Published May 2015
Calcium chloride (CaCl2) is a salt, appearing as a white crystal. It is commercially available as anhydrous and dihydrate flakes, pellets, and powder, or as a 30–45% solution. Calcium chloride is produced by refining naturally occurring brine, by neutralizing hydrochloric acid with limestone, or as a by-product from the Solvay process of synthetic sodium carbonate (soda ash) production. The major applications for calcium chloride include road deicing, dust control, and oil extraction and completion fluids.
The following pie chart shows world consumption of calcium carbide:
Total consumption of calcium chloride is expected to increase at about 3% per year in 2014–19, mostly because of expected increases in the oil recovery segment, as well as increasing use in dust control and other industrial applications, particularly in Asia. Deicing is the largest consumption end use, but a forecast is only reasonable as an average of several years, since winter conditions and consumption of calcium chloride can vary significantly from one year to the next. In the winter of 2014/2015, North America had an unusually strong snowfall, whereas Europe had a rather low snowfall. With consumption being much larger in North America than in Europe, consumption in deicing reached a high level in 2014, but further large increases in consumption for the coming years are not expected.
Use of calcium chloride in dust control is expected to grow, not only from its increasing use on unpaved roads and in mining operations, but also from increased use in urban areas, to bind fine dust and maintain levels below the maximum tolerated for fine dust under critical conditions.