When two unlike metals are submerged in an electrolyte solution, which metal accumulates electrons?

When two unlike metals are submerged in an electrolyte solution, the metal that accumulates electrons is indeed associated with the negative pole of a galvanic cell or a similar electrochemical setup. This phenomenon occurs due to the differing tendencies of metals to lose or gain electrons, which is related to their electrochemical potentials.

In this scenario, one metal will have a higher tendency to lose electrons (becoming an anode), while the other metal will have a higher tendency to gain electrons (becoming a cathode). The cathode is where reduction occurs, leading to the accumulation of electrons, while the anode is where oxidation occurs, resulting in a loss of electrons.

As a result, the negative pole, associated with the cathode, will accumulate electrons during the electrochemical reaction. This understanding is foundational in electrochemistry and helps to predict the behavior of different metals in various electrolyte solutions.