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

Calculate the amount of $KCl$ $(MW=74.5 \ g \ mol^{-1})$ required to depress the freezing point of $500 \ g$ of water by $2 \ K$ (in $g$)? $(K_f=1.86 \ K \ kg \ mol^{-1})$

Which of the following $0.1 \, M$ aqueous solutions has the lowest freezing point?

The osmotic pressure of a dilute solution of an ionic compound $XY$ in water is four times that of a solution of $0.01\, M\, BaCl_2$ in water. Assuming complete dissociation of the given ionic compounds in water,the concentration of $XY$ (in $mol\, L^{-1}$) in solution is

$K_2HgI_4$ is $40 \%$ ionized in aqueous solution. The value of its van't Hoff factor $(i)$ is:

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)