The Van't Hoff factor of the compound $K_3[Fe(CN)_6]$ 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 $g$)? $(K_f=1.86 \ K \ kg \ mol^{-1})$

What is the freezing point of a solution containing $8.1 \ g \ HBr$ in $100 \ g$ water,assuming the acid to be $90 \ \%$ ionised ($K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$)?

$0.004 \ M \ K_2SO_4$ solution is isotonic with $0.01 \ M$ glucose solution. The percentage dissociation of $K_2SO_4$ is $........$ (Nearest integer).

Which of the following will have the lowest vapor pressure?

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