Calcium hydroxychloride

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Not to be confused with calcium hypochlorite.
Calcium hydroxychloride
Names
IUPAC name
Calcium chloride hydroxide[1]
Other names
  • Calcium chloride hydroxide (1/1/1)[1]
  • Calcium hydroxychloride
Identifiers
3D model (JSmol)
  • InChI=1S/Ca.ClH.H2O/h;1H;1H2/q+2;;/p-2
    Key: CTUDRLGCNRAIEA-UHFFFAOYSA-L
  • [OH-].[Cl-].[Ca+2]
Properties
Ca(OH)Cl
Molar mass 92.54 g·mol−1
Appearance white solid
Density 2.4 g/cm3[2]
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Calcium hydroxychloride or calcium chloride hydroxide is an inorganic compound with the chemical formula Ca(OH)Cl. It consists of calcium cations (Ca2+) and chloride (Cl−) and hydroxide (−OH) anions. A white solid, it forms by the reaction of hydrogen chloride with calcium hydroxide[3] According to X-ray crystallography, it adopts a layered structure related to brucite (magnesium hydroxide, Mg(OH)2).[4]

Calcium hydroxychloride is sometimes confused with calcium hypochlorite. Calcium hydroxychloride is a double salt, which consists of calcium cations Ca2+ and two kinds of anions, chloride Cl− and hydroxide −OH, while calcium hypochlorite consists of calcium cations Ca2+ and only one kind of anions, hypochlorite −OCl.

Calcium hydroxychloride may form on concrete roads and bridges as a consequence of the use of calcium chloride as a deicing agent. Calcium chloride reacts with calcium hydroxide (portlandite) present in cement hydration products and forms a deleterious expanding phase also named CAOXY (abbreviation for calcium oxychloride) by concrete technologists. The stress induced into concrete by crystallisation pressure and CAOXY salt expansion can considerably reduce the strength of concrete.[5][6]

References

  1. ^ a b https://pubchem.ncbi.nlm.nih.gov/compound/Calcium-chloride-hydroxide-_1_1_1
  2. ^ Westman, Sven; Werner, Per-Erik; Schuler, Thomas; Raldow, Wiktor; Nielsen, P. H. (1981). "X-Ray Investigations of Ammines of Alkaline Earth Metal Halides. I. The Structures of CaCl2(NH3)8, CaCl2(NH3)2 and the Decomposition Product CaClOH". Acta Chemica Scandinavica. 35a: 467–472. doi:10.3891/acta.chem.scand.35a-0467.
  3. ^ Bausach, M.; Krammer, G.; Cunill, F. (2004). "Reaction of Ca(OH)2 with HCL in the presence of water vapour at low temperatures". Thermochimica Acta. 421 (1–2): 217–223. doi:10.1016/j.tca.2004.04.011.
  4. ^ Oswald, H. R.; Feitknecht, W. (1961). "Über die Hydroxidchloride Me(OH)Cl. (Me = Mg, Ni, Co, Cu, Zn, Fe, Mn, Cd, Ca, Sn)". Helvetica Chimica Acta. 44 (3): 847–858. doi:10.1002/hlca.19610440329.
  5. ^ "Calcium-munching bacteria could be a secret weapon against road salt eating away at concrete roads and bridges". The Conversation. Retrieved 7 April 2019.
  6. ^ Suraneni, Prannoy; Monical, Jonathan; Unal, Erol; Farnam, Yaghoob; Weiss, Jason (2017). "Calcium Oxychloride Formation Potential in Cementitious Pastes Exposed to Blends of Deicing Salt". ACI Materials Journal. 114 (4). doi:10.14359/51689607.
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