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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1:20 minutes

Problem 11a

Textbook Question

Write the formula for the conjugate acid for each of the following bases:
a. CO₃^2-

Verified step by step guidance

Identify the base given in the problem. In this case, the base is the carbonate ion, CO₃²⁻.

Recall the definition of a conjugate acid: it is formed when a base accepts a proton (H⁺).

Add one proton (H⁺) to the base, CO₃²⁻. This involves increasing the hydrogen count by 1 and reducing the charge by 1, as the proton carries a positive charge.

Write the resulting formula after adding the proton. The formula becomes HCO₃⁻, which is the conjugate acid of CO₃²⁻.

Verify the result by checking that the conjugate acid has one more hydrogen atom and a charge that is one unit less positive than the original base.

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Key Concepts

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

Conjugate Acid-Base Theory

Conjugate acid-base theory, rooted in the Brønsted-Lowry definition, describes acids as proton donors and bases as proton acceptors. When a base accepts a proton (H⁺), it forms its conjugate acid. Understanding this relationship is crucial for predicting the behavior of chemical species in acid-base reactions.

Carbonate Ion (CO₃²⁻)

The carbonate ion (CO₃²⁻) is a polyatomic ion consisting of one carbon atom covalently bonded to three oxygen atoms, carrying a -2 charge. It acts as a base in chemical reactions, capable of accepting protons to form its conjugate acid. Recognizing its structure and charge is essential for determining its conjugate acid.

Formation of Conjugate Acids

The formation of a conjugate acid involves the addition of a proton to a base. For the carbonate ion (CO₃²⁻), when it accepts a proton, it transforms into bicarbonate (HCO₃⁻), which is its conjugate acid. This process illustrates the dynamic nature of acid-base chemistry and the importance of understanding proton transfer.