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At least 19 recordsLinked to original sources
PubMed1999

Effective inhibition by beta-carotene of cellular DNA breaking induced by peroxynitrous acid.

Peroxynitrous acid synthesized by reaction of hydrogen peroxide and nitrite and generated from 3-morpholinosydononimine (SIN-1) induced cellular DNA breaking of human promyelocytic leukemia HL-60 cells in phosphate buffer (pH 7.5) as assessed by alkaline single cell gel electrophoresis (comet) assay and quantification of comet types. Ascorbate and Trolox inhibited cellular DNA breaking induced by peroxynitrous acid, but the concentrations of these antioxidants required for effective inhibition was about 50-fold higher than that of peroxynitrous acid. beta-Carotene protected DNA breaking by peroxynitrous acid in 20% tetrahydrofuran-phosphate buffer (pH 7.5) much more effectively than ascorbate and Trolox. The concentrations of beta-carotene required for effective inhibition was lower than the concentration of peroxynitrous acid.

Antioxidants↗
PubMed1999

Acidic conditions exacerbate interferon-gamma-induced intestinal epithelial hyperpermeability: role of peroxynitrous acid.

OBJECTIVE: Nitric oxide (NO*) derived from exogenous donors has been shown to increase the permeability of cultured intestinal epithelial monolayers, an effect that is augmented by mildly acidic conditions. Because interferon-gamma (IFN-gamma) also increases intestinal epithelial permeability, at least partly by an NO*-dependent mechanism, we sought to determine whether IFN-gamma-induced hyperpermeability is increased under acidic conditions. METHODS: Human intestinal epithelial (Caco-2BBe) cells were grown as monolayers on permeable supports in bicameral chambers. Permeability was assessed by measuring transepithelial electrical resistance (TER) or the transepithelial passage of fluorescein disulfonic acid. Inducible nitric oxide synthase (iNOS) messenger RNA expression was determined by northern blot analysis. Concentrations of nitrite and nitrate (NO2-/NO3-), stable oxidation products of NO*, were determined using the Greiss reaction. Cellular adenosine triphosphate (ATP) levels were determined using the luciferin/luciferase method. MEASUREMENTS AND MAIN RESULTS: Incubation of Caco-2BBe monolayers with INF-gamma (1000 units/mL) at an extracellular pH (pHo) of 7.4 increased permeability to fluorescein disulfonic acid and decreased TER. However, incubation of monolayers with IFN-gamma under mildly acidic conditions (i.e., pHo 7.0-6.6) accelerated the decrease in TER and augmented the increase in permeability induced by the cytokine. IFN-gamma-induced iNOS messenger RNA expression and NO2-/NO3- accumulation in medium were unaffected by acidic conditions. At pHo 7.4, incubation of Caco-2BBe monolayers with IFN-gamma (1000 units/mL) for 72 hrs had no effect on intracellular ATP content compared with monolayers simultaneously incubated under the same conditions but in the absence of the cytokine. However, when the cells were incubated for 72 hrs with the same concentration of IFN-gamma under mildly acidic conditions (i.e., pHo 7.0 or 6.6), ATP levels were significantly decreased. At pHo 7.0, IFN-gamma-induced increases in permeability were ameliorated by addition of the following agents: 2-phenyl-4,4,5,5- tetramethylimidazoline-1-oxyl-3-oxide (a NO* scavenger), N(G)-monomethyl-L-arginine (a iNOS inhibitor), dimethyl sulfoxide (a hydroxyl radical scavenger), and ascorbate (a peroxynitrous acid scavenger). CONCLUSION: Mild acidosis augments IFN-gamma-induced intestinal epithelial hyperpermeability and ATP depletion, possibly by fostering the formation of peroxynitrous acid and/or hydroxyl radical.

Adenosine Triphosphate↗
PubMed1999

Effect of beta-carotene on the transformation of tyrosine by nitrogen dioxide and peroxynitrous acid.

In the NO2-exposure of tyrosine in 70% dioxane/phosphate buffer (pH 7.4), beta-carotene enhanced the degradation of tyrosine and/or 3-nitrotyrosine produced, whereas alpha-tocopherol and ascorbyl palmitate inhibited the transformation of tyrosine into 3-nitrotyrosine. Generation of certain active species in the interaction of beta-carotene with NO2 was suggested. Ascorbyl palmitate effectively and alpha-tocopherol slightly inhibited the transformation of tyrosine in the NO2-exposure in the presence of beta-carotene. In the reaction of tyrosine with ONOO-/ONOOH, beta-carotene enhanced the degradation of 3-nitrotyrosine produced suggesting generation of certain active species, whereas alpha-tocopherol and ascorbyl palmitate completely suppressed the transformation of tyrosine into 3-nitrotyrosine.

Ascorbic Acid↗
PubMed1997

Nitric oxide-induced hyperpermeability of human intestinal epithelial monolayers is augmented by inhibition of the amiloride-sensitive Na(+)-H+ antiport: potential role of peroxynitrous acid.

BACKGROUND: Nitric oxide (NO.) increases the permeability of cultured intestinal epithelial monolayers. NO. reacts with superoxide anion to form peroxynitrite anion, which can be protonated under mildly acidic conditions to form the potent and versatile oxidizing agent, peroxynitrous acid. We hypothesized that intracellular acidosis induced by the Na(+)-H+ antiport blocker, amiloride, would favor the formation of peroxynitrous acid and thereby augment hyperpermeability induced by the NO. donor, SIN-1. METHODS: Caco-2BBe human intestinal epithelial monolayers were grown on permeable supports in bicameral chambers. The permeability of monolayers was assessed by measuring the transepithelial flux of fluorescein disulfonic acid (FS). RESULTS: Incubation of monolayers with SIN-1 increased permeability to FS. Adding amiloride augmented SIN-1-induced hyperpermeability. SIN-1 plus amiloride also decreased cellular adenosine triphosphate content and caused derangements of the actin-based cytoskeleton as demonstrated by fluorescence microscopy. Coincubation of monolayers with several free-radical or peroxynitrous acid scavengers (deferoxamine, mannitol, dimethyl sulfoxide, or ascorbate) ameliorated hyperpermeability induced by SIN-1 plus amiloride. CONCLUSIONS: Amiloride augments NO.-induced intestinal epithelial permeability, apparently by promoting the development of intracellular acidosis and thereby favoring the formation of the peroxynitrous acid.

Amiloride↗
PubMed2003

15N CIDNP study of formation and decay of peroxynitric acid: evidence for formation of hydroxyl radicals.

The reaction of nitrous acid with hydrogen peroxide leads to nitric acid as the only stable product. In the course of this reaction, peroxynitrous acid (ONOOH) and, in the presence of CO(2), a peroxynitrite-CO(2) adduct (ONOOCO(2)(-)) are intermediately formed. Both intermediates decompose to yield highly oxidizing radicals, which subsequently react with excess hydrogen peroxide to yield peroxynitric acid (O(2)NOOH) as a further intermediate. During these reactions, (15)N chemically induced dynamic nuclear polarization (CIDNP) effects are observed, the analysis of the pH dependency of which allows the elucidation of mechanistic details. The formation and decay of peroxynitric acid via free radicals NO(2)(*) and HOO(*) is demonstrated by the appearance of (15)N CIDNP leading to emission (E) in the (15)N NMR signal of O(2)NOOH during its formation and to enhanced absorption (A) during its decay reaction. Additionally, the (15)N NMR signal of the nitrate ion (NO(3)(-)) appears in emission at pH approximately 4.5. These observations are explained by proposing the intermediate formation of short-lived radical anions O(2)NOOH(*)(-) probably generated by electron transfer between peroxynitric acid and peroxynitrate anion, followed by decomposition of O(2)NOOH(*)(-) into NO(3)(-) and HO(*) and NO(2)(-) and HOO(*) radicals, respectively. The feasibility of such reactions is supported by quantum-chemical calculations at the CBS-Q level of theory including PCM solvation model corrections for aqueous solution. The release of free HO(*) radicals during decomposition of O(2)NOOH is supported by (13)C and (1)H NMR product studies of the reaction of preformed peroxynitric acid with [(13)C(2)]DMSO (to yield the typical "HO(*) products" methanesulfonic acid, methanol, and nitromethane) and by ESR spectroscopic detection of the HO(*) and CH(3)(*) radical adducts to the spin trap compound POBN in the absence and presence of isotopically labeled DMSO, respectively.

Journal Article↗
PubMed2000

Characterization of the Tetrahymena ribozyme folding pathway using the kinetic footprinting reagent peroxynitrous acid.

Large RNAs fold into complex structures which determine their biological activities. A full understanding of both RNA structure and dynamics will include the description of the pathways by which these structures are formed. Kinetic footprinting [Sclavi, B., et al. (1997) J. Mol. Biol. 266, 144-159] has been shown to be a powerful method for the study of dynamic processes involving RNA. Here we describe the use of a readily available reagent, peroxynitrous acid, as a kinetic footprinting tool for the study of RNA folding. Hydroxyl radicals generated from this reagent were used to footprint the Tetrahymena ribozyme during its magnesium-dependent folding-in agreement with synchroton X-ray footprinting [Sclavi, B., et al. (1998) Science 279, 1940-1943] and oligonucleotide/hybridization cleavage experiments [Zarrinkar, P. P., and Williamson, J. R. (1994) Science 265, 918-924], this work suggests an ordered, hierarchical folding pathway for the ribozyme. Several slow steps in the folding pathway were observed in the peroxynitrous acid footprinting, but none of these corresponded to the rate-determining step of folding. This suggests that the formation of the global, protected structure is followed by one or more slow local rearrangements to yield the final active structure. These studies illustrate the utility of peroxynitrous acid as a reagent for the elucidation of RNA folding pathways and the study of RNA dynamics.

Animals↗
PubMed2003

Direct determination of the Gibbs' energy of formation of peroxynitrous acid.

The kinetics of decomposition of peroxynitrous acid (ONOOH) was investigated in the presence of 0.1-0.75 M HClO(4) and at a constant ionic strength. The decay rate of ONOOH decreased in the presence of H(2)O(2), approaching a limiting value well below 75 mM H(2)O(2). It also decreased in the presence of relatively low [HNO(2)] but did not approach a lower limiting value, since ONOOH reacts directly with HNO(2). The latter reaction corresponds to a HNO(2)- and H(+)-catalyzed isomerization of ONOOH to nitrate, and its third-order rate constant was determined to be 520 +/- 30 M(-)(2) s(-)(1). The mechanism of formation of O(2)NOOH from ONOOH in the presence of H(2)O(2) was also scrutinized. The results demonstrated that in the presence of 0.1-0.75 M HClO(4) and 75 mM H(2)O(2) the formation of O(2)NOOH is insignificant. The most important finding in this work is the reversibility of the reaction ONOOH + H(2)O right harpoon over left harpoon HNO(2) + H(2)O(2), and its equilibrium constant was determined to be (7.5 +/- 0.4) x 10(-)(4) M. Using this value, the Gibbs' energy of formation of ONOOH was calculated to be 7.1 +/- 0.2 kcal/mol. This figure is in good agreement with the value determined previously from kinetic data using parameters for radicals formed during homolysis of peroxynitrite.

Journal Article↗
PubMed2000

Kinetic Footprinting of an RNA-Folding Pathway Using Peroxynitrous Acid.

Following footprints to discover a path is easier with peroxynitrous acid. The folding of the Tetrahymena ribozyme was studied using this readily available reagent to generate hydroxyl radicals for kinetic footprinting studies. The different domains of the ribozyme appear to assemble at different rates following an ordered, hierarchical pathway (see scheme).

Journal Article↗
PubMed1998

Free radical formation in the peroxynitrous acid (ONOOH)/peroxynitrite (ONOO-) system.

The rate constant of homolysis of peroxynitrite, ONOO-, into O2- and NO was determined to be 0.017 s-1 at 20 degrees C. In combination with other experimental data taken from the literature, this value yields the Gibbs free energy of formation of ONOO-, delta f G o(ONOO-) = 16.6 kcal/mol. On the basis of this result, we conclude that peroxynitrous acid homolyzes to yield nitrogen dioxide (NO2) and hydroxyl (OH) free radicals and derive delta f G o(ONOOH) = 7.7 kcal/mol. The rate constant of the reaction between NO and ONOO- was found to be 5 x 10(-)2 M-1 s-1 at most. The implications of the two homolysis reactions are discussed.

Free Radicals↗
PubMed1992

Free radical yields from the homolysis of peroxynitrous acid.

A recent study reports discordant results for maximal free-radical yields from the decomposition of peroxynitrous acid using different assay reagents and a puzzling decrease (to zero) of the radical yields with increasing pH. An assay method using 2,2,'azino-bis(3-ethyl-benzthiazoline sulphonate) (ABTS) has been tested using stopped-flow kinetic studies, and the results imply that the assay is satisfactory when [HOONO] much greater than [-OONO] but that reactions involving peroxynitrite anion interfere at higher pH. Evidence is presented that peroxynitrite was an interfering species in the earlier studies.

Benzothiazoles↗
PubMed2003

Hydroxyl radical formation by O-O bond homolysis in peroxynitrous acid.

Peroxynitrite decay in weakly alkaline media occurs by two concurrent sets of pathways which are distinguished by their reaction products. One set leads to net isomerization to NO(3)(-) and the other set to net decomposition to O(2) plus NO(2)(-). At sufficiently high peroxynitrite concentrations, the decay half-time becomes concentration-independent and approaches a limiting value predicted by a mechanism in which reaction is initiated by unimolecular homolysis of the peroxo O-O bond, i.e., the following reaction: ONOOH --> (*)OH + (*)NO(2). This dynamical behavior excludes alternative postulated mechanisms that ascribe decomposition to bond rearrangement within bimolecular adducts. Nitrate and nitrite product distributions measured at very low peroxynitrite concentrations also correspond to predictions of the homolysis model, contrary to a recent report from another laboratory. Additionally, (1) the rate constant for the reaction ONOO(-) --> (*)NO + (*)O(2)(-), which is critical to the kinetic model, has been confirmed, (2) the apparent volume of activation for ONOOH decay (DeltaV() = 9.7 +/- 1.4 cm(3)/mol) has been shown to be independent of the concentration of added nitrite and identical to most other reported values, and (3) complex patterns of inhibition of O(2) formation by radical scavengers, which are impossible to rationalize by alternative proposed reaction schemes, are shown to be quantitatively in accord with the homolysis model. These observations resolve major disputes over experimental data existing in the literature; despite extensive investigation of these reactions, no verifiable experimental evidence has been advanced that contradicts the homolysis model.

Algorithms↗
PubMed1997

beta-Carotene effectively scavenges toxic nitrogen oxides: nitrogen dioxide and peroxynitrous acid.

beta-Carotene absorbed 2 equimolar amounts of NO2 accompanying the complete destruction of beta-carotene. Electron spin resonance study using 2-phenyl-4,4,5,5-tetramethylimidazoline-3-oxide-1-oxyl revealed that no significant amounts of NO were released by the interaction. Nitrogen atoms derived from NO2 were tightly bound to the beta-carotene molecules. Destruction of beta-carotene was inhibited little by alpha-tocopherol and polyunsaturated fatty esters, and slightly by ascorbyl palmitate, indicating that beta-carotene was a more effective scavenger of NO2. ONOOH/ONOO- and 3-morpholinosydononimine similarly destroyed beta-carotene. The results suggest that beta-carotene contributes to the prevention of cytotoxicity and genotoxicity of NO2 and ONOOH/ONOO- derived from NO.

Amiloride↗
PubMed1995

The chemistry of peroxynitrite: a product from the reaction of nitric oxide with superoxide.

Nitric oxide and superoxide, which are produced by several cell types, rapidly combine to form peroxynitrite. This reaction can result in nitric oxide scavenging, and thus mitigation of the biological effects of superoxide. Also, superoxide can trap and hence modulate the effects of nitric oxide; superoxide dismutase, by controlling superoxide levels, therefore can influence the reaction pathways open to nitric oxide. The production of peroxynitrite, however, causes its own sequelae of events: Although neither .NO nor superoxide is a strong oxidant, peroxynitrite is a potent and versatile oxidant that can attack a wide range of biological targets. The peroxynitrite anion is relatively stable, but its acid, peroxynitrous acid (HOONO), rearranges to form nitrate with a half-life of approximately 1 s at pH 7, 37 degrees C. HOONO exists as a Boltzmann distribution of rotamers; at 5-37 degrees C HOONO has an apparent acidity constant, pKa,app, of 6.8. Oxidation reactions of HOONO can involve two-electron processes (such as an SN2 displacement) or a one-electron transfer (ET) reaction in which the substrate is oxidized by one electron and peroxynitrite is reduced. These oxidation reactions could involve one of two mechanisms. The first mechanism is homolysis of HOONO to give HO. and .NO2, which initially are held together in a solvent cage. This caged pair of radicals (the "geminate" pair) can either diffuse apart, giving free radicals that can perform oxidations, or react together either to form nitrate or to reform HOONO (a process called cage return). A large amount of cage return can explain the small entropy of activation (Arrhenius A-factor) observed for the decomposition of HOONO. A cage mechanism also can explain the residual yield of nitrate that appears to be formed even in the presence of high concentrations of all of the scavengers studied to date, since scavengers capture only free HO. and .NO2 and not caged radicals. If the cage mechanism is correct, the rate of disappearance of peroxynitrite be slower in solvents of higher viscosity, and we do not find this to be the case. The second mechanism is that an activated isomer of peroxynitrous acid, HOONO*, can be formed in a steady state. The HOONO* mechanism can explain the inability of hydroxyl radical scavengers to completely block either nitrate formation or the oxidation of substrates such as methionine, since HOONO* would be less reactive, and therefore more selective, than the hydroxyl radical itself.(ABSTRACT TRUNCATED AT 400 WORDS)

Animals↗
PubMed1991

Peroxynitrite oxidation of sulfhydryls. The cytotoxic potential of superoxide and nitric oxide.

Peroxynitrite anion (ONOO-) is a potent oxidant that mediates oxidation of both nonprotein and protein sulfhydryls. Endothelial cells, macrophages, and neutrophils can generate superoxide as well as nitric oxide, leading to the production of peroxynitrite anion in vivo. Apparent second order rate constants were 5,900 M-1.s-1 and 2,600-2,800 M-1.s-1 for the reaction of peroxynitrite anion with free cysteine and the single thiol of albumin, respectively, at pH 7.4 and 37 degrees C. These rate constants are 3 orders of magnitude greater than the corresponding rate constants for the reaction of hydrogen peroxide with sulfhydryls at pH 7.4. Unlike hydrogen peroxide, which oxidizes thiolate anion, peroxynitrite anion reacts preferentially with the undissociated form of the thiol group. Peroxynitrite oxidizes cysteine to cystine and the bovine serum albumin thiol group to an arsenite nonreducible product, suggesting oxidation beyond sulfenic acid. Peroxynitrous acid was a less effective thiol-oxidizing agent than its anion, with oxidation presumably mediated by the decomposition products, hydroxyl radical and nitrogen dioxide. The reactive peroxynitrite anion may exert cytotoxic effects in part by oxidizing tissue sulfhydryls.

Animals↗
PubMed1994

On the pH-dependent yield of hydroxyl radical products from peroxynitrite.

Nitric oxide reacts rapidly with superoxide to give the strongly oxidizing peroxynitrite anion (ONOO-), which undergoes spontaneous first-order decomposition when protonated. The oxidative chemistry of peroxynitrite (ONOO-) is highly pH-dependent. At acidic pH, peroxynitrous acid (ONOOH) oxidizes dimethylsulfoxide to formaldehyde and 2,2'-azino-bis-(3-ethyl-1,2- dihydrobenzothiazoline 6-sulfonate) (ABTS) to the greenish-colored ABTS+ radical cation. The product yield from dimethylsulfoxide and ABTS decreased at more alkaline pH with apparent pK(a)s of 7.9 and 8.2, respectively. Decreasing yield with increasing pH could not be explained by the oxidation of either formaldehyde or ABTS+ by peroxynitrite. In the presence of 50 mM dimethylsulfoxide, nitrogen dioxide was formed in approximately equimolar amounts to the other reaction product, formaldehyde. The yield of nitrogen dioxide also decreased with an apparent pK(a) of 8.0. We propose that the complex oxidative chemistry of peroxynitrite is controlled by the pH-dependent isomerization of the relatively stable cis-configuration (predominant at high pH) to the trans-configuration. Trans-peroxynitrous acid can form a vibrationally excited intermediate capable of reacting like hydroxyl radical. The vibrationally excited intermediate can also directly rearrange to nitric acid, reducing the apparent hydroxyl radical yield to less than 30%. The loss of hydroxyl radical-like reactivity can be explained on the basis of ionization of trans-peroxynitrous acid to the trans-anion, which in turn undergoes internal rearrangement to nitrate without forming a strong oxidant.(ABSTRACT TRUNCATED AT 250 WORDS)

Benzothiazoles↗
PubMed2003

Peroxynitrite and NO+ donors form colored nitrite adducts with sinapinic acid: potential applications.

Sinapinic acid (3,5-dimethoxy-4-hydroxycinnamic acid, SA) reacted with peroxynitrous acid at neutral pH with a second-order rate constant of 812 M(-1)s(-1), to yield a red product (lambda(max), 532 nm). The identical colored product could be formed with acidified decomposed peroxynitrous acid solutions or nitrite at slower rates (0.1M HCl, 8.32 M(-1)s(-1); 10% acetic acid, 0.0004 M(-1)s(-1)). The red compound is thought to be O-nitrososinapinic acid (3,5-dimethoxy-4-nitrosooxycinnamic acid) which can be formed by reaction with either peroxynitrous acid or nitrous acid. The extinction coefficient of O-nitrososinapinic acid (ONSA) was estimated to be 8419 M(-1)cm(-1) at 510 nm in 10% acetic acid and 90% acetonitrile. ONSA was also formed via NO(+) transfer from S-nitrosoglutathione (GSNO). ONSA in turn can S-nitrosate low molecular weight thiols and protein thiols. SA was also shown to act as a peroxynitrite sink as it effectively prevented the oxidation of dihydrorhodamine under physiological conditions. The fact that O-nitrososinapinic acid is stable and can be used to S-nitrosate thiol containing amino acids, peptides, and proteins makes it a potentially useful reagent in the study of S-nitrosothiol biochemistry and physiology. In addition, the relatively high extinction coefficient of O-nitrososinapinic acid means that it could be utilized as an analyte for the spectroscopic detection of peroxynitrite or NO(+)-donors in the submicromolar range.

Coumaric Acids↗