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

Intro to Acid-Base Titration Curves

General Chemistry

18. Aqueous Equilibrium

Intro to Acid-Base Titration Curves

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Multiple Choice

In an acid-base titration, how is the pH at the beginning of the titration determined?

By adding a strong acid to the solution

By measuring the pH of the titrant solution

By calculating the pH of the analyte solution

By using the Henderson-Hasselbalch equation

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Verified step by step guidance

Identify the analyte solution, which is the solution being titrated. This is the solution whose pH you need to determine at the beginning of the titration.

Determine the concentration of the analyte solution. This information is crucial for calculating the pH.

Recognize the nature of the analyte: is it a strong acid, strong base, weak acid, or weak base? This will influence the method used to calculate the pH.

For a strong acid or base, use the concentration directly to calculate the pH or pOH. For a strong acid, pH = -log[H⁺], and for a strong base, pOH = -log[OH⁻], then convert to pH.

For a weak acid or base, use the equilibrium expression and the acid or base dissociation constant (Ka or Kb) to find the concentration of H⁺ or OH⁻ ions, and then calculate the pH using the formula pH = -log[H⁺].