Barium bicarbonate sulphate

E. W. Hilgard verified the conclusion and suggested the reaction as an explanation of the formation of natural soda but G. Lunge showed that dil. soln. are required, and on evaporation, the reaction is reversed. H. Taylor (1851) used barium bicarbonate under similar conditions and R. von Wagner showed that a clear soln. of barium bicarbonate decomposes sodium sulphate, forming barium sulphate and sodium bicarbonate, and that a comparatively small proportion of the bicarbonate will complete the reaction between barium carbonate and sodium sulphate. 

If not handled responsibly, geofluids are a potential source of water and soil contamination due to presence of toxic minerals, such as arsenic, barium, antimony, and elevated dissolved solid elements, such as sodium chloride, bicarbonate, sulphate, silica, calcium and potassium (e.g., Clark et al., 2011). Arsenic is highly toxic for the environment and human health thus it could be seriously dangerous in case of geofluids release (e.g., due to pipeline leakage), into the environment. 

The use of barium sulphide as a secondary sulphidizer [4] was examined on oxidized lead ores from Sicily (BaS). The results obtained were encouraging. Sulphidization using Na2S can also be improved with the use of ammonium salts (chloride and sulphate). These reagents are used in cases where the ore contains clay minerals and calcium carbonate, which prevents suphidization due to the production of soluble calcium bicarbonate. The ammonium increases the solubility of calcium carbonate and improves sulphidization. 

Potassium iodide can also be obtained from the aq. extract of kelp or from the mother liquid remaining after the separation of sodium chloride and potassium sulphate from sea-water by evaporation. In E. Allary and J. Pellieux process,8 the liquid is evaporated to dryness and roasted in a special furnace so as to avoid a loss of iodine. The product is fractionally extracted with cold water, when a soln. is obtained which on evaporation gives a residue with 50 per cent, of alkali iodide. This product is extracted.in a special digester with 50 per cent, alcohol. The solvent dissolves little more than the iodides. The alcohol is distilled off, and on evaporation a residue containing about 34 per cent, of potassium iodide, and 66 per cent, of sodium iodide is obtained. To convert the latter into potassium iodide, the proper quantity of a soln. of potassium carbonate is added and carbon dioxide passed into the liquid whereby sodium bicarbonate is precipitated. The precipitate is separated by a filter press, and the small amount of sodium bicarbonate remaining in the soln. is separated by the addition of a little hydrochloric acid and the sodium chloride and potassium iodide separated by fractional crystallization. In E. Sonstadt s process, the mother liquid is treated with chlorine mixed with potassium chlorate or permanganate so as to convert the iodine into iodate. A soln. of a barium salt is added, and the barium iodate treated with potassium sulphate. Barium sulphate is precipitated, and the soln. of potassium iodate is evaporated to dryness and calcined to convert the iodate to iodide. The latter is purified by crystallization. 

J. Townsend patented the use of a mixture of barium carbonate and calcium oxide for converting the sulphate to carbonate. D. Hill and G. Lunge found that the reaction is complete with precipitated barium carbonate, but not with native carbonate, provided an excess of the carbonate and lime be used, the cost also is prohibitive. M. Pongowsky patented the process of converting sodium sulphate into carbonate by adding powdered limestone to an alkaline soln. of the sulphate, and treating the mixture with carbon dioxide with constant agitation. Calcium bicarbonate is formed, and this converts the sodium sulphate into carbonate. 

Sulphates. — Digest 5 gm. of lead peroxide with 30 cc. of a cold saturated aqueous solution of sodium bicarbonate for three or four hours, shaking frequently. Then filter, acidulate the filtrate with hydrochloric acid, boil the solution for ten minutes, and add 2 cc. of barium chloride solution. No precipitate of barium sulphate should form on standing twelve hours. 

Sulphates. — On boiling Mm solution of3 gin. of potassium bicarbonate in 50 cc. of water and (i re. or hydrochloric acid for several minutes, and Mien adding barium chloride solution, no precipitate of barium sulphate should form within twelve hours. 

Scale Soluble salts Bicarbonates of lime, magnesium, etc. Sulphate of lime Blow down. Heat feed to 212° and filter. Use lime or lime and soda or barium carbonate. Live steam feed water heating. Soda or barium carbonate. 

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