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Block 2 Week 6 > The Fundamentals of Body Buffers and Gases > Flashcards

The Fundamentals of Body Buffers and Gases Flashcards

1
Q

What is the goal of the cellular metabolism

A

to get oxygen in and acids out

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2
Q

(blank) of carbon dioxide (volatile acid) per day excreted by lung

A

12 moles

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3
Q

(blank) metabolic acid (non-volatile acid) per day excreted by kidney

A

0.1 moles

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4
Q

The rate of acid production equals the rate of acid (blank) which results in homeostasis of blood content.

A

excretion

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5
Q

How is the pH of the blood measured?

A

extracellularly

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6
Q

If you have balanced ECF pH what else do you have?

A

balanced interstitial pH and balanced ICF pH

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7
Q

What is a healthy pH? what is a healthy H concentration?

A

7.35 -7.45

45-35

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8
Q

At what pH can life not be sustained?

A

below 6.8 and after 7.8

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9
Q

Is HCO3, pH and PaCO2 calculated or measured

A

HCO3 is calculated

pH and PaCO2 is measured

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10
Q

acid production originated (blank)

A

intracellularly

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11
Q

Which is more acidic, ICF or ECF?

A

ICF

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12
Q

Concentrations of buffers in the ICF are (blank) than ECF (~3X)

A

higher

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13
Q

Cells can (blank) acids and buffers across their membranes to maintain a pH distinct from ECF

A

actively transport

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14
Q

most body acids are essentally fully ionized at what pH

A

7.4

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15
Q

what is the standard H concentration to use for equations?

A

40 nM

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16
Q

At pH 7.4 metabolic intermediates in the charged form are effectively (blank) within the cell

A

trapped

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17
Q

What is the isohydric principle?

A

An alteration in pH effects relative concentrations of every conjugate acid and base of all the weak electrolytes.

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18
Q

If the concentration of hydrogen ions is less than the Ka then most of the metabolite will be in its (blank) formed

A

ionized

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19
Q

buffers can be compared by (blank)

A

buffer capacity

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20
Q

High capacity buffers are higher in (blank) and their pka’s are closer to the (blank)

A

concentration

working pH

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21
Q

What is the purpose of a buffer?

A

pH homeostasis

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22
Q

What is the definition of a buffer?

A

weak acid-base pai

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23
Q

What do buffers do?

A

lessen (mitigate) pH changes due to addition of strong acids or bases

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24
Q

What are the main buffers in the ECF?

A
  • hemoglobin (non volatile)
  • plasma proteins (non volatile)
  • phosphates(non volatile)
  • bicarb buffer (volatile)
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25
Q

Why is the bicarb buffer volatile?

A

cuz CO2 gas is involved

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26
Q

What has the highest buffering capacity?

A

hemoglobin

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27
Q

Where do you find hemoglobin?

A

intracellular (in RBC)

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28
Q

RBC membranes are permeable to (blank).

A

protons

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29
Q

What has an important and rapid impact on the ECF pH?

A

hemoglobin

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30
Q

Is hemoglobin considered an intracellular or extracellular buffer?

A

extracellular

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31
Q

Hb has a lot of (blank) at a pka of (blank)

A

histidine side chains; 6.5

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32
Q

Proteins act as (blank) and are in high concentration in the blod

A

buffers

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33
Q

(blank) is the most plentiful plasma protein.

A

albumin

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34
Q

(blank) is an important buffer in the renal tubular filtrate

A

Phosphate

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35
Q

the functional ionization in the blood has a pKa of what?

A

6.8

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36
Q

What do all buffers have in common?

A

weak acid dissociates to conjugate base and a proton

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37
Q

Which kind of buffers mitigate pH changes due to changes in volatile acid (CO2)?

A

non-volatile buffers (i.e bicarb cannot do this)

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38
Q

Can buffers, buffer endogenous acids?

A

yes

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39
Q

What is the main source of CO2?

A

aerobic respiration in mitochondria releases CO2 via the Kreb’s cycle

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40
Q

What is the most powerful buffer of ECF?

A

bicarbonate buffer (has high buffering capacity but does not buffer CO2)

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41
Q

How many reactions take place within the bicarbonate buffer system?

A

2 (dissolves CO2, doesnt buffer it)

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42
Q

Pressures of all gases in air add up to the (blank)

A

barometric pressure

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43
Q

What is the partial pressure of air in reno?

A

680 mmHg

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44
Q

partial pressure depends upon (blank)

A

altitude

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45
Q

Pressure units are (blank) units

A

concentration

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46
Q

What is the ideal gas law equation?

A

PV=nRT (gives you absolute concentration)

47
Q

(blank) law states that in a mixture of gases, the pressure exerted by any one gas is proportional to the fraction of the total number of molecules accounted for by that gas.

A

Dalton’s law (partial pressure)

48
Q

(blank) is the pressure that the gas would have if it alone occupied the volume.

A

partial pressure

49
Q

In a gas, the relative concentration is simply the (blank)

A

partial pressure

50
Q

What is the standard Pa at sea level?

A

760 mm Hg

51
Q

(blank) is so low that it is clinically considered zero.

A

PCO2

52
Q

What is the PO2 in reno? normally?

A

143, 159

53
Q

(blank) is the partial pressure of the gas above the liquid.

A

Pgas

54
Q

The (blank) of a gas dissolved in a liquid is the partial pressure of that gas which would be genereated in a gas phase in equilibrium with the liquid.

A

partial pressure

55
Q

WHy dont you see CO2 bubbles in blood or in a sealed soda?

A

because it is in equilibrium

56
Q

In an unopened bottle of soda water, the partial pressure of the gas above the liquid is (blank)

A

the same as in the liquid

57
Q

Gases always travel (blank) partial pressure gradients between biological compartments

A

down

58
Q

Gases may or may not travel (blank) concentration gradients.

A

down

59
Q

which is more important in pulmonary medicine, pressure or concentrations?

A

pressure!!!

60
Q

(blank) law quantifies how much gas dissolves in a liquid

A

henrys law (P X Kh=C)

61
Q

Use (blanks) law to determine how much gas is dissolved in the blood

A

henry’s

62
Q

Henrys constant (Kh) is also called thes olutbility coeffecient and is different for every (blank) an is (blank) dependent.

A

gas, temperature

63
Q

What is the standard PCO2?

A

0.23 mm Hg

64
Q

What is the standard PaCO2?

A

35-45 mmHg ~40 mm Hg

65
Q

(blank) percent of O2 is consumed by the body?

A

4%

66
Q

Henry’s constant gives you the (blank) at equilibrium

A

concentration

67
Q

If you hold the PaCO2 constant, you will be able to maintain what?

A

Steady-state

68
Q

What is the equilbrium dissociation/ henderson eqn?

A

K acid (dissociation constant)= (hydrogen ions X bicarbonate)/(CO2)

69
Q

With the bicarb buffer; when HCO3/CO2 equals 1 then Kacid is equal to (blank)

A

Hydrogen ion concentration

70
Q

What is the normal Hydrogen ion concentration? What is the normal HCO3-? What is the normal PaCO2?

A

40 nM
24 nM
40 nM

71
Q

When using the henderson equation and you get the concentration of the Hydrogen ions, what do you have to do next to determine the pH off of that concentration?

A

you must remember that the Hydrogen ion concentration is in nanomolars so times that concentration by 10 ^-9 and take th e neftaive log of that number

72
Q

When the equilibrium concentrations of PaCO2 and HCO3- are known, you can calculate the (blank)

A

[H+].

73
Q

Clinically significant deviations from the normal pH correspond to a (blank)-fold changes in hydrogen ion concentrations

A

2

74
Q

The solubility coefficient of CO2, in water at 37 C is (blank).

A

.03 mM/mm Hg

75
Q

Normal (hco3-/co2) ratio is (blank)

A

20

76
Q

If you have hyperventilation what happens to your henderson’s equation?

A

your Co2 will go down which makes log term go up and pH goes up

77
Q

If you have hypoventilation, what happens to your henderson’s equation?

A

ratio goes down,your log term goes down and your pH will go down

78
Q

How is a buffer with a pKa of 6.1 physiologically important in the maintenance of the normal plasma pH of 7.4?

A

total concentration of buffer is high and the system is a cheater (gets rid of acid and adds base when you are not looking)

79
Q

(blank) is open to the atmosphere due to breathing

A

bicarbonate system

80
Q

(blank) do act as buffers in response to changes in CO2

A

Non-volatile buffers

81
Q

When you are hypoventilating it shifts the equation to the right, what does hemoglobin do now?

A

hemoglobing sucks up the h+ and acts as a buffer and increases the pH

82
Q

shift in equilibrium (blank) buffering.

A

does not equal

83
Q

Which buffer system is used in metabolic acid production (MAP) and gastrointestinal acid production (GAP)?

A

Bicarbonate system (volatile)

84
Q

What are the 2 main processes that acidify the body?

A

metabolism produces CO2 and endogenous acid production

85
Q

When metabolism produces CO2 does it produce or consume bicarbonate?

A

it produces

86
Q

What is considered all other acidifying processes other than CO2 production?

A

EAP

87
Q

(blank) is all Strong acids (from body perspective) MAP and GAP and consumes bicarbonate.

A

endogenous acid production (EAP)

88
Q

carbs and lipids have a (blank) effect

A

net acidifying

89
Q

(blank) have a net acidifying effect and is the major source of metabolic acid production. Higher % on average of cationic and sulfur-containing amino acids. Amino acid back bone has no effect.

A

proteins

90
Q

Organic anions found in fruits and vegetables (potassium salts of acids) have a net (blank) effect

A

alkanizing

91
Q

Organic acids are (blank) from the body’s persepctive

A

strong acids

92
Q

different (blank) produce different amounts of metabolic acids

A

diets

93
Q

Non-industrialized diets (lots of fruits and veggies) results in lower rates of (blank)

A

metabolic acid production

94
Q

Industrialized diets (high in meat and eggs, low in fruits and veggies) results in higher rates of (blank)

A

metabolic acid production

95
Q

Often hospitalized patients have (blank) acid production

A

high metabolic

96
Q

You have a big production of metabolic (non volatile) acid but an even bigger production of (blank) (volatile).

A

CO2

97
Q

What is this:

  • Acid secreted by the gut into the blood
  • Consumes bicarbonate
  • Bicarbonate system serves as the buffer for this type of acid load
A

Gastrointestinal acid production (GAP)

98
Q

Although the gut secretes both acids and bases into the blood, on average more acid is secreted than base, so there is a net (blank) effect.

A

acidifying

99
Q

(blank) can separate HCO3- from H+

Where the H+ go depends upon where in the gut

A

Gut cells

100
Q

On balance the gut secretes slightly more (blank) into the blood than HCO3-.These H+ must be buffered by plasma bicarbonate buffering system, thus consuming HCO3-. Therefore the (blank) is buffering this type of acid production

A

H+

bicarbonate buffer system

101
Q

EAP is made up of what?

A

2/3 MAP and 1/3 GAP

i.e. EAP=MAP + GAP

102
Q

If lungs and kidney function are normal, body can maintain system pH because…..

A

Using the bicarbonate system and blowing off CO2

Adding bicarbonate back to the blood from the kidneys

103
Q

What does vomiting cause?

A

alkalosis

104
Q

What does diarrhea cause?

A

acidosis

105
Q

(blank) puts acid into the blood.
Therefore HCO3 is consume and slight increase in acidity, (blank) allows these levels to return to normal while consuming HCO3 (so they start to deplete). (blank) then adds more HCO3 to blood. THese levels are topped off so system homestasis is achieved.

A

EAP
alveolar ventilation
Kidney

106
Q

(blank) eats away at body bicarbonate

A

EAP

107
Q

Whose job is it to replace the bicarbonate?

A

the kidney

108
Q

What is this:

bicarbonate passes through the glomeruli into the tubular fluid in the nephron.

A

bicarbonate filtration

109
Q

What is this:

filtered bicarbonate is actively returned to the blood to make sure that plasma HCO3 does not fall.

A

bicarbonate reabsorption

110
Q

What is this:

new bicarbonate is made to replace that used to buffer endogenous acids. (ammonium excretion, titratable acid excretion)

A

bicarbonate regeneration (acid excretion)

111
Q

Which of the following has the highest PCO2 in the normal human?
inspired air, expired air, alveolar air, venous blood, arterial blood

A

venous blood

112
Q

Which of the following has the lowest PCO2 in the normal human?
inspired air, expired air, alveolar air, venous blood, arterial blood

A

inspired air

113
Q

Which is the buffer system with the highest capacity to mitigate pH changes in the blood due to endogenous acid production?

A

bicarbonate system (cuz open system and high concentration)

114
Q

What is the fraction of O2 in air at any altitude?

A

.21

Block 2 Week 6 (6 decks)

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