Solubility Product Constant — MCQ Practice

The solubility product constant ($K_{sp}$) of $CaF_2$ is $3.9 \times 10^{-11}$ at $25^circ C$. What is the molar solubility of $CaF_2$ in pure water at this temperature?

The solubility of $Ag_2CrO_4$ in water is $1.3 \times 10^{-4}$ mol/L. Calculate its solubility product constant ($K_{sp}$).

The $K_{sp}$ of $Mg(OH)_2$ is $1.8 \times 10^{-11}$. What is its solubility in a solution buffered at pH 12?

Which of the following sparingly soluble salts has the highest molar solubility in pure water? Given $K_{sp}$ values: I. $AgCl = 1.8 \times 10^{-10}$ II. $CaSO_4 = 2.4 \times 10^{-5}$ III. $PbI_2 = 7.1 \times 10^{-9}$ IV. $Ag_2CrO_4 = 1.1 \times 10^{-12}$

A solution is prepared by mixing 50 mL of $0.01$ M $AgNO_3$ with 50 mL of $0.001$ M $NaCl$. Given $K_{sp}$ for $AgCl = 1.8 \times 10^{-10}$. Will a precipitate of $AgCl$ form?

The solubility of $PbSO_4$ in $0.01$ M $Na_2SO_4$ solution is $1.2 \times 10^{-6}$ M. Calculate the $K_{sp}$ of $PbSO_4$.

Which of the following statements about the solubility product constant ($K_{sp}$) is INCORRECT?