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BIOL 204 > Lecture 17 -- review questions > Flashcards

Lecture 17 -- review questions Flashcards

1
Q

what is acid-base balance?

A

adequate levels of acid and bases in blood and body for proper cell functioning

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2
Q

what is the normal pH range of the blood?

A

7.35-7.45

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3
Q

what is a volatile acid?

A

acid that is produced from CO2

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4
Q

what is a physiological example of a volatile acid?

A

carbonic acid (from CO2)

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5
Q

what is a non-volatile or fixed acid?

A

acid that is produced form anything other than CO2

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6
Q

what is a physiological example of a non-volatile or fixed acid?

A

lactic acid (anaerobic fermentation)

phosophoric acids (nucleic acid catabolism)

fatty acids and ketones (fat catabolism)

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7
Q

what is acidosis?

A

blood pH below 7.4

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8
Q

what is alkalosis?

A

blood pH above 7.4

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9
Q

how is blood pH kept within a narrow range when our bodies are constantly producing acid?

A

buffer systems

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10
Q

what buffers does the body use as a 1st line of defense in response to an increase in pH?

And as the 2nd line?

3rd line?

A

1st line – chemical buffers – seconds

2nd line – physiological buffer – respiratory system – min to hrs

3rd line – physiological buffer – urinary system – days to weeks

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11
Q

what 2 organs play an essential role in maintaining acid-base balance? (think about physiological buffers)

A

lungs

kidneys

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12
Q

what is a chemical buffer?

A

molecules that maintain pH by releasing or binding H+

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13
Q

what are the 3 chemical buffer systems in the body

A

bicarbonate buffer system

phosphate buffer system

protein buffer system

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14
Q

why is the role of chemical buffers in controlling blood pH limited?

A

chemical buffers guard against sudden swings in pH

don’t eliminate or add H+ to the body, only release or bind

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15
Q

where is the bicarbonate buffer system more critical, in the ECF or ICF? How about the phosphate buffer system?

(tip: which anion is more abundant in the ICF?)

A

(phosphate is most abundant anion in ICF)

bicarbonate buffer system –> more critical in ECF

phosphate buffer system –> more critical in urine and ICF

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16
Q

if the pH of a solution decreases, what happens to the concentration of H+ in the solution: increase or decrease?

A

pH decreases == more acidic == increased [H+]

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17
Q

if the pH of a solution increases, what happens to the concentration of H+ in the solution: increase or decrease?

A

pH increases == more basic == decreased [H+]

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18
Q

which group in a protein acts as an acid, the amino or the carboxyl group? why?

A

(think carboxylic acid is an acid)

carboxyl group –> COOH can become COO- and H+

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19
Q

which group in a protein acts as a base, the amino or the carboxyl group? why?

A

amino group –> NH2 can accept a H+ to become NH3+

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20
Q

when the body experiences alkalosis, how do proteins help restore the acid-base balance?

A

carboxyl group in amino acid releases an H+

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21
Q

when the body experiences acidosis, how do proteins help restore the acid-base balance?

A

amino group in amino acid binds an H+

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22
Q

what is the chemical formula for carbonic acid?

A

H2CO3

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23
Q

what is the chemical formula for the bicarbonate ion?

A

HCO3-

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24
Q

what volatile gas is carbonic acid (H2CO3) in equilibrium with?

A

CO2

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25
Q

how is the carbonic acid created in our body?

A

CO2 (released from tissues) + H2O –> (carbonic anhydrase) –> H2CO3

26
Q

why is CO2 elimination crucial? (which acid does it form?)

A

CO2 must be eliminated to form H2CO3 which can release H+

27
Q

what chemical reaction is catalyzed by carbonic anhydrase?

A

CO2 (released from tissues) + H20 –> (carbonic anhydrase) –> H2CO3

28
Q

which component acts as an acid (=H+ donor) in the carbonic acid-bicarbonate buffer system?

A

H2CO3

carbonic acid (weak acid)

29
Q

which component acts as a base (=H+ acceptor) in the carbonic acid-bicarbonate buffer system?

A

HCO3-

bicarbonate ion (weak conj. base)

30
Q

what is the equation for the bicarbonate-carbonic acid buffering system?

A

CO2 + H2O –> (carbonic anhydrase) –> H2CO3 –> HCO3- + H+

31
Q

suppose there is an excess of acid (H+) in the blood (=acidosis or acdiemia), and the bicarbonate ion accepts those extra H+ of the solution (“neutralize the excess of acid”).

What happens to the pH of the solution, increase or decrease?

A

increase back to normal range (7.35-7.45)

32
Q

suppose there is a deficiency of acid (H+) or excess of a base in the blood (=alkalosis or alkalemia), and the carbonic acid donates H+ to the solution (releases the H+).

what happens to the pH of the solution, increase or decrease?

A

decrease back to normal range (7.35-7.45)

33
Q

what is the way the body gets rid of volatile acid?

A

respiratory –> increase rate and depth of breathing –> expel CO2

34
Q

what is the way the body gets rid of fixed acid?

A

kidneys –> increase H+ excretion by producing more bicarb (HCO3-)

35
Q

which organ maintains bicarbonate levels?

A

kidneys

36
Q

which organ maintains CO2 levels?

A

lungs

37
Q

can the respiratory system get rid of increased fixed acids in blood?

A

no – it can only directly get rid of volatile acids –> but getting rid of more CO2 helps bring H+ fixed acid levels down

38
Q

why does increasing breathing rate and depth (=hyperventilation) increase pH?

what happens to CO2 and H+ levels?

what is the name of this disorder? (respiratory/metabolic, acidosis/alkalosis?)

in which direction (to the right or the left) would the carbonic acid-bicarbonate buffer system equation move in this case?

A

hyperventilation == get rid of CO2 == lower H+ levels

respiratory alkalosis

carbonic acid-bicarbonate buffer system equation move to the left –> decrease CO2 == decrease H+

39
Q

why does a decrease in breathing rate and depth decrease pH? What happens to CO2 and H+ levels? What is the name of this disorder? (respiratory/metabolic, acidosis/alkalosis?).

In which direction (to the right or the left) would the carbonic acid-bicarbonate buffer system equation move in this case?

A

hypoventilation == more CO2 in body == higher H+ levels

respiratory alkalosis

carbonic acid-bicarbonate buffer system equation moves to the right –> more CO2 == more H+

40
Q

reabsorption of HCO3- in the renal tubule is always tied to the secretion of which ion?

A

H+

41
Q

what is the goal of reabsorbing H+ from the urine? (to counteract acidosis or alkalosis)

A

lower pH to make more acidic

counteract alkalosis

42
Q

what is the goal of secreting more H+ in the urine? (to counteract acidosis or alkalosis)

A

increase pH to make more basic

counteract acidosis

43
Q

what is the goal of reabsorbing more bicarbonate ions from the urine? (to counteract acidosis or alkalosis?)

A

reabsorb HCO3- ==> get more base

secrete H+ ==> get rid of acid

counteract acidosis

44
Q

what is the goal of secreting bicarbonate ions in the urine? (to counteract acidosis or alkalosis?)

A

secrete HCO3- ==> get rid of base

reabsorb H+ ==> get more acid

counteract alkalosis

45
Q

which 3 transport proteins of the renal tubule are related to acid-base regulation, and where are they located?

A

Na+ H+ exchanger –> found in PCT

K+/H+ ATPase –> found in a-intercalated cells in CD

H+ ATPase –> found in a-intercalated cells in CD

46
Q

in order to reabsorb bicarbonate ions from the lumen of the renal tubule, this ion must be decomposed to water and CO2: why (tip: is the membrane permeable to bicarbonate ions?)

A

membrane is not permeable to HCO3- ions

HCO3- combines with H+ to H2CO3 –> H2CO3

H2CO3 decomposes thru carbonic anhydrase to H2O + CO2

47
Q

where is the H+ secreted into the renal tubule coming from? (tip: check what happens to the carbonic acid inside of the tubule cells in the PCT)

A

HCO3- + H+ originally in tubular fluid

–> become H2CO3

–> become H2O + CO2 (via carbonic anhydrase)

–> diffuse into renal tubular cell

–> become H2CO3 (via CA)

–> become H+ and HCO3-

H+ starts at renal tubular cell and gets secreted into tubular lumen

48
Q

what metabolic changes would you check to see for acid-base balance? (ie the concentration of which ion in the blood)

A

check HCO3- concentration

when [HCO3-] is high
==> more base and less acid
==> [H+] secretion is high
==> low [H+] in blood
==> pH is high
==> alkalosis

when [HCO3-] is low
==> less base and more acid
==> H+ reabsorption is high
==> high [H+] in blood
==> pH is low
==> acidosis

49
Q

what is acid-base disorder developed when there is an increased PCO2?

A

respiratory acidosis

50
Q

what is acid-base disorder developed when there is decreased PCO2?

A

respiratory alkalosis

51
Q

what acid-base disorder is developed when there is an increased HCO3-?

A

metabolic alkalosis

(more base == less acid == basic)

52
Q

what acid-base disorder is developed when there is an decreased HCO3-?

A

metabolic acidosis

(more acid == less base == acidic)

53
Q

what are the 2 ways that metabolic acidosis can occur?

A

diabetic ketoacidosis ==> (increased acid production)

renal failure ==> (lower acid elimiation)

54
Q

what are the 2 ways that metabolic alkalosis can occur?

A

overuse of antacids (excess HCO3-)

loss of acids H+ (vomiting)

54
Q

what are the 2 ways that metabolic alkalosis can occur?

A

overuse of antacids (excess HCO3-)

loss of acids H+ (vomiting)

55
Q

which organ compensates for acid-base disorders of metabolic origin

A

lungs

56
Q

which organ compensates for acid-base disorders of respiratory origin?

A

kidneys

57
Q

how do the lungs compensate for metabolic alkalosis?

A

metabolic alkalosis == high [HCO3-]

lungs increase pCO2 levels
–> increase [H+] –> more acidic
–> lower pH to normal levels

58
Q

how do the lungs compensate for metabolic acidosis?

A

metabolic acidosis == low [HCO3-]

lungs decrease pCO2 levels
–> decrease [H+] –> more basic
–> increase pH to normal levels

59
Q

how do the kidneys compensate for respiratory alkalosis?

A

respiratory alkalosis == low pCO2

kidneys decrease [HCO3-] levels:
–> less base –> more acidic
–> decrease pH to normal levels

60
Q

how do the kidneys compensate for respiratory acidosis?

A

respiratory acidosis == high pCO2

kidneys increase [HCO3-] levels:
–> more base
–> increase pH to normal levels

61
Q

classify the following conditions as possible causes of respiratory acidosis/alkalosis or metabolic acidosis/alkalosis:

  • inhibition of the respiratory center
  • lung damage
  • airway obstruction
  • diarrhea
  • diabetic ketoacidosis
  • renal failure
  • high altitude (decreased O2)
  • anxiety
  • overuse of antacids (e.g. bicarbonate)
  • vomiting gastric contents
A

respiratory acidosis:
- inhibition of the respiratory center
- lung damage
- airway obstruction
- diarrhea

metabolic acidosis:
- diabetic ketoacidosis
- renal failure

respiratory alkalosis:
- high altitude (decreased O2)
- anxiety

metabolic alkalosis:
- overuse of antacids (e.g. bicarbonate)
- vomiting gastric contents

BIOL 204 (35 decks)

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