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      Modelling changes in glutathione homeostasis as a function of quinone redox metabolism

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          Abstract

          Redox cycling is an understated mechanism of toxicity associated with a plethora of xenobiotics, responsible for preventing the effective treatment of serious conditions such as malaria and cardiomyopathy. Quinone compounds are notorious redox cyclers, present in drugs such as doxorubicin, which is used to treat a host of human cancers. However, the therapeutic index of doxorubicin is undermined by dose-dependent cardiotoxicity, which may be a function of futile redox cycling. In this study, a doxorubicin-specific in silico quinone redox metabolism model is described. Doxorubicin-GSH adduct formation kinetics are thermodynamically estimated from its reduction potential, while the remainder of the model is parameterised using oxygen consumption rate data, indicative of hydroquinone auto-oxidation. The model is then combined with a comprehensive glutathione metabolism model, facilitating the simulation of quinone redox cycling, and adduct-induced GSH depletion. Simulations suggest that glutathione pools are most sensitive to exposure duration at pharmacologically and supra-pharmacologically relevant doxorubicin concentrations. The model provides an alternative method of investigating and quantifying redox cycling induced oxidative stress, circumventing the experimental difficulties of measuring and tracking radical species. This in silico framework provides a platform from which GSH depletion can be explored as a function of a compound’s physicochemical properties.

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          Analysis of glutathione: implication in redox and detoxification.

          Glutathione is a ubiquitous thiol-containing tripeptide, which plays a central role in cell biology. It is implicated in the cellular defence against xenobiotics and naturally occurring deleterious compounds, such as free radicals and hydroperoxides. Glutathione status is a highly sensitive indicator of cell functionality and viability. Its levels in human tissues normally range from 0.1 to 10 mM, being most concentrated in liver (up to 10 mM) and in the spleen, kidney, lens, erythrocytes and leukocytes. In humans, GSH depletion is linked to a number of disease states including cancer, neurodegenerative and cardiovascular diseases. The present review proposes an analysis of the current knowledge about the methodologies for measuring glutathione in human biological samples and their feasibility as routine methods in clinical chemistry. Furthermore, it elucidates the fundamental role of glutathione in pathophysiological conditions and its implication in redox and detoxification process. Several methods have been optimised in order to identify and quantify glutathione forms in human biological samples. They include spectrophotometric, fluorometric and bioluminometric assays, often applied to HPLC analysis. Recently, a liquid chromatography-mass spectrometry technique for glutathione determination has been developed that, however, suffers from the lack of total automation and the high cost of the equipment. Glutathione is a critical factor in protecting organisms against toxicity and disease. This review may turn useful for analysing the glutathione homeostasis, whose impairment represents an indicator of tissue oxidative status in human subjects.
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            Electrode potentials of partially reduced oxygen species, from dioxygen to water.

            We use published Gibbs energies of formation and equilibrium constants to determine electrode potentials for the partially reduced intermediates along the pathway of reduction of dioxygen to water, as well as of ozone and singlet dioxygen. The results are summarized in an oxidation state (Frost) diagram. Our review of the literature on electrode potentials leads us to revise values for the O(2)/O(2)(*-) couple to E degrees (O(2g)/O(2)(*-))=-0.35+/-0.02V and E degrees (O(2aq)/O(2)(*-))=-0.18+/-0.02V from -0.33 and -0.16V, respectively. Other electrode potentials (pH 7) for the radical species covered are E degrees '(O(3g)/O(3)(*-))=+0.91V, E degrees '(HO(2)(*), H(+)/H(2)O(2))=+1.05V, E degrees '(H(2)O(2), H(+)/HO(*), H(2)O)=+0.39V, and E degrees '(HO(*), H(+)/H(2)O)=+2.31V. Copyright 2010 Elsevier Inc. All rights reserved.
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              Thermodynamic and kinetic considerations for the reaction of semiquinone radicals to form superoxide and hydrogen peroxide.

              The quinone/semiquinone/hydroquinone triad (Q/SQ(*-)/H(2)Q) represents a class of compounds that has great importance in a wide range of biological processes. The half-cell reduction potentials of these redox couples in aqueous solutions at neutral pH, E degrees ', provide a window to understanding the thermodynamic and kinetic characteristics of this triad and their associated chemistry and biochemistry in vivo. Substituents on the quinone ring can significantly influence the electron density "on the ring" and thus modify E degrees' dramatically. E degrees' of the quinone governs the reaction of semiquinone with dioxygen to form superoxide. At near-neutral pH the pK(a)'s of the hydroquinone are outstanding indicators of the electron density in the aromatic ring of the members of these triads (electrophilicity) and thus are excellent tools to predict half-cell reduction potentials for both the one-electron and two-electron couples, which in turn allow estimates of rate constants for the reactions of these triads. For example, the higher the pK(a)'s of H(2)Q, the lower the reduction potentials and the higher the rate constants for the reaction of SQ(*-) with dioxygen to form superoxide. However, hydroquinone autoxidation is controlled by the concentration of di-ionized hydroquinone; thus, the lower the pK(a)'s the less stable H(2)Q to autoxidation. Catalysts, e.g., metals and quinone, can accelerate oxidation processes; by removing superoxide and increasing the rate of formation of quinone, superoxide dismutase can accelerate oxidation of hydroquinones and thereby increase the flux of hydrogen peroxide. The principal reactions of quinones are with nucleophiles via Michael addition, for example, with thiols and amines. The rate constants for these addition reactions are also related to E degrees'. Thus, pK(a)'s of a hydroquinone and E degrees ' are central to the chemistry of these triads. Copyright 2010 Elsevier Inc. All rights reserved.
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                Author and article information

                Contributors
                j.leedale@liverpool.ac.uk
                Journal
                Sci Rep
                Sci Rep
                Scientific Reports
                Nature Publishing Group UK (London )
                2045-2322
                19 April 2019
                19 April 2019
                2019
                : 9
                : 6333
                Affiliations
                [1 ]ISNI 0000 0004 0368 0654, GRID grid.4425.7, Department of Applied Mathematics, , Liverpool John Moores University, ; Byrom Street, Liverpool, L3 3AF UK
                [2 ]ISNI 0000 0004 1936 8470, GRID grid.10025.36, EPSRC Liverpool Centre for Mathematics in Healthcare, Department of Mathematical Sciences, , University of Liverpool, ; Liverpool, L69 7ZL UK
                [3 ]ISNI 0000 0004 1936 8470, GRID grid.10025.36, Institute for Risk and Uncertainty, , University of Liverpool, ; Liverpool, L69 7ZF UK
                [4 ]ISNI 0000 0004 0368 0654, GRID grid.4425.7, School of Pharmacy and Biomolecular Sciences, , Liverpool John Moores University, ; Byrom Street, Liverpool, L3 3AF UK
                [5 ]GlaxoSmithKline, David Jack Centre for Research, Park Road, Ware, SG12 0DP UK
                [6 ]ISNI 0000 0004 1936 8470, GRID grid.10025.36, MRC Centre for Drug Safety Science, Department of Molecular and Clinical Pharmacology, , University of Liverpool, ; Ashton Street, Liverpool, L69 3GE UK
                Author information
                http://orcid.org/0000-0002-5505-460X
                http://orcid.org/0000-0001-9010-4126
                Article
                42799
                10.1038/s41598-019-42799-2
                6474874
                31004119
                56bc4586-0453-4f70-897f-68ce37a21f2f
                © The Author(s) 2019

                Open Access This article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in a credit line to the material. If material is not included in the article’s Creative Commons license and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this license, visit http://creativecommons.org/licenses/by/4.0/.

                History
                : 27 December 2018
                : 9 April 2019
                Funding
                Funded by: FundRef https://doi.org/10.13039/501100000268, RCUK | Biotechnology and Biological Sciences Research Council (BBSRC);
                Award ID: BB/L502273/2
                Award Recipient :
                Funded by: FundRef https://doi.org/10.13039/501100000266, RCUK | Engineering and Physical Sciences Research Council (EPSRC);
                Award ID: EP/N014499/1
                Award ID: EP/N014499/1
                Award Recipient :
                Categories
                Article
                Custom metadata
                © The Author(s) 2019

                Uncategorized
                biochemical reaction networks,bioenergetics
                Uncategorized
                biochemical reaction networks, bioenergetics

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