| Revision as of 13:49, 5 December 2011 editBeetstra (talk | contribs)Edit filter managers, Administrators172,116 edits Saving copy of the {{chembox}} taken from revid 463587979 of page Potassium_chlorate for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 01:47, 12 January 2025 edit Vertexrocketry (talk | contribs)2 editsmNo edit summaryTag: Visual edit |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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{{chembox |
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| Watchedfields = changed |
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| verifiedrevid = 447892540 |
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| verifiedrevid = 477003444 |
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| Name = Potassium Chlorate |
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| ImageFile = Potassium-chlorate-composition.png |
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| Name = Potassium chlorate |
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| ImageSize = 200px |
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| ImageFile = |
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| ImageFile1 = Potassium-chlorate-composition.png |
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| ImageName = The structure of the ions in potassium chlorate |
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| ImageSize1 = 120px |
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| ImageFile1 = Potassium-chlorate-crystal-3D-vdW.png |
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| ImageClass1 = skin-invert |
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| ImageSize1 = 200px |
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| ImageName1 = The crystal structure of potassium chlorate |
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| ImageName1 = The structure of the ions in potassium chlorate |
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| ImageFile2 = Potassium chlorate-substance.jpg |
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| ImageFile2 = Potassium chlorate-substance.jpg |
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| ImageSize2 = 200px |
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| ImageSize2 = 200px |
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| ImageName2 = Potassium chlorate crystals <!--don't know why this didn't have a picture--> |
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| ImageName2 = Potassium chlorate crystals |
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| OtherNames = Potassium chlorate(V), Potcrate |
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| OtherNames = Potassium chlorate(V), Potcrate, Berthollet salt |
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| IUPACName = |
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| Section1 = {{Chembox Identifiers |
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| SystematicName = |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| Section1 = {{Chembox Identifiers |
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| ChEMBL = 3188561 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 18512 |
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| ChemSpiderID = 18512 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| StdInChIKey = VKJKEPKFPUWCAS-UHFFFAOYSA-M |
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| StdInChIKey = VKJKEPKFPUWCAS-UHFFFAOYSA-M |
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| CASNo = 3811-04-9 |
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| CASNo = 3811-04-9 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = 6426889 |
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| PubChem = 6426889 |
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| EINECS = 223-289-7 |
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| EINECS = 223-289-7 |
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| RTECS = FO0350000 |
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| RTECS = FO0350000 |
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| UNNumber = 1485 |
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| UNNumber = 1485 |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = KClO<sub>3</sub> |
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| Formula = KClO<sub>3</sub> |
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| MolarMass = 122.55 g/mol |
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| MolarMass = 122.55 g mol<sup>−1</sup> |
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| Appearance = White crystals or powder |
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| Appearance = white crystals or powder |
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| Density = 2.34 g/cm<sup>3</sup> |
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| Density = 2.32 g/cm<sup>3</sup> |
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| Solubility = 3.13 g/100 mL (0 °C)<br> 4.46 g/100 mL (10 °C)<br> 8.15 g/100 mL (25 °C)<br> 13.21 g/100 mL (40 °C)<br> 53.51 g/100 mL (100 °C)<br> 183 g/100 g (190 °C)<br> 2930 g/100 g (330 °C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1952|title = Solubilities of Inorganic and Organic Compounds|publisher = Van Nostrand|url = https://books.google.com/books?id=k2e5AAAAIAAJ |access-date = 2014-05-29}}</ref> |
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| Solubility = 7.19 g/100 ml (20 °C) <br> 57 g/100 mL (100 °C) |
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| SolubleOther = insoluble in ], liquid ] |
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| SolubleOther = soluble in ]<br> negligible in ] and liquid ]<ref name=chemister /> |
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| Solubility1 = 1 g/100 g (20 °C)<ref name=chemister /> |
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| MeltingPt = 356 °C |
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| Solvent1 = glycerol |
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| BoilingPt = 400 °C ''decomp.'' |
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| MeltingPtC = 356 |
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| RefractIndex = 1.40835 |
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| BoilingPtC = 400 |
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| BoilingPt_notes = decomposes<ref name=chemister /> |
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| RefractIndex = 1.40835 |
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| MagSus = −42.8·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Section3 = {{Chembox Structure |
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| Section3 = {{Chembox Structure |
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| Coordination = |
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| Coordination = |
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| CrystalStruct = monoclinic |
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| CrystalStruct = monoclinic |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = −391.2 kJ/mol<ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A22}}</ref><ref name=chemister>{{cite web|url=http://chemister.ru/Database/properties-en.php?dbid=1&id=331|title=potassium chlorate|access-date=9 July 2015}}</ref> |
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| ExternalMSDS = |
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| Entropy = 142.97 J/mol·K<ref name=b1 /><ref name=chemister /> |
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| EUClass = Oxidant ('''O''')<br/>Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''') |
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| DeltaGf = -289.9 kJ/mol<ref name=chemister /> |
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| EUIndex = 017-004-00-3 |
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| HeatCapacity = 100.25 J/mol·K<ref name=chemister /> |
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| RPhrases = {{R9}}, {{R22}}, {{R51/53}} |
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}} |
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| SPhrases = {{S2}}, {{S13}}, {{S16}}, {{S27}}, {{S61}} |
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| NFPA-H = 2 |
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| Section5 = |
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| NFPA-F = 0 |
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| Section6 = |
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| Section7 = {{Chembox Hazards |
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| NFPA-R = 3 |
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| ExternalSDS = |
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| NFPA-O = OX |
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| GHSPictograms = {{GHS03}}{{GHS07}}{{GHS09}}<ref name="sigma">{{cite web|url=https://www.sigmaaldrich.com/US/en/product/sigald/255572|title=Potassium chlorate|access-date=14 February 2022}}</ref> |
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| FlashPt = 400 °C |
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| GHSSignalWord = Danger |
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| LD50 = 1870 mg/kg |
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| HPhrases = {{H-phrases|271|302|332|411}}<ref name="sigma" /> |
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| PPhrases = {{P-phrases|220|273}}<ref name="sigma" /> |
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| NFPA-H = 2 |
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| NFPA-F = 0 |
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| NFPA-R = 3 |
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| NFPA-S = OX |
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| LD50 = 1870 mg/kg (oral, rat)<ref>{{cite web|url=https://chem.nlm.nih.gov/chemidplus/rn/3811-04-9|title=ChemIDplus - 3811-04-9 - VKJKEPKFPUWCAS-UHFFFAOYSA-M - Potassium chlorate - Similar structures search, synonyms, formulas, resource links, and other chemical information.|author=Michael Chambers|access-date=9 July 2015}}</ref> |
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}} |
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| Section8 = {{Chembox Related |
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| Section8 = {{Chembox Related |
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| OtherAnions = ]<br/>] |
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| OtherAnions = ]<br>]<br>] |
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| OtherCations = ]<br/>]<br/>] |
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| OtherCations = ]<br>]<br>] |
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| OtherCpds = ]<br/>]<br/>]<br/>] |
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| OtherCompounds = ]<br>]<br>]<br>] |
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'''Potassium chlorate''' is the ] with the molecular formula KClO<sub>3</sub>. In its pure form, it is a white solid. After ], it is the second most common ] in industrial use. It is a strong ] and its most important application is in safety ]es.<ref name="ullmann_2000">{{cite book |
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| last1=Vogt | first1=Helmut |
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| last2=Balej | first2=Jan |
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| last3=Bennett | first3=John E. |
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| last4=Wintzer | first4=Peter |
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| last5=Sheikh | first5=Saeed Akbar |
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| last6=Gallone | first6=Patrizio |
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| date=June 15, 2000 |
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| editor-last=Ullmann |
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| title=Ullmann's Encyclopedia of Industrial Chemistry |
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| publisher=Wiley‐VCH Verlag |
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| chapter=Chlorine Oxides and Chlorine Oxygen Acids |
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| isbn=9783527303854 |
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| doi=10.1002/14356007.a06_483 |
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}}</ref> In other applications it is mostly obsolete and has been replaced by safer alternatives in recent decades. It has been used |
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* in ], ]s and ], |
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* to prepare ], both in the lab and in ]s, |
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* as a ], for example in ]s and medical ]es, |
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* in ] as an ]. |
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==Production== |
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On the industrial scale, potassium chlorate is produced by the ] of ] and ]: |
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:{{chem2 | NaClO3 + KCl -> NaCl + KClO3 }} |
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The reaction is driven by the low solubility of potassium chlorate in water. The equilibrium of the reaction is shifted to the right hand side by the continuous precipitation of the product (]). The precursor sodium chlorate is produced industrially in very large quantities by ] of ], common table salt.<ref name="ullmann_2000"/> |
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The direct electrolysis of ] in aqueous solution is also used sometimes, in which elemental chlorine formed at the ] reacts with KOH '']''. The low ] of KClO<sub>3</sub> in water causes the salt to conveniently isolate itself from the ] by simply precipitating out of solution. |
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Potassium chlorate can be produced in small amounts by ] in a ] solution followed by ] with potassium chloride:<ref>{{cite web|url=http://chemistry.about.com/od/makechemicalsyourself/a/Potassium-Chlorate-From-Bleach-And-Salt-Substitute.htm|title=Potassium Chlorate Synthesis (Substitute) Formula|author=Anne Marie Helmenstine, Ph.D.|work=About.com Education|access-date=9 July 2015}}</ref> |
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:{{chem2 | 3 NaOCl -> 2 NaCl + NaClO3 }} |
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:{{chem2 | KCl + NaClO3 -> NaCl + KClO3 }} |
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It can also be produced by passing chlorine gas into a hot solution of caustic potash:<ref name="Pradyot Patnaik 2002">Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref> |
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:{{chem2 | 3 Cl2 + 6 KOH -> KClO3 + 5 KCl + 3 H2O }} |
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:as seen in this |
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According to ], potassium chlorate is a dense salt-like structure consisting of chlorate and potassium ions in close association. |
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] |
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==Uses== |
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] |
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Potassium chlorate was one key ingredient in early ] ]s (primers). It continues in that application, where not supplanted by ]. |
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Chlorate-based ]s are more efficient than traditional ] and are less susceptible to damage by water. However, they can be extremely unstable in the presence of ] or ] and are much more expensive. Chlorate propellants must be used only in equipment designed for them; failure to follow this precaution is a common source of accidents. Potassium chlorate, often in combination with ], is used in trick ] known as "crackers", "snappers", "pop-its", "caps" or "bang-snaps", a popular type of novelty ] |
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Another application of potassium chlorate is as the oxidizer in a ] such as that used in ]s. Since 2005, a cartridge with potassium chlorate mixed with ] and ] is used for generating the white smoke signaling the election of new pope by a ].<ref>{{cite news |title=New Round of Voting Fails to Name a Pope |author=Daniel J. Wakin and Alan Cowell |url=https://www.nytimes.com/2013/03/14/world/europe/vatican-pope-selection-conclave.html |newspaper=] |date=March 13, 2013 |access-date=March 13, 2013}}</ref> |
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High school and college laboratories often use potassium chlorate to generate oxygen gas. {{Citation needed|date=June 2009}} It is a far cheaper source than a pressurized or cryogenic oxygen tank. Potassium chlorate readily decomposes if heated while in contact with a ], typically ] (MnO<sub>2</sub>). Thus, it may be simply placed in a test tube and heated over a burner. If the test tube is equipped with a one-holed stopper and hose, warm oxygen can be drawn off. The reaction is as follows: |
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:{{chem2 | 2 KClO3(s) + MnO2(cat) -> 3 O2(g) + 2 KCl(s) }} |
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Heating it in the absence of a catalyst converts it into ]:<ref name="Pradyot Patnaik 2002"/> |
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:{{chem2 | 4 KClO3 -> 3 KClO4 + KCl }} |
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With further heating, potassium perchlorate decomposes to ] and oxygen: |
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:{{chem2 | KClO4 -> KCl + 2 O2 }} |
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The safe performance of this reaction requires very pure reagents and careful temperature control. Molten potassium chlorate is an extremely powerful oxidizer and spontaneously reacts with many common materials such as sugar. Explosions have resulted from liquid chlorates spattering into the latex or PVC tubes of oxygen generators and from contact between chlorates and hydrocarbon sealing greases. Impurities in potassium chlorate itself can also cause problems. When working with a new batch of potassium chlorate, it is advisable to take a small sample (~1 gram) and heat it strongly on an open glass plate. Contamination may cause this small quantity to explode, indicating that the chlorate should be discarded. |
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Potassium chlorate is used in ]s (also called chlorate candles or oxygen candles), employed as oxygen-supply systems of e.g. aircraft, space stations, and submarines, and has been responsible for at least one ]. A fire on the space station ] was traced to oxygen generation candles that use a similar lithium perchlorate. The decomposition of potassium chlorate was also used to provide the oxygen supply for ]s. |
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Potassium chlorate is used also as a ]. In Finland it was sold under trade name Fegabit. |
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Potassium chlorate can react with sulfuric acid to form a highly reactive solution of chloric acid and potassium sulfate: |
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:{{chem2 | 2 KClO3 + H2SO4 -> 2 HClO3 + K2SO4 }} |
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The solution so produced is sufficiently reactive that it spontaneously ignites if combustible material (sugar, paper, etc.) is present. |
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] |
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In schools, molten potassium chlorate is used in ], ], ], and ] candy demonstration where the candy is dropped into the molten salt. |
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In chemical labs it is used to oxidize HCl and release small amounts of gaseous chlorine. |
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Militant groups in ] also use potassium chlorate extensively as a key component in the production of ] (IEDs). When significant effort was made to reduce the availability of ] fertilizer in Afghanistan, IED makers started using potassium chlorate as a cheap and effective alternative. In 2013, 60% of IEDs in Afghanistan used potassium chlorate, making it the most common ingredient used in IEDs.<ref>{{cite news|url=https://www.usatoday.com/story/news/world/2013/06/25/ammonium-nitrate-potassium-chlorate-ieds-afghanistan/2442191/ |title=Afghan bomb makers shifting to new explosives for IEDs |publisher=USAToday.com |date= June 25, 2013|access-date=2013-06-25}}</ref> |
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Potassium chlorate was also the main ingredient in the car bomb used in ] that killed 202 people. |
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Potassium chlorate is used to force the blossoming stage of the ] tree, causing it to produce fruit in warmer climates.<ref>{{Cite journal |
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| last1 = Manochai | first1 = P. |
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| last2 = Sruamsiri | first2 = P. |
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| last3 = Wiriya-alongkorn | first3 = W. |
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| last4 = Naphrom | first4 = D. |
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| last5 = Hegele | first5 = M. |
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| last6 = Bangerth | first6 = F. |
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| title = Year around off-season flower induction in longan (Dimocarpus longan, Lour.) trees by KClO3 applications: potentials and problems |
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| journal = Scientia Horticulturae |
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| volume = 104 |
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| issue = 4 |
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| pages = 379–390 |
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| location = Department of Horticulture, Maejo University, Chiang Mai, Thailand; Department of Horticulture, Chiang Mai University, Chiang Mai, Thailand; Institute of Special Crops and Crop Physiology, University of Hohenheim, 70593 Stuttgart, Germany |
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| date = February 12, 2005 |
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| url = http://www.actahort.org/books/863/863_48.htm |
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| access-date = November 28, 2010 | doi=10.1016/j.scienta.2005.01.004}}</ref> |
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==Safety== |
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Potassium chlorate should be handled with care. It reacts vigorously, and in some cases spontaneously ignites or explodes, when mixed with many ] materials. It burns vigorously in combination with virtually any combustible material, even those normally only slightly flammable (including ordinary dust and lint). Mixtures of potassium chlorate and a fuel can ignite by contact with sulfuric acid, so it should be kept away from this reagent. |
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] should be avoided in pyrotechnic compositions containing potassium chlorate, as these mixtures are prone to spontaneous ]. Most sulfur contains trace quantities of sulfur-containing acids, and these can cause spontaneous ignition - "Flowers of sulfur" or "sublimed sulfur", despite the overall high purity, contains significant amounts of sulfur acids. Also, mixtures of potassium chlorate with any compound with ignition promoting properties, such as ], are very dangerous to prepare, as they are extremely shock sensitive. |
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==See also== |
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*] |
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==References== |
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{{Reflist}} |
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*"Chlorate de potassium. Chlorate de sodium", ''Fiche toxicol. n° 217'', Paris:Institut national de recherche et de sécurité, 2000. 4pp. |
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* |
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==External links== |
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{{Commons category|Potassium chlorate}} |
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{{Potassium compounds}} |
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{{Chlorates}} |
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] |
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] |
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] |