According to the reaction $PbCl_2 \rightleftharpoons Pb^{2+} + 2Cl^-$,the solubility product constant $(K_{sp})$ of $PbCl_2$ is

The values of $K_{sp}$ of two sparingly soluble salts $Ni(OH)_2$ and $AgCN$ are $2.0 \times 10^{-15}$ and $6 \times 10^{-17}$ respectively. Which salt is more soluble? Explain.

The solubility product of $BaSO_4$ is $1.5 \times 10^{-9}$. The precipitation in a $0.01 \ M \ Ba^{2+}$ solution will start,on adding $H_2SO_4$ of concentration:

The moles of $Ag^{+}$ which must be added to decrease the concentration of $Cl^{-}$ from $4 \times 10^{-5} \ M$ to $10^{-5} \ M$ in $100 \ mL$ solution,if $K_{sp}$ for $AgCl$ is $10^{-10} \ M^2$ at $25 \ ^oC$.

What is the molar solubility of $Al(OH)_3$ in $0.2 \ M \ NaOH$ solution? Given that,the solubility product of $Al(OH)_3 = 2.4 \times 10^{-24}$.

The solubility of $CaCO_3$ in water is $3.05 \times 10^{-4} \, mol/L$. Its solubility product will be: