Magnesium Nitrate Formula
Magnesium nitrate is a highly water-soluble crystalline. The nitrate compounds are usually soluble in water. The nitrate materials are also known to be the oxidizing agents. When it is mixed with hydrocarbons, the nitrate compounds have a tendency to form the flammable mixture. Nitrates are the excellent precursors for the production of the ultra-high purity compounds and a certain catalyst and the nanoscale materials. All the metallic nitrates are known to be the inorganic salts of a particular given metal cation and the nitrate anion. In this article, we will learn about magnesium nitrate, the magnesium nitrate formula, use of magnesium nitrate, the magnesium nitrate structure, and the health hazards of magnesium nitrate.
What is Magnesium Nitrate?
Mg(NO3)2 is a type of an inorganic nitrate salt of the element magnesium that has a chemical name magnesium nitrate.
Magnesium nitrate is also known as magniosan, magnesium dinitrate or Nntromagnesite. It is widely used in the field of pyrotechnics.
Magnesium dinitrate is a type of hygroscopic and crystalline solid which is white in colour. It is highly soluble in water and ethanol and it occurs naturally in the caverns and mines.
Magnesium Nitrate Structure
The structure of magnesium nitrate is given as follows:
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Properties of Magnesium Nitrate
Preparation of Magnesium Nitrate
Magnesium nitrate is prepared by the reaction of the element magnesium oxide with nitric acid. The reaction is given as follows:
MgO + 2HNO3 ---> Mg(NO3)2 + H2O
This reaction can also be prepared by using magnesium carbonate or hydroxide in the nitric acid.
It can also be prepared by mixing the magnesium sulfate, also known as Epsom salt with calcium nitrate.
MgSO4 + Ca(NO3)2 → Mg(NO3)2 + CaSO4
Filter off the insoluble calcium sulfate from this mixture for obtaining a solution of Mg(NO3)2. To dry it, you need to heat it gently on a water bath and then cool the concentrated solution. Then use a seed crystal for obtaining crystals of the compound and then remove the excess water using a vacuum.
By adding nitric acid to magnesium oxide, hydroxide or carbonate it will give you magnesium nitrate.
Anhydrous magnesium nitrate can be easily obtained by boiling the hydrated form in the concentrated nitric acid, though this process has not been confirmed yet. Passing nitrogen dioxide through the heated magnesium oxide at 100 °C should also give magnesium nitrate anhydrous and nitric oxide. Another process would be by mixing the anhydrous calcium or barium nitrate that is dissolved in anhydrous methanol or ethanol, with anhydrous magnesium sulfate.
Use of Magnesium Nitrate
Magnesium nitrate is used as the dehydrating agent for preparing concentrated nitric acid.
Magnesium nitrate is also used in the manufacturing of the petrochemicals.
It is used as a desensitizer for the lithographic plates.
It is used for the manufacturing of the ammonium nitrate.
Magnesium nitrate is used in the purification of the nitric acid.
It is used in the industries as a viscosity adjuster.
It is used in the manufacturing of agricultural products.
It is used in the making of toners and colourant products.
It is also used in the process of mining.
Magnesium Nitrate Reaction
Let us take a look at some of the magnesium nitrate reactions.
Magnesium dinitrate reacts with the alkali metal hydroxide for producing the following:
Mg(NO3)2 + 2NaOH ---> Mg(OH)2+ 2 NaNO3
Magnesium nitrate has a higher affinity for water. Hence, heating it would result to decomposition of magnesium oxide, oxygen, and nitrogen oxides.
2Mg(NO3)2 ----> 2MgO + 4NO2 + O2
Health Hazards of Magnesium Nitrate
Let us take a look at some of the health hazards of magnesium nitrate.
Exposure to magnesium nitrate leads to mild irritation in the mucous membranes. The symptoms of this include the shortness of breath and coughing. Swallowing larger doses of this may result in weakness, dizziness, vomiting, bloody diarrhoea, abdominal pain, and convulsions. When it comes in contact with the skin it leads to pain, redness, and irritation.
On heating, the compound magnesium nitrate leads to the decomposition and it emits toxic fumes of the nitrogen oxides. On contact with the oxidizable compound, it may result in an extremely violent combustion.
FAQs on Magnesium Nitrate
1. What is Magnesium Nitrate and what is its correct chemical formula?
Magnesium Nitrate is a hygroscopic inorganic salt of magnesium. It is a white, crystalline solid that is highly soluble in water and ethanol. The correct chemical formula for Magnesium Nitrate is Mg(NO₃)₂. It is also known by other names such as magnesium dinitrate or nitromagnesite (in its hydrated form).
2. What are the primary industrial uses of Magnesium Nitrate?
Magnesium Nitrate has several important applications across various industries. Its main uses include:
- As a dehydrating agent in the preparation of concentrated nitric acid.
- In the manufacturing of petrochemicals and agricultural products like fertilisers.
- As an oxidizing agent in pyrotechnics to create fireworks.
- As a viscosity adjuster in industrial processes.
- In the production of ammonium nitrate, where it acts as a coating and prilling agent.
3. How is Magnesium Nitrate typically prepared in a laboratory?
Magnesium Nitrate is prepared by reacting nitric acid (HNO₃) with a magnesium-containing base. The most common reaction involves adding magnesium oxide to nitric acid, which produces Magnesium Nitrate and water. The chemical equation for this reaction is: MgO + 2HNO₃ → Mg(NO₃)₂ + H₂O. Alternatively, magnesium hydroxide (Mg(OH)₂) or magnesium carbonate (MgCO₃) can be used instead of magnesium oxide.
4. Why is the formula for Magnesium Nitrate Mg(NO₃)₂, and not simply MgNO₃?
The formula Mg(NO₃)₂ is determined by the ionic charges of its constituent ions. The magnesium ion (Mg²⁺) has a valency of +2. The nitrate ion (NO₃⁻) is a polyatomic ion with a charge of -1. To form a neutral salt, the total positive charge must balance the total negative charge. Therefore, two nitrate ions, each with a -1 charge, are required to balance the single +2 charge of the magnesium ion, resulting in the formula Mg(NO₃)₂.
5. What is the difference between anhydrous Magnesium Nitrate and its hexahydrate form?
The primary difference lies in the presence of water molecules. Anhydrous Magnesium Nitrate (Mg(NO₃)₂) is the pure salt without any associated water. In contrast, Magnesium Nitrate hexahydrate (Mg(NO₃)₂·6H₂O) is the hydrated form, where each formula unit of the salt is chemically bound to six molecules of water. Because Mg(NO₃)₂ is highly hygroscopic (readily absorbs moisture from the air), the hexahydrate is the more common and stable form found in nature and commerce.
6. What happens when Magnesium Nitrate is strongly heated, and why is this reaction significant?
When strongly heated, Magnesium Nitrate undergoes thermal decomposition. It does not simply melt but breaks down into magnesium oxide (MgO), nitrogen dioxide (NO₂) gas, and oxygen (O₂) gas. The balanced equation is: 2Mg(NO₃)₂ (s) → 2MgO (s) + 4NO₂ (g) + O₂ (g). This reaction is significant because it is characteristic of the decomposition of nitrates of moderately reactive metals and results in the release of nitrogen dioxide, a toxic reddish-brown gas.
7. Is an aqueous solution of Magnesium Nitrate acidic, basic, or neutral?
An aqueous solution of Magnesium Nitrate is slightly acidic. This is because it is a salt formed from the reaction of a strong acid (Nitric Acid, HNO₃) and a relatively weak base (Magnesium Hydroxide, Mg(OH)₂). When dissolved in water, the Mg²⁺ ion undergoes hydrolysis, which releases H⁺ ions into the solution, thereby lowering the pH and making the solution acidic.
8. Given its composition, can Magnesium Nitrate be used as a fertilizer, and what are the associated safety precautions?
Yes, Magnesium Nitrate is an effective fertilizer because it provides two essential nutrients for plant growth: magnesium (for chlorophyll synthesis) and nitrogen (for leaf and stem growth). However, it must be handled with care. As a strong oxidizing agent, it can cause violent combustion if it comes into contact with flammable materials. Direct contact can cause irritation to the skin and eyes, and inhaling its dust can irritate the respiratory system. Ingestion is toxic and can lead to severe health issues.
