Oxygen Transport Blood Buffers  Elmhurst College
Carbon Dioxide Transport Respiratory Acidosis Metabolic Acidosis  Chemistry Department
Buffers in the Kidneys Respiratory Alkalosis Metabolic Alkalosis  Virtual ChemBook

Hemoglobin - Oxygen Equation:

HHgb + O 2 <===> HgbO 2 + H+

Blood Buffer Equation:

CO2 + HOH <===> H2CO3 <===> H+ + HCO3-

Respiratory Alkalosis

QUES. 7: Case 3:
Uncompensated Laboratory Results: pH =7.58, pCO2 = 27, HCO3- = 24.

a. List the condition - acidosis or alkalosis, metabolic or respiratory, compensated or uncompensated.

pH =7.58 = alkalosis, uncompensated
pCO2 = 27 = respiratory
HCO3- = 24 = respiratory uncompensated

b. What is the primary cause of the condition?

Hyperventilation - excess loss of CO2 gas.

c. Explain why the pH is high using the other lab results, using the primary cause, and equilibrium principles.

CO2 + HOH <===> H2CO3 <===> H+ + HCO3-

If there is an excess loss of carbon dioxide from the lungs, it is also low in the blood. If carbon dioxide is low, the equilibrium shifts left, as a result the hydrogen ion concentration decrease, which results in the pH increasing.

d. State and explain how the compensation will return pH to normal using equilibrium principles.

Compensation is for the kidney's to excrete more bicarbonate, which gives a lower bicarbonate in the blood. As a result the equilibrium shifts to the right to compensate for the loss of bicarbonate. As a result, the hydrogen ion concentration then increase, which gives a decrease in the pH more toward normal.

e. Explain how the treatment with __?___ will work using equilibrium principles.

The treatment according to the Table 2 is to hold breath or breath into a paper bag. What will this do? This will serve to help retain more carbon dioxide in the blood. If the carbon dioxide level is higher in the blood, the equilibrium will shift right to increase the hydrogen ion and decrease the pH.