Calcium hypochlorite

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Calcium hypochlorite
Calcium oxychloride
Names
Other names
  • Hypochlorous acid calcium salt
  • Bleaching powder
  • Chloride of lime
Identifiers
3D model (
JSmol
)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard
 100.029.007 Edit this at Wikidata
EC Number
  • 231-908-7
KEGG
RTECS number
  • NH3485000
UNII
UN number 1748 2208
  • InChI=1S/Ca.2ClO/c;2*1-2/q+2;2*-1 checkY
    Key: ZKQDCIXGCQPQNV-UHFFFAOYSA-N checkY
  • InChI=1S/Cacl.ClO/c;1-2/q+2;2*-1
    Key: ZKQDCIXGCQPQNV-UHFFFAOYAV
  • Cl[O-].[Ca+2].Cl[O-]
Properties
Ca(OCl)2
Molar mass 142.98 g·mol−1
Appearance white/gray powder
Density 2.35 g/cm3 (20 °C)
Melting point 100 °C (212 °F; 373 K)
Boiling point 175 °C (347 °F; 448 K) decomposes
21 g/(100 mL) at 25 °C
Solubility reacts in alcohol
Hazards
GHS labelling:
GHS03: OxidizingGHS05: CorrosiveGHS07: Exclamation markGHS09: Environmental hazard
Danger
H272, H302, H314, H400
P210, P220, P221, P260, P264, P270, P273, P280, P301+P312, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P330, P363, P370+P378, P391, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
1
OX
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
850 mg/kg (oral, rat)
Safety data sheet (SDS) ICSC 0638
Related compounds
Other anions
Other cations
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Calcium hypochlorite is an

bleaching agent.[3]

History

Charles Tennant and Charles Macintosh developed an industrial process in the late 18th century for the manufacture of chloride of lime, patenting it 1799.[4] Tennant's process is essentially still used today,[4][3] and became of military importance during World War I, because calcium hypochlorite was the active ingredient in trench disinfectant.[4]

Uses

Sanitation

Calcium hypochlorite is commonly used to sanitize public swimming pools and disinfect drinking water. Generally the commercial substances are sold with a purity of 65% to 73% with other chemicals present, such as calcium chloride and calcium carbonate, resulting from the manufacturing process. In solution, calcium hypochlorite could be used as a general purpose sanitizer,[5] but due to calcium residue (making the water harder), sodium hypochlorite (bleach) is usually preferred.

Organic chemistry

Calcium hypochlorite is a general

α-hydroxy carboxylic acids and keto acids to yield fragmented aldehydes or carboxylic acids.[7] Calcium hypochlorite can also be used in the haloform reaction to manufacture chloroform.[8]
Calcium hypochlorite can be used to oxidize thiol and sulfide byproducts in organic synthesis and thereby reduce their odour and make them safe to dispose of.[9] The reagent used in organic chemistry is similar to the sanitizer at ~70% purity.[10]

Production

Calcium hypochlorite is produced industrially by treating moist slaked lime (Ca(OH)2) with chlorine. The one-step reaction is shown below:[3]

2 Cl2 + 2 Ca(OH)2 → CaCl2 + Ca(OCl)2 + 2 H2O

Industrial setups allow for the reaction to be conducted in stages to give various compositions, each producing different ratios of calcium hypochlorite, unconverted lime, and calcium chloride.[3] In one process, the chloride-rich first stage water is discarded, while the solid precipitate is dissolved in a mixture of water and lye for another round of chlorination to reach the target purity.[2] Commercial calcium hypochlorite consists of anhydrous Ca(OCl)2, dibasic calcium hypochlorite Ca3(OCl)2(OH)4 (also written as Ca(OCl)2·2Ca(OH)2), and dibasic calcium chloride Ca3Cl2(OH)4 (also written as CaCl2·2Ca(OH)2).[11][12]

Reactions

Calcium hypochlorite reacts rapidly with acids producing calcium chloride, chlorine gas, and water:[citation needed]

Ca(ClO)2 + 4 HCl → CaCl2 + 2 Cl2 + 2 H2O

Safety

It is a strong oxidizing agent, as it contains a hypochlorite ion at the valence +1 (redox state: Cl+1).[citation needed]

Calcium hypochlorite should not be stored wet and hot, or near any acid, organic materials, or metals. The unhydrated form is safer to handle.[citation needed]

See also

References

  1. ^ also chlorine powder, chloride of lime, chlorinated lime, "dry chlorine"
  1. ^ Gerald F. Connell. "Key operating strategies for chlorine disinfection operating systems" (PDF). Retrieved 19 October 2014.
  2. ^ a b "Calcium Hypochlorite - 3V Tech". www.3v-tech.com.
  3. ^
    S2CID 96905077
    .
  4. ^ a b c "Calcium hypochlorite". Chemistry World.
  5. ^ Chemical Products Synopsis: Calcium Hypochlorite (Technical report). Asbuiy Park, NJ: Mannsvile Chemical Products. 1987.
  6. doi:10.1016/S0040-4039(00)88577-9
    .
  7. doi:10.1016/S0040-4039(00)88578-0
    .
  8. ^ Cohen, Julius (1900). Practical Organic Chemistry for Advanced Students. New York: Macmillan & Co. p. 63.
  9. ISBN 978-0-309-05229-0
    .
  10. ^ "8.41799 Calcium hypochlorite for synthesis". Sigma-Aldrich. Assay (iodometric): 67.0 - 75.0 %
  11. ISBN 978-0-8247-0349-3
  12. ^ Aleksandrova, M.M.; Dmitriev, G.A.; Avojan, R.L. (1968). "The probable model of the crystal structure of the twobase calcium hypochlorite". Armyanskii Khimicheskii Zhurnal. 21: 380-386.{{cite journal}}: CS1 maint: multiple names: authors list (link)

External links

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