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What is the standard potential value of a nitrate ion?
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Julie Marks
What is the standard potential value of a nitrate ion?
Electrochemical potentials, included standard ones, do not refer to a single species (e. g., nitrate ion), but to a redox couple, or, if preferred, to a half-reaction, taking place in one of the two half-cells of an electrochemical cell. If you are referring to this half-reaction: NO3-(aq) + 4H+(aq) + 3e- -> NO(g) + 2H2O(l) , well, its standard potential is +0.96 V.
Electrochemical potentials, included standard ones, do not refer to a single species (e. g., nitrate ion), but to a redox couple, or, if preferred, to a half-reaction, taking place in one of the two half-cells of an electrochemical cell. If you are referring to this half-reaction: NO3-(aq) + 4H+(aq) + 3e- -> NO(g) + 2H2O(l) , well, its standard potential is +0.96 V.
The nitrate ions are already in a reduced state, having a charge of -1. The copper instead reduces the silver ions, since they are able to accept electrons from the copper.
The nitrate ions are already in a reduced state, having a charge of -1. The copper instead reduces the silver ions, since they are able to accept electrons from the copper.
Electrochemical potentials, included standard ones, do not refer to a single species (e. g., nitrate ion), but to a redox couple, or, if preferred, to a half-reaction, taking place in one of the two half-cells of an electrochemical cell. If you are referring to this half-reaction: NO3-(aq) + 4H+(aq) + 3e- -> NO(g) + 2H2O(l) , well, its standard potential is +0.96 V.
Electrochemical potentials, included standard ones, do not refer to a single species (e. g., nitrate ion), but to a redox couple, or, if preferred, to a half-reaction, taking place in one of the two half-cells of an electrochemical cell. If you are referring to this half-reaction: NO3-(aq) + 4H+(aq) + 3e- -> NO(g) + 2H2O(l) , well, its standard potential is +0.96 V.
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The nitrate ions are already in a reduced state, having a charge of -1.
The copper instead reduces the silver ions, since they are able to accept electrons from the copper.
The nitrate ions are already in a reduced state, having a charge of -1.
The copper instead reduces the silver ions, since they are able to accept electrons from the copper.
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