Exam 1 Flashcards
AA/Water Chem/
name two reasons nature chose phosphates
why dont ochemists use p-fate
- negative charge at physio pH so that is sequesters within the membrane. it can link two nucleotides and still ionize
- stable bonding (ester formation) which are resistant to hydrolysis
ochemists dont use p-fate b/c it is not reactive enough as an intermediary
name 8 unique prop. of water
- h-bond
- high heat capacity (thermal Buffer)
- high dialectric const.
- universal solvent (almost)
- hydrophobic effect
- surface tension
- expands when freezes
- participates in reactions
state ECF/ICF concentration as high or low for each:
Na+
K+
Cl-
HCO3-
inorganic phosphate**
why is each high or low?
All in mmol/L and ECF = extra cellular fluid (outside the cell)
ICF = intracellular fluid
Na+: ECF = high (145) ICF=low(12)
K+: ECF = low(4), ICF = high(150)
Cl-: ECF = high(105), ICF = low(5)
HCO3-: ECF = high(25), ICF = low(12)
inorganic p-fate: ECF = low(2), ICF = high(100)
ECF = low b/c of higher Ca2+ concentration outside the cell, and calcium p-fate ppts out.
primary noncoalent driving force holding biomacromolecules together?
hydrophobic effect
normal AA with NH3 to the left side, what is the chiral config?
which ones can we use?
left = L
Right = D
humans use L AA
what AA can be phosphorlyzed and how?
Ser/Thr/Tyr = phosphoester bond formation
His/Lys/Arg = Phosphoramidate bonds
Asp/Glu = mixed anhydride linkages
What is the assumed (for class) pka of alpha Carboxyl group
and for alpha amino group
pka = 3 COOH
pka = 10 NH3
formula of hendersonhassel eq and its use?
pH = pKa + log([A-]/[HA]) ; where A- = conj. base and HA = acid
it is the eq for buffer calc. shows where HA = A- and where pH = pKa
applies to all ionizable groups no matter the charge state
if pH = 6 and pKa = 4, what does this tell you about A- and HA
each pH unit = factor of 10.
therefore since the pH is 6 which is greater than 4, A- is 100x greater concentration than HA.
the lower the pKa
the sttronger the acid
defn of a buffer
weak acid + its conjugate base that cause solution to resist changes in pH despite acid/base being added.
when do buffers work best (what is effectiveness of buffer casued by?)
effectivness is determined by the
- pH of soln, they work best within 1 pH unit of their pKa
- concentration of buffer, works best with more buffer present, greater amnt of buffer = bigger buffer capacity
when looking at a buffer titration curve, pay very close attention to what?
the axis, some have eq. of OH- on the x-axis while some have it on Y which changes the slope of the titration curve buffer zone
describe the blood buffer system and a common disease
give overall formula
CO2 = acid, HCO3 = base
they buffer the pH to maintain at 7.4 = normal
pulmonary obstruction = increase in CO2 = incrrease acid = decrease pH = respiratory acidosis
H+ + HCO3- –> H2CO3 –> Water byprod. –> CO2
drug charge and membrane crossing trend
explain why aspirin readily crosses into bloodstream in stomach
uncharged drugs (more nonpolar) cross more readily than charged drugs.
aspirin = lots of COOH residue AA, therefore at pH = 1.5 in stomach, and the lowest pKa of AA residues on aspirin around 3, the aspirin are protonated and thus uncharged and readily move across membranes