Systems 2 - Integrated Physiology Flashcards
Equivalents
= moles x valence
So 1 mol Na⁺ = 1 eq/L
1 mol Ca²⁺ = 2 eq/L
Moles are unit of quantity, 6 x 10²³
PaCO₂
PaCO₂ (arterial) = Rate of CO₂ production / alveolar ventilation rate
Quantity of moles
1 mole =
10³ mmol
10⁶ μmol
10⁹ nmol
pH equations
pH = -log[H⁺]
So minor changes in pH -> major changes in [H⁺]
pH = pk + log[A⁻]/[HA]
Importance of pH in body
- enzyme activity/protein strucure affected
- Ca²⁺ ions - 50% are free in blood, ionised, to stabilise nerve and muscle membranes. 50% are bound to albumin, which competes with H⁺ for binding. -> when decreased H⁺, less free Ca²⁺, so less of a membrane stabilising effect
- –> so in hyperventilation, increased pH, hyperexcitable nerves
Trousseau sign, Chvostek’s sign
Trousseau - hand cramped forward, claw
Chvostek - muscle twitch when tap facial nerve
-> indicate disturbance of plasma calcium, or acid/base balance disruption
Buffers
Resist a change in pH by absorbing or releasing H⁺ when an acid or base is added
pH will still change slightly - buffer pair is weak acid and its conjugate base
pk
= the pH where an acid is 50% dissociated, [A⁻]/[HA] = 1
Lower pk -> stronger acid
Extracellular buffers
Bicarbonate
Haemoglobin
Phosphate
Plasma proteins
-> work together to resist change, isohydric principle
Bicarbonate buffer system
pk = 6.1 CO₂ + H₂O = H₂CO₃ = H⁺ + HCO₃⁻
BUT rarely know [H₂CO₃], so use solubility coefficient of 0.03 - [H₂CO₃] = 0.03 x PCO₂
- > pH ∝ [HCO₃⁻]/PaCO₂
- > pH depends on the ratio of bicarbonate to carbon dioxide
IMPORTANT
- high conc of buffer pair in plasma
- PaCO₂ regulated by respiratory system
- [HCO₃⁻] regulated by kidney
Acid production in body
Body is net producer of acid
Kreb’s cycle makes CO₂
Metabolism makes H⁺
Gut below pylorus -> HCO₃⁻ to lumen in alkaline tide, H⁺ into blood
Renal handling of bicarbonate
Reabsorption - of bicarbonate ions by glomerular filtration. If too high, exceeds tubular threshold and spills into urine
Regeneration - of bicarbonate lost in buffering, by secreting protons into nephron to be trapped and excreted by non-bicarbonate buffers, and by secreting ammonium
-aemia
Acidaemia - acidic blood, pH less than 7.35
Alkalaemia - alkaline blood, pH more than 7.45
-osis
Acidosis/alkalosis - processes that cause a change in pH of blood
Usually -> -aemia
‘osis-without-aemia’ when pH in normal range
Compensation
Attempts to return pH to normal
Pathological chronic change in PCO₂ or HCO₃⁻ is compensated by homeostatic change in the other
Renal compensation (adjusting HCO₃⁻) is more effective than respiratory compensation (adjusting CO₂) but takes longer to get effect, days
-> if renal and lung disease, big problem
Change in same direction, if increase in HCO₃⁻, body will increase CO₂ to compensate
Normal range of pH, PCO₂, HCO₃⁻
pH - 7.35-7.45
PCO₂ - 35-45
HCO₃⁻ - 21-29
Alkalaemia
pH > 7.45
HCO₃⁻ raised, metabolic alkalosis
PCO₂ decreased, respiratory alkalosis
Acidaemia
pH < 7.45
HCO₃⁻ decreased, metabolic acidosis
PCO₂ raised, respiratory acidosis
Acid base map
Electroneutrality
Total [cations] = total [anions] in body fluids, can’t have net charge
Anion gap in -ve ions, unsure where from
Normally 8-16mEq/L
Other anions are Cl⁻ and HCO₃⁻
Hyperchloraemic metabolic acidosis with normal anion gap
As cations have increased, to fill in gap, Cl⁻ increases
Anion gap remains unchanged
Caused by too much bicarb out
Increased anion gap metabolic acidosis
As bicarbonate has decreased, to fill in gap, anion gap increasases
Cl⁻ remains unchanged
Caused by too much acid in
Causes of increased anion gap metabolic acidosis
- more fixed acid production, eg lactic acidosis/ketoacidosis
- ingestion of fixed acids, eg aspirin
- inability to excrete fixed acids, eg in renal failure
Causes of hyperchloraemic metabolic acidosis with normal anion gap
- loss of bicarb from gut, eg diarrhoea, ileostomy
- loss of bicarb via kidney, eg renal tubular acidosis
Causes of metabolic alkalosis
SALINE RESPONSIVE
- vomiting, diuretic use, volume contraction
- treated with saline to decrease RAAS activity
SALINE UNRESPONSIVE
- primary hyperaldosteronism
Causes of respiratory alkalosis
Decreased PCO₂, caused by:
- mechanical ventilation, hyperventilation
- stimulation of respiratory centre
Causes of respiratory acidosis
Increased PCO₂, caused by ALVEOLAR HYPOVENTILATION
- defects in neuromuscular chain
- work of breathing exceeds the strength of respiratory pump, eg in obstruction to airflow, restrictive lung diseases, decreased lung compliance, so increased CO₂ production
Constant body temperature
Homeotherms (birds and mammals) have physiological mechanisms to regulate temperature
- allows them to inhabit physiological niches
- enzyme reactions work in narrow range so good to keep constant
Humans do vary by location in body in order to preserve core temperature (isotherms areas of equal heat), and also varies with time
BMR
Basal metabolic rate
- without doing anything, we produce heat, ~100W
Clinical measurement of body temperature
Must be a representative site (into core)
Must be easily accessible
External auditory meatus most common now
Major routes for heat gain and loss equation
Metabolism - Evaporation ± Conduction ± Convection ± Radiation = 0, when heat gain = heat loss
20% loss by evaporation
40% loss by radiation
40% loss by convection