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

Calculate the molar solubility of $Ni(OH)_{2}$ in $0.10 \, M$ $NaOH$. The solubility product constant $(K_{sp})$ of $Ni(OH)_{2}$ is $2.0 \times 10^{-15}$.

Express the relationship between $K_{sp}$ and solubility $(S)$ for the salt $Ca_3(PO_4)_2$.

The solubility of $AgBr_{(s)}$,having solubility product $5 \times 10^{-10}$ in $0.2 \ M$ $NaBr$ solution,equals

What are the products formed when an aqueous solution of $CuCl_2$ and $(NH_4)_2S$ are mixed?

Find the concentration of the ion which is first precipitated at the point when the third ion starts precipitating,if $AgNO_3$ is added gradually to a solution that contains $0.1 \ M \ Cl^{-}$,$0.1 \ M \ Br^{-}$,and $0.1 \ M \ I^{-}$.
Given that:

Salt	$K_{sp}$
$AgCl$	$2 \times 10^{-10}$
$AgBr$	$5 \times 10^{-13}$
$AgI$	$9 \times 10^{-17}$