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| | Chloroacetic acid Basic information |
| | Chloroacetic acid Chemical Properties |
| Melting point | 60-63 °C (lit.) | | Boiling point | 189 °C (lit.) | | density | 1.58 | | vapor density | 3.26 (vs air) | | vapor pressure | 0.75 mm Hg ( 20 °C) | | refractive index | 1.4330 | | Fp | 126°C | | storage temp. | Store below +30°C. | | solubility | Soluble in methanol, acetone, diethyl ether, benzene, chloroform and ethanol. | | pka | 2.85(at 25℃) | | form | Liquid | | color | White | | Odor | Penetrating, burning odor | | PH Range | < 1 at 800 g/l at 20 °C | | explosive limit | 8% | | Water Solubility | SOLUBLE | | Sensitive | Hygroscopic | | Merck | 14,2112 | | Specific Activity | 5-10 Ci/mmol | | Solvent | Sterile water in sealed ampoule | | Concentration | 1 mCi/ml | | BRN | 605438 | | Stability: | Stable. Deliquescent. Incompatible with strong bases, alkalies, most common metals, strong oxidizing agents. | | LogP | 0.49 at 20℃ | | CAS DataBase Reference | 79-11-8(CAS DataBase Reference) | | NIST Chemistry Reference | Acetic acid, chloro-(79-11-8) | | EPA Substance Registry System | Chloroacetic acid (79-11-8) |
| | Chloroacetic acid Usage And Synthesis |
| Description | Chloroacetic acid (CAA) is a monohalogenated acetic acid
(m-HAA) that is used as a photosensitizing agent and in
industrial synthesis of certain organic chemicals such as indigoid
dyes. The m-HAAs are a major class of drinking water
disinfection by-products during chlorination of drinking water. | | Chemical Properties | Chloroacetic acid is a colorless to white crystalline solid. It has a strong vinegar-like odor and an Odor
Threshold of 0.15 milligram per cubic meter. | | Chemical Properties | colourless or white crystals | | Uses | CAA is one of these agents used in the topical treatment of
warts in most European countries and also as an herbicidal
agent and a bleaching agent for silkworm cocoons. It can be
found in wines and beers using static headspace extraction
coupled with gas chromatography–mass spectrometry. CCA is
the main toxic metabolite of vinyl chloride. CAA and volatile
organochlorines are suspected to contribute to forest dieback
and stratospheric ozone destruction. | | Uses | Herbicide, preservative, bacteriostat, intermediate in production of carboxymethylcellulose; ethyl
chloroacetate, glycine, synthetic caffeine, sarcosine, thioglycolic acid, EDTA, 2,4-D, 2,4,5-T. | | Uses | Chloroacetic acid behaves as a very strong monobasic acid and is used as a strong acid catalyst for diverse reactions. The Cl function can be displaced in base-catalyzed reactions. | | Definition | A colorless crystalline
solid made by substituting one of the hydrogen
atoms of the methyl group of
ethanoic acid with chlorine, using red
phosphorus. It is a stronger acid than
ethanoic acid because of the electron-withdrawing
effect of the chlorine atom.
Dichloroethanoic acid (dichloroacetic
acid, CHCl2COOH) and trichloroethanoic
acid (trichloroacetic acid,CCl3COOH) are
made in the same way. The acid strength
increases with the number of chlorine
atoms present. | | Definition | ChEBI: A chlorocarboxylic acid that is acetic acid carrying a 2-chloro substituent. | | Production Methods | Chloroacetic acid can be synthesized by the radical chlorination of acetic acid, treatment of trichloroethylene with concentrated H2SO4, oxidation of 1,2-dichloroethane or chloroacetaldehyde, amine displacement from glycine, or chlorination of ketene. | | General Description | Chloroacetic acid, solution is a colorless solution of the white crystalline solid. The acid concentration can be up to 80%.It is used in manufacturing dyes and in medicine. Chloroacetic acid is toxic by inhalation, ingestion and skin contact. Chloroacetic acid is corrosive to metals and tissue. Chloroacetic acid is used as an herbicide, preservative and bacteriostat.
| | Air & Water Reactions | Water soluble. | | Reactivity Profile | These organic compounds donate hydrogen ions if a base is present to accept them. They react in this way with all bases, both organic (for example, the amines) and inorganic. Their reactions with bases, called "neutralizations", are accompanied by the evolution of substantial amounts of heat. Neutralization between an acid and a base produces water plus a salt. Soluble carboxylic acid dissociate to an extent in water to yield hydrogen ions. The pH of solutions of carboxylic acids is therefore less than 7.0. Carboxylic acids in aqueous solution and liquid or molten carboxylic acids can react with active metals to form gaseous hydrogen and a metal salt. Such reactions occur in principle for solid carboxylic acids as well, but are slow if the solid acid remains dry. Even "insoluble" carboxylic acids may absorb enough water from the air and dissolve sufficiently in Chloroacetic acid to corrode or dissolve iron, steel, and aluminum parts and containers. Carboxylic acids, like other acids, react with cyanide salts to generate gaseous hydrogen cyanide. The reaction is slower for dry, solid carboxylic acids. Flammable and/or toxic gases and heat are generated by the reaction of carboxylic acids with diazo compounds, dithiocarbamates, isocyanates, mercaptans, nitrides, and sulfides. Carboxylic acids, especially in aqueous solution, also react with sulfites, nitrites, thiosulfates (to give H2S and SO3), dithionites (SO2), to generate flammable and/or toxic gases and heat. Their reaction with carbonates and bicarbonates generates a harmless gas (carbon dioxide) but still heat. Like other organic compounds, carboxylic acids can be oxidized by strong oxidizing agents and reduced by strong reducing agents. These reactions generate heat. A wide variety of products is possible. Like other acids, carboxylic acids may initiate polymerization reactions; like other acids, they often catalyze (increase the rate of) chemical reactions. | | Hazard | Use in foods prohibited by FDA. Irritating and corrosive to skin. Upper respiratory tract
irritant. Questionable carcinogen. | | Health Hazard | Inhalation causes mucous membrane irritation. Contact with liquid causes severe irritation and burns of the eyes and irritation and burns of skin. Ingestion causes burns of mouth and stomach. | | Fire Hazard | Special Hazards of Combustion Products: Toxic gases, such as hydrogen chloride, phosgene and carbon monoxide, may be generated. | | Flammability and Explosibility | Nonflammable | | Safety Profile | Poison by ingestion,
inhalation, subcutaneous, and intravenous
routes. A corrosive skin, eye, and mucous
membrane irritant. Questionable carcinogen
with experimental tumorigenic data.
Mutation data reported. Combustible liquid
when exposed to heat or flame. To fight
fire, use water spray, fog, mist, dry chemical, foam. When heated to decomposition it
emits toxic fumes of Cl-. See also
CHLORIDES. | | Potential Exposure | This haloacetic acid can be a byproduct
of drinking water disinfection and may increase the risk of
cancer. Monochloracetic acid is used primarily as a chemical
intermediate in the synthesis of sodium carboxymethyl cellulose; and such other diverse substances as ethyl chloroacetate,
glycine, synthetic caffeine, sarcosine, thioglycolic acid, and
various dyes. Hence, workers in these areas are affected. It is
also used as an herbicide. Therefore, formulators and applicators of such herbicides are affected. | | Environmental Fate | CCA by inhibition of the pyruvate-dehydrogenase, aconitase,
and a-ketoglutarate dehydrogenase that contribute in tricarboxylic
acid cycle and also inhibition of glyceraldehyde-
3-phosphate dehydrogenase can impair production of
cellular energy and conversion to anaerobic glycolysis, resulting
in increasing acidosis with accumulation of glycolic
acid, oxalate, and lactate production. CCA can also affect
cellular components via sulfhydryl groups. Both of these
effects may contribute to central nervous system (CNS),
cardiovascular, renal, and hepatic effects. The metabolites
glycolic acid and oxalate may contribute to CNS and renal
toxicity (myoglobin and oxalate precipitation in the tubuli).
Binding of calcium to oxalates probably causes the hypocalcemia,
but hypocalcemia can be secondary to rhabdomyolysis.
CAA by reduction of cellular glutathione can cause
oxidative stress. Inhibition of mitochondrial aconitase causes
hypoglycemia. | | Shipping | UN1750 (liquid) & UN1751 (solid) Chloroacetic
acid, solid or liquid, Hazard class: 6.1; Labels: 6.1-Poison
Inhalation Hazard, 8-Corrosive material. | | Purification Methods | Crystallise the acid from CHCl3, CCl4, *benzene or water. Dry it over P2O5 or conc H2SO4 in a vacuum desiccator. Further purification is by distillation from MgSO4, and by fractional crystallisation from the melt. Store it under vacuum or under dry N2. [Bernasconi et al. J Am Chem Soc 107 3621 1985, Beilstein 2 IV 474.] | | Toxicity evaluation | Occupational exposure to CAA can occur through inhalation
and dermal contact with this compound at workplaces where
it is produced or used. The general population can be exposed
to CAA via ingestion of chlorinated or chloraminated drinking
water.
The atmospheric photochemical oxidation of some volatile
organochlorine compounds is one source of CAAs in the
environment. CAA can be generated during water disinfection
processes and during metabolic detoxification of industrial
solvents such as trichloroethylene. | | Incompatibilities | Compounds of the carboxyl group react
with all bases, both inorganic and organic (i.e., amines)
releasing substantial heat, water, and a salt that may be
harmful. Incompatible with arsenic compounds (releases
hydrogen cyanide gas), diazo compounds, dithiocarbamates, isocyanates, mercaptans, nitrides, sulfides (releasing
heat, toxic, and possibly flammable gases), thiosulfates,
and dithionites (releasing hydrogen sulfate and oxides of
sulfur). The solution in water is a strong acid. Contact with
strong oxidizers, strong bases; and strong reducing agents
such as hydrides can cause violent reactions. Chloracetic
acid decomposes on heating, producing toxic and corrosive
hydrogen chloride, phosgene, and carbon monoxide gases.
Attacks metals in the presence of moisture. | | Waste Disposal | Incineration, preferably after
mixing with another combustible fuel; care must be exercised to assure complete combustion to prevent the formation of phosgene; an acid scrubber is necessary to remove
the halo acids produced. |
| | Chloroacetic acid Preparation Products And Raw materials |
| Raw materials | Hydrochloric acid-->Acetic acid-->Chlorine-->Sulfur-->2-Chloroethanol-->Trichloroethylene-->Disulfur dichloride-->Trichloroacetic acid-->Glycolic acid-->Dichloroacetic acid-->1,1,2,2-Tetrachloroethane-->Dichloroacetic acid methyl ester | | Preparation Products | 2-Benzofurancarboxaldehyde-->Sodium edetate-->Acetochlor E.C.-->2-Quinoxalinone-->ORALITH BRILLIANT PINK R-->N-METHYL-N-PHENYL-2-PIPERAZIN-1-YLACETAMIDE-->2,4-Dichlorophenoxyacetic acid-->MALONIC ACID DISODIUM SALT-->[(2-OXO-2H-CHROMEN-7-YL)OXY]ACETIC ACID-->Phenoxyacetic acid-->Dichloroacetic acid methyl ester-->Diisopropyl malonate-->Diethyl ethylmalonate-->Nitrilotriacetic acid-->Methoxyacetyl chloride-->Propacetamol-->EDTA ferric sodium salt-->Synthetic greasing agent-->2,4-Dichlorophenoxybutyric acid-->ETHYL O-CARBOETHOXYMETHYLSALICYLATE-->4-Chlorophenoxyacetic acid-->2-(CARBOXYMETHYLTHIO)-4,6-DIMETHYLPYRIMIDINE MONOHYDRATE-->(METHYLTHIO)ACETIC ACID-->3-(2,4-difluorophenoxy)propanoic acid-->2-Nitrophenoxyacetic acid-->Iodoacetic acid-->S-Carboxymethyl-L-Cysteine-->2-Methyl-4-chlorophenoxyacetic acid-->2-Chloro-3',4'-dihydroxyacetophenone-->(1-METHYL-1H-BENZIMIDAZOL-2-YL)METHYLAMINE-->Ethionine ester-->N-Methylmethanamine 2,4-dichlorophenoxyacetate-->sulfate AEC-->Betaine hydrochloride-->2-Hydrazinyl-N,N-dimethylacetamide-->2-Hydrazinyl-N-methylacetamide-->2-Hydrazinylacetamide-->1-NAPHTHOXYACETIC ACID-->Sodium glycolate-->instant soluble Tian-jing gum |
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