Barium perchlorate
| Names | |
|---|---|
| IUPAC name
Barium perchlorate
| |
| Other names
Barium diperchlorate
Perchloric acid, barium salt | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| BaCl2O8 Ba(ClO4)2 | |
| Molar mass | 336.228 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 3.2 g/cm3 (20 °C) |
| Melting point | 470–505 °C (878–941 °F; 743–778 K) |
| Boiling point | Decomposes |
| 198 g/100 ml (25 °C)[1] | |
| Solubility | Soluble in acetone, ethanol Insoluble in diethyl ether |
| Solubility in acetone | 125 g/100 ml (25 °C)[1] |
| Solubility in ammonia | 67.2 g/100 ml[2] |
| Solubility in butanol | 58.2 g/100 ml (20 °C)[3] |
| Solubility in ethanol | 125 g/100 ml (25 °C)[1] |
| Solubility in isobutanol | 56.2 g/100 ml (20 °C)[3] |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
251 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
-774 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Related compounds | |
| Related compounds
|
Barium chloride Barium chlorate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Barium perchlorate (Ba(ClO4)2) is a powerful oxidizing agent, mainly used in pyrotechnics.
Contents
Properties
Chemical
Barium perchlorate decomposes when heated to high temperatures to liberate oxygen.
Addition of conc. sulfuric acid will produce anhydrous perchloric acid. The resulting barium sulfate is insoluble in solvents, thus the perchloric acid can be purified by simply filtering the product.
- H2SO4 + Ba(ClO4)2 → 2 HClO4 + BaSO4 ↓
Physical
Barium perchlorate is a white solid, soluble in water.
Availability
Some fireworks may contain barium perchlorate.
Barium perchlorate can be bought from chemical suppliers.
Preparation
Can be prepared by reacting perchloric acid with barium oxide, hydroxide or carbonate. The resulting barium perchlorate solution is then concentrated and cooled to recrystallize the salt.
- 2 HClO4 + BaO → Ba(ClO4)2 + H2O
- 2 HClO4 + Ba(OH)2 → Ba(ClO4)2 + 2 H2O
- 2 HClO4 + BaCO3 → Ba(ClO4)2 + H2O + CO2
Another route involves the reaction between barium chloride and silver perchlorate.
- BaCl2 + 2 AgClO4 → Ba(ClO4)2 + 2 AgCl ↓
Projects
- Make flash powder
- Make concentrated perchloric acid
- Make transition metal perchlorates
Handling
Safety
Barium perchlorate is a strong oxidizer and also toxic if ingested.
Storage
In closed bottles, away from combustible materials.
Disposal
Barium perchlorate, like other perchlorates, can be reduced with elemental iron in the absence of air under UV light to barium chloride, which in term can be precipitated to barium sulfate, which has low toxicity and can be safely disposed of.
References
- ↑ 1.0 1.1 1.2 Nekrasov B.V. Fundamentals of General Chemistry. - T.1. - M.: Chemistry, 1973 (Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973)
- ↑ Handbook of experimental data on the solubility of salt systems. - T. 4. - L .: GNTIHL, 1963 pp. 2694 (Справочник экспериментальных данных по растворимости солевых систем. - Т. 4. - Л.: ГНТИХЛ, 1963 pp. 2694)
- ↑ 3.0 3.1 3.2 3.3 Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940
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- Chemical compounds
- Inorganic compounds
- Barium compounds
- Perchlorates
- Oxidizing agents
