Acid Base Physiology Flashcards Preview

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Flashcards in Acid Base Physiology Deck (135)
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1

Acid

Proton donor

2

Acidosis

Condition which causes an increase in [H+]

3

Acidemia

Presence of greater than normal [H+] in blood

4

Base

Proton acceptor

5

Alkalosis

Condition which causes a decrease in [H+]

6

Alkalemia

Presence of less than normal [H+] in blood

7

CO2 added to H2O is an ________

Acid

8

Explain the Law of Electrical Neutrality in regards to [HCO3-] and [H+]

Increase in [H+] = Increase in [HCO3-]

9

Capacity

Volume added to a volume

10

Acidic animal's physical response to increased acidity of plasma

Release CO2 by panting

11

An increase of acid or base is more common

Acid

12

Organ that gets rid of the most acid

Lungs

13

Importance of maintaining acid-base balance

Protein structure is dependent on prevailing [H+]

14

Departure from normal [H+] has what influence on drugs?

Changes in the structures they bind to, but also because many drugs are acids or bases their ability to donate/accept H+ is altered

15

Domestic animals can withstand proton concentrations that are between__________ the homeostatic normal [H+]

1/3 and 3 times

16

At equilibrium, the concentrations of _____, ______ and _______ are constant

Water, Proton and Hydroxide

17

Keq=

Keq= [H+] [OH-] / [H2O]

18

[H2O] Constant = ______

55.6 M

19

Keq constant = ______

1.8x10^-16

20

pH =

-log10 [H+]

21

Strong Acid/Base

One that readily dissociates

22

Weak Acid/Base

One which does not readily dissociate

23

Titratable Acidity/ Alkalinity

Total amount of proton/ proton acceptor which may be obtained from or complexed by another substance

24

Dissociation constant, Ka

Relative strength of an acid or base

25

Ka = [H+] under what circumstances?

When protonated and dissociated species are present in equal concentrations

26

pK

pH at which protonated and dissociated species are present in equal concentrations

27

Buffer

Weak acid able to resist changes in pH in the face of addition or removal of H+ from a solution

28

Relationship between buffer and pK

Buffer does its best buffering at its pK because it exists abundantly in both the protonated and dissociated forms. Permitting it to donate or titrate H+

29

Henderson-Hasselbalch Equation

pH= pK + log10 [A-] / [HA]

30

______________ is the most important buffer in the body.

CO2 + H2O H2CO3 H+ + HCO3-