Precipitated calcium carbonate is produced by slaking high-calcium quicklime to create a lime slurry that is then combined with captured carbon dioxide (CO 2). The precipitated calcium carbonate production process consists of decarbonating limestone, which separates the CaO (calcium oxide) and CO 2 (carbon dioxide). Precipitated Calcium Carbonate (PCC) production requires consistent quicklime quality to produce a quality carbonate. The strontium exists as strontianite in solid solution within the host calcite with the strontium content of up to one percent.How Is Precipitated Calcium Carbonate (PCC) Made? The cyanobacteria Calothrix, Synechococcus and Gloeocapsa can precipitate strontian calcite in groundwater. Other dopants can also be used such as gallium, or yttrium to get a yellow/orange glow instead.īecause 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. This is the "blue/green" phosphor which is sensitive to frequency and changes from lime green to blue. 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. It is also used in the manufacturing of strontium ferrites for permanent magnets which are used in loudspeakers and door magnets. It has some properties similar to barium carbonate. It acts as a flux and also modifies the color of certain metallic oxides. It is widely used in the ceramics industry as an ingredient in glazes. It is used in the preparation of iridescent glass, luminous paint, strontium oxide, and strontium salts and in refining sugar and certain drugs. It is used for manufacturing color television receivers to absorb electrons resulting from the cathode. Strontium carbonate is used for electronic applications. Another similar application is in road flares. Its ability to neutralize acid is also very helpful in pyrotechnics. Unlike other strontium salts, the carbonate salt is generally preferred because of its cost and the fact that it is not hygroscopic. Strontium and its salts emit a brilliant red color in flame. The most common use is as an inexpensive colorant in fireworks. Nitric acid reacts with strontium carbonate to form strontium nitrate. Carbon dioxide or sodium carbonate is then used to re-precipitate strontium carbonate, as in the black-ash process. This material is mixed with hydrochloric acid, which dissolves the strontium carbonate to form a solution of strontium chloride. 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. SrS + H 2O + CO 2 → SrCO 3 + H 2S SrS + Na 2CO 3 → SrCO 3 + Na 2S The sulfate is reduced, leaving the sulfide:Ī mixture of strontium sulfide with either carbon dioxide gas or sodium carbonate then leads to formation of a precipitate of strontium carbonate. In the "black ash" process, celesite is roasted with coke at 1100–1300 ☌ to form strontium sulfide. 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 (SrSO 4). The solubility is increased significantly if the water is saturated with carbon dioxide, to 0.1 g per 100 ml. It is practically insoluble in water (0.0001 g per 100 ml). It is otherwise stable and safe to work with. Being a carbonate, it is a weak base and therefore is reactive with acids. Strontium carbonate is a white, odorless, tasteless powder. It occurs in nature as the mineral strontianite. Strontium carbonate (SrCO 3) is the carbonate salt of strontium that has the appearance of a white or grey powder.
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