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} $
$\left[\mathrm{K}_{\mathrm{a}}:\right.$ dissociation constant $]$
The osmotic pressure of 0.03 M aqueous solution of HX at 300 K is $\_\_\_\_$ $\times 10^{-2}$ bar (nearest integer).
[Given : $\mathrm{R}=0.083 \mathrm{LbarMol}^{-1} \mathrm{~K}^{-1}$ ]