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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

Which of the following equations correctly shows NO₂⁻ acting as a Bronsted-Lowry base?

NO₂⁻ + H₂O → NO₂⁻ + H₂O

NO₂⁻ + H₂O → HNO₂ + OH⁻

NO₂⁻ + H₂O → NO₂ + H₃O⁺

NO₂⁻ + H₂O → NO₂⁺ + H₂O

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Verified step by step guidance

Identify the role of a Bronsted-Lowry base: A Bronsted-Lowry base is a substance that can accept a proton (H⁺) from another substance.

Examine the given options to determine which reaction involves NO₂⁻ accepting a proton from water (H₂O).

In the correct reaction, NO₂⁻ should accept a proton from H₂O, forming HNO₂ and leaving behind OH⁻. This indicates that NO₂⁻ is acting as a base by accepting a proton.

Analyze the chemical equation: NO₂⁻ + H₂O → HNO₂ + OH⁻. Here, NO₂⁻ accepts a proton from H₂O, forming HNO₂, and OH⁻ is produced as a result.

Verify that the other options do not show NO₂⁻ acting as a Bronsted-Lowry base. In those reactions, NO₂⁻ does not accept a proton, which is inconsistent with the definition of a Bronsted-Lowry base.