[Rabn]

What if my H+ and OH- cancel out completely?

You mean when they are not present in the final reaction equation? They don't matter.

This may be a little irrelevant to this thread and may best be served by starting a new thread.  Thinking of redox reactions in terms of initial and final state, the equilibrium constants of redox intermediates that completely cancel out are irrelevant, but if you think about redox reactions in terms of their kinetics, the equilibrium constants of reaction intermediates become very relevant to the rate of the reaction....just a thought.

[c0d3]

This may be a little irrelevant to this thread and may best be served by starting a new thread.  Thinking of redox reactions in terms of initial and final state, the equilibrium constants of redox intermediates that completely cancel out are irrelevant, but if you think about redox reactions in terms of their kinetics, the equilibrium constants of reaction intermediates become very relevant to the rate of the reaction....just a thought.

You mentioned the rate. What about the amount of product?
Will it get affected by the kinetics??

P.S. Would Rabn mind to start a new thread discussing about your thought relating to kinetic side? I think you are the most suitable since it came out from your mind

[Rabn]

I would think that the amount of product should not be affected by a change in rate.  That is because  :delta: G is a state function, and as a state function the process it takes to get to the final state is irrelevant.  The Nernst equation tells us that as long as the two half-cells aren't at equilibrium, there will be a voltage.  What I'm not sure of is how voltage effects kinetics if at all.

[c0d3]

I would think that the amount of product should not be affected by a change in rate.  That is because  :delta: G is a state function, and as a state function the process it takes to get to the final state is irrelevant.  The Nernst equation tells us that as long as the two half-cells aren't at equilibrium, there will be a voltage.  What I'm not sure of is how voltage effects kinetics if at all.

My guess would be voltage difference initiate a reaction but can't affect its kinetic. Something like when two neutral compound can't react spontaneously, you need to ionize one of it to initiate the reaction. Once the reaction has been initiated, the amount of the ionizing agent present would not affect the kinetic of the reaction. So, voltage defference is actually like the ionizing agent.

P.S. This is plainly my opinion. Someone who has certain answer please leave your reasoning here.