eLFH - Gases in Solution Flashcards
Liquid at equilibrium
In a closed container, a liquid exists in 2 phases - liquid at bottom and vapour at top
Equilibrium occurs when evaporation rate = condensation rate
Saturated Vapour Pressure
Partial pressure exerted by the vapour molecules at the point of equilibrium
Henry’s Law
At a fixed temperature, the amount of a gas dissolved in a given liquid is directly proportional to the partial pressure of the gas in equilibrium with the liquid
I.e the higher the pressure, the more dissolved gas
What causes the ‘bends’ when diving
Henry’s Law
Rapid decompression and decrease in pressure as re-surfacing
Nitrogen comes out of solution and forms bubbles in joints
Effect of temperature on solubility
Solubility decreases as temperature increases
Describing solubility
Described as volume of gas dissolved in a volume of liquid
2 ways of describing this are:
- Bunsen solubility coefficient
- Ostwald solubility coefficient
Bunsen solubility coefficient
Volume of gas is corrected to standard temperature and pressure dissolved in a unit volume of a liquid at the temperature concerned where the partial pressure of the gas above the liquid is 1 atmosphere
Ostwald solubility coefficient
The volume of gas dissolved in a unit volume of liquid at the temperature concerned
Preferred by anaesthetists as not corrected to standard temperature and pressure, but measured at a known temp and pressure
Partition coefficient
Ratio of the amount of a given substance present in one phase compared with another at equilibrium
Higher number = more soluble
Similar to Ostwald coefficient but need to specify the order of the phases being compared (i.e blood-gas coefficient is different to gas-blood coefficient)
Gas tension in solution
Same as partial pressure of the gas in equilibrium with it
How does solubility of gas affect speed of anaesthesia induction
Lower solubility gases induce anaesthesia faster
Less soluble agent achieves equilibrium in the alveoli faster than more soluble agents