Lecture's 1 & 2 Flashcards
Hydrophobic Effect
Water fearing molecules come together and break apart water molecules in the process, releasing energy
Coulomb’s Law
E=kq1q2/Dr
(D=dielectric constant of solvent/environment where bond is located)
(r=distance b/w two charges)
Small r = Large E
Gibbs Free Energy Equations (2)
XXXXXX
Le Chatelier’s Principle
aka Mass Action: Concentrations drive reaction
EX: lots of glucose drives glycolysis
Coupled Reactions
Involves an input of energy
Possible if there is a shared intermediate
pH range for physiological conditions
7.37-7.43
pH= (equation)
pH=-log[H+]
pH of 7=
1x10^-7M
Hyperventilating
Causes your pH to increases, become more alkaline (basic)
Hypoventilating
Causes your pH to decrease, become more acidic
3 main Ketone bodies
1) Beta-hydroxybuterate
2) Acetoacetone
3) Acetone
4 examples of creating acidic environment in body
1) Diabetes- ketone bodies
2) Working out- lactic acid build up
3) Diarrhea- lose of bicarbonate
4) Vomitting- creating metabolic alkalosis
Henderson-Hasselbalch Equation
pH=pKa+log([A-]/[HA])
A- is conjugate base
HA is conjugate acid
If pH=pKa=
Max buffering potential
If pH<pKa=
More [acidic]
