Strontium sulfate

Strontium sulfate^[1]
Names
	IUPAC name Strontium sulfate
	Other names Celestine
Identifiers
CAS Number	7759-02-6 ;
3D model (JSmol)	Interactive image;
ChemSpider	2341151 ;
ECHA InfoCard	100.028.955
EC Number	231-850-2;
PubChem CID	3084026;
CompTox Dashboard (EPA)	DTXSID10884419 ;
	InChI InChI=1S/H2O4S.Sr/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2 Key: UBXAKNTVXQMEAG-UHFFFAOYSA-L ; InChI=1/H2O4S.Sr/c1-5(2,3)4;/h(H2,1,2,3,4);/q;+2/p-2 Key: UBXAKNTVXQMEAG-NUQVWONBAV;
	SMILES [Sr+2].[O-]S([O-])(=O)=O;
Properties
Chemical 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
Structure
Crystal structure	Orthorhombic, oP24
Space group	Pnma, No. 62
Thermochemistry
Std molar; entropy (S⦵298)	117.0 J·mol-1·K-1
Std enthalpy of; formation (ΔfH⦵298)	-1453.1 kJ·mol-1
Hazards
Flash point	Non-flammable
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). verify (what is ?) 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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[hand-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.

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