Ionic Equilibrium

Consider the dissociation of the weak acid HX as given below

\(\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}^{-}(\mathrm{aq}), \mathrm{Ka}=1.2 \times 10^{-5}\)

[\(\mathrm{K}_{\mathrm{a}}\) : dissociation constant]

The osmotic pressure of \(0.03 \mathrm{M}\) aqueous solution of \(\mathrm{HX}\) at \(300 \mathrm{~K}\) is _________ \(\times 10^{-2}\) bar (nearest integer).

[Given : \(\mathrm{R}=0.083 \mathrm{~L} \mathrm{~bar} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\)]