Magnesium Nitrate: Properties, Structure, Formula, Uses

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Magnesium nitrate is also known as magnesium dinitrate or magniosan or nitromagnesite (hexahydrate). Magnesium dinitrate is a hygroscopic, strong white crystalline. It is highly soluble in water and ethanol and occurs naturally in caves and mines. Magnesium is widely used in pyrotechnics. It is an essential element in the growth of healthy plants. It is a major component of the chlorophyll molecule, which is why it is so important for photosynthesis and the formation of carbohydrates.

Table of Content

What is Magnesium Nitrate?
Magnesium Nitrate Formula
Properties of Magnesium Nitrate
Structure of Magnesium Nitrate
Uses of Magnesium Nitrate
Health Hazards of Magnesium Nitrate
Magnesium Nitrate Reaction
Things to Remember
Sample Questions

What is Magnesium Nitrate?

Magnesium nitrate is an inorganic compound that is highly soluble in water and ethanol. The chemical formula of magnesium nitrate is Mg(NO₃)₂. It is a hygroscopic and crystalline solid that is white. The nitrate in Magnisal helps the plant to absorb magnesium, thus, improving its efficiency.

It also enriches plant nutrients with easily available and easily absorbed nitrogen. It is ideal for efficient applications by fertigation and foliar spray. Magnesium nitrate is better than magnesium sulfate fertilizer. Because it has a high amount of nutritional value and better physical ingredients that make it easier to manage and use.

Also Read:

Magnesium Carbonate	Hard Water and Soft Water

Magnesium Nitrate Formula

The formula of magnesium nitrate is Mg(NO₃)₂. Nitrate compounds are usually dissolved in water. Nitrate substances are also known as oxidizing agents. When mixed with hydrocarbons, nitrate compounds tend to form a flammable mixture. Nitrates are excellent precursors for the production of compounds of the highest purity and specific catalyst and nanoscale materials. All iron nitrates are known as inorganic salts of a given iron cation and nitrate anion.

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Properties of Magnesium Nitrate

Properties of Magnesium Nitrate have been tabulated below:

Mg(NO₃)₂	Magnesium Nitrate
Molecular weight of Mg(NO₃)₂	48.32 g/mol (anhydrous)
Density of Magnesium Nitrate	2.3 g/cm³ (anhydrous)
Melting point of Magnesium Nitrate	129°C
Boiling point of Magnesium Nitrate	330°C

Structure of Magnesium Nitrate

By adding nitric acid to magnesium oxide, hydroxide or carbonate will give you magnesium nitrate. Anhydrous magnesium nitrate may be easily obtained by boiling a hydrated form in concentrated nitric acid.

Structure of Magnesium Nitrate

Uses of Magnesium Nitrate

Magnesium nitrate is used as a desensitizer for the lithographic plates.
It is used in the making of toners and colorant products.
It is used to manufacture ammonium nitrate.
It is used as a dehydrating agent to prepare concentrated nitrate acid.
Also, magnesium nitrate is used in the process of mining.
It is used in the manufacturing of petrochemicals.
Moreover, it is used in the industries as a viscosity adjuster.
Magnesium nitrate is used in the purification of nitric acid.
It is used in the manufacturing of agricultural products.

Also Read:

Surface Chemistry	Surface Tension

Health Hazards of Magnesium Nitrate

Exposure to magnesium causes minor irritation to the mucous membranes. Symptoms include shortness of breath and coughing. Swallowing large doses can cause dizziness, vomiting, weakness, and falls. abdominal pain, bloody diarrhea, and convulsions. Contact with the skin causes redness, pain, and irritation. When it combines to decompose, it releases toxic fumes from nitrogen oxide. Contact with an oxidizable compound can lead to extremely violent temperatures.

Also Read:

Adsorption	Emulsion

Magnesium Nitrate Reaction

Let us take a look at some examples of magnesium nitrate reactions.

Magnesium nitrate 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. Thus, heating would result in the decomposition of magnesium oxide, oxygen, and nitrogen oxides.

2Mg(NO₃)₂ → 2MgO + 4NO₂ + O₂

Things to Remember

Magnesium nitrate is an inorganic compound. It is highly soluble in water and ethanol. It melts quickly and does not produce a precipitate, even at low temperatures.
It is also called magnesium dinitrate, nitromagnesite, or magniosan.
The cation of magnesium and polyatomic anion of nitrate combine to form a neutral salt compound with the formula magnesium nitrate. Therefore, the chemical formula of magnesium nitrate is given as Mg (NO₃).
Nitrates are an excellent precursor to the development of high purity compounds as well as catalyst and nanoscale compounds when combined with hydrocarbons. Nitrate compounds appear to form a flammable mixture.
Magnesium nitrate deficiency in plants is indicated by yellow bands between the arteries of the leaves. Symptoms first appear on older leaves, and then on younger leaves as the deficiency becomes worse. In severe cases, necrosis may occur.

Also Read:

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Sample Questions

Ques. Is magnesium nitrate acid or base? (2 Marks)

Ans. Magnesium nitrate is a crystal source with high water solubility for use in combination with nitrates and low (acidic) pH. Nitrate compounds are usually dissolved in water. Even nitrate products are oxidizing agents. Nitrate compounds can form a combustible mixture when mixed with hydrocarbons.

Ques. How is magnesium nitrate prepared? (2 Marks)

Ans. Magnesium nitrate, which is highly soluble in water, occurs naturally only in mines and caves such as nitromagnesite, in the form of hexahydrate. Commercially available magnesium nitrate is produced by reaction with nitric acid and various other magnesium salts.

Ques. Which metals will not react with magnesium nitrate? (2 Marks)

Ans. Zinc, copper, and lead do not react with magnesium nitrate because in terms of activity magnesium is higher because it is more active than other metals. Therefore, no zinc, copper, or lead will remove magnesium ions from the solution, so that there is no reaction.

Ques. Is magnesium nitrate toxic in nature? (3 Marks)

Ans. Magnesium nitrate is a toxic agent and irritates the skin, eyes, respiratory tract, digestive issues, and lethargy. Skin or eye contact can cause redness and discomfort. Cough and shortness of breath can be caused by sniffing. In rare cases, excessive magnesium can be fatal. Magnesium toxicity is rare in otherwise healthy people, and levels are more likely to be lower than high.

Ques. What is magnesium nitrate used for? (3 Marks)

Ans. Magnesium nitrate is used in pyrotechnics is magnesium nitrate and in the manufacture of concentrated nitric acid where it extracts water and concentrates the acid vapors to 90–95% HNO?. It is also used to help in the processing of ammonium nitrate for coating and prilling. Moreover, magnesium nitrate is 100% plant-friendly, which increases the quality of the plant.

Ques. What type of compound is magnesium nitrate? (2 Marks)

Ans. Magnesium Nitrate is an ionic compound composed of the cation Magnesium Mg²+ and the polyatomic anion Nitrate NO?-. The charges must be equal and uniform for the two ions to bind. Thus, one magnesium ion + 2 will need two nitrates -1 to balance.

Ques. What is magnesium nitrate fertilizer? (2 Marks)

Ans. Magnesium nitrate fertilizer provides plants with easily available magnesium, which is essential for their healthy growth. Nitrate in magnesium helps the absorption of magnesium by the plant, therefore, improving its efficiency. It cures magnesium deficiency in plants.

Ques. Name some of the use of magnesium nitrate in household products. (3 Marks)

Ans. The use of magnesium nitrate in household products are in the following category -

Auto products
Home maintenance
Personal care
Landscaping/yard
Commercial/institutional

CBSE CLASS XII Related Questions

1.
In the button cells widely used in watches and other devices the following reaction takes place:
Zn(s) + Ag₂O(s) + H₂O(l) \(\rightarrow\) Zn²⁺_(aq) + 2Ag(s) + 2OH^- (aq)
Determine \(\triangle _rG^\ominus\) and \(E^\ominus\) for the reaction.

View Solution

2.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

View Solution

3.
Give the IUPAC names of the following compounds:
(i)CH₃CH(Cl)CH(Br)CH₃
(ii)CHF₂CBrClF
(iii)ClCH₂C≡CCH₂Br
(iv)(CCl3)₃CCl
(v)CH₃C(p-ClC₆H₄)₂CH(Br)CH₃
(vi)(CH₃)₃CCH=CClC₆H₄I-p

View Solution

4.
Write equations of the following reactions:
(i)Friedel-Crafts reaction–alkylation of anisole.
(ii)Nitration of anisole.
(iii)Bromination of anisole in ethanoic acid medium.
(iv)Friedel-Craft’s acetylation of anisole.

View Solution

5.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

View Solution

6.
The rate constant for the decomposition of hydrocarbons is 2.418 x 10^-5 s^-1 at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.

View Solution

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Magnesium Nitrate: Properties, Structure, Formula, Uses

What is Magnesium Nitrate?

Magnesium Nitrate Formula

Properties of Magnesium Nitrate

Structure of Magnesium Nitrate

Uses of Magnesium Nitrate

Health Hazards of Magnesium Nitrate

Magnesium Nitrate Reaction

Things to Remember

Sample Questions

CBSE CLASS XII Related Questions

1.
In the button cells widely used in watches and other devices the following reaction takes place:
Zn(s) + Ag₂O(s) + H₂O(l) \(\rightarrow\) Zn²⁺_(aq) + 2Ag(s) + 2OH^- (aq)
Determine \(\triangle _rG^\ominus\) and \(E^\ominus\) for the reaction.

2.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

3.
Give the IUPAC names of the following compounds:
(i)CH₃CH(Cl)CH(Br)CH₃
(ii)CHF₂CBrClF
(iii)ClCH₂C≡CCH₂Br
(iv)(CCl3)₃CCl
(v)CH₃C(p-ClC₆H₄)₂CH(Br)CH₃
(vi)(CH₃)₃CCH=CClC₆H₄I-p

4.
Write equations of the following reactions:
(i)Friedel-Crafts reaction–alkylation of anisole.
(ii)Nitration of anisole.
(iii)Bromination of anisole in ethanoic acid medium.
(iv)Friedel-Craft’s acetylation of anisole.

5.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

6.
The rate constant for the decomposition of hydrocarbons is 2.418 x 10^-5 s^-1 at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.

Comments

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Magnesium Nitrate: Properties, Structure, Formula, Uses

What is Magnesium Nitrate?

Magnesium Nitrate Formula

Properties of Magnesium Nitrate

Structure of Magnesium Nitrate

Uses of Magnesium Nitrate

Health Hazards of Magnesium Nitrate

Magnesium Nitrate Reaction

Things to Remember

Sample Questions

CBSE CLASS XII Related Questions

1. In the button cells widely used in watches and other devices the following reaction takes place:Zn(s) + Ag2O(s) + H2O(l) \(\rightarrow\) Zn2+(aq) + 2Ag(s) + 2OH- (aq) Determine \(\triangle _rG^\ominus\) and \(E^\ominus\) for the reaction.

2. Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s) takes place. Further show: (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.

3. Give the IUPAC names of the following compounds:(i)CH3CH(Cl)CH(Br)CH3(ii)CHF2CBrClF(iii)ClCH2C≡CCH2Br(iv)(CCl3)3CCl(v)CH3C(p-ClC6H4)2CH(Br)CH3(vi)(CH3)3CCH=CClC6H4I-p

4. Write equations of the following reactions: (i)Friedel-Crafts reaction–alkylation of anisole.(ii)Nitration of anisole.(iii)Bromination of anisole in ethanoic acid medium.(iv)Friedel-Craft’s acetylation of anisole.

5. How would you account for the following: Of the d4 species, Cr2+ is strongly reducing while manganese(III) is strongly oxidising. Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised. The d1 configuration is very unstable in ions.

6. The rate constant for the decomposition of hydrocarbons is 2.418 x 10-5 s-1 at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.

Comments

SUBSCRIBE TO OUR NEWS LETTER

1.
In the button cells widely used in watches and other devices the following reaction takes place:
Zn(s) + Ag₂O(s) + H₂O(l) \(\rightarrow\) Zn²⁺_(aq) + 2Ag(s) + 2OH^- (aq)
Determine \(\triangle _rG^\ominus\) and \(E^\ominus\) for the reaction.

2.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

3.
Give the IUPAC names of the following compounds:
(i)CH₃CH(Cl)CH(Br)CH₃
(ii)CHF₂CBrClF
(iii)ClCH₂C≡CCH₂Br
(iv)(CCl3)₃CCl
(v)CH₃C(p-ClC₆H₄)₂CH(Br)CH₃
(vi)(CH₃)₃CCH=CClC₆H₄I-p

4.
Write equations of the following reactions:
(i)Friedel-Crafts reaction–alkylation of anisole.
(ii)Nitration of anisole.
(iii)Bromination of anisole in ethanoic acid medium.
(iv)Friedel-Craft’s acetylation of anisole.

5.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

6.
The rate constant for the decomposition of hydrocarbons is 2.418 x 10^-5 s^-1 at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.