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CHEM71030 > Unit 11: Acid-Base > Flashcards

Unit 11: Acid-Base Flashcards

1
Q

Carbonic acid levels in the body are controlled with the:

A

Respiratory system

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2
Q

Condition wherein a deficiency in carbonic acid or CO2 levels causes the blood to be overly alkaline

A

Respiratory Alkalosis

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3
Q

Condition where a deficiency of bicarbonate causes the blood to be overly acidic

A

Metabolic Acidosis

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4
Q

Condition wherein an excess of CO2 or carbonic acid causes the blood to be overly acidic

A

Respiratory Acidosis

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5
Q

Condition wherein an excess of bicarbonate causes the blood to be overly alkaline

A

Metabolic Alkalosis

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6
Q

The following symptom group is most likely to be found in BOTH acidosis and alkalosis:

A

Confusion, nausea, vomiting

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7
Q

Organic acids or excessive ketone bodies in the blood are common causes of metabolic acidosis.

A

True

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8
Q

Hypercapnia (high CO2) is most likely to occur in the following situations EXCEPT:

A

Salicylate toxicity

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9
Q

Protein buffer systems work primarily in the:

A

INTRAcellular space

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10
Q

List the following from most ACIDIC to most BASIC:
Pure water, Ammonia, HCl, Saliva, Blood, Baking soda, NaOH

A

HCl
Saliva
Pure water
Blood
Baking soda
Ammonia
NaOH

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11
Q

The acidity of a solution with HCl can be buffered with a weak base like Na2HPO4 (sodium monohydrogen phosphate). Chemical products of this (strong acid + weak base) reaction include:

A

Weak acid and salt (NaH2PO4 + NaCl)

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12
Q

An individual has a blood pH of 7.1. This individual requires immediate:

A

Medical attention

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13
Q

An individual has high pH, normal PCO2, and high bicarbonate. This individual is likely experiencing:

A

Metabolic alkalosis

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14
Q

An excessive loss of bicarbonate through diarrhea would most likely lead to:

A

Metabolic acidosis

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15
Q

To maintain electrical neutrality, in metabolic acidosis the excessive loss of bicarbonate through diarrhea might lead to:

A

hyperchloremia

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16
Q

Diabetic ketoacidosis is an emergency because:

A

Metabolic processes require a narrow range of pH to function

17
Q

Order the following buffers from quickest to slowest:
Respiratory
Renal
Chemical

A

1) Chemical
2) Respiratory
3) Renal

18
Q

In the conversion of carbon dioxide into bicarbonate, hydrogen ions are buffered by hemoglobin.

A

True

19
Q

Match the following values with the type of acid-base disorder.

Reference ranges:
pH : 7.35-7.45
pCO2: 32-45mmHg (female)
Bicarb: 22-29mmol/L

pH: 7.33
pCO2: 36mmHg then 30mmHg
Bicarb: 19mmol/L

A

Metabolic acidosis - Compensated

20
Q

Match the following values with the type of acid-base disorder.

Reference ranges:
pH : 7.35-7.45
Bicarb: 22-29mmol/L
pCO2: 32-45mmHg (female)

pH:7.47
pCO2: 35mmHg
Bicarb: 32mmol/L

A

Metabolis alkalosis - Uncompensated

21
Q

Match the following values with the type of acid-base disorder.

Reference ranges:
pH : 7.35-7.45
Bicarb: 22-29mmol/L
pCO2: 32-45mmHg (female)

pH: 7.46
pCO2: 28mmHg
Bicarb: 25mmol/L

A

Respiratory alkalosis - Uncompensated

22
Q

In acid-base disorders, compensation refers to the underlying primary etiology.

A

False

23
Q

The majority of the body’s waste products are basic or neutral in pH.

A

False

24
Q

In the phosphate buffer system, the following chemical acts as a weak acid that can help to neutralize the high pH of sodium hydroxide:

A

NaH2PO4

25
Q

Protein Buffers

A
  • When the blood becomes too acidic (low pH), proteins like hemoglobin, albumin, and others can bind to excess H⁺ ions. Conversely, if the blood becomes too alkaline (high pH), the proteins can release H⁺ ions to lower the pH.
26
Q

Hemoglobin Buffer

A
  • Principal protein found inside of RBCs.
  • During conversion of CO2 into bicarbonate, hydrogen ions are liberated.
     CO2 + H2O = H2CO3 = H+ + HCO3
  • Reaction is buffered by hemoglobin.
  • Process is reversed by pulmonary capillaries to form CO2.
27
Q

Phosphate Buffer

A
  • Found in the blood in 2 forms:
    –> sodium dihydrogen phosphate (weak acid)
    –> sodium monohydrogen phosphate (weak base)
  • Is regulated by SODIUM.
  • When sodium monohydrogen phosphate (weak BASE) comes into contact with a strong ACID like HCl, the base picks up a second hydrogen to form a weak acid and sodium chloride.
  • When sodium dihydrogen phosphate (weak ACID) comes into contact with a strong BASE such as sodium hydroxide, the acid reverts back into a base and produces water.
28
Q

Bicarbonate-Carbonic Acid Buffer

A
  • Bicarbonate-carbonic acid buffer works similarly to phosphate buffers.
  • Bicarbonate is regulated in the blood by sodium.
  • When sodium bicarbonate (NaHCO3), comes into contact with a strong acid, such as HCl, carbonic acid (H2CO3), which is a weak acid, and NaCl are formed.
  • When carbonic acid comes into contact with a strong base, such as NaOH, bicarbonate and water are formed.
29
Q

Respiratory Contributions to Acid-Base Balance

A
  • CO2 levels are too HIGH, the blood becomes acidic (low pH), so the body will increase the rate and depth of breathing to expel more CO2 and raise the blood pH levels back up.
  • CO2 levels are too LOW, the blood becomes alkaline (high pH), so the body decreases the rate of breaths to lessen the amount of CO2 being expelled and lower the blood pH levels back down.
30
Q

Renal Contribution to Acid-Base Balance

A
  • When the blood is acidic (low pH), the kidneys increase hydrogen ion secretion and bicarbonate reabsorption to raise the blood pH.
  • When the blood is alkaline (high pH), the kidneys reduce hydrogen ion secretion and may even excrete bicarbonate to lower the blood pH.
31
Q

Metabolic Acidosis

A
  • Occurs when the blood is too acidic due to too little bicarbonate.
  • Caused by diarrhea, uremia, diabetic ketoacidosis.

pH: <7.35
PaCO2: 35-45 mmHg, normal
HCO3: <22 mEq/L

Compensation Mechanism:
- Lower than normal amounts of bicarb would be present.

pH = decreased
PCO2 = normal, then decreases
HCO3 = decreased

32
Q

Respiratory Acidosis

A
  • Blood is too acidic due to an excess of carbonic acid from too much CO2 in the blood. - Caused by pneumonia, emphysema, congestive heart failure.

pH: <7.35
PaCO2: >45 mmHg
HCO3: 22-26 mEq/L, normal

Compensation Mechanism:
- Excess CO2 is present in the blood.

pH = decreased
PaCO2 = increased
HCO3 = normal, then increased

33
Q

Metabolic Alkalosis

A
  • When the blood is too alkaline due to too much bicarbonate.
  • Caused by Cushing’s disease, antacids, vomiting, hypertension.

pH: >7.45
PaCO2: 35-45 mmHg, normal
HCO3: >26 mEq/L

Compensation Mechanism:
- Excess bicarbonate is present.

pH = increased
PaCO2 = normal, then increased
HCO3 = increased

34
Q

Respiratory Alkalosis

A
  • When the blood is alkaline to not enough carbonic acid and low CO2 levels in the blood. -Caused by hyperventilation.

pH: >7.45
PaCO2: <35 mmHg
HCO3: 22-26 mEq/L, normal

Compensation Mechanism:
- CO2 deficiency would occur

pH = increased
PCO2 = decreased
HCO3 = normal, then decreased

35
Q

pH

A

Measure of acidity or alkalinity of the blood.

Normal range: 7.35 - 7.45
<7.35 = acidosis
>7.45 = alkalosis

36
Q

PCO2

A

The pressure exerted by dissolved CO2 in the blood, which shows how well CO2 is being excreted by the lungs.

Normal range: 35 - 45 mmHg
<35 mmHg = alkalotic
>45 mmHg = acidotic

37
Q

HCO3

A

A buffer in the blood that helps maintain the pH balance, primarily influenced by renal function.

Normal range: 22-26 mEq/L
<22 mEq/L = acidotic
>26 mEq/L = akalotic

CHEM71030 (12 decks)

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