The Henderson-Hasselbalch equation relates the pH of a solution of a weak acid to its acid dissociation constant ([latex]pK_a[/latex]) and the ratio of the concentrations of the deprotonated species (conjugate base, [latex][A^-][/latex]) to the protonated species (acid, [latex][HA][/latex]). The equation is [latex]pH = pK_a + \log_{10}\left(\frac{[A^-]}{[HA]}}\right)[/latex]. It is fundamental for understanding and preparing buffer solutions.

















