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Calcium oxide has been known since the beginning of time. In 184 BC, the Roman writer Cato the Elder (234 – 149 BC) documented one technique of producing the combination. Many Europeans were employing calcium oxide (commonly known as lime) in the construction of structures by the early fifteenth century. Some of the earliest scientific studies of calcium oxide were conducted by the Scottish chemist Joseph Black (1728–1799). When the chemical is exposed to air, it reacts with carbon dioxide to form calcium carbonate.
Calcium Oxide
Calcium oxide is a chemical substance with colourless and odourless qualities that has been used since ancient times. CaO is the chemical formula for calcium oxide. It is an amorphous substance in the shape of a crystalline or powdered solid. Calcium oxide is also referred to as fast lime, caustic lime, and burnt lime. Calcium oxide is white or off-white in its pure form. In the presence of impurities such as iron, magnesia, silica, or alumina, it turns yellow or brownish. Calcium oxide can also be found in reds and subdued browns.
Calcium and oxygen are the two major ingredients that make up calcium oxide.
It is made by heating calcium carbonate (e.g., limestone) to 500°C to 600°C in a special lime kiln and decomposing it into oxide and carbon dioxide.
Calcification is the process of obtaining charred lime. It begins by degrading the natural components at high temperatures while ensuring that they do not approach the melting point. This is accomplished by heating them to temperatures ranging from 1070 to 1270 degrees Celsius.
CaO + CO2 → CaCO3
Calcium oxide is used in the production of porcelain and glass. It is also employed in the purification of sugar, the production of bleaching powder, calcium carbide, and calcium cyanamide. It is also used in water softeners, mortars, and cement.
Calcium oxide (CaO), sometimes known as quicklime or burnt lime, is a chemical substance that is widely used. At room temperature, it is solid. The term lime refers to calcium-containing inorganic compounds that contain oxides and hydroxides of calcium, magnesium, aluminium, silicon, and iron. Quicklime, on the other hand, refers to the single chemical molecule calcium oxide. However, contaminants are frequently found in commercial lime.
Calcium oxide is also commonly used in pharmaceuticals and pesticides. Calcium oxide is an important element in the production of caustic soda since alkali is readily available. It is also utilised in the production of steel, paper, and cement.
Health Benefits of Calcium in the Human Body
Calcium is mostly required for the formation of strong bones and the maintenance of good oral health. The bones and teeth contain 99 percent of the calcium in the body. It is required for the body’s growth, development, and maintenance. Calcium also aids in the maintenance of blood activity and the smooth flow of blood throughout the body.
The availability of enough calcium in the body results in lower blood pressure, more energy, and effective skin and bone renewal. It also aids in muscular contraction and cholesterol function.
Interesting Facts of Calcium Oxide
1.Calcium oxide is widely used to “lime” acidified lake waters; it reacts with them and neutralises acids in the lake. It is also generated when nitric and sulfuric acid in acid rain is brought to earth by rain, sleet, snow, and other precipitation processes.
2.Calcium oxide emits a bright white light when heated towards its melting point. Prior to the discovery of electricity for lighting, notably in the second half of the nineteenth century, heated lime was used to provide the strong lights required to illuminate theatrical shows.
3.Quicklime has traditionally been used in the funerals of ill animals and humans because it was supposed to accelerate the disintegration of soft tissue. For example, in 1666, the bodies of plague victims in London were commanded to be buried in quicklime.
Health Danger
Calcium oxide can cause harm to the skin, nose, eyes, and respiratory system if it comes into contact with it. People who use the product at work or at home for (gardening reasons), for example, must be exceedingly cautious not to breathe in, consume, or otherwise come into touch with the chemical. If such contact happens, it should be thoroughly rinsed away with water and medical attention should be sought.
Conclusion
This is all about the properties of calcium oxide. The high solubility of calcium oxide makes the production of phosphate-based cements challenging. Calcium oxide, on the other hand, can be transformed to less soluble compounds such as silicates, aluminates, or even hydrophosphates, which can then be employed in an acid-base reaction with phosphate.
