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 elevation depends on the concentration of solute particles in the solution.

2. How Does the Calculator Work?

The calculator uses the boiling point elevation formula:

Where:

• \( \Delta T_b \) — Boiling point elevation (°C)
• \( K_b \) — Ebullioscopic constant (°C kg/mol)
• \( W \) — Mass of solvent (kg)
• 3 — Van't Hoff factor for CaCl₂
• 10 — Mass of CaCl₂ added (g)
• 111 — Molar mass of CaCl₂ (g/mol)

Explanation: The formula calculates the boiling point elevation when 10g of CaCl₂ (which dissociates into 3 ions) is added to a solvent of mass W.

3. Importance of Boiling Point Elevation

Details: Understanding boiling point elevation is crucial in various applications including cooking, industrial processes, and chemical engineering where precise temperature control is required.

4. Using the Calculator

Tips: Enter the ebullioscopic constant (K_b) for your solvent in °C kg/mol and the mass of solvent (W) in kilograms. Both values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: Why is the van't Hoff factor 3 for CaCl₂?
A: CaCl₂ dissociates into three ions in solution: one Ca²⁺ ion and two Cl⁻ ions, giving it a van't Hoff factor of 3.

Q2: What are typical values for K_b?
A: Common values are 0.512 °C kg/mol for water, 2.53 °C kg/mol for benzene, and 3.63 °C kg/mol for acetic acid.

Q3: Does this work for any solute?
A: This specific calculator is designed for 10g of CaCl₂. For other solutes, the formula would need to be adjusted.

Q4: Why is the solvent mass in kg?
A: The ebullioscopic constant is defined in °C kg/mol, so using kg for solvent mass maintains consistent units.

Q5: Can I use this for freezing point depression?
A: No, freezing point depression uses a different constant (K_f) and follows a similar but distinct formula.