“Hypobromous acid”的意思、由来-开放百科全书

词条

Hypobromous acid

释义

Synthesis and properties
Uses
References

{{Chembox
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| Watchedfields = changed
| verifiedrevid = 461774490
| ImageFile1 = hypobromous_acid.png
| ImageSize1 =
| ImageFile2 = Hypobromous-acid-3D-vdW.png
| ImageSize2 = 150px
| ImageName2 = Space-filling model of hypobromous acid
| IUPACName = hypobromous acid, bromic(I) acid
| OtherNames =
|Section1={{Chembox Identifiers
| InChIKey1 = CUILPNURFADTPE-UHFFFAOYSA-N
| InChI1 = 1S/BrHO/c1-2/h2H
| CASNo_Ref = {{cascite|changed|??}}
| CASNo = 13517-11-8
| PubChem = 83547
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 75379
| SMILES = OBr
| InChI2 = 1/BrHO/c1-2/h2H
| InChIKey2 = CUILPNURFADTPE-UHFFFAOYAL
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/BrHO/c1-2/h2H
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = CUILPNURFADTPE-UHFFFAOYSA-N
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 29249
|Section2={{Chembox Properties
| Formula = HOBr
| MolarMass = 96.911
| Appearance =
| Density = 2.470 g/cm
| MeltingPt =
| BoilingPtC = 20-25
| Solubility =
| pKa = 8.65
| ConjugateBase = Hypobromite
|Section3={{Chembox Hazards
| MainHazards =
| FlashPt =
| AutoignitionPt =
}}

Hypobromous acid is a very weak and unstable acid with chemical formula of HOBr. It is also called bromic(I) acid, bromanol or hydroxidobromine. It occurs only in solution and has chemical and physical properties that are very similar to those of other hypohalites. Its salts (hypobromites) are also unstable.

Synthesis and properties

Addition of bromine to water gives hypobromous acid and hydrobromic acid (HBr) via a disproportionation reaction.

Br₂ + H₂O {{EqmR}} HOBr + HBr

Hypobromous acid has a pK_a of 8.65 and is therefore only partially dissociated in water at pH 7. Like the acid, hypobromite salts are unstable and undergo a slow disproportionation reaction to yield the respective bromate and bromide salts.

3BrO⁻(aq) → 2Br⁻(aq) + {{chem|BrO|3|−}}(aq)

Uses

HOBr is used as a bleach, an oxidizer, a deodorant, and a disinfectant, due to its ability to kill the cells of many pathogens. The compound is generated in warm-blooded vertebrate organisms especially by eosinophils, which produce it by the action of eosinophil peroxidase, an enzyme which preferentially uses bromide.^[1] Bromide is also used in hot tubs and spas as a germicidal agent, using the action of an oxidizing agent to generate hypobromite in a similar fashion to the peroxidase in eosinophils.

It is especially effective when used in combination with its congener, hypochlorous acid.

References

1. ^{{cite journal |last1=Mayeno |url=http://www.jbc.org/cgi/content/abstract/264/10/5660 |first1=AN |last2=Curran |first2=AJ |last3=Roberts |first3=RL |last4=Foote |first4=CS |title=Eosinophils preferentially use bromide to generate halogenating agents |accessdate=2008-01-12 |format= |work= |journal=The Journal of Biological Chemistry |volume=264 |issue=10 |pages=5660–8 |year=1989 |pmid=2538427}}

5 : Hypobromites|Hydrogen compounds|Oxidizing acids|Oxidizing agents|Halogen oxoacids

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