Barium Acetate Hydrate

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. 

Metal carboxvlates M(OOCR)x Ba(OOCCH3)2, Barium acetate tri-hydrate... 

At temperatures above 0 , barium acetate can form two stable hydrates, a trihydrate and a monohydrate. The solubility of the trihydrate increases very rapidly with rise of temperature, and has been determined up to 26 1 . At temperatures above 247 , however, the trihydrate is metastable with respect to the monohydrate for at this temperature the solubility curve of the latter hydrate cuts that of the former. This is, therefore, the transition temperature for the trihydrate and monohydrate. The solubility curve of the monohydrate succeeds that of the trihydrate, and exhibits a conspicuous point of minimum solubility at about 30 . Below 247 the monohydrate is the less stable hydrate, but its solubility has been determined to a temperature of 22 . At 41 the solubility curve of the monohydrate... 

The diagram of solubilities of barium acetate not only illustrates the way in which the solubility curves of the different stable hydrates of a salt succeed one another, but it has also an interest and importance from another point of view. In Fig. 77 there is also shown a faintly drawn curve which is continuous throughout its whole course This curve represents the solubility of barium acetate as determined by Krasnicki. Since, however, three different solid phases can exist under the conditions of experiment, it is evident, from what has... 

Drum dryers potatoes, cereals, buttermilk, skim milk, dextrins, yeasts, instant oat meal, polyacylamides, sodium benzoate, propionates, acetates, phosphates, chelates, aluminum oxide, m-disulfuric acid, barium sulfate, calcium acetate-arsenate-carbonate-hydrate-phosphate, caustic, ferrous sulfate, glue, lead arsenate, sodium benzene sulfonate, and sodium chloride... 

AnalaR glacial acetic acid and tetra-sodium pyrophosphate decahydrate were from BDH. Chemicals/reagents from Aldrich acetonitrile, anhydrous 1,4-dioxane (dioxan), barium 2-cyanoethylphosphate hydrate, 2,4,6-collidine (99%), anhydrous DMF, phosphoryl chloride (phosphorus oxychloride) (99 and 99.999%), thiophosphoryl chloride (98%), salicyl chlorophosphite (2-chloro-4//-l,3,2-benzodioxaphosphorin-4-one), tri-n-butylamine (99+%), triethylamine (99%), tri-n-octylamine (99+%), trimethylphosphate (99+%), 3 A molecular sieves. 

Barium Diuranate, BaUjO, is obtained by heating barium uranyl acetate, or by heating together the green oxide and barium chlorate. It is obtained in a hydrated condition when ammonia is added to mixed solutions of barium chloride and uranyl nitrate, or when excess of baryta water is added to uranyl nitrate solution. It is a deep yellow crystalline powder. 

Calcium, strontium and barium form some poorly characterised /9-diketone complexes and rather unstable ammines tendency to covalence, even as indicated by hydration of the ions, has decreased with cation size. The determination of magnesium and calcium with sodium ethylenediamine tetra-acetate, e.d.t.a., probably involves the formation of a chelate complex whose stability is enhanced by the presence of 5-membered rings. 

This, the best known of the glycols, is prepared by the action of dry silver acetate upon ethylene bromide. The ether so obtained is purified by redistiUation, and decomposed by heating for some time with barium hydrate. 

BARIUM HYDRATE (17194-00-2) A strong base. Reacts with phosphorus, releasing phosphine gas. Violent exothermic reaction with maleic anhydride. Reacts violently with acids, chlorinated rubber (when heated), 1-nitropropane, zirconium powder or dust. Incompatible with organic anhydrides, acrylates, alcohols, aldehydes, alkylene oxides, substituted allyls, cresols, caprolactam solution, epichlorohydrin, ethylene dichloride, glycols, isocyanates, ketones, nitrates, nitromethane, phenols, vinyl acetate. Attacks chemically active metals (e.g. aluminum, magnesium, zinc). 

Potassium nitridotrisulfate crystallizes as the 2-hydrate in long brilliant needles. It is very slightly soluble in water and not appreciably soluble in liquid ammonia. In aqueous solutions it gives no precipitate with manganese-(II), mercury(II), silver, cadmium, cobalt(II), copper(II), or iron (II) ion but yields a white precipitate with lead acetate. Potassium nitridotrisulfate yields a precipitate with barium ion only in basic solution. 

A review in Russian on the synthesis of carbohydrates from formaldehyde has appeared. An investigation of the formose reaction by g.c.-n.m.r. has shown that intermediate glycoaldehyde, glyceraldehyde, and dihydroxyacetone are present as mixtures of monomers, e.g. hydroxy carbonyl compounds, epoxides and hydrates, and dimers such as half and full acetals. Further study of the barium chloride-catalysed formose reaction at pH 12 has shown that the main product forming 33% of the total sugars is the branched pentulose (1). The sugar yield reached a constant value at 70% completion of the reaction, i.e., within... 

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