Identify the compound amongst the following whose $0.1 \ M$ aqueous solution has the highest boiling point.

The freezing point (in ${}^{\circ}C$) of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ (Mol. Wt. $329$) in $100 \ g$ of water $(K_f = 1.86 \ K \ kg \ mol^{-1})$ is

The freezing point depression of a $0.01 \ m$ aqueous solution of $[Pt(NH_3)_4Cl_4]$ is $0.0054^\circ C$. If $K_f$ for water is $1.80 \ K \ kg \ mol^{-1}$,what is the correct formula for the complex?

$0.2 \ molal$ aqueous solution of an electrolyte $A_3B$ is $90\%$ ionised. The boiling point of the solution at $1 \ atm$ is ........ $K.$ ($K_b$ for $H_2O = 0.52 \ K \ Kg \ mol^{-1}$ and $B.pt.$ of $H_2O = 373 \ K$)

Calculate the depression in the freezing point of water when $10 \ g$ of $CH_3CH_2CHClCOOH$ is added to $250 \ g$ of water. $K_a = 1.4 \times 10^{-3}$,$K_f = 1.86 \ K \ kg \ mol^{-1}$

The osmotic pressure of a $0.1 \ M$ solution of $NaCl$ and $Na_2SO_4$ will be: