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Potassium hypochlorite is produced by the disproportionation reaction of chlorine with a solution of potassium hydroxide: [2]. Cl 2 + 2 KOH → KCl + KOCl + H 2 O. This is the traditional method, first used by Claude Louis Berthollet in 1789.
3 Cl 2 + 6 KOH → KClO 3 + 5 KCl + 3 H 2 O as seen in this video. According to X-ray crystallography, potassium chlorate is a dense salt-like structure consisting of chlorate and potassium ions in close association. The crystal structure of potassium chlorate. Color code: red = O, violet = K, green = Cl
2 KCl + 2 H 2 O → 2 KOH + Cl 2 + H 2. Hydrogen gas forms as a byproduct on the cathode; concurrently, an anodic oxidation of the chloride ion takes place, forming chlorine gas as a byproduct. Separation of the anodic and cathodic spaces in the electrolysis cell is essential for this process. [17]
2 NaCl + 2 H 2 O → 2 NaOH + H 2 + Cl 2. Without a membrane, the OH − ions produced at the cathode are free to diffuse throughout the electrolyte. As the electrolyte becomes more basic due to the production of OH −, less Cl 2 emerges from the solution as it begins to disproportionate to form chloride and hypochlorite ions at the anode:
Potassium chloride (KCl, or potassium salt) is a metal halide salt composed of potassium and chlorine.It is odorless and has a white or colorless vitreous crystal appearance. The solid dissolves readily in water, and its solutions have a salt-like taste.
Metal chlorates can be prepared by adding chlorine to hot metal hydroxides like KOH: 3 Cl 2 + 6 KOH 5 KCl + KClO 3 + 3 H 2 O {\displaystyle {\ce {3 Cl2 + 6 KOH -> 5 KCl + KClO3 + 3 H2O}}} In this reaction, chlorine undergoes disproportionation , both reduction and oxidation.
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
Dichlorine monoxide reacts with metal halides, with the loss of Cl 2, to form unusual oxyhalides. [11] [12] [3] VOCl 3 + Cl 2 O → VO 2 Cl + 2 Cl 2 TiCl 4 + Cl 2 O → TiOCl 2 + 2 Cl 2 SbCl 5 + 2 Cl 2 O → SbO 2 Cl + 4 Cl 2. Similar reactions have also been observed with certain inorganic halides. [13] [14] AsCl 3 + 2 Cl 2 O → AsO 2 Cl + 3 ...