Sodium perborate

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Sodium perborate
Perborate dimer, peroxide bond shown in red, charges in blue
Names
Other names
PBS-1 (mono), PBS-4 (tetra)
Identifiers
ATC code A01AB19
7632-04-4 YesY
10332-33-9 (monohydrate) YesY
10486-00-7 (tetrahydrate) YesY
ChEBI CHEBI:30178 YesY
ChemSpider 4574023 YesY
EC number 231-556-4
Jmol-3D images Image
PubChem 5460514
RTECS number SC7350000
UNII Y52BK1W96C YesY
UN number 1479
Properties
NaBO3·nH2O
Molar mass 99.815 g/mol (monohydrate);
153.86 g/mol (tetrahydrate)
Appearance white powders
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)
Hazards
MSDS ICSC 1046
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oil Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point non-flammable
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY verify (what isYesY/N?)
Infobox references

Sodium perborate (PBS) is a white, odorless, water-soluble chemical compound with the chemical formula NaBO3. It crystallizes as the monohydrate, NaBO3·H2O, trihydrate, NaBO3·3H2O and tetrahydrate, NaBO3·4H2O.[1] The monohydrate and tetrahydrate are the commercially important forms.[1] The elementary structural unit of sodium perborates is a dimer anion B2O4(OH)42−, in which two boron atoms are joined by two peroxo bridges in a chair-shaped 6-membered ring, and the simplistic NaBO3·nH2O-type formulas are just a convenient way to express the average chemical composition.

Preparation and chemistry[edit]

Sodium perborate is manufactured by reaction of disodium tetraborate pentahydrate, hydrogen peroxide, and sodium hydroxide.[1] The monohydrate form dissolves better than the tetrahydrate and has higher heat stability; it is prepared by heating the tetrahydrate. Sodium perborate undergoes hydrolysis in contact with water, producing hydrogen peroxide and borate.[1]

Structure[edit]

Unlike sodium percarbonate and perphosphate, the sodium perborate is not simply an adduct with hydrogen peroxide, and it does not contain an individual BO3 ion.[2] Rather, there is a cyclic dimer anion B2O4(OH)42−, in which two boron atoms are joined by two peroxo bridges in a chair-shaped 6-membered ring.[3] This makes the substance more stable, and safer for handling and storage. The formula of the sodium salt is thus Na2H4B2O8.[1]

Uses[edit]

It serves as a source of active oxygen in many detergents, laundry detergents, cleaning products, and laundry bleaches.[1] It is also present in some tooth bleaching formulas. It is used as a bleaching agent for internal bleaching of a non vital root treated tooth. The sodium perborate is placed inside the tooth 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. It has antiseptic properties and can act as a disinfectant. It is also used as a "disappearing" preservative in some brands of eye drops.

Sodium perborate is a less aggressive bleach than sodium hypochlorite, causing less degradation to dyes and textiles. Borates also have some non-oxidative bleaching properties.

Sodium perborate releases oxygen rapidly at temperatures over 60 °C. To make it active at lower temperatures (40–60 °C), it has to be mixed with a suitable activator, typically tetraacetylethylenediamine (TAED).

See also[edit]

References[edit]

  1. ^ a b c d e f B.J Brotherton Boron: Inorganic Chemistry Encyclopedia of Inorganic Chemistry (1994) Ed. R. Bruce King, John Wiley & Sons ISBN 0-471-93620-0
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419. 
  3. ^ Carrondo, M. A. A. F. de C. T.; Skapski, A. C. (1978). "Refinement of the X-ray crystal structure of the industrial bleaching agent disodium tetrahydroxo-di-μ-peroxo-diborate hexahydrate, Na2[B2(O2)2(OH)4]·6H2O". Acta Crystallogr B34: 3551. doi:10.1107/S0567740878011565. 

External links[edit]