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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2:56 minutes

Problem 42

Textbook Question

What is the difference between a monoprotic acid and a diprotic acid? Give an example of each.

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A monoprotic acid is an acid that can donate only one proton (H⁺) per molecule during a chemical reaction. For example, hydrochloric acid (HCl) is a monoprotic acid because it donates one H⁺ ion when dissolved in water.

A diprotic acid is an acid that can donate two protons (H⁺) per molecule during a chemical reaction, typically in two separate steps. For example, sulfuric acid (H₂SO₄) is a diprotic acid because it can donate two H⁺ ions sequentially.

To understand this concept, consider the dissociation of HCl in water: HCl → H⁺ + Cl⁻. This shows that HCl donates one proton, making it monoprotic.

For a diprotic acid like H₂SO₄, the dissociation occurs in two steps: (1) H₂SO₄ → H⁺ + HSO₄⁻, and (2) HSO₄⁻ → H⁺ + SO₄²⁻. This demonstrates the donation of two protons, one in each step.

In summary, the key difference is the number of protons the acid can donate: one for monoprotic acids and two for diprotic acids. Examples include HCl (monoprotic) and H₂SO₄ (diprotic).

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Key Concepts

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

Monoprotic Acid

A monoprotic acid is an acid that can donate only one proton (H⁺ ion) per molecule during the process of dissociation in an aqueous solution. This characteristic means that it has a single acidic hydrogen atom. A common example of a monoprotic acid is hydrochloric acid (HCl), which dissociates in water to release one proton.

Diprotic Acid

A diprotic acid is an acid that can donate two protons (H⁺ ions) per molecule when it dissociates in solution. This means it has two acidic hydrogen atoms, allowing it to undergo two separate ionization steps. Sulfuric acid (H₂SO₄) is a well-known example of a diprotic acid, as it can release two protons in two stages of dissociation.

Acid Dissociation

Acid dissociation refers to the process by which an acid releases protons into a solution, resulting in the formation of hydronium ions (H₃O⁺). The strength of an acid is often measured by its dissociation constant (Ka), which indicates how completely the acid ionizes in water. Understanding this concept is crucial for distinguishing between monoprotic and diprotic acids, as it highlights their differing capacities to donate protons.

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