BIOL 3090 Study Guide - Midterm Guide: Chemical Equilibrium, Equilibrium Constant, Reaction Rate

70 views20 pages
2 Jul 2014
School
Course
Professor

Document Summary

2-23: the rate of formation of b = rate of consumption of b. These individual reactions do not reach equilibrium, but instead reach a steady state. In pure water [h+] and [-oh] are the same, so [-oh] also = 1x10^-7m. [h+][-oh] = 1x10^-14 m^2: for any solution based in water, this is true but [h+] and [-oh] fluctuate, for any acqueous solution, [h+][-oh] = 1x10^-14 m^2. Henderson-hasselbalch equation: relates ph and equilibrium constant (keq) ph = pka + log [a-]/[ha: note that half the acid has dissociated into a- and the other half remains as ha. Ch3coo- and h: notice that the ph does not change that much around the pka, fig. Ans: pka of acetic acid is too low. Instead, our cells use phosphoric acid as the intracellular buffer because it"s middle pka is 7. 2. Intracellular ph is around 7-7. 2 so phosphoric acid is perfect for biological reactions: fig.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers

Related Documents

Related Questions