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Hydrobromic acid
Ball-and-stick model of hydrogen bromide	Ball-and-stick model of water
Ball-and-stick model of the bromide anion	Ball-and-stick model of the hydronium cation
Names
	IUPAC name Bromane
	Other names Hydronium bromide ; Bromhydric acid
Identifiers
CAS Number	10035-10-6 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:47266 ;
ChEMBL	ChEMBL1231461;
ChemSpider	255 ;
ECHA InfoCard	100.240.772
EC Number	233-113-0;
Gmelin Reference	620
KEGG	C13645;
PubChem CID	260;
RTECS number	MW3850000;
UNII	3IY7CNP8XJ ;
UN number	1048 1788
	InChI InChI=1S/BrH/h1H Key: CPELXLSAUQHCOX-UHFFFAOYSA-N ; InChI=1/BrH/h1H Key: CPELXLSAUQHCOX-UHFFFAOYAZ;
	SMILES [OH3+].[Br-];
Properties
Chemical formula	HBr(aq)
Molar mass	80.91 g·mol−1
Appearance	colorless liquid; (impure samples can appear yellowish)
Odor	acrid
Density	1.49 g/cm3 (48% w/w aq.)
Melting point	−11 °C (12 °F; 262 K) (47–49% w/w aq.)
Boiling point	122 °C (252 °F; 395 K) at 700 mmHg (47–49% w/w aq.)
Solubility in water	221 g/100 mL (0 °C) ; 204 g/100 mL (15 °C) ; 130 g/100 mL (100 °C)
Acidity (pKa)	−9
Viscosity	0.84 cP (−75 °C)
Thermochemistry
Heat capacity (C)	29.1 J/(K·mol)
Std molar; entropy (S⦵298)	198.7 J/(K·mol)
Std enthalpy of; formation (ΔfH⦵298)	−36.3 kJ/mol
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H314, H335
Precautionary statements	P260, P261, P264, P271, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P312, P321, P363, P403+P233, P405, P501
NFPA 704 (fire diamond)	3 0 0 ACID
Flash point	Non-flammable
Safety data sheet (SDS)	ICSC 0282
Related compounds
Other anions	Hydrofluoric acid; Hydrochloric acid; Hydroiodic acid
Related compounds	Hydrogen bromide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Hydrobromic acid is an aqueous solution of hydrogen bromide. It is a strong acid formed by dissolving the diatomic molecule hydrogen bromide (HBr) in water. "Constant boiling" hydrobromic acid is an aqueous solution that distills at 124.3 °C (255.7 °F) and contains 47.6% HBr by mass, which is 8.77 mol/L. Hydrobromic acid is one of the strongest mineral acids known.

Uses

Hydrobromic acid is mainly used for the production of inorganic bromides, especially the bromides of zinc, calcium, and sodium. It is a useful reagent for generating organobromine compounds. Certain ethers are cleaved with HBr. It also catalyzes alkylation reactions and the extraction of certain ores. Industrially significant organic compounds prepared from hydrobromic acid include allyl bromide, tetrabromobis(phenol), and bromoacetic acid. HBr almost uniquely participates in anti-Markovnikov hydrohalogenation of alkenes. The resulting 1-bromoalkanes are versatile alkylating agents, giving rise to fatty amines and quaternary ammonium salts.^[3]

Synthesis

Hydrobromic acid can be prepared in the laboratory via the reaction of Br₂, SO₂, and water.^[4]

{\ce {Br2 + SO2 + 2 H2O -> H2SO4 + 2 HBr}}

More typically laboratory preparations involve the production of anhydrous HBr, which is then dissolved in water.

Hydrobromic acid has commonly been prepared industrially by reacting bromine with either sulfur or phosphorus and water. However, it can also be produced electrolytically.^[4] It can also be prepared by treating bromides with non-oxidising acids like phosphoric or acetic acids.

Alternatively the acid can be prepared with dilute (5.8M) sulfuric acid and potassium bromide:^[5]

{\ce {H2SO4 + KBr -> KHSO4 + HBr}}

Using more concentrated sulfuric acid or allowing the reaction solution to exceed 75 °C further oxidizes HBr to elemental bromine. The acid is further purified by filtering out the KHSO₄ and by distilling off the water until the solution reaches an azeotrope (124.3 °C). The yield is approximately 85%.^[5]

Hydrobromic acid is available commercially in various concentrations and purities.

References

^ Favre, Henri A.; Powell, Warren H., eds. (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. Cambridge: The Royal Society of Chemistry. p. 131. ISBN 9781849733069.
^ Bell, R. P. The Proton in Chemistry, 2nd ed., Cornell University Press, Ithaca, NY, 1973.
^ Dagani, M. J.; Barda, H. J.; Benya, T. J.; Sanders, D. C. (2012). "Bromine Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a04_405. ISBN 978-3527306732.
^ ^a ^b Scott, A. (1900). "Preparation of Pure Hydrobromic Acid". Journal of the Chemical Society, Transactions. 77: 648–651. doi:10.1039/ct9007700648.
^ ^a ^b Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry. Vol. 1 (2nd ed.). New York: Academic Press. p. 285. ISBN 978-0121266011.