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{{Other uses|Sodium peroxycarbonate}}
{{chembox {{chembox
| Name =
| verifiedrevid = 433533860
| ImageFile = Sodium-percarbonate-xtal-100K-2x2x2-3D-bs-17.png
| ImageFile1 = Sodium_percarbonate.svg<!--there is a file sodium percarbonate.png which is incorrect so I changed the file name to prevent it dispalying-->
| ImageCaption = Crystal structure at 100 K <ref name="prit1"/>
| ImageSize1 = 250px
| ImageFile1 =
| ImageFile2 = Sodium-percarbonate-xtal-100K-2003-CM-3D-balls.png
| ImageSize2 = 300px | ImageSize1 =
| ImageFile2 =
| IUPACName = sodium carbonate—hydrogen peroxide (2/3)
| ImageSize2 = 300px
| IUPACName = sodium carbonate—hydrogen peroxide (2/3)
| SystematicName = | SystematicName =
| OtherNames = PCS, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate | OtherNames = Sodium carbonate peroxide,<ref>{{cite web|title=Substance Name: Sodium carbonate peroxide|url=https://chem.nlm.nih.gov/chemidplus/rn/15630-89-4|access-date=2021-09-09}}</ref> sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate
| Section1 = {{Chembox Identifiers | Section1 = {{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 13399092 | ChemSpiderID = 140471
| InChI = 1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1 | InChI = 1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1
| InChIKey = MWNQXXOSWHCCOZ-REWHXWOFAO | InChIKey = MWNQXXOSWHCCOZ-REWHXWOFAO
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| InChIKey1 = MWNQXXOSWHCCOZ-UHFFFAOYSA-M | InChIKey1 = MWNQXXOSWHCCOZ-UHFFFAOYSA-M
| CASNo = 15630-89-4 | CASNo = 15630-89-4
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| EINECS = 239-707-6 | EINECS = 239-707-6
| UNII_Ref = {{fdacite|correct|FDA}}
| PubChem = 159762
| InChI = | UNII = Z7G82NV92P
| RTECS = | UNNumber = 3378
| PubChem = 159762
}}
| RTECS = FG0750000
| Section2 = {{Chembox Properties
}}
| Formula = Na<sub>2</sub>CO<sub>3</sub><nowiki>&middot;</nowiki>1.5H<sub>2</sub>O<sub>2</sub>
| Section2 = {{Chembox Properties
| MolarMass = 157.01 g/mol
| Formula = Na<sub>2</sub>CO<sub>3</sub><nowiki>·</nowiki>1.5 H<sub>2</sub>O<sub>2</sub>
| Appearance = white solid
| MolarMass = 156.982 g/mol
| Density =
| Appearance = White solid
| MeltingPt =
| BoilingPt = | Density =
| MeltingPt =
| Solubility = 150 g/l
| SolubleOther = | BoilingPt =
| Solubility = 150 g/l
| Solvent =
| pKb = | SolubleOther =
| Solvent =
}}
| pKb =
| Section7 = {{Chembox Hazards
}}
| ExternalMSDS =
| EUClass = | Section3 =
| EUIndex = Not listed | Section4 =
| Section5 =
| MainHazards = Irritant, Oxidizer
| NFPA-H = | Section6 =
| Section7 = {{Chembox Hazards
| NFPA-F =
| NFPA-R = | ExternalSDS =
| MainHazards = Irritant, oxidizer
| NFPA-O =
| RPhrases = | NFPA-H =
| SPhrases = | NFPA-F =
| NFPA-R =
| FlashPt = Non-flammable
| PEL = | NFPA-S =
| HPhrases =
}}
| PPhrases =
| Section8 = {{Chembox Related
| GHS_ref =
| OtherAnions = ]<br/>]
| FlashPt = Non-flammable
| OtherCations =
| OtherFunctn = | PEL =
}}
| Function =
| Section8 = {{Chembox Related
| OtherCpds = ]<br/>]<br/>]
| OtherAnions = ]<br />]
| OtherCations = ]<br />]
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| OtherFunction_label =
| OtherCompounds = ]<br />]<br />]
}} }}
}} }}


'''Sodium percarbonate''' is a ], an ] of ] and ] (a ]), with formula Na<sub>2</sub>CO<sub>3</sub> · 1.5H<sub>2</sub>O<sub>2</sub>. 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 = ] | isbn = 0854045368}}</ref> It is used in some ] cleaning products and as a laboratory source of ] hydrogen peroxide. '''Sodium percarbonate''' or '''sodium carbonate peroxide''' is a ] with empirical formula {{chem2|Na2H3CO6}}. It is an ] of ] ("soda ash" or "washing soda") and ] (that is, a ]) whose formula is more properly written as {{chem2|2 Na2CO3 * 3 H2O2}}. It is a colorless, crystalline, ] and water-soluble solid.<ref name = "Jones">{{cite book | author = Craig W. Jones | title = Applications of hydrogen peroxide and derivatives | year = 1999 | publisher = ] | 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 ] ]es and other ]s.<ref name = "Jones"/>
This product contains the ] ], and should not be confused with sodium ] Na<sub>2</sub>CO<sub>4</sub> or ] Na<sub>2</sub>C<sub>2</sub>O<sub>6</sub>, which contain different anions.

==History==
Sodium percarbonate was first prepared in 1899 by ] chemist ] (7 October 1849 – 30 November 1917).<ref>{{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}}</ref>


==Structure== ==Structure==
At room temperature, solid sodium percarbonate has the ] ], with the ''Cmca'' crystallographic ]. The structure changes to ''Pbca'' as the crystals are cooled below about −30 °C.<ref name="prit1"> At room temperature, solid sodium percarbonate has the ] ], with the ''Cmca'' crystallographic ]. The structure changes to ''Pbca'' as the crystals are cooled below about −30&nbsp;°C.<ref name="prit1">
{{cite journal {{cite journal
| title = Sodium percarbonate between 293 and 100 K | title = Sodium percarbonate between 293 and 100 K
| author = R. G. Pritchard and E. Islam | author1=R. G. Pritchard
| author2=E. Islam
| journal = ]
| name-list-style=amp
| volume = B59
| journal = ]
| issue =
| pages = 596–605 | volume = B59
| year = 2003 | issue = 5
| url = | pages = 596–605
| year = 2003
| doi = 10.1107/S0108768103012291 }}
| url =
</ref>
| 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 ]), ] ]s ({{chem|Na|+}}), and ] ({{chem|CO|3|2-}}).<ref name = "Jones"/><ref name="rscvanish" />

:{{chem2|2 Na2CO3 * 3 H2O2 -> 3 H2O2 + 4 Na+ + 2 CO3(2-)}}
:{{chem2|2 H2O2 -> 2 H2O + O2}}


==Production== ==Production==
Sodium percarbonate is produced industrially by crystallization of a solution of sodium carbonate and hydrogen peroxide, with proper control of the ] 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): "". US Patent US6231828B1, priority date 1997-03-26.</ref> This is also a convenient laboratory method.
Sodium percarbonate is produced industrially by reaction of sodium carbonate and hydrogen peroxide, followed by crystallization. Also, dry sodium carbonate may be reacted directly with concentrated hydrogen peroxide solution. World production capacity of this compound was estimated at several hundred thousand tonnes 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> It can be obtained in the laboratory by reacting the two substances in aqueous solution with proper control of the ].<ref name="prit0">

{{cite journal
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): "". US Patent US5851420A, priority date 1996-02-29</ref>
| title = The crystal structure of sodium percarbonate: an unusual layered solid

| author = J. M. Adams and R. G. Pritchard
It may also be formed from a process starting from sodium peroxide; when absolute ethyl alcohol reacts with sodium peroxide at 0{{nbsp}}°C, a perhydroxide is produced.{{citation needed|date=September 2021}}
| journal = ]

| volume = B33
:{{chem2|C2H5OH + Na2O2 -> NaOOH + C2H5ONa}}
| issue =

| pages = 3650–3653
Carbon dioxide converts it into sodium hydrogen percarbonate.
| year = 1977

| url =
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>
| doi = 10.1107/S0567740877011790 }} </ref> or concentrations.<ref name="prit1"/>


==Uses== ==Uses==
Sodium percarbonate is an ] and ingredient in a number of home and ] products, including ] products such as ] and ].<ref name = "Jones"/> It contains no phosphorus or nitrogen. Dissolved in water, it yields a mixture of hydrogen peroxide (which eventually decomposes to water and ]) and sodium carbonate ("soda ash").<ref name = "Jones"/> As an ], sodium percarbonate is an ingredient in a number of home and ] products, including non-chlorine ] products such as ], ], ],<ref name = "Jones"/> and ].<ref name="rscvanish">" {{webarchive|url=https://web.archive.org/web/20120124185550/http://www.chemistryinyourcupboard.org/vanish/4 |date=2012-01-24 }}", The ], and ] (the manufacturers of Vanish).</ref>


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 can be used in ] as a convenient source of anhydrous H<sub>2</sub>O<sub>2</sub>, in particular in solvents that cannot dissolve the carbonate but can leach the H<sub>2</sub>O<sub>2</sub> 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 | year = 1995 | doi = 10.1016/0040-4020(95)00304-Q}}</ref>

Sodium percarbonate is also used as a cleaning agent in ].<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 ] as a convenient source of anhydrous H<sub>2</sub>O<sub>2</sub>, in particular in solvents that cannot dissolve the carbonate but can leach the H<sub>2</sub>O<sub>2</sub> 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 ] ''in situ'' for use in ]s from sodium percarbonate and ] 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 = ]|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=}}</ref><ref>{{cite encyclopedia|doi = 10.1002/047084289X.rt254.pub2|encyclopedia = ]|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== ==References==
{{reflist}} {{reflist}}


==External links== ==External links==
* *
*
* {{HPD|2888}}
{{sodium compounds}}


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Latest revision as of 00:32, 28 December 2024

For other uses, see Sodium peroxycarbonate.
Sodium percarbonate

Crystal structure at 100 K
Names
IUPAC name sodium carbonate—hydrogen peroxide (2/3)
Other names Sodium carbonate peroxide, sodium carbonate sesquiperhydrate, PCS, SPC, solid hydrogen peroxide, Sodium carbonate hydrogen peroxide, sodium carbonate peroxyhydrate
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.036.082 Edit this at Wikidata
EC Number
  • 239-707-6
PubChem CID
RTECS number
  • FG0750000
UNII
UN number 3378
CompTox Dashboard (EPA)
InChI
  • InChI=1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1Key: MWNQXXOSWHCCOZ-UHFFFAOYSA-M
  • InChI=1S/CH2O4.Na/c2-1(3)5-4;/h4H,(H,2,3);/q;+1/p-1Key: MWNQXXOSWHCCOZ-REWHXWOFAO
  • Key: MWNQXXOSWHCCOZ-UHFFFAOYSA-M
SMILES
  • .C(=O)OO
Properties
Chemical formula Na2CO3·1.5 H2O2
Molar mass 156.982 g/mol
Appearance White solid
Solubility in water 150 g/l
Hazards
Occupational safety and health (OHS/OSH):
Main hazards Irritant, oxidizer
Flash point Non-flammable
Related compounds
Other anions Sodium carbonate
Sodium bicarbonate
Other cations Calcium percarbonate
Magnesium percarbonate
Related compounds Sodium perborate
Sodium persulfate
Sodium perphosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Infobox references
Chemical compound

Sodium percarbonate or sodium carbonate peroxide is a chemical substance with empirical formula Na2H3CO6. 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 Na2CO3 · 3 H2O2. It is a colorless, crystalline, hygroscopic and water-soluble solid. 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).

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.

Chemistry

Dissolved in water, sodium percarbonate yields a mixture of hydrogen peroxide (which eventually decomposes to water and oxygen), sodium cations (Na
), and carbonate (CO
3).

2 Na2CO3 · 3 H2O2 → 3 H2O2 + 4 Na + 2 CO2−3
2 H2O2 → 2 H2O + O2

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. This is also a convenient laboratory method.

Alternatively, dry sodium carbonate may be treated directly with concentrated hydrogen peroxide solution.

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 → NaOOH + C2H5ONa

Carbon dioxide converts it into sodium hydrogen percarbonate.

World production capacity of this compound was estimated at several hundred thousand tons for 2004.

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.

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.

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. 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.

References

  1. ^ R. G. Pritchard & E. Islam (2003). "Sodium percarbonate between 293 and 100 K". Acta Crystallographica Section B. B59 (5): 596–605. doi:10.1107/S0108768103012291. PMID 14586079.
  2. "Substance Name: Sodium carbonate peroxide". Retrieved 2021-09-09.
  3. ^ Craig W. Jones (1999). Applications of hydrogen peroxide and derivatives. Royal Society of Chemistry. ISBN 0-85404-536-8.
  4. Tanatar, S. (1899). "Percarbonate". Berichte der Deutschen Chemischen Gesellschaft zu Berlin (in German). 32 (2): 1544–1546. doi:10.1002/cber.18990320233.
  5. ^ "Oxygen-based bleaches Archived 2012-01-24 at the Wayback Machine", The Royal Society of Chemistry, and Reckitt Benckiser (the manufacturers of Vanish).
  6. 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
  7. Alun P. James, Graham R. Horne, Richard Roesler, and others (1997): "Process for producing sodium percarbonate". US Patent US6231828B1, priority date 1997-03-26.
  8. Sang Ryul Kim, Chong Yun Kwag, Hwan Kee Heo, Jong-Pill Lee (1996): "Process for manufacturing granular sodium percarbonate". US Patent US5851420A, priority date 1996-02-29
  9. Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort. "Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3527306732.{{cite encyclopedia}}: CS1 maint: multiple names: authors list (link)
  10. "Sodium Percarbonate". MoreBeer.com. Retrieved 26 June 2020.
  11. McKillop, A (1995). "Sodium perborate and sodium percarbonate: Cheap, safe and versatile oxidising agents for organic synthesis". Tetrahedron. 51 (22): 6145–6166. doi:10.1016/0040-4020(95)00304-Q.
  12. Kang, Ho-Jung; Jeong, Hee-Sun (1996). "New Method of Generating Trifluoroperoxyacetic acid for the Baeyer-Villiger Reaction". Bull. Korean Chem. Soc. 17 (1): 5–6.
  13. Caster, Kenneth C.; Rao, A. Somasekar; Mohan, H. Rama; McGrath, Nicholas A.; Brichacek, Matthew (2012). "Trifluoroperacetic Acid". Encyclopedia of Reagents for Organic Synthesis. e-EROS Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rt254.pub2. ISBN 978-0471936237.

External links

Sodium compounds
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Halides
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