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Boiling Point Elevation Calculator

Calculate how solutes increase the boiling point of solutions using colligative properties

Calculate Boiling Point Elevation

Select Solvent

Select a common solvent or use custom values

Pure Solvent Boiling Point (T_solvent)

Boiling point of the pure solvent

Ebullioscopic Constant (K_b)

°C⋅kg/mol

Boiling point elevation constant for the solvent

Molality (m)

mol/kg

Moles of solute per kg of solvent

Van't Hoff Factor (i)

Number of particles formed per formula unit

Common Solute Types (Quick Select)

Boiling Point Elevation Results

Boiling Point Elevation (ΔT)

0.000°C

Celsius

0.000°F

Fahrenheit

0.000K

Kelvin

New Boiling Point (T_solution)

100.00°C

Celsius

212.00°F

Fahrenheit

373.15K

Kelvin

Formula: ΔT = i × K_b × m

Calculation: 1 × 0.512 × 0 = 0.000°C

Analysis: Pure solvent - no elevation

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Quick Examples

Salt Water

1 M NaCl in water

ΔT = 1.9 × 0.512 × 1 = 0.97°C

New BP: 100.97°C

Sugar Water

1 M Sugar in water

ΔT = 1 × 0.512 × 1 = 0.51°C

New BP: 100.51°C

Antifreeze Solution

2 M CaCl₂ in water

ΔT = 2.9 × 0.512 × 2 = 2.97°C

New BP: 102.97°C

Ebullioscopic Constants

Water0.512 °C⋅kg/mol

Benzene2.53 °C⋅kg/mol

Phenol3.04 °C⋅kg/mol

Acetic Acid3.07 °C⋅kg/mol

Naphthalene5.8 °C⋅kg/mol

Related Chemistry Calculators

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Freezing Point Depression

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Molality Calculator

Calculate solution molality

Osmotic Pressure Calculator

Calculate osmotic pressure of solutions

Understanding Boiling Point Elevation and Colligative Properties

What is Boiling Point Elevation?

Boiling point elevation is a colligative property where the addition of a non-volatile solute to a solvent increases the solution's boiling point. This occurs because solute particles disrupt the solvent's ability to vaporize, requiring more energy (higher temperature) to reach the boiling point.

Boiling Point Elevation Formula

ΔT = i × K_b × m

ΔT: Boiling point elevation (°C)
i: Van't Hoff factor (particles formed)
K_b: Ebullioscopic constant (°C⋅kg/mol)
m: Molality of solution (mol/kg)

Van't Hoff Factor Examples

Non-electrolytes (i = 1)

Sugar, glucose, urea - don't dissociate in solution

Binary electrolytes (i ≈ 2)

NaCl, KCl - dissociate into 2 ions

Ternary electrolytes (i ≈ 3)

CaCl₂, Na₂SO₄ - dissociate into 3 ions

Real-World Applications

• Automotive antifreeze solutions
• Road salt for winter ice melting
• Food preservation and cooking
• Laboratory purification processes
• Pharmaceutical formulations

Important Considerations

Molality vs Molarity

Use molality (mol/kg solvent) not molarity for temperature-dependent calculations

Ideal vs Real Solutions

Van't Hoff factors may differ from theoretical values due to ion pairing and other effects

Concentration Limits

Equation works best for dilute solutions; concentrated solutions show deviations

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