Common Ion Effect — MCQ Practice

The solubility of $BaSO_4$ in water is $2.42 \times 10^{-3}\,g/L$. Its solubility product ($K_{sp}$) will be (Molar mass of $BaSO_4 = 233\,g/mol$):

The solubility of $AgCl$ in $0.1\,M$ $NaCl$ solution is ($K_{sp}$ of $AgCl = 1.8 \times 10^{-10}$):

Which of the following will decrease the solubility of $CaF_2$ in an aqueous solution?

Calculate the solubility of $Mg(OH)_2$ in a buffer solution maintained at $pH = 12$. ($K_{sp}$ of $Mg(OH)_2 = 1.8 \times 10^{-11}$)

A solution contains $0.01\,M$ $Ca^{2+}$ and $0.01\,M$ $Ba^{2+}$. If $K_{sp}$ for $CaSO_4$ is $2.4 \times 10^{-5}$ and for $BaSO_4$ is $1.1 \times 10^{-10}$, which ion will precipitate first upon gradual addition of $Na_2SO_4$?

The solubility of $PbI_2$ is $S_1$ in pure water and $S_2$ in $0.1\,M$ $KI$ solution. What is the relationship between $S_1$ and $S_2$?