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Bio 472 > Acid - Base Balance > Flashcards

Acid - Base Balance Flashcards

1
Q

Regular Body pH

A

7.4

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2
Q

Acidosis

A

pH < 7.4

high hydrogen ion concentration

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3
Q

Alkalosis

A

pH > 7.4

low hydrogen ion concentration

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4
Q

change in pH resulting in death

A

a change of 0.6 in either direction can result in death

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5
Q

Normal Concentration of Hydrogen Ions

A

4x10^-8 eq/L or 4x10^5 meq/L

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6
Q

Body Buffers

A
  1. Intracellular Fluid
  2. Blood
  3. Interstitial Fluid
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7
Q

Intracellular Fluid as a Buffer

A
  1. Protein (non-exchangable)
  2. HPO4^2-
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8
Q

Blood as a Buffer

A
  1. Hemoglobin
  2. Protein (albumin)
  3. HCO3^-
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9
Q

Interstitial Fluid as a Buffer

A
  1. HCO3-
  2. HPO4^2- (Kidney)
  3. NH3 (Kidney)
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10
Q

Lines of Defense in an Acid Base Crisis

A
  1. Hemoglobin and Proteins
  2. HCO3^- buffer system (most important)
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11
Q

Protein Anion Buffer System

A

75% of the body’s buffering power
not physiologically significant

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12
Q

Protein Anion Buffer System Reactions

A

R-COOH <-> R-COO- + H+
R-NH2 + H+ <-> R-NH3+

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13
Q

Major ECF Buffer Systems

A
  1. Bicarbonate
  2. Phosphate
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14
Q

CO2/HCO3- Bicarbonate Buffer System

A

Most important ECF buffer

regulation from Lungs, Kidneys, Blood Buffer System

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15
Q

Bicarbonate Buffer System Reaction

A

CO2 + H2O + Enzyme <-> H2CO3 <-> H+ + HCO3-

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16
Q

Henderson-Hasselbach Equation for Bicarbonate Buffer System

A

pH= pK + log([HCO3-]/[H2CO3])
or pH = pK +log([HCO3-]/0.3PCO2)

pK = 6.1

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17
Q

Normal Ratio of HCO3 to H2CO3

A

20:1

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18
Q

Bicarbonate Buffer System

A

mixture of NaHCO3 and H2CO3

NaHCO3 can react with an acid to make H2CO2, H2CO3 can react with a base to make NaHCO3

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19
Q

Carbonic Anhydrase

A

enzyme that helps convert CO2 in blood to bicarbonate(HCO3) in the bicarbonate buffer system

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20
Q

When do buffers work best?

A

When pH is close numerically to pK

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21
Q

Why is the Bicarbonate Buffer system the most important buffer system?

A
  1. can be regulated by lungs and kidney (CO2&HCO3-)
  2. Erythrocytes are capable of “Chloride shift”
  3. Abundant supplies of Bicarbonate anion are available for buffering (HCO3-:H2CO3, 20:1)
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22
Q

Chloride Shift

A
  1. Chloride transported into the blood cell
  2. HCO3- buffer transport is favored out of the cell, into plasma
23
Q

Phosphate Buffer System Reactions

A

HCl + Na2HPO4 <-> NaH2PO4 + NaCl
NaOh + NaH2PO4 <-> Na2HPO4 +H2O

24
Q

Phosphate Buffer system

A

more active in the kidney tubule system than ECF

1/12 concentration in ECF compared to Bicarbonate Buffer System

tubular fluid has low pH that is closer to pK of the buffer

25
3 levels of pH regulation
1. Bicarbonate Buffer System 2. Respiratory System 3. Renal Buffer System
26
Bicarbonate Buffer System in pH regulation
weak link, can become saturated
27
Respiratory System role in pH regulation
fast acting, within minutes, | Central Receptor and Peripheral Chemoreceptors ## Footnote buffer power 2x greater than all chemical buffer systems
28
# Respiratory System role in pH regulation Central Receptor(Medulla Oblongata)
detects rise in [H+], causes increase in RR
29
# Respiratory System role in pH regulation Peripheral Chemorecptors
detects decrease in pH, pO2, increase in pCO2 causes increased RR
30
# Respiratory System role in pH regulation Flaw of Respiratory System in pH regulation
cannot stop breathing so it is less effective in an alkalotic crisis
31
Renal Buffer System
recruited after 3-5 hours if respiratory system fails to compensate | reabsorbs base while excreting acid ## Footnote Works using secretion and reabsorbtion
32
# Renal Buffer System Secretion
secretes H+, leading to it being excreted | counter transport of Na+ and H+ ## Footnote secondary active transport,
33
# Renal Buffer System Reabsorbtion
reabsorbs HCO3-, prevents its excretion ## Footnote HCO3- from the glomerular filtrate will combine with H+ to form H2CO3 which will then form CO2 + H2O
34
# Renal Buffer System In the Proximal Convoluted Tubule
for every Na+ reabsorbed 1. H+ secreted 2. HCO3- reabsorbed 3. H+ combines with HCO3- to form H2CO3 ## Footnote both K+ and H+ compete for cotransport with Na+
35
In the Distal Convoluted Tubule
1. H+ is secreted 2. K+ stays in the ECF 3. H+ is buffered in the tubule by HPO4-2 and NH3 4. NH4+ is the excretory form of H+
36
Normal pCO2 level
40 mmHg | respiratory proxy ## Footnote pCO2 = H+ = acid
37
Normal HCO3- level
24 mEq/L | metabolism proxy ## Footnote HCO3- = OH- = base
38
Metabolic Acidosis
acidic condition resulting from metabilism problem ## Footnote Diabetic Ketoacidosis
39
Respiratory Acidosis
acidic condition resulting from an inability to maintain normal ventilation rate or move normal respiratory volumes ## Footnote Chronic Emphysema, Asthma Attack
40
Metabolic Acidosis Signs
pH<7.4 HCO3-<24mEq/L pCO2<40mmHg (increased ventilation rate) ## Footnote HCO3- is the cause, pCO2 is the compensation
41
Respiratory Acidosis Signs
pH<7.4 pCO2>40mmHg (poor breathing) HCO3->24mEq/L(secrete more H+, increase NaHCO3- in ECF) ## Footnote pCO2 is the cause, HCO3- is the compensation
42
Metabolic Alkalosis
exsessive vomiting, poisoning, overingestion of antacids, toothpaste by kids
43
Respiratory Alkalosis
pulmonary hyperventilation, ascent to high altitude, person in Hysteria ## Footnote breath into a brown paper bag
44
Metabolic Alkalosis Signs
pH>7.4 HCO3->24meq/L pCO2>40mmHg (hypoventilate) ## Footnote HCO3- is the cause, pCO2 is the compensation
45
Respiratory Alkalosis Signs
pH>7.4 pCO2<40mmHg (Hyperventilation) HCO3-<24meq/L (increased secretion of HCO3- for excretion) ## Footnote pCO2 is the cause, HCO3- is the compensation
46
Buffer Base
sum of all conjugate bases in 1 liter of systemic arterial blood
47
Buffer Base Example
[HCO3-] = 24mmol/L [Protein] = 15mmol/L [HHb/HbO2] = 9mmol/L Total (Buffer Base) = 48mmol/L
48
Base Excess
change in concentration of Buffer Base from normal ## Footnote Base Excess = Observed Buffer Base - Normal Buffer Base
49
Base Excess example
observed [HCO3-] = 16meq/l normal [HCO3-] = 24meq/l then Base excess = 16meq/l - 24meq/l = -8meq/l
50
Base Excess in Metabolic Acidosis
< -5
51
Base Excess in Metabolic Alkalosis
>5
52
Anion Gap
the difference in concentration between measured cations and anions in 1 liter of plasma ## Footnote Sum of 2 cations - sum of 2 anions
53
Anion Gap in Metabolic Acidosis
[HCO3-] decreases in metabolic acidosis so the anion gap increases
54
Anion Gap in Metabolic Alkalosis
[HCO3-] increases in metabolic alkalosis so the anion gap decreases

Bio 472 (23 decks)

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