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Hydrobromic acid

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Title: Hydrobromic acid  
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Subject: Gold(III) bromide, HBr, Bromous acid, List of MeSH codes (D01), Acid strength
Collection: Acids, Bromides, Mineral Acids, Nonmetal Halides
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Hydrobromic acid

Hydrobromic acid
Identifiers
 Y
ChEBI  Y
ChemSpider  Y
EC number 233-113-0
Jmol-3D images Image
PubChem
RTECS number MW3850000
Properties
HBr
Molar mass 80.91
Appearance colorless/faint yellow liquid
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[1]
Viscosity 0.84 cP (-75 °C)
Thermochemistry
29.1 J/K mol
198.7 J/K mol
-36.3 kJ/mol
Hazards
Safety data sheet ICSC 0282
Corrosive (C)
R-phrases R34, R37
S-phrases (S1/2), S7/9, S26, S45
NFPA 704
0
3
0
Flash point Non-flammable
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).
 N  (: Y/N?)

Hydrobromic acid 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 and contains 47.6% HBr by weight, which is 8.89 mol/L. Hydrobromic acid has a pKa of −9, making it a stronger acid than hydrochloric acid, but not as strong as hydroiodic acid. Hydrobromic acid is one of the strongest mineral acids known.

Contents

  • Uses 1
  • Synthesis 2
  • References 3
  • External links 4

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



  • International Chemical Safety Card 0282
  • NIOSH Pocket Guide to Chemical Hazards
  • Carlin, W. W. U.S. Patent 4,147,601

Media related to at Wikimedia Commons

External links

  1. ^ Bell, R.P. The Proton in Chemistry, 2nd ed., Cornell University Press, Ithaca, NY, 1973.
  2. ^ Dagani, M. J.; Barda, H. J.; Benya, T. J.; Sanders, D. C. (2005), "Bromine Compounds",  
  3. ^ a b Scott, A. (1900). "Preparation of Pure Hydrobromic Acid". Journal of the Chemical Society, Transactions 77: 648–651.  
  4. ^ a b Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 1, 2nd Ed. Newyork: Academic Press. p. 285.  

References

Hydrobromic acid is available commercially in various concentrations and purities.

Using more concentrated sulfuric acid or allowing the reaction solution to exceed 75 °C further [4]

H2SO4 + KBr → KHSO4 + HBr

Alternatively the acid can be prepared with dilute (5.8[4]

Hydrobromic acid has commonly been prepared industrially by reacting bromine with either sulfur or phosphorus and water. However, it can also be produced electrolytically.[3] It can also be prepared by treating bromides with non-oxidising acids like phosphoric or acetic acids.

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

Br2 + SO2 + 2 H2O → H2SO4 + 2 HBr

Hydrobromic acid can be prepared in the laboratory via the reaction of Br2, SO2, and water.[3]

Synthesis

[2]

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