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Bicarbonate Buffer System – Blood pH Regulation

The bicarbonate buffer system is the most important buffering system in human blood, maintaining the pH within a narrow, life-sustaining range through a balance of carbon dioxide and bicarbonate.

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Things worth knowing about "Bicarbonate Buffer System"

The bicarbonate buffer system is the most important buffering system in human blood, maintaining the pH within a narrow, life-sustaining range through a balance of carbon dioxide and bicarbonate.

What is the Bicarbonate Buffer System?

The bicarbonate buffer system (also known as the hydrogen carbonate buffer system) is the primary chemical buffering system in the human body. It maintains the blood pH within a narrow range of 7.35 to 7.45. Deviations from this range can be life-threatening and are classified as acidosis (pH too low) or alkalosis (pH too high).

Mechanism of Action

The bicarbonate buffer system is based on the chemical equilibrium between carbon dioxide (CO2), carbonic acid (H2CO3), and bicarbonate (HCO3-). The underlying equilibrium reaction can be simplified as:

CO2 + H2O ⇌ H2CO3 ⇌ H+ + HCO3-

When acid levels rise in the blood (excess H+ ions), these ions react with bicarbonate to form carbonic acid, which then breaks down into water and CO2. The excess CO2 is expelled through the lungs. When excess base is present, the reaction proceeds in the opposite direction.

Regulation by the Lungs and Kidneys

A key feature of the bicarbonate buffer system is its close connection to two organ systems:

Lungs (respiratory component): By adjusting breathing rate and depth, CO2 levels in the blood are rapidly regulated. Increased breathing lowers CO2 and raises blood pH.
Kidneys (metabolic component): The kidneys regulate bicarbonate concentration more slowly but with longer-lasting effects. They can reabsorb or excrete bicarbonate to adjust pH over hours to days.

Clinical Relevance

Disturbances of the bicarbonate buffer system are central to many medical conditions:

Respiratory acidosis: Excess CO2 in the blood, for example due to lung diseases such as COPD or respiratory failure.
Respiratory alkalosis: Insufficient CO2, for example during hyperventilation.
Metabolic acidosis: Low bicarbonate levels, for example in kidney failure, diabetes, or severe diarrhea.
Metabolic alkalosis: Elevated bicarbonate, for example due to prolonged vomiting or excessive use of antacids.

Diagnostics

The bicarbonate buffer system is assessed clinically using arterial blood gas analysis (ABG). Key parameters measured include:

Blood pH
Partial pressure of CO2 (pCO2)
Bicarbonate concentration (HCO3-)
Base excess (BE)

These values allow a precise evaluation of respiratory function, kidney function, and overall acid-base balance.

Henderson-Hasselbalch Equation

The bicarbonate buffer system is quantitatively described by the Henderson-Hasselbalch equation:

pH = pKa + log ([HCO3-] / [H2CO3])

The pKa of this system is approximately 6.1. Under physiological conditions, the ratio of bicarbonate to carbonic acid is approximately 20:1, resulting in a normal blood pH of 7.4.

References

Boron, W. F. & Boulpaep, E. L. (2017). Medical Physiology. Elsevier, Philadelphia.
World Health Organization (WHO). Acid-base disorders and clinical fluid management. WHO Clinical Guidelines.
Silbernagl, S. & Despopoulos, A. (2015). Color Atlas of Physiology. Thieme, Stuttgart.

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