Peroxides sodium

CONTACT WITH COMBUSTIBLE MATERIALS MAY CAUSE FIRE, CAUSES SEVERE BURNS 

Yellowish-white powder absorbs water and carbon dioxide from the air.1 

If in contaet, or mixed, with organic or other oxidizable substances, ignition or explosion may take place. Use flooding quantities of water or dry chemical extinguisher to fight fire.2 

Reacts violently with water forming sodium hydroxide and oxygen.3 

Ammonium Peroxydisulfate. Mixture explodes on heating above 75°C, grinding in a mortar, or exposure to drops of water or carbon dioxide.5 Calcium Acetylide. Mixture is liable to explode.6 

Step 1 Formation of Na O Step 2 Further oxidation to Na202 

Sodium peroxide is produced from sodium metal and oxygen (from air) in two steps  

Sodium monoxide is first produced by adding sodium metal intermittently to sodium monoxide in a rotary tube reactor while passing air through it countercurrently. The sodium metal rapidly distributes itself over the surface of the monoxide and in doing so is oxidized. The reaction temperature is 200 to 700°C and the heat of reaction is sufficient to maintain this temperature. In this way a noncaking material is obtained. The monoxide formed, containing a few per cent of peroxide and less than 1% sodium is withdrawn from the reactor intermittently. 

The oxidation of the monoxide to sodium peroxide is carried out in a similar reactor at 350°C. As this step is only slightly exothermic (-79.5 kJ/mol) heating is needed. The end product is formed as beads with a diameter of 0.5 to 1 mm and a purity of 97 to 98%. 

---

Alternatively an ice-cold dilute solution of sodium peroxide is passed through a column containing a cation-exchanger of the synthetic type (p. 274) where the cation is hydrogen (i.e. H3O then exchange occurs ... 

Only chloric(III) acid, HCIO2, is definitely known to exist. It is formed as one of the products of the reaction of water with chlorine dioxide (see above). Its salts, for example NaClOj, are formed together with chlorates)V) by the action of chlorine dioxide on alkalis. Sodium chlorate(III) alone may be obtained by mixing aqueous solutions of sodium peroxide and chlorine dioxide ... 

A solution of the free acid may be obtained by using hydrogen peroxide, instead of sodium peroxide. 

The chromates of the alkali metals and of magnesium and calcium are soluble in water the other chromates are insoluble. The chromate ion is yellow, but some insoluble chromates are red (for example silver chromate, Ag2Cr04). Chromates are often isomorph-ous with sulphates, which suggests that the chromate ion, CrO has a tetrahedral structure similar to that of the sulphate ion, SO4 Chromates may be prepared by oxidising chromium(III) salts the oxidation can be carried out by fusion with sodium peroxide, or by adding sodium peroxide to a solution of the chromium(IIl) salt. The use of sodium peroxide ensures an alkaline solution otherwise, under acid conditions, the chromate ion is converted into the orange-coloured dichromate ion ... 

Addition of sodium peroxide to a solution gives a yellow colour of the chromate. 

Principle. An organic compound which contains chlorine is mixed with sodium peroxide and ignited in a closed metal bomb. The chlorine is thus converted to sodium chloride, and after acidification the chloride is estimated by the Volhard volumetric method. Bromine and iodine, when constituents of organic compounds similarly treated, are converted largely into sodium bromate and iodate respectively these ions are therefore subsequently reduced by hydrazine to bromide and iodide ions, and estimated as before. 

Control experiment. This is not necessary if the sodium peroxide is known to be chlorine-free. If there is any doubt on this point, the whole operation should be repeated precisely as before, but omitting the organic halogen compound. A small thiocyanate titration value may be found, and this should be deducted from all determinations in which the above quantity of the particular batch of sodium peroxide is used. 

By the reaction between a solution of an acyl halide in a dry organic solvent, such as toluene, with a cold solution of sodium peroxide, for example ... 

It is usually preferable to oxidise the compound directly as follows. Intimately mix 0 02-0 05 g. of the eompound with 3 g. of sodium peroxide and 2 g. of anhydrous sodium carbonate in a niekel erucible. Heat the crueible and its eontents with a small flame, gently at first, afterwards more strongly until the eontents are fused, and eontinue heating for a further 10 minutes. Allow to stand, extract the contents of the crucible with water, and filter. Add exeess of eoneentrated nitrie acid to the filtrate and test with ammonium molybdate reagent as above. A yellow preeipitate indicates the presenee of phosphorus. It must be borne in mind that the above treatment 1 eonvert any arsenie present into arsenate. 

It is recommended that the eompound be fused with a mixture of sodium carbonate (2 parts) and sodium peroxide (1 part) as in the test for Plvoaphoms. Extract the fused mass with water, filter, and acidify with dilute hydrochloric acid. Pass hydrogen sulphide through the hot solution arsenic is precipitated as yellow arsenic sulphide. If antimony is present, it will be precipitated as orange antimony trisulphide. 

Oldhamite, see Calcium sulfide Opal, see Silicon dioxide Orpiment, see Arsenic trisulfide Oxygen powder, see Sodium peroxide... 

Sodium bismuthate (oxidation of manganese) heat 20 parts of NaOH nearly to redness in an iron or nickel crucible, and add slowly 10 parts of basic bismuth nitrate which has been previously dried. Add 2 parts of sodium peroxide, and pour the brownish-yellow fused mass on an iron plate to cool. When cold break up in a mortar, extract with water, and collect on an asbestos filter. 

Calcium carbide Moisture, selenium, silver nitrate, sodium peroxide, tin(II) chloride, potassium hydroxide plus chlorine, HCl gas, magnesium... 

Manganese dioxide Aluminum, hydrogen sulfide, oxidants, potassium azide, hydrogen peroxide, peroxosulfuric acid, sodium peroxide... 

Sodium peroxide Glacial acetic acid, acetic anhydride, aniline, benzene, benzaldehyde, carbon di-sulflde, diethyl ether, ethanol or methanol, ethylene glycol, ethyl acetate, furfural, glycerol, metals, methyl acetate, organic matter... 

Sodium chlorite [sodium chlorate (IV)] Sodium peroxide ... 

Because of the delay in decomposition of the peroxide, oxygen evolution follows carbon dioxide sorption. A catalyst is required to obtain total decomposition of the peroxides 2 wt % nickel sulfate often is used. The temperature of the bed is the controlling variable 204°C is required to produce the best decomposition rates (18). The reaction mechanism for sodium peroxide is the same as for lithium peroxide, ie, both carbon dioxide and moisture are required to generate oxygen. Sodium peroxide has been used extensively in breathing apparatus. 

AH the peroxides are colorless and diamagnetic when pure. Traces of the superoxide in technical-grade sodium peroxide impart a yellow color. Storage containers must be sealed to prevent reaction with atmospheric carbon dioxide and water vapor. 

All the simple peroxides form hydrogen peroxide (qv) on contact with water. Some, eg, sodium peroxide, hydrolyze almost instantaneously ... 

Alkali metal peroxides are stable under ambient conditions in the absence of water. They dissolve vigorously in water, forming hydrogen peroxide and the metal hydroxide. They are strong oxidizing agents and can react violendy with organic substances. Only lithium peroxide and sodium peroxide have been commercialized. 

Sodium Peroxide. Sodium peroxide [1313-60-6] Na202, is a pale yellow soHd, stable at ambient temperature, and hygroscopic. On heating, it... 

The octahydrate of sodium peroxide [12136-94-6] Na202 8H20, was made commercially ia Finland ia the 1950s (5) by reaction of hydra2oben2ene and sodium ethoxide ... 

This octahydrate, and the other hydrates and peroxohydrates of sodium peroxide that are known, no longer have commercial significance. 

Although neither inflammable nor self-igniting, sodium peroxide is highly inflammable when mixed with oxidi2able substances. Such mixtures bum violendy, even ia the absence of air. Tme sodium peroxocarbonates can be formed under the influence of atmospheric moisture and carbon dioxide. At temperatures >50° C and when exposed to pressure or friction, these peroxocarbonates can decompose and generate flame. 

Sodium peroxide is a powerful irritant to skin, eyes, and mucous membranes (2) protective clothing should be worn when handling. This product has been assigned UN No. 1504 and should be transported ia accordance with international transport regulations pertaining to Class 5.1, oxidi2ing substances. It is manufactured by Metaux Speciaux (France), Nippon Soda (Japan), and Tosoh Corp. (Japan). Trade names that have been used for this product are Solo2one and Flocool 180. 

The compound has been prepared ia reasonably high purity by the reaction of oxygen with sodium peroxide at 490°C and 298 atm (111). No appHcations are known. 

Of the binary peroxides made from hydrogen peroxide, calcium peroxide is the most important. World production is about 2000 t/yr, which is dominated by the dough-conditioning market in the United States. The markets for the other binary peroxides, such as those of zinc, magnesium, and strontium, total only a few hundred metric tons. Sodium peroxide and potassium superoxide are made from the alkaU metals and thek total markets are in the hundreds of tons. 

Petoxycatboxyhc acids also have been prepared by the reaction of acid chlorides, anhydrides, or boric-catboxyhc anhydrides with hydrogen or sodium peroxide. These reactions ate carried out at low temperature and with excess peroxide to avoid the formation of diacyl peroxides (44,168,181,184). 

Organoperoxysulfonic acids and their salts have been prepared by the reaction of arenesulfonyl chlorides with calcium, silver, or sodium peroxide treatment of metal salts of organosulfonic acids with hydrogen peroxide hydrolysis of di(organosulfonyl) peroxides, RS(0)2—OO—S(02)R, with hydrogen peroxide and sulfoxidation of saturated, non aromatic hydrocarbons, eg, cyclohexane (44,181). 

Synthesis. Symmetrical diacyl peroxides (20, R = R = alkyl or aryl) are prepared by the reaction of an acyl chloride or anhydride with sodium peroxide or hydrogen peroxide and a base ... 

Dialkyl peroxydicarbonates (21) are produced by reaction of alkyl chloroformates with sodium peroxide (44,187) ... 

---