Cobalt Nitrate II is the inorganic compound. It is a pale red powder colour crystalline compound. It’s an odourless chemical that sinks and mixes with water. And it may be a nitrate salt during which the metal cobalt is in +2 oxidation number and therefore the anion is nitrate. During this chapter, we will discuss the cobalt nitrate II formula, its properties, and its applications.
Cobalt Nitrate II Formula
The most common sort of it is that the hexahydrate Co(NO3)2·6H2O. It may be a red-brown deliquescent salt and soluble in water and other polar solvents. Anhydrous cobalt(II) nitrate forms a three-dimensional polymeric network structure. In which each cobalt(II) atom approximately octahedrally coordinated by six oxygen atoms, each from a special nitrate ion.
- Molecular Formula = Co(NO3)2
- IUPAC name = Cobalt(II) nitrate hexahydrate
- The Simplified molecular-input line-entry system (SMILES) =[N+](=O)([O-][O].[N+](=O)([O-])[O-].[Co+2]
Each nitrate ion coordinates to 3 cobalt. The dihydrate may be a two-dimensional polymer, with nitrate bridges between Co(II) centres and hydrogen bonding holding the layers together. The tetrahydrate consists of discrete, octahedral [(H2O)4Co(NO3)2] molecules.
The hexahydrate is analogous as hexaaquacobalt(II) nitrate, [Co(OH2)6][NO3]2 because it consists of discrete [Co(OH2)6]2+ and [NO3]− ions. It is usually reduced to metallic high purity cobalt. And it is often absorbed into varied catalyst supports to be used in Fischer-Tropsch catalysis. It is utilized in the preparation of dyes and ink
Production of Cobalt Nitrate II
Preparation of Cobalt Nitrate II (hexahydrate) includes treating metallic cobalt or one among its oxide. It also includes hydroxides or carbonate with aqua fortis. The subsequent reactions occur to offer Cobalt Nitrate II.
Co + 4HNO3 + 4H2O → Co(H2O)6(NO3)2 + 2NO2
CoO + 2HNO3 + 5H2O → Co(H2O)6(NO3)2
CoCO3 + 2 NO3 + 5H2O → Co(H2O)6(NO3)2 + CO2
Another method is putting metal cobalt into a pressure-resistant and anti-nitric acid corrosion container. And introducing industrial pure oxygen to perform dissolving reaction of metal cobalt with the reaction temperature between 20° C and 100° C.
The reaction pressure between 0.05MPa and 0.5MPa and therefore the aqua fortis concentration for the reaction between 1mol/L and 14mol/L. The quantity of cobalt for the reaction is larger than the quantity calculated by the chemical equation. And, therefore, the reaction lasts for 1 to 10 hours.
3 dissolution process occurs as a reaction of metallic cobalt;
Co + 4HNO3 → Co (NO3) 2 + 2NO2 + 2H2O
3Co + 8 hops → 3Co (NO3) 2 + 2NO + 4H2O
3NO2 + H2O → 2 + NO hop overall reaction is:
2Co + 4HNO3 + 02 → 2Co (NO3) 2 + 2H2O
Solved Examples for Cobalt Nitrate II Formula
Q1] How Ligand Exchange of hexaaquacobalt(II) ions with hydroxide ions occur?
Solution: Hydroxide ions remove hydrogen ions from the water ligands attached to the cobalt ion. Once a proton has been faraway from two of the water molecules, you’re left with a complex with no charge – a neutral complex. this is often insoluble in water and a precipitate is made.
Co(H2O)62+ + 2OH- → [Co(H2O)4(OH)2] + 2H2O
Q 2] How Ligand Exchange of hexaaquacobalt(II) ions with ammonia solution occurs?
Solution: The ammonia acts as both a base and a ligand. However, with the little amount of ammonia, hydrogen ions are achieved. The hexaaqua ion exactly as within the hydroxyl ion case to offer an equivalent neutral complex.
[Co(H2O)6]2+ + 2NH3 → [Co(H2O)4(OH)2] + 2NH4
That precipitate dissolves if you add a more than ammonia. The ammonia replaces water as a ligand to provide hexaamminecobalt(II) ions.
[Co(H2O)6]2+ + 6NH3 → [Co(NH3)6]2+ + 6H2O