Copper II Carbonate is also referred to as Cupric Carbonate. Further, it is essentially a chemical compound. The Copper II Carbonate Formula is CuCO 3. Further, it is an ionic solid compound which consists of copper (II) cations Cu2+ and carbonate anions CO2− 3. It is not that easy to be found because it is quite difficult to prepare. Learn Copper II Carbonate Formula here.
Copper II Carbonate
Most commonly, the term of copper carbonate or cupric carbonate is referred to as a basic copper carbonate like Cu2(OH)2CO3. This occurs in nature in the form of the mineral malachite or Cu3(OH)2(CO3)2 which is azurite. It is because of this reason that the qualifier neutral can be utilized in place of basic which refers particularly to CuCO3.
It is generally expected of reactions like mixing solutions of Copper II sulfate CuSO 4 and sodium carbonate Na 2CO 3 in ambient conditions to produce CuCO 3, but instead, it produces a basic carbonate and CO2 because of the great attraction of the Cu2+ ion for the hydroxide anion HO−
When the basic carbonate thermally decomposes at atmospheric pressure, it produces Copper (II) oxide CuO instead of the carbonate.
W. F. T. Pistorius in the year, 1960, claimed synthesis. He did so when he heated basic copper carbonate at 180 °C in an atmosphere containing carbon dioxide, CO 2(450 atm) and water (50 atm) up to 36 hours. The majority of these products came out to be well-crystallized malachite Cu 2CO 3(OH)2, however, there was also a small quantity of the rhombohedral substance in the result which was claimed as CuCO 3. But, it is important to note that this synthesis was actually not reproduced.
If we look at the origin, we will see that the reliable synthesis of true Copper (II) carbonate was testified for the first time in 1973 by Hartmut Ehrhardt and others. Thus, this compound was acquired in the form of gray powder.
It was after they heated basic copper carbonate in an atmosphere containing carbon dioxide (which we produce by decomposing silver oxalate Ag 2C2O 4) at 500 °C and 2 GPa (20,000 atm). The compound was said to have a monoclinic structure.
Chemical Properties & Physical Properties
The stability of dry CuCO3 is dependent significantly on the partial pressure of carbon dioxide (pCO2). It can remain stable for months in dry air but will decompose slowly into CuO and CO2 if pCO2 is less than 0.11 atm.
In the company of water or moist air at 25 °C, CuCO3 is constant only for pCO2 above 4.57 atmospheres and pH between about 4 and 8. Further, below that partial pressure, it reacts with water to make a very basic carbonate (azurite, Cu3(CO3)2(OH)2).
3 CuCO3 + H2O → Cu3(CO3)2(OH)2 + CO2
In highly basic solutions, the complex anion Cu(CO3)22− is formed as an alternative.
Solved Example for You
Question- Which of the following is the colour of Copper II Carbonate?
Answer- The correct answer is option A. It is a grey ionic solid compound.