“…Moreover rate of polymerization increased considerably and their growing will not be stopped. Effect of surfactant addition on rate of polymerization was previously reported for other polymers [20,21].…”
Poly(o-anisidine) (POA) was formed by successive cyclic voltammetry in monomer solution containing sodium dodecyl sulfate (SDS) at the surface of carbon paste electrode. Then Ni(II) ions were incorporated to electrode by immersion of the polymeric modified electrode having amine group in 0.1 M Ni(II) ion solution. Cyclic voltammetric and chronoamperometric experiments were used for the electrochemical study of this modified electrode; a good redox behavior of Ni(OH) 2 /NiOOH couple at the surface of electrode can be observed. The capability of this modified electrode for catalytic oxidation of folic acid was demonstrated. The amount of a and surface coverage (G*) of the redox species and catalytic chemical reaction rate constant (k) for folic acid oxidation were calculated. The catalytic oxidation peak current of folic acid was linearly dependent on its concentration and a linear calibration curve was obtained in the range of 0.1 to 5 mM with a correlation coefficient of 0.9994. The limit of detection (3s) was determined as 0.091 mM. This electrocatalytic oxidation was used as simple, selective and precise voltammetric method for determination of folic acid in pharmaceutical preparations.
“…Moreover rate of polymerization increased considerably and their growing will not be stopped. Effect of surfactant addition on rate of polymerization was previously reported for other polymers [20,21].…”
Poly(o-anisidine) (POA) was formed by successive cyclic voltammetry in monomer solution containing sodium dodecyl sulfate (SDS) at the surface of carbon paste electrode. Then Ni(II) ions were incorporated to electrode by immersion of the polymeric modified electrode having amine group in 0.1 M Ni(II) ion solution. Cyclic voltammetric and chronoamperometric experiments were used for the electrochemical study of this modified electrode; a good redox behavior of Ni(OH) 2 /NiOOH couple at the surface of electrode can be observed. The capability of this modified electrode for catalytic oxidation of folic acid was demonstrated. The amount of a and surface coverage (G*) of the redox species and catalytic chemical reaction rate constant (k) for folic acid oxidation were calculated. The catalytic oxidation peak current of folic acid was linearly dependent on its concentration and a linear calibration curve was obtained in the range of 0.1 to 5 mM with a correlation coefficient of 0.9994. The limit of detection (3s) was determined as 0.091 mM. This electrocatalytic oxidation was used as simple, selective and precise voltammetric method for determination of folic acid in pharmaceutical preparations.
“…solid electrolytic capacitors, metal protection coatings, etc. [22,23]. Protonation (p-doping) of amino sites at low pH allows charge transfer through the film during the EP and, therefore, virtually non-restricted growth [24].…”
Section: General Considerations and The Choice Of Materialsmentioning
A novel approach to preparation of composite asymmetric nanofiltration membranes is reported based on a thin selective layer deposited by electropolymerization (EP) on top of an asymmetrically porous and electronically conductive porous support. Support films with ultrafiltration characteristics were cast from a concentrated dispersion of carbon black particles, a few tens of nanometers large, in a solution of polysulfone followed by precipitation in a non-solvent bath (phase inversion). Composite membranes with poly(phenylene oxide) and polyaniline thin top layers were prepared by EP deposition from solutions of phenol and aniline, respectively, of which polyaniline film demonstrated a dense uniform structure and water flux and rejection to sucrose and magnesium sulfate in the nanofiltration range.
“…The adsorption and/or precipitation of a corrosion inhibitor onto a metal surface can be evaluated perfectly by the quartz crystal analysis (QCA) method (Kanungo, Kumar, and Contractor 2002, Park and Yoo 2003, Losito et al 2005, 1313, and Akrout, et al 2007. By using this technique, the increase in mass at the QCA electrode is calculated from the decrease in frequency according to the Sauerbrey equation (Park and Yoo 2003),…”
Section: Inhibition Efficiencies Of Corrosion Inhibitorsmentioning
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