If $0.001435 \ g$ of $AgCl$ is present in $100 \ mL$ of water,calculate the $K_{sp}$.

Increasing order of solubility of $AgCl$ in $(i) H_2O$,$(ii) 1 \ M \ NaCl \ (aq.)$,$(iii) 1 \ M \ CaCl_2 \ (aq.)$ and $(iv) 1 \ M \ NaNO_3 \ (aq.)$ solution.

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 $S$.

The solubility of $AgBr$ is $7.1 \times 10^{-7} \ mol \ dm^{-3}$. Calculate its solubility product at the same temperature.

The $K_{sp}$ of $AgCl$ at $18\, ^oC$ is $1.8 \times 10^{-10}$. If the concentration of $Ag^{+}$ is $4 \times 10^{-3}\ mol/L$,what is the minimum concentration of $Cl^{-}$ required for $AgCl$ precipitation?

If $pH$ of a saturated solution of $Ba(OH)_2$ is $12$,the value of its $K_{sp}$ is