In a buffered solution, the concentration of free protons is constant. Any protons that areeither taken up or released during a biochemical process must come from or end up onthe buffer molecules. This applies to biochemical reactions as well as ligand binding.When protons are released upon ligand binding to a protein, the protons can beconsidered to bind to the buffer. If protons are taken up from solution upon ligandbinding, they are taken from protonated buffer molecules. As a result, if binding ismonitored by ITC, the heat measured must also include the heat of ionization of thebuffer if it loses or picks up protons during complex formation. An example of this isdescribed in slides 44 and 45 of lecture 19, which we did not go through in class. Lookthese over before doing the following problem. Also, look at Practice Problem 28.The following ITC data were obtained in studying the binding of the estrogen receptor αto duplex DNA. It was found that the observed heat of the reaction depended on thebuffer in which the experiment was performed. (from Deegan et al, Biochemistry (2010)49, 5978-5988)2a) Phosphate; b) Hepes; c) Tricine; d) Tris buffersThe buffers used have different enthalpies of ionization ( ) o ∆HionPhosphate: 1.22 kcal/molHepes: 5.02 kcal/molTricine: 7.64 kcal/molTris: 11.35 kcal/mola) In the presence of phosphate buffer, is the binding of DNA to the protein endothermicor exothermic? What is your reasoning?b) When Tris is deprotonated (ionization), is heat released or taken up from thesurroundings?c) Are protons taken up or released upon binding of the protein and DNA, or is there nochange in protonation upon forming the complex.Explain.
Answer to 2c? HELP ASAP!
Protons are released by the buffer solution to help in the DNA combination thus formation of a complex, as evident they have... View the full answer