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==Overview==<br />
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In [[inorganic chemistry]], a '''bicarbonate''' ([[IUPAC]]-recommended nomenclature: '''hydrogencarbonate''') is an intermediate form in the [[deprotonation]] of [[carbonic acid]].<br />
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==Chemical properties==<br />
[[Image:Bicarbonate.png|thumb|150px|Structure of bicarbonate]]<br />
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The '''bicarbonate ion (hydrogen carbonate)''' is an [[anion]] with the [[empirical formula]] [[hydrogen|H]][[carbon|C]][[oxygen|O]]<sub>3</sub><sup>&minus;</sup> and a molecular mass of 61.01 [[atomic mass unit|daltons]]; it consists of one central carbon [[atom]] surrounded by three oxygen atoms in a [[trigonal planar]] arrangement, with a hydrogen atom attached to one of the oxygens. The bicarbonate ion carries a negative one [[formal charge]] and is the [[conjugate acid|conjugate base]] of [[carbonic acid]], H<sub>2</sub>CO<sub>3</sub>; it is the conjugate acid of CO<sub>3</sub><sup>2&minus;</sup>, the [[carbonate]] ion as shown by these equilibrium reactions. <br />
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CO<sub>3</sub><sup>2-</sup> +2 H<sub>2</sub>O ⇋ '''HCO<sub>3</sub><sup>1-</sup>''' + H<sub>2</sub>O + OH<sup>1-</sup> ⇋ H<sub>2</sub>CO<sub>3</sub> +2 OH<sup>1-</sup><br />
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H<sub>2</sub>CO<sub>3</sub> +2 H<sub>2</sub>O ⇋ '''HCO<sub>3</sub><sup>1-</sup>''' + H<sub>3</sub>O<sup>1+</sup> + H<sub>2</sub>O ⇋ CO<sub>3</sub><sup>2-</sup> +2 H<sub>3</sub>O<sup>1+</sup><br />
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A bicarbonate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic [[chemical compound|compound]]. Many bicarbonates are [[solubility|soluble]] in [[water]] at [[standard temperature and pressure]], particularly [[sodium bicarbonate]] and [[magnesium bicarbonate]]; both of these substances contribute to [[total dissolved solids]], a common parameter for assessing [[water quality]].<br />
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==Physiological role==<br />
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Bicarbonate is a crucial component of the [[pH]] buffering system of the body (maintaining [[homeostasis]]). 86%-90% of CO<sub>2</sub> in the body is converted into [[carbonic acid]] (H<sub>2</sub>CO<sub>3</sub>), which can quickly turn into bicarbonate (HCO<sub>3</sub><sup>-</sup>). <br />
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With carbonic acid as the [[Reaction intermediate|central intermediate]] [[Chemical species|species]], bicarbonate, in conjunction with water, hydrogen ions, and carbon dioxide forms this buffering system which is maintained at the volatile [[chemical equilibrium|equilibrium]] required to provide prompt resistance to drastic pH changes in both the acidic and basic directions. This is especially important for protecting [[tissues]] of the [[central nervous system]], where pH changes too far outside of the normal range in either direction could prove disastrous. (See [[acidosis]], or [[alkalosis]].)<br />
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==Other uses==<br />
The most common salt of the bicarbonate ion is [[sodium bicarbonate]], NaHCO<sub>3</sub>, which is used as [[baking soda]]. When exposed to an [[acid]] such as [[acetic acid]] ([[vinegar]]), bicarbonates release [[carbon dioxide]]. This is used as a leavening agent in [[baking]].<br />
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The flow of bicarbonate ions from rocks weathered by the carbonic acid in rainwater is an important part of the [[carbon cycle]].<br />
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Bicarbonate also serves in the digestive system. It raises the internal pH of the stomach, after highly acidic digestive juices have finished in their digestion of food.<br />
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== Bicarbonate Compounds ==<br />
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* [[Sodium bicarbonate]]<br />
* [[Potassium bicarbonate]]<br />
* [[Calcium bicarbonate]]<br />
* [[Ammonium bicarbonate]]<br />
* [[Carbonic anhydrase]]<br />
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==See also==<br />
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* [[Carbon dioxide]]<br />
* [[Carbonic acid]]<br />
* [[Carbonate]]<br />
* [[Hard water]]<br />
* [[Blood gas]]<br />
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==External links==<br />
{{Wiktionary}}<br />
* {{MeshName|Bicarbonates}}<br />
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[[Category:Salts]]<br />
[[Category:Biochemistry]]<br />
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