Chlorate
 |
This article is a stub. Please help Sciencemadness Wiki by expanding it, adding pictures, and improving existing text.
|
A chlorate is chemical compound containing the ClO3− ion.
Contents
General properties
Chlorates are powerful oxidizers and should be kept away from organics or easily oxidized materials. Mixtures of chlorate salts with virtually any combustible material (sugar, sawdust, charcoal, organic solvents, metals, etc.) will readily deflagrate.
Mixtures of potassium chlorate and sulfur are very sensitive to friction, and are know to detonate when subjected to shock or friction.
Ammonium chlorate is highly unstable in both solution and solid, and has been known to spontaneously detonate at room temperature in solid form.
Availability
Sodium and potassium chlorates were available in the past as weedkiller, but due to their hazards they're been banned in many countries. Safety match heads contain potassium chlorate, but extracting it might not be very economical.
In the EU, the sale and ownership of sodium and potassium chlorate is restricted, to any product containing more than 40% chlorates. The EU directive that restricts chlorates only applies to the two chlorate salts, and thus would not apply to other chlorates, however individual countries may either ban them totally or partially, so always check the national laws of each country.
Preparation
Chlorates can be prepared via electrolysis of a hot solution of chloride (~70 °C). Sodium or potassium chloride is the most commonly used starting material, the difference being the lower solubility of potassium chlorate.
- 2 Cl− → Cl2 + 2 e−
- Cl2 + H2O ⇌ HClO + Cl− + H+
- 3 HClO → ClO3− + 2 Cl− + 3 H+
Platinum or lead dioxide coated electrodes are used for this procedure, as they can handle the extreme corrosion of the medium. Graphite also able to withstand the conditions of a chlorate cell for some time, but it will eventually corrode.[1]
Another route involves bubbling chlorine through hot metal hydroxides like potassium hydroxide:
- 3 Cl2 + 6 KOH → 5 KCl + KClO3 + 3 H2O
The chlorine can be easily produced by acidifying a hypochlorite salt or TCCA with hydrochloric acid.
Safety
Chlorates are powerful oxidizers. Keep them away from open flames and flammable materials.
Chlorates are toxic if ingested.
References
- ↑ The Chlorates and Perchlorates - Anodes, http://www.chlorates.exrockets.com/anodes.html
