Water with barium oxide

B. C. Dutt and S. N. Sen found that when nitric oxide is passed into a suspension of barium dioxide in water, barium nitrite, not nitrate, is formed. P. Sabatier and J. B. Senderens observed no change when nitric oxide is passed over Cuprous Oxide at 500°. H. A. Auden and G. J. Fowler observed that dry nitric oxide and Silver oxide, at ordinary temp., form silver and silver nitrate P. Sabatier and J. B. Senderens also obtained silver and silver nitrite by passing nitric oxide into water with silver oxide in suspension. C. F. Schonbein found gold oxide is reduced by moist nitric oxide, forming nitrous acid. P. Sabatier and J. B. Senderens found that titanium sesquioxide forms white titanic oxide when heated in an atm. of nitric oxide and that stannous oxide below 500° burns in an atm. of nitric oxide, forming stannic oxide. If nitric oxide be passed into water with lead dioxide in suspension, the water is coloured, and in about 3 hrs., lead nitrite and nitrate are formed, and later, rhombic crystals of a basic nitrite. B. C. Dutt and S. N. Sen said that the nitrate is formed by the action of the dioxide on the nitrite. Lead dioxide is reduced to lead oxide by nitric oxide at 315°, and H. A. Auden and G. J. Fowler found that the reaction begins at 15°, when a basic lead nitrite is... 

It was shown in [18] that practically monophase fine barium hexaaluminate can be obtained by mechanical activation of a mixture of barium oxide with Y-AI2O3, which exhibits acid properties to a larger extent than a-Al203, and by consequent thermal treatments at increased temperature. The product then is grinded in the presence of water. The synthesis was shown to proceed almost completely after activation for 5 min in the AGO-2 planetary mill and thermal treatment at 1300°C for 1 h. Mechanical activation of the mixture of aluminium hydroxide with barium oxide, followed by thermal treatment at 900°C, results in the formation of the final product and a-Al203 as an admixture which remains even at 1300°C. Mechanochemical synthesis helped also to synthesize barinm hexaaluminate in which a part of aluminium cations is replaced with manganese, iron, cobalt cations. Such compounds are nsed as active ceramics in catalysis [17]. 

The diaquo compound is placed in an Abderhalden dr3dng apparatus with barium oxide as the desiccant. After 14 hours at 57° (or 6 hours at 67°) and pressure of 30 mm. (a water... 

The distillate which contains the allyl alcohol is redistilled slowly from a flask fitted in the usual way with a thermometer. When the temperature reaches 103°, test from time to time about 2 cc. of the distillate for allyl alcohol by saturating it with solid anhydrous potassium carbonate. When an oil no longer separates, stop the distillation. Combine the products and saturate the solution with solid anhydrous potassium carbonate. Separate the layer of oil, and redistil. The allyl alcohol obtained in this way boils at 87°-97° and contains water. Weigh the product obtained and note its odor. The alcohol can be used for the experiments described below. In order to obtain the alcohol in dry condition, it should be placed in a flask and treated with barium oxide until the pieces project from the surface of the... 

Sodium and potassium hydroxides. The use of these efficient reagents is generally confined to the drying of amines (soda lime, barium oxide and quicklime may also be employed) potassium hydroxide is somewhat superior to the sodium compound. Much of the water may be first removed by shaking with a concentrated solution of the alkali hydroxide. They react with many organic compounds (e.g., acids, phenols, esters and amides) in the presence of water, and are also soluble in certain organic liquids so that their use as desiccants is very limited... 

Ethyl chloride can be dehydrochlorinated to ethylene using alcohoHc potash. Condensation of alcohol with ethyl chloride in this reaction also produces some diethyl ether. Heating to 625°C and subsequent contact with calcium oxide and water at 400—450°C gives ethyl alcohol as the chief product of decomposition. Ethyl chloride yields butane, ethylene, water, and a soHd of unknown composition when heated with metallic magnesium for about six hours in a sealed tube. Ethyl chloride forms regular crystals of a hydrate with water at 0°C (5). Dry ethyl chloride can be used in contact with most common metals in the absence of air up to 200°C. Its oxidation and hydrolysis are slow at ordinary temperatures. Ethyl chloride yields ethyl alcohol, acetaldehyde, and some ethylene in the presence of steam with various catalysts, eg, titanium dioxide and barium chloride. 

For best results the commercial triethylamine (Matheson, b.p. 89-90°) should be purified to remove primary and secondary amines and water, either by distillation from acetic anhydride and then from barium oxide, or by reaction with phenyliso-cyanate.5 2 3 4... 

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). 

Recently, we have shown that the combination of barium tetratitanate, BaTi40g and sodium hexatitanate, NagTigOis, with ruthenium oxides leads to active photocatalysts for water decomposition[1,2]. The unique feature of these photocatalysts is that no reduction of the titanates is required to be activated this is intrinsically different from conventional photocatalysts using TIO2 which are often heat-treated in a reducing atmosphere. Such different photocatalytic characteristics suggest that efficiency for the separation of photoexcited charges (a pair of electrons and holes) which is the most important step in photocatalysis is... 

As with calcium and strontium oxides, barium oxide reacts very exothermically with water, forming hydrogen.The heat which is released is such that it can, like... 

In dim red light, the weighed hydrazide contained in one of the 500 ml flasks (ca. 67 g 95% of theory) is washed into a 1000 ml beaker with 263 ml IN hydrochloric acid. 239 ml distilled water, 239 ml ethanol (95%), and 37 ml 2,4-pentanedione are added, and the well-mixed solution left to stand in the dark at room temperature until the reaction is complete, i.e., about 30 minutes. The reaction mixture is neutralized with the addition of 263 ml 1 N sodium hydroxide, and the beaker covered with parafilm and refrigerated to ensure complete precipitation. The pyrazole is filtered at the pump, the mother liquor being returned to the beaker and used to wash out the last few crystals, washed with cold water, and sucked dry under a stream of dry nitrogen. The product is dried in vacuo over barium oxide or phosphorus pentoxide for at least twelve hours before proceeding to the next step, wherein anhydrous conditions will increase yield. Hofmann calls for drying the pyrazole in vacuo at 60°, which indicated the product to be fairly stable. So all the hydrazide is converted prior to aminization. 

Barium hydroxide is made by dissolving barium oxide in hot water. The octahydrate, Ba(0H)2 8H20, crystaUizes upon cooling. It also is prepared by precipitation with caustic soda from an aqueous solution of barium sulfide ... 

Barium oxide reacts with water forming hydroxide, and with carhon dioxide it forms harium carbonate. Both reactions are rapid and exothermic ... 

Barium oxide is toxic by subcutaneous route. Because of its affinity for moisture, the compound is corrosive to skin. Contact with water or CO2 evolves much heat. Therefore, any use of CO2 to extinguish a BaO fire may cause further incandescence. Accumulation of barium oxide or peroxide dust... 

Barium peroxide decomposes to barium oxide and oxygen when heated to 700°C. At lower temperatures, decomposition occurs slowly. It also decomposes slowly in contact with water, forming barium hydroxide. It reacts with dilute acids to form hydrogen peroxide ... 

In one of J. S. Stas processes, the iodine was dissolved in a soln. of potassium iodide. The soln. was diluted with water until a precipitate began to form, and then three-fourths of the amount of water required to precipitate all the iodine were added. The separated iodine was washed free from potassium iodide by decantation, the crystals, after draining, were dried over calcium nitrate in vacuo, and then distilled twice from barium oxide. In another process, J. S. Stas purified the iodine by first treating the iodide with ammonia which converts about 95 per cent, of it into the explosive nitrogen iodide. The washed nitrogen iodide decomposes quietly when warmed with an excess of water. J. S. Stas thus describes the procedure ... 

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