Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Potassium chlorate: Difference between pages

| Watchedfields = changed

| verifiedrevid = 477003444

| Name = Potassium chlorate

| ImageFile =

| ImageFileL1 = Potassium-chlorate-composition.png

| ImageSizeL1 = 120px

| ImageNameL1 = The structure of the ions in potassium chlorate

| ImageFileR1 = Potassium-chlorate-crystal-3D-vdW.png

| ImageSizeR1 = 100px

| ImageNameR1 = The crystal structure of potassium chlorate

| ImageFile2 = Potassium chlorate-substance.jpg

| ImageSize2 = 200px

| ImageName2 = Potassium chlorate crystals

| OtherNames = Potassium chlorate(V), Potcrate, Berthollet salt

| IUPACName =

| SystematicName =

| Section1 = {{Chembox Identifiers

| ChEMBL = 3188561

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| CASNo_Ref = {{cascite|correct|CAS}}

| PubChem = 6426889

| EINECS = 223-289-7

| RTECS = FO0350000

| UNNumber = 1485

| Section2 = {{Chembox Properties

| Formula = KClO₃

| MolarMass = 122.55 g mol⁻¹

| Appearance = white crystals or powder

| Density = 2.32 g/cm³

| 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>

| SolubleOther = soluble in [[glycerol]]<br> negligible in [[acetone]] and liquid [[ammonia]]<ref name=chemister />

| Solubility1 = 1 g/100 g (20 °C)<ref name=chemister />

| Solvent1 = glycerol

| MeltingPtC = 356

| BoilingPtC = 400

| BoilingPt_notes = decomposes<ref name=chemister />

| RefractIndex = 1.40835

| MagSus = &minus;42.8·10⁻⁶ cm³/mol

| Section3 = {{Chembox Structure

| Coordination =

| CrystalStruct = monoclinic

| Section4 = {{Chembox Thermochemistry

| 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>

| Entropy = 142.97 J/mol·K<ref name=b1 /><ref name=chemister />

| DeltaGf = -289.9 kJ/mol<ref name=chemister />

| HeatCapacity = 100.25 J/mol·K<ref name=chemister />

| Section5 =

| Section6 =

| Section7 = {{Chembox Hazards

| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0548.htm ICSC 0548]

| 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>

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|271|302|332|411}}<ref name="sigma" />

| PPhrases = {{P-phrases|220|273}}<ref name="sigma" />

| NFPA-H = 2

| NFPA-F = 0

| NFPA-R = 3

| NFPA-S = OX

| 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>

| Section8 = {{Chembox Related

| OtherAnions = [[Potassium bromate]]<br>[[Potassium iodate]]<br>[[Potassium nitrate]]

| OtherCations = [[Ammonium chlorate]]<br>[[Sodium chlorate]]<br>[[Barium chlorate]]

| OtherCompounds = [[Potassium chloride]]<br>[[Potassium hypochlorite]]<br>[[Potassium chlorite]]<br>[[Potassium perchlorate]]

'''Potassium chlorate''' is a compound containing [[potassium]], [[chlorine]] and [[oxygen]], with the molecular formula KClO₃. In its pure form, it is a white crystalline substance. After [[sodium chlorate]], it is the second most common [[chlorate]] in industrial use. It is a strong [[oxidizing agent]] and its most important application is in safety [[match]]es.<ref name="ullmann_2000">{{cite book

| last1=Vogt | first1=Helmut

| last2=Balej | first2=Jan

| last3=Bennett | first3=John E.

| last4=Wintzer | first4=Peter

| last5=Sheikh | first5=Saeed Akbar

| last6=Gallone | first6=Patrizio

| date=June 15, 2000

| editor-last=Ullmann

| title=Ullmann's Encyclopedia of Industrial Chemistry

| publisher=Wiley‐VCH Verlag

| chapter=Chlorine Oxides and Chlorine Oxygen Acids

| isbn=9783527303854

| doi=10.1002/14356007.a06_483

}}</ref> In other applications it is mostly obsolete and has been replaced by safer alternatives in recent decades. It has been used

* in [[fireworks]], [[propellant]]s and [[explosives]],

* to prepare [[oxygen]], both in the lab and in [[chemical oxygen generator]]s,

* as a [[disinfectant]], for example in [[dentifrice]]s and medical [[mouthwash]]es,

* in [[agriculture]] as a [[herbicide]].

==Production==

On the industrial scale, potassium chlorate is produced by the [[salt metathesis reaction]] of [[sodium chlorate]] and [[potassium chloride]]:

:<chem>NaClO3 + KCl -> NaCl + KClO3</chem>

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 ([[Le Chatelier's Principle]]). The precursor sodium chlorate is produced industrially in very large quantities by [[electrolysis]] of [[sodium chloride]], common table salt.<ref name="ullmann_2000"/>

The direct electrolysis of [[Potassium chloride|KCl]] in aqueous solution is also used sometimes, in which elemental chlorine formed at the [[anode]] reacts with KOH ''[[in situ]]''. The low [[solubility]] of KClO₃ in water causes the salt to conveniently isolate itself from the [[reaction mixture]] by simply precipitating out of solution.

Potassium chlorate can be produced in small amounts by [[disproportionation]] in a [[sodium hypochlorite]] solution followed by [[salt metathesis reaction|metathesis reaction]] 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>

:<chem>3 NaOCl -> 2 NaCl + NaClO3</chem>

:<chem>KCl + NaClO3 -> NaCl + KClO3</chem>

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>

:<chem>3 Cl2 + 6 KOH -> KClO3 + 5 KCl + 3 H2O</chem>

==Uses==

[[Image:KClO3-sugar1.gif|thumb|left|Potassium chlorate burning sugar]]

Potassium chlorate was one key ingredient in early [[firearms]] [[percussion cap]]s (primers). It continues in that application, where not supplanted by [[potassium perchlorate]].

Chlorate-based [[propellant]]s are more efficient than traditional [[gunpowder]] and are less susceptible to damage by water. However, they can be extremely unstable in the presence of [[sulfur]] or [[phosphorus]] 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 [[silver fulminate]], is used in trick [[Bang snaps|noise-makers]] known as "crackers", "snappers", "pop-its", "caps" or "bang-snaps", a popular type of novelty [[firecracker|firework.]]

Another application of potassium chlorate is as the oxidizer in a [[smoke composition]] such as that used in [[smoke grenade]]s. Since 2005, a cartridge with potassium chlorate mixed with [[lactose]] and [[rosin]] is used for generating the white smoke signaling the election of new pope by a [[papal conclave]].<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=[[The New York Times]] |date=March 13, 2013 |access-date=March 13, 2013}}</ref>

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 [[catalyst]], typically [[manganese dioxide|manganese(IV) dioxide]] (MnO₂). 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:

:<chem>2 KClO3(s) ->[\Delta][MnO_2] 3 O2(g) + 2 KCl(s)</chem>

Heating it in the absence of a catalyst converts it into [[potassium perchlorate]]:<ref name="Pradyot Patnaik 2002"/>

:<chem>4 KClO3 -> 3 KClO4 + KCl</chem>

With further heating, potassium perchlorate decomposes to [[potassium chloride]] and oxygen:

:<chem>KClO4 -> KCl + 2O2</chem>

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&nbsp;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.

Potassium chlorate is used in [[chemical oxygen generator]]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 [[ValuJet Flight 592|plane crash]]. A fire on the space station [[Mir]] 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 [[limelight]]s.

Potassium chlorate is used also as a [[pesticide]]. In Finland it was sold under trade name Fegabit.

Potassium chlorate can react with sulfuric acid to form a highly reactive solution of chloric acid and potassium sulfate:

:<chem>2 KClO3 + H2SO4 -> 2 HClO3 + K2SO4</chem>

The solution so produced is sufficiently reactive that it spontaneously ignites if combustible material (sugar, paper, etc.) is present.

In schools, molten potassium chlorate is used in [[screaming jelly babies]], [[Gummy bear]], [[Haribo]], and [[Trolli]] candy demonstration where the candy is dropped into the molten salt.

In chemical labs it is used to oxidize HCl and release small amounts of gaseous chlorine.

Militant groups in [[Afghanistan]] also use potassium chlorate extensively as a key component in the production of [[improvised explosive devices]]. When significant effort was made to reduce the availability of [[ammonium nitrate]] 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>

Potassium chlorate was also the main ingredient in the car bomb used in [[2002 Bali bombings]] that killed 202 people.

Potassium chlorate is used to force the blossoming stage of the [[longan]] tree, causing it to produce fruit in warmer climates.<ref>{{Cite journal

| last1 = Manochai | first1 = P.

| last2 = Sruamsiri | first2 = P.

| last3 = Wiriya-alongkorn | first3 = W.

| last4 = Naphrom | first4 = D.

| last5 = Hegele | first5 = M.

| last6 = Bangerth | first6 = F.

| title = Year around off-season flower induction in longan (Dimocarpus longan, Lour.) trees by KClO3 applications: potentials and problems

| journal = Scientia Horticulturae

| volume = 104

| issue = 4

| pages = 379–390

| 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

| date = February 12, 2005

| url = http://www.actahort.org/books/863/863_48.htm

| access-date = November 28, 2010 | doi=10.1016/j.scienta.2005.01.004}}</ref>

==Safety==

Potassium chlorate should be handled with care. It reacts vigorously, and in some cases spontaneously ignites or explodes, when mixed with many [[combustible]] 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.

[[Sulfur]] should be avoided in pyrotechnic compositions containing potassium chlorate, as these mixtures are prone to spontaneous [[deflagration]]. 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 (ex. [[antimony(III) sulfide]]) are very dangerous to prepare, as they are extremely shock sensitive.

==See also==

*[[Chloric acid]]

==References==

{{Reflist}}

*"Chlorate de potassium. Chlorate de sodium", ''Fiche toxicol. n° 217'', Paris:Institut national de recherche et de sécurité, 2000. 4pp.

*[http://www.freepatentsonline.com/5087334.html Continuous process for the manufacture of potassium chlorate by coupling with a sodium chlorate production plant]

==External links==

{{Commons category|Potassium chlorate}}

{{Potassium compounds}}

{{Chlorates}}

[[Category:Potassium compounds]]

[[Category:Chlorates]]

[[Category:Pyrotechnic oxidizers]]