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# a solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution..

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 a solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution.. ...which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x10^-10.A. Assuming that the hydroxide is 1.0 x 10^-2 M, calculate the concentration of Fe2+ ions in the solution.B. 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.c. use the nerst equation to calculate the potential of the above cell....which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x10^-10.A. Assuming that the hydroxide is 1.0 x 10^-2 M, calculate the concentration of Fe2+ ions in the solution.B. 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.c. use the nerst equation to calculate the potential of the above cell.Fe2+ + 2e- -> Fe(s)  Volts -0.15Ni2+ +  2e- ->Ni(s)     Volts 0.00Fe2+ + 2e- -> Fe(s)  Volts -0.15Ni2+ +  2e- ->Ni(s)     Volts 0.00 Read 3374 times 24 Replies
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!JRon@n!JRon@n
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