Sodium ferrite

The resultant sodium ferrite and sodium hypoferrite are washed away by fresh BW and the process repeats itself, eventually resulting in extensive thinning of the steel through the development of longitudinal gouging or grooving. 

Lowig Also called Ferrite. A causticization process—the conversion of sodium carbonate to sodium hydroxide. The sodium carbonate is mixed with iron oxide and heated for several hours in a rotating kiln. Carbon dioxide is evolved and sodium ferrite remains ... 

Sodium ferrate, in sodium nitrite production, 22 855 Sodium ferrite, 14 543 Sodium fluoride, 22 825, 8 340 Sodium fluoroborate manufacture, 4 155 physical properties of, 4 152t thermodynamic properties of, 4 154t uses of, 4 156... 

What happens when iron(III) chloride reacts with hydrogen sulphide and ammonium sulphide Conduct the relevant reactions and write their equations. List the properties of iron(III) salts. How can sodium ferrite be prepared Which salts hydrolyze more strongly—ferrites or iron(III) salts What does this depend on ... 

Preparation and Properties of Sodium Ferrite. Mix 2 g of an iron(III) oxide powder and 20 g of anhydrous sodium carbonate in an iron crucible. Fuse the mixture on the flame of a gas burner or in a muffle furnace at 800-900 °C. Pour out the hot melt onto a glazed tile. When it solidifies, grind pieces of the melt in a mortar and spill the powder into a beaker with water. What settles onto the bottom of the beaker Write the equations of the reactions. What type of oxides does iron(III) oxide belong to Which salts hydrolyze more strongly, iron(II) or iron(III) salts What does this depend on ... 

There are no new principles involved as far as an electrolytic sensor is concerned. The electrolyte membrane is /i-alumina and the reference sodium activity fixed, at constant oxygen activity, by a mixture of sodium ferrite (Na10Fe16O29, which can be written 5Na20 8Fe203) and Fe203, just as it is common practice to fix oxygen activity by a mixture of a metal and its oxide. 

Ferrous acid, HFe02, is obtained 1 by the action of water on sodium ferrite, NaFe02. It has the same crystalline form and transparency as the sodium salt, but differs from Goethite in that it begins to lose water below 100° C., whereas Goethite is stable even at 300° C. 

Sodium ferrite, NaFe02, is obtained 4 by continued heating of ferric oxide in concentrated sodium hydroxide solution, and by heating ferric oxide with fused sodium carbonate or chloride. The salt crystallises in hexagonal plates, which, when treated with water, yield ferrous acid, HFe02. 

I. Preparation of Reduced Iron (Cobalt, Nickel) (245). 2. Pr ara-tion of Pyrophoric Iron (246). 3. Preparation of Iron(II) Oxide (246). 4. Preparation of Macrocrystalline Iron(III) Oxide (246). 5. Preparation of Nickel(III) Oxide (247). 6. Preparation and Properties of Sodium Ferrite (247). 7. Preparation of Anhydrous Cobalt (Nickel) Chloride in an Ethanol Solution (247). 8. Preparation of Anhydrous Iron(IlI) Chloride in a Fluidized Bed (247). 9. Preparation of Potassium Trioxalatoferrate(III) (247). 10. Preparation of Tetraamminecarbonatocobalt(III) Nitrate (248). 

The soda-AQ proeess ean use the same ehemieal recovery system as for kraft pulping but is teehnieally well suited to a simpler, more compact system known as DARS (direet alkali reeovery system), whieh has been explored on the pilot plant seale. Here ferrie oxide is added to the blaek liquor in a fluidized bed furnace. The residue of sodium ferrite partieles is removed and on leaching under controlled eonditions regenerates sodium hydroxide and ferrie oxide ... 

Another topochemical method for preparation of hydrated oxides consists of an extension of the procedure proposed by Raney in the case of metals. The required starting mixtures may be obtained by fusion of the components or by coprecipitation. A commercial fusion procedure yields Vycor glasses with interesting adsorptive and catalytic properties [4, 5, 9]. The fusion procedure is also used to obtain sodium ferrite-aluminate mixed crystals these then yield hydrated iron (III) oxide skeletal structures showing considerable chemical activity (reacting with hot aqueous NaOH) provided the starting mixture contains an excess of aluminate [7]. The activity of such structures is due both to the small particle size of the product and to a strongly distorted crystal lattice due to frozen thermal vibrations [8]. 

The sodium ferrite/ferrate solution is very alkaline and lends to absorb other acid gases such as HCN, CO2. and S02- HCN is a weak acid that reacts with the alkaline solution to form NaCN by a reversible acid/base reaction. Since it is not destroyed (as is H2S) the NaCN builds up in the solution until the vapor pressure of HCN over the solution is high enough to impede absorption. At this point most of the HCN in the feed gas leaves the absorber with the product gas. A small fraction of the HCN will react with solution components to form NaSCN and ferric ferrocyanide (Prussian blue). This fetrocyanide complex is identical to the oxygen carrier employed in the Staatsmijnen-Otto process, and contributes to the oxidation of hydrogen sulfide to elemental sulfur. 

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