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

17. Acid and Base Equilibrium

Bronsted-Lowry Acids and Bases

General Chemistry

17. Acid and Base Equilibrium

Bronsted-Lowry Acids and Bases

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Multiple Choice

The equilibrium constant for the reaction below has the value Ka = 3.5 x 10^-4. In this reaction, the stronger Brønsted-Lowry acid is and the weaker Brønsted-Lowry acid is . HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)

H3O+ and F-

F- and H2O

HF and H3O+

H2O and HF

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Verified step by step guidance

Identify the acids and bases in the given chemical equation. In the reaction HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq), HF and H3O+ are the acids, while H2O and F- are the bases.

Understand the concept of Brønsted-Lowry acids and bases. A Brønsted-Lowry acid is a substance that donates a proton (H+), and a Brønsted-Lowry base is a substance that accepts a proton.

Analyze the equilibrium constant (Ka) value. The equilibrium constant provides information about the strength of the acids involved in the reaction. A smaller Ka value indicates a weaker acid, while a larger Ka value indicates a stronger acid.

Compare the acids in the reaction. HF is the acid on the reactant side, and H3O+ is the acid on the product side. Since the equilibrium constant Ka = 3.5 x 10^-4 is relatively small, HF is the stronger acid compared to H3O+.

Conclude which acids are stronger and weaker. Based on the analysis, HF is the stronger Brønsted-Lowry acid, and H3O+ is the weaker Brønsted-Lowry acid in this reaction.