The solubility product of $M(OH)_2$ is $10^{-14}$. What will be the concentration of $M^{+2}$ in a $0.1 \, M$ solution of $NH_4OH$,if $NH_4OH$ is $10\%$ ionized?

The solubility product of a sulphide $MS$ is $3 \times 10^{-25}$ and that of another sulphide $NS$ is $4 \times 10^{-40}$. In an ammoniacal solution,which of the following occurs?

The solubility product of $Hg_2I_2$ is equal to

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

The solubility product of silver bromide is $5.0 \times 10^{-13}$. The quantity of potassium bromide (molar mass taken as $120 \ g \ mol^{-1}$) to be added to $1 \ L$ of $0.05 \ M$ solution of silver nitrate to start the precipitation of $AgBr$ is

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