Hypobromous acid: Difference between revisions
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| verifiedrevid = 461774490 |
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| ImageFile1 = hypobromous_acid.png |
| ImageFile1 = hypobromous_acid.png |
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| ImageFile2 = Hypobromous-acid-3D-vdW.png |
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| ImageCaption2 = {{legend|white|[[Hydrogen]], H}}{{legend|red|[[Oxygen]], O}}{{legend|rgb(160, 64, 64)|[[Bromine]], Br}} |
| ImageCaption2 = {{legend|white|[[Hydrogen]], H}}{{legend|red|[[Oxygen]], O}}{{legend|rgb(160, 64, 64)|[[Bromine]], Br}} |
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| ImageName2 = [[Space-filling model]] of hypobromous acid |
| ImageName2 = [[Space-filling model]] of hypobromous acid |
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| IUPACName = Hypobromous acid |
| IUPACName = Hypobromous acid |
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| OtherNames = {{ubl|Bromanol|Bromic(I) acid|Bromooxidane|Hydroxidobromine}} |
| OtherNames = {{ubl|Bromanol|Bromic(I) acid|Bromooxidane|Hydroxidobromine}} |
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|Section1={{Chembox Identifiers |
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| InChIKey1 = CUILPNURFADTPE-UHFFFAOYSA-N |
| InChIKey1 = CUILPNURFADTPE-UHFFFAOYSA-N |
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| InChI1 = 1S/BrHO/c1-2/h2H |
| InChI1 = 1S/BrHO/c1-2/h2H |
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| ChEBI = 29249 |
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|Section2={{Chembox Properties |
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| Formula = HOBr |
| Formula = HOBr |
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| H=1|O=1|Br=1 |
| H=1|O=1|Br=1 |
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| ConjugateBase = [[Hypobromite]] |
| ConjugateBase = [[Hypobromite]] |
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| MainHazards = {{GHS03}}{{GHS05}}{{GHS06}}{{GHS08}}{{GHS09}} |
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|Section9={{Chembox Related |
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| OtherCations = [[Sodium hypobromite]] |
| OtherCations = [[Sodium hypobromite]] |
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| OtherCompounds = {{ubl|[[Hypofluorous acid]]|[[Hypochlorous acid]]|[[Hypoiodous acid]]|[[Hypobromite]]}} |
| OtherCompounds = {{ubl|[[Hypofluorous acid]]|[[Hypochlorous acid]]|[[Hypoiodous acid]]|[[Hypobromite]]}} |
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Revision as of 14:22, 28 September 2024
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| Names | |
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| IUPAC name
Hypobromous acid
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Other names
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.119.006 |
PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| HOBr | |
| Molar mass | 96.911 g·mol−1 |
| Density | 2.470 g/cm3 |
| Boiling point | 20–25 °C (68–77 °F; 293–298 K) |
| Acidity (pKa) | 8.65[1] |
| Conjugate base | Hypobromite |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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| Related compounds | |
Other cations
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Sodium hypobromite |
Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hypobromous acid is an inorganic compound with chemical formula of HOBr. It is a weak, unstable acid. It is mainly produced and handled in an aqueous solution. It is generated both biologically and commercially as a disinfectant. Salts of hypobromite are rarely isolated as solids.
Synthesis and properties
Addition of bromine to water gives hypobromous acid and hydrobromic acid (HBr(aq)) via a disproportionation reaction.
- Br2 + H2O HOBr + HBr
In nature, hypobromous acid is produced by bromoperoxidases, which are enzymes that catalyze the oxidation of bromide with hydrogen peroxide:[2][3]
- Br− + H2O2 HOBr + OH−
Hypobromous acid has a pKa 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.
- 3 BrO−(aq) → 2 Br−(aq) + BrO−3(aq)
Its chemical and physical properties are similar to those of other hypohalites.
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.[4] 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
- ^ Perrin, D. D., ed. (1982) [1969]. Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 117. ISBN 0-08-029214-3. LCCN 82-16524.
- ^ Ximenes, V. F., Morgon, N. H., & de Souza, A. R. (2015). Hypobromous acid, a powerful endogenous electrophile: Experimental and theoretical studies. Journal of inorganic biochemistry, 146, 61-68.
- ^ Butler, Alison.; Walker, J. V. (1993). "Marine haloperoxidases". Chemical Reviews. 93 (5): 1937–1944. doi:10.1021/cr00021a014.
- ^ Mayeno, AN; Curran, AJ; Roberts, RL; Foote, CS (1989). "Eosinophils preferentially use bromide to generate halogenating agents". The Journal of Biological Chemistry. 264 (10): 5660–8. doi:10.1016/S0021-9258(18)83599-2. PMID 2538427. Archived from the original on 2009-05-26. Retrieved 2008-01-12.