Boiling Water Elevation Calculator

Boiling Point Elevation Formula:

\[ \Delta T_b = i K_b m \]

Van't Hoff Factor (i):

dimensionless

Boiling Point Constant (K_b):

°C kg/mol

Molality (m):

mol/kg

Boiling Point Elevation (ΔT_b):

Unit Converter ▲

Unit Converter ▼

From:	To:

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:

\[ \Delta T_b = i K_b m \]

Where:

\( \Delta T_b \) — Boiling point elevation (°C)
\( i \) — Van't Hoff factor (dimensionless)
\( K_b \) — Ebullioscopic constant (°C kg/mol)
\( m \) — Molality (mol/kg)

Explanation: The van't Hoff factor accounts for the number of particles a compound dissociates into in solution. For non-electrolytes, i = 1; for electrolytes, i equals the number of ions produced per formula unit.

3. Importance of Boiling Point Elevation Calculation

Details: Understanding boiling point elevation is crucial in various applications including cooking, industrial processes, pharmaceutical formulations, and determining molecular weights of unknown compounds through ebullioscopy.

4. Using the Calculator

Tips: Enter the van't Hoff factor (i), boiling point constant (K_b), and molality (m). All values must be positive numbers. Common K_b values: water = 0.512 °C kg/mol, benzene = 2.53 °C kg/mol, acetic acid = 3.07 °C kg/mol.

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 solute dissociates into in solution. For example, NaCl has i = 2, while glucose has i = 1.

Q2: How is molality different from molarity?
A: Molality (m) is moles of solute per kilogram of solvent, while molarity is moles of solute per liter of solution. Molality is temperature-independent, making it preferred for colligative property calculations.

Q3: Why does boiling point elevation occur?
A: Adding solute particles to a solvent reduces the vapor pressure, which requires a higher temperature to reach atmospheric pressure (the boiling point).

Q4: What are typical K_b values for common solvents?
A: Water: 0.512 °C kg/mol, Ethanol: 1.22 °C kg/mol, Benzene: 2.53 °C kg/mol, Acetic acid: 3.07 °C kg/mol.

Q5: Can this calculator be used for any solvent?
A: Yes, as long as you use the appropriate K_b value for your specific solvent and ensure all units are consistent.