For water,$K_f = 1.86 \ K \ kg \ mol^{-1}$. If your car radiator contains $1.0 \ kg$ of water,how many grams of ethylene glycol $(C_2H_6O_2)$ must be added to lower the freezing point of the solution to $-2.8 \ ^\circ C$?

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 $[K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1}]$

Calculate the cryoscopic constant $(K_f)$ of a solvent if the depression in freezing point of a $0.4 \ m$ solution of a non-volatile solute is $1.8 \ K$.

What is the mass of solute having molar mass $60 \ g \ mol^{-1}$ when dissolved in $98 \ g$ of solvent decreases its freezing point by $0.2 \ K$ (in $g$)? (The numerical value of cryoscopic constant of solvent is $1.71 \ K \ kg \ mol^{-1}$)

Which of the following will produce the maximum depression in freezing point of its aqueous solution?

$1\%$ solution of $Ca(NO_3)_2$ has a freezing point: