On the mechanism of hydrogen peroxide formation during precipitation of hemoglobin with perchloric acid

During acid precipitation of hemoglobin, hydrogen peroxide is formed. The oxidant is generated from hemoglobin-bound as well as from physically dissolved oxygen, provided divalent hemoglobin-iron is present. The extent of hydrogen peroxide formation seems to be dependent on the precipitating reagent. From experiments on GSH oxidation during precipitation of red cells and from a literature survey formation of at least one second reactive oxygen species has to be assumed. Different reaction pathways for generating these oxidants during acid precipitation are discussed: Hydroperoxide which is probably liberated by proton catalysis may contribute to the observed oxidation reactions. At pH approximately 1 it rapidly disproportionates yielding oxygen and hydrogen peroxide, which might produce reactive oxidants with hemoglobin intermediates formed during precipitation. In addition a new hypothesis is presented explaining the ability of N-ethylmaleimide to inhibit GSH oxidation during precipitation of red cells. Accordingly, the SH-reagent rapidly penetrates the cell membrane and reacts with GSH before access of protons prevents alkylation.     

An enzyme-chromogenic surface plasmon resonance biosensor probe for hydrogen peroxide determination using a modified Trinder's reagent

An absorption-based surface plasmon resonance (SPR(Abs)) biosensor probe has been developed for simple and reproducible measurements of hydrogen peroxide using a modified Trinder's reagent (a chromogenic reagent). The reagent enabled the determination of the hydrogen peroxide concentration by the development of deep color dyes (lambda(max)=630nm) through the oxidative coupling reaction with N-ethyl-N-(2-hydroxy-3-sulfopropyl)-3,5-dimethylaniline sodium salt monohydrate (MAOS; C(13)H(20)NNaO(4)S.H(2)O) and 4-aminoantipyrine (4-AA) in the presence of hydrogen peroxide and horseradish peroxidase (HRP). In the present study, urea as an adduct of hydrogen peroxide for color development could be omitted from the measurement solution. The measurement solution containing 5mM hydrogen peroxide was deeply colored at a high absorbance value calculated as 46.7cm(-1) and was directly applied to the SPR(Abs) biosensing without dilution. The measurement was simply performed by dropping the measurement solution onto the surface of the SPR sensor probe, and the SPR(Abs) biosensor response to hydrogen peroxide was obtained as a reflectivity change in the SPR spectrum. After investigation of the pH profiles in the SPR(Abs) biosensor probe, a linear calibration curve was obtained between 1.0 and 50mM hydrogen peroxide (r=0.991, six points, average of relative standard deviation; 0.152%, n=3) with a detection limit of 0.5mM. To examine the applicability of this SPR(Abs) biosensor probe, 20mM glucose detection using glucose oxidase was also confirmed without influence of the refractive index in the measurement solution. Thus, the SPR(Abs) biosensor probe employing the modified Trinder's reagent demonstrated applicability to other analyte biosensing tools.     

Amines for detection of dopamine by generation of hydrogen peroxide and peroxyoxalate chemiluminescence

A range of nitrogen-containing compounds (alkyl amines, piperazines, cyclohexylamines and nitrogen heterocyclics) were investigated for generation of hydrogen peroxide from dopamine and detection by peroxyoxalate chemiluminescence. Imidazole, ethyleneurea and allantoin among the nitrogen heterocyclic compounds tested generated hydrogen peroxide from dopamine following incubation at 60°C, pH 9.5–10.5, for 0–30 min. Imidazole was the most effective for generation of hydrogen peroxide, but imidazole derivatives with a primary amine side chain (histamine) or thiol (ethylenethiourea) were not effective. The presence of a ketone group (ethyleneurea, allantoin) did not hinder the reaction. Under optimal conditions (30 min incubation, 50 mmol/L imidazole) 10.5 nmol of dopamine could be detected. The cyclohexylamines tested produced low amounts of hydrogen peroxide (0.09–2.74% of light intensity with imidazole), and the piperazines and the alkyl amines tested produced no detectable hydrogen peroxide. Imidazole reacts with the phenolic groups of dopamine in a different manner from monoamine oxidase, and a reagent containing imidazole, ethyleneurea or allantoin was useful for non-enzymatic detection of dopamine by peroxyoxalate chemiluminescence.© John Wiley & Sons, Ltd.     

Simultaneous protective and damaging effects of cysteamine on intracellular DNA of leukocytes

Incubation of human leukocytes with cysteamine can lead to the induction of DNA strand breaks. The induction of breaks is biphasic with increasing concentration of scavenger. The number of breaks increases in a dose-dependent manner to a maximum and then decreases at higher concentrations. Catalase has been shown to prevent the production of breaks, indicating an involvement of hydrogen peroxide. Cysteamine reacts with oxygen to generate hydrogen peroxide but at higher concentrations it also reacts with hydrogen peroxide. Thus, the biphasic effect of cysteamine on leukocyte DNA may be due to the sum of two separate reaction pathways. (i) Cysteamine reacts with oxygen to generate hydrogen peroxide which leads to DNA strand breakage. (ii) At higher concentrations, it eliminates hydrogen peroxide by reacting with it, thereby protecting the cellular DNA. Other antioxidant scavengers such as WR2721, acetylcysteine and ascorbate can also autooxidize to produce strand breaks. Thiourea and tetramethylurea do not. When tested for their ability to protect cells against DNA damage from added H2O2, the agent which most damaging by itself, cysteamine, was also the most protective.     

Peroxidase-catalyzed color removal from bleach plant effluent

Effluent from the caustic extraction stage of a bleach plant is highly colored due to the presence of dissolved products from lignin chlorination and oxidation. Color removal from the effluent by hydrogen peroxide at neutral pH was catalyzed by addition of horseradish peroxidase. The catalysis with peroxidase (20 mg/L) was observed over a wide range of peroxide concentrations (0.1mM-500mM), but the largest effect was between 1mM and 100mM. The pH optimum for catalysis was around 5.0, while the basal rate of noncatalyzed peroxide color removal simply increased with pH within the range tested (3-10). Peroxidase catalysis at pH 7.6 reached a maximum at 40 degrees C in 4 h assays with 10mM peroxide, and disappeared above 60 degrees C. Compared with mycelial color removal by Coriolus versicolor, the rate of color removal by peroxide plus peroxidase was initially faster (first 4 h), but the extent of color removal after 48 h was higher with the fungal treatment. Further addition of peroxidase to the enzyme-treated effluent did not produce additional catalysis. Thus, the peroxide/peroxidase system did not fully represent the metabolic route used by the fungus.     

Inhibition of porcine kidney betaine aldehyde dehydrogenase by hydrogen peroxide

Renal hyperosmotic conditions may produce reactive oxygen species, which could have a deleterious effect on the enzymes involved in osmoregulation. Hydrogen peroxide was used to provoke oxidative stress in the environment of betaine aldehyde dehydrogenase in vitro. Enzyme activity was reduced as hydrogen peroxide concentration was increased. Over 50% of the enzyme activity was lost at 100 μM hydrogen peroxide at two temperatures tested. At pH 8.0, under physiological ionic strength conditions, peroxide inhibited the enzyme. Initial velocity assays of betaine aldehyde dehydrogenase in the presence of hydrogen peroxide (0-200 μM) showed noncompetitive inhibition with respect to NAD(+) or to betaine aldehyde at saturating concentrations of the other substrate at pH 7.0 or 8.0. Inhibition data showed that apparent V(max) decreased 40% and 26% under betaine aldehyde and NAD(+) saturating concentrations at pH 8.0, while at pH 7.0 V(max) decreased 40% and 29% at betaine aldehyde and NAD(+) saturating concentrations. There was little change in apparent Km(NAD) at either pH, while Km(BA) increased at pH 7.0. K(i) values at pH 8 and 7 were calculated. Our results suggest that porcine kidney betaine aldehyde dehydrogenase could be inhibited by hydrogen peroxide in vivo, thus compromising the synthesis of glycine betaine.     

pH Dependence of heme iron coordination, hydrogen peroxide reactivity, and cyanide binding in cytochrome c peroxidase(H52K)

Replacement of the distal histidine, His-52, in cytochrome c peroxidase (CcP) with a lysine residue produces a mutant cytochrome c peroxidase, CcP(H52K), with spectral and kinetic properties significantly altered compared to those of the wild-type enzyme. Three spectroscopically distinct forms of the enzyme are observed between pH 4.0 and 8.0 with two additional forms, thought to be partially denatured forms, making contributions to the observed spectra at the pH extremes. CcP(H52K) exists in at least three, slowly interconverting conformational states over most of the pH range that was investigated. The side chain epsilon-amino group of Lys-52 has an apparent pK(a) of 6.4 +/- 0.2, and the protonation state of Lys-52 affects the spectral properties of the enzyme and the reactions with both hydrogen peroxide and HCN. In its unprotonated form, Lys-52 acts as a base catalyst facilitating the reactions of both hydrogen peroxide and HCN with CcP(H52K). The major form of CcP(H52K) reacts with hydrogen peroxide with a rate approximately 50 times slower than that of wild-type CcP but reacts with HCN approximately 3 times faster than does the wild-type enzyme. The major form of the mutant enzyme has a higher affinity for HCN than does native CcP.     

Oxidation of the His-52 --> Leu mutant of cytochrome c peroxidase by p-nitroperoxybenzoic acid: role of the distal histidine in hydroperoxide activation

Both cytochrome c peroxidase (CcP) and a mutant cytochrome c peroxidase in which the distal histidine has been replaced by leucine, CcP(H52L), are converted to hydroxy-ligated derivatives at alkaline pH. In CcP, the hydroxy-ligated derivative is subsequently converted to a bis-imidazole species prior to protein denaturation while the initial hydroxy-ligated CcP(H52L) is converted to a second, spectroscopically distinct hydroxy-ligated species prior to denaturation. The spectra of the alkaline forms of CcP and CcP(H52L) have been determined between 310 and 700 nm. The pH dependence of the rate of reaction between CcP(H52L) and hydrogen peroxide has been extended to pH 10. The hydroxy-ligated form of CcP(H52L) reacts with hydrogen peroxide 4 times more rapidly than the pentacoordinate, high-spin form of CcP(H52L) that exists at neutral pH. The rate of the reaction between p-nitroperoxybenzoic acid and CcP(H52L) has been measured between pH 4 and pH 8. Neutral p-nitroperoxybenzoic acid reacts with CcP(H52L) 10(5) times more slowly than with CcP while the negatively charged p-nitroperoxybenzoate reacts with CcP(H52L) 10(3) times more slowly than with CcP. These data indicate that the role of the distal histidine during the initial formation of the peroxy anion/heme iron complex is not simply base catalysis.     

Mechanism of DNA cleavage induced by sodium chromate(VI) in the presence of hydrogen peroxide

Reactivities of chromium compounds with DNA were investigated by the DNA sequencing technique using 32P 5'-end-labeled DNA fragments, and the reaction mechanism was investigated by ESR spectroscopy. Incubation of double-stranded DNA with sodium chromate(VI) plus hydrogen peroxide or potassium tetraperoxochromate(V) led to the cleavage at the position of every base, particularly of guanine. Even without piperidine, the formation of oligonucleotides was observed, suggesting the breakage of the deoxyribose-phosphate backbone. ESR studies using hydroxyl radical traps demonstrated that hydroxyl radical is generated both during the reaction of sodium chromate(VI) with hydrogen peroxide and the decomposition of potassium tetraperoxochromate(V), and that hydroxyl radical reacts significantly not only with mononucleotides but also with deoxyribose 5-phosphate. ESR studies using a singlet oxygen trap demonstrated that singlet oxygen is also generated both by the same reaction and decomposition, and reacts significantly with deoxyguanylate, but scarcely reacts with other mononucleotides. Furthermore, ESR studies suggested that tetraperoxochromate(V) is formed by the reaction of sodium chromate(VI) with hydrogen peroxide. These results indicate that sodium chromate(VI) reacts with hydrogen peroxide to form tetraperoxochromate(V), leading to the production of the hydroxyl radical, which causes every base alteration and deoxyribose-phosphate backbone breakage. In addition, sodium chromate(VI) plus hydrogen peroxide generates singlet oxygen, which subsequently oxidizes the guanine residue. The mechanism by which both hydroxyl radical and singlet oxygen are generated during the reaction of sodium chromate(VI) with hydrogen peroxide was presented. Finally, the possibility that this reaction may be one of the primary reactions of carcinogenesis induced by chromate(VI) is discussed.     

A new cleavable reagent for cross-linking and reversible immobilization of proteins.

We have prepared a new bifunctional reagent for the cross-linking and reversible immobilization of proteins through their amine groups. This compound, ethylene glycolyl bis(succinimidyl succinate), reacts rapidly with proteins, at pH 7 and at high dilution. The resulting protein cross-links are readily cleaved at pH 8.5 using hydroxylamine for 3–6 hr. at 37°C. Substantial enzymatic activity was observed with lactic dehydrogenase after such reversible cross-linking. Trypsin immobilized on agarose using this reagent retains full specific activity, is stable for weeks in the cold, and may be released with hydroxylamine at 25°C. This compound appears suitable for studies involving proteins with essential disulfide linkages.     

Acetaminophen stimulates the peroxidative metabolism of anthracyclines

Acetaminophen, a common analgesic and antipyretic drug, is frequently administered to individuals undergoing anthracycline chemotherapy. Here, the effect of acetaminophen on the metabolism of daunorubicin and doxorubicin by isolated enzymes lactoperoxidase and myeloperoxidase, and by myeloperoxidase-containing human leukemia HL-60 cells was investigated using spectrophotometric and EPR techniques. We report that at pharmacological concentrations acetaminophen strongly stimulates oxidation of the anthracyclines by lactoperoxidase and myeloperoxidase systems, which results in irreversibly altered (colorless) products. The initial rate and efficacy of daunorubicin oxidation depends on pH. While at pH approximately 7 the oxidation is rapid and extensive, almost no oxidation occurs at pH approximately 5. In the absence of daunorubicin, oxidation of acetaminophen by lactoperoxidase/hydrogen peroxide is only weakly dependent on pH, however, at pH 7.4 it strongly depends on [daunorubicin]. Ascorbate and reduced glutathione strongly inhibited oxidation of anthracyclines by lactoperoxidase and HL-60 systems. Using EPR, a daunorubicin-derived radical was detected in a daunorubicin/acetaminophen/peroxidase/hydrogen peroxide system as a narrow single line (0.175 mT) with g = 2.0047. When daunorubicin was omitted, only an acetaminophen-melanin EPR signal was detected (g = 2.0043, line width approximately 0.5 mT). Similar results were obtained with doxorubicin. We suggest that the stimulation by acetaminophen is primarily due to its preferential oxidation by peroxidases to the corresponding phenoxyl radical, which subsequently reacts with daunorubicin (doxorubicin). Because biological properties of oxidatively transformed anthracyclines will certainly be different from those of their parent compounds, the possible acetaminophen-enhanced degradation of the anthracyclines in vivo is likely to interfere with anticancer and/or cardiotoxic activities of these agents.     

Mechanism of oxidation reaction of NADH models and phynylglyoxal with hydrogen peroxide. Hypothesis on separate transport of hydrogen and electron atom in certain enzymatic reactions with the participation of NADH and NADPH]

Kinetics of co-oxidation of 1-benzen-3-carbamido-1,4-dihydropyridine (BDN) and phenylglyoxal (PG) with hydrogen peroxide is studied. Dimeric product (di-e11-benzen-5-carbamido-1,2-dihydropyridyl-2]) is found to be formed at pH 9, and quaternal pyridinium salt (BNA)--at pH 7. Molecular oxigen is determined to participate in the reaction at pH 7. Copper (II) ions catalyze this process. Significant catalytic effect of p-dinitrobenzen (p-DNB) is found. The reaction mechanism is postulated to form hydroperoxide from PG and hydrogen peroxide which are capable to split the hydrogen attom from dihydropyridine, molecular oxigen or p-DNB being an acceptor of the electrone. Hypothesis on separate transfer of hydrogen atom and electrone in biological systems are proposed.     

The reaction mechanism of the novel vanadium-bromoperoxidase. A steady-state kinetic analysis

The reaction of vanadium-bromoperoxidase from the brown alga Ascophyllum nodosum with hydrogen peroxide, bromide, and 2-chlorodimedone has been subjected to an extensive steady-state kinetic analysis. Systematic variation of pH and the concentrations of these three components demonstrate that the reaction model includes four enzyme species: native bromoperoxidase, a bromoperoxidase-bromide inhibitory complex, a bromoperoxidase-hydrogen peroxide intermediate, and a bromoperoxidase-HOBr species. This latter intermediate did not display any direct interaction with the nucleophilic reagent as oxidized bromine species (Br-3, Br2, and/or HOBr) were the primary reaction products. The generation of oxidized bromine species was as fast as the bromination of 2-chlorodimedone. The enzyme did not show any specificity with regard to bromination of various organic compounds. Formation of the bromoperoxidase-bromide inhibitory complex was competitive with the reaction between hydrogen peroxide and enzyme. From the steady-state kinetic data lower limits for the second-order rate constants at various pH values were calculated for individual steps in the catalytic cycle. This pH study showed that native enzyme must be unprotonated prior to binding of hydrogen peroxide (second-order association rate constant of 2.5.10(6) M-1.s-1 at pH greater than 6). The pKa for the functional group controlling the binding of hydrogen peroxide was 5.7 and is ascribed to a histidine residue. The reaction rate between bromide and enzyme-hydrogen peroxide intermediate also depended on pH (second-order association rate constant of 1.7.10(5) M-1.s-1 at pH 4.0).     

Reversible oxidation of glyceraldehyde 3-phosphate dehydrogenase thiols in human lung carcinoma cells by hydrogen peroxide

Human lung carcinoma cells (A549) were oxidatively stressed with mildly-toxic or non-toxic amounts of hydrogen peroxide (H2O2, 0.1 mM to 120 mM) for 5 min. Hydrogen peroxide exposure resulted in a dose dependent inhibition of binding (pH 7) of the thiol reagent iodoacetic acid (IAA) to a 38 kDa cell protein. Incubation of cells in saline for 60 min following H2O2 removal restored the ability of IAA to bind to the protein. Treatment with 20 mM dithiothreitol or 2 M urea also restored IAA binding, but 10% Triton X102 or 1 mM Brij 58 had no effect. Increasing to pH 11 during the IAA binding also increased thiol availability. Glyceraldehyde 3-phosphate dehydrogenase (EC 1.2.1.12) has been identified as the protein undergoing thiol/disulfide redox status and enzymic activity changes.     

Nitric oxide and Fenton/Haber-Weiss chemistry: nitric oxide is a potent antioxidant at physiological concentrations

We have examined the action of nitric oxide (NO) on the ability of Fenton's reagent (ferrous iron and hydrogen peroxide), to oxidize a number of organic optical probes. We found that NO is able to arrest the oxidation of organic compounds at concentrations of NO found in brain, in vivo. We present evidence that Fenton's reagent proceeds via a ferryl intermediate ([Fe[double bond]O]2+), before the generation of hydroxyl radical *OH. NO reacts rapidly with this ferryl, blocking the production of *OH. We propose that NO has an important role in protecting biological tissues, and the brain in particular, from Fenton chemistry.     

An enzymatic determination of hydrogen peroxide by using spectrophotometry.

A new spectrophotometric method for determining low hydrogen peroxide concentrations by using horseradish peroxidase in the presence of NADH at pH 7.5 has been described. Both total NADH consumption and initial reaction rate may be used for the determination. Using the NADH consumption, a linear response with respect to hydrogen peroxide was observed in the concentration range 7 x 10(-8)-2.5 x 10(-6) M. Due to the presence of superoxide dismutase, hydrogen peroxide is partly regenerated and an amplification of the signal results, which explains the sensitivity.     

Decoloring hemoglobin as a feedstock for second-generation bioplastics

The color of red blood cell concentrate (RBCC) limits its application in human food, but there is potential to use it for second-generation bioplastics. Several methods have been developed to remove color from RBCC, but they are expensive or may produce difficult-to-remove toxic residues. Hydrogen peroxide treatment is a cheaper alternative. The effects of RBCC concentration, pH, and reaction temperature were the most important factors influencing the decolorizing process. They were investigated with the aim of developing a method that could be scaled to commercial level for producing a bioplastic feedstock. Initial trials showed pH was an important factor for decolorization and foaming. At pH 15 there was a 96% reduction in solution color and 8.4% solids were lost due to foaming. There was a 76% reduction in solution color at pH 2 and only 2.6% solids were lost due to foaming. The optimal reaction conditions were to centrifuge 9% w/w, pH 2 aqueous RBCC solution to remove aggregates. The solution was reacted at 30°C with 7.5?g of 30% (w/w) hydrogen peroxide. These conditions achieved a 93% reduction in solution color after 3?hr and the molecular weight of the decolored protein was not significantly reduced.     

The reactivity of myeloperoxidase compound I formed with hypochlorous acid

The reaction of human myeloperoxidase (MPO) with hypochlorous acid (HOCl) was investigated by conventional stopped-flow spectroscopy at pH 5, 7, and 9. In the reaction of MPO with HOCl, compound I is formed. Its formation is strongly dependent on pH. HOCl (rather than OCl-) reacts with the unprotonated enzyme in its ferric state. Apparent second-order rate constants were determined to be 8.1 x 10(7) M(-1)s(-1) (pH 5), 2.0 x 10(8) M(-1)s(-1) (pH 7) and 2.0 x 10(6) M(-1)s(-1) (pH 9) at 15 degrees C. Furthermore, the kinetics and spectra of the reactions of halides and thiocyanate and of physiologically relevant one-electron donors (ascorbate, nitrite, tyrosine and hydrogen peroxide) with this compound I were investigated using the sequential-mixing technique. The results show conclusively that the redox intermediates formed upon addition of either hydrogen peroxide or hypochlorous acid to native MPO exhibit the same spectral features and reactivities and thus are identical. In stopped-flow investigations, the MPO/HOCl system has some advantage since: (i) in contrast to H2O2, HOCl cannot function as a one-electron donor of compound I; and (ii) MPO can easily be prevented from cycling by addition of methionine as HOCl scavenger. As a consequence, the observed absorbance changes are bigger and errors in data analysis are smaller.     

Interaction of glutathione transferase from horse erythrocytes with 7-chloro-4-nitrobenzo-2-oxa-1,3-diazole

7-Chloro-4-nitrobenzo-2-oxa-1,3-diazole reacts with two thiol groups of the dimeric horse erythrocyte glutathione transferase at pH 5.0, with strong inactivation reversible on dithiothreitol treatment. The inactivation kinetic follows a biphasic pattern, similar to that caused by other thiol reagents as recently reported. Both S-methylglutathione and 1-chloro-2,4-dinitrobenzene protect the enzyme from inactivation. Analysis of the reactive SH group-containing peptide gives the sequence Ala-Ser-Cys-Leu-Tyr, identical with that of the peptide that contains the reactive cysteine 47 of the human placental transferase. In the presence of glutathione, the enzyme is not inactivated by this reagent, but it catalyzes its conjugation to glutathione. At higher pH values, 7-chloro-4-nitrobenzo-2-oxa-1,3-diazole reacts with 2 tyrosines/dimer and lysines, as well as with cysteines. Reaction with lysine seems essentially without effect on activity; whether the reactive tyrosines are important for activity could not be determined using this reagent only. However, 2 tyrosines among the 4 that are nitrated by tetranitro-methane are important for activity.     

A kinetic analysis of the catalase activity of myeloperoxidase

The predominant physiological activity of myeloperoxidase is to convert hydrogen peroxide and chloride to hypochlorous acid. However, this neutrophil enzyme also degrades hydrogen peroxide to oxygen and water. We have undertaken a kinetic analysis of this reaction to clarify its mechanism. When myeloperoxidase was added to hydrogen peroxide in the absence of reducing substrates, there was an initial burst phase of hydrogen peroxide consumption followed by a slow steady state loss. The kinetics of hydrogen peroxide loss were precisely mirrored by the kinetics of oxygen production. Two mols of hydrogen peroxide gave rise to 1 mol of oxygen. With 100 microM hydrogen peroxide and 6 mM chloride, half of the hydrogen peroxide was converted to hypochlorous acid and the remainder to oxygen. Superoxide and tyrosine enhanced the steady-state loss of hydrogen peroxide in the absence of chloride. We propose that hydrogen peroxide reacts with the ferric enzyme to form compound I, which in turn reacts with another molecule of hydrogen peroxide to regenerate the native enzyme and liberate oxygen. The rate constant for the two-electron reduction of compound I by hydrogen peroxide was determined to be 2 x 10(6) M(-1) s(-1). The burst phase occurs because hydrogen peroxide and endogenous donors are able to slowly reduce compound I to compound II, which accumulates and retards the loss of hydrogen peroxide. Superoxide and tyrosine drive the catalase activity because they reduce compound II back to the native enzyme. The two-electron oxidation of hydrogen peroxide by compound I should be considered when interpreting mechanistic studies of myeloperoxidase and may influence the physiological activity of the enzyme.