The solubility product of a salt $AB$ is $1 \times 10^{-8}$ in a solution in which the concentration of $A$ is $10^{-3} \ M$. The salt will precipitate when the concentration of $B$ becomes more than:

If $[S^{2-}] = 0.6 \times 10^{-2} \ mol \ m^{-3}$ and $[Hg^{2+}] = [Mn^{2+}] = [Fe^{2+}] = [Zn^{2+}] = 1 \times 10^{-16} \ mol \ m^{-3}$,which of the following will precipitate first in an aqueous solution?

$A$ precipitate of $CaF_2$ $(K_{sp} = 1.7 \times 10^{-10})$ will be obtained when equal volumes of the following are mixed:

Solubility of $CaF_2$ in a solution of $Ca(NO_3)_2$ will be represented by the concentration term?

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 $pH$ of a saturated solution of $Ca(OH)_2$ is $12.25$. Calculate its solubility product $(K_{sp})$.