The solubility product of $BaCl_2$ is $4 \times 10^{-9}$. Its solubility in $mol/L$ is .......

Which one of the following arrangements represents the correct order of solubilities of sparingly soluble salts $Hg_2Cl_2$,$Cr_2(SO_4)_3$,$BaSO_4$ and $CrCl_3$ respectively?

Solubility product of a salt $AB$ is $1 \times 10^{-8}$ in a solution in which the concentration of $A^{+}$ ions is $10^{-3} \ M$. The salt will precipitate when the concentration of $B^{-}$ ions is kept

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.

The solubility of a salt of a weak acid $MX$ (e.g.,phosphoric acid salts) increases at lower $pH$. Explain with equations.

For the precipitation reaction of $Ag^{+}$ ions with $NaCl$,which of the following statements is correct?