The maximum freezing point depression constant $(K_f)$ is observed for which of the following solvents?

$50 \ g$ of antifreeze (ethylene glycol) is added to $200 \ g$ of water. What amount of ice will separate out at $-9.3 \ ^oC$? $(K_f = 1.86 \ K \ kg \ mol^{-1})$

Identify the correct relation between depression in freezing point and the freezing point of a pure solvent.

The freezing point of a solution prepared from $1.25 \ g$ of a non-electrolyte and $20 \ g$ of water is $271.9 \ K$. If the molar depression constant is $1.86 \ K \ kg \ mol^{-1}$,then the molar mass of the solute will be:

The freezing point of a $0.05 \ molal$ solution of a non-electrolyte in water is $.......... \ ^oC$. $(K_f = 1.86 \ K \ kg \ mol^{-1})$

An aqueous solution containing $0.2 \ g$ of a non-volatile solute '$A$' in $21.5 \ g$ of water freezes at $272.814 \ K$. If the freezing point of water is $273.16 \ K$,the molar mass (in $g \ mol^{-1}$) of solute '$A$' is $[K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1}]$