Kinetics of reduction of tyrosine phenoxyl radicals by glutathione

Modification of tyrosine (TyrOH) is used as a marker of oxidative and nitrosative stress. 3,3′-Dityrosine formation, in particular, reflects oxidative damage and results from the combination of two tyrosyl phenoxyl radicals (TyrO). This reaction is in competition with reductive processes in the cell which ‘repair’ tyrosyl radicals: possible reductants include thiols and ascorbate. In this study, a rate constant of 2 × 10⁶ M⁻¹ s⁻¹ was estimated for the reaction between tyrosyl radicals and glutathione (GSH) at pH 7.15, generating the radicals by pulse radiolysis and monitoring the tyrosyl radical by kinetic spectrophotometry. Earlier measurements have suggested that this ‘repair’ reaction could be an equilibrium, and to investigate this possibility the reduction (electrode) potential of the (TyrO,H⁺/TyrOH) couple was reinvestigated by observing the fast redox equilibrium with the indicator 2,2′-azinobis(3-ethylbenzothiazoline-6-sulphonate). Extrapolation of the reduction potential of TyrO measured at pH 9–11 indicated the mid-point reduction potential of the tyrosyl radical at pH 7, E_m7(TyrO,H⁺/TyrOH) = 0.93 ± 0.02 V. This is close to the reported reduction potential of the glutathione thiyl radical, E_m7 = 0.94 ± 0.03 V, confirming the ‘repair’ equilibrium constant is of the order of unity and suggesting that efficient reduction of TyrO by GSH might require removal of thiyl radicals to move the equilibrium in the direction of repair. Loss of thiyl radicals, facilitating repair of TyrO, can arise either via conjugation of thiyl with thiol/thiolate or oxygen, or unimolecular transformation, the latter important at low concentrations of thiols and oxygen.     

Redox state of glutathione in human plasma

Thiol and disulfide forms of glutathione (GSH) and cysteine (Cys) were measured in plasma from 24 healthy individuals aged 25-35 and redox potential values (E(h)) for thiol/disulfide couples were calculated using the Nernst equation. Although the concentration of GSH (2.8 +/- 0.9 microM) was much greater than that of GSSG (0.14 +/- 0.04 microM), the redox potential of the GSSG/2GSH pool (-137 +/- 9 mV) was considerably more oxidized than values for tissues and cultured cells (-185 to -258 mV). This indicates that a rapid oxidation of GSH occurs upon release into plasma. The difference in values between individuals was remarkably small, suggesting that the rates of reduction and oxidation in the plasma are closely balanced to maintain this redox potential. The redox potential for the Cys and cystine (CySS) pool (-80 +/- 9 mV) was 57 mV more oxidized, showing that the GSSG/2GSH and the CySS/2Cys pools are not in redox equilibrium in the plasma. Potentials for thiol/disulfide couples involving CysGly were intermediate between the values for these couples. Regression analyses showed that the redox potentials for the different thiol/disulfide couples within individuals were correlated, with the E(h) for CySS-mono-Gly/(Cys. CysGly) providing the best correlation with other low molecular weight pools as well as protein disulfides of GSH, CysGly and Cys. These results suggest that E(h) values for GSSG/2GSH and CySS-mono-Gly/(Cys. CysGly) may provide useful means to quantitatively express the oxidant/antioxidant balance in clinical and epidemiologic studies.     

Kinetics of the reaction between nitric oxide and glutathione: implications for thiol depletion in cells

Nitric oxide in the absence of oxygen was suggested to react with 5-50 mM glutathione (GSH) over many minutes when [NO*] < [GSH] (N. Hogg et al., FEBS Lett. 382:223-228; 1996). However, Aravindakumar et al. (J. Chem. Soc. Perkin Trans. 2:663-669; 2002) provided data suggesting approximately 200-fold higher reactivity under conditions of [NO*] > [GSH]. To help resolve these differences, the rate of loss of NO* ( approximately 9 microM) in aqueous solutions of GSH (2.5-20 mM) was measured by chemiluminescence. An apparent second-order rate constant of 0.080 +/- 0.008 M(-1) s(-1) at pH 7.4, 37 degrees C, was calculated based on the total [GSH] and "pseudo-first-order" kinetics; thiolate anion was much more reactive than undissociated thiol. These data imply a half-life of approximately 30 min for low concentrations of NO* with 5 mM GSH, 37 degrees C, pH 7.4, in the absence of oxygen. Possible kinetic schemes that can partially explain the divergent literature reports are discussed, notably an equilibrium in the reaction between NO* and GSH. Human breast carcinoma MCF-7 cells were exposed to NO* (initially approximately 18 microM) in alidded six well plate in an anaerobic chamber in vitro; intracellular GSH levels decreased by half in approximately 60 min. Aerobic exposure depletes GSH in cells in vitro much faster because of autoxidation of NO* to NO2*, >10(8) times more reactive toward GSH.     

Glutathione-thiyl radical scavenging and transferase properties of human glutaredoxin (thioltransferase). Potential role in redox signal transduction

Glutaredoxin (GRx, thioltransferase) is implicated in cellular redox regulation, and it is known for specific and efficient catalysis of reduction of protein-S-S-glutathione-mixed disulfides (protein-SSG) because of its remarkably low thiol pK(a) ( approximately 3.5) and its ability to stabilize a catalytic S-glutathionyl intermediate (GRx-SSG). These unique properties suggested that GRx might also react with glutathione-thiyl radicals (GS(.)) and stabilize a disulfide anion radical intermediate (GRx-SSG), thereby facilitating the conversion of GS(.) to GSSG or transfer of GS(.) to form protein-SSG. We found that GRx catalyzes GSSG formation in the presence of GS-thiyl radical generating systems (Fe(2+)/ADP/H(2)O(2) + GSH or horseradish peroxidase/H(2)O(2) + GSH). Catalysis is dependent on O(2) and results in concomitant superoxide formation, and it is distinguished from glutathione peroxidase-like activity. With the horseradish peroxidase system and [(35)S]GSH, GRx enhanced the rate of GS-radiolabel incorporation into GAPDH. GRx also enhanced the rate of S-glutathionylation of glyceraldehyde-3-phosphate dehydrogenase with GSSG or S-nitrosoglutathione, but these glutathionyl donors were much less efficient. Both actin and protein-tyrosine phosphatase-1B were superior substrates for GRx-facilitated S-glutathionylation with GS-radical. These studies characterize GRx as a versatile catalyst, facilitating GS-radical scavenging and S-glutathionylation of redox signal mediators, consistent with a critical role in cellular regulation.     

Arsenic transport by the human multidrug resistance protein 1 (MRP1/ABCC1). Evidence that a tri-glutathione conjugate is required

Inorganic arsenic is an established human carcinogen, but its metabolism is incompletely defined. The ATP binding cassette protein, multidrug resistance protein (MRP1/ABCC1), transports conjugated organic anions (e.g. leukotriene C(4)) and also co-transports certain unmodified xenobiotics (e.g. vincristine) with glutathione (GSH). MRP1 also confers resistance to arsenic in association with GSH; however, the mechanism and the species of arsenic transported are unknown. Using membrane vesicles prepared from the MRP1-overexpressing lung cancer cell line, H69AR, we found that MRP1 transports arsenite (As(III)) only in the presence of GSH but does not transport arsenate (As(V)) (with or without GSH). The non-reducing GSH analogs L-gamma-glutamyl-L-alpha-aminobutyryl glycine and S-methyl GSH did not support As(III) transport, indicating that the free thiol group of GSH is required. GSH-dependent transport of As(III) was 2-fold higher at pH 6.5-7 than at a more basic pH, consistent with the formation and transport of the acid-stable arsenic triglutathione (As(GS)(3)). Immunoblot analysis of H69AR vesicles revealed the unexpected membrane association of GSH S-transferase P1-1 (GSTP1-1). Membrane vesicles from an MRP1-transfected HeLa cell line lacking membrane-associated GSTP1-1 did not transport As(III) even in the presence of GSH but did transport synthetic As(GS)(3). The addition of exogenous GSTP1-1 to HeLa-MRP1 vesicles resulted in GSH-dependent As(III) transport. The apparent K(m) of As(GS)(3) for MRP1 was 0.32 microM, suggesting a remarkably high relative affinity. As(GS)(3) transport by MRP1 was osmotically sensitive and was inhibited by several conjugated organic anions (MRP1 substrates) as well as the metalloid antimonite (K(i) 2.8 microM). As(GS)(3) transport experiments using MRP1 mutants with substrate specificities differing from wild-type MRP1 suggested a commonality in the substrate binding pockets of As(GS)(3) and leukotriene C(4). Finally, human MRP2 also transported As(GS)(3). In conclusion, MRP1 transports inorganic arsenic as a tri-GSH conjugate, and GSTP1-1 may have a synergistic role in this process.     

Thiol/disulfide exchange in the thioredoxin-catalyzed reductive activation of spinach chloroplast fructose-1,6-bisphosphatase. Kinetics and thermodynamics

Two kinetically and thermodynamically distinct thiol/disulfide redox changes are observed during the reversible thioredoxin fb-catalyzed reduction and oxidation of spinach chloroplast fructose-1,6-bisphosphatase by dithiothreitol. The two processes, which occur at different rates and with different equilibrium constants, can be observed independently in either the reduction (activation) or oxidation (inactivation) direction by assaying the enzyme activity at different magnesium and fructose-1,6-bisphosphate concentrations. The two processes, in both the reduction and oxidation directions, are kinetically zero-order in dithiothreitol concentration and first-order in thioredoxin fb concentration. The rate-limiting step in both directions is the reaction of fructose-1,6-bisphosphatase with thioredoxin. The more kinetically and thermodynamically favored reduction of fructose-1,6-bisphosphatase lowers the apparent Km for fructose-1,6-bisphosphate while the less favorable process lowers the Km for magnesium. Both of the thiol/disulfide redox changes reach equilibrium in redox buffers consisting of different ratios of reduced to oxidized dithiothreitol (Ered + DTTox in equilibrium Eox + DTTred). The equilibrium constants (Kox) are 0.12 +/- 0.02 and 0.39 +/- 0.08 for the fast and slow reduction processes at pH 8.0. The equilibrium constants for oxidation of the enzyme by glutathione disulfide (Ered + GSSG in equilibrium Eox + 2 GSH) can be estimated to be approximately 2400 and 7800 M, respectively. Thermodynamically the fructose-1,6-bisphosphatase/thioredoxin fb system is extremely sensitive to oxidation, comparable to disulfide bond formation in extracellular proteins.     

Kinetic characterization of thiolate anion formation and chemical catalysis of activated microsomal glutathione transferase 1

Microsomal glutathione transferase 1 (MGST1) displays the unique ability to be activated, up to 30-fold, by the reaction with sulfhydryl reagents, e.g., N-ethylmaleimide. Analysis of glutathione (GSH) thiolate formation, which occurs upon mixing activated MGST1 with GSH, reveals biphasic kinetics, where the rapid phase dominated at higher GSH concentrations. The kinetic behavior suggests a two-step mechanism consisting of a rapid GSH-binding step (K(D)(GSH) approximately 10 mM), followed by slower formation of thiolate (k(2) approximately 10 s(-1)). The release rate (or protonation of the enzyme GSH thiolate complex) of GS(-) was slow (k(-2) = 0.016 s(-1)), consistent with overall tight binding of GSH. Electrophilic second substrates react rapidly with the E*GS(-) complex, and again, a two-step mechanism is suggested. In comparison to the unactivated enzyme [Morgenstern et al. (2001) Biochemistry 40, 3378-3384], the mechanisms of GSH thiolate formation and electrophile interaction are similar; however, thiolate anion formation is enhanced 30-fold in the activated enzyme, contributing to an increased k(cat) (3.6 s(-1)). Interestingly, in the activated enzyme, thiolate formation and proton release from the enzyme are not strictly coupled, because proton release (as well as k(cat)) was found to be approximately 4 times slower than GSH thiolate formation in an unbuffered system. Solvent kinetic isotope effect measurements demonstrated a 2-fold decrease in the rate constant (k(2)) for thiolate formation and k(cat) (in the reaction with 1-chloro-2,4-dinitrobenzene) for both unactivated and activated MGST1. This indicates that thiolate formation contributes to k(cat) for the activated enzyme, as suggested previously for unactivated MGST1. The stoichiometry of thiolate formation, proton release, and burst kinetics suggested utilization of one GSH molecule per enzyme trimer.     

Determination of the absolute redox potential of Rutin: experimental and theoretical studies

The conditional formal potential, E degrees', of Rutin has been studied by cyclic voltammetry using a Rutin film deposited at the multi-wall carbon nanotubes modified glassy carbon electrode (GCE) as the working electrode in different pH phosphate buffered solutions. The experimental standard redox potential, E degrees, of Rutin is obtained to be 0.88 V versus SHE (Standard Hydrogen Electrode). High-level ab initio calculations have been also performed on a chemical model of Rutin and the absolute reduction potential has been calculated. The theoretical standard reduction potential relative to SHE (0.83 V) is in relatively good agreement with experiment.     

Redox characteristics of the tungsten DMSO reductase of Rhodobacter capsulatus

The dimethylsulfoxide reductase (DMSOR) from Rhodobacter capsulatus is known to retain its three-dimensional structure and enzymatic activity upon substitution of molybdenum, the metal that occurs naturally at the active site, by tungsten. The redox properties of tungsten-substituted DMSOR (W-DMSOR) have been investigated by a dye-mediated reductive titration with the concentration of the W(V) state monitored by EPR spectroscopy. At pH 7.0, E(m)(W(VI)/W(V)) is -194 mV and E(m)(W(V)/W(IV)) is -134 mV. Each E(m) value of W-DMSOR is significantly lower (220 and 334 mV, respectively) than that of the corresponding couple of Mo-DMSOR. These redox potentials are consistent with the ability of Mo-DMSOR to catalyze both the reduction of DMSO to DMS and the back reaction, whereas W-DMSOR is very effective in catalyzing the forward reaction, but shows no ability to catalyze the oxidation of DMS to DMSO.     

Thiol/disulfide exchange between rabbit muscle phosphofructokinase and glutathione. Kinetics and thermodynamics of enzyme oxidation

Reversible thiol/disulfide exchange equilibria between rabbit muscle phosphofructokinase and glutathione redox buffers results in a dependence of the activity of the enzyme on the thiol to disulfide ratio of the redox buffer (Gilbert, H. F. (1982) J. Biol. Chem. 257, 12086-12091). The transition between fully reduced (active) and fully oxidized (inactive) enzyme is half complete at a [GSH]/[GSSG] ratio of 6.5 +/- 1 at pH 8.0 and 5.6 +/- 0.9 at pH 7.2. In the presence of excess GSSG approximately 40-50% of the activity is lost in a rapid process (k = 110 M-1 min-1), while the remaining activity is lost more slowly (k = 1.9 M-1 min-1). Two equivalents of radiolabeled glutathione are incorporated covalently, one coincident with each phase of inactivation. The most rapidly oxidized sulfhydryl group is also the most rapidly reduced by GSH in the reverse reaction (k = 150 M-1 min-1). Reduction of a more slowly reacting protein-glutathione mixed disulfide is required to regenerate the original activity (k = 0.33 M-1 min-1). The thiol/disulfide oxidation equilibrium constant (Kox) for the most rapidly oxidized sulfhydryl group is estimated to be 0.7 while that for the more slowly oxidized group is 6.1. The sulfhydryl group which is more easily oxidized kinetically is the more thermodynamically resistant to oxidation. The magnitude of the equilibrium constants for these reversible oxidations would suggest that the oxidation state (and activity) of phosphofructokinase would not be significantly affected by typical metabolic changes in the glutathione oxidation state in vivo.     

Antioxidant properties of melatonin: a pulse radiolysis study

Various one-electron oxidants such as OH*, tert-BuO*, CCl3OO*, Br2*- and N3*, generated pulse radiolytically in aqueous solutions at pH 7, were scavenged by melatonin to form two main absorption bands with lambda(max) = 335 nm and 500 nm. The assignment of the spectra and determination of extinction coefficients of the transients have been reported. Rate constants for the formation of these species ranged from 0.6-12.5x10(9) dm3 mol(-1) s(-1). These transients decayed by second order, as observed in the case of Br2*- and N3* radical reactions. Both the NO2* and NO* radicals react with the substrate with k = 0.37x10(7) and 3x10(7) dm3 mol(-1) s(-1), respectively. At pH approximately 2.5, the protonated form of the transient is formed due to the reaction of Br2*- radical with melatonin, pKa ( MelH* <=> Mel* + H+) = 4.7+/-0.1. Reduction potential of the couple (Mel*/MelH), determined both by cyclic voltammetric and pulse-radiolytic techniques, gave a value E(1)7 = 0.95+/-0.02 V vs. NHE. Repair of guanosine radical and regeneration of melatonin radicals by ascorbate and urate ions at pH 7 have been reported. Reactions of the reducing radicals e(aq)- and H* atoms with melatonin have been shown to occur at near diffusion rates.     

Kinetic analysis of the slow ionization of glutathione by microsomal glutathione transferase MGST1

An important aspect of the catalytic mechanism of microsomal glutathione transferase (MGST1) is the activation of the thiol of bound glutathione (GSH). GSH binding to MGST1 as measured by thiolate anion formation, proton release, and Meisenheimer complex formation is a slow process that can be described by a rapid binding step (K(GSH)d = 47 +/- 7 mM) of the peptide followed by slow deprotonation (k2 = 0.42 +/- 0.03 s(-1). Release of the GSH thiolate anion is very slow (apparent first-order rate k(-2) = 0.0006 +/- 0.00002 s(-)(1)) and thus explains the overall tight binding of GSH. It has been known for some time that the turnover (kcat) of MGST1 does not correlate well with the chemical reactivity of the electrophilic substrate. The steady-state kinetic parameters determined for GSH and 1-chloro-2,4-dinitrobenzene (CDNB) are consistent with thiolate anion formation (k2) being largely rate-determining in enzyme turnover (kcat = 0.26 +/- 0.07 s(-1). Thus, the chemical step of thiolate addition is not rate-limiting and can be studied as a burst of product formation on reaction of halo-nitroarene electrophiles with the E.GS- complex. The saturation behavior of the concentration dependence of the product burst with CDNB indicates that the reaction occurs in a two-step process that is characterized by rapid equilibrium binding ( = 0.53 +/- 0.08 mM) to the E.GS- complex and a relatively fast chemical reaction with the thiolate (k3 = 500 +/- 40 s(-1). In a series of substrate analogues, it is observed that log k3 is linearly related (rho value 3.5 +/- 0.3) to second substrate reactivity as described by Hammett sigma- values demonstrating a strong dependence on chemical reactivity that is similar to the nonenzymatic reaction (rho = 3.4). Microsomal glutathione transferase 1 displays the unusual property of being activated by sulfhydryl reagents. When the enzyme is activated by N-ethylmaleimide, the rate of thiolate anion formation is greatly enhanced, demonstrating for the first time the specific step that is activated. This result explains earlier observations that the enzyme is activated only with more reactive substrates. Taken together, the observations show that the kinetic mechanism of MGST1 can be described by slow GSH binding/thiolate formation followed by a chemical step that depends on the reactivity of the electrophilic substrate. As the chemical reactivity of the electrophile becomes lower the rate-determining step shifts from thiolate formation to the chemical reaction.     

Breaking and re-forming the disulfide bond at the high-potential,respiratory-type Rieske [2Fe-2S] center of thermus thermophilus: characterization of the sulfhydryl state by protein-film voltammetry

A disulfide bond, adjacent to the [2Fe-2S] cluster, is conserved in all high-potential Rieske proteins from the respiratory and photosynthetic cytochrome bc(1) and b(6)f complexes but is absent from the low-potential, bacterial dioxygenase Rieske proteins. The role of the disulfide is unclear, since cysteine mutants have resulted in only apoprotein. The high stability of the soluble Thermus thermophilus Rieske protein permits chemical reduction of the disulfide bond and characterization of the sulfhydryl (dithiol) form by protein-film voltammetry. The effect of disulfide reduction on the cluster potential is small (DeltaE(0)' 相似文献   

Glutathione redox state regulates mitochondrial reactive oxygen production

Oxidative stress induced by 2,3,7,8-tetrachlorodibenzo-p-dioxin (TCDD; dioxin) is poorly understood. Following one dose of TCDD (5 microg/kg body weight), mitochondrial succinate-dependent production of superoxide and H2O2 in mouse liver doubled at 7-28 days, then subsided by day 56; concomitantly, levels of GSH and GSSG increased in both cytosol and mitochondria. Cytosol displayed a typical oxidative stress response, consisting of diminished GSH relative to GSSG, decreased potential to reduce protein-SSG mixed disulfide bonds (type 1 thiol redox switch) or protein-SS-protein disulfide bonds (type 2 thiol redox switch), and a +10 mV change in GSSG/2GSH reduction potential. In contrast, mitochondria showed a rise in reduction state, consisting of increased GSH relative to GSSG, increases in type 1 and type 2 thiol redox switches, and a -25 mV change in GSSG/2GSH reduction potential. Comparing Ahr(-/-) knock-out and wild-type mice, we found that TCDD-induced thiol changes in both cytosol and mitochondria were dependent on the aromatic hydrocarbon receptor (AHR). GSH was rapidly taken up by mitochondria and stimulated succinate-dependent H2O2 production. A linear dependence of H2O2 production on the reduction potential for GSSG/2GSH exists between -150 and -300 mV. The TCDD-stimulated increase in succinate-dependent and thiol-stimulated production of reactive oxygen paralleled a four-fold increase in formamidopyrimidine DNA N-glycosylase (FPG)-sensitive cleavage sites in mitochondrial DNA, compared with a two-fold increase in nuclear DNA. These results suggest that TCDD produces an AHR-dependent oxidative stress in mitochondria, with concomitant mitochondrial DNA damage mediated, at least in part, by an increase in the mitochondrial thiol reduction state.     

Enzymatic and nonenzymatic formation of reactive oxygen species from 6-anilino-5,8-quinolinequinone

The nonenzymatic and enzymatic formation of reactive oxygen species (ROS) from LY83583 (6-anilino-5,8-quinolinequinone) was investigated by electron paramagnetic resonance (EPR) spectroscopy. In the presence of thiol compounds such as glutathione and L-cysteine, LY83583 underwent a one-electron reduction due to low redox potential (-0.3+/-0.01 V vs. SCE), followed by formation of LY83583 semiquinone anion radical. This species was characterized by EPR spectroscopy under an argon atmosphere at neutral pH. Under an aerobic condition, this species interacts with molecular oxygen to form a superoxide anion radical. GSH-conjugated LY83583 was also identified by NMR and FAB-MS. When LY83583 was applied to PC12 cells, ROS formation was completely inhibited by both the flavoenzyme inhibitor DPI and the DT-diaphorase inhibitor dicumarol. On the other hand, ROS generation occurred independent of intracellular GSH level. These results indicate that LY83583 can generate ROS both enzymatically and nonenzymatically, although the enzymatic formation is dominant over the nonenzymatic system in PC12 cells.     

Redox properties of the couples compound I/compound II and compound II/native enzyme of human myeloperoxidase

Myeloperoxidase (MPO) is an important component of the neutrophil's antimicrobial armory and has been implicated in promoting tissue damage in numerous inflammatory diseases. For the first time the standard reduction potential of the redox couple compound II/native enzyme has been determined to be (0.97+/-0.01)V at pH 7.0 and 25 degrees C. This was achieved by rapid mixing of preformed compound II with either tyrosine or nitrite by using the sequential-mixing stopped-flow technique and measuring spectrophotometrically the concentrations of the reacting species and products at equilibrium. Using the recently determined standard reduction potential for the couple compound I/native enzyme (1.16 V), the reduction potential of the couple compound I/compound II was calculated to be 1.35 V at pH 7 and 25 degrees C. These data reveal substantial differences between the two known heme peroxidase superfamilies and reflect the dramatic differences observed in the oxidisability of substrates by the MPO redox intermediates compound I and compound II.     

Determination of the redox potential of deazariboflavin by equilibration with flavins.

The redox potential of deazariboflavin has been determined for pH values from 5.5 to 9.2 by equilibration with riboflavin and lumiflavin 3-acetate. The position of the equilibrium with riboflavin was measured spectrophotometrically and fluorimetrically; the equilibrium potential with lumiflavin 3-acetate was measured spectrophotometrically and potentiometrically. The Em7 for deazariboflavin was found to be--0.273 +/- 0.003 V against the standard hydrogen electrode. Equilibrium with flavodoxin at pH 9.5 and 10.0 was also used to determine the redox potential of deazariboflavin at high pH values. The pK of dihydrodeazariboflavin was found from the break in the potential vs. pH diagram and from spectrophotometric pH titration. The pK value obtained by both methods is 7.00 +/- 0.05. We found that borate, a product of the reducing agent borohydride, complexed with the ribityl sidechain of deazariboflavin, causing a shift in the pK for the reduced form to values of about 8.     

Determination of glucose oxidase oxidation-reduction potentials and the oxygen reactivity of fully reduced and semiquinoid forms.

The oxidation-reduction potential values for the two electron transfers to glucose oxidase were obtained at pH 5.3, where the neutral radical is the stable form, and at pH 9.3, where the anion radical is the stable form. The midpoint potentials at 25 degrees were: pH 5.3 EFl1ox + e- H+ equilibrium EFlH. Em1 = -0.063 +/- 0.011 V EFlH. + e- + H+ equilibrium EFlredH2 Em2 = -0.065 +/- 0.007 V pH 9.3 EFlox + e- EFi- Em1 = -0.200 +/- 0.010 V EFi- + e- + H+ equilibrium EFlredH- Em2 = -0.240 +/- 0.005 V All potentials were measured versus the standard hydrogen electrode (SHE). The potentials indicated that glucose oxidase radicals are stabilized by kinetic factors and not by thermodynamic energy barriers. The pK for the glucose oxidase radical was 7.28 from dead time stopped flow measurements and the extinction coefficient of the neutral semiquinone was 4140 M-1 cm-1 at 570 nm. Both radical forms reacted with oxygen in a second order fashion. The rate at 25 degrees for the neutral semiquinone was 1.4 X 10(4) M-1 s-1; that for the anion radical was 3.5 X 10(4) M-1 s-1. The rate of oxidation of the neutral radical changed by a factor of 9 for a temperature difference of 22 degrees. For the anion radical, the oxidation rate changed by a factor of 6 for a 22 degrees change in temperature. We studied the oxygen reactivity of the 2-electron reduced form of the enzyme over a wide wavelength range and failed to detect either oxygenated flavin derivatives or semiquinoid forms as intermediates. The rate of reoxidation of fully reduced glucose oxidase at pH 9.3 was dependent on ionic strength.     

Redox environment of the cell as viewed through the redox state of the glutathione disulfide/glutathione couple

Redox state is a term used widely in the research field of free radicals and oxidative stress. Unfortunately, it is used as a general term referring to relative changes that are not well defined or quantitated. In this review we provide a definition for the redox environment of biological fluids, cell organelles, cells, or tissue. We illustrate how the reduction potential of various redox couples can be estimated with the Nernst equation and show how pH and the concentrations of the species comprising different redox couples influence the reduction potential. We discuss how the redox state of the glutathione disulfide-glutathione couple (GSSG/2GSH) can serve as an important indicator of redox environment. There are many redox couples in a cell that work together to maintain the redox environment; the GSSG/2GSH couple is the most abundant redox couple in a cell. Changes of the half-cell reduction potential (E(hc)) of the GSSG/2GSH couple appear to correlate with the biological status of the cell: proliferation E(hc) approximately -240 mV; differentiation E(hc) approximately -200 mV; or apoptosis E(hc) approximately -170 mV. These estimates can be used to more fully understand the redox biochemistry that results from oxidative stress. These are the first steps toward a new quantitative biology, which hopefully will provide a rationale and understanding of the cellular mechanisms associated with cell growth and development, signaling, and reductive or oxidative stress.