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'{{Other uses|Sodium peroxycarbonate}} {{chembox | Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 464402772 | Name = | ImageFile = | 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|correct|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<nowiki>&middot;</nowiki>1.5 H₂O₂ | MolarMass = 156.982 g/mol | Appearance = white solid | Density = | MeltingPt = | BoilingPt = | Solubility = 150 g/l | SolubleOther = | Solvent = | pKb = }} | Section3 = | Section4 = | Section5 = | Section6 = | 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]]<br/>[[Sodium bicarbonate]] | OtherCations = [[Calcium percarbonate]]<br/>[[Magnesium percarbonate]] | OtherFunction = | OtherFunction_label = | OtherCompounds = [[Sodium perborate]]<br/>[[Sodium persulfate]]<br/>[[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 [[wikt:perhydrate|perhydrate]]) whose formula is more properly written as 2&nbsp;{{chem|Na|2|CO|3}}&nbsp;·&nbsp;1.5&nbsp;{{chem|H|2|O|2}}. It is a colorless, crystalline, [[hygroscopic]] and water-soluble solid.<ref name = "Jones">{{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}}</ref> It is sometimes abbreviated as '''SPC'''. It contains 32.5% by weight of hydrogen peroxide. The product is used in some [[eco-friendly]] [[bleach]]es and other [[cleaning product]]s. ==History== Sodium percarbonate was first prepared in 1899 by [[Russian Empire|Russian]] chemist [[Sebastian Moiseevich Tanatar]] (7 October 1849 – 30 November 1917).<ref>S. Tanatar (1899) [http://gallica.bnf.fr/ark:/12148/bpt6k90753b/f193.image.langEN "Percarbonate"], ''Berichte der Deutschen chemischen Gesellschaft zu Berlin'', '''32''' : 1544–1546.</ref> ==Structure== At 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&nbsp;°C.<ref name="prit1"> {{cite journal | title = Sodium percarbonate between 293 and 100 K |author1=R. G. Pritchard |author2=E. Islam |name-list-style=amp | journal = [[Acta Crystallographica Section B]] | volume = B59 | issue = 5 | pages = 596–605 | year = 2003 | url = | doi = 10.1107/S0108768103012291 |pmid=14586079 }} </ref> ==Chemistry== Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and [[oxygen]]), [[sodium]] [[cation]]s {{chem|Na|+}}, and [[carbonate]] {{chem|CO|3|2-}}.<ref name = "Jones"/><ref name="rscvanish" /> : <chem> 2Na2CO3*3H2O2 -> 3H2O2 + 4Na+ + 2CO3^2- </chem> : <chem> 2H2O2 -> 2H2O + O2 </chem> ==Production== Sodium percarbonate is produced industrially by crystallization of a solution of sodium carbonate and hydrogen peroxide, with proper control of the [[pH]] and concentrations.<ref name="prit0">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}}</ref><ref name="prit1"/><ref name=ajames>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.</ref> This is also a convenient laboratory method. Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.<ref name=kimpat>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</ref> It may also be formed from a process starting from sodium peroxide When absolute ethyl alcohol reacts with sodium peroxide at 0° C. a perhydroxide is produced. C2H5OH + Na2O2 - O:NaOH + C2H5ONa. Carbon dioxide converts it into sodium hydrogen percarbonate. World production capacity of this compound was estimated at several hundred thousand tons for 2004.<ref name = Ullmann>{{Ullmann | title = Peroxo Compounds, Inorganic | author = Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort | doi = 10.1002/14356007.a19_177.pub2}}</ref> ==Uses== As an [[oxidizing agent]], sodium percarbonate is an ingredient in a number of home and [[laundry detergent|laundry cleaning]] products, including non-chlorine [[bleach]] products such as [[Oxyper]], [[OxiClean]], [[Tide (detergent)|Tide laundry detergent]],<ref name = "Jones"/> and [[Vanish (stain remover)|Vanish]].<ref name="rscvanish">"[http://www.chemistryinyourcupboard.org/vanish/4 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).</ref> 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 {{citation needed|date=May 2017}} and can be adjusted to any percentage the user desires. Sodium percarbonate is also used as a cleaning agent by many home brewers. <ref name="Sodium Percarbonate | MoreBeer">{{cite web |title=Sodium Percarbonate |url=https://www.morebeer.com/products/sodium-percarbonate.html |website=MoreBeer.com |accessdate=26 June 2020}}</ref> 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.<ref name="mckill">{{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 = 6145–6166 | year = 1995 | doi = 10.1016/0040-4020(95)00304-Q | issue = 22}}</ref> A method for generating [[trifluoroperacetic acid]] ''in situ'' for use in [[Baeyer–Villiger oxidation]]s 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.<ref>{{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}}</ref><ref>{{cite encyclopedia|doi = 10.1002/047084289X.rt254.pub2|encyclopedia = [[Encyclopedia of Reagents for Organic Synthesis|e-EROS Encyclopedia of Reagents for Organic Synthesis]]|chapter = Trifluoroperacetic Acid|first1 = Kenneth C.|title = Encyclopedia of Reagents for Organic Synthesis|last1 = Caster|first2 = A. Somasekar|last2 = Rao|first3 = H. Rama|last3 = Mohan|first4 = Nicholas A.|last4 = McGrath|first5 = Matthew|last5 = Brichacek|year = 2012|isbn = 978-0471936237}}</ref> ==References== {{reflist}} ==External links== * [https://www.organic-chemistry.org/chemicals/oxidations/sodiumpercarbonate.shtm Organic Chemistry Portal: Sodium percarbonate] * [https://www.whatsinproducts.com/chemicals/view/1/3259/003313-92-6/Sodium%20percarbonate Consumer Product Information Database: Sodium percarbonate] * [https://belchem.com/Sodium-Percarbonate.php Sodium percarbonate] {{sodium compounds}} [[Category:Sodium compounds]] [[Category:Hydrogen peroxide]] [[Category:Carbonates]] [[Category:Cleaning product components]] [[Category:Antiseptics]] [[Category:Bleaches]] [[Category:Oxidizing agents]]'