IrO2 Oxygen Evolution Catalysts Prepared by an Optimized Photodeposition Process on TiO2 Substrates

Preparing high-performance oxygen evolution reaction (OER) catalysts with low precious metal loadings for water electrolysis applications (e.g., for green hydrogen production) is challenging and requires electrically conductive, high-surface-area, and stable support materials. Combining the properties of stable TiO2 with those of active iridium oxide, we synthesized highly active electrodes for OER in acidic media. TiO2 powders (both commercially available Degussa P-25® and hydrothermally prepared in the laboratory from TiOSO4, either as received/prepared or following ammonolysis to be converted to titania black), were decorated with IrO2 by UV photodeposition from Ir(III) aqueous solutions of varied methanol scavenger concentrations. TEM, EDS, FESEM, XPS, and XRD measurements demonstrate that the optimized version of the photodeposition preparation method (i.e., with no added methanol) leads to direct deposition of well-dispersed IrO2 nanoparticles. The electroactive surface area and electrocatalytic performance towards OER of these catalysts have been evaluated by cyclic voltammetry (CV), Linear Sweep Voltammetry (LSV), and Electrochemical Impedance Spectroscopy (EIS) in 0.1 M HClO4 solutions. All TiO2-based catalysts exhibited better mass-specific (as well as intrinsic) OER activity than commercial unsupported IrO2, with the best of them (IrO2 on Degussa P-25® ΤiO2 and laboratory-made TiO2 black) showing 100 mAmgIr−1 at an overpotential of η = 243 mV. Chronoamperometry (CA) experiments also proved good medium-term stability of the optimum IrO2/TiO2 electrodes during OER.


Introduction
Among water splitting technologies (towards a hydrogen economy [1]), proton exchange membrane water electrolyzers (PEMWEs), especially when coupled with renewable energy sources, have been considered as the most promising and appealing systems for high-purity hydrogen production due to their fast load change, high current density, and energy efficiency [2].However, the highly corrosive operating potential (E > 1.5 V vs. RHE), the sluggish kinetics of the OER, and the acidic environment (pH < 1) at the anode of a PEMWE cell are the main hindrances for the water electrolysis reaction, and studies have focused on investigating suitable stable and low-overpotential OER catalysts [3].Among the electrode materials quoted in the literature, and in line with the relevant catalytic activity volcano plots as well as stability issues, only precious metal oxides, especially IrO 2 and iridium-based oxides, are suitable anode catalysts, as these combine high catalytic activity and long-term stability in the acidic conditions of PEMWEs [4].Considering the high cost and limited availability of iridium, many efforts have been devoted to preparing a cost-effective OER electrocatalyst with the minimum amount of the noble and scarce metal.This can be achieved by increasing the intrinsic catalytic activity of IrO 2 as well as its surface area; both challenges can be addressed by the choice of an appropriate catalyst support material [5].
Among various support candidates, TiO 2 is a promising material both at a pilot scale and for large scale applications, given its low cost, abundance, high stability, corrosion resistance, and mature industry production [6,7].Despite its poor electrical conductivity and catalytic activity, the decoration of the TiO 2 oxide support with conducting IrO 2 nanoparticles as well as the electronic interaction between them form an electrically percolating structure (with a specific conductivity of >0.1 S cm −1 ) with improved overall activity and stability [8][9][10][11][12], in line with theoretical predictions [13].
Preparation methods for IrO x /TiO 2 catalysts include the Adams fusion method [10,12,14,15], thermal treatment in air or H 2 [11,[16][17][18], hydrothermal reactions [19,20], and electrodeposition [21,22].Photocatalytic deposition of IrO x on semiconductors is neither a common practice nor a straightforward process from a mechanistic point of view (it usually involves photolytic hydrolysis of Ir salts), among the number of methods reported for IrO x preparation [23].There have been very few publications on Ir or IrO x photodeposition on semiconductor substrates from Ir(III) or Ir(IV) solutions [24][25][26][27] and a single one from Ir(III) complexes onto TiO 2 photoanodes [27].We have recently photodeposited Ir/IrO x from Ir(III) solutions onto TiO 2 using methanol as a hole scavenger and testing the resulting materials as a catalyst for OER in the dark [28].However, the role of methanol and the mechanism of photodeposition remained unclear; commercial Degussa P25 ® was the only substrate used and the resulting catalyst did not outperform the commercial IrO 2 catalyst for OER.
The aim of the work presented here has been to decipher the mechanism of IrO x photodeposition onto TiO 2 , explore the use of various TiO 2 substrates, and optimize the OER performance of the thus prepared IrO x /TiO 2 material.To that direction, (a) we have studied the effect of methanol on Ir deposition; (b) we have used four different TiO 2 supports: Degussa P25 ® TiO 2 , laboratory-made TiO 2 from titanium oxysulphate, and their titania black analogs prepared by ammonolysis (seeking alternative, more conducting substrates); and (c) we have tested the materials' catalytic performance towards OER by CV, LSV, EIS, and CA electrochemical techniques.Hence, the main novelty of this work is unraveling the mechanism of Ir/IrO x photodeposition on TiO 2 and preparing catalysts that can outperform the state-of-the-art Ir-based OER catalysts, in terms of Ir mass-specific activity.
The only significant change in the XRD diffractograms after the ammonolysis process is that both materials show new rutile peaks which correspond to the formation of titanium nitride (TiN); these peaks appear at 2θ values of 37.3°, 43.3°, and 62.3° and they can be indexed to (111), ( 200) and (220), planes.The morphology of the TiO2 powders can be seen in the FESEM images of Figure 2 below.White-P25 (Figure 2a) and black-P25 (Figure 2b) consist of nanoparticles with diameters around ~20 nm and have similar morphology (in black-P25, nanoparticles are slightly more agglomerated).White-TiO2-oxy (Figure 2c) consists of nanoparticles (~30 nm) that aggregate into rod-like structures which change into smaller nodular particles and rougher aggregates upon their transformation to black-TiO2-oxy (Figure 2d).The nanoparticle size agrees with calculations from the XRD data, using the Scherrer equation.The only significant change in the XRD diffractograms after the ammonolysis process is that both materials show new rutile peaks which correspond to the formation of titanium nitride (TiN); these peaks appear at 2θ values of 37.3 • , 43.3 • , and 62.3 • and they can be indexed to (111), ( 200) and (220), planes.
The morphology of the TiO 2 powders can be seen in the FESEM images of Figure 2 below.White-P25 (Figure 2a) and black-P25 (Figure 2b) consist of nanoparticles with diameters around ~20 nm and have similar morphology (in black-P25, nanoparticles are slightly more agglomerated).White-TiO 2 -oxy (Figure 2c) consists of nanoparticles (~30 nm) that aggregate into rod-like structures which change into smaller nodular particles and rougher aggregates upon their transformation to black-TiO 2 -oxy (Figure 2d).The nanoparticle size agrees with calculations from the XRD data, using the Scherrer equation.In addition, elemental analysis (Table 1) and EDS mapping confirms the presence of titanium and oxygen in the appropriate ratios for these oxides as well as the presence of nitrogen in the ammonia-treated samples, due to TiN formation.The diffuse reflectance spectra (DRS) of TiO2 nanoparticles before and after ammonolysis are shown in Figure 3a,b (for P25 and TiO2-oxy samples, respectively), with the corresponding Tauc plots in Figure 3c,d.The former plots confirm that the "black" catalyst variants absorb light in the visible range too.The optical band gaps of the commercial (P25) and synthesized (TiO2-oxy) photocatalysts were estimated using the Tauc method, as described in Section 4 below.For white-P25, this can be estimated at 3.06 eV and can be attributed to the mixture of anatase (3.2 eV) and rutile (3.0 eV) phases of TiO2 (Figure 3c); for white-TiO2-oxy, it is estimated at 3.21 eV, which agrees with the anatase phase of TiO2.Although for the "black" variants the Tauc plots cannot lead to accurate band gap values, these can be approximated to ≤1 eV for black-P25 and ca 1.5 eV for black-TiO2-oxy.The significant decrease in the band gap of ammonia-treated samples should also lead to a substantial increase in their electronic conductivity.The maximum absorbance of white-TiO2 and white-TiO2-oxy at 365 and 300 nm, respectively, means that UV illumination is mandatory for Ir/IrOx photodeposition.On the contrary, the absorbance of am- In addition, elemental analysis (Table 1) and EDS mapping confirms the presence of titanium and oxygen in the appropriate ratios for these oxides as well as the presence of nitrogen in the ammonia-treated samples, due to TiN formation.The diffuse reflectance spectra (DRS) of TiO 2 nanoparticles before and after ammonolysis are shown in Figure 3a,b (for P25 and TiO 2 -oxy samples, respectively), with the corresponding Tauc plots in Figure 3c,d.The former plots confirm that the "black" catalyst variants absorb light in the visible range too.The optical band gaps of the commercial (P25) and synthesized (TiO 2 -oxy) photocatalysts were estimated using the Tauc method, as described in Section 4 below.For white-P25, this can be estimated at 3.06 eV and can be attributed to the mixture of anatase (3.2 eV) and rutile (3.0 eV) phases of TiO 2 (Figure 3c); for white-TiO 2 -oxy, it is estimated at 3.21 eV, which agrees with the anatase phase of TiO 2 .Although for the "black" variants the Tauc plots cannot lead to accurate band gap values, these can be approximated to ≤1 eV for black-P25 and ca 1.5 eV for black-TiO 2 -oxy.The significant decrease in the band gap of ammonia-treated samples should also lead to a substantial increase in their electronic conductivity.The maximum absorbance of white-TiO 2 and white-TiO 2 -oxy at 365 and 300 nm, respectively, means that UV illumination is mandatory for Ir/IrO x photodeposition.On the contrary, the absorbance of ammonia-treated ("black") samples means that photodeposition could, in principle, take place under visible light illumination too (however, this has not been possible).
Molecules 2024, 29, x FOR PEER REVIEW 5 of 19 monia-treated ("black") samples means that photodeposition could, in principle, take place under visible light illumination too (however, this has not been possible).

Structural, Chemical, and Morphological Characterization of IrOx/TiO2 materials
The XRD patterns of IrOx/TiO2 modified samples did not show well-defined peaks of crystalline IrO2 and were practically identical to those of Figure 1, pointing to the catalyst being deposited in its amorphous form.(It should be noted that literature data [29,30] indicate that IrOx catalysts are more active for OER if the material crystallinity is low or intermediate.) The morphology of the electroactive IrOx particles is expected to have an important influence on their surface area and on their intrinsic catalytic activity (via their interaction with the substrate) as well as, in this case, on electronic conductivity (since the latter is expected to depend on interparticle contacts).TEM analysis was performed to characterize the morphology of the IrO2/TiO2 electrocatalysts.
Figure 4a shows the morphology of the photocatalytically prepared powder of IrO2/TiO2 (white-P25 ® ), while Figure 4b depicts that of the commercial IrO2 catalyst (Alfa Aesar, Karlsruhe, Germany).TEM micrographs provide a first indication of the successful photodeposition of Ir or IrO2 particles/films (26% w/w Ir, as further confirmed by EDS) onto the TiOx particles (the latter having a ca 30 nm nominal size in the case of white-P25 ® ).Ir or IrOx can be seen as black areas, partly covering the TiO2 particles, in a non-uniform manner.On the other hand, unsupported commercial IrO2 nanoparticles (of 2-3 nm nominal size) tend to form aggregates of different sizes.

Structural, Chemical, and Morphological Characterization of IrO x /TiO 2 Materials
The XRD patterns of IrO x /TiO 2 modified samples did not show well-defined peaks of crystalline IrO 2 and were practically identical to those of Figure 1, pointing to the catalyst being deposited in its amorphous form.(It should be noted that literature data [29,30] indicate that IrO x catalysts are more active for OER if the material crystallinity is low or intermediate.).
The morphology of the electroactive IrO x particles is expected to have an important influence on their surface area and on their intrinsic catalytic activity (via their interaction with the substrate) as well as, in this case, on electronic conductivity (since the latter is expected to depend on interparticle contacts).TEM analysis was performed to characterize the morphology of the IrO 2 /TiO 2 electrocatalysts.
Figure 4a shows the morphology of the photocatalytically prepared powder of IrO 2 /TiO 2 (white-P25 ® ), while Figure 4b depicts that of the commercial IrO 2 catalyst (Alfa Aesar, Karlsruhe, Germany).TEM micrographs provide a first indication of the successful photodeposition of Ir or IrO 2 particles/films (26% w/w Ir, as further confirmed by EDS) onto the TiO x particles (the latter having a ca 30 nm nominal size in the case of white-P25 ® ).Ir or IrO x can be seen as black areas, partly covering the TiO 2 particles, in a non-uniform manner.On the other hand, unsupported commercial IrO 2 nanoparticles (of 2-3 nm nominal size) tend to form aggregates of different sizes.Higher-resolution TEM images of all the obtained catalysts are shown in Figure 5a-d and a uniform dispersion of Ir/IrOx nanoparticles on the larger TiO2 support particles can be seen.Such a good conducting Ir/IrOx particle dispersion is crucial for providing good interparticle contact and electronic conductivity.The energy-dispersive spectroscopy (EDS) of the samples shows the existence of Ir-more specifically, for all catalysts, a ca 26 w/w % Ir content, except for black-P25 with a 15 w/w % Ir content.The chemical state of Ir in the TiO2-supported catalyst was examined by XPS analysis for catalysts prepared in the presence and absence of methanol (Figure 6).The Ir4f peak was used as a first approach for chemical state identification.Measurements at the 4f band of the sample resulted in peak positions of 65.4 eV and 62.4 eV for the Ir 4f5/2 and Ir 4f7/2 peaks, respectively.These values are close to those reported for hydrated amorphous iridium dioxide, which also correlates with the XRD results.Higher-resolution TEM images of all the obtained catalysts are shown in Figure 5a-d and a uniform dispersion of Ir/IrO x nanoparticles on the larger TiO 2 support particles can be seen.Such a good conducting Ir/IrO x particle dispersion is crucial for providing good interparticle contact and electronic conductivity.The energy-dispersive spectroscopy (EDS) of the samples shows the existence of Ir-more specifically, for all catalysts, a ca 26 w/w % Ir content, except for black-P25 with a 15 w/w % Ir content.Higher-resolution TEM images of all the obtained catalysts are shown in Figure 5a-d and a uniform dispersion of Ir/IrOx nanoparticles on the larger TiO2 support particles can be seen.Such a good conducting Ir/IrOx particle dispersion is crucial for providing good interparticle contact and electronic conductivity.The energy-dispersive spectroscopy (EDS) of the samples shows the existence of Ir-more specifically, for all catalysts, a ca 26 w/w % Ir content, except for black-P25 with a 15 w/w % Ir content.The chemical state of Ir in the TiO2-supported catalyst was examined by XPS analysis for catalysts prepared in the presence and absence of methanol (Figure 6).The Ir4f peak was used as a first approach for chemical state identification.Measurements at the 4f band of the sample resulted in peak positions of 65.4 eV and 62.4 eV for the Ir 4f5/2 and Ir 4f7/2 peaks, respectively.These values are close to those reported for hydrated amorphous iridium dioxide, which also correlates with the XRD results.The chemical state of Ir in the TiO 2 -supported catalyst was examined by XPS analysis for catalysts prepared in the presence and absence of methanol (Figure 6).The Ir4f peak was used as a first approach for chemical state identification.Measurements at the 4f band of the sample resulted in peak positions of 65.4 eV and 62.4 eV for the Ir 4f5/2 and Ir 4f7/2 peaks, respectively.These values are close to those reported for hydrated amorphous iridium dioxide, which also correlates with the XRD results.
Fitting the data to a curve resulting from the convolution of peaks corresponding to the various oxidation states of Ir proves that the catalyst prepared in pure water (Figure 6a) consists almost exclusively of iridium oxides (mainly iridium dioxide-Ir(IV)).However, there is some metallic Ir (Ir(0)) when MeOH is added to the preparation solution (Figure 6b) since the anodic deposition route (Ir(III) oxidized by photogenerated holes) may be partially suppressed (as MeOH competes for holes) and the cathodic deposition route (Ir(III) reduced to Ir by photogenerated electrons) may start to operate too (see also Section 3 below).
Molecules 2024, 29, x FOR PEER REVIEW 7 of 20 Fitting the data to a curve resulting from the convolution of peaks corresponding to the various oxidation states of Ir proves that the catalyst prepared in pure water (Figure 6a) consists almost exclusively of iridium oxides (mainly iridium dioxide-Ir(IV)).However, there is some metallic Ir (Ir(0)) when MeOH is added to the preparation solution (Figure 6b) since the anodic deposition route (Ir(III) oxidized by photogenerated holes) may be partially suppressed (as MeOH competes for holes) and the cathodic deposition route (Ir(III) reduced to Ir by photogenerated electrons) may start to operate too (see also Section 3 below).

Electrochemical Performance
IrOx surface electrochemistry was studied by cyclic voltammetry (CV) experiments in the potential range between hydrogen and oxygen evolution (−0.30V to +1.10 V vs. SCE) at a 25 mV s −1 potential sweep rate.Figure 7 shows the stabilized CV curve for each catalyst (prepared in the absence of methanol).On the anodic part of the CV curve of the commercial, unsupported IrOx catalyst (Inset to Figure 7), one can clearly observe two peaks corresponding to the transformation of Ir(III) to Ir(IV) and Ir(IV) to Ir(V), typical of IrOx surface electrochemistry of thermally or electrochemically (by anodization) prepared IrOx catalysts [29,30].On the other hand, the photochemically prepared catalysts (main Figure 7) show only one oxidation peak (at ca 0.9 V, corresponding to the Ir(IV) to Ir(V) transformation), pointing to the initial photodeposition mainly of Ir(IV) as IrO2 on the TiO2 support, which can only be further oxidized to Ir(V) (see also Discussion below).Also, the electrochemically active surface area of the prepared catalysts is lower than that of the commercial one (for similar Ir loadings in the 0.5-1 mg cm −2 range).Given the similar particle morphology of the commercial and prepared IrOx particles (see Figure 5), this difference may be attributed to the TiO2 substrate, which cannot provide sufficient electronic conductivity between all IrOx nanoparticles.Only those IrOx nanoparticles that are in contact with each other and eventually with the glassy carbon (GC) electrode current collector can act as electroactive material.
Figure 8 depicts the effect of methanol used in catalyst preparation based on surface electrochemistry.An absence of methanol (the purple line) leads to higher iridium content (26 w/w % as confirmed by EDS) and thus a higher electroactive area and dominance of the Ir(IV) to Ir(V) peak.The suppression of iridium deposition when methanol is added can be inferred by the suppression of Ir surface electrochemistry (and is confirmed

Electrochemical Performance
IrO x surface electrochemistry was studied by cyclic voltammetry (CV) experiments in the potential range between hydrogen and oxygen evolution (−0.30V to +1.10 V vs. SCE) at a 25 mV s −1 potential sweep rate.Figure 7 shows the stabilized CV curve for each catalyst (prepared in the absence of methanol).On the anodic part of the CV curve of the commercial, unsupported IrO x catalyst (Inset to Figure 7), one can clearly observe two peaks corresponding to the transformation of Ir(III) to Ir(IV) and Ir(IV) to Ir(V), typical of IrO x surface electrochemistry of thermally or electrochemically (by anodization) prepared IrO x catalysts [29,30].On the other hand, the photochemically prepared catalysts (main Figure 7) show only one oxidation peak (at ca 0.9 V, corresponding to the Ir(IV) to Ir(V) transformation), pointing to the initial photodeposition mainly of Ir(IV) as IrO 2 on the TiO 2 support, which can only be further oxidized to Ir(V) (see also Discussion below).Also, the electrochemically active surface area of the prepared catalysts is lower than that of the commercial one (for similar Ir loadings in the 0.5-1 mg cm −2 range).Given the similar particle morphology of the commercial and prepared IrO x particles (see Figure 5), this difference may be attributed to the TiO 2 substrate, which cannot provide sufficient electronic conductivity between all IrO x nanoparticles.Only those IrO x nanoparticles that are in contact with each other and eventually with the glassy carbon (GC) electrode current collector can act as electroactive material.
Figure 8 depicts the effect of methanol used in catalyst preparation based on surface electrochemistry.An absence of methanol (the purple line) leads to higher iridium content (26 w/w % as confirmed by EDS) and thus a higher electroactive area and dominance of the Ir(IV) to Ir(V) peak.The suppression of iridium deposition when methanol is added can be inferred by the suppression of Ir surface electrochemistry (and is confirmed by EDS results that give 19% and 2.5% w/w Ir in the presence of 0.15% and 1.5% v/v MeOH).This is additional proof that IrO x is formed by Ir(III) oxidation by photogenerated holes at the TiO 2 valence band where MeOH also competes for these photogenerated holes.(Note also that, in the case of 0.15% v/v MeOH (green line curve), there appears an oxidation wave at ca. +0.5 V corresponding to the Ir(III) to Ir(IV) transformation, indicative of the presence of some metallic Ir too, which is initially converted to Ir(III).).
by EDS results that give 19% and 2.5% w/w Ir in the presence of 0.15% and 1.5% v/v MeOH).This is additional proof that IrOx is formed by Ir(III) oxidation by photogenerated holes at the TiO2 valence band where MeOH also competes for these photogenerated holes.(Note also that, in the case of 0.15% v/v MeOH (green line curve), there appears an oxidation wave at ca. +0.5 V corresponding to the Ir(III) to Ir(IV) transformation, indicative of the presence of some metallic Ir too, which is initially converted to Ir(III).)  Near-steady-state Linear Sweep Voltammetry (LSV) at a slow potential sweep rate (5 mV s −1 ) was employed to investigate the OER activity of the Ir-based catalysts.In Figure by EDS results that give 19% and 2.5% w/w Ir in the presence of 0.15% and 1.5% v/v MeOH).This is additional proof that IrOx is formed by Ir(III) oxidation by photogenerated holes at the TiO2 valence band where MeOH also competes for these photogenerated holes.(Note also that, in the case of 0.15% v/v MeOH (green line curve), there appears an oxidation wave at ca. +0.5 V corresponding to the Ir(III) to Ir(IV) transformation, indicative of the presence of some metallic Ir too, which is initially converted to Ir(III).)   Near-steady-state Linear Sweep Voltammetry (LSV) at a slow potential sweep rate (5 mV s −1 ) was employed to investigate the OER activity of the Ir-based catalysts.In Figure 9, currents, i m , are reported per Ir mass, and all prepared catalysts (except for those supported on black-P25, bearing the lower Ir content and hence lower conductivity) show improved mass activity compared to the commercial IrO 2 catalyst.This means that a higher intrinsic catalytic activity of the prepared catalysts (because of strong IrO 2 and TiO 2 -support interactions) offsets their lower electroactive surface area (because of their lower electronic conductivity and catalyst utilization).This is further confirmed by the LSVs of Figure 9, whereby the OER currents are normalized per the charge corresponding to the 1e − transformation of Ir species, i.e., per its electroactive surface area, resulting in a current descriptor, i q , that should be independent of surface area and catalyst utilization (e.g., by conductivity restrictions).The intrinsic catalytic activities of IrO 2 onto white-P25, black-P25, and black-TiO 2 -oxy are almost identical and higher than that of IrO 2 on white-TiO 2 -oxy and commercial unsupported IrO 2 .A mismatch between Ir and Ti size within their oxide network may destabilize Ir-OH bonds (a reactive intermediate of OER) and increase OER activity.Electrochemical Impedance Spectroscopy measurements were performed at 1.2 V in the frequency range of 100 kHz to 100 mHz for the best catalysts according to LSV screening (of Figure 9 above).The experimental data are presented as Nyquist plots in Figure 10 and were fitted to the equivalent electrical circuit Rs[RfQf][RctQdl] (inset of Figure 10).Rs corresponds to the ohmic losses (due to the ionic resistance of the solution between the reference and working electrodes, as well as the electronic resistance of the dispersed IrO2 electrode); RfQf accounts for the characteristics of ionic transport through Electrochemical Impedance Spectroscopy measurements were performed at 1.2 V in the frequency range of 100 kHz to 100 mHz for the best catalysts according to LSV screening (of Figure 9 above).The experimental data are presented as Nyquist plots in Figure 10 and were fitted to the equivalent electrical circuit R s [R f Q f ][R ct Q dl ] (inset of Figure 10).R s corresponds to the ohmic losses (due to the ionic resistance of the solution between the reference and working electrodes, as well as the electronic resistance of the dispersed IrO 2 electrode); R f Q f accounts for the characteristics of ionic transport through the porous electrode and R ct Q dl to the OER charge transfer process and the constant-phase element of the IrO 2 /electrolyte interface.(Q dl is transformed to double-layer capacitance C dl using the Mansfield or Brug equations [31,32].)It has recently been argued that low R ct C dl values mean high intrinsic electrocatalytic activity [33].
Molecules 2024, 29, x FOR PEER REVIEW 11 of 20 capacitance Cdl using the Mansfield or Brug equations [31,32].)It has recently been argued that low RctCdl values mean high intrinsic electrocatalytic activity [33].Table 2 below shows the results of equivalent circuit analysis, from which it follows that the intrinsic catalytic activity of the IrO2/TiO2 catalysts towards OER is higher than that of commercial IrO2, as the former are characterized by lower RctCdl values.Table 2 below shows the results of equivalent circuit analysis, from which it follows that the intrinsic catalytic activity of the IrO 2 /TiO 2 catalysts towards OER is higher than that of commercial IrO 2 , as the former are characterized by lower R ct C dl values.Finally, to confirm the medium-term stability of this type of nano-composite catalyst, after their preliminary electrochemical testing, they were systematically investigated through chronoamperometry experiments at constant potential, and indicative results are shown in Figure 11.It can be seen that catalyst performance retains ca 90% of its initial OER activity during a 7 h experiment.
Molecules 2024, 29, x FOR PEER REVIEW 12 of 20 through chronoamperometry experiments at constant potential, and indicative results are shown in Figure 11.It can be seen that catalyst performance retains ca 90% of its initial OER activity during a 7h experiment.

Analysis of Possible Photodeposition Routes and Mechanisms for Ir Deposition onto TiO2 from Ir(III) Solutions
Being in an intermediate valence state between (0) and (IV), Ir(III) can either be photodeposited as metallic Ir or IrO2.The first route involves the cathodic deposition of Ir at the Conduction Band (CB) of the illuminated TiO2 semiconductor particles, whereby Ir(III) is photo-reduced to metallic Ir(0) by the photogenerated electrons at the Conduction Band (CB) (Figure 12a); this may be oxidized to IrO2 during subsequent electrochemical potential cycling to sufficiently positive potential values (anodization) [28] or chemically oxidized by the OH • radicals resulting from water photo-oxidation.In this case, the presence of methanol (in addition to water as a hole scavenger) should help the Ir(0) deposition process, minimizing electron-hole recombination.The second route (Figure 12b) involves the anodic deposition of IrO2 at the valence band (VB), where Ir(III) is photo-oxidized to Ir(VI) by photogenerated holes (or OH • ) and, in the presence of hydroxyl anions (either in the bulk of an alkaline solution or photo-produced at the CB of the illuminated semiconductor by water photo-reduction), can be chemically converted directly to IrO2.In this case, methanol may limit IrO2 deposition as it competes for the photogenerated holes (or OH • ).Irrespective of the photodeposition route followed, and in accordance with the literature [23,27], the first step is reported to be the photo-assisted hydrolysis of the Ir(III) chloro-complex (Equations ( 1) and ( 2)): Predictions for the most favorable processes from a thermodynamic point of view can be made by studying the energy diagram (Figure 13) of TiO2 (VB and CB energy levels for the given pH, deduced from data in [34,35]), as well as of the relevant red/ox couples (estimated from data in [36] to account for a pH of 11 and the Ir(III) concentration of 2 × 10 −3 M).The higher the potential difference, |ΔΕ|, between the energy levels of the TiO2 photogenerated holes and electrons and that of a red/ox couple, the more likely the

Analysis of Possible Photodeposition Routes and Mechanisms for Ir Deposition onto TiO 2 from Ir(III) Solutions
Being in an intermediate valence state between (0) and (IV), Ir(III) can either be photodeposited as metallic Ir or IrO 2 .The first route involves the cathodic deposition of Ir at the Conduction Band (CB) of the illuminated TiO 2 semiconductor particles, whereby Ir(III) is photo-reduced to metallic Ir(0) by the photogenerated electrons at the Conduction Band (CB) (Figure 12a); this may be oxidized to IrO 2 during subsequent electrochemical potential cycling to sufficiently positive potential values (anodization) [28] or chemically oxidized by the OH • radicals resulting from water photo-oxidation.In this case, the presence of methanol (in addition to water as a hole scavenger) should help the Ir(0) deposition process, minimizing electron-hole recombination.The second route (Figure 12b) involves the anodic deposition of IrO 2 at the valence band (VB), where Ir(III) is photooxidized to Ir(VI) by photogenerated holes (or OH • ) and, in the presence of hydroxyl anions (either in the bulk of an alkaline solution or photo-produced at the CB of the illuminated semiconductor by water photo-reduction), can be chemically converted directly to IrO 2 .In this case, methanol may limit IrO 2 deposition as it competes for the photogenerated holes (or OH • ).Irrespective of the photodeposition route followed, and in accordance with the literature [23,27], the first step is reported to be the photo-assisted hydrolysis of the Ir(III) chloro-complex (Equations ( 1) and ( 2)): e.g., IrCl 6 Ir 3+ (aq) + 3e − → Ir (5) e.g., Ir(OH)6  Predictions for the most favorable processes from a thermodynamic point of view can be made by studying the energy diagram (Figure 13) of TiO 2 (VB and CB energy levels for the given pH, deduced from data in [34,35]), as well as of the relevant red/ox couples (estimated from data in [36] to account for a pH of 11 and the Ir(III) concentration of 2 × 10 −3 M).The higher the potential difference, |∆E|, between the energy levels of the TiO 2 photogenerated holes and electrons and that of a red/ox couple, the more likely the oxidation/reduction reaction, respectively.From the four possible reactions that the red/ox species shown in Figure 13 can undergo (two oxidations (red lines); two reductions (blue lines)), the oxidation of Ir(III) aq to IrO 2 (|∆E| = 2.77 V) is the most favorable, followed by its reduction to metallic Ir ((|∆E| = 2.01 V): e.g., Ir(OH) 6 or Ir 3+ (aq) + 3e − → Ir e.g., Ir(OH) 6

Evidence for the Photodeposition Mechanism and Form of Ir onto TiO2 from Ir(III) Solutions
The interpretation of the spectroscopic and electrochemical results presented in the Results section above points to the photodeposition of Ir onto TiO2 mainly as IrO2, i.e., according to the reaction scheme of Figure 12 and reactions (3) and ( 4) above.
A first indication that this is the case is given by the effect of methanol addition on Ir content as measured by EDS: this falls from 26% w/w Ir in the absence of methanol to 19% and 2.5% w/w Ir upon addition of small quantities of methanol (0.15% and 1.5% v/v MeOH, respectively).As methanol is expected to compete with Ir(III) for the oxidizing photogenerated species (h + and/or OH • ), it is expected to adversely affect Ir photodeposition, as has indeed been the case.
Second, the surface electrochemistry of Ir oxides and hydroxides depicted in the CV curves of Figures 7 and 8 shows a single redox peak in the case of catalysts prepared in the absence of methanol, at potentials where Ir(IV) oxide is known to be inter-converted to Ir(V) oxide, without the presence of additional Ir(III)/Ir(IV) redox peaks (as in the case of the commercial catalyst and catalysts prepared in the presence of methanol), whereby Ir(III) would originate from the electrochemical oxidation of metallic Ir to Ir(OH)3 at lower applied potentials.
Finally, XPS confirmed that photodeposited Ir was mainly in its Ir(IV) oxidation state (with its percentage diminishing upon methanol addition).

Electrochemical Performance of the TiO2-Supported IrO2 towards OER
The surface electrochemistry of Ir oxides/hydroxides of the laboratory-prepared samples (depicted in the CV curves of Figure 7) allows for an estimate of the charge associated with the Ir(IV)/Ir(V) one-electron transformation (by integration of the single anodic peak/wave recorded in the 0.9-1.1 V potential range); this charge, qIrOx, is in turn an indicator of the electrocatalyst electroactive surface area (esa).Both the esa and qIrOx of IrOx/TiO2 catalysts are expected to depend on IrOx quantity, specific surface area dispersion, and conductivity-IrOx inter-connection, while their mass-specific variants (i.e., esa and qIrOx per unit mass of IrOx, esa and qm,IrOx) should depend only on the latter two parameters.Table 3 below presents the values of mass-specific IrOx-charge; in the case of the commercial, unsupported IrOx catalyst (inset of Figure 7), since there are two couples of redox peaks/waves, corresponding to the 2e transformation of Ir(III) to Ir(V) via an In(IV) intermediate, half of the corresponding charge was used for comparison.
Table 3. Charge associated with 1e electrochemical oxidation of Ir in its surface oxides, as estimated from the anodic part of the CV curves of Figure 7.

Evidence for the Photodeposition Mechanism and Form of Ir onto TiO 2 from Ir(III) Solutions
The interpretation of the spectroscopic and electrochemical results presented in the Results section above points to the photodeposition of Ir onto TiO 2 mainly as IrO 2 , i.e., according to the reaction scheme of Figure 12 and reactions (3) and ( 4) above.
A first indication that this is the case is given by the effect of methanol addition on Ir content as measured by EDS: this falls from 26% w/w Ir in the absence of methanol to 19% and 2.5% w/w Ir upon addition of small quantities of methanol (0.15% and 1.5% v/v MeOH, respectively).As methanol is expected to compete with Ir(III) for the oxidizing photogenerated species (h + and/or OH • ), it is expected to adversely affect Ir photodeposition, as has indeed been the case.
Second, the surface electrochemistry of Ir oxides and hydroxides depicted in the CV curves of Figures 7 and 8 shows a single redox peak in the case of catalysts prepared in the absence of methanol, at potentials where Ir(IV) oxide is known to be inter-converted to Ir(V) oxide, without the presence of additional Ir(III)/Ir(IV) redox peaks (as in the case of the commercial catalyst and catalysts prepared in the presence of methanol), whereby Ir(III) would originate from the electrochemical oxidation of metallic Ir to Ir(OH) 3 at lower applied potentials.
Finally, XPS confirmed that photodeposited Ir was mainly in its Ir(IV) oxidation state (with its percentage diminishing upon methanol addition).

Electrochemical Performance of the TiO 2 -Supported IrO 2 towards OER
The surface electrochemistry of Ir oxides/hydroxides of the laboratory-prepared samples (depicted in the CV curves of Figure 7) allows for an estimate of the charge associated with the Ir(IV)/Ir(V) one-electron transformation (by integration of the single anodic peak/wave recorded in the 0.9-1.1 V potential range); this charge, q IrOx , is in turn an indicator of the electrocatalyst electroactive surface area (esa).Both the esa and q IrOx of IrO x /TiO 2 catalysts are expected to depend on IrO x quantity, specific surface area dispersion, and conductivity-IrO x inter-connection, while their mass-specific variants (i.e., esa and q IrOx per unit mass of IrO x , esa and q m,IrOx ) should depend only on the latter two parameters.Table 3 below presents the values of mass-specific IrO x -charge; in the case of the commercial, unsupported IrO x catalyst (inset of Figure 7), since there are two couples of redox peaks/waves, corresponding to the 2e transformation of Ir(III) to Ir(V) via an In(IV) intermediate, half of the corresponding charge was used for comparison.It can be seen that the commercial catalyst has the highest mass-specific esa, despite the fact that, according to the TEM results of Figures 4 and 5, its aggregates are larger than the well-dispersed nanoparticles of the laboratory-made catalyst.This means that the decrease in conductivity/interparticle contact of the IrO x /TiO 2 system (due to the semiconductor character of TiO 2 ) offsets their higher surface area.
Despite the apparent decrease in their esa, all of the prepared IrO 2 /TiO 2 catalysts show better mass-specific electrocatalytic activity towards the OER than the commercial unsupported IrO 2 catalyst, as follows from the i m vs. E curves of Figure 9a.In fact, the IrO 2 /white-P25 and IrO 2 /black-TiO 2 -oxy catalysts show currents that are better than those of typical state-of-the-art catalysts reported in the literature; e.g., the ATO (antimony tin oxide)-supported IrNiO x catalysts of [37] exhibit a mass-specific current density of i m = 90 mA/mg Ir at an overpotential of η = 280 mV, whereas our best catalysts provide the same currents at the lower overpotential of η = 240 mV.A more detailed comparison of the catalytic behavior of the materials reported in this work and some state-of-the-art catalysts in the literature is given in Table 4, which presents Ir mass-specific currents for OER at given overpotentials and was constructed by quoting or estimating values based on data reported in the referenced literature and in this work (corrected for IR-drop).The increased mass-specific activity of the prepared catalysts of this work with respect to the commercial catalyst (despite the latter having a larger apparent esa) is due to their higher intrinsic activity as highlighted by the curves of Figure 9b, where currents are normalized by the IrO x charge (esa descriptor).The higher activity of IrO 2 /TiO 2 with respect to the unsupported IrO 2 may be interpreted (in a way similar to the effect of Ni on IrO 2 [41]) by the difference in electronegativity and size of Ir and Ti, which may destabilize the Ir-OH bonds and increase the presence of activated O species that are intermediates in the OER mechanism.Also, Ir-O-Ir bonds may be disrupted by the formation of Ir-O-Ti bonds as suggested in [20] based on XPS data (in a way similar to the formation/partial decomposition of Ir-O-Ni bridges proposed in [42]).As suggested in [43], XPS analysis of the O 1s is crucial in determining the presence of oxygenated species that are key to OER at oxide electrodes; such measurements, carried out by our group on similar IrO 2 /TiO 2 samples, have shown the existence of significant quantities of OH species on the surface of the catalyst [28].

Experimental Section 4.1. Synthesis of IrO 2 on Various TiO 2 Powders
Preparation of black-P25: Black-P25 was produced by ammonolysis.In a typical process, ~100 mg of commercially available white-P25 (Sigma-Aldrich Chemie GmbH, Taufkirchen, Germany) powder was loaded on a crucible and placed inside a quartz tube furnace.The tube ends were sealed, and the air inside was fully replaced by ammonia gas (NH 3 flushing).After sufficient flushing, the ammonia flow was significantly reduced and set at a constant flow rate.Then, the white-P25 was treated under ammonia at 100 • C, 300 • C, 500 • C, and 650 • C, staying at each temperature step for a total of 30 min (10 min reaching the set point temperature and 20 min for conditioning).After the last step at 650 • C, the TiO 2 P25 ® powder was treated there for 3 h and then freely cooled down to room temperature.
Preparation of TiO 2 from hydrated TiOSO 4 (white-TiO 2 -oxy): Titanium (IV) oxysulfate hydrate (TiOSO 4 •xH 2 O) purchased from Sigma Aldrich, Taufkirchen, Germany, was used to prepare the white-TiO 2 -oxy by a co-precipitation method.Titanium dioxide was precipitated at pH ~7 from an aqueous solution of TiOSO 4 titanium (IV) oxysulfate hydrate (0.1 M) by the addition of ammonia (VWR Chemicals, Lutterworth, UK).After aging overnight, the suspension was filtered with distilled water until it became sulfate-and ammonium ion-free and dried in air at 100 • C. The residue was crushed to a fine powder and calcined in a furnace at 700 • C for 3 h with a heating ramp rate of 5 • C min −1 .
Preparation of black TiO 2 black oxysulfate (black-TiO 2 -oxy): The powder was produced by ammonolysis, as previously described.
Photodeposition of iridium nanoparticles on various TiO 2 supports: A photodeposition method was used for the preparation of supported OER catalysts.It is a simple and ambient temperature process, leading to the direct deposition of iridium dioxide onto the TiO 2 semiconducting powders by UV light irradiation, as described in our previous work [28].An appropriate iridium salt aqueous solution of 120 mL (0.002 M K 3 IrCl 6 , Sigma-Aldrich Chemie GmbH, Taufkirchen, Germany), adjusted to pH = 11 (using 1 M KOH), was prepared and deaerated under N 2 purge for 15 min.The aqueous solution was transferred to a photochemical cylindrical reactor (250 cm 3 ), and TiO 2 powder (0.008 M) was also added.The UVA lamp (Radium Ralutec 9 W/78, λ = 350-400 nm, λ max = 369 nm) was placed in a cylindrical quartz tube in the center of the photo-reactor.The materials were stirred for 20 min to prepare a homogeneous slurry.The latter was kept under UV light irradiation for 8 h to achieve (in most cases) ca 25 wt% of Ir photodeposited on the TiO 2 nanoparticle substrate.Vacuum filtration followed with distilled water, and the resulting powder catalyst (gray, blue-black, or black in color, depending on the TiO 2 support) was dried overnight at room temperature.The resulting solid was ground to a fine powder using an agate mortar.The four types of prepared samples were (a) IrO 2 /TiO 2 (white-P25), (b) IrO 2 /TiO 2 (black-P25), (c) IrO 2 /TiO 2 (white-TiO 2 -oxy), and (d) IrO 2 /TiO 2 (black-TiO 2 -oxy).

Structural, Chemical, and Morphological Measurements
The lattice parameters and the crystalline phases of the prepared TiO 2 substrates were characterized by an X-ray Diffractometer (XRD) (Brucker AXS D8, Karlsruhe, Germany) equipped with a nickel foil monochromator (40 kV, 20 mA) at scattering angles 2θ between 10 and 80 • (0.05 • s −1 scan rate) using Cu Ka 1 radiation.The diffraction pattern was analyzed by the Scherrer equation giving the crystallite size of each synthesized powder.The surface morphology and elemental composition were analyzed using a Field Emission Scanning Electron Microscope (FESEM; 7000 JEOL, Tokyo, Japan) with energy-dispersive X-ray spectroscopy, operating at 20 keV.Diffuse reflectance (DR) UV-visible spectra were measured by a Perkin Elmer Lambda 950 UV/Vis/NIR spectrophotometer working at λ = 250-2500 nm, and it was employed to measure the absorption/reflection spectrums.The optical energy bandgaps were extracted by the Tauc plot of Equation (7).
(ahν) n = hν − E g (7) where α is the absorption coefficient, h is the Planck constant, ν is the radiation frequency, and n is 0.5 or 2 for indirect or direct transition.The energy gap was also calculated at the interception of the linear fit of the appropriate region on the Tauc plot (where α is zero).X-ray photoelectron spectroscopy (XPS) measurements were performed using a Kratos Axis Ultra DLS spectrometer, Manchester, UK, equipped with a non-monochromatic Al X-ray source (under vacuum better than 10 −8 Pa at a 90 • take-off angle).The Ir4f line was subjected to an additional fitting procedure with XPSPEK4.1 software to determine the chemical oxidation states in the absence and presence of methanol.Transmission Electron Microscopy (TEM) images were obtained for the photocatalytically prepared powders on a JEM 2100 (JEOL, Tokyo, Japan) equipped with a LaB 6 filament at an accelerating voltage of 200 kV.

Electrochemical Measurements
Procedure: The surface electrochemistry and the electrochemical oxygen evolution activity and stability of the synthesized catalysts were studied using a PGSTAT302N potentiostat (Metrohm Autolab, Herisau, Switzerland), in a standard three-compartment glass cell equipped with a Luggin capillary and comprising a Pt foil counter electrode, a saturated calomel electrode reference electrode, and a glassy carbon (GC) working electrode substrate-current collector (3 mm diameter).The experiments were recorded in a 0.1 M HClO 4 (70%, Sigma-Aldrich, Chemie GmbH, Taufkirchen, Germany) electrolyte at 25 • C. The system was purged with N 2 for 15 min before the working electrode was placed in the electrolyte to remove dissolved oxygen before the electrochemical measurements were recorded.
Electrode preparation: Prior to every measurement, the glassy carbon (GC) working electrode was polished with an alumina slurry, and then it was sonicated to remove impurities and any residual polishing slurry.Catalyst inks were coated as a thin-film layer on the GC surface of a Rotating Disk Electrode (RDE) with the resulting loading of Ir in the 0.5-1.0mg cm −2 range.The ink suspension was composed of x mg catalyst (according to the w/w % Ir composition from EDS), 6% w/w Nafion ® perfluorinated resin solution (5 wt% Sigma-Aldrich) and ethanol as the ionic binder and solvent, respectively.It was mixed and ultrasonically homogenized for 30 min.The temperature of the sonication was kept at ca 35 • C to avoid evaporation of the solvent.
Electrochemical characterization: The surface electrochemistry of IrO 2 /TiO 2 was studied by cyclic voltammetry (CV) experiments in the potential range between −0.3 and 1.1 V vs. SCE at 25 mV s −1 until a stable CV was obtained.The last stable cycle was used to estimate the IrO x charge.The OER polarization curves were recorded by Linear Sweep Voltammetry (LSV) at 1600 rpm and a slow scan rate (5 mV s −1 ).Electrochemical Impedance Spectroscopy (EIS) measurements were carried out in the frequency range of 100 kHz to 100 mHz with an amplitude of 10 mV.The ohmic resistance was estimated from the EIS measurements and use for IR compensation of the LSV curves.For the mediumterm stability tests, the electrode was held at a constant potential of 1.3 V vs. SCE under a rotation speed of 1600 rpm.

Conclusions
Summarizing, this study has demonstrated the following: a.
We showed the successful UV light photodeposition of iridium from IrCl 6 −3 solutions onto TiO 2 powders in the form of IrO x nanoparticles.This comprises an ambient temperature and simple chemistry alternative for the preparation of IrO 2 -TiO 2 composites (advantages characteristic of photocatalytic synthetic methods when compared to other techniques for electrocatalyst preparation such as hydrothermal or/and sonochemical techniques; see, for example, [44,45]).b.All of the thus prepared IrO x /TiO 2 catalysts (despite a moderate apparent electroactive surface area due to electronic conductivity losses) exhibited superior mass-specific

Figure 6 .
Figure 6.X-ray photoelectron spectra in the Ir4f binding energy range of IrOx/TiO2 (white-P25) powder nanocatalyst prepared by UV photodeposition in the absence (a) and presence (b) of 0.15% v/v MeOH.

Figure 6 .
Figure 6.X-ray photoelectron spectra in the Ir4f binding energy range of IrO x /TiO 2 (white-P25) powder nanocatalyst prepared by UV photodeposition in the absence (a) and presence (b) of 0.15% v/v MeOH.

Figure 7 .
Figure 7. Cyclic voltammetry curves of IrOx/TiO2 electrodes as well as of commercial IrO2 electrode (inset), at 25 mV s −1 , in a deaerated 0.1 M HClO4 solution.Current density, ig, is reported per geometric glassy carbon electrode current collector area.

Figure 7 .
Figure 7. Cyclic voltammetry curves of IrO x /TiO 2 electrodes as well as of commercial IrO 2 electrode (inset), at 25 mV s −1 , in a deaerated 0.1 M HClO 4 solution.Current density, i g , is reported per geometric glassy carbon electrode current collector area.

Figure 7 .
Figure 7. Cyclic voltammetry curves of IrOx/TiO2 electrodes as well as of commercial IrO2 electrode (inset), at 25 mV s −1 , in a deaerated 0.1 M HClO4 solution.Current density, ig, is reported per geometric glassy carbon electrode current collector area.

Figure 8 .
Figure 8.Effect of MeOH content (0, 0.15, 1.5% v/v) during catalyst preparation by photodeposition onto TiO2 from Ir(III) chloro-complex solutions to Ir/IrO2 surface electrochemistry.Near-steady-state Linear Sweep Voltammetry (LSV) at a slow potential sweep rate (5 mV s −1 ) was employed to investigate the OER activity of the Ir-based catalysts.In Figure

Figure 9 .
Figure 9. LSVs at 1600 rpm and 5 mVs −1 (a) per mg of Ir and (b) per mC of Ir(IV) to Ir(V) transformation.The potential has been corrected for IR-drop.

Figure 9 .
Figure 9. LSVs at 1600 rpm and 5 mVs −1 (a) per mg of Ir and (b) per mC of Ir(IV) to Ir(V) transformation.The potential has been corrected for IR-drop.

Figure 12 .
Figure 12.Photodeposition routes of Ir(III) on TiO2; (a) cathodic deposition of Ir at CB and (b) anodic deposition of IrO2 at VB. Methanol reactions at VB are also considered.Figure 12. Photodeposition routes of Ir(III) on TiO 2 ; (a) cathodic deposition of Ir at CB and (b) anodic deposition of IrO 2 at VB. Methanol reactions at VB are also considered.

Figure 12 .
Figure 12.Photodeposition routes of Ir(III) on TiO2; (a) cathodic deposition of Ir at CB and (b) anodic deposition of IrO2 at VB. Methanol reactions at VB are also considered.Figure 12. Photodeposition routes of Ir(III) on TiO 2 ; (a) cathodic deposition of Ir at CB and (b) anodic deposition of IrO 2 at VB. Methanol reactions at VB are also considered.

Figure 13 .
Figure 13.Energy diagram for TiO2 (VB and CB) and various ox/red couples.

Figure 13 .
Figure 13.Energy diagram for TiO 2 (VB and CB) and various ox/red couples.

Table 1 .
EDS elemental analysis of the TiO2 powders before and after ammonolysis.

Table 2 .
Parameters of the fitted equivalent circuit [R s (R f Q f )(R ct Q dl )] to EIS results, for the commercial IrO 2 , white-25, and black-TiO 2 -oxy electrodes, in 0.1 M HClO 4 and at +1.20 V vs. SCE.

Table 3 .
Charge associated with 1e electrochemical oxidation of Ir in its surface oxides, as estimated from the anodic part of the CV curves of Figure7.

Table 4 .
Ir mass-specific currents for OER recorded at η = 260 mV and 280 mV, for OER from acid solutions, at supported IrO 2 nanoparticles.