Calculate The Boiling Point Of A Solution Containing 0.150 M Mgf2

Boiling Point Elevation Formula:

\[ T_b = T_0 + i \times K_b \times m \]

Pure Solvent Boiling Point (T₀):

°C

Boiling Point Constant (K_b):

°C·kg/mol

Molality (m):

mol/kg

Van't Hoff Factor (i):

(unitless)

Boiling Point Elevation (ΔT_b):

Solution Boiling Point (T_b):

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1. What is Boiling Point Elevation?

Boiling point elevation is a colligative property that occurs when a non-volatile solute is added to a solvent, raising its boiling point. 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:

\[ T_b = T_0 + i \times K_b \times m \]

Where:

\( T_b \) — Boiling point of the solution (°C)
\( T_0 \) — Boiling point of the pure solvent (°C)
\( i \) — Van't Hoff factor (number of particles per formula unit)
\( K_b \) — Ebullioscopic constant (°C·kg/mol)
\( m \) — Molality of the solution (mol/kg)

For MgF₂: The van't Hoff factor (i) is 3 because MgF₂ dissociates into three ions: Mg²⁺ and 2F⁻.

3. Importance of Boiling Point Calculation

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

4. Using the Calculator

Tips: Enter the pure solvent boiling point (100°C for water), the ebullioscopic constant (0.512°C·kg/mol for water), molality of the solution, and van't Hoff factor (3 for MgF₂).

5. Frequently Asked Questions (FAQ)

Q1: Why is the van't Hoff factor 3 for MgF₂?
A: MgF₂ dissociates completely in water to form three ions: one Mg²⁺ cation and two F⁻ anions.

Q2: What is the ebullioscopic constant?
A: The ebullioscopic constant (K_b) is a property of the solvent that indicates how much the boiling point will elevate per molal concentration of solute.

Q3: Does boiling point elevation depend on the type of solute?
A: Only indirectly through the van't Hoff factor. The elevation depends on the number of particles, not their chemical nature.

Q4: Why use molality instead of molarity?
A: Molality (moles per kg of solvent) is temperature-independent, making it more suitable for calculations involving temperature changes like boiling point elevation.

Q5: Is this calculation accurate for concentrated solutions?
A: The formula works best for dilute solutions. For concentrated solutions, deviations may occur due to ion pairing and other non-ideal behaviors.