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

6. Chemical Quantities & Aqueous Reactions

Solubility Rules

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Solubility Rules

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Multiple Choice

Which of the following will increase the solubility of CO_2(g) in water?

Adding NaCl to the water

Decreasing the temperature of the water

Decreasing the pressure of CO_2 above the water

Increasing the temperature of the water

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Verified step by step guidance

Understand that the solubility of gases in liquids is generally governed by Henry's Law, which states that the solubility of a gas is directly proportional to the partial pressure of that gas above the liquid: $S = k_H \times P$, where $S$ is solubility, $k_H$ is Henry's law constant, and $P$ is the partial pressure.

Recognize that temperature affects gas solubility because gas solubility typically decreases as temperature increases. This is due to the exothermic nature of gas dissolution; higher temperatures provide energy for gas molecules to escape from the liquid.

Consider the effect of adding NaCl (salt) to water, which usually decreases the solubility of gases due to the 'salting out' effect, where dissolved salts reduce the amount of gas that can dissolve.

Analyze the effect of pressure changes: decreasing the pressure of CO$_2$ above the water will reduce its solubility according to Henry's Law, while increasing pressure would increase solubility.

Conclude that decreasing the temperature of the water increases the solubility of CO$_2$ because lower temperatures favor gas dissolution, making this the correct choice among the options.