First, I present an example, which provides a quantitative description of how the hydration enthalpy could impact the electrode potential. In particular, select salts can undergo hydrolysis resulting in the liberation of H+, for example with copper or iron:
$\ce{Fe[(H2O)6](3+) (aq) + H2O (l) = [Fe(H2O)5(OH)](2+) (aq) + H3O+ (aq)}$
Reference: one of many possible links .
This produces a pH effect, which per a source on the question: 'What is the equation that connects pH and its effect on electric potential of an electrochemical cell?', the answer employs the Nernst equation to derive an explanation. I will quote but a small summary part of the results relating to acidic conditions:
As the pH decreases, the solution is more acidic, so 10−pH=[H+] increases and 10pH−14=[OH−] decreases.
- If H+ is a product, Q therefore increases, and the nonstandard cell potential decreases.
- If H+ is a reactant, Q therefore decreases, and the nonstandard cell potential increases.
Next, with respect to the impact of sublimation (and relatedly, ionization), I note that this can be energy (and especially temperature) related. Quoting a reference:
As you supply heat (or any form of energy) to the system containing the atom, it's kinetic energy will increase and it will move faster through space. ... Continue to supply even more energy and more electrons will be removed from the atom.
On the connection of temperature to the electrode potential, I cite an answer from The Student Room:
Increasing the temperature AFFECTS electrode potentials, not increases them.
The electrode potential is a measure of the extent of a redox process - negative and the equilibrium lies relatively to the LHS (compared to the standard hydrogen electrode)
example: $\ce{Zn(2+)(aq) + 2e- -> Zn(s)}$
The process is not quite as simple as it appears. To move from right to left the equilibrium has to have the zinc atomised and then ionised and then the ions solvated.
Each of these processes is either exo or endothermic and is affected by the temperature.
The equilibrium between the ions and the pure metal is also affected by the temperature.
If the equilibrium is exothermic overall from left to right then an increase in the temperature will make the equilibrium move more to the left hand side making the electrode potential more negative.
The reverse is also true - if the equilibrium is endothermic overall from left to right then increasing the temperature makes the electrode potential more positive.
Note, both provided answers, are in effect, very situational, with, for example, is the removal of atoms via sublimation an exothermic or endothermic process.