Preparation of Chlorate
Sodium Chlorate Industrial Preparation
On a large scale, we prepare chlorates by starting the synthesis for sodium chlorate with aqueous sodium chloride (brine) rather than chlorine gas. Furthermore, if the electrolysis apparatus allows for the mixing of chlorine and sodium hydroxide, the disappropriation process occurs. Furthermore, the electrical power required for electrolysis is used to heat the reactants to 50-70°C.
Chlorate Preparation in Laboratory
Metal chlorates can be produced in the laboratory by adding chlorine to heated metal hydroxide. For example, to make potassium chlorate (KClO3) add chlorine to hot potassium hydroxide (KOH). This is an example of a disproportionation or dismutation process, in which Cl is reduced and oxidation from oxidation state 0 to -1 and +5, respectively.
3Cl2 + 6 KOH → 5 KCl + KClO3 + 3 H2O
Chlorate Formula
Chlorate refers to any molecule that contains the chlorate anion, most often metal salts of chloric acid. Chlorine has an oxidation state of +5 in these ions. Chlorate oxyanion is indicated by roman numerals in parenthesis, for example, Chlorate oxyanion (VII). In the lab, they may be made by adding chlorine to heated metal hydroxides such as KOH. They are extremely potent oxidising agents that are utilised in bleaching paper, herbicides, medicines, explosives, and other applications. Sodium Chlorate is the most common type of chlorate (NaClO3). Because they are strong oxidizers, they should be stored away from organics and quickly oxidised materials. Combinations of chlorates with almost any flammable substance (sawdust, sugar, organic solvents, charcoal, metals, etc.) can also explode. Because of this, chlorates were once widely used in pyrotechnics, although their use has since declined due to their instability.