The solubility product of silver chloride at $298 \ K$ is $1.8 \times 10^{-10}$. The solubility of $AgCl$ in $0.01 \ M \ HCl$ solution will be ............

The solubility product of $Hg_2Cl_2$ in water at $25 \, ^\circ C$ is $3.2 \times 10^{-17} \, mol^3 \, dm^{-9}$. The solubility of $Hg_2Cl_2$ at $25 \, ^\circ C$ is:

For a sparingly soluble salt $MX_4$,the molar solubility is $S$ (mol/$L$) and its solubility product is $K_{sp}$. Determine the relationship between $K_{sp}$ and $S$.

Solubility products $(K_{sp})$ of the salts of types $MX, MX_2$ and $M_3X$ at temperature $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$ respectively. Solubilities (in $mol \text{ dm}^{-3}$) of the salts at temperature $T$ are in the order:

Which of the following pairs of ions,when their solutions are mixed,will result in precipitation?

Solid $Ba(NO_3)_2$ is gradually dissolved in $1 \times 10^{-4} \ M \ Na_2CO_3$ solution. At what concentration of $Ba^{+2}$ will the precipitation of $BaCO_3$ start? (Given: $K_{sp}$ of $BaCO_3 = 5.1 \times 10^{-9}$)