Barium carbonate , solubility

White precipitate of barium carbonate soluble in dilute acids White precipitate of barium oxalate soluble in dilute acids Heavy, white, finely divided precipitate of barium sulfate White precipitate of barium sulfate... 

Ammonium carbonate solution white precipitate of barium carbonate, soluble in acetic acid and in dilute mineral acids. 

Although the superoxide ion was also successful in destroying some aliphatic and aromatic halogenated hydrocarbons, resulting in the formation of barium carbonate, soluble halides, and water, it was unsuccessful in destroying nitroaromatic compounds, or aliphatic compounds having an amine or a nitrile group attached to them... 

Precipitated or synthetic barium carbonate is the most commercially important of all the barium chemicals except for barite. Barium carbonate is an unusually dense material, that is almost kisoluble ki water and only slightly soluble ki carbonated water. It does dissolve ki dilute hydrochloric, nitric, and acetic acids and is also soluble ki ammonium nitrate and ammonium chloride solutions. 

Barium carbonate prevents formation of scum and efflorescence in brick, tile, masonry cement, terra cotta, and sewer pipe by insolubilizing the soluble sulfates contained in many of the otherwise unsuitable clays. At the same time, it aids other deflocculants by precipitating calcium and magnesium as the carbonates. This reaction is relatively slow and normally requites several days to mature even when very fine powder is used. Consequentiy, often a barium carbonate emulsion in water is prepared with carbonic acid to further increase the solubiUty and speed the reaction. 

In the oil-weU drilling industry, the barite suspension used as drilling mud can be destabilized by the presence of soluble materials such as gypsum. Addition of barium carbonate precipitates the gypsum, inhibits coagulation, and thus permits the mud to retain the desired consistency and dispersion. 

Formolysis and acetolysis are not common methods for cleavage of glycosidic linkages. They do have some unique applications, however. For instance, methylated polysaccharides are not generally soluble in hot water, and consequently, hydrolysis is best preceded by formolysis under these circumstances. For example, 5 mg of methylated polysaccharide is dissolved in 3 mL of 90% formic acid, and the solution is kept for 2 h at 100°. The formic acid is removed by evaporation at 40°. The residue is dissolved in 1 mL of 250 mM sulfuric acid and the solution is heated for 12 h at 100°, cooled, the acid neutralized with barium carbonate, the... 

Barium carbonate decomposes to barium oxide and carbon dioxide when heated at 1,300°C. In the presence of carbon, decomposition occurs at lower temperatures. Barium carbonate dissolves in dilute HCl and HNO3 liberating CO2. Similar reaction occurs in acetic acid. The solid salts, chloride, nitrate and acetate that are water soluble may be obtained by evaporation of the solution. Dissolution in HF, followed by evaporation to dryness, and then heating to red heat, yields barium fluoride. 

Barium hydroxide decomposes to barium oxide when heated to 800°C. Reaction with carbon dioxide gives barium carbonate. Its aqueous solution, being highly alkahne, undergoes neutrahzation reactions with acids. Thus, it forms barium sulfate and barium phosphate with sulfuric and phosphoric acids, respectively. Reaction with hydrogen sulfide produces barium sulfide. Precipitation of many insoluble, or less soluble barium salts, may result from double decomposition reaction when Ba(OH)2 aqueous solution is mixed with many solutions of other metal salts. 

Rubidium is recovered from its ore lepidolite or pollucite. Mineral lepidolite is a lithium mica having a composition KRbLi(OH,F)Al2Si30io. The ore is opened by fusion with gypsum (potassium sulfate) or with a mixture of barium sulfate and barium carbonate. The fused mass is extracted with hot water to leach out water-soluble alums of cesium, rubidium, and potassium. The solution is filtered to remove insoluble residues. Alums of alkali metals are separated from solution by fractional crystallization. Solubility of rubidium alum or rubidium aluminum sulfate dodecahydrate, RbAl(S04)2 I2H2O falls between potassium and cesium alum. 

Precipitate with aq. ammonia. Evaporate the soln. down to about 100 c.c., and filter the ot liquid so as to remove calcium sulphate. The cone. soln. is sat. with ammonium alum and allowed to stand for some time. The mixed crystals of potassium, rubidium, and oeesium alums and of lithium salt are dissolved in 100 c.c. of distilled water and recrystal-lized. The recrystallization is repeated until the crystals show no spectroscopic reaction for potassium or lithium. The yield naturally depends on the variety of lepidolite employed. 100. grms of an average sample gives about 10 grms. of crude crystals and about 3 grms. of the purified caesium and rubidium alums. For the purification of caesium and rubidium salts, see the chlorides. The mother-liquors are treated with an excess of barium carbonate, boiled, and filtered. The filtrate is acidified with hydrochloric acid, and evaporated to dryness. The residue is extracted with absolute alcohol in which lithium chloride is soluble, and the other alkali chlorides are sparingly soluble. 

Solubility in Dilute Hydrochloric Acid. — 5 gm. of barium carbonate should bo completely soluble in 10 cc. of hydrochloric acid diluted with 50 cc. of water. 

White crystals, soluble in 20 parts of cold, and in 3 parts of boiling, water, a trace of barium carbonate almost invariably remaining undissolved. The aqueous solution is alkaline to litmus paper. 

Barium acetate. [CAS 543-80-6], Ba(C2H302)2, white crystals, solubility 76.4 g/100 ml H20 at 26°C. formed by reaction of barium carbonate or hydroxide and acetic acid. 

Isolation of Sulphonic Acids.—Sulphonic acids are usually isolated in the form of their salts in order to get rid of the excess of sulphuric acid used in the reaction. The calcium or barium salts are formed where these are soluble by adding lime or barium carbonate, and the excess sulphuric acid precipitated as CaS04 or BaS04, and removed by filtra-... 

Barium chloride White precipitate of barium carbonate that is soluble in HCI (calcium chloride may be substituted for barium chloride)... 

The high-temperature reduction of barium sulfate with coke yields the water-soluble barium sulfide (BaS), which is subsequently leached out. Treatment of barium sulfide with the relevant chemical yields the desired barium salt. Purification of the product is complicated by the impurities introduced in the coke. Pure barium carbonate and barium sulfate are made by precipitation from solutions of water-soluble barium salts. 

As pH levels increase above 9.3 and in the presence of carbonate, barium carbonate becomes the dominant species (Bodek et al. 1988 Singer 1974). Barium carbonate also exhibits fast precipitation kinetics and very low solubility and in alkaline environments limits the soluble barium concentration (Faust and Aly 1981 Hem 1959 Rai et al. 1984 Singer 1974). Barium forms salts of low solubility with arsenate, chromate, fluoride, oxalate, and phosphate ions (Bodek et al. 1988 EPA 1983a Kunesh 1978). The chloride, hydroxide, and nitrate of barium are water-soluble (Bodek et al. 1988 EPA 1983a Kirkpatrick 1978) and are frequently detected in aqueous environments (Rai et al. 

Barium Cobalti-cyanide, Ba3[Co(CN)s]2. Aq., is a convenient starting-point for the preparation of other metallic cobalti-cyanides by double decomposition. It may be prepared by adding barium carbonate to a solution of the free acid but a better method consists in exposing to aerial oxidation a mixture of cobalt sulphate and the cyanides of hydrogen and barium. The salt crystallises out in colourless prisms, winch are readily soluble in water, but not in alcohol. They contain some 20 or 22 molecules of water.4... 

Solubility of sparingly soluble salts of weak acids in strong mineral acids The solubility product principle enables us to give a simple explanation of this phenomenon, which is of relatively frequent occurrence in quantitative analysis. Typical examples are the solubilities of calcium oxalate or barium carbonate in hydrochloric acid. When dilute hydrochloric acid is added to a suspension of calcium oxalate, the following equilibria will occur simultaneously ... 

Ammonia solution no precipitate of barium hydroxide because of its relatively high solubility. If the alkaline solution is exposed to the atmosphere, some carbon dioxide is absorbed and a turbidity, due to barium carbonate, is produced. 

If barium sulphate is boiled with a concentrated solution of sodium carbonate, partial transformation into the less soluble barium carbonate occurs in accordance with the equation ... 

Strontium carbonate is somewhat less soluble than barium carbonate otherwise its characteristics (slight solubility in ammonium salts, decomposition with acids) are similar to those of the latter. 

It is relatively simple to determine the extent to which a sulfonation reaction has proceeded. The reaction mixture is neutralized with barium carbonate and treated with enough soda to form the sodium siplt. The number of sulfo groups present can be calculated from the amount of soda used up. One sulfo group requires 53 grams of NaaCOs. Calcium carbonate cannot be used for this purpose since calcium sulfate is soluble in solutions of naphthalenesulfonic acids. 

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