BLOOD GASES PH

Question 1

• A substance that can donate hydrogen ions (H+ ) when dissolved in water.

Answer 1

Acid

Question 2

Bronsted-Lowry Acid (Proton Donor )

A species that donates protons

Answer 2

Acid

Question 3

A substance that can yield hydroxyl ions (OH-) when dissolved in water

Answer 3

Base

Question 4

Bronsted-Lowry Base (Proton Acceptor)
• A species that accept protons

Answer 4

Base

Question 5

• The relative strengths of acids and bases, their ability to dissociate in water.

Answer 5

Dissociation Constant (Ka).

Question 6

The ratio of dissociated ion to the original acid

Answer 6

Dissociation Constant (Ka).

Question 7

pH at which protonated and unprotonated species are present in equal concentrations.

Answer 7

pKa

Question 8

defined as the negative log of the dissociation constant.

Answer 8

pKa

Question 9

• Have pK values of less than 3.0

Answer 9

Strong Acids

Question 10

• Raising the pH above the pK will cause it to dissociate and yield a H+

• Complete dissociates in a solution

Answer 10

Strong Acids

Question 11

• Have pK values greater than 9.0

Answer 11

Strong Bases

Question 12

• Lowering the pH below the pK will cause it to release OH

• Completely dissociates in a solution

Answer 12

Strong Bases

Question 13

• Are species that partially/ incompletely dissociate in a solution

Answer 13

Weak Acids/ Bases

Question 14

• consists of a weak acid and a salt of its conjugate base

Answer 14

Buffer

Question 15

it resists the change in pH upon adding acid or base.

Answer 15

Buffer

Question 16

• Pressure or tension exerted by CO2 gas dissolved in blood.
• An index of efficiency of gas exchange in the lungs
• Not a measure of CO2 concentration in the blood

Answer 16

Partial Pressure of CO2 (pCO2)

Question 17

Partial Pressure of CO2 (pCO2)

Reference Range:

Answer 17

35-45 mm Hg

Question 18

When we say______ that is the pressure exerted by the gas in the blood and does not mean the concentration of the gas in the blood

Answer 18

partial pressure

Question 19

• Total CO2 Content (tCO2)
• Refers to the total concentration of CO2 in the blood

Answer 19

Total Carbon Dioxide Concentration

Question 20

• Consisting of lonized (HCO3-, CO3-, Carbamino compound) and unionized fraction (H2CO3)
• 23 - 27 mmol/L

Answer 20

Total Carbon Dioxide Concentration

Question 21

• The bicarbonate ion concentration in the blood has been equilibrated with CO2 at 40 mm Hg at 37 degree Celsius

Answer 21

Bicarbonate lon Concentration

Question 22

Main samples used in blood gas is arterial blood
Reference Range:_____ mmol/L
It can be calculated through
_________

Answer 22

22-26mmol/ L

Henderson Hasselbalch equation

Question 23

• The pressure or tension exerted by oxygen gas dissolved in arterial blood which reflects the availability of the gas in blood but not its content

• 80 - 110 mm Hg

Answer 23

Partial Pressure of Oxygen (pO2)

Question 24

• A collection of chemical compounds and reactions in the body that help maintain the pH level of the blood and other bodily fluids within a narrow and optimal range.

The pH level is a measure of the acidity or basicity of a solution, and maintaining the proper pH is essential for many biological processes to function properly.

Answer 24

BUFFER SYSTEMS

Question 25

The____ together with the____ provide the first line of defense to change the acid-base status.

Answer 25

lungs buffer systems

Question 26

So for the extracellular fluid the main buffer system is the carbonic acid- bicarbonate buffer system Remember when cells metabolize they release______ as a waste product Now this carbon dioxide will combine with water to form______

Answer 26

carbon dioxide carbonic acid

Question 27

Since carbonic acid is an unstable molecule so it immediately dissociates into hydrogen and bicarbonate ions which is accelerated by the enzyme _________

Answer 27

Carbonic Anhydrase

Question 28

_______ ions accumulate in the blood, to avoid a pH change, so chloride ions will go inside the cell to maintain electroneutrality.

Answer 28

Bicarbonate

Question 29

• Why does chloride need to go inside the cell? Remember bicarbonate and chloride ions bear a net negative charge. So if both anions are accumulating in the blood there will be an electrolyte imbalance. To fix this chloride ions will enter the cell in an even known as_______

Answer 29

Chloride Shift

Question 30

pH ↑ H+ — ↓ Blood pH

Answer 30

Acidic

Question 31

pH ↓ H+ — ↑ Blood pH

Answer 31

Alkaline

Question 32

• <7.35 = • >7.45 =

Answer 32

acidosis alkalosis

Question 33

•_____ – process in the body

Answer 33

-osis

Question 34

– state in blood

Answer 34

-emia

Question 35

Bicarbonate-Carbonic Acid System ↓ HCO3- ↓ Blood pH

Answer 35

(Directly proportional) Acidic

Question 36

Bicarbonate-Carbonic Acid System ↑ HCO3- ↑ Blood pH

Answer 36

Alkaline

Question 37

Buffer sustems occur in

Answer 37

Intracellular fluid Extracellular fluid

Question 38

Buffer system Intracellular fluid

Answer 38

Phosphate buffer system Protein buffer systems

Question 39

Buffer system Extracellular fluid

Answer 39

Protein buffer systems Carbonic acid-bicarbonate buffer system

Question 40

Protein buffer systems

Answer 40

Hemoglobin buffer system Amino acid buffer system Plasma protein buffers

Question 41

The main site for retaining bicarbonate is in the

Answer 41

Proximal Convoluted Tubule

Question 42

Respiratory component

Answer 42

CO2 - lungs

Question 43

Metabolic component

Answer 43

Kidneys - bicarbonate

Question 44

Bicarbonate-Carbonic Acid System ↓ HCO3- ↓ Blood pH

Answer 44

Acidic

Question 45

Bicarbonate-Carbonic Acid System ↑ HCO3- ↑ Blood pH

Answer 45

Alkaline

Question 46

Maintenance of H+ • Normal:

Answer 46

36 – 44 nmol/L (pH 7.34 – 7.44)

Question 47

Maintenance of H+ • Through metabolism, the body produces much greater quantities of_____ • The body controls and excretes H+ in order to maintain______ (lungs and kidneys)

Answer 47

H+ pH homeostasis

Question 48

Maintenance of H+ • Increase ____ will cause alterations in the rates of chemical reactions within the cell and affect the many metabolic processes of the body • Can lead to alterations in consciousness, neuromuscular irritability, tetany, coma, and death

Answer 48

H+

Question 49

Henderson-Hasselbalch Equation • [A-] = • [HA] = • pK’ =

Answer 49

proton acceptor (HCO3 - ) proton donor or weak acid (H2 CO3 ) pH at which there is an equal concentration of protonated and unprotonated species

Question 50

= pK’ of HCO3-

Answer 50

6.1

Question 51

= the value for the combination of the solubility constant for pCO 2 and the factor to convert mm Hg to mmol/L

Answer 51

0.0307 mmol/L/mm Hg

Question 52

= equilibrium between H2 CO 3 and CO 2 in plasma

Answer 52

1:800

Question 53

= proportional to the pCO2

Answer 53

cH2CO 3

Question 54

are measured in blood gas analysis

Answer 54

pH and pCO 2