The protocol used for the follow-up measurement is shown in Figure . The objective was to record the activity, dissolution behavior, and change in surface area over a prolonged time span. The protocol was applied in a loop up to 19 times, starting with with three cyclic voltammograms (CVs) between 1.1 and 1.3 VRHE. Scan rates of 25, 50, 100, and 200 mV s -1 were chosen to extract the capacitance from the capacitive current, which was treated as a proxy metric for the electrochemical surface area. A final hold at 1 mA cm -2 and 80 AST cycles between 0 and 1 mA cm -2 conclude the protocol. Figure and show the dissolution traces for Mn and Ti, respectively, for each iteration of the protocol. The traces were overlaid for Mn, which helps visualize the change in their shape over time. Interestingly, the initial Mn dissolution during the AST shows a transient behavior. However, the transience gradually disappears toward the end, where the dissolution rate remains constant throughout the AST until a complete deactivation is reached, which in this case occured around iteration 17. A tentative hypothesis includes the increasing upper potential limit for the ASTs towards the end, which would destabilize Mn more due to its transition to a soluble MnO4 - phase based on the Pourbaix diagram. Similar OER-triggered MnO2 dissolution was reported in alkaline media, where the main driver for destabilization was attributed to the MnO2/MnO4 -redox transition. It is worth noting that the highest Mn dissolution was actually recorded when changing the potentiostat from galvanostatic (CP hold) to potentiostatic (CV) between each iteration, which resulted in a sharp potential drop from around 1.4 -1.5 VRHE to 1.1 VRHE (see Figure ). This pronounced Mn leaching could result from the redox transition from MnO2 to an aqueous Mn 2+ phase, which would thermodynamically occur at these potentials. Based on this argumentation, it is logical that the Mn dissolution observed when initiating the CP hold at 1 mA cm -2 is comparatively less, as the reverse redox transition is triggered, going from Mn 2+ to the solid MnO2 phase. Due to the lower signal-to-noise ratio for Ti, a stacked representation was chosen. A slight peak is present during the hold for the first two to four iterations, after which no clear dissolution signal is recognizable. This behavior could imply that Ti stabilizes over time or dissolves at rates lower than the detection limit of the ICP-MS. Nevertheless, TiO2 is thermodynamically much more stable in acidic media compared to Mn and should be resistive to dissolution up until 2.1 V at pH 0. Hence, most of the Ti dissolution could be originating from a cooperative dissolution mechanism, in which predominant Mn leaching rips off Ti atoms from the surface. Similar behavior was observed for Fe-Ni oxide systems during neutral OER. Figure shows the total dissolved amount of Mn calculated as the integral of the dissolution rates for the hold and AST.