How to describe the enthalpy of acid dissociation in aqueous solutions? If we had a weak acid "PB" that dissociates to give a proton and a conjugate base. Classically it would be described like the following:
Unfortunately, things aren't that simple in aqueous solutions. Each of the dissociated molecules will have a charge which will change its polarity and water hydration (solvation).
Is this description accurate? Is the enthalpy of protonation measured by calorimetry or calculated by the Van't Hoff analysis the "dissociation" or the "Ionization"?