Calculate boiling-point elevation from solute mass, molar mass, solvent mass and the van’t Hoff factor.
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New boiling point
How to use this tool
Enter solute mass in grams and molar mass in g/mol.
Enter solvent mass in kilograms.
Choose the van’t Hoff factor and the solvent.
Read molality, elevation and the new boiling point.
Formula & worked example
58.44 g of NaCl (1 mol) in 1 kg of water with i = 2 raises the boiling point by 1.024 °C, to 101.02 °C.
Limitations — read this before you rely on it
Dilute-solution model only: it assumes a non-volatile solute and ideal dissociation, and overstates elevation at high concentrations.
Frequently asked questions
The number of particles a solute splits into: 1 for sugar, 2 for NaCl, 3 for CaCl2, in the ideal limit.
Electrolytes dissociate incompletely and ions interact, so the effective factor falls below the nominal count as concentration rises.
Moles of solute per kilogram of solvent; unlike molarity it does not change as the solution warms and expands.
Yes, each solvent has its own ebullioscopic constant Kb and its own pure boiling point.
A pinch of salt is a tiny molality, so the elevation is hundredths of a degree, not a practical cooking difference.