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

The solubility of a salt of weak acid $(AB)$ at $pH = 3$ is $Y \times 10^{-3} \ mol \ L^{-1}$. The value of $Y$ is (Given that the value of solubility product of $AB$ $(K_{sp}) = 2 \times 10^{-10}$ and the value of ionization constant of $HB$ $(K_{a}) = 1 \times 10^{-8}$)

The $K_{sp}$ values of $Al(OH)_3$ and $Zn(OH)_2$ are $8.5 \times 10^{-23}$ and $1.8 \times 10^{-14}$ respectively. If $NH_4OH$ is added to a solution containing $Al^{3+}$ and $Zn^{2+}$ ions,which will precipitate earlier?

Precipitation occurs if the ionic product is ........

When $150 \ mL$ of $0.0008 \ M$ ammonium sulfate solution is mixed with $50 \ mL$ of $0.04 \ M$ calcium nitrate solution,given $K_{sp} = 2.4 \times 10^{-5}$ for $CaSO_4$,what is the ionic product of $CaSO_4$?

Solubility product expression of salt $MX_4$ which is sparingly soluble with a solubility $(S)$ can be given as