| 词条 | Selenous acid |
| 释义 |
| verifiedrevid = 464388887 | Name = Selenous acid | ImageFile_Ref = {{chemboximage|correct|??}} | ImageFile = Selenous-acid-2D.png | ImageSize = 150 | ImageName = Structural formula | ImageFile1 = Selenous-acid-from-xtal-1971-3D-balls.png | ImageSize1 = 150 | ImageName1 = Ball-and-stick model | IUPACName = Selenous acid Selenic(IV) acid | OtherNames = Selenious acid | Reference = [1] |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 1060 | PubChem = 1091 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = F6A27P4Q4R | KEGG_Ref = {{keggcite|correct|kegg}} | KEGG = D05814 | InChI = 1/H2O3Se/c1-4(2)3/h(H2,1,2,3) | InChIKey = MCAHWIHFGHIESP-UHFFFAOYAW | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 26642 | SMILES = O[Se+]([O-])O | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/H2O3Se/c1-4(2)3/h(H2,1,2,3) | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = MCAHWIHFGHIESP-UHFFFAOYSA-N | CASNo = 7783-00-8 | CASNo_Ref = {{cascite|correct|CAS}} | CASNoOther = | RTECS = | EINECS = |Section2={{Chembox Properties | Formula = H2SeO3 | MolarMass = 128.97 g/mol | Appearance = white hygroscopic crystals | Density = 3.0 g/cm3 | MeltingPt = decomposes at 70°C | ConjugateBase = Hydrogenselenite | pKa = 2.46, 7.3[2] | BoilingPt = | Solubility = very soluble | SolubleOther = soluble in ethanol | MagSus = −45.4·10−6 cm3/mol |Section3={{Chembox Structure | Coordination = | CrystalStruct = |Section7={{Chembox Hazards | ExternalSDS = | NFPA-H = | NFPA-F = | NFPA-R = | RPhrases = | SPhrases = | FlashPt = |Section8={{Chembox Related | OtherCations = sodium selenite | OtherAnions = selenic acid hydrogen selenide | OtherCompounds = sulfurous acid tellurous acid polonous acid }} Selenous acid (or selenious acid) is the chemical compound with the formula H2SeO3. Structurally, it is more accurately described by (HO)2SeO. It is the principal oxoacid of selenium; the other being selenic acid. Formation and propertiesSelenous acid is analogous to sulfurous acid, but it is more readily isolated. Selenous acid is easily formed upon the addition of selenium dioxide to water. As a crystalline solid, the compound can be seen as pyramidal molecules that are interconnected with hydrogen bonds. In solution it is a diprotic acid:[3] {{chem|H|2|SeO|3}} {{eqm}} {{chem|H|+}} + {{chem|HSeO|3|-}} (pKa = 2.62) {{chem|HSeO|3|-}} {{eqm}} {{chem|H|+}} + {{chem|SeO|3|2-}} (pKa = 8.32) It is moderately oxidizing in nature, but kinetically slow. In 1 M {{chem|H|+}}: {{chem|H|2|SeO|3}} + 4 {{chem|H|+}} + 4 e− {{eqm}} Se + 3 {{chem|H|2|O}} (E In 1 M {{chem|OH|-}}: {{chem|SeO|3|2-}} + 4 e− + 3 {{chem|H|2|O}} {{eqm}} Se + 6 {{chem|OH|-}} (E It is used in organic synthesis for the synthesis of 1,2-diketones (e.g. glyoxal).[4] UsesThe major use is in protecting and changing the color of steel, especially steel parts on firearms.[5] The so-called cold-bluing process uses selenous acid, copper(II) nitrate, and nitric acid to change the color of the steel from silver-grey to blue-grey or black. Alternative procedures use copper sulfate and phosphoric acid instead. This process deposits a coating of copper selenide and is fundamentally different from other bluing processes which generate black iron oxide. Some older razor blades were also made of blued steel.[5] Another use for selenious acid is the chemical darkening and patination of copper, brass and bronze, producing a rich dark brown color that can be further enhanced with mechanical abrasion.{{Citation needed|date=September 2009}} It can be use used as an oxidizing agent e.g. in laboratory preparation of glyoxal (ethane-1,2-dione) from glycol. Selenious acid is a key component of the Mecke reagent used for drug checking.[6] Health effectsLike many selenium compounds, selenous acid is highly toxic in excessive quantities, and ingestion of any significant quantity of selenous acid is usually fatal, however it is an approved dietary source in proper amounts. Symptoms of selenium poisoning can occur several hours after exposure, and may include stupor, nausea, severe hypotension and death.[7] References1. ^{{cite book |last= Lide |first= David R. |author-link= |last2= |first2= |author2-link= |publication-date= |year= 1998 |title= Handbook of Chemistry and Physics |edition= 87 |volume= |series= |publication-place= Boca Raton, Florida |place= |publisher= CRC Press |id= |isbn= 0-8493-0594-2 |doi= |oclc= |pages= 4–81 |url= |accessdate=}} {{Hydrogen compounds}}2. ^Ka and pKa for Polyprotic Acids. ucdsb.on.ca 3. ^Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. 4. ^"Glyoxal Bisulfite", Organic Syntheses, Collected Volume 3, p.438 (1955). 5. ^1 {{cite web|url=http://www.inchem.org/documents/pims/chemical/pim483.htm#4.%20USES/HIGH%20RISK%20CIRCUMSTANCES%20OF%20POISONING|last=Scarlato|first=E.A.|author2=Higa, J. |title=SELENIUM (PIM483)|date=28 June 1990|accessdate=29 December 2010}} 6. ^{{cite web |title= Colour Test Reagents-Kits for Preliminary Identification of Drugs of Abuse |url=https://www.ncjrs.gov/pdffiles1/nij/183258.pdf |accessdate= 2012-01-26 |date= 2000-07-01 |publisher= National Institute of Justice}} 7. ^{{cite web|title=Material Safety Data Sheet - Product Name: Reagent for Special Opiates|url=https://www.sirchie.com/msds/NARK20010.pdf|publisher=Sirchie Finger Print Laboratories, Inc.|date=May 12, 2006|archive-url=https://web.archive.org/web/20061018155315/http://www.sirchie.com/msds/NARK20010.pdf|archive-date=October 18, 2006|dead-url=yes}} 5 : Hydrogen compounds|Oxidizing acids|Oxidizing agents|Oxoacids|Selenium compounds |
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