Potassium chlorate
Names Other names Identifiers ChEMBL ChemSpider ECHA InfoCard 100.021.173 EC Number RTECS number UNII UN number 1485 Properties 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 negligible in acetone and liquid ammonia[1] Solubility in glycerol 1 g/100g (20 °C (68 °F; 293 K))[1] −43.8×10−6 cm3/mol 1.40835 Structure monoclinic Thermochemistry[1] −391.2 J/(mol·K) 142.97 J/(mol·K)[3] −391.2 kJ/mol[3] −289.9 kJ/mol Hazards GHS labelling:[4] Danger H271, H301, H401[4] P210, P220, P221, P264, P270, P273, P280, P283, P301+P310+P330, P306+P360, P370+P378, P371+P380+P375, P405, P501[4] NFPA 704 (fire diamond) Lethal dose or concentration (LD, LC): 100 mg/kg (oral, rat)[5] >5.1 mg/L[5] Related compounds
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.[6]
On the industrial scale, potassium chlorate is produced by the salt metathesis reaction of sodium chlorate and potassium chloride:
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:[citation needed]
3 NaOCl → 2 NaCl + NaClO3 KCl + NaClO3 → NaCl + KClO3
It can also be produced by passing chlorine gas into a hot solution of potassium hydroxide:[7][page needed]
3 Cl2 + 6 KOH → KClO3 + 5 KCl + 3 H2O
Potassium chlorate was one key ingredient in early firearms percussion caps (primers).[8]
Another application of potassium chlorate is as the oxidizer in smoke compositions such as those used in smoke grenades.[9]
Potassium chlorate readily decomposes if heated while in contact with a catalyst, typically manganese(IV) dioxide (MnO2).[10] 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) + MnO2(cat) → 3 O2(g) + 2 KCl(s)
Heating it in the absence of a catalyst converts it into potassium perchlorate:[7][page needed]
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 and from contact between chlorates and hydrocarbon sealing greases. Impurities in potassium chlorate itself can also cause problems.
Potassium chlorate reacts with sulfuric acid to form highly reactive chlorine dioxide, potassium sulfate, oxygen, and water:[11]
4 KClO3 + 2 H2SO4 → 2 K2SO4 + 4 ClO2 (g) + O2 (g) + 2 H2O
Chlorine dioxide, combined with oxygen gas (and any remaining potassium chlorate) is sufficiently reactive that it spontaneously ignites if combustible material (sugar, paper, etc.) is present.[citation needed]
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.[12]
Potassium chlorate is used also as a pesticide. In Finland it was sold under trade name Fegabit.[citation needed]
Potassium chlorate is used to force the blossoming stage of the longan tree, causing it to produce fruit in warmer climates.[13][14]
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.[15] Potassium chlorate was also the main ingredient in the car bomb used in the 2002 Bali bombings that killed 202 people.[16]
Potassium chlorate is a very powerful oxidizer. 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 on contact with sulfuric acid. Mixtures of potassium chlorate with lactose,[17] sulfur,[17]: 18-5 sulfides such as antimony(III) sulfide,[17]: 18-5 or phosphorus are extremely shock and friction sensitive.
- Chloric acid
