Basic information Physical Properties Occurrence and Uses Preparation Reactions Safety Related Supplier
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Magnesium nitrate

Basic information Physical Properties Occurrence and Uses Preparation Reactions Safety Related Supplier
Magnesium nitrate Basic information
Magnesium nitrate Chemical Properties
  • Melting point:648 °C(lit.)
  • Boiling point:1090 °C(lit.)
  • Density 0.889 g/mL at 25 °C
  • vapor pressure 1 mm Hg ( 621 °C)
  • RTECS OM3756000
  • Flash point:−26 °F
  • solubility H2O: soluble
  • form turnings
  • Water Solubility Freely soluble in water. Moderately soluble in ethanol and ammonia.
  • Sensitive Hygroscopic
  • Merck 13,5697
  • CAS DataBase Reference10377-60-3(CAS DataBase Reference)
  • EPA Substance Registry SystemMagnesium nitrate (10377-60-3)
Safety Information
MSDS
Magnesium nitrate Usage And Synthesis
  • Physical PropertiesThe anhydrous salt consists of white cubic crystals; density 2.3 g/cm3; very soluble in water. The dihydrate is white crystalline solid having density 1.45 g/cm3; decomposes at about 100°C; soluble in water and ethanol. The hexahydrate, MgNO3•6H2O is a colorless solid having monoclinic crystal structure and density 1.46 g/cm3. The salt is hygroscopic and very soluble in water and moderately soluble in ethanol.
  • Occurrence and UsesThe hexahydrate, Mg(NO3)2•6H2O, occurs in nature as mineral nitromagnesite. Magnesium nitrate is used in pyrotechnics; and in the manufacture of concentrated nitric acid to remove water and concentrate the acid vapors to 90–95% HNO3. It also is used to aid coating and prilling in production of ammonium nitrate. The salt also is used as an analytical standard for magnesium and a matrix modifier in furnace atomic absorption spectroscopic analysis. It also finds some limited application as a nitrogenous fertilizer.
  • PreparationMagnesium nitrate is prepared by the action of nitric acid on magnesium carbonate, oxide or hydroxide:
    MgCO3 + 2HNO3 → Mg(NO3)2 + CO2 + H2O
    Mg(OH)2 + 2HNO3 → Mg(NO3)2 + 2H2O
    The salt crystallizing at room temperature after evaporation is the hexahydrate, Mg(NO3)2•2H2O.
  • ReactionsThermal decomposition of anhydrous Mg(NO3)2 yields magnesium oxide and nitrogen oxides. Heating the hexahydrate above its melting point forms basic nitrates, such as Mg(NO3)2•4 Mg(OH)2. The latter decomposes at 400°C, forming magnesium oxide and oxides of nitrogen. Magnesium nitrate forms addition compounds with a number of nitrogen-containing organics such as pyridine, aniline, and urea.
  • DescriptionMagnesium nitrate has the molecular formula of Mg(NO3)2 and the molecular weight of 148.3152 g/ mol.
    Magnesium nitrate is prepared by the action of nitric acid on magnesium carbonate, oxide or hydroxide:
    MgCO3 + 2HNO3 ? Mg(NO3)2 + CO2 +H2O
    Mg(OH)2 + 2HNO3 ? Mg(NO3)2 + 2H2O
    The salt crystallizing at room temperature after evaporation is the hexahydrate, Mg(NO3)2·6H2O. Two stable hydrates are formed, the hexahydrate [CAS number =13446-18-9] and the dihydrate, Mg(NO3)2· 2H2O [CAS number = 15750-45-5].
  • Chemical PropertiesMagnesium nitrate is white crystalline solid.
  • Chemical PropertiesWhite crystals.Soluble in water and alcohol; deliquescent.
  • UsesIn pyrotechnics; in the concentration of nitric acid.
  • PreparationThe magnesium nitrate used in commerce has been synthesized in a variety of ways. The reaction between nitric acid and magnesium metal is one way and reaction with MgO is another. Magnesium hydroxide and ammonium nitrate also form the product but ammonia
  • DefinitionChEBI: The inorganic nitrate salt of magnesium.
  • General DescriptionA white crystalline solid. Produces toxic oxides of nitrogen if heated to decomposition. Used in pyrotechnics.
  • Air & Water ReactionsDeliquescent. Water soluble.
  • Reactivity ProfileMixtures of Magnesium nitrate with alkyl esters may explode owing to the formation of alkyl nitrates; mixtures with phosphorus, tin(II) chloride, or other reducing agents may react explosively [Bretherick 1979 p. 108-109]. Noncombustible but will accelerate the burning of combustible materials. If large quantities are involved in a fire or the combustible material is finely divided an explosion may result. Prolonged exposure to fire or heat may result in an explosion. Magnesium nitrate has been reported to undergo spontaneous decomposition in dimethylformamide [Bretherick 5th ed., 1995]. Magnesium nitrate tends to behave as a strong oxidizer.
  • HazardDangerous fire and explosion risk in contact with organic materials, strong oxidizing agent.
  • Health HazardExposure can cause mild irritation to the mucous membranes. Symptoms may include coughing and shortness of breath. Ingestion of large doses may cause dizziness, abdominal pain, vomiting, bloody diarrhea, weakness, convulsions, and collapse. Contact with skin may cause irritation, redness, and pain.
  • Safety ProfileProbably a severe irritant to the eyes, skin, and mucous membranes. A powerful oxidizer. Violent decomposition on contact with dmethylformamide. When heated to decomposition it emits toxic fumes of NOx. See also NITRATES and MAGNESIUM COMPOUNDS.
  • Potential ExposureMagnesium nitrate is used in fireworks and in the production of concentrated nitric acid.
  • ShippingUN1474 Magnesium nitrate, Hazard Class: 5.1; Labels: 5.1-Oxidizer
  • IncompatibilitiesA powerful oxidizer. Violent reaction with dimethylformamide, reducing agents; combustibles, fuels, organic and easily oxidizable matter
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