What is the solubility (in $mol \ L^{-1}$) of $AgCl$ $(K_{sp} = 1.0 \times 10^{-10})$ in a $0.1 \ M \ Cl^-$ solution?

Precipitation of $CaF_2$ $(K_{sp} = 1.7 \times 10^{-10})$ occurs when equal volumes of which of the following are mixed?

Predict whether a precipitate of $PbI_2$ will be formed or not on mixing $20 \ mL$ of $3 \times 10^{-3} \ M$ $Pb(NO_3)_2$ solution with $80 \ mL$ of $2 \times 10^{-3} \ M$ $NaI$ solution. $K_{sp}$ for lead iodide $(PbI_2)$ is $6.0 \times 10^{-9}$.

Calculate the solubility in $mol \ dm^{-3}$ of sparingly soluble salt $BA$ if its solubility product is $4.9 \times 10^{-13}$ at the same temperature.

The solubility product of a sparingly soluble salt $AX_2$ is $3.2 \times 10^{-8}$. What is its solubility (in $mol \ dm^{-3}$)?

The solubility of $BaSO_{4}$ in water is $2.42 \times 10^{-3} \ g \ L^{-1}$ at $298 \ K$. The value of solubility product $(K_{sp})$ will be (Given molar mass of $BaSO_{4} = 233 \ g \ mol^{-1}$)