Calcium chloride is a highly soluble inorganic compound with the formula CaCl2. It is commonly used as a de-icing agent, desiccant, and in the production of calcium salts and chemicals.
| IUPAC Name | Calcium chloride |
| Molecular Formula | CaCl2 |
| CAS Number | 10043-52-4 |
| Synonyms | Calcium dichloride, Calcium(II) chloride |
| E509, Pickling salt, Dowflake, Peladow, TETRA | |
| InChI | InChI=1S/Ca.2ClH/h;2*1H/q+2;;/p-2 |
Calcium chloride formula
The chemical formula for calcium chloride is CaCl2. This means that each unit of calcium chloride is composed of one calcium ion (Ca2+) and two chloride ions (Cl-). Calcium chloride is an ionic compound, meaning that it is held together by electrostatic attraction between the positively charged calcium ion and the negatively charged chloride ions.
Calcium chloride molar mass
Calcium chloride has a molar mass of 110.98 g/mol, which is the sum of the atomic masses of one Ca atom and two Cl atoms. It is an inorganic compound that is highly soluble in water and is commonly used as a drying agent, desiccant, and de-icing agent. Calcium chloride is also used in the production of calcium salts and other chemicals.
CaCl2 boiling point
The boiling point of CaCl2 is 1935 °C, which is very high for an inorganic compound. This is due to the strong ionic bonds between the Ca+2 and Cl- ions, which require a lot of energy to break. CaCl2 is a hygroscopic compound, meaning it absorbs moisture from the air and can dissolve in water to form a highly concentrated solution.
CaCl2 melting point
CaCl2 has a melting point of 772 °C. It has a crystalline structure and is commonly found in its anhydrous form, which means it does not contain any water molecules. When CaCl2 is heated, it will decompose into calcium oxide and hydrogen chloride gas.
CaCl2 density g/ml
The density of CaCl2 depends on the concentration of the solution. A 1 M solution of CaCl2 has a density of approximately 1.4 g/mL, while a 3 M solution has a density of approximately 1.6 g/mL. The density of solid CaCl2 is 2.15 g/cm³.
CaCl2 molecular weight
The molecular weight of CaCl2 is 110.98 g/mol. It is an inorganic compound that is composed of one Ca atom and two Cl atoms. CaCl2 is a white crystalline solid at room temperature and is highly soluble in water.
CaCl2 Structure
CaCl2 has a crystal lattice structure, which is held together by ionic bonds between the calcium cation (Ca2+) and the chloride anion (Cl-). Each Ca+2 ion is surrounded by six Cl- ions, and each chloride ion is surrounded by six calcium ions. The crystal structure of CaCl2 is cubic, with each unit cell containing one calcium ion and two chloride ions.
| Appearance | White solid |
| Specific Gravity | 2.15 (solid), 1.4-1.6 (solution) |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 110.98 g/mol |
| Density | 2.15 g/cm³ (solid), 1.4-1.6 g/cm³ (solution) |
| Melting Point | 772 °C |
| Boiling Point | 1935 °C |
| Flash Point | Not applicable |
| Water Solubility | Highly soluble in water |
| Solubility | Soluble in ethanol and acetone |
| Vapor Pressure | Negligible |
| Vapor Density | Not applicable |
| pKa | – |
| pH | 4.5-11.0 (10% solution) |
Calcium Chloride Safety and Hazards
CaCl2 can cause skin and eye irritation, and inhalation of its dust or mist may cause respiratory irritation. It can also cause burns if it comes in contact with skin or eyes. CaCl2 is hygroscopic, meaning it can absorb moisture and release heat, which can cause containers to rupture or explode. It is also corrosive to some metals and can react with some organic materials. Proper protective equipment, such as gloves and goggles, should be used when handling CaCl2. Spills should be cleaned up immediately, and containers should be stored in a cool, dry, well-ventilated area.
| Hazard Symbols | Corrosive, Irritant |
| Safety Description | Wear protective gloves and eye/face protection. Do not breathe dust/fume/gas/mist/vapors. |
| UN IDs | UN 3077, UN 1786 (when hydrated) |
| HS Code | 2827.39.90 |
| Hazard Class | 8 (Corrosive substances) |
| Packing Group | III |
| Toxicity | Toxicity is low for most applications, but it can be hazardous in large quantities |
Calcium Chloride Synthesis Methods
To synthesize CaCl2, there are several methods available.
One method is by reacting calcium carbonate or calcium hydroxide with hydrochloric acid. One method involves adding either calcium carbonate or calcium hydroxide to hydrochloric acid. The solution evaporates to yield CaCl2.
Another method involves reacting calcium oxide with hydrochloric acid. This method is to add calcium oxide to hydrochloric acid, and then evaporate the solution to obtain CaCl2.
A third method involves reacting calcium metal with chlorine gas. A less common method is to heat calcium metal in the presence of chlorine gas. The reaction yields CaCl2, but experts do not frequently use this approach because of calcium metal’s high reactivity and the need for specialized handling.
To produce CaCl2 using a different method, one can use the byproduct of the Solvay process, which generates sodium chloride and CaCl2. The process involves extracting CaCl2 from the byproduct through filtration, evaporation, and purification techniques. These steps help to remove any impurities and produce high-purity CaCl2.
Calcium Chloride Uses
CaCl2 has many industrial applications:
- Used as a desiccant to absorb moisture, a de-icing agent for roads and sidewalks, and a coagulant in the production of tofu and other foods.
- Used in the oil and gas industry to increase the density of drilling fluids and to reduce the freezing point of water in pipelines.
- Used in concrete mixes to accelerate the curing process and to increase the strength and durability of the finished product.
- Used in the production of paper to increase the strength and stability of the paper fibers.
- Used in water treatment to remove impurities and to soften water.
- Used as a source of calcium ions in medical applications, such as intravenous fluids and to treat hypocalcemia.
- Used in the production of plastics and rubber to increase the hardness and durability of the final product.
- Used in the preservation of fruits and vegetables to prevent spoilage and to maintain the texture and flavor of the produce.
- Used in the production of textiles to improve dye absorption and to increase the strength and flexibility of the fibers.
- Also used in the production of fire extinguishers and as a component of fire-retardant materials to prevent the spread of flames.
Questions:
Q: What is calcium chloride?
A: Calcium chloride is a chemical compound made up of Ca2+ and Cl- ions with the chemical formula CaCl2.
Q: Is calcium chloride ionic or covalent?
A: CaCl2 is an ionic compound because it is composed of positively charged Ca2+ ions and negatively charged Cl- ions held together by ionic bonds.
Q: What is calcium chloride used for?
A: CaCl2 has many industrial, commercial, and medical uses, including as a desiccant, a de-icing agent, a coagulant in food production, an accelerator in concrete, a water softener, and a source of calcium ions in medical treatments.
Q: What is the formula for calcium chloride?
A: The formula for calcium chloride is CaCl2, indicating that each molecule contains one calcium ion and two chloride ions.
Q: Is CaCl2 ionic or covalent?
A: CaCl2 is an ionic compound because it is composed of positively charged calcium ions and negatively charged chloride ions held together by ionic bonds.
Q: Is CaCl2 soluble in water?
A: Yes, CaCl2 is highly soluble in water, meaning that it can easily dissolve in water to form a clear solution.
Q: If CaCl2 is dissolved in water, what can be said about the concentration of the Ca2+ ion?
A: When CaCl2 is dissolved in water, it dissociates into its constituent ions, Ca2+ and 2Cl-. Since CaCl2 dissociates completely in water, the concentration of Ca2+ ions in solution is twice the concentration of CaCl2.