For a dilute solution of $K_3[Fe(CN)_6]$,the van't Hoff factor $(i)$ is ..... [assuming $100\%$ ionization]

$19.5 \text{ g}$ of fluoroacetic acid (molar mass = $78 \text{ g mol}^{-1}$) is dissolved in $500 \text{ g}$ of water at $298 \text{ K}$. The depression in the freezing point of water was $1^\circ\text{C}$. What is $K_a$ of fluoroacetic acid? (For water, $K_f = 1.86 \text{ K kg mol}^{-1}$). Assume molarity and molality to have same values.

Assuming $100\%$ ionization,the correct order of freezing point for the following solutions is:

What would the boiling point elevation of $0.1 \ m$ $KNO_3$ be equal to?

At a constant temperature,the vapor pressures of aqueous solutions of $Na_2SO_4$,urea,$AlCl_3$,and $1.2 \, m \, KCl$ are approximately equal. The molalities of the aqueous solutions of $Na_2SO_4$,urea,and $AlCl_3$ are,respectively: (Assume $100 \%$ dissociation of the solute)

$0.1 \ m$ solutions of sodium sulphate,urea,and sodium chloride are taken. The correct ratio of the elevation of boiling point of these solutions is