Box 1 ( EVERYDAY)

Question 1

a substance that can yield a hydrogen ion

(H+) or hydronium ion (H30+)when dissolved in water

Answer 1

Acid

Question 2

a substance that can yield hydroxyl ions (OH-)

Answer 2

Base

Question 3

defined as the negative log of the ionization constant, is also the pH in which the protonated and unprotonated forms are present in equal concentrations.
measures the strength of an acid in solution. Also known as the “acid dissociation constant”.

Answer 3

pKa

Question 4

Pk values < 3

Answer 4

Strong acids

Question 5

Pk values >9

Answer 5

Strong bases

Question 6

For acids, raising the pH

above the pK will cause _____.

Answer 6

will cause the acid to dissociate and yield

an H+.

Question 7

For bases, lowering the pH below the pK will cause_____.

Answer 7

will cause the base to release OH+.

Question 8

the combination of a weak acid or weak

base and its salt, is a system that resists changes in pH.

Answer 8

Buffer

Question 9

effectiveness of a buffer depends on the _____ and the in ___________.
.

Answer 9

on the pK of the

buffering system , pH of the environment which it is placed

Question 10

has pK of 6.1, and is one of the principal

buffers in the plasma

Answer 10

bicarbonate–carbonic

Question 11

A scale used to measure the acidity or basicity of an aqueous solution.

Answer 11

pH

Question 12

pH < 7

Answer 12

acid

Question 13

pH > 7

Answer 13

base

Question 14

reference value for blood plasma pH is _____

Answer 14

7.40

Question 15

an increase in H+ concentration

____ the pH

Answer 15

decreases

Question 16

decrease in H+

concentration _____ the pH

Answer 16

increases

Question 17

normal pH of H+ in the extracellular body fluid ranges from ______.

Answer 17

pH 7.34–7.44 (36–44 nmol/L)

Question 18

reference value for arterial blood pH is

Answer 18

7.40

Question 19

below the reference
range (<7.34) is referred to as ____ , whereas a
pH above the reference range (>7.44) is referred to as
______.

Answer 19

acidosis , alkalosis

Question 20

Three reasons why bicarbonate-carbonic acid system is still an important buffer in the system.

Answer 20

(1) H2CO3 dissociates into CO2 and H2O,
allowing CO2 to be eliminated by the lungs and H as
water; (2) changes in CO2 modify the ventilation (respiratory)
rate; and (3) HCO3-concentration can be altered
by the kidneys.

Question 21

Partial pressure of oxygen

Answer 21

pO2

Question 22

Reference value pO2

Answer 22

81 - 100 mmHg

Question 23

Mild hypoxemia

Answer 23

61 - 80 mmHg

Question 24

Moderate hypoxemia:

Answer 24

41 – 60 mmHg

Question 25

Severe hypoxemia:

Answer 25

<41 mmHg

Question 26

Partial pressure of carbon dioxide.

Answer 26

pCO2

Question 27

Reference value pCO2:

Answer 27

35 – 45 mmHg

Question 28

Respiratory alkalosis:

Answer 28

<35 mmHg

Question 29

Respiratory acidosis: pCO2

Answer 29

>45 mmHg

Question 30

its salt or conjugate base for the bicarbonate–carbonic acid buffer system

Answer 30

bicarbonate | HCO3-

Question 31

weak acid of bicarbonate–carbonic acid buffer system

Answer 31

carbonic acid (H2CO3)

Question 32

When an acid is added to the bicarbonate–carbonic acid system, the HCO3- will combine with the H+ from the acid to form _____.

Answer 32

H2CO3

Question 33

When a base is added, H2CO3 will combine with the OH group to form____.

Answer 33

H2O and HCO3

Question 34

Conjugate base of bicarbonate-carbonic acid. 20:1 ratio with H2CO3

Answer 34

HCO3–

Question 35

Reference value of HCO3-:

Answer 35

21 – 28 mEq/L

Question 36

Metabolic alkalosis:

Answer 36

>28 mEq/L

Question 37

Metabolic acidosis:

Answer 37

<21 mEq/L

Question 38

1:20 ratio with HCO3

Answer 38

Bicarbonate

Question 39

reference value of H2CO3

Answer 39

1.05 - 1.4 mEq/L

Question 40

CO2 excess.

Answer 40

RESPIRATORY ACIDOSIS

Question 41

Compensated by the kidneys (↑ HCO3– against ↑ pCO2 and pH < 7.35)

Answer 41

RESPIRATORY ACIDOSIS

Question 42

CO2 deficit.

Answer 42

RESPIRATORY ALKALOSIS

Question 43

Compensated by the kidneys (↓ HCO3– against ↓ pCO2 and pH > 7.45)

Answer 43

RESPIRATORY ALKALOSIS

Question 44

HCO3– deficit.

Answer 44

METABOLIC ACIDOSIS

Question 45

Observed in COPD, myasthenia gravis, CNS diseases, drug overdose, botulism, stroke, myxedema, and pneumonia.

Answer 45

RESPIRATORY ACIDOSIS

Question 46

Observed during anxiety, severe pain, aspirin/salicylate overdose, hepatic cirrhosis, Gram (-) sepsis, progesterone drugs intake.

Answer 46

RESPIRATORY ALKALOSIS

Question 47

Observed in diabetic ketoacidosis, lactic acidosis, renal failure, and diarrhea.

Answer 47

METABOLIC ACIDOSIS

Question 48

Compensated by the lungs (↓ pCO2 against ↓ HCO3– and pH < 7.35)

Answer 48

METABOLIC ACIDOSIS

Question 49

HCO3– excess.

Answer 49

METABOLIC ALKALOSIS

Question 50

Observed in vomiting (chloride loss).

Answer 50

METABOLIC ALKALOSIS

Question 51

Compensated by the lungs (↑ pCO2 against ↑ HCO3– and pH > 7.45)

Answer 51

METABOLIC ALKALOSIS

Question 52

Most severe. Inappropriate compensation. The blood pH determines the dominant disorder.

Answer 52

MIXED ACID-BASE DISORDER

Question 53

an important factor in maintaining the normal biological processes of an organism

Answer 53

Blood pH

Question 54

Anticoagulant to use is_____ grams of _____ per ml of blood.

Answer 54

0.05 , dry heparin

Question 55

Use syringe and needle and must be _____ prior to blood collection.

Answer 55

pre-heparinized

Question 56

Upon completion of the draw, ______.

Answer 56

remove the trapped air .

Question 57

Arterial blood has _____,_____ , and slightly basic than venous blood (-0.03).

Answer 57

>pO2 ,

Question 58

Common pre-analytical errors

Answer 58

form and concentration of heparin, speed of syringe filling, air exposure, mixing of samples, collection device, pre-analytical storage/transport time. Specimen exposed to air loses pCO2

Question 59

Common analytical errors

Answer 59

temperature and protein coating of electrodes.

Question 60

Gasometers for BGA

Answer 60

Van Slyke manometer Natelson gasometer

Question 61

measures pCO2 and pO2

Answer 61

Van Slyke manometer

Question 62

Natelson gasometer utilizes ____??

Answer 62

1. mercury - produces vacuum 2. caprylic alcohol – anti-foam agent 3. lactic acid – counteracts presence of pyruvate/lactate 4. NaOH and NaHSO3 – buffer system

Question 63

Electrodes

Answer 63

pH (potentiometry) pO2 – Clark electrode (polarography-amperometry) pCO2 – Severinghaus electrode (potentiometer)

Question 64

measure the amount of current flow in a circuit that is related to the amount of O2 being reduced at the cathode.

Answer 64

Clarke electrodes

Question 65

Formula for acid base balance

Answer 65

pH = pKa + log ([A-]/[HA])

Question 66

pKa = ____

Answer 66

6.1, dissociation constant for CO2

Question 67

A- = ____

Answer 67

concentration of HCO3–

Question 68

HA = ______

Answer 68

concentration of H2CO3

Question 69

AG = (Na+ + K+) - (Cl- + HCO3-)

Answer 69

Indicator if acidosis is due to increased acid accumulation or bicarbonate loss. May also indicate presence of mixed acid-base disorder.Reference value: 3 – 11 mEq/L

Question 70

Correction by changes in temperature: Normal temperature is 37°C, each exceeding degree, decrease _____ and _______.

Answer 70

pO2 by 7%, increase pCO2 by 3%

Question 71

Normal arterial blood pH =

Answer 71

7.35 – 7.45

Question 72

Increase in pCO2= ____ in pH

Answer 72

Decrease

Question 73

Decrease in pCO2=____ in pH

Answer 73

Increase

Question 74

The relation of pCO2 and pH is _____

Answer 74

Indirectly proportional

Question 75

The relation of pO2 and pH is _____

Answer 75

Directly proportional

Question 76

20:1 ratio to Bicarbonate

Answer 76

Carbonic acid