The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of Van't Hoff factor $i$ is

If the degree of ionisation of $KI_3$ is $80\%$,then what will be its van't Hoff factor?

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)

When $9.45 \text{ g}$ of $ClCH_2COOH$ is added to $500 \text{ mL}$ of water,its freezing point drops by $0.5^\circ \text{C}$. The dissociation constant of $ClCH_2COOH$ is $x \times 10^{-3}$. The value of $x$ is ............... (Rounded off to the nearest integer) $[K_{f(H_2O)} = 1.86 \text{ K kg mol}^{-1}]$

If sodium sulfate $(Na_2SO_4)$ undergoes complete dissociation into its constituent ions in an aqueous solution,what will be the depression in freezing point $(\Delta T_f)$ when $0.01 \ mol$ of sodium sulfate is dissolved in $1 \ kg$ of water (in $K$)? (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$)

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