SUMMARY
The forum discussion centers on the calculation of pH during the titration of ethanoic acid (acetic acid) with sodium hydroxide (NaOH). The user initially calculated a pH of 3.03 using the dissociation constant (Ka) of acetic acid, but this was incorrect due to misinterpretation of the equilibrium conditions. The correct pH at the half-titration point, where [CH3COOH] equals [CH3COO-], is 4.74, as derived using the Henderson-Hasselbalch equation. The discussion emphasizes the importance of recognizing acetate presence and correctly applying equilibrium constants in titration calculations.
PREREQUISITES
- Understanding of acid-base titration principles
- Familiarity with the Henderson-Hasselbalch equation
- Knowledge of equilibrium constants and their applications
- Basic skills in logarithmic calculations
NEXT STEPS
- Study the Henderson-Hasselbalch equation in detail
- Learn about equilibrium constants for weak acids
- Practice titration calculations involving weak acids and their conjugate bases
- Explore the concept of half-titration points in acid-base chemistry
USEFUL FOR
Chemistry students, educators, and anyone involved in laboratory titration experiments, particularly those focusing on acid-base equilibria and pH calculations.