Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

14. Solutions

Boiling Point Elevation

General Chemistry

14. Solutions

Boiling Point Elevation

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Multiple Choice

Pure water boils at 100°C. What is the new boiling point of water after the addition of 13.12 g aluminum chloride, AlCl₃, to 615 g water?

100.25°C

100.08°C

100.33°C

100.16°C

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Verified step by step guidance

First, understand that the boiling point elevation is a colligative property, which means it depends on the number of solute particles in a solution, not their identity. The formula for boiling point elevation is ΔT_b = i * K_b * m, where ΔT_b is the change in boiling point, i is the van't Hoff factor, K_b is the ebullioscopic constant of the solvent, and m is the molality of the solution.

Calculate the molality (m) of the solution. Molality is defined as moles of solute per kilogram of solvent. First, find the moles of AlCl3 using its molar mass. The molar mass of AlCl3 is approximately 133.34 g/mol. Use the formula: moles = mass (g) / molar mass (g/mol).

Determine the van't Hoff factor (i) for AlCl3. When dissolved, AlCl3 dissociates into Al^3+ and 3 Cl^- ions, resulting in i = 4 because one formula unit of AlCl3 produces four ions.

Calculate the molality using the formula: m = moles of solute / mass of solvent (kg). Convert the mass of water from grams to kilograms by dividing by 1000.

Finally, use the boiling point elevation formula: ΔT_b = i * K_b * m. The ebullioscopic constant (K_b) for water is approximately 0.512°C kg/mol. Calculate ΔT_b and add it to the normal boiling point of water (100°C) to find the new boiling point.