Lime, sometimes referred to as quicklime, is a term commonly applied to a number of related materials. Pure lime is calcium oxide (CaO) formed by “burning” a form of calcium carbonate such as limestone or marble (CaCO3). Carbon dioxide gas (CO2) is released and leaves lime behind. Dolomite, a calcium magnesium carbonate (CaMg(CO3)2) can also be calcined to form dolomitic lime, which has different reactivity due to the presence of MgO.
Lime can be mixed with water to form hydrated lime (Ca(OH)2), which some also call lime. To further muddy the waters, in agriculture adding lime to the soil is not done with true lime but with limestone.
Uses for Lime
Many applications for lime exploit the alkalinity that is created when the lime is formed. Lime is a strong base, so reacts with, and neutralizes, acids. In this capacity, it is used to treat wastewater, drinking water
Lime enjoys its most extensive use as a flux in purifying steel in
Lime is one of the world’s oldest components in
Finally, lime is widely used in the manufacture of precipitated calcium carbonate (PCC). Carbon dioxide gas is introduced into a lime slurry and CaCO3 is precipitated out of solution. Precipitated calcium carbonates are produced in large quantities
Specialty Minerals Lime Products
Specialty Minerals manufactures lime at its Adams, Massachusetts plant— both for internal use in precipitated calcium carbonate
Two types of lime are produced: metallurgical grade and chemical grade. The high-calcium metallurgical grade’s high reactivity and low impurity levels make it suitable for many steel desulfurization applications. The chemical grade quicklime is used in many industrial applications.