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

A solution of a nonvolatile solute in water has a boiling point of 380.5 K. Calculate the vapor pressure of water above this solution at 338 K. The vapor pressure of pure water at this temperature is 0.2467 atm. Which of the following is the vapor pressure of water above the solution?

0.2500 atm

0.2400 atm

0.2600 atm

0.2467 atm

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Verified step by step guidance

Identify the colligative property involved: boiling point elevation, which indicates the presence of a nonvolatile solute.

Understand that the vapor pressure of a solution is lower than that of the pure solvent due to the presence of a nonvolatile solute.

Use Raoult's Law to relate the vapor pressure of the solution to the mole fraction of the solvent: \( P_{solution} = X_{solvent} \times P_{pure} \), where \( P_{solution} \) is the vapor pressure of the solution, \( X_{solvent} \) is the mole fraction of the solvent, and \( P_{pure} \) is the vapor pressure of the pure solvent.

Calculate the mole fraction of the solvent using the boiling point elevation data, if necessary, or assume it is close to 1 for dilute solutions.

Substitute the known values into Raoult's Law to find the vapor pressure of the solution at 338 K: \( P_{solution} = X_{solvent} \times 0.2467 \text{ atm} \).