Difference between revisions of "Chlorate"
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==Preparation== | ==Preparation== | ||
| − | Chlorates can be prepared via electrolysis of a hot solution of chloride (~70 °C). | + | 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<sup>−</sup> → Cl<sub>2</sub> + 2 e<sup>−</sup> | : 2 Cl<sup>−</sup> → Cl<sub>2</sub> + 2 e<sup>−</sup> | ||
| Line 19: | Line 19: | ||
: 3 HClO → ClO<sub>3</sub><sup>−</sup> + 2 Cl<sup>−</sup> + 3 H<sup>+</sup> | : 3 HClO → ClO<sub>3</sub><sup>−</sup> + 2 Cl<sup>−</sup> + 3 H<sup>+</sup> | ||
| − | Platinum or lead dioxide coated [[electrode]]s are used for this procedure, as they can handle the extreme corrosion of the medium. | + | Platinum or lead dioxide coated [[electrode]]s 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.<ref>The Chlorates and Perchlorates - Anodes, [http://www.chlorates.exrockets.com/anodes.html http://www.chlorates.exrockets.com/anodes.html]</ref> |
| − | Another route involves | + | Another route involves bubbling [[chlorine]] through hot metal hydroxides like [[potassium hydroxide]]: |
: 3 Cl<sub>2</sub> + 6 KOH → 5 KCl + KClO<sub>3</sub> + 3 H<sub>2</sub>O | : 3 Cl<sub>2</sub> + 6 KOH → 5 KCl + KClO<sub>3</sub> + 3 H<sub>2</sub>O | ||
Latest revision as of 19:15, 13 August 2023
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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.
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
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
