Back بيربورات الصوديوم Arabic سودیوم پربورات AZB Натриев перборат Bulgarian Perborat de sodi Catalan Natriumperborat German Natria perborato Esperanto Perborato de sodio Spanish Sodio perborato Basque سدیم پربورات Persian Perborate de sodium French
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| Names | |
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| Other names
Sodium peroxoborate,[1] PBS-1 ("monohydrate"), PBS-4 ("tetrahydrate")
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.035.597 |
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PubChem CID
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| RTECS number |
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| UNII |
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| UN number | 1479 |
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| Properties | |
| NaBO3·nH2O | |
| Molar mass | 99.815 g/mol ("monohydrate"); 153.86 g/mol ("tetrahydrate") |
| Appearance | White powder |
| Odor | Odorless |
| Melting point | 63 °C (145 °F; 336 K) ("tetrahydrate") |
| Boiling point | 130 to 150 °C (266 to 302 °F; 403 to 423 K) ("tetrahydrate", decomposes) |
| 2.15 g/(100 mL) ("tetrahydrate", 18 °C) | |
| Pharmacology | |
| A01AB19 (WHO) | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Safety data sheet (SDS) | ICSC 1046 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium perborate are chemical compounds with chemical formula [Na+]2[B2O4(OH)4]2−(H2O)x. Commonly encountered salts are the anhydrous form (x = 0) and as a hexahydrate (x = 6). These two species are sometimes called, respectively, "monohydrate" or PBS-1 and "tetrahydrate" or PBS-4, after the historic assumption that NaBO3 would be the anhydrous form).[2] Both the anhydrous and hexahydrate salts are white, odorless, water-soluble solids.[3]
Peroxyborates are widely used in laundry detergents, as one of the peroxide-based bleaches.
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.[4][5][6]
- ^ Harald Jakob; et al. "Peroxy Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_177.pub2. ISBN 978-3527306732.
- ^ McKillop, Alexander; Sanderson, William R. (1995). "Sodium Perborate and Sodium Percarbonate: Cheap, Safe and Versatile Oxidising Agents for Organic Synthesis". Tetrahedron. 51: 6145-6166. doi:10.1016/0040-4020(95)00304-Q.
- ^ B.J. Brotherton (1994). "Boron: Inorganic Chemistry". In R. Bruce King (ed.). Encyclopedia of Inorganic Chemistry. John Wiley & Sons. ISBN 0-471-93620-0.
- ^ Tanatar, S. (1898). "Perborate und ihre Konstitution" [Perborates and their composition]. Zeitschrift für physikalische Chemie (Journal for Physical Chemistry) (in German). 26: 132–134.
- Tanatar, S. (1898). "Notiz über Perborate" [Notice about perborates]. Zeitschrift für physikalische Chemie (in German). 29: 162–166.
- Tanatar, S. (1901). "Über Perborate" [About perborates]. Zeitschrift für anorganische und allgemeine Chemie (Journal for Inorganic and General Chemistry) (in German). 26: 345–347.
- ^ Melikoff, P.; Pissadewsky, L. (1898). "Hypertitanate und Hyperborate". Berichte der Deutschen Chemischen Gesellschaft (in German). 31: 678–680.
- ^ Jakob, Harold; Leininger, Stefan; Lehmann, Thomas; Jacobi, Sylvia; Gutewort, Sven (2007). "Ch. 26: Peroxo Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Vol. A19. Hoboken, New Jersey, USA: Wiley‐VCH Verlag GmbH & Co. pp. 293–324. doi:10.1002/14356007.a19_177.pub2. See p. 299.