Chemistry
posted by Jaden .
If the freezing point of pure toluene is 95.15 oC and its freezing point depression constant is 8.38 oC/molal, what is the freezing point of a solution made by dissolving 39.338g of anthracene (C14H10) in 150.0mL of toluene? (Density of toluene = 0.8669g/mL)

mol anthracene = grams/molar mass
grams toluene = volume x density
molality = mol anthracene/kg toluene.
delta T = Kf*m. Solve for delta T.
Subtract from zero to find new freezing point.