Write equations for the half-reactions that occur at the anode and cathode for t

Question

Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of the following aqueous solution. (See the table. Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) Ni(NO3)2(aq)

Explanation / Answer

Ni(NO3)2 (aq) + NaOH (aq) --> NiOH (s) + Na(NO3)2 (aq) There are a few mistakes. Ni is a 2+ or 3+ charge. We know it is a 2+ charge from Ni(NO3)2 Ni(NO3)2 (aq) + 2NaOH (aq) --> Ni(OH)2 (s) + 2NaNO3 (aq) or A net-ionic equation shows only components that actually react during a reaction. So...what I personally would do when working this problem would first put it into a complete ionic equation because it just makes it simpler for me to see which ones actually react, oh, and showing the stage the compounds are in helps me also! (I'm assuming the reactions are being described in solutions) So, here's what I would do: Molecular equation - Ni(NO3)2 (aq) + Na2CO3 (aq) ---> NiCO3 (s) + 2NaNO3 (aq) Complete Ionic equation - Ni+2(aq) + NO3-(aq) + Na+(aq) + CO3-2(aq) ---> NiCO3 (s) + 2Na+(aq) + NO3-(aq) The complete ionic equation helps me because I can easily see which compounds actually react, so I would write the net-ionic equation like this: Ni+2(aq) + CO3-2(aq) ---> NiCO3 (s) And your spectator ions would be Na+ and NO3- (because they remain unchanged) I really hope this makes sense, and I hope this helps!

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