Bromic acid
| Bromic acid | |
|---|---|
 | |
 | |
| IUPAC name Bromic acid | |
| Other names Bromic(V) acid | |
| Identifiers | |
| CAS number | 10035-10-6  |
| PubChem | 24445  |
| ChemSpider | 22853 |
| EC number | 232-158-3 |
| MeSH | Bromic+acid |
| ChEBI | CHEBI:49382 |
| ChEMBL | CHEMBL1161635 |
| RTECS number | TP8580000 |
| Gmelin Reference | 25861 |
| Jmol-3D images | {{#if:O[Br](=O)=OO=Br(=O)O|Image 1 Image 2 |
| |
| |
| Properties | |
| Molecular formula | HBrO3 |
| Molar mass | 128.91 g/mol |
| Acidity (pKa) | -2 |
| (verify) (what is: /?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
| Infobox references | |
Bromic acid, also known as hydrogen bromate, is an oxoacid with the molecular formula HBrO3. It only exists in aqueous solution.[1][2] It is a colorless solution that turns yellow at room temperature as it decomposes to bromine.[1][3] Bromic acid and bromates are powerful oxidizing agents and are common ingredients in Belousov-Zhabotinsky reactions.[3][4] Belousov-Zhabotinsky reactions are a classic example of non-equilibrium thermodynamics.
Dissociation
Low concentrations dissociate completely to hydrogen and bromate while high concentrations decompose to form bromine. Bromic acid's high instability can be explained because the electoposively charged hypervalent bromine is connected to the electropositive hydrogen.[5]
Structure
There are several isomers of HBrO3.[5][6] The calculated bond lengths are listed below based on three high level theories G2MP2, CCSD(T), and QCISD(T).[5]
| Species | HOOOBr | HOOBrO | HOBrO2 | HBrO3 |
|---|---|---|---|---|
| Br-O bridged (Å) | 1.867 | 1.919 | 1.844 | ----- |
| Br-O terminal (Å) | ----- | 1.635 | 1.598 | 1.586 |
The large energy barriers between these structures do not make isomerization possible. HOBrO2 is the most stable isomer and is the one pictured above.[6]
Synthesis
Bromic acid is the product of a reaction of barium bromate and sulfuric acid.[1]
- Ba(BrO
3)
2 + H
2SO
4 → HBrO
3 + BaSO
4
Barium sulfate is insoluble in water and forms a precipitate. The aqueous bromic acid can be decanted removing the barium sulfate.
References
- ↑ 1.0 1.1 1.2 The Merck Index: An Encyclopedia of Chemicals, Drugs, and Biologicals. 14th Edition. 2006.
- ↑ Van Nostrand's Scientific Encyclopedia. Glenn D. Considine. Ninth Edition. Volume 1. p 554
- ↑ 3.0 3.1 Recipes for Belousov-Zhabotinsky reagents. J. Chem. Educ., 1991, 68 (4), 320. DOI: 10.1021/ed068p320
- ↑ The Source of the Carbon Monoxide in the Classical Belousov-Zhabotinsky Reaction. J. Phys. Chem. A., 2007, 111 (32), 7805-12 DOI: 10.1021/jp073512+
- ↑ 5.0 5.1 5.2 Theoretical investigation of halogen-oxygen bonding and its implications in halogen chemistry and reactivity. Bioinorganic Chemistry and Applications, 2007, 1, 11/1-11/9
- ↑ 6.0 6.1 A Theoretical Examination of the Isomerization Pathways for HBrO3 Isomers. J. Phys. Chem. A, 2000, 104 (41), 9321-27. DOI: 10.1021/jp001604s