| 词条 | Sodium percarbonate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 464402772 | ImageFile1 = | ImageSize1 = 250px | ImageFile2 = Sodium-percarbonate-xtal-100K-2003-CM-3D-balls.png | ImageSize2 = 300px | IUPACName = sodium carbonate—hydrogen peroxide (2/3) | SystematicName = | OtherNames = sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 140471 | InChI = 1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1 | InChIKey = MWNQXXOSWHCCOZ-REWHXWOFAO | SMILES = [Na+].[O-]C(=O)OO | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = MWNQXXOSWHCCOZ-UHFFFAOYSA-M | InChIKey1 = MWNQXXOSWHCCOZ-UHFFFAOYSA-M | CASNo = 15630-89-4 | CASNo_Ref = {{cascite|correct|CAS}} | EINECS = 239-707-6 | UNII_Ref = {{fdacite|changed|FDA}} | UNII = Z7G82NV92P | PubChem = 159762 | RTECS = FG0750000 |Section2={{Chembox Properties | Formula = Na2CO3·1.5 H2O2 | MolarMass = 156.982 g/mol | Appearance = white solid | Density = | MeltingPt = | BoilingPt = | Solubility = 150 g/l | SolubleOther = | Solvent = | pKb = |Section7={{Chembox Hazards | ExternalSDS = | EUClass = | MainHazards = Irritant, Oxidizer | NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S = | RPhrases = | SPhrases = | FlashPt = Non-flammable | PEL = |Section8={{Chembox Related | OtherAnions = Sodium carbonate Sodium bicarbonate | OtherCations = Calcium percarbonate Magnesium percarbonate | OtherFunction = | OtherFunction_label = | OtherCompounds = Sodium perborate Sodium persulfate Sodium perphosphate }} Sodium percarbonate is a chemical substance with formula {{chem|Na|2|H|3|CO|6}}. It is an adduct of sodium carbonate ("soda ash" or "washing soda") and hydrogen peroxide (that is, a perhydrate) whose formula is more properly written as 2 {{chem|Na|2|CO|3}} · 3 {{chem|H|2|O|2}}. It is a colorless, crystalline, hygroscopic and water-soluble solid.[1] It is sometimes abbreviated as SPC. It contains 32.5% by weight of hydrogen peroxide. The product is used in some eco-friendly bleaches and other cleaning products, and as a laboratory source of anhydrous hydrogen peroxide. HistorySodium percarbonate was first prepared in 1899 by Russian chemist Sebastian Moiseevich Tanatar ({{lang-ru|Севастьян Моисеевич Танатар}}) (7 October 1849, Odessa – 30 November 1917, Odessa).[2] StructureAt room temperature, solid sodium percarbonate has the orthorhombic crystal structure, with the Cmca crystallographic space group. The structure changes to Pbca as the crystals are cooled below about −30 °C.[3] ChemistryDissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and oxygen), sodium cations {{chem|Na|+}}, and carbonate {{chem|CO|3|2-}}.[1][5]
ProductionSodium percarbonate is produced industrially by crystallization of a solution of sodium carbonate and hydrogen peroxide, with proper control of the pH and concentrations.[4][3][5] This is also a convenient laboratory method. Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.[6] World production capacity of this compound was estimated at several hundred thousand tonnes for 2004.[7] UsesAs an oxidizing agent, sodium percarbonate is an ingredient in a number of home and laundry cleaning products, including non-chlorine bleach products such as OxyBoost, OxiClean, Tide laundry detergent,[1] and Vanish.[8] Many commercial products mix a percentage of sodium percarbonate with sodium carbonate. The average percentage of an "Oxy" product in the supermarket is 65% sodium percarbonate and 35% sodium carbonate. The "ultra boosters" seen on infomercials may contain as much as 80% sodium percarbonate. However, sodium percarbonate is less expensive in its pure form {{fact|date=May 2017}} and can be adjusted to any percentage the user desires. Sodium percarbonate can be used in organic synthesis as a convenient source of anhydrous H2O2, in particular in solvents that cannot dissolve the carbonate but can leach the H2O2 out of it.[9] A method for generating trifluoroperacetic acid in situ for use in Baeyer–Villiger oxidations from sodium percarbonate and trifluoroacetic anhydride has been reported; it provides a convenient and cheap approach to this reagent without the need to obtain highly concentrated hydrogen peroxide.[10][11] Commercial products
References1. ^1 2 {{cite book | author = Craig W. Jones | title = Applications of hydrogen peroxide and its derivatives | year = 1999 | publisher = Royal Society of Chemistry | isbn = 0-85404-536-8}} 2. ^S. Tanatar (1899) "Percarbonate", Berichte der Deutschen chemischen Gesellschaft zu Berlin, 32 : 1544–1546. 3. ^1 {{cite journal | title = Sodium percarbonate between 293 and 100 K|author1=R. G. Pritchard |author2=E. Islam |lastauthoramp=yes | journal = Acta Crystallographica Section B| volume = B59 | issue = 5| pages = 596–605| year = 2003 | url = | doi = 10.1107/S0108768103012291 }} 4. ^J. M. Adams and R. G. Pritchard (1977): "The crystal structure of sodium percarbonate: an unusual layered solid". Acta Crystallographica Section B, volume B33, issue 12, pages 3650–3653. {{doi|10.1107/S0567740877011790}} 5. ^Alun P. James, Graham R. Horne, Richard Roesler, and others (1997): "[https://patents.google.com/patent/US6231828 Process for producing sodium percarbonate]". US Patent US6231828B1, priority date 1997-03-26. 6. ^Sang Ryul Kim, Chong Yun Kwag, Hwan Kee Heo, Jong-Pill Lee (1996): "[https://patents.google.com/patent/US5851420 Process for manufacturing granular sodium percarbonate]". US Patent US5851420A, priority date 1996-02-29 7. ^{{Ullmann | title = Peroxo Compounds, Inorganic | author = Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort | doi = 10.1002/14356007.a19_177.pub2}} 8. ^1 "Oxygen-based bleaches {{webarchive|url=https://web.archive.org/web/20120124185550/http://www.chemistryinyourcupboard.org/vanish/4 |date=2012-01-24 }}", The Royal Society of Chemistry, and Reckitt Benckiser (the manufacturers of Vanish). 9. ^{{cite journal | last1 = McKillop | first1 = A | title = Sodium perborate and sodium percarbonate: Cheap, safe and versatile oxidising agents for organic synthesis | journal = Tetrahedron | volume = 51 | pages = 6145 | year = 1995 | doi = 10.1016/0040-4020(95)00304-Q | issue = 22}} 10. ^{{cite journal|title = New Method of Generating Trifluoroperoxyacetic acid for the Baeyer-Villiger Reaction|first1 = Ho-Jung|last1 = Kang|first2 = Hee-Sun|last2 = Jeong|journal = Bull. Korean Chem. Soc.|volume = 17|issue = 1|year = 1996|pages = 5-6|url = http://journal.kcsnet.or.kr/main/j_search/j_download.htm?code=B960104}} 11. ^{{cite encyclopedia|doi = 10.1002/047084289X.rt254.pub2|encyclopedia = e-EROS Encyclopedia of Reagents for Organic Synthesis|title = Trifluoroperacetic Acid|first1 = Kenneth C.|last1 = Caster|first2 = A. Somasekar|last2 = Rao|first3 = H. Rama|last3 = Mohan|first4 = Nicholas A.|last4 = McGrath|first5 = Matthew|last5 = Brichacek|year = 2012}} External links
7 : Sodium compounds|Peroxides|Carbonates|Cleaning product components|Antiseptics|Bleaches|Oxidizing agents |
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