Potassium chlorate: Difference between revisions
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| DeltaHf = −391.2 kJ/mol<ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th | | DeltaHf = −391.2 kJ/mol<ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles |edition=6th | 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 /> | | Entropy = 142.97 J/mol·K<ref name=b1 /><ref name=chemister /> | ||
| DeltaGf = −289.9 kJ/mol<ref name=chemister /> | | DeltaGf = −289.9 kJ/mol<ref name=chemister /> | ||
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* to prepare [[oxygen]], both in the lab and in [[chemical oxygen generator]]s, | * 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, | * as a [[disinfectant]], for example in [[dentifrice]]s and medical [[mouthwash]]es, | ||
* in [[agriculture]] as | * in [[agriculture]] as a [[herbicide]]. | ||
==Production== | ==Production== | ||
[[Image:Potassium-chlorate-crystal-3D-vdW.png|thumb|left|100px|The crystal structure of potassium chlorate. Color code: red = O, violet = K, green = Cl]] | |||
On the industrial scale, potassium chlorate is produced by the [[salt metathesis reaction]] of [[sodium chlorate]] and [[potassium chloride]]: | On the industrial scale, potassium chlorate is produced by the [[salt metathesis reaction]] of [[sodium chlorate]] and [[potassium chloride]]: | ||
:{{ | |||
: {{Chem2 | NaClO3 + KCl -> NaCl + KClO3 }} | |||
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 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"/> | ||
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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> | 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> | ||
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 | : {{Chem2 | 3 NaOCl -> 2 NaCl + NaClO3 }} | ||
:{{ | : {{Chem2 | KCl + NaClO3 -> NaCl + KClO3 }} | ||
:as seen in this | |||
It can also be produced by passing chlorine gas into a hot solution of caustic potash:<ref name="Pradyot Patnaik 2002">Pradyot Patnaik (2002). ''Handbook of Inorganic Chemicals''. McGraw-Hill. {{ISBN|0-07-049439-8}}</ref> | |||
: {{Chem2 | 3 Cl2 + 6 KOH -> KClO3 + 5 KCl + 3 H2O }} | |||
: as seen in this video.<ref>https://www.youtube.com/watch?v=NuHIClcoHTs</ref> | |||
According to [[X-ray crystallography]], potassium chlorate is a dense salt-like structure consisting of chlorate and potassium ions in close association. | According to [[X-ray crystallography]], potassium chlorate is a dense salt-like structure consisting of chlorate and potassium ions in close association. | ||
==Uses== | ==Uses== | ||
[[Image:KClO3-sugar1.gif|thumb|left|Potassium chlorate burning sugar]] | [[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]]. | Potassium chlorate was one key ingredient in early [[firearms]] [[percussion cap]]s (primers). It continues in that application, where not supplanted by [[potassium perchlorate]]. | ||
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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 [[catalyst]], typically [[manganese dioxide|manganese(IV) dioxide]] (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: | 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]] (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: | ||
:{{ | |||
: {{Chem2 | 2 KClO3(s) + MnO2(cat) -> 3 O2(g) + 2 KCl(s) }} | |||
Heating it in the absence of a catalyst converts it into [[potassium perchlorate]]:<ref name="Pradyot Patnaik 2002"/> | Heating it in the absence of a catalyst converts it into [[potassium perchlorate]]:<ref name="Pradyot Patnaik 2002"/> | ||
:{{ | |||
: {{Chem2 | 4 KClO3 -> 3 KClO4 + KCl }} | |||
With further heating, potassium perchlorate decomposes to [[potassium chloride]] and oxygen: | With further heating, potassium perchlorate decomposes to [[potassium chloride]] and oxygen: | ||
:{{ | |||
: {{Chem2 | KClO4 -> KCl + 2 O2 }} | |||
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. | 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 can react with sulfuric acid to form a highly reactive solution of chloric acid and potassium sulfate: | Potassium chlorate can react with sulfuric acid to form a highly reactive solution of chloric acid and potassium sulfate: | ||
:{{ | |||
: {{Chem2 | 2 KClO3 + H2SO4 -> 2 HClO3 + K2SO4 }} | |||
The solution so produced is sufficiently reactive that it spontaneously ignites if combustible material (sugar, paper, etc.) is present. | The solution so produced is sufficiently reactive that it spontaneously ignites if combustible material (sugar, paper, etc.) is present. | ||
[[File:Screaming gummy bear (chlorate) abridged.ogg|thumb|Candy being dropped into molten salt]] | [[File:Screaming gummy bear (chlorate) abridged.ogg|thumb|left|Candy being dropped into molten salt]] | ||
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 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. | ||
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| last5 = Hegele | first5 = M. | | last5 = Hegele | first5 = M. | ||
| last6 = Bangerth | first6 = F. | | last6 = Bangerth | first6 = F. | ||
| title = Year | | date = 15 May 2005 | ||
| title = Year Around Off-season Flower Induction in Longan (''Dimocarpus Longan'', Lour.) Trees by KClO<sub>3</sub> Applications: Potentials and Problems | |||
| url = https://www.sciencedirect.com/science/article/abs/pii/S0304423805000063?via%3Dihub | |||
| url-access = subscription | |||
| journal = Scientia Horticulturae | | journal = Scientia Horticulturae | ||
| volume = 104 | | volume = 104 | ||
| issue = 4 | | issue = 4 | ||
| pages = 379–390 | | pages = 379–390 | ||
| | | doi=10.1016/j.scienta.2005.01.004 | ||
}} See also "[http://www.actahort.org/books/863/863_48.htm Seasonal Effect of Potassium Chlorate on Flowering and Yield of Longan (Dimocarpus Longan Lour.)]".</ref> | |||
==Safety== | ==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. | 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, such as [[antimony(III) sulfide]], are very dangerous to prepare, as they are extremely shock sensitive. | ||
[[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, such as [[antimony(III) sulfide]], are very dangerous to prepare, as they are extremely shock sensitive. | |||
==See also== | ==See also== | ||
*[[Chloric acid]] | * [[Chloric acid]] | ||
==References== | ==References== | ||
{{Reflist}} | {{Reflist}} | ||
*"Chlorate de potassium. Chlorate de sodium", ''Fiche toxicol. | * "[https://www.inrs.fr/publications/bdd/fichetox/fiche.html?refINRS=FICHETOX_217 Chlorate de potassium. Chlorate de sodium]" {{In lang|fr}}, ''Fiche toxicol.'' no. 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] | * [http://www.freepatentsonline.com/5087334.html Continuous process for the manufacture of potassium chlorate by coupling with a sodium chlorate production plant]. United States Patent 5087334. | ||
==External links== | ==External links== | ||
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{{Chlorates}} | {{Chlorates}} | ||
[[Category:Chlorates]] | |||
[[Category:Potassium compounds]] | [[Category:Potassium compounds]] | ||
[[Category:Pyrotechnic oxidizers]] | [[Category:Pyrotechnic oxidizers]] | ||
Latest revision as of 19:12, 28 June 2025
Potassium chlorate is the inorganic compound with the molecular formula KClO3. In its pure form, it is a white solid. 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 matches.[1] In other applications it is mostly obsolete and has been replaced by safer alternatives in recent decades. It has been used
- in fireworks, propellants and explosives,
- to prepare oxygen, both in the lab and in chemical oxygen generators,
- as a disinfectant, for example in dentifrices and medical mouthwashes,
- 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:
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.[1]
The direct electrolysis of 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 metathesis reaction with potassium chloride:[2]
It can also be produced by passing chlorine gas into a hot solution of caustic potash:[3]
- Template:Chem2
- as seen in this video.[4]
According to X-ray crystallography, potassium chlorate is a dense salt-like structure consisting of chlorate and potassium ions in close association.
Uses
Potassium chlorate was one key ingredient in early firearms percussion caps (primers). It continues in that application, where not supplanted by potassium perchlorate.
Chlorate-based propellants 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 noise-makers known as "crackers", "snappers", "pop-its", "caps" or "bang-snaps", a popular type of novelty firework.
Another application of potassium chlorate is as the oxidizer in a smoke composition such as that used in smoke grenades. 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.[5]
High school and college laboratories often use potassium chlorate to generate oxygen gas. Script error: No such module "Unsubst". 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(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:
Heating it in the absence of a catalyst converts it into potassium perchlorate:[3]
With further heating, potassium perchlorate decomposes to potassium chloride and oxygen:
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.
Potassium chlorate is used in chemical oxygen generators (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 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 limelights.
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:
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 (IEDs). 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.[6] Potassium chlorate was also the main ingredient in the car bomb used in the 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.[7]
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, such as antimony(III) sulfide, are very dangerous to prepare, as they are extremely shock sensitive.
See also
References
- "Chlorate de potassium. Chlorate de sodium" Template:In lang, Fiche toxicol. no. 217, Paris: Institut national de recherche et de sécurité, 2000. 4pp.
- Continuous process for the manufacture of potassium chlorate by coupling with a sodium chlorate production plant. United States Patent 5087334.
External links
Template:Potassium compounds Template:Chlorates
- ↑ a b Script error: No such module "citation/CS1".
- ↑ Script error: No such module "citation/CS1".
- ↑ a b Pradyot Patnaik (2002). Handbook of Inorganic Chemicals. McGraw-Hill. Template:ISBN
- ↑ https://www.youtube.com/watch?v=NuHIClcoHTs
- ↑ Script error: No such module "citation/CS1".
- ↑ Script error: No such module "citation/CS1".
- ↑ Script error: No such module "Citation/CS1". See also "Seasonal Effect of Potassium Chlorate on Flowering and Yield of Longan (Dimocarpus Longan Lour.)".