Lecture 7- CO2 transport in the blood Flashcards
how is carbon dioxide transported in the blood
- dissolved (CO2 is more soluble than oxygen)
- CO2 reacts chemically with water to form bicarbonate- HCO3-
- As a carbamino-haemoglobin compound
total content of O2 in arterial blood
8.9 mmol/L
total content of CO2 in arterial blood
21
Lots of CO2 in blood going to tissues- not a waste product.
CO2 has a major role in
controlling blood pH (acid-base balance)
Chemical reactant in the major pH buffering system of blood
blood pH must be kept within a narrow range
arterial pH 7.35 – pH 7.45; venous 7.31-7.41
body has several buffering systems to control blood pH but…..
one using CO2 most important
what is a buffer
- Buffers are compounds which are able to bind or release hydrogen ions such that they dampen swings in the pH.
outline the bicarbonate buffer system
- CO2 reacts with H20 to form carbonic acid
- carbonic acid dissoaciates to form H+ and HCO3-

how to workout CO2 dissolved in arterial blood
[CO2] dissolved= solubility x pCO2
- solubility factor for CO2 at 37 degrees= 0.23 mmol/L/kPa
- pCO2 of CO2 arterial blood= 5.3 kPa
- therefore:
- 5.3 kPa x 0.23 mmol/L/kPa= 1.2 mmol/L dissolved CO2
why is [CO2] dissolved higher than [O2] dissolved
more dissolved CO2 even though lower pCO2 than pO2 because of markedly increased solubility
carbon dioxide in plasma
- dissolved CO2 reacts with water to form carbonic acid –> H2CO3

Carbonic acid very quickly
dissociates to H+ and HCO3-
bicarbonate buffer equation is
reversible
the direction the bicarbonate buffer favours depends on
- The rate of the reaction depends on the amount of reactants (on the left) and productions (on the right)- “law of mass action”
- Reaction can go on either direction- dependent on conc of chemical
which equation can be used to calculate the pH of plasma
Henderson-Hasselbalch
Henderson Hasselbalch equation applied to the carbon dioxide-bicarb buffer system

plasma pH is dependent on
- on how much [CO2] reacts with water to form H+
- if CO2 is high then the reaction will be favoured towards the right producing lots of H+ and HCO3-

higher [HCO3-] in plasma will
push the reaction to the left
in the body the reaction is favoured in this direction because HCO3-> CO2- why our body pH slightly alkaline 7.4

- Amount of Co2 dissolved depends directly
- on the partial pressure of CO2
*
If pCO2 rises (and no change in bicarbonate)
plasma pH will fall (become more acidic)
If pCO2 falls (and there is no change in bicarbonate)
plasma pH will rise (become more alkaline)
what is the determining factor of the amount of CO2 dissolved
- The pCO2 of alveoli’s is the determining factor- determines arterial pCO2
- Alveolar, and hence arterial pCOP2 controlled by altering the rate of breathing
how much HCO3- in plasma
25 mmol/L
- cation associated with this is mainly na+ not H+






