Relation between binding free energy and solubility

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SUMMARY

The discussion centers on the relationship between binding free energy and solubility in the context of ligand-receptor interactions in a solvent medium. Key equations presented include the Gibbs free energy equation, ΔG = ΔH - TΔS, and the equilibrium constant K, defined as K = exp(ΔG/RT). The conversation emphasizes that binding free energy (ΔG) is directly related to solubility, highlighting the importance of both enthalpy (ΔH) and entropy (ΔS) in this relationship.

PREREQUISITES
  • Understanding of Gibbs free energy and its components (ΔG, ΔH, ΔS)
  • Familiarity with equilibrium constants and their calculations
  • Knowledge of ligand-receptor interactions in pharmacology
  • Basic principles of thermodynamics as applied to chemical systems
NEXT STEPS
  • Study the implications of ΔG in pharmacokinetics and drug design
  • Explore advanced topics in thermodynamics related to solubility
  • Learn about computational methods for predicting binding free energy
  • Investigate the role of entropy in molecular interactions and solubility
USEFUL FOR

Researchers in pharmacoinformatics, chemists studying ligand-receptor dynamics, and professionals involved in drug formulation and solubility optimization will benefit from this discussion.

Chirag740
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Suppose we have a ligand binding to a receptor in solvent medium. I am interested to know whether there is any relation between "Binding free energy" and "Solubility".

Extemely sorry if I posted my question in the wrong section. I'd be glad if anyone could help me out with this.

Regards,
Chirag V. Vora
Department of Pharmacoinformatics,
Block - A, Bioinformatics Infrastructure Facility,
National Institute of Pharmaceutical Education and Research (NIPER)
Sector 67, S.A.S. Nagar,
Punjab (INDIA) - 160 062
 
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That's not only a question of energetics but even more of entropy.
The equilibrium constant for dissociation can be calculated from
\Delta G=\Delta H -T \Delta S \approx \Delta U -T \Delta S
where \Delta U is the dissociation energy per mole and in solution is practically equal to the enthalpy change,
and \Delta S the entropic change due to dissociation.
The equilibrium constant K is
K=\exp(\Delta G/RT)

Edit: Excuse me, I overread "free" in your post.
\Delta G is the free energy of binding, so the relation is quite direct.
 

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