Which of the following has the lowest freezing point?

$K_f$ for water is $1.86 \, K \, kg \, mol^{-1}$. If your automobile radiator holds $1.0 \, kg$ of water,how many $gm$ of ethylene glycol $(C_2H_6O_2)$ must you add to lower the freezing point of the solution to $-2.8 \, ^oC$?

What is the freezing point of a $1 \ molal$ aqueous solution of a non-volatile solute (in $^{\circ} C$)? $(K_{f} = 1.86 \ K \ kg \ mol^{-1}, T_{f}^{\circ} \text{ for water } = 0^{\circ} C)$

An aqueous solution of a weak monobasic acid containing $0.1 \text{ g}$ in $21.7 \text{ g}$ of water freezes at $272.813 \text{ K}$. If the value of $K_f$ for water is $1.86 \text{ K kg/mol}$,what is the molecular mass of the monobasic acid in $\text{g/mol}$?

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

$150 \ g$ of acetic acid was contaminated with $10.2 \ g$ ascorbic acid $(C_{6}H_{8}O_{6})$ to lower its freezing point by $(x \times 10^{-1})^{\circ} C$. The value of $x$ is (Nearest integer). [Given $K_{f} = 3.9 \ K \ kg \ mol^{-1}$; Molar mass of ascorbic acid $= 176 \ g \ mol^{-1}$]