The freezing point of a $0.05 \ m \ BaCl_2$ solution in water ($100 \%$ ionisation) is about $(K_f = 1.86 \ K \ kg \ mol^{-1})$. (in $^oC$)

$17.4\% \text{ (mass/volume) } K_2SO_4$ solution at $27^\circ C$ is isotonic to $5.85\% \text{ (mass/volume) } NaCl$ solution at $27^\circ C$. If $NaCl$ is $100\%$ ionized,what is the $\%$ ionization of $K_2SO_4$ in aqueous solution? [Atomic weights: $K = 39, Na = 23, S = 32, O = 16, Cl = 35.5$]

$A$ centimolar solution of acetic acid is $50 \%$ dissociated at $27^{\circ} C$. The osmotic pressure of the solution (in $atm$) is $\left(R=0.083 \ L \ atm \ K^{-1} \ mol^{-1}\right)$

The correct relationship between the boiling points of very dilute solutions of $AlCl_3$ $(t_1)$ and $CaCl_2$ $(t_2)$,having the same molar concentration is

The freezing point of a solution prepared by adding $8.1 \ g$ of $HBr$ ($90\%$ ionized) to $100 \ g$ of water is $...... \ ^\circ C$. (Given $K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$)

Which of the following solutes dissolved in water,having the same concentration,exhibits the highest value of colligative property?