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:

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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).

a better way would be to describe dissociation in gas phase then the solvation of each: enter image description here

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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"?


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