Final answer:
The statement that a more positive E(Mn/M) value indicates greater stability of Mn ions in an aqueous solution is true. The standard reduction potential reflects the tendency of the ion to be reduced and thereby its stability in solution.
Step-by-step explanation:
The statement 'The more positive the value of E(Mn/M), greater is the stability of Mn ion in an aqueous solution' is true. The more positive the standard reduction potential (E°), the greater the tendency for the metal ion to gain electrons and be reduced, and thus the more stable the ion is in solution. In the context of manganese (Mn), which can exist in multiple oxidation states, the stability of Mn ions in different oxidation states can be compared by their respective E° values. The Mn2+ ion is known to be the most stable in aqueous solution, but proteins can modify the redox potential to facilitate necessary biochemical reactions.
Furthermore, E° values influence the direction of electrochemical reactions. For instance, in an electrochemical cell, manganese will dissolve from the electrode in a more dilute solution (lower concentration of Mn2+ ions) and will be deposited on the electrode in a compartment with a more concentrated solution of Mn2+ ions, driven by the potential difference across the cell.