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| pH | Measurement of amount of free H+ in a solution.
pH = -log[H+]
[H+] = antilog (-pH)
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| Acids | release H+ into water
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| Bases | Accept Free hydrogen ions
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| Buffers | minimize changes in pH in a solution.
Bind Any excess h+ present (decrease pH)
release h+ if too few are present(increase pH)
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| Henderson hasselback equation | pH = pka + log([A-]/[HA])
A = deprotonated form, HA = protonated
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| pH above and below pKa | pH above pKa = more OH- ions, take away H+ from molecules, more negative
pH below pKa = more H+ ions, add h+ onto molecule, make more positive
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| Isoelectric point calculation | First find the one with net zero charge. Then find two pKas that go from +1 to 0 charge and from -1 to 0 charge. Add them up, divide by two. that is your pI.
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| Isoelectric point | pH value in which net charge is zero.
pI below 6 = acidic
pI above 8 = basic
pI 6-8 = neutral
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| Buffering zone | maximally resists buffer at this.
pKa +1 and -1.
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| Papain | breaks down proteins. most active between pH 6 and 7. Enzyme.
cysteine 25 and histidine 159 are involved. charged at this pH.
Enzymatic activity lost when
lower pH, cysteine is protonated
higher pH, histidine deprotonated.
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| pH of blood | Must be around 7.4. below 7.4 = acidosis. indiciation of diabetes. Serious, many enzymes pH dependent.
above 7.4 = alkalosis. caused by hyperventilation and persistent vomiting.
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| Below pH 7.3, what happens to the blood | Carbon dioxide cant be removed efficiently.
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| Why does extreme acidosis and alkalosis lead to death? | protein is denatured. change in protein shape.
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| Zwitterion | dipolar. physiological pH, carboxyl deprotonated, amine protonated.
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| Ionic state of AA | depends on pH of solution.
low pH = AA protonated at amine and carboxyl, + charge.
high pH = AA deprotonated at amine and carboxyl, - charge.
neutral pH = zwitter ion. also called isoelectric point.
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| How is blood pH maintained? | CArbonic acid-Bicarbonate buffer, kidneys- take too long. Lungs faster way to control pH.
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| Carbonic Acid-Bicarbonate Buffer | Most important buffer for maintaining pH in blood. [HCO3] in blood fixed by [CO2] in gas phase. [CO2] in lungs depends on rate of CO2 production in metabolism and rate of breathing
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| Respiratory Acidosis | acidosis resulting from failure of lungs to eliminate CO2 as fast as possible as it is produced
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| Increasing breathing during exercise | Meant to counteract pH lowering effects of exercise by removing CO2, component of principal pH buffer in blood
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| Slow breathing vs Fast breathing | Slow breathing, raises CO2 content, hypoventilaton.
fast breathing, lowers CO2 concent, hyperventilation
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| If H+ ions released into blood | H+ ions react with HCO3- to form H2CO3. Carbonic Anhydrase converts this to CO2 and H2O, releases CO2 as gas in lungs. H2CO3 remains constant.
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| If OH- ions are released into blood | OH- react with H2CO3, produce HCO3- and H2O. More CO2 dissolves in solution, H2CO3 remains constant.
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| If a person hyperventilates | pCO2 in lungs drops. lungs remove excess CO2 from blood(raise pH).
This ultimate causes a drop in H+ concentration and results in an increase in bloods pH. causes alkalosis
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| Increase CO2 in blood/lungs | lower pH
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| Lower BiCarbonate | lower pH
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Created by:
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