UMDNJSOM
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| pH | Measurement of amount of free H+ in a solution. pH = -log[H+] [H+] = antilog (-pH) | ||||
| Acids | release H+ into water | ||||
| Bases | Accept Free hydrogen ions | ||||
| Buffers | minimize changes in pH in a solution. Bind Any excess h+ present (decrease pH) release h+ if too few are present(increase pH) | ||||
| Henderson hasselback equation | pH = pka + log([A-]/[HA]) A = deprotonated form, HA = protonated | ||||
| 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 | ||||
| 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. | ||||
| Isoelectric point | pH value in which net charge is zero. pI below 6 = acidic pI above 8 = basic pI 6-8 = neutral | ||||
| Buffering zone | maximally resists buffer at this. pKa +1 and -1. | ||||
| 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. | ||||
| 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. | ||||
| Below pH 7.3, what happens to the blood | Carbon dioxide cant be removed efficiently. | ||||
| Why does extreme acidosis and alkalosis lead to death? | protein is denatured. change in protein shape. | ||||
| Zwitterion | dipolar. physiological pH, carboxyl deprotonated, amine protonated. | ||||
| 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. | ||||
| How is blood pH maintained? | CArbonic acid-Bicarbonate buffer, kidneys- take too long. Lungs faster way to control pH. | ||||
| 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 | ||||
| Respiratory Acidosis | acidosis resulting from failure of lungs to eliminate CO2 as fast as possible as it is produced | ||||
| Increasing breathing during exercise | Meant to counteract pH lowering effects of exercise by removing CO2, component of principal pH buffer in blood | ||||
| Slow breathing vs Fast breathing | Slow breathing, raises CO2 content, hypoventilaton. fast breathing, lowers CO2 concent, hyperventilation | ||||
| 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. | ||||
| If OH- ions are released into blood | OH- react with H2CO3, produce HCO3- and H2O. More CO2 dissolves in solution, H2CO3 remains constant. | ||||
| 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 | ||||
| Increase CO2 in blood/lungs | lower pH | ||||
| Lower BiCarbonate | lower pH |
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Created by:
nady
on 2011-09-18