Van't Hoff factor of $BaCl_2$ in its aqueous solution will be: ($BaCl_2$ is $60 \%$ ionized in the solution)

$0.004 \ M$ $Na_2SO_4$ solution is isotonic with $0.01 \ M$ glucose solution,then the degree of dissociation of $Na_2SO_4$ is ........... $\%$.

Solutions $A$,$B$,$C$ and $D$ are respectively $0.1 \ M$ glucose,$0.05 \ M \ NaCl$,$0.05 \ M \ BaCl_{2}$ and $0.1 \ M \ AlCl_{3}$. Which one of the following pairs is isotonic?

Which of the following solutes has the ratio of theoretical molar mass to the experimentally observed molar mass equal to $3$?

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).
$[\text{Given: } R = 0.083 \ L \ bar \ mol^{-1} \ K^{-1}]$

An aqueous solution of a salt $MX_2$ at a certain temperature has a van't Hoff factor of $2$. The degree of dissociation for this solution of the salt is