The pH of the buffer solution is 4.74.
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:
The Henderson-Hasselbalch equation is a mathematical expression that relates the pH of a solution containing a weak acid (HA) and its conjugate base (A⁻) to the pKa of the acid.
The equation is commonly used in chemistry and biochemistry to understand and calculate the pH of a buffer solution.
pH = pKa + log([A-]/[HA])
where:
pKa is the dissociation constant of the weak acid
[A-] is the concentration of the conjugate base
[HA] is the concentration of the weak acid
In this case, the weak acid is acetic acid (CH3COOH) and the conjugate base is sodium acetate (CH3COO-).
The pKa of acetic acid is 4.76.
The concentration of sodium acetate is 0.27 mol/L and the concentration of acetic acid is 0.29 mol/L.
Plugging these values into the Henderson-Hasselbalch equation, we get:
pH = 4.76 + log(0.27/0.29)
pH = 4.74
Therefore, the pH of the buffer solution is 4.74.