Solubility (in molarity) of sparingly soluble salts $MX, MX_2$ and $MX_3$ in water are same. The order of $K_{sp}$ of $MX, MX_2$ and $MX_3$ is

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.

At $298 \ K$,the solubility of silver chloride in water is $1.434 \times 10^{-3} \ g \ L^{-1}$. The value of $-\log K_{sp}$ for silver chloride is $........$ (Given: molar mass of $Ag = 107.9 \ g \ mol^{-1}$ and $Cl = 35.5 \ g \ mol^{-1}$)

What is the solubility of $PbSO_4$ in centinormal $(0.01 \ N)$ $H_2SO_4$ solution? The solubility product $(K_{sp})$ of $PbSO_4$ at a given temperature is $1 \times 10^{-8} \ (mol/L)^2$.

The solubility of $CdSO_{4}$ in water is $8.0 \times 10^{-4} \ mol \ L^{-1}$. Its solubility in $0.01 \ M \ H_{2}SO_{4}$ solution is $..... \ \times 10^{-6} \ mol \ L^{-1}$.
(Round off to the Nearest integer) (Assume that solubility is much less than $0.01 \ M$)

The solubility product of $Mg(OH)_2$ is $1.0 \times 10^{-12}$. Concentrated aqueous $NaOH$ solution is added to a $0.01 \ M$ aqueous solution of $MgCl_2$. The $pH$ at which precipitation occurs is