Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

17. Acid and Base Equilibrium

pH of Weak Bases

General Chemistry

17. Acid and Base Equilibrium

pH of Weak Bases

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following methods can be used to estimate the pH of a weak base solution if the pKa values are not provided?

Use the Henderson-Hasselbalch equation

Use the Kb value and the initial concentration to calculate pH

Estimate pH using the average of pKa values

Assume complete dissociation and use the pH = 7

Previous problemNext problem

Verified step by step guidance

Identify that the problem involves estimating the pH of a weak base solution without pKa values.

Recognize that the Henderson-Hasselbalch equation requires pKa values, which are not provided, so this method is not applicable.

Understand that assuming complete dissociation and using pH = 7 is incorrect for weak bases, as they do not fully dissociate and typically have a pH greater than 7.

Realize that estimating pH using the average of pKa values is not possible without the pKa values themselves.

Conclude that the correct method is to use the Kb value and the initial concentration of the weak base to calculate the pH. This involves setting up an equilibrium expression using the Kb value and solving for the concentration of OH⁻ ions, then converting this to pH.