1. Matter and Measurements4h 29m
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 35m
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. Amines38m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 46m
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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2:59 minutes

Problem 39McMurry - 8th Edition

Textbook Question

What happens when a weak acid such as CH₃CO₂H is dissolved in water?

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Identify the weak acid: In this case, the weak acid is acetic acid, CH₃CO₂H.

Understand the dissociation process: When a weak acid like CH₃CO₂H is dissolved in water, it partially dissociates into its ions.

Write the chemical equation for the dissociation: CH₃CO₂H (aq) ⇌ CH₃CO₂⁻ (aq) + H⁺ (aq).

Recognize the equilibrium nature: Since CH₃CO₂H is a weak acid, the dissociation is not complete and an equilibrium is established between the undissociated acid and the ions.

Consider the role of water: Water acts as a solvent and also participates in the equilibrium by accepting the H⁺ ions, forming H₃O⁺ (hydronium ions), which can be represented as CH₃CO₂H (aq) + H₂O (l) ⇌ CH₃CO₂⁻ (aq) + H₃O⁺ (aq).

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Key Concepts

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

Weak Acids

Weak acids, like acetic acid (CH₃CO₂H), do not fully dissociate in water. Instead, they establish an equilibrium between the undissociated acid and its ions. This partial ionization is crucial for understanding their behavior in solution, as it affects pH and the acid's reactivity.

Dissociation Equilibrium

When a weak acid dissolves in water, it reaches a state of dissociation equilibrium, represented by the equation CH₃CO₂H ⇌ CH₃CO₂⁻ + H⁺. This means that some molecules remain intact while others break apart into ions, influencing the concentration of hydrogen ions and thus the solution's acidity.

pH and Acidity

The pH scale measures the acidity of a solution, with lower values indicating higher acidity. When a weak acid like CH₃CO₂H is dissolved in water, it contributes hydrogen ions (H⁺) to the solution, lowering the pH. Understanding this relationship is essential for predicting the behavior of weak acids in various chemical contexts.