An aqueous solution of a non electrolyte boils at 100.32 degrees C. The expected freezing point for this solution is ______?
(Kb water = 0.512 degrees Cm^-1, Kf water= 1.86 Degree C m^-1)
a. 0 Degrees
b. -0.32
c. -0.83
d. -1.16
e insufficient information
d. The lowering effect upon the freezing point due to a solvent is 1.86/0.512 = 3.63 times the boiling point raising effect. Multiply -3.63 by 0.32 C to get the lowering.
To determine the expected freezing point for a solution, we need to use the formula for freezing point depression:
ΔTf = Kf * m
Where:
ΔTf = Freezing point depression
Kf = Freezing point constant
m = Molality of the solution
However, in this case, we are not given the molality of the solution. Therefore, we cannot calculate the freezing point depression.
Hence, the answer is (e) insufficient information.