How does the Freezing Point Depression work?

ΔTf = i × Kf × m (molality, not molarity) Then: Kf(water) = 1.86 °C·kg/mol Then: Molality m = moles solute / kg solvent Then: van't Hoff factor i = number of particles per formula unit (1 for glucose, 2 for NaCl, 3 for CaCl₂).

Can you give an example of how to use the Freezing Point Depression?

Example: Input 1 mol NaCl in 1 kg water · i=2 · Kf=1.86 gives a result of ΔTf = 3.72°C → freezes at −3.72°C (2×1.86×1=3.72°C depression).

Is the Freezing Point Depression free to use?

Yes — completely free with no registration, download, or subscription required. All calculations happen instantly in your browser.

How accurate is the Freezing Point Depression?

Our Freezing Point Depression uses verified mathematical formulas and is accurate to multiple decimal places. Results are calculated in real-time using the same methods used by professionals.

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Freezing Point Depression

❄️Freezing Point Depression (ΔTf=iKfm)

Kf (°C·kg/mol)

Water=1.86

Molality m (mol/kg)

van't Hoff factor i

NaCl=2, glucose=1

Freezing point depression is a colligative property: adding a solute to a pure solvent lowers the freezing point. ΔTf = i × Kf × m, where i is the van't Hoff factor, Kf is the cryoscopic constant, and m is molality.

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Did You Know?

Road salt (NaCl) works by freezing point depression, but only down to about −9°C. At lower temperatures, CaCl₂ (which gives i=3 and larger ΔTf) is used for de-icing.

References

›Freezing-point depression — Wikipedia

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Freezing Point Depression

❄️Freezing Point Depression (ΔTf=iKfm)

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❄️Freezing Point Depression (ΔTf=iKfm)