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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1:27 minutes

Problem 72b

Textbook Question

Identify each of the following as an acid or a base:
b. H₂SO₃

Verified step by step guidance

Step 1: Recall the definition of acids and bases. Acids are substances that donate protons (H⁺ ions) in aqueous solutions, while bases are substances that accept protons or produce hydroxide ions (OH⁻) in aqueous solutions.

Step 2: Examine the chemical formula of the given compound, H₂SO₃. This is sulfurous acid, which contains hydrogen atoms that can potentially be donated as H⁺ ions.

Step 3: Recognize that the presence of hydrogen atoms at the beginning of the formula (H₂) is a common indicator of an acid. These hydrogens are ionizable and can dissociate in water to release H⁺ ions.

Step 4: Consider the context of the compound in water. When H₂SO₃ dissolves in water, it dissociates partially to form H⁺ ions and HSO₃⁻ ions, confirming its behavior as an acid.

Step 5: Conclude that H₂SO₃ is an acid because it donates H⁺ ions in aqueous solutions, which aligns with the definition of an acid.

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Key Concepts

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

Acids and Bases

Acids are substances that can donate protons (H⁺ ions) in a solution, while bases are substances that can accept protons. This definition is rooted in the Brønsted-Lowry theory, which emphasizes the transfer of protons in acid-base reactions. Understanding this distinction is crucial for classifying compounds like H₂SO₃.

Sulfurous Acid (H₂SO₃)

H₂SO₃, or sulfurous acid, is a weak acid formed when sulfur dioxide (SO₂) dissolves in water. It can dissociate in solution to release H⁺ ions, which is characteristic of acids. Recognizing H₂SO₃ as an acid is essential for understanding its behavior in chemical reactions and its role in various environmental processes.

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 (strongly acidic) to 14 (strongly basic), with 7 being neutral. A solution with a pH less than 7 indicates the presence of more H⁺ ions, typical of acids like H₂SO₃. Familiarity with the pH scale helps in predicting the properties and reactions of acids and bases.