Increased $CO_2$ in Blood Causes pH Drop
An increase in the concentration of dissolved carbon dioxide ($CO_2$) in the blood triggers a series of chemical reactions that affect blood acidity.
Carbon Dioxide Transport in Blood
Carbon dioxide dissolves in blood and reacts with water ($H_2O$) primarily within red blood cells, catalyzed by the enzyme carbonic anhydrase. This forms carbonic acid ($H_2CO_3$), which then dissociates:
$CO_2 + H_2O \rightleftharpoons H_2CO_3 \rightleftharpoons H^+ + HCO_3^-$
This reaction explains how $CO_2$ influences hydrogen ion ($H^+$) and bicarbonate ion ($HCO_3^-$) concentrations.
Impact on Hydrogen Ion ($H^+$) Concentration
As the concentration of dissolved $CO_2$ rises:
- More carbonic acid ($H_2CO_3$) is formed.
- This leads to an increased dissociation into hydrogen ions ($H^+$) and bicarbonate ions ($HCO_3^-$).
- Therefore, the concentration of $H^+$ ions in the blood increases.
Effect on Blood pH
Blood pH is a measure of its acidity, defined as the negative logarithm of the hydrogen ion concentration:
$pH = -\log_{10}[H^+]$
A higher concentration of $H^+$ ions results in a lower pH value. Thus, increased $CO_2$ leads to a decrease in blood pH, making the blood more acidic (a condition known as respiratory acidosis).
Analysis of Options
- $HCO_3^-$ concentration: The reaction shows that $HCO_3^-$ concentration increases, not decreases.
- $H^+$ concentration: As shown, $H^+$ concentration increases, it does not decrease.
- Blood pH: The increase in $H^+$ concentration directly causes the blood pH to decrease.
- Oxygen transport: Increased $CO_2$ (and resulting lower pH) shifts the oxygen-hemoglobin dissociation curve to the right (Bohr effect), enhancing oxygen delivery to tissues, thus affecting oxygen transport.
Consequently, the primary effect of increased dissolved $CO_2$ is a decrease in blood pH.
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