View source for Sodium perborate

{{chembox
| Watchedfields = changed
| verifiedrevid = 477200388
| ImageFile = Disodium perborate dimer.png
| ImageClass = skin-invert-image
| ImageSize = 250px
| ImageName = Perborate unit in the "monohydrate"
| IUPACName =
| OtherNames = Sodium peroxoborate,<ref name=Ullmann>{{Ullmann | author = Harald Jakob |display-authors=etal | title = Peroxy Compounds, Inorganic | doi = 10.1002/14356007.a19_177.pub2}}</ref> PBS-1 ("monohydrate"), PBS-4 ("tetrahydrate")
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 4574023
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = Y52BK1W96C
| UNII1_Ref = {{fdacite|correct|FDA}}
| UNII1 = Y9UKD0XE6F
| UNII1_Comment =("monohydrate")
| UNII2_Ref = {{fdacite|correct|FDA}}
| UNII2 = 822HSQ655R
| UNII2_Comment =("tetrahydrate")
| InChI = 1/B2H4O8.2Na/c3-1(4)7-9-2(5,6)10-8-1;;/h3-6H;;/q-2;2*+1
| InChIKey = JBUKJLNBQDQXLI-UHFFFAOYAG
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 30178
| SMILES = [Na+].[Na+].O[B-]1(OO[B-](O)(O)OO1)O
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/B2H4O8.2Na/c3-1(4)7-9-2(5,6)10-8-1;;/h3-6H;;/q-2;2*+1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = JBUKJLNBQDQXLI-UHFFFAOYSA-N
| CASNo = 7632-04-4
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo1 = 10332-33-9
| CASNo1_Comment = ("monohydrate")
| CASNo1_Ref = {{cascite|correct|CAS}}
| CASNo2 = 10486-00-7
| CASNo2_Comment = ("tetrahydrate")
| CASNo2_Ref = {{cascite|correct|CAS}}
| PubChem = 5460514
| RTECS = SC7350000
| UNNumber = 1479
| EINECS = 231-556-4
}}
|Section2={{Chembox Properties
| Formula = {{chem2|NaBO3*''n''H2O}}
| MolarMass = 99.815{{nbsp}}g/mol ("monohydrate");<br />153.86{{nbsp}}g/mol ("tetrahydrate")
| Appearance = White powder
| Odor = Odorless
| Density =
| MeltingPtC = 63
| MeltingPt_notes = ("tetrahydrate")
| BoilingPtC = 130 to 150
| BoilingPt_notes = ("tetrahydrate", decomposes)
| Solubility = 2.15{{nbsp}}g/(100 mL) ("tetrahydrate", 18{{nbsp}}°C)
}}
|Section6={{Chembox Pharmacology
| ATCCode_prefix = A01
| ATCCode_suffix = AB19
}}
|Section7={{Chembox Hazards
| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics1046.htm ICSC 1046]
| MainHazards =
| NFPA-H = 1
| NFPA-F = 1
| NFPA-R = 0
| NFPA-S =
| FlashPt = Non-flammable
| AutoignitionPt =
 }}
}}
{{hatnote|In the following text, hydration states in quotation marks indicate incorrect common names.}}
'''Sodium perborate''' are [[chemical compound]]s with [[chemical formula]]  {{chem2|[Na+]2[B2O4(OH)4](2-)}}(H<sub>2</sub>O)<sub>x</sub>. Commonly encountered salts are the anhydrous form (x = 0) and as a [[hydrate|hexahydrate]] (x = 6).  These two species are sometimes called, respectively, "monohydrate" or '''PBS-1''' and "tetrahydrate" or '''PBS-4''', after the historic assumption that {{chem2|NaBO3}} would be the anhydrous form).<ref name=killop>{{cite journal|first1=Alexander|last1=McKillop|first2=William R.|last2=Sanderson|year=1995|title=Sodium Perborate and Sodium Percarbonate: Cheap, Safe and Versatile Oxidising Agents for Organic Synthesis|journal=Tetrahedron|volume=51|issue=22 |page= 6145-6166|doi=10.1016/0040-4020(95)00304-Q}}</ref> Both the anhydrous and hexahydrate salts are white, odorless, water-soluble solids.<ref name = "Brotherton">{{cite book|author=B.J. Brotherton|chapter=Boron: Inorganic Chemistry|title=Encyclopedia of Inorganic Chemistry|year=1994|editor= R. Bruce King|publisher=John Wiley & Sons|isbn=0-471-93620-0}}</ref>

Peroxyborates are widely used in [[laundry detergent]]s, as one of the [[peroxide-based bleach]]es.

Sodium perborate was first obtained in 1898, independently, by [[Sebastian Tanatar]] and by P. Melikoff and L. Pissadewsky; the researchers prepared sodium perborate by treating sodium borate with a solution of hydrogen peroxide and sodium hydroxide, but Tanatar also obtained sodium perborate by electrolysis of a solution of sodium borate.<ref>{{cite journal |last1=Tanatar |first1=S. |title=Perborate und ihre Konstitution |journal=Zeitschrift für physikalische Chemie (Journal for Physical Chemistry) |date=1898 |volume=26 |pages=132–134 |url=https://babel.hathctrust.org/cgi/pt?id=uva.x002278159&seq=146 |trans-title=Perborates and their composition |language=German}}
* {{cite journal |last1=Tanatar |first1=S. |title=Notiz über Perborate |journal=Zeitschrift für physikalische Chemie |date=1898 |volume=29 |pages=162–166 |url=https://babel.hathitrust.org/cgi/pt?id=uva.x030529723&seq=180 |trans-title=Notice about perborates |language=German}}
* {{cite journal |last1=Tanatar |first1=S. |title=Über Perborate |journal=Zeitschrift für anorganische und allgemeine Chemie (Journal for Inorganic and General Chemistry) |date=1901 |volume=26 |pages=345–347 |url=https://babel.hathitrust.org/cgi/pt?id=mdp.39015072644282&seq=353 |trans-title=About perborates |language=German}}</ref><ref>{{cite journal |last1=Melikoff |first1=P. |last2=Pissadewsky |first2=L. |title=Hypertitanate und Hyperborate |journal=Berichte der Deutschen Chemischen Gesellschaft |date=1898 |volume=31 |pages=678–680 |doi=10.1002/cber.189803101144 |url=https://babel.hathitrust.org/cgi/pt?id=iau.31858002475550&view=1up&page=root&size=100&seq=686&num=143 |language=German}}</ref><ref>{{cite book |last1=Jakob |first1=Harold |last2=Leininger |first2=Stefan |last3=Lehmann |first3=Thomas |last4=Jacobi |first4=Sylvia |last5=Gutewort |first5=Sven |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2007 |publisher=Wiley-VCH Verlag GmbH & Co. |location=Hoboken, New Jersey, USA |volume=A19 |pages=293–324 |chapter=Ch. 26: Peroxo Compounds, Inorganic |doi=10.1002/14356007.a19_177.pub2 }}  See p. 299.</ref> 

==Structure==
Unlike [[sodium percarbonate]], the peroxyborates are not [[adduct]]s of hydrogen peroxide.<ref>{{Greenwood&Earnshaw}}</ref><ref name=Ullmann/> Rather, they contain a [[peroxyborate]] [[anion]] {{chem2|[(B(OH)2OO)2](2-)}}, which consists of a cyclic {{chem2|\sB\sO\sO\sB\sO\sO\s}} core with a pair of [[hydroxy group]]s bonded to each boron atom. The ring adopts a [[cyclohexane conformation|chair conformation]].<ref>{{cite journal |author1=Carrondo, M. A. A. F. de C. T. |author2=Skapski, A. C. |journal= Acta Crystallogr B|volume=34 |page= 3551 |title= Refinement of the X-ray Crystal Structure of the Industrial Bleaching Agent Disodium Tetrahydroxo-di-μ-peroxo-diborate Hexahydrate, Na<sub>2</sub>[B<sub>2</sub>(O<sub>2</sub>)<sub>2</sub>(OH)<sub>4</sub>]·6H<sub>2</sub>O |year= 1978 |doi= 10.1107/S0567740878011565}}</ref> The hexahydrate has the formula {{chem2|Na2H4B2O8*6H2O}}, that is, {{chem2|Na2H16B2O14}} or {{chem2|NaH8BO7}}.<ref name=UllBO>{{cite book |doi=10.1002/14356007.a04_263.pub2 |chapter=Boric Oxide, Boric Acid, and Borates |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2015 |last1=Schubert |first1=David M. |pages=1–32 |isbn=978-3-527-30385-4 }}</ref>

The anhydrous compound is commonly but incorrectly called a "monohydrate" with the historical but misleading formula {{chem2|NaBO3*H2O}}. Instead, a more descriptive formula is {{chem2|Na2[(HO)2B]2(O2)2}}. Likewise, the hexahydrate is usually called "tetrahydrate" and formulated as {{chem2|NaBO3*4H2O}}.<ref name=killop/> Both forms are white, odorless, water-soluble solids.<ref name = "Brotherton"/> The "monohydrate" and the "tetrahydrate" are the commercially important forms.<ref name = "Brotherton"/>

A true tetrahydrate {{chem2|Na2H4B2O8*4H2O}}, traditionally known as the "trihydrate", is also known but has no industrial significance. There is a [[registry number|CAS number]] for each of the three traditional "hydrates", the three "peroxyborate" versions of each (interpreted as a hydrogen peroxide adduct) and the poorly-defined "anhydrate" {{chem2|NaBO3}}, a total of seven.<ref name=Ullmann/>

==Chemistry==
Sodium perborate [[hydrolysis|hydrolyzes]] (i.e. breaks down in contact with water), producing [[hydrogen peroxide]] and [[borate]]:<ref name = "Brotherton"/>
:{{chem2|(HO)2B]2(OO)2)(2-)  +  2 H2O  <->  2 [(HO)2B(OH)(OOH)]-}}
The resulting [[hydroperoxide]] then enter in equilibrium with [[boric acid]] {{chem2|B(OH)3}}, hydrogen peroxide {{chem2|H2O2}}, the [[hydroperoxyl]] anion {{chem2|-OOH}}, and the [[tetrahydroxyborate]] anion {{chem2|[B(OH)4]-}}:<ref name=killop/>
:{{chem2|[B(OH)3(OOH)]- ⇌ B(OH)3 + HO2-}}
:{{chem2|B(OH)3 + HO2- + H2O ⇌ [B(OH)4]- + H2O2}}

As the concentration of the solution increases, other peroxoborate species become significant. With excess {{chem2|H2O2}}, the anions {{chem2|[B(OH)2(OOH)2]-}}, {{chem2|[B(OH)(OOH)3]-}}, and eventually {{chem2|[B(OOH)4]-}} appear. At high borate concentrations, the sodium perborate with dimeric anion crystallizes out, due to its relatively low solubility.<ref name=killop/>

The "monohydrate" form dissolves faster than the "tetrahydrate" and has higher heat stability; it is prepared by heating the "tetrahydrate".<ref name=Ullmann/> The commercial "anhydrate", or ''Oxoborate'', is prepared by further heating of "monohydrate" and actually consists of [[sodium borate]] and boron–oxygen radical.<ref name=Ullmann/>

==Preparation==
Sodium perborate is manufactured by reaction of [[borax]] {{chem2|Na2B4O7}} and [[sodium hydroxide]] NaOH to give [[sodium metaborate]] {{chem2|NaBO2}}, which is then reacted with hydrogen peroxide to give hydrated sodium perborate:<ref name = "Brotherton"/><ref>{{cite web|url=http://www.perborates.eu/docs/PBS_SIP1010.pdf|title=Sodium Perborate REACH Consortium|accessdate=2012-06-07|archive-date=2014-04-26|archive-url=https://web.archive.org/web/20140426234530/http://www.perborates.eu/docs/PBS_SIP1010.pdf|url-status=dead}}</ref>

:{{chem2|Na2B4O7 + 2 NaOH → 4 NaBO2 + H2O}}
:{{chem2|2 NaBO2 + 2 H2O2 → Na2B2O4(OH)4}}

A [[surfactant]] may be added to control crystal size.<ref name=duguaI>J. Dugua and B.Simon (1978): "Crystallization of sodium perborate from aqueous solutions: I. Nucleation rates in pure solution and in presence of a surfactant". ''Journal of Crystal Growth'', volume 44, issue 3, pages 265-279.{{doi|10.1016/0022-0248(78)90025-8}}</ref><ref name=duguaII>J. Dugua and B.Simon (1978): "Crystallization of sodium perborate from aqueous solutions: II. Growth kinetics of different faces in pure solution and in the presence of a surfactant". ''Journal of Crystal Growth'', volume 44, issue 3, pages 280-286.{{doi|10.1016/0022-0248(78)90026-X}}</ref>

It may also be produced in the electrolysis of an aqueous solution containing borax, sodium carbonate and sodium bicarbonate (potassium dichromate is added to improve yield along with sodium silicate). A copper pipe is used as a cathode and platinum for the anode, the current being 6 amperes at 7 to 8 volts, and the temperature 10{{nbsp}}°C.<ref>{{cite web |last1=Paul |first1=Mollard |title=US3038842A Process of making sodium perborate by electrolysis |url=https://patents.google.com/patent/US3038842A/en |website=Google Patents |date=12 June 1962}}</ref>

==Uses==
Sodium perborate serves as a stable source of [[active oxygen]] in many [[detergent]]s, [[laundry detergent]]s, [[cleaning product]]s, and laundry [[bleach]]es.<ref name = "Brotherton"/> It is a less aggressive bleach than [[sodium hypochlorite]] and other [[chlorine-based bleach]]es, causing less degradation to [[dye]]s and [[textile]]s. Sodium perborate releases oxygen rapidly at temperatures greater than 60&nbsp;°C. Addition of the activator, typically [[tetraacetylethylenediamine]] (TAED), makes it active at lower temperatures (40–60&nbsp;°C). 

The compound has [[antiseptic]] properties and can act as a [[disinfectant]]. It is also used as a "disappearing" [[preservative]] in some brands of [[eye drop]]s.{{cn|date=September 2023}}

===Dental use===
Sodium perborate monohydrate is quickly hydrolyzed into [[hydrogen peroxide]] and [[borate]] on contact with water.<ref name = "Brotherton"/> A 1979 double-blind [[crossover study]]<ref name="10.1111/j.1600-051x.1979.tb02190.x">{{cite journal | pmid = 379049 | volume=6 | issue=2 | title=Effect of hydrogen peroxide on developing plaque and gingivitis in man. | date=Apr 1979 | journal=J Clin Periodontol | pages=115–30 | doi=10.1111/j.1600-051x.1979.tb02190.x| last1=Wennstrom | first1=Jan | last2=Lindhe | first2=Jan }}</ref> suggests that [[hydrogen peroxide]], which is released during the use of this product, may prevent or retard colonization and multiplication of anaerobic bacteria, such as those that inhabit oral wounds.

Sodium perborate is also present in some [[tooth bleaching]] formulas for non vital root treated teeth. The compound is inserted in the root canal and left in place for an extended period of time to allow it to diffuse into the tooth and bleach stains from the inside out. However, this use has been banned in the [[European Union]].<ref name=EUban/>

===Organic synthesis===
Sodium perborate is also used as an [[oxidation|oxidizing]] reagent in [[organic synthesis]]. For example, it converts [[thioether]]s into [[sulfoxide]]s and [[sulfone]]s.<ref>{{Citation|last1=McKillop|first1=Alexander|title=Sodium Perborate|date=2008-09-15|url=http://doi.wiley.com/10.1002/047084289X.rs094.pub2|encyclopedia=Encyclopedia of Reagents for Organic Synthesis|pages=rs094.pub2|editor-last=John Wiley & Sons, Ltd|place=Chichester, UK|publisher=John Wiley & Sons, Ltd|language=en|doi=10.1002/047084289x.rs094.pub2|isbn=978-0-471-93623-7|access-date=2021-01-18|last2=Kabalka|first2=George W.|last3=Reddy|first3=Marepally Srinivasa|url-access=subscription}}</ref> Another use of sodium perborate in organic synthesis is as a convenient alternative to [[Hydrogen peroxide|{{chem2|H2O2}}]], for example in the 2 step conversion of an [[aryl halide]] to a [[Phenols|phenol]] (the first step is a [[Miyaura borylation]]).<ref>[https://www.commonorganicchemistry.com/Patents/BMS/WO2016010950.pdf#page=223.pdf Spirocycloheptanes as inhibitors of rock]</ref>

[[File:Oxidation of Boronate in a 2 step synthesis of a phenol.svg|class=skin-invert-image|800px|thumb|center|Oxidation of Boronate with sodium perborate]]

==Safety==
In the [[European Union]], sodium perborate, like most perborates, was classified as "carcinogenic, mutagenic, or toxic for reproduction" (CMR), category 1B of Regulation (EC) 790/2009, as a result of being included in Part 3 of Annex VI of the regulation 1272/2008 on Classification, Labelling and Packaging (CLP) of substances and mixtures. As a result, their use has been automatically banned in cosmetic products in the EU, in any concentration, starting 1 December 2010. That extends to the use of perborates for tooth whitening.<ref>{{Cite web |title=Substance Information - ECHA |url=https://echa.europa.eu/substance-information/-/substanceinfo/100.035.597 |access-date=2025-01-22 |website=echa.europa.eu |language=en-GB}}</ref><ref name=EUban>Nature Inc. (2015): "Chemical used in beauty salon teeth whitening banned by EU". ''BDJ Team'', volume 2, article 15075, 26 June 2015. {{doi|10.1038/bdjteam.2015.75}}</ref>

==Brands==
===Bocasan===
'''Bocasan''' was an oral wound cleanser manufactured in the [[United Kingdom]] by Knox Laboratories Ltd of London from 1960&ndash;1975,<ref>{{cite web|url=http://www.culturegrid.org.uk/static/showResource/3051671|title=Two sachets of Bocasan mouthwash powder, supplied by Knox la < CultureGrid}}</ref> before being rebranded as an [[Oral-B]] product
<ref>Medicines: The Comprehensive Guide edited by Dr. Ian Morton, Judith M. Hall. Royal Society of Medicine. Bloomsbury Publishing, London, 2002. Pg 118</ref>
[[File:Bocasan dental rinse front.JPG|thumb|Bocasan dental rinse front]]
[[File:Bocasan dental rinse back.JPG|thumb|Bocasan dental rinse back]]
<!--
 belonging to [[Procter & Gamble]] after its recent acquisition of [[Gillette (brand)|Gillette]] (2005). 
-->
Production of Bocasan appears to have ceased by 2003. A similar product, [[Amosan]] was available for a period before also ceasing production in 2010. As of 2013, a [[Netherlands|Dutch]] pharmacy offers the same formulation under the name Bikosan<ref>{{cite web|url=https://www.bik-bik.com/info/14/bikosan-replaces-bocasan|title = Home ⋆ Bik & Bik Online Pharmacy}}</ref>

It was used to aid treatment, in adults or children over 5 years old, of [[periodontal]] conditions such as [[canker sores]], [[denture irritation]], orthodontic irritation, or after dental procedures.

Bocasan was packaged in a 1.7 gram envelope, and contained 69.72% sodium perborate monohydrate and 29.68% sodium hydrogen tartrate anhydrous. To use, the contents were dissolved in 30 cubic centimetres of warm water. Half the amount was swilled around the mouth for two minutes and discarded, and the procedure repeated with the remainder. Treatment was recommended three times a day after meals.

A 1979 double-blind crossover study<ref>{{cite journal | pmid = 379049 | volume=6 | issue=2 | title=Effect of hydrogen peroxide on developing plaque and gingivitis in man | date=April 1979 | journal=Journal of Clinical Periodontology | pages=115–30 | doi=10.1111/j.1600-051x.1979.tb02190.x| last1=Wennstrom | first1=Jan | last2=Lindhe | first2=Jan }}<!-- says H2O2, but measures Amosan. Classic.--></ref> suggests that [[hydrogen peroxide]], which is released during the use of this product, may prevent or retard colonization and multiplication of anaerobic bacteria, such as those that inhabit oral wounds. A small (n=12) 1998 RCT shows that Bocasan combined with [[chlorhexidine]] mouthwash is better than chlorhexidine alone in preventing plaque.<ref>{{cite journal |last1=Dona |first1=BL |last2=Gründemann |first2=LJ |last3=Steinfort |first3=J |last4=Timmerman |first4=MF |last5=van der Weijden |first5=GA |title=The inhibitory effect of combining chlorhexidine and hydrogen peroxide on 3-day plaque accumulation. |journal=Journal of Clinical Periodontology |date=November 1998 |volume=25 |issue=11 Pt 1 |pages=879–83 |doi=10.1111/j.1600-051x.1998.tb02385.x |pmid=9846796}}<!-- Title says H2O2, but read the abstract! --></ref> A further study (n=28) shows that Bocasan reduces the staining associated with chlorhexidine.<ref>{{cite journal |last1=Gründemann |first1=LJ |last2=Timmerman |first2=MF |last3=Ijzerman |first3=Y |last4=van der Weijden |first4=GA |last5=van der Weijden |first5=GA |title=Stain, plaque and gingivitis reduction by combining chlorhexidine and peroxyborate. |journal=Journal of Clinical Periodontology |date=January 2000 |volume=27 |issue=1 |pages=9–15 |doi=10.1034/j.1600-051x.2000.027001009.x |pmid=10674956}}</ref>

====Drug facts====
*'''Active ingredient''': [[Sodium perborate monohydrate]] 
*'''Inactive ingredients''': [[Sodium hydrogen tartrate]]
*'''Purpose''': Oral cleanser
*'''Normal use''': Use up to three times daily, after meals or as directed by a dentist

===Amosan===
[[File:Amosan Oral Antiseptic Rinse 2014 - Product Photo.jpg|thumb|right|Amosan Oral Antiseptic Rinse, 2014]]
'''Amosan'''<ref name=AmosanCA>{{cite web |url=http://www.amosan.ca/ |title=Home |website=amosan.ca}}</ref> is an oral [[antiseptic]] [[oral rinse|rinse]]. It contains 68.635% [[sodium perborate monohydrate]] by weight. Sold as a powder customarily packaged in 1.7g envelopes, it reconstitution with warm water, after which it is used as a mouth rinse. It is used to aid in the prevention of, as well as speed the recovery from [[canker sores]], [[denture irritation]], orthodontic irritation, and oral injuries or after dental procedures.

==== History ====
Amosan was originally made by [[Oral-B]]; a mention of the powder appeared in the February 6, 1970 [[Federal Register]].<ref>[https://www.govinfo.gov/content/pkg/FR-1970-02-06/pdf/FR-1970-02-06.pdf Federal register]</ref> Between 2005 and 2010, Amosan was manufactured in [[Belgium]] and sold under the Oral-B brand, belonging to [[Procter & Gamble]] after its 2005 acquisition of Gillette. In December 2010, its use was banned in the EU, as the product is based on borate, which the union considers "carcinogenic, mutagenic, or toxic for reproduction".<ref name=EUban>Nature Inc. (2015): "Chemical used in beauty salon teeth whitening banned by EU". ''BDJ Team'', volume 2, article 15075, 26 June 2015. {{doi|10.1038/bdjteam.2015.75}}</ref>

Vintage Brands Limited began manufacturing and selling Amosan Oral Antiseptic Rinse in 2014 because many consumers were disappointed that it was no longer available.<ref name=FB-Amosan>[https://www.facebook.com/AmosanOralProducts Amosan Oral Products] Facebook {{User-generated source|certain=yes|date=March 2022}}</ref> Product review pages on Amazon<ref name="amazon">{{cite web |url= https://www.amazon.com/Amosan-Oral-Wound-Cleanser-Powder/dp/B000GGHT52 |title= Amosan Oral Wound Cleanser Powder |publisher= Amazon |website= Amazon.com}}</ref> and public comment forums elsewhere<ref name="mouthulcers">{{cite web|url=http://www.mouthulcers.org/messages.php?thread=1463|title=Bocasan/Amosan|publisher=Mouthulcers.org}}</ref> indicate a high level of frustration with the discontinuation by users who could find no effective alternative treatment.

In April 2012, it was reported that [[Shoppers Drug Mart]] in Canada had produced a comparable product under their house brand: 'Life Brand Oral Wound Cleanser'.<ref name=Pharamaprix-057800802228>{{cite web |url=http://www1.shoppersdrugmart.ca/en/health-and-pharmacy/personal-care/oral-lip-care/details/057800802228 |access-date=2014-09-25 |archive-url=https://web.archive.org/web/20160304040826/http://www1.shoppersdrugmart.ca/en/health-and-pharmacy/personal-care/oral-lip-care/details/057800802228 |archive-date=2016-03-04 |url-status=dead |title= Life Brand Oral Wound Cleanser Mouthwash 1.7g x 20 Sachets SKU 057800802228 |publisher= Shopper Drug Mart / Pharmaprix }}</ref> Also, Jean Coutu and Rexall has their own house brand versions.

====Drug facts====
* '''Active ingredient''': [[Sodium perborate monohydrate]] 1.2 g
* '''Inactive ingredients''': L-[[Tartaric acid]], [[sodium saccharin]], flavors
* '''Purpose''': Oral wound cleanser
* '''Normal use''': Use up to 4 times daily, after meals and before bedtime or as directed by a dentist or physician

==See also==
* [[Amosan]]
* [[Sodium percarbonate]]
* [[Persil]]

==References==
{{reflist}}
{{notelist}}

== External links ==
* [https://web.archive.org/web/20051123101005/http://www.borax.com/detergents/bleaching.html Borax Detergent Book: Bleaching]
* [https://web.archive.org/web/20060209040519/http://www.npi.gov.au/database/substance-info/profiles/15.html National Pollutant Inventory - Boron and compounds]
* [http://history.evonik.com/sites/geschichte/en/chemicals/inventions/degussa/sodium-perborate/Pages/default.aspx Sodium perborate history, image] {{Webarchive|url=https://web.archive.org/web/20110407065711/http://history.evonik.com/sites/geschichte/en/chemicals/inventions/degussa/sodium-perborate/pages/default.aspx |date=2011-04-07 }}
* [https://www.organic-chemistry.org/chemicals/oxidations/sodiumperborate.shtm Sodium perborate in organic synthesis]

{{Stomatological preparations}}
{{sodium compounds}}
{{Borates}}

[[Category:Sodium compounds]]
[[Category:Borates]]
[[Category:Peroxides]]
[[Category:Cleaning product components]]
[[Category:Antiseptics]]
[[Category:Bleaches]]
[[Category:Oxidizing agents]]