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freddy0622 freddy0622
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8 years ago
...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 -0.15
Ni2+ +  2e- ->Ni(s)     Volts 0.00
Fe2+ + 2e- -> Fe(s)  Volts -0.15
Ni2+ +  2e- ->Ni(s)     Volts 0.00
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!JRon@n!JRon@n
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8 years ago
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For the ppt of Fe(OH)2, the k = [OH]2 x [Fe]

Therefore, the concentration of Fe is 8.0 x 10-6, and for the next 2 parts we need to know the E values for Fe and Ni.
chemistryprobs,  Sarah Fergus

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