Answer:
See below
Explanation:
[tex]\rm CO_{2} + H_{2}O \rightleftharpoons H_{2}CO_{3} \rightleftharpoons H^{+} + HCO_{3}^{-}[/tex]
According to Le Châtelier's Principle, when a stress is applied to a system at equilibrium, the system will respond in a way that tends to relieve the stress.
(i) Increasing [H⁺]
If [H⁺] increases, the rate of the reaction with HCO₃⁻ increases, so the rate of formation of H₂CO₃ is greater than the rate of ionization.
The increased concentration of H₂CO₃ causes its rate of decomposition to increase, and more CO₂ is expelled to the atmosphere.
(ii) Decreasing [H⁺]
If [H⁺] decreases, the rate of the reaction with HCO₃⁻ decreases, so the rate of ionization of H₂CO₃ is faster than the reverse reaction.
The decreased concentration of H₂CO₃ causes its rate of decomposition to CO₂ to decrease. The rate of formation of H₂CO₃ from CO₂ is greater than the rate of decomposition.
The net effect is that CO₂ is absorbed into the blood.
