Calculate freezing point depression for any solution using Kf, molality, and van't Hoff factor. Free chemistry calculator for students, researchers, and engineers.
The molal freezing point depression constant is specific to the solvent. Common values: Water (1.86), Benzene (5.12), Acetic Acid (3.90).
The concentration of solute in moles per kilogram of solvent.
The number of particles a solute forms when dissolved. For non-electrolytes like sugar, i = 1. For strong electrolytes, i equals the number of ions formed.
ΔTf = i × Kf × m
Where ΔTf is the freezing point depression, i is the van't Hoff factor, Kf is the molal freezing point depression constant, and m is the molality.
ΔTf = 1 × 1.86 × 1.00 = 0.00 °C
Visual representation of freezing point depression (not to scale)
This is how much the freezing point of the solvent will decrease due to the dissolved solute.
| Solvent | Kf (°C·kg/mol) |
|---|---|
| Water | 1.86 °C·kg/mol |
| Benzene | 5.12 °C·kg/mol |
| Acetic Acid | 3.90 °C·kg/mol |
| Cyclohexane | 20.0 °C·kg/mol |
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