Strontium bicarbonate

Strontium carbonate, [CAS 1633-05-2J. STCO3, while solid, insoluble (K.t — 9.4 > 10-lC). formed (l) by reaction of strontium salt solution and sodium carbonate or bicarbonate solntion. (2i by reaction of strontium hydroxide solution and CO2. Strontium carbonate decomposes at l,200nC to form strontium oxide and CO , and is dissolved by excess C02, forming strontium bicarbonate, Sr(HCC>3)2, solution. 

Strontium hydrogencarbonate (strontium bicarbonate Sr(HC03)2) A compound present in solutions formed by the action of carbon dioxide on a suspension in cold water of strontium carbonate, to which it reverts on heating ... 

Information from the WebElements site strontium bicarbonate SeesxRoNTiuM... 

Major constituents (greater than 5 mg/L) Minor constituents (O.Ol-lO.Omg/L) Selected trace constituents (less than 0.1 mg/L) Bicarbonate, calcium, carbonic acid, chloride, magnesium, silicon, sodium, sulfate Boron, carbonate, fluoride, iron, nitrate, potassium, strontium Aluminum, arsenic, barium, bromide, cadmium, chromium, cobalt, copper, gold, iodide, lead, Uthium, manganese, molybdenum, nickel, phosphate, radium, selenium, silver, tin, titanium, uranium, vanadium, zinc, zirconium... 

Admixture incompatibilities - Magnesium sulfate in solution may result in a precipitate formation when mixed with solutions containing Alcohol (in high concentrations) alkali carbonates and bicarbonates alkali hydroxides arsenates barium calcium clindamycin phosphate heavy metals hydrocortisone sodium succinate phosphates polymyxin B sulfate procaine hydrochloride salicylates strontium tartrates. 

IV.2 CARBONATES, CO2- Solubility All normal carbonates, with the exception of those of the alkali metals and of ammonium, are insoluble in water. The hydrogen carbonates or bicarbonates of calcium, strontium, barium, magnesium, and possibly of iron exist in aqueous solution they are formed by the action of excess carbonic acid upon the normal carbonates either in aqueous solution or suspension and are decomposed on boiling the solutions. 

At intermediate depths (down to 500 m) groundwaters rapidly increase in concentration primarily by the addition of SO4 and Cl. The concentration of bicarbonate ions decreases because of the precipitation of mineral phases such as calcite. Local variations in chemistry and anions may be due to a variety of rock-water interactions or local processes that result in Na-SO4, Na-HC03, and Mg-S04 type waters. The pH begins to rise in this zone and oxygenconsuming reactions and redox mineral controls tend to lower the Eh. The brackish and saline waters found at these intermediate depths have longer residence times. Deep saline waters and brines occur in most locations below depths of 500 m. These fluids are Ca-Na-Cl or Na-Ca-Cl in composition and can have total dissolved loads up to 350 g L. Minor elements such as bromide and strontium can here be thousands of milligrams per liter. 

Strontium carbonate is almost insoluble in water 0.001 gram per 100 grams of water at 24 C. The solution is alkaline and the pH value was 8.9 at 35 C. If a composition consists mainly of aluminium and nitrates including strontium carbonate, such an alkaline mixture has a risk of spontaneous decomposition in wet state. Strontium carbonate dissolves in water as the bicarbonate, if the water contains COa.. 

Magnesium is the third most abundant element in seawater, behind sodium and chorine, and has an average concentration of approximately 1300 ppm. Table 3.2 displays the major and some minor elemental constituents of seawater. Eleven major constituent ions account for 99.5% of the total solutes present in seawater. These 11 are chloride, sulfate, bicarbonate, bromide, fluoride, sodium, magnesium, calcium, potassium, strontium, and boron, and they largely determine the chemistry of seawater. 

Sodium and potassium bicarbonates are less soluble than the carbonates. Magnesium, calcium, strontium and barium bicarbonates exist only in solution. Attempts to remove the water destroy the compounds... 

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