Boiling Point Solution Calculator

Boiling Point Elevation Equation:

\[ T_b = T_0 + i K_b m \]

Solvent Boiling Point (T₀):

°C

Van't Hoff Factor (i):

Boiling Point Constant (K_b):

°C kg/mol

Molality (m):

mol/kg

Boiling Point (T_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.

2. How Does the Calculator Work?

The calculator uses the boiling point elevation equation:

\[ T_b = T_0 + i K_b m \]

Where:

\( T_b \) — Boiling point of the solution (°C)
\( T_0 \) — Boiling point of the pure solvent (°C)
\( i \) — Van't Hoff factor (dimensionless)
\( K_b \) — Boiling point elevation constant (°C kg/mol)
\( m \) — Molality of the solution (mol/kg)

Explanation: The equation shows how each solute particle contributes to raising the boiling point of the solvent proportionally to its concentration.

3. Importance of Boiling Point Calculation

Details: Calculating boiling point elevation is crucial in various chemical processes, pharmaceutical formulations, food processing, and determining molecular weights of unknown compounds through ebullioscopy.

4. Using the Calculator

Tips: Enter the pure solvent boiling point, van't Hoff factor, boiling point constant, and molality. All values must be valid (non-negative numbers).

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 compound dissociates into in solution. For non-electrolytes, i = 1; for strong electrolytes, i equals the number of ions produced.

Q2: How do I find K_b values?
A: K_b is a solvent-specific constant. Common values: water (0.512 °C kg/mol), benzene (2.53 °C kg/mol), ethanol (1.22 °C kg/mol).

Q3: Why use molality instead of molarity?
A: Molality (moles per kg solvent) is temperature-independent, making it more suitable for boiling point and freezing point calculations.

Q4: Does this work for all solutions?
A: The equation works best for dilute solutions. For concentrated solutions, deviations may occur due to non-ideal behavior.

Q5: Can I use this for mixed solvents?
A: The standard equation is designed for single solvents. Mixed solvents require more complex calculations and are not covered by this simple formula.