The normal freezing point of a certain organic solvent is 5.50 degrees C. When 0.3003 g of naphthalene (C10H8) is dissolved in 9.9876 g of this solvent, the solution has a freezing point of 4.32 Degrees C. What is the freezing point depression constant (kf) in Degree C/m, for this solvent?
Given that
mass of naphthalene, w = 0.3003 g
molar mass of naphthalene M = 128 g/mol
mass of solvent W = 9.9876 g = 0.0099876 kg
Kf = ? oC/m
depression in freezing point dT = 5.50 oC - 4.32 oC = 1.18 oC
We know that
depression in freezing point ΔT = Kf x molality
molality = (w/M) x (1/W in kg)
Then, depression in freezing point ΔT = Kf x { (w/M) x (1/W) }
1.18 oC = Kf [ (0.3003 g / 128 g/mol) x (1 x 0.0099876 kg)
kf = 5.02 oC/m
Therefore, freezing point depression constant (kf) = 5.02 oC/m
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