Cobalt II Carbonate Formula

Cobalt (II) carbonate is an inorganic compound that is also known as cobaltous carbonate. It is a reddish paramagnetic solid whose chemical or molecular formula is CoCO₃. Its molecular weight is 118.941 g/mol and it has a density of 4.13 g/cm³. It is an intermediate in obtaining cobalt from their ores by hydrometallurgical purification. Spherocobaltite or sphaerocobaltite is a cobalt carbonate mineral that exists in a rose-red colour in its rare pure form, while its impure specimens exist in shades of pink to pale brown. Cobalt (II) carbonate hexahydrate on heating becomes anhydrous by 140 °C while the anhydrous cobalt (II) carbonate decomposes at 427 °C before melting into cobalt (II) oxide. It is soluble in acids and liquid ammonia, almost insoluble in alcohol, methyl acetate, water, and decomposes in hot water, and is insoluble in ethanol. It is used in the preparation of cobalt compounds, ceramics, pigments, fertilizers, and catalysts.

Structure of Cobalt II Carbonate

The molecular formula of cobalt II carbonate is CoCO₃, and its canonical SMILES is C(=O)([O-])[O-].[Co⁺²]. The crystal structure of cobalt II carbonate (anhydrous) is rhombohedral, and cobalt II carbonate hexahydrate is trigonal.

Structure of Cobalt II Carbonate

Preparation of Cobalt II Carbonate

• Cobalt II carbonate can be prepared by combining solutions of cobaltous sulfate and sodium bicarbonate. The below reaction is used in the precipitation of cobalt from an extract of its roasted ores.

CoSO4 + 2NaHCO₃ → CoCO₃ + Na₂SO₄ + H₂O + CO₂

• It can also be prepared by heating a solution of a cobaltous salt with sodium carbonate. For example, cobalt (II) nitrate reacts with sodium carbonate to form Cobalt (II) carbonate and sodium nitrate.

Na₂CO₃ + Co(NO₃)₂ → CoCO₃ + 2NaNO₃

Physical Properties of Cobalt II Carbonate

Chemical formula	CoCO3
IUPAC Name	Cobalt (II) carbonate
Molar mass	118.941 g/mol
Appearance	Red-pink solid
Structure	Rhombohedral crystals
Melting point	427 °C
Density	4.13 g/cm3
Solubility	Soluble in acids and liquid ammonia, almost insoluble in water, alcohol, methyl acetate, and Insoluble in ethanol
Refractive index	1.855

Chemical Properties of Cobalt II Carbonate

• Cobalt III Carbonate (Co₂(CO₃)₃) is formed when cobalt II carbonate is oxidized by air on weak oxidizing agents.
• Cobalt (II) carbonate and hydrochloric acid react in an aqueous solution to form Cobalt chloride.

CoCO₃ + 2HCl(aq) → CoCl₂(aq) + CO₂ + H₂O

• Cobalt chloride hexahydrate can be prepared from the reaction of cobalt II carbonate and hydrochloric acid in an aqueous solution. 

CoCO₃ + 2HCl + 5H₂O → [Co(H₂O)₆]Cl₂ + CO₂

• When cobalt (II) carbonate and acetylacetone (C₅H₈O₂) react in the presence of hydrogen peroxide, tris(acetylacetonate)cobalt(III) [Co(C₅H₇O₂)3] is produced.

 2CoCO₃ + H₂O₂ + 15C₅H₈O₂ → 2 Co(C₅H₇O₂)₃ + 2CO₂ + 4H₂O 

• When cobalt (II) carbonate is heated, it emits carbon dioxide and produces cobalt (IV) oxide, which converts reversibly to cobalt oxide (CoO) at high temperatures.

6CoCO₃ + O₂ → 2 Co₃O₄ + 6CO₂

Uses of Cobalt(II) carbonate

• Cobalt(II) carbonate is used in the preparation of various cobalt compounds.
• It is used in porcelain colouring, pigments, fertilizers, and catalysts.
• It is used as a temperature indicator and veterinary medication.
• As cobalt is an essential element, it is a component of dietary supplements.
• It is also used in animal feeds as cobalt carbonate aids in the production of vitamin B12 in ruminants such as cattle and sheep.

Hazards

• Cobalt(II) carbonate powder may irritate the skin, eye, and/or respiratory tract. 
• Prolonged contact may cause an allergic skin reaction. 
• It is harmful if swallowed and may cause allergy or asthma symptoms or breathing difficulties if inhaled. 

FAQs on Cobalt II Carbonate Formula

Question 1: What is cobalt(II) carbonate?

Answer:

Cobalt (II) carbonate is an inorganic compound that is also known as cobaltous carbonate. It is a reddish paramagnetic solid whose chemical or molecular formula is CoCO₃. Its molecular weight is 118.941 g/mol and it has a density of 4.13 g/cm³. It is an intermediate in obtaining cobalt from their ores by hydrometallurgical purification. Spherocobaltite or spherocobaltite is a cobalt carbonate mineral that exists in a rose-red color in its rare pure form, while its impure specimens exist in shades of pink to pale brown.

Question 2: Mention a preparation method for cobalt(II) carbonate.

Answer:

Cobalt II carbonate can be prepared by combining solutions of cobaltous sulfate and sodium bicarbonate. The below reaction is used in the precipitation of cobalt from an extract of its roasted ores.

CoSO₄ + 2NaHCO₃ → CoCO₃ + Na₂SO₄ + H₂O + CO₂

Question 3: What happens when cobalt(II) carbonate reacts with acetylacetone in the presence of hydrogen peroxide?

Answer:

When cobalt (II) carbonate and acetylacetone (C₅H₈O₂) react in the presence of hydrogen peroxide, tris(acetylacetonato)cobalt(III) [Co(C₅H₇O₂)₃] is produced.

2CoCO₃ + H₂O₂ + 15C₅H₈O₂ → 2 Co(C₅H₇O₂)₃ + 2CO₂ + 4H₂O 

Question 4: What are the uses of cobalt(II) carbonate?

Answer:

Cobalt(II) carbonate is used in the preparation of various cobalt compounds. It is used in porcelain coloring, pigments, fertilizers, and catalysts. It is used as a temperature indicator and veterinary medication. As cobalt is an essential element, it is a component of dietary supplements. It is also used in animal feeds as cobalt carbonate aids in the production of vitamin B12 in ruminants such as cattle and sheep.

Question 5: Mention some health hazards of cobalt(II) carbonate.

Answer:

Cobalt(II) carbonate powder may irritate the skin, eye, and/or respiratory tract. Prolonged contact may cause an allergic skin reaction. It is harmful if swallowed and may cause allergy or asthma symptoms or breathing difficulties if inhaled.

Question 6: How is cobalt chloride hexahydrate prepared from cobalt(II) carbonate?

Answer:

Cobalt chloride hexahydrate can be prepared from the reaction of cobalt II carbonate and hydrochloric acid in an aqueous solution.

CoCO₃ + 2HCl + 5H₂O → [Co(H₂O)₆]Cl₂ + CO₂