The observed osmotic pressure for a $0.10 \ M$ solution of $Fe(NH_4)_2(SO_4)_2$ at $25 \ ^oC$ is $10.8 \ atm$. The expected and experimental (observed) values of van't Hoff factor $(i)$ will be respectively: $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

If $A_2 B$ is $30 \%$ ionised in an aqueous solution,then the value of van't Hoff factor $(i)$ is $............ \times 10^{-1}$.

The osmotic pressure $(O.P.)$ of equimolar solutions of $Urea$,$BaCl_2$,and $AlCl_3$ will be in the order:

The freezing points of equimolar solutions of glucose,$KNO_3$ and $AlCl_3$ are in the order of:

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

Which of the following substances shows the highest colligative properties?