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

$0.2 \ molal$ 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 $H_2O = 373 \ K$)

Which one of the following electrolytes has the same value of van't Hoff factor $(i)$ as that of $Al_2(SO_4)_3$ (if all are $100 \%$ ionised)?

The freezing point of a $1.00 \ m$ aqueous solution of $HF$ is found to be $-1.91 \ ^oC$. The freezing point constant of water,$K_f$ is $1.86 \ K \ kg \ mol^{-1}$. The percentage dissociation of $HF$ at this concentration is ................ $\%$

If the freezing point of a $0.01 \ m$ aqueous solution of a cobalt $(III)$ chloride-ammonia complex (which behaves as a strong electrolyte) is $-0.0558^{\circ} C$,the number of chloride $(Cl^-)$ ions in the coordination sphere of the complex is.
$\left[ K_{f} \text{ of water } = 1.86 \ K \ kg \ mol^{-1} \right]$

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 $K_3[Fe(CN)_6] = 329 \ g \ mol^{-1}$; $K_f = 1.86 \ K \ kg \ mol^{-1}$)