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

Acid-Base Introduction

GOB Chemistry

10. Acids and Bases

Acid-Base Introduction

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2: minutes

Problem 9b

Textbook Question

Write the formula for the conjugate base for each of the following acids:
b. H₂O

Verified step by step guidance

Identify the definition of a conjugate base: A conjugate base is formed when an acid donates a proton (H⁺). This means the acid loses one hydrogen ion, resulting in a species with one less hydrogen and a charge that is more negative by 1.

Start with the given acid, H₂O (water). Recognize that H₂O can act as an acid by donating one proton (H⁺).

Remove one hydrogen ion (H⁺) from H₂O. This leaves behind the hydroxide ion, OH⁻.

Determine the charge of the resulting species: Since a neutral H₂O molecule loses a positively charged H⁺ ion, the resulting species, OH⁻, will have a negative charge.

Write the formula for the conjugate base of H₂O: The conjugate base is OH⁻.

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Key Concepts

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

Conjugate Base

A conjugate base is the species that remains after an acid donates a proton (H⁺) during a chemical reaction. It is formed when an acid loses a hydrogen ion, and it can potentially accept a proton in a subsequent reaction. Understanding conjugate bases is essential for grasping acid-base chemistry and the concept of equilibrium in reactions.

Acid-Base Theory

Acid-base theory encompasses various models that define acids and bases, including the Brønsted-Lowry theory, which defines acids as proton donors and bases as proton acceptors. This theory is fundamental for predicting the behavior of substances in chemical reactions, particularly in aqueous solutions where water often acts as both an acid and a base.

Water as an Acid and Base

Water (H₂O) can act as both an acid and a base, making it amphoteric. When it donates a proton, it forms the hydroxide ion (OH⁻), which is its conjugate base. This dual behavior is crucial in many chemical reactions and helps explain the role of water in acid-base equilibria and the pH scale.