Zinc Nitrate Formula

Explain Zinc Nitrate Formula

The zinc Nitrate formula is also called either the Zinc di-nitrate formula or the Celloxan formula. This particular inorganic compound is composed of two nitrogen atoms, six oxygen atoms, and one zinc atom. The molecular or chemical formula of Zinc Nitrate is given as Zn(NO\[_{3}\])\[_{2}\]. This is also called zinc nitrate hexahydrate chemical formula.

Often, it appears as colorless to a withe crystalline solid. It is highly deliquescent and dissolves in water and alcohol. It may be synthesized by mixing zinc in nitric acid and is naturally found as hexahydrate. It can be widely used as a catalyst in the manufacturing of dyes, chemicals, and medicines.

Zinc Nitrate Formula Structure

[Image will be Uploaded Soon]

Properties of Zinc Nitrate Formula

Zinc nitrate Chemical formula or molecular formula of zinc nitrate



2.065 g/cm\[^{3}\] (hexahydrate)

Zinc nitrate molecular weight

189.36 g/mol (anhydrous)

297.49 g/mol (hexahydrate)

Melting point

110 °C (anhydrous)

45.5 °C (trihydrate)

36.4 °C (hexahydrate)

Boiling point

Approx 125 °C (hexahydrate)

Symbol of zinc nitrate or zinc nitrate hexahydrate formula


Zn(NO\[_{3}\])\[_{2}\] is given as a non-combustible compound, but it holds the ability to enhance the burning of combustible compounds. Inhaling this specific inorganic chemical can lead to severe coughing and sore throat. When it comes in contact with eyes and skin, it causes redness and also pain. Ingesting this compound leads to abdominal pain, nausea, and more.


Zinc nitrate has no large-scale application, but it can be used on a laboratory scale for the coordination polymer synthesis. Also, its controlled decomposition to the zinc oxide has been used for the generation of different ZnO-based structures, including nanowires.

It may be used as a mordant in the process of dyeing. An example reaction that gives a precipitate of zinc carbonate:

Zn(NO\[_{3}\])\[_{2}\] + Na\[_{2}\]CO\[_{3}\] → ZnCO\[_{3}\] + 2 NaNO\[_{3}\]

Health Hazards

Inhaling dust causes irritation in the nose and throat. Swallowing the Zinc di-nitrate compound can lead to alimentary tract corrosion. Contact with skin can cause rashes and results in irritation.

It may liberate toxic oxides of nitrogen when heated. When it comes in contact with the combustible material, it may increase the fire intensity.

Book your Free Demo session
Get a flavour of LIVE classes here at Vedantu
FAQs (Frequently Asked Questions)

1. Is Zinc Nitrate Acidic or Basic?

Answer: Hydroxide anions that are coming from water may liberate the nitrate anions when the zinc nitrate is kept in an aqueous solution. We should remember that HNO3 does not look like a molecule. The specific reaction results in the formation of hydronium ions and that is why the solution may be considered acidic.

2. What is Zinc Nitrate Used For?

Answer: Zinc nitrate does not hold a broad scale use, but it can be used for the synthesis of coordinating polymers on a laboratory scale. Also, the controlled decomposition of the zinc oxide may be used for the generation of multiple structures, including nanowires. In addition, it can be used as a dyeing mordant.

3. Does Nitric Acid React With Zinc?

Answer: Zinc and Aluminum do not react with the concentrated nitric acid because of the formation of a dense, hard to dissolve oxidation layer because of the process called passive oxidation. This protects the metal against further corrosion and reaction. Nevertheless, zinc does react with dilute nitric acid.

4. Give the Reason Why Zinc Nitrate Decreases When Heated?

Answer: On heating, zinc Nitrate gives off Nitrogen Dioxide gas (with the chemical formula NO2) that has characteristic reddish-brown fumes. Also, a solid residue is left behind whose color is very interesting. It is Zinc Oxide (ZnO). I say it is interesting because its color turns white when cold and yellow when hot. Also, oxygen is released as a by-product.

Since from the solid reactant we are getting a solid and two gaseous products as well, the solid residue (Zinc Oxide) would obviously weigh below the original reactant (Zinc Nitrate).