Fig. 2 Partial E -pH diagram for the equilibrium Ni 2+ + 2 e − = Ni for various values of log a Ni 2 + More

Fig. 3 Partial E -pH diagram for the equilibrium Ni + H 2 O = NiO + 2H + + 2 e − More

Fig. 39 Superimposed E -pH diagram of a 70Cu-30Zn alloy in 0.1 M NaCl. Lightly shaded area indicates the domain in which selective removal of zinc is expected in solutions free of copper ions. Intermediate shaded area indicates the domain in which both copper and zinc dissolves. Dark shaded More

Fig. 1 Iron E -pH diagram. Dashed lines a and b are explained in Fig. 7 and in the corresponding text. More

Fig. 4 Partial E -pH diagram for the equilibrium NO 2 − + 8 H + + 6 e − = NH 4 + + 2 H 2 O More

Fig. 5 Partial E -pH diagram for the Co 2+ /Co and CoO/Co couples for a Co 2 + = 1 More

Fig. 6 E -pH diagram for the cobalt-water system for various values of log a Co 2 + . (a) Partial E -pH diagram. (b) Complete E -pH diagram More

Fig. 7 The water E -pH diagram at 25 °C (298.15 K) and 1 bar More

Fig. 9 Simplified E -pH diagram for the iron-water system at 25 °C for a molality of dissolved iron equal to 10 −6 mol/kg. Pressure of hydrogen and oxygen, 1 atm More

Fig. 10 Simplified E -pH diagram for the sulfur-water system at 25 °C. The solid lines represent the stable system. The dashed lines represent the equilibria involving the metastable thiosulfates instead of the stable sulfates. Sulfur molality is 10 −4 mol/kg. Pressure of hydrogen and oxygen More

Fig. 11 E -pH diagram for nickel for a Ni 2 + = 10 − 4 More

Fig. 12 Partial E -pH diagram for copper for a Cu 2 + = 10 − 4 More

Fig. 13 E -pH diagram for the iron-sulfur-water system at 25 °C (298.15 K) in the case where the metastable thiosulfates are the only oxidized forms of sulfur. The stability domains are limited by the dotted lines for the water system, dashed lines for the sulfur-water system, and solid lines More

Fig. 14 E -pH diagram for the chromium-sulfur-water system at 25 °C (298.15 K) in the case where the thiosulfates are the only oxidized forms of sulfur. The stability domains are limited by the dotted lines for the water system, dashed lines for the sulfur-water system, and solid lines More

Fig. 16 E -pH diagram for the iron-water system at 300 °C (573.15 K). m Fe = 10 −6 mol/kg More

Fig. 17 E -pH diagram for the chromium-water system at 300 °C (573.15 K). m Cr = 10 −6 mol/kg More

Fig. 18 E -pH diagram for the iron-sulfur-water system at 300 °C (573.15 K) in the case where the thiosulfates are the only oxidized forms of sulfur. m S = 10 −4 mol/kg, m Fe = 10 −6 mol/kg More

Fig. 19 E -pH diagram for the system of sulfur, oxygen, and water adsorbed on iron at 25 °C (298.15 K) in the case where the thiosulfates are the only oxidized forms of sulfur. The stability domains are limited by the dotted lines for the water system, dashed lines for the sulfur-water system More

Fig. 20 E -pH diagram for the system of sulfur, oxygen, and water adsorbed on iron at 300 °C (573.15 K) in the case where the thiosulfates are the only oxidized forms of sulfur. The stability domains are limited by the dotted lines for the water system, dashed lines for the sulfur-water More

Fig. 1 E -pH diagram for iron-water system at 25 °C (77 °F). It is a graphic representation of thermodynamic stability. The potential E H is expressed in reference to the standard hydrogen potential. pε is defined as −log a e − where a e − is the activity of the free aqueous electrons More