A solution is prepared in which a small amount of Fe 2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates.
* the Molarity of OH- may be extra unneeded info.
A battery is prepared using the above solution with an iron wire dipping into it as one half-cell. The other half-cell is the standard nickel electrode. Write the balanced net ionic equation for the cell reaction.
Please help! I think the reaction to start off with is Fe2+ + OH- = Fe(OH)2...from there, I write the half reactions, but Idk how to write the half reactions, and what to do afterwards!
* the Molarity of OH- may be extra unneeded info.
A battery is prepared using the above solution with an iron wire dipping into it as one half-cell. The other half-cell is the standard nickel electrode. Write the balanced net ionic equation for the cell reaction.
Please help! I think the reaction to start off with is Fe2+ + OH- = Fe(OH)2...from there, I write the half reactions, but Idk how to write the half reactions, and what to do afterwards!