# Problem: Which of the following ideal solutions would be predicted to have the lowest freezing point?A. 0.35 m NaClB. 0.15 m C6H12O6C.  0.20 m MgCl2D. 0.10 m Na3PO4

###### FREE Expert Solution

The change in freezing point is also related to the molality of the solution:

$\overline{){{\mathbf{\Delta T}}}_{{\mathbf{f}}}{\mathbf{=}}{{\mathbf{imK}}}_{{\mathbf{f}}}}$

where:

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

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###### Problem Details

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