Strontium perchlorate
Chemical compound (Sr(ClO4)2)
From Wikipedia, the free encyclopedia
Strontium perchlorate is a deliquescent white crystalline compound with the formula Sr(ClO4)2.[1]
| Names | |
|---|---|
| Other names
Strontium(II) perchlorate; Strontium diperchlorate | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.033.272 |
| EC Number |
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PubChem CID |
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CompTox Dashboard (EPA) |
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| Properties | |
| Sr(ClO4)2 | |
| Molar mass | 286.51 g·mol−1 |
| Appearance | White crystals |
| Density | 2.973 g/cm3[1] |
| Melting point | 477 °C (891 °F; 750 K)[1] (decomposes vigorously) |
| 309.7 g/100 g | |
| Solubility in ethyl acetate | 136.9 g/100 g |
| Solubility in methanol | 221.0 g/100 g |
| Solubility in ethanol | 180.7 g/100 g |
| Solubility in 1-propanol | 140.4 g/100 g |
| Solubility in 1-butanol | 113.5 g/100 g |
| Solubility in isobutanol | 77.9 g/100 g |
| Solubility in acetone | 140.1 g/100 g |
| Structure[2] | |
| orthorhombic | |
| Pbca | |
a = 14.18206 Å, b = 9.78934 Å, c = 9.37624 Å α = 10.009°, β = 90°, γ = 90° | |
Lattice volume (V) |
1301.73 Å3 |
| 8 | |
| Hazards | |
| GHS labelling:[3] | |
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| Danger | |
| H272, H315, H319, H335 | |
| P210, P221, P280, P305+P351+P338, P403+P233, P501 | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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It is a strong oxidizer which gives red flames. It can be used in pyrotechnics; however, usually the more common strontium nitrate is used. Strontium perchlorate has been used in gelled flame compositions where its hygroscopic nature isn't an issue, in a polymerized candle composition that excluded water, and in an experimental high-atmosphere flash powder.[1]
It is also used in Liquid Injection Thrust Vector Control (LITVC) in solid-propellant rockets to enable steering control with a simple fixed nozzle.[citation needed]
Strontium perchlorate has been characterized in multiple hydrated forms; a trihydrate (Sr(ClO4)2·3H2O), tetrahydrate (Sr(ClO4)2·4H2O) and nonahydrate (Sr(ClO4)2·9H2O).[2]
Synthesis
Hydrated forms may be prepared by dissolving pure strontium nitrate in an excess of perchloric acid, neutralizing the excess acid with strontium carbonate, centrifuging off solids, and chilling to precipitate crystals.
The anhydrous form may be prepared by drying the hydrate at 250 °C (482 °F), which gives a yield of 50%, or by the addition of anhydrous perchloric acid to a solution of strontium ion in anhydrous trifluoroacetic acid followed by filtration of the precipitated solid and removal of excess acid under vacuum.[1]
