At $298 \ K$,the solubility of $PbCl_2$ is $2 \times 10^{-2} \ mol/L$. Calculate the $K_{sp}$.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ba(AcO)_2 + K_2CrO_4 \longrightarrow BaCrO_4 \downarrow + 2AcOK$

The solubility product of $PbI_2$ is $1.08 \times 10^{-7}$. Calculate its solubility in $mol \ dm^{-3}$ at $298 \ K$?

The solubility product of magnesium hydroxide $Mg(OH)_2$ is $1.2 \times 10^{-11}$. Calculate its solubility in pure water and $0.05 \ M$ $NaOH$.

The solubility of $PbI_2$ at $25 \, ^\circ C$ is $0.7 \, g \, L^{-1}$. What is the solubility product $(K_{sp})$ of $PbI_2$ at this temperature? (Molar mass of $PbI_2 = 461.2 \, g \, mol^{-1}$)

If the $K_{sp}$ of $Mg(OH)_2$ is $1 \times 10^{-12}$,at what $pH$ will $Mg(OH)_2$ precipitate from a $0.01 \ M$ solution of $Mg^{2+}$ ions?