If the solubility product of $AB _{2}$ is $3.20 \times 10^{-11}\, M ^{3}$,

then the solubility of $AB _{2}$ in pure water is……… $\times 10^{-4}$ $mol$ $L ^{-1}$.

[Assuming that neither kind of ion reacts with water]

If the solubility product of $PbS$ is $8 \times 10^{-28}$, then the solubility of $PbS$ in pure water at $298\; K$ is $x \times 10^{-16}\; mol\; L ^{-1}$. The value of $x$ is $\dots$.

[Given $\sqrt2 = 1.41$]

The solubility product of a sparingly soluble salt $A{X_2}$ is $3.2 \times {10^{ – 11}}$. Its solubility (in moles / litres) is

The solubility product of a sparingly soluble salt $AB$ at room temperature is $1.21 \times {10^{ – 6}}$. Its molar solubility is

Which one of the following arrangements represents the correct order of solubilities of sparingly soluble salts $Hg_2Cl_2,\,\,Cr_2(SO_4 )_3,\,\,BaSO_4$ and $CrCl_3$ respectively ?