|Systematic name||Calcium chloride|
|Other names|| calcium(II) chloride|
calcium dichloride, E509
|Molecular formula|| CaCl2|
|Molar mass|| Molar mass::110.99 g/mol, anhydrous |
Molar mass::147.02 g/mol, dihydrate
Molar mass::182.04 g/mol, tetrahydrate
Molar mass::219.08 g/mol, hexahydrate
|Appearance||white or colorless solid|
|CAS number||CAS number::10043-52-4|
|Density and phase|| [[Density::2.15 g/cm3]], anhydrous|
[[Density::0.835 g/cm3]], dihydrate
[[Density::1.71 g/cm3]], hexahydrate
|Solubility in water||74.5 g/100 ml (20°C)|
|Melting point||Melting point::772°C (anhydrous)|
|Boiling point||Boiling point::1600°C|
|Crystal structure||deformed rutile|
|Flash point||Not considered to be flammable|
|Other anions|| calcium fluoride|
|Other cations|| magnesium chloride|
| Except where noted otherwise, data are given for|
materials in their standard state (at 25 °C, 100 kPa)
Disclaimer and references
Calcium chloride is an ionic compound of calcium and chlorine forming a structure held together by ionic bonds. This compound is easy to dissolve in water and it is deliquescent, that is, it absorbs so much humidity from the air that it actually dissolves and becomes a solution on exposure to humid air. If kept in a sealed container, it remains a solid at room temperature. It also behaves as a typical ionic halide like many salts do. It is used for common things for our environment; such as brine for refrigeration plants, ice and dust control on roads, and in cement. It can be produced directly from limestone, but large amounts are also produced as a by-product of the Solvay process. Because of its hygroscopic nature, it must be kept in tightly-sealed containers.
Calcium chloride (CaCl2), in solution is hygroscopic (it attracts water) and is also exothermic, that is, as it absorbs water it gives off heat. It is dangerous, not because it is poisonous, but because it can heat a small amount of water quickly so that it will burn skin or mouth parts, and possibly start fires.
Since it draws in moisture from its surroundings, resists evaporation, and can release heat; it is considered helpful for road construction and maintenance. It can melt ice by heat, control dust by remaining liquid, and stabilize the base soil by keeping it from drying out.
Calcium Chloride is very popular chemical and it is used in many common ways. Ward Chemical  is one producer that uses a naturally occurring brine that is high in Calcium Chloride to produce liquid products.
Calcium chloride is often found as a powder in boxes that absorb humidity from the air, and in mixtures of salt used to melt ice from sidewalks. It also lowers the freezing point of water and is used to melt ice and snow in the same way as common salt.
It is also used in the production of calcium salts, cold-weather concrete additives, soil solidification and shoulder and base stabilization. It is used for tractor tire weighting, direct drying compounds, and dust proofing and making ores and coal freeze-resistant. It can increase the web strength of corrugating media, and improve dye retention. It is used as an additive to oil well completion fluids, cementing finished oil wells, drilling mud additives and in drying petroleum fractions.* 
Here is a list of Calcium Chloride uses mentioned by Ward Chemical;
-Base stabilization for road construction
-Freeze-proofing sand for winter road application
-Sewage purification aid, as a flocculent and for removal of phosphates and fluorides
-Grouting agent for mines and oil wells
-Environmental additive for cement kilns
-Nitrogen inhibitor for plant fertilizers
-Salt substitute in animal feed (as a supplement or for calcium deficiency)
-Organic calcium fertilizer
-Liquid odor control
-Soil pH adjuster
-Antifreeze for recreation vehicles, curling & skating rinks and more...
- calcium chlorideMultiple authors. Peter's Chemical Company
- Calcium chloride Multiple authors. Wikipedia.
- calcium chloride Multiple authors. Columbia Encyclopedia, Answers.com
- Calcium Chloride Multiple authors. Ward Chemical