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