8013-54-5

Usage

Uses

Used in Pharmaceutical Industry:
Chloroform is used as a solvent for the extraction and purification of various organic compounds, including pharmaceuticals. Its ability to dissolve a wide range of substances makes it a valuable tool in the synthesis and production of drugs.
Used in Chemical Industry:
Chloroform is used as an intermediate in the production of various chemicals, such as pesticides, dyes, and plastics. Its versatility as a chemical building block contributes to its widespread use in the chemical industry.
Used in Analytical Chemistry:
Chloroform is used as a reference material in gas chromatography and other analytical techniques. Its distinct properties, such as its boiling point and polarity, make it useful for calibrating instruments and ensuring accurate measurements.
Used in Research:
Chloroform is used as a reagent and solvent in various research applications, including organic synthesis, biochemical studies, and materials science. Its unique properties allow researchers to explore new reactions and develop innovative solutions to scientific challenges.

Potential Exposure

Chloroform was one of the earliest general anesthetics, but its use for this purpose has been abandoned because of toxic effects. Chloroform is widelyused as a solvent (especially in the lacquer industry); in the extraction and purification of penicillin and other pharmaceuticals; in the manufacture of artificial silk, propellents, plastics, floor polishes, and fluorocarbons (R-22); and in sterilization of catgut. Chemists and support workers as well as hospital workers are believed to be at a higher risk than the general population. Chloroform is widely distributed in the atmosphere and water (including municipal drinking water primarily as a consequence of chlorination). A survey of 80 American cities by EPA found chloroform in every water system in levels ranging from ,0.3 to 311 ppb.

Shipping

UN1888 Chloroform, Hazard Class: 6.1; Labels: 6.1-Poisonous materials.

Incompatibilities

Though nonflammable, chloroform decomposes to form hydrogen chloride, phosgene, and chlorine upon contact with a flame. Chloroform decomposes slowly in air and light. Reacts violently with strong caustics (bases), strong oxidants, chemically active metals (especially powders), such as aluminum, lithium, magnesium, potassium, and sodium, causing fire and explosion hazard. Attacks plastic, rubber, and coatings. Corrodes iron and other 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. Where possible it should be recovered, purified by distillation, and returned to the supplier.

Upstream product

• 110-86-1 pyridine 
• 117889-84-6 2-trichloromethyl-[1,3]dioxolan-2-ol 
• 67-56-1 methanol 
• 56-23-5 tetrachloromethane 
• 2229-07-4 methyl radical 
• 64-17-5 ethanol 
• 74-98-6 propane 
• 110-05-4 di-tert-butyl peroxide 
• 75-28-5 Isobutane 
• 16841-51-3 3,4-dihydro-2H-thiopyran 1,1-dioxide 
• 515-83-3 chloral ethyl hemiacetal 
• 127-09-3 sodium acetate 
• 79-36-7 dichloroacethyl chloride 
• 74-87-3 methylene chloride 

Downstream Products

• 10022-13-6 1,3,4,6-tetra-O-acetyl-2-deoxy-2-phthalimido-β-D-glucopyranose 
• 66674-15-5 methyl 4,6-O-benzylidene-3-O-(p-tolylsulfonyl)-α-D-glucopyranoside 
• 223606-07-3 (R,S)-N-1-(phenoxy)-2-aminobutane 
• 23703-03-9 2,5-diethyl-piperazine 
• 4982-08-5 1-hydroxy-3-phenylpropan-2-one 
• 860729-68-6 9-benzyl-1,5-dichloro-10-piperidino-9,10-dihydro-[9]anthrol 
• 26211-73-4 (2-methyl-1H-indol-3-yl)phenylmethanone 
• 30319-44-9 1,2,3,4-tetra-O-benzoyl-α-D-xylopyranose 
• 103728-81-0 penta-O-benzoyl-aldehydo-D-glucose-diethyldithioacetal 
• 16752-01-5 tri-O-benzoyl-L-threonic acid isopropyl ester 
• 93324-55-1 1-iodo-2,3-bis-(4-nitro-benzoyloxy)-propane 

Relevant academic research and scientific papers

Synthesis of Decorated Carbon Structures with Encapsulated Components by Low-Voltage Electric Discharge Treatment

Abstract: Polycondensation of complexes of chloromethanes with triphenylphosphine by the action of low-voltage electric discharges in the liquid phase gives nanosized solid products. The elemental composition involving the generation of element distribution maps (scanning electron microscopy–energy dispersive X?ray spectroscopy mapping) and the component composition (by direct evolved gas analysis–mass spectrometry) of the solid products have been studied. The elemental and component compositions of the result-ing structures vary widely depending on the chlorine content in the substrate and on the amount of triphenylphosphine taken. Thermal desorption analysis revealed abnormal behavior of HCl and benzene present in the solid products. In thermal desorption spectra, these components appear at an uncharacteristically high temperature. The observed anomaly in the behavior of HCl is due to HCl binding into a complex of the solid anion HCI-2 with triphenyl(chloromethyl)phosphonium chloride, which requires a relatively high temperature (up to 800 K) to decompose. The abnormal behavior of benzene is associated with its encapsulated state in nanostructures. The appearance of benzene begins at 650 K and continues up to temperatures above 1300?K.

Revisiting Alkane Hydroxylation with m-CPBA (m-Chloroperbenzoic Acid) Catalyzed by Nickel(II) Complexes

Mechanistic studies are performed on the alkane hydroxylation with m-CPBA (m-chloroperbenzoic acid) catalyzed by nickel(II) complexes, NiII(L). In the oxidation of cycloalkanes, NiII(TPA) acts as an efficient catalyst with a high yield and a high alcohol selectivity. In the oxidation of adamantane, the tertiary carbon is predominantly oxidized. The reaction rate shows first-order dependence on [substrate] and [NiII(L)] but is independent on [m-CPBA]; vobs=k2[substrate][NiII(L)]. The reaction exhibited a relatively large kinetic deuterium isotope effect (KIE) of 6.7, demonstrating that the hydrogen atom abstraction is involved in the rate-limiting step of the catalytic cycle. Furthermore, NiII(L) supported by related tetradentate ligands exhibit apparently different catalytic activity, suggesting contribution of the NiII(L) in the catalytic cycle. Based on the kinetic analysis and the significant effects of O2 and CCl4 on the product distribution pattern, possible contributions of (L)NiII?O. and the aroyloxyl radical as the reactive oxidants are discussed.

A process of preparing methyl chloride using multistage reaction

The present invention relates to a method of producing methyl chloride by multistage reactions. The method of the present invention comprises: a) a chlorination step for sufficiently increasing the conversion rate of methane, which is an initial reactant; and b) a subsequent reaction step for actively utilizing hydrogen chloride (HCl), which is a hazardous byproduct of chlorination, efficiently treating harmful hydrogen chloride, and at the same time, improving the overall production of methyl chloride.COPYRIGHT KIPO 2020

PRODUCTION OF CARBON TETRACHLORIDE FROM NATURAL GAS

The present invention provides processes to prepare carbon tetrachloride by the chlorination of natural gas in the presence of a diluent.

Control of methane chlorination with molecular chlorine gas using zeolite catalysts: Effects of Si/Al ratio and framework type

CH4 chlorination with Cl2 gas is used for the production of chlorinated products via C–H bond activation in CH4. Due to the high reactivity of Cl2, this reaction can occur spontaneously under UV irradiation or with mild thermal energy even in the absence of a catalyst via a free radical-mediated chain reaction mechanism that undesirably causes excessive chlorination of the CH4 and is thus non-selective. In this work, CH4 chlorination is investigated using HY and MFI zeolites with various Si/Al ratios, by which the reaction is catalytically controlled for selective production of the mono-chlorinated product (CH3Cl). Depending on the framework type, Si/Al ratio of the zeolites, and reaction conditions, different degrees of CH4 conversion, CH3Cl selectivity, and hence CH3Cl yield were achieved, by which systematic relationships between the catalyst properties and performance were discovered. A high aluminum content facilitated the production of CH3Cl with up to ～20 % yield at a high gas hourly space velocity of 2400 cm3gcat?1 h?1 with a CH4/Cl2 ratio of 1 at 350 °C. HY zeolites generally furnished a slightly higher CH3Cl yield than MFI zeolites, which can be attributed to the larger micropores of the HY zeolites that support facile molecular diffusion. With various flow rates and ratios of CH4 and Cl2, the CH4 conversion and CH3Cl selectivity changed simultaneously, with a trade-off relationship. Unfortunately, all zeolite catalysts suffered from framework dealumination due to the HCl produced during the reaction, but it was less pronounced for the zeolites having a low aluminum content. The results shed light on the detailed roles of zeolites as solid-acid catalysts in enhancing CH3Cl production during electrophilic CH4 chlorination.

Reaction of Lithium Acylate α-Carbanions with Carbon Tetrachloride

Metalation of acetic, butanoic, or 2-methylpropanoic acid with lithium diisopropylamide in tetrahydrofuran under argon gave the corresponding lithium acylate α-carbanions which reacted with carbon tetrachloride at 20–25°C for 2 h to afford butanedioic acid or its 2,3-diethyl and 2,2,3,3-tetramethyl derivatives, as well as the corresponding α-chlorocarboxylic acids and chloroform. A radical mechanism was proposed for the formation of dicarboxylic and α-chlorocarboxylic acids.

Photocatalytic degradation of gaseous trichloroethylene on porous titanium dioxide pellets modified with copper(II) under visible light irradiation

Porous titanium dioxide pellets modified with copper(II) ion (Cu-TiO2) were synthesized by sol-gel method with dialysis for photocatalytic degradation of gaseous trichloroethylene (TCE) under visible light (VL) irradiation. TCE was completely degraded by passing the gas stream (mole fractions of oxygen and TCE were 0.2 and 1.75 × 10?4, respectively) at the flow rate of 25 mL min?1 through 0.2 g of the Cu-TiO2 pellets (Cu content: 0.1 atom%) calcined at 200 °C. TCE was converted mainly to carbon dioxide, dichloroacetic acid (DCAA), and inorganic chlorine species. Relatively small quantities of pentachloroethane (PCA) and trichloroacetaldehyde (TCAH) were detected as products on the Cu-TiO2 surface. Comparison with porous TiO2 pellets under ultraviolet irradiation revealed that more chlorinated products and less carbon dioxide were formed on Cu-TiO2 under VL irradiation. The mineralization of TCE to carbon dioxide was calculated to be only ca. 30.0%. It is noted that DCAA, PCA and TCAH were accumulated on the surface and were extracted with ethyl acetate. The porous Cu-TiO2 pellets show promise as the photocatalyst acting under VL irradiation for converting TCE gas to chlorinated compounds which can be used in industries.

Nb-doped variants of high surface aluminium fluoride: A very strong bi-acidic solid catalyst

A niobium doped high surface aluminium fluoride (HS-AlF3) catalyst was prepared, using an approach in which niobium doped aluminium hydroxide fluoride obtained via reaction of aqueous HF with the respective metal alkoxides in isopropanol is further fluorinated under flow of CHClF2 at 200 °C. A comparable procedure was used to synthesize a Nb-free variant for comparison. Both catalysts exhibit very strong Lewis acidic surface sites which are capable to activate strong carbon-halogen bonds at room temperature, just as the classical high-surface AlF3 (HS-AlF3), obtained by reacting aluminium isopropoxide with anhydrous HF, does. The catalysts were characterized by elemental analysis, P-XRD, MAS NMR spectroscopy, N2 adsorption, NH3-TPD, and pyridine photoacoustic FT-IR spectroscopy. In contrast to previously reported niobium doped HS-AlF3, which was prepared using anhydrous HF, the doped catalyst obtained via this aqueous HF-route shows excellent performance both in the isomerization of 1,2-dibromohexafluoropropane, a reaction that occurs only in the presence of the strongest Lewis acids, and in the cyclization of citronellal to isopulegol, a reaction which requires both, Lewis and Br?nsted acid sites.

METHOD OF CONVERTING ALKANES TO ALCOHOLS, OLEFINS AND AROMATICS

A cost-effective and energy-efficient process is disclosed for converting a methane-containing gas to a methane sulfonyl halide comprising reacting the methane-containing gas, under illumination by a light emitting diode (LED) source, with a sulfuryl halide or a halogen in the presence of sulfur dioxide, whereby the methane sulfonyl halide is obtained for isolation or further reactions. The further reactions may sequentially include, in order, contacting the methane sulfonyl halide with a catalyst complex to form a methane monohalide; catalytically converting the methane monohalide to a value-added chemical such as an alcohol, an olefin, an aromatic, derivatives thereof, or mixtures thereof; releasing any hydrogen halide formed in the process; and converting the hydrogen halide to a halogen and recycling it for re-use.

Activation of Chlorinated Methanes at the Surface of Nanoscopic Lewis Acidic Aluminum Fluorides

We report on the activation of chlorinated methanes by the heterogeneous catalysts aluminum chlorofluoride (ACF) and high-surface aluminum fluoride (HS-AlF3) under moderate conditions. For comparison, chlorinated toluenes and 1,2-dichloroethane