| 词条 | Sodium selenite |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 464403878 | ImageFile = Natriumseleniet t.png | ImageSize = | IUPACName = | OtherNames = |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 23308 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = HIW548RQ3W | InChI = 1/2Na.H2O3Se/c;;1-4(2)3/h;;(H2,1,2,3)/q2*+1;/p-2 | InChIKey = BVTBRVFYZUCAKH-NUQVWONBAC | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 48843 | SMILES = [Na+].[Na+].[O-][Se]([O-])=O | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/2Na.H2O3Se/c;;1-4(2)3/h;;(H2,1,2,3)/q2*+1;/p-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = BVTBRVFYZUCAKH-UHFFFAOYSA-L | CASNo = 10102-18-8 (hydrate: 26970-82-1) | CASNo_Ref = {{cascite|changed|CAS}} | ChEMBL_Ref = {{ebicite|correct|EBI}} | ChEMBL = 112302 | PubChem = 24934 | EINECS = 233-267-9 | RTECS = VS7350000 | UNNumber = 2630 | KEGG_Ref = {{keggcite|changed|kegg}} | KEGG = D10530 |Section2={{Chembox Properties | Na=2 | Se=1 | O=3 | Appearance = colourless solid | Density = 3.1 g/cm3 | MeltingPt = decomposes at 710 °C | BoilingPt = | Solubility = 85 g/100 mL (20 °C) | SolubleOther = insoluble in alcohol, ethanol |Section3={{Chembox Structure | CrystalStruct = tetragonal |Section6={{Chembox Pharmacology | ATCCode_prefix = A12 | ATCCode_suffix = CE02 }} |Section7={{Chembox Hazards | ExternalSDS = ICSC 0698 | EUClass = Very toxic (T+) Dangerous for the environment (N) | RPhrases = {{R23}}, {{R28}}, {{R31}}, {{R43}}, {{R51/53}} | SPhrases = {{S1/2}}, {{S28}}, {{S36/37}}, {{S45}}, {{S61}} | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 0 | FlashPt = |Section8={{Chembox Related | OtherCompounds = Sodium sulfite Sodium selenate Sodium selenide }} Sodium selenite is the inorganic compound with the formula Na2SeO3. This salt is a colourless solid. The pentahydrate Na2SeO3(H2O)5 is the most common water-soluble selenium compound. Synthesis and fundamental reactionsSodium selenite usually is prepared by the reaction of selenium dioxide with sodium hydroxide:[1] SeO2 + 2 NaOH → Na2SeO3 + H2O The hydrate converts to the anhydrous salt upon heating to 40 °C. Akin to the related salt sodium sulfite, Na2SeO3 features a pyramidal dianion SeO32−.[2] Oxidation of this anion gives sodium selenate, Na2SeO4. ApplicationsTogether with the related barium and zinc selenites, sodium selenite is mainly used in the manufacture of colorless glass. The pink color imparted by these selenites cancels out the green color imparted by iron impurities.[3] Because selenium is an essential element, sodium selenite is an ingredient in dietary supplements such as multi-vitamin/mineral products, but supplements that provide only selenium use L-selenomethionine or a selenium-enriched yeast. The US Food and Drug Administration approved a selenium supplement to animal diets; the most common form is sodium selenite for pet foods. According to one article, "not much was known about which selenium compounds to approve for use in animal feeds when the decisions were made back in the 1970s .. At the time the regulatory action was taken, only the inorganic selenium salts (sodium selenite and sodium selenate) were available at a cost permitting their use in animal feed.” [4]SafetySelenium is toxic in high concentrations. As sodium selenite, the chronic toxic dose for human beings was described as about 2.4 to 3 milligrams of selenium per day.[5] In 2000, the U.S. Institute of Medicine set the adult Tolerable upper intake levels (UL) for selenium from all sources - food, drinking water and dietary supplements - at 400 μg/day.[6] The European Food Safety Authority reviewed the same safety question and set its UL at 300 μg/day.[7] See also
References1. ^F. Féher, "Sodium Selenite" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 432. 2. ^{{cite journal|last1=Wickleder|first1=Mathias S.|title=Sodium selenite, Na2SeO3|journal=Acta Crystallographica Section E|volume=58|issue=11|year=2002|pages=i103–i104|issn=1600-5368|doi=10.1107/S1600536802019384}} 3. ^Bernd E. Langner "Selenium and Selenium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry (published on-line in 2000) Wiley-VCH, Weinheim, 2002 {{doi|10.1002/14356007.a23_525}} 4. ^{{cite journal|last1=Schrauzer|first1=GN|title=Nutritional selenium supplements: product types, quality, and safety|journal=Journal of the American College of Nutrition|volume=20|issue=1|pages=1–4|year=2001|pmid=11293463|doi=10.1080/07315724.2001.10719007}} 5. ^{{cite journal|last = Wilber|first = C. G.|title = Toxicology of selenium|year = 1980|journal = Clinical Toxicology|volume = 17|pages = 171–230|doi = 10.3109/15563658008985076|pmid = 6998645|issue = 2|format = Free full text (see p. 211)}} 6. ^{{cite book | last1 = Institute of Medicine | title = Dietary Reference Intakes for Vitamin C, Vitamin E, Selenium, and Carotenoids | chapter = Selenium | publisher = The National Academies Press | year = 2000 | location = Washington, DC | pages = 284–324 | url = https://www.nap.edu/read/9810/chapter/9}} 7. ^{{citation| title = Tolerable Upper Intake Levels For Vitamins And Minerals| publisher = European Food Safety Authority| year = 2006| url = http://www.efsa.europa.eu/sites/default/files/efsa_rep/blobserver_assets/ndatolerableuil.pdf}} External links
5 : Hazardous air pollutants|Selenites|Sodium compounds|Dietary minerals|Dietary supplements |
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