Sodium peroxide, properties

On addition of 30 per cent, peroxide to sodium hydroxide or ethoxidc a precipitate of sodium perhydroxide is obtained to which the formula 4 2NaH02. H202 is given. This possesses marked basic properties, and on saturation with carbon dioxide yields the acid percarbonate,5 NaHC04. The same compound is formed when hydrogen peroxide is added to sodyl hydroxide,4 NaO. OH. This latter substance was first prepared by Tafel6 by the action of sodium peroxide upon well-cooled absolute alcohol. 

The decrease in the basicity of ionic melts owing to both the strengthening of the acidic properties of constituent cations of the melt [300] and the decreasing equilibrium concentration of oxygen ions [101, 220] reduces peroxide-ion stability the O2- ion becomes the main form of existence of oxygen ions under these conditions. The addition of sodium peroxide to molten LiNC>3 has been found [301] to result in a yield of 0.5 mol of... 

Of the two metals it is only sodium that is used to any extent in its metallic state. It is required in manufacturing sodium peroxide, cyanide and sodamide. An alloy with potassium is liquid at the ordinary temperature and is used in thermometry. Sodium is a useful reagent in organic chemistry as in the manufacture of synthetic rubber it was at one time used in manufactujing metallic aluminium and magnesium by replacement in the chlorides but these metals are now obtained electrolytically. An alloy with lead finds application in the manufacture of ethyl , that is, lead tetraethyl, for anti-knock motor spirit. Its property of emitting electrons when exposed to light enables it to be used in photoelectric cells. 

CHEMICAL PROPERTIES nonflammable gas forms carbonic acid in water absorbed by alkaline solutions with the formation of carbonates gas is affected by heat when the temperature reaches about 2000°C reacts vigorously with cesium oxide, lithium, potassium, sodium, titanium, aluminum and sodium peroxide, magnesium and sodium peroxide, and diethyl magnesium FP (NA) LFL/UFL (NA) AT (NA) HF (-393.5 kJ/mol gas at 25°C) T (31.3 C, 88.3°F) P (72.9 atm, 55,404 mmHg). 

Sodium Peroxide (Na202) - Properties similar to potassium hydroxide above. 

Industrial uses of sodium are based primarily on its strong reducing properties. A large part of the annual sodium production is needed to produce the gasoline antiknock agents tetramethyllead and tetraethyllead. It is also employed for the reduction of titanium and zirconium chlorides to produce titanium and zirconium metals. The remaining part of sodium is used to produce compounds such as sodium hydride, sodium alkoxides, and sodium peroxide. Sodium is also used, especially in alloys with potassium, as a heat exchange liquid in fast-breeder nuclear reactors. 

Uses Solvent and detergent scour for removal of oil and grease stable over broad pH range can be used in sodium peroxide and sodium hypochlorite bleach baths Properties Amber cl. liq., mild alcoholic odor sp.gr. 0.93 dens. 7.75 Ib/gal pH 6.0-6.5... 

Potassium Superoxide. Potassium, mbidium, and cesium form superoxides, MO2, upon oxidation by oxygen or air. Sodium yields the peroxide, Na202 lithium yields the oxide, Li20, when oxidized under comparable conditions. Potassium superoxide [12030-88-5] KO2 liberates oxygen in contact with moisture and carbon dioxide (qv). This important property enables KO2 to serve as an oxygen source in self-contained breathing equipment. 

Greater selectivity in purification can often be achieved by making use of differences in chemical properties between the substance to be purified and the contaminants. Unwanted metal ions may be removed by precipitation in the presence of a collector (see p. 54). Sodium borohydride and other metal hydrides transform organic peroxides and carbonyl-containing impurities such as aldehydes and ketones in alcohols and ethers. Many classes of organic chemicals can be purified by conversion into suitable derivatives, followed by regeneration. This chapter describes relevant procedures. 

Potassium borohydride is similar in properties and reactions to sodium borohydride, and can similarly be used as a reducing agent for removing aldehydes, ketones and organic peroxides. It is non-hygroscopic and can be used in water, ethanol, methanol or water-alcohol mixtures, provided some alkali is added to minimise decomposition, but it is somewhat less soluble than sodium borohydride in most solvents. For example, the solubility of potassium borohydride in water at 25° is 19g per lOOmL of water (as compared to sodium borohydride, 55g). 

The third period is characterized by the extensive studies, both in the USSR and abroad, of the structure, properties, and bond characteristics of peroxide compounds. This period includes the work of Kazamovskii and his coworkers concerning the structure of a series of peroxide compounds, his discovery of sodium superoxide, and the fundamental investigations carried out by the Canadian scientist Otto Maas and his co-workers concerning concentrated hydrogen peroxide. . . ... 

The first synthesis of stable 3-hydroperoxy-sultams (24) which are a new class of sultam with oxidising properties, was reported. The synthesis involved oxidation of the isothiazolium salts (23) with hydrogen peroxide in acetic acid. Reduction of (24) with aqueous sodium bisulphite afforded the corresponding novel 3-hydroxysultams whereas thermolysis in ethanol resulted in the elimination of water to give 3-ketone derivatives, which are versatile as dieneophiles <96T783>. 

Other oxidizers, including barium chromate (BaCrO,), lead chromate (PbCrO 4), sodium nitrate (NaNO 3), lead dioxide (PbO 2), and barium peroxide (BaO 2) will also be encountered in subsequent chapters. Bear in mind that reactivity and ease of ignition are often related to the melting point of the oxidizer, and the volatility of the reaction products determines the amount of gas that will be formed from a given oxidizer /fuel combination. Table 3.2 contains the physical and chemical properties of the common oxidizers, and Table 5.8 lists the melting and boiling points of some of the common reaction products. 

Several preparation methods have been reported for the synthesis of TS-1. In this work, we have investigated the physicochemical properties of TS-1 samples synthesized by different preparation metiiods and tested these materials as catalysts for the oxidation of n-octane, 1-hexene and phenol using aqueous hydrogen peroxide (30 wt%) as oxidant at temperatures below 100 C. For comparison, Ti02 (anatase) and the octahedral titanium-containing silicate molecular sieve (ETS-10) (5) have been studied. The effect of the presence of aluminum and/or sodium on the catalytic activity of TS-1 is also discussed. 

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