Calcium chloride
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| Calcium chloride | |
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| IUPAC name | calcium chloride |
| Other names | calcium(II) chloride, calcium dichloride |
| Identifiers | |
| CAS number | |
| RTECS number | EV9800000, anhydrous |
| Properties | |
| Molecular formula | CaCl2 CaCl2.2H2O [Dihydrate] CaCl2.4H2O [Tetrahydrate] CaCl2.6H2O [Hexahydrate] |
| Molar mass | 110.99 g/mol, anhydrous 147.02 g/mol, dihydrate 182.04 g/mol, tetrahydrate 219.08 g/mol, hexahydrate |
| Appearance | white or colorless solid |
| Density | 2.15 g/cm³, anhydrous 0.835 g/cm³, dihydrate 1.71 g/cm³, hexahydrate |
| Melting point |
772 °C (anhydrous) |
| Boiling point |
>1600 °C |
| Solubility in water | 74.5 g/100 ml (20 °C) |
| Structure | |
| Crystal structure | deformed rutile |
| Coordination geometry | octahedral, 6-coordinate |
| Hazards | |
| EU classification | Irritant (Xi) |
| NFPA 704 |
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| R-phrases | R36 |
| S-phrases | (S2), S22, S24 |
| Related Compounds | |
| Other anions | calcium fluoride calcium bromide calcium iodide |
| Other cations | magnesium chloride strontium chloride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references | |
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Calcium chloride is an ionic compound of calcium and chlorine. It is highly soluble in water and it is deliquescent. It is a salt that is solid at room temperature, and it behaves as a typical ionic halide. It has several common applications 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.
Chemical properties
Calcium chloride can serve as a source of calcium ions in solution, for instance for precipitation because many calcium compounds are insoluble:
3 CaCl2(aq) + 2 potassium phosphate|K3PO4(aq) → Ca3(PO4)2(s) + 6 KCl(aq)
Molten CaCl2 can be electrolysed to give calcium metal:
Preparation
Calcium chloride is a by-product of the Solvay process used for the manufacture of sodium carbonate. It can also be produced by the action of hydrochloric acid on calcium carbonate.
CaCO3(s) + 2 HCl → CaCl2(aq) + H2O(l) + CO2(g)
Uses
Millions of tonnes of calcium chloride are made each year in the US alone, and it has a variety of applications:
- Aqueous Calcium Chloride is used in genetic transformation of cells by increasing the cell membrane permeability. This allows DNA fragments to enter the cell more readily.
- It is used in Smartwater and some sports drinks as an Electrolyte
- It is used in Emergency Medicine to treat Calcium Channel Blocker toxicity with overdoses of drugs such as Cardizem. It is also used to treat certain electrolyte imbalances along with Calcium Gluconate.
- It is also used to induce competence for DNA uptake in experiments involving uptake of DNA from outside the cell
Precautions
Calcium chloride is an irritant; wear gloves and goggles to protect hands and eyes; avoid inhalation.
Although calcium chloride is relatively safe to handle, care should be taken that it is not ingested. Calcium chloride reacts exothermically with water and can burn the mouth and esophagus.
References
General references
- Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
External links
- International Chemical Safety Card 1184
- Calcium Chloride Handbook from Dow Chemical (pdf 1.6MB)
- Report on steel corrosion by chloride including CaCl2
da:Kalciumklorid de:Calciumchloridfr:Chlorure de calcium gl:Cloruro de calcio it:Cloruro di calcio hu:Kalcium-klorid nl:Calciumchloride ja:塩化カルシウムfi:Kalsiumkloridi sv:Kalciumklorid
Acknowledgement and Attribution Regarding Sources of Content
Some of the initial content on this page may be incorporated in part from copyleft sources in the public domain including wikis such as Wikipedia and AskDrWiki. Drug information for patients came from the The National Library of Medicine. Infectious disease information may have come from the Centers for Disease Control (CDC). Differential Diagnoses are drawn from clinicians as well as an amalgamation of 3 sources: 1.The Disease Database; 2. Kahan, Scott, Smith, Ellen G. In A Page: Signs and Symptoms. Malden, Massachusetts: Blackwell Publishing, 2004:3; 3. Sailer, Christian, Wasner, Susanne. Differential Diagnosis Pocket. Hermosa Beach, CA: Borm Bruckmeir Publishing LLC, 2002:7 .
