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ChemBench
Salt in the pot, a higher boiling point.
Adding a solute lowers the solvent's vapor pressure at any given temperature, so the solution needs a higher temperature to reach the boiling point — more dissolved particles (higher molality × van 't Hoff factor) means a bigger elevation.
A solute that splits into multiple ions in solution (like NaCl splitting into Na⁺ and Cl⁻) raises the boiling point roughly twice as much as a solute that stays as one particle, for the same molar amount — this is captured by the factor i.
Molar mass of any chemical formula (e.g. H2O, C6H12O6, Ca(OH)2).
OpenPercent composition of an element within a chemical formula.
OpenSimplest whole-number ratio formula from elemental masses or percentages.
OpenPercent yield from actual and theoretical reaction yields.
OpenBoiling point elevation
0.512 °C
What you entered
ΔTb = i × Kb × m
1 × 0.512 × 1= 0.512 °CResult
Boiling point elevation: 0.512 °C
This solution's boiling point rises by 0.512°C above pure solvent.