Ammonium Nitrite Formula

The ammonium nitrite is a chemical compound that is also known as Ammoniumnitrit or Azanium nitrite. It is highly unstable in nature hence we do not use it in its purest form. Moreover, when it is at room temperature, it decomposes to nitrogen and the water (H₂O). The ammonium nitrite forms naturally in the air and we can synthesize it by the process of absorption of the equal parts of nitric oxide and the nitrogen dioxide in liquid ammonia. In addition, we can also obtain it by the oxidation of ammonia with hydrogen peroxide or ozone.  The Ammonium Nitrite Formula helps you understand this better.

However, it can also be produced by precipitating the lead nitrite or barium with the ammonium sulfate as well, or potassium nitrite with the ammonium perchlorate, or ammonium chloride with the involvement of silver nitrite. The precipitate that we get as a result is filtered. The crystals we get are colourless and soluble in the water.

Formula and Structure

The molecular formula or the chemical formula for the chemical compound ammonium nitrite is NH₄NO₂. The chemical structure of the ammonium nitrite is present below in the form of an image that is in the common representations that we basically use for the organic molecules.

Preparation

The chemical compound Ammonium nitrite occurs naturally in the air. It can be synthesized by oxidizing ammonia with ozone or hydrogen peroxide as well. It forms crystals which are soluble in water and has no color.

Physical and Chemical Properties

The ammonium nitrite can explode at a temperature of 60 to 70 °C, and it will decompose faster when we dissolve it in a concentrated aqueous solution than in the form of a dry crystal. However, even in the room temperature, this compound decomposes into water and nitrogen.

NH₄NO₂ → N₂ + 2H₂0

It decomposes when we provide heat to it or also in the presence of acid into water and nitrogen. Ammonium nitrite solution is stable at higher pH levels and lower temperature levels. If there is any decrease in the pH level that is lower than 7.0, it may result in an explosion, since the nitrite can react to it. Moreover, we can maintain a safe pH level by adding an ammonia solution into it. The mole ratio of ammonium nitrite to ammonia should be more than 10 percent.

Uses

The ammonium nitrite is useful as a micro biocide, rodenticide, and agricultural pesticides as well. Moreover, we can also use it for the synthesis of nitrogen gas and ammonium cobalt-nitrite. However, it is most commonly useful while making the explosives.

Safety Hazards

The chemical compound ammonium nitrite is highly toxic to the humans and aquatic animals at the same time. It can cause a heavy explosion hazard if we use it carelessly. If we will be providing heat to the ammonium nitrite it will be able to produce toxic fumes of the ammonia and the nitrogen oxides at the same time.

Solved Example for You

Question: The ammonium nitrite (NH₄NO₂) decomposes when we heat it for producing nitrogen gas and water vapors. What is the total volume of gases formed when 32.0 g ammonium nitrite decomposes completely at 350 degrees Celsius and a pressure of 1.00 atm?

Solution:

NH₄NO₂ → N₂ + 2H₂O.

Moles of ammonium nitrite = 0.5.

As per the stoichiometry,

0.5 moles of ammonium nitrite produces 0.5 moles of nitrogen gas and 1 mole of water vapor.

Thus, total moles of the products = 0.5 + 1 = 1.5.

As per the ideal gas law,

PV = nRT.

Thus, V = nRT/P.

Or, V = 76.63 L.

Thus, total volume = 76.63 L.