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)
−5.47·10−5cm3/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⦵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
ATC code
A12AA07 (WHO) B05XA07 (WHO), G04BA03 (WHO)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Irritant
GHS labelling:
Pictograms
[7]
Signal word
Warning
Hazard statements
H319[7]
Precautionary statements
P305+P351+P338[7]
NFPA 704 (fire diamond)
[9]
2
0
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
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Nverify (what is YN ?)
Infobox references
Chemical compound
Calcium chloride is an inorganic compound, a salt with the chemical formula CaCl2. 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 CaCl2·nH2O, 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]
^ abcdefghiLide DR, ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
^"Calcium chloride (anhydrous)". ICSC. International Programme on Chemical Safety and the European Commission. Archived from the original on 25 September 2015. Retrieved 18 September 2015.
^Seidell A, Linke WF (1919). Solubilities of Inorganic and Organic Compounds (second ed.). New York: D. Van Nostrand Company. p. 196.
^ abcdefAnatolievich KR. "Properties of substance: calcium chloride". chemister.ru. Archived from the original on 24 June 2015. Retrieved 7 July 2014.
^ abcdefPradyot P (2019). Handbook of Inorganic Chemicals. The McGraw-Hill Companies, Inc. p. 162. ISBN 978-0-07-049439-8.
^ abcdMüller U (2006). Inorganic Structural Chemistry (second ed.). England: John Wiley & Sons Ltd. p. 33. ISBN 978-0-470-01864-4.
^ abcSigma-Aldrich Co., Calcium chloride.
^Garrett DE (2004). Handbook of Lithium and Natural Calcium Chloride. Elsevier. p. 379. ISBN 978-0-08-047290-4. Archived from the original on 31 October 2023. 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...)
^"MSDS of Calcium chloride". fishersci.ca. Fisher Scientific. Archived from the original on 25 September 2015. Retrieved 7 July 2014.
^Robert Kemp, Suzanne E. Keegan "Calcium Chloride" in Ullmann's Encyclopedia of Industrial Chemistry 2000, Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_547
Calciumchloride is an inorganic compound, a salt with the chemical formula CaCl2. It is a white crystalline solid at room temperature, and it is highly...
chemicals present, such as calciumchloride and calcium carbonate, resulting from the manufacturing process. In solution, calcium hypochlorite could be used...
Other examples of ionic chlorides are sodium chloride NaCl, calciumchloride CaCl2 and ammonium chloride [NH4]Cl. The chloride is also a neutral chlorine...
Ca(OH)2 → CaO + H2O Calcium hydroxide reacts with hydrogen chloride to first give calcium hydroxychloride and then calciumchloride. Calcium hydroxide adopts...
of calcium include calciumchloride and calcium gluconate. The forms that are taken by mouth include calcium acetate, calcium carbonate, calcium citrate...
when magnesium chloride and salt are mixed together before they are loaded onto trucks and spread onto paved roads. Calciumchloride damages concrete...
soap, and aluminium etc. Sodium chloride is used in the Solvay process to produce sodium carbonate and calciumchloride. Sodium carbonate, in turn, is...
general use could worsen outcomes. If calcium is used, calciumchloride is generally the recommended form. Calcium gluconate side effects include nausea...
Calcium alginate is a water-insoluble, gelatinous, cream-coloured substance that can be created through the addition of aqueous calciumchloride to aqueous...
such as calciumchloride. It is used in photography. It is also used in cat food as a source of iodine. Henri Moissan first isolated pure calcium in 1898...
eliminating the production of calciumchloride, since ammonia no longer needs to be regenerated. The by-product ammonium chloride can be sold as a fertilizer...
dust-suppression techniques are the application of a chloride solution (calciumchloride, magnesium chloride, sodium chloride), the application of a resin compound,...
intermediate between those for barium chloride, which is more toxic, and calciumchloride. Strontium chloride can be prepared by treating aqueous strontium...
high in iron, and can have a high calcium or magnesium content depending on the coagulants (e.g. calciumchloride, calcium sulphate, magnesium sulphate) used...
calcium hydroxide depositing on the cathode, preventing the flow of current. When concentrated solutions of calcium chlorate and potassium chloride are...
Isopropyl chloride can be easily produced in the lab by reacting concentrated hydrochloric acid with isopropyl alcohol in the presence of a calciumchloride or...
much electrolyte.[citation needed] Examples of electrolytes include calcium, chloride, magnesium, phosphate, potassium, and sodium. Electrolyte disturbances...
Calcium hydroxychloride or calciumchloride hydroxide is an inorganic compound with the chemical formula Ca(OH)Cl. It consists of calcium cations (Ca2+)...
as muriatic acid or spirits of salt, is an aqueous solution of hydrogen chloride (HCl). It is a colorless solution with a distinctive pungent smell. It...
between barium sulfide and hydrogen chloride: BaS + 2 HCl → BaCl2 + H2S or between barium sulfide and calciumchloride: BaS + CaCl2 → CaS + BaCl2 In place...
with a high-concentration solution of salt (typically sodium chloride or calciumchloride). In diverse contexts, brine may refer to the salt solutions...
magnesium a person is getting. Treatment when levels are very high include calciumchloride, intravenous normal saline with furosemide, and hemodialysis. Hypermagnesemia...
hydrogen, and chlorine result. When using calciumchloride or potassium chloride, the products contain calcium or potassium instead of sodium. Related processes...
is with intravenous calciumchloride and possibly magnesium sulfate. Other treatments may include vitamin D, magnesium, and calcium supplements. If due...
chloride is used in some de-icing products designed to be safer for pets and plants, though these are inferior in melting quality to calciumchloride...
Initial treatment in those with ECG changes is salts, such as calcium gluconate or calciumchloride. Other medications used to rapidly reduce blood potassium...