$pH$ of a $0.1 \ M$ monobasic acid is found to be $2$. Hence its osmotic pressure at a given temperature $T \ K$ is (in $RT$)

$MX_{2}$ dissociates into $M^{2+}$ and $X^{-}$ ions in an aqueous solution,with a degree of dissociation $(\alpha)$ of $0.5$. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is

If a $0.25 \, m$ solution of electrolyte $X_3Y_2$ undergoes $50 \%$ ionization,the van't Hoff factor will be ...... .

The freezing point of a $2\%$ aqueous solution of $[Ag(CH_3NH_2)_2]Cl$ is:

The percentage dissociation of a salt $(MX_3)$ solution at a given temperature $($van't Hoff factor $i = 2)$ is $..........\%$ ($Nearest$ $integer$).

The freezing point of a $0.0020 \ m$ aqueous solution of $[CO(NH_3)_5(NO_2)]$ is $-0.00732 \ ^oC$. The number of ions produced (van't Hoff factor,$i$) when $1 \ mol$ of this ionic compound is dissolved in water is ..... $(K_f = 1.86 \ K \ kg \ mol^{-1})$