Names | |
---|---|
Other names
| |
Identifiers | |
3D model (
JSmol)
|
|
ChEBI | |
ChEMBL | |
ChemSpider | |
ECHA InfoCard | 100.029.007 |
EC Number |
|
KEGG | |
PubChem
CID
|
|
RTECS number |
|
UNII | |
UN number | 1748 2208 |
CompTox Dashboard (
EPA)
|
|
| |
| |
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: | |
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) | |
Flash point | Non-flammable |
Lethal dose or concentration (LD, LC): | |
LD50 (
median dose)
|
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).
|
Calcium hypochlorite is an inorganic compound with chemical formula Ca( Cl O)2, also written as Ca(OCl)2. It is a white solid, although commercial samples appear yellow. It strongly smells of chlorine, owing to its slow decomposition in moist air. This compound is relatively stable as a solid and solution and has greater available chlorine than sodium hypochlorite. [1] "Pure" samples have 99.2% active chlorine. Given common industrial purity, an active chlorine content of 65-70% is typical. [2] It is the main active ingredient of commercial products called bleaching powder, [a] used for water treatment and as a bleaching agent. [3]
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]
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.
Calcium hypochlorite is a general oxidizing agent and therefore finds some use in organic chemistry. [6] For instance the compound is used to cleave glycols, 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]
Calcium hypochlorite is produced industrially by treating moist slaked lime (Ca(OH)2) with chlorine. The one-step reaction is shown below: [3]
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]
Calcium hypochlorite reacts rapidly with acids producing calcium chloride, chlorine gas, and water:[ citation needed]
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]
Assay (iodometric): 67.0 - 75.0 %
{{
cite journal}}
: CS1 maint: multiple names: authors list (
link)
Names | |
---|---|
Other names
| |
Identifiers | |
3D model (
JSmol)
|
|
ChEBI | |
ChEMBL | |
ChemSpider | |
ECHA InfoCard | 100.029.007 |
EC Number |
|
KEGG | |
PubChem
CID
|
|
RTECS number |
|
UNII | |
UN number | 1748 2208 |
CompTox Dashboard (
EPA)
|
|
| |
| |
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: | |
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) | |
Flash point | Non-flammable |
Lethal dose or concentration (LD, LC): | |
LD50 (
median dose)
|
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).
|
Calcium hypochlorite is an inorganic compound with chemical formula Ca( Cl O)2, also written as Ca(OCl)2. It is a white solid, although commercial samples appear yellow. It strongly smells of chlorine, owing to its slow decomposition in moist air. This compound is relatively stable as a solid and solution and has greater available chlorine than sodium hypochlorite. [1] "Pure" samples have 99.2% active chlorine. Given common industrial purity, an active chlorine content of 65-70% is typical. [2] It is the main active ingredient of commercial products called bleaching powder, [a] used for water treatment and as a bleaching agent. [3]
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]
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.
Calcium hypochlorite is a general oxidizing agent and therefore finds some use in organic chemistry. [6] For instance the compound is used to cleave glycols, 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]
Calcium hypochlorite is produced industrially by treating moist slaked lime (Ca(OH)2) with chlorine. The one-step reaction is shown below: [3]
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]
Calcium hypochlorite reacts rapidly with acids producing calcium chloride, chlorine gas, and water:[ citation needed]
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]
Assay (iodometric): 67.0 - 75.0 %
{{
cite journal}}
: CS1 maint: multiple names: authors list (
link)