Difference between revisions of "Peroxydisulfuric acid"
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| MeltingPt_notes = (decomposes) | | MeltingPt_notes = (decomposes) | ||
| Odor = Odorless | | Odor = Odorless | ||
| − | | pKa = | + | | pKa = -3.5 |
| pKb = | | pKb = | ||
| Solubility = Soluble | | Solubility = Soluble | ||
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==Preparation== | ==Preparation== | ||
| − | Can be prepared by adding | + | Can be prepared by adding concentrated [[sulfuric acid]] to [[sodium persulfate]]. |
The acid can also be prepared by the reaction of [[chlorosulfuric acid]] with [[hydrogen peroxide]].<ref>https://onlinelibrary.wiley.com/doi/abs/10.1002/14356007.a19_177.pub2</ref> | The acid can also be prepared by the reaction of [[chlorosulfuric acid]] with [[hydrogen peroxide]].<ref>https://onlinelibrary.wiley.com/doi/abs/10.1002/14356007.a19_177.pub2</ref> | ||
: 2 ClSO<sub>3</sub>H + H<sub>2</sub>O<sub>2</sub> → H<sub>2</sub>S<sub>2</sub>O<sub>8</sub> + 2 HCl | : 2 ClSO<sub>3</sub>H + H<sub>2</sub>O<sub>2</sub> → H<sub>2</sub>S<sub>2</sub>O<sub>8</sub> + 2 HCl | ||
| + | |||
| + | The solid form is extremely difficult to obtain, and it's more often encountered as solution. | ||
==Projects== | ==Projects== | ||
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[[Category:Strong acids]] | [[Category:Strong acids]] | ||
[[Category:Oxoacids]] | [[Category:Oxoacids]] | ||
| + | [[Category:Sulfur oxoacids]] | ||
[[Category:Mineral acids]] | [[Category:Mineral acids]] | ||
[[Category:Persulfates]] | [[Category:Persulfates]] | ||
[[Category:Corrosive chemicals]] | [[Category:Corrosive chemicals]] | ||
Latest revision as of 00:22, 29 March 2020
| Names | |
|---|---|
| IUPAC name
Peroxydisulfuric acid
| |
| Other names
Marshall's acid
Peroxodisulfuric acid Persulfuric acid μ-peroxido-bis(hydroxidodioxidosulfur) | |
| Properties | |
| H2S2O8 | |
| Molar mass | 194.143 g/mol |
| Appearance | Colorless solid |
| Odor | Odorless |
| Melting point | 65 °C (149 °F; 338 K) (decomposes) |
| Boiling point | Decomposes |
| Soluble | |
| Solubility | Reacts with amines Soluble in alcohols (reacts) Insoluble in ether |
| Acidity (pKa) | -3.5 |
| Hazards | |
| Safety data sheet | None |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Sulfuric acid Peroxymonosulfuric acid |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Peroxydisulfuric acid or Marshall's acid, is a chemical compound, a strong oxoacid with the chemical formula H2S2O8. The free acid is not used in chemistry, but it's salts are more often encountered.
Contents
Properties
Chemical
Peroxydisulfuric acid will react violently with many organic compounds.
Hydrolysis of peroxydisulfuric acid produces hydrogen peroxide and sulfuric acid:
- H2S2O8 + 2 H2O → 2 H2SO4 + H2O2
Partial hydrolysis of peroxydisulfuric acid produces peroxymonosulfuric acid and sulfuric acid.
- H2S2O8 + H2O → H2SO5 + H2SO4
Physical
Peroxydisulfuric acid is a hygroscopic colorless solid, that is soluble in water.
Availability
The pure acid is not sold, instead its salts are more readily available.
Preparation
Can be prepared by adding concentrated sulfuric acid to sodium persulfate.
The acid can also be prepared by the reaction of chlorosulfuric acid with hydrogen peroxide.[1]
- 2 ClSO3H + H2O2 → H2S2O8 + 2 HCl
The solid form is extremely difficult to obtain, and it's more often encountered as solution.
Projects
- Make persulfate salts
Handling
Safety
Peroxydisulfuric acid is highly corrosive and may explode in contact with organic substances.
Storage
Peroxydisulfuric acid is not very stable, but at least one source claims it can be kept relative stable at low temperatures, for up to 8 weeks.[2]. Aqueous solutions of this acid are more stable at 0-17 °C.[3]
Peroxoacids should not be stored, as they will react violently with anything organic (dust, particulates, hair strands, etc.).
Disposal
Should be dissolved in water and neutralized with a reducing agent and a base.
References
- ↑ https://onlinelibrary.wiley.com/doi/abs/10.1002/14356007.a19_177.pub2
- ↑ D'Ans, J.; Zeitschrift fuer Elektrochemie; vol. 17; (1911); p. 849 - 851
- ↑ Elbs, K.; Schoenherr, O.; Zeitschrift fuer Elektrochemie; vol. 1; (1894); p. 468 - 472,
