10377-60-3 Usage
Description
Magnesium nitrate, with the molecular formula Mg(NO3)2 and a molecular weight of 148.3152 g/mol, is a white crystalline solid that is soluble in water and alcohol. It is prepared by the action of nitric acid on magnesium carbonate, oxide, or hydroxide. The anhydrous salt consists of white cubic crystals with a density of 2.3 g/cm3, while the dihydrate is a white crystalline solid with a density of 1.45 g/cm3. The hexahydrate, Mg(NO3)2·6H2O, is a colorless solid with a monoclinic crystal structure and a density of 1.46 g/cm3. Magnesium nitrate is hygroscopic and produces toxic oxides of nitrogen when heated to decomposition.
Uses
Used in Pyrotechnics:
Magnesium nitrate is used as a component in pyrotechnics for its ability to produce bright, white light and heat when burned.
Used in Chemical Industry:
Magnesium nitrate is used in the concentration of nitric acid, as it helps to remove water and concentrate the acid vapors to 90-95% HNO3.
Used in Agriculture:
The fertilizer grade of magnesium nitrate contains 10.5% nitrogen and 9.4% magnesium, making it a valuable nutrient source for crops.
Used in Printing Industry:
Magnesium nitrate is used in the printing industry, likely due to its properties as a nitrogenous fertilizer and its ability to aid in coating and prilling processes.
Used in Ceramics Industry:
Magnesium nitrate is used in the ceramics industry, possibly for its ability to aid in coating and prilling processes, as well as its role as a matrix modifier in furnace atomic absorption spectroscopic analysis.
Used as an Analytical Standard:
Magnesium nitrate is used as an analytical standard for magnesium, which is important for the accurate measurement and analysis of magnesium in various applications.
Used in the Production of Ammonium Nitrate:
Magnesium nitrate is used to aid in the coating and prilling process during the production of ammonium nitrate, a widely used fertilizer and explosive.
Preparation
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?2H2O.
Preparation
The 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 is released as a by-product: 2HNO3 + Mg Mg(NO3)2 +H2 2HNO3 + MgO Mg(NO3)2 +H2O Mg(OH)2 + 2NH4NO3 Mg(NO3)2 + 2NH3 + 2H2O Since magnesium nitrate has a high affinity for water, heating the hexahydrate does not result in the dehydration of the salt. Instead, it decomposes into magnesium oxide, oxygen and nitrogen oxides: 4Mg(NO3)2·6H2O + heat 4MgO + 2NO2 + 2N2O + O2 + 6H2O Heating the hexahydrate above its melting point first forms basic nitrates, such as Mg(NO3)2·4Mg(OH)2. It is this salt that decomposes at 400 C, forming magnesium oxide and oxides of nitrogen. The absorption of these nitrogen oxides in water is one possible way to synthesize HNO3. Although it is inefficient, it does not require the use of another strong acid and the mineral, nitromagnesite, can be used in this context.
Reactions
Thermal 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.
Air & Water Reactions
Deliquescent. Water soluble.
Reactivity Profile
Mixtures 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.
Hazard
Dangerous fire and explosion risk in contact
with organic materials, strong oxidizing agent.
Health Hazard
Exposure 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.
Flammability and Explosibility
Nonflammable
Safety Profile
Probably 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.
Check Digit Verification of cas no
The CAS Registry Mumber 10377-60-3 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,0,3,7 and 7 respectively; the second part has 2 digits, 6 and 0 respectively.
Calculate Digit Verification of CAS Registry Number 10377-60:
(7*1)+(6*0)+(5*3)+(4*7)+(3*7)+(2*6)+(1*0)=83
83 % 10 = 3
So 10377-60-3 is a valid CAS Registry Number.
InChI:InChI=1/Mg.NO3/c;2-1(3)4/q+2;-1