PubMed · 12074232
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Chris H Miller. 2002. Tips on preparing instruments for sterilization.. https://pubmed.ncbi.nlm.nih.gov/12074232/
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This study investigated the surface characterizations and corrosion resistance of as-received commercial nickel-titanium (NiTi) dental orthodontic archwires from different manufacturers using a cyclic potentiodynamic test in artificial saliva with various acidities. An atomic force microscope was used to evaluate the surface topography of the NiTi wires. The surface chemical analysis of the passive film on the NiTi wires was characterized using X-ray photoelectron spectroscopy and Auger electron spectroscopy. A scanning electron microscope, together with an energy-dispersive spectrometer, was used to analyze the surface characterizations of the NiTi wires before and after the corrosion tests. Two-way analysis of variance was used to analyze the corrosion-resistance parameters with the factors of wire manufacturer and solution pH. The results showed that the surface structure of the passive film on the tested NiTi wires were identical, containing mainly TiO2, with small amounts of NiO. A different surface topography was observed on the NiTi wires from various manufacturers. The corrosion tests showed that both the wire manufacturer and solution pH had a statistically significant influence on the corrosion potential, corrosion rate, passive current, breakdown potential, and crevice-corrosion susceptibility. The difference in the corrosion resistance among these NiTi dental orthodontic archwires did not correspond with the surface roughness and pre-existing defects.
Apparent corrosion rates have been measured for several commercially available zerovalent irons by monitoring hydrogen evolution in closed cells. Sievert-type rate constants (ks) were determined to account for hydrogen entering the iron lattice. Thus corrected corrosion rates (Rcorr) are provided for all irons tested in this study. Because the rate of hydrogen entering the iron lattice increases with PH2(1/2), and the rate of hydrogen production from corrosion, far from equilibrium conditions, is independent of PH2, at some time under closed system conditions the two rates become equal and a steady-state PH2 is attained. A relation describing this condition has been derived: PH2SS = [Rcorr/ ks]2 For the granular irons considered in this study, PH2SS values vary from less than one to eight bars, in contrast to the calculated thermodynamic equilibrium PH2 values for anaerobic corrosion, which range from 138 to 631 bar depending on the assumed product of corrosion. Because groundwater flow at an iron permeable reactive barrier removes hydrogen gas in the dissolved state, PH2SS values will be less than calculated using the relation above. A method is presented to calculate PH2 values along the flow direction in a PRB, and thus the maximum PH2 value that can possibly develop, assuming no bacterial utilization of the produced hydrogen.
Recent strategies to reduce elevated nitrate concentrations employ metallic Fe0 as a reductant. Secondary products of Fe0 corrosion include magnetite (Fe3O4), green rust [Fe6(OH)12SO4], and wüstite [FeO(s)]. To our knowledge, no studies have been reported on the reactivity of NO3- with FeO(s). This project was initiated to evaluate the reactivity of FeO(s) with NO3- under abiotic conditions. Stirred batch reactions were performed in an anaerobic chamber over a range of pH values (5.45, 6.45, and 7.45), initial FeO(s) concentrations (1, 5, and 10 g L(-1)), initial NO3- concentrations (1, 10, and 15 mM), and temperatures (3, 21, 31, and 41 degrees C) for kinetic and thermodynamic determinations. Suspensions were periodically removed and filtered to measure dissolved nitrogen and iron species. Solid phases were characterized using X-ray diffraction (XRD) and scanning electron microscopy (SEM). Nitrate reduction by FeO was rapid and characterized by nearly stoichiometric conversion of NO3- to NH4+. Transient NO2- formation also occurred. The XRD and SEM results indicated the formation of Fe3O4 as a reaction product of the heterogeneous redox reaction. Kinetics of NO3- reduction suggested a rate equation of the type: -d[NO3-]/dt = k[FeO]0.57[H]0.22[NO3-]1.12 where k = 3.46 x 10(-3) +/- 0.38 x 10(-3) M(-1) s(-1), at 25 degrees C. Arrhenius and Eyring plots indicate that the reaction is surface chemical-controlled and proceeds by an associative mechanism involving a step where both NO3- and FeO(s) bind together in an intermediate complex.