Calcium Carbonate shares the typical properties of other carbonates. Notably:
- it reacts with strong acids, releasing carbon dioxide:
CaCO3(s) + 2HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l) - it releases carbon dioxide on heating (to above 840 °C in the case of CaCO3), to form calcium oxide, commonly called quicklime, with reaction enthalpy 178 kJ / mole:
CaCO3 → CaO + CO2
Calcium carbonate will react with water that is saturated with carbon dioxide to form the soluble calcium bicarbonate.
- CaCO3 + CO2 + H2O → Ca(HCO3)2
This reaction is important in the erosion of carbonate rocks, forming caverns, and leads to hard water in many regions.
Calcium Carbonate, as it is used for industrial purposes, is extracted by mining or quarrying. Pure calcium carbonate can be produced from marble, or it can be prepared by passing carbon dioxide into a solution of calcium hydroxide. In the latter case calcium carbonate is derived from the mixture, forming a grade of product called “precipitated calcium carbonate,” or PCC. PCC has a very fine and controlled particle size, on the order of 2 microns in diameter, particularly useful in production of paper. The other primary type of industrial product is “ground calcium carbonate,” or GCC. GCC, as the name implies, involves crushing and processing limestone to create a powdery-like form graded by size and other properties for many different industrial and pharmaceutical applications.
A study of Calcium Carbonate provides important lessons about the history of the earth, since chalk, limestone and marble trace their origin to shallow water. Thus, observation that large amounts of chalk deposits of the same age are found on many continents led to the discovery that there existed a period in which there was shallow water world-wide where shelled organisms thrived. Some offer this as proof for the Biblical flood. Nature returns the favor as calcium carbonate solutions from current deposits provide living organisms today with the material they need to grow their protective shells and skeletons. Eggshells, for example, are composed of approximately 95% calcium carbonate.
Calcium carbonate causes a unique reaction with acids. Upon contact with an acid - no matter the strength - it produces carbon dioxide. This provides geologists with a reliable test to identify calcium carbonate. This same phenomenon is important to the formation of caves. Acidic rain water runs off and goes underground where it dissolves the calcium carbonate limestone. The calcium carbonate water runs down and eventually reaches an air-filled cavity underground where the carbon dioxide can be released. When it is released, the calcium carbonate crystallizes again. Stalactite and stalagmite formations are created when water containing calcium carbonate drips, leaving some mineral at the source of the drip at the roof of the cave and some where it falls. This is an extremely long process, and often takes place over many thousands of years.
As interesting as calcium carbonate may be in nature, its impact and value to our everyday life are truly extraordinary.
Paper, Plastics, Paints, and Coatings: Calcium carbonate is the most widely used mineral in the paper, plastics, paints and coatings industries both as a filler – and due to its special white color - as a coating pigment. In the paper industry it is valued worldwide for its high brightness and light scattering characteristics, and is used as an inexpensive filler to make bright opaque paper. Filler is used at the wet-end of paper making machines, and calcium carbonate filler allows for the paper to be bright and smooth. As an extender, calcium carbonate can represent as much as 30% by weight in paints. Calcium carbonate also is used widely as a filler in adhesives, and sealants.
Personal Health and Food Production: Calcium carbonate is used widely as an effective dietary calcium supplement, antacid, phosphate binder, or base material for medicinal tablets. It also is found on many grocery store shelves in products such as baking powder, toothpaste, dry-mix dessert mixes, dough, and wine. Calcium carbonate is the active ingredient in agricultural lime, and is used in animal feed. Calcium Carbonate also benefits the environment through water and waste treatment.
Building Materials and Construction: Calcium carbonate is critical to the construction industry, both as a building material in its own right (e.g. marble), and as an ingredient of cement. It contributes to the making of mortar used in bonding bricks, concrete blocks, stones, roofing shingles, rubber compounds, and tiles. Calcium carbonate decomposes to form carbon dioxide and lime, an important material in making steel, glass, and paper. Because of its antacid properties, Calcium Carbonate is used in industrial settings to neutralise acidic conditions in both soil and water.
Calcium carbonate crystals are referred to as calcite. The calcite crystal generally is considered a rhombohedron because of its cleavage properties. Cleavage is what causes crystals to angle where the bonding forces are weak and are apt to break into planes. Calcite is unique in that its cleavage takes three distinct directions. There are more than 300 forms of calcite crystals. Calcite crystals also come in many different colors, but usually are white or transparent. Another important property of the calcite crystal is its property of double refraction. Double refraction occurs when a ray of light travels through a medium and is spilt into two different beams, one traveling slowly, one traveling fast. The two different beams are bent at two different angles of refraction. As a result of this property a person looking through calcite sees two images. This property of double refraction is a feature valuable to a number of optical applications.
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