Molar Mass Of Magnesium Nitrate
Magnesium nitrate or magnesium dinitrate is an inorganic nitrate common salt of magnesium. Magnesium nitrate is a white crystalline solid usually used in pyrotechnics, that is hygroscopic in nature. It occurs naturally in mines and caverns. The following sections explore the formula for magnesium nitrate, its molar mass, structure, properties, and uses.
The Formula for Magnesium Nitrate
The formula for magnesium nitrate is Mg(NO3)2. The formula is derived using the crisscross method. The valency of magnesium is plus ane, while that of nitrate is minus two. So, the formula is written every bit follows:
Magnesium Nitrate
Due to this chemical formula, magnesium nitrate has the post-obit names:
- Magnesium dinitrate (IUPAC proper name)
- Magniosan
- Nitromagnesite
- Magnesium nitrate hexahydrate
When magnesium nitrate is exposed to air, it transforms into its hexahydrate form (Mg(NOiii)2.6HiiO) as it is highly hygroscopic. However, magnesium nitrate is called nitromagnesite when it naturally occurs in the hexahydrate form.
Magnesium Nitrate Construction
Magnesium nitrate comprises magnesium and nitrate ions. The construction of magnesium is as follows:
Magnesium Nitrate
It contains a magnesium cation and two nitrate anions. An ionic bail occurs betwixt magnesium and nitrate ions. Therefore, the compound is an ionic compound. Covalent bonds practise exist in the chemical compound nitrate anions equally each nitrogen is covalently bonded to three oxygen atoms.
Lewis Dot Structure of Magnesium Nitrate
To depict the Lewis structure of Mg(NO3)2, you must understand the following concepts:
Ionic compounds are formed when metals react with nonmetals and give ascension to a neatly packed crystalline solid. Magnesium nitrate is an ionic compound, and information technology is held together by ionic bonds. The chemical compound has an overall neutral charge despite containing positively and negatively charged ions.
The nitrate anion in the compound contains covalent bonding. We can write its covalent Lewis structure as follows:
Nitrate ion
However, when y'all accept to write the final Lewis structure of magnesium nitrate, you must follow the ionic compounds' rule as write as follows:
Lewis Structure of Magnesium nitrate
Preparation of Magnesium Nitrate
Several methods accept been employed to set magnesium nitrate in laboratories. Some of the most popular grooming methods are shared below:
From Magnesium Hydroxide and Nitric Acid
When 1 mole of magnesium hydroxide reacts with two moles of nitric acrid, it gives one mole of magnesium nitrate. Nitric acid works equally a dehydrating agent in the reaction. The counterbalanced chemic reaction is as follows:
Mg(OH)2+ii HNO3→Mg(NO3)2+2 HtwoO
From Magnesium Sulphate and Calcium Nitrate
Magnesium nitrate can exist obtained when magnesium sulphate reacts with calcium nitrate. The balanced chemical equation for the reaction is as follows:
MgSO4 + Ca(NOiii)2 → Mg(NO3)2 + CaSO4
From Magnesium Oxide and Nitric Acid
Just like the previous training method, when nitric acid reacts with magnesium oxide, it gives magnesium nitrate and water. The chemical reaction can be represented as follows:
MgO+ 2 HNO3→Mg(NO3)two+H2O
From Magnesium Carbonate and Nitric Acid
Some other table salt of magnesium, magnesium carbonate, tin can react with nitric acid to produce magnesium nitrate. The chemical equation for the reaction tin exist represented as follows:
MgCO3+ ii HNO3→COii + Mg(NOthree)2+HtwoO
From Magnesium and Dilute Nitric Acid
Yous can too use magnesium rather than its salts to produce magnesium nitrate. The chemic equation tin be represented as follows:
Mg(s) + 2 HNO3(aq) → Mg(NOiii)2(aq) + H2(yard)
Properties of Magnesium Nitrate
- Magnesium nitrate molar mass: 148.32 g/mol (anhydrous)
- Density: 2.iii thou/cm3 (anhydrous)
- Colour: White
- State: Crystalline solid
- Melting point: 129 °C
- Boiling bespeak: 330 °C
- Solubility: Readily soluble in h2o and moderately in ammonia and ethanol
- Nature: Hygroscopic
- Crystal construction: Cubic
Magnesium Nitrate Tooth Mass Calculation
You lot tin can easily calculate the magnesium nitrate molar mass using its chemical formula Mg(NOthree)2.
The atomic weight of an atom of Mg is 24.
Nitrogen = 14
Oxygen = 16
The molecular mass of magnesium nitrate = Atomic weight of 1 Mg atom + Atomic weight of 2 Nitrogen atoms + Diminutive weight of 6 oxygen atoms
Magnesium nitrate molecular mass = one×24 + 2×14 + 6×sixteen
Total mass = 24 + 28 +96
Full mass =148 g/mol
Therefore, the molecular mass of magnesium nitrate is 148 g/mol.
Chemical Reactions of Magnesium Nitrate
Magnesium reacts with diverse hydroxides and carbonates to give desired products. Following are some of the important reactions of magnesium nitrate:
Reaction with Hydroxides
Magnesium nitrate reacts with sodium hydroxide or other brine metal hydroxide to give the post-obit reaction:
Mg(NO3)2 + 2 NaOH → Mg(OH)ii + 2 NaNO3
Decomposition Reaction
Magnesium nitrate possesses a stiff affinity for h2o. On heating, it decomposes into oxygen, magnesium oxide, and nitrogen oxide.
2 Mg(NO3)2 → 2 MgO + 4 NO2 + O2
Double Decomposition Reaction with Sodium Carbonate
It reacts with sodium carbonate to produce magnesium carbonate and sodium nitrate.
Mg(NOiii)2 + Na2COiii → MgCOiii + 2 NaNO3
Reaction with H2o
It decomposes in h2o to give magnesium hydroxide, oxygen and ammonia. The following equation represents the reaction:
Mg(NO3)two + 4 HiiO → Mg(OH)2 + two NH3 + 4 O2
Thermal Decomposition On Heating
When magnesium nitrate is heated, it decomposes to give magnesium oxide. The reaction gain as follows:
2 Mg(NOiii)2 → 2 MgO + iv NO2 + O2
Reaction with Sulphuric Acid
Magnesium nitrate and sulphuric acid react to class nitric acid and magnesium sulphate. The chemical equation tin can be represented every bit follows:
HtwoSo4 +Mg(NO3)2→ MgSOfour +2 HNO3
Magnesium Nitrate Uses
Magnesium nitrate finds usage in various industries, including
- It is used as a desensitiser for lithographic plates.
- Information technology is used as a dehydrating agent in the preparation of concentrated nitric acrid and its purification.
- In the manufacturing of petrochemicals
- In manufacturing ammonium nitrate.
- As a viscosity adjuster in various industries
- In the manufacturing of agricultural products
- In the mining procedure
- It is used in making toner and colourant products.
- Magnesium nitrate can also exist used as a binding agent.
Benefits of Using Magnesium Nitrate Fertilisers
Magnesium nitrate fertilisers provide plants with readily-available macro food-magnesium. The master benefits of using magnesium nitrate are as follows:
- It is essential for the healthy growth of plants.
- It too facilitates the uptake of magnesium by the plant.
- Lack of proper magnesium leads to necrosis in plants.
- It enriches establish nutrition and provides them with vitality.
- Since magnesium is the central cantlet in a chlorophyll molecule, its deficiency causes a shortage of chlorophyll and thus stunted plant growth. Conversely, a sufficient magnesium supply augments growth.
Wellness Hazards of Magnesium Nitrate
The seriousness of the bear upon of magnesium nitrate depends on the exposure level. Less exposure to magnesium nitrate can lead to the following weather:
- Mild irritation in the mucous membranes
- Shortness of breath
- Coughing
Exposure to large quantities of magnesium nitrate tin can atomic number 82 to:
- Dizziness
- Vomiting
- Weakness
- Collapse
- Abdominal pain
- Encarmine diarrhoea
- Convulsions
When magnesium nitrate comes into contact with the skin, it causes:
- Redness
- Irritation
- Hurting
In addition to its impact on humans, the compound can be dangerous if handled carelessly. It can effect in violent combustion when in contact with oxidisable compounds. Also, one should be careful when heating this compound every bit it decomposes to emit toxic fumes of nitrogen oxides.
Decision
We at present know that magnesium nitrate is an inorganic chemical chemical compound with the chemical formula Mg(NO3)2. It is hygroscopic in nature and usually occurs equally a white crystalline solid at room temperature. Magnesium nitrate is an ionic compound. You can easily obtain magnesium nitrate by reacting nitric acid with magnesium salts. It finds its application in textiles, mining, agriculture and several other industries. However, one must exist careful while handling magnesium nitrate every bit information technology serves as an irritant.
Frequently Asked Questions
1. What is the employ of magnesium nitrate in nitric acid production?
A. Magnesium nitrate is used in the industry of concentrated nitric acrid as it extracts water and provides concentrated acid vapours upwards to 90–95 per cent.
2. Is magnesium nitrate acidic?
A. Magnesium nitrate is a crystalline solid, but it is highly hygroscopic. It has a pH of about five-7 and is thus acidic in nature.
3. What metal will react with magnesium nitrate?
A. Magnesium nitrate does non react with zinc, lead, and copper because magnesium is higher than these in the reactivity series, i.e., it is more reactive than other metals. And then, these metals cannot readapt magnesium ions from the solution.
4. Is magnesium nitrate good for you?
A. No, magnesium nitrate is harmful if ingested or inhaled. Information technology can cause skin irritation also every bit allergic reactions in the eyes and the respiratory tract. It irritates or burns the respiratory tract depending on the level of exposure. The person experiences coughing and shortness of jiff.
v. How can you obtain magnesium nitrate crystals?
A. Although magnesium nitrate is hygroscopic, you tin can obtain its crystals by drying it. Y'all will have to estrus it gently in a h2o bath. Cool the full-bodied solution to obtain crystals. The heating procedure has to be slow; else, magnesium nitrate would decompose and give magnesium oxide, nitrogen oxides, and oxygen.
Molar Mass Of Magnesium Nitrate,
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