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Physicochemical and biological properties of oxovanadium(IV), cobalt(II) and nickel(II) complexes with oxydiacetate anions.

Wyrzykowski D, Kloska A, Pranczk J, Szczepańska A, Tesmar A, Jacewicz D, Pilarski B, Chmurzyński L - Biol Trace Elem Res (2014)

Bottom Line: The influence of DMSO as a co-solvent on the stability of the complexes as well as the oxydiacetic acid was evaluated.Furthermore, the reactivity of the complexes towards superoxide free radicals was assessed by employing the nitro blue tetrazolium (NBT) assay.The relationship between physicochemical and biological properties of the complexes was discussed.

View Article: PubMed Central - PubMed

Affiliation: Faculty of Chemistry, University of Gdańsk, Wita Stwosza 63, 80-308, Gdańsk, Poland, dariusz.wyrzykowski@ug.edu.pl.

ABSTRACT
The potentiometric and conductometric titration methods have been used to characterize the stability of series of VO(IV)-, Co(II)- and Ni(II)-oxydiacetato complexes in DMSO-water solutions containing 0-50 % (v/v) DMSO. The influence of DMSO as a co-solvent on the stability of the complexes as well as the oxydiacetic acid was evaluated. Furthermore, the reactivity of the complexes towards superoxide free radicals was assessed by employing the nitro blue tetrazolium (NBT) assay. The biological properties of the complexes were investigated in relation to their cytoprotective activity against the oxidative damage generated exogenously by using hydrogen peroxide in the Human Dermal Fibroblasts adult (HDFa) cell line as well as to their antimicrobial activity against the bacteria (Bacillus subtilis, Escherichia coli, Enterococcus faecalis, Pseudomonas aeruginosa, Staphylococcus aureus, Staphylococcus epidermidis). The relationship between physicochemical and biological properties of the complexes was discussed.

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Concentration distribution curves of the complexes as a function of pH (M:L = 1:1) calculated based on the stability constants listed in Table 2
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Fig1: Concentration distribution curves of the complexes as a function of pH (M:L = 1:1) calculated based on the stability constants listed in Table 2

Mentions: The equilibrium constants defined by Eqs. (1) and (2):1\documentclass[12pt]{minimal} \usepackage{amsmath} \usepackage{wasysym} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{amsbsy} \usepackage{mathrsfs} \usepackage{upgreek} \setlength{\oddsidemargin}{-69pt} \begin{document}$$ \mathrm{p}\mathrm{M}+\mathrm{q}\mathrm{L}+\mathrm{r}\mathrm{H}={\mathrm{M}}_{\mathrm{p}}{\mathrm{L}}_{\mathrm{q}}{\mathrm{H}}_{\mathrm{r}} $$\end{document}pM+qL+rH=MpLqHr2\documentclass[12pt]{minimal} \usepackage{amsmath} \usepackage{wasysym} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{amsbsy} \usepackage{mathrsfs} \usepackage{upgreek} \setlength{\oddsidemargin}{-69pt} \begin{document}$$ {\mathit{\mathsf{\beta}}}_{\mathrm{p}\mathrm{qr}}=\frac{\left[{\mathrm{M}}_{\mathrm{p}}{\mathrm{L}}_{\mathrm{q}}{\mathrm{H}}_{\mathrm{r}}\right]}{{\left[\mathrm{M}\right]}^{\mathrm{p}}{\left[\mathrm{L}\right]}^{\mathrm{q}}{\left[\mathrm{H}\right]}^{\mathrm{r}}} $$\end{document}βpqr=MpLqHrMpLqHr(where M is VO2+, Co2+ or Ni2+, L denotes the oxydiacetate ion, H is the proton and p, q, r are stoichiometric coefficients for the reaction) were refined by least-squares calculations using the Hyperquad2008 (version 5.2.19) computer program [20]. For the oxovanadium(IV) system, the formation of the hydroxo complexes of VO(IV) were taken into account in the calculations of the stability constants. The following formation constants were taken from the literature [35] and were fixed: logβ10–1 = −5.94, logβ20–2 = −6.95 and logβ10–3 = −18. The equilibrium models presented in Table 2 have given the best fitting of the calculated data to the experimental ones. Species distributions as a function of pH (molar ratio M:L equals 1:1) are shown in Fig. 1.Table 2


Physicochemical and biological properties of oxovanadium(IV), cobalt(II) and nickel(II) complexes with oxydiacetate anions.

Wyrzykowski D, Kloska A, Pranczk J, Szczepańska A, Tesmar A, Jacewicz D, Pilarski B, Chmurzyński L - Biol Trace Elem Res (2014)

Concentration distribution curves of the complexes as a function of pH (M:L = 1:1) calculated based on the stability constants listed in Table 2
© Copyright Policy - OpenAccess
Related In: Results  -  Collection

Show All Figures
getmorefigures.php?uid=PMC4352194&req=5

Fig1: Concentration distribution curves of the complexes as a function of pH (M:L = 1:1) calculated based on the stability constants listed in Table 2
Mentions: The equilibrium constants defined by Eqs. (1) and (2):1\documentclass[12pt]{minimal} \usepackage{amsmath} \usepackage{wasysym} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{amsbsy} \usepackage{mathrsfs} \usepackage{upgreek} \setlength{\oddsidemargin}{-69pt} \begin{document}$$ \mathrm{p}\mathrm{M}+\mathrm{q}\mathrm{L}+\mathrm{r}\mathrm{H}={\mathrm{M}}_{\mathrm{p}}{\mathrm{L}}_{\mathrm{q}}{\mathrm{H}}_{\mathrm{r}} $$\end{document}pM+qL+rH=MpLqHr2\documentclass[12pt]{minimal} \usepackage{amsmath} \usepackage{wasysym} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{amsbsy} \usepackage{mathrsfs} \usepackage{upgreek} \setlength{\oddsidemargin}{-69pt} \begin{document}$$ {\mathit{\mathsf{\beta}}}_{\mathrm{p}\mathrm{qr}}=\frac{\left[{\mathrm{M}}_{\mathrm{p}}{\mathrm{L}}_{\mathrm{q}}{\mathrm{H}}_{\mathrm{r}}\right]}{{\left[\mathrm{M}\right]}^{\mathrm{p}}{\left[\mathrm{L}\right]}^{\mathrm{q}}{\left[\mathrm{H}\right]}^{\mathrm{r}}} $$\end{document}βpqr=MpLqHrMpLqHr(where M is VO2+, Co2+ or Ni2+, L denotes the oxydiacetate ion, H is the proton and p, q, r are stoichiometric coefficients for the reaction) were refined by least-squares calculations using the Hyperquad2008 (version 5.2.19) computer program [20]. For the oxovanadium(IV) system, the formation of the hydroxo complexes of VO(IV) were taken into account in the calculations of the stability constants. The following formation constants were taken from the literature [35] and were fixed: logβ10–1 = −5.94, logβ20–2 = −6.95 and logβ10–3 = −18. The equilibrium models presented in Table 2 have given the best fitting of the calculated data to the experimental ones. Species distributions as a function of pH (molar ratio M:L equals 1:1) are shown in Fig. 1.Table 2

Bottom Line: The influence of DMSO as a co-solvent on the stability of the complexes as well as the oxydiacetic acid was evaluated.Furthermore, the reactivity of the complexes towards superoxide free radicals was assessed by employing the nitro blue tetrazolium (NBT) assay.The relationship between physicochemical and biological properties of the complexes was discussed.

View Article: PubMed Central - PubMed

Affiliation: Faculty of Chemistry, University of Gdańsk, Wita Stwosza 63, 80-308, Gdańsk, Poland, dariusz.wyrzykowski@ug.edu.pl.

ABSTRACT
The potentiometric and conductometric titration methods have been used to characterize the stability of series of VO(IV)-, Co(II)- and Ni(II)-oxydiacetato complexes in DMSO-water solutions containing 0-50 % (v/v) DMSO. The influence of DMSO as a co-solvent on the stability of the complexes as well as the oxydiacetic acid was evaluated. Furthermore, the reactivity of the complexes towards superoxide free radicals was assessed by employing the nitro blue tetrazolium (NBT) assay. The biological properties of the complexes were investigated in relation to their cytoprotective activity against the oxidative damage generated exogenously by using hydrogen peroxide in the Human Dermal Fibroblasts adult (HDFa) cell line as well as to their antimicrobial activity against the bacteria (Bacillus subtilis, Escherichia coli, Enterococcus faecalis, Pseudomonas aeruginosa, Staphylococcus aureus, Staphylococcus epidermidis). The relationship between physicochemical and biological properties of the complexes was discussed.

Show MeSH
Related in: MedlinePlus