$pH$ of a $0.1 \ M$ monobasic acid is found to be $2$. Hence its osmotic pressure at a given temperature $T \ K$ is (in $RT$)

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

Calculate the depression in the freezing point of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ in $100 \ g$ of $H_2O$. (Molecular weight of $K_3[Fe(CN)_6] = 329 \ g \ mol^{-1}$; $K_f = 1.86 \ K \ kg \ mol^{-1}$)

The freezing point of an equimolal aqueous solution will be highest for:

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 van 't Hoff factor $(i)$ for these solutions will be in the order:

Which one of the following is the ratio of the lowering of vapour pressure of $0.1 \ M$ aqueous solutions of $BaCl_2, NaCl$ and $Al_2(SO_4)_3$ respectively?