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:

The solubility of a sparingly soluble salt $A_x B_y$ in water at $25\,^{\circ}C$ is $1.4 \times 10^{-4} \ M$. The solubility product is $1.1 \times 10^{-11}$. The values of $x$ and $y$ may be

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 $H_2S$,$K_{NET} = K_1 K_2 = 1 \times 10^{-21}$.

Calculate the molar solubility of calcium hydroxide $Ca(OH)_2$ in $0.10 \ M \ NaOH$ solution. The solubility product constant $(K_{sp})$ of calcium hydroxide is $5.5 \times 10^{-6}$.

The saturated solution of $Ag_2SO_4$ is $2.5 \times 10^{-2} \ M$. Its solubility product $(K_{sp})$ is

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