Barium oxide electrolytes

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. 

Chemists did not discover the mineral witherite (BaCO ) until the eighteenth century. Carl Wilhelm Scheele (1742—1786) discovered barium oxide in 1774, but he did not isolate or identify the element barium. It was not until 1808 that Sir Humphry Davy used molten barium compounds (baryta) as an electrolyte to separate, by electrolysis, the barium cations, which were deposited at the negative cathode as metallic barium. Therefore, Davy received the credit for bariums discovery. 

V.M. Ivenko, Determination of Solubility of Barium Oxide in BaC12-KCl-NaCl Eutectic by Potentiometric Method (Abstract of 10th All-Union Conference on Physics, Chemistry and Electrochemistry of Ionic Melts and Solid Electrolytes, Ekaterinbourg, Vol. 1. 1992) p. 74. 

The principle of detection is as follows. On the surface of the Ba-Ce-Y-O electrolyte, barium oxide exists as a result of the decomposition of the protonic conductor. Barium oxide reacts with water vapor in a humid atmosphere and forms barium hydroxide on the surface. This hydroxide absorbs carbon dioxide to form a carbonate, and as a result, the conductivity decreases. 

These can be prepared by electrolytic oxidation of chlorates(V) or by neutralisation of the acid with metals. Many chlorates(VII) are very soluble in water and indeed barium and magnesium chlorates-(VII) form hydrates of such low vapour pressure that they can be used as desiccants. The chlorate(VII) ion shows the least tendency of any negative ion to behave as a ligand, i.e. to form complexes with cations, and hence solutions of chlorates (VII) are used when it is desired to avoid complex formation in 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 ... 

Sodinm perchlorate is produced industrially by electrolytic oxidation of NaC103. Perchloric acid is prepared by reacting a sodium or barium salt with concentrated HCl, filtering off the chloride, and concentrating the filtrate by distillation. The anhydrous acid can be obtained by low-pressure distillation in an all-glass apparatus in the presence of sulfuric acid, which combines with the rest of the water. 

An alternative electrolyte material, lanthanum-doped barium indium oxide, (Ba,La)In205+3, has been proposed. This new material has been shown to have an ionic transference number of 1.0 with an oxygen ion conductivity better than that of YSZ. 

The first recorded synthesis of silver(I) sulfamate was that by Berglund in 1876 he used the very slow reaction between silver(I) sulfate and barium(II) sulfamate. Later methods have employed the reaction between sulfamic acid and silver(I) oxide or silver(I) carbonate an electrolytic process has also been described. ... 

The temperature required to produce a suitable weighing form varies from precipitate to precipitate. Figure 12-6 shows mass loss as a function of temperature for several common analytical precipitates. These data were obtained with an automatic thermobalance, an instrument that records the mass of a substance continuously as its temperature is increased at a constant rate (Figure 12-7). Heating three of the precipitates—silver chloride, barium sulfate, and aluminum oxide—simply causes removal of water and perhaps volatile electrolytes. Note the vastly different temperatures required to produce an anhydrous precipitate of constant mass. Moisture is completely removed from silver chloride at temperatures higher than 110°C, but dehydration of aluminum oxide is not complete until a temperature greater than 1000°C is achieved. Aluminum oxide formed homogeneously with urea can be completely dehydrated at about 650°C. 

Barium peroxide and electrolytic methods have now been superseded by a process based on the oxidation of 2-ethyl anthraquinol by atmospheric oxygen ... 

Since, all strong electrolytes are completely dissociated, hence only the ions actually taking part or resulting from the reaction need appear in the equation. Substances which are only slightly ionised such as water or which are sparingly soluble and thus yield only as small concentration of ions e.g. silver chloride and barium sulphate are in general written as molecular formulae because they are present mainly in the undissociated state. Equation 4.6.17.4 is an example to prove that oxidation and reductions occurs simultaneously. Ion-electron balance therefore can be performed based on the step mentioned below ... 

O 42.11%. Prepd by electrolytic oxidation of iodic add or from barium periodate and nitric acid Willard,... 

Consequently, we are in the startup phase of our program. Our first task was to identify candidate perovskite oxide materials with high protonic conductivities. We have identified ytterbium doped strontium cerate and yttrium doped strontium zirconate materials as possible electrolyte materials. Barium cerate perovskites exhibit higher protonic conductivity, but the reactivity with carbon dioxide would require pretreatment of the steam. 

Aminobutyric acid has been prepared by the electrolytic reduction of succinimide to pyrrolidone and hydrolysis of the latter by means of barium hydroxide,1 by the oxidation of piperylurethan with fuming nitric acid and the treatment of the resulting product with concentrated hydrochloric acid in sealed tubes at 100°,3 and by the hydrolysis of the condensation product from 2V-(/3-bromoethyl)-phthalimide and sodiomalonic ester.4 The present method is a slight modification of that of Gabriel.2... 

Periodic acid and periodates are the most important, commercially available compounds of iodine(VII). Periodates were first prepared in 1833 by oxidation of NalOs with chlorine in alkaline solutions [727]. The industrial preparation of periodates is based on electrolytic oxidation of iodates. Aqueous solutions of periodic acid are best obtained by treating barium paraperiodate with concentrated nitric acid. In solution it exists as a fairly weak orthoperiodic acid, HsIOe, which can be dehydrated to HIO4 by heating to 100 °C in vacuum [643]. Structural investigations indicate an octahedral configuration about iodine in most periodates [643,728]. 

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