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Bicarbonate Buffer – Blood pH Regulation

The bicarbonate buffer is the most important buffer system in human blood, regulating the pH level in the body and maintaining a stable acid-base balance.

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Things worth knowing about "Bicarbonate Buffer"

The bicarbonate buffer is the most important buffer system in human blood, regulating the pH level in the body and maintaining a stable acid-base balance.

What is the Bicarbonate Buffer?

The bicarbonate buffer system (also called the hydrogen carbonate buffer) is the primary buffer system in human blood and tissue fluid. It maintains the blood pH within the narrow physiological range of 7.35 to 7.45. Without this system, even small amounts of acids or bases could cause life-threatening disturbances in metabolism.

Mechanism of Action

The bicarbonate buffer system consists of two components in equilibrium with each other:

Carbonic acid (H₂CO₃) – the weak acid of the system
Bicarbonate (HCO₃⁻) – the conjugate base of the system

The chemical equilibrium reaction is:

CO₂ + H₂O ⇌ H₂CO₃ ⇌ H⁺ + HCO₃⁻

When excess acid (H⁺ ions) accumulates in the blood, it reacts with bicarbonate to form carbonic acid, which then breaks down into carbon dioxide (CO₂) and water. The CO₂ is exhaled via the lungs. Conversely, when there is an excess of base, more carbonic acid can be formed to neutralize it.

Regulation by the Lungs and Kidneys

The bicarbonate buffer system is closely linked to the function of two key organs:

Lungs (Respiratory Regulation)

The lungs regulate blood CO₂ levels through breathing rate. When the pH drops (acidosis), the breathing rate increases to exhale more CO₂, raising the pH back to normal. When the pH rises (alkalosis), breathing slows down to retain more CO₂.

Kidneys (Renal Regulation)

The kidneys provide long-term regulation of bicarbonate levels in the blood. They can reabsorb or excrete bicarbonate to fine-tune the pH over hours to days.

Clinical Significance

Disturbances in the bicarbonate buffer system lead to the following conditions:

Metabolic acidosis: Too little bicarbonate in the blood, pH falls below 7.35 – commonly seen in diabetes mellitus, kidney failure, or severe diarrhea.
Metabolic alkalosis: Too much bicarbonate, pH rises above 7.45 – commonly caused by prolonged vomiting or excessive diuretic use.
Respiratory acidosis: Excess CO₂ due to reduced respiratory function (e.g., COPD).
Respiratory alkalosis: Too little CO₂ due to hyperventilation.

Clinically, the bicarbonate buffer system is assessed using blood gas analysis (BGA), which measures pH, partial pressure of CO₂, and bicarbonate concentration.

Medical and Therapeutic Use

Sodium bicarbonate (sodium hydrogen carbonate) is used therapeutically to treat severe metabolic acidosis. It is administered intravenously to directly increase the bicarbonate level in the blood and normalize the pH value.

References

Silbernagl S., Despopoulos A. – Color Atlas of Physiology, 6th Edition, Thieme Publishers (2009).
Guyton A. C., Hall J. E. – Textbook of Medical Physiology, 13th Edition, Elsevier (2016).
World Health Organization (WHO) – Acid-base balance and disorders, WHO Technical Reports.

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