ZFundamentals of Drug Action
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Bronstead- Lowry acid/ base | show 🗑
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| show | HCl; HNO3; H2SO4; HClO4
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| 2 strong bases | show 🗑
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| show | strong acid; no basic properties in water
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| show | weak acid; very weak conjugate base
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| pKa 8-10 is a | show 🗑
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| pKa > 12 | show 🗑
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| show | no answer
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| show | Conj acid= H3O; conj base is A-
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| show | [products]/ [reactants]
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| difference between pH and pKa | show 🗑
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| Henderson Hasselbalch eq: | show 🗑
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| show | henderson- hasselbalch equation
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| Drugs that are amines are: | show 🗑
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| show | conjugate base gets ionized; ex: HCl --> Cl-
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| show | the acid is ionized
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| show | salicylate
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| show | basic
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| In an acid, what gets ionized | show 🗑
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| show | the acid is ionized
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| show | salicylate
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| show | always protonated form on the left (reactant) side of the equation (DENOMINATOR)
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| For ionized acids, pH is above or below pKa? | show 🗑
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| For a base, the percent ionization gets higher as pH | show 🗑
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| show | Action of the body on the chemical (what the body does to the drug)
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| show | What the drug does to the body
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| Processes of pharmacokinetics ADME | show 🗑
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| Output: Concentration- time relationships | show 🗑
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| Process of pharmacodynamics: | show 🗑
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| show | Pharmacodynamics
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| show | pharmacodynamics response; drug- receptor complex/ pharmacologic response
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| show | pass thru barriers (membranes) avoid wrong turn (ex: accumulating in fat cells; avoid metabolic destruction; stability at different pH levels
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| show | true; affects drug;s ability to pass thru membranes
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| acids like aspirin are absorbed where | show 🗑
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| show | intestines because as pH increases, bases get LESS ionized
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| why precipitation of bases? | show 🗑
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| ases are 100% ionized where in the absorption process | show 🗑
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| to pass thru lipid barrier, a weak acid would be on the left side of the equation because | show 🗑
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| show | they are neutral (unionized); they are protonated on the left side of the rxn; example: BH+ +H2O <-> H3O + B(neutral)
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| PH maintenance mechanisms (3) | show 🗑
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| show | bicarbonate buffer;phosphate buffer; ammonia buffer; proteins
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| show | left because the A- will pick up an H+ which drives the rxn to make HA
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| The most important extracellular (plasma) buffering system | show 🗑
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| Carbonic acids (H2CO3) exist in low amounts in the body; CO2 is considered the weak acid | show 🗑
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| Co2 and HCO3 act as buffers | show 🗑
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| show | an index of the amount of carb on dioxide in the body (normally 40mm Hg)
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| Normal concentration of bicarbonate is | show 🗑
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| Intracellular buffer; also in the kidneys | show 🗑
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| By-product of amino acid metabolism | show 🗑
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| show | proteins; side chains can accept or donate a proton
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| CO2 is an acid and the lungs remove it to raise pH | show 🗑
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| show | Renal (kidney); excrete acidic or basic urine depending on whats needed
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| show | in the urine; bicarbonate is not well absorbed by itself, must combine with a proton
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| Bicarbonate and H+ combine to form what? | show 🗑
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| excess acid in plasma, what does kidney do? | show 🗑
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| Alkalosis, what does kidney do with bicarbonate? | show 🗑
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| show | increased pCO2; high bicarbonate indicates compensation
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| show | low bicarbonate; normal pCO2 indicates not related to respiratory but can be low as compensation
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