Hydrobromic acid
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Names | |||
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IUPAC name
Bromane[1]
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Other names
Hydronium bromide
Bromhydric acid | |||
Identifiers | |||
3D model (
JSmol ) |
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ChEBI | |||
ChEMBL | |||
ChemSpider | |||
ECHA InfoCard
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100.240.772 | ||
EC Number |
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620 | |||
KEGG | |||
PubChem CID
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RTECS number
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UNII | |||
UN number | 1048 1788 | ||
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Properties | |||
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.) | ||
221 g/100 mL (0 °C) 204 g/100 mL (15 °C) 130 g/100 mL (100 °C) | |||
Acidity (pKa) | −9[2] | ||
Viscosity | 0.84 cP (−75 °C) | ||
Thermochemistry | |||
Heat capacity (C)
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29.1 J/(K·mol) | ||
Std molar
entropy (S⦵298) |
198.7 J/(K·mol) | ||
Std enthalpy of (ΔfH⦵298)formation |
−36.3 kJ/mol | ||
Hazards | |||
GHS labelling: | |||
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Danger | |||
H314, H335 | |||
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) | |||
Flash point | Non-flammable | ||
Safety data sheet (SDS) | ICSC 0282 | ||
Related compounds | |||
Other anions
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Hydrofluoric acid Hydrochloric acid Hydroiodic acid | ||
Related compounds
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Hydrogen bromide | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hydrobromic acid is an
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
Synthesis
Hydrobromic acid can be prepared in the laboratory via the reaction of Br2, SO2, and water.[4]
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 (5.8
Using more concentrated sulfuric acid or allowing the reaction solution to exceed 75 °C further
Hydrobromic acid is available commercially in various concentrations and purities.
References
- ISBN 9781849733069.
- ^ Bell, R. P. The Proton in Chemistry, 2nd ed., Cornell University Press, Ithaca, NY, 1973.
- ISBN 978-3527306732.
- ^ .
- ^ ISBN 978-0121266011.
External links
Media related to Hydrogen bromide at Wikimedia Commons