Answer: The pH of blood is a measure of its acidity or basicity and is related to the concentration of hydrogen ions (H+) in the blood. The pH of 7.371 indicates that the blood is slightly basic. Carbonic acid (H2CO3) is a weak acid that dissociates into bicarbonate (HCO3-) and hydrogen ions (H+) in water. The carbonic acid concentration of 1.5 indicates the concentration of H2CO3 in the blood.
The concentration of bicarbonate (HCO3-) in the blood can be approximated by using the relationship between the pH, carbonic acid concentration and the bicarbonate concentration. The Henderson-Hasselbalch equation, which relates the pH and the pK of a buffer, to the ratio of the buffer's conjugate base to its acid form is:
pH = pK + log [HCO3-]/[H2CO3]
The pK of carbonic acid is 6.1 and the concentration of H2CO3 is given as 1.5.
Plugging these values into the Henderson-Hasselbalch equation,
7.371 = 6.1 + log [HCO3-]/1.5
Solving for [HCO3-],
[HCO3-] ≈ 25.8 mM
The approximate concentration of bicarbonate (HCO3-) in the person's blood is 25.8 mM.
Please note that this is an approximation, the actual value may vary depending on the person's health condition.
Explanation: