Consider the dissociation of the weak acid HX as given below HX ( aq ) ⇌ H^+( aq )+ X^-( aq ), Ka =1.2 × 10^-5 [ K_a:. dissociation constant ] The…

Consider the dissociation of the weak acid HX as given below $$\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}^{-}(\mathrm{aq}), \mathrm{Ka}=1.2 \times 10^{-5} $$ $\displaystyle \left[\mathrm{K}_{\mathrm{a}}:\right.$ dissociation constant $\displaystyle ]$ The osmotic pressure of $\displaystyle 0.03$ M aqueous solution of HX at $\displaystyle 300$ K is $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-2}$ bar (nearest integer). [Given : $\displaystyle \mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$ ]