Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
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

18. Aqueous Equilibrium

Titrations: Weak Acid-Strong Base

General Chemistry

18. Aqueous Equilibrium

Titrations: Weak Acid-Strong Base

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Multiple Choice

In a titration of a weak acid with a strong base, how is the pH determined before reaching the equivalence point?

The pH is determined by the concentration of water.

The pH is determined by the concentration of the strong base alone.

The pH is determined by the buffer system formed by the weak acid and its conjugate base.

The pH is determined by the concentration of the weak acid alone.

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Verified step by step guidance

Understand that in a titration of a weak acid with a strong base, a buffer system is formed before reaching the equivalence point. This buffer system consists of the weak acid and its conjugate base.

Recognize that the pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:

p_{H} = p_{K} a + log (\frac{[A^-]}{[HA]})

, where

p_{K} a

is the acid dissociation constant,

[A^-]

is the concentration of the conjugate base, and

[HA]

is the concentration of the weak acid.

Calculate the concentrations of the weak acid and its conjugate base. As the strong base is added, it reacts with the weak acid to form its conjugate base. Use stoichiometry to determine the amounts of acid and conjugate base present.

Apply the Henderson-Hasselbalch equation using the calculated concentrations to find the pH of the solution. This equation accounts for the buffer system and provides a way to determine the pH before reaching the equivalence point.

Remember that the pH will gradually increase as more strong base is added, but the buffer system will resist drastic changes in pH until the equivalence point is approached.