SUMMARY
The pH of a 0.15 M sodium acetate solution is determined by its behavior as a weak base, specifically the acetate anion (C2H3O2-), which is the conjugate base of acetic acid. The dissociation constant (Ka) for acetic acid is 1.8 x 10^-5, indicating that the acetate will react with water to produce hydroxide ions (OH-). Therefore, the pH of the solution will be higher than 7.0, contrary to the assumption that it would remain neutral.
PREREQUISITES
- Understanding of weak bases and their conjugate acids
- Knowledge of acid-base equilibrium and dissociation constants
- Familiarity with the concept of pH and its calculation
- Basic chemistry principles regarding aqueous solutions
NEXT STEPS
- Learn about the Henderson-Hasselbalch equation for buffer solutions
- Study the calculation of pH for weak base solutions
- Explore the properties of acetic acid and its conjugate base, acetate
- Investigate the effects of concentration on pH in weak acid-base systems
USEFUL FOR
Chemistry students, educators, and anyone involved in laboratory work or research related to acid-base chemistry and solution pH calculations.