Difference between revisions of "Sulfurous acid"
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| − | '''Sulfurous acid''' is the [[chemical compound]] with the [[chemical formula|formula]] H<sub>2</sub>SO<sub>3</sub>. There is no evidence that sulfurous acid exists in solution, but the molecule has been detected in the gas phase.<ref>{{citation | first1 = | + | '''Sulfurous acid''' is the [[chemical compound]] with the [[chemical formula|formula]] H<sub>2</sub>SO<sub>3</sub>. There is no evidence that sulfurous acid exists in solution, but the molecule has been detected in the gas phase.<ref>{{citation | first1 = Detlev | last1 = Sülzle | first2 = Marjon | last2 = Verhoeven | first3 = Johan K. | last3 = Terlouw | first4 = Helmut | last4 = Schwarz | title = Generation and Characterization of Sulfurous Acid (H<sub>2</sub>SO<sub>3</sub>) and of Its Radical Cation as Stable Species in the Gas Phase | journal = Angew. Chem., Int. Ed. Engl. | volume = 27 | pages = 1533–34 | year = 1988 | doi = 10.1002/anie.198815331}}.</ref> The conjugate bases of this elusive acid are, however, common anions, [[bisulfite]] (or hydrogensulfite) and [[sulfite]]. |
[[Raman spectroscopy|Raman spectra]] of solutions of [[sulfur dioxide]] in water show only signals due to the SO<sub>2</sub> molecule and the bisulfite ion, HSO<sub>3</sub><sup>−</sup>.<ref>{{Jolly2nd|page=227}}.</ref> The intensities of the signals are consistent with the following [[chemical equilibrium|equilibrium]]: | [[Raman spectroscopy|Raman spectra]] of solutions of [[sulfur dioxide]] in water show only signals due to the SO<sub>2</sub> molecule and the bisulfite ion, HSO<sub>3</sub><sup>−</sup>.<ref>{{Jolly2nd|page=227}}.</ref> The intensities of the signals are consistent with the following [[chemical equilibrium|equilibrium]]: | ||
Latest revision as of 19:14, 23 August 2009
| Sulfurous acid | |
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| IUPAC name | Sulfurous acid |
| Identifiers | |
| InChI | InChI=1/H2O3S/c1-4(2)3/h(H2,1,2,3) |
| InChIKey | LSNNMFCWUKXFEE-UHFFFAOYAJ |
| Standard InChI | InChI=1S/H2O3S/c1-4(2)3/h(H2,1,2,3) |
| Standard InChIKey | LSNNMFCWUKXFEE-UHFFFAOYSA-N |
| CAS number | [] |
| EC number | |
| ChemSpider | |
| Properties | |
| Chemical formula | H2SO3 |
| Molar mass | 82.07 g/mol |
| Hazards[1] | |
| Material safety data sheet (MSDS) | ICSC |
| EU index number | 016-011-00-9 |
| GHS pictograms |  
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| GHS signal word | DANGER |
| GHS hazard statements | H331, H314 |
| Flash point | Non-flammable |
| Related compounds | |
| Other compounds | Sulfur dioxide Sulfuric acid |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Sulfurous acid is the chemical compound with the formula H2SO3. There is no evidence that sulfurous acid exists in solution, but the molecule has been detected in the gas phase.[2] The conjugate bases of this elusive acid are, however, common anions, bisulfite (or hydrogensulfite) and sulfite.
Raman spectra of solutions of sulfur dioxide in water show only signals due to the SO2 molecule and the bisulfite ion, HSO3−.[3] The intensities of the signals are consistent with the following equilibrium:
- SO2 + H2O ⇌ HSO3− + H+
- Ka = 1.54 × 10−2; pKa = 1.81.
- SO2 + H2O ⇌ HSO3− + H+
Aqueous solutions of sulfur dioxide, which sometimes are referred to as sulfurous acid are used as reducing agents and as disinfectants, as are solutions of bisulfite and sulfite salts. They are also mild bleaches, and are used for materials which may be damaged by chlorine-containing bleaches.
References
- ↑ Index no. 016-011-00-9 of Annex VI, Part 3, to Regulation (EC) No 1272/2008 of the European Parliament and of the Council of 16 December 2008 on classification, labelling and packaging of substances and mixtures, amending and repealing Directives 67/548/EEC and 1999/45/EC, and amending Regulation (EC) No 1907/2006. OJEU L353, 31.12.2008, pp 1–1355 at p 399.
- ↑ Sülzle, Detlev; Verhoeven, Marjon; Terlouw, Johan K.; Schwarz, Helmut Generation and Characterization of Sulfurous Acid (H2SO3) and of Its Radical Cation as Stable Species in the Gas Phase. Angew. Chem., Int. Ed. Engl. 1988, 27, 1533–34. DOI: 10.1002/anie.198815331.
- ↑ Jolly, William L. Modern Inorganic Chemistry, 2nd ed.; McGraw-Hill: New York, 1991; p 227. ISBN 0-07-032768-8.
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