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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