Resolving coupled pH titrations using alchemical free energy calculations
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Updated: Jul 1, 2025

Titration ELISA as a Method to Determine the Dissociation Constant of Receptor Ligand Interaction
Published on: February 15, 2018
Carter J Wilson1,2,3, Bert L de Groot3, Vytautas Gapsys3,4
1Department of Mathematics, The University of Western Ontario, London, Ontario, Canada.
Abstract:
In a protein, nearby titratable sites can be coupled: the (de)protonation of one may affect the other. The degree of this interaction depends on several factors and can influence the measured . Here, we derive a formalism based on double free energy differences ( ) for quantifying the individual site values of coupled residues. As values can be obtained by means of alchemical free energy calculations, the presented approach allows for a convenient estimation of coupled residue s in practice. We demonstrate that our approach and a previously proposed microscopic formalism, can be combined with alchemical free energy calculations to resolve pH-dependent protein values. Toy models and both, regular and constant-pH molecular dynamics simulations, alongside experimental data, are used to validate this approach. Our results highlight the insights gleaned when coupling and microstate probabilities are analyzed and suggest extensions to more complex enzymatic contexts. Furthermore, we find that naïvely computed values that ignore coupling, can be significantly improved when coupling is accounted for, in some cases reducing the error by half. In short, alchemical free energy methods can resolve the values of both uncoupled and coupled residues.
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Titration Calculations: Weak Acid - Strong Base
For the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH, the reaction can be represented as:
Titration Calculations: Strong Acid - Strong Base
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows:
(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then:

