Bicarbonate

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Overview

In inorganic chemistry, a bicarbonate (IUPAC-recommended nomenclature: hydrogencarbonate) is an intermediate form in the deprotonation of carbonic acid.

Chemical properties

The bicarbonate ion (hydrogen carbonate) is an anion with the empirical formula HCO₃⁻ and a molecular mass of 61.01 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 base of carbonic acid, H₂CO₃; it is the conjugate acid of CO₃²⁻, the carbonate ion as shown by these equilibrium reactions.

CO₃^2- +2 H₂O ⇋ HCO₃^1- + H₂O + OH^1- ⇋ H₂CO₃ +2 OH^1-

H₂CO₃ +2 H₂O ⇋ HCO₃^1- + H₃O¹⁺ + H₂O ⇋ CO₃^2- +2 H₃O¹⁺

A bicarbonate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic compound. Many bicarbonates are 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.

Physiological role

Bicarbonate is a crucial component of the pH buffering system of the body (maintaining homeostasis). 86%-90% of CO₂ in the body is converted into carbonic acid (H₂CO₃), which can quickly turn into bicarbonate (HCO₃^-).

With carbonic acid as the central intermediate species, bicarbonate, in conjunction with water, hydrogen ions, and carbon dioxide forms this buffering system which is maintained at the volatile 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.)

Other uses

The most common salt of the bicarbonate ion is sodium bicarbonate, NaHCO₃, 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.

The flow of bicarbonate ions from rocks weathered by the carbonic acid in rainwater is an important part of the carbon cycle.

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.

Bicarbonate Compounds

• Sodium bicarbonate
• Potassium bicarbonate
• Calcium bicarbonate
• Ammonium bicarbonate
• Carbonic anhydrase

See also

• Carbon dioxide
• Carbonic acid
• Carbonate
• Hard water
• Blood gas

External links

• MeSH Bicarbonates

cs:Hydrogenuhličitan de:Hydrogencarbonatefr:Bicarbonate he:ביקרבונטfi:Vetykarbonaatti sv:Vätekarbonatjon

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Acknowledgement and Attribution Regarding Sources of Content

Some of the initial content on this page may be incorporated in part from copyleft sources in the public domain including wikis such as Wikipedia and AskDrWiki. Drug information for patients came from the The National Library of Medicine. Infectious disease information may have come from the Centers for Disease Control (CDC). Differential Diagnoses are drawn from clinicians as well as an amalgamation of 3 sources: 1.The Disease Database; 2. Kahan, Scott, Smith, Ellen G. In A Page: Signs and Symptoms. Malden, Massachusetts: Blackwell Publishing, 2004:3; 3. Sailer, Christian, Wasner, Susanne. Differential Diagnosis Pocket. Hermosa Beach, CA: Borm Bruckmeir Publishing LLC, 2002:7 .