The solubility of $CaF_2$ is $2 \times 10^{-4} \, mol/L$. Its solubility product $(K_{sp})$ is:

Select the ion exchange reaction,which proceeds in the forward direction in an aqueous medium.

Which substance precipitates when $HCl$ is added to a solution of $SnS$ in yellow ammonium sulfide?

For $AgCl$,$K_{sp} = 1.2 \times 10^{-10}$ and for $AgBr$,$K_{sp} = 3.5 \times 10^{-13}$. What is the relationship between their solubilities $(S)$?

The solubility of $AgBr$ with solubility product $5.0 \times 10^{-13}$ at $298 \ K$ in $0.1 \ M$ $NaBr$ solution would be:

At $310 \, K$,the solubility of $CaF_{2}$ in water is $2.34 \times 10^{-3} \, g / 100 \, mL$. The solubility product of $CaF_{2}$ is $x \times 10^{-8} \, (mol / L)^{3}$. Find the value of $x$. (Given molar mass: $CaF_{2} = 78 \, g \, mol^{-1}$)