Overview
The bicarbonate buffer system is essential for maintaining the pH of blood, which is critical for proper physiological function. It operates through a dynamic equilibrium between bicarbonate ions and carbonic acid, allowing the body to neutralize excess acids and bases effectively. This system works...
Key Terms
Example: A pH of 7 is neutral, below 7 is acidic, and above 7 is basic.
Example: Bicarbonate is a buffer in blood.
Example: Bicarbonate ions neutralize excess acids in the blood.
Example: Carbonic acid dissociates into bicarbonate and hydrogen ions.
Example: Respiratory acidosis can occur due to lung diseases.
Example: Metabolic alkalosis can result from excessive vomiting.
Related Topics
Acid-Base Chemistry
Study of acids, bases, and their reactions, crucial for understanding pH.
intermediateRespiratory Physiology
Explores how the respiratory system influences blood pH through gas exchange.
intermediateRenal Physiology
Focuses on kidney functions and their role in maintaining homeostasis.
advancedKey Concepts
pH regulationbicarbonate ionscarbonic acidacid-base balance