# Why is concentration of nickel nitrate constant? [closed]

Consider a cell with both nickel electrodes and a solution of nickel nitrate ($$\ce{Ni(NO3)2}$$). Current is passed through the solution. The $$E°$$ values predict that nitrate in the solution should get reduced to nitrogen oxide. But a question regarding this has the answer given that the concentration does not change. Why is the concentration of nickel nitrate constant?

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• Are both electrodes made up of nickel and immersed in the same solution of nickel nitrate? What type of cell is it? If you can elaborate on the question, then it would be easier to answer. – Shoubhik Raj Maiti Dec 31 '18 at 13:43
• Yes both are immersed in the same solution of nickel nitrate. – Harsh Dec 31 '18 at 15:32
• Negatively-charged nitrate ions travelling to the also negatively-charged cathode doesn’t seem to be efficient. – Loong Dec 31 '18 at 15:50
• Also, the reduction of nitrate requires acid: $$\ce{NO3- + 2H+ + e- -> NO2 + H2O}$$ – Ben Norris Dec 31 '18 at 16:03
• Okay then the next possibility is reduction of $H+$ . Are there any other reactions taking place? – Harsh Dec 31 '18 at 16:09