1. What is Boiling Point Elevation?

Boiling point elevation is a colligative property where the boiling point of a solvent increases when a non-volatile solute is added. The extent of 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:

• \( \Delta T_b \) — Boiling point elevation (°C)
• \( i \) — van't Hoff factor (3 for Na₂SO₄)
• \( K_b \) — Boiling point elevation constant (°C kg/mol)
• \( M \) — Molar mass of solute (142 g/mol for Na₂SO₄)
• \( W \) — Mass of solvent (kg)

Explanation: The formula calculates how much the boiling point increases when 2g of Na₂SO₄ is dissolved in a given mass of solvent.

3. Importance of Boiling Point Elevation

Details: Understanding boiling point elevation is crucial in various applications including chemical engineering, food processing, and pharmaceutical manufacturing where precise temperature control is essential.

4. Using the Calculator

Tips: Enter the boiling point elevation constant (K_b) in °C kg/mol and the solvent mass in kilograms. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: Why is the van't Hoff factor 3 for Na₂SO₄?
A: Na₂SO₄ dissociates into 3 ions in solution (2 Na⁺ and 1 SO₄²⁻), making the van't Hoff factor 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 acetic acid, and 3.63 °C kg/mol for benzene.

Q3: Does this work for all solvents?
A: Yes, but you need to use the appropriate K_b value for the specific solvent being used.

Q4: Why is the solute mass fixed at 2g?
A: This calculator is specifically designed for calculations with 2g of Na₂SO₄ as specified in the problem.

Q5: Can this be used for other solutes?
A: This calculator is specifically designed for Na₂SO₄. For other solutes, you would need to adjust the van't Hoff factor and molar mass values.