The freezing point of pure benzene is 278.70K and Kf4.90K/m. When 2.30g of an unknown solute is added to 63.0g of benzene, the freezing point of the solution is 276.50K. Determine the molecular weight of the unknown. Calculate the freezing point (C) of a solution prepared by dissolving 48.0g of glycerin (C3H8O3, a nonelectrolyte) in 184g of ethanol. Ethanol has a freezing point of 114.6C and a molal freezing point depression constant of 2.00C/m