The solubility of $PbCl_2$ is given by:

$A$ solution containing $0.01 \ M \ Zn^{2+}$ and $0.01 \ M \ Cu^{2+}$ is saturated with $H_2S$ gas. The concentration of $S^{2-}$ is $8.1 \times 10^{-21} \ M$. Given that the $K_{sp}$ values for $ZnS$ and $CuS$ are $3.0 \times 10^{-22}$ and $8.0 \times 10^{-36}$ respectively,which of the following will occur in the solution?

The solubility product of $AgCl$ is $4.0 \times 10^{-10}$ at $298 \ K$. The solubility of $AgCl$ in $0.04 \ m \ CaCl_2$ will be

The solubility of $AgCl$ is $1 \times 10^{-5} \ mol/L$. Its solubility in $0.1 \ M$ sodium chloride solution is

What is the minimum volume of water required to dissolve $1 \, g$ of calcium sulphate at $298 \, K$? (For calcium sulphate,$K_{sp}$ is $9.1 \times 10^{-6}$).

$A$ $1.0 \ L$ of aqueous solution contains $1 \times 10^{-8} \ M \ NaBr$,$1 \times 10^{-8} \ M \ NaCl$ and $1 \times 10^{-8} \ M \ NaI$. To this solution,$1 \times 10^{-10} \ M$ aqueous $AgNO_3$ solution is added dropwise. The order of precipitation of $AgX$ $(X = Cl, Br, I)$ is:
$(K_{sp}(AgCl) = 1.8 \times 10^{-10}; K_{sp}(AgBr) = 5 \times 10^{-13}; K_{sp}(AgI) = 8.3 \times 10^{-17})$