Van't Hoff factor of $BaCl_2$ in its aqueous solution will be: ($BaCl_2$ is $60 \%$ ionized in the solution)

Observe the following statements:
Statement-$I$: The boiling point of $0.1 \ M$ urea solution is less than that of $0.1 \ M$ $KCl$ solution.
Statement-$II$: Elevation of boiling point is inversely proportional to molar mass of solute.
The correct answer is:

Which of the following aqueous solutions exhibits the minimum freezing point depression upon complete dissociation?

The Van't Hoff factor of the compound $K_3[Fe(CN)_6]$ is

Which of the following aqueous solutions having same molality exhibits maximum boiling point elevation? (Assume complete dissociation)

What is the percentage of dissociation of a $0.011 \ m$ aqueous solution of $K_3[Fe(CN)_6]$ having a freezing point of $-0.063 \ ^oC$? (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water)