Strontium sulfate

Strontium sulfate[1]
Names
IUPAC name
Strontium sulfate
Other names
Identifiers
7759-02-6 Yes
ChemSpider 2341151 Yes
EC number 231-850-2
Jmol-3D images Image
PubChem 3084026
Properties
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)
0.0135 g/100 mL (25 °C)
0.014 g/100 mL (30 °C)
3.44 x 10−7
Solubility insoluble in ethanol, alkalis
slightly soluble in acids
1.622 [2]
Structure
Crystal structure Orthorhombic, oP24
Space group Pnma, No. 62 [3]
Thermochemistry
117.0 J·mol−1·K−1
Std enthalpy of
formation (ΔfHo298)
 -1453.1 kJ·mol−1
Hazards
MSDS External MSDS data
EU Index Not listed
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
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
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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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

  1. ↑ 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.
  2. ↑ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. pp. 560–576. ISBN 0-07-049439-8. Retrieved 2009-06-06.
  3. ↑ Krystek, M. (1979). "Lattice Parameters of (BaxSr100-x)SO4 Doped with Europium". Physica Status Solidi (a) 54 (2): K133. doi:10.1002/pssa.2210540256.
  4. ↑ 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.