If the solubility product of $BaSO_4$ is $1.5 \times 10^{-9}$ in water,its solubility in moles per litre is

$150 \, mL$ of $0.0008 \, M$ ammonium sulphate is mixed with $50 \, mL$ of $0.04 \, M$ calcium nitrate. The ionic product of $CaSO_4$ will be ($K_{SP} = 2.4 \times 10^{-5}$ for $CaSO_4$)

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ will occur in - ($K_{sp}$ of $AgCl = 1.8 \times 10^{-10}$)

The solubility products of $NiS$,$ZnS$,$CdS$,and $HgS$ are $4.7 \times 10^{-5}$,$1.6 \times 10^{-24}$,$8 \times 10^{-27}$,and $4 \times 10^{-53}$ respectively. An aqueous solution contains $Ni^{2+}$,$Zn^{2+}$,$Cd^{2+}$,and $Hg^{2+}$ of equal concentration. $H_2S$ gas was passed into this solution very slowly. The first and the last ions that precipitate as sulphides are respectively.

If the solubility of $MX_2$ in water is $0.0002 \ mol/L$,then its $K_{sp}$ is:

The solubility product constants $(K_{sp})$ for some silver salts are given as: $AgCl = 2 \times 10^{-10}$,$AgBr = 5 \times 10^{-13}$,$Ag_2CO_3 = 8 \times 10^{-12}$,and $AgI = 8 \times 10^{-17}$. Which of the following salts has the highest solubility?