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Journal articles on the topic 'Diagramme potentiel ph'

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Published: 4 June 2021

Last updated: 8 February 2022

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1

Galicia, Laura, Yunny Meas, and Ignacio Gonzalez. "Diagramme potentiel—pH pour le systeme Fe(III)Fe(II)/H2O en presence de 1,10 phenanthroline." Electrochimica Acta 31, no. 10 (October 1986): 1333–34. http://dx.doi.org/10.1016/0013-4686(86)80156-6.

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2

Inoue, Hiroyuki. "The use of Potential-pH Equilibrium Diagram." Zairyo-to-Kankyo 45, no. 12 (1996): 746–48. http://dx.doi.org/10.3323/jcorr1991.45.746.

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3

Lee, Kyu Hwan. "Formation of Metallic Nanoparticles Using Potential-pH Diagram." Journal of the Korean institute of surface engineering 50, no. 2 (April 30, 2017): 131–39. http://dx.doi.org/10.5695/jkise.2017.50.2.131.

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4

Angus, John C., Bei Lu, and Michael J. Zappia. "Potential-pH diagrams for complex systems." Journal of Applied Electrochemistry 17, no. 1 (January 1987): 1–21. http://dx.doi.org/10.1007/bf01009127.

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5

Wood, P. M. "The potential diagram for oxygen at pH 7." Biochemical Journal 253, no. 1 (July 1, 1988): 287–89. http://dx.doi.org/10.1042/bj2530287.

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Successive one-electron reductions of molecular oxygen yield the superoxide radical (O2-) H2O2, the hydroxyl radical (OH) and water. Redox potentials at pH 7 for one-, two- and four-electron couples involving these states are presented as a potential diagram. The significance of each of these potentials is explained. The complete potential diagram enables complex systems to be rationalized, such as production of OH by H2O2 plus Fe3+.

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6

Reymond, Frédéric, Guillaume Steyaert, Pierre-Alain Carrupt, Bernard Testa, and Hubert Girault. "Ionic Partition Diagrams: A Potential−pH Representation." Journal of the American Chemical Society 118, no. 47 (January 1996): 11951–57. http://dx.doi.org/10.1021/ja962187t.

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7

Kriksunov, L. B., and D. D. Macdonald. "Potential-pH Diagrams for Iron in Supercritical Water." CORROSION 53, no. 8 (August 1997): 605–11. http://dx.doi.org/10.5006/1.3290292.

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8

Muñoz-Portero, M. J., T. Nachiondo, E. Blasco-Tamarit, A. Vicent-Blesa, and J. García-Antón. "Potential-pH Diagrams of Iron in Concentrated Aqueous LiBr Solutions at 25°C." Corrosion 74, no. 10 (June 29, 2018): 1102–16. http://dx.doi.org/10.5006/2865.

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Potential-pH diagrams of iron are developed in aqueous LiBr solutions with concentrations of 400 g/L, 700 g/L, 850 g/L, and 992 g/L LiBr at 25°C, which are common concentrations in different parts of absorption machines. Comparison of the potential-pH diagrams of iron in the absence and the presence of concentrated aqueous LiBr solutions shows that the corrosion area at acid, neutral, and weak alkaline pH extends to lower potentials and higher pH values with the increase of LiBr concentration, as a result of formation of the aqueous species FeBr2(aq) and FeBr3(aq) and destabilization of the solid species Fe, Fe(OH)2(s), Fe3O4, and Fe2O3.

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9

Minguzzi, Alessandro, Fu-Ren F. Fan, Alberto Vertova, Sandra Rondinini, and Allen J. Bard. "Dynamic potential–pH diagrams application to electrocatalysts for wateroxidation." Chem. Sci. 3, no. 1 (2012): 217–29. http://dx.doi.org/10.1039/c1sc00516b.

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10

Nikolaychuk, Pavel Anatolyevich. "The revised potential – pH diagram for Pb – H2O system." Ovidius University Annals of Chemistry 29, no. 2 (August 22, 2018): 55–67. http://dx.doi.org/10.2478/auoc-2018-0008.

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Abstract Thermodynamic properties of lead species in aqueous solution are collected. The chemical equilibria between various forms of Pb(II) are considered. The speciation diagrams for the equilibria 4[PbOH]+(aq) ⇄ [Pb4(OH)4]4+(aq) and 2[Pb3(OH)4]2+(aq) ⇄ [Pb6(OH)8]4+(aq), and the thermodynamic activity - pH diagram of Pb(II) species are plotted. Basic chemical and electrochemical equilibria for lead are calculated. The potential - pH diagram for Pb - H2O system is revised.

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11

KUBAL, M., and F. PANACEK. "Potential-pH diagram for Fe–H2O–citric acid system." British Corrosion Journal 30, no. 4 (January 1995): 309–11. http://dx.doi.org/10.1179/bcj.1995.30.4.309.

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12

Tyurin, Aleksandr Georgievich, Dmitriy Andreevich Manannikov, Vladimir Pavlovich Parshukov, Anna Valeryevna Antonova, and Pavel Anatolyevich Nikolaychuk. "Method of estimation of corrosion stability of multicomponent alloys using equilibrium and polarization potential – pH diagrams." Anti-Corrosion Methods and Materials 63, no. 5 (2016): 386–97. http://dx.doi.org/10.1108/acmm-12-2014-1479.

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Purpose The purpose of this study is to develop a method of thermodynamic and kinetic evaluation of corrosion properties of alloys. Design/methodology/approach Method of estimation of corrosion-electrochemical behaviour of multicomponent alloys is proposed. The method takes into account both thermodynamic and kinetic data and is based on mutual construction of equilibrium and polarization potential – pH diagrams. The usage of the proposed method is illustrated in the example of the structural steel 20KT. Findings Passivation of steel 20KT is determined by formation of oxide film based on magnetite (Fe3O4); silicon, manganese and copper oxides as well as manganese sulphides can be locally included into the inner side of the passivation layer. An experimental potential – pH diagram of steel 20KT is constructed. Interpreting the results of polarization measurements revealed good agreement between equilibrium and polarization potential – pH diagrams. Originality/value It is shown in the example of structural steel 20KT that for interpretation of experimental potential – pH diagrams, one should compare them with corresponding equilibrium diagrams for multicomponent alloys rather than with Pourbaix diagrams for pure metals. The corrosion properties of steel 20KT are estimated using equilibrium and polarization potential – pH diagrams.

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13

SHINAGAWA, Tsutomu, and Masanobu IZAKI. "Application of Potential-pH Diagrams to the Electrodeposition of Metal Oxides." Journal of The Surface Finishing Society of Japan 64, no. 2 (2013): 94–98. http://dx.doi.org/10.4139/sfj.64.94.

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14

YOU, Hai-xia, Hong-bin XU, Yi ZHANG, Shi-li ZHENG, and Yi-ying GAO. "Potential—pH diagrams of Cr-H2O system at elevated temperatures." Transactions of Nonferrous Metals Society of China 20 (May 2010): s26—s31. http://dx.doi.org/10.1016/s1003-6326(10)60006-4.

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15

Kolodziej, Barbara, and Fathi Habashi. "High temperature potential/pH diagrams for the chlorine–water system." Canadian Journal of Chemistry 63, no. 4 (April 1, 1985): 935–39. http://dx.doi.org/10.1139/v85-155.

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Thermodynamic evidence supports the view that the reaction [Formula: see text] takes place above 127 °C at pH = 0. An increase in HCl concentration and/or oxygen partial pressure allow the reaction to proceed at lower temperature.

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16

Cubicciotti, Daniel. "Potential-pH diagrams for alloy-water systems under LWR conditions." Journal of Nuclear Materials 201 (May 1993): 176–83. http://dx.doi.org/10.1016/0022-3115(93)90173-v.

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17

Chandra-ambhorn, Somrerk, Wisarut Wachirasiri, and Gobboon Lothongkum. "E-pH diagrams for 316L stainless steel in chloride solutions containing SO42− ions." Anti-Corrosion Methods and Materials 63, no. 6 (November 7, 2016): 431–36. http://dx.doi.org/10.1108/acmm-10-2014-1454.

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Purpose This paper aims to construct the E-pH diagrams for AISI 316L stainless steel in chloride solutions containing SO42− ions and therefore investigate the role of SO42− ions on pitting corrosion of stainless steel. Design/methodology/approach A cyclic potentiodynamic polarisation method was performed to obtain polarisation curves at different pH. From these curves, corrosion, primary passivation, pitting and repassivation potentials were determined and plotted as a function of pH giving the E-pH diagram. Findings The addition of SO42− ions to 10,650 ppm NaCl solution up to 3,000 ppm widened the passivation regime of the E-pH diagram mainly by shifting the pitting corrosion potential to the noble direction. This indicated the inhibiting role of SO42− on the nucleation of new pits in the transpassive region. It also stabilised the pitting corrosion potential at the pH ranging from 5 to 11. However, at pH 7, it caused the pit area to increase, implying the catalytic role of SO42− on the pit growth. Finally, it did not change the types of ions dissolved in solutions after pitting. Practical implications The diagrams can be used as a guideline in industries to determine the passivation regime of the AISI 316L stainless steel in chloride- and sulphate-containing solutions. Originality/value This paper reported the E-pH diagrams for the AISI 316L stainless steel in chloride solutions containing SO42− ions. The roles of pH and SO42− ions on pitting corrosion were innovatively discussed using a point defect model.

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18

Seo, Yong-Jin, Sung-Woo Park, and Woo-Sun Lee. "Application of Potential-pH Diagram and Potentiodynamic Polarization of Tungsten." Transactions on Electrical and Electronic Materials 7, no. 3 (June 1, 2006): 108–11. http://dx.doi.org/10.4313/teem.2006.7.3.108.

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19

Tamilmani, Subramanian, Wayne Huang, Srini Raghavan, and Robert Small. "Potential-pH Diagrams of Interest to Chemical Mechanical Planarization of Copper." Journal of The Electrochemical Society 149, no. 12 (2002): G638. http://dx.doi.org/10.1149/1.1516224.

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20

YAGI, Shunsuke. "Construction of the Formation Processes of Metallic Nanoparticles Using Potential-pH Diagrams." Journal of The Surface Finishing Society of Japan 64, no. 2 (2013): 88–93. http://dx.doi.org/10.4139/sfj.64.88.

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21

Pound, BG, GA Wright, and RM Sharp. "Electrochemical Phase Diagrams for the Fe/S/H2O System under Geothermal Conditions." Australian Journal of Chemistry 38, no. 5 (1985): 643. http://dx.doi.org/10.1071/ch9850643.

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Previously published electrochemical phase (potential-pH) diagrams for the Fe/S/H2O system at elevated temperatures are assessed. It is concluded that the potential-pH equations derived by Biernat and Robins1 can be used to provide reliable diagrams over the temperature range 298-573 K. These equations were used to derive a set of diagrams relevant to geothermal fluids in general terms, so that the corrosion products of iron and ferrous alloys immersed in these fluids may be predicted. In addition, diagrams are presented for geothermal fluids in the Broadlands and Wairakei fields in New Zealand. The significant changes in the E-pH diagrams as the temperature increases over the range 298-573 K are that the region of stability for Fe(OH)3- widens and the regions of stability for FeS2 and Fe3O4 and, at higher temperatures, FeS, shrink in size.

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22

OHTSUKA, Toshiaki. "Potential-pH Diagram for Understanding the Metallic Corrosion and its Limitation." Journal of The Surface Finishing Society of Japan 64, no. 2 (2013): 99–103. http://dx.doi.org/10.4139/sfj.64.99.

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23

Tominaga, Masato, Yuto Yatsugi, and Noriaki Watanabe. "Oxidative corrosion potential vs. pH diagram for single-walled carbon nanotubes." RSC Advances 4, no. 52 (2014): 27224. http://dx.doi.org/10.1039/c4ra02875a.

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24

Chai, Liyuan, Zhihui Yang, Yunyan Wang, Rong Deng, Wenjie Zhu, and Shunhong Huang. "Potential-pH diagram for “Leucobacter sp. Ch-1–Cr–H2O” system." Journal of Hazardous Materials 157, no. 2-3 (September 2008): 518–24. http://dx.doi.org/10.1016/j.jhazmat.2008.01.064.

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25

Marcus, Philippe, and Elie Protopopoff. "Potential‐pH Diagrams for Sulfur and Oxygen Adsorbed on Chromium in Water." Journal of The Electrochemical Society 144, no. 5 (May 1, 1997): 1586–90. http://dx.doi.org/10.1149/1.1837645.

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26

Protopopoff, Elie, and Philippe Marcus. "Potential–pH diagrams for hydroxyl and hydrogen adsorbed on a copper surface." Electrochimica Acta 51, no. 3 (October 2005): 408–17. http://dx.doi.org/10.1016/j.electacta.2005.04.036.

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27

Genies, E. M., and E. Vieil. "Theoretical charge and conductivity ‘state - diagrams’ for polyaniline versus potential and pH." Synthetic Metals 20, no. 1 (April 1987): 97–108. http://dx.doi.org/10.1016/0379-6779(87)90549-2.

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28

Lin, Peijia, Xinbo Yang, Joshua M. Werner, and Rick Q. Honaker. "Application of Eh-pH Diagrams on Acid Leaching Systems for the Recovery of REEs from Bastnaesite, Monazite and Xenotime." Metals 11, no. 5 (April 29, 2021): 734. http://dx.doi.org/10.3390/met11050734.

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Bastnaesite, monazite and xenotime are rare earth minerals (REMs) that are typical sources for rare earth elements (REEs). To advance the understanding of their leaching and precipitation behavior in different hydrometallurgical processes, Eh-pH diagrams were constructed and modified using the HSC 9.9 software. The aqueous stability of rare earth elements in H2O and acid leaching systems, i.e., the REE-Ligands-H2O systems, were depicted and studied based on the Eh-pH diagrams. This study considers the most relevant lixiviants, their resulting equilibrium states and the importance in the hydrometallurgical recovery of rare earth elements (REMs). A literature review was performed summarizing relevant Eh-pH diagrams and associated thermodynamic data. Shifting stability regions for REEs were discovered with additions of acid ligands and a narrow stability region for soluble REE-(SO4/Cl/NO3) complexes under highly acidic conditions. As such, the recovery of REEs can be enhanced by adjusting pH and Eh values. In addition, the Eh-pH diagrams of the major contaminants (i.e., Fe, Ca and Al) in leaching systems were studied. The resulting Eh-pH diagrams provide possible insights into potential passivation on the particle surfaces due to the formation of an insoluble product layer.

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29

Jin-Ming, WU, and ZENG Ying. "Predominance Diagrams of Dissolved Species and Potential-pH Diagrams of V-H₂O System." Acta Physico-Chimica Sinica 23, no. 09 (2007): 1411–14. http://dx.doi.org/10.3866/pku.whxb20070919.

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30

Demidov, A. I., and E. N. Volkova. "Potential-pH diagram for the nickel-water system containing nickel(III) metahydroxide." Russian Journal of Applied Chemistry 82, no. 8 (August 2009): 1498–500. http://dx.doi.org/10.1134/s1070427209080333.

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31

Cushman, Richard J., Peter M. McManus, and Sze Cheng Yang. "Spectroelectrochemical study of polyaniline: the construction of a pH-potential phase diagram." Journal of Electroanalytical Chemistry and Interfacial Electrochemistry 219, no. 1-2 (March 1987): 335–46. http://dx.doi.org/10.1016/0022-0728(87)85051-9.

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32

Muñoz-Portero, M. J., J. García-Antón, J. L. Guiñón, and V. Pérez-Herranz. "Pourbaix Diagrams for Copper in Aqueous Lithium Bromide Concentrated Solutions." Corrosion 60, no. 8 (August 1, 2004): 749–56. http://dx.doi.org/10.5006/1.3287854.

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Abstract Pourbaix diagrams (electrode potential-pH diagrams) for Cu-Br−-H2O systems at 25°C were developed in 400-g/L and 700-g/L (4.61-M and 8.06-M) lithium bromide (LiBr) solutions, common concentrations in different parts of refrigeration plants. The diagrams were compared with the simple Cu-H2O system at 25°C. Pourbaix diagrams were constructed from standard Gibbs free energy data (ΔG°) of all the species considered. Conventional procedures were followed to calculate the electrochemical and chemical equilibria from standard Gibbs free energy data. Equilibria for Cu-Br−-H2O systems at 25°C were determined for bromide ion activities of 15.61 and 194.77, which correspond to 400-g/L and 700-g/L LiBr solutions, respectively. Activities of all the ion species containing copper were plotted for 10−6, 10−4, 10−2, and 100. Comparison of the simple Cu-H2O system with the diagrams for Cu-Br−-H2O systems at 25°C showed that the formation of CuBr2− complexes extended the copper solubility range to both higher pH values and lower potentials by destabilizing the formation of copper oxides and promoting more active behavior of the metal. The effect was enhanced at higher bromide ion activities.

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33

Silverman, D. C., and A. L. Silverman. "Potential-pH (Pourbaix) Diagrams as Aids for Screening Corrosion Inhibitors and Sequestering Agents." CORROSION 66, no. 5 (May 2010): 055003–055003. http://dx.doi.org/10.5006/1.3430463.

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34

Aksu, Serdar. "Potential-pH Diagrams of Copper for the Planarization Slurries with Different Complexing Agents." ECS Transactions 19, no. 7 (December 18, 2019): 15–24. http://dx.doi.org/10.1149/1.3123770.

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35

Jingyi, Zuo, Marcel Pourbaix, Xu Chunchun, and Liu Youping. "Kinetic and thermodynamic behaviour inside occluded corrosion cells interpreted by potential/pH diagrams." Corrosion Science 29, no. 5 (January 1989): 557–66. http://dx.doi.org/10.1016/0010-938x(89)90007-3.

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36

KUBAL, M., and F. PANACEK. "Potential-pH diagram for Fe–H₂O–citric acid system." British Corrosion Journal 30, no. 4 (January 1, 1995): 309–11. http://dx.doi.org/10.1179/000705995798113745.

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37

Loučka, T. "The potential-pH diagram for the Ru−H2O−Cl− system at 25°C." Journal of Applied Electrochemistry 20, no. 3 (May 1990): 522–23. http://dx.doi.org/10.1007/bf01076067.

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38

Muñoz-Portero, M. J., J. García-Antón, J. L. Guiñón, and V. Pérez-Herranz. "Pourbaix Diagrams for Nickel in Concentrated Aqueous Lithium Bromide Solutions at 25°C." Corrosion 63, no. 7 (July 1, 2007): 625–34. http://dx.doi.org/10.5006/1.3278412.

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Abstract Pourbaix diagrams (electrode potential-pH diagrams) for the Ni-Br−-H2O system at 25°C were developed in 400-g/L, 700-g/L, and 850-g/L (4.61-M, 8.06-M, and 9.79-M) lithium bromide (LiBr) solutions, which are common concentrations found in different parts of absorption devices. The diagrams were compared with the simple Ni-H2O system at 25°C. Pourbaix diagrams were constructed from standard Gibbs free energy of formation (ΔGfo) data at 25°C for all the species considered. Conventional procedures were followed to calculate the electrochemical and chemical equilibria from ΔGfo data Equilibria for the Ni-Br−-H2O system at 25°C were determined for bromide ion activities of 15.61, 194.77, and 650.06, which corresponded to the 400-g/L, 700-g/L, and 850-g/L LiBr solutions, respectively. Activities of all the dissolved species containing nickel were plotted for 10−6, 10−4, 10−2, and 100. Comparison of the simple Ni-H2O system at 25°C with the diagrams illustrating the effect of Br− activity showed that the formation of aqueous NiBr2(aq) extended the nickel solubility range to both higher pH values and lower potentials, particularly in acid, neutral, and weak alkaline areas of the diagrams, as a result of destabilization of β-Ni(OH)2, and promotion of a more active behavior of nickel. The effect was enhanced at higher bromide ion activities.

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39

Povar, Igor, and Oxana Spinu. "Ruthenium redox equilibria: 3. Pourbaix diagrams for the systems Ru-H2O and Ru-Cl--H2O." Journal of Electrochemical Science and Engineering 6, no. 1 (April 21, 2016): 145. http://dx.doi.org/10.5599/jese.229.

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<p class="PaperAbstract"><span lang="EN-US">On the basis of selected thermodynamic data, the standard electrode potentials of possible half reactions in the Ru-H<sub>2</sub>O and Ru-Cl<sup>-</sup>-H<sub>2</sub>O systems have been calculated. Using the thermodynamic approach developed by the authors, the potential - pH and potential - pCl diagrams for the considered system have been built.</span></p>

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40

Povar, Igor, Oxana Spinu, Inga Zinicovscaia, Boris Pintilie, and Stefano Ubaldini. "Revised Pourbaix diagrams for the vanadium – water system." Journal of Electrochemical Science and Engineering 9, no. 2 (February 28, 2019): 75–84. http://dx.doi.org/10.5599/jese.620.

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The forms of occurrence of vanadium metal are determined by the major chemical reactions in the aquatic environment such as hydrolysis, oxidation, reduction, and precipitation. Depending on pH, potential and total concentration of inorganic ions and organic ligands, vanadium compounds may undergo various transformations to produce a whole range of chemical forms in aqueous systems. In this paper, a novel approach has been applied for calculating potential-pH (Pourbaix) diagrams, based on the developed thermodynamic analysis of chemical equilibria in the V–H2O system. On the basis of currently revised thermodynamic data for V(III), V(IV) and V(V) hydrolysis and original thermodynamic and graphical approach used, the repartition of their soluble and insoluble chemical species has been investigated. By means of ΔG–pH diagrams, the areas of thermodynamic stability of V(IV) and V(V) hydroxides have been established for a number of analytical concentrations of vanadium in heterogeneous mixtures. The obtained results, based on the thermodynamic analysis and graphic design of calculated data, are in good agreement with available experimental data.

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41

Zuo, J. Y., M. Pourbaix, Y. P. Liu, and C. C. Xu. "Potential-pH Diagrams of Stress Effects on Occluded Cell Corrosion Inside Stress Corrosion Cracks." CORROSION 51, no. 3 (March 1995): 177–84. http://dx.doi.org/10.5006/1.3294359.

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42

Loučka, Tomáš, and Zdenko Ternbach. "Potential-pH diagrams for the systems Ir-H2O-Cl-, Pt-H2O-Cl-, and Pd-H2O-Cl- at 25 °C." Collection of Czechoslovak Chemical Communications 55, no. 4 (1990): 987–93. http://dx.doi.org/10.1135/cccc19900987.

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43

Bai, X. D., D. H. Zhu, and B. X. Liu. "The establishment of a potential-pH diagram for phosphorous implanted iron in aqueous solutions." Nuclear Instruments and Methods in Physics Research Section B: Beam Interactions with Materials and Atoms 103, no. 4 (December 1995): 440–45. http://dx.doi.org/10.1016/0168-583x(95)00666-4.

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44

Protopopoff, Elie, and Philippe Marcus. "Potential–pH diagram for sulfur and hydroxyl adsorbed on silver in water containing sulfides." Electrochimica Acta 63 (February 2012): 22–27. http://dx.doi.org/10.1016/j.electacta.2011.12.030.

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45

Maliy, Liubov, and Gennady Mokrousov. "Thermodynamic Stability and Interfacial Reactions of CdS, ZnS and Cd_1-xZn_xS in Aqueous Solution." Solid State Phenomena 194 (November 2012): 175–78. http://dx.doi.org/10.4028/www.scientific.net/ssp.194.175.

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This study is devoted to understanding the thermodynamic basis of the process of synthesis of ZnS, CdS and their solid solutions in aqueous solutions in order to obtain thin films of required composition. The typical interfacial reactions were considered, and the thermodynamic calculations of the possible redox reactions and the reaction standard electrode potentials have been done. The composition of a solution is analyzed by means of thermodynamic diagrams as a function of redox potential versus pH. It has been demonstrated that the near-surface layer with the defect structure and the excess of sulfur on a surface can be formed in case of ZnS at pH < 1.5 during the synthesis. The application of obtained data in the synthesis of semiconducting materials is also shown.

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46

Shih, H. C., J. C. Oung, J. T. Hsu, J. Y. Wu, and F. I. Wei. "Applications of electrochemical hysteresis for constructing the experimental potential-pH diagram for steels in seawater." Materials Chemistry and Physics 37, no. 3 (April 1994): 230–36. http://dx.doi.org/10.1016/0254-0584(94)90158-9.

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47

Loučka, Tomáš. "The Potential-pH Diagrams Depicting the Hydrogen Chemisorption in the Pt-H2O, Ir-H2O, and Rh-H2O Systems at 25 °C." Collection of Czechoslovak Chemical Communications 60, no. 4 (1995): 553–58. http://dx.doi.org/10.1135/cccc19950553.

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Thermodynamic data for the chemisorption of hydrogen on the Pt, Ir, and Rh electrodes were evaluated from data in the literature. On the basis of these data, the potential-pH diagrams were calculated for the Pt-H2O, Ir-H2O, and Rh-H2O systems describing the hydrogen chemisorption. For the hydrogen chemisorption, the surface was considered to be uniformly inhomogeneous.

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48

Guo, Yonglang. "A New Potential‐pH Diagram for an Anodic Film on Pb in H 2 SO 4." Journal of The Electrochemical Society 139, no. 8 (August 1, 1992): 2114–20. http://dx.doi.org/10.1149/1.2221188.

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49

Montiel Hernández, J. F., M. I. Reyes Valderrama, I. Rivera Landero, C. H. Rios-Reyes, M. A. Veloz Rodríguez, F. Patiño Cardona, and V. E. Reyes-Cruz. "Thermodynamic Study of Leached Metals (Cu, Zn and Ni) from Waste Printed Circuits by Electrochemical Method." Advanced Materials Research 976 (June 2014): 86–90. http://dx.doi.org/10.4028/www.scientific.net/amr.976.86.

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A thermodynamic study (Pourbaix type diagrams, using the software Hydra/Medusa) of acid leaching solutions to obtain the electrochemical recovery of Ni, Cu and Zn present in printed circuit boards is reported. Solutions were characterized by atomic absorption spectroscopy at room temperature. The metals were leached in a 0.9237 M H2SO4 solution (pH = 1.56) at temperatures of 313, 323, 333 and 343 K. From this data, the reduction potentials were determined for each metal, finding the values of -0.0024, -1.1274 and-0.5892 V vs calomel for Cu, Ni and Zn, respectively. Displacement in the reduction potential with the increase of the metal concentration in the leaching solution was observed.

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MANANNIKOV, Dmitrii Andreevich, Vladimir Pavlovich PARSHUKOV, and Pavel Anatolyevich NIKOLAYCHUK. "EXPERIMENTAL AND THEORETICAL INVESTIGATION OF THE CORROSION PROPERTIES OF STEEL X13 IN THE ACETIC ACID AT 20 AND 80°С." Periódico Tchê Química 14, no. 27 (January 20, 2017): 19–29. http://dx.doi.org/10.52571/ptq.v14.n27.2017.19_periodico27_pgs_19_29.pdf.

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Abstract:

Polarisation curves of stainless steel Х13 in a 5% NaCl + 0.5% CH3COOH + CH3COONa + CO2 (PCO2 = 0.1 МPa) solution at рН 3 and 4 and temperatures 20 and 80°С were obtained by the potentiostatic method. The corrosion-electrochemical characteristics of the steel in these environments were measured. The potential – pH diagrams of system steel X13 – CH3COOH – CO2 – H2O were constructed and the corrosion behaviour of the steel was determined using these diagrams. The passivation of the steel may proceed due to the formation of iron chromite (FeCr2O4) phase layer and of iron oxalate (FeC2O4) polylayer.

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