The solubility product of $PbCl_2$ at $298 \ K$ is $3.2 \times 10^{-5}$. What is its solubility in $mol \ dm^{-3}$?

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

At $20 \, ^\circ C$,the concentration of $Ag^+$ ions in a saturated solution of $Ag_2CrO_4$ is $1.5 \times 10^{-4} \, M$. The solubility product $(K_{sp})$ of $Ag_2CrO_4$ at $20 \, ^\circ C$ is:

The solubility product of lead bromide is $8 \times 10^{-5}$. If the salt is $80\%$ dissociated in a saturated solution,find the solubility of the salt.

If $K_{sp}$ of $CaF_2$ at $25\,^{\circ}C$ is $1.7 \times 10^{-10}$,the combination amongst the following which gives a precipitate of $CaF_2$ is

The solubility product constants of $Ag_{2}CrO_{4}$ and $AgBr$ are $1.1 \times 10^{-12}$ and $5.0 \times 10^{-13}$ respectively. Calculate the ratio of the molarities of their saturated solutions.