Potassium hypochlorite

Potassium hypochlorite

Potassium hypochlorite
Identifiers
CAS Number	7778-66-7 Y
ChemSpider	56409 Y
EC Number	231-909-2
Jmol 3D model	Interactive image
PubChem	23665762
UNII	G27K3AQ7DW Y
UN number	1791
InChI InChI=1/ClO.K/c1-2;/q-1;+1 Key: SATVIFGJTRRDQU-UHFFFAOYAH
SMILES [K+].[O-]Cl
Properties
Chemical formula	KClO
Molar mass	90.55 g/mol
Appearance	Liquid light grey
Odor	Chlorine-like
Density	1.160 g/cm3
Melting point	−2 °C (28 °F; 271 K)
Boiling point	102 °C (216 °F; 375 K) (decomposes)
Solubility in water	25%
Pharmacology
ATC code	D08[1]
Vapor pressure	{{{value}}}
Related compounds
Other anions	Potassium chloride Potassium chlorite Potassium chlorate Potassium perchlorate
Other cations	Sodium hypochlorite Lithium hypochlorite Calcium hypochlorite
Related compounds	Hypochlorous acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Potassium hypochlorite (chemical formula KClO) is the potassium salt of hypochlorous acid. It is used in variable concentrations, often diluted in water solution. It has a light grey color and a strong chlorine smell. It can be used as a disinfectant.

Preparation

Potassium hypochlorite is produced by the reaction of chlorine with a solution of potassium hydroxide:

Cl₂ + 2 KOH → KCl + KClO + H₂O

This is the traditional method, first used by Claude Louis Berthollet in in 1789.

Another production method is electrolysis of potassium chloride solution:

2 KCl + H₂O → KClO + KCl + H₂

With both methods, the reaction mixture must be kept cold to prevent formation of potassium chlorate.

Uses

Potassium hypochlorite is used for sanitizing surfaces as well as disinfecting drinking water. Because its degradation leaves behind potassium chloride rather than sodium chloride, its use has been promoted in agriculture, where addition of potassium to soil is desired.

History

Potassium hypochlorite was first produced in 1789 by Claude Louis Berthollet in his laboratory located in Javel in Paris, France, by passing chlorine gas through a solution of potash lye. The resulting liquid, known as "Eau de Javel" ("Javel water"), was a weak solution of potassium hypochlorite. Due to production difficulties, the product was then modified using sodium instead of potassium, giving rise to sodium hypochlorite, widely used today as a disinfectant.

Safety and toxicology

Like sodium hypochlorite, potassium hypochlorite is an irritant. It can cause severe damage on contact with the skin, eyes, and mucous membranes. Inhalation of a mist of KClO can cause bronchial irritation, difficulty breathing, and in severe cases pulmonary edema. Ingestion of strong concentrations can be lethal.

Potassium hypochlorite is not considered a fire or explosive hazard by itself. However, it can react explosively with numerous chemicals, including urea, ammonium salts, methanol, acetylene, and many organic compounds. Heating and acidification can produce toxic chlorine gas.