|This article is a stub. Please help Sciencemadness Wiki by expanding it, adding pictures, and improving existing text.
| IUPAC name
|Molar mass||90.55 g/mol|
|Appearance||Light gray liquid|
|Melting point||−2 °C (28 °F; 271 K)|
|Boiling point||102 °C (216 °F; 375 K) (decomposes)|
|Solubility||Reacts with alcohols, aldehydes, ketones|
| Lithium hypochlorite|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Potassium hypochlorite is the potassium salt of hypochlorous acid, with the chemical formula KClO.
Potassium hypochlorite rapidly disproportionates into potassium chloride and chloride.
- 3 KClO → KClO3 + 2 KCl
Potassium hypochlorite is an unstable compound that mainly occurs in solution.
Potassium hypochlorite is not readily available and has to be made.
Potassium hypochlorite is produced by the reaction of chlorine with a solution of potassium hydroxide. This can be done by bubbling chlorine gas in a cooled solution of KOH, similar to the method used for the production of NaClO,
- 2 KOH + Cl2 → KCl + KClO + H2O
Electrolysis of potassium chloride solution will also produce potassium hypochlorite.
With both methods, the reaction mixture must be kept cold to prevent formation of potassium chlorate.
- Make potassium chlorate and perchlorate
Like sodium hypochlorite, potassium hypochlorite is a powerful oxidizer and very corrosive. Addition of acid will liberate large amounts of chlorine gas.
Potassium hypochlorite is unstable and can only be stored for short periods of time at low temperatures.
Potassium hypochlorite can be neutralized with a reducing agent, like sodium thiosulfate, sulfite or metabisulfite, or just heated to turn it into the more useful potassium hypochlorite.