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 is a candidate for production and can be used if exotic chlorates are currently inaccessible or need to be synthesized. Warm solutions of potassium chlorate and ammonium bitartrate are needed. The latter can be synthesized by adding aqueous ammonia to an excess of tartaric acid. Then, a double displacement reaction will result in precipitation of ammonium chlorate.
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 powerful oxidizer and should never be stored with flammable materials, as it can easily form sensitive explosive compositions.
Ammonium chlorate is a very unstable oxidizer and will decompose independently, sometimes violently, at room temperature.[1] 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
Ammonium chlorate can be made by mixing stoichiometric solutions of ammonium nitrate and sodium chlorate or ammonium sulfate and barium chlorate.[2]
References
^Fairbrother, Fred (1922). "The Spontaneous Decomposition of Ammonium Chlorate". Journal of the American Chemical Society. 44 (11): 2419–2422. doi:10.1021/ja01432a009. ISSN 0002-7863.
^Gillespie, R. B.; Gantzel, P. K.; Trueblood, K. N. (1962-05-17). "The Crystal Structure of Ammonium Chlorate". Acta Crystallographica. 15 (12): 1271–1272. doi:10.1107/S0365110X62003345.
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ammonium, chlorate, this, article, needs, additional, citations, verification, please, help, improve, this, article, adding, citations, reliable, sources, unsourced, material, challenged, removed, find, sources, news, newspapers, books, scholar, jstor, april, . This article needs additional citations for verification Please help improve this article by adding citations to reliable sources Unsourced material may be challenged and removed Find sources Ammonium chlorate news newspapers books scholar JSTOR April 2022 Learn how and when to remove this template message Ammonium chlorate is an inorganic compound with the formula NH4ClO3 Ammonium chlorate NamesIUPAC name Ammonium chlorateIdentifiersCAS Number 10192 29 7 Y3D model JSmol Interactive imageChemSpider 55411 YECHA InfoCard 100 030 413PubChem CID 61491CompTox Dashboard EPA DTXSID90144346InChI InChI 1S ClHO3 H3N c2 1 3 4 h H 2 3 4 1H3 YKey KHPLPBHMTCTCHA UHFFFAOYSA N YInChI 1 ClHO3 H3N c2 1 3 4 h H 2 3 4 1H3Key KHPLPBHMTCTCHA UHFFFAOYAQSMILES O Cl O O NPropertiesChemical formula NH4ClO3Appearance small colorless crystalsDensity 2 42 g cm3Melting point 380 C 716 F 653 K decomposes Magnetic susceptibility x 42 1 10 6 cm3 molHazardsOccupational safety and health OHS OSH Main hazards strong oxidant decomposes when heatedRelated compoundsOther anions Ammonium chloride Ammonium perchlorateOther cations Barium chlorate Potassium chlorate Sodium chlorateExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa Y verify what is Y N Infobox references 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 is a candidate for production and can be used if exotic chlorates are currently inaccessible or need to be synthesized Warm solutions of potassium chlorate and ammonium bitartrate are needed The latter can be synthesized by adding aqueous ammonia to an excess of tartaric acid Then a double displacement reaction will result in precipitation of ammonium chlorate 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 powerful oxidizer and should never be stored with flammable materials as it can easily form sensitive explosive compositions Ammonium chlorate is a very unstable oxidizer and will decompose independently sometimes violently at room temperature 1 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 EditAmmonium chlorate can be made by mixing stoichiometric solutions of ammonium nitrate and sodium chlorate or ammonium sulfate and barium chlorate 2 References Edit Fairbrother Fred 1922 The Spontaneous Decomposition of Ammonium Chlorate Journal of the American Chemical Society 44 11 2419 2422 doi 10 1021 ja01432a009 ISSN 0002 7863 Gillespie R B Gantzel P K Trueblood K N 1962 05 17 The Crystal Structure of Ammonium Chlorate Acta Crystallographica 15 12 1271 1272 doi 10 1107 S0365110X62003345 This inorganic compound related article is a stub You can help Wikipedia by expanding it vte Retrieved from https en wikipedia org w index php title Ammonium chlorate amp oldid 1136179734, wikipedia, wiki, book, books, library,
