Hydrogen bromide
Chemical compound From Wikipedia, the free encyclopedia
Hydrogen bromide is the inorganic compound with the formula HBr. It is a hydrogen halide consisting of hydrogen and bromine. A colorless gas, it dissolves in water, forming hydrobromic acid, which is saturated at 68.85% HBr by weight at room temperature. Aqueous solutions that are 47.6% HBr by mass form a constant-boiling azeotrope mixture that boils at 124.3 °C (255.7 °F). Boiling less concentrated solutions releases H2O until the constant-boiling mixture composition is reached.
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| Names | |||
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| IUPAC name
Hydrogen bromide | |||
| Preferred IUPAC name
Bromane[1] | |||
| Identifiers | |||
3D model (JSmol) |
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| 3587158 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| ECHA InfoCard | 100.030.090 | ||
| EC Number |
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| KEGG | |||
| MeSH | Hydrobromic+Acid | ||
PubChem CID |
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| RTECS number |
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| UNII | |||
| UN number | 1048 | ||
CompTox Dashboard (EPA) |
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| Properties | |||
| HBr | |||
| Molar mass | 80.91 g/mol | ||
| Appearance | Colorless gas | ||
| Odor | Acrid | ||
| Density | 3.307 g/L (25 °C)[2] | ||
| Melting point | −86.9 °C (−124.4 °F; 186.2 K) | ||
| Boiling point | −66.8 °C (−88.2 °F; 206.3 K) | ||
| 221 g/100 mL (0 °C) 204 g/100 mL (15 °C) 193 g/100 mL (20 °C) 130 g/100 mL (100 °C) | |||
| Solubility | Soluble in alcohol, organic solvents | ||
| Vapor pressure | 2.308 MPa (at 21 °C) | ||
| Acidity (pKa) | −8.8 (±0.8);[3] ~−9[4] | ||
| Basicity (pKb) | ~23 | ||
| Conjugate acid | Bromonium | ||
| Conjugate base | Bromide | ||
Refractive index (nD) |
1.325[citation needed] | ||
| Structure | |||
| Linear | |||
| 820 mD | |||
| Thermochemistry | |||
Heat capacity (C) |
350.7 mJ/(K·g) | ||
Std molar entropy (S⦵298) |
198.696–198.704 J/(K·mol)[5] | ||
Std enthalpy of formation (ΔfH⦵298) |
−36.45...−36.13 kJ/mol[5] | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards |
Highly corrosive | ||
| GHS labelling: | |||
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| Danger | |||
| H314, H335 | |||
| P261, P280, P305+P351+P338, P310 | |||
| NFPA 704 (fire diamond) | |||
| Lethal dose or concentration (LD, LC): | |||
LC50 (median concentration) |
2858 ppm (rat, 1 h) 814 ppm (mouse, 1 h)[6] | ||
| NIOSH (US health exposure limits): | |||
PEL (Permissible) |
TWA 3 ppm (10 mg/m3)[7] | ||
REL (Recommended) |
TWA 3 ppm (10 mg/m3)[7] | ||
IDLH (Immediate danger) |
30 ppm[7] | ||
| Safety data sheet (SDS) | hazard.com | ||
| Related compounds | |||
Related compounds |
Hydrogen fluoride Hydrogen chloride Hydrogen iodide Hydrogen astatide | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hydrogen bromide, and its aqueous solution, hydrobromic acid, are commonly used reagents in the preparation of bromide compounds.
Reactions
Summarize
Perspective
Organic chemistry
Hydrogen bromide and hydrobromic acid are important reagents in the production of organobromine compounds.[8][9][10] In an electrophilic addition reaction, HBr adds to alkenes:
- RCH=CH2 + HBr → R−CHBr−CH3
The resulting alkyl bromides are useful alkylating agents, e.g., as precursors to fatty amine derivatives. Related free radical additions to allyl chloride and styrene give 1-bromo-3-chloropropane and phenylethylbromide, respectively.
Hydrogen bromide reacts with dichloromethane to give bromochloromethane and dibromomethane, sequentially:
- HBr + CH2Cl2 → HCl + CH2BrCl
- HBr + CH2BrCl → HCl + CH2Br2
These metathesis reactions illustrate the consumption of the stronger acid (HBr) and release of the weaker acid (HCl).
Allyl bromide is prepared by treating allyl alcohol with HBr:
- CH2=CHCH2OH + HBr → CH2=CHCH2Br + H2O
HBr adds to alkynes to yield bromoalkenes. The stereochemistry of this type of addition is usually anti:
- RC≡CH + HBr → RC(Br)=CH2
Also, HBr adds epoxides and lactones, resulting in ring-opening.
With triphenylphosphine, HBr gives triphenylphosphonium bromide, a solid "source" of HBr.[11]
- P(C6H5)3 + HBr → [HP(C6H5)3]+Br−
Inorganic chemistry
Vanadium(III) bromide and molybdenum(IV) bromide were prepared by treatment of the higher chlorides with HBr. These reactions proceed via redox reactions:[12]
- 2 VCl4 + 8 HBr → 2 VBr3 + 8 HCl + Br2
Industrial preparation
Hydrogen bromide (along with hydrobromic acid) is produced by combining hydrogen and bromine at temperatures between 200 and 400 °C. The reaction is typically catalyzed by platinum or asbestos.[9][13]
Laboratory synthesis
HBr can be prepared by distillation of a solution of sodium bromide or potassium bromide with phosphoric acid or sulfuric acid:[14]
- KBr + H2SO4 → KHSO4 + HBr
Concentrated sulfuric acid is less effective because it oxidizes HBr to bromine:
- 2 HBr + H2SO4 → Br2 + SO2 + 2 H2O
The acid may be prepared by:
- reaction of bromine with water and sulfur:[14]
- 2 Br2 + S + 2 H2O → 4 HBr + SO2
- bromination of tetralin:[14]
- C10H12 + 4 Br2 → C10H8Br4 + 4 HBr
- reduction of bromine with phosphorous acid:[9]
- Br2 + H3PO3 + H2O → H3PO4 + 2 HBr
Anhydrous hydrogen bromide can also be produced on a small scale by thermolysis of triphenylphosphonium bromide in refluxing xylene.[11]
Hydrogen bromide prepared by the above methods can be contaminated with Br2, which can be removed by passing the gas through a solution of phenol at room temperature in tetrachloromethane or other suitable solvent (producing 2,4,6-tribromophenol and generating more HBr in the process) or through copper turnings or copper gauze at high temperature.[13]
Safety
HBr is highly corrosive and, if inhaled, can cause lung damage.[15]
References
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