On a standard titration curve for a weak acid neutralized by a strong base, what mathematical identi — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

At half-neutralization, exactly half the weak acid has converted to its conjugate salt, so $[Salt] = [Acid]$. By the Henderson-Hasselbalch equation, $pH = pK_a + \log(1) \implies pH = pK_a$.