Advanced System Buffering - meaning and definition. What is Advanced System Buffering
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What (who) is Advanced System Buffering - definition

BUFFER SOLUTION
Bicarbonate buffering system
  • Carbon dioxide, a by-product of [[cellular respiration]], is dissolved in the blood, where it is taken up by red blood cells and converted to carbonic acid by carbonic anhydrase. Most of the carbonic acid then dissociates to bicarbonate and hydrogen ions.

3.67 m Advanced Electro Optical System Telescope         
U.S. AIR FORCE OPTICAL TELESCOPE IN HAWAII
3.67m Advanced Electro Optical System Telescope; AEOS
The 3.67 m Advanced Electro Optical System Telescope is a Department of Defense telescope at Haleakala Observatory.
Bicarbonate buffer system         
The bicarbonate buffer system is an acid-base homeostatic mechanism involving the balance of carbonic acid (H2CO3), bicarbonate ion (HCO), and carbon dioxide (CO2) in order to maintain pH in the blood and duodenum, among other tissues, to support proper metabolic function. Catalyzed by carbonic anhydrase, carbon dioxide (CO2) reacts with water (H2O) to form carbonic acid (H2CO3), which in turn rapidly dissociates to form a bicarbonate ion (HCO ) and a hydrogen ion (H+) as shown in the following reaction:
Advanced Traffic Management System         
INTELLIGENT TRANSPORTATION SYSTEM DOMAIN
Advanced traffic management system
The Advanced Traffic Management System (ATMS) field is a primary subfield within the Intelligent Transportation System (ITS) domain. The ATMS view is a top-down management perspective that integrates technology primarily to improve the flow of vehicle traffic and improve safety.

Wikipedia

Bicarbonate buffer system

The bicarbonate buffer system is an acid-base homeostatic mechanism involving the balance of carbonic acid (H2CO3), bicarbonate ion (HCO
3
), and carbon dioxide (CO2) in order to maintain pH in the blood and duodenum, among other tissues, to support proper metabolic function. Catalyzed by carbonic anhydrase, carbon dioxide (CO2) reacts with water (H2O) to form carbonic acid (H2CO3), which in turn rapidly dissociates to form a bicarbonate ion (HCO
3
) and a hydrogen ion (H+) as shown in the following reaction:

As with any buffer system, the pH is balanced by the presence of both a weak acid (for example, H2CO3) and its conjugate base (for example, HCO
3
) so that any excess acid or base introduced to the system is neutralized.

Failure of this system to function properly results in acid-base imbalance, such as acidemia (pH < 7.35) and alkalemia (pH > 7.45) in the blood.