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Bronstead- Lowry acid/ base
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4 strong acids
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ZPhar410 Acid/ Base
ZFundamentals of Drug Action
| Question | Answer |
|---|---|
| Bronstead- Lowry acid/ base | Acid is proton donor; Base is proton acceptor |
| 4 strong acids | HCl; HNO3; H2SO4; HClO4 |
| 2 strong bases | NaOH; KOH |
| pKa < 2 is a strong | strong acid; no basic properties in water |
| pKa 4-6 is a ? | weak acid; very weak conjugate base |
| pKa 8-10 is a | very weak acid; weak conjugate base |
| pKa > 12 | no acidic properties in water; strong conjugate base |
| the stronger an acid, the weaker its conjugate base | no answer |
| what is the conjugate acid and base of HA + H20 | Conj acid= H3O; conj base is A- |
| Keq= | [products]/ [reactants] |
| difference between pH and pKa | pH is property of a solution/ pKa is property of a molecule- the tendency of protonated for to give up a proton |
| Henderson Hasselbalch eq: | pH= pKa+ log [conj base/ acid]; the conj base is proton acceptor, acid is donor |
| Relates pH/ pKa to relative amount of acid/ base | henderson- hasselbalch equation |
| Drugs that are amines are: | basic |
| In an acid, what gets ionized | conjugate base gets ionized; ex: HCl --> Cl- |
| In a base, what gets ionized? | the acid is ionized |
| Conjugate base of salicylic acid | salicylate |
| Drugs that are amines are: | basic |
| In an acid, what gets ionized | conjugate base gets ionized; ex: HCl --> Cl- |
| In a base, what gets ionized? | the acid is ionized |
| Conjugate base of salicylic acid | salicylate |
| Henderson Hasselbalch; not always charged reactant | always protonated form on the left (reactant) side of the equation (DENOMINATOR) |
| For ionized acids, pH is above or below pKa? | pH is above pks (chart) |
| For a base, the percent ionization gets higher as pH | gets lower (think chart) |
| Pharmaco-kinetics | Action of the body on the chemical (what the body does to the drug) |
| Pharmaco- dynamics | What the drug does to the body |
| Processes of pharmacokinetics ADME | absorpion, distribution, metabolism, elimination |
| Output: Concentration- time relationships | Pharmacokinetics |
| Process of pharmacodynamics: | Biological ligands acting on their molecular targets in the body |
| Output: Biological response | Pharmacodynamics |
| when drug reached site of action we see | pharmacodynamics response; drug- receptor complex/ pharmacologic response |
| Prior to reaching targets the drug must go thru what obstacles? These barriers affect the pharmacokinetics ofthe drug | pass thru barriers (membranes) avoid wrong turn (ex: accumulating in fat cells; avoid metabolic destruction; stability at different pH levels |
| absorption is affected by ionization state | true; affects drug;s ability to pass thru membranes |
| acids like aspirin are absorbed where | stomach, low pH- the thing that is UNionized is absorbed..aspirin in unionized on the chart until about pH 5. after that it would not be too useful |
| Bases are absorbed in | intestines because as pH increases, bases get LESS ionized |
| why precipitation of bases? | go from charged NH3+ to uncharged NH2; less polar and may precipitate because out of solution; wants to get away from water (hydrophobic) |
| ases are 100% ionized where in the absorption process | stomach |
| to pass thru lipid barrier, a weak acid would be on the left side of the equation because | it is unionized |
| weak bases pass thru lipid barrier on the right side of the equation because | they are neutral (unionized); they are protonated on the left side of the rxn; example: BH+ +H2O <-> H3O + B(neutral) |
| PH maintenance mechanisms (3) | chemical buffering; lungs; kidney (renal) |
| Chemical buffering (quick) name 4 systems | bicarbonate buffer;phosphate buffer; ammonia buffer; proteins |
| If strong acid is introduced, the reaction will move in which direction? | left because the A- will pick up an H+ which drives the rxn to make HA |
| The most important extracellular (plasma) buffering system | bicarbonate buffer system; generally considered clinically |
| Carbonic acids (H2CO3) exist in low amounts in the body; CO2 is considered the weak acid | no answer |
| Co2 and HCO3 act as buffers | true |
| pCO2 is used as? | an index of the amount of carb on dioxide in the body (normally 40mm Hg) |
| Normal concentration of bicarbonate is | 24 mEq/L; ratio of HCO3-/ H2CO3 is 20:1 |
| Intracellular buffer; also in the kidneys | phosphate buffer system |
| By-product of amino acid metabolism | ammonia; amino acids can serve as buffers in the ammonia buffer system |
| most plentiful chemical buffers; high concentrations inside cell | proteins; side chains can accept or donate a proton |
| CO2 is an acid and the lungs remove it to raise pH | no answer |
| The slowest most powerful acid/ base balance | Renal (kidney); excrete acidic or basic urine depending on whats needed |
| If bicarbonate is not reabsorbed( back into bloodstream) it is excreted | in the urine; bicarbonate is not well absorbed by itself, must combine with a proton |
| Bicarbonate and H+ combine to form what? | CO2 and H2O; then can enter renal tubule; once in the renal tubule they can separate and bicarbonate returns to capillary |
| excess acid in plasma, what does kidney do? | kidney reabsorbs ALL bicarbonate to raise pH |
| Alkalosis, what does kidney do with bicarbonate? | less bicarbonate is reabsorbed, more is excreted |
| respiratory acidosis | increased pCO2; high bicarbonate indicates compensation |
| Metabolic acidosis | low bicarbonate; normal pCO2 indicates not related to respiratory but can be low as compensation |
Created by:
angieryx
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