If the $O.P.$ (Osmotic Pressure) of $1 \ M$ solutions of the following compounds in water can be measured,which one will show the maximum $O.P.$?

In which case is Raoult's law not applicable?

Identify the compound amongst the following whose $0.1 \ M$ aqueous solution has the highest boiling point.

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

At a certain temperature,the vapour pressure of pure water is $76 \ mm$ of $Hg$. When $1 \ mol$ of $Na_2SO_4$ is dissolved in $36 \ mL$ of water,the vapour pressure of the solution becomes $38 \ mm$ of $Hg$. What is the percentage dissociation of $Na_2SO_4$ in the solution?

In equimolar solutions of glucose,$NaCl$,and $BaCl_2$,the order of osmotic pressure is as follows: