Calcium chloride

Short description: Chemical compound

Calcium chloride

Names
IUPAC name

Calcium chloride

Other names

Neutral calcium chloride; calcium(II) chloride, calcium dichloride (1:2), E509

Identifiers

CAS Number

* 10043-52-4 Y
* 22691-02-7 (monohydrate) Y
* 10035-04-8 (dihydrate) Y
* 25094-02-4 (tetrahydrate) N
* 7774-34-7 (hexahydrate) Y

3D model (JSmol)

* Interactive image
* Interactive image
* monohydrate: Interactive image
* dihydrate: Interactive image
* hexahydrate: Interactive image

ChEBI |

* CHEBI:3312 Y

ChEMBL |

* ChEMBL1200668 N

ChemSpider |

* 23237 Y

DrugBank |

* DB01164 Y

EC Number |

* 233-140-8

PubChem CID

* 24854

RTECS number |

* EV9800000

UNII |

* OFM21057LP Y
* LEV48803S9 (monohydrate) Y
* M4I0D6VV5M (dihydrate) Y
* 1D898P42YW (hexahydrate) Y

InChI

* InChI=1S/Ca.2ClH/h;2*1H/q+2;;/p-2 Y

Key: UXVMQQNJUSDDNG-UHFFFAOYSA-L Y

* 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 hygroscopic powder
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 acetic acid, alcohols
* Insoluble in liquid ammonia, dimethyl sulfoxide (DMSO), ethyl acetate[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

* 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 at Ca2+ centres (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 (S ~~o~~ 298)

| 108.4 J/(mol·K)[1][5]

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)[5]

Gibbs free energy (ΔfG˚)

| −748.81 kJ/mol[1][5]
Pharmacology
1=ATC code }}  | A12AA07 (WHO) B05XA07 (WHO), G04BA03 (WHO)
Hazards
Main hazards | Irritant
GHS pictograms | [7]
GHS Signal word | Warning

GHS hazard statements

| H319[7]

GHS precautionary statements

| P305+351+338[7]
NFPA 704 (fire diamond)  |

[9]

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

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

Tracking categories (test):

* SizeSet

Calcium chloride is an inorganic compound, a salt with the chemical formula CaCl
2. It is a white 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 CaCl
2 * nH
2O, where n = 0, 1, 2, 4, and 6. These compounds are mainly used for de-icing and dust control. Because the anhydrous salt is hygroscopic and deliquescent, it is used as a desiccant.[10]

## Contents

* 1 History
* 2 Uses
* 2.1 De-icing and freezing-point depression
* 2.2 Road surfacing
* 2.3 Food
* 2.4 Laboratory and related drying operations
* 2.5 Other applications
* 2.6 Metal reduction flux
* 2.7 Medical use
* 3 Hazards
* 4 Properties
* 5 Preparation
* 5.1 Occurrence
* 6 See also
* 7 References
* 8 External links

## History

Calcium chloride was apparently discovered in the 15th century but wasn't studied properly until the 18th century.[11] It was historically called "fixed sal ammoniac" (Latin: sal ammoniacum fixum[12]) because it was synthesized during the distillation of ammonium chloride with lime and was nonvolatile (while the former appeared to sublime); in more modern times (18th-19th cc.) it was called "muriate of lime" (Latin: murias calcis, calcaria muriatica[12]).[13]

## Uses

### De-icing and freezing-point depression

Bulk CaCl
2 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.[14]

It is also used in domestic and industrial chemical air dehumidifiers.[15]

### 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 its hygroscopic nature and the tackiness of its hydrates; calcium chloride is highly hygroscopic and its hydration is an exothermic process. 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%.[16]

### Food

The average intake of calcium chloride as food additives has been estimated to be 160–345 mg/day.[17] 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.[18] Its use in organic crop production is generally prohibited under the US National Organic Program.[19]

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.[20] 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.[21]

### Laboratory and related drying operations

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).[22]

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.

### Other 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.[23] The anhydrous form of calcium chloride may also be used for this purpose and can provide a measure of the moisture in concrete.[24]

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.

CaCl
2 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.

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

Calcium chloride can be used to precipitate fluoride ions from water as insoluble CaF

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.[25][26]

Cocaine producers in Colombia import tons of calcium chloride to recover solvents that are on the INCB Red List and are more tightly controlled.[27]

### Metal reduction flux

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

### Medical use

Calcium chloride infusions may be used as an intravenous therapy to prevent hypocalcemia.

## Hazards

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.[28]

Consumption of calcium chloride can lead to hypercalcemia.[29]

## Properties

Flame test of CaCl

Calcium chloride dissolves in water, producing chloride and the aquo complex [Ca(H
2O)
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 CaCl
2 \+ 2 PO3−
4 → Ca
3(PO

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:

CaCl
2 → Ca + Cl

## Preparation

File:Ca(aq)6 improved image.tif

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 + CaCO
3 → Na
2CO
3 \+ CaCl

North American consumption in 2002 was 1,529,000 tonnes (3.37 billion pounds).[30] 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.[10]

### Occurrence

Calcium chloride occurs as the rare evaporite minerals sinjarite (dihydrate) and antarcticite (hexahydrate).[31][32][33] Another natural hydrate known is ghiaraite – a tetrahydrate.[34][33] The related minerals chlorocalcite (potassium calcium chloride, KCaCl
3) and tachyhydrite (calcium magnesium chloride, CaMg
2Cl
6 * 12H
2O) are also very rare.[35][36][33] The same is true for rorisite, CaClF (calcium chloride fluoride).[37][33]

## See also

* Calcium(I) chloride
* Calcium chloride transformation
* Magnesium chloride

## References

1. ↑ 1.0 1.1 1.2 1.3 1.4 1.5 1.6 1.7 1.8 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. ↑ "Calcium chloride (anhydrous)". International Programme on Chemical Safety and the European Commission. http://www.inchem.org/documents/icsc/icsc/eics1184.htm.
3. ↑ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. p. 196. https://archive.org/details/solubilitiesino01seidgoog.
4. ↑ 4.0 4.1 4.2 4.3 4.4 4.5 Anatolievich, Kiper Ruslan. "Properties of substance: calcium chloride". chemister.ru. http://chemister.ru/Database/properties-en.php?dbid=1&id=558.
5. ↑ 5.0 5.1 5.2 5.3 5.4 5.5 Pradyot, Patnaik (2019). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc.. p. 162. ISBN 978-0-07-049439-8.
6. ↑ 6.0 6.1 6.2 6.3 Müller, Ulrich (2006). Inorganic Structural Chemistry (2nd ed.). England: John Wiley & Sons Ltd.. p. 33. ISBN 978-0-470-01864-4. https://books.google.com/books?id=s3KlfXCY11sC&pg=PA33.
7. ↑ 7.0 7.1 7.2 Sigma-Aldrich Co., Calcium chloride.
8. ↑ Donald E. Garrett (2004). Handbook of Lithium and Natural Calcium Chloride. Elsevier. p. 379. ISBN 978-0080472904. https://books.google.com/books?id=Ua2SVcUBHZgC&pg=PA379. Retrieved 2018-08-29. "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. https://www.fishersci.ca/viewmsds.do?catNo=C6143.
10. ↑ 10.0 10.1 10.2 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. ↑ Peck, Eugene L.; Hamilton, J. Hugh; Lewis, John Roberts; Hogan, Mervin B.; Kusian, Ross Northey; Cope, William J. (1954) (in en). Proceedings of the First Annual Heating and Air Conditioning Conference: 1953-1955. University of Utah, Department of Metallurgy. https://books.google.ge/books?id=ZFZLAQAAMAAJ&q=+15th+century.
12. ↑ 12.0 12.1 Hartmann, Philipp Karl (1816) (in la). Pharmacologia Dynamica: Usui Academico Adcommodata. Kupffer et Wimmer. https://books.google.com/books?id=Lx9VAAAAcAAJ&pg=PA299.
13. ↑ Ottley, William Campbell (1826) (in en). A dictionary of chemistry and of mineralogy as connected with it. Murray. https://books.google.com/books?id=5LzUgQngwHgC&pg=PP374.
14. ↑ "Binary Phase diagram: The Calcium Chloride – water system". Aqueous Solutions Aps. October 2016. http://www.phasediagram.dk/binary/calcium_chloride.htm.
15. ↑ "Keeping Things Dry". humantouchofchemistry.com. http://humantouchofchemistry.com/keeping-things-dry.htm.
16. ↑ "Dust: Don't Eat It! Control It!". Road Management & Engineering Journal. US Roads (TranSafety Inc.). 1 June 1998. http://www.usroads.com/journals/rmej/9806/rm980603.htm.
17. ↑ Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, pp. 13–14.
18. ↑ 21 CFR § 184.1193
19. ↑ 7 CFR § 205.602
20. ↑ "Apple Caviar Technique". StarChefs Studio. StarChefs.com. April 2004. http://www.starchefs.com/events/studio/techniques/FAdria/index.shtml.
21. ↑ "Cork Spot and Bitter Pit of Apples", Richard C. Funt and Michael A. Ellis, Ohioline.osu.edu/factsheet/plpath-fru-01
22. ↑ "CPG 7117.02". FDA Compliance Articles. US Food and Drug Administration. March 1995. https://www.fda.gov/ora/compliance_ref/cpg/cpgfod/cpg500-400.html.
23. ↑ "Accelerating Concrete Set Time". Federal Highway Administration. 1 June 1999. http://www.fhwa.dot.gov/infrastructure/materialsgrp/acclerat.htm.
24. ↑ 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.
25. ↑ Koger, Nov 1977, "Calcium Chloride, Practical Necrotizing Agent", Journal of the American Association of Bovine Practitioners (USA), (Nov 1977), v. 12, p. 118–119
26. ↑ 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. PMID 21774835.
27. ↑ Smith, Michael; Simpson, Cam (26 October 2020). "Narcos Are Waging a New Drug War Over a Texas Company's Basic Chemical". https://www.bloomberg.com/news/features/2020-10-26/tetra-s-tti-calcium-chloride-is-fueling-a-cocaine-war-in-south-america.
28. ↑ "Product Safety Assessment (PSA): Calcium Chloride". Dow Chemical Company. 2 May 2006. http://www.dow.com/productsafety/finder/cacl_2.htm.
29. ↑ "Calcium Chloride Possible Side Affects". www.drugs.com. https://www.drugs.com/pro/calcium-chloride.html.
30. ↑ Calcium Chloride SIDS Initial Assessment Profile, UNEP Publications, SIAM 15, Boston, 22–25 October 2002, page 11.
31. ↑ "Sinjarite". www.mindat.org. https://www.mindat.org/min-3673.html.
32. ↑ "Antarcticite". www.mindat.org. https://www.mindat.org/min-251.html.
33. ↑ 33.0 33.1 33.2 33.3 "List of Minerals". www.ima-mineralogy.org. 21 March 2011. https://www.ima-mineralogy.org/Minlist.htm.
34. ↑ "Ghiaraite". www.mindat.org. https://www.mindat.org/min-43592.html.
35. ↑ "Chlorocalcite". www.mindat.org. https://www.mindat.org/min-1020.html.
36. ↑ "Tachyhydrite". www.mindat.org. https://www.mindat.org/min-3865.html.
37. ↑ "Rorisite". www.mindat.org. https://www.mindat.org/min-3446.html.

## External links

* International Chemical Safety Card 1184[yes|permanent dead link|dead link}}]
* 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)"

* v
* t
* e

Calcium compounds

* CaAl2O4
* CaB6
* CaBr2
* Ca(BrO3)2
* CaC2
* CaCN2
* Ca(CN)2
* CaCO3
* CaC2O4
* CaCl2
* Ca(ClO)2
* Ca(ClO3)2
* CaCrO4
* CaF2
* CaH2
* Ca(HCO3)2
* CaH2S2O6
* CaI2
* Ca(IO3)2
* Ca(MnO4)2
* CaN6
* Ca(NO3)2
* CaO
* CaO2
* Ca(OH)2
* CaP
* CaS
* CaSO3
* CaSO4
* CaSe
* CaSi
* CaSi2
* CaTiO3
* Ca2P2O7
* Ca2SiO4
* Ca3Al2O6
* Ca3(AsO4)2
* Ca3(BO3)2
* Ca3(C6H5O7)2
* Ca3N2
* Ca3P2
* Ca4(PO4)2O
* Ca3(PO4)2
* Ca(H2PO4)2
* CaHPO4
* C36H70CaO4

* v
* t
* e

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
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

* v
* t
* e

Mineral supplements (A12)

Major|

| Calcium|

* β-hydroxy-β-methylbutyrate
* carbonate
* chloride
* +cholecalciferol
* citrate
* glubionate
* glucoheptonate
* gluconate#
* glycerylphosphate
* hydroxyapatite
* lactate gluconate
* lactate
* pangamate
* phosphate

|

Magnesium|

* aspartate
* chloride
* citrate
* gluconate
* glycinate
* lactate
* levulinate
* malate
* orotate
* oxide
* pidolate
* sulfate
* taurate

Phosphorus|

* adenosine triphosphate disodium
* hydroxyapatite
* monosodium phosphate

Potassium|

* bicarbonate
* bitartrate
* chloride
* citrate
* gluconate

Sodium|

* chloride
* sulfate

Sulfur|

* L-cysteine
* L-cystine
* L-glutathione
* L-methionine
* methylsulfonylmethane
* N-acetyl-L-cysteine
* R-α-lipoic acid
* S-adenosyl methionine
* taurine

Trace|

| Copper|

* gluconate

|

Iodine|

* potassium iodide

Iron|

* (II) fumarate
* (II) sulfate

Selenium|

* selenate
* selenite

Zinc|

* acetate
* L-aspartate
* L-carnosine
* gluconate
* oxide
* proteinate
* sulfate

Ultratrace|

| Chromium|

* (III) picolinate
* (III) chloride

|

Fluorine|

* fluoride#
* monofluorophosphate

Lithium|

* aspartate
* carbonate
* orotate

Vanadium|

* (IV) sulfate

* #WHO-EM
* ‡Withdrawn from market
* Clinical trials:
* †Phase III
* §Never to phase III

* v
* t
* e

Urologicals, including antispasmodics (G04B)

Acidifiers|

* Ammonium chloride
* Calcium chloride

Urinary antispasmodics
(primarily antimuscarinics)|

* Darifenacin
* Desfesoterodine
* Emepronium
* Fesoterodine
* Flavoxate
* Imidafenacin
* Meladrazine
* Mirabegron
* Oxybutynin
* Propiverine
* Solifenacin
* Terodiline
* Tolterodine
* Trospium chloride

Other urologicals|

* Urea analogues: Acetohydroxamic acid
* Salicylhydroxamic acid

* Other: Collagen
* Dimethyl sulfoxide
* Magnesium hydroxide
* Pentosan polysulfate
* Phenazopyridine
* Phenyl salicylate
* Succinimide

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Original source: https://en.wikipedia.org/wiki/Calcium chloride. Read more

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