Barium bicarbonate

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. 

Give the chemical formula for (a) hydrocyanic acid, (b) nickel tetracarbonyl, (c) barium bicarbonate, (d) calcium acetylide (e) potassium carbonate. 

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... 

Information from the WebElemenfs site barium bicarbonate See barium hydro-... 

Calcium ions in seawater muds can be controlled and removed by forming insoluble precipitates accomplished by adding alkalis such as caustic soda, lime, or barium hydroxide. Soda ash or sodium bicarbonate is of no value in controlling the total hardness of sea water. 

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. 

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. 

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. 

Preparation,—In a state of purity, carbonate of soda iB most conveniently prepared from the bicarbonate. To obtain it, the latter salt is washed with cold water until the filtrate, after being acidified with nitric acid, is not rendered turbid by chloride of barium or nitrate of silver. The washed salt is then dried, and by gentle Ignition one half of thB carbonic acid is expelled, and the pure neutral carbonate remains. 

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. 

Other physical phenomena that may be associated, at least partially, with complex formation are the effect of a salt on the viscosity of aqueous solutions of a sugar and the effect of carbohydrates on the electrical conductivity of aqueous solutions of electrolytes. Measurements have been made of the increase in viscosity of aqueous sucrose solutions caused by the presence of potassium acetate, potassium chloride, potassium oxalate, and the potassium and calcium salt of 5-oxo-2-pyrrolidinecarboxylic acid.81 Potassium acetate has a greater effect than potassium chloride, and calcium ion is more effective than potassium ion. Conductivities of 0.01-0.05 N aqueous solutions of potassium chloride, sodium chloride, potassium sulfate, sodium sulfate, sodium carbonate, potassium bicarbonate, potassium hydroxide, and sodium hydroxide, ammonium hydroxide, and calcium sulfate, in both the presence and absence of sucrose, have been determined by Selix.88 At a sucrose concentration of 15° Brix (15.9 g. of sucrose/100 ml. of solution), an increase of 1° Brix in sucrose causes a 4% decrease in conductivity. Landt and Bodea88 studied dilute aqueous solutions of potassium chloride, sodium chloride, barium chloride, and tetra-... 

Because of this transformation, cardiac aglycons and cardenolides should not be exposed to alkalinity greater than that provided by aqueous bicarbonate solution. The use of the Zempl6n procedure88 for the saponification of O-acylated cardenolides is likewise hazardous, although Elderfield and coworkers12 18 were successful in deacetylating their synthetic cardenolides with barium methoxide in methanol. 

Barium carbonate. [CAS 513-77-9). BaC03, white solid, insoluble (Ksp = 5.13 x 10-9), formed (1) by reaction of barium salt solution and sodium carbonate or bicarbonate solution (2) by reaction of barium hydroxide solution and C02. With excess C02 barium hydrogen carbonate, Ba(HC03)2, solution is formed. Barium carbonate decomposes at 1450"C. 

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