Strontium sulfate
| Strontium sulfate[1] | |
|---|---|
 | |
| IUPAC name Strontium sulfate | |
| Other names | |
| Identifiers | |
| CAS number | 7759-02-6  |
| PubChem | 3084026 |
| ChemSpider | 2341151 |
| EC number | 231-850-2 |
| Jmol-3D images | {{#if:[Sr+2].[O-]S([O-])(=O)=O|Image 1 |
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| Properties | |
| Molecular formula | SrSO4 |
| Molar mass | 183.68 g/mol |
| Appearance | white orthorhombic crystals |
| Density | 3.96 g/cm3 |
| Melting point | 1,606 °C; 2,923 °F; 1,879 K |
| Solubility in water | 0.0135 g/100 mL (25 °C) 0.014 g/100 mL (30 °C) |
| Solubility product, Ksp | 3.44 x 10-7 |
| Solubility | insoluble in ethanol, alkalis slightly soluble in acids |
| Refractive index (nD) | 1.622 [2] |
| Structure | |
| Crystal structure | Orthorhombic, oP24 |
| Space group | Pnma, No. 62 [3] |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-1453.1 kJ·mol-1 |
| Standard molar entropy S |
117.0 J·mol-1·K-1 |
| Hazards | |
| MSDS | External MSDS data |
| EU Index | Not listed |
| NFPA 704 |
 0
1
0
|
| Flash point | Non-flammable |
| Related compounds | |
| Other anions | Strontium chloride Strontium oxide |
| Other cations | Beryllium sulfate Magnesium sulfate Calcium sulfate Barium sulfate |
(verify) (what is: / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
| Infobox references | |
Strontium sulfate (SrSO4) is the sulfate salt of strontium. It is a white crystalline powder and occurs in nature as the mineral celestine. It is poorly soluble in water to the extent of 1 part in 8,800. It is more soluble in dilute HCl and nitric acid and appreciably soluble in alkali chloride solutions (e.g. sodium chloride).
Structure
Strontium sulfate is a polymeric material, isostructural with barium sulfate. Crystallized strontium sulfate is utilized by a small group of radiolarian protozoa, called the Acantharea, as a main constituent of their skeleton.
Applications
Strontium sulfate is of interest as a naturally occurring precursor to other strontium compounds, which are more useful. In industry it is converted to the carbonate for use as ceramic precursor and the nitrate for use in pyrotechnics.[4]
References
- ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–87; 1364. ISBN 0-8493-0594-2.
- ↑ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. pp. 560–576. ISBN 0-07-049439-8. Retrieved 2009-06-06.
- ↑ Krystek, M. (1979). "Lattice Parameters of (BaxSr100-x)SO4 Doped with Europium". Physica Status Solidi (a) 54 (2): K133. doi:10.1002/pssa.2210540256.
- ↑ J. Paul MacMillan, Jai Won Park, Rolf Gerstenberg, Heinz Wagner, Karl Köhler, Peter Wallbrecht “Strontium and Strontium Compounds” in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a25_321.
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