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11-SEPTEMBER-2008 13:54:10 - Bicarbonate November 2007 For baking soda, see Sodium bicarbonate. In inorganic chemistry, bicarbonate IUPAC-recommended nomenclature: hydrogencarbonate is an intermediate form in the deprotonation of carbonic acid. Bicarbonate serves a crucial biochemical role in the physiological pH buffering system.1 Contents 1 Chemical properties 2 Biochemical role 3 Other uses 4 Diagnostics 5 Bicarbonate compounds 6 References 7 See also 8 External links Chemical properties Structure of bicarbonate Structure of bicarbonate 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. CO32- +2 H2O ⇋ HCO3- + H2O + OH- ⇋ H2CO3 +2 OH- H2CO3 +2 H2O ⇋ HCO3- + H3O+ + H2O ⇋ CO32- +2 H3O+ 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. Biochemical role Bicarbonate is an alkaline, and a vital component of the pH buffering system1 of the body maintaining acid-base 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 equilibrium1 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. Bicarbonate also acts to regulate pH in the small intestine. It is released from the pancreas in response to the hormone secretin to neutralize the acid chyme entering the duodenum from the stomach 2 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, sodium bicarbonate releases 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. Ammonium bicarbonate is used in digestive biscuit manufacture. Diagnostics In diagnostic medicine, the blood value of bicarbonate is one of several indicators of the state of acid-base physiology in the body. The parameter Standard bicarbonate concentration SBCe is the bicarbonate concentration in the blood at a CO2 of 5.33kPa, full oxygen saturation and 37 degrees Celsius.3 Bicarbonate compounds Sodium bicarbonate Potassium bicarbonate Calcium bicarbonate Ammonium bicarbonate References ^ a b c http://www.biology.arizona.edu/biochemistry/problem_sets/medph/intro.html Biology.arizona.edu - October 2006. Clinical correlates of pH levels: bicarbonate as a buffer. ^ Berne Levy, Principles of Physiology ^ Acid Base Balance page 3 See also Carbon dioxide Carbonic acid Carbonate Carbonic anhydrase Hard water Arterial blood gas External links Look up Bicarbonate in Wiktionary, the free dictionary. MeSH Bicarbonates v d e Inorganic compounds of carbon Common oxides: CO2 ♦ CO -- Exotic oxides: C3O2 ♦ C2O ♦ CO3 Compounds derived from oxides: Metal carbonyls ♦ Carbonic acid ♦ Bicarbonates ♦ Carbonates Ionic compounds: Cyanides ♦ Isocyanides ♦ Cyanates ♦ Thiocyanates ♦ Isothiocyanates ♦ Carbides Retrieved from http://en..org/wiki/Bicarbonate Categories: SaltsHidden category: Articles needing additional references from November 2007 Views Article Discussion this page History Personal tools Log in / create account Navigation Main page Contents Featured content Current events Random article Search Go Search Interaction Community portal Recent changes Contact Donate to Help Toolbox What links here Related changes Upload file Special pages Printable version Permanent link Cite this page Languages ÄŒesky Deutsch Español Français Italiano עברית Nederlands Polski Português РуÑ?Ñ?кий Suomi Svenska УкраїнÑ?ька ä¸æ–‡ This page was last modified on 6 August 2008, at 20
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