what would be the freezing point for a 5.7 molal aqueous sucrose (C12H22O11)solution

Question

the freezing point depression constant water =1.86 C/m. show your work

Answer 1

The first thing to determine is if the solute, in this case sucrose, is an electrolyte our a non electrolyte. Sucrose is s non electrolyte so the van’t Hoff factor(i) will be1.

ΔT = imK

ΔT = change in temperature =?

i = van’t Hoff factory = 1

m = molality = 5.7

K = freezing point constant = 1.86

ΔT = (1)(5.7)(1.86) = 10.6 degrees

New freezing point = 0 - 10.6 = -10.6 degrees C