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Block 2 Exam 3 > Cremo 1: Fundamentals of body buffers and gases > Flashcards

Cremo 1: Fundamentals of body buffers and gases Flashcards

1
Q

What is the concentration of H+ ions in a healthy individual?

A

35 and 45 nM

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2
Q

Normal range for pH

A

7.35-7.45

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3
Q

Acid production originates intracellularly. What is the average intracellular pH?

A

7

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4
Q

Non bicarbonate buffers

A

hemoglobin
plasma proteins
phosphates

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5
Q

This has the highest buffer capacity of non-volatile buffers

A

hemoglobin

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6
Q

What two things does buffering capacity depend on?

A
  1. concentration of the buffer

2. PKA (how close is the PKA to 7.4?)

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7
Q

Hemoglobin has abundant (blank) side chains, therefore it has a PKA of about (blank)

A

histidine; 6.5

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8
Q

Plasma proteins have about (blank) percent of the buffering capacity of Hb

A

20%

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9
Q

The most plentiful plasma protein

A

Albumin

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10
Q

An important buffer in the renal tubular filtrate

A

Phosphate

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11
Q

List the non-bicarbonate (non-volatile) buffers in order of buffering capacity

A
  1. hemoglobin
  2. plasma proteins
  3. phosphate
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12
Q

What is the most important function of the non-volatile buffers?

A

Mitigate pH changes due to changes in volatile acid (CO2)

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13
Q

Can the bicarbonate system mitigate changes in the levels of CO2?

A

No! Non-volatile buffers are the only ones that can do this.

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14
Q

Most powerful buffer of the ECF

A

Bicarbonate buffer system

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15
Q

Atmospheric pressure

A

760mmHg

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16
Q

Total of partial pressures (barometric pressure) at sea level? Total of partial pressure in Reno?

A

760mmHg; 680mmHg

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17
Q

Partial pressure of CO2.

A

0.23mmHg

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18
Q

Clinical PCO2

A

Zero (0.23 at sea level)

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19
Q

PO2 at sea level? In Reno?

A

159mmHg; 143mmHg

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20
Q

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

A

the same as the liquid.

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21
Q

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

A

in equilibrium

22
Q

Gases always travel down (blank) gradients, but may or may not travel down (blank) gradients.

A

partial pressure gradients; concentration gradients

23
Q

What does Henry’s law quantify?

A

How much gas is dissolved in a liquid

24
Q

What’s the formula for Henry’s law?

A

P•KH = C = Concentration

Where KH is different for each gas.

25
Q

At equilibrium, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

A

Henry’s law

26
Q

K acid equation for the bicarbonate buffer system

A

K = ([H+][HCO3-])/CO2

27
Q

Simplified bicarbonate buffer system

A

CO2 H+ + HCO3-

28
Q

Normal concentration of bicarbonate in the body in a healthy individual

A

24mM

29
Q

In a healthy individual, the ratio of bicarbonate to CO2 is…

A

20

30
Q

The Henderson equation

A

Kacid = ([H+][HCO3-])/PaCO2

31
Q

Normal [H+] concentration
Normal [HCO3-] concentration
Normal PaCO2

A

40nM
24mM
40mmHg

32
Q

When a sample of whole blood is exposed to an increased PCO2, what will happen?

A

This will shift the equilibrium to the right, increasing H+ and HCO3-

33
Q

Henderson Hasselbalch Equation for clinical use

A

pH = 6.1 + log [HCO3-]/(0.3*PaCO2)

34
Q

Rearranged Henderson equation to solve for [H+]

A

(24 * PaCO2)/HCO3- = [H+]

35
Q

The bicarbonate system is open to the atmosphere, so it allows for the removal of (blank) to give effective buffering even though the PKA of 6.1 is far from 7.4

A

CO2

36
Q

What kind of buffers responds to changes in CO2?

A

Non-volatile buffers, like hemoglobin

37
Q

Describe what happens when Hb is present during hypoventilation.

A

During hypoventilation, there is an increase in the PCO2, so the system produces more H+ and more HCO3-. Hb can act as a buffer by pulling out some of the H+ to make HbH+.

38
Q

Is a shift in equilibrium equal to a buffering effect?

A

No!

39
Q

Two main processes that acidify the body

A
  1. Metabolism produces CO2

2. Endogenous acid production

40
Q

Does metabolism consume bicarbonate? Does endogenous acid production consume bicarbonate?

A

No; Yes

41
Q

Major source of metabolic acid production

A

Eating protein

42
Q

Industrialized diets (high in meat and eggs) have (blank) rates of metabolic acid production, while non-industrialized diets (more fruits and veggies) have (blank) rates of metabolic acid production.

A

high; low

43
Q

Compare the daily production of CO2 to the daily production of metabolic acid

A

Daily CO2»»metabolic acid

Volatile acid is about 100 times that of non-volatile.

44
Q

Acid secreted by the gut into the blood

A

Gastrointestinal acid production

45
Q

Does GAP consume bicarbonate?

A

yes

46
Q

(blank) serves as a buffer for gastrointestinal acid production

A

Bicarbonate system

47
Q

In the upper gut, (blank) enters the lumen of the gut, while (blank) is pushed out into the bloodstream. In the lower gut, (blank) enters the lumen of the gut and (blank) is pushed out into the bloodstream.

A

H+, HCO3-

HCO3-, H+

48
Q

On balance, the gut secretes slightly more (blank) into the blood stream than (blank)

A

H+ ; HCO3-

49
Q

Endogenous acid production equation

A

EAP = MAP + GAP

50
Q

Prolonged vomiting can lead to metabolic (blank), while diarrhea can lead to prolonged metabolic (blank).

A

alkalosis; acidosis

51
Q

Vomiting causes (blank) to leave the stomach lumen, and (blank) to enter the blood.

A

H+ ; bicarbonate

52
Q

Diarrhea causes (blank) to leave the stomach lumen, and (blank) to enter the blood.

A

bicarbonate; H+

Block 2 Exam 3 (19 decks)

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