Store grade Oxone on a watch glass.
| IUPAC name
| Other names
|Molar mass||152.2 g/mol (614.76 as triple salt)|
|Solubility||Reacts with ketones|
|Safety data sheet||ScienceLab|
| Potassium persulfate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Potassium peroxymonosulfate, also known potassium monopersulfate or MPS, is the potassium acid salt of peroxymonosulfuric acid, with the chemical formula KHSO5. It is sold under the trade names Caroat and Oxone, where it exists as a mixture consisting of of 2KHSO5·KHSO4·K2SO4, as pure potassium peroxymonosulfate is unstable and breaks down in the latter two compounds.
Potassium peroxymonosulfate is a strong oxidizer, capable of oxidizing organic substances into various compounds, such as: aldehydes to carboxylic acids, alcoholic solvents to their coresponding esters, cleaving internal alkenes to two carboxylic acids and terminal alkenes to epoxides, ketones to dioxiranes, thioethers to sulfones, tertiary amines to amine oxides and phosphines to phosphine oxides.
Oxone is a white granular solid, with a weak bleach-like smell, that decomposes in the presence of water.
Potassium peroxymonosulfate is sold under the name of Oxone in most swimming pool stores and various home-improvement and gardening retailer stores.
Adding hydrogen peroxide to potassium persulfate also yields potassium peroxymonosulfate.
Another method involves the hydrolysis of sodium persulfate at 100 °C to yield peroxydisulfuric acid. Solid potassium bisulfite is added, and the solution is filtered to remove the resulting potassium sulfate. The filtrate is freeze-dried and then washed with distilled water and filtered again at room temperature. The resulting filtrate is chilled on an ice bath, and the product is recrystallized for better purity.
- Oxidize organic compounds
- Make dimethyldioxirane
Potassium peroxymonosulfate is a strong oxidizer and should be kept away from any reducing agents or organic compounds.
Oxone should be kept in closed plastic or glass containers, away from any combustible materials.
Can be neutralized by dissolving it in water and adding an alkali, then poured down the drain.
- "Thomas Slater Price, J. Chem. Soc., Trans., 1906, vol 89, p 56".
- Klemenc, A.; Zeitschrift fuer Physikalische Chemie, Abteilung A: Chemische Thermodynamik, Kinetik, Elektrochemie, Eigenschaftslehre; vol. 185; (1939); p. 1 - 36
- "Price, J. S.; Tasker, I. R.; Appelman, E. H.; O'Hare, P. A. G.; Journal of Chemical Thermodynamics; vol. 18; nb. 10; (1986); p. 923 - 930".