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.

If the solubility of $PbBr_2$ is $S \, mol/L$,and it undergoes $100\%$ ionization,then the solubility product constant $(K_{sp})$ is equal to:

Which from the following equations represents the relation between solubility ($S$ in $mol \ L^{-1}$) and solubility product $(K_{sp})$ for a salt $B_3A_2$?

The $K_{sp}$ of $Ag_2CrO_4, AgCl, AgBr$ and $AgI$ are respectively,$1.1 \times 10^{-12}, 1.8 \times 10^{-10}, 5.0 \times 10^{-13}, 8.3 \times 10^{-17}$. Which one of the following salts will precipitate last if $AgNO_3$ solution is added to the solution containing equal moles of $NaCl, NaBr, NaI$ and $Na_2CrO_4$?

The compound insoluble in acetic acid is

The solubility of $CaF_2$ is $s$ moles/litre. Then its solubility product is ....