In a buffer solution of CH3COOH and CH3COONa concentration of both acid and salt are equal. The pH of buffer will be equal to

Explanation

A buffer solution resists changes in pH when small amounts of acid or base are added. Its effectiveness depends on the pKa of the weak acid (CH3COOH) and the concentration ratio of the acid and its conjugate base (CH3COO⁻).In this case, where the concentrations of CH3COOH and CH3COONa are equal, the buffer solution is at its Henderson-Hasselbalch equation minimum pH:pH = pKa + log([A⁻] / [HA])where:[A⁻] is the concentration of the conjugate base (CH3COO⁻)[HA] is the concentration of the weak acid (CH3COOH)Since the concentrations of both are equal:[A⁻] = [HA]Substituting this into the equation:pH = pKa + log(1)Logarithm of 1 is 0, so:pH = pKaTherefore, when the concentrations of the acid and its conjugate base are equal, the pH of the buffer is equal to the pKa of the weak acid.