The solubility product of $BaCl_2$ is $4 \times 10^{-9}$. Its solubility in moles/litre would be:

If the solubility product of $AB_2$ is $3.20 \times 10^{-11} \ mol^3 L^{-3}$,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]

The solubility of $AgCl$ is $1 \times 10^{-5} \ mol/L$. Its solubility in $0.1 \ M$ sodium chloride solution is

If the solubility product of $BaSO_4$ is $1.44 \times 10^{-12}$,then the solubility of $SO_4^{2-}$ is .....

Which compound is soluble in $NH_4OH$?

Solid $Ba(NO_3)_2$ is gradually dissolved in $1 \times 10^{-4} \ M \ Na_2CO_3$ solution. At what concentration of $Ba^{+2}$ will the precipitation of $BaCO_3$ start? (Given: $K_{sp}$ of $BaCO_3 = 5.1 \times 10^{-9}$)