|This article does not cite any sources. (December 2009)|
|Jmol interactive 3D||Image|
|Appearance||small colorless crystals|
|Melting point||380 °C (716 °F; 653 K) (decomposes)|
|Main hazards||strong oxidant, decomposes when heated|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Ammonium chlorate is an inorganic compound with the formula NH4ClO3.
It is obtained by neutralizing chloric acid with either ammonia or ammonium carbonate, or by precipitating barium, strontium or calcium chlorates with ammonium carbonate or ammonium sulfate, producing the respective carbonate or sulfate precipitate and an ammonium chlorate solution. Ammonium chlorate crystallizes in small needles, readily soluble in water.
The bitartrate method candidate be used if exotic chlorate are inaccessible or need to be synthesized. Warm solutions of potassium chlorate and ammonium bitartrate are needed need warm solutions. The latter can be synthesized by adding aqueous ammonia to an excess of tartric acid. Then, a double displacement reaction will result in precipitation of potassium bitartrate.
On heating, ammonium chlorate decomposes at about 102 °C, with liberation of nitrogen, chlorine and oxygen. It is soluble in dilute aqueous alcohol, but insoluble in strong alcohol. This compound is a strong oxidizer and should never be stored with flammable materials.
Ammonium chlorate is a very unstable oxidizer and will decompose, sometimes violently, at room temperature. This results from the mixture of the reducing ammonium cation and the oxidizing chlorate anion. Even solutions are known to be unstable. Because of the dangerous nature of this salt it should only be kept in solution when needed, and never be allowed to crystallize.
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