Calcium chloride – Wikipedia

You are viewing the article: Calcium chloride – Wikipedia at Traloitructuyen.com

Or you want a quick look: Uses[edit]

Calcium chloride
Names
IUPAC name

Calcium chloride

Other names

Neutral calcium chloride; calcium(II) chloride, calcium dichloride, E509

[external_link_head]
Identifiers

CAS Number

  • updating Calcium chloride - Wikipedia
  • updating (monohydrate) Calcium chloride - Wikipedia
  • updating (dihydrate) Calcium chloride - Wikipedia
  • updating (tetrahydrate) Calcium chloride - Wikipedia
  • updating (hexahydrate) Calcium chloride - Wikipedia

3D model (JSmol)

  • Interactive image
  • Interactive image
  • monohydrate: Interactive image
  • dihydrate: Interactive image
  • hexahydrate: Interactive image
ChEBI
  • CHEBI:3312 Calcium chloride - Wikipedia
ChEMBL
  • ChEMBL1200668 Calcium chloride - Wikipedia
ChemSpider
  • 23237 Calcium chloride - Wikipedia
DrugBank
  • DB01164 Calcium chloride - Wikipedia
ECHA InfoCard updating
EC Number
  • updating
E number E509 (acidity regulators, ...)

PubChem CID

  • 24854
RTECS number
  • EV9800000
UNII
  • OFM21057LP Calcium chloride - Wikipedia
  • LEV48803S9 (monohydrate) Calcium chloride - Wikipedia
  • M4I0D6VV5M (dihydrate) Calcium chloride - Wikipedia
  • 1D898P42YW (hexahydrate) Calcium chloride - Wikipedia

CompTox Dashboard (EPA)

  • DTXSID5020235

InChI

  • InChI=1S/Ca.2ClH/h;2*1H/q+2;;/p-2 Calcium chloride - Wikipedia

    Key: UXVMQQNJUSDDNG-UHFFFAOYSA-L Calcium chloride - Wikipedia

  • InChI=1/Ca.2ClH/h;2*1H/q+2;;/p-2

    Key: UXVMQQNJUSDDNG-NUQVWONBAG

SMILES

  • Cl[Ca]Cl

  • [Ca+2].[Cl-].[Cl-]

  • monohydrate: Cl[Ca]Cl.O

  • dihydrate: Cl[Ca]Cl.O.O

  • hexahydrate: Cl[Ca]Cl.O.O.O.O.O.O

Properties

Chemical formula

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[5]

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[5]

30 °C (86 °F; 303 K)

hexahydrate, decomposes[1]
Boiling point 1,935 °C (3,515 °F; 2,208 K) anhydrous[1]

Solubility in water

Anhydrous:

74.5 g/100 mL (20 °C)[2]

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)[3]
Solubility
  • Soluble in CH3COOH, alcohols
  • Insoluble in liquid NH3, DMSO, CH3COOC2H5[4]
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)[4]
Solubility in methanol
  • 21.8 g/100 g (0 °C)
  • 29.2 g/100 g (20 °C)
  • 38.5 g/100 g (40 °C)[4]
Solubility in acetone 0.1 g/kg (20 °C)[4]
Solubility in pyridine 16.6 g/kg[4]
Acidity (pKa)
  • 8–9 (anhydrous)
  • 6.5–8.0 (hexahydrate)

Magnetic susceptibility (χ)

−5.47·10−5 cm3/mol[1]

Refractive index (nD)

1.52
Viscosity
  • 3.34 cP (787 °C)
  • 1.44 cP (967 °C)[4]
Structure

Crystal structure

  • Orthorhombic (rutile, anhydrous), oP6
  • Tetragonal (anhydrous, > 217 °C), oP6[6]
  • Trigonal (hexahydrate)

Space group

[external_link offset=1]
  • Pnnm, No. 58 (anhydrous)
  • P42/mnm, No. 136 (anhydrous, >217 °C)[6]

Point group

  • 2/m 2/m 2/m (anhydrous)
  • 4/m 2/m 2/m (anhydrous, >217 °C)[6]

Lattice constant

a = 6.259 Å, b = 6.444 Å, c = 4.17 Å (anhydrous, 17 °C)[6]

α = 90°, β = 90°, γ = 90°

Coordination geometry

Octahedral (Ca2+, anhydrous)
Thermochemistry

Heat capacity (C)

  • 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)[5]

Std molar
entropy (So298)

108.4 J/mol·K[1][5]

Std enthalpy of
formation fH298)

  • −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)[5]

Gibbs free energy fG˚)

−748.81 kJ/mol[1][5]
Pharmacology

ATC code

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]

GHS precautionary statements

Pupdating[7]
NFPA 704 (fire diamond)

[9]

2

1

Lethal dose or concentration (LD, LC):

LD50 (median dose)

1,000-1,400 mg/kg (rats, oral)[8]
Related compounds

Other anions

  • Calcium fluoride
  • Calcium bromide
  • Calcium iodide

Other cations

  • Beryllium chloride
  • Magnesium chloride
  • Strontium chloride
  • Barium chloride
  • Radium chloride
Supplementary data page

Structure and
properties

Refractive index (n),

Dielectric constant (εr), etc.

Thermodynamic

data

Phase behaviour

solid–liquid–gas

Spectral data

UV, IR, NMR, MS

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Calcium chloride - Wikipedia verify (what is Calcium chloride - WikipediaCalcium chloride - Wikipedia ?)
Infobox references

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 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[edit]

De-icing and freezing-point depression[edit]

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[edit]

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 its hygroscopic nature 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[edit]

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.

[external_link offset=2]

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]

Laboratory and related drying operations[edit]

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[edit]

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 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 can be used to precipitate fluoride ions from water as insoluble CaF2.

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]

Cocaine producers in Colombia import tons of Calcium Chloride to recover solvents that are on the INCB Red List and are more tightly controlled.[24]

Hazards[edit]

Although non-toxic in small quantities when wet, the strongly hygroscopic properties of the non-hydrated salt present some 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.[25]

Consumption of calcium chloride can lead to hypercalcemia.[26]

Properties[edit]

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[edit]

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).[27]

In the US, most of calcium chloride is obtained by purification from brine.[citation needed ]

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.[citation needed ]

Occurrence[edit]

Calcium chloride occurs as the rare evaporite minerals sinjarite (dihydrate) and antarcticite (hexahydrate).[28][29][30] Another natural hydrate known is ghiaraite - a tetrahydrate.[31][30] The related minerals chlorocalcite (potassium calcium chloride, KCaCl3) and tachyhydrite (calcium magnesium chloride, Ca Mg2Cl6·12H2O) are also very rare.[32][33][30] So is true for rorisite, CaClF (calcium chloride fluoride).[34][30]

See also[edit]

  • Calcium(I) chloride
  • Calcium chloride transformation
  • Magnesium chloride

References[edit]

  1. ^ a b c d e f g h i Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN updating.
  2. ^ "Calcium chloride (anhydrous)". ICSC. International Programme on Chemical Safety and the European Commission.
  3. ^ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. p. 196.
  4. ^ a b c d e f Anatolievich, Kiper Ruslan. "Properties of substance: calcium chloride". chemister.ru. Retrieved 7 July 2014.
  5. ^ a b c d e f Pradyot, Patnaik (2019). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. p. 162. ISBN updating.
  6. ^ a b c d Müller, Ulrich (2006). Inorganic Structural Chemistry. wiley.com (2nd ed.). England: John Wiley & Sons Ltd. p. 33. ISBN updating.
  7. ^ a b c Sigma-Aldrich Co., Calcium chloride. Retrieved on updating.
  8. ^ Donald E. Garrett (2004). Handbook of Lithium and Natural Calcium Chloride. p. 379. ISBN updating. 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...)
  9. ^ "MSDS of Calcium chloride". fishersci.ca. Fisher Scientific. Retrieved 7 July 2014.
  10. ^ a b Robert Kemp, Suzanne E. Keegan "Calcium Chloride" in Ullmann's Encyclopedia of Industrial Chemistry 2000, Wiley-VCH, Weinheim. doi:10.1002/updating.a04_547
  11. ^ "Binary Phase diagram: The Calcium Chloride – water system". Aqueous Solutions Aps. October 2016. Archived from the original on 26 June 2019. 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 § updating
  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/updating. PMC 3152893. PMID updating.
  24. ^ Smith, Michael; Simpson, Cam (26 October 2020). "Narcos Are Waging a New Drug War Over a Texas Company's Basic Chemical". Bloomberg. Retrieved 26 October 2020.
  25. ^ "Product Safety Assessment (PSA): Calcium Chloride". Dow Chemical Company. 2 May 2006. Archived from the original on 17 September 2009. Retrieved 22 July 2008.
  26. ^ "Calcium Chloride Possible Side Affects".
  27. ^ Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, page 11.
  28. ^ "Sinjarite".
  29. ^ "Antarcticite".
  30. ^ a b c d "List of Minerals". 21 March 2011.
  31. ^ "Ghiaraite".
  32. ^ "Chlorocalcite".
  33. ^ "Tachyhydrite".
  34. ^ "Rorisite".
  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN updating.

External links[edit]

  • International Chemical Safety Card 1184
  • Product and Application Information (Formerly Dow Chemical Calcium Chloride division)
  • Report on steel corrosion by chloride including CaCl2
  • Collection of calcium chloride reports and articles
  • Calcium chloride, Anhydrous MSDS
  • Difusivity of calcium chloride
  • Centers for Disease Control and Prevention, National Institutes of Occupational Safety and Health, "Calcium Chloride (anhydrous)"

Salts and covalent derivatives of the chloride ion

[external_footer]
See more articles in the category: Hóa học
READ  Từ Điển Phương Trình Hoá Học

Leave a Reply