# Rapid and Automated Analytical Methods for Redox Species Based on Potentiometric Flow Injection Analysis Using Potential Buffers

Authors: Hiroki Ohura; Toshihiko Imato
Journal: Journal of Automated Methods and Management in Chemistry
 (2011)

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## Abstract

Two analytical methods, which prove the utility of a potentiometric flow injection technique for determining various redox species, based on the use of some redox potential buffers, are reviewed. The first is a potentiometric flow injection method in which a redox couple such as Fe(III)-Fe(II), Fe(CN)63−-Fe(CN)(CN)64−, and bromide-bromine and a redox electrode or a combined platinum-bromide ion selective electrode are used. The analytical principle and advantages of the method are discussed, and several examples of its application are reported. Another example is a highly sensitive potentiometric flow injection method, in which a large transient potential change due to bromine or chlorine as an intermediate, generated during the reaction of the oxidative species with an Fe(III)-Fe(II) potential buffer containing bromide or chloride, is utilized. The analytical principle and details of the proposed method are described, and examples of several applications are described. The determination of trace amounts of hydrazine, based on the detection of a transient change in potential caused by the reaction with a Ce(IV)-Ce(III) potential buffer, is also described.


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## Body

## 1. Introduction

Titrimetric analysis, the characteristics of which include a high precision and the measurement of an absolute quantity, is in widespread use in the chemical industry and the pharmaceutical industry [1, 2], and a wide variety of applications have been developed. However, a titrimetric analysis, while a versatile technique, is time-consuming. It is particularly tedious when the rate of the titration reaction is slow, since the operation must wait for a steady reading, even when an automatic-titrator is used. A promising approach to achieve more rapid throughput for analyses required in various fields is the application of flow titration techniques.  The flow titration method has been reported by many investigators [3–9]. In the continuous flow titration method, Nagy et al. [5] developed the “triangle-programmed titration technique” and applied it to an argentometric titration. Continuous flow titration, namely, the gas-segmented flow technique, is somewhat complicated and cumbersome in terms of both the apparatus used and the procedures required, in comparison with the nongas-segmented flow injection analysis (FIA), because, in the gas-segmented flow method, the streams need to be debubbled before detection. Thus, flow injection analysis (FIA) [10] has been applied to titration analysis, in attempts to shorten and simplify this time-consuming procedure. Růžička and Hansen [6, 7] reported on  an FIA titration method based on the measurement of peak widths. Åström [8] reported on a flow analysis method using both a universal buffer solution and a glass electrode, which was designed to give a linear pH-response to the sample concentration, referred to as a “single point titration.” One of authors also proposed an FIA titration method for the determinations of acids and bases or metal ions, which involved the reaction of the sample with a pH buffer or a metal buffer solution containing an indicator and applied the method to potentiometric detection using a glass electrode or metal ion-selective electrode [11, 12].We recently proposed an FIA titration method for determination of various redox species utilizing a redox reaction with some redox potential buffers and applied the method to potentiometric detection using a redox electrode. The idea of our proposed FIA titration is the use of characteristics of the potential buffer solution, in which the potential change due to redox reaction of an analyte with the buffer component is directly proportional to the analyte concentration. In addition the potential of the redox electrode is very stable in the potential buffer solution. In this paper, the proposed potentiometric FIA method is discussed, and the subject is divided into two sections. First, we describe a potentiometric FIA method for the determination of redox species using a simple redox reaction of a sample with a potential buffer solution consisting of a redox couple such as Fe(III)-Fe(II) orFe(CN)63--Fe(CN)64-. This method is based on the detection of a change in the potential of a redox electrode caused by a change in the composition of the potential buffer solution after completion of a reaction between the sample and the potential buffer. Some similar papers that preceeded our method have been published by Porter and Sawyer [13], Brunt [14], and Karlberg and Thelander [15] with respect to the determination of redox species by potentiometry employing a redox reaction in an FIA system. Porter and Sawyer [13] and Brunt [14] reported the determination of glucose and other reducing sugars based on changes in the redox potentials of an Fe(CN)63--Fe(CN)64- buffer solution caused by the reaction of sugars with Fe(CN)63-. Karlberg and Thelander [15] reported the determination of Fe(II) and ascorbic acid by monitoring the composition of Ce(IV)-Ce(III) formed by a reaction with a stream of a cerium(IV) reagent with redox detection. These potentiometric detection methods can be performed with only the use of an oxidant without a reductant as the stream of reagent solution in a flow system. On the contrary, our proposed method involves the use of a potential buffer solution consisting of a redox couple, which stabilizes the measuring potential of the redox electrode. The advantages of the proposed method are that samples in a wide concentration range can be determined by selecting an appropriate concentration of potential buffer solution. In this paper, applications of the proposed method to the rapid determination of redox compounds such as concentrated hydrogen peroxide, ethanol in alcoholic beverages, reducing sugars, manganese(II), and phenol are discussed.On the other hand, the excellent characteristics of the FIA method permits its use in detecting a final product at an equilibrium state as well as a transient intermediate that appears before chemical equilibrium is reached, where an appropriate chemical reaction is employed. Among the many redox reactions, there are several reactions in which an intermediate compound with a short lifetime is generated. In such a case, the FIA method would be useful for detecting such an intermediate, since a reaction time can be easily controlled in the flow system. During our research on the use of potentiometric FIA for the determination of redox species using a potential buffer, as described above, we discovered an interesting phenomena in which a large transient potential change in the redox electrode with a mountain-shape appeared, when a bromate solution was added to an Fe(III)-Fe(II) potential buffer containing bromide [16]. The large change in potential was found to be due to bromine generated during the redox reaction of an analyte with the potential buffer, as an intermediate. The electrode potential of the intermediate, bromine/bromide, is much higher than that of the potential buffer. Therefore, in the case of potentiometric FIA, a highly sensitive determination of the analyte can be achieved, provided that the intermediate substance in the FIA system can be detected. No report of a highly sensitive potentiometric FIA method for the determination of oxidative species involving the detection of an intermediate formed during a redox reaction has appeared, so far.Second, we describe a highly sensitive potentiometric FIA method based on the detection of a large transient potential change in the redox electrode, which appears a short period after an analyte is mixed with the potential buffer. In the case where an Fe(III)-Fe(II) potential buffer is used, it was found that the addition of bromide or chloride to the potential buffer enhances the sensitivity for various oxidizing species such as bromate, chromium (VI), hydrogen peroxide, and oxychlorine. A high sensitivity to such oxidative species was achieved by the potentiometric detection of a large transient potential change due to the generation of intermediate bromine or chlorine during the reaction of the analyte with bromide or chloride in the potential buffer. The advantage of the proposed method, in which the detection of an intermediate is involved, is that the bromide or chloride in the Fe(III)-Fe(II) potential buffer functions as a homogeneous catalyst for the formation of bromine or chlorine as an intermediate during the reaction. Thus, the proposed method was also applied to the rapid and highly sensitive determination of redox compounds in actual samples, such as residual chlorine in tap water, chromium (VI) in seawater, and hydrazine in boiler water.Furthermore, the analytical methodology and mechanism for the potential change of the two proposed methods indicate that, in both cases, an equilibrium potential reached after a simple redox reaction and a transient potential generated during a complexed redox reaction could be measured.


## 2. Experimental

A typical two-channel flow system for the determination of redox species is shown in Figure1. The flow-injection apparatus consisted of a peristaltic pump (Model Minipuls 2, Gilson), a sample injector (HPV6, GLC Sciences Co.), a flow-through type redox electrode detector (Model FLC-11, DKK Co.) equipped with a platinum or gold plate electrode and a silver/silver chloride reference electrode, and a potentiometer (Model IOC 10, DKK Co.) for measuring the potential of the electrode detector. The manifold was constructed of Teflon tubing (0.5 mm i.d.) throughout. A potential buffer solution consisting of an Ox1-Red1 mixture, such as Fe(III)-Fe(II), Fe(CN)63--Fe(CN)64-, and Ce(IV)-Ce(III) was pumped through the reagent channel (VBuff). The potential change of the electrode detector was recorded as a peak-shaped signal, and the concentration of the sample, Ox2, can be determined from the peak height.Figure 1
Manifolds for the FIA of oxidative and reductive species using a potential buffer solution. R.S.: reagent solution (a mixture of Ox1-Red1); Ox1-Red1: oxidants and reductants; C.S.: carrier (H2O); P: peristaltic pump; Ox2: oxidative sample; S: sample injector; C: confluence point; R.C.: reaction coil; D: flow-through type redox electrode detector; E: potentiometer; R: recorder; W: waste. VBuff and VS are flow rates of a buffer solution and water, respectively.Standard analyte solutions of oxidative or reductive substances were prepared by dissolving the corresponding analytical-reagent grade reagents in deionized water. The potential buffer solutions consisting of Fe(III)-Fe(II),Fe(CN)63--Fe(CN)64-, and Ce(IV)-Ce(III) were prepared by dissolving of ammonium iron(III) and ammonium iron(II), potassium hexacyanoferrate(III) and potassium hexacyanoferrate(II), and sulfate cerium(IV) and sulfate cerium(III) in dilute sulfuric acid or a sodium hydroxide solution, respectively.


## 3. Potential Buffers Consisting of a Redox Couple, and the Characteristics of the Electrode Potential Using a Potential Buffer in FIA

It is desirable for the potential buffer solution, consisting of a redox couple, employed in the proposed method to be reversible electrochemically and to obey the Nernst equation. The reactivity of a redox sample with one of the redox couples in the potential buffer can be estimated by the order of the magnitude ofE0 of the redox couple in the potential buffer. The redox electrode showed a Nernstian response to an Fe(III)-Fe(II) couple (E0=0.77 V versus NHE) and a Ce(IV)-Ce(III) couple (E0=1.68 V) in an acidic solution and to an Fe(CN)63--Fe(CN)64- couple (E0=0.36 V) in a basic solution in the range of concentration ratio of the oxidized form to the reduced form from 0.1 to 10 in the each redox couple, according to (2). In particular, the redox electrode showed a Nernstian response in the Fe(CN)63--Fe(CN)64- potential buffer, even at a lower concentration down to 10−5 M. On the other hand, the redox electrode did not show a stable potential to Cr(VI)-Cr(III) and Mn(VII)-Mn(II) couples which are typically employed as a titrant of redox titrimetry. In the case of an Mn(VII)-Mn(II) couple, when the concentration of the couple was higher than 10−3 M, the precipitation of MnO2 occurred. This may be due to the fact that a disproportionation reaction occurs in the mixed solution of the redox couple.The characteristics of the electrode potential which detected the composition of the potential buffer solution in the proposed FIA are summarized as follows.(1)
The baseline potential is stable, and the response is reproducible in the buffer solution, even at low concentrations, because an electrode is immersed in a well-defined potential buffer solution.(2)
For a small change in the composition of a buffer solution, a potential change, namely, the peak height, is nearly proportional to the concentration of a sample.(3)
A wide concentration range can be measured, although the measurable concentration level depends on the concentration of the buffer solution used.(4)
The method has potential applications to liquid chromatography.


## 4. Analytical Methodology for a Potentiometric Flow Method by Redox  Couple Potential Buffer

### 4.1. Equilibrium Potential Change of a Redox Electrode after Simple Redox Reaction with Potential Buffer

In the flow system shown in Figure1, when an oxidative species, Ox2, as a sample, is injected into a carrier channel, where water is pumped at flow rate of VS, and mixed with the potential buffer solution  consisting of a redox couple, Ox1-Red1, the following redox reaction occurs in the FIA system: (1)Ox2+mRed1⟶Red2+mOx1
where m is the number of moles of Red1 required to reduce 1 mole of Ox2. The potential of the redox electrode (E1 in milivolt) in the detector is governed by the concentration ratio of the potential buffer solution and is expressed by the Nernst equation, as shown in (2),(2)E1=E0+(59n)log⁡⁡([Ox1][Red1])(mV,25°C),
where E0 is the formal redox potential, and n is the number of moles of electrons involved in the electrode reaction, and [Ox1] and [Red1] are the concentrations of Ox1 and Red1, respectively. The baseline potential, E1 (the potential when a sample is not injected), can be written in terms of the initial concentrations of Ox1 and Red1, based on (2). In the case where the sample, Ox2, is injected, the redox potential, E2, can be expressed as follows under the assumption that reaction (1) is complete before the sample zone reaches the detector when the flow rates of VBuff and VS are equal:(3)E2=E0+(59n)log⁡⁡{[Ox1]+m[Ox2][Red1]-m[Ox2]}(mV),
where [Ox2] is the initial concentration of Ox2. Under the assumption that no dispersion of the sample and reaction products occur while flowing through the manifold, the potential change (ΔE) (peak height) of the redox electrode can be expressed by the following equation, which is derived from (2) and (3):(4)ΔE=(59n)log⁡⁡{(1+m[Ox2]/[Ox1])(1-m[Ox2]/[Red1])}(mV).
The relationship between ΔE and [Ox2] depends on both the initial concentration ratio of Ox1 to Red1 and the value of n, which can be estimated from (4). The variation in ΔE with [Ox2], under the condition that the value of n is 1, becomes linear within ca. 40 mV, when the value of [Ox1]/[Red1] is about 0.5. When [Ox1]/[Red1] is higher than 2 or lower than 0.2, the sensitivity, slope of the calibration curve, increases, but the shapes of the curves become concave or convex, respectively. Thus, the potential change and baseline potential of the redox electrode are governed by the change in the composition of the redox couple in the potential buffer solution, according to (4). The linear relationship can be utilized as a calibration curve for an Ox2 sample. However, the upper limit for the measurable concentration of the Ox2 with linearity is limited by the concentration of the potential buffer, as predicted from (4). This limitation means that the concentration of the potential buffer should be chosen in accordance with the concentration of the analyte. In other words, the measurable concentration level of the Ox2 can be altered by choosing the concentrations of the potential buffer.When an Fe(III)-Fe(II) couple in a sulfuric acid solution is used as the redox couple, Ox1-Red1 (1) can be replaced with the following equation:(5)Ox+mFe2++aH+⟶Red+mFe3++bH2O
where m is the number of moles of Fe2+ required to reduce 1 mol of an analyte, Ox, and a and b are stoichiometric coefficients. If reaction (5) is complete, the potential change (ΔE) of the redox electrode at 25°C can be expressed by (6) in the same as(4)(6)ΔE=59log⁡⁡{(1+m[Ox]0/[Fe3+]0)(1-m[Ox]0/[Fe2+]0)}(mV),
where [Ox]0, [Fe3+]0, and [Fe2+]0 are the initial concentrations of Ox, Fe3+, and Fe2+, respectively. In the case of completion of reaction (5), the variation in ΔE with [Ox] becomes relatively linear in the concentration range of Ox, where the ΔE is within ca. 20 mV, when the value of [Fe3+]0/[Fe2+]0 is nearly equal to unity. The theoretical sensitivities, defined as the slope of the linear portion of the ΔE versus [Ox] plot, are calculated to be 10.4, 20.9, and 31.3 mV mM−1 for m=2, 4, and 6, respectively, from (6), when the concentration of [Fe3+]0 and [Fe2+]0, respectively, is equal to 0.01 M. These calculated values for sensitivity to several oxidative species are given in Table 3.In practice, the potential change,ΔE, is influenced, not only by the concentration of the sample but also by the dispersion of the sample zone in the flow system. However, one of the advantages of FIA is that it is capable of precisely controlling the dispersion of the flow condition. Hence, the peak height would be expected to be proportional to the concentration of sample.The theoretical potential change for a reductive sample can be predicted by changing the signs in front ofm of (4) opposite.


### 4.2. Transient Potential Change of a Redox Electrode due to Intermediate Generated during Complex Redox Reaction with Fe(III)-Fe(II) Potential Buffer Containing Bromide or Chloride

Figure2 shows the typical potential responses of the redox electrode arising in which Ox sample is added to an Fe(III)-Fe(II) potential buffer without bromide or chloride or containing bromide or chloride in the batchwise experiments. In the case that an Fe(III)-Fe(II) potential buffer without bromide or chloride is used, the response potential increase gradually with time and finally reaches a constant equilibrium potential, as shown in Figure 2(b). The potential change between the initial potential and the equilibrium potential agrees well with the value calculated from (6). On the other hand, in the case that an Fe(III)-Fe(II) potential buffer containing bromide or chloride is used, the response potential with a mountain-shaped transient change appears with increasing reaction time, as shown in Figure 2(a), although the concentration of Ox is lower by about three orders magnitude than that in the potential buffer. The potential increases quickly, decreases with time after passing through a maximum, and finally reaches a constant equilibrium potential which is almost the same as that of Figure 2(b). The transient potential change is due to the generation of bromine or chlorine as an intermediate formed by the reaction of Ox with bromide or chloride in the potential buffer.Figure 2
Potential changes during the reaction of Ox with an Fe(III)-Fe(II) buffer solution containing bromide or chloride (a) and without bromide or chloride (b) as a function of time.The mechanism of the transient change in potential shown in Figure2(a) can be explained qualitatively by considering the following reactions: Ox reacts first with bromide or chloride in the potential buffer, and the reaction generates bromine or chlorine as an intermediate during the course of the reaction. Second, the intermediate (Br2 or Cl2) reacts with Fe(II) in the potential buffer. Thus, these reactions can be expressed by the following:(7)Ox+aBr-+bH+⟶Red+a2Br2+cH2O(8)Ox+aCl-+bH+⟶Red+a2Cl2+cH2O(9)a2Br2+Fe2+⟶aBr-+Fe3+(10)a2Cl2+Fe2+⟶aCl-+Fe3+
where Red is the reduced form of Ox. For the mountain-shaped transient change, the initial potential is governed by the Fe(III)-Fe(II) ratio in the potential buffer. When Ox is added to the potential buffer, since Br2 or Cl2 is generated by (7) or (8), the electrode potential is shifted from Fe(III)/Fe(II) to Br2/Br− or Cl2/Cl−. Since the redox potential of the Br2/Br− couple (E0=1.09 V) or the Cl2/Cl− couple (E0=1.33 V) is much higher than that of the Fe(III)/Fe(II) redox couple (E0=0.77 V), the electrode potential increases towards a positive potential due to (7) or (8). The potential then decreases towards an equilibrium potential due to (9) or (10). The overall reaction which is the sum of elementary reactions (7) and (9) or of reactions (8) and (10) is given by (5) in equilibrium potential. That is, bromide or chloride in the potential buffer may act as a homogeneous catalyst for the formation and reduction of bromine or chlorine.  The magnitude of the large transient potential change increases with decreasing concentration of Fe(III)-Fe(II) in the potential buffer components. This is due to the fact that the rate of reduction of bromine or chlorine by Fe(II) expressed by (9) or (10), respectively, decreases.  In addition, since reactions (7) and (9) or (8) and (10) proceed successively, the amount of bromine or chlorine generated as an intermediate is calculated to be proportional to the initial concentration of Ox at anytime of reaction period, if the generation rate of bromine or chlorine is governed by the first-order reaction in terms of the concentration of Ox and depletion rate of bromine or chlorine is also governed by the first-order reaction in terms of bromine or chlorine. Therefore the linear calibration between the potential change ΔE and the concentration of Ox is expected.In the FIA system, the reaction time for the reaction of a sample with a reagent can be easily controlled by using different coil lengths and/or different flow rates for the carrier and reagent streams. The concentrations of sulfuric acid, bromide or chloride, and Fe(III)-Fe(II) in the potential buffer solution are also important factors in terms of enhancing sensitivity. By determining these optimum analytical conditions for the highly sensitive determination of oxidative species, a two-channel flow system, carrier stream (H2O) and reagent stream (Fe3+-Fe2+, NaBr, or NaCl in H2SO4 solution), was designed to detect the large transient potential change within a reasonable time, where the maximum appears transiently. The flow-injection apparatus was the same as that shown in Figure 1. The potential changes (peak signals) measured at appropriate reaction times were proportional to the concentration of oxidative species.


## 4.1. Equilibrium Potential Change of a Redox Electrode after Simple Redox Reaction with Potential Buffer

In the flow system shown in Figure1, when an oxidative species, Ox2, as a sample, is injected into a carrier channel, where water is pumped at flow rate of VS, and mixed with the potential buffer solution  consisting of a redox couple, Ox1-Red1, the following redox reaction occurs in the FIA system: (1)Ox2+mRed1⟶Red2+mOx1
where m is the number of moles of Red1 required to reduce 1 mole of Ox2. The potential of the redox electrode (E1 in milivolt) in the detector is governed by the concentration ratio of the potential buffer solution and is expressed by the Nernst equation, as shown in (2),(2)E1=E0+(59n)log⁡⁡([Ox1][Red1])(mV,25°C),
where E0 is the formal redox potential, and n is the number of moles of electrons involved in the electrode reaction, and [Ox1] and [Red1] are the concentrations of Ox1 and Red1, respectively. The baseline potential, E1 (the potential when a sample is not injected), can be written in terms of the initial concentrations of Ox1 and Red1, based on (2). In the case where the sample, Ox2, is injected, the redox potential, E2, can be expressed as follows under the assumption that reaction (1) is complete before the sample zone reaches the detector when the flow rates of VBuff and VS are equal:(3)E2=E0+(59n)log⁡⁡{[Ox1]+m[Ox2][Red1]-m[Ox2]}(mV),
where [Ox2] is the initial concentration of Ox2. Under the assumption that no dispersion of the sample and reaction products occur while flowing through the manifold, the potential change (ΔE) (peak height) of the redox electrode can be expressed by the following equation, which is derived from (2) and (3):(4)ΔE=(59n)log⁡⁡{(1+m[Ox2]/[Ox1])(1-m[Ox2]/[Red1])}(mV).
The relationship between ΔE and [Ox2] depends on both the initial concentration ratio of Ox1 to Red1 and the value of n, which can be estimated from (4). The variation in ΔE with [Ox2], under the condition that the value of n is 1, becomes linear within ca. 40 mV, when the value of [Ox1]/[Red1] is about 0.5. When [Ox1]/[Red1] is higher than 2 or lower than 0.2, the sensitivity, slope of the calibration curve, increases, but the shapes of the curves become concave or convex, respectively. Thus, the potential change and baseline potential of the redox electrode are governed by the change in the composition of the redox couple in the potential buffer solution, according to (4). The linear relationship can be utilized as a calibration curve for an Ox2 sample. However, the upper limit for the measurable concentration of the Ox2 with linearity is limited by the concentration of the potential buffer, as predicted from (4). This limitation means that the concentration of the potential buffer should be chosen in accordance with the concentration of the analyte. In other words, the measurable concentration level of the Ox2 can be altered by choosing the concentrations of the potential buffer.When an Fe(III)-Fe(II) couple in a sulfuric acid solution is used as the redox couple, Ox1-Red1 (1) can be replaced with the following equation:(5)Ox+mFe2++aH+⟶Red+mFe3++bH2O
where m is the number of moles of Fe2+ required to reduce 1 mol of an analyte, Ox, and a and b are stoichiometric coefficients. If reaction (5) is complete, the potential change (ΔE) of the redox electrode at 25°C can be expressed by (6) in the same as(4)(6)ΔE=59log⁡⁡{(1+m[Ox]0/[Fe3+]0)(1-m[Ox]0/[Fe2+]0)}(mV),
where [Ox]0, [Fe3+]0, and [Fe2+]0 are the initial concentrations of Ox, Fe3+, and Fe2+, respectively. In the case of completion of reaction (5), the variation in ΔE with [Ox] becomes relatively linear in the concentration range of Ox, where the ΔE is within ca. 20 mV, when the value of [Fe3+]0/[Fe2+]0 is nearly equal to unity. The theoretical sensitivities, defined as the slope of the linear portion of the ΔE versus [Ox] plot, are calculated to be 10.4, 20.9, and 31.3 mV mM−1 for m=2, 4, and 6, respectively, from (6), when the concentration of [Fe3+]0 and [Fe2+]0, respectively, is equal to 0.01 M. These calculated values for sensitivity to several oxidative species are given in Table 3.In practice, the potential change,ΔE, is influenced, not only by the concentration of the sample but also by the dispersion of the sample zone in the flow system. However, one of the advantages of FIA is that it is capable of precisely controlling the dispersion of the flow condition. Hence, the peak height would be expected to be proportional to the concentration of sample.The theoretical potential change for a reductive sample can be predicted by changing the signs in front ofm of (4) opposite.


## 4.2. Transient Potential Change of a Redox Electrode due to Intermediate Generated during Complex Redox Reaction with Fe(III)-Fe(II) Potential Buffer Containing Bromide or Chloride

Figure2 shows the typical potential responses of the redox electrode arising in which Ox sample is added to an Fe(III)-Fe(II) potential buffer without bromide or chloride or containing bromide or chloride in the batchwise experiments. In the case that an Fe(III)-Fe(II) potential buffer without bromide or chloride is used, the response potential increase gradually with time and finally reaches a constant equilibrium potential, as shown in Figure 2(b). The potential change between the initial potential and the equilibrium potential agrees well with the value calculated from (6). On the other hand, in the case that an Fe(III)-Fe(II) potential buffer containing bromide or chloride is used, the response potential with a mountain-shaped transient change appears with increasing reaction time, as shown in Figure 2(a), although the concentration of Ox is lower by about three orders magnitude than that in the potential buffer. The potential increases quickly, decreases with time after passing through a maximum, and finally reaches a constant equilibrium potential which is almost the same as that of Figure 2(b). The transient potential change is due to the generation of bromine or chlorine as an intermediate formed by the reaction of Ox with bromide or chloride in the potential buffer.Figure 2
Potential changes during the reaction of Ox with an Fe(III)-Fe(II) buffer solution containing bromide or chloride (a) and without bromide or chloride (b) as a function of time.The mechanism of the transient change in potential shown in Figure2(a) can be explained qualitatively by considering the following reactions: Ox reacts first with bromide or chloride in the potential buffer, and the reaction generates bromine or chlorine as an intermediate during the course of the reaction. Second, the intermediate (Br2 or Cl2) reacts with Fe(II) in the potential buffer. Thus, these reactions can be expressed by the following:(7)Ox+aBr-+bH+⟶Red+a2Br2+cH2O(8)Ox+aCl-+bH+⟶Red+a2Cl2+cH2O(9)a2Br2+Fe2+⟶aBr-+Fe3+(10)a2Cl2+Fe2+⟶aCl-+Fe3+
where Red is the reduced form of Ox. For the mountain-shaped transient change, the initial potential is governed by the Fe(III)-Fe(II) ratio in the potential buffer. When Ox is added to the potential buffer, since Br2 or Cl2 is generated by (7) or (8), the electrode potential is shifted from Fe(III)/Fe(II) to Br2/Br− or Cl2/Cl−. Since the redox potential of the Br2/Br− couple (E0=1.09 V) or the Cl2/Cl− couple (E0=1.33 V) is much higher than that of the Fe(III)/Fe(II) redox couple (E0=0.77 V), the electrode potential increases towards a positive potential due to (7) or (8). The potential then decreases towards an equilibrium potential due to (9) or (10). The overall reaction which is the sum of elementary reactions (7) and (9) or of reactions (8) and (10) is given by (5) in equilibrium potential. That is, bromide or chloride in the potential buffer may act as a homogeneous catalyst for the formation and reduction of bromine or chlorine.  The magnitude of the large transient potential change increases with decreasing concentration of Fe(III)-Fe(II) in the potential buffer components. This is due to the fact that the rate of reduction of bromine or chlorine by Fe(II) expressed by (9) or (10), respectively, decreases.  In addition, since reactions (7) and (9) or (8) and (10) proceed successively, the amount of bromine or chlorine generated as an intermediate is calculated to be proportional to the initial concentration of Ox at anytime of reaction period, if the generation rate of bromine or chlorine is governed by the first-order reaction in terms of the concentration of Ox and depletion rate of bromine or chlorine is also governed by the first-order reaction in terms of bromine or chlorine. Therefore the linear calibration between the potential change ΔE and the concentration of Ox is expected.In the FIA system, the reaction time for the reaction of a sample with a reagent can be easily controlled by using different coil lengths and/or different flow rates for the carrier and reagent streams. The concentrations of sulfuric acid, bromide or chloride, and Fe(III)-Fe(II) in the potential buffer solution are also important factors in terms of enhancing sensitivity. By determining these optimum analytical conditions for the highly sensitive determination of oxidative species, a two-channel flow system, carrier stream (H2O) and reagent stream (Fe3+-Fe2+, NaBr, or NaCl in H2SO4 solution), was designed to detect the large transient potential change within a reasonable time, where the maximum appears transiently. The flow-injection apparatus was the same as that shown in Figure 1. The potential changes (peak signals) measured at appropriate reaction times were proportional to the concentration of oxidative species.


## 5. Analyses Utilizing an Equilibrium Potential after Completion of a Simple Redox Reaction

### 5.1. Analyses of Concentrated Hydrogen Peroxide and Ethanol in Alcoholic Beverages Using Fe(III)-Fe(II) Potential Buffer [17–19]

Concentrated hydrogen peroxide is used in the breaching of pulp and textiles and for washing silicon wafers. For process control in the production of hydrogen peroxide in the pulp and semiconductor industries, the determination of concentrated hydrogen peroxide is routinely carried out by titrimetry after a moderate sample dilution procedure. However, a more rapid method for the determination of concentrated hydrogen peroxide would be desirable, because titrimetry is tedious and time-consuming. The determination of hydrogen peroxide was proposed by using the Fe(III)-Fe(II) couple in an acidic solution as the potential buffer solution, according to (11)H2O2+2Fe2++2H+⟶2Fe3++2H2O
In the flow system, an analyte at high concentration can be determined by utilizing the controlled dispersion of the sample zone, and its dispersion depends on the sample volume and coil length (residence time) from the injector to the detector. In this method [17], which does not require any sample dilution, the determination of hydrogen peroxide in concentrations of up to ~10 M (30%) was successfully achieved using a 0.4 M Fe(III)-0.4 M Fe(II) potential buffer containing 1 M H2SO4, where the sample could be diluted by ca. 80-fold by injecting a very small volume to 1 μL and by setting the residence time of the sample zone to 1 min, as a standard procedure in flow system. Even in such a high dispersion system, the R.S.D for the determination of 9.86 M H2O2 was 0.7% (n=10). A sampling rate of ~30 h−1 was possible at the present flow condition. The proposed method could be used in the online monitoring of the production of hydrogen peroxide, as well as for bleaching and washing processes which use concentrated hydrogen peroxide.An accurate and selective determination method for the ethanol content in alcoholic beverages usually involves the use of a gas chromatographic technique or a specific-gravity method (currently, the official method in Japan). However, a simpler, rapid, and selective method is possible using a flow-injection technique, in which the alcohol is separated using a porous membrane. In this method, the selective determination method of ethanol in alcoholic beverages (Japanese sake, beer, wine, whisky, and shochu) was proposed, using the Fe(III)-Fe(II) potential buffer solution and a gas-diffusion unit equipped with a membrane [19]. The flow injection manifold, equipped for gas-diffusion separation is shown in Figure 3. The gas-diffusion separation unit (G.D.) is comprised of two Daiflon blocks furnished with a shallow groove (37 mm long, 3 mm wide, 0.5 mm deep) and separated by a porous poly (tetrafluoroethylene) (PTFE) plane membrane, which allows the transfer of ethanol from a stream of C.S. to a stream of R.S.1. The PTFE membrane is 50 μm thick, with a pore size of 0.4 μm. The method is based on the detection of the composition change of the Fe(III)-Fe(II) couple in the potential buffer, caused by the reduction of acidic dichromate by ethanol that had permeated through a membrane as vapor, according to (12)3C2H5OH+2Cr2O72-+16H+⟶3CH3COOH+4Cr3++11H2O(13)Cr2O72-+6Fe2++14H+⟶2Cr3++6Fe3++7H2OFigure 3
Flow-injection manifold equipped with a gas-diffusion separation unit for the determination of ethanol and calibration peaks for ethanol. C.S: carrier (H2O): R.S.1: reagent solution (0.015 M K2Cr2O7, 2 M H2SO4); R.S.2: reagent solution (0.135 M Fe(NH4)2SO4); S: sample injector (140 μL); G.D: gas-diffusion separation unit; R.C.1: reaction coil (1 m, 0.5 mm); R.C.2: reaction coil (2 m, 0.5 mm); B.P.C: back pressure coil (10 m, 0.5 mm).The PTFE membrane for the separation of alcohol was superior to a poly(substituted-acetylene)/polysiloxane graft copolymer membrane [18], because of the high permeability of alcohol and the simplicity of the manifold. The flow injection peaks for a calibration curve were obtained in the ethanol concentration range from 5 to 40% (v/v) using the flow condition indicated in Figure 3. Sampling rate was ~25 h−1. The analytical results for the ethanol content in alcoholic beverages determined by the proposed method were in good agreement with data obtained by either the specific-gravity method or a gas chromatographic method, as shown in Table 1. The R.S.D for the proposed method was smaller than those by the other methods.Table 1
Determination of ethanol content in alcoholic beverages.
Ethanol content, % (v/v)Certified valueSpecific gravity methodGC methodFIA method (without G.D.)Proposed method (G.D.)Beera 4.54.54.36.64.4Wine <1411.516.511.5Sake 16-1716.816.019.516.1Whisky 4342.542.642.6Shochu 2524.524.625.0aThe sample was debubbled for 20 min before analysis.Incidentally, when the FIA technique was employed without using the G.D., positive errors of 20–30% were observed for Japanese sake, beer, and wine, which also contain compounds such as sugars, organic acids, and amino acids, which are also oxidized by the dichromate solution.


### 5.2. Analyses of Reducing Sugars, Amylase, and Manganese(II) Using anFe(CN)63--Fe(CN)64- Potential Buffer [20–25]

The redox coupleFe(CN)63--Fe(CN)64- has a lower redox potential of 0.36 V and is known to show unique redox behavior in the presence of reducing sugars. The redox electrode shows a stable potential to the Fe(CN)63--Fe(CN)64- couple in alkaline media, but is not stable in neutral to acidic solution because the auto-oxidation of Fe(CN)64- to Fe(CN)63- occurs in such media. The redox electrode also showed a Nernstian response even at lower concentrations of  Fe(CN)63--Fe(CN)64- potential buffer down to 10−5 M in alkaline media. Thus, it would be expected that system could be used in the sensitive determination of certain compounds and could also be used in a wide concentration range of analytes, as described above.For an example of an analysis utilizing a change in the composition of theFe(CN)63--Fe(CN)64- potential buffer, an analytical method for reducing sugars [20] was proposed based on the reaction of a reducing sugar with of  Fe(CN)63- in alkaline solution, according to (14)Reducing sugar+mFe(CN)63-⟶mFe(CN)64-+other products
where m is the number of moles required to oxidize one mole of reducing sugar.In the case for the determination of glucose [21], the concentration of NaOH in the potential buffer and the temperature of the reaction, as a standard procedure in flow system shown in Figure 1, were 0.6 M and 85°C, respectively. These conditions were selected for showing the highest sensitivity by changing the NaOH concentration from 0.01 M to 1.0 M and the temperature from 50°C to 90°C. The time required for a reaction between glucose and Fe(CN)63- to be completed is about 2.5 min and m values of Fe(CN)63- for the oxidation of 1 mol glucose was 6, as calculated from response potential(ΔE) after completion of the reaction. The total time required was about 4.2 min from sample injection (140 μL) to the detection of a peak maximum in the flow system. FIA peaks for injections at 2 min intervals were reproducible, and, as a result, it is possible to analyze 30 samples/h using the proposed procedure. Table 2 lists the sensitivity values and measurable concentration ranges for various concentrations of buffer solutions. The sensitivity increased with decreasing concentration of buffer solution. A sample in the concentration range from 10−7 M to 10−3 M could be determined by changing the concentration of the  Fe(CN)63--Fe(CN)64- potential buffer solution from 1×10-5 M to 1×10-2 M. For the 1×10-5 M  Fe(CN)63--Fe(CN)64- potential buffer, the fluctuations and drifts in the baseline potential were within 0.3 mV and less than 0.8 mV/h, respectively, and the lowest detectable concentration was 0.1 μM (peak heights: 0.6 mV). When the concentration of the potential buffer was lower than 5×10-6 M, the drift and fluctuation of the baseline potential became larger, and peak heights were not reproducible. The high sensitivity of the proposed FIA method can be attributed to, in part, the high stability of the electrode potentials in buffer solutions at low concentrations.Table 2
Effect of concentrations ofFe(CN)63--Fe(CN)64- potential buffer solution on sensitivity.
Concentration      (M)Sensitivitya (mV mM−1)Measurable concentration range (M)1×10-29.72.0×10-4~1.8×10-31×10-39.5×102.0×10-5~1.8×10-41×10-49.4×1022.0×10-6~1.8×10-55×10-51.9×1031.0×10-6~1.0×10-51×10-56.2×1032.5×10-7~2.5×10-6aSensitivity: slope of calibration curve (peak height/mV obtained by injection of 1 mM glucose).Table 3
Sensitivities to oxidative species.
Oxidative speciesSensitivity (mv/mM)bEnhancement factor, (A)/(B)(A) Observed in FIA system(B) CalculatedaBrO3-10.6 × 10331.3 (m=6)338Cr2O72-2.6 × 10331.3 (m=6)83H2O22.5 × 102 c10.4 (m=2)24ClO2-6.9 × 10320.9 (m=4)339O38.0 × 10210.4 (m=2)77aSensitivity calculated from (6).bBuffer, consisting of 0.01 M Fe(III)-0.01 M Fe(II) containing 0.4 M NaBr and 1.2 M H2SO4, was used as the reagent solution.cBuffer containing 0.5% ammonium molybdate to above buffer was used.Other reducing sugars, in addition to glucose (2-deoxy-D-ribose, L-rhamnose, D-ribose, and D-mannose as monosaccharides, and cellobiose, maltose, and lactose as disaccharides), were also determined by the same proposed FA method [20]. The sensitivity of the disaccharides was higher by about 1.5-fold than that of monosaccharides, although there are somewhat sensitivity differences among disaccharides and monosaccharides. The reason for difference in sensitivity between monosaccharides and disaccharides is not clear at this stage.The separate determination of mixtures of reducing sugars was achieved by combining proposed FIA method with HPLC as a postcolumn technique [22]. In this case, the sugars were converted to borate complexes by dissolving them in a borate solution, which was used as an eluent, followed by separation on an anion-exchange column. The lower detection limit of reducing sugars was as low as 0.4–2.0 μM for an injection of 20 μL sample. The sensitivity of the proposed potentiometric method is similar or higher than corresponding values for amperometric, fluorometric, and spectrophotometric detection methods. Furthermore, it was possible to simultaneously determine sucrose and glucose using the proposed FIA method, by incorporating a bypass coil connected with invertase-immobilized column in parallel [23].As an application for the determination of reducing sugars, the determination of amylase activity [24] was carried out by utilizing the redox reaction of Fe(CN)63- with reducing sugars, produced by the enzymatic hydrolysis (37°C) of starch with amylase. The flow system consisted of three streams, a carrier stream of water, a stream of 10 mM soluble-starch (pH: 5.0), and a stream of an  Fe(CN)63--Fe(CN)64-  potential buffer solution. It was possible to determine 15 samples/h with good reproducibility, although about 6 min from sample injection to the detection of a peak maximum in the flow system was required. Amylase in a wide activity concentration range (10−2 U mL−1–10−4 U mL−1) could be determined by appropriate selection of the concentration of the potential buffer (10−3 M–10−5 M). The proposed FIA method was applied to the determination of amylase in digestive medicines from five pharmaceutical companies. The analytical results obtained using the proposed method were in good agreement with those obtained using the official titrimetric method (modified Somogyi method) within relative errors of 4.5–8.7%. No significant interference was observed in the digestive medicines examined in this study.The determination of metal ions such as manganese(II) and cobalt(II) was found to be possible using the sameFe(CN)63--Fe(CN)64- potential buffer as was used for reducing sugars [25]. The flow system of the proposed FIA method consisted of two-channel streams, a water and the  Fe(CN)63--Fe(CN)64- potential buffer (pH: 8.0) containing 0.2 M ammonium citrate and 0.01 M NaOH. The addition of ammonium citrate to the potential buffer in alkaline media accelerated the reaction of manganese(II) or cobalt(II) with Fe(CN)63-. However, the reactivity of Fe(CN)63- with manganese(II) and cobalt(II), respectively, was quite different in various pH media and that of Fe(CN)63- with manganese(II) was much higher than that with cobalt(II). Hence, the selective determination of manganese(II), even in the presence of cobalt(II), the concentration of which was 50-fold that of Mn(II), was possible by selecting reaction conditions near pH 8. During our studies of the effects of several metal ions on the determination of manganese(II) by the proposed FIA method, the tolerated concentrations of coexisting metal ions for the determination of 3×10-6 M Mn(II) were determined to be 3×10-3 M for Ca(II), Mg(II), and Ni(II), 1.5×10-3 M for Cu(II), Zn(II), and Al(III), and 3×10-4 M for Cr(III) and Fe(III). The lower detection limit for manganese(II) was 1×10-7 M, and the proposed method provided almost the same sensitivity compared with the other flow injection technique. Manganese(II) in soils is known to be one of essential components for plant growth.  The proposed method was applied to the determination of manganese(II) levels in four soil samples obtained from a tea field. The analytical results obtained by the proposed method were in good agreement with those obtained using atomic absorption spectrometry. The contents (mg g−1 soil) of the main coexisting metals in the soil samples were magnesium (ca. 15), calcium (ca. 14), aluminum (ca. 145), and iron (ca. 45), as determined by inductively coupled plasma spectrophotometry. Thus, the proposed method would be useful for monitoring manganese(II) in environmental samples, such as sea water and raw water, judging from the concentration of various coexisting metal ions that can be tolerated.


### 5.3. Analysis of Phenol Using a Bromine-Bromide Potential Buffer and a Combined Platinum Electrode with Bromide Ion-Electrode [26, 27]

The analysis of phenols in the presence of other organic compounds can be typically achieved  by titrimetry utilizing bromination reactions. In this proposed method, phenol is determined via a bromination reaction with a bromine-bromide potential buffer solution in the stream, where a combined electrode detector consisting of a platinum electrode and a bromide-selective electrode instead of the silver/silver chloride reference electrode shown in Figure1 was used for detecting the change in bromine concentration [26]. The bromination reaction is expressed by (15)C6H5OH+3Br2⟶C6H2Br3OH+3HBr
When the bromination reaction reaches completion, according to (15), the potential change (ΔE) of the combined electrode is expressed as follows from Nernstian equations for both electrodes:(16)ΔE=29.5log⁡⁡{([Br2]0-3[C6H5OH]0)[Br2]0}(mV),
where [Br2]0 and [C6H5OH]0 are the initial concentrations of bromine and phenol, respectively. The theoretical calibration curve (i.e., the case of a complete reaction) calculated from (16) became concave. However, assuming a second-order reaction on a transient reaction between phenol and bromine in a large excess of sulfuric acid, the relationship between ΔE and [C6H5OH]0 is approximately linear, when the amount of bromine reacted is smaller than ca. 38% against the initial concentration of bromine. Thus, the analysis was conducted by utilizing the detection of the transient potential change in the initial stage of the bromination of phenol in a flow system. As the standard conditions in the flow system, when the reagent solution (R.S.) was used 1.5×10-5 M Br2–0.4 M Br− containing 0.2 M H2SO4, a linear relationship between peak signals and phenol concentration can be seen in the range of 5×10-6 M to 2.5×10-5 M. Incidentally, the transient reaction in (15) was confirmed to be a second-order reaction by stopped-flow spectrophotometry [26].The proposed method can also be used for the determination of other phenols, includingp-nitrophenol, p-chlorophenol, β-naphthol, and m-cresol and was further applied to the separate determination of phenols by combining the proposed FIA method with HPLC, as a postcolumn technique [27].


## 5.1. Analyses of Concentrated Hydrogen Peroxide and Ethanol in Alcoholic Beverages Using Fe(III)-Fe(II) Potential Buffer [17–19]

Concentrated hydrogen peroxide is used in the breaching of pulp and textiles and for washing silicon wafers. For process control in the production of hydrogen peroxide in the pulp and semiconductor industries, the determination of concentrated hydrogen peroxide is routinely carried out by titrimetry after a moderate sample dilution procedure. However, a more rapid method for the determination of concentrated hydrogen peroxide would be desirable, because titrimetry is tedious and time-consuming. The determination of hydrogen peroxide was proposed by using the Fe(III)-Fe(II) couple in an acidic solution as the potential buffer solution, according to (11)H2O2+2Fe2++2H+⟶2Fe3++2H2O
In the flow system, an analyte at high concentration can be determined by utilizing the controlled dispersion of the sample zone, and its dispersion depends on the sample volume and coil length (residence time) from the injector to the detector. In this method [17], which does not require any sample dilution, the determination of hydrogen peroxide in concentrations of up to ~10 M (30%) was successfully achieved using a 0.4 M Fe(III)-0.4 M Fe(II) potential buffer containing 1 M H2SO4, where the sample could be diluted by ca. 80-fold by injecting a very small volume to 1 μL and by setting the residence time of the sample zone to 1 min, as a standard procedure in flow system. Even in such a high dispersion system, the R.S.D for the determination of 9.86 M H2O2 was 0.7% (n=10). A sampling rate of ~30 h−1 was possible at the present flow condition. The proposed method could be used in the online monitoring of the production of hydrogen peroxide, as well as for bleaching and washing processes which use concentrated hydrogen peroxide.An accurate and selective determination method for the ethanol content in alcoholic beverages usually involves the use of a gas chromatographic technique or a specific-gravity method (currently, the official method in Japan). However, a simpler, rapid, and selective method is possible using a flow-injection technique, in which the alcohol is separated using a porous membrane. In this method, the selective determination method of ethanol in alcoholic beverages (Japanese sake, beer, wine, whisky, and shochu) was proposed, using the Fe(III)-Fe(II) potential buffer solution and a gas-diffusion unit equipped with a membrane [19]. The flow injection manifold, equipped for gas-diffusion separation is shown in Figure 3. The gas-diffusion separation unit (G.D.) is comprised of two Daiflon blocks furnished with a shallow groove (37 mm long, 3 mm wide, 0.5 mm deep) and separated by a porous poly (tetrafluoroethylene) (PTFE) plane membrane, which allows the transfer of ethanol from a stream of C.S. to a stream of R.S.1. The PTFE membrane is 50 μm thick, with a pore size of 0.4 μm. The method is based on the detection of the composition change of the Fe(III)-Fe(II) couple in the potential buffer, caused by the reduction of acidic dichromate by ethanol that had permeated through a membrane as vapor, according to (12)3C2H5OH+2Cr2O72-+16H+⟶3CH3COOH+4Cr3++11H2O(13)Cr2O72-+6Fe2++14H+⟶2Cr3++6Fe3++7H2OFigure 3
Flow-injection manifold equipped with a gas-diffusion separation unit for the determination of ethanol and calibration peaks for ethanol. C.S: carrier (H2O): R.S.1: reagent solution (0.015 M K2Cr2O7, 2 M H2SO4); R.S.2: reagent solution (0.135 M Fe(NH4)2SO4); S: sample injector (140 μL); G.D: gas-diffusion separation unit; R.C.1: reaction coil (1 m, 0.5 mm); R.C.2: reaction coil (2 m, 0.5 mm); B.P.C: back pressure coil (10 m, 0.5 mm).The PTFE membrane for the separation of alcohol was superior to a poly(substituted-acetylene)/polysiloxane graft copolymer membrane [18], because of the high permeability of alcohol and the simplicity of the manifold. The flow injection peaks for a calibration curve were obtained in the ethanol concentration range from 5 to 40% (v/v) using the flow condition indicated in Figure 3. Sampling rate was ~25 h−1. The analytical results for the ethanol content in alcoholic beverages determined by the proposed method were in good agreement with data obtained by either the specific-gravity method or a gas chromatographic method, as shown in Table 1. The R.S.D for the proposed method was smaller than those by the other methods.Table 1
Determination of ethanol content in alcoholic beverages.
Ethanol content, % (v/v)Certified valueSpecific gravity methodGC methodFIA method (without G.D.)Proposed method (G.D.)Beera 4.54.54.36.64.4Wine <1411.516.511.5Sake 16-1716.816.019.516.1Whisky 4342.542.642.6Shochu 2524.524.625.0aThe sample was debubbled for 20 min before analysis.Incidentally, when the FIA technique was employed without using the G.D., positive errors of 20–30% were observed for Japanese sake, beer, and wine, which also contain compounds such as sugars, organic acids, and amino acids, which are also oxidized by the dichromate solution.


## 5.2. Analyses of Reducing Sugars, Amylase, and Manganese(II) Using anFe(CN)63--Fe(CN)64- Potential Buffer [20–25]

The redox coupleFe(CN)63--Fe(CN)64- has a lower redox potential of 0.36 V and is known to show unique redox behavior in the presence of reducing sugars. The redox electrode shows a stable potential to the Fe(CN)63--Fe(CN)64- couple in alkaline media, but is not stable in neutral to acidic solution because the auto-oxidation of Fe(CN)64- to Fe(CN)63- occurs in such media. The redox electrode also showed a Nernstian response even at lower concentrations of  Fe(CN)63--Fe(CN)64- potential buffer down to 10−5 M in alkaline media. Thus, it would be expected that system could be used in the sensitive determination of certain compounds and could also be used in a wide concentration range of analytes, as described above.For an example of an analysis utilizing a change in the composition of theFe(CN)63--Fe(CN)64- potential buffer, an analytical method for reducing sugars [20] was proposed based on the reaction of a reducing sugar with of  Fe(CN)63- in alkaline solution, according to (14)Reducing sugar+mFe(CN)63-⟶mFe(CN)64-+other products
where m is the number of moles required to oxidize one mole of reducing sugar.In the case for the determination of glucose [21], the concentration of NaOH in the potential buffer and the temperature of the reaction, as a standard procedure in flow system shown in Figure 1, were 0.6 M and 85°C, respectively. These conditions were selected for showing the highest sensitivity by changing the NaOH concentration from 0.01 M to 1.0 M and the temperature from 50°C to 90°C. The time required for a reaction between glucose and Fe(CN)63- to be completed is about 2.5 min and m values of Fe(CN)63- for the oxidation of 1 mol glucose was 6, as calculated from response potential(ΔE) after completion of the reaction. The total time required was about 4.2 min from sample injection (140 μL) to the detection of a peak maximum in the flow system. FIA peaks for injections at 2 min intervals were reproducible, and, as a result, it is possible to analyze 30 samples/h using the proposed procedure. Table 2 lists the sensitivity values and measurable concentration ranges for various concentrations of buffer solutions. The sensitivity increased with decreasing concentration of buffer solution. A sample in the concentration range from 10−7 M to 10−3 M could be determined by changing the concentration of the  Fe(CN)63--Fe(CN)64- potential buffer solution from 1×10-5 M to 1×10-2 M. For the 1×10-5 M  Fe(CN)63--Fe(CN)64- potential buffer, the fluctuations and drifts in the baseline potential were within 0.3 mV and less than 0.8 mV/h, respectively, and the lowest detectable concentration was 0.1 μM (peak heights: 0.6 mV). When the concentration of the potential buffer was lower than 5×10-6 M, the drift and fluctuation of the baseline potential became larger, and peak heights were not reproducible. The high sensitivity of the proposed FIA method can be attributed to, in part, the high stability of the electrode potentials in buffer solutions at low concentrations.Table 2
Effect of concentrations ofFe(CN)63--Fe(CN)64- potential buffer solution on sensitivity.
Concentration      (M)Sensitivitya (mV mM−1)Measurable concentration range (M)1×10-29.72.0×10-4~1.8×10-31×10-39.5×102.0×10-5~1.8×10-41×10-49.4×1022.0×10-6~1.8×10-55×10-51.9×1031.0×10-6~1.0×10-51×10-56.2×1032.5×10-7~2.5×10-6aSensitivity: slope of calibration curve (peak height/mV obtained by injection of 1 mM glucose).Table 3
Sensitivities to oxidative species.
Oxidative speciesSensitivity (mv/mM)bEnhancement factor, (A)/(B)(A) Observed in FIA system(B) CalculatedaBrO3-10.6 × 10331.3 (m=6)338Cr2O72-2.6 × 10331.3 (m=6)83H2O22.5 × 102 c10.4 (m=2)24ClO2-6.9 × 10320.9 (m=4)339O38.0 × 10210.4 (m=2)77aSensitivity calculated from (6).bBuffer, consisting of 0.01 M Fe(III)-0.01 M Fe(II) containing 0.4 M NaBr and 1.2 M H2SO4, was used as the reagent solution.cBuffer containing 0.5% ammonium molybdate to above buffer was used.Other reducing sugars, in addition to glucose (2-deoxy-D-ribose, L-rhamnose, D-ribose, and D-mannose as monosaccharides, and cellobiose, maltose, and lactose as disaccharides), were also determined by the same proposed FA method [20]. The sensitivity of the disaccharides was higher by about 1.5-fold than that of monosaccharides, although there are somewhat sensitivity differences among disaccharides and monosaccharides. The reason for difference in sensitivity between monosaccharides and disaccharides is not clear at this stage.The separate determination of mixtures of reducing sugars was achieved by combining proposed FIA method with HPLC as a postcolumn technique [22]. In this case, the sugars were converted to borate complexes by dissolving them in a borate solution, which was used as an eluent, followed by separation on an anion-exchange column. The lower detection limit of reducing sugars was as low as 0.4–2.0 μM for an injection of 20 μL sample. The sensitivity of the proposed potentiometric method is similar or higher than corresponding values for amperometric, fluorometric, and spectrophotometric detection methods. Furthermore, it was possible to simultaneously determine sucrose and glucose using the proposed FIA method, by incorporating a bypass coil connected with invertase-immobilized column in parallel [23].As an application for the determination of reducing sugars, the determination of amylase activity [24] was carried out by utilizing the redox reaction of Fe(CN)63- with reducing sugars, produced by the enzymatic hydrolysis (37°C) of starch with amylase. The flow system consisted of three streams, a carrier stream of water, a stream of 10 mM soluble-starch (pH: 5.0), and a stream of an  Fe(CN)63--Fe(CN)64-  potential buffer solution. It was possible to determine 15 samples/h with good reproducibility, although about 6 min from sample injection to the detection of a peak maximum in the flow system was required. Amylase in a wide activity concentration range (10−2 U mL−1–10−4 U mL−1) could be determined by appropriate selection of the concentration of the potential buffer (10−3 M–10−5 M). The proposed FIA method was applied to the determination of amylase in digestive medicines from five pharmaceutical companies. The analytical results obtained using the proposed method were in good agreement with those obtained using the official titrimetric method (modified Somogyi method) within relative errors of 4.5–8.7%. No significant interference was observed in the digestive medicines examined in this study.The determination of metal ions such as manganese(II) and cobalt(II) was found to be possible using the sameFe(CN)63--Fe(CN)64- potential buffer as was used for reducing sugars [25]. The flow system of the proposed FIA method consisted of two-channel streams, a water and the  Fe(CN)63--Fe(CN)64- potential buffer (pH: 8.0) containing 0.2 M ammonium citrate and 0.01 M NaOH. The addition of ammonium citrate to the potential buffer in alkaline media accelerated the reaction of manganese(II) or cobalt(II) with Fe(CN)63-. However, the reactivity of Fe(CN)63- with manganese(II) and cobalt(II), respectively, was quite different in various pH media and that of Fe(CN)63- with manganese(II) was much higher than that with cobalt(II). Hence, the selective determination of manganese(II), even in the presence of cobalt(II), the concentration of which was 50-fold that of Mn(II), was possible by selecting reaction conditions near pH 8. During our studies of the effects of several metal ions on the determination of manganese(II) by the proposed FIA method, the tolerated concentrations of coexisting metal ions for the determination of 3×10-6 M Mn(II) were determined to be 3×10-3 M for Ca(II), Mg(II), and Ni(II), 1.5×10-3 M for Cu(II), Zn(II), and Al(III), and 3×10-4 M for Cr(III) and Fe(III). The lower detection limit for manganese(II) was 1×10-7 M, and the proposed method provided almost the same sensitivity compared with the other flow injection technique. Manganese(II) in soils is known to be one of essential components for plant growth.  The proposed method was applied to the determination of manganese(II) levels in four soil samples obtained from a tea field. The analytical results obtained by the proposed method were in good agreement with those obtained using atomic absorption spectrometry. The contents (mg g−1 soil) of the main coexisting metals in the soil samples were magnesium (ca. 15), calcium (ca. 14), aluminum (ca. 145), and iron (ca. 45), as determined by inductively coupled plasma spectrophotometry. Thus, the proposed method would be useful for monitoring manganese(II) in environmental samples, such as sea water and raw water, judging from the concentration of various coexisting metal ions that can be tolerated.


## 5.3. Analysis of Phenol Using a Bromine-Bromide Potential Buffer and a Combined Platinum Electrode with Bromide Ion-Electrode [26, 27]

The analysis of phenols in the presence of other organic compounds can be typically achieved  by titrimetry utilizing bromination reactions. In this proposed method, phenol is determined via a bromination reaction with a bromine-bromide potential buffer solution in the stream, where a combined electrode detector consisting of a platinum electrode and a bromide-selective electrode instead of the silver/silver chloride reference electrode shown in Figure1 was used for detecting the change in bromine concentration [26]. The bromination reaction is expressed by (15)C6H5OH+3Br2⟶C6H2Br3OH+3HBr
When the bromination reaction reaches completion, according to (15), the potential change (ΔE) of the combined electrode is expressed as follows from Nernstian equations for both electrodes:(16)ΔE=29.5log⁡⁡{([Br2]0-3[C6H5OH]0)[Br2]0}(mV),
where [Br2]0 and [C6H5OH]0 are the initial concentrations of bromine and phenol, respectively. The theoretical calibration curve (i.e., the case of a complete reaction) calculated from (16) became concave. However, assuming a second-order reaction on a transient reaction between phenol and bromine in a large excess of sulfuric acid, the relationship between ΔE and [C6H5OH]0 is approximately linear, when the amount of bromine reacted is smaller than ca. 38% against the initial concentration of bromine. Thus, the analysis was conducted by utilizing the detection of the transient potential change in the initial stage of the bromination of phenol in a flow system. As the standard conditions in the flow system, when the reagent solution (R.S.) was used 1.5×10-5 M Br2–0.4 M Br− containing 0.2 M H2SO4, a linear relationship between peak signals and phenol concentration can be seen in the range of 5×10-6 M to 2.5×10-5 M. Incidentally, the transient reaction in (15) was confirmed to be a second-order reaction by stopped-flow spectrophotometry [26].The proposed method can also be used for the determination of other phenols, includingp-nitrophenol, p-chlorophenol, β-naphthol, and m-cresol and was further applied to the separate determination of phenols by combining the proposed FIA method with HPLC, as a postcolumn technique [27].


## 6. Analyses Utilizing a Large Transient Potential Change Caused by a Complex Redox Reaction

### 6.1. Analysis of Bromate Using Fe(III)-Fe(II) Potential Buffer Containing Bromide [28–30]

Bromate is employed as bleaching agent for some food products and is known to be generated as a byproduct in water purification processes. Thus, the sensitive determination of residual bromate in foods or tap water would be desirable for the safety of food products and water quality. In a batchwise experiment [28], the time course for the response potential after the addition of bromate to a potential buffer consisting of Fe(III)-Fe(II) containing bromide showed a mountain-shaped form, as shown in Figure 2. The large transient potential process which is due to bromine, generated as an intermediate, can be expressed by the following reactions, as described in Section 4.2:(17)BrO3-+5Br-+6H+⟶3Br2+3H2O(18)BrO3-+5Fe2++6H+⟶12Br2+5Fe3++3H2O(19)12Br2+Fe2+⟶Br-+Fe3+(20)BrO3-+6Fe2++6H+⟶Br-+6Fe3++3H2O(21)ΔE=59log⁡⁡{(1+6[BrO3-]0/[Fe3+]0)(1-6[BrO3-]0/[Fe2+]0)}.
The overall reaction, which is the sum of elementary reactions (17), (18), and (19), is given by (20). The equilibrium potential, normalized by the concentration of bromate, as observed from the time course agreed well with the value (31.3 mV/mM, Table 2) calculated from (2). In a transient potential, the maximum change of 20–30 mV was found for a 10−6 M concentration of bromate, when a 1×10-2 M potential buffer containing 0.4 M bromide and 1 M sulfuric acid was used. Since sensitivity enhancement would be expected if a transient potential change could be determined in a timely manner, a flow system was then designed to detect the maximum potential. As a result, a linear calibration for bromate was obtained at a level of 10−6 M with a sensitivity (mV/mM) of 10.6×103. This sensitivity was enhanced by 338-fold compared with that using the change in equilibrium potential, as shown in Table 3. The detection limit (S/N = 3) was 5×10-8 M. The sampling rate was ca. 35 samples/h.Evidence that the origin of the large transient potential change with a mountain-shaped form was the formation and reduction of bromine as an intermediate was confirmed by stopped-flow spectrophotometry [29]. Concretely, in order to confirm the putative reaction pathway and the rate of the reactions (17), (18), (19), the overall reaction rate among BrO3-, Fe2+, and Br− in sulfuric acid solution and reaction rates of each steps (17), (18), (19) were determined by measuring the bromine concentration. The change in absorbance at 447 nm was used for the determination of bromine. The bromine concentration-time relation for the absorbance change during the reaction among BrO3-, Fe2+, and Br− in sulfuric acid solution showed a mountain-shaped form and was in good agreement with that calculated from an equation for a successive first-order reaction using the rates of reactions in (17), (18), and (19). Thus, for the transient potential change, it was verified experimentally that the potential change, namely, the peak height, is proportional to the initial concentration of bromate in a constant reaction time.Furthermore, repetitive determinations of a large number of trace samples of bromate were proposed by the circulating (closed-loop) FIA (CFIA), which is more suited to the concept of the Zero Emission Research Initiative [30]. The equilibrium potential obtained via the large transient potential change was nearly equal to the initial potential because the concentration of Fe(III)-Fe(II) in the potential buffer was sufficiently higher than that of bromate in the sample. For example, even when a 7.0 μM bromate solution (5 μL) was injected 104 times (corresponding to 50 mL of 7.0 μM bromate) into the stream of the circulating reservoir solution (100 mL) containing 1×10-2 M Fe(III)-Fe(II) and 0.35 M sodium bromide, the concentration change from Fe(II) to Fe(III) was calculated to be only 0.21%, based on (20). This indicates that the change in potential from the initial potential was less than 0.11 mV, as calculated from (21), taking into account the increase in the reservoir volume. Therefore, very large numbers of repetitive determinations of bromate would be carried out using a small volume of reservoir solution in the CFIA system, such as that shown in Figure 4. As a result in experiments, flow signals for the four sets of calibration peaks obtained using 1×10-2 M and 1×10-3 M Fe(III)-Fe(II) potential buffer, respectively, are shown in Figures 4(A) and 4(B). Ten milliliters of a 6.0 μM solution and 5 mL of a 1.0 μM bromate solution, corresponding to 2000 and 1000 repetitive injections of 5 μL samples, respectively, were added to each reservoir after preparing appropriate calibration peaks. The sensitivities were nearly constant within 5.56–5.32 mV/μM for Figures 4(A)(a)–(c) and 30.9–29.5 mV/μM for Figures 4(B)(a)–(c). Thus, ca. 4000 and 2000 repetitive determinations, corresponding to each calibration in Figure 4(A)(c) and Figure 4(B)(c), in which relative sensitivities within 5% were regarded as acceptable, were possible with high reproducibility using the proposed CFIA method with only 100 mL of potential buffer solution being required. If 100 mL of potential buffer were used in the two-channel FIA method reported previously [28], only 65 samples could be determined.Figure 4
Schematic diagram of the CFIA system used in this study. R.S: reservoir (100 mL, Fe(III)-Fe(II) 0.35 M NaBr and 0.2% (NH4)6Mo7O24 in 1 M H2SO4); S: sample injection valve(5μL loop); RC: reaction coil (13 cm); BC: back pressure coil (3 m); D: the same detectors as in Figure 1. Calibration peaks (A) and (B) for bromate sample obtained by 1×10-2 M Fe(III)-Fe(II) and 1×10-3 M Fe(III)-Fe(II) potential buffer, respectively. 10 mL of 6 μM and 5 mL of 1.0 μM bromate sample solutions were added after every calibration (A) and (B), respectively.


### 6.2. Analyses of Chromium(VI) and Chromium(III) Using an Fe(III)-Fe(II) Potential Buffer Containing Bromide [31, 32]

In batchwise experiments, when chromium(VI) was added to the Fe(III)-Fe(II) potential buffer containing bromide in a sulfuric acid solution, the magnitude of the response potential with a mountain-shaped transient change as shown in Figure2 increased with increasing reaction time. The mechanism of the transient potential change can be attributed to the generation of bromine via the reaction of bromide in the potential buffer with Cr(V), which was generated as an intermediate during the reaction of Cr(VI) and Fe(II). That is, the oxidative conversion of bromide to bromine by Cr(VI) appears to have been due to  Fe(II), as evidenced by spectrophotometric studies. Thus, the transient potential process can be expressed by (22) and (23). The decrease in potential after a maximum is explained by the progress of reaction (19), that is, the bromine generated in reaction (23) is subsequently consumed:(22)Cr(VI)+Fe2+⟶Cr(V)+Fe3+(23)Cr(V)+2Br-⟶Cr(III)+Br2In the flow system used for the determination of Cr(VI), a two-channel flow system shown Figure1 was then designed to detect the maximum transient potential [31]. As a result, a linear calibration for chromium(VI) was obtained at a level of 10−6 M with a sensitivity (mV/mM) of 2.6×103. This sensitivity was enhanced by 83-fold compared to that based on the change in equilibrium potential, as shown in Table 2. A detection limit of 2×10-8 M Cr(VI) was achieved using a 1×10-4 M Fe(III)-Fe(II) potential buffer containing 0.4 M NaBr and 1.2 M H2SO4. The R.S.D. was 0.6% (n=6) for the determination of 1×10-6 M Cr(VI) with a sampling rate of ca. 40 h−1. A variety of heavy metal ions, including Cr(III), Cu(II), Zn(II), Ni(II), and Cd(II), did not interfere with the determination of Cr(VI) even in the case where their concentration exceeded 102 times that of Cr(VI). The proposed method was designed to meet the Japan standards level for Cr(VI) in effluent water (500 ppb) and was sufficiently sensitive to use for the precise determination of Cr(VI) at the 100 ppb level in an actual seawater sample containing Cr(VI) at the 100 ppb level.The simultaneous determination of chromium(VI) and chromium(III) in a mixed sample was achieved using a three-channel flow system equipped with a six-way valve, as shown in Figure5 [32]. The three-channel streams consisted of carrier (water), a reagent (H2SO4 solution or Ce(IV) solution containing H2SO4), and the Fe(III)-Fe(II) potential buffer containing bromide. The six-way valve was used to switch the two reagent streams between the H2SO4 solution for the selective determination of Cr(VI) in the sample containing solutions of Cr(III) and Ce(IV) in H2SO4 in order to oxidize Cr(III) to Cr(VI) by Ce(IV) thus permitting the determination of total chromium, as the the sum of Cr(VI) and Cr(III). The determination of Cr(III) in a mixed sample was achieved from the difference in peak height obtained for the two reagent streams. The detection of Cr(VI) was based on the measurement of a large transient potential change due to the generation of bromine by (22) and (23). A linear calibration was obtained over the range of 1×10-6 M to 1×10-5 M for Cr(VI) and from 4×10-6 M to 4×10-5 M for Cr(III).Figure 5
Schematic diagram for the simultaneous determination of Cr(VI) and Cr(III) and flow injection peaks of  Cr(VI) ((A), (B)) for different reagent solutions and of Cr(III) (C). C.S: carrier stream (water); R.S.1: reagent solution 1 (0.05 M H2SO4); R.S.2: reagent solution 2 (2×10-4 M Ce(IV), 0.05 M H2SO4); R.S.3: potential buffer solution (1×10-2 M Fe(III)-Fe(II) 0.6 M NaBr, 3.6 M H2SO4); R.C.1: reaction coil 1 (230 cm); R.C.2: reaction coil 2 (75 cm); B: switching six-way valve.


### 6.3. Analyses of Trace Hydrogen Peroxide and Other Oxidative Species Using Fe(III)-Fe(II) Potential Buffer Containing Bromide [33, 34]

As described in Section5.1, the determination of high concentrations of hydrogen peroxide by utilizing a large dispersion of a sample zone was achieved using a stream of an Fe(III)-Fe(II) potential buffer without bromide. While the use of a stream of an Fe(III)-Fe(II) potential buffer containing bromide and Mo(VI) enhanced the sensitivity of the method for hydrogen peroxide, a highly sensitive determination of trace levels of hydrogen peroxide was achieved by detecting the large transient potential change due to the production of bromine as an intermediate [33]. The oxidation of bromide to bromine by hydrogen peroxide occurred very rapidly with the assistance of Mo(VI) when Fe(II) was present in the potential buffer in a similar manner to that when bromide is oxidized by Cr(V) in the presence of Fe(II), as discussed above. The reaction mechanism for the transient potential change was estimated by batchwise experiments in which hydroxyl radicals, OH∙, were generated by the reaction of hydrogen peroxide with Fe(II) as an intermediate, and the bromide subsequently oxidized to bromine. The elementary reactions for the transient process can be expressed by (24) and (25) for the generation of bromine and (19) for the consumption of bromine. The overall reaction, which is the sum of reactions (24), (25), and (19), is expressed by reaction (26). That is, the presence of bromide in the potential buffer functions as a homogeneous catalyst for the formation and reduction of bromine:(24)H2O2+Fe2++H+⟶OH∙+Fe3++H2O(25)OH∙+Br-+H+⟶12Br2+H2O(26)H2O2+2Fe2++2H+⟶2Fe3++2H2O
In the flow system involving the detection of a large transient potential change, the sensitivity to hydrogen peroxide was enhanced by 24-fold compared with that obtained by the detection of the equilibrium potential, as shown in Table 3. The detection limit of 4×10-7 M (13.6 ppb) was achieved using a 1×10-4 M Fe(III)-Fe(II) buffer containing 0.4 M NaBr, 1.0 M H2SO4, and 0.5% (NH4)6Mo7O24.Trace amounts of hydrogen peroxide in rainwater play a role in the formation of acid rain.  As a result, the development of an analytical method for hydrogen peroxide is an important aspect of atmospheric environmental analysis. This method was applied to the determination of hydrogen peroxide in actual samples of rainwater and was found to provide a good recovery for H2O2 added to rainwater samples.Other oxidative species such as chlorite and ozone were also determined by the detection of large transient potential changes [34]. The sensitivities to oxidative species examined in this work increased in the order H2O2 < O3 < Cr(VI) < ClO2- < BrO3-, as shown in Table 3. This sequence of sensitivity most likely depends on the rate of reaction of oxidative species with bromide.


### 6.4. Analyses of Residual Chlorine and Oxychlorine Species Using Fe(III)-Fe(II) Potential Buffer Containing Chloride [35, 36]

Since oxychlorinated species are considered to be hazardous to human health, the monitoring of levels of residual oxychlorines in drinking water is important for health safety. Furthermore, since HClO andClO2- are unstable and easily decomposed by air oxidation, a rapid analytical method that can be operated in a substantially closed system is desirable. A large transient potential change was observed by the generation of chlorine based on (27), (28), and (29) when oxychlorine species, ClO3-, ClO2-, and HClO, were added to an Fe(III)-Fe(II) potential buffer containing chloride, although the magnitude of the potential change was dependent on the reactivity of the oxychlorines. It is noteworthy that the rate of reaction (29) was relatively slower than that of reactions (27) and (28):     (27)HClO+Cl-+H+⟶Cl2+H2O(28)HClO2+3Cl-+3H+⟶2Cl2+2H2O(29)ClO3-+5Cl-+6H+⟶3Cl2+3H2OIn the FIA system, the analytical sensitivity to HClO andClO2- obtained by the detection of a transient potential change, where an Fe(III)-Fe(II) potential buffer containing chloride was used, was enhanced by ~700-fold compared with that obtained using an equilibrium potential, as shown in Table 4. The detection limits for HClO and ClO2-were 5×10-8 M, when a potential buffer consisting of 5×10-4 M Fe(III)-1×10-3 M Fe(II), 0.3 M KCl and 0.5 M H2SO4 (buffer-A) was used. For the determination of ClO3-, a concentration of 10−5 M was detected when 9 M H2SO4 was added to buffer-A, instead of 0.5 M H2SO4, as shown in the bottom line in Table 4.Table 4
Sensitivities to oxychlorine species.
Oxychlorine speciesSensitivity (mV/mM)Enhancement factor, (A)/(B)(A) Observed in  FIA system(B) CalculatedaHClO1.2 × 10415 (m= 2)800ClO2-2.1 × 10430 (m = 4)700ClO3-3.445 (m = 6)0.08ClO3-4.3 × 102 b45 (m = 6)9.8aSensitivity calculated from (6) using 5×10-3 M Fe(III)-1×10-2 M Fe(II).bSlope of the calibration curve observed in the FIA system with buffer-A containing 9.0 M H2SO4 and reaction coil of 200 cm in length.The simultaneous determination ofClO3--ClO2- or ClO3--HClO (for the case of [ClO3-] > [HClO] and [ClO3-] > [ClO2-]) was achieved using a flow system with dual detectors, as shown in Figure 6(A), where the differences in reactivity of the oxychlorine species with chloride in two potential buffers containing different concentrations of sulfuric acid were utilized. Figures 6(B)(a) and 6(B)(b) show the calibration peaks for ClO3- obtained using detector D1 and for ClO2- obtained using detector D2, respectively, where the mixed sample solutions contained at different concentration but the same molar ratio of [ClO3-]/[ClO2-] was 25. Figure 6(B)(c) and 6(B)(d) show the calibration peaks for ClO3- obtained using detector D1 and for HClO obtained using detector D2, respectively, where the concentrations of the mixed sample solutions were different but the molar ratio of [ClO3-]/[HClO] was the same, that is, 16.7. The method was applied to the determination of residual chlorine in a tap water sample containing a large amount of chlorate and was found to provide an analytical result for HClO, which was in good agreement with that obtained by the o-tolidine method. The presence of monochloramine interfered with the determination HClO, since the sensitivity of this method to monochloramine was one-fifth of that to HClO.Figure 6
(A) Schematic diagram of a three-channel FIA system for the determination ofClO3--ClO2- or ClO3--HClO∙ (for the case of [ClO3-]>[HClO] and [ClO3-]>[ClO2-]). R.S.1: 5×10-3 M Fe(III)- 1×10-2 M Fe(II), 0.3 M KCl and 9 M H2SO4; R.S.2: 5×10-3 M Fe(III)- 1×10-2 M Fe(II), 0.3 M KCl and 0.3 M H2SO4. D1 and D2: the same detectors as in Figure 1. (B) Calibration peaks ((a), (b)) for ClO3- and ClO2- obtained using detectors D1 and D2, respectively. Concentrations of ClO3- and ClO2- in the mixed sample are indicated in the figure. Calibration peaks ((c), (d)) for ClO3- and HClO obtained with detector D1 and D2, respectively. Concentrations of ClO3- and HClO in the mixed sample are indicated in the figure.Furthermore, under the condition of[ClO3-]≅ [HClO] and [ClO3-]≅[ClO2-], the simultaneous determination of mixed oxychlorines was conducted using a four-channel flow system equipped with a cation-exchange column in the Fe(II) form.


### 6.5. Analysis of Hydrazine Using a Ce(IV)-Ce(III) Potential Buffer [37]

The determination of sub-micromolar levels of hydrazine (N2H4) was accomplished using a two-channel flow system with a Ce(IV)-Ce(III) couple in acidic solution instead of the Fe(III)-Fe(II) couple as a potential buffer solution. The method is based on the measurement of a transient potential change, which appeared in a negative direction. The shape of the transient potential change for hydrazine was different from that observed in the determination of bromate, Cr(VI), and oxychlorine:(30)N2H5+⇄N2H4+H+K=1.02×10-8(31)N2H5+⇄N2H4+2H++e-Eo>-0.6V(32)(H++N2H3⇄12N2+NH4+)Ce(IV)+e-⇄Ce(III)(1MH2SO4)E0=1.44V(33)Ce(IV)+N2H5+⟶12N2+Ce(III)+NH4++H+
We examined the reaction mechanism for reactions (30), (31), and (32) by spectrophotometric and potentiometric batch experiments, in which the transient potential change was the potential shift from the Ce(IV)-Ce(III) couple to the N2H5+-N2 couple, using a much lower electrode potential during the reaction of hydrazine with Ce(IV). The overall reaction which is the sum of elementary reactions (31) and (32) can be expressed by (33). The flow system was designed so as to detect the maximum of the transient potential change. Hydrazine, in a wide range of concentrations from 10−7 M to 10−3 M was determined by appropriately adjusting the concentration of the potential buffer from 10−4 M to 10−2 M, and the detection limit was found to be 1×10-7 M (3.2 ppb) when a 2×10-4 M Ce(IV)-Ce(III) potential buffer was used. The method was capable of determining the concentration of hydrazone in boiler water at the 10 ppb level.


## 6.1. Analysis of Bromate Using Fe(III)-Fe(II) Potential Buffer Containing Bromide [28–30]

Bromate is employed as bleaching agent for some food products and is known to be generated as a byproduct in water purification processes. Thus, the sensitive determination of residual bromate in foods or tap water would be desirable for the safety of food products and water quality. In a batchwise experiment [28], the time course for the response potential after the addition of bromate to a potential buffer consisting of Fe(III)-Fe(II) containing bromide showed a mountain-shaped form, as shown in Figure 2. The large transient potential process which is due to bromine, generated as an intermediate, can be expressed by the following reactions, as described in Section 4.2:(17)BrO3-+5Br-+6H+⟶3Br2+3H2O(18)BrO3-+5Fe2++6H+⟶12Br2+5Fe3++3H2O(19)12Br2+Fe2+⟶Br-+Fe3+(20)BrO3-+6Fe2++6H+⟶Br-+6Fe3++3H2O(21)ΔE=59log⁡⁡{(1+6[BrO3-]0/[Fe3+]0)(1-6[BrO3-]0/[Fe2+]0)}.
The overall reaction, which is the sum of elementary reactions (17), (18), and (19), is given by (20). The equilibrium potential, normalized by the concentration of bromate, as observed from the time course agreed well with the value (31.3 mV/mM, Table 2) calculated from (2). In a transient potential, the maximum change of 20–30 mV was found for a 10−6 M concentration of bromate, when a 1×10-2 M potential buffer containing 0.4 M bromide and 1 M sulfuric acid was used. Since sensitivity enhancement would be expected if a transient potential change could be determined in a timely manner, a flow system was then designed to detect the maximum potential. As a result, a linear calibration for bromate was obtained at a level of 10−6 M with a sensitivity (mV/mM) of 10.6×103. This sensitivity was enhanced by 338-fold compared with that using the change in equilibrium potential, as shown in Table 3. The detection limit (S/N = 3) was 5×10-8 M. The sampling rate was ca. 35 samples/h.Evidence that the origin of the large transient potential change with a mountain-shaped form was the formation and reduction of bromine as an intermediate was confirmed by stopped-flow spectrophotometry [29]. Concretely, in order to confirm the putative reaction pathway and the rate of the reactions (17), (18), (19), the overall reaction rate among BrO3-, Fe2+, and Br− in sulfuric acid solution and reaction rates of each steps (17), (18), (19) were determined by measuring the bromine concentration. The change in absorbance at 447 nm was used for the determination of bromine. The bromine concentration-time relation for the absorbance change during the reaction among BrO3-, Fe2+, and Br− in sulfuric acid solution showed a mountain-shaped form and was in good agreement with that calculated from an equation for a successive first-order reaction using the rates of reactions in (17), (18), and (19). Thus, for the transient potential change, it was verified experimentally that the potential change, namely, the peak height, is proportional to the initial concentration of bromate in a constant reaction time.Furthermore, repetitive determinations of a large number of trace samples of bromate were proposed by the circulating (closed-loop) FIA (CFIA), which is more suited to the concept of the Zero Emission Research Initiative [30]. The equilibrium potential obtained via the large transient potential change was nearly equal to the initial potential because the concentration of Fe(III)-Fe(II) in the potential buffer was sufficiently higher than that of bromate in the sample. For example, even when a 7.0 μM bromate solution (5 μL) was injected 104 times (corresponding to 50 mL of 7.0 μM bromate) into the stream of the circulating reservoir solution (100 mL) containing 1×10-2 M Fe(III)-Fe(II) and 0.35 M sodium bromide, the concentration change from Fe(II) to Fe(III) was calculated to be only 0.21%, based on (20). This indicates that the change in potential from the initial potential was less than 0.11 mV, as calculated from (21), taking into account the increase in the reservoir volume. Therefore, very large numbers of repetitive determinations of bromate would be carried out using a small volume of reservoir solution in the CFIA system, such as that shown in Figure 4. As a result in experiments, flow signals for the four sets of calibration peaks obtained using 1×10-2 M and 1×10-3 M Fe(III)-Fe(II) potential buffer, respectively, are shown in Figures 4(A) and 4(B). Ten milliliters of a 6.0 μM solution and 5 mL of a 1.0 μM bromate solution, corresponding to 2000 and 1000 repetitive injections of 5 μL samples, respectively, were added to each reservoir after preparing appropriate calibration peaks. The sensitivities were nearly constant within 5.56–5.32 mV/μM for Figures 4(A)(a)–(c) and 30.9–29.5 mV/μM for Figures 4(B)(a)–(c). Thus, ca. 4000 and 2000 repetitive determinations, corresponding to each calibration in Figure 4(A)(c) and Figure 4(B)(c), in which relative sensitivities within 5% were regarded as acceptable, were possible with high reproducibility using the proposed CFIA method with only 100 mL of potential buffer solution being required. If 100 mL of potential buffer were used in the two-channel FIA method reported previously [28], only 65 samples could be determined.Figure 4
Schematic diagram of the CFIA system used in this study. R.S: reservoir (100 mL, Fe(III)-Fe(II) 0.35 M NaBr and 0.2% (NH4)6Mo7O24 in 1 M H2SO4); S: sample injection valve(5μL loop); RC: reaction coil (13 cm); BC: back pressure coil (3 m); D: the same detectors as in Figure 1. Calibration peaks (A) and (B) for bromate sample obtained by 1×10-2 M Fe(III)-Fe(II) and 1×10-3 M Fe(III)-Fe(II) potential buffer, respectively. 10 mL of 6 μM and 5 mL of 1.0 μM bromate sample solutions were added after every calibration (A) and (B), respectively.


## 6.2. Analyses of Chromium(VI) and Chromium(III) Using an Fe(III)-Fe(II) Potential Buffer Containing Bromide [31, 32]

In batchwise experiments, when chromium(VI) was added to the Fe(III)-Fe(II) potential buffer containing bromide in a sulfuric acid solution, the magnitude of the response potential with a mountain-shaped transient change as shown in Figure2 increased with increasing reaction time. The mechanism of the transient potential change can be attributed to the generation of bromine via the reaction of bromide in the potential buffer with Cr(V), which was generated as an intermediate during the reaction of Cr(VI) and Fe(II). That is, the oxidative conversion of bromide to bromine by Cr(VI) appears to have been due to  Fe(II), as evidenced by spectrophotometric studies. Thus, the transient potential process can be expressed by (22) and (23). The decrease in potential after a maximum is explained by the progress of reaction (19), that is, the bromine generated in reaction (23) is subsequently consumed:(22)Cr(VI)+Fe2+⟶Cr(V)+Fe3+(23)Cr(V)+2Br-⟶Cr(III)+Br2In the flow system used for the determination of Cr(VI), a two-channel flow system shown Figure1 was then designed to detect the maximum transient potential [31]. As a result, a linear calibration for chromium(VI) was obtained at a level of 10−6 M with a sensitivity (mV/mM) of 2.6×103. This sensitivity was enhanced by 83-fold compared to that based on the change in equilibrium potential, as shown in Table 2. A detection limit of 2×10-8 M Cr(VI) was achieved using a 1×10-4 M Fe(III)-Fe(II) potential buffer containing 0.4 M NaBr and 1.2 M H2SO4. The R.S.D. was 0.6% (n=6) for the determination of 1×10-6 M Cr(VI) with a sampling rate of ca. 40 h−1. A variety of heavy metal ions, including Cr(III), Cu(II), Zn(II), Ni(II), and Cd(II), did not interfere with the determination of Cr(VI) even in the case where their concentration exceeded 102 times that of Cr(VI). The proposed method was designed to meet the Japan standards level for Cr(VI) in effluent water (500 ppb) and was sufficiently sensitive to use for the precise determination of Cr(VI) at the 100 ppb level in an actual seawater sample containing Cr(VI) at the 100 ppb level.The simultaneous determination of chromium(VI) and chromium(III) in a mixed sample was achieved using a three-channel flow system equipped with a six-way valve, as shown in Figure5 [32]. The three-channel streams consisted of carrier (water), a reagent (H2SO4 solution or Ce(IV) solution containing H2SO4), and the Fe(III)-Fe(II) potential buffer containing bromide. The six-way valve was used to switch the two reagent streams between the H2SO4 solution for the selective determination of Cr(VI) in the sample containing solutions of Cr(III) and Ce(IV) in H2SO4 in order to oxidize Cr(III) to Cr(VI) by Ce(IV) thus permitting the determination of total chromium, as the the sum of Cr(VI) and Cr(III). The determination of Cr(III) in a mixed sample was achieved from the difference in peak height obtained for the two reagent streams. The detection of Cr(VI) was based on the measurement of a large transient potential change due to the generation of bromine by (22) and (23). A linear calibration was obtained over the range of 1×10-6 M to 1×10-5 M for Cr(VI) and from 4×10-6 M to 4×10-5 M for Cr(III).Figure 5
Schematic diagram for the simultaneous determination of Cr(VI) and Cr(III) and flow injection peaks of  Cr(VI) ((A), (B)) for different reagent solutions and of Cr(III) (C). C.S: carrier stream (water); R.S.1: reagent solution 1 (0.05 M H2SO4); R.S.2: reagent solution 2 (2×10-4 M Ce(IV), 0.05 M H2SO4); R.S.3: potential buffer solution (1×10-2 M Fe(III)-Fe(II) 0.6 M NaBr, 3.6 M H2SO4); R.C.1: reaction coil 1 (230 cm); R.C.2: reaction coil 2 (75 cm); B: switching six-way valve.


## 6.3. Analyses of Trace Hydrogen Peroxide and Other Oxidative Species Using Fe(III)-Fe(II) Potential Buffer Containing Bromide [33, 34]

As described in Section5.1, the determination of high concentrations of hydrogen peroxide by utilizing a large dispersion of a sample zone was achieved using a stream of an Fe(III)-Fe(II) potential buffer without bromide. While the use of a stream of an Fe(III)-Fe(II) potential buffer containing bromide and Mo(VI) enhanced the sensitivity of the method for hydrogen peroxide, a highly sensitive determination of trace levels of hydrogen peroxide was achieved by detecting the large transient potential change due to the production of bromine as an intermediate [33]. The oxidation of bromide to bromine by hydrogen peroxide occurred very rapidly with the assistance of Mo(VI) when Fe(II) was present in the potential buffer in a similar manner to that when bromide is oxidized by Cr(V) in the presence of Fe(II), as discussed above. The reaction mechanism for the transient potential change was estimated by batchwise experiments in which hydroxyl radicals, OH∙, were generated by the reaction of hydrogen peroxide with Fe(II) as an intermediate, and the bromide subsequently oxidized to bromine. The elementary reactions for the transient process can be expressed by (24) and (25) for the generation of bromine and (19) for the consumption of bromine. The overall reaction, which is the sum of reactions (24), (25), and (19), is expressed by reaction (26). That is, the presence of bromide in the potential buffer functions as a homogeneous catalyst for the formation and reduction of bromine:(24)H2O2+Fe2++H+⟶OH∙+Fe3++H2O(25)OH∙+Br-+H+⟶12Br2+H2O(26)H2O2+2Fe2++2H+⟶2Fe3++2H2O
In the flow system involving the detection of a large transient potential change, the sensitivity to hydrogen peroxide was enhanced by 24-fold compared with that obtained by the detection of the equilibrium potential, as shown in Table 3. The detection limit of 4×10-7 M (13.6 ppb) was achieved using a 1×10-4 M Fe(III)-Fe(II) buffer containing 0.4 M NaBr, 1.0 M H2SO4, and 0.5% (NH4)6Mo7O24.Trace amounts of hydrogen peroxide in rainwater play a role in the formation of acid rain.  As a result, the development of an analytical method for hydrogen peroxide is an important aspect of atmospheric environmental analysis. This method was applied to the determination of hydrogen peroxide in actual samples of rainwater and was found to provide a good recovery for H2O2 added to rainwater samples.Other oxidative species such as chlorite and ozone were also determined by the detection of large transient potential changes [34]. The sensitivities to oxidative species examined in this work increased in the order H2O2 < O3 < Cr(VI) < ClO2- < BrO3-, as shown in Table 3. This sequence of sensitivity most likely depends on the rate of reaction of oxidative species with bromide.


## 6.4. Analyses of Residual Chlorine and Oxychlorine Species Using Fe(III)-Fe(II) Potential Buffer Containing Chloride [35, 36]

Since oxychlorinated species are considered to be hazardous to human health, the monitoring of levels of residual oxychlorines in drinking water is important for health safety. Furthermore, since HClO andClO2- are unstable and easily decomposed by air oxidation, a rapid analytical method that can be operated in a substantially closed system is desirable. A large transient potential change was observed by the generation of chlorine based on (27), (28), and (29) when oxychlorine species, ClO3-, ClO2-, and HClO, were added to an Fe(III)-Fe(II) potential buffer containing chloride, although the magnitude of the potential change was dependent on the reactivity of the oxychlorines. It is noteworthy that the rate of reaction (29) was relatively slower than that of reactions (27) and (28):     (27)HClO+Cl-+H+⟶Cl2+H2O(28)HClO2+3Cl-+3H+⟶2Cl2+2H2O(29)ClO3-+5Cl-+6H+⟶3Cl2+3H2OIn the FIA system, the analytical sensitivity to HClO andClO2- obtained by the detection of a transient potential change, where an Fe(III)-Fe(II) potential buffer containing chloride was used, was enhanced by ~700-fold compared with that obtained using an equilibrium potential, as shown in Table 4. The detection limits for HClO and ClO2-were 5×10-8 M, when a potential buffer consisting of 5×10-4 M Fe(III)-1×10-3 M Fe(II), 0.3 M KCl and 0.5 M H2SO4 (buffer-A) was used. For the determination of ClO3-, a concentration of 10−5 M was detected when 9 M H2SO4 was added to buffer-A, instead of 0.5 M H2SO4, as shown in the bottom line in Table 4.Table 4
Sensitivities to oxychlorine species.
Oxychlorine speciesSensitivity (mV/mM)Enhancement factor, (A)/(B)(A) Observed in  FIA system(B) CalculatedaHClO1.2 × 10415 (m= 2)800ClO2-2.1 × 10430 (m = 4)700ClO3-3.445 (m = 6)0.08ClO3-4.3 × 102 b45 (m = 6)9.8aSensitivity calculated from (6) using 5×10-3 M Fe(III)-1×10-2 M Fe(II).bSlope of the calibration curve observed in the FIA system with buffer-A containing 9.0 M H2SO4 and reaction coil of 200 cm in length.The simultaneous determination ofClO3--ClO2- or ClO3--HClO (for the case of [ClO3-] > [HClO] and [ClO3-] > [ClO2-]) was achieved using a flow system with dual detectors, as shown in Figure 6(A), where the differences in reactivity of the oxychlorine species with chloride in two potential buffers containing different concentrations of sulfuric acid were utilized. Figures 6(B)(a) and 6(B)(b) show the calibration peaks for ClO3- obtained using detector D1 and for ClO2- obtained using detector D2, respectively, where the mixed sample solutions contained at different concentration but the same molar ratio of [ClO3-]/[ClO2-] was 25. Figure 6(B)(c) and 6(B)(d) show the calibration peaks for ClO3- obtained using detector D1 and for HClO obtained using detector D2, respectively, where the concentrations of the mixed sample solutions were different but the molar ratio of [ClO3-]/[HClO] was the same, that is, 16.7. The method was applied to the determination of residual chlorine in a tap water sample containing a large amount of chlorate and was found to provide an analytical result for HClO, which was in good agreement with that obtained by the o-tolidine method. The presence of monochloramine interfered with the determination HClO, since the sensitivity of this method to monochloramine was one-fifth of that to HClO.Figure 6
(A) Schematic diagram of a three-channel FIA system for the determination ofClO3--ClO2- or ClO3--HClO∙ (for the case of [ClO3-]>[HClO] and [ClO3-]>[ClO2-]). R.S.1: 5×10-3 M Fe(III)- 1×10-2 M Fe(II), 0.3 M KCl and 9 M H2SO4; R.S.2: 5×10-3 M Fe(III)- 1×10-2 M Fe(II), 0.3 M KCl and 0.3 M H2SO4. D1 and D2: the same detectors as in Figure 1. (B) Calibration peaks ((a), (b)) for ClO3- and ClO2- obtained using detectors D1 and D2, respectively. Concentrations of ClO3- and ClO2- in the mixed sample are indicated in the figure. Calibration peaks ((c), (d)) for ClO3- and HClO obtained with detector D1 and D2, respectively. Concentrations of ClO3- and HClO in the mixed sample are indicated in the figure.Furthermore, under the condition of[ClO3-]≅ [HClO] and [ClO3-]≅[ClO2-], the simultaneous determination of mixed oxychlorines was conducted using a four-channel flow system equipped with a cation-exchange column in the Fe(II) form.


## 6.5. Analysis of Hydrazine Using a Ce(IV)-Ce(III) Potential Buffer [37]

The determination of sub-micromolar levels of hydrazine (N2H4) was accomplished using a two-channel flow system with a Ce(IV)-Ce(III) couple in acidic solution instead of the Fe(III)-Fe(II) couple as a potential buffer solution. The method is based on the measurement of a transient potential change, which appeared in a negative direction. The shape of the transient potential change for hydrazine was different from that observed in the determination of bromate, Cr(VI), and oxychlorine:(30)N2H5+⇄N2H4+H+K=1.02×10-8(31)N2H5+⇄N2H4+2H++e-Eo>-0.6V(32)(H++N2H3⇄12N2+NH4+)Ce(IV)+e-⇄Ce(III)(1MH2SO4)E0=1.44V(33)Ce(IV)+N2H5+⟶12N2+Ce(III)+NH4++H+
We examined the reaction mechanism for reactions (30), (31), and (32) by spectrophotometric and potentiometric batch experiments, in which the transient potential change was the potential shift from the Ce(IV)-Ce(III) couple to the N2H5+-N2 couple, using a much lower electrode potential during the reaction of hydrazine with Ce(IV). The overall reaction which is the sum of elementary reactions (31) and (32) can be expressed by (33). The flow system was designed so as to detect the maximum of the transient potential change. Hydrazine, in a wide range of concentrations from 10−7 M to 10−3 M was determined by appropriately adjusting the concentration of the potential buffer from 10−4 M to 10−2 M, and the detection limit was found to be 1×10-7 M (3.2 ppb) when a 2×10-4 M Ce(IV)-Ce(III) potential buffer was used. The method was capable of determining the concentration of hydrazone in boiler water at the 10 ppb level.


## 7. Conclusion

The proposed potentiometric flow methods, which involve the detection of change in an equilibrium potential or a transient potential, have the potential for using a wide variety of applications, ranging from process control to environmental monitoring. The method is subject to the nature of the redox species under consideration in an analyte sample.  Based on our studies, if the redox species react with the components of the potential buffer, the method has the potential for use. However, if the flow system is equipped with an effective scavenger column, to eliminate interfering substance, this promises to expand the applicability of the proposed method to a considerable extent. When the method involves the detection of an intermediate substance, it may also be applicable to the other techniques such as CFIA, batch injections, and potentiometric gas sensors, when a potential buffer that contains bromide or chloride is used.



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*Source: 516165-2011-04-20.xml*