Magnesium ammonium nitrate hydroxide

Acidic Properties. As a typical acid, it reacts readily with alkaUes, basic oxides, and carbonates to form salts. The largest iadustrial appHcation of nitric acid is the reaction with ammonia to produce ammonium nitrate. However, because of its oxidising nature, nitric acid does not always behave as a typical acid. Bases having metallic radicals ia a reduced state (eg, ferrous and staimous hydroxide becoming ferric and stannic salts) are oxidized by nitric acid. Except for magnesium and manganese ia very dilute acid, nitric acid does not Hberate hydrogen upon reaction with metals. [Pg.39]

Sodium hydroxide. Sodium cyanide. Bromine, Sulfuric acid Sulfuric acid. Bromine, Sodium cyanide Acetone, Sulfuric acid. Bromine, Methylene chloride Biguanide, Ethanol, Perchloric acid. Ethyl acetate l,3-Dichloro-2-propanol, Trioxane, 1,2-Dichloroethane, Sulfuric acid, Sodium bicarbonate, Dimethylsulfoxide, Sodium azide. Methylene chloride Ammonium nitrate, Nitromethane Ammonium nitrate, Hydrazine Sodium nitrate, Sulfur, Charcoal Potassium nitrate, Sulfur, Charcoal Magnesium powder, Hexachlorethane, Naphthalene... [Pg.96]

Ammonia gas, Carbon dioxide, Sodium chlorate Ammonia, Carbon dioxide. Sodium chlorate Hydrogen cyanide. Hydrocyanic acid. Prussic acid, Blausaure Hydrochloric acid. Methanol, ADNB, Methylene chloride. Nitric acid. Sodium bicarbonate. Magnesium sulfate 4,4-DNB, Methylene chloride. Magnesium sulfate. Sodium azide. Sodium hydroxide. Acetyl chloride. Ethyl acetate. Hexane TetranUine, Glacial acetic acid. Sodium azide Ammonium nitrate, TNT Sodium azide. Ammonia... [Pg.327]

Ethyl chloride. Magnesium metal turnings, Tetrahydrofuran, Arsenic trichloride. Hexanes Tetraethyl lead. Arsenic trichloride Ethylenediamine, Nitric acid. Ethanol Nitric acid. Ethanol, N,N"-Diethanolethylenediamine Dinitrate ethylene glycol. Nitric acid. Sulfuric acid Ammonium nitrate. Water, Oil, Oleic acid. Sodium hydroxide Sulfuric acid, Erythritol, Nitric acid. Sodium carbonate. Ethanol... [Pg.330]

The electrical conductivities of soln. of a great many compounds in liquid hydrogen halides have been measured by E. H. Archibald and D. McIntosh. The conductivity is raised considerably by phosphoryl chloride. Sodium sodium sulphide, borate, phosphate, nitrate, thiosulphate, and arsenate chromic anhydride potassium nitrate, hydroxide, chromate, sulphide, bisulphate, and ferro- and ferri- cyanide ammonium fluoride and carbonate j rubidium and caesium chloride magnesium sulphate calcium fluoride ... [Pg.179]

Ammonium Chloride Ammonium Hydroxide Ammonium Nitrate Ammonium Sulfate Boric Acid Calcium Carbonate Calcium Hydroxide Calcium Oxide Calcium Phosphate Calcium Silicate Calcium Sulfate Carbon Dioxide Carbon Monoxide Copper(I) Oxide Copper(II) Oxide Copper(II) Sulfate Hydrogen Chloride Iron(II) Oxide Iron(III) Oxide Magnesium Chloride Magnesium Hydroxide Magnesium Oxide... [Pg.904]

Solubility of Magnesium Hydroxide in Aqueous Solutions of Ammonium Chloride and of Ammonium Nitrate at 29 . [Pg.182]

Ionic compounds include salts such as sodium bromide, magnesium sulfate and ammonium nitrate. Acids and alkalis also contain ions. For example H+(aq) and Cl (aq) ions are present in hydrochloric acid and Na+(aq) and OH (aq) ions are present in sodium hydroxide. [Pg.23]

The silver nitrate solution is extracted as described above with three portions of -pentane to remove aVcyclooctene (Note 16). The aqueous silver nitrate solution is added slowly to 300 ml. of concentrated ammonium hydroxide containing cracked ice. The hydrocarbon that separates is extracted with 300 ml. of -pentane as described above and the pentane solution is dried over anhydrous magnesium sulfate and the pentane distilled through a 23 x 250 mm. column packed with glass beads. [Pg.103]

The monazite sand is heated with sulfuric acid at about 120 to 170°C. An exothermic reaction ensues raising the temperature to above 200°C. Samarium and other rare earths are converted to their water-soluble sulfates. The residue is extracted with water and the solution is treated with sodium pyrophosphate to precipitate thorium. After removing thorium, the solution is treated with sodium sulfate to precipitate rare earths as their double sulfates, that is, rare earth sulfates-sodium sulfate. The double sulfates are heated with sodium hydroxide to convert them into rare earth hydroxides. The hydroxides are treated with hydrochloric or nitric acid to solubihze all rare earths except cerium. The insoluble cerium(IV) hydroxide is filtered. Lanthanum and other rare earths are then separated by fractional crystallization after converting them to double salts with ammonium or magnesium nitrate. The samarium—europium fraction is converted to acetates and reduced with sodium amalgam to low valence states. The reduced metals are extracted with dilute acid. As mentioned above, this fractional crystallization process is very tedious, time-consuming, and currently rare earths are separated by relatively easier methods based on ion exchange and solvent extraction. [Pg.806]