acid-base balance Flashcards

1
Q

proton regulation

A

must be tightly regulated because very reactive
ECF levels kept al low levels, 4nEq/L
should be 3-5nEq/L

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2
Q

pH of ECF

A

7.4

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3
Q

acidosis

A

process

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4
Q

acidaemia

A

state

<7.35

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5
Q

alkalosis

A

process

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6
Q

alkalaemia

A

state

>7.45

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7
Q

venous blood compared to arterial blood

A

more acidic

higher partial pressure of carbon dioxide

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8
Q

interstitial fluid

A

usually same an venous blood pH

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9
Q

pH effects of metabolism

A

practically every step of every metabolic process is pH dependant
deviate from optimal pH causes decrease in reaction efficiency, especially due to compromised enzyme activity

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10
Q

acidosis affect on neuromuscular system

A

inhibitory

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11
Q

alkalosis affect of neuromuscular system

A

excitatory

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12
Q

why does pH affect neuromuscular system

A

plasma Ca2+ binding to albumin is pH dependant
acidosis increases free Ca2_
bathmotropy - calcium blocks Na channels, raises AP threshold

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13
Q

bathmotropy

A

when free calcium interacts with Na channels and switches them off, which raises the AP threshold

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14
Q

potassium balance in pH

A

acidosis - more serum [K]

alkalosis - less serum K

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15
Q

consequences of acidosis

A

headaches, confusion, lethargy, tremors, sleepiness, cerebral dysfunction,
come
hyperventilation

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16
Q

consequences of alkalosis

A

muscular weakness, pain, cramps, spasms, (smooth and skeletal muscle), tetany
hypoventilation

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17
Q

most acid comes from

A

CHO/fat metabolism (CO2)

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18
Q

acids produced in the body

A
  • metabolic activities continuously add H to the body
  • glycolytic metabolism - lactic acid
  • oxidative metabolism - CO2/carbonic acid
  • FA/AA metabolism - ketoacids
  • inorganic acids produced from intermediary metabolism
  • stomach acid production loads HCO3 - blood
  • pancreatic HCO3 production loads H+ - blood
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19
Q

vomiting causes

A

alkalosis

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20
Q

buffers

A

HCO3- in ECF
proteins, haemoglobin, phosphates in cells
phosphates, ammonia in urine

21
Q

chemical buffering

A
  • solutions preventing change in pH
  • intracellular and extracellular buffers provide an immediate response to acid-base disturbances
  • bonde also buffers acid loads
  • immediate but exhaustible
22
Q

pulmonary regulation

A
  • PCO2 is regulated by changes in tidal volume and respiratory rate
  • CO2 is exhaled - blood pH increases
  • can only removed acid
23
Q

renal regulation

A
  • kidneys control adjust the amount of HCO3- and/or H+ that is excreted
  • excreting HCO3- causes decrease in blood pH
  • excreting H + causes increase in blood pH
24
Q

buffer power

A
  • determined by the pH appropriateness of the system

- pKa should patch pH

25
capacity of buffer determined by
total [buffer] | relative [HB] and [B]
26
chemical buffer systems
HCO3- (ECF buffer) NH3 (renal tubular fluid) PO42- (ICF) proteins (ICF, Hb n RBCs)
27
ventilation
ventilation rates control pH balance | - increased ventilation removes CO2
28
hyperventilation causes
increase pH | decrease [H]
29
hypoventilation causes
increase [H] | decrease pH
30
renal control
kidneys constantly remove HCO3- from blood to maintain balance, we must re absorb HCO3- back into the blood kidneys can't do that first it has to be converted
31
conversion of HCO3- for reabsorption
HCO3- + H+ > H2CO3 > H2O + CO2 to do this, kidney must secrete H+ at a 1:1 ration with HCO3-
32
if H secretion = HCO3- filtration
no change in pH
33
if H secretion > HCO3- filtration
acid loss
34
if H secretion < HCO3- filtration
base loss
35
how is HCO3- reabsorbed
2nd degree active transport - CO2 diffuses into cells - carbonic anhydrase inside the cell forms CO2 into H2CO3 which becomes HCO3- and H+ - the H+ then leaves the cell again 1st degree active transport - H+ pumped directly put into the lumen
36
acid being secreted as ammonium
ammonium is produced by removing amine group from amino acids amine group is actively transported out of the cells as ammonium via counter transportation for Na
37
2 direct mechanisms
1. Na/K ATPase - alkalosis causes a shift of K+ from the plasma > ICF 2. electronuetrality - K+ will be passively secreted as an obligate cation partner to HCO3-
38
why do states of alkalosis cause hypokalaemia
because K+ ions are being secreted with the HCO3- ions to maintain electronuetrality
39
arterial blood gas analysis
PCO2 - reflect respiratory component | HCO3- - reflects the metabolic component
40
AB disorders
- may be metabolic or respiratory - metabolic - due to production, ingestion or loss of acids/bases - respiratory - due to hyper/hypoventilation
41
riased HCO3-
alkalosis
42
raised pCO2
acidosis
43
respiratory disorder leads to
metabolic compensation
44
metabolic disorder
respiratory compensation
45
subtypes of metabolic acidosis
[Na+] is greater than [HCO3-] + [Cl-] difference between the two issues the anion gap usually 12 mEq/L major increase in anion gap implies existence of an organic acidosis (poisoning)
46
plasma anion gap exists because
- gap exists because there must be elctronuetrality
47
increased anion gap
organic acidosis diabetic/sstarvation ketoacidosis, lactic acidosis, poisoning sulphates, methanol, ethylene glycol, os salicylates (aspirin)
48
normal anion gap acidosis
diarrhoea (HCO3- loss) | carbonic anhydrase-inhibitors