Calcium chloride

Calcium chloride is an inorganic compound, a salt with the chemical formula CaCl2. It is a white coloured crystalline solid at room temperature, and it is highly soluble in water. It can be created by neutralising hydrochloric acid with calcium hydroxide.

Calcium chloride
Names
IUPAC name
Calcium chloride
Other names
Calcium(II) chloride, calcium dichloride, E509
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.030.115
EC Number
  • 233-140-8
E number E509 (acidity regulators, ...)
RTECS number
  • EV9800000
UNII
Properties
CaCl2
Molar mass 110.98 g·mol−1
Appearance White powder, hygroscopic
Odor Odorless
Density
  • 2.15 g/cm3 (anhydrous)
  • 2.24 g/cm3 (monohydrate)
  • 1.85 g/cm3 (dihydrate)
  • 1.83 g/cm3 (tetrahydrate)
  • 1.71 g/cm3 (hexahydrate)[1]
Melting point 772–775 °C (1,422–1,427 °F; 1,045–1,048 K)
anhydrous[2]
260 °C (500 °F; 533 K)
monohydrate, decomposes
175 °C (347 °F; 448 K)
dihydrate, decomposes
45.5 °C (113.9 °F; 318.6 K)
tetrahydrate, decomposes[2]
30 °C (86 °F; 303 K)
hexahydrate, decomposes[1]
Boiling point 1,935 °C (3,515 °F; 2,208 K) anhydrous[1]
Anhydrous:
74.5 g/100 mL (20 °C)[3]
Hexahydrate:
49.4 g/100 mL (−25 °C)
59.5 g/100 mL (0 °C)
65 g/100 mL (10 °C)
81.1 g/100 mL (25 °C)[1]
102.2 g/100 mL (30.2 °C)
α-Tetrahydrate:
90.8 g/100 mL (20 °C)
114.4 g/100 mL (40 °C)
Dihydrate:
134.5 g/100 mL (60 °C)
152.4 g/100 mL (100 °C)[4]
Solubility
Solubility in ethanol
  • 18.3 g/100 g (0 °C)
  • 25.8 g/100 g (20 °C)
  • 35.3 g/100 g (40 °C)
  • 56.2 g/100 g (70 °C)[5]
Solubility in methanol
  • 21.8 g/100 g (0 °C)
  • 29.2 g/100 g (20 °C)
  • 38.5 g/100 g (40 °C)[5]
Solubility in acetone 0.1 g/kg (20 °C)[5]
Solubility in pyridine 16.6 g/kg[5]
Acidity (pKa)
  • 8–9 (anhydrous)
  • 6.5–8.0 (hexahydrate)
−5.47·10−5 cm3/mol[1]
1.52
Viscosity
  • 3.34 cP (787 °C)
  • 1.44 cP (967 °C)[5]
Structure
  • Pnnm, No. 58 (anhydrous)
  • P42/mnm, No. 136 (anhydrous, >217 °C)[6]
  • 2/m 2/m 2/m (anhydrous)
  • 4/m 2/m 2/m (anhydrous, >217 °C)[6]
a = 6.259 Å, b = 6.444 Å, c = 4.17 Å (anhydrous, 17 °C)[6]
α = 90°, β = 90°, γ = 90°
Octahedral (Ca2+, anhydrous)
Thermochemistry
  • 72.89 J/mol·K (anhydrous)[1]
  • 106.23 J/mol·K (monohydrate)
  • 172.92 J/mol·K (dihydrate)
  • 251.17 J/mol·K (tetrahydrate)
  • 300.7 J/mol·K (hexahydrate)[2]
108.4 J/mol·K[1][2]
Std enthalpy of
formation (ΔfH⦵298)
  • −795.42 kJ/mol (anhydrous)[1]
  • −1110.98 kJ/mol (monohydrate)
  • −1403.98 kJ/mol (dihydrate)
  • −2009.99 kJ/mol (tetrahydrate)
  • −2608.01 kJ/mol (hexahydrate)[2]
−748.81 kJ/mol[1][2]
Pharmacology
A12AA07 (WHO) B05XA07 (WHO), G04BA03 (WHO)
Hazards
Main hazards Irritant
Safety data sheet See: data page
GHS pictograms [7]
GHS Signal word Warning
GHS hazard statements
 H319[7]
P305+351+338[7]
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
1,000-1,400 mg/kg (rats, oral)[9]
Related compounds
Other anions
Other cations
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Calcium chloride is commonly encountered as a hydrated solid with generic formula CaCl2(H2O)x, where x = 0, 1, 2, 4, and 6. These compounds are mainly used for de-icing and dust control. Because the anhydrous salt is hygroscopic, it is used as a desiccant.[10]

Uses

De-icing and freezing-point depression
Bulk CaCl2 for de-icing in Japan

By depressing the freezing point of water, calcium chloride is used to prevent ice formation and is used to de-ice. This application consumes the greatest amount of calcium chloride. Calcium chloride is relatively harmless to plants and soil. As a deicing agent, it is much more effective at lower temperatures than sodium chloride. When distributed for this use, it usually takes the form of small, white spheres a few millimeters in diameter, called prills. Solutions of calcium chloride can prevent freezing at temperatures as low as −52 °C (−62 °F), making it ideal for filling agricultural implement tires as a liquid ballast, aiding traction in cold climates.[11]

It is also used in domestic and industrial chemical air dehumidifiers.[12]

Road surfacing
Calcium chloride was sprayed on this road to prevent weathering, giving it a wet appearance even in dry weather.

The second largest application of calcium chloride exploits hygroscopic properties and the tackiness of its hydrates. Calcium chloride is highly hygroscopic and its hydration is an exothermic reaction. A concentrated solution keeps a liquid layer on the surface of dirt roads, which suppresses the formation of dust. It keeps the finer dust particles on the road, providing a cushioning layer. If these are allowed to blow away, the large aggregate begins to shift around and the road breaks down. Using calcium chloride reduces the need for grading by as much as 50% and the need for fill-in materials as much as 80%.[13]

Food

The average intake of calcium chloride as food additives has been estimated to be 160–345 mg/day.[14] Calcium chloride is permitted as a food additive in the European Union for use as a sequestrant and firming agent with the E number E509. It is considered as generally recognized as safe (GRAS) by the U.S. Food and Drug Administration.[15] Its use in organic crop production is generally prohibited under the US National Organic Program.[16]

In marine aquariums, calcium chloride is one way to introduce bioavailable calcium for calcium carbonate-shelled animals such as mollusks and some cnidarians. Calcium hydroxide (kalkwasser mix) or a calcium reactor can also be used.

As a firming agent, calcium chloride is used in canned vegetables, in firming soybean curds into tofu and in producing a caviar substitute from vegetable or fruit juices.[17] It is commonly used as an electrolyte in sports drinks and other beverages, including bottled water. The extremely salty taste of calcium chloride is used to flavor pickles without increasing the food's sodium content. Calcium chloride's freezing-point depression properties are used to slow the freezing of the caramel in caramel-filled chocolate bars. Also, it is frequently added to sliced apples to maintain texture.

In brewing beer, calcium chloride is sometimes used to correct mineral deficiencies in the brewing water. It affects flavor and chemical reactions during the brewing process, and can also affect yeast function during fermentation.

In cheesemaking, calcium chloride is sometimes added to processed (pasteurized/homogenized) milk to restore the natural balance between calcium and protein in casein. It is added before the coagulant.

Calcium chloride is used to prevent cork spot and bitter pit on apples by spraying on the tree during the late growing season.[18]

Drying tubes are frequently packed with calcium chloride. Kelp is dried with calcium chloride for use in producing sodium carbonate. Anhydrous calcium chloride has been approved by the FDA as a packaging aid to ensure dryness (CPG 7117.02).[19]

The hydrated salt can be dried for re-use but will dissolve in its own water of hydration if heated quickly and form a hard amalgamated solid when cooled.

Miscellaneous applications

Calcium chloride is used in concrete mixes to accelerate the initial setting, but chloride ions lead to corrosion of steel rebar, so it should not be used in reinforced concrete.[20] The anhydrous form of calcium chloride may also be used for this purpose and can provide a measure of the moisture in concrete.[21]

Calcium chloride is included as an additive in plastics and in fire extinguishers, in wastewater treatment as a drainage aid, in blast furnaces as an additive to control scaffolding (clumping and adhesion of materials that prevent the furnace charge from descending), and in fabric softener as a thinner.

The exothermic dissolution of calcium chloride is used in self-heating cans and heating pads.

In the oil industry, calcium chloride is used to increase the density of solids-free brines. It is also used to provide inhibition of swelling clays in the water phase of invert emulsion drilling fluids.

CaCl2 acts as flux material, decreasing the melting point, in the Davy process for the industrial production of sodium metal through the electrolysis of molten NaCl.

Similarly, CaCl2 is used as a flux and electrolyte in the FFC Cambridge process for titanium production, where it ensures the proper exchange of calcium and oxygen ions between the electrodes.

Calcium chloride is also used in the production of activated charcoal.

Calcium chloride is also an ingredient used in ceramic slipware. It suspends clay particles so that they float within the solution, making it easier to use in a variety of slipcasting techniques.

Calcium chloride dihydrate (20 percent by weight) dissolved in ethanol (95 percent ABV) has been used as a sterilant for male animals. The solution is injected into the testes of the animal. Within one month, necrosis of testicular tissue results in sterilization.[22][23]

Hazards

Calcium chloride can act as an irritant by desiccating moist skin. Solid calcium chloride dissolves exothermically, and burns can result in the mouth and esophagus if it is ingested. Ingestion of concentrated solutions or solid products may cause gastrointestinal irritation or ulceration.[24]

Consumption of calcium chloride can lead to hypercalcemia.[25]

Properties
Flame test of CaCl2

Calcium chloride dissolves in water, producing chloride and the aquo complex [Ca(H2O)6]2+. In this way, these solutions are sources of "free" calcium and free chloride ions. This description is illustrated by the fact that these solutions react with phosphate sources to give a solid precipitate of calcium phosphate:

3 CaCl2 + 2 PO3−
4 → Ca3(PO4)2 + 6 Cl−

Calcium chloride has a very high enthalpy change of solution, indicated by considerable temperature rise accompanying dissolution of the anhydrous salt in water. This property is the basis for its largest-scale application.

Molten calcium chloride can be electrolysed to give calcium metal and chlorine gas:

CaCl2 → Ca + Cl2

Preparation
Structure of the polymeric [Ca(H2O)6]2+ center in crystalline calcium chloride hexahydrate, illustrating the high coordination number typical for calcium complexes.

In much of the world, calcium chloride is derived from limestone as a by-product of the Solvay process, which follows the net reaction below:[10]

2 NaCl + CaCO3 → Na2CO3 + CaCl2

North American consumption in 2002 was 1,529,000 tonnes (3.37 billion pounds).[26]

In the US, most of calcium chloride is obtained by purification from brine.

As with most bulk commodity salt products, trace amounts of other cations from the alkali metals and alkaline earth metals (groups 1 and 2) and other anions from the halogens (group 17) typically occur, but the concentrations are trifling.

Occurrence

Calcium chloride occurs as the rare evaporite minerals sinjarite (dihydrate) and antarcticite (hexahydrate). The related minerals chlorocalcite (potassium calcium chloride, KCaCl3) and tachyhydrite (calcium magnesium chloride, CaMg2Cl6·12H2O) are also very rare.

See also

References
  1. Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
  2. Pradyot, Patnaik (2019). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. p. 162. ISBN 978-0-07-049439-8.
  3. "Calcium chloride (anhydrous)". ICSC. International Programme on Chemical Safety and the European Commission.
  4. Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. p. 196.
  5. Anatolievich, Kiper Ruslan. "Properties of substance: calcium chloride". chemister.ru. Retrieved 7 July 2014.
  6. Müller, Ulrich (2006). Inorganic Structural Chemistry. wiley.com (2nd ed.). England: John Wiley & Sons Ltd. p. 33. ISBN 978-0-470-01864-4.
  7. Sigma-Aldrich Co., Calcium chloride. Retrieved on 2014-07-07.
  8. "MSDS of Calcium chloride". fishersci.ca. Fisher Scientific. Retrieved 7 July 2014.
  9. Donald E. Garrett (2004). Handbook of Lithium and Natural Calcium Chloride. p. 379. ISBN 978-0080472904. Retrieved 29 August 2018. Its toxicity upon ingestion, is indicated by the test on rats: oral LD50 (rat) is 1.0–1.4 g/kg (the lethal dose for half of the test animals, in this case rats...)
  10. Robert Kemp, Suzanne E. Keegan "Calcium Chloride" in Ullmann's Encyclopedia of Industrial Chemistry 2000, Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_547
  11. "Binary Phase diagram: The Calcium Chloride – water system". Aqueous Solutions Aps. October 2016. Retrieved 20 April 2017.
  12. "humantouchofchemistry.com Keeping Things Dry". Archived from the original on 26 October 2014. Retrieved 23 October 2014.
  13. "Dust: Don't Eat It! Control It!". Road Management & Engineering Journal. US Roads (TranSafety Inc.). 1 June 1998. Archived from the original on 29 October 2007. Retrieved 9 August 2006.
  14. Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, pp. 13–14.
  15. 21 CFR § 184.1193
  16. 7 CFR § 205.602
  17. "Apple Caviar Technique". StarChefs Studio. StarChefs.com. April 2004. Retrieved 9 August 2006.
  18. "Cork Spot and Bitter Pit of Apples", Richard C. Funt and Michael A. Ellis, Ohioline.osu.edu/factsheet/plpath-fru-01
  19. "CPG 7117.02". FDA Compliance Articles. US Food and Drug Administration. March 1995. Retrieved 3 December 2007.
  20. "Accelerating Concrete Set Time". Federal Highway Administration. 1 June 1999. Retrieved 16 January 2007.
  21. National Research Council (U.S.). Building Research Institute (1962). Adhesives in Building: Selection and Field Application; Pressure-sensitive Tapes. National Academy of Science-National Research Council. pp. 24–5.
  22. Koger, Nov 1977, "Calcium Chloride, Practical Necrotizing Agent", Journal of the American Association of Bovine Practitioners (USA), (Nov 1977), v. 12, p. 118–119
  23. Jana, K.; Samanta, P.K. (2011). "Clinical evaluation of non-surgical sterilization of male cats with single intra-testicular injection of calcium chloride". BMC Vet. Res. 7: 39. doi:10.1186/1746-6148-7-39. PMC 3152893. PMID 21774835.
  24. "Product Safety Assessment (PSA): Calcium Chloride". Dow Chemical Company. 2 May 2006. Archived from the original on 17 September 2009. Retrieved 22 July 2008.
  25. "Calcium Chloride Possible Side Affects".
  26. Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, page 11.
Salts and covalent derivatives of the chloride ion
HCl He
LiCl BeCl2 BCl3
B2Cl4		 CCl4 NCl3
ClN3		 Cl2O
ClO2
Cl2O7		 ClF
ClF3
ClF5		 Ne
NaCl MgCl2 AlCl
AlCl3		 SiCl4 P2Cl4
PCl3
PCl5		 S2Cl2
SCl2
SCl4		 Cl2 Ar
KCl CaCl
CaCl2		 ScCl3 TiCl2
TiCl3
TiCl4		 VCl2
VCl3
VCl4
VCl5		 CrCl2
CrCl3
CrCl4		 MnCl2 FeCl2
FeCl3		 CoCl2
CoCl3		 NiCl2 CuCl
CuCl2		 ZnCl2 GaCl2
GaCl3		 GeCl2
GeCl4		 AsCl3
AsCl5		 Se2Cl2
SeCl4		 BrCl KrCl
RbCl SrCl2 YCl3 ZrCl3
ZrCl4		 NbCl4
NbCl5		 MoCl2
MoCl3
MoCl4
MoCl5
MoCl6		 TcCl4 RuCl3 RhCl3 PdCl2 AgCl CdCl2 InCl
InCl2
InCl3		 SnCl2
SnCl4		 SbCl3
SbCl5		 Te3Cl2
TeCl4		 ICl
ICl3		 XeCl
XeCl2
XeCl4
CsCl BaCl2   HfCl4 TaCl5 WCl2
WCl3
WCl4
WCl5
WCl6		 Re3Cl9
ReCl4
ReCl5
ReCl6		 OsCl4 IrCl2
IrCl3
IrCl4		 PtCl2
PtCl4		 AuCl
AuCl3		 Hg2Cl2,
HgCl2		 TlCl PbCl2,
PbCl4		 BiCl3 PoCl2,
PoCl4		 AtCl RnCl2
FrCl RaCl2   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
LaCl3 CeCl3 PrCl3 NdCl2,
NdCl3		 PmCl3 SmCl2,
SmCl3		 EuCl2,
EuCl3		 GdCl3 TbCl3 DyCl2,
DyCl3		 HoCl3 ErCl3 TmCl2
TmCl3		 YbCl2
YbCl3		 LuCl3
AcCl3 ThCl4 PaCl5 UCl3
UCl4
UCl5
UCl6		 NpCl4 PuCl3 AmCl2
AmCl3		 CmCl3 BkCl3 CfCl3 EsCl3 Fm Md No LrCl3
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.