Micro-Sized pH Sensors Based on Scanning Electrochemical Probe Microscopy

Monitoring pH changes at the micro/nano scale is essential to gain a fundamental understanding of surface processes. Detection of local pH changes at the electrode/electrolyte interface can be achieved through the use of micro-/nano-sized pH sensors. When combined with scanning electrochemical microscopy (SECM), these sensors can provide measurements with high spatial resolution. This article reviews the state-of-the-art design and fabrication of micro-/nano-sized pH sensors, as well as their applications based on SECM. Considerations for selecting sensing probes for use in biological studies, corrosion science, in energy applications, and for environmental research are examined. Different types of pH sensitive probes are summarized and compared. Finally, future trends and emerging applications of micro-/nano-sized pH sensors are discussed.


Introduction
Chemical reactions are often strongly influenced by the concentration of hydrogen ions (H + ) in solution, making its measurement crucial to characterize aqueous solutions [1]. As H + concentration may span many orders of magnitude, it is commonly represented on a logarithmic scale as pH. Many biological mechanisms depend heavily on electrochemical gradients or differences in pH across a membrane to enable their biological functions. Proton transfer plays a key role in biological systems, underlying the functioning of many enzymatic reactions and ion channels. H + concentration greatly influences the function of proteins that act as proton regulators, especially if the pH reaches beyond acceptable working levels. Further, when a cell undergoes inflammation or tumorigenesis, the unhealthy cell acidifies its environment, thus promoting tumor metastasis and contributing to normal cell death. A cancer cell's local pH plays an important role in cancer progression by modulating its invasiveness and resistance to therapy [2][3][4].
Solution pH also has a strong influence on many industrial processes, such as metal electroplating and paint electrodeposition. For example, pH influences the conductivity and current density needed to electrodeposit metallic alloy coatings [5,6], as well as the surface thickness, roughness, resistance to cracking, and corrosion of the coatings [6,7]. The stability of coatings and their resistance to bacterial growth are also influenced by the environmental pH both before and after the deposition of the coating [8][9][10][11].
Local pH measurements can be useful to elucidate and modify the chemical environment, such as in microfluidic applications [12][13][14]. They can also help to decode reaction mechanisms that depend on or affect the local pH. Scanning electrochemical microscopy (SECM) is a type of scanning probe microscopy (SPM) that generates images by scanning a specialized probe over the sample. Using SECM allows the transformation of individual pH measurements into two-dimensional (2D) or three-dimensional (3D) pH images. Electrochemical pH sensors have several advantages over optical and spectroscopic methods: pH M x O y + 2y H + + 2y e − ⇔ x M + y H 2 O Multiple proposed pH-sensing mechanisms are possible, but the most likely is the oxygen intercalation mechanism proposed by Fog and Buck [23] as it closely matches the known non-stoichiometric oxygen content of these metal oxides. The pH-sensing mechanism of IrOx is likely due to the reversible electrochemical reaction of Ir(III) and Ir(IV) [26]: 2 IrO 2 + 2 H + + 2 e − ⇔ Ir 2 O 3 + H 2 O The mechanism may be affected by the environment being hydrated or non-hydrated. While much work has been conducted to uncover the exact mechanism, complex reactions involving other hydrated or anhydrous iridium oxides may occur. Similar mechanisms have also been proposed for other metal oxides, such as ruthenium oxide (RuOx), antimony oxide (SbOx), cerium oxide (CeOx), and tin oxide (SnOx) [16,20,23,24]. Antimony oxide pH sensing electrodes are often used in pH-SECM applications. Like other MOx materials, although the exact mechanism is unknown, it is believed that multiple redox reactions may be involved, but the main detection redox reaction is the following [1,27]: However, research on antimony oxide pH electrodes has also shown that continuous adsorption of oxide species onto the surface increases the coating thickness and reduces the accuracy of the sensor for pH measurements [27,28].
Like MOx materials, polymers such as polyaniline (PANI) and syringaldazine (Syr) have also gained popularity in pH sensing in recent years [29][30][31][32][33][34][35][36][37][38]. PANI is a promising solid-state pH sensor due to its good conductivity, low cost, biocompatibility, high stability, and well-established electrochemical polymerization procedure. PANI may undergo two redox processes-protonation during reduction and deprotonation during oxidation. The favorability of the two processes strongly depends on the pH of the aqueous electrolyte, which allows sensitive pH determination [30,31]. Those pH-sensitive polymers, such as syringaldezine, are insoluble in water, thus making them less likely to desorb from the electrode when used in aqueous solutions. Syringaldezine, similar to PANI, can also easily and readily undergo electrochemical conversion between its two reversable forms, involving two protons and two electrons, thus making it sensitive to the concentration of protons in solution. The pH change may be monitored by the shift in peaks observed in cyclic voltammetry, where a more positive peak indicates a lower pH value [36,37].

Sensor Fabrication
Almost all of the methods currently in use for fabricating SECM sensor probes, whether based on micropipettes and/or microelectrodes, involve heat-pulled glass pipettes as the backbone onto which the rest of the sensor components are assembled. While there are a variety of methods to fabricate these sensing probes, a typical procedure for making a micropipette is illustrated in Figure 1a-c, and a typical procedure for preparing a microelectrode is illustrated in Figure 1d-f [39]. mers, such as syringaldezine, are insoluble in water, thus making them less likely to desorb from the electrode when used in aqueous solutions. Syringaldezine, similar to PANI, can also easily and readily undergo electrochemical conversion between its two reversable forms, involving two protons and two electrons, thus making it sensitive to the concentration of protons in solution. The pH change may be monitored by the shift in peaks observed in cyclic voltammetry, where a more positive peak indicates a lower pH value [36,37].

Sensor Fabrication
Almost all of the methods currently in use for fabricating SECM sensor probes, whether based on micropipettes and/or microelectrodes, involve heat-pulled glass pipettes as the backbone onto which the rest of the sensor components are assembled. While there are a variety of methods to fabricate these sensing probes, a typical procedure for making a micropipette is illustrated in Figure 1a-c, and a typical procedure for preparing a microelectrode is illustrated in Figure 1d-f [39].

Micropipette Glass Backbone Fabrication
Typically, a heating coil-or laser-based pipette puller is used to heat and pull apart a single glass capillary made of soda-lime, borosilicate, or quartz glass until it is split in half, resulting in two micropipettes, as shown in Figure 1a-c. The geometric properties of the formed pipettes can be controlled and tuned by adjusting the parameters of the micropipette puller. These micropipettes are now ready to be modified with a pH-sensing material either on the inside or outside surface using sputtering or other methods. Figure 1. UME fabrication technique [39]: (a) bare soda-lime glass capillary, (b) heating the capillary with a CO2 laser and pulling to form a sharp tip, (c) the two separated micropipette ends, (d) an electroactive wire is inserted into the micropipette and maneuvered to the tip before a vacuum tube is attached to the open end, (e) the electroactive wire is sealed in position under vacuum with a heating coil, and (f) the UME is finalized by adding the connective wires and the outer protective glass capillary. Adapted from ref. [39]. Copyright (2015) with permission from the American Chemical Society. Figure 1. UME fabrication technique [39]: (a) bare soda-lime glass capillary, (b) heating the capillary with a CO 2 laser and pulling to form a sharp tip, (c) the two separated micropipette ends, (d) an electroactive wire is inserted into the micropipette and maneuvered to the tip before a vacuum tube is attached to the open end, (e) the electroactive wire is sealed in position under vacuum with a heating coil, and (f) the UME is finalized by adding the connective wires and the outer protective glass capillary. Adapted from ref. [39]. Copyright (2015) with permission from the American Chemical Society.

Micropipette Glass Backbone Fabrication
Typically, a heating coil-or laser-based pipette puller is used to heat and pull apart a single glass capillary made of soda-lime, borosilicate, or quartz glass until it is split in half, resulting in two micropipettes, as shown in Figure 1a-c. The geometric properties of the formed pipettes can be controlled and tuned by adjusting the parameters of the micropipette puller. These micropipettes are now ready to be modified with a pH-sensing material either on the inside or outside surface using sputtering or other methods.

Microelectrode Glass Backbone Fabrication
A similar procedure is used to prepare the glass supports for microelectrode-style probes. After using the pipette puller to obtain the two glass pipettes, a small diameter electroactive wire (typically gold, platinum, or carbon-fiber) is inserted into the open end and then carefully maneuvered to the sharp end with the help of a micromanipulator or other methods, as shown in Figure 1d. Alternatively, the wire may be inserted into the glass capillary before it is pulled apart. The wire is then fixed into position using a small heating coil to collapse the glass around the wire at the pipette tip under vacuum (Figure 1d,e). The connecting wire is then inserted through the open back end of the pipette and attached to the smaller wire using conductive silver epoxy, as shown in Figure 1f. A general-purpose SECM sensor probe can be made by sanding and polishing the pipette tip to expose the tip of the electroactive wire. Alternatively, depending on the required tip geometry (disk, needle, ring, etc.), other methods, such as ion beam or electrochemical etching, can be employed to optimize the portion of the electroactive wire that will later be modified. Next, the electroactive surface is functionalized with a pH-sensitive material. In the next sections, steps for modifying a general tip into a pH sensor, along with methods for implementing tip-to-substrate measurements, will be presented.

Microelectrode-Based pH Sensors
Once the glass backbone of the microelectrode has been prepared, it needs to be coated with a pH-sensitive material. There are many methods used to achieve this, and only a few notable methods are highlighted here. A facile procedure for fabricating pHsensitive microelectrodes was reported by Khani and Wipf [40] in which a carbon fiber (CF) was electrochemically etched, its tip was then shielded, and poly(oxyphenylene) was electropolymerized onto the unshielded portion of the tip to insulate it, as illustrated in Figure 2. With this procedure, only the very tip of the needle-like ultramicroelectrode was exposed, making it ready for electrodeposition of IrOx using an adapted procedure from Pikulski and Gorski [41]. Briefly, a three-electrode set up was used with the CF-UME as the working electrode, while an Ag/AgCl wire served as the reference electrode, and a Pt wire served as the counter electrode. The electrodeposition solution was 0.2 mM Na 3 IrCl 6 and 0.1 M KNO 3 solution, which was previously heated up for 3 h and cooled to encourage the aquation of the iridium complexes. In that solution, 50 cyclic voltammetric cycles from −0.2 V to 1.2 V were run, followed by holding the potential at 0.6 V for 5 min, resulting in the formation of IrOx onto the exposed area of the CF-UME tip, thus creating a pH-sensitive UME. More details about this design can be found in references [40][41][42].
Another good approach for the fabrication of probes capable of performing two types of measurements (pH and tip-to-sample distance) was proposed by Santos et al. [43], where a single disk-shaped electroactive surface was covered with intentionally defective layers of IrOx. The porosity and defects of the IrOx film are intended and required for this method to work, since this correctly allows the species in the solution to reach both the IrOx to perform the pH measurements and the underlying gold electrode for use in distance control in SECM feedback mode. The above was achieved by encapsulating a 25 µm diameter gold wire in a borosilicate glass capillary and pulling it apart in a similar procedure as the one described in the beginning of this section. Once the bare Au electrode was fabricated, the IrOx electrodeposition solution was made according to a procedure that was adapted from earlier work by Yamanaka and Elsen et al. [22,44]. A three-electrode cell system was used for the electrochemical deposition, with the gold electrode as the working electrode, Ag/AgCl for the reference electrode, and a platinum wire as the counter electrode. The first step was to hold the potential at 0.8 V for 600 s, then cyclic voltammetry in the range between 0 to 0.8 V was run for 5 cycles or more, with thicker and more homogenous coverage of the Au surface as the number of cycles increased. Unfortunately, methods like these that rely on the same surface to do separate measurements may result in competition between the two measurement types, in which one measurement would have to be sacrificed in order to improve the other. There may also be some stability and longevity drawbacks for this design. If the film was made thicker, it would improve the stability of the IrOx film on the gold electrode; however, the thicker film might also restrict the species in the solution from reaching the underlying Au surface, thus making the tip-to-substrate measurements less accurate and often resulting in crashing the tip to the sample.
have to be sacrificed in order to improve the other. There may also be some stability an longevity drawbacks for this design. If the film was made thicker, it would improve th stability of the IrOx film on the gold electrode; however, the thicker film might also restri the species in the solution from reaching the underlying Au surface, thus making the tip to-substrate measurements less accurate and often resulting in crashing the tip to the sam ple. Monteiro et al. [45] designed a probe that consisted of adsorbing an organic self-as sembled monolayer (SAM) of 4-nitrothiophenol (4-NTP) onto a disk gold UME, whic was then converted into the redox couple hydroxylaminothiophenol (4-HATP)/4-nitro sothiophenol (4-NSTP). Briefly, a gold wire was encapsulated in glass, cleaned, and po ished using similar procedures as described above. Once the bare gold UME was pre pared, it was modified by immersing it into a 4-NTP/ethanol solution for 20 min, whic spontaneously resulted in the irreversible adsorption of a 4-NTP monolayer onto the A surface through the thiol anchor group. After the UME was rinsed, it was transferred int a 0.1 M H2SO4 solution and polarized in the range of 0.1 to −0.25 (vs. Ag/AgCl) in order t convert the 4-NTP into 4-HATP and 4-NSTP species to make the probe sensitive to pH changes. To make pH measurements, the reversable oxidation of the 4-HATP to 4-NST species through the transfer of two protons and two electrons is monitored using cycl voltammetry [45][46][47].

Micropipette-Based pH Sensors
A popular pH sensor design is the use of an ion-selective cocktail for the detection o local pH changes. There are a variety of methods used to fabricate such probes, includin both single-and double-barrel pH sensors, and a variety of different ion-selective cocktai are capable of detecting local concentrations of protons. For example, Joshi et al. [48] de veloped this type of pH sensor based on an H + ion-selective cocktail consisting of 5% Monteiro et al. [45] designed a probe that consisted of adsorbing an organic self-assembled monolayer (SAM) of 4-nitrothiophenol (4-NTP) onto a disk gold UME, which was then converted into the redox couple hydroxylaminothiophenol (4-HATP)/4-nitrosothiophenol (4-NSTP). Briefly, a gold wire was encapsulated in glass, cleaned, and polished using similar procedures as described above. Once the bare gold UME was prepared, it was modified by immersing it into a 4-NTP/ethanol solution for 20 min, which spontaneously resulted in the irreversible adsorption of a 4-NTP monolayer onto the Au surface through the thiol anchor group. After the UME was rinsed, it was transferred into a 0.1 M H 2 SO 4 solution and polarized in the range of 0.1 to −0.25 (vs. Ag/AgCl) in order to convert the 4-NTP into 4-HATP and 4-NSTP species to make the probe sensitive to pH changes. To make pH measurements, the reversable oxidation of the 4-HATP to 4-NSTP species through the transfer of two protons and two electrons is monitored using cyclic voltammetry [45][46][47].

Micropipette-Based pH Sensors
A popular pH sensor design is the use of an ion-selective cocktail for the detection of local pH changes. There are a variety of methods used to fabricate such probes, including both single-and double-barrel pH sensors, and a variety of different ion-selective cocktails are capable of detecting local concentrations of protons. For example, Joshi et al. [48] developed this type of pH sensor based on an H + ion-selective cocktail consisting of 5% proton ionophore I, 2% potassium tetrakis(4-chlorophenyl)borate, 30% 1-(2-nitrophenoxy) octane (NPOE), 3% poly(vinyl chloride) (PVC), 60% Vulcan carbon powder, and 500 µL of tetrahydrofuran (THF). Their procedure started with pulling a borosilicate glass pipette apart using a similar procedure as described above. Once a glass backbone was created, their H + ion-selective cocktail was mixed and backfilled into the pipette from its back end, then pushed further into the tip using a copper wire, before adding a mixture of 5% Vulcan carbon in dioctyl sebacate (DOS). The electrical connection was made using a copper wire, which was stabilized in position using epoxy. Another example of the use of ion-selective pH sensors is the work published by Etienne et al. [7], in which a different commercially available ion-selective cocktail was chosen: pH-ionophore II-cocktail A. A similar procedure was employed to pull apart the borosilicate glass capillary to obtain a micropipette. The micropipette was then polished on a microelectrode beveller, and hexamethyldisilazane was used to silanize the inner cavity of the micropipette before filling it with the ion-selective cocktail, then backfilling it with 0.1 M KCl solution on top for use as the internal electrode.
Huang et al. [49] designed a miniaturized coaxial pH sensor that encapsulated the Ag/AgCl reference electrode inside of the pipette cavity of the sensor, while the gold and pH-sensitive IrOx were deposited on the outside of the sensor. A thin layer of Au was deposited on the outside of the pipette by RF magnetron sputtering. Conductive silver epoxy paste was used to attach a copper wire to the Au layer. Agar and KCl were mixed, boiled, and then inserted into the pipette from its back end using a syringe. While the solution was still hot, an Ag/AgCl wire was inserted into the back of the pipette, which was then sealed using silicon rubber. Finally, to make the tip of the pipette sensitive to pH, IrOx was electrodeposited onto the Au film using a modified Yamanaka procedure [21,22]. The resultant pH sensor is illustrated in Figure 3a and an SEM image of the tip of the pH sensor is displayed in Figure 3b [49], further confirming the success of the fabrication.
pipette apart using a similar procedure as described above. Once a glass backbone w created, their H + ion-selective cocktail was mixed and backfilled into the pipette from i back end, then pushed further into the tip using a copper wire, before adding a mixtu of 5% Vulcan carbon in dioctyl sebacate (DOS). The electrical connection was made usin a copper wire, which was stabilized in position using epoxy. Another example of the u of ion-selective pH sensors is the work published by Etienne et al. [7], in which a differe commercially available ion-selective cocktail was chosen: pH-ionophore II-cocktail A. similar procedure was employed to pull apart the borosilicate glass capillary to obtain micropipette. The micropipette was then polished on a microelectrode beveller, and he amethyldisilazane was used to silanize the inner cavity of the micropipette before fillin it with the ion-selective cocktail, then backfilling it with 0.1 M KCl solution on top for u as the internal electrode.
Huang et al. [49] designed a miniaturized coaxial pH sensor that encapsulated th Ag/AgCl reference electrode inside of the pipette cavity of the sensor, while the gold an pH-sensitive IrOx were deposited on the outside of the sensor. A thin layer of Au w deposited on the outside of the pipette by RF magnetron sputtering. Conductive silv epoxy paste was used to attach a copper wire to the Au layer. Agar and KCl were mixe boiled, and then inserted into the pipette from its back end using a syringe. While th solution was still hot, an Ag/AgCl wire was inserted into the back of the pipette, whic was then sealed using silicon rubber. Finally, to make the tip of the pipette sensitive pH, IrOx was electrodeposited onto the Au film using a modified Yamanaka procedu [21,22]. The resultant pH sensor is illustrated in Figure 3a and an SEM image of the tip the pH sensor is displayed in Figure 3b [49], further confirming the success of the fabric tion. Zhang et al. [2] developed two versions, single-barrel and double-barrel, of a pH se sitive nanopipette based on self-assembled zwitterion-like nanomaterials, which may f vor the permeability of anions at low pH and cations at high pH, as illustrated in Figu 4. The single-barrel pH-sensing nanoprobe was fabricated using a similar procedure described above for pulling a borosilicate glass capillary to the required size for a nanop pette, as seen in Figure 4a. Glucose oxidase (GOx) denatured at 70 °C for 10 min was the dissolved in 0.01% poly-l-lysin (PLL) at a concentration of 0.4 mg/mL to make a hydroge which provided the positively charged residues through the amines of PLL and th Zhang et al. [2] developed two versions, single-barrel and double-barrel, of a pH sensitive nanopipette based on self-assembled zwitterion-like nanomaterials, which may favor the permeability of anions at low pH and cations at high pH, as illustrated in Figure 4. The single-barrel pH-sensing nanoprobe was fabricated using a similar procedure as described above for pulling a borosilicate glass capillary to the required size for a nanopipette, as seen in Figure 4a. Glucose oxidase (GOx) denatured at 70 • C for 10 min was then dissolved in 0.01% poly-l-lysin (PLL) at a concentration of 0.4 mg/mL to make a hydrogel, which provided the positively charged residues through the amines of PLL and the negatively charged residues through GOx. The hydrogel was drawn up into the pulled glass pipette through capillary action to a height of around 1 mm from the opening of the tip. The hydrogel was then used to self-assemble the residues onto the opening of the pipette through drying of the sensing material nanomembrane. The vapor of glutaraldehyde (25% v/v) was used to slowly crosslink the hydrogel residues inside the glass pipette, as seen in Figure 4a.
Strong covalent bonds were expected to form between the amino groups left by the PLL, GOx, and glutaraldehyde vapor, forming a robust nanomembrane (~200 nm) capable of sensing local pH at the tip of the pipette. The remaining steps included cleaning the probe with KCl (100 mM pH 7.0) to remove any remaining glutaraldehyde and unreacted or unlinked residues. To prepare the double-barrel nanopipette, a similar procedure was followed for making the glass backbone and the rest of the probe, except for the use of "Blu-tack" to block one of the two barrels. A small pressure of~200 kPa was applied to the second barrel to resist drawing up the PLL/GOx hydrogel through capillary action. The second pipette barrel would remain open for use in SICM tip-to-substrate distance measurements. The single-barrel probe was capable of sensing both localized pH as well as tip-to-sample distance measurements through the linear ionic response at the same single pipette tip during its approach to the sample. However, while measuring the SICM ionic current as a feedback control signal (as detailed in Section 4.4), along with the localized pH, the single-barrel sensor is sensitive to any extracellular pH changes and can introduce some unexpected artifacts, which appear as a ball-like shape at the H + source. This can be remedied with the use of the dual-barrel version of the pH probe or, alternatively, by making a height measurement with the single-barrel probe relatively far away from the H + source, and then constant-height mode can be used to image the rest of the sample [2].
negatively charged residues through GOx. The hydrogel was drawn up into the pulled glass pipette through capillary action to a height of around 1 mm from the opening of the tip. The hydrogel was then used to self-assemble the residues onto the opening of the pipette through drying of the sensing material nanomembrane. The vapor of glutaraldehyde (25% v/v) was used to slowly crosslink the hydrogel residues inside the glass pipette, as seen in Figure 4a. Strong covalent bonds were expected to form between the amino groups left by the PLL, GOx, and glutaraldehyde vapor, forming a robust nanomembrane (~200 nm) capable of sensing local pH at the tip of the pipette. The remaining steps included cleaning the probe with KCl (100 mM pH 7.0) to remove any remaining glutaraldehyde and unreacted or unlinked residues. To prepare the double-barrel nanopipette, a similar procedure was followed for making the glass backbone and the rest of the probe, except for the use of "Blu-tack" to block one of the two barrels. A small pressure of ~200 kPa was applied to the second barrel to resist drawing up the PLL/GOx hydrogel through capillary action. The second pipette barrel would remain open for use in SICM tip-to-substrate distance measurements. The single-barrel probe was capable of sensing both localized pH as well as tip-to-sample distance measurements through the linear ionic response at the same single pipette tip during its approach to the sample. However, while measuring the SICM ionic current as a feedback control signal (as detailed in Section 4.4), along with the localized pH, the single-barrel sensor is sensitive to any extracellular pH changes and can introduce some unexpected artifacts, which appear as a ball-like shape at the H + source. This can be remedied with the use of the dual-barrel version of the pH probe or, alternatively, by making a height measurement with the single-barrel probe relatively far away from the H + source, and then constant-height mode can be used to image the rest of the sample [2]. (i) Schematic of the carbon-based pH sensor before deposition of iridium oxide. Images (a-d) were reprinted from ref. [2] under CC-BY 4.0 license. Images (e,f) were adapted from ref. [50]. Copyright (2013) with permission (i) Schematic of the carbon-based pH sensor before deposition of iridium oxide. Images (a-d) were reprinted from ref. [2] under CC-BY 4.0 license. Images (e,f) were adapted from ref. [50]. Copyright (2013) with permission from the American Chemical Society. Images (g-i) were adapted from ref. [51]. Copyright (2011) with permission from John Wiley and Sons.
Nadappuram et al. [50] proposed a simple procedure to build pH probes based on SECM-SICM, using a procedure similar to the one described by Takahashi et al. [51]. The sensor is a double-barrel nanopipette that is capable of measuring localized pH through one of the barrels using a pyrolytically deposited carbon electrode that has been modified with IrOx by electrodeposition. The other side of the electrode is left open and used to measure tip-to-substrate distances. To achieve this, Nadappuram et al. pulled apart a quartz theta (i.e., double-barrel) capillary and blocked one of the pipette openings with "Blu-Tack" putty, while a butane gas tube was attached to the other opening. In an argon atmosphere, butane was supplied through the tube, and the tip of the probe was heated using a torch to induce pyrolytic decomposition of butane, resulting in the deposition of carbon inside one of the pipette's tips. A simple schematic of this procedure is illustrated in Figure 4e, while the probe's optical and SEM side-image micrographs are presented in Figure 4f and g, respectively. An SEM micrograph and illustration of the bottom of the tip of the sensor are also presented in Figure 4h and i, respectively. Next, a wire was connected to the deposited carbon through the back of the pipette and hydrated IrOx was deposited onto the carbon-filled tip of the pipette by electrodeposition using similar methods as described previously [22], which was achieved by holding a constant potential at 0.68 V (vs. Ag/AgCl QRCE in 0.1 KCl) for 600 s [50].

Positioning Methods
Successful implementation of a pH sensor requires precise positioning of the tip above the sample's surface. This can be achieved through different means, including qualitative and quantitative approaches. The simplest method used to place the sensor tip near the substrate is by observing it with the aid of a microscope [52][53][54]. This procedure is useful for UME diameters ≥ 10 µm. Although it provides a reasonable approximation, the true tip-to substrate distance remains unknown. For smaller UME diameters, the optical approach becomes challenging to apply. Liu et al. [34] utilized a charge-coupled device to establish the distance between the UME and the substrate. It must be noted that the methodology worked to place the tip at a far distance from the substrate (200 µm). Another simple way to position the tip is by monitoring its potential while approaching the sample and stopping when a signal "jump" is observed [55]. The main disadvantage is that the tip could be damaged and negatively affect the pH measurements.
The most popular method, by far, is the feedback mode of SECM. However, this method still has two main drawbacks: the need of a redox mediator and the convolution of topography/reactivity in the current signal. Alternatively, other methods, such as shear force (SF) sensing, alternating current-scanning electrochemical microscopy (AC-SECM), and scanning ion-conductance microscopy (SICM), have been successfully applied in the literature. These methods have been demonstrated to provide reliable strategies for fine control of the tip-to-substrate distance, and at the same time, they overcome the issues experienced by the feedback mode. Some of these methods can also be useful when imaging rough surfaces or samples with 3D geometry [56]. Although there are other positioning methods, this review presents exclusively those used alongside localized pH measurements. In the following sections, a more detailed description of each method will be presented.

Feedback Mode of Scanning Electrochemical Microscopy
Feedback mode is the native mode of SECM, which employs a three-electrode configuration: the UME as the working electrode, a reference electrode, and a counter electrode. In brief, a redox reaction occurring at the biased UME induces a steady state current when the probe is far from the substrate. The relationship between the diffusion limited steady-state current, i T,∞ , redox mediator parameters, and the geometry of the UME is described as follow [57]: where n is the number of electrons involved in the redox reaction, F is the Faraday constant, D is the diffusion coefficient of the redox mediator, C is the concentration of the redox mediator, r UME is the radius of the true electroactive surface of the UME, and b is a geometric constant that depends on the RG value of the UME (ratio between r UME and the radius of the insulting sheath, rg). For large RG values (>10), b is equal to 1. However, there is an increase in the diffusion-limited current for small RG values (RG < 10), where the b value can be calculated to account for the i T,∞ enhancement [58]. Figure 5a shows the two pure feedback cases and examples of their corresponding approach curves. The value of the current changes when the tip is close to the substrate's surface, depending on the reactivity of the latter. For example, if the UME approaches to an insulating substrate, the diffusion of the redox species is physically blocked and therefore the current decreases. On the other hand, if the UME approaches a conductive substrate, redox species are regenerated at the substrate's surface, enabling a feedback loop and thus, an increase in current. These alterations in the steady-state current are known as negative feedback (i NFB < i T,∞ ) and positive feedback (i PFB < i T,∞ ), respectively. Once the experimental approach curve is recorded, it can be fitted to analytical expressions to quantitatively establish the tip-to-substrate distance [58].
The feedback mode has been widely employed for positioning the UME prior to pH measurements [28,[35][36][37]43,48,[59][60][61][62][63][64]. There are two ways to accomplish this: one is using a single-electrode probe, whereas the other is using a dual-electrode probe. The only requirement is that the probe be able to perform both amperometric and potentiometric measurements. Examples of using a single-electrode probe include UMEs made of Sb/SbOx [59], W/WOx [63], and Pt/IrOx [43]. In order to achieve dual function in this type of UME, the oxide film must be defective to allow the redox reaction to occur at the tip [43]. Alternatively, dual-electrode probes can be used to overcome issues with using a defective film. In this case, one electrode is used in amperometric mode, whereas the other electrode is modified to work as a potentiometric pH sensor. This approach has gained popularity and is widely reported in the literature [28,35,60,62,64,65].

Shear Force Sensing
Another technique used to position the probe is so-called shear force control. This method is based on sensing the hydrodynamic forces between the oscillating probe and a surface in close proximity. The probe is stimulated through lateral vibrations (by applying an AC voltage to a piezoelectric plate) while measuring the amplitude/phase of the oscillations at a certain frequency. When the tip-to-substrate distance reaches tens to hundreds of nanometers, shear force damping occurs, and a change in the amplitude/phase is detected.
There are a few ways of measuring this shear force damping. The first method involves detecting the frequency of damping by means of a laser and split photodiode [66]. The second method involves a tuning fork fixed to the probe, with the resonance peak being sensitive to the changes in shear force [67]. Finally, the most practical method is to use two piezo crystals, one as a dither and the other as a receiver, where the latter directly measures the oscillations produced by the former [68]. Figure 5b presents the shear force setup with the dither-receiver piezo elements. In the approach curve, the amplitude value for a specific frequency sharply decreases when the tip is very close to the substrate. The greatest advantage of the shear force method is that it provides independent control of the tip-to-substrate distance, which is not affected by the electrochemical reactivity of the substrate nor the electrical properties of the probe. Therefore, both topography and pH data can be gathered simultaneously. This is very useful when employing potentiometric sensors, as they could be destabilized if current passes thought them. Therefore, coupling shear force with local pH sensing has been successfully carried out in the literature [7,[69][70][71][72][73].

Alternating Current-Scanning Electrochemical Microscopy
The use of an alternating current (AC) signal has also been applied to position SECM probes [79]. In this technique, a low-amplitude oscillating potential is imposed to the UME while its alternating current response is acquired. Therefore, the localized impedance of the system can be measured. AC-SECM works well in low-conductivity electrolytes and does not require the presence of a redox mediator. By using a low amplitude, electrochemical modification of the pH sensor can be avoided. Figure 5c shows the equivalent circuit for modeling the overall impedance response [77]: Rsol represents the solution resistance between the tip and auxiliary electrodes; Rs is the substrate's resistance; Rts is the solution resistance between the tip and the substrate; Ct is the capacitance of the tip; Cs is the capacitance of the substrate right below the tip; and Ras and Cs' are associated with the resistance and capacitance between the substrate and the auxiliary electrodes, respectively. Considering an electrolyte with low conductivity and an insulating substrate, the equivalent circuit can be simplified to Rsol in series with Ct, where Ct is considered insensitive to tip-to-substrate distance. Therefore, the impedance becomes a function of only the

Alternating Current-Scanning Electrochemical Microscopy
The use of an alternating current (AC) signal has also been applied to position SECM probes [79]. In this technique, a low-amplitude oscillating potential is imposed to the UME while its alternating current response is acquired. Therefore, the localized impedance of the system can be measured. AC-SECM works well in low-conductivity electrolytes and does not require the presence of a redox mediator. By using a low amplitude, electrochemical modification of the pH sensor can be avoided. Figure 5c shows the equivalent circuit for modeling the overall impedance response [77]: R sol represents the solution resistance between the tip and auxiliary electrodes; R s is the substrate's resistance; R ts is the solution resistance between the tip and the substrate; C t is the capacitance of the tip; C s is the capacitance of the substrate right below the tip; and R as and C s ' are associated with the resistance and capacitance between the substrate and the auxiliary electrodes, respectively. Considering an electrolyte with low conductivity and an insulating substrate, the equivalent circuit can be simplified to R sol in series with C t , where C t is considered insensitive to tipto-substrate distance. Therefore, the impedance becomes a function of only the solution resistance. The resistance in bulk solution is a function of solution resistivity, ρ, and the radius of the UME, as presented below: When the tip approaches the insulating substrate, the solution resistance increases due to blockage of the AC current pathway. By normalizing the solution resistance measured, the recorded approach curve can be fitted with negative feedback theory [79].
If the substrate is conductive, the AC current encounters an alternative pathway through the substrate. In this case, the equivalent circuit is more complex. Furthermore, if the substrate is connected to the system and held at a constant potential, the equivalent electrical circuit becomes challenging to construct [80]. Hence, the main strategy followed in literature is to approach pH sensors over an insulating region of the substrate [81][82][83][84].

Scanning Ion-Conductance Microscopy
Positioning of micropipette-based probes has been achieved using scanning ionconductance microscopy (SICM). In this approach, the ionic currents flowing between an electrode inside a micropipette and a secondary electrode placed in bulk solution are measured and used as a feedback signal [85]. Figure 5d displays the principle of operation of SICM and an example of an approach curve.
The value of the ionic current, i ∞ , depends on the applied potential, E, and the resistance of the pipette (R p ), which is a function of electrolyte conductivity and the geometric parameters of the micropipette [86]: The ion current is highly sensitive when the tip-to-substrate distance is similar to the radius of the micropipette. As the separation distance becomes smaller, the ionic conductance current sharply decreases because the flow of the ions is hindered by the proximity of the substrate. This characteristic distance-dependent ion current has been exploited to measure the topography of a wide variety of different samples [87]. One important aspect of SICM is that the resolution is mostly dependent on the size of the micropipette tip opening, which makes it relatively easy to reach the nanometer range. Combining SICM with pH sensors has enabled not only positioning of the probe, but also acquiring simultaneously topographic and pH information. For such purpose, both singlechannel [33,88] and double-channel [2,50] pipettes have been successfully demonstrated in the literature.

Other Positioning Methods
There are a couple of other positioning methods that are less commonly used than those highlighted above. The first method is the capacitive approach, which is based on determining the tip−substrate capacitance in air [89]. The main feature of this methodology is that it does not require electrolyte. In brief, an AC potential is imposed on the substrate, while the current at the UME is followed with a low-noise preamplifier, and the capacitance is calculated using a lock-in amplifier [45]. In this scenario, the tip-sample capacitance can be described as follows [89]: where ε 0 is the permittivity of air; A is the area of the UME; and d is the separation distance between the tip and substrate. When the tip gets closer to the substrate, the capacitance suddenly increases. This capacitive approach was successfully used by Monteiro et al. [45][46][47] to position a voltammetric pH sensor before measurements. The second method relies on using the concentration profile obtained experimentally and fitting it to the theoretical profile according to the substrate's geometrical and electrochemical properties [90]. The main requirement for this procedure is that the system must be in a steady state, as the fitting is calculated using Fick's second law of diffusion [91]. The other important assumption to be made is that the redox species are stable and not involved in a homogeneous reaction in solution [92]. Additionally, the tip affects the concentration profile by introducing both shielding and convection effects as it moves and gets closer to the substrate. All the aforementioned drawbacks restrict a wide application of this method.

Applications
In the previous sections, we highlighted the fabrication and positioning of micro-/nano-sized pH probes. Some recent work focusing on localized pH measurements using pH probes in the fields of biology, corrosion, energy, and the environment will be described below.

Biological Systems
pH measurements in live systems are important as even small changes at the intracellular and/or extracellular level can dramatically affect numerous biological functions. The pH can also influence the activity of microorganisms and the physiological response of the human body. The use of pH probes for localized pH measurements in biological systems has served as a powerful tool to study bacteria, human cells, and other microorganisms [2,28,37,48,64,65,88]. For example, Harris et al. [65] monitored urea hydrolysis and subsequent calcification processes induced by a Sporosarcina pasteurii biofilm in real time. It was found that the pH near the surface of the biofilm increased from 7.4 to 9.2 within 2 min, whereas the Ca 2+ concentration decreased from 85 to 10 mM within 10 min. The CaCO 3 precipitation caused an increase of 50 µm in biofilm height after 4 h. The authors concluded that bacterial enzymes promoted a fast urea hydrolysis process and that CaCO 3 formation/precipitation was the rate-limiting step.
In another study, Joshi et al. [48] evaluated the microbial metabolic exchange between two bacterial species, Streptococcus gordonii and Streptococcus mutans. It was shown that H 2 O 2 generated by S. gordonii was inhibited by the lactic acid produced by S. mutans. Figure 6a displays the application of pH sensors in 3D mapping, showing that the chemical environment was initially dominated by S. gordonii while the buffering capacity of the saliva was still valid (∼pH 6.0−7.2) and that eventually, S. mutans took control by decreasing the local pH (≤5.0). Figure 6b illustrates the investigation of pH gradients in the extracellular space of cancer cells and normal cells carried out by Munteanu et al. [37]. The authors observed that cancer cells (HT-29) subjected to hypoxia displayed a more acidic (>0.4 pH units) extracellular environment than normal (HEK-293) or normoxic cancer cells. Work conducted by Liu et al. [88] evaluated the phycosphere pH of marine microorganisms subjected to different environmental conditions. Figure 6c displays the application of a micropipette-based pH sensor to measure the phycosphere pH of single phytoplankton cells (~5 µm diameter) under consecutive light/dark cycles. It was demonstrated that the pH in the phycosphere was consistently different from that of bulk seawater, which challenged the previous assumption on both having the same pH. Zhang et al. [2] employed pH nanoprobes to measure dynamic changes in pH gradients in breast cancer MCF7 cells at the single-cell level. The authors achieved pH mapping with high spatiotemporal resolution, which revealed that the peri-cellular environments of melanoma and breast cancer cells display tumor heterogeneity.
Song et al. [28,64] and Xiong et al. [28,64] used a potentiometric dual-microelectrode to monitor the extracellular pH of MCF-7, HeLa, and HFF cells under electrical stimulation. Their studies showed that by increasing the stimulation potential, the extracellular pH decreased due to the cell membrane becoming more permeable, and that the extracellular pH of cancer cells was lower than that of normal cells. Aref et al. [93] applied a potentiometric pH nanosensor for intracellular measurements, revealing the pH gradient from the extracellular environment to the intracellular environment of a single PC12 cell, as well as variations in its intracellular pH after administration of the drug cariporide. Song et al. [28,64] and Xiong et al. [28,64] used a potentiometric dual-microelectrode to monitor the extracellular pH of MCF-7, HeLa, and HFF cells under electrical stimulation. Their studies showed that by increasing the stimulation potential, the extracellular pH decreased due to the cell membrane becoming more permeable, and that the extracellular pH of cancer cells was lower than that of normal cells. Aref et al. [93] applied a potentiometric pH nanosensor for intracellular measurements, revealing the pH gradient from the extracellular environment to the intracellular environment of a single PC12 cell, as well as variations in its intracellular pH after administration of the drug cariporide.

Corrosion
Corrosion processes involve anodic metal dissolution often accompanied by a cathodic reaction, which produces a local increase in pH. Moreover, metal ions released during corrosion may cause hydrolysis reactions and acidify the surrounding environment [94]. Consequently, it is evident that analyzing localized pH changes can help gain a better understanding of corrosion mechanisms and help to develop corrosion mitigation strategies.
The initial application of pH microsensors in corrosion research was performed with galvanic couples of pure metals, such as Zn-Fe pairs, as model systems [59,94]. In another study, Filotás et al. employed double-barrel electrode assemblies to explore galvanic corrosion of Zn-Fe [95], Zn-Cu [96], and Cu-Fe couples [97]. Figure 7a displays the reactions taking place, optical images, and the pH map of the Cu-Fe galvanic corrosion process. Further application of local pH sensing includes the evaluation of metallic coatings. Lowe et al. [98] modelled the cut edge corrosion of metallic coatings (Zn, 55% Al-Zn and solid solution Al-40% Zn) on steel. Their results showed that pH decrease caused by steel corrosion, along with the buffering effect of Al 3+ and Zn 2+ ions, impacted both the corrosion potential and cathodic current during electrochemical polarization. Etienne et al. [69] evaluated the local corrosion phenomena, the self-healing properties of an organic/metallic coating on steel, and tracked the sealing process of nanoporous alumina anodized layers [7]. In brief, the authors observed an increase in pH during metal dissolution, followed by the formation of a protective/sealing layer, and finally the consolidation of this layer indicated by the local pH value reaching the bulk pH.
Magnesium and its alloys have also been explored in biomedical applications through these pH sensors [82]. Jamali et al. studied the degradation of AZ31 [52] and AZNd coated with Pr(NO3)3 [99] in simulated body fluid. The authors found that in the case of AZ31, the interfacial pH was highly alkaline and significantly different from the bulk pH, even in a buffered solution. On the other hand, for the Pr(NO3)3 conversion

Corrosion
Corrosion processes involve anodic metal dissolution often accompanied by a cathodic reaction, which produces a local increase in pH. Moreover, metal ions released during corrosion may cause hydrolysis reactions and acidify the surrounding environment [94]. Consequently, it is evident that analyzing localized pH changes can help gain a better understanding of corrosion mechanisms and help to develop corrosion mitigation strategies.
The initial application of pH microsensors in corrosion research was performed with galvanic couples of pure metals, such as Zn-Fe pairs, as model systems [59,94]. In another study, Filotás et al. employed double-barrel electrode assemblies to explore galvanic corrosion of Zn-Fe [95], Zn-Cu [96], and Cu-Fe couples [97]. Figure 7a displays the reactions taking place, optical images, and the pH map of the Cu-Fe galvanic corrosion process. Further application of local pH sensing includes the evaluation of metallic coatings. Lowe et al. [98] modelled the cut edge corrosion of metallic coatings (Zn, 55% Al-Zn and solid solution Al-40% Zn) on steel. Their results showed that pH decrease caused by steel corrosion, along with the buffering effect of Al 3+ and Zn 2+ ions, impacted both the corrosion potential and cathodic current during electrochemical polarization. Etienne et al. [69] evaluated the local corrosion phenomena, the self-healing properties of an organic/metallic coating on steel, and tracked the sealing process of nanoporous alumina anodized layers [7]. In brief, the authors observed an increase in pH during metal dissolution, followed by the formation of a protective/sealing layer, and finally the consolidation of this layer indicated by the local pH value reaching the bulk pH.
Magnesium and its alloys have also been explored in biomedical applications through these pH sensors [82]. Jamali et al. studied the degradation of AZ31 [52] and AZNd coated with Pr(NO 3 ) 3 [99] in simulated body fluid. The authors found that in the case of AZ31, the interfacial pH was highly alkaline and significantly different from the bulk pH, even in a buffered solution. On the other hand, for the Pr(NO 3 ) 3 conversion coating on AZNd, they found that Pr +3 acted as an effective corrosion inhibitor with self-healing characteristics, taking advantage of its dynamic deposition at highly alkaline domains. Filotás et al. [61] explored the use of a multi-barrel electrode assembly to characterize the corrosion of AZ63 magnesium alloy. The authors achieved simultaneous detection of Mg 2+ ions and pH changes, avoiding at the same time the effect of the electric field developed around local anodes and cathodes. Tefashe et al. [70] described the local degradation of PEDOTcoated AZ31B Mg alloy. They measured the pH changes of a coated AZ31B/bare AZ31B couple. The authors noticed that the PEDOT coating gradually lost its initial protective ability due to localized coverage of corrosion products. Gnedenkov et al. [100] identified differences in the corrosion process of MA8 Mg alloy in 0.83% NaCl solution and MEM at the microscale level. The authors found that the local pH of MEM was stabilized over time by the formation of a hydroxyapatite layer, which decelerated the corrosion process. Figure 7b shows the distribution of currents and pH obtained using the scanning vibrating electrode technique (SVET) and scanning ion-selective electrode technique (SIET) on the MA8 alloy in cell culture medium, as well as the SEM-EDS information of the product layer.
terize the corrosion of AZ63 magnesium alloy. The authors achieved simultaneous detection of Mg 2+ ions and pH changes, avoiding at the same time the effect of the electric field developed around local anodes and cathodes. Tefashe et al. [70] described the local degradation of PEDOT-coated AZ31B Mg alloy. They measured the pH changes of a coated AZ31B/bare AZ31B couple. The authors noticed that the PEDOT coating gradually lost its initial protective ability due to localized coverage of corrosion products. Gnedenkov et al. [100] identified differences in the corrosion process of MA8 Mg alloy in 0.83% NaCl solution and MEM at the microscale level. The authors found that the local pH of MEM was stabilized over time by the formation of a hydroxyapatite layer, which decelerated the corrosion process. Figure 7b shows the distribution of currents and pH obtained using the scanning vibrating electrode technique (SVET) and scanning ion-selective electrode technique (SIET) on the MA8 alloy in cell culture medium, as well as the SEM-EDS information of the product layer.  [97]. Copyright (2016) with permission from Elsevier. (b) Localized currents and pH maps accompanied with optical and SEM images of the MA8 Mg alloy after being exposed to MEM solution Adapted from reference [100]. Copyright (2020) with permission from Elsevier. (c) Distribution of pH at the 3D-printed plate/base material boundary exposed to corrosive medium. Reprinted from reference [63]. Copyright (2020) with permission from John Wiley and Sons.
There are also other metallic materials that have been examined with pH probes. Zhu et al. explored the local pH and Fe 2+ distribution over a 316 L stainless steel surface [53,62]. They detected high concentrations of Fe 2+ at the local anode and an increase in pH values at the local cathode. These measurements allowed tracking the formation of a stable pit over the steel surface. Ramírez-Cano et al. [101] reported the pH distribution over Cu samples treated with an organic corrosion inhibitor. The authors found that the treated Cu surface displayed more alkaline pH values than the non-treated one. This behavior was attributed to the protective effect of the inhibitor, making the treated surface act as a cathode where oxygen reduction reaction took place. Asserghine et al. [55] monitored the local pH during the self-healing of the TiO2 passive layer on a Ti dental implant. They observed that during the formation of the passive layer, the pH decreased and that this process was not instantaneous, as previously assumed. Da Silva et al. [54] analyzed the distribution of reactive sites and local pH change during severe localized corrosion on 2098-T351 Al alloy. They observed that at the severe localized corrosion sites, there was lower pH, higher H2 evolution, and lower O2 consumption. More recently, additive manufacturing alloys have also been studied by means of tracking local pH changes [63,102]. Meiszterics et al. [63] investigated and compared the corrosion performance of a 3Dprinted AlMg4.5Mn0.7 Al alloy and its conventional counterpart as a substrate plate. They Figure 7. (a) Depiction of the galvanic corrosion process of a Cu-Fe pair and its associated local pH map. Adapted from ref. [97]. Copyright (2016) with permission from Elsevier. (b) Localized currents and pH maps accompanied with optical and SEM images of the MA8 Mg alloy after being exposed to MEM solution Adapted from reference [100]. Copyright (2020) with permission from Elsevier. (c) Distribution of pH at the 3D-printed plate/base material boundary exposed to corrosive medium. Reprinted from reference [63]. Copyright (2020) with permission from John Wiley and Sons.
There are also other metallic materials that have been examined with pH probes. Zhu et al. explored the local pH and Fe 2+ distribution over a 316 L stainless steel surface [53,62]. They detected high concentrations of Fe 2+ at the local anode and an increase in pH values at the local cathode. These measurements allowed tracking the formation of a stable pit over the steel surface. Ramírez-Cano et al. [101] reported the pH distribution over Cu samples treated with an organic corrosion inhibitor. The authors found that the treated Cu surface displayed more alkaline pH values than the non-treated one. This behavior was attributed to the protective effect of the inhibitor, making the treated surface act as a cathode where oxygen reduction reaction took place. Asserghine et al. [55] monitored the local pH during the self-healing of the TiO 2 passive layer on a Ti dental implant. They observed that during the formation of the passive layer, the pH decreased and that this process was not instantaneous, as previously assumed. Da Silva et al. [54] analyzed the distribution of reactive sites and local pH change during severe localized corrosion on 2098-T351 Al alloy. They observed that at the severe localized corrosion sites, there was lower pH, higher H 2 evolution, and lower O 2 consumption. More recently, additive manufacturing alloys have also been studied by means of tracking local pH changes [63,102]. Meiszterics et al. [63] investigated and compared the corrosion performance of a 3D-printed AlMg 4.5 Mn 0.7 Al alloy and its conventional counterpart as a substrate plate. They applied SECM and a W/WOx pH sensor along with conventional electrochemical measurements for such a purpose. Figure 7c presents the pH distribution over the printed material/base material boundary region and its optical image, confirming that the printed plate displayed higher corrosion resistance than the substrate material.

Energy and Environment
Measuring pH in fields like green energy production and environmental remediation can help to understand and tune the electrochemical processes involved, thus making them more efficient. Chemical solubility and reaction kinetics are affected by a change in pH, and electrocatalytic reactions can also induce a shift in the local pH values. The first attempts to determine pH changes at the electrode/electrolyte interface were for hydrogen evolution and oxygen reduction reactions. The hydrogen evolution reaction (HER) at noble metals has been used as a model system to test both potentiometric [40] and voltammetric [45] pH sensors. During HER, water is reduced and the generated OHions increase the interfacial pH: The oxygen reduction reaction (ORR) has also been used as a standard system for pH measurements [36]. As ORR occurs, the local environment becomes more alkaline due to the production of hydroxide anions: Figure 8a presents a 3D plot of the pH values at a Pt UME during ORR in aerated PBS, obtained using a voltammetric sensor [36]. Regarding energy applications, Ben Jadi et al. [103] analyzed the permeability resistance and proton conductivity of Nafion membranes modified with polypyrrole [104] and polyaniline [103] for direct methanol fuel cells. The authors measured local pH changes at the membrane/solution interface caused by the diffusion of H + through the membrane. Compared to commercial Nafion-112, the polypyrrole-modified membrane showed a decrease in proton conductivity, whereas the polyaniline-modified membrane displayed an increase in proton conductivity.

Conclusions and Outlook
In summary, there has been great interest in probing the pH at the microscale, and significant progress has been achieved in the development of miniaturized, stable, and multifunctional pH probes over the last decade. Table 1 summarizes some advanced pH sensors with their respective parameters and applications, ranging from measuring pH changes in single cells to those in biofilms, from corrosion of biomedical alloys to novel 3D-printed metal parts, and from water splitting to CO2 reduction. The sensitivity, range, and response time of pH sensors have been notably improved. The most popular type of pH sensor is the potentiometric solid microelectrode, with different versions designed by various research groups from all over the world. Ion-selective microelectrodes based on a liquid membrane cocktail are also widely used, especially for corrosion applications. Nevertheless, potentiometric sensors display a low success rate and often need recalibration. As an alternative, voltammetric sensors have attracted more attention due to their high temporal resolution and stability of the pH response. One of the main advantages of these joint efforts is that there are a wide variety of options for fabricating a micro pH sensor, which can be tailored depending on the instrumental capabilities and final applications [106][107][108]. When integrated with scanning probe methods, these pH sensors can provide information with high spatial resolution. Single measurements, diffusion/concentration For electrocatalysis, Botz et al. [71] investigated the local activities of OHand H 2 O in an operating oxygen depolarized cathode (ODC) as shown in Figure 8b. It was demonstrated that the H 2 O/OHactivity ratio was double the value in bulk solution at 1 µm above the ODC surface during ORR. The authors suggested that this drastic change in the reaction environment resulted in the switch of the reaction inside the confined pores of the working ODC.
Monteiro et al. explored changes in pH at the diffusion layer during CO electrooxidation [46] and CO 2 electrochemical reduction [47,105]. In their first work, the authors noticed that the two distinct peaks from CO oxidation voltammetry were related to the diffusion limitation of CO and OHspecies in the pH range between 7 and 11. Figure 8c shows a schematic representation of the Au/4-NTP sensor operating during CO 2 reduction to detect local pH changes in their second work. Their studies showed a time-dependent decay in the interfacial pH after CO 2 RR was stopped at the electrode, and how the species at the interface recovered their initial concentration, similar to the bulk solution.

Conclusions and Outlook
In summary, there has been great interest in probing the pH at the microscale, and significant progress has been achieved in the development of miniaturized, stable, and multifunctional pH probes over the last decade. Table 1 summarizes some advanced pH sensors with their respective parameters and applications, ranging from measuring pH changes in single cells to those in biofilms, from corrosion of biomedical alloys to novel 3D-printed metal parts, and from water splitting to CO 2 reduction. The sensitivity, range, and response time of pH sensors have been notably improved. The most popular type of pH sensor is the potentiometric solid microelectrode, with different versions designed by various research groups from all over the world. Ion-selective microelectrodes based on a liquid membrane cocktail are also widely used, especially for corrosion applications. Nevertheless, potentiometric sensors display a low success rate and often need recalibration. As an alternative, voltammetric sensors have attracted more attention due to their high temporal resolution and stability of the pH response. One of the main advantages of these joint efforts is that there are a wide variety of options for fabricating a micro pH sensor, which can be tailored depending on the instrumental capabilities and final applications [106][107][108]. When integrated with scanning probe methods, these pH sensors can provide information with high spatial resolution. Single measurements, diffusion/concentration profiles, line scans, and 3D maps are examples of the typical results that can be obtained with so-called pH microscopy. In addition, some of the positioning methods, namely shear force and SICM, can concurrently provide topographical information. On the other hand, the field of micro-sized pH sensors is relatively new, and more research & development is required to: (i) improve sensor stability, especially in extreme environments; (ii) incorporate finite element modeling to account for probe effects [109]; and (iii) enhance sensor capabilities for measuring multiple features of a system in a single experiment. It is anticipated that micro-/nano-sized pH sensors will play an important role in studying the kinetics of electrochemical reactions by monitoring local pH changes, as well as in understanding the structure-activity relationship at electrode/electrolyte interfaces.  Corrosion of biomedical grade Mg alloys [100,116,117] Galvanic corrosion in Al alloys [118][119][120] Metabolic exchange between two bacterial species [48] H + ionophore II (4-nonadecyl pyridine; ETH 1907) 1.5-20 49-59 3-9 3-10 Sealing reaction at anodized Al alloy surface.