Solubility Equilibria of Sparingly Soluble Salts — MCQ Practice

The solubility product ($K_{sp}$) of $Ag_2CrO_4$ is $3.2 \times 10^{-12}$. What is the molar solubility of $Ag_2CrO_4$ in pure water?

The $K_{sp}$ of $CaF_2$ is $3.9 \times 10^{-11}$ at $25^circ C$. What is the concentration of $Ca^{2+}$ ions in a saturated solution of $CaF_2$ in $0.01$ M $NaF$ solution?

A solution contains $0.01$ M $Ba^{2+}$ and $0.01$ M $Sr^{2+}$. If $Na_2SO_4$ solution is slowly added, which ion will precipitate first? ($K_{sp}$ of $BaSO_4 = 1.1 \times 10^{-10}$, $K_{sp}$ of $SrSO_4 = 3.2 \times 10^{-7}$)

Which of the following statements is INCORRECT regarding the solubility of $Mg(OH)_2$ ($K_{sp} = 1.8 \times 10^{-11}$)?

If $100$ mL of $1.0 \times 10^{-3}$ M $Pb(NO_3)_2$ is mixed with $100$ mL of $2.0 \times 10^{-3}$ M $NaCl$, will $PbCl_2$ precipitate? ($K_{sp}$ of $PbCl_2 = 1.6 \times 10^{-5}$)

The solubility of $AgCl$ in $0.1$ M $AgNO_3$ solution is $X$. The solubility of $AgCl$ in $0.1$ M $NaCl$ solution is $Y$. The solubility of $AgCl$ in pure water is $Z$. Which of the following relationships is correct?

Which of the following sparingly soluble salts would have its solubility significantly increased in an acidic solution?