Another production method is electrolysis of potassium chloride solution.
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.[4]
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.[5] Inhalation of a mist of KOCl can cause bronchus and lung irritation, difficulty breathing, and in severe cases pulmonary edema. Ingestion of strong concentrations can be lethal.[6] Symptoms of contact or inhalation can be delayed.[1]
Potassium hypochlorite is not considered to cause a fire or explosive hazards by itself.[6] 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.[7] Containers may explode upon exposure to heat.[1] Potassium hypochlorite forms highly explosive NCl3 upon contact with urea or ammonia.[1]
^Helmut Vogt; Jan Balej; John E. Bennett; Peter Wintzer; Saeed Akhbar Sheikh; Patrizio Gallone (2007), "Chlorine Oxides and Chlorine Oxygen Acids", Ullmann's Encyclopedia of Industrial Chemistry (7th ed.), Wiley, p. 2
