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