Final answer:
The pH at which you would find an equal amount of acetic acid and its conjugate base is equal to the pKa value of acetic acid, which is 4.76.
Step-by-step explanation:
The pH at which you would find an equal amount of acetic acid and its conjugate base can be determined using the Henderson-Hasselbalch equation and the pKa value of the acid. The Henderson-Hasselbalch equation is given by:
pH = pKa + log([A-]/[HA])
Since we want the concentrations of the acid and its conjugate base to be equal, [A-] = [HA]. Therefore, the Henderson-Hasselbalch equation simplifies to:
pH = pKa + log(1)
And since the logarithm of 1 is 0, the pH at which you would find an equal amount of acetic acid and its conjugate base is equal to the pKa value of acetic acid, which is 4.76.