Consider a cell based on the following reaction:

GeO(s) + H2O(l) + 2 Ag+(aq) ===> GeO2(s) + 2 H+(aq) + 2 Ag(s)

If [Ag+] = 1 M, at 25°C, would it be.....

pH = 2 ( E° - E ) / 0.059159 V.

or

pH = ( E° - E ) / 0.059159 V.

It wouldn't be either of those it would end up being...

pH = (E - E°) / 0.059159 V.
because E° always comes second.

To determine which equation to use for calculating the pH, we first need to understand the context of the given reaction. It appears to be a redox reaction that takes place in an electrochemical cell.

In this case, the standard potential (E°) refers to the standard reduction potential of the half-reaction in which silver ions (Ag+) are reduced to silver (Ag). The value of E° for this half-reaction can be found in a standard reduction potentials table.

The term (E) represents the measured cell potential or the difference between the standard potential of the cathode and the anode (E°cathode - E°anode).

Now, let's analyze the equations you provided:

1. pH = 2(E° - E) / 0.059159 V
2. pH = (E° - E) / 0.059159 V

Based on the equations, it seems that you are trying to relate the cell potential difference (E) to the pH of the solution. However, neither of these equations is directly related to pH and the given redox reaction.

The pH of a solution depends on the concentration of hydrogen ions (H+). To determine the pH based on the redox reaction, you would need to consider the balanced chemical equation and the concentration of hydrogen ions (H+) present in the system.

If you have additional information about the concentration of H+ or any other relevant factors, please provide them, and I can help you calculate the pH accurately.