Potassium chlorate

Potassium chlorate

The structure of the ions in potassium chlorate The crystal structure of potassium chlorate
Names
Other names Potassium chlorate(V), Potcrate, Berthollet salt
Identifiers
CAS Number	3811-04-9  Y
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL3188561
ChemSpider	18512  Y
ECHA InfoCard	100.021.173
EC Number	223-289-7
PubChem CID	6426889
RTECS number	FO0350000
UNII	H35KS68EE7  Y
UN number	1485
CompTox Dashboard (EPA)	DTXSID6047448
InChI InChI=1S/ClHO3.K/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Y Key: VKJKEPKFPUWCAS-UHFFFAOYSA-M Y InChI=1/ClHO3.K/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Key: VKJKEPKFPUWCAS-REWHXWOFAC
SMILES [K+].[O-]Cl(=O)=O
Properties
Chemical formula	KClO3
Molar mass	122.55 g mol−1
Appearance	white crystals or powder
Density	2.32 g/cm3
Melting point	356 °C (673 °F; 629 K)
Boiling point	400 °C (752 °F; 673 K) decomposes [1]
Solubility in water	3.13 g/100 mL (0 °C) 4.46 g/100 mL (10 °C) 8.15 g/100 mL (25 °C) 13.21 g/100 mL (40 °C) 53.51 g/100 mL (100 °C) 183 g/100 g (190 °C) 2930 g/100 g (330 °C) [2]
Solubility	soluble in glycerol negligible in acetone and liquid ammonia [1]
Solubility in glycerol	1 g/100 g (20 °C) [1]
Magnetic susceptibility (χ)	−42.8·10−6 cm3/mol
Refractive index (nD)	1.40835
Structure
Crystal structure	monoclinic
Thermochemistry
Heat capacity (C)	100.25 J/mol·K [1]
Std molar entropy (S⦵298)	142.97 J/mol·K [3] [1]
Std enthalpy of formation (ΔfH⦵298)	−391.2 kJ/mol [3] [1]
Gibbs free energy (ΔfG⦵)	-289.9 kJ/mol [1]
Hazards
GHS labelling:
Pictograms	[4]
Signal word	Danger
Hazard statements	H271, H302, H332, H411 [4]
Precautionary statements	P220, P273 [4]
NFPA 704 (fire diamond)	2 0 3 OX
Lethal dose or concentration (LD, LC):
LD50 (median dose)	1870 mg/kg (oral, rat) [5]
Safety data sheet (SDS)	ICSC 0548
Related compounds
Other anions	Potassium bromate Potassium iodate Potassium nitrate
Other cations	Ammonium chlorate Sodium chlorate Barium chlorate
Related compounds	Potassium chloride Potassium hypochlorite Potassium chlorite Potassium perchlorate
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

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 matches. ^[6] 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 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:

${\displaystyle {\ce {NaClO3 + KCl -> NaCl + KClO3}}}$

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. ^[6]

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: ^[7]

${\displaystyle {\ce {3 NaOCl -> 2 NaCl + NaClO3}}}$

${\displaystyle {\ce {KCl + NaClO3 -> NaCl + KClO3}}}$

It can also be produced by passing chlorine gas into a hot solution of caustic potash: ^[8]

${\displaystyle {\ce {3 Cl2 + 6 KOH -> KClO3 + 5 KCl + 3 H2O}}}$

Uses

Potassium chlorate burning sugar

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. ^[9]

High school and college laboratories often use potassium chlorate to generate oxygen gas. ^{[ citation needed ]} 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:

${\displaystyle {\ce {2 KClO3(s) ->[\Delta][MnO_2] 3 O2(g) + 2 KCl(s)}}}$

Heating it in the absence of a catalyst converts it into potassium perchlorate: ^[8]

${\displaystyle {\ce {4 KClO3 -> 3 KClO4 + KCl}}}$

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

${\displaystyle {\ce {KClO4 -> KCl + 2O2}}}$

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:

${\displaystyle {\ce {2 KClO3 + H2SO4 -> 2 HClO3 + K2SO4}}}$

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

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.

Insurgents 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. ^[10] 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. ^[11]

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

1. "potassium chlorate" . Retrieved 9 July 2015.
2. Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand. Retrieved 2014-05-29.
3. Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN   978-0-618-94690-7.
4. "Potassium chlorate" . Retrieved 14 February 2022.
5. Michael Chambers. "ChemIDplus - 3811-04-9 - VKJKEPKFPUWCAS-UHFFFAOYSA-M - Potassium chlorate - Similar structures search, synonyms, formulas, resource links, and other chemical information" . Retrieved 9 July 2015.
6. Vogt, Helmut; Balej, Jan; Bennett, John E.; Wintzer, Peter; Sheikh, Saeed Akbar; Gallone, Patrizio (June 15, 2000). "Chlorine Oxides and Chlorine Oxygen Acids". In Ullmann (ed.). Ullmann's Encyclopedia of Industrial Chemistry. Wiley‐VCH Verlag. doi:10.1002/14356007.a06_483. ISBN   9783527303854.
7. Anne Marie Helmenstine, Ph.D. "Potassium Chlorate Synthesis (Substitute) Formula". About.com Education. Retrieved 9 July 2015.
8. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN   0-07-049439-8
9. Daniel J. Wakin and Alan Cowell (March 13, 2013). "New Round of Voting Fails to Name a Pope". The New York Times . Retrieved March 13, 2013.
10. "Afghan bomb makers shifting to new explosives for IEDs". USAToday.com. June 25, 2013. Retrieved 2013-06-25.
11. Manochai, P.; Sruamsiri, P.; Wiriya-alongkorn, W.; Naphrom, D.; Hegele, M.; Bangerth, F. (February 12, 2005). "Year around off-season flower induction in longan (Dimocarpus longan, Lour.) trees by KClO3 applications: potentials and problems". Scientia Horticulturae. 104 (4). 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: 379–390. doi:10.1016/j.scienta.2005.01.004 . Retrieved November 28, 2010.

• "Chlorate de potassium. Chlorate de sodium", Fiche toxicol. n° 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