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The bicarbonate buffer system is an acid-base homeostatic mechanism involving the balance of carbonic acid (H 2 CO 3), bicarbonate ion (HCO − 3 ), and carbon dioxide (CO 2 ) in order to maintain pH in the blood and duodenum , among other tissues, to support proper metabolic function. [ 1 ]
In inorganic chemistry, bicarbonate (IUPAC-recommended nomenclature: hydrogencarbonate [2]) is an intermediate form in the deprotonation of carbonic acid. It is a polyatomic anion with the chemical formula H C O − 3. Bicarbonate serves a crucial biochemical role in the physiological pH buffering system. [3]
Carbonic acid is a chemical compound with the chemical formula H 2 C O 3. ... as a function of pH. [8] [9] ... Carbonic acid/bicarbonate/carbonate equilibrium in ...
For the carbonic acid-bicarbonate buffer, a molar ratio of weak acid to weak base of 1:20 produces a pH of 7.4; and vice versa—when the pH of the extracellular fluids is 7.4 then the ratio of carbonic acid to bicarbonate ions in that fluid is 1:20. [14]
In plants, carbonic anhydrase helps raise the concentration of CO 2 within the chloroplast in order to increase the carboxylation rate of the enzyme RuBisCO. This is the reaction that integrates CO 2 into organic carbon sugars during photosynthesis, and can use only the CO 2 form of carbon, not carbonic acid or bicarbonate. [citation needed]
Carbonic anhydrase catalyzes the conversion of carbon dioxide and water into carbonic acid. This molecule breaks down into bicarbonate and hydrogen ions. This break down process occurs in red blood cells. Ultimately, the concentration of bicarbonate ions in the bloodstream affects the formation of the protein carbaminohemoglobin in the body. [11]
Aqueous carbon dioxide reacts with water to form carbonic acid which is very unstable and will dissociate rapidly into hydronium and bicarbonate. Therefore, in seawater, dissolved inorganic carbon is commonly referred to as the collection of bicarbonate, carbonate ions, and dissolved carbon dioxide (CO 2, H 2 CO 3, HCO − 3, CO 2− 3).
Carbonic acid then spontaneously dissociates to form bicarbonate Ions (HCO 3 −) and a hydrogen ion (H +). In response to the decrease in intracellular pCO 2, more CO 2 passively diffuses into the cell. Cell membranes are generally impermeable to charged ions (i.e. H +, HCO 3 −) but RBCs are able to exchange bicarbonate for chloride using ...