sodium percarbonate
{{Other uses|Sodium peroxycarbonate}}
{{chembox
| Name =
| ImageFile = Sodium-percarbonate-xtal-100K-2x2x2-3D-bs-17.png
| ImageClass = bg-transparent
| ImageCaption = Crystal structure at 100 K
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| ImageSize2 = 300px
| IUPACName = sodium carbonate—hydrogen peroxide (2/3)
| SystematicName =
| OtherNames = Sodium carbonate peroxide,{{cite web|title=Substance Name: Sodium carbonate peroxide|url=https://chem.nlm.nih.gov/chemidplus/rn/15630-89-4|access-date=2021-09-09}} 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|correct|FDA}}
| UNII = Z7G82NV92P
| UNNumber = 3378
| PubChem = 159762
| RTECS = FG0750000
}}
| Section2 = {{Chembox Properties
| Formula = Na2CO3
| MolarMass = 156.982 g/mol
| Appearance = White solid
| Density =
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| Solubility = 150 g/l
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| Solvent =
| pKb =
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| Section7 = {{Chembox Hazards
| ExternalSDS =
| MainHazards = Irritant, oxidizer
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| NFPA-S =
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| FlashPt = Non-flammable
| PEL =
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| 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 or sodium carbonate peroxide is an inorganic compound with the formula {{chem2|2 Na2CO3 * 3 H2O2}}. It is an adduct of sodium carbonate ("soda ash" or "washing soda") and hydrogen peroxide (that is, a perhydrate). It is a colorless, crystalline, hygroscopic, and water-soluble solid.{{cite book | author = Craig W. Jones | title = Applications of Hydrogen Peroxide and Derivatives | year = 1999 | publisher = Royal Society of Chemistry | isbn = 0-85404-536-8}} 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.
History
Sodium percarbonate was first prepared in 1899 by Ukrainian chemist Sebastian Moiseevich Tanatar (7 October 1849 – 30 November 1917).{{cite journal |last1=Tanatar |first1=S. |title=Percarbonate |journal=Berichte der Deutschen Chemischen Gesellschaft zu Berlin |date=1899 |volume=32 |issue=2 |pages=1544–1546 |doi=10.1002/cber.18990320233 |url=https://babel.hathitrust.org/cgi/pt?id=hvd.cl1i1w&view=1up&seq=198&skin=2021 |language=German|url-access=subscription }}
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 °C.
{{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
}}
Chemistry
Production
Sodium percarbonate is produced industrially by crystallization of a solution of sodium carbonate and hydrogen peroxide, with attention to the pH and concentrations.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}}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. This method is also convenient for the laboratory preparation. Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.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
World production capacity of this compound was estimated at several hundred thousand tons for 2004.{{Ullmann | title = Peroxo Compounds, Inorganic | author = Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort | doi = 10.1002/14356007.a19_177.pub2}}
Uses
As an oxidizing agent, sodium percarbonate is an ingredient in a number of home and laundry cleaning products, including non-chlorine bleach products such as Oxyper, OxiClean, Tide laundry detergent, and Vanish."{{usurped|1=[https://web.archive.org/web/20120124185550/http://www.chemistryinyourcupboard.org/vanish/4 Oxygen-based bleaches]}}", The Royal Society of Chemistry, and Reckitt Benckiser (the manufacturers of Vanish).
Many commercial products mix a percentage of sodium percarbonate with sodium carbonate. The average "Oxy" product in the supermarket contains 35–40% sodium percarbonate with about 5% active oxygen when titrated.
Sodium percarbonate is also used as a cleaning agent in homebrewing.{{cite web |title=Sodium Percarbonate |url=https://www.morebeer.com/products/sodium-percarbonate.html |website=MoreBeer.com |accessdate=26 June 2020}}
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.{{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}} 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.{{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_abstract_view.htm?code=B960104&cpage=3&qpage=j_search&spage=j_search&journal=B&vol=17&no=1&page=&year1=1990&year2=1999&view=10&qpage=j_search&abstract=}}{{cite encyclopedia|doi = 10.1002/047084289X.rt254.pub2|encyclopedia = 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}}
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]
{{sodium compounds}}