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, not their identity.

2. How Does the Calculator Work?

The calculator uses the boiling point elevation formula:

Where:

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

Explanation: The formula calculates how much the boiling point increases when 3g of CaCl₂ is dissolved in a given amount of solvent.

3. Importance of Boiling Point Elevation

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

4. Using the Calculator

Tips: Enter the boiling point elevation constant (K_b) for your solvent and the mass of solvent in kilograms. Common K_b values: 0.512 °C·kg/mol for water, 2.53 °C·kg/mol for acetic acid, 3.63 °C·kg/mol for benzene.

5. Frequently Asked Questions (FAQ)

Q1: Why is the van't Hoff factor 3 for CaCl₂?
A: CaCl₂ dissociates into three ions in solution (Ca²⁺ and 2Cl⁻), so i = 3.

Q2: What is the molar mass of CaCl₂?
A: The molar mass of CaCl₂ is 111 g/mol (40 g/mol for Ca + 71 g/mol for Cl₂).

Q3: Does this work for any solvent?
A: Yes, but you need to know the specific K_b value for your solvent.

Q4: Why is boiling point elevation important?
A: It's used in various applications including determining molecular weights, cooking, and industrial processes where temperature control is critical.

Q5: Can I use this for other solutes?
A: This specific calculator is designed for 3g of CaCl₂. For other solutes, you would need to adjust the mass and van't Hoff factor.