Calcium chloride

Calcium chloride is an ionic compound with formula CaCl₂, consisting of calcium ions and chloride ions. It readily absorbs water and releases heat as it dissolves.

Hygroscopy: The tendency of a substance to absorb water vapor from its surroundings. Calcium chloride absorbs atmospheric moisture, making it useful as a desiccant and dust suppressant.
Road salt: Salt spread on roads to lower ice’s freezing point and improve winter traction. Calcium chloride can melt ice at lower temperatures than sodium chloride, though it costs more.
Calcium: A reactive alkaline-earth metal with atomic number 20, common in minerals and living organisms. Calcium atoms form the doubly charged cations in calcium chloride.
Brine: Water containing a high concentration of dissolved salts. Calcium chloride occurs in natural brines and is also produced as a concentrated brine.
Sodium chloride: An ionic compound with formula NaCl, commonly known as table salt or rock salt. It is the cheaper common road de-icer, but works less effectively at lower temperatures.
Deliquescence: The absorption of enough atmospheric moisture for a solid to dissolve into the resulting liquid. Under humid conditions, calcium chloride can take up enough water to form a liquid brine.
Desiccant: A material used to remove moisture from air or other substances. Anhydrous calcium chloride binds water and is used to dry gases and enclosed spaces.
Chloride: The negatively charged ion Cl⁻, formed when a chlorine atom gains an electron. Each formula unit contains two chloride ions for every calcium ion.
Evaporite: A sedimentary deposit formed when dissolved minerals precipitate as water evaporates. Calcium chloride can occur in saline deposits and ancient evaporite-related brines.
Magnesium chloride: An ionic compound with formula MgCl₂, used in de-icing and dust control. It shares moisture-attracting uses with calcium chloride but differs in cost and solution behavior.

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