1. What is Boiling Point Elevation?

Boiling point elevation is a colligative property that describes how the boiling point of a solvent increases when a non-volatile solute is added. The extent of boiling point elevation depends on the number of solute particles in the solution.

2. How Does the Calculator Work?

The calculator uses the boiling point elevation formula:

Where:

• \( T_{\text{solution}} \) — Boiling point of the solution (°C)
• \( T_{\text{solvent}} \) — Boiling point of the pure solvent (°C)
• \( \Delta T_b \) — Boiling point elevation (°C)

Explanation: The boiling point elevation is directly proportional to the molality of the solute particles in the solution.

3. Importance of Boiling Point Calculation

Details: Understanding boiling point elevation is crucial for various applications including cooking, antifreeze formulations, and chemical process design where precise temperature control is needed.

4. Using the Calculator

Tips: Enter the boiling point of the pure solvent and the calculated boiling point elevation. Both values should be in degrees Celsius.

5. Frequently Asked Questions (FAQ)

Q1: What factors affect boiling point elevation?
A: The main factors are the nature of the solvent and the concentration of solute particles (molality).

Q2: How is ΔT_b calculated?
A: ΔT_b = K_b × m × i, where K_b is the ebullioscopic constant, m is molality, and i is the van't Hoff factor.

Q3: Why does boiling point elevation occur?
A: Solute particles lower the vapor pressure of the solvent, requiring more energy (higher temperature) for boiling to occur.

Q4: Does the type of solute matter?
A: For ideal solutions, only the number of particles matters (colligative property). For non-ideal solutions, solute-solvent interactions become important.

Q5: What are common applications?
A: Used in antifreeze formulations, cooking (adding salt to water), and determining molecular weights of solutes.