A 0.1 molal aqueous solution of a weak electrolyte, HX, freezes at -0.208 °C. Assuming ideal behavior, what is the van't Hoff factor (i) for HX in this solution? (K$_f$ for water = 1.86 K kg mol$^{-1}$)

Which of the following aqueous solution has highest boiling point?

The osmotic pressure of a solution can be accurately measured in the shortest possible time by :

The mass of glucose that should be dissolved in 50 g of water in order to produce the same lowering of vapour pressure as is produced by dissolving 1 g of urea in the same quantity of water is

Which of the following statements is false?

If molality of the dilute solution is doubled, the value of molal depression constant $({K_f})$ will be

The empirical formula of a nonelectrolyte is $C{H_2}O$. A solution containing 3 g of the compound exerts the same osmotic pressure as that of $0.05\;M$ glucose solution. The molecular formula of the compound is

The molal elevation/depression constant depends upon :

If the elevation in boiling point of a solution of 10 g of solute (mol. wt. = 100 g of water is $\Delta {T_b}$, the ebullioscopic constant of water is

$20\;g$ of binary electrolyte (mol. wt. =100) are dissolved in $500\;g$ of water. The depression in freezing point of the solution is $0.74^\circ C\;({k_f} = 1.86\;K{m^{ - 1}})$ the degree of ionisation of the electrolyte is

The depression in f.p. is directly proportional to :