POTASSIUM CHLORATE

Synonyms:
POTASSIUM CHLORATE; 3811-04-9; Fekabit; Potcrate; Kaliumchlorat; Anforstan; Berthollet salt; Salt of tarter; Berthollet's salt; Chlorate of potash; Chloric acid, potassium salt; Potassium oxymuriate; Oxymuriate of potash; Chlorate of potassium; Potash chlorate (DOT); Chlorate de potassium [French], HSDB 1110; Potassio (clorato di) [Italian]; Potassium (chlorate de) [French]; EINECS 223-289-7; Potassium chlorate, 99%, extra pure; Potassium chlorate, 99+%, ACS reagent; Potassium chlorate(V); Postassium Chlorate; Potasyum clorat; Potassyum clorat; Potasyum klorat; Potasyum klorate; chlorate de potassium; chlorat de potassium; POTASYUM KLORAT; POTASSIUM CHLORATE; POTASSIUM CHLORAT; POTASSİUM CHLORATE; POTASSİUM CHLORAT; Potassium chlorate(V);  Potcrate; Chlorate de potassium; OXYMURIATE DE POTASSIUM; POTASSIUM (CHLORATE DE); POTASSIUM, CHLORATE DE; BERTHOLLET SALT; BERTHOLLET'S SALT; CHLORATE OF POTASH; CHLORIC ACID, POTASSIUM SALT; OXYMURIATE OF POTASH; Potassium chlorate; POTASSIUM OXYMURIATE

POTASSIUM CHLORATE

Potassium chlorate

Potassium chlorate
The structure of the ions in potassium chlorate
The crystal structure of potassium chlorate
Potassium chlorate crystals
Names
Other names
Potassium chlorate(V), Potcrate
Identifiers
CAS Number    
3811-04-9 check
3D model (JSmol)    
Interactive image
ChemSpider    
18512 check
ECHA InfoCard    100.021.173 
EC Number    
223-289-7
PubChem CID    
6426889
RTECS number    
FO0350000
UNII    
H35KS68EE7 check
UN number    1485
CompTox Dashboard (EPA)    
DTXSID6047448 
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 (So298)    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
Safety data sheet    ICSC 0548
GHS pictograms    GHS03: OxidizingGHS07: HarmfulGHS09: Environmental hazard[4]
GHS Signal word    Danger
GHS hazard statements    H271, H302, H332, H411[4]
GHS precautionary statements    P220, P273[4]
NFPA 704 (fire diamond)    
NFPA 704 four-colored diamond
023OX
Lethal dose or concentration (LD, LC):
LD50 (median dose)    1870 mg/kg (oral, rat)[5]
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).
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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. It is the most common chlorate in industrial use. It is used,

as an oxidizing agent,
to prepare oxygen,
as a disinfectant,
in safety matches,
in explosives and fireworks,
in cultivation, forcing the blossoming stage of the longan tree, causing it to produce fruit in warmer climates.[6]

Production
On the industrial scale, potassium chlorate is produced by the Liebig process: passing chlorine into hot calcium hydroxide, subsequently adding potassium chloride:[7]

6 Ca(OH)2 + 6 Cl2 → Ca(ClO3)2 + 5 CaCl2 + 6 H2O
Ca(ClO3)2 + 2 KCl → 2 KClO3 + CaCl2
The electrolysis of KCl in aqueous solution is also used sometimes, in which elemental chlorine formed at the anode react 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:[8]

3 NaOCl(aq) → 2 NaCl(s) + NaClO3(aq)
KCl(aq) + NaClO3(aq) → NaCl(aq) + KClO3(s)
It can also be produced by passing chlorine gas into a hot solution of caustic potash:[9]

3 Cl2(g) + 6 KOH(aq) → KClO3(aq) + 5 KCl(aq) + 3 H2O(l)
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", 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.[10]

Potassium chlorate is often used in high school and college laboratories 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:

2 KClO3(s) → 3 O2(g) + 2 KCl(s)
Heating it in the absence of a catalyst converts it into potassium perchlorate:[9]

4 KClO3 → 3 KClO4 + KCl
With further heating, potassium perchlorate decomposes to potassium chloride and oxygen:

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, as well as 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 also traced to this substance. 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:

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 the dramatic 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.[11] Potassium chlorate was also the main ingredient in the car bomb used in 2002 Bali bombings that killed 202 people.

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.

Molecular Weight of Potassium chlorate    122.55 g/mol    Computed by PubChem 2.1 (PubChem release 2019.06.18)
Hydrogen Bond Donor Count of Potassium chlorate    0    Computed by Cactvs 3.4.6.11 (PubChem release 2019.06.18)
Hydrogen Bond Acceptor Count of Potassium chlorate    3    Computed by Cactvs 3.4.6.11 (PubChem release 2019.06.18)
Rotatable Bond Count of Potassium chlorate    0    Computed by Cactvs 3.4.6.11 (PubChem release 2019.06.18)
Exact Mass of Potassium chlorate    121.917303 g/mol    Computed by PubChem 2.1 (PubChem release 2019.06.18)
Monoisotopic Mass of Potassium chlorate    121.917303 g/mol    Computed by PubChem 2.1 (PubChem release 2019.06.18)
Topological Polar Surface Area of Potassium chlorate    57.2 Ų    Computed by Cactvs 3.4.6.11 (PubChem release 2019.06.18)
Heavy Atom Count of Potassium chlorate    5    Computed by PubChem
Formal Charge of Potassium chlorate    0    Computed by PubChem
Complexity of Potassium chlorate    49.8    Computed by Cactvs 3.4.6.11 (PubChem release 2019.06.18)
Isotope Atom Count of Potassium chlorate    0    Computed by PubChem
Defined Atom Stereocenter Count of Potassium chlorate    0    Computed by PubChem
Undefined Atom Stereocenter Count of Potassium chlorate    0    Computed by PubChem
Defined Bond Stereocenter Count of Potassium chlorate    0    Computed by PubChem
Undefined Bond Stereocenter Count of Potassium chlorate    0    Computed by PubChem
Covalently-Bonded Unit Count of Potassium chlorate    2    Computed by PubChem
Compound  of Potassium chlorate Is Canonicalized    Yes

Physical Description    
Potassium chlorate appears as a white crystalline solid. Forms a very flammable mixture with combustible materials. Mixture may be explosive if combustible material is very finely divided. Mixture may be ignited by friction. Contact with strong sulfuric acid may cause fires or explosions. May spontaneously decompose and ignite when mixed with ammonium salts. May explode under prolonged exposure to heat or fire. Used to make matches, paper, explosives, and many other uses.

Potassium chlorate, aqueous solution appears as a colorless liquid. Denser than water. Contact may irritate skin, eyes and mucous membranes. May be toxic by ingestion. Used to make other chemicals. Ignites organic materials upon contact 

Product Information

CAS number of Product Information    3811-04-9
EC index number of Product Information    017-004-00-3
EC number of Product Information    223-289-7
Grade of Product Information    ACS,Reag. Ph Eur
Hill Formula of Product Information    ClKO₃
Chemical formula of Product Information    KClO₃
Molar Mass of Product Information    122.55 g/mol
HS Code of Product Information    2829 19 00    3811-04-9
EC index number    017-004-00-3
EC number of Product Information    223-289-7
Grade of Product Information    ACS,Reag. Ph Eur
Hill Formula of Product Information    ClKO₃
Chemical formula of Product Information    KClO₃
Molar Mass of Product Information    122.55 g/mol

Potassium chlorate (KClO3) is a strong oxidizing agent that has a wide variety of uses. It is or has been a component of explosives, fireworks, safety matches, and disinfectants. As a high school or college chemistry student, you may have used it to generate oxygen in the lab.

Because it is a strong oxidizer, KClO3 must be kept from contacting organic matter; reduced inorganic materials such as elemental sulfur, phosphorus; and iodine; and concentrated acids.

The use of KClO3 in matches dates back to 1826, when English chemist John Walker combined it with antimony(III) sulfide, gum, and starch. When formed into matches, the mixture sometimes (but not always) ignited when struck on sandpaper. Later on, white phosphorus replaced antimony sulfide to make matches more reliable. Eventually, the toxic white phosphorus was superseded by the red allotrope.

Modern safety matches contain no phosphorus; but red phosphorus is embedded in the rough surfaces of matchboxes. Upon striking, the phosphorus ignites, liberating oxygen from the match’s KClO3, which in turn ignites combustible substances (e.g., sulfur) in the matchhead.