The solubility of $AgCl$ at $20 \, ^oC$ is $1.435 \times 10^{-3} \, g/L$. The solubility product $(K_{sp})$ of $AgCl$ is:

The solubility of a salt $A_2B_3$ is $10^{-3} \ M$. What will be its solubility product?

The solubility products of some sparingly soluble electrolytes are given below. The increasing order of their molar solubility is:
$(a)$ Formula: $MX$,$K_{sp} = 4.0 \times 10^{-20}$
$(b)$ Formula: $P_2Q$,$K_{sp} = 3.2 \times 10^{-11}$
$(c)$ Formula: $LY_3$,$K_{sp} = 2.7 \times 10^{-31}$

What is the concentration of $Ba^{2+}$ when $BaF_2$ $(K_{sp} = 1.0 \times 10^{-6})$ begins to precipitate from a solution that is $0.30 \, M \ F^{-}$?

Calculate the solubility product of sparingly soluble salt $BA$ at $300 \ K$ if its solubility is $9.1 \times 10^{-3} \ mol \ dm^{-3}$ at same temperature.

The solubility product of a sparingly soluble salt $A_2B$ is $3.2 \times 10^{-11}$. Its solubility in $mol \cdot L^{-1}$ is