Magnesium Nitrate: Overview, Questions, Preparation

This chapter has multiple topics listed below:

Acids, Bases and Salts Acid Strength Difference between Acid and Bas...Examples of Bases Zinc carbonate Zinc Nitrate Aluminium Phosphate Aspartic Acid Butyric Acid Tannic acid Uses of Folic Acid Uses of Acetic Acid Lactic Acid formula Uses of Citric Acid Magnesium Nitrate Barium Iodide Dilute Acids Magnesium Phosphate Uses of Hydrochloric Acid List of Strong Acids Butanoic Acid Sodium Chlorate Barium Carbonate Chloroacetic Acid Magnesium Bicarbonate Red Cabbage Indicator Sodium Hexametaphosphate Zinc Hydroxide Potassium Iodate Peroxydisulfuric Acid Ph of Acids and Bases Potassium Bromate Weak Acid Examples Weak Bases Magnesium Hydroxide Monosodium Glutamate Potassium Hydroxide Nitrous Acid Henderson Hasselbalch Equation Difference between Alkali and B...Properties of Bases Sodium Citrate Ammonium Phosphate Chemical Indicators Chromic Acid Perchloric Acid Uses of Sodium Hydroxide Zinc Acetate

Jasleen Taneja

Updated on Jun 4, 2024 16:49 IST

With the formula, Mg(NO₃)₂(H₂O)x, magnesium nitrate refers to an inorganic compound, where x can be equal to 6, 2, and 0. They are white solids. This anhydrous substance is hygroscopic, creating the hexahydrate easily. In both water and ethanol, both of the salts are readily soluble. Often known as magniosan/nitro magnesite/magnesium dinitrate, magnesium nitrate is hexahydrate.

Table of Contents

What are nitrates?
Properties of Magnesium Nitrate
Uses of Magnesium Nitrate:
Magnesium Nitrate Reactions
Illustrated Examples
FAQs on Magnesium Nitrate

What are nitrates?

It is used extensively in pyrotechnics. Nitrates are excellent precursors to the development of ultra-high purity compounds and certain catalyst and nanoscale materials when combined with hydrocarbons. Nitrate compounds appear to form the flammable mixture.

Properties of Magnesium Nitrate

Magnesium Nitrate	Mg(NO₃)₂
Density	2.3gm/cm³
Molecular weight	148.32gm/mol
Melting point	129°C
Boiling point	330°C

Uses of Magnesium Nitrate:

Magnesium nitrate is used for the preparation of distilled nitric acid as an agent for dehydration.
Used in the petrochemical processing sector.
Used in ammonium nitrate manufacturing.
Used as a lithographic plate desensitiser.
Used in nitric acid purification.
Used in the manufacturing of toner or colouring goods.
Used as a viscosity adjuster in sectors.
Mining is used in the process.

Magnesium Nitrate Reactions

To create the following, the magnesium dinitrate reacts with alkali metal hydroxide:

Mg(NO₃)₂ + 2 NaOH → Mg(OH)₂ + 2 NaNO₃

Mg(NO₃)₂(H₂O)_x is closely correlated with water. Heating, however, comprises the decomposition of nitrogen oxide, oxygen, and magnesium oxide.

2 Mg(NO₃)₂ → 2 MgO + 4 NO₂ + O₂

The Reaction of a Basic Salt in Water

There are many types of salts, and we will include simple salts in this section. What's the simple salt? That is because the anion in the salt is the conjugate base of a weak acid. With a generalised anion B–, the net ion reaction is:

B⁻(aq) + H2O (l) ⇌ BH (aq) + OH− (aq)

Sodium bicarbonate, NaHCO3, is an indicator of simple salt. The bicarbonate ion is a conjugate base to low acid carbonic acid. It then interacts with water in the following way:

HCO−3 (aq) + H₂O (l) ⇌ H2CO3 (aq) + OH⁻(aq)

Since it is capable of deprotonation of water and having a basic solution, sodium bicarbonate is a specific salt.

Other representations of basic salts are:

Calcium carbonate (CaCO₃)
Sodium acetate (NaOOCCH₃)
Potassium cyanide (KCN)
Sodium sulfide (Na₂S)

Remember that for any of these cases, the anion is a conjugate base of a weak acid (carbonic acid, bisulfate (second dissociation stage of sulphuric acid), acetic acid, hydrocyanic acid, hydrogen sulphide).

Magnesium Nitrate in Class 10:

Class 10 has a basic study of the compound under the chapter Acid, Bases, and Salts. Weightage is 3 marks.

Magnesium Nitrate in Class 11:

In Class 11, there are a lot of chapters having some concept of magnesium nitrate in it. One of the main chapters is Chemical Reactions and Equations.

Illustrated Examples

1. Does magnesium react with magnesium nitrate?

Answer: This is a displacement reaction since magnesium has displaced the copper ions (copper in solution) from the solution (redox). As magnesium is higher in the action sequence, zinc, copper, and lead don’t undergo reaction with magnesium nitrate as it is highly reactive than the other metals.

2. How can you make a nitrate solution for magnesium?

Answer: By suspending a magnesium compound in water, applying 50-60 percent w/w nitric acid in such a quantity that the final pH is from 5.0 to 6.0, and filtering the product as a transparent filtrate to isolate magnesium nitrate, a magnesium nitrate solution (32-40 percent w/v) is prepared.

3. What three gases are released as magnesium nitrate is heated?

Answer: It decomposes to form magnesium oxide, nitrogen(IV) oxide, and oxygen as magnesium nitrate(V) is heated. Nitrogen(IV) oxide is an acidic gas that reacts with alkalis readily and entirely.

2 Mg(NO₃)₂ → 2 MgO + 4 NO₂ + O₂

FAQs on Magnesium Nitrate

Q: Is magnesium nitrate acid or base?

A: Magnesium nitrate is a high water solubility crystalline source for use, compatible with nitrates and lower (acidic) pH. In water, nitrate compounds are typically soluble. Even nitrate products are drivers of oxidation.

Q: What type of compound is magnesium nitrate?

A: Mg(NO 3 ) 2 (H 2 O) x is an ionic alloy made up of Mg +2 cation and NO −3 polyatomic anion nitrate.

Q: How many atoms does magnesium nitrate have?

A: The magnesium nitrate complex contains one magnesium atom, two nitrogen atoms, and six oxygen atoms.

Q: What is magnesium nitrate used for?

A: Mg(NO 3 ) 2 (H 2 O) x is put to use in pyrotechnics and also for the processing of nitric acid in concentrated form.

Q: Is magnesium nitrate toxic?

A: Magnesium nitrate is a poisonous agent and an irritant to the skin, eyes, and respiratory tract. Action with the skin or eye can cause redness and discomfort. Coughing and shortness of breath can be caused by inhalation.