$$ \ce{H^+ + HCO3^- <=> H2O + CO2} $$

The equation above shows one of the reversible reactions that occur in blood. After exercise, an athlete’s blood pH has dropped below the normal level. How will normal blood pH be restored?

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The equation shows that when \(\ce{CO2}\) concentration is high, the reverse reaction will occur at a faster rate than the forward reaction.

$$ \ce{CO2 + H2O -> H^+ + HCO3^-} $$

This causes the \(\ce{H^+}\) concentration to increase, which leads to a lower pH.

In order to combat this, a person can increase their rate of breathing so that the carbon dioxide is exhaled in exchange for oxygen. A decrease in blood \(\ce{CO2}\) will cause the reverse reaction above to occur at a slower rate. \(\ce{H^+}\) will form less or be used up by the forward reaction, resulting in a higher pH.