3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||147.63 g/mol|
|Melting point||1,494 °C (2,721 °F; 1,767 K) (decomposes)|
|0.0011 g/100 mL (18 °C) |
0.065 g/100 mL (100 °C)
Solubility product (Ksp)
|Solubility in other solvents||Soluble in ammonium chloride |
Slightly soluble in ammonia
Refractive index (nD)
|Safety data sheet||External MSDS data|
|NFPA 704 (fire diamond)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Strontium carbonate is a white, odorless, tasteless powder. Being a carbonate, it is a weak base and therefore is reactive with acids. It is otherwise stable and safe to work with. It is practically insoluble in water (1 part in 100,000). The solubility is increased significantly if the water is saturated with carbon dioxide, to 1 part in 1,000. It is soluble in dilute acids.
Other than the natural occurrence as a mineral, strontium carbonate is prepared synthetically in one of two processes, both of which start with naturally occurring celestine, a mineral form of strontium sulfate (SrSO4). In the "black ash" process, celesite is roasted with coke at 110–1300 °C to form strontium sulfide. The sulfate is reduced, leaving the sulfide:
- SrSO4 + 2 C → SrS + 2 CO2
- SrS + H2O + CO2 → SrCO3 + H2S
- SrS + Na2CO3 → SrCO3 + Na2S
In the "direct conversion" or double-decomposition method, a mixture of celesite and sodium carbonate is treated with steam to form strontium carbonate with substantial amounts of undissolved other solids. This material is mixed with hydrochloric acid, which dissolves the strontium carbonate to form a solution of strontium chloride. Carbon dioxide or sodium carbonate is then used to re-precipitate strontium carbonate, as in the black-ash process.
The most common use is as an inexpensive colorant in fireworks. Strontium and its salts emit a brilliant red color in flame. Unlike other strontium salts, the carbonate salt is generally preferred because of its cost and the fact that it is not hygroscopic. Its ability to neutralize acid is also very helpful in pyrotechnics. Another similar application is in road flares.
Strontium carbonate is also used for making some superconductors such as BSCCO and also for electroluminescent materials where it is first calcined into SrO and then mixed with sulfur to make SrS:x where x is typically europium. This is the "blue/green" phosphor which is sensitive to frequency and changes from lime green to blue. Other dopants can also be used such as gallium, or yttrium to get a yellow/orange glow instead.
Because of its status as a weak Lewis base, strontium carbonate can be used to produce many different strontium compounds by simple use of the corresponding acid.
The cyanobacteria Calothrix, Synechococcus and Gloeocapsa can precipitate strontian calcite in groundwater. The strontium exists as strontianite in solid solution within the host calcite with the strontium content of up to one percent.
- John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–189. ISBN 1138561630.
- Aydoğan, Salih; Erdemoğlu, Murat; Aras, Ali; Uçar, Gökhan; Özkan, Alper (2006). "Dissolution kinetics of celestite (SrSO4) in HCl solution with BaCl2". Hydrometallurgy. 84 (3–4): 239–246. doi:10.1016/j.hydromet.2006.06.001.
- MacMillan, J. Paul; Park, Jai Won; Gerstenberg, Rolf; Wagner, Heinz; Köhler, Karl; Wallbrecht, Peter. "Strontium and Strontium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a25_321.
- "Strontium Carbonate". primaryinfo.com. Retrieved May 31, 2017.
- Henry Lutz Ehrlich; Dianne K Newman (2009). Geomicrobiology, Fifth Edition. CRC Press. p. 177.