2 Ag+(aq) + Fe(s) --> 2 Ag(s) + Fe2+(aq)
In which directions do the cations and anions migrate through the solution?
cations
toward the silver cathode or
toward the iron cathode
thanks
Here is a film that explains it very well. After the film is finished you can click on the buttons at the bottom of the picture to get an explanation of how the ions move on the Zn side of the salt bridge and on the Cu side of the salt bridge.
http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/galvan5.swf
In the given chemical equation, 2 Ag+ ions (cations) are reacting with a solid Fe (iron), resulting in the formation of 2 Ag (silver) atoms and Fe2+ ions (cations) in the solution.
To determine the direction in which the cations migrate through the solution, we need to consider the process of electrolysis. During electrolysis, cations will move towards the cathode, which is the negatively charged electrode.
In this case, we have two potential cathodes: the silver cathode and the iron cathode. To determine which cathode the cations will migrate towards, we need to consider the standard reduction potentials of the two cation species involved.
Standard reduction potentials are a measure of the tendency of a species to gain electrons and be reduced. The species with a more positive reduction potential will be preferentially reduced (gain electrons) at the cathode.
By referring to a table of standard reduction potentials, we can determine that Ag+ has a more positive reduction potential compared to Fe2+. Therefore, the cations (Ag+) will migrate towards the silver cathode.
So, in the given electrochemical reaction, the cations (Ag+) will migrate towards the silver cathode.