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Strontium: Strontium Carbonate
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Strontium carbonate is derived from strontium, one of the alkaline-earth metal elements (main Group IIa of the periodic table). It comprises 0.04 percent of the earth's crust, and is found naturally principally when combined as strontianate or celestite. Strontium alone (in the form of the strontium-90 isotope) is notable as the principal health hazard in radioactive fallout; at the same time... the element has been used for the treatment of bone cancer. This contrasts with the stability of the naturally occurring minerals, which are stable and used reliably and safely in a variety of areas, including food production.
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Strontium sulphide, SrS, is formed when the carbonate is heated to redness in a stream of sulphuretted hydrogen. It phosphoresces very slightly when pure. Strontium sulphate, SrSO 4, found in the mineral kingdom as celestine, is formed when sulphuric acid or a soluble sulphate is added to a solution of a strontium salt. It is a colourless, amorphous solid, which is almost insoluble in water, its solubility diminishing with increasing temperature; it is appreciably soluble in concentrated sulphuric acid. When boiled with alkaline carbonates it is converted into strontium carbonate.
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Strontium has uses similar to those of calcium and barium, but it is rarely employed because of its higher cost. Principal uses of strontium compounds are in pyrotechnics, for the brilliant reds in fireworks and warning flares and in greases. A little is used as a getter in vacuum tubes to remove the last traces of air. Most strontium is used as the carbonate in special glass for television screens and visual display units. Although strontium-90 is a dangerously radioactive isotope, it is a useful by-product of nuclear reactors from whose spent fuel is extracted. Its high-energy radiation can be used to generate an electric current, and for this reason it can be used in space vehicles, remote weather stations and navigation buoys.
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Strontium occurs in nature in celestite (strontium sulfate) use strontianite (strontium carbonate). In earth's crust total amt is est to be 430 g/ton; in sea water 10 ppm. Found in small quantities associated with calcium or barium minerals.
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Strontium is present in seawater as the Sr++ ion, meaning that it carries two positive charges, just as calcium and magnesium do. Most of the strontium is present as the free ion, with only water molecules attached to it.7 A small portion (about 10%) of the strontium is present as a soluble ion pair with sulfate (SrSO4), and much smaller portions are paired with bicarbonate (SrHCO3+), carbonate (SrCO3), fluoride (SrF+), borate (SrB(OH)4+), and hydroxide (SrOH+).7 Habib Sekha (owner of Salifert) has suggested that strontium in seawater may be ion paired to sulfate to a much greater degree than suggested above, but I have not seen strong evidence to support that hypothesis.
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Strontium fluoride, SrF 2, is obtained by the action of hydrofluoric acid on the carbonate, or by the addition of potassium fluoride to strontium chloride solution. It may be obtained crystalline by fusing the anhydrous chloride with a large excess of potassium hydrogen fluoride or by heating the amorphous variety to redness with an excess of an alkaline chloride. Strontium chloride, SrC1 2.6H 2 O, is obtained by dissolving the carbonate in hydrochloric acid, or by fusing the carbonate with calcium chloride and extracting the melt with water. It crystallizes in small colourless needles and is easily soluble in water; the concentrated aqueous solution dissolves bromine and iodine readily. By concentrating the aqueous solution between 90-130° C., or by passing hydrochloric acid gas into a saturated aqueous solution, a second hydrated form of composition, SrC1 2.2H 2 O, is obtained. The anhydrous chloride is formed by heating strontium or its monoxide in chlorine, or by heating the hydrated chloride in a current of hydrochloric acid gas.
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Strontium Carbonate