$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \%$ ionised. The freezing point of this solution is .......... $^oC$. ($K_f = 1.86 \, K \cdot kg \cdot mol^{-1}$ for water) :-

Which of the following has the highest boiling point?

$A$ $0.1 \ mol$ of a binary electrolyte undergoes complete dissociation in $250 \ g$ of a protic solvent. If the elevation in boiling point is $1.5 \ K$,the molal elevation constant $(K_b)$ is ............. $K \ kg \ mol^{-1}$.

Considering acetic acid dissociates in water,its dissociation constant is $6.25 \times 10^{-5}$. If $5 \ mL$ of acetic acid is dissolved in $1 \ L$ water,the solution will freeze at $-x \times 10^{-2} \ {}^{\circ}C$,provided pure water freezes at $0 \ {}^{\circ}C$.
$x = . . . . . . . . .$ (Nearest integer)
Given: $(K_{f})_{\text{water}} = 1.86 \ K \ kg \ mol^{-1}$.
Density of acetic acid is $1.2 \ g \ mL^{-1}$.
Molar mass of water $= 18 \ g \ mol^{-1}$.
Molar mass of acetic acid $= 60 \ g \ mol^{-1}$.
Density of water $= 1 \ g \ cm^{-3}$.
Acetic acid dissociates as:
$CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$

Which of the following salts has the same value of Van't Hoff factor $i$ as that of $K_4[Fe(CN)_6]$?

Which of the following aqueous solutions has the highest freezing point?