Two moles of a nonelectrolyte solute are dissolved in 1 kg of an unknown solvent. The solution freezes at 7.8 degrees Celsius below its normal freezing point. What is the molal freezing point constant of the unknown solvent? What is your prediction for the identity of the solvent?
Chemistry - DrBob222, Tuesday, May 18, 2010 at 12:07am
m = moles/kg solvent
m = 2/1 = 2m
delta T = Kf*m
7.8 = Kf*2
Kf = 7.8/2 = ??
Here is a list of constants. Pick yours.