1. What is Boiling Point Elevation?

Boiling point elevation is a colligative property that describes how the boiling point of a liquid increases when another compound is added, meaning the solution has a higher boiling point than the pure solvent.

2. How Does the Calculator Work?

The calculator uses the boiling point elevation equation:

Where:

• \( T_b \) — Boiling point of solution (°C)
• \( T_0 \) — Boiling point of pure solvent (°C)
• \( i \) — Van't Hoff factor (dimensionless)
• \( K_b \) — Boiling point elevation constant (°C·kg/mol)
• \( m \) — Molality (mol/kg)

Explanation: The equation calculates how much the boiling point increases based on the number of particles in solution and the concentration.

3. Importance of Boiling Point Calculation

Details: Calculating boiling point elevation is important in various chemical processes, food preparation, and industrial applications where precise temperature control is required.

4. Using the Calculator

Tips: Enter the pure solvent boiling point, van't Hoff factor, boiling point constant, and molality. All values must be valid (K_b > 0, m ≥ 0).

5. Frequently Asked Questions (FAQ)

Q1: What is the van't Hoff factor?
A: The van't Hoff factor (i) represents the number of particles a compound dissociates into in solution. For non-electrolytes, i = 1.

Q2: What are typical K_b values?
A: Common values: water (0.512 °C·kg/mol), benzene (2.53 °C·kg/mol), ethanol (1.22 °C·kg/mol).

Q3: Why use molality instead of molarity?
A: Molality is temperature-independent since it's based on mass, not volume, making it more suitable for boiling point calculations.

Q4: Does this work for all solutions?
A: The equation works best for dilute solutions. For concentrated solutions, deviations may occur due to non-ideal behavior.

Q5: Can I use this for freezing point depression too?
A: Freezing point depression uses a similar equation but with the freezing point depression constant (K_f) instead of K_b.