If the solubility of $Ca_3(PO_4)_2$ in water is $x \ mol \ L^{-1}$,its solubility product in $mol^5 \ L^{-5}$ is (in $x^5$)

The solubility of $Ca(OH)_{2}$ is $s \ mol \ L^{-1}$. The solubility product $(K_{sp})$ under the same condition is:

The solubility of $AgBr_{(s)}$,having solubility product $5 \times 10^{-10}$ in $0.2 \ M$ $NaBr$ solution,equals

On passing $H_2S$ gas through a solution of $Cu^{2+}$ and $Zn^{2+}$ ions,$CuS$ is precipitated first because

The values of $K_{sp}$ of $CaCO_{3}$ and $CaC_{2}O_{4}$ are $4.7 \times 10^{-9}$ and $1.3 \times 10^{-9}$ respectively at $25 \, ^oC$. If the mixture of these two is washed with water,what is the concentration of $Ca^{2+}$ ions in water $\dots \times 10^{-5} \, M$?

Find the solubility of $PbI_2$ if its solubility product is $7.0 \times 10^{-9}$.