Bicarbonate Ion Theory

The Bicarbonate Ion Theory explains how our body maintains a stable pH balance (around 7.4) in the blood. It involves the bicarbonate ion (HCO₃⁻), which acts as a buffer by neutralizing excess acids or bases. When acid levels rise, bicarbonate reacts with hydrogen ions (H⁺) to form carbonic acid (H₂CO₃), preventing dangerous acidity. Conversely, if the blood becomes too basic, carbonic acid can break down to release hydrogen ions. This system helps keep blood pH steady, ensuring proper function of cells and organs.