Magnesium nitrate is a white crystalline compound with the chemical formula Mg(NO3)2. It is used in the production of fertilizers, explosives, and pyrotechnics due to its high reactivity and oxidizing properties.
| IUPAC Name | Magnesium dinitrate |
| Molecular Formula | Mg(NO3)2 |
| CAS Number | 10377-60-3 |
| Synonyms | Nitric acid, magnesium salt; UN 1474; Magnesium(II) nitrate; Nitric acid magnesium(2+) salt |
| InChI | InChI=1S/Mg.2NO3/c;22-1(3)4/q+2;2-1 |
Magnesium nitrate formula
The chemical formula for magnesium nitrate is Mg(NO3)2, which indicates that the compound contains one magnesium cation (Mg²⁺) and two nitrate anions (NO₃⁻). This formula is used to represent the stoichiometry of the compound in chemical equations, and it is also used in determining the molecular weight and other properties of magnesium nitrate.
Magnesium nitrate molar mass
The molar mass of magnesium nitrate, which is represented by the chemical formula Mg(NO3)2, is approximately 148.31 g/mol. This value can be calculated by adding the atomic masses of magnesium (24.31 g/mol), two nitrogen atoms (28.02 g/mol each), and six oxygen atoms (16.00 g/mol each) present in the compound. The knowledge of the molar mass is crucial in determining the amount of magnesium nitrate required in chemical reactions or in the preparation of solutions.
Magnesium nitrate boiling point
Mg(NO3)2 has a relatively high boiling point of approximately 330 °C (626 °F) at atmospheric pressure. This value can vary slightly depending on the purity and concentration of the compound. The boiling point of Mg(NO3)2 is important in industrial processes that involve the production of fertilizers, explosives, and pyrotechnics, as well as in laboratory experiments.
Magnesium nitrate melting point
The melting point of Mg(NO3)2, which is the temperature at which the solid compound changes into a liquid state, is approximately 89 °C (192 °F) for the anhydrous form and 95 °C (203 °F) for the hexahydrate form. The hexahydrate form of Mg(NO3)2 is more commonly used due to its stability and ease of handling. The melting point is an essential physical property that is used to determine the purity of Mg(NO3)2 and also in various industrial processes.
Magnesium nitrate density g/ml
The density of Mg(NO3)2 varies with the form of the compound. The anhydrous form has a density of approximately 2.3 g/cm³, while the hexahydrate form has a density of approximately 1.46 g/cm³. The density of Mg(NO3)2 is a crucial factor in determining the volume of the compound required in chemical reactions, as well as its storage and transportation.
Magnesium nitrate molecular weight
The molecular weight of Mg(NO3)2, which is the sum of the atomic weights of all the elements in the compound, is approximately 148.31 g/mol. This value is important in various chemical calculations, including determining the amount of Mg(NO3)2 required in reactions or in preparing solutions.
Magnesium nitrate structure
Mg(NO3)2 has a crystal structure that belongs to the orthorhombic crystal system. The compound consists of magnesium cations (Mg²⁺) and nitrate anions (NO₃⁻), with each magnesium cation surrounded by six nitrate anions in an octahedral arrangement. The crystal structure of Mg(NO3)2 plays a crucial role in its reactivity and properties.
| Appearance | White crystalline solid |
| Specific Gravity | 2.3 (anhydrous), 1.46 (hexahydrate) |
| Color | White |
| Odor | Odorless |
| Molar Mass | 148.31 g/mol |
| Density | 2.3 g/cm³ (anhydrous), 1.46 g/cm³ (hexahydrate) |
| Melting Point | 89 °C (anhydrous), 95 °C (hexahydrate) |
| Boiling Point | 330 °C |
| Flash Point | Not applicable |
| Water Solubility | 234 g/L (anhydrous), 156 g/L (hexahydrate) at 20 °C |
| Solubility | Soluble in water, ethanol, methanol |
| Vapour Pressure | 0.000009 mmHg at 20 °C |
| Vapour Density | Not applicable |
| pKa | 1.8 |
| pH | 4.5-6.0 (5% solution) |
Magnesium Nitrate Safety and Hazards
Mg(NO3)2 can pose a variety of safety hazards if not handled properly. It can cause irritation and burns to the skin, eyes, and respiratory tract upon contact or inhalation. The compound is also a strong oxidizing agent and can react violently with organic materials, including flammable and combustible substances. Inhaling Mg(NO3)2 dust can cause respiratory irritation and even lung damage. Store and handle Mg(NO3)2 in a cool, dry, and well-ventilated area, away from any sources of ignition. When handling this compound, use proper personal protective equipment such as gloves and safety glasses.
| Hazard Symbols | Oxidizing Agent |
| Safety Description | Avoid contact with combustible materials. Wear personal protective equipment. Keep away from sources of ignition. |
| UN Ids | UN 1474 |
| HS Code | 283429 |
| Hazard Class | 5.1 (Oxidizing agents) |
| Packing Group | II |
| Toxicity | LD50 (oral, rat): 3500 mg/kg; LD50 (dermal, rabbit): > 2000 mg/kg. Magnesium nitrate is not considered to be a carcinogen, mutagen, or teratogen. |
Magnesium Nitrate Synthesis Methods
One can synthesize magnesium nitrate (Mg(NO3)2) through several methods, including reacting magnesium oxide or magnesium hydroxide with nitric acid.
One method involves adding magnesium oxide to a solution of nitric acid in a flask, then gently heating the mixture until it dissolves. To obtain the Mg(NO3)2 crystals, filter the solution to remove any impurities, and evaporate the solvent.
Another synthesis method involves reacting magnesium metal with nitric acid. Add magnesium strips to the acid and allow the reaction to proceed until all the metal dissolves. Then evaporate the resulting solution to obtain the Mg(NO3)2 crystals.
Dissolve magnesium carbonate in nitric acid to form Mg(NO3)2 and carbon dioxide. Filter the resulting solution and evaporate it to yield crystals of Mg(NO3)2.
Another method involves reacting magnesium hydroxide with nitric acid to produce Mg(NO3)2 and water. The resulting solution is then purified by filtration and evaporation to obtain the Mg(NO3)2 crystals.
Magnesium Nitrate Uses
Magnesium nitrate has a variety of uses in various industries and applications. Some of the major uses of Mg(NO3)2 are:
- Agriculture: Used as a fertilizer, especially for crops that require high levels of magnesium, such as tomatoes, peppers, and citrus fruits. It helps improve plant growth and enhances the quality and yield of the crops.
- Pyrotechnics: Used as an oxidizer in fireworks and other pyrotechnic applications, as it can produce bright and intense flames and help control the burn rate.
- Glass production: Used as a flux in glass production to lower the melting point of the glass and improve its flow properties.
- Chemical synthesis: Used as a reactant in various chemical synthesis reactions, such as the production of other magnesium compounds, catalysts, and pharmaceuticals.
- Preservation: Used as a food preservative to inhibit the growth of bacteria and other microorganisms.
- Industrial applications: Used in the production of magnesium oxide and magnesium hydroxide, which are used as flame retardants, in wastewater treatment, and as a neutralizing agent in acid soils.
- Laboratory research: Used in various laboratory experiments and research, such as the preparation of standard solutions and the testing of analytical procedures.
Questions:
Q: Is Mg(NO3)2 soluble?
A: Yes, magnesium nitrate is highly soluble in water.
Q: What is the formula for magnesium nitrate?
A: The formula for magnesium nitrate is Mg(NO3)2.
Q: What is the molar mass of Mg(NO3)2?
A: The molar mass of Mg(NO3)2 is 148.31 g/mol.
Q: What is the formula weight of Mg(NO3)2?
A: The formula weight of Mg(NO3)2 is 148.31 g/mol.
Q: What is the systematic name of Mg(NO3)2?
A: The systematic name of Mg(NO3)2 is magnesium dinitrate.
Q: What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution?
A: The concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution is 0.25 M, as there are two nitrate ions for every one magnesium ion.
Q: What is the formula mass of Mg(NO3)2?
A: The formula mass of Mg(NO3)2 is 148.31 g/mol.