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

pH of Strong Acids and Bases

GOB Chemistry

10. Acids and Bases

pH of Strong Acids and Bases

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1:08 minutes

Problem 108a

Textbook Question

Determine each of the following for a 0.100 M HBr solution:
a. [H₃O⁺]

Verified step by step guidance

Step 1: Recognize that HBr is a strong acid, meaning it completely dissociates in water. The dissociation reaction can be written as:

HBr → H⁺ + Br⁻

. Since it dissociates completely, the concentration of

[H⁺]

(or equivalently

[H₃O⁺]

) will be equal to the initial concentration of HBr.

Step 2: Identify the given concentration of HBr, which is 0.100 M. This means that for every mole of HBr, 1 mole of

H⁺

ions is produced.

Step 3: Use the relationship between the concentration of HBr and

[H₃O⁺]

. Since HBr dissociates completely,

[H₃O⁺] = [HBr]

. Therefore,

[H₃O⁺]

is equal to 0.100 M.

Step 4: Write the final expression for

[H₃O⁺]

[H₃O⁺] = 0.100 \text{ M}

. This is the hydronium ion concentration in the solution.

Step 5: Verify the logic by recalling that strong acids like HBr fully dissociate, so the concentration of

[H₃O⁺]

directly matches the initial molarity of the acid.

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Key Concepts

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

Strong Acids and Ionization

Strong acids, like HBr, completely dissociate in water, meaning that all the acid molecules break apart into ions. For a 0.100 M HBr solution, this results in a concentration of H⁺ ions equal to the concentration of the acid, which is 0.100 M. This complete ionization is crucial for calculating the hydronium ion concentration.

Hydronium Ion Concentration

The concentration of hydronium ions, [H₃O⁺], in a solution is a measure of the acidity of that solution. In the case of strong acids, the concentration of H₃O⁺ is directly derived from the concentration of the acid. For a 0.100 M HBr solution, the [H₃O⁺] is also 0.100 M, reflecting the complete dissociation of the acid.

pH Scale

The pH scale quantifies the acidity or basicity of a solution, with lower values indicating higher acidity. It is calculated using the formula pH = -log[H₃O⁺]. For a 0.100 M HBr solution, knowing the [H₃O⁺] allows us to calculate the pH, which is an essential aspect of understanding the solution's properties.

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