Magnesium ammonium nitrate

Uses. A soluble form of magnesium nitrate is used as a fertilizer ia states such as Florida where drainage through the porous, sandy soil depletes the magnesium (see Fertilizers). Magnesium nitrate is also used as a prilling aid in the manufacture of ammonium nitrate. A 0.25—0.50% addition of magnesium nitrate to the process improves the stabHity of the prills and also improves durabHity and abrasion resistance. 

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. 

Alkali and alkaline earth metals, e.g. sodium, potassium lithium, magnesium, calcium, powdered aluminium Anhydrous ammonia Ammonium nitrate... 

Ammonium nitrate Sodium chloride Magnesium sulfate Potassium chloride Bacon oil (axonge oil) Water, balance to Trade Mark... 

Magnesium sets off a violent reaction or even an expiosion with ammonium nitrate around 200°C or in contact with moiten sodium nitrate. 

Iodine reacts dangerously with numerous elements. Thus, with aluminium, magnesium or powdered zinc, the mixture with iodine in contact with a drop of water gives rise to a flash , which is extremely violent and blinding. In the very spectacular experiment involving ammonium nitrate and zinc described on p.208 and carried out with students, it is recommended to Incorporate a small quantity of iodine before throwing a few drops of water on the mixture. 

Many of the following powdered metals reacted violently or explosively with fused ammonium nitrate below 200°C aluminium, antimony, bismuth, cadmium, chromium, cobalt, copper, iron, lead, magnesium, manganese, nickel, tin, zinc also brass and stainless steel. Mixtures with aluminium powder are used as the commercial explosive Ammonal. Sodium reacts to form the yellow explosive compound sodium hyponitrite, and presence of potassium sensitises the nitrate to shock [1], Shock-sensitivity of mixtures of ammonium nitrate and powdered metals decreases in the order titanium, tin, aluminium, magnesium, zinc, lead, iron, antimony, copper [2], Contact between molten aluminium and the salt is violently explosive, apparently there is a considerable risk of this happening in scrap remelting [3],... 

Interaction with fused ammonium nitrate or with metal nitrates, phosphates or sulfates may be explosively violent [1]. Lithium and sodium carbonates may also react vigorously [2], The mixture with magnesium sulfate has been described as a noisy but low power bursting charge for pyrotechny [3],... 

Campbell and Ottaway [136] also used selective volatilisation of the cadmium analyte to determine cadmium in seawater. They could detect 0.04 pg/1 cadmium (2pg in 50 pi) in seawater. They dried at 100 °C and atomised at 1500 °C with no char step. Cadmium was lost above 350 °C. They could not use ammonium nitrate because the char temperature required to remove the ammonium nitrate also volatilised the cadmium. Sodium nitrate and sodium and magnesium chloride salts provided reduced signals for cadmium at much lower concentrations than their concentration in seawater if the atomisation temperature was in excess of 1800 °C. The determination required lower atomisation temperatures to avoid atomising the salts. Even this left the magnesium interference, which required the method of additions. 

Magnesium, potassium and sodium are extracted from the soil with 1 M ammonium nitrate. 

Magnesium pipette 2 ml sample solution into a 100-ml volumetric flask, add 5 ml releasing agent, make up to the mark with 1 M ammonium nitrate and mix. Nebulize into the AAS and record the readings (computer, chart recorder or manually, as appropriate). 

Thermal dissociation yields lanthanum oxide, La203. Its reactions in aqueous solutions are those of La ion. It forms double salts with magnesium, calcium and ammonium nitrates and many other salts when mixed in stoi-chiometic amounts. Such double salts are obtained from solution mixtures on crystalhzation and may vary in their compositions. 

After removing cerium (and thorium), the nitric acid solution of rare earths is treated with ammonium nitrate. Lanthanum forms the least soluble double salt with ammonium nitrate, which may be removed from tbe solution by repeated crystallization. Neodymium is recovered from this solution as the double magnesium nitrate by continued fractionation. 

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... 

Ammonium nitrate, Diesel fuel TNT, Dioxane, Hydrogen sulfide gas. Ammonia, Hydrochloric acid. Potassium iodide, Sulfuric acid, Paraformaldehyde, Methylene chloride, Nitric acid, Magnesium sulfate. Chloroform, Methanol Ammonium nitrate. Sulfur... 

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... 

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... 

Potassium bichromate. Antimony sulfide Potassium permanganate. Powdered sugar Barium chlorate, Paraffln wax Potassium perchlorate. Cane sugar Sodium nitrate. Sulfur Sodium peroxide. Sulfur Sodium chlorite. Aluminum powder Magnesium chlorate. Aluminum powder Guanidine nitrate. Antimony powder Ammonium nitrate. Gasoline... 

Recent developments to the hydrothermal process include improvements in yield and reaction rate and in overcoming the difficulty associated with the coproduct salt. One method of overcoming the co-product problem is to use magnesium nitrate instead of chloride, with the ammonium nitrate being utiHsed for fertiliser production [102-104]. At least one plant based on this concept is now in commercial production. While a considerable advance on the initial chloride process, the nitrate route does require close integration with a fertiliser process and thus lacks flexibility. An alternative approach being developed is to recycle the ammonium salt co-product (nitrate or chloride) and use it to leach magnesium oxide, a potentially inexpensive raw material [103]. 

A family of high performance and clean space motor/gas generators and large launch vehicle solid propellants based on poly(GlyN) binder, ammonium nitrate oxidizer and small amounts of aluminum and/or boron with optimized performance at low solids loading (without the presence of plasticizers) and also poly(GlyN) binder, ammonium nitrate oxidizer and aluminum or magnesium fuel have been reported in the literature [141, 142]. These solid propellant formulations produce essentially no HC1 or chloride ions in the exhaust and are considered eco-friendly. 

A different method for lowering the melting point of ammonium nitrate was suggested a few years before World War II. It consists of the addition of hydrated magnesium nitrate (i.e. containing water of crystallization) Mg(N03)2.6H20 to... 

The maximum nitrogen content of nitrocellulose was reached in these experiments when a 5% solutions of sodium, potassium or ammonium nitrate in nitric arid were used. The highest nitrogen percentage, i.e. 13.5%, was attained when using anhydrous salts that readily form hydrates, namely magnesium nitrate, Mg(N03)2, and sodium sulphate, NajSO ... 

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