Chemistry Formulas

Copper (II) Nitrate Formula

Copper (II) Nitrate is also referred to as Cupric Nitrate. Further, it is an inorganic salt which is commonly recognized for the brilliant blue colour it has. Moreover, it is used in the form of a catalyst in various reactions. Let us study further about the Copper (II) Nitrate Formula in detail below.

Formula and Structure

The chemical formula for Copper (II) Nitrate is Cu (NO3)2. Similarly, the structure for this anhydrous salt is formed by 1 cation Cu2+ and 2 anions NO3. The compound shows up to 5 different hydrate forms. The trihydrated being Cu (NO3)2 and the pentahydrated being Cu (NO 3)2. 5H2O salts are the most common.

Similarly, the molar mass of this anhydrous form is 187.55 g mol-1 and the trihydrate form is 241.60 g mol-1. In order to write the chemical structure, follow the diagram below, in the common representations used for organic molecules.

Copper (II) Nitrate Formula

Occurrence

Copper (II) nitrates, as well as other copper nitrates, occur naturally in nature. Moreover, you can find them as parts of some minerals like gerhardtite and rouaite.

Preparation

Copper (II) nitrate can be prepared from metallic copper treated with nitric acid. In addition, one can also produce it by treating metallic copper with dinitrogen tetroxide:

Cu + 4 HNO3 → Cu(NO3)2 + 2 H2O + 2 NO2

Cu + 2 N2O4 → Cu(NO3)2 + 2 NO

Physical Properties

In all the hydrated forms, Copper (II) nitrate exists in blue colour and is hygroscopic, crystalline solid. The density of Copper (II) nitrate varies as per the hydration of it. The density is 3.05 g mL-1 (anhydrous), 2.32 g mL-1 (trihydrate) or 2.07 g mL-1 (hexahydrate).

Similarly, if we talk about its melting point, the anhydrous has a melting point of 256°C and for trihydrate is 114.5 °C whereas 26.5 °C is for hexahydrate. Most of it decomposes at high temperatures. Further, the 3 forms are extremely soluble in water, ethanol, and ammonia. On the other hand, they are insoluble in organic solvents like ethyl acetate.

Chemical Properties

In chemical synthesis, Copper (II) nitrate suffers several interesting reactions.  One of these reactions is the preparation of cupric oxide by pyrolysis above 180 °C:

2 Cu(NO3)2 → 2 CuO + 4 NO2 + O2

Copper (II) nitrate can react with acetic anhydride to encourage the nitration of aromatic compounds like benzene.

Uses

Copper (II) nitrate has many uses. One can use it to produce pyrotechnic and blue colours as well as coats. Moreover, it is also used as a classical demonstration of the voltaic cell because of the redox reaction between the copper (II) nitrate and one copper electrode. Similarly, Copper (II) nitrate is also used to produce copper (II) oxide.

Safety Hazards

Copper (II) nitrate is injurious to health. It is responsible for causing irritation in the throat, lungs, eyes and skin. It is non-combustible, however, when you combine it with wood, paper and other combustibles, it may burn.

Solved Question for You

Question- Copper (II) nitrate is used in the production of which of the following?

a) Carbon Disulfide

b) Copper (II) oxide.

c) Chromic Acid

d) Cyanide

Answer- The correct answer is option B. It is used to produce Copper (II) oxide.

Share with friends

Customize your course in 30 seconds

Which class are you in?
5th
6th
7th
8th
9th
10th
11th
12th
Get ready for all-new Live Classes!
Now learn Live with India's best teachers. Join courses with the best schedule and enjoy fun and interactive classes.
tutor
tutor
Ashhar Firdausi
IIT Roorkee
Biology
tutor
tutor
Dr. Nazma Shaik
VTU
Chemistry
tutor
tutor
Gaurav Tiwari
APJAKTU
Physics
Get Started

Leave a Reply

avatar
  Subscribe  
Notify of

Customize your course in 30 seconds

Which class are you in?
No thanks.