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

Which of the following solutions has the lowest freezing point?

Which of the following solutions has an osmotic pressure nearest to that of an equimolar solution of $K_4[Fe(CN)_6]$?

$0.6 \, mL$ of acetic acid $(CH_{3}COOH)$,having density $1.06 \, g \, mL^{-1}$,is dissolved in $1 \, L$ of water. The depression in freezing point observed for this strength of acid was $0.0205^{\circ} \, C$. Calculate the van't Hoff factor and the dissociation constant of acid.

$A$ $0.1 \ mol$ 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 ............. $K \ kg \ mol^{-1}$.

The depression in freezing point for $0.01 \ m$ aqueous solution of $K_{x}[Fe(CN)_6]$ is $0.0744 \ K$. The molal depression constant for solvent is $1.86 \ K \ kg \ mol^{-1}$. If the solute undergoes complete dissociation,what is the correct molecular formula for the solute?