The $K_{sp}$ of $AgCl$ is $1.0 \times 10^{-10}$. Calculate the solubility of $AgCl$ in $0.2 \ M \ AgNO_3$.

The solubility product of Lead sulphate,$PbSO_4$ is $1.3 \times 10^{-8}$. Calculate its solubility in pure water. The molecular mass of $PbSO_4 = 303 \ g \ mol^{-1}$.

The compound insoluble in water is

If $H_2S$ is passed in a solution of $0.1 \ M \ Zn^{2+}$ and $0.01 \ M \ Cu^{+}$ and the concentration of $S^{2-}$ is made $8.1 \times 10^{-31} \ M$. Which precipitation of $ZnS$ and $CuS$ will take place? Given: $K_{sp}(ZnS) = 3.0 \times 10^{-23}$ and $K_{sp}(CuS) = 8.0 \times 10^{-34}$.

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 $\dots \times 10^{-5} \, M$?

Solid $Ba(NO_3)_2$ is gradually added to a $1.0 \times 10^{-4} \, M \, Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will precipitation start? (Given $K_{sp}$ for $BaCO_3 = 5.1 \times 10^{-9}$)