Boiling Point Elevation
ΔTb = Kb·m·i. Colligative property: nonvolatile solute raises BP. Depends on particle count (van't Hoff i), not solute identity.
Why This Chemistry Calculation Matters
Why: Colligative property: solute particles lower vapor pressure, raising BP. Salt in water, sugar in syrup. Ebullioscopy.
How: ΔTb = Kb × m × i. Kb = ebullioscopic constant (water 0.512°C·kg/mol). i = van't Hoff (NaCl→2, sucrose→1).
- ●Water Kb = 0.512°C·kg/mol.
- ●Electrolytes: i = number of ions (NaCl i=2).
- ●Nonvolatile solute only.
- ●New BP = normal BP + ΔTb.
Solution Examples
🧂 Salt Water Solution
NaCl in water - common example
🍬 Sugar Solution
Sucrose in water - non-electrolyte
⚖️ Calculate from Mass
Determine elevation from solute mass
🔬 CaCl₂ Solution
Strong electrolyte with i=3
🍷 Ethanol Solvent
Solution in ethanol instead of water
🍇 Glucose Solution
Biological solution example
📊 Find Molality from ΔT
Calculate concentration from elevation
🧪 Urea Solution
Non-electrolyte example
⚗️ Benzene Solvent
Organic solvent with high Kb
🚗 Antifreeze Solution
Ethylene glycol in water
🧬 KCl Solution
Potassium chloride electrolyte
📝 Custom Values
Enter your own parameters
Calculate Boiling Point Elevation
For educational and informational purposes only. Verify with a qualified professional.
🔬 Chemistry Facts
ΔTb = Kb·m·i. Colligative, particle-count dependent.
— IUPAC
Water Kb = 0.512°C·kg/mol.
— CRC
Van't Hoff i: NaCl=2, CaCl₂=3, sucrose=1.
— Solution chem
Ebullioscopy: BP elevation for molecular weight.
— Analytical
Boiling Point Elevation
Boiling point elevation is a colligative property - it depends on the number of solute particles, not their identity. Adding a nonvolatile solute raises the boiling point of a solvent.
ΔTb = boiling point elevation, Kb = ebullioscopic constant, m = molality, i = van't Hoff factor
Key Concepts
Colligative Property
Depends only on the number of particles, not their chemical nature. More particles = greater elevation.
Van't Hoff Factor
Accounts for dissociation. i=1 for non-electrolytes, i> 1 for electrolytes (e.g., NaCl → i=2).
Ebullioscopic Constant
Kb is unique to each solvent. Water: 0.512 °C·kg/mol. Higher Kb = greater elevation per molal.
Common Solvents and Kb Values
| Solvent | Formula | Kb (°C·kg/mol) | Normal BP (°C) |
|---|---|---|---|
| Water | H_{2}O | 0.512 | 100 |
| Ethanol | C_{2}H₅ ext{OH} | 1.22 | 78.37 |
| Benzene | C₆H₆ | 2.53 | 80.1 |
| Chloroform | CHCl_{3} | 3.63 | 61.2 |
| Carbon tetrachloride | ext{CCl}₄ | 5.03 | 76.7 |
| Acetic acid | CH_{3} ext{COOH} | 3.07 | 118.1 |
| Diethyl ether | (C_{2}H₅)_{2}O | 2.02 | 34.6 |
| Camphor | C_{1}_{0}H_{1}₆O | 5.95 | 204 |
| Phenol | C₆H₅ ext{OH} | 3.56 | 181.7 |
| Naphthalene | C_{1}_{0}H₈ | 5.65 | 218 |
Common Solutes and Van't Hoff Factors
| Solute | Formula | i (van't Hoff) | Type |
|---|---|---|---|
| Sodium chloride | ext{NaCl} | 2 | Strong electrolyte |
| Calcium chloride | CaCl_{2} | 3 | Strong electrolyte |
| Sucrose | C_{1}_{2}H_{2}_{2}O_{1}_{1} | 1 | Non-electrolyte |
| Glucose | C₆H_{1}_{2}O₆ | 1 | Non-electrolyte |
| Potassium chloride | ext{KCl} | 2 | Strong electrolyte |
| Magnesium sulfate | ext{MgSO}₄ | 2 | Strong electrolyte |
| Urea | ext{CH}₄N_{2}O | 1 | Non-electrolyte |
| Ethylene glycol | C_{2}H₆O_{2} | 1 | Non-electrolyte |
📚 Official Data Sources
⚠️ Disclaimer: This calculator provides estimates for educational and research use. Ebullioscopic constants and van't Hoff factors vary with concentration. For critical applications verify with primary literature or NIST data.
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