An acidified solution of $0.05 \ M \ Zn^{2+}$ is saturated with $0.1 \ M \ H_2S$. What is the minimum molar concentration $(M)$ of $H^{+}$ required to prevent the precipitation of $ZnS$? Use $K_{sp}(ZnS) = 1.25 \times 10^{-22}$ and overall dissociation constant of $H_2S$,$K_{NET} = K_1 K_2 = 1 \times 10^{-21}$.

For a sparingly soluble strong electrolyte $AgIO_3$ (molar mass = $283 \, g/mol$),the equilibrium in a saturated solution is given by $AgIO_3(s) \rightleftharpoons Ag^+(aq) + IO_3^-(aq)$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,how many grams of $AgIO_3$ are contained in $100 \, mL$ of its saturated solution?

Solubility of $AgCl$ in $0.2 \, M \, NaCl$ is $x$ and that in $0.1 \, M \, AgNO_3$ is $y$. Then which of the following is correct?

The solubility of $AgCl$ is $1.43 \times 10^{-3} \ g/L$. If the molar mass of $AgCl$ is $143 \ g/mol$,then the solubility product $(K_{sp})$ is:

If the solubility of a sparingly soluble salt of the type $BA_2$ (giving three ions on dissociation of a molecule) is $x \ mol \ L^{-1}$,then its solubility product is given by

The solubility product of $AgCl$ is $1 \times 10^{-6}$ at $298 \, K$. Its solubility in $mol \, L^{-1}$ would be: