Bicarbonate - wikipedia Bicarbonate This is the current revision of this page, as edited by InternetArchiveBot ( talk contribs ) at 18 : 49, 19 July 2017 ( Rescuing 1 sources and tagging 0 as dead. # IABot ( v1. 4.2 ) ). The present address ( URL ) is a permanent link to this version. Revision as of 18 : 49, 19 July 2017 by InternetArchiveBot ( talk contribs ) ( Rescuing 1 sources and tagging 0 as dead. # IABot ( v1. 4.2 ) ) ( diff ) ← Previous revision Latest revision ( diff ) Newer revision → ( diff ) For baking soda, see sodium bicarbonate. For the programming principle, see Tim Toady Bicarbonate. `` Hydrogen carbonate '' redirects here. For the oxoacid, see carbonic acid. Bicarbonate Names Systematic IUPAC name Hydroxidodioxidocarbonate ( 1 − ) Other names Hydrogencarbonate Identifiers CAS Number 71 - 52 - 3 3D model ( JSmol ) Interactive image 3DMet B00080 Beilstein Reference 3903504 ChEBI CHEBI : 17544 ChemSpider 749 Gmelin Reference 49249 KEGG C00288 PubChem CID 769 UNII HN1ZRA3Q20 InChI InChI = 1S / CH2O3 / c2 - 1 ( 3 ) 4 / h ( H2, 2, 3, 4 ) / p - 1 Key : BVKZGUZCCUSVTD - UHFFFAOYSA - M SMILES OC ( ( O - ) ) = O Properties Chemical formula HCO − 3 Molar mass 61.0168 g mol log P − 0.82 Acidity ( pK ) 10.3 ( Conjugate acid of carbonate ) Basicity ( pK ) 7.7 ( Conjugate base of carbonic acid ) Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). Infobox references In inorganic chemistry, bicarbonate ( IUPAC - recommended nomenclature : hydrogencarbonate ) 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. The term `` bicarbonate '' was coined in 1814 by the English chemist William Hyde Wollaston. The prefix `` bi '' in `` bicarbonate '' comes from an outdated naming system and is based on the observation that there is twice as much carbonate ( CO 2 − 3 ) per sodium ion in sodium bicarbonate ( NaHCO ) and other bicarbonates than in sodium carbonate ( Na CO ) and other carbonates. The name lives on as a trivial name. Contents 1 Chemical properties 2 Physiological role 3 Bicarbonate in the environment 4 Other uses 5 Diagnostics 6 Bicarbonate compounds 7 See also 8 References 9 External links Chemical properties The bicarbonate ion ( hydrogencarbonate ion ) is an anion with the empirical formula HCO − 3 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. It is isoelectronic with nitric acid HNO 3. The bicarbonate ion carries a negative one formal charge and is the conjugate base of carbonic acid H 2CO 3 ; at the same time, it is the conjugate acid of CO 2 − 3, the carbonate ion, as shown by these equilibrium reactions : CO 2 − 3 + 2 H O ⇌ HCO − 3 + H O + OH ⇌ H CO + 2 OH H CO + 2 H O ⇌ HCO − 3 + H O + H O ⇌ CO 2 − 3 + 2 H O. 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 ; in particular, sodium bicarbonate contributes to total dissolved solids, a common parameter for assessing water quality. Physiological role CO produced as a waste product of the oxidation of sugars in the mitochondria reacts with water in a reaction catalyzed by carbonic anhydrase to form H CO, which is in equilibrium with the cation H and anion HCO. It is then carried to the lung, where the reverse reaction occurs and CO gas is released. In the kidney ( left ), cells ( green ) lining the proximal tubule conserve bicarbonate by transporting it from the glomerular filtrate in the lumen ( yellow ) of the nephron back into the blood ( red ). The exact stoichiometry in the kidney is omitted for simplicity. Bicarbonate ( HCO − 3 ) is alkaline, and a vital component of the pH buffering system of the human body ( maintaining acid -- base homeostasis ). 70 -- 75 % of CO in the body is converted into carbonic acid ( H CO ), which can quickly turn into bicarbonate. 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 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 acidic chyme entering the duodenum from the stomach. Bicarbonate in the environment Bicarbonate is the dominant form of dissolved inorganic carbon in sea water, and in most fresh waters. As such it is an important sink in the carbon cycle. In freshwater ecology, strong photosynthetic activity by freshwater plants in daylight releases gaseous oxygen into the water and at the same time produces bicarbonate ions. These shift the pH upward until in certain circumstances the degree of alkalinity can become toxic to some organisms or can make other chemical constituents such as ammonia toxic. In darkness, when no photosynthesis occurs, respiration processes release carbon dioxide, and no new bicarbonate ions are produced, resulting in a rapid fall in pH. Other uses The most common salt of the bicarbonate ion is sodium bicarbonate, NaHCO, which is commonly known as baking soda. When heated or 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 much 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. It is measured, along with carbon dioxide, chloride, potassium, and sodium, to assess electrolyte levels in an electrolyte panel test ( which has Current Procedural Terminology, CPT, code 80051 ). The parameter standard bicarbonate concentration ( SBC ) is the bicarbonate concentration in the blood at a P CO of 40 mmHg ( 5.33 kPa ), full oxygen saturation and 36 ° C. Reference ranges for blood tests, comparing blood content of bicarbonate ( shown in blue at right ) with other constituents. Bicarbonate compounds Sodium bicarbonate Potassium bicarbonate Caesium bicarbonate Magnesium bicarbonate Calcium bicarbonate Ammonium bicarbonate Carbonic acid See also Carbon dioxide Carbonate Carbonic anhydrase Hard water Arterial blood gas References ^ Jump up to : `` hydrogencarbonate ( CHEBI : 17544 ) ''. Chemical Entities of Biological Interest ( ChEBI ). UK : European Institute of Bioinformatics. IUPAC Names. Jump up ^ Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005 ( PDF ), IUPAC, p. 137 ^ Jump up to : `` Clinical correlates of pH levels : bicarbonate as a buffer ''. Biology.arizona.edu. October 2006. Jump up ^ William Hyde Wollaston ( 1814 ) `` A synoptic scale of chemical equivalents, '' Philosophical Transactions of the Royal Society, 104 : 1 - 22. On page 11, Wollaston coins the term `` bicarbonate '' : `` The next question that occurs relates to the composition of this crystallized carbonate of potash, which I am induced to call bi-carbonate of potash, for the purpose of marking more decidedly the distinction between this salt and that which is commonly called a subcarbonate, and in order to refer at once to the double dose of carbonic acid contained in it. '' Jump up ^ http://www.newton.dep.anl.gov/askasci/chem99/chem99492.htm Jump up ^ Berne & Levy, Principles of Physiology Jump up ^ `` The chemistry of ocean acidification : OCB - OA ''. www.whoi.edu. Woods Hole Oceanographic Institution. 24 September 2012. Retrieved 17 May 2017. Jump up ^ Acid Base Balance ( page 3 ) Archived 2002 - 06 - 13 at the Wayback Machine. External links Look up bicarbonate in Wiktionary, the free dictionary. Bicarbonates at the US National Library of Medicine Medical Subject Headings ( MeSH ) Oxocarbons Common oxides CO CO 2 Exotic oxides CO 3 CO 4 CO 5 CO 6 C 2O C 2O 2 C 2O 3 C 2O 4 C 2O 4 C 3O C 3O 2 C 3O 3 C 3O 6 C 4O 2 C 4O 4 C 4O 6 C 5O 2 C 5O 5 C 6O 6 C 6O 6 C 8O 8 C 9O 9 C 10 O 8 C 10 O 10 C 12 O 6 C 12 O 9 C 12 O 12 Polymers Graphite oxide C O CO CO Compounds derived from oxides Metal carbonyls Carbonic acid Bicarbonates Carbonates Dicarbonates Tricarbonates Reference ranges for blood tests ( CPT 82000 -- 84999 ) Electrolytes Sodium Potassium Chloride Calcium Renal function Creatinine Urea BUN - to - creatinine ratio Plasma osmolality Serum osmolal gap Acid - base Anion gap Arterial blood gas Base excess Bicarbonate CO content Iron tests Ferritin Serum iron Transferrin saturation Total iron - binding capacity Transferrin Transferrin receptor Hormones ACTH stimulation test Thyroid function tests Thyroid - stimulating hormone Metabolism Blood lipids Cardiovascular Cardiac marker Troponin test CPK - MB test Lactate dehydrogenase Myoglobin Glycogen phosphorylase isoenzyme BB Liver function tests Proteins Human serum albumin Serum total protein ALP transaminases ALT AST AST / ALT ratio Bilirubin Unconjugated Conjugated Pancreas Amylase Lipase Pancreatic lipase Inorganic compounds of carbon and related ions Compounds CBr CCl CF CF CI CO CO CO COS CS CS CSe C O C S SiC Carbon ions Carbides ( : C ≡ C : ), ( : : C : : ), ( : C = C = C : ) Cyanides ( : C ≡ N : ) Cyanates ( : O-C ≡ N : ) Thiocyanates ( : S-C ≡ N : ) Fulminates ( : C ≡ N-O : ) Thiofulminates ( : C ≡ N-S : ) Oxides and related Oxides Metal carbonyls Carbonic acid Bicarbonates Carbonates Retrieved from `` https://en.wikipedia.org/w/index.php?title=Bicarbonate&oldid=791358635 '' Categories : Anions Bicarbonates Hidden categories : Webarchive template wayback links Articles without InChI source Articles containing unverified chemical infoboxes All articles with unsourced statements Articles with unsourced statements from March 2011 Talk Article Talk More Contents About Wikipedia In other projects Wikimedia Commons Afrikaans العربية Беларуская Bosanski Català Čeština Dansk Deutsch Eesti Español فارسی Français Gaeilge Galego 한국어 Italiano עברית Кыргызча Magyar Nederlands 日本 語 Norsk Polski Português Română Русский Shqip Simple English Српски / srpski Srpskohrvatski / српскохрватски Suomi Svenska Türkçe Українська اردو 中文 Edit links This page was last edited on 19 July 2017, at 18 : 49. Text is available under the Creative Commons Attribution - ShareAlike License ; additional terms may apply. By using this site, you agree to the Terms of Use and Privacy Policy. Wikipedia ® is a registered trademark of the Wikimedia Foundation, Inc., a non-profit organization. About Wikipedia

Question: compound formed in solution from the negative ion of an acid and the positive ion of a base
Answer: bicarbonate