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Sodium perborate
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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 |
| EC Number |
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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.
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