Peroxide, barium hydrogen

Mitkevich, Preparation of Barium Peroxide From Hydrogen Peroxide and Barium Hydroxide , KhimPromUkr (6), 17-19 (1968) CA... 

Additional Exercise Barium peroxide from hydrogen peroxide. 

Many other oxidising agents can effect the same change in a thiosulphate, for example permanganates,3 chlorates,4 selenium dioxide,5 barium peroxide,8 hydrogen peroxide 7 and lead dioxide, in the presence of sufficient sulphuric acid to neutralise the alkali as it is produced ... 

Pure barium peroxide hydrate Ba02-8H20 is precipitated when barium hydroxide is added to a hydrogen peroxide solution. Hydrogen peroxide is not a stable substance its solution decomposes slowly in any event into oxygen and water. This decomposition is greatly hastened by suspended solid matter and by hydroxyl ions in the following preparation one should work to minimize the amount of this decomposition. 

BaO p 2HNO3—> Ba (NO3) 2 P H20 and barium peroxide yields hydrogen peroxide ... 

In (b) the barium peroxide acts as we should expect with hydrochloric acid, yielding hydrogen peroxide. Since hydrogen peroxide is unstable, breaking down into water and oxygen, we should expect that it would react, at least to some extent, with the excess of hydrochloric acid and set free chlorine. 

Instead of using free hydrogen peroxide, barium peroxide may be used, lumps of u mixture of barium peroxide, gypsum, and manganese dioxide being introduced into the Kipp, the liquid reagent consisting of hydrochloric acid.2... 

The barium carbonate can be separated by filtration and when heated loses carbon dioxide, leaving barium oxide which is available for reconversion into barium peroxide. The hydrogen peroxide will be in the filtrate which can be concentrated by evaporation under reduced pressure. 

Hydrogen Peroxide (H2O2). Hydrogen peroxide can be prepared by the reaction of barium peroxide and sulfuric acid (see equation 13). As barium sulfate precipitates out, hydrogen peroxide is easily separated. 

Aluminum acetate Aluminum caprylate Aluminum distearate Aluminum myristates/palmitates Aluminum stearate Aluminum tristearate N-2-Aminoethyl-3-aminopropyl trimethoxysilane Aminoethylethanolamine Aminomethyl propanol Aminopropyltriethoxysilane Aminopropyltrimethoxysilane Ammonium benzoate Ammonium borate Ammonium citrate dibasic Ammonium laureth sulfate Ammonium laureth-5 sulfate Ammonium laureth-7 sulfate Ammonium laureth-12 sulfate Ammonium laureth-30 sulfate Ammonium lauryl sulfate Ammonium maleic anhydride/diisobutylene copolymer Ammonium oleate Ammonium persulfate Ammonium polyacrylate Ammonium potassium hydrogen phosphate Ammonium stearate Ammonium sulfamate Ammonium thiocyanate Ammonium thiosulfate Amyl acetate Antimony trioxide Asbestos Asphalt Azelaic acid 2,2 -Azobisisobutyronitrile Barium acetate Barium peroxide Barium sulfatej Bentonite Benzalkonium chloride Benzene Benzethonium chloride Benzothiazyl disulfide Benzoyl peroxide Benzyl alcohol Benzyl benzoate 1,3-Bis (2-benzothiazolylmercaptomethyl) urea 1,2-Bis (3,5-di-t-butyl-4-hydroxyhydrocinnamoyl) hydrazine 4,4 -Bis (a,a-dimethylbenzyl) diphenylamine Bisphenol A Bis (trichloromethyl) sulfone Boric acid 2-Bromo-2-nitropropane-1,3-diol 1,4-Butanediol Butoxydiglycol Butoxyethanol Butoxyethanol acetate n-Butyl acetate Butyl acetyl ricinoleate Butyl alcohol Butyl benzoate Butyl benzyl phthalate Butyidecyl phthalate Butylene glycol t-Butyl hydroperoxide... 

The best-known peroxide is hydrogen peroxide (H2O2). It is a colorless, syrupy liquid (m.p. -0.9°C), prepared in the laboratory by the action of cold dilute sulfuric acid on barium peroxide octahydrate ... 

One of the ways that aqueous emulsion polymerization processes can be classified is on the basis of the types of the initiators also referred to as catalysts. In one type of polymerization system, an organic peroxide, preferably water-soluble, is used. The organic peroxides include cumene hydroperoxide, diisopropyl benzene hydroperoxide, triisopropyl benzene hydroperoxide, and tertiary butyl hydroperoxide. A second type of emulsion polymerization employs an inorganic peroxide. Suitable compounds include perborates, persulfates, perphosphates, percarbonates, barium peroxide, zinc peroxide, and hydrogen peroxide. Specific examples of inorganic peroxides are ammonium persulfate and sodium perphosphate. 

In the laboratory, hydrogen peroxide can be prepared in dilute aqueous solution by adding barium peroxide to ice-cold dilute sulphuric acid ... 

Chlorine, bromine and iodine form halic(V) acids but only iodic(V) acid, HIO3, can be isolated. Solutions of the chloric) V) and bromic) V) acids can be prepared by the addition of dilute sulphuric acid to barium chlorate(V) and bromate(V) respectively, and then filtering (cf. the preparation of hydrogen peroxide). These two acids can also be prepared by decomposing the corresponding halic(I) acids, but in this case the halide ion is also present in the solution. 

Inorganic Methods. Before the development of electrolytic processes, hydrogen peroxide was manufactured solely from metal peroxides. Eady methods based on barium peroxide, obtained by air-roasting barium oxide, used dilute sulfuric or phosphoric acid to form hydrogen peroxide in 3—8% concentration and the corresponding insoluble barium salt. Mote recent patents propose acidification with carbon dioxide and calcination of the by-product barium carbonate to the oxide for recycle. 

In spite of widespread usage of these compounds, the stmctures of only the calcium, barium, and strontium compounds are reasonably weU-estabhshed. The materials are generally made by trituratiag the oxides, or hydroxides, with aqueous hydrogen peroxide and dryiag the soHd products. The commercial products are typically mixtures of the peroxides with varyiag amounts of hydroxides, oxides, carbonates, hydrates, and peroxohydrates. 

Analytical Methods. The official NIOSH recommended method for determining sulfur dioxide in air consists of drawing a known prefiltered volume of air through a bubbler containing hydrogen peroxide, thus oxidising the sulfur dioxide to sulfuric acid. Isopropyl alcohol is then added to the contents in the bubbler and the pH of the sample is adjusted with dilute perchloric acid. The resultant solution is then titrated for sulfate with 0.005 M. barium perchlorate, and Thorin is used as the indicator. 

Barium is a member of the aLkaline-earth group of elements in Group 2 (IIA) of the period table. Calcium [7440-70-2], Ca, strontium [7440-24-6], Sr, and barium form a closely aUied series in which the chemical and physical properties of the elements and thek compounds vary systematically with increa sing size, the ionic and electropositive nature being greatest for barium (see Calcium AND CALCIUM ALLOYS Calcium compounds Strontium and STRONTIUM compounds). As size increases, hydration tendencies of the crystalline salts increase solubiUties of sulfates, nitrates, chlorides, etc, decrease (except duorides) solubiUties of haUdes in ethanol decrease thermal stabiUties of carbonates, nitrates, and peroxides increase and the rates of reaction of the metals with hydrogen increase. 

Pilocarpine dissolves in dilute soda solution, and the rotation is thereby reduced, due to the formation of the sodium salt of pilocarpic acid, CiiHigOgNa, of which pilocarpine is the lactone. Amorphous barium and copper salts have been prepared. Pilocarpine in dilute sulphuric acid gives with hydrogen peroxide, followed by potassium dichromate, a bluish-violet colour soluble in benzene. For the identification of the alkaloid Wagenaar recommends precipitation with gold chloride solution. 

Hydrogen peroxide was first made in 1818 by J. L. Thenard who acidified barium peroxide (p. 121) and then removed excess H2O by evaporation under reduced pressure. Later the compound was prepared by hydrolysis of peroxodisulfates obtained by electrolytic oxidation of acidified sulfate solutions at high current densities ... 

Determination of sulphite by oxidation to sulphate and precipitation as barium sulphate Discussion. Sulphites may be readily converted into sulphates by boiling with excess of bromine water, sodium hypochlorite, sodium hypobromite, or ammoniacal hydrogen peroxide (equal volumes of 20-volume hydrogen peroxide and 1 1 ammonia solution). The excess of the reagent is decomposed by boiling, the solution acidified with hydrochloric acid, precipitated with barium chloride solution, and the barium sulphate collected and weighed in the usual manner (Section 11.72). 

Conversion of thiosulphate to sulphate and determination as barium sulphate Discussion. Thiosulphates are oxidised to sulphates by methods similar to those described for sulphites (Section 11.74), e.g. by heating on a water bath with an ammoniacal solution of hydrogen peroxide, followed by boiling to expel the excess of the reagent. The sulphate is then determined as barium sulphate, BaS04. 

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