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Clinical chemistry > Box 1 ( EVERYDAY) > Flashcards

Box 1 ( EVERYDAY) Flashcards

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1
Q

a substance that can yield a hydrogen ion

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

A

Acid

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2
Q

a substance that can yield hydroxyl ions (OH-)

A

Base

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3
Q

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”.

A

pKa

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4
Q

Pk values < 3

A

Strong acids

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5
Q

Pk values >9

A

Strong bases

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6
Q

For acids, raising the pH

above the pK will cause _____.

A

will cause the acid to dissociate and yield

an H+.

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7
Q

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

A

will cause the base to release OH+.

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8
Q

the combination of a weak acid or weak

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

A

Buffer

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9
Q

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

A

on the pK of the

buffering system , pH of the environment which it is placed

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10
Q

has pK of 6.1, and is one of the principal

buffers in the plasma

A

bicarbonate–carbonic

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11
Q

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

A

pH

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12
Q

pH < 7

A

acid

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13
Q

pH > 7

A

base

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14
Q

reference value for blood plasma pH is _____

A

7.40

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15
Q

an increase in H+ concentration

____ the pH

A

decreases

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16
Q

decrease in H+

concentration _____ the pH

A

increases

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17
Q

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

A

pH 7.34–7.44 (36–44 nmol/L)

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18
Q

reference value for arterial blood pH is

A

7.40

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19
Q

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

A

acidosis , alkalosis

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20
Q

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

A

(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.

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21
Q

Partial pressure of oxygen

A

pO2

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22
Q

Reference value pO2

A

81 - 100 mmHg

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23
Q

Mild hypoxemia

A

61 - 80 mmHg

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24
Q

Moderate hypoxemia:

A

41 – 60 mmHg

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25
Q

Severe hypoxemia:

A

<41 mmHg

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26
Q

Partial pressure of carbon dioxide.

A

pCO2

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27
Q

Reference value pCO2:

A

35 – 45 mmHg

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28
Q

Respiratory alkalosis:

A

<35 mmHg

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29
Q

Respiratory acidosis: pCO2

A

> 45 mmHg

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30
Q

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

A

bicarbonate

HCO3-

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31
Q

weak acid of bicarbonate–carbonic acid buffer system

A

carbonic acid (H2CO3)

32
Q

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

A

H2CO3

33
Q

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

A

H2O and HCO3

34
Q

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

A

HCO3–

35
Q

Reference value of HCO3-:

A

21 – 28 mEq/L

36
Q

Metabolic alkalosis:

A

> 28 mEq/L

37
Q

Metabolic acidosis:

A

<21 mEq/L

38
Q

1:20 ratio with HCO3

A

Bicarbonate

39
Q

reference value of H2CO3

A

1.05 - 1.4 mEq/L

40
Q

CO2 excess.

A

RESPIRATORY ACIDOSIS

41
Q

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

A

RESPIRATORY ACIDOSIS

42
Q

CO2 deficit.

A

RESPIRATORY ALKALOSIS

43
Q

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

A

RESPIRATORY ALKALOSIS

44
Q

HCO3– deficit.

A

METABOLIC ACIDOSIS

45
Q

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

A

RESPIRATORY ACIDOSIS

46
Q

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

A

RESPIRATORY ALKALOSIS

47
Q

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

A

METABOLIC ACIDOSIS

48
Q

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

A

METABOLIC ACIDOSIS

49
Q

HCO3– excess.

A

METABOLIC ALKALOSIS

50
Q

Observed in vomiting (chloride loss).

A

METABOLIC ALKALOSIS

51
Q

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

A

METABOLIC ALKALOSIS

52
Q

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

A

MIXED ACID-BASE DISORDER

53
Q

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

A

Blood pH

54
Q

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

A

0.05 , dry heparin

55
Q

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

A

pre-heparinized

56
Q

Upon completion of the draw, ______.

A

remove the trapped air .

57
Q

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

A

> pO2 ,

58
Q

Common pre-analytical errors

A

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

59
Q

Common analytical errors

A

temperature and protein coating of electrodes.

60
Q

Gasometers for BGA

A

Van Slyke manometer Natelson gasometer

61
Q

measures pCO2 and pO2

A

Van Slyke manometer

62
Q

Natelson gasometer utilizes ____??

A
  1. mercury - produces vacuum
  2. caprylic alcohol – anti-foam agent
  3. lactic acid – counteracts presence of pyruvate/lactate
  4. NaOH and NaHSO3 – buffer system
63
Q

Electrodes

A

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

64
Q

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

A

Clarke electrodes

65
Q

Formula for acid base balance

A

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

66
Q

pKa = ____

A

6.1, dissociation constant for CO2

67
Q

A- = ____

A

concentration of HCO3–

68
Q

HA = ______

A

concentration of H2CO3

69
Q

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

A

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

70
Q

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

A

pO2 by 7%, increase pCO2 by 3%

71
Q

Normal arterial blood pH =

A

7.35 – 7.45

72
Q

Increase in pCO2= ____ in pH

A

Decrease

73
Q

Decrease in pCO2=____ in pH

A

Increase

74
Q

The relation of pCO2 and pH is _____

A

Indirectly proportional

75
Q

The relation of pO2 and pH is _____

A

Directly proportional

76
Q

20:1 ratio to Bicarbonate

A

Carbonic acid

Clinical chemistry (5 decks)

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