The most prominent chemical buffering system that is used to regulate pH is the relationship of HCO₃- to:

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The bicarbonate buffer system involves the relationship between bicarbonate ions (HCO₃-) and carbonic acid (H₂CO₃). When there is an increase in the concentration of H+ ions (decreased pH), the bicarbonate ion accepts a H+ ion to form carbonic acid, thus buffering the pH. When there is a decrease in the concentration of H+ ions (increased pH), the carbonic acid dissociates to release H+ ions, therefore buffering the pH. CO2 is indirectly involved in this system as it reacts with water to form carbonic acid, which can then dissociate into hydrogen ions and bicarbonate ions. HCO₃- (bicarbonate) acts as a buffer in the blood by reacting with H+ ions to form carbonic acid (H2CO3), which then dissociates into H2O and CO2. This reaction is reversible and can shift in either direction to help maintain a stable pH. Therefore, the relationship of HCO₃- to carbonic acid is the most prominent chemical buffering system used to regulate pH. CO2 (choice B) and H+ (choice C) are involved in this process as well, but they are not the primary components of the buffering system.

The Most Prominent Chemical Buffering System That Is Used to Regulate