $Mg(OH)_2$ in pure water.

At $25 \, ^\circ C$,the $K_{sp}$ of $CaF_2$ is $1.7 \times 10^{-10}$. Which of the following combinations will result in the precipitation of $CaF_2$?

What is the minimum volume of water required to dissolve $1 \, g$ of calcium sulphate at $298 \, K$? (For calcium sulphate,$K_{sp}$ is $9.1 \times 10^{-6}$).

The expression for solubility product of mercurous iodide $(Hg_2I_2)$ is