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

Bronsted Lowry Acid and Base

GOB Chemistry

10. Acids and Bases

Bronsted Lowry Acid and Base

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1:55 minutes

Problem 10c

Textbook Question

Write the formula for the conjugate base for each of the following acids:
c. HPO₄^2-

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, and the charge of the species decreases by 1.

Start with the given acid, HPO₄²⁻. This species has one hydrogen atom that can be donated as a proton (H⁺).

Remove one hydrogen ion (H⁺) from HPO₄²⁻. This results in the chemical formula PO₄³⁻ because the removal of H⁺ decreases the charge by 1.

Verify the result: The conjugate base of HPO₄²⁻ is PO₄³⁻. This makes sense because the acid has donated a proton, leaving behind the phosphate ion with a charge of -3.

Write the final formula for the conjugate base: PO₄³⁻.

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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⁺). In the context of Brønsted-Lowry theory, when an acid loses a proton, it transforms into its conjugate base, which can then potentially accept a proton in future reactions. Understanding this concept is crucial for predicting the behavior of acids and bases in chemical reactions.

Acid-Base Reaction

An acid-base reaction involves the transfer of protons between reactants. In these reactions, acids donate protons while bases accept them. Recognizing the nature of these reactions helps in identifying the conjugate pairs, which is essential for determining the conjugate base of a given acid.

Phosphate Ion

The phosphate ion (PO₄³⁻) is a polyatomic ion that plays a significant role in biochemistry and inorganic chemistry. In the case of HPO₄²⁻, it is a dihydrogen phosphate ion, which can lose a proton to form its conjugate base, PO₄³⁻. Understanding the structure and charge of phosphate ions is important for correctly identifying their conjugate bases.