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### 18 Cards in this Set

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 What is the normal pH in blood 7.4 Define the ion product of H20 It is the [H+]*[0H-] = Kw Kw= [H+][0H-] = [H20]*Keq What is the ion product of H20 at 25 deg celcius 1e-14 When is a solution of water said to be neutral When [H+]=[0H-] What is pH? It is the negative logarithm of the [H+] What is an acid? A proton donor What is a base? A proton acceptor What is Ka? ([H+][A-])/[HA] = Ka The stronger the tendency to give up a proton, the _____ the acid, the _______ the pKa stronger; lower What is titration? A method used to determine the amount of acid in a given solution What is a buffer? A mixture of weak acids and their conjugate base that tend to resist changes in pH when small amounts of acid or base are added. When is the buffering power of a system maximal. When [HA] = [A-] What is the pKa of a buffer system? The pH at which [HA]=[A-] Why does the addition of strong acid or base to a buffer not result in a large pH change Because the ratio of the concentration of the conjugate base to the acid only changes very slightly What is the H-H equation? pH=pKa + log([A-]/[HA]) What happens when the [H+] increases in the blood? Increased H2C03; Increased dissolved C02; Increased gaseous C02 -> Excess C02 gas is exhaled What happens when blood plasma pH increases? Decreases H2C03, dissociates into H+ and HC03-; causes C02 gas to dissolve in blood plasma The pH of a bicarbonate buffer system ultimately depends on what? 1.The concentration of HCO3- in the aqeous phase 2.The partial pressure of C02