Magnesium nitrate
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| Magnesium nitrate | |
|---|---|
| Image:Magnesium nitrate.jpg | |
| IUPAC name | Magnesium nitrate |
| Other names | nitromagnesite |
| Identifiers | |
| CAS number | 10377-60-3 (anhydrous), 13446-18-9 (hexahydrate) |
| RTECS number | OM3750000 (anhydrous), OM3756000 (hexahydrate) |
| Properties | |
| Molecular formula | Mg(NO3)2 |
| Molar mass | 148.30 g/mol |
| Appearance | White crystalline solid |
| Density | 1.46 g/cm3, solid |
| Melting point |
89 °C (362 K) |
| Boiling point |
none, |
| Solubility in water | 125g/100ml |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | Eye & Skin Irritant |
| NFPA 704 |
|
| R-phrases | R8 R36 |
| S-phrases | S7 S15 |
| Flash point | Non-flammable |
| Related Compounds | |
| Other anions | MgCl2, MgSO4, Mg(OH)2, MgO, Mg3N2 |
| Other cations | Ca(NO3)2, NH4NO3, NaNO3, KNO3, Cu(NO3)2, Al(NO3)3 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references | |
Magnesium nitrate is a hygroscopic salt with the formula Mg(NO3)2. In air, it quickly forms the hexahydrate with the formula Mg(NO3)2.6H2O. It is very soluble in both water and ethanol.
Uses
Magnesium nitrate occurs in mines and caverns as nitromagnesite. This form is not common, although it may be present where guano contacts magnesium-rich rock. It is used in the ceramics, printing, chemical and agriculture industries. Its fertilizer grade has 10.5% nitrogen and 9.4% magnesium, so it is listed as 10.5-0-0 + 9.4% Mg. Fertilizer blends containing magnesium nitrate usually have ammonium nitrate, calcium nitrate, potassium nitrate and micronutrients; these blends are used in the greenhouse and hydroponics trade.
Reactions
The magnesium nitrate used in commerce is a man-made product. It can be synthesized in a variety of ways. The reaction between nitric acid and magnesium metal or magnesium oxide results in magnesium nitrate.
- 2HNO3 + MgO → Mg(NO3)2 + H2O
Magnesium hydroxide and ammonium nitrate also react to form magnesium nitrate as ammonia is released as a by-product.
- 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, magnesium nitrate hexahydrate decomposes into magnesium oxide, oxygen, and nitrogen oxides.
- 2Mg(NO3)2 → 2MgO + 4NO2 + O2
The absorbption of these nitrogen oxides in water is one possible route way to synthesize nitric acid. Although it is inefficient, it does not require the use of another strong acid.
Anhydrous magnesium nitrate is also used to increase the concentration of nitric acid past its azeotrope of approximently 68% nitric acid and 32% water. It is also occasionally used as a desiccant.
References
External links
Acknowledgement and Attribution Regarding Sources of Content
Some of the initial content on this page may be incorporated in part from copyleft sources in the public domain including wikis such as Wikipedia and AskDrWiki. Drug information for patients came from the The National Library of Medicine. Infectious disease information may have come from the Centers for Disease Control (CDC). Differential Diagnoses are drawn from clinicians as well as an amalgamation of 3 sources: 1.The Disease Database; 2. Kahan, Scott, Smith, Ellen G. In A Page: Signs and Symptoms. Malden, Massachusetts: Blackwell Publishing, 2004:3; 3. Sailer, Christian, Wasner, Susanne. Differential Diagnosis Pocket. Hermosa Beach, CA: Borm Bruckmeir Publishing LLC, 2002:7 .
