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

Which of the following $0.10 \ m$ aqueous solution will have the lowest freezing point?

Which of the following has the highest boiling point at $1 \, atm$ pressure?

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

We have three aqueous solutions of $NaCl$ labelled as '$A$','$B$' and '$C$' with concentrations $0.1 \ M$,$0.01 \ M$,and $0.001 \ M$ respectively. The value of the Van't Hoff factor for these solutions will be in the order . . . . . . .

$17.4\%\, (w/v)$ $K_2SO_4$ $(Mw=174\, g/mol)$ solution at $27\, ^\circ C$ is isotonic to $4\%\, (w/v)\, NaOH$ solution at the same temperature. If $NaOH$ is $100\%$ ionized,what is the $\%$ ionization of $K_2SO_4$ in aqueous solution .......... $\%$.