Related Experiment Video
Updated: May 27, 2026

Sedimentation Equilibrium of a Small Oligomer-forming Membrane Protein: Effect of Histidine Protonation on Pentameric Stability
Published on: April 2, 2015
Histidine in continuum electrostatics protonation state calculations
Vernon Couch1, Alexei Stuchebrukhov
1Department of Chemistry, University of California, Davis, California 95616, USA.
This study presents a modified continuum electrostatics method to accurately calculate protein pKa values. The new approach effectively separates histidine tautomers, improving predictions for protonation states.
Area of Science:
- Biophysical Chemistry
- Computational Biology
- Protein Biochemistry
Background:
- Calculating protein pKa values is crucial for understanding protein function.
- Standard continuum electrostatics methods struggle with histidine's complex protonation states.
- Histidine's imidazole ring has coupled protonatable sites, complicating electrostatic calculations.
Purpose of the Study:
- To develop a modified continuum electrostatics approach for accurate protein pKa calculations.
- To enable the decoupling of histidine tautomers within a two-state model.
- To incorporate all histidine protonation states into electrostatic calculations.
Main Methods:
- Modification of the standard continuum electrostatics approach.
- Introduction of a two-state model for histidine tautomers.
- Application of a single approximation for interrelations between histidine charge states.
Main Results:
- Successfully decoupled histidine tautomers within the two-state model.
- Enabled natural separation of the two protonatable sites of the imidazole ring.
- Allowed inclusion of all histidine protonation states in the calculation.
Conclusions:
- The modified method provides a more accurate way to calculate protein pKa values.
- This approach overcomes limitations of standard methods in handling histidine residues.
- The findings facilitate better computational modeling of protein behavior and function.
More Related Videos
Related Concept Videos
Polyprotic Acids
Strong Acid and Base Solutions
Henderson-Hasselbalch Equation
Titration of a Weak Base with a Strong Acid
Using the ICE table and substituting the Kb value, we calculate the initial pH of 50 mL of 0.1 M ammonia to be 11.11. Addition of 25 mL of 0.1 M hydrochloric acid to this solution of ammonia results in a buffer with an equal concentration of ammonia and ammonium ions. The pH of this buffer can be calculated by substituting these...
Weak Acid Solutions
Relative Strengths of Conjugate Acid-Base Pairs

