Chem Chem Chem Chem Chemly Chem Chem Chem

Front 1

how does an increase in H affect pH

Back 1

increase in H = decrease in pH

Front 2

how does a decrease in H affect pH

Back 2

decrease in H = increase in pH

Front 3

pH >7.45

Back 3

alkalosis

Front 4

pH <7.35

Back 4

acidosis

Front 5

normal PaO2

Back 5

80-100mmHg

Front 6

normal PaCo2

Back 6

35-35mmHg

Front 7

normal ph

Back 7

7.35 - 7.45

Front 8

normal HCO3

Back 8

22-26

Front 9

normal BE

Back 9

-2 - +2

Front 10

what is a volatile acid

Back 10

waste product from cellular metabolism (ex. CO2)

Front 11

decrease PaCO2 (hypocapnia) are indicative of

Back 11

respiratory alkalosis (blowing off too much)

Front 12

increase PaCO2 (hypercapnia) are indicative of

Back 12

respiratory acidosis (retaining)

Front 13

PaO2 <80mmHg

Back 13

mild hypoxemia

Front 14

PaO2 <60mmHg

Back 14

moderate hypoxemia

Front 15

PaO2 <40mmHg

Back 15

severe hypoxemia

Front 16

decrease bicarb levels are indicative of

Back 16

metabolic acidosis

Front 17

increase bicarb levels are indictive of

Back 17

metabolic alkalosis

Front 18

how is PO2 measured

Back 18

clark electrode

Front 19

how is PCO2 measured

Back 19

severinghaus electrode

Front 20

how is pH measured

Back 20

SANZ electrode

Front 21

what is the henderson-hasselbalch equation

Back 21

how we calculate pH number

Front 22

normal pKc within the blood

Back 22

6.1

Front 23

if pH is effected by dissolved CO2 then it is...

Back 23

a respiratory problem

Front 24

if pH is effected by HCO3 then it is...

Back 24

a metabolic problem

Front 25

how do you measure the total CO2

Back 25

venous blood sample

Front 26

normal total CO2 levels

Back 26

22-28mmol/L

Front 27

normal anion gap range

Back 27

9-14mmHg

Front 28

what does the anion gap reflect

Back 28

normally unmeasured anions in the plasma (phosphates, sulfates, proteins)

Front 29

what do we use the anion gap to determine

Back 29

causes of metabolic acidosis

Front 30

anion gap equation

Back 30

Na - (Cl + HCO3)

Front 31

what is hyperchloremic metabolic acidosis

Back 31

if excessive bicarbonate were to be lost from the body, the chloride concentration would have to increase to maintain anions for electroneutrality ... would cause the anion gap stays normal

Front 32

if the anion gap is high, the metabolic acidosis is caused by...

Back 32

an accumulation of fixed acids

Front 33

acronym for causes of high anion gap

Back 33

M.u.d. p.i.l.e.s

Front 34

if anion gap is normal it is caused by

Back 34

loss of base

Front 35

henry's law

Back 35

gases dissolve in liquids in direct proportion to their partial pressures

Front 36

CO2 solubility coefficient

Back 36

0.072 vol%/mmHg

Front 37

O2 solubility coefficient

Back 37

0.003vol%/mmHg

Front 38

which diffuses faster, CO2 or O2?

Back 38

CO2 (diffuses about 20x faster)

Front 39

some of the CO2 that enters the plasma will end up forming bicarbonate, but it tends to be a small amount.. why?

Back 39

1. accumulation of products from the hydrolysis reaction with halt the reaction

2. no enzyme to catalyze the hydrolysis reaction

Front 40

when CO2 diffuses through the cell membrane, what other level rises?

Back 40

levels of RBC's rise

Front 41

why is chloride shift much faster in the RBCs than the plasma? (2)

Back 41

-the enzyme carbonic anhydrase

-HCO2 and H are not able to accumulate

Front 42

protein combined with CO2 is called

Back 42

carbamino compound

Front 43

hemoglobin + CO2 =

Back 43

carbaminohemoglobin

Front 44

what percentage is CO2 transport with dissolved CO2

Back 44

8%

Front 45

what percentage is CO2 transported with bicarbonate

Back 45

80%

Front 46

what percentage is CO2 transported in carbamino compounds

Back 46

12%

Front 47

how do certain conditions (diabetes, hypoxia) effect regulation of fixed acids

Back 47

diabetes/hypoxia can increase the production of fixed acids, so the kidneys increase acid excretion

Front 48

what fixed acid does protein catabolism make

Back 48

inorganic sulfuric acid + phosphoric acid

Front 49

what fixed acid does lipid metabolism make

Back 49

organic acetoacetic + beta-hydroxybutyric acid

Front 50

what fixed acid does carbohydrate metabolism make (absence of oxygen)

Back 50

lactic acid

Front 51

how would renal disease effect fixed acid regulation?

Back 51

retention of fixed acids (could lead to excess of H and a fall in pH)

Front 52

how can bicarbonate reabsorption be increased

Back 52

1. increase blood PCo2

2. low serum K

3. decrease blood volume

Front 53

formula for dissociation of acids

Back 53

HA <---> H (hydrogen ion) + A (base)

Front 54

The greater the degree of association....

Back 54

the stronger the acid is said to be

Front 55

strong acids = ____ dissociation

Back 55

strong acids =HIGH dissociation

Front 56

weak acids = ____ dissociation

Back 56

weak acids = LOW dissociation

Front 57

weak acids are associated with ___ bases

Back 57

weak acids are associated with strong bases

Front 58

strong acids are associated with ____ bases

Back 58

strong acids are associated with weak bases

Front 59

what is an ampholyte

Back 59

a substance that can act as either an acid or a base

Front 60

who's conjugate base is stronger, deoxygenated hemoglobin or oxygenated hemoglobin

Back 60

the conjugate base of deoxygenated hemoglobin is stronger (can pick up hydrogen ions easier)

Front 61

what are buffer solutions made up of?

Back 61

the acid & salt of the conjugate base (can buffer either acid or base)

Front 62

how does ammonia minimize changes in pH

Back 62

combines with hydrogen then excreted therefore minimizing decrease in pH (

Front 63

how does an increase in acid production effect ammonia and hydrogen

Back 63

when there is an increased acid production, there is an increase ammonia production and h excretion

Front 64

how does an increase in acid production effect phosphate and hydrogen

Back 64

when there is an increased acid production, there is an increased phosphate + h excretion (H2PO4)

Front 65

how do chemical buffers work?

Back 65

act as sponges to soak up or release free H (so pH is not altered greatly)

Front 66

bicarbonate is important in... (chemical buffers)

Back 66

plasma & interstitial fluid

Front 67

organic phosphates & proteins play a major role in... (chemical buffers)

Back 67

ICF

Front 68

Bone plays an important role in... (chemical buffers)

Back 68

chronic conditions

Front 69

which kind of buffers are the primary defense against abrupt changes in pH

Back 69

blood buffers

Front 70

the effectiveness of a given buffer system depends on what 3 factors?

Back 70

1. the quantity of the buffer

2. the pK

3. whether the buffer is an open or closed system

Front 71

how does quantity effect the buffer system

Back 71

the larger the quantity... the more acid or base it can buffer

Front 72

how does pK effect the buffer system

Back 72

buffers are considered to function well within 1 pH UNIT OF THEIR pK

Front 73

how does open vs closed system effect buffer systems

Back 73

in a closed system a buffer is less effective

Front 74

example of a closed buffer system

Back 74

hemoglobin

Front 75

example of a open buffer system

Back 75

the bicarbonate buffer system

Front 76

which buffer system takes care more of 50% of total buffering?

Back 76

the bicarbonate system

Front 77

most important ECF buffer

Back 77

plasma bicarbonate

Front 78

most important ICF buffer

Back 78

hemoglobin

Front 79

strong acid

Back 79

dissociation where HYDROGEN COMPLETELY DISSOCIATES

Front 80

weak acids

Back 80

dissociation where NOT ALL OF THE HYDROGEN DISSOCIATED

Front 81

what is the only way excess K can be excreted in the distal tubule

Back 81

in the NaHCO3 mechanism, K instead of an H is secreted into the filtrate in exchange for the Na cation

Front 82

where does the NaCl mechanism take place

Back 82

renal tubule