Hydrobromic acid

{{chembox

| Verifiedfields = changed

| Watchedfields = changed

| verifiedrevid = 447182371

| ImageFileL1 = Hydrogen-bromide-3D-vdW.svg

| ImageNameL1 = Ball-and-stick model of hydrogen bromide

| ImageFileR1 = Water molecule 3D.svg

| ImageNameR1 = Ball-and-stick model of water

| ImageFileL2 = Bromide_ion.svg

| ImageNameL2 = Ball-and-stick model of the bromide anion

| ImageFileR2 = Hydronium-3D-vdW.svg

| ImageNameR2 = Ball-and-stick model of the hydronium cation

| ImageFile3 = Hydrobromic acid.jpg

| ImageSize3 = 100px

| Name = Hydrobromic acid

| OtherNames = Hydronium bromide

Bromhydric acid

| IUPACName = Bromane{{cite book|title=Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013|editor-last=Favre |editor-first=Henri A. |editor2-first=Warren H.|editor2-last=Powell|date=2014|publisher=The Royal Society of Chemistry|place=Cambridge|isbn=9781849733069 | page=131}}

| ImageFile =

| ImageSize = 100px

| ImageCaption = A jar containing hydrobromic acid

| ImageName = A jar storing hydrobromic acid inside

| Section1 = {{Chembox Identifiers

| CASNo = 10035-10-6

| CASNo_Ref = {{cascite|correct|CAS}}

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChemSpiderID = 255

| InChI = 1/BrH/h1H

| ChEBI_Ref = {{ebicite|correct|EBI}}

| ChEBI = 47266

| ChEMBL = 1231461

| EINECS = 233-113-0

| Gmelin = 620

| KEGG = C13645

| PubChem = 260

| RTECS = MW3850000

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 3IY7CNP8XJ

| UNNumber = 1048 1788

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChI = 1S/BrH/h1H

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey = CPELXLSAUQHCOX-UHFFFAOYSA-N

| SMILES = [OH3+].[Br-]

| InChIKey = CPELXLSAUQHCOX-UHFFFAOYAZ

}}

| Section2 = {{Chembox Properties

| Formula = HBr_(aq)

| MolarMass = 80.91 g·mol⁻¹

| Appearance = colorless liquid
(impure samples can appear yellowish)

| Odor = acrid

| Density = 1.49 g/cm³ (48% w/w aq.)

| Solubility = 221 g/100 mL (0 °C)
204 g/100 mL (15 °C)
130 g/100 mL (100 °C)

| MeltingPtC = −11

| MeltingPt_notes = (47–49% w/w aq.)

| BoilingPtC = 122

| BoilingPt_notes = at 700 mmHg (47–49% w/w aq.)

| pKa = −9Bell, R. P. The Proton in Chemistry, 2nd ed., Cornell University Press, Ithaca, NY, 1973.

| Viscosity = 0.84 cP (−75 °C)

}}

| Section4 = {{Chembox Thermochemistry

| DeltaHf = −36.3 kJ/mol

| HeatCapacity = 29.1 J/(K·mol)

| Entropy = 198.7 J/(K·mol)

}}

| Section7 = {{Chembox Hazards

| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0282.htm ICSC 0282]

| NFPA-H = 3

| NFPA-F = 0

| NFPA-R = 0

| NFPA-S = ACID

| GHSPictograms = {{GHS05}}{{GHS07}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|314|335}}

| PPhrases = {{P-phrases|260|261|264|271|280|301+330+331|303+361+353|304+340|305+351+338|310|312|321|363|403+233|405|501}}

| FlashPt = Non-flammable

}}

| Section8 = {{Chembox Related

| OtherAnions = Hydrofluoric acid
Hydrochloric acid
Hydroiodic acid

| OtherCompounds = Hydrogen bromide

}}

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 {{convert|124.3|C|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 participates in anti-Markovnikov hydrohalogenation of alkenes in the presence of peroxides. The resulting 1-bromoalkanes are versatile alkylating agents, giving rise to fatty amines and quaternary ammonium salts.{{ Ullmann | author = Dagani, M. J. | author2 = Barda, H. J. | author3 = Benya, T. J. | author4 = Sanders, D. C. | title = Bromine Compounds|year=2012 | doi = 10.1002/14356007.a04_405}}

Synthesis

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

:{{Chem2 | 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.{{ cite journal | author = Scott, A. | title = Preparation of Pure Hydrobromic Acid | journal = Journal of the Chemical Society, Transactions | year = 1900 | volume = 77 | pages = 648–651 | doi = 10.1039/ct9007700648 | url = https://zenodo.org/record/1429698 }} 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:{{cite book|last=Brauer|first=Georg|title=Handbook of Preparative Inorganic Chemistry|volume=1|edition=2nd|date=1963|publisher=Academic Press|location=New York|isbn=978-0121266011|page=285|url=https://books.google.com/books?id=TLYatwAACAAJ&q=Handbook+of+Preparative+Inorganic+Chemistry}}

:{{Chem2 | 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%.

Hydrobromic acid is available commercially in various concentrations and purities.

References

External links

[http://www.inchem.org/documents/icsc/icsc/eics0282.htm International Chemical Safety Card 0282]
[https://www.cdc.gov/niosh/npg/npgd0331.html NIOSH Pocket Guide to Chemical Hazards]
Carlin, W. W. {{US patent|4147601}}

Category:Bromides

Category:Nonmetal halides

Category:Mineral acids

pl:Bromowodór#Kwas bromowodorowy