Q3 (10 pts). 1) Under what pH conditions can NO3 be reduced by Fe2+ into NO (via the following reaction), assuming [Fe2+} = 0.0001 and the ratio of {NO3} to [NO] is 1. NO3 + Fe2+ + H2O NO₂ + H+ + Fe(OH)3(s) 2) What is the ratio of the concentrations (or activity) of NO to NO in equilibrium with an aqueous Fe2+ - Fe(OH)3(s) system that has a pH of 7 and {Fe2+} = 0.0001. Note: The E, pe, and log K of the half reactions for the above redox reaction can be found in the appendix below. For 1) you need to balance the equation and get the log K for the complete reaction, which is related to the activity ratio of products and reactants. For 2) you are given pH, but to determine the ratio of one pair.

Q3 (10 pts). 1) Under what pH conditions can NO3 be reduced by Fe2+ into NO (via the following reaction), assuming [Fe2+} = 0.0001 and the ratio of {NO3} to [NO] is 1. NO3 + Fe2+ + H2O NO₂ + H+ + Fe(OH)3(s) 2) What is the ratio of the concentrations (or activity) of NO to NO in equilibrium with an aqueous Fe2+ - Fe(OH)3(s) system that has a pH of 7 and {Fe2+} = 0.0001. Note: The E, pe, and log K of the half reactions for the above redox reaction can be found in the appendix below. For 1) you need to balance the equation and get the log K for the complete reaction, which is related to the activity ratio of products and reactants. For 2) you are given pH, but to determine the ratio of one pair.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.6: Equilibria Involving Complex Ions

Problem 2.1ACP: Phosphate ions are abundant in cells, both as the ions themselves and as important substituents on...

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