Calculate Boiling Point Equation

Boiling Point Elevation Equation:

\[ T_b = T_0 + i K_b m \]

Pure Solvent Boiling Point (T₀):

°C

Van't Hoff Factor (i):

Ebullioscopic Constant (K_b):

°C kg/mol

Molality (m):

mol/kg

Boiling Point (T_b):

Unit Converter ▲

Unit Converter ▼

From:	To:

1. What is the Boiling Point Elevation Equation?

The boiling point elevation equation calculates the increase in boiling point of a solvent when a non-volatile solute is added. It's a colligative property that 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 solution (°C)
\( T_0 \) — Boiling point of pure solvent (°C)
\( i \) — Van't Hoff factor (dimensionless)
\( K_b \) — Ebullioscopic constant (°C kg/mol)
\( m \) — Molality of solution (mol/kg)

Explanation: The equation shows how the boiling point increases proportionally with the molality of the solution and the number of particles the solute dissociates into.

3. Importance of Boiling Point Calculation

Details: Boiling point elevation is important in various applications including determining molecular weights of compounds, food processing, and industrial applications where precise temperature control is required.

4. Using the Calculator

Tips: Enter the boiling point of pure solvent in °C, van't Hoff factor (typically 1 for non-electrolytes, 2 for NaCl, etc.), ebullioscopic constant (specific to each solvent), and molality in mol/kg.

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 non-electrolytes, i = 1; for strong electrolytes, i equals the number of ions produced.

Q2: What are typical values for K_b?
A: Common values: Water = 0.512 °C kg/mol, Benzene = 2.53 °C kg/mol, Ethanol = 1.22 °C kg/mol. The constant is specific to each solvent.

Q3: Why use molality instead of molarity?
A: Molality (moles per kg of solvent) is used because it doesn't change with temperature, unlike molarity (moles per liter of solution) which is temperature-dependent.

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 this be used for freezing point depression too?
A: Yes, a similar equation exists for freezing point depression: \( T_f = T_0 - i K_f m \), where K_f is the cryoscopic constant.