{{#if:183.68 g/molwhite orthorhombic crystalsSrSO43.44 x 10-73.96 g/cm31606°C0.0135 g/100 mL (25 °C)
0.014 g/100 mL (30 °C)insoluble in ethanol, alkalis
slightly soluble in acids1.622 [2]|! style="background: #F8EABA; text-align: center;" colspan="2" | Properties
Strontium sulfate[1]
File:Barite-unit-cell-3D-vdW.png
Identifiers
CAS number 7759-02-6 7pxY
PubChem 3084026
ChemSpider 2341151 7pxY
Jmol-3D images Image 1
Molecular formula SrSO4
Molar mass 183.68 g/mol
Appearance white orthorhombic crystals
Density 3.96 g/cm3
Melting point

1606°C

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
ΔfHo298
-1453.1 kJ·mol-1
Standard molar
entropy
So298
117.0 J·mol-1·K-1
Hazards
MSDS External MSDS data



EU Index Not listed
Flash point Non-flammable
Related compounds
Other anions Strontium chloride
Strontium oxide
Other cations Beryllium sulfate
Magnesium sulfate
Calcium sulfate
Barium sulfate
 14pxY (verify) (what is: 10pxY/10pxN?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 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]

SrSO4 Scale in Oilfield

SrSO4 scale is typically only a problem in water-flooded fields because the strontium in the formation water can mix with the sulphate in the injected seawater and drop out SrSO4 scale as they are mixed in the producing wells. It is less a problem in non-water-flooded fields because its formation kinetics is typically slow (unless the temperature is very high, >100C)and the sulphate is typically taken up by barium to form barium sulfate, which has a much faster kinetics.

References

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  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.