Strontium sulfate


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).

Strontium sulfate[1]
IUPAC name
Strontium sulfate
Other names
  • 7759-02-6 checkY
3D model (JSmol)
  • Interactive image
  • 2341151 checkY
ECHA InfoCard 100.028.955 Edit this at Wikidata
EC Number
  • 231-850-2
  • 3084026
  • 7Q3KX2L47F ☒N
  • DTXSID10884419 Edit this at Wikidata
  • InChI=1S/H2O4S.Sr/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2 checkY
  • InChI=1/H2O4S.Sr/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2
  • [Sr+2].[O-]S([O-])(=O)=O
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
−57.9·10−6 cm3/mol
Orthorhombic, oP24
Pnma, No. 62[3]
117.0 J·mol−1·K−1
-1453.1 kJ·mol−1
NFPA 704 (fire diamond)
Flash point Non-flammable
Safety data sheet (SDS) External MSDS data
Related compounds
Other anions
Strontium chloride
Strontium oxide
Other cations
Beryllium sulfate
Magnesium sulfate
Calcium sulfate
Barium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references


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 and chemistryEdit

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]

The low aqueous solubility of strontium sulfate can lead to scale formation in processes where these ions meet. For example, it can form on surfaces of equipment in underground oil wells depending on the groundwater conditions.[5][6]


  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. Bibcode:1979PSSAR..54..133K. 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.
  5. ^ Jacques, Donald F.; Bourland, Brent I. (1983). "A Study of Solubility of Strontium Sulfate". Society of Petroleum Engineers Journal. 23 (2): 292–300. doi:10.2118/9625-PA.
  6. ^ doi:10.1520/JAI100958