Calcium chloride



Calcium chloride
IUPAC name calcium chloride
Other names calcium(II) chloride,
calcium dichloride,
E509
Identifiers
CAS number 10043-52-4
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
MSDS External MSDS
EU classification Irritant (Xi)
NFPA 704
0
1
0
 
R-phrases R36
S-phrases S24
Related Compounds
Other anions calcium fluoride
calcium bromide
calcium iodide
Other cations strontium chloride
Supplementary data page
Structure and
properties 		εr, etc.
Thermodynamic
data 		Phase behaviour
Solid, liquid, gas
Spectral data MS
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references

Calcium chloride (CaCl2) is an hygroscopic nature, it must be kept in tightly-sealed containers.

Chemical properties

Calcium chloride can serve as a source of calcium ions in compounds are insoluble:

3 CaCl2(aq) + 2 K3PO4(aq) → KCl(aq)

Molten CaCl2 can be calcium metal:

CaCl2(g)

Preparation

Uses (industrial)

Millions of tonnes of calcium chloride are made each year in the US alone, and it has a wide variety of industrial applications:

Because it is strongly water vapor from the substance to be dried:

CaCl2 + 2 H2O → CaCl2·2H2O

Aided by the intense heat evolved during its dissolution, calcium chloride is also used as an sodium chloride (rock salt or halite), it is relatively harmless to plants and soil. It is also more effective at lower temperatures than sodium chloride. When distributed for this use, it usually takes the form of small white balls a few millimetres in diameter, called prills (see picture at top of page).

Used for its reinforced concrete.[2]

The aqueous form of calcium chloride is used in genetic transformation of cells by increasing the cell membrane permeability, inducing competence for DNA uptake (allowing DNA fragments to enter the cell more readily). In this form it can lower the freezing point of water as low as -52°C (-62°F), making it ideal for filling agricultural implement tires as a liquid ballast, aiding traction in cold climates.[3]

It can be used in Medicine to treat Calcium Channel Blocker toxicity with overdoses of drugs such as Diltiazem (Cardizem), to treat certain electrolyte imbalances along with Calcium Gluconate or to help correct hypocalcemia. It can also be used to assist treatment of cardiac arrest.

Other industrial applications include use as as an additive in plastics, as a drainage aid for wastewater treatment, as an additive in fire extinguishers, as an additive in control scaffolding in fabric softener.

Uses (food)

As an ingredient, it is listed as a permitted food additive in the European Union for use as a sequestrant and firming agent with the E number E509. The anhydrous form has been approved by the FDA as a packaging aid to ensure dryness (CPG 7117.02).[4]

Calcium chloride is commonly used as an sodium content. It is even found in snack foods, including Cadbury Caramilk chocolate bars (purpose unknown).

Other than as a preservative, it can be used to make ersatz caviar from vegetable or fruit juices[5] or added to processed milk to restore the natural balance between calcium and protein for the purposes of making cheese such as brie and stilton. Calcium chloride's exothermic properties are exploited in many 'self heating' food products where it is activated (mixed) with water to start the heating process, providing a non-explosive, dry fuel that is easily activated.

Precautions

Calcium chloride is an irritant, particularly on moist skin. Wear gloves and goggles or a full face shield to protect hands and eyes; avoid inhalation.

Dry calcium chloride reacts exothermically when exposed to water. Burns can result in the mouth and esophagus if humans or other animals ingest dry calcium chloride pellets. Small children are more susceptible than adults (who generally have had experience trying to eat hot food, and can react accordingly) so calcium chloride pellets should be kept out of their reach.

References

  1. ^ Dust: Don't Eat It! Control It!. Road Management & Engineering Journal. US Roads (TranSafety Inc.) (1 June 1998). Retrieved on 9 August, 2006.
  2. ^ Accelerating Concrete Set Time (1 June 1999). Retrieved on January 16, 2007.
  3. ^ Agricultural Tire Hydroinflation. www.firestoneag.com. Firestone Tires (December 2007). Retrieved on 3 December, 2007.
  4. ^ CPG 7117.02. FDA Compliance Articles. US Food and Drug Administration (March 1995). Retrieved on 3 December, 2007.
  5. ^ Apple Caviar Technique. StarChefs Studio. StarChefs.com (April 2004). Retrieved on 9 August, 2006.

General references

  • Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements, 2nd Edition, Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4. 
  • Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
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Selenium		Sodium selenate - Sodium selenite
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Urologicals (Finasteride

Terazosin

Herbals: Pygeum africanum, Serenoa repens
 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Calcium_chloride". A list of authors is available in Wikipedia.