Ammonium chlorate

Ammonium chlorate
Names

IUPAC name Ammonium chlorate
Identifiers
CAS Number	10192-29-7^Y
3D model (Jmol)	Interactive image
ChemSpider	55411^Y
ECHA InfoCard	100.030.413
PubChem	61491
InChI InChI=1S/ClHO3.H3N/c2-1(3)4;/h(H,2,3,4);1H3^Y Key: KHPLPBHMTCTCHA-UHFFFAOYSA-N^Y InChI=1/ClHO3.H3N/c2-1(3)4;/h(H,2,3,4);1H3 Key: KHPLPBHMTCTCHA-UHFFFAOYAQ
SMILES O=Cl(=O)O.N
Properties
Chemical formula	NH₄ClO₃
Appearance	small colorless crystals
Density	2.42 g/cm³
Melting point	380 °C (716 °F; 653 K) (decomposes)
Hazards
Main hazards	strong oxidant, decomposes when heated
Related compounds
Other anions	Ammonium chloride Ammonium perchlorate
Other cations	Barium chlorate Potassium chlorate Sodium chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is ^YN ?)
Infobox references

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.

Preparation

It can be made by mixing a solution of ammonium chloride with potassium chlorate.

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