balancing redox rxns [ENDORSED]

[emmaferry2D]

Write the half-reactions and devise a galvanic cell (write a cell diagram) to study each of the following reactions:

(a)
AgBr(s)⇌Ag+(aq)+Br−(aq),a solubilityequilibrium
(b) H+(aq)+OH−(aq)→H2O(l),the Brønsted neutralizationreaction
(c) Cd(s)+2Ni(OH)3(s)→Cd(OH)2(s)+2Ni(OH)2(s), the reaction in the nickel−cadmium cell

For redox reactions like a and b I am confused on how to write the half reactions and determine the oxidation states.
For example in a:
I thought the half reactions would be
AgBr--> Ag+
AgBr--> Br-
But then I would think the two oxidation states would be the same on both sides of the reaction for both Ag and Br
in anyone could explain this to me that would be great!

[Chem_Mod]

This is a harder one to figure out with the information given.

If one was given the cell diagram then straight forward.

Ag(s) is the same electrode for anode and cathode.
What makes the two half-reactions different are the solutions (electrolytes) the electrodes are in.

Ag(s) anode is in contact with a solution that contains Br-(aq), and the Ag(s) is oxidized to Ag+(aq).

Ag(s) cathode is in contact with a solution that contains Ag+(aq), and the Ag+(aq) is reduced to Ag(s).

I am not in favor of this type of example in general chemistry but I assigned the 6L.7 because of parts b and c.

Hope this helps.