The change in freezing point is also related to the molality of the solution:
ΔTf = change in freezing point = Tf pure solvent –Tf solution
i = van’t Hoff factor
m = molality of the solution (in m or mol/kg)
Kf = freezing point depression constant (in ˚C/m) of the solvent
Which of the following ideal solutions would be predicted to have the lowest freezing point?
A. 0.35 m NaCl
B. 0.15 m C6H12O6
C. 0.20 m MgCl2
D. 0.10 m Na3PO4
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