1. Construct the potential-pH (Pourbaix) diagram for zinc using the following reactions and assuming the activity of all dissolved substances (i.e. any metal cations or anions) is 106. Label the stable species in each region. Designate regions as Active (Corrosion), Passive, or Immune. Ranges for potential -2.5 VSHE to +2 VSHE (Y-axis) and for pH -2 to 14 (X-axis) while plotting the results. {1} Zn²++2e−=Zn(s) (E。= -0.764 V vs.SHE) {2} ZnO(s)+2H++2e¯¯=Zn(s)+H₂O (E。=-0.439 V vs.SHE) {3} ZnO2+4H+2e¯=Zn(s)+ 2H2O (E0= +0.441V) {4}Zn²++H20=Zn0+2H+ (equilibrium constant = 3.16 X 10-³) {5} ZnO+H20=ZnO₂²+2H+ (equilibrium constant = 1.58 X 10-30)

1. Construct the potential-pH (Pourbaix) diagram for zinc using the following reactions and assuming the activity of all dissolved substances (i.e. any metal cations or anions) is 106. Label the stable species in each region. Designate regions as Active (Corrosion), Passive, or Immune. Ranges for potential -2.5 VSHE to +2 VSHE (Y-axis) and for pH -2 to 14 (X-axis) while plotting the results. {1} Zn²++2e−=Zn(s) (E。= -0.764 V vs.SHE) {2} ZnO(s)+2H++2e¯¯=Zn(s)+H₂O (E。=-0.439 V vs.SHE) {3} ZnO2+4H+2e¯=Zn(s)+ 2H2O (E0= +0.441V) {4}Zn²++H20=Zn0+2H+ (equilibrium constant = 3.16 X 10-³) {5} ZnO+H20=ZnO₂²+2H+ (equilibrium constant = 1.58 X 10-30)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 82AP

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