Barium Acetate Carbonate

Synthetic chemical approaches to the preparation of carbon-14 labeled materials iavolve a number of basic building blocks prepared from barium [ CJ-carbonate (2). These are carbon [ C]-dioxide [ CJ-acetjlene [U— C]-ben2ene, where U = uniformly labeled [1- and 2- C]-sodium acetate, [ C]-methyl iodide, [ C]-methanol, sodium [ C]-cyanide, and [ CJ-urea. Many compHcated radiotracers are synthesized from these materials. Some examples are [l- C]-8,ll,14-eicosatrienoic acid [3435-80-1] inoxn. [ CJ-carbon dioxide, [ting-U— C]-phenyhsothiocyanate [77590-93-3] ftom [ " CJ-acetjlene, [7- " C]-norepinephrine [18155-53-8] from [l- " C]-acetic acid, [4- " C]-cholesterol [1976-77-8] from [ " CJ-methyl iodide, [l- " C]-glucose [4005-41-8] from sodium [ " C]-cyanide, and [2- " C]-uracil [626-07-3] [27017-27-2] from [ " C]-urea. All syntheses of the basic radioactive building blocks have been described (4). 

Barium acetate [543-80-6] Ba(C2H202)2, crystallines from an aqueous solution of acetic acid and barium carbonate or barium hydroxide. The level of hydration depends on crystallization temperature. At <24.7°C the trihydrate, density 2.02 g/mL is formed from 24.7 to 41 °C barium acetate monohydrate [5908-64-5] density 2.19 g/mL precipitates and above 41 °C the anhydrous salt, density 2.47 g/mL results. The monohydrate becomes anhydrous at 110°C. At 20°C, 76 g of the monohydrate dissolves in 100 g of water. Barium acetate is used in printing fabrics, lubricating grease, and as a catalyst for organic reactions. 

Barium acetate is made by the reaction of barium carbonate with acetic acid ... 

Barium acetate converts to barium carbonate when heated in air at elevated temperatures. Reaction with sulfuric acid gives harium sulfate with hydrochloric acid and nitric acid, the chloride and nitrate salts are obtained after evaporation of the solutions. It undergoes double decomposition reactions with salts of several metals. For example, it forms ferrous acetate when treated with ferrous sulfate solution and mercurous acetate when mixed with mercurous nitrate solution acidified with nitric acid. It reacts with oxahc acid forming barium oxalate. 

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. 

Barium is a silvery-white metal that occurs in nature in many different forms called compounds. These compounds are solids and they do not burn well. Two forms of barium, barium sulfate and barium carbonate, are often found in nature as underground ore deposits. Barium is sometimes found naturally in drinking water and food. Because certain forms of barium (barium sulfate and barium carbonate) do not mix well with water, the amount of barium usually found in drinking water is of a small quantity. Other barium compounds, such as barium chloride, barium nitrate, and barium hydroxide, are manufactured from barium sulfate. Barium compounds such as barium acetate, barium carbonate, barium chloride, barium hydroxide, barium nitrate, and barium sulfide dissolve more easily in water than barium sulfate and barium carbonate. 

The health effects of the different barium compounds depend on how well the specific barium compound dissolves in water. For example, barium sulfate does not dissolve well in water and has few adverse health effects. Doctors sometimes give barium sulfate orally or by placing it directly in the rectum of patients for purposes of making x-rays of the stomach or intestines. The use of this particular barium compound in this type of medical test is not harmful to people. Barium compounds such as barium acetate, barium carbonate, barium chloride, barium hydroxide, barium nitrate, and barium sulfide that dissolve in water can cause adverse health effects. Most of what we know comes from studies in which a small number of individuals were exposed to fairly large amounts of barium for short periods. Eating or drinking very large amounts of barium compounds that dissolve in water may cause paralysis or death in a few... 

Synonyms Elemental barium barium ion barium, alloys, non-pyrophoric barium, alloys, pyrophoric barium, metal, non-pyrophoric0 Acetic acid, barium salt barium diacetate barium acetate monohydrated,e Carbonic acid, barium salt witheritee,f... 

Barium poisonings are uncommon and usually result from accidental contamination of food sources, suicidal ingestion, or occupational inhalation exposure. The water-soluble barium salts (acetate, carbonate, chloride, fluoride, hydroxide, nitrate, and sulfide) are highly toxic, whereas the insoluble salt, barium sulfate, is nontoxic because it is not absorbed. Soluble barium salts are found in depilatories, fireworks, ceramic glazes, and rodenticides and are used in the manufacture of glass and in dyeing textiles. Barium sulfide and polysulfide may also produce hydrogen sulfide toxicity (see p 224). 

Acetates of lead, copper and mercury as simple aqueous solutions, in 1 N acetic acid and as amine complexes, are applied to similar slides. Barium acetate, in neutral and acidic solutions for sulfate and other oxy-thio ions, and other reagents which dissolve sulfur, such as carbon disulfide, may be tried. These require an understanding of their reactions with all substances which may be present or be formed by reactions of such chemicals as are present, to be of diagnostic use. The reader should consultthe chemical literature. 

The sensitivity increase for some selective carbohydrates that is caused by the addition of Ba(II) is shown in Figure 3.229. While retention of the first three components remains practically the same when adding barium acetate, a slight retention decrease is observed for fructose and sucrose. At first view, this seems surprising one might suppose that the complete removal of carbonate would lead to a retention increase. However, since in this case Ba(II) has been added as acetate salt, and acetate is a stronger eluent than hydroxide, even traces of acetate in the mobile phase will result in a retention decrease. The sensitivity increase is attributed by Cataldi et al [219] to the inhibition of the gold oxide formation by alkaline-earth metals in the order Ca(ll) > Sr(II) > Ba(II) that, in turn, results in an increase of the electrocatalytic activity of the electrode. 

Figure 2. CP/MAR spectrum (16) at 22.6 MHz of barium acetate monohydrate, showing at the left the carboxyl carbon resonances and at the right the methyl resonances. The chemical shifts are given in ppm from the signal of liquid Me4Si.

Since Procedures B, C and D require fractional distillation to purify the product, as well as additional chemical manipulations. Procedure A has become the method of choice, even though half of the radioactivity originally contained in Cl of the acetate is diverted back to lithium or barium [ " C]carbonate. The use of barium [ " C]acetate is favored, since the... 

Nantokite, see Copper(I) chloride Natron, see Sodium carbonate Naumannite, see Silver selenide Neutral verdigris, see Copper(H) acetate Nitre (niter), see Potassium nitrate Nitric oxide, see Nitrogen(II) oxide Nitrobarite, see Barium nitrate Nitromagnesite, see Magnesium nitrate 6-water Nitroprusside, see Sodium pentacyanonitrosylfer-rate(II) 2-water... 

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. 

The more soluble forms of barium such as the carbonate, chloride, acetate, sulfide, oxide, and nitrate, tend to be more acutely toxic (50). Mean lethal doses for ingested barium chloride were 300—500 mg/kg in rats and 7—29 mg/kg in mice (47). 

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