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Developments in Electrochemistry: The PhaseShift Method and Correlation Constants for Determining the Electrochemical Adsorption Isotherms at Noble and Highly CorrosionResistant Metal/Solution Interfaces
Written By
Jinyoung Chun and Jang H. Chun
Submitted: 05 July 2012Published: 21 November 2012
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Department of Chemical Engineering, Pohang University of Science and Technology, Pohang, Kyungbuk, Republic of Korea
Jang H. Chun*
Department of Electronic Engineering, Kwangwoon University, Seoul, Republic of Korea
*Address all correspondence to: jhchun@kw.ac.kr
1. Introduction
To obtain an environmentally clean energy source, many experimental methods have been developed and used to study the adsorption of hydrogen for the cathodic H_{2} evolution reaction (HER) and hydroxide for the anodic O_{2} evolution reaction (OER) at noble and highly corrosionresistant metal and alloy/aqueous solution interfaces [1−7]. The cathodic HER is one of the most extensively studied topics in electrochemistry, electrode kinetics, renewable and sustainable energy, etc. It is well known that underpotentially deposited hydrogen (UPD H) and overpotentially deposited hydrogen (OPD H) occupy different surface adsorption sites and act as two distinguishable electroadsorbed H species, and that only OPD H can contribute to the cathodic HER [2−7]. Similarly, one can interpret that underpotentially deposited deuterium (UPD D) and overpotentially deposited deuterium (OPD D) occupy different surface adsorption sites and act as two distinguishable electroadsorbed D species, and that only OPD D can contribute to the cathodic D_{2} evolution reaction (DER). However, there is not much reliable electrode kinetic data for OPD H and OPD D, i.e. the fractional surface coverage, interaction parameter, and equilibrium constant for the Frumkin adsorption isotherm, at the interfaces. Also, a quantitative relationship between the Temkin and Frumkin or Langmuir adsorption isotherms has not been developed to study the cathodic HER and DER. Thus, there is a technological need for a useful, effective, and reliable method to determine the Frumkin, Langmuir, and Temkin adsorption isotherms of OPD H and OPD D and related electrode kinetic and thermodynamic parameters. In the following discussions, H and D mean OPD H and OPD D, respectively.
Although the electrochemical Frumkin and Langmuir adsorption isotherms may be regarded as classical models and theories, it is preferable to consider the Frumkin and Langmuir adsorption isotherms for H and D rather than electrode kinetics and thermodynamics equations for H and D because these adsorption isotherms are associated more directly with the atomic mechanisms of H and D [8]. However, there is not much reliable information on the Frumkin and Langmuir adsorption isotherms of H for the cathodic HER and related electrode kinetic and thermodynamic data [1−7]. Furthermore, there is not much reliable information on the Frumkin and Langmuir adsorption isotherms of D for the cathodic DER and related electrode kinetic and thermodynamic data. Because, to the authors’ knowledge, the interaction parameter and equilibrium constant for the Frumkin adsorption isotherm of H and D cannot be experimentally and readily determined using other conventional methods [3,7].
To determine the Frumkin, Langmuir, and Temkin adsorption isotherms, the phaseshift method and correlation constants have been originally developed on the basis of relevant experimental results and data. The phaseshift method is a unique electrochemical impedance spectroscopy technique for studying the linear relationship between the phase shift (90° ≥ −φ ≥ 0°) vs. potential (E) behavior for the optimum intermediate frequency (f_{o}) and the fractional surface coverage (0 ≤ θ ≤ 1) vs. E behavior of the intermediates (H, D, OH, OD) for the sequential reactions (HER, DER, OER) at noble and highly corrosionresistant metal and alloy/solution interfaces [9−29]. The θ vs. E behavior is well known as the Frumkin or Langmuir adsorption isotherm.
At first glance, it seems that there is no linear relationship between the −φ vs. E behavior for f_{o} and the θ vs. E behavior at the interfaces. Thus, the tedious experimental procedures presented there [e.g. 13, 16, 19−21, 27] have been used to verify or confirm the validity and correctness of the phaseshift method. This is discussed in more detail in the section on theoretical and experimental backgrounds of the phaseshift method. However, note that many scientific phenomena have been interpreted by their behavior rather than by their nature. For example, the wave−particle duality of light and electrons, i.e. their wave and particle behaviors, is well known in science and has been applied in engineering. To explain the photoelectric effect of light, the behavior of light is interpreted as a particle, i.e. a photon, on the basis of the observed phenomena or the measured experimental data. Note that the nature of light is a wave. Similarly, to explain the tunneling effect of electrons, the behavior of electrons is interpreted as a wave on the basis of the observed phenomena or the measured experimental data. Note that the nature of the electron is a real particle, which has a negative charge and a mass. Notably, these wave and particle behaviors are complementary rather than contradictory to each other.
The comments and replies on the phaseshift method are described elsewhere [30−34]. New ideas or methods must be rigorously tested, especially when they are unique, but only with pure logic and objectivity and through scientific procedures. However, the objections to the phaseshift method do not fulfill these criteria. The objections to the phaseshift method are substantially attributed to a misunderstanding of the phaseshift method itself [27, 28]. Note especially that all of the objections to the phaseshift method can be attributed to confusion regarding the applicability of related impedance equations for intermediate frequencies and a unique feature of the faradaic resistance for the recombination step [35]. The validity and correctness of the phaseshift method should be discussed on the basis of numerical simulations with a single equation for −φ vs. θ as functions of E and frequency (f) or relevant experimental data which are obtained using other conventional methods. The lack of the single equation for −φ vs. θ as functions of E and f and use of incorrect values of the electrode kinetic parameters or the equivalent circuit elements for the numerical simulations given in the comments result in the confused conclusions on the phaseshift method.
In practice, the numerical calculation of equivalent circuit impedances of the noble and highly corrosionresistant metal and alloy/solution interfaces is very difficult or impossible due to the superposition of various effects. However, it is simply determined by frequency analyzers, i.e. tools. Note that the phaseshift method and correlation constants are useful and effective tools for determining the Frumkin, Langmuir, and Temkin adsorption isotherms and related electrode kinetic and thermodynamic parameters.
This work is one of our continuous studies on the phaseshift method and correlation constants for determining the Frumkin, Langmuir, and Temkin adsorption isotherms. In this paper, as a selected example of the phaseshift method and correlation constants for determining the electrochemical adsorption isotherms, we present the Frumkin and Temkin adsorption isotherms of (H + D) for the cathodic (HER + DER) and related electrode kinetic and thermodynamic parameters of a Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface. These experimental results are compared with the relevant experimental data of the noble and highly corrosionresistant metal and alloy/solution interfaces [11, 13, 16, 19−21, 23−29]. The interaction parameters, equilibrium constants, standard Gibbs energies of adsorptions, and rates of change of the standard Gibbs energies with θ for the Frumkin, Langmuir, and Temkin adsorption isotherms of H, D, (H + D), OH, and (OH + OD) are summarized and briefly discussed.
Taking into account the H^{+} and D^{+} concentrations [27] and the effects of the diffusedouble layer and pH [36], a mixture (1:1 volume ratio) of 0.1 M LiOH (H_{2}O) and 0.1 M LiOH (D_{2}O) solutions, i.e. 0.1 M LiOH (H_{2}O + D_{2}O) solution, was prepared from LiOH (Alfa Aesar, purity 99.995%) using purified water (H_{2}O, resistivity > 18 MΩ · cm) obtained from a Millipore system and heavy water (D_{2}O, Alfa Aesar, purity 99.8%). The p(H + D) of 0.1 M LiOH (H_{2}O + D_{2}O) solution was 12.91. This solution was deaerated with 99.999% purified nitrogen gas for 20 min before the experiments.
A standard threeelectrode configuration was employed. A saturated calomel electrode (SCE) was used as the standard reference electrode. A platinum−iridium alloy wire (Johnson Matthey, 90:10 Pt/Ir mass ratio, 1.5 mm diameter, estimated surface area ca. 1.06 cm^{2}) was used as the working electrode. A platinum wire (Johnson Matthey, purity 99.95%, 1.5 mm diameter, estimated surface area ca. 1.88 cm^{2}) was used as the counter electrode. Both the Pt−Ir alloy working electrode and the Pt counter electrode were prepared by flame cleaning and then quenched and cooled sequentially in Millipore MilliQ water and air.
2.2. Measurements
A cyclic voltammetry (CV) technique was used to achieve a steady state at the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface. The CV experiments were conducted for 20 cycles at a scan rate of 200 mV · s^{−1} and a scan potential of (0 to −1.0) V vs. SCE. After the CV experiments, an electrochemical impedance spectroscopy (EIS) technique was used to study the linear relationship between the −φ vs. E behavior of the phase shift (90° ≥ −φ ≥ 0°) for the optimum intermediate frequency (f_{o}) and the θ vs. E behavior of the fractional surface coverage (0 ≤ θ ≤ 1). The EIS experiments were conducted at scan frequencies (f) of (10^{4} to 0.1) Hz using a single sine wave, an alternating current (ac) amplitude of 5 mV, and a direct current (dc) potential of (0 to −1.20) V vs. SCE.
The CV experiments were performed using an EG&G PAR Model 273A potentiostat controlled with the PAR Model 270 software package. The EIS experiments were performed using the same apparatus in conjunction with a Schlumberger SI 1255 HF frequency response analyzer controlled with the PAR Model 398 software package. To obtain comparable and reproducible results, all of the measurements were carried out using the same preparations, procedures, and conditions at 298 K. The international sign convention is used: cathodic currents and laggedphase shifts or angles are taken as negative. All potentials are given on the standard hydrogen electrode (SHE) scale. The Gaussian and adsorption isotherm analyses were carried out using the Excel and Origin software packages.
3.1. Theoretical and experimental backgrounds of the phaseshift method
The equivalent circuit for the adsorption of (H + D) for the cathodic (HER + DER) at the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface can be expressed as shown in Fig. 1a [27, 28, 37−39]. Taking into account the superposition of various effects (e.g. a relaxation time effect, a real surface area problem, surface absorption and diffusion processes, inhomogeneous and lateral interaction effects, an oxide layer formation, specific adsorption effects, etc.) that are inevitable under the experimental conditions, we define the equivalent circuit elements as follows: R_{S} is the real solution resistance; R_{F} is the real resistance due to the faradaic resistance (R_{ϕ}) for the discharge step and superposition of various effects; R_{P} is the real resistance due to the faradaic resistance (R_{R}) for the recombination step and superposition of various effects; C_{P} is the real capacitance due to the adsorption pseudocapacitance (C_{ϕ}) for the discharge step and superposition of various effects; and C_{D} is the real doublelayer capacitance. Correspondingly, neither R_{F} nor C_{P} is constant; both depend on E and θ and can be measured. Note that both R_{ϕ} and C_{ϕ} also depend on E and θ but cannot be measured.
The numerical derivation of C_{ϕ} from the Frumkin and Langmuir adsorption isotherms (θ vs. E) is described elsewhere, and R_{ϕ} depends on C_{ϕ} [37,39]. A unique feature of R_{ϕ} and C_{ϕ} is that they attain maximum values at θ ≈ 0.5 and intermediate E, decrease symmetrically with E at other values of θ, and approach minimum values or 0 at θ ≈ 0 and low E and θ ≈ 1 and high E; this behavior is well known in interfacial electrochemistry, electrode kinetics, and EIS. The unique feature and combination of R_{ϕ} and C_{ϕ} vs. E imply that the normalized rate of change of −φ with respect to E, i.e. Δ(−φ)/ΔE, corresponds to that of θ vs. E, i.e. Δθ/ΔE, and vice versa (see footnotes in Table 1). Both Δ(−φ)/ΔE and Δθ/ΔE are maximized at θ ≈ 0.5 and intermediate E, decrease symmetrically with E at other values of θ, and are minimized at θ ≈ 0 and low E and θ ≈ 1 and high E. Notably, this is not a mere coincidence but rather a unique feature of the Frumkin and Langmuir adsorption isotherms (θ vs. E). The linear relationship between and Gaussian profiles of −φ vs. E or Δ(−φ)/ΔE and θ vs. E or Δθ/ΔE most clearly appear at f_{o}. The value of f_{o} is experimentally and graphically evaluated on the basis of Δ(−φ)/ΔE and Δθ/ΔE for intermediate and other frequencies (see Figs. 3 to 5). The importance of f_{o} is described elsewhere [21]. These aspects are the essential nature of the phaseshift method for determining the Frumkin and Langmuir adsorption isotherms.
The frequency responses of the equivalent circuit for all f that is shown in Fig. 1a are essential for understanding the unique feature and combination of (R_{S}, R_{F}) and (C_{P}, C_{D}) vs. E for f_{o}, i.e. the linear relationship between the −φ vs. E behavior for f_{o} and the θ vs. E behavior. At intermediate frequencies, one finds regions in which the equivalent circuit for all f behaves as a series circuit of R_{S}, R_{F}, and C_{P} or a series and parallel circuit of R_{S}, C_{P}, and C_{D}, as shown in Fig. 1 b. However, note that the simplified equivalent circuits shown in Fig. 1b do not represent the change of the cathodic (HER + DER) itself but only the intermediate frequency responses.
At intermediate frequencies, the impedance (Z) and lagged phaseshift (−φ) are given by [27−29]
for the lower circuit in Fig. 1b, where j is the imaginary unit (i.e. j^{2} = −1) and ω is the angular frequency, defined as ω = 2πf, where f is the frequency. Under these conditions,
RP>> 1/ωCP and RP>>RS+RFE3
In our previous papers [9−24], only Eq. (1) was used with a footnote stating that C_{P} practically includes C_{D} (see Tables 1 and 2 in Ref. 20, Table 1 in Ref. 19, etc.). Both Eqs. (1) and (2) show that the effect of R_{P} on −φ for intermediate frequencies is negligible. These aspects are completely overlooked, confused, and misunderstood in the comments on the phaseshift method by HorvatRadosevic et al. [30,32,34]. Correspondingly, all of the simulations of the phaseshift method using Eq. (1) that appear in these comments (where C_{P} does not include C_{D}) [30,32,34] are basically invalid or wrong [27,28]. All of the analyses of the effect of R_{P} on −φ for intermediate frequencies are also invalid or wrong (see Supporting Information of Refs. 27 and 28).
The following limitations and conditions of the equivalent circuit elements for f_{o} are summarized on the basis of the experimental data in our previous papers [9−29]. Neither R_{S} nor C_{D} is constant. At θ ≈ 0, R_{S} > R_{F} and C_{D} > C_{P}, or vice versa, and so forth. For a wide range of θ (i.e. 0.2 < θ < 0.8), R_{F} >> R_{S} orR_{F} > R_{S} and C_{P} >> C_{D} or C_{P} > C_{D}, and so forth. At θ ≈ 1, R_{S} > R_{F} or R_{S} < R_{F} and C_{P} >> C_{D}. The measured −φ for f_{o} depends on E and θ. In contrast to the numerical simulations, the limitations and conditions for Eq. (1) or (2) are not considered for the phaseshift method because all of the measured values of −φ for intermediate frequencies include (R_{S}, R_{F}) and (C_{P}, C_{D}). Correspondingly, the measured −φ for f_{o} is valid and correct regardless of the applicability of Eq. (1) or (2). Both the measured values of −φ at f_{o} and the calculated values of −φ at f_{o} using Eq. (1) or (2) are exactly the same (see Supporting Information in Refs. 27 and 28). The unique feature and combination of (R_{S}, R_{F}) and (C_{P}, C_{D}) are equivalent to those of R_{ϕ} and C_{ϕ}. This is attributed to the reciprocal property of R_{F} and C_{P} vs. E and suggests that only the polar form of the equivalent circuit impedance, i.e. −φ described in Eq. (1b) or (2b), is useful and effective for studying the linear relationship between the −φ (90° ≥ −φ ≥ 0°) vs. E behavior at f_{o} and the θ (0 ≤ θ ≤ 1) vs. E behavior. Note that the phaseshift method for determining the electrochemical (Frumkin, Langmuir, Temkin) adsorption isotherms has been proposed and verified on the basis of the phaseshift curves (−φ vs. log f) at various E (see Fig. 2). The unique feature and combination of (R_{S}, R_{F}) and (C_{P}, C_{D}) vs. E, i.e. −φ vs. E or Δ(−φ)/ΔE and θ vs. E or Δθ/ΔE, most clearly appear at f_{o}. The linear relationship between and Gaussian profiles of −φ vs. E or Δ(−φ)/ΔE and θ vs. E or Δθ/ΔE for f_{o} imply that only one Frumkin or Langmuir adsorption isotherm is determined on the basis of relevant experimental results (see Figs. 3 to 5). The shape and location of the −φ vs. E or Δ(−φ)/ΔE profile for f_{o} and the θ vs. E or Δθ/ΔE profile correspond to the interaction parameter (g) and equilibrium constant (K_{o}) for the Frumkin or Langmuir adsorption isotherm, respectively. These aspects have been experimentally and consistently verified or confirmed in our previous papers [9−29].
3.2. Basic procedure and description of the phaseshift method
Note that the following description of the phaseshift method for determining the Frumkin adsorption isotherm is similar to our previous papers due to use of the same method and procedures [27,28].
Figure 2 compares the phaseshift curves (−φ vs. log f) for different E at the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface. As shown in Fig. 2, −φ depends on both f and E [37−39]. Correspondingly, the normalized rate of change of −φ vs. E, i.e. Δ(−φ)/ΔE, depends on both f and E. In electrosorption, θ depends on only E [40]. The normalized rate of change of θ vs. E, i.e. Δθ/ΔE, obeys a Gaussian profile. This is a unique feature of the Frumkin and Langmuir adsorption isotherms (θ vs. E).
The intermediate frequency of 1.259 Hz, shown as a vertical solid line on the −φ vs. log f plot in Fig. 2, can be set as f_{o} for −φ vs. E and θ vs. E profiles. The determination of f_{o} is experimentally and graphically evaluated on the basis of Δ(−φ)/ΔE and Δθ/ΔE for intermediate and other frequencies (see Figs. 3 and 4). At the maximum −φ shown in curve a of Fig. 2, it appears that the adsorption of (H + D) and superposition of various effects are minimized; i.e. θ ≈ 0 and E is low. Note that θ (0 ≤ θ ≤ 1) depends only on E. At the maximum −φ, when θ ≈ 0 and E is low, both Δ(−φ)/ΔE and Δθ/ΔE are minimized because R_{ϕ} and C_{ϕ} approach minimum values or 0. At the minimum −φ, shown in curve k of Fig. 2, it appears that the adsorption of (H + D) and superposition of various effects are maximized or almost saturated; i.e. θ ≈ 1 and E is high. At the minimum −φ, when θ ≈ 1 and E is high, both Δ(−φ)/ΔE and Δθ/ΔE are also minimized because R_{ϕ} and C_{ϕ} approach minimum values or 0. At the medium −φ between curves d and e in Fig. 2, it appears that both Δ(−φ)/ΔE and Δθ/ΔE are maximized because R_{ϕ} and C_{ϕ} approach maximum values at θ ≈ 0.5 and intermediate E (see Table 1 and Fig. 4b). If one knows the three points or regions, i.e. the maximum −φ (θ ≈ 0 and low E region, where Δ(−φ)/ΔE and Δθ/ΔE approach the minimum value or 0), the medium −φ (θ ≈ 0.5 and intermediate E region, where Δ(−φ)/ΔE and Δθ/ΔE approach the maximum value), and the minimum −φ (θ ≈ 1 and high E region, where Δ(−φ)/ΔE and Δθ/ΔE approach the minimum value or 0) for f_{o}, then one can easily determine the object, i.e. the Frumkin or Langmuir adsorption isotherm. In other words, both Δ(−φ)/ΔE and Δθ/ΔE for f_{o} are maximized at θ ≈ 0.5 and intermediate E, decrease symmetrically with E at other values of θ, and are minimized at θ ≈ 0 and low E and θ ≈ 1 and high E (see Table 1 and Fig. 4b). As stated above, this is a unique feature of the Frumkin and Langmuir adsorption isotherms. The linear relationship between and Gaussian profiles of −φ vs. E or Δ(−φ)/ΔE and θ vs. E or Δθ/ΔE most clearly appear at f_{o}.
Measured values of the phase shift (−φ) for the optimum intermediate frequency (f_{o} = 1.259 Hz), the fractional surface coverage (θ) of (H + D), and the normalized rates of change of −φ and θ vs. E (i.e. Δ(−φ)/ΔE, Δθ/ΔE) at the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface
The procedure and description of the phaseshift method for determining the Frumkin adsorption isotherm of (H + D) at the interface are summarized in Table 1. The values of −φ and θ as a function of E at f_{o} = 1.259 Hz shown in Fig. 3 are illustrated on the basis of the experimental results summarized in Table 1. The values of −φ and θ as a function of E at f = 0.1 Hz, 10 Hz, and 100 Hz shown in Fig. 3 are also illustrated through the same procedure summarized in Table 1. However, note that the differences between the −φ vs. E profile at f_{o} = 1.259 Hz and the −φ vs. E profiles at f = 0.1 Hz, 10 Hz, and 100 Hz shown in Fig. 3a do not represent the measurement error but only the frequency response. In practice, the θ vs. E profiles at f = 0.1 Hz, 10 Hz, and 100 Hz shown in Fig. 3b should be exactly the same as the θ vs. E profile at f_{o} = 1.259 Hz. Because, as stated above, θ depends on only E and this unique feature most clearly appears at f_{o}. This is the reason why the comparison of −φ and θ vs. E profiles for different frequencies shown in Fig. 3 is necessary to determine f_{o}.
The Gaussian profile shown in Fig. 4b is illustrated on the basis of Δ(−φ)/ΔE and Δθ/ΔE data for f_{o} = 1.259 Hz summarized in Table 1. Figure 4b shows that both Δ(−φ)/ΔE and Δθ/ΔE are maximized at θ ≈ 0.5 and intermediate E, decrease symmetrically with E at other values of θ, and are minimized at θ ≈ 0 and low E and θ ≈ 1 and high E. The Gaussian profiles for f = 0.1 Hz, 10 Hz, and 100 Hz shown in Fig. 4 were obtained through the same procedure summarized in Table 1. Finally, one can conclude that the θ vs. E profile at f_{o} = 1.259 Hz shown in Fig. 3b is applicable to the determination of the Frumkin adsorption isotherm of (H + D) at the interface. As stated above, the shape and location of the −φ vs. E or Δ(−φ)/ΔE profile and the θ vs. E or Δθ/ΔE profile for f_{o} correspond to g and K_{o} for the Frumkin adsorption isotherm, respectively.
3.3. Frumkin, Langmuir, and Temkin adsorption isotherms
The derivation and interpretation of the practical forms of the electrochemical Frumkin, Langmuir, and Temkin adsorption isotherms are described elsewhere [41−43]. The Frumkin adsorption isotherm assumes that the Pt−Ir alloy surface is inhomogeneous or that the lateral interaction effect is not negligible. It is well known that the Langmuir adsorption isotherm is a special case of the Frumkin adsorption isotherm. The Langmuir adsorption isotherm can be derived from the Frumkin adsorption isotherm by setting the interaction parameter to be zero. The Frumkin adsorption isotherm of (H + D) can be expressed as follows [42]
[θ/(1 −θ)] exp(gθ)=KoC+exp(−EF/RT)E4
g=r/RTE5
K=Koexp(−gθ)E6
where θ (0 ≤ θ ≤ 1) is the fractional surface coverage, g is the interaction parameter for the Frumkin adsorption isotherm, K_{o} is the equilibrium constant at g = 0, C^{+} is the concentration of ions (H^{+}, D^{+}) in the bulk solution, E is the negative potential, F is Faraday’s constant, R is the gas constant, T is the absolute temperature, r is the rate of change of the standard Gibbs energy of (H + D) adsorption with θ, and K is the equilibrium constant. The dimension of K is described elsewhere [44]. Note that when g = 0 in Eqs. (4) to (6), the Langmuir adsorption isotherm is obtained. For the Langmuir adsorption isotherm, when g = 0, the inhomogeneous and lateral interaction effects on the adsorption of (H + D) are assumed to be negligible.
At the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface, the numerically calculated Frumkin adsorption isotherms using Eq. (4) are shown in Fig. 5. Curves a, b, and c in Fig. 5 show the three numerically calculated Frumkin adsorption isotherms of (H + D) corresponding to g = 0, −2.2, and −5.5, respectively, for K_{o} = 5.3 × 10^{−5} mol^{−1}. The curve b shows that the Frumkin adsorption isotherm, K = 5.3 × 10^{−5} exp(2.2θ) mol^{−1}, is applicable to the adsorption of (H + D), and Eq. (5) gives r = −5.5 kJ · mol^{−1}. The Frumkin adsorption isotherm implies that the lateral interaction between the adsorbed (H + D) species is not negligible. In other words, the Langmuir adsorption isotherm for g = 0, i.e. K = 5.3 × 10^{−5} mol^{−1}, is not applicable to the adsorption of (H + D) at the interface (see Fig. 8).
At intermediate values of θ (i.e. 0.2 < θ < 0.8), the preexponential term, [θ/(1 − θ)], varies little with θ in comparison with the variation of the exponential term, exp(gθ). Under these approximate conditions, the Temkin adsorption isotherm can be simply derived from the Frumkin adsorption isotherm. The Temkin adsorption isotherm of (H + D) can be expressed as follows [42]
exp(gθ)=KoC+exp(−EF/RT)E7
Figure 6 shows the determination of the Temkin adsorption isotherm corresponding to the Frumkin adsorption isotherm shown in curve b of Fig. 5. The dashed line labeled b in Fig. 6 shows that the numerically calculated Temkin adsorption isotherm of (H + D) using Eq. (7) is K = 5.3 × 10^{−4} exp(−2.4θ) mol^{−1}, and Eq. (5) gives r = 6.0 kJ · mol^{−1}. The values of g and K for the Frumkin and Temkin adsorption isotherms of H, D, (H + D), OH, and (OH + OD) at the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces are summarized in Tables 2 and 3, respectively.
3.4. Applicability of the Frumkin, Langmuir, and Temkin adsorption isotherms
Figure 7 shows the applicability of ranges of θ, which are estimated using the measured phase shift (−φ) shown in Table 1, for the Frumkin adsorption isotherm at the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface. Fig. 7 also shows that the phaseshift method for determining the Frumkin adsorption isotherm (θ vs. E) is valid, effective, and reasonable at 0 ≤ θ ≤ 1.
Figures 8 and 9 show the applicability of the Langmuir and Temkin adsorption isotherms at the same potential ranges, respectively. Figs. 8 and 9 also show that the Langmuir and Temkin adsorption isotherms are not applicable to the adsorption of (H + D) at the interface.
At extreme values of θ, i.e. θ ≈ 0 and 1, the Langmuir adsorption isotherm is often applicable to the adsorption of intermediates [42]. However, as shown in Figs. 8b and c, the validity and correctness of the Langmuir adsorption isotherm are unclear and limited even at θ ≈ 0 and 1. As stated in the introduction, the value of g for the Frumkin adsorption isotherm is not experimentally and consistently determined using other conventional methods. This is the reason why the Langmuir adsorption isotherm is often used even though it has the critical limitation and applicability. On the other hand, the Temkin adsorption isotherm is only valid and effective at 0.2 < θ < 0.8 (see Fig. 6). Note that the short potential range (ca. 37 mV) is difficult to observe in the Temkin adsorption isotherm correlating with the Frumkin adsorption isotherm. At other values of θ, i.e. 0 ≤ θ < 0.2 and 0.8 < θ ≤ 1, only the Frumkin adsorption isotherm is applicable to the adsorption of (H + D). Finally, one can conclude that the Frumkin adsorption isotherm is more useful, effective, and reliable than the Langmuir and Temkin adsorption isotherms at the interface.
interface
adsorbate
g
K/mol^{−1 }
Ref.
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O+D_{2}O)
H+D
−2.2
5.3 × 10^{−5 }exp(2.2θ)
−
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
H
−2.2
8.6 × 10^{−5 }exp(2.2θ)
27
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
D
−2.3
2.1 × 10^{−5 }exp(2.3θ)
27
Pt−Ir alloy^{a}/0.5 M H_{2}SO_{4} (H_{2}O)
H
−2.5
3.3 × 10^{−5 }exp(2.5θ)
28
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
OH
0.6
5.4 × 10^{−9 }exp(−0.6θ)
26
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
OH+OD
2.7
3.9 × 10^{−9 }exp(−2.7θ)
26
Pt−Ir alloy^{b}/0.5 M H_{2}SO_{4} (H_{2}O)
H
−2.5
3.1 × 10^{−5 }exp(2.5θ)
20
Pt−Ir alloy^{b}/0.1 M KOH (H_{2}O)
OH
1.8
4.7 × 10^{−10 }exp(−1.8θ)
20
Pt/0.1 M KOH (H_{2}O)
H
−2.4
1.2 × 10^{−4 }exp(2.4θ)
25
Pt/0.5 M H_{2}SO_{4} (H_{2}O)
H
−2.4
3.5 × 10^{−5 }exp(2.4θ)
21
Ir/0.1 M KOH (H_{2}O)
H
−2.4
9.4 × 10^{−5 }exp(2.4θ)
25
Ir/0.5 M H_{2}SO_{4} (H_{2}O)
H
−2.4
2.7 × 10^{−5 }exp(2.4θ)
21
Pd/0.5 M H_{2}SO_{4} (H_{2}O)
H
1.4
3.3 × 10^{−5 }exp(−1.4θ)
19
Au/0.5 M H_{2}SO_{4} (H_{2}O)
H
0^{e}
2.3 × 10^{−6}
13
Re/0.1 M KOH (H_{2}O)
H
0^{e}
1.9 × 10^{−6}
16
Re/0.5 M H_{2}SO_{4} (H_{2}O)
H
0^{e}
4.5 × 10^{−7}
16
Ni^{c}/0.05 M KOH (H_{2}O)
H
10
1.3 × 10^{−1 }exp(−10θ)
11
Ni^{d}/0.1 M LiOH (H_{2}O)
H
7.4
3.6 × 10^{−4 }exp(−7.4θ)
29
Ni^{d}/0.5 M H_{2}SO_{4} (H_{2}O)
H
5.3
4.1 × 10^{−9 }exp(−5.3θ)
29
Ti/0.5 M H_{2}SO_{4} (H_{2}O)
H
6.6
8.3 × 10^{−12 }exp(−6.6θ)
23
Zr/0.2 M H_{2}SO_{4} (H_{2}O)
H
3.5
1.4 × 10^{−17 }exp(−3.5θ)
24
Table 2.
^{a} Pt−Ir (90:10 mass ratio) alloy. ^{b} Pt−Ir (70:30 mass ratio) alloy. ^{c} Ni (purity 99.994%) foil. ^{d} Ni (purity 99.999%) wire. ^{e} Langmuir adsorption isotherm.
Comparison of the interaction parameters (g) and equilibrium constants (K) for the Frumkin adsorption isotherms at the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces
interface
adsorbate
g
K/mol^{−1 }
Ref.
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O+D_{2}O)
H+D
2.4
5.3 × 10^{−4 }exp(−2.4θ)
−
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
H
2.4
8.6 × 10^{−4 }exp(−2.4θ)
27
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
D
2.3
2.1 × 10^{−4 }exp(−2.3θ)
27
Pt−Ir alloy^{a}/0.5 M H_{2}SO_{4} (H_{2}O)
H
2.1
3.3 × 10^{−4 }exp(−2.1θ)
28
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
OH
5.2
5.4 × 10^{−8 }exp(−5.2θ)
26
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
OH+OD
7.3
3.9 × 10^{−8 }exp(−7.3θ)
26
Pt−Ir alloy^{b}/0.5 M H_{2}SO_{4} (H_{2}O)
H
2.1
3.1 × 10^{−4 }exp(−2.1θ)
20
Pt−Ir alloy^{b}/0.1 M KOH (H_{2}O)
OH
6.4
4.7 × 10^{−9 }exp(−6.4θ)
20
Pt/0.1 M KOH (H_{2}O)
H
2.2
1.2 × 10^{−3 }exp(−2.2θ)
25
Pt/0.5 M H_{2}SO_{4} (H_{2}O)
H
2.2
3.5 × 10^{−4 }exp(−2.2θ)
21
Ir/0.1 M KOH (H_{2}O)
H
2.2
9.4 × 10^{−4 }exp(−2.2θ)
25
Ir/0.5 M H_{2}SO_{4} (H_{2}O)
H
2.2
2.7 × 10^{−4 }exp(−2.2θ)
21
Pd/0.5 M H_{2}SO_{4} (H_{2}O)
H
6
3.3 × 10^{−4 }exp(−6θ)
19
Au/0.5 M H_{2}SO_{4} (H_{2}O)
H
4.6
2.3 × 10^{−5 }exp(−4.6θ)
13
Re/0.1 M KOH (H_{2}O)
H
4.6
1.9 × 10^{−5 }exp(−4.6θ)
16
Re/0.5 M H_{2}SO_{4} (H_{2}O)
H
4.6
4.5 × 10^{−6 }exp(−4.6θ)
16
Ni^{c}/0.05 M KOH (H_{2}O)
H
14.6
1.3 exp(−14.6θ)
11
Ni^{d}/0.1 M LiOH (H_{2}O)
H
12
3.6 × 10^{−3 }exp(−12θ)
29
Ni^{d}/0.5 M H_{2}SO_{4} (H_{2}O)
H
9.9
4.1 × 10^{−8 }exp(−9.9θ)
29
Ti/0.5 M H_{2}SO_{4} (H_{2}O)
H
11.2
8.3 ×10^{−11 }exp(−11.2θ)
23
Zr/0.2 M H_{2}SO_{4} (H_{2}O)
H
8.1
1.4 × 10^{−16 }exp(−8.1θ)
24
Table 3.
^{a} Pt−Ir (90:10 mass ratio) alloy. ^{b} Pt−Ir (70:30 mass ratio) alloy. ^{c} Ni (purity 99.994%) foil. ^{d} Ni (purity 99.999%) wire.
Comparison of the interaction parameters (g) and equilibrium constants (K) for the Temkin adsorption isotherms at the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces
3.5. Standard Gibbs energy of adsorption
Under the Frumkin adsorption conditions, the relationship between the equilibrium constant (K) for (H + D) and the standard Gibbs energy (∆G_{θ}^{○}) of (H + D) adsorption is [42]
2.3RTlogK=−ΔGθ○E8
For the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface, use of Eqs. (6) and (8) shows that ∆G_{θ}^{○} is in the range (24.4 ≥ ∆G_{θ}^{○} ≥ 18.9) kJ · mol^{−1} for K = 5.3 × 10^{−5} exp(2.2θ) mol^{−1} and 0 ≤ θ ≤ 1. This result implies an increase in the absolute value of ∆G_{θ}^{○}, i.e. ∆G_{θ}^{○}, with θ. Note that ∆G_{θ}^{○} is a negative number, i.e. ∆G_{θ}^{○} < 0 [42]. The values of ∆G_{θ}^{○} and r for the Frumkin and Temkin adsorption isotherms at the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces are summarized in Tables 4 and 5, respectively.
Curves a, b, and c in Fig. 10 show the K vs. θ behaviors of H, (H + D), and D at the Pt−Ir alloy/0.1 M LiOH (H_{2}O), 0.1 M LiOH (H_{2}O + D_{2}O), and 0.1 M LiOH (D_{2}O) solution interfaces, respectively [27]. In Fig. 10, the value of K for (H + D) is approximately equal to the average value of K for H and D isotopes. The value of K for (H + D) decreases with increasing D_{2}O. In other words, the value of K decreases in going from H_{2}O to D_{2}O. Over the θ range (i.e. 1 ≥ θ ≥ 0), the value of K for H is approximately 3.7 to 4.1 times greater than that for D (see Table 2). As shown in Tables 2 and 4, the values of g, K, ∆G_{θ}^{○}, and r for the Frumkin adsorption isotherms of H, (H + D), and D are readily distinguishable using the phaseshift method. Fig. 10 also shows that the kinetic isotope effect, i.e. the ratio of rate constants of H and D or equilibrium constants of H and D, is readily determined using the phaseshift method (also see Table 2) [45]. Note that the kinetic isotope effect is widely used and applied in electrochemistry, surface science, biochemistry, chemical geology, physics, etc.
interface
adsorbate
∆G_{θ}^{○}/kJ·mol^{−1}
r/kJ·mol^{−1}
Ref.
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O+D_{2}O)
H+D
24.4 ≥ ∆G_{θ}^{○ }≥ 18.9
−5.5
−
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
H
23.2 ≥ ∆G_{θ}^{○ }≥ 17.7
−5.5
27
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
D
26.7 ≥ ∆G_{θ}^{○ }≥ 21.0
−5.7
27
Pt−Ir alloy^{a}/0.5 M H_{2}SO_{4} (H_{2}O)
H
25.6 ≥ ∆G_{θ}^{○ }≥ 19.4
−6.2
28
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
OH
47.2 ≤ ∆G_{θ}^{○ }≤ 48.6
1.5
26
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
OH+OD
48.0 ≤ ∆G_{θ}^{○ }≤54.7
6.7
26
Pt−Ir alloy^{b}/0.5 M H_{2}SO_{4} (H_{2}O)
H
25.7 ≥ ∆G_{θ}^{○ }≥ 19.5
−6.2
20
Pt−Ir alloy^{b}/0.1 M KOH (H_{2}O)
OH
53.2 ≤ ∆G_{θ}^{○ }≤57.7
4.5
20
Pt/0.1 M KOH (H_{2}O)
H
22.4 ≥ ∆G_{θ}^{○ }≥ 16.5
−6.0
25
Pt/0.5 M H_{2}SO_{4} (H_{2}O)
H
25.4 ≥ ∆G_{θ}^{○ }≥ 19.5
−6.0
21
Ir/0.1 M KOH (H_{2}O)
H
23.0 ≥ ∆G_{θ}^{○ }≥ 17.1
−6.0
25
Ir/0.5 M H_{2}SO_{4} (H_{2}O)
H
26.1 ≥ ∆G_{θ}^{○ }≥ 20.1
−6.0
21
Pd/0.5 M H_{2}SO_{4} (H_{2}O)
H
25.6 ≤ ∆G_{θ}^{○ }≤ 29.0
3.5
19
Au/0.5 M H_{2}SO_{4} (H_{2}O)
H
32.2
0^{e}
13
Re/0.1 M KOH (H_{2}O)
H
32.6
0^{e}
16
Re/0.5 M H_{2}SO_{4} (H_{2}O)
H
36.2
0^{e}
16
Ni^{c}/0.05 M KOH (H_{2}O)
H
5.1 ≤ ∆G_{θ}^{○ }≤ 29.8
24.8
11
Ni^{d}/0.1 M LiOH (H_{2}O)
H
19.6 ≤ ∆G_{θ}^{○ }≤ 38.0
18.4
29
Ni^{d}/0.5 M H_{2}SO_{4} (H_{2}O)
H
47.8 ≤ ∆G_{θ}^{○ }≤ 61.0
13.1
29
Ti/0.5 M H_{2}SO_{4} (H_{2}O)
H
63.2 ≤ ∆G_{θ}^{○ }≤ 79.6
16.4
23
Zr/0.2 M H_{2}SO_{4} (H_{2}O)
H
96.1 ≤ ∆G_{θ}^{○ }≤ 104.8
8.7
24
Table 4.
^{a} Pt−Ir (90:10 mass ratio) alloy. ^{b} Pt−Ir (70:30 mass ratio) alloy. ^{c} Ni (purity 99.994%) foil. ^{d} Ni (purity 99.999%) wire. ^{e} Langmuir adsorption isotherm.
Comparison of the standard Gibbs energies (∆G_{θ}^{○}) of adsorptions and rates of change (r) of ∆G_{θ}^{○} with θ (0 ≤ θ ≤ 1) for the Frumkin adsorption isotherms at the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces
interface
adsorbate
∆G_{θ}^{○}/kJ·mol^{−1}
r/kJ·mol^{−1}
Ref.
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O+D_{2}O)
H+D
19.9 < ∆G_{θ}^{○ }< 23.4
6.0
−
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
H
18.7 < ∆G_{θ}^{○ }< 22.2
6.0
27
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
D
22.2 < ∆G_{θ}^{○ }< 25.6
5.7
27
Pt−Ir alloy^{a}/0.5 M H_{2}SO_{4} (H_{2}O)
H
20.9 < ∆G_{θ}^{○ }< 24.0
5.2
28
Pt−Ir alloy^{a}/0.1 M LiOH (H_{2}O)
OH
44.0 < ∆G_{θ}^{○ }< 51.8
12.9
26
Pt−Ir alloy^{a}/0.1 M LiOH (D_{2}O)
OH+OD
45.9 < ∆G_{θ}^{○ }<56.8
18.1
26
Pt−Ir alloy^{b}/0.5 M H_{2}SO_{4} (H_{2}O)
H
21.1 < ∆G_{θ}^{○ }<24.2
5.2
20
Pt−Ir alloy^{b}/0.1 M KOH (H_{2}O)
OH
50.7 < ∆G_{θ}^{○ }< 60.2
15.9
20
Pt/0.1 M KOH (H_{2}O)
H
17.8 < ∆G_{θ}^{○ }< 21.0
5.5
25
Pt/0.5 M H_{2}SO_{4} (H_{2}O)
H
20.8 < ∆G_{θ}^{○ }< 24.1
5.5
21
Ir/0.1 M KOH (H_{2}O)
H
18.3 < ∆G_{θ}^{○ }< 21.7
5.5
25
Ir/0.5 M H_{2}SO_{4} (H_{2}O)
H
21.5 < ∆G_{θ}^{○ }< 24.7
5.5
21
Pd/0.5 M H_{2}SO_{4} (H_{2}O)
H
22.8 < ∆G_{θ}^{○ }< 31.8
14.9
19
Au/0.5 M H_{2}SO_{4} (H_{2}O)
H
28.7 < ∆G_{θ}^{○ }< 35.6
11.4
13
Re/0.1 M KOH (H_{2}O)
H
29.2 < ∆G_{θ}^{○ }< 36.0
11.4
16
Re/0.5 M H_{2}SO_{4} (H_{2}O)
H
32.7 < ∆G_{θ}^{○ }< 39.7
11.4
16
Ni^{c}/0.05 M KOH (H_{2}O)
H
6.6 < ∆G_{θ}^{○ }< 28.3
36.2
11
Ni^{d}/0.1 M LiOH (H_{2}O)
H
19.9 < ∆G_{θ}^{○ }< 37.8
29.8
29
Ni^{d}/0.5 M H_{2}SO_{4} (H_{2}O)
H
47.0 < ∆G_{θ}^{○ }< 61.7
24.6
29
Ti/0.5 M H_{2}SO_{4} (H_{2}O)
H
63.1 < ∆G_{θ}^{○ }< 79.6
27.8
23
Zr/0.2 M H_{2}SO_{4} (H_{2}O)
H
94.4 < ∆G_{θ}^{○ }< 106.5
20.1
24
Table 5.
^{a} Pt−Ir (90:10 mass ratio) alloy. ^{b} Pt−Ir (70:30 mass ratio) alloy. ^{c} Ni (purity 99.994%) foil. ^{d} Ni (purity 99.999%) wire.
Comparison of the standard Gibbs energies (∆G_{θ}^{○}) of adsorptions and rates of change (r) of ∆G_{θ}^{○} with θ (0.2 < θ < 0.8) for the Temkin adsorption isotherms at the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces
4.2. Correlation constants between the adsorption isotherms
Curves a, b, c, and d in Fig. 8 show the four numerically calculated Langmuir adsorption isotherms of (H + D) corresponding to K = 5.3 × 10^{−3}, 5.3 × 10^{−4}, 5.3 × 10^{−5}, and 5.3 × 10^{−6} mol^{−1}, respectively. For 0.2 < θ < 0.8, all of the Langmuir adsorption isotherms are always parallel to each other [13,16,42]. Correspondingly, all of the slopes of the Langmuir adsorption isotherms, i.e. all of g for the Temkin adsorption isotherms, are all the same regardless of the values of K. As summarized in Tables 2 and 3, we have experimentally and consistently found and confirmed that the values of g for the Temkin adsorption isotherms are approximately 4.6 greater than those for the Langmuir adsorption isotherms, i.e. g = 0. Similarly, the values of g for the Temkin adsorption isotherms are approximately 4.6 greater than those for the Frumkin adsorption isotherms. Because the Frumkin adsorption isotherm is determined on the basis of the Langmuir adsorption isotherm, i.e. g = 0 (see Fig. 5).
In addition, we have experimentally and consistently found and confirmed that the equilibrium constants (K_{o}) for the Temkin adsorption isotherms are approximately 10 times greater than those (K_{o} or K) for the correlated Frumkin or Langmuir adsorption isotherms (see Fig. 6 and Tables 2 and 3). These factors (ca. 4.6 and 10) can be taken as correlation constants between the Temkin and Frumkin or Langmuir adsorption isotherms. The two different adsorption isotherms, i.e. the Temkin and Frumkin or Langmuir adsorption isotherms, appear to fit the same data regardless of their adsorption conditions. These aspects are described elsewhere [19, 20, 23−29].
In this work, one can also confirm that the values of g and K_{o} for the Temkin adsorption isotherm are approximately 4.6 and 10 times greater than those for the correlated Frumkin adsorption isotherm, respectively. The Temkin adsorption isotherm correlating with the Frumkin adsorption isotherm, and vice versa, is readily determined using the correlation constants. Note that this is a unique feature between the Temkin and Frumkin or Langmuir adsorption isotherms.
4.3. Negative and positive values of the interaction parameters for the Frumkin adsorption isotherms
A negative value of g for the Frumkin adsorption isotherm is qualitatively and quantitatively interpreted elsewhere [42,46]. Negative and positive values of g correspond to lateral attractive and repulsive interactions between the adsorbed species, respectively. At Pt, Ir, and Pt−Ir alloy/H_{2}O and D_{2}O solution interfaces, the lateral attractive interaction (g < 0) between the adsorbed H, D, or (H + D) species is determined [22]. As stated above, this implies an increase in ∆G_{θ}^{○} of H, D, or (H + D) adsorption with θ (0 ≤ θ ≤ 1). At Pd, Ni, Ti, and Zr/H_{2}O solution interfaces, the lateral repulsive interaction (g > 0) between the adsorbed H species is determined. This implies a decrease in ∆G_{θ}^{○} of H adsorption with θ (0 ≤ θ ≤ 1). At Au and Re/H_{2}O solution interfaces, the lateral interaction between the adsorbed H species is negligible, i.e. g = 0 or g ≈ 0. This implies that the Langmuir adsorption isotherm is applicable. At Pt−Ir alloy/H_{2}O and D_{2}O solution interfaces, the lateral repulsive interaction (g > 0) between the adsorbed OH or (OH + OD) species is determined. This is significantly different from the lateral attractive interaction (g < 0) between the adsorbed H, D, or (H + D) species at the Pt−Ir alloy/H_{2}O and D_{2}O solution interfaces.
In contrast to Table 2, Table 3 shows that only the lateral repulsive interaction (g > 0) between the adsorbed H, D, (H + D), OH, or (OH + OD) species is determined. This is attributed to the values of g for the Frumkin adsorption isotherms, i.e. g > −4.6. Finally, one can conclude that the lateral attractive interaction (g < 0) between the adsorbed H, D, or (H + D) species is a unique feature of the Pt, Ir, and Pt−Ir alloy/H_{2}O and D_{2}O solution interfaces. The duality of the lateral attractive and repulsive interactions between the adsorbed H, D, or (H + D) species at the Pt, Ir, and Pt−Ir alloy interfaces is attributed to the negative values of g for the Frumkin adsorption isotherms. The Frumkin adsorption isotherm is more useful, effective, and reliable than the Temkin adsorption isotherm. As previously stated, the values of g for the Frumkin adsorption isotherms have never been experimentally and consistently determined using other conventional methods.
4.4. Equilibrium constants
In the acidic H_{2}O solutions, the values of K_{o}, i.e. K at g = 0, for H at the noble metal and alloy (Pt, Ir, Pt−Ir alloy, Pd, Au, Re) interfaces are much greater than those at the highly corrosionresistant metal (Ni, Ti, Zr) interfaces. In general, the values of K_{o} for H in the alkaline H_{2}O solutions are greater than those in the acidic H_{2}O solutions. The values of K_{o} for H in the acidic H_{2}O solutions are much greater than those for OH in the alkaline H_{2}O solutions. In the alkaline H_{2}O solutions, the values of K_{o} for H at the Ni interfaces are greater than those at the Pt, Ir, Pt−Ir alloy, Pd, Au, Re, Ti, and Zr interfaces. This is a unique feature of Ni and Ni alloy/alkaline H_{2}O solution interfaces. Note that Ni and Ni alloys are the metals most widely used for the cathodic HER in alkaline H_{2}O solutions.
The lateral interaction between the adsorbed H, D, (H + D), OH, or (OH + OD) species cannot be interpreted by the value of K_{o} for the Frumkin adsorption isotherm. For example, the lateral attractive interaction (g < 0) between the adsorbed H, D, or (H + D) species at the Pt, Ir, and Pt−Ir alloy interfaces is significantly different from the lateral repulsive interaction (g > 0) between the adsorbed H species at the Pd interface even though all of the Pt, Ir, Pt−Ir alloys, and Pd are the same platinum group metals and the values of K_{o} for H, D, and (H + D) are similar.
The Frumkin and Temkin adsorption isotherms (θ vs. E) of (H + D) and the related electrode kinetic and thermodynamic parameters (g, K, ∆G_{θ}^{○}, r) of the Pt−Ir alloy/0.1 M LiOH (H_{2}O + D_{2}O) solution interface have been determined using the phaseshift method and correlation constants and are compared with the relevant experimental data. The value of K decreases with increasing D_{2}O. The value of K for (H + D) is approximately equal to the average value of K for H and D isotopes. The Frumkin adsorption isotherms of H, D, and (H + D) are readily distinguishable at the interface. For 0.2 < θ < 0.8, the lateral attractive (g < 0) or repulsive (g > 0) interaction between the adsorbed (H + D) species appears at the interface. The Temkin adsorption isotherm correlating with the Frumkin or Langmuir adsorption isotherm, and vice versa, is readily determined using the correlation constants.
The lateral attractive interaction (g < 0) between the adsorbed H, D, or (H + D) species appears at the Pt, Ir, and Pt−Ir alloy interfaces. The lateral repulsive interaction (g > 0) between the adsorbed H species appears at the Pd, Ni, Ti, and Zr interfaces. At the Au and Re interfaces, the lateral interaction between the adsorbed H species is negligible, i.e. g = 0 or g ≈ 0. The lateral repulsive interaction (g > 0) between the adsorbed OH or (OH + OD) species appears at the Pt−Ir alloy interfaces. The lateral attractive interaction (g < 0) between the adsorbed H, D, or (H + D) species is a unique feature of the Pt, Ir, and Pt−Ir alloy interfaces. For 0.2 < θ < 0.8, the duality of the lateral attractive and repulsive interactions between the adsorbed H, D, or (H + D) species appears at the Pt, Ir, and Pt−Ir alloy interfaces. This unique feature of the Pt, Ir, and Pt−Ir alloy interfaces is attributed to the range of g for the Frumkin adsorption isotherms of H, D, and (H + D), i.e. −4.6 < g < 0.
The phaseshift method and correlation constants are the most accurate and efficient techniques to determine the Frumkin, Langmuir, and Temkin adsorption isotherms and the related electrode kinetic and thermodynamic parameters of the noble and highly corrosionresistant metal and alloy/H_{2}O and D_{2}O solution interfaces. They are useful and effective in facilitating selection of optimal electrode materials to yield electrochemical systems of maximum hydrogen, deuterium, and oxygen evolution performances. We expect that numerical simulations with a single equation for −φ vs. θ as functions of E and f or relevant experimental data for the phaseshift method and correlation constants will be obtained, compared, and discussed by other investigators.
The authors would like to thank Dr. Mu S. Cho (First President of Kwangwoon University, Seoul, Republic of Korea) for supporting the EG&G PAR 273A potentiostat/galvanostat, Schlumberger SI 1255 HF frequency response analyzer, and software packages. The section on theoretical and experimental backgrounds of the phaseshift method was reprinted with permission from Journal of Chemical & Engineering Data 55 (2010) 5598−5607. Copyright 2010 American Chemical Society. The authors wish to thank the American Chemical Society. This work was supported by the Research Grant of Kwangwoon University in 2012.
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18.ChunJ. H.KimN. Y.2006The phaseshift method for determining adsorption isotherms of hydrogen in electrochemical systems.
19.ChunJ. H.JeonS. K.ChunJ. Y.2007The phaseshift method and correlation constants for determining adsorption isotherms of hydrogen at a palladium electrode interface.
20.ChunJ. H.KimN. Y.ChunJ. Y.2008Determination of adsorption isotherms of hydrogen and hydroxide at Pt−Ir alloy electrode interfaces using the phaseshift method and correlation constants.
21.ChunJ. H.ChunJ. Y.2008Correction and supplement to the determination of the optimum intermediate frequency for the phaseshift method [Chun et al., Int. J. Hydrogen Energy 30 (2005) 247−259, 1423−1436].
22.ChunJ. Y.ChunJ. H.2009A negative value of the interaction parameter for overpotentially deposited hydrogen at Pt, Ir, and Pt−Ir alloy electrode interfaces.
23.ChunJ. Y.ChunJ. H.2009Determination of adsorption isotherms of hydrogen on titanium in sulfuric acid solution using the phaseshift method and correlation constants.
24.ChunJ. H.ChunJ. Y.2009Determination of adsorption isotherms of hydrogen on zirconium in sulfuric acid solution using the phaseshift method and correlation constants.
25.ChunJ.LeeJ.ChunJ. H.2010Determination of adsorption isotherms of overpotentially deposited hydrogen on platinum and iridium in KOH aqueous solution using the phaseshift method and correlation constants.
26.ChunJ.KimN. Y.ChunJ. H.2010Determination of adsorption isotherms of hydroxide and deuteroxide on Pt−Ir alloy in LiOH solutions using the phaseshift method and correlation constants.
27.ChunJ.KimN. Y.ChunJ. H.2010Determination of the adsorption isotherms of hydrogen and deuterium isotopes on a Pt−Ir alloy in LiOH solutions using the phaseshift method and correlation constants.
28.ChunJ.KimN. Y.ChunJ. H.2011Determination of the adsorption isotherms of overpotentially deposited hydrogen on a Pt−Ir alloy in H_{2}SO_{4}aqueous solution using the phaseshift method and correlation constants.
29.ChunJ. H.2012Determination of the Frumkin and Temkin adsorption isotherms of hydrogen at nickel/acidic and alkaline aqueous solution interfaces using the phaseshift method and correlation constants. J. Korean Electrochem. Soc, 15(1), 5466.
30.KvastekK.HorvatRadosevicV.2004Comment on: Langmuir adsorption isotherms of overpotentially deposited hydrogen at polyAu and Rh/H_{2}SO_{4} aqueous electrolyte interfaces; Qualitative analysis using the phaseshift method.
31.ChunJ. H.RaK. H.KimN. Y.2004Response to comment on: Langmuir adsorption isotherms of overpotentially deposited hydrogen at polyAu and Rh/H_{2}SO_{4} aqueous electrolyte interfaces; Qualitative analysis using the phaseshift methodJ. Electrochem. Soc 150 (2003) E207−217. J. Electrochem. Soc, 151(9), L1113.
32.LasiaA.2005Comments on: The phaseshift method for determining Langmuir adsorption isotherms of overpotentially deposited hydrogen for the cathodic H_{2} evolution reaction at polyRe/aqueous electrolyte interfacesInt. J. Hydrogen Energy 30 (2005) 485−499. Int. J. Hydrogen Energy,30(8), 913917.
33.ChunJ. H.JeonS. K.KimN. Y.ChunJ. Y.2005Response to comments on: The phaseshift method for determining Langmuir adsorption isotherms of overpotentially deposited hydrogen for the cathodic H_{2} evolution reaction at polyRe/aqueous electrolyte interfacesInt. J. Hydrogen Energy 30 (2005) 485−499. 308919928
34.HorvatRadosevicV.KvastekK.2009Pitfalls of the phaseshift method for determining adsorption isotherms.
35.In our email communications, HorvatRadosevic et al. admitted that all of their objections to the phaseshift method in Ref. 34 were confused and misunderstood. The exact same confusion and misunderstanding about the phaseshift method also appear in Refs. 30 and 32.