Vanadium Chloroperoxidases: The Missing Link in the Formation of Chlorinated Compounds and Chloroform in the Terrestrial Environment?

It is well established that the majority of chlorinated organic substances found in the terrestrial environment are produced naturally. The presence of these compounds in soils is not limited to a single ecosystem. Natural chlorination is also a widespread phenomenon in grasslands and agricultural soils typical for unforested areas. These chlorinated compounds are formed from chlorination of natural organic matter consisting of very complex chemical structures, such as lignin. Chlorination of several lignin model compounds results in the intermediate formation of trichloroacetyl-containing compounds, which are also found in soils. These decay, in general, through a haloform-type reaction mechanism to CHCl3 . Upon release into the atmosphere, CHCl3 will produce chlorine radicals through photolysis, which will, in turn, lead to natural depletion of ozone. There is evidence that fungal chloroperoxidases able to produce HOCl are involved in the chlorination of natural organic matter. The objective of this review is to clarify the role and source of the various chloroperoxidases involved in the natural formation of CHCl3 .

Decarboxylation without CO2: why bicarbonate forms directly as trichloroacetate is converted to chloroform.

Patterns in the observed catalysis of decarboxylation reactions required us to conclude that these reactions involve initial hydration of the carboxylate and subsequent loss of bicarbonate. This raises the important and general question of why CO2 is not formed directly. Reaction profiles for the direct decarboxylation of trichloroacetate were generated with DFT calculations and show no significant barrier to the recombination of the incipient trichloromethide and CO2. In contrast, cleavage of the C-C bond from the hydrated intermediate shows a substantial barrier to recombination that allows separation of the products. The free energy of the transition state for C-C bond cleavage following hydration is higher than the free energy for formation of the hydrate and is comparable to the free energy of activation for direct decarboxylation. Thus, we conclude that the advantage of the hydrolytic pathway is that it provides a means to overcome the problems of separation and solvation that hinder the direct loss of CO2. The resulting concepts are readily extended to explicating the mechanisms of processes in enzymic catalysis as well as providing a basis for producing C-C bonds by the addition of derivatives of carbanions to carbonates.

Influencing factors of disinfection byproducts formation during chloramination of Cyclops metabolite solutions.

Effects of reaction time, chlorine dosage, pH and temperature on the formation of disinfection byproducts (DBPs), were investigated during the chloramination of Cyclops metabolite solutions. The results showed that some species of DBPs like trichloromethane (TCM), dichloroacetic acid (DCAA) and trichloroacetic acid (TCAA) could accumulate to their respective stable values with a progressive elevation in reaction time and monochloramine concentration. And 1,1,1-2-trichloropropanone (1,1,1-TCP) content decreased correspondingly with a continuous increase of reaction time. The amounts of chloral hydrate (CH), chloropicrin (TCNM), 1,1,1-TCP and DCAA firstly increased and then decreased with increasing monochloramine doses. Higher temperature resulted in a decrease of CH, dichloroacetonitrile (DCAN), 1,1-dichloropropanone (1,1-DCP), 1,1,1-TCP, DCAA and TCAA concentration. pH affected the formation of the different DBPs distinctly. TCM accumulateded with the increase of pH under 9, and DCAA, TCAA, CH and 1,1-DCP decreased continuously with increasing pH from 5 to 10, and other DBPs had the maximum concentrations at pH 6-7.

Early drug discovery and the rise of pharmaceutical chemistry.

Studies in the field of forensic pharmacology and toxicology would not be complete without some knowledge of the history of drug discovery, the various personalities involved, and the events leading to the development and introduction of new therapeutic agents. The first medicinal drugs came from natural sources and existed in the form of herbs, plants, roots, vines and fungi. Until the mid-nineteenth century nature's pharmaceuticals were all that were available to relieve man's pain and suffering. The first synthetic drug, chloral hydrate, was discovered in 1869 and introduced as a sedative-hypnotic; it is still available today in some countries. The first pharmaceutical companies were spin-offs from the textiles and synthetic dye industry and owe much to the rich source of organic chemicals derived from the distillation of coal (coal-tar). The first analgesics and antipyretics, exemplified by phenacetin and acetanilide, were simple chemical derivatives of aniline and p-nitrophenol, both of which were byproducts from coal-tar. An extract from the bark of the white willow tree had been used for centuries to treat various fevers and inflammation. The active principle in white willow, salicin or salicylic acid, had a bitter taste and irritated the gastric mucosa, but a simple chemical modification was much more palatable. This was acetylsalicylic acid, better known as Aspirin®, the first blockbuster drug. At the start of the twentieth century, the first of the barbiturate family of drugs entered the pharmacopoeia and the rest, as they say, is history.

Chlorination of chlortoluron: kinetics, pathways and chloroform formation.

Chlortoluron chlorination is studied in the pH range of 3-10 at 25 ± 1°C. The chlorination kinetics can be well described by a second-order kinetics model, first-order in chlorine and first-order in chlortoluron. The apparent rate constants were determined and found to be minimum at pH 6, maximum at pH 3 and medium at alkaline conditions. The rate constant of each predominant elementary reactions (i.e., the acid-catalyzed reaction of chlortoluron with HOCl, the reaction of chlortoluron with HOCl and the reaction of chlortoluron with OCl(-)) was calculated as 3.12 (± 0.10)×10(7)M(-2)h(-1), 3.11 (±0.39)×10(2)M(-1)h(-1) and 3.06 (±0.47)×10(3)M(-1)h(-1), respectively. The main chlortoluron chlorination by-products were identified by gas chromatography-mass spectrometry (GC-MS) with purge-and-trap pretreatment, ultra-performance liquid chromatography-electrospray ionization-MS and GC-electron capture detector. Six volatile disinfection by-products were identified including chloroform (CF), dichloroacetonitrile, 1,1-dichloropropanone, 1,1,1-trichloropropanone, dichloronitromethane and trichloronitromethane. Degradation pathways of chlortoluron chlorination were then proposed. High concentrations of CF were generated during chlortoluron chlorination, with maximum CF yield at circumneutral pH range in solution.

Liquor made quicker: alcohol as a synthetic reagent for molecules in anesthesia.

Ethanol was an early anesthetic, and chemists transformed it into better ones. Hypnotic/anesthetic/analgesic molecules prepared from ethanol include barbiturates, benzocaine, chloral hydrate, chloroform, diethyl ether, ethyl chloride, ethylene, etomidate, meperidine, paraldehyde, phenacetin, procaine, tribromoethanol, and urethane. Ethanol was sometimes mixed deliberately with the other anesthetics, and John Snow's inhaled amylene came from the "fusel oil" fraction of rotgut whisky.

Influence of Na2S on the degradation kinetics of CCl4 in the presence of very pure iron.

This paper presents the results of kinetic studies to investigate the effect of FeS film formation on the degradation rate of CCl(4) by 99.99% pure metallic iron. The film was formed by submersing metallic iron grains in an oxygen free HCO(3)(-)/CO(3)(2-) electrolyte solution. When the grains had reached a quasi steady-state value of the corrosion potential, Na(2)S((aq)) was injected. Upon injection, a microm thick poorly crystalline FeS film formed immediately on the iron surface. Over time, the iron became strongly corroded and both the FeS film and the metallic iron grains began to crack leading to exposure of bare metallic iron to the solution. The effect of the surface film on the degradation rate of CCl(4) was investigated following four periods of aging, 1, 10, 30, and 60 days. Relative to the controls, the 1-day sulfide-aged iron showed a substantial decrease in rate of degradation of CCl(4.) However, over time, the rate of degradation increased and surpassed the degradation rate obtained in the controls. It has been proposed that CCl(4) is reduced to HCCl(3) by metallic iron by electron transfer. The FeS film is substantially less conducting than the bulk iron metal or non-stoichiometric magnetite and from the results of this study, greatly decreases the rate of CCl(4) degradation relative to iron that has not been exposed to Na(2)S. However, continued aging of the FeS film results in breakdown and stress-induced cracking of the film, followed by dissolution and cracking of the iron itself. The cracking of the bulk iron is believed to be a consequence of hydrogen embrittlement, which is promoted by sulfide. The increase in CCl(4) degradation rate, as the FeS films age, suggests that the process of hydrogen cracking increases the surface area available for charge transfer.

[Study on intermediate products in chloroform formation from L-tyrosine treated with sodium hypochlorite].

Possible intermediates in the formation of chloroform during by the sodium hypochlorite (NaClO) treatment of L-tyrosine were investigated using HPLC and LC/MS. One product showed the same MS characteristics as the substance formed by the NaClO treatment of 4-hydroxybenzyl cyanide (4-HBC), and it was suggested to be m-chloro-4-hydroxybenzyl cyanide (m-C-4-HBC). Since m-C-4-HBC is not commercially available it was synthesized by treating 4-HBC with NaClO, and purified by extraction with ethyl acetate, followed by HPLC on preparative isolation columns, using a column switching method. The product was confirmed to be 3-chloro-4-hydroxybenzyl cyanide (3-C-4-HBC), by means of NMR spectral analysis. When L-tyrosine or 4-HBC was treated with NaClO, 3-C-4-HBC and CHCl3 were generated. When 3-C-4-HBC was treated with NaClO, CHCl3 was generated. Judging from these results, 3-C-4-HBC was confirmed to be an intermediate in the formation of CHCl3 from L-tyrosine. Thus, the reaction pathway of CHCl3 formation from L-tyrosine treated with NaClO is concluded to be: L-tyrosine-->4-HBC-->3-C-4-HBC-->CHCl3.

Production of [11C]chloroform by direct chlorination of [11C]methane without catalyst support for the synthesis of [11C]diazomethane.

The preparation of [11C]chloroform by direct chlorination of [11C]methane using gaseous chlorine by variation of temperature and reaction time (inert gas flow) without catalyst support for the online production of [11C]diazomethane in a flow-through synthesis apparatus is described in this work. At an oven temperature of 400 degrees C and a He flow of 50 mL/min, [11C]chloroform was synthesized inside a quartz glass column in a radiochemical yield of 31+/-2% with respect to [11C]methane. The online preparation of [11C]diazomethane by reaction of [11C]chloroform with hydrazine in an ethanolic KOH solution with small amounts of 18-crown-6-crownether succeeded with a radiochemical yield of 20+/-3% with respect to [11C]methane. The product [11C]diazomethane was measured indirectly in the form of 4-nitrobenzoic acid[11C]methylester using the esterification of 4-nitrobenzoic acid as a monitor reaction.

Formation of chloroform and other chlorinated byproducts by chlorination of triclosan-containing antibacterial products.

Triclosan is a widely used antibacterial agent found in many personal hygiene products. Although it has previously been established that pure triclosan and free chlorine readily react, interactions between triclosan-containing consumer products and free chlorine have not previously been analyzed in great depth. Sixteen double-blinded solutions including both triclosan-containing (1.14-3.12 mg triclosan/g product) and triclosan-free products were contacted with free chlorine at pH 7. Products detected included (chlorophenoxy) phenols, 2,4-dichlorophenol, 2,4,6-trichlorophenol, and chloroform. The daughter product yields were found to be highly variable and were dependent on the antimicrobial product investigated, the free chlorine to triclosan ratio, and the temperature at which the study was conducted. Lowering the temperature from 40 to 30 degrees C resulted in a decreased average chloroform yield from 0.50 to 0.37 mol chloroform/mol triclosan consumed after 1 min of reaction time for an initial free chlorine concentration of 4.0 mg/L as Cl2. At 40 degrees C the average molar chloroform yields decreased to 0.29 and <0.1 when the initial free chlorine concentration was decreased to either 2.0 or 1.0 mg/L as Cl2, respectively. Field experiments, in which Atlanta, GA and Danville, VA tap waters were augmented with various soap products, exhibited results varying from the laboratory experiments in that different productyields were observed. These differences are attributed to the chlorine demand of constituents in the tap water. A simple exposure model suggests that exposure to chloroform can be significant under some conditions.

pH dependence of carbon tetrachloride reductive dechlorination by magnetite.

Magnetite is precipitated by dissimilatory iron-reducing bacteria or forms through corrosion of zero-valent iron (ZVI) in permeable reactive barriers. Reduction of carbon tetrachloride (CCl4) by synthetic magnetite was examined in batch reactors to evaluate the pH dependence of the reaction rates and product distributions. This work presents the first data where magnetite promotes CCl4 dechlorination independent of added sorbed Fe(II) or coexisting minerals that maintained Fe2+ above the magnetite solubility limit. In this system, reaction rate constants increase with increasing pH values between 6 and 10. The pH dependence is explained by acid-base equilibrium between two surface sites, where the more deprotonated exhibits greater dechlorination reactivity. The distribution of reaction products was also found to depend on pH. The primary reaction product is carbon monoxide (CO) followed by chloroform (CHCl3). CHCl3 production is at a minimum at pH 6 but increases through pH 10. Formation rate constants for both products increase with increasing pH, but the values for CHCl3 increase at a much faster rate. A hypothesis is proposed that relates the CHCl3 rate enhancement to the reduced capacity of deprotonated surface sites to stabilize the trichlorocarbanion transition-state complex. These data form a basis to assess the natural attenuation capacity of magnetite formed under iron reducing conditions. Application of this information to permeable barrier technology suggests that, in the long term, oxidation of ZVI to magnetite may be accompanied by a shift toward more benign reaction products as well as a 2 order of magnitude decrease in reaction rate constants.

[Influence of the mixed disinfectant of ClO2 and Cl2 on formation of chloroform].

The study on influence of mixed solution of ClO2 and Cl2 on formation of chloroform from 9 THMs precursors, such as fulvic acid (FA), resorcinol, phloroglucinol and cresorcinol etc. under conditions of different ClO2/Cl2 ratio, content of precursors, reaction pH, reaction time and reaction temperature etc. was studied. Results showed that as the mass percentage of ClO2 in the mixed disinfectant was increased, the amount of chloroform formed was reduced; such as when mass percentages of ClO2 were 25%, 50% and 75%, CHCl3 formed reduced 55%-65%, 70%-86% and 80%-93% respectively; until ClO2 was 90%, reduction of CHCl3 reached 95%-99%. In order to control the formation of chloroform thoroughly, mass percentage of ClO2 must be higher than 90%. This provided important scientific base for the necessity of using highly pure ClO2 in disinfection and developing generator which produced high quality ClO2.

Mechanism of chloroform formation by chlorine and its inhibition by chlorine dioxide.

Chlorination of drinking waters leads to the formation of trihalomethanes arising from the reaction of chlorine and organic substances. Therefore, chlorine dioxide (ClO2) which does not produce trihalomethanes is being considered as an alternative disinfectant. It has been reported that rat blood chloroform levels were significantly decreased after treatment with ClO2. Studies were conducted to investigate the mechanisms of chloroform formation by chlorine (HOCl) and its inhibition by ClO2 (5 mg/liter) in the presence of HOCl (5, 10, 20 mg/liter) using sodium citrate (1 mM) as an organic substance. When citrate was reacted with HOCl, beta-ketoglutaric acid, monochloroacetone, dichloroacetone, and trichloroacetone were produced as reaction intermediates and chloroform as a final product. There was a linear relationship between the concentrations of HOCl and the formation of chloroform. When ClO2 was substituted for HOCl, neither chloroform was formed nor citrate concentration was changed. Further, chloroform formation was inhibited by ClO2 in the presence of HOCl and citrate and the degree of inhibition depends on the ratio of ClO2/HOCl. Gas chromatograph/mass spectrometer analysis indicates that this inhibition is related to the reaction of ClO2 with beta-ketoglutaric acid to form malonic acid. Chlorine dioxide also oxidizes other intermediates such as monochloroacetone and dichloroacetone to acetic acid. These studies indicate that ClO2 inhibits chloroform formation from citrate and HOCl by the oxidation of the intermediates which were involved in the reaction of chloroform formation.