Calculate The Boiling Point Of A Solution Containing 0.61

Boiling Point Elevation Equation:

\[ T_b = T_0 + i K_b \left( \frac{0.61 / M}{W} \right) \]

Pure Solvent Boiling Point (T₀):

°C

Van't Hoff Factor (i):

Molal Boiling Point Elevation Constant (K_b):

°C kg/mol

Molar Mass of Solute (M):

g/mol

Mass of Solvent (W):

Boiling Point of Solution (T_b):

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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 concentration of solute particles in the solution.

2. How Does the Calculator Work?

The calculator uses the boiling point elevation equation:

\[ T_b = T_0 + i K_b \left( \frac{0.61 / M}{W} \right) \]

Where:

\( T_b \) — Boiling point of solution (°C)
\( T_0 \) — Pure solvent boiling point (°C)
\( i \) — Van't Hoff factor (dimensionless)
\( K_b \) — Molal boiling point elevation constant (°C kg/mol)
\( M \) — Molar mass of solute (g/mol)
\( W \) — Mass of solvent (kg)

Explanation: The equation calculates how much the boiling point increases when 0.61 g of solute is dissolved in a given mass of solvent, accounting for the number of particles the solute dissociates into.

3. Importance of Boiling Point Calculation

Details: Boiling point elevation calculations are important in various applications including determining molecular weights of unknown compounds, quality control in industrial processes, and understanding colligative properties in physical chemistry.

4. Using the Calculator

Tips: Enter the pure solvent boiling point, van't Hoff factor, molal boiling point elevation constant, molar mass of solute, and mass of solvent. All values must be valid (molar mass > 0, mass of solvent > 0).

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 electrolytes, it depends on the degree of dissociation.

Q2: Why is the mass of solute fixed at 0.61 g?
A: The equation is specifically designed to calculate the boiling point elevation when exactly 0.61 g of solute is dissolved in the solvent.

Q3: What are typical values for K_b?
A: Common values include 0.512 °C kg/mol for water, 2.53 °C kg/mol for benzene, and 3.63 °C kg/mol for carbon disulfide.

Q4: Does this work for all solvents?
A: Yes, but you need to use the appropriate K_b value for the specific solvent being used in the calculation.

Q5: How accurate is this calculation?
A: The calculation provides a theoretical estimate. Actual results may vary slightly due to non-ideal behavior, especially at high concentrations.