Which of the following aqueous solutions has the highest freezing point?

$5 \ g$ sucrose (molar mass $= 342 \ g \ mol^{-1}$) is dissolved in $100 \ g$ of solvent,decreasing the freezing point by $2.15 \ K$. What is the cryoscopic constant $(K_{f})$ of the solvent?

Two elements $A$ and $B$ form compounds with molecular formulas $AB_2$ and $AB_4$. When $1 \ g$ of $AB_2$ is dissolved in $20 \ g$ of $C_6H_6$,the freezing point decreases by $2.3 \ K$. When $1 \ g$ of $AB_4$ is dissolved in $20 \ g$ of $C_6H_6$,the freezing point decreases by $1.3 \ K$. The molal depression constant for benzene is $5.1 \ K \ kg \ mol^{-1}$. Calculate the atomic weights of $A$ and $B$.

The freezing point depression of a solution containing $0.6 \ g$ of urea (molar mass $= 60 \ g \ mol^{-1}$) in $100 \ mL$ of benzene (in $K$) is ($K_f$ of benzene $= 4.0 \ K \ kg \ mol^{-1}$).

In cold countries,ethylene glycol is added to water in the radiators to:

Which of the following solutions exhibits the highest freezing point depression?