If the concentration of sodium ions in a saturated solution of $Na_2SO_4$ is $10^{-5} \ mol/L$,find the solubility product $(K_{sp})$.

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

If $S$ and $K_{sp}$ are respectively solubility and solubility product of a sparingly soluble binary electrolyte,then

The solubility product of $Ag_2CO_3$ and $FeCO_3$ in water at $25 \, ^\circ C$ are $4 \times 10^{-12}$ and $2.5 \times 10^{-11}$ respectively. If $S_1$ and $S_2$ are their solubilities in water respectively when dissolved separately,then $S_1/S_2$ is

Which statement is incorrect for the solubility product $(K_{sp})$?

The volume of water required to dissolve $0.1 \ g$ $PbCl_2$ to get a saturated solution (in $mL$) is (Given $K_{sp}(PbCl_2) = 3.2 \times 10^{-8}$; Atomic mass of $Pb = 207 \ u$, $Cl = 35.5 \ u$)