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pH & CO2 quiz prep > pH & CO2 quiz prep > Flashcards

pH & CO2 quiz prep Flashcards

1
Q

What catalyst speeds of the reaction of the hydrolysis equation?

A

Carbonic Anyhydrase

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2
Q

What is the Hydrolysis equation?

A

CO2 + H2O = H2CO3 = H+ + HCO3-

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3
Q

What is the pH range compatible with life?

A

6.80 - 7.80

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4
Q

What is the normal pH scale?

A

0-14

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5
Q

When you increase H+ what effect does it have on pH? Increase or decrease?

A

Increase

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6
Q

What is the ratio of Bicarb to pH balance?

A

1:20

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7
Q

How much acid does body produce each day during normal function?

A

13,050 mEq/l of acid is produced each day

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8
Q

Name the 2 ways that the body deals with the acid it produces?

A

Acid excretion via lungs or kidneys

Acid Buffering

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9
Q

How much acid does the lungs excrete each day?

A

13,000 mEq/L

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10
Q

What is H+Cl?

A

Hydrochloric Acid–this is a strong acid

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11
Q

What is H2CO3?

A

Carbonic Acid–this is a weak acid

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12
Q

What is the formula to compute pH?

A

pH= - log [H+]

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13
Q

Name the two ways O2 is carried in the blood?

A

Dissolved (PaO2- partial pressure of O2 dissolved in arterial blood)
Combined (SaO2) = oxygen saturation of arterial Hb & combined O2

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14
Q

Which value for oxygenation is directly measured so is more reliable? PaO2 or SaO2

A

PaO2

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15
Q

This acid is a by-product of the Kreb’s cycle?

A

Lactic Acid

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16
Q

What is the definition of pH?

A

Measurement of the acidity or alkalinity of a substance

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17
Q 
This law deals with solubility of a substance.  It states that CO2 is much more soluble than O2- Per this law the amount of gas dissolving in liquid is directly proportional to gas partial pressure;  Co2 is 24 x more soluble than CO2;  What is this principle?
A.  Graham's Law
B.  Henderson-Hasselbach
C.  Henry's Law
D.  Haldane Effect
A

C. Henry’s Law

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18
Q 
This law deals with diffusion of a gas through a liquid which is directly proportional to its solubility coefficient & inversely proportional to sq root of its density;  Because O2 is a lighter molecule it diffuses through a gas medium 1.17 times faster than CO2;  What is this principle?
A.  Graham's Law
B.  Henderson-Hasselbach
C.  Henry's Law
D.  Haldane Effect
A

A. Graham’s Law

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19
Q

Hydrogen in chemical combination with other elements is/is not part of the pH measurement?

A

Is Not; Only hydrogen in free ionic form is part of the measurement of free hydrogen ion concentration; therefore, hydrogen in chemical combination with other elements is not part of the free [H+]

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20
Q

What is the pH measurement?

A

pH is a method of assessing the amount of H+ present in a given fluid
-log [H+]

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21
Q

The relationship between pH and [H+] is?
A. Direct
B. Linear
C. Inverse

A

C. Inverse

The relationship is inverse & logarithmic

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22
Q

A large increase in [H+] reflects a ______ change in pH. Doubling the normal [H+] results in _____ change to pH.

A

A large increase in [H+] reflects only slight change in pH; 0.3 change in pH

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23
Q

pH measures activity or concentration of [H+]?

A

Activity; It is the balance of acids & bases at any given moment

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24
Q

Most [H+] are not really free but are combined with ______ to form ______ ions

A

Most [H+] are not really free but are combined with H2O to form hydronium ions.

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25
Q

CNS depression is a clinical manifestation of academic pH; Name 4 signs of this condition.

A 
Drowsiness
Lethargy
Disorientation
Coma
Death
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26
Q

CNS excitability is a clinical manifestation of alkalotic pH; Name the 5 signs of this condition.

A 
Excitability
Irritability
Arrhythmias
Spasms/Tetany
Convulsions
Deatb
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27
Q

What is the ratio of Bicarb to Carbonic Acid

A

1 carbonic acid H2CO3 : 20 Bicarbs HCO3-

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28
Q

What are the two ways that the body deals with acids?

A

Excretion

Buffering

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29
Q

Carbonic Acid is removed in the lungs in the form of what?

A

CO2

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30
Q

What is a volatile acid? Give an example

A

An acid that can be converted from a liquid to a gas; Carbonic acid is an example of a volatile gas

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31
Q

Doubling the normal [H+] results in a (0.03/0.3) increase or decrease in pH?

A

Doubling the normal [H+] results in a 0.3 decrease in pH.

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32
Q

Any chemical substance capable of combing with or accepting a hydrogen ion in solution is called a ?

A

Base

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33
Q

Any chemical substance capable of donating a hydrogen ion is a ?

A

Acid

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34
Q

What are the 2 major organs of acid excretion?

A

Lungs & kidneys

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35
Q

The lungs excrete (volatile/fixed) acids?

A

The lungs excrete volatile acids

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36
Q

The major blood base of clinical significance is?

A

HCO3-

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37
Q

The organs responsible for the regulation of blood bases is the lungs/kidneys?

A

kidneys

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38
Q

Name a weak acid & a strong acid:

A

Weak: CO2
Strong: Hydrochloric acid HCl

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39
Q

A substance that can act either as an acid or base is referred to as? What is an example?

A

amphoteric; Hb can act as either an acid or base in the blood

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40
Q

Which organ removes fixed acids?

A

kidneys

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41
Q

What is a fixed acid?

A

Those that cannot be converted to a gas; this is a normal part of metabolism

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42
Q

What is catabolism?

A

A part of metabolism that involves the breakdown of substances into smaller units & release of energy

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43
Q

What is anabolism?

A

A type of function of metabolism in which involves creation of a larger molecule from a smaller substance. This reaction requires energy

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44
Q

Catabolism of proteins produces what 2 acids?

A

Phosphoric acids & sulfuric acids

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45
Q

Some diseases will produce too much _____ and the kidneys cannot handle them?

A

Fixed acids; they will build up in the body

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46
Q

Renal failure by the mechanism of protein metabolism produces too much?

A

Phosphoric & sulfuric acids

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47
Q

Diabetes by the mechanism of ______ metabolism produces to much _________?

A

Diabetes by the mechanism of incomplete lipid metabolism (fat) produces to much ketoacids (aka acetoacidic or beta-hydroxybutaric acid

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48
Q

Anoxia by the mechanism of _______ metabolism produces too much ________ acid.

A

Anoxia by mechanism of carbohydrate metabolism produces too much lactic acid

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49
Q

_______ soak up acids or neutralize bases minimizing changes in pH.

A

Buffers

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50
Q

Every acid must have a related _____ that is present on dissociation of the hydrogen ion.

A

Base

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51
Q

An acid in conjunction with its associated base is sometimes referred to as a ______.

A

Conjugate base

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52
Q

The conjugate base of H2CO3 is ________, and the conjugate base of HHb is _________.

A

weak acid; salt of the conjugate base of weak acid

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53
Q

What is the conjugate base of this pair: HCl = H+ + Cl-

A

Cl-

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54
Q

Strong acids have a high/low degree of disassociation (many free H+ ions)

A

Strong acids have a high degree of disassociation

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55
Q

Water is a strong/weak acid

A

weak acid

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56
Q

A buffer system converts strong acids to _______ or strong bases to _________ .

A

A buffer system converts strong acids to weak acids or strong bases to weak bases

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57
Q

What releases the most H+ (strong acids or weak acids)?

A

Strong acids

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58
Q

What are the two types of buffer systems the body uses?

A

Bicarb system

Non-Bicarbonate system

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59
Q

A bicarbonate buffer system is made up of __________ acid & ____________

A

A bicarbonate buffer system is made up of a weak acid & the salt of its conjugate base.

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60
Q

List a Bicarbonate buffer:

A

H2CO3/NaHCO3-

61
Q

In a buffer pair if a strong acid is added what happens to the buffer pair, how is it changed?

A

It is changed to a weak acid & a salt

HCL + H2CO3/NaHCO3- = NaCL + H2CO3

62
Q

In general, the stronger the acid the stronger/weaker is its conjugate base.

A

Weaker

63
Q

Deoxygenated/oxygenated hemoglobin most readily picks up hydrogen ions.

A

deoxygenated

64
Q

If a strong base sodium hydroxide NaOH- is added to the system, the buffer system will change to a strong/weak base & _________

A

It will change to a weak base & water

NaOH- + H2CO3/NaHCO3 = NaHCO3 + H2O

65
Q

Metabolic compensation is also known as ?

A

Buffering

66
Q

Which type of acid breaks apart easiest, a strong/weak acid?

A

A strong acid breaks apart easieast

67
Q

Bicarbonate buffering represents how much of the bodies buffering system? what percentage?

A

53%

68
Q

Name 4 other ways the body can buffer? The non-bicarb systems which account for the other 47% of buffering that takes place in the body

A

Hb
Organic Phosphates
Inorganic Phosphates
Plasma proteins

69
Q

The body buffers in both the extra-cellular fluid & intra-cellular fluid; Name the buffering systems in both systems & the percentages.

A

Extra-cellular buffers:
Plasma Bicarbonate = 35%
Plamsa Protein = 7%
Inorganic Phosphates = 1%

Intra-cellular buffers:
Erythrocyte Bicarbonate = 18%
Hb = 35%
Oxyhemoglobin = 1%
Inorganic/organic phosphates 3%
70
Q

The largest extra-cellular buffer is plasma ________ & the largest intra-cellular buffer is _____.

A 
Extra-cellular = plasma bicarbonate
Intra-cellular = Hb
71
Q

What is the most important intra-cellular fluid buffer?

A

Hemoglobin

72
Q

The effectiveness of buffering depends on 3 qualities?

A
  1. pK
  2. Quantity
  3. Open vs. Closed System
73
Q

What is pk?

A

Point at 50% dissociation

74
Q

What is the pk of carbonic acid in the blood?

A

6.1

75
Q

Strong acids are buffered by the dissociated portion of the buffer pair which is?

A

NaHCO3

76
Q

Strong bases are buffered by the undissociated portion which is?

A

H2CO3

77
Q

Which is better for buffering an open or closed system & why?

A

An open system is most effective. In a closed system the buffer becomes less effective as the products of buffering accumulate which is what happens for most blood buffers. Bicarbonate functions in an open system as CO2 does not accumulate. Hb is a closed system

78
Q

What describes the fixed inter-relationship between PCO2, pH, & HCO3-;

A

Henderson-Hasselbach Equation

79
Q

Which do we buffer better, acids or bases & why?

A

We buffer acids better as it is closest to the pk of 6.1

80
Q

What is KA mean

A

Equilibration Constant= this means the equilibration both ways is constant

81
Q

This principle is known as?

The product of the concentrations on the right equals the product of the concentrations on the left

A

The law of mass action

82
Q

Because the concentration of H+ in the blood is very small Henderson resolved this by how?

A

taking the negative log of both sides of an equation

83
Q

What is the formula for KA

A

KA = [H+] [HCO3-] / H2CO3

84
Q

What is the formula for pK?

A

pK = - log KA

85
Q

What does pK represent or why is it important?

A

pk represents the pH at which maximum buffering can be achieved; the pk of bicarbonate & carbonic acid is 6.1

86
Q

Since the amount of carbonic acid is very small we measure what?

A

CO2

87
Q

How is carbonic acid & CO2 related? Directly/indirectly or linearly/logarithmically

A

direct/linearly related

88
Q

In the Henderson Hasselbach equation, carbonic acid concentration is replaced by what?

A

partial pressure of CO2 (which is 40) x the solubility coeffficent (0.03)= 1.2

89
Q

What is the value of bicarb in the Henderson hasselbach equation which is the amt in arterial plasma?

A

24 mEq/L

90
Q

Write the formula for the Henderson Hasselbach equation:

A

pH = pk + log HCO3/H2CO3

91
Q

If HCO3- drops by half & PaCO2 remains the same then ph will?

A

Decrease

92
Q 
A pH of 7.40 means?
a. HCO3- is normal
b.  PaCO2 is normal
C.  The ratio of HCO3- to PaCO2 is normal
D.  All of the above
A

C. The ratio of HCO3- to PaCO2 is normal

93
Q

What is the relationship between CO2 and pH?

Direct/inverse

A

Inverse

94
Q

Where is CO2 measured? intracellular plasma or extracellular plasma

A

Extra-cellular plasma

95
Q

T or F: CO2 is a gas that can move across the cell membrane

A

True

96
Q

What is the equation that regulates CO2?

A

hydrolysis equation

97
Q

T or F: CO2 will be the same in the ICF & ECF

A

True

98
Q

A CO2 greater than 45 is referred to as?

A

Hypoventilation, hypercarbia, hypercapnia

99
Q

Name 3 terms used to describe CO2 less than 35

A

Hyperventilation, Hypocarbia, Hypocapnia

100
Q

What are some clinical manifestations of hypercarbia or hypoventilation, when PaCO2 is greater than 45 or acidic? 6 symptoms

A 
Pinpoint pupils
Lethargy
Coma
Hallucinations
Headaches
Peripheral vasodilation
101
Q

What are some clinical manifestations of hypocarbia or hyperventilation, when PaCO2 is less than 35 or alkalitic?

A 
Dizziness
Tingling fingers/toes
Spasms
Tetany
Arrhythmia
102
Q

T or F: Chemical Equilibiration means concentrations on each side are equal.

A

False; when concentrations are greater on one side than the other the reaction is said to be shifted; the rate of the reaction on one side is equal to the rate of reaction on the other side; in a closed system the reaction continues until it reaches dynamic equilibration

103
Q

What is described here?
If one constituent is added to the system a new equilibration is reached; If add one reactant on right reaction will shift to the left

A

Law of mass action

104
Q

What demonstrates the relationship between CO2 & H2CO3; Each mole of H2CO3 is in equilibration with 340 moles of CO2

A

Hydrolysis equation

105
Q

Where is the hydrolysis equation faster, inside or outside the cell & why?

A

It is faster inside of the cell because of the presence of carbonic anhydrase

106
Q

Where is carbonic anhydrase found?

A

Kidneys & Liver

107
Q

What does PaCO2 equal?

A

combination of the quantity of entering the system & CO2 leaving the lungs

108
Q

What is VCO2?

A

Volume of CO2 produced in a minute

109
Q

What is VA?

A

Alveolar Ventilation which is the amount of fresh gas that reaches the alveoli each minute

110
Q

What determines the amount of PaCO2?

A

The balance of VCO2 & VA at any moment

111
Q

PaCO2 is directly/indirectly related to production; PaCO2 is directly/indirectly related to excretion

A

PaCO2 is directly related to production & indirectly related to excretion

112
Q

List two factors that affect CO2 production?

A

Temperature & Metabolism

113
Q

An increase in CO2 production is normally balanced by ________.

A

Increase in ventilation

114
Q

Give examples of things that cause excessive CO2 production?

A

Sepsis
Burns
TPN (Total parenteral nutrition)
NaHCO3 administration

115
Q

Give examples of conditions that cause the ventilation system to be impaired, causing too much CO2 buildup?

A

CNS depression, muscle paralysis
Chronic lung disease
Pharmacologic intervention

116
Q

CO2 excretion is directly/inversely related to alveolar minute ventilation?

A

CO2 excretion is inversely related to alveolar minute ventilation

117
Q

T or F: Minute ventilation is a reliable indicator of the adequacy of ventilation.

A

False: Minute ventilation cannot tell us if the lungs are excreting CO2 in proportion to production

118
Q

What is the best indicator to assess the adequacy of ventilation in relationship to CO2 & how is it obtained?

A

PaCO2 is the best index to assess adequacy of ventilation & it is obtained via ABG

119
Q

How is alveolar ventilation different from minute ventilation?

A

Only the gas that reaches functional (perfused) alveoli is considered alveolar ventilation; dead-space volume is subtracted from the tidal volume

120
Q

What is the formula for alveolar ventilation?

A

VA (with period above V)

VA = (Vt - VD) x RR

121
Q

The amount of gas moving in and out of the lungs with each breath is?

A

Tidal volume

122
Q

PaCO2 varies directly/inversely with alveolar ventilation?

A

Inversely

123
Q 
What is the only reliable index of the adequacy of ventilation?
A.  O2
B.  CO2
C.  PaCO2
D.  H2CO3
E.  HCO3-
A

C. PaCO2

124
Q

List 2 general mechanisms in which CO2 is transported in the blood?

A

Dissolved & Combined

125
Q

State the amount & significance of CO2 that is dissolved & where it is dissolved.

A

10% is dissolved. 5% dissolved in the plasma; & 5% is dissolved in the RBC

126
Q

What is the major mechanism of CO2 transport?

A

HCO3; accounts for 68%; 63% in RBC & 5% in plasma

127
Q

Why is dissolved transport so important in CO2 transport even though it represents only 10%?

A

All combined CO2 must become dissolved to get in/out of the cell

128
Q

Name the 4 basic forms that CO2 is transported:

A

dissolved CO2, carbonic acid, bicarbonate, carbamino compounds

129
Q

What is the solubility coefficient of CO2 in mEq/L

A

.03 mEq/L

130
Q

What phenomenon is responsible for the large amount of CO2 transported via bicarbonate?

A

Chloride Shift–the exchange of bicarbonate ions for chloride anions across the RBC; this is due to the electrical gradient created between intracellular fluid and plasma; results in movement of chloride anions into RBC from plasma

131
Q

Another form of CO2 transport which is small amount occurs when CO2 can combine with hemoglobin which contains the protein globin; the combined form of Hb and CO2 is called and accounts for what percent of the combined transport of CO2?

A

Carbamino & 21%

132
Q

What are 3 causes of respiratory failure?

A

Failure to ventilate
Failure to oxygenate
Failure to protect airway

133
Q

The amount of CO2 entering the blood depends primarily on the ______?

A

Metabolic Rate

134
Q

The volume of CO2 produced per minute is designated as the?

A

VCO2

135
Q

______ is the amount of fresh gas that reaches functional alveoli?

A

Alveolar ventilation

136
Q

An increase in blood PaCO2 can increase after IV administration of what drug?

A

Sodium Bicarbonate

137
Q

An increase in alveolar ventilation results in an increase/decrease of PaCO2?

A

Decrease

138
Q

What is the formula for minute ventilation?

A

Vt x RR

139
Q

The change in equilibrium in response to a change in the amount of one of the reaction constituents is called?

A

Law of Mass Action

140
Q

There is an increase/decrease/no change in the amount of carbonic acid present in the blood as it passes the tissues

A

Increase

141
Q

The solubility coefficient of CO2 is higher/lower than the solubility coefficient of O2. Which laws states this?

A

CO2 is 24 x more soluble than O2; so it is higher; per henry’s law

142
Q

The hydrolysis reaction occurs faster in the plasma or RBC?

A

RBC

143
Q 
Hydrogen ions generated by Hydrolysis reaction within the RBC are buffered by?
a.  Hb
b.  Bicarbonate
C.  Carbonic Acid
D.  they are not buffered
A

A. Hb

144
Q

Bicarbonate ions are transported through the cell membrane in exchange for :

a. Cl-
b. PO4-
c. K+

A

A. Cl-

145
Q

The affinity of hemoglobin for CO2 is greater/less when it is combined with O2?

A

Less

146
Q

The regulation of _______ Is the single most important role of the kidneys in acid base balance.

A

Bicarbonates

147
Q

Name 2 substances that must be present in a buffer solution?

A

Weak acid

Salt of the conjugate base of weak acid

148
Q 
A strong acid in a buffer solution will react with?
A.  Salt
B.  Weak Acid
C.  Base
D.  H2O
A

A. Salt

pH & CO2 quiz prep (1 decks)

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