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Ebullioscopic Constant given Elevation in Boiling Point Calculator

Formula Used:

\[ k_b = \frac{\Delta T_b}{i \times m} \]

K
mol/kg

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1. What is Ebullioscopic Constant?

Definition: The ebullioscopic constant (kb) relates molality to boiling point elevation when a solute is added to a solvent.

Purpose: It helps determine how much the boiling point of a solvent will increase when a non-volatile solute is dissolved in it.

2. How Does the Calculator Work?

The calculator uses the formula:

\[ k_b = \frac{\Delta T_b}{i \times m} \]

Where:

Explanation: The boiling point elevation is divided by the product of Van't Hoff factor and molality to determine the solvent's ebullioscopic constant.

3. Importance of Ebullioscopic Constant

Details: This constant is crucial for understanding colligative properties and is specific to each solvent. It helps predict boiling point changes in solutions.

4. Using the Calculator

Tips: Enter the boiling point elevation (ΔTb) in Kelvin, Van't Hoff factor (default 1.0 for non-electrolytes), and molality in mol/kg. All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is the Van't Hoff factor?
A: It accounts for the number of particles a solute dissociates into (e.g., 1 for sugar, ~2 for NaCl, 3 for CaCl2).

Q2: What are typical values for kb?
A: Common values are 0.512 K·kg/mol for water, 2.53 for benzene, and 3.63 for acetic acid.

Q3: How is boiling point elevation measured?
A: It's the difference between the solution's boiling point and the pure solvent's boiling point.

Q4: Does this work for all solvents?
A: Yes, but each solvent has its own characteristic kb value.

Q5: What's the difference between kb and kf?
A: kb is for boiling point elevation, while kf (cryoscopic constant) is for freezing point depression.

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