Q55. 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 :\\
$\mathrm { R } = 0.083 \mathrm { Lbarmol } ^ { - 1 } \mathrm {~K} ^ { - 1 }$ ]\\