BIOCHEM 2EE3 Study Guide - Final Guide: Acid Dissociation Constant, Amine, Thermodynamics

• School: McMaster University
• Department: Biochemistry
• Course: BIOCHEM 2EE3
• Professor: Boris Zhorov

Document Summary

Example: charge-charge interactions our dna is negative, and small ions such as k+ and cl- help stabilize this macromolecule via charge-charge interactions. *on an energy vs. distance graph, can see that electrons too far won"t attract and too close will repel. Example: hydrogen bonds bond bw hydrogen atom and f, o, n - these are hydrogen bond acceptors. Arrhenius theory acids = proton (h+) donors bases = proton acceptors water is amphiprotic so acts are both acid/base. Kw = [h+] x [oh-] = 1 x 10^-14 ph = -log[h+] low ph = acidic (0) high ph = basic (14) Henderson hassalbach/bu ers if equation is: ha -> h+ + a- then ka = [h+][a-]/[ha] pka = -logka pka + pkb = 14. Bu er equation - ph = pka + log[a-]/[ha] Ha = weak acid ph = pka at neutralization point.