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





