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

Freezing Point Depression

General Chemistry

14. Solutions

Freezing Point Depression

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Multiple Choice

Which of the following occurs during the process of freezing in terms of freezing point depression?

The freezing point of the solution is not affected by the presence of solute.

The freezing point of the solution remains the same as the pure solvent.

The freezing point of the solution is raised compared to the pure solvent.

The freezing point of the solution is lowered compared to the pure solvent.

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Verified step by step guidance

Understand the concept of freezing point depression: Freezing point depression is a colligative property, which means it depends on the number of solute particles in a solution, not their identity.

Recognize that when a solute is added to a solvent, the solute particles disrupt the formation of the solid structure of the solvent, requiring a lower temperature to achieve the same solid state.

Identify that the presence of solute particles in a solution lowers the freezing point compared to the pure solvent because the solute particles interfere with the solvent molecules' ability to form a solid lattice.

Recall the formula for freezing point depression: ΔT_f = i * K_f * m, where ΔT_f is the change in freezing point, i is the van't Hoff factor (number of particles the solute breaks into), K_f is the freezing point depression constant of the solvent, and m is the molality of the solution.

Conclude that the correct statement is: 'The freezing point of the solution is lowered compared to the pure solvent,' as the presence of solute particles causes the freezing point to decrease.