Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

10. Acids and Bases

Bronsted Lowry Acid and Base

GOB Chemistry

10. Acids and Bases

Bronsted Lowry Acid and Base

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1:38 minutes

Problem 13b

Textbook Question

Identify the Brønsted–Lowry acid–base pairs in each of the following equations:
b. NH₄⁺(aq) + H₂O(l) ⇄ NH₃(aq) + H₃O⁺(aq)

Verified step by step guidance

Step 1: Recall the Brønsted–Lowry definition of acids and bases. A Brønsted–Lowry acid is a substance that donates a proton (H⁺), while a Brønsted–Lowry base is a substance that accepts a proton.

Step 2: Analyze the reactants and products in the equation: NH₄⁺(aq) + H₂O(l) ⇄ NH₃(aq) + H₃O⁺(aq). Identify which species donates a proton and which species accepts a proton.

Step 3: Observe that NH₄⁺ (ammonium ion) donates a proton (H⁺) to H₂O (water), forming NH₃ (ammonia) and H₃O⁺ (hydronium ion). This makes NH₄⁺ the Brønsted–Lowry acid and NH₃ its conjugate base.

Step 4: Recognize that H₂O accepts the proton from NH₄⁺, forming H₃O⁺. This makes H₂O the Brønsted–Lowry base and H₃O⁺ its conjugate acid.

Step 5: Conclude that the Brønsted–Lowry acid–base pairs are: (1) NH₄⁺ (acid) and NH₃ (conjugate base), and (2) H₂O (base) and H₃O⁺ (conjugate acid).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Brønsted–Lowry Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework allows for a broader understanding of acid-base reactions beyond just the presence of hydroxide or hydronium ions. In this theory, the transfer of protons (H⁺ ions) between species is the central focus, making it essential for analyzing chemical equations involving acids and bases.

Acid-Base Pairs

An acid-base pair consists of two species that differ by the presence or absence of a proton. In a Brønsted–Lowry context, the acid in the pair donates a proton, while the base accepts it. Identifying these pairs in a reaction helps to clarify the roles of different species and the direction of proton transfer, which is crucial for understanding the dynamics of the reaction.

Equilibrium in Acid-Base Reactions

Acid-base reactions often reach a state of equilibrium, where the rates of the forward and reverse reactions are equal. This concept is important for understanding how the concentrations of reactants and products change over time. In the given equation, recognizing the equilibrium allows for the identification of the acid-base pairs and the direction of proton transfer, which is vital for predicting the behavior of the system.