Dissociation of strong acids in aqueous solutions

Abstract

The dissociation of strong acids has been considered as the interaction between the acids (HA) and water (W). The equilibrium constant (K) expression of that interaction, rearranged in the form log (a_±²/a_w²)= y = log K+ log a_HA/a_w, has been used to determine K. Plotting of experimental data as y= f(a_w) leads to the appearance of an inflexion point where the quotient a_HA/a_w can be substituted by the ratio of total concentrations of acid and water at the inflexion point. The values for the dissociation constants of H₂SO₄, HBr, HI, HClO₄, HCl, and HNO₃ are 34.96 (first dissociation constant) 23.63, 15.28, 12.30, 8.39, and 2.82 respectively.