Calcium Chloride

Calcium chloride (chemical formula: CaCl2) is a white or yellowish solid inorganic compound, belonging to the salt class, is a typical ionic halide, because of its high solubility, moisture absorption and water removal and widely used in many fields. According to its hydrated form exists in different physical forms, the most common is dihydrate (CaCl2·2H2O), its high solubility allows it to dissolve quickly in water, releasing a large amount of heat, and is therefore very useful in applications requiring rapid heating or drying. In addition, calcium chloride is also commonly used in salt water, including road deicing agents and desiccant used in refrigeration equipment.

Colorless cubic crystal, white or off-white, granular, honeycomb block, spheroid, irregular granular, powdered. Slightly toxic, odorless, slightly bitter taste. It deliqueses easily when exposed to air. It is easily soluble in water, with a solubility of 74.0g /100 g water at 20 ° C, while releasing a large amount of heat (the dissolution enthalpy of calcium chloride is -176.2cal /g). This property makes it very useful in applications where rapid heat generation is required, such as as a heat source in certain heating processes, in addition, the specific heat capacity and thermal conductivity of calcium chloride are also important physical parameters that affect its efficiency in thermal management and regulatory applications. The calcium chloride solution is neutral. Soluble in a variety of polar, protic solvents, solubility at 20℃ in the following solvents (g/100mL solvent) : methanol: 29.2, anhydrous ethanol: 25.8, n-propanol: 15.8, n-butanol: 25.0, n-amyl alcohol: 11.5, ethylene glycol: 21.6 (25℃), formic acid: 43.1, acetic acid: 15.0 (30℃), hydrazine: 16.0. However, in dipolar solvents and low polar solvents, such as ether, tetrahydrofuran, etc., it is only slightly soluble or insoluble. Reacting with ammonia or ethanol, CaCl2·8NH3 and CaCl2·4C2H5OH complexes were formed, respectively. At low temperature, the solution crystallizes and precipitates as a hexahydrate, which is gradually dissolved in its own crystalline water when heated to 30 ° C, and gradually loses water when heated to 200 ° C, and becomes a dihydrate when heated to 260 ° C, which becomes a white porous anhydrous calcium chloride. Some hydrolysis reactions occur in the process of heating dehydration of hydrated calcium chloride, so the products often contain a small amount of CaO impurities.

Use 1: Used as refrigerant, also used in food processing, pharmaceutical and so on.

Use 2: Used in the food industry as calcium fortifying agent, chelating agent, curing agent and refrigerating refrigerant.

Use 3: for feed calcium supplement.

Use 4: As a coagulant, China stipulates that it can be used in soybean products according to production needs.

Use 5: used as a refrigerant (such as frozen brine for freezers, frozen brine for ice making and Popsicle making), antifreeze, automobile antifreeze, fire extinguishing agent. Flame retardant for melting ice and melting snow, finishing and finishing of cotton fabrics. Used as a adhesive and wood preservative. It is a raw material for the manufacture of anhydrous calcium chloride. Used in wall painting and plastering operations to increase condensation capacity. Rubber is produced for use as a condensate agent. Mix starch paste as gluing agent. It is also used for non-ferrous metal smelting. Used as medicine.

Use 6: oxygen, sulfur absorbent. Food protectant. Sizing agent. Water purification agent. Antifreeze.

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Electrolyte properties:
In an aqueous solution, calcium chloride fully ionizes into Ca² + and Cl⁻ ions, exhibiting the properties of a strong electrolyte. This electrolyte property makes calcium chloride solution with high conductivity and effective conduction of current, but also makes it an important chemical raw material and analytical reagent. In the fields of water treatment, metal processing and chemical synthesis, this property of calcium chloride can be used effectively for ion exchange, pH regulation and precipitation of metal ions.

Reactions with other chemicals:
Calcium chloride can also undergo a double substitution reaction with sodium sulfate (Na2SO4) and other salts to produce sodium chloride and calcium sulfate precipitation. The properties of this chemical reaction have important applications in industrial production and laboratory analysis, such as for the adjustment of water hardness or as a precipitating agent.