calculate tge pH of a buffer system containing 1.0M CH3COOH and 0.1M CH3COONa

To calculate the pH of a buffer system, you need to consider the acid and its conjugate base in the system. The Henderson-Hasselbalch equation is typically used in this case:

pH = pKa + log([A-]/[HA])

Where:
- pH is the desired pH of the buffer system.
- pKa is the acid dissociation constant of the acid in the buffer system.
- [A-] is the concentration of the conjugate base.
- [HA] is the concentration of the acid.

In this case, the acid is CH3COOH (acetic acid) and its conjugate base is CH3COONa (sodium acetate). Acetic acid has a pKa of approximately 4.75.

Given:
- [HA] = 1.0 M (concentration of CH3COOH)
- [A-] = 0.1 M (concentration of CH3COONa)
- pKa = 4.75

Substituting these values into the Henderson-Hasselbalch equation:

pH = 4.75 + log(0.1/1.0)

pH = 4.75 - 0.91

pH = 3.84

Therefore, the pH of the buffer system containing 1.0 M CH3COOH and 0.1 M CH3COONa is approximately 3.84.