Excess protons in the blood decrease the amount of hco − 3 and thus reduce the buffering capacity of blood. a rapid drop in ph could lead to death. normal values for blood are ph = 7.4 , [ hco − 3 ] = 24.0 mm , [ co 2 ] = 1.2 mm . (a) if a patient has a blood ph = 7.03 and [co2] = 1.2 mm, what is the [hco3−] in the patient’s blood? the pka of hco3−= 6.1.
(b) suggest a possible treatment for metabolic acidosis.
(c) why might the suggestion for part (b) be of benefit to middle-distance runners?

a) [HCO₃⁻] = 10,2 mM.

b) Sodium bicarbonate.

c) Yes.

Explanation:

a) The equilibrium of this reaction is:

CO₂ + H₂O ⇄ HCO₃⁻ + H⁺

Using Henderson-Hasselbalch equation:

pH = pka + log₁₀  

Replacing:

7,03 = 6,1 + log₁₀  

Thus, [HCO₃⁻] = 10,2 mM

b) A possible treatment of metabolic acidosis is with sodium bicarbonate. By Le Chateleir's principle the increasing of HCO₃⁻ will shift the equilibrium to the left decreasing thus, H⁺ concentration.

c) The shifting of the equilibrium to the left will increase CO₂ concentration producing in the body the need to increase breathing, increasing, thus, concentration of O₂ improving cardiac function in exercise.