Difference between revisions of "Barium perchlorate"
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==Preparation== | ==Preparation== | ||
| − | Can be prepared by reacting [[perchloric acid]] with barium oxide, hydroxide or carbonate. | + | 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. |
| + | |||
| + | Another route involves the reaction between [[barium chloride]] and [[silver perchlorate]]. | ||
==Projects== | ==Projects== | ||
Revision as of 20:49, 31 May 2017
| Names | |
|---|---|
| IUPAC name
Barium perchlorate
| |
| Other names
Barium diperchlorate
Perchloric acid, barium salt | |
| Properties | |
| Ba(ClO4)2 | |
| Molar mass | 336.228 g/mol |
| Appearance | White solid |
| Density | 3.2 g/cm3 |
| Melting point | 505 °C (941 °F; 778 K) |
| 66.48 g/100 ml (25 °C) | |
| 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.
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.
Another route involves the reaction between barium chloride and silver perchlorate.
Projects
- Make flash powder
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.
