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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1:20 minutes

Problem 108b

Textbook Question

Determine each of the following for a 0.100 M HBr solution:
b. pH

Verified step by step guidance

Step 1: Recognize that HBr is a strong acid, meaning it completely dissociates in water. This implies that the concentration of H⁺ ions ([H⁺]) in the solution is equal to the initial concentration of HBr.

Step 2: Write the relationship between the concentration of H⁺ ions and the pH of the solution. The formula is:

pH = - log (H_{+})

Step 3: Substitute the given concentration of HBr (0.100 M) into the formula for [H⁺], since [H⁺] = 0.100 M for a strong acid like HBr.

Step 4: Use the logarithmic function to calculate the pH. Specifically, take the negative logarithm (base 10) of the [H⁺] concentration:

pH = - log (0.100)

Step 5: Interpret the result. The pH value will indicate the acidity of the solution, with lower values corresponding to higher acidity. Since HBr is a strong acid, the pH should be relatively low.

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Key Concepts

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

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, while values below 7 indicate acidity and values above 7 indicate alkalinity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.

Strong Acids

Strong acids, like HBr, completely dissociate in water, releasing all their hydrogen ions (H+). This complete dissociation means that the concentration of the acid directly correlates with the concentration of H+ ions in the solution, making it straightforward to calculate the pH of strong acid solutions.

Calculating pH

To calculate the pH of a solution, the formula pH = -log[H+] is used, where [H+] is the concentration of hydrogen ions. For a 0.100 M HBr solution, since it fully dissociates, the [H+] is also 0.100 M, leading to a pH calculation of -log(0.100), which results in a pH of 1.00.