The solubility product $(K_{sp})$ values of $CuS$,$Ag_2S$,and $HgS$ are $10^{-31}$,$10^{-44}$,and $10^{-54}$ respectively. The solubilities of these sulphides are in the order:

At $T(K)$ in a saturated solution of $MgCO_3$ and $Ag_2CO_3$, if the concentration of $Mg^{2+}$ ion is $3.2 \times 10^{-5} \ M$, then the concentration of $Ag^{+}$ ion in the solution will be [Given: $K_{sp}(MgCO_3) = 1.6 \times 10^{-6}$ and $K_{sp}(Ag_2CO_3) = 8.0 \times 10^{-12}$ at $T(K)$]

The values of $K_{sp}$ for $CuS$,$Ag_2S$ and $HgS$ are $10^{-31}$,$10^{-42}$ and $10^{-54}$ respectively. The correct order of their solubility in water is

The solubility product $(K_{sp})$ of $AgCl$ at $100 \, ^\circ C$ is $1.44 \times 10^{-4}$. The solubility of $AgCl$ in boiling water is $.......$

The solubility product of a sparingly soluble salt $BA$ is $6.4 \times 10^{-13}$. Calculate its solubility in $\text{g dm}^{-3}$. The molar mass of the salt is $190 \text{ g mol}^{-1}$.

The solubility product of $PbI_{2}$ is $8.0 \times 10^{-9}$. The solubility of lead iodide in $0.1 \ M$ solution of lead nitrate is $x \times 10^{-6} \ mol/L$. The value of $x$ is ....... .(Rounded off to the nearest integer)
$[$Given: $\sqrt{2}=1.41]$