# Spectrophotometric Analysis of Phosphoric Acid Leakage in High-Temperature Phosphoric Acid-Doped Polybenzimidazole Membrane Fuel Cell Application

Authors: Seungyoon Han; Yeon Hun Jeong; Ju Hae Jung; Alina Begley; Euiji Choi; Sung Jong Yoo; Jong Hyun Jang; Hyoung-Juhn Kim; Suk Woo Nam; Jin Young Kim
Journal: Journal of Sensors
 (2016)

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## Abstract

High-temperature proton exchange membrane fuel cells (HT-PEMFCs) utilize a phosphoric acid- (PA-) doped polybenzimidazole (PBI) membrane as a polymer electrolyte. The PA concentration in the membrane can affect fuel cell performance, as a significant amount of PA can leak from the membrane electrode assembly (MEA) by dissolution in discharged water, which is a byproduct of cell operation. Spectrophotometric analysis of PA leakage in PA-doped polybenzimidazole membrane fuel cells is described here. This spectrophotometric analysis is based on measurement of absorption of an ion pair formed by phosphomolybdic anions and the cationoid color reagent. Different color reagents were tested based on PA detection sensitivity, stability of the formed color, and accuracy with respect to the amount of PA measured. This method allows for nondestructive analysis and monitoring of PA leakage during HT-PEMFCs operation.


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## Body

## 1. Introduction

Proton exchange membrane fuel cells (PEMFCs) have been of great interest to research, as these energy conversion devices pose a promising environmentally friendly alternative to fossil fuel-based technologies [1]. In particular, high-temperature (HT) PEMFCs operating at temperatures between 100°C and 200°C offer many benefits over low-temperature PEMFCs operating systems below 100°C, such as improved electrode reaction kinetics, superior water and heat management, tolerance of fuel impurities, and increased waste heat utilization [2–5].In HT-PEMFCs the usual solvent, water, is replaced with the proton conductive phosphoric acid (PA) in order to operate at such high temperatures (~200°C) and provide improved chemical and physical characteristics [6, 7]. PA is also an essential component for proton transport in the membrane structure. For HT-PEMFCs, the PA-doped polybenzimidazole (PBI) membrane [8] is the only membrane which satisfies the U.S. Department of Energy target of 2015, so that many studies attempt to improve and optimize the material selection as well as investigate the degradation mechanism of the membrane in HT-PEMFCs [9–12].The membrane degradation mechanism has been studied in depth in the last few decades [13–20]; however, the distribution and quantitative analysis of PA has been more or less neglected. A study concerning the amount and distribution of PA in PA-doped PBI membrane electrode assembly [21] is critical for the deep understanding of the degradation mechanism on the HT-PEMFCs performance [13, 22–24].In this study, a simple colorimetric analysis of PA leakage in the PA-PBI membrane fuel cell is reported for the first time. The applicability of the colorimetric analysis method on HT-PEMFCs for PA at constant current density operation is presented. The selected method is shown to be a reliable and sensitive method of detection of PA, with a linear dynamic range of up to 1 × 10−5 M and a detection limit of 1 × 10−8 M.


## 2. Materials and Methods

### 2.1. Color Developing Solution

All chemicals used were analytical grade reagents, and deionized water was used to produce all solutions.For the molybdenum blue reaction (Table1), 0.6 g of ammonium molybdate tetrahydrate and 0.024 g of potassium antimony tartrate hydrate were dissolved in 30 mL deionized water. 10 mL of 7.4 M concentrated sulfuric acid, 10 mL of 0.44 M ammonium sulfamate, and 10 mL of 0.4 M L-ascorbic acid were added to produce the color reagent solution. Then, 1 mL of the color reagent solution was added to 6 mL of the sample solution.Table 1
Color reagent, molybdenum blue.
Compound
Quantity
Ammonium molybdate tetrahydrate
0.6 g
Potassium antimony tartrate hydrate
0.024 g
Deionized water
30 mL
Sulfuric acid (7.4 M)
10 mL
Ammonium sulfamate (0.44 M)
10 mL
L-Ascorbic acid (0.4 M)
10 mLFor the crystal violet reaction (Table3), 1.2 × 10−2M ammonium molybdate tetrahydrate, 6.5 N of 98% concentrated sulphuric acid, and 1 × 10−3M of crystal violet solution were prepared. Then, 3 mL of prepared color reagent solution was added to 7 mL of the sample solution in a 1 : 1 : 1 v/v mixture of ammonium molybdate tetrahydrate, 6.5 N sulphuric acid, and 1 × 10−5M crystal violet solution.For the rhodamine B reaction (Table2), 7.4 × 10−3M ammonium molybdate tetrahydrate, 1 × 10−3M rhodamine B, 0.6 N of 98% concentrated sulphuric acid, and 0.05 M NaOCl solution were prepared. Then, 4 mL of color reagent solution was mixed with 6 mL of the sample solution in a 1 : 1 : 1 : 1 v/v mixture of molybdate, 0.6 N sulphuric acid, NaOCl, and diluted rhodamine B solution (1 × 10−5M).Table 2
Color reagent, rhodamine B.
Compound
Volume ratio
Ammonium molybdate tetrahydrate (7.4 × 10−3 M)
1
Rhodamine B (1 × 10−3 M)
1
Sulphuric acid (0.6 N)
1
NaOCl solution (0.05 M)
1Table 3
Color reagent, crystal violet.
Compound
Volume ratio
Ammonium molybdate tetrahydrate (1.2 × 10−2 M)
1
Sulphuric acid (6.5 N)
1
Crystal violet solution (1 × 10−3 M)
1


### 2.2. Measurement of Sample Solutions from the Operating Cell

Commercially available MEA (20.25 cm2 active area, Dongjin Semichem), Teflon gaskets, and graphite bipolar plates were assembled and used for HT-PEMFC operation. The unit cell was operated on constant current density at 1.1 A cm−2 for 84 hours, the cell operation temperature was 150°C, and the stoichiometry of hydrogen and air was 1.2 and 2.0, respectively. During the cell operation, the exhaust gases from both anode and cathode were cooled and collected in liquid state in the vials which contained 10 mL of distillated water. Then, the reagents were added to the vent solutions from the unit cell. After the color reaction, the solutions with added reagent were analyzed by UV/Vis spectroscopy. The spectrophotometer used was a LAMBDA 25 UV/Vis spectrophotometer from PerkinElmer.


## 2.1. Color Developing Solution

All chemicals used were analytical grade reagents, and deionized water was used to produce all solutions.For the molybdenum blue reaction (Table1), 0.6 g of ammonium molybdate tetrahydrate and 0.024 g of potassium antimony tartrate hydrate were dissolved in 30 mL deionized water. 10 mL of 7.4 M concentrated sulfuric acid, 10 mL of 0.44 M ammonium sulfamate, and 10 mL of 0.4 M L-ascorbic acid were added to produce the color reagent solution. Then, 1 mL of the color reagent solution was added to 6 mL of the sample solution.Table 1
Color reagent, molybdenum blue.
Compound
Quantity
Ammonium molybdate tetrahydrate
0.6 g
Potassium antimony tartrate hydrate
0.024 g
Deionized water
30 mL
Sulfuric acid (7.4 M)
10 mL
Ammonium sulfamate (0.44 M)
10 mL
L-Ascorbic acid (0.4 M)
10 mLFor the crystal violet reaction (Table3), 1.2 × 10−2M ammonium molybdate tetrahydrate, 6.5 N of 98% concentrated sulphuric acid, and 1 × 10−3M of crystal violet solution were prepared. Then, 3 mL of prepared color reagent solution was added to 7 mL of the sample solution in a 1 : 1 : 1 v/v mixture of ammonium molybdate tetrahydrate, 6.5 N sulphuric acid, and 1 × 10−5M crystal violet solution.For the rhodamine B reaction (Table2), 7.4 × 10−3M ammonium molybdate tetrahydrate, 1 × 10−3M rhodamine B, 0.6 N of 98% concentrated sulphuric acid, and 0.05 M NaOCl solution were prepared. Then, 4 mL of color reagent solution was mixed with 6 mL of the sample solution in a 1 : 1 : 1 : 1 v/v mixture of molybdate, 0.6 N sulphuric acid, NaOCl, and diluted rhodamine B solution (1 × 10−5M).Table 2
Color reagent, rhodamine B.
Compound
Volume ratio
Ammonium molybdate tetrahydrate (7.4 × 10−3 M)
1
Rhodamine B (1 × 10−3 M)
1
Sulphuric acid (0.6 N)
1
NaOCl solution (0.05 M)
1Table 3
Color reagent, crystal violet.
Compound
Volume ratio
Ammonium molybdate tetrahydrate (1.2 × 10−2 M)
1
Sulphuric acid (6.5 N)
1
Crystal violet solution (1 × 10−3 M)
1


## 2.2. Measurement of Sample Solutions from the Operating Cell

Commercially available MEA (20.25 cm2 active area, Dongjin Semichem), Teflon gaskets, and graphite bipolar plates were assembled and used for HT-PEMFC operation. The unit cell was operated on constant current density at 1.1 A cm−2 for 84 hours, the cell operation temperature was 150°C, and the stoichiometry of hydrogen and air was 1.2 and 2.0, respectively. During the cell operation, the exhaust gases from both anode and cathode were cooled and collected in liquid state in the vials which contained 10 mL of distillated water. Then, the reagents were added to the vent solutions from the unit cell. After the color reaction, the solutions with added reagent were analyzed by UV/Vis spectroscopy. The spectrophotometer used was a LAMBDA 25 UV/Vis spectrophotometer from PerkinElmer.


## 3. Results and Discussion

The quantitative analysis of PA leakage during the PA-doped PBI membrane HT-PEMFCs operation was performed by spectrophotometric analysis of the colorimetric reaction of the PA-molybdenum compound [25, 26]. As shown in Figure 1, during cell operation the water byproduct dragged the PA, which was then discharged from the MEA. In the molybdenum blue color developing reaction, PA ions reacted with ammonium molybdate and formed phosphomolybdenum complexes. The complexes were reduced by ascorbic acid and heteropoly molybdenum blue was formed. The chemical equation is as follows [27–29]: (1)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
H
2
P
M
o
12
O
40
+
Ascorbic  acid
⟶
Heteropoly  molybdenum  blueThe quantitative analysis was carried out on the resulting colored sample.Figure 1
A schematic depiction of the approach of colorimetric detection of PA leakage in HT-PEMFCs used in the experiment.


### 3.1. Selection of Color Reagent Solution

One of the PA detection methods used in this study was based on the analysis of the absorption spectrum of heteropoly molybdenum blue, the product of PA ions reacting with molybdate, followed by reduction with stannous chloride. The chemical equation is shown below [27, 28, 30]: (2)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
H
2
P
M
o
12
O
40
+
S
n
C
l
2
⟶
Heteropoly  molybdenum  blueThis compound showed poor detection limit (>10 ppb) and low sensitivity. As an improvement to the heteropoly molybdenum blue method, stannous chloride was replaced with ascorbic acid to provide a stable reduction reaction, as well as a clear spectrum of molybdenum blue [28].The sensitivity of the color reagent is defined in terms of apparent molar absorptivity. Color reagents must have a high apparent molar absorptivity and be a cationoid dye, which allows the formation of an ion pair with molybdophosphoric acid. Table4 [28] lists the apparent molar absorptivity of various commercially available color reagents.Table 4
Molar absorptivity of color reagents [28].
Color reagent
Molar absorptivity (M−1 cm−1)
Molybdenum blue
2.0 × 104
Brilliant green
0.88 × 105
Crystal violet
1.28 × 105
Malachite green
7.8 × 104
Rhodamine B
1.19 × 105
Servon red L
0.7 × 104Three major selection criteria are applied to the choice of color reagent for PA analysis: (1) the detection accuracy; (2) the color formation time and color stability; and (3) the detection limit at low PA concentration. There are many well-studied color reagents that can be applied to detecting low PA concentrations; however, the three chosen for this experiment were molybdenum blue [31], rhodamine B [32, 33], and crystal violet [34] methods. These color reagents have high apparent molar absorptivities, which result in higher detection sensitivity; they are also readily soluble in water and form cationic aqueous solutions.


### 3.2. Visual Inspection of Color Formation on PA Standard Solution

Each color reagent was tested with PA standard solution with a concentration range of 0 M to 1 × 10−3M. Gradation of each color dye is shown in Figure 2. Each color reagent solution had a similar color gradation pattern but different color spectral wavelength range in standard solution. As in Figures 2(a) and 2(c), both molybdenum blue and crystal violet resulted in blue color formation; however, the crystal violet resulted in a weaker color gradation than the molybdenum blue. This may imply that the visual detection sensitivity of crystal violet is constant over a wide PA concentration range. Also, the color developing time of molybdenum blue and crystal violet was 15 min and 60 min, respectively. The longer reaction time of crystal violet was mainly due to the strong color of the dye itself, so that unreacted crystal violet ions had to decolorize by reaction with acid before only the product could be detected. The chemical equation of the crystal violet method is as follows [27]:(3)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
C
V
+
+
H
2
P
M
o
12
O
40
-
⟶
C
V
H
2
P
M
o
12
O
40
+
C
V
+
C
V
+
+
C
V
H
2
P
M
o
12
O
40
+
H
+
⟶
C
V
H
2
P
M
o
12
O
40in which CV represents crystal violet compound.Figure 2
PA analysis from model PA compound solution. (a) Molybdenum blue method, (b) rhodamine B, and (c) crystal violet color reagent.
(a)
(b)
(c)The reaction with rhodamine B resulted in a distinct, light pink color. The chemical equation of the rhodamine B reaction is as follows [27]:(4)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
R
h
B
+
+
H
2
P
M
o
12
O
40
-
⟶
R
h
B
H
2
P
M
o
12
O
40
+
R
h
B
+
R
h
B
+
+
R
h
B
H
2
P
M
o
12
O
40
+
N
a
O
C
l
⟶
R
h
B
H
2
P
M
o
12
O
40where RhB represents rhodamine B compound. In reaction (4), the concentration of rhodamine B and NaOCl had a critical impact on the color formation [27, 28]. The NaOCl bleached rhodamine B, but the optimized concentration of NaOCl required bleaching only the unreacted rhodamine B in the solution.


### 3.3. Spectrophotometric Measurement of PA Standard Solution

The PA concentration was determined by the absorption spectra in standard solution, molybdenum blue, crystal violet, and rhodamine B solution. Clear absorption peaks were observed in each color reagent as shown in Figure3. As mentioned above, since the heteropolyphosphoric acid, which is a colorific compound, was formed after the color developing reaction, the curves have more than one peak. In this case, the peak of maximum absorbance is chosen. The range of the absorption maxima of each reagent was as follows: 770 nm to 900 nm for molybdenum blue; 500 nm to 575 nm for crystal violet; and 550 nm to 700 nm for rhodamine B [26, 28]. The maximum absorbance was plotted against PA concentration, yielding a linear correlation. The degree of linearity was analyzed by the Least Mean Square method [35] and the residual value (R
2). The R
2-value was 0.99996 for molybdenum blue; 0.98768 for rhodamine B; and 0.99879 for the crystal violet solution. In addition to the residual value, a Lambert-Beer plot [36], obtained by standard solution PA concentration, and measured resulting absorbance are compared in Figure 4. The calibration curves in Figure 4 were plotted with apparent molar absorptivity data obtained from other investigators [28]. Linearity of the rhodamine B and crystal violet methods, Figures 4(b) and 4(c), respectively, was low. This revealed that the light pink rhodamine B has a low detection range and high potential error, crystal violet less so. Both color reagents required the decoloring of unreacted pigment through chemical reaction [28]. During the bleaching process, the pH of the decolorizing solution was a major factor that could destroy the desired, fully reacted product. Lastly, the detection limit for each color reagent was defined as a 1 : 1 signal to noise ratio, by which the noise was the maximum signal variance of the determined PA concentration. Upon analysis of all coloring reagents, molybdenum blue was best suited for the detection of PA concentration.Figure 3
Spectrometric measurement of standard solution reacted with (a) molybdenum blue, (b) rhodamine B, and (c) crystal violet color reagent.
(a)
(b)
(c)Figure 4
Relationship between PA concentration and the absorbance of standard solutions reacted with (a) molybdenum blue, (b) rhodamine B, and (c) crystal violet color reagent.
(a)
(b)
(c)


### 3.4. High-Temperature PEMFC Application

The molybdenum blue method was applied for quantitative analysis of leaked PA concentration from HT-PEMFCs (Figure5). After 100 hours of constant current density fuel cell operation, the exhaust water was removed from the anode and cathode side outlets. During constant current cell operation with a fixed current density of 1.1 A cm−2, the rate of water discharge was also constant as the oxygen reduction reaction produced water in the fuel cell at a constant rate. It is known that the PA is in the liquid state inside the fuel cell and is presumably moved out of the membrane by water, as the dominant leakage source was discharged water [19]. Figure 5(b) indicates the amount of phosphoric acid from cathode of the unit cell during constant current operation at 1.1 A cm−2 for 84 hours. The average PA leakage of the seven samples was 0.397 μg h−1 cm−2, which is a negligible amount when compared to the initial PA concentration in the HT-PEMFCs MEA. The reliability of the molybdenum blue method was confirmed through inductively coupled plasma atomic emission spectroscopy (ICP-OES). The accuracy of PA concentration from the molybdenum blue method was over 99.21%, which supported the computability and accuracy of the molybdenum blue method.Figure 5
Applicability of the colorimetric method to real device. (a) Photograph of operating real device. (b) Histogram of PA contents and discharged water as a function of operation time.
(a)
(b)


## 3.1. Selection of Color Reagent Solution

One of the PA detection methods used in this study was based on the analysis of the absorption spectrum of heteropoly molybdenum blue, the product of PA ions reacting with molybdate, followed by reduction with stannous chloride. The chemical equation is shown below [27, 28, 30]: (2)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
H
2
P
M
o
12
O
40
+
S
n
C
l
2
⟶
Heteropoly  molybdenum  blueThis compound showed poor detection limit (>10 ppb) and low sensitivity. As an improvement to the heteropoly molybdenum blue method, stannous chloride was replaced with ascorbic acid to provide a stable reduction reaction, as well as a clear spectrum of molybdenum blue [28].The sensitivity of the color reagent is defined in terms of apparent molar absorptivity. Color reagents must have a high apparent molar absorptivity and be a cationoid dye, which allows the formation of an ion pair with molybdophosphoric acid. Table4 [28] lists the apparent molar absorptivity of various commercially available color reagents.Table 4
Molar absorptivity of color reagents [28].
Color reagent
Molar absorptivity (M−1 cm−1)
Molybdenum blue
2.0 × 104
Brilliant green
0.88 × 105
Crystal violet
1.28 × 105
Malachite green
7.8 × 104
Rhodamine B
1.19 × 105
Servon red L
0.7 × 104Three major selection criteria are applied to the choice of color reagent for PA analysis: (1) the detection accuracy; (2) the color formation time and color stability; and (3) the detection limit at low PA concentration. There are many well-studied color reagents that can be applied to detecting low PA concentrations; however, the three chosen for this experiment were molybdenum blue [31], rhodamine B [32, 33], and crystal violet [34] methods. These color reagents have high apparent molar absorptivities, which result in higher detection sensitivity; they are also readily soluble in water and form cationic aqueous solutions.


## 3.2. Visual Inspection of Color Formation on PA Standard Solution

Each color reagent was tested with PA standard solution with a concentration range of 0 M to 1 × 10−3M. Gradation of each color dye is shown in Figure 2. Each color reagent solution had a similar color gradation pattern but different color spectral wavelength range in standard solution. As in Figures 2(a) and 2(c), both molybdenum blue and crystal violet resulted in blue color formation; however, the crystal violet resulted in a weaker color gradation than the molybdenum blue. This may imply that the visual detection sensitivity of crystal violet is constant over a wide PA concentration range. Also, the color developing time of molybdenum blue and crystal violet was 15 min and 60 min, respectively. The longer reaction time of crystal violet was mainly due to the strong color of the dye itself, so that unreacted crystal violet ions had to decolorize by reaction with acid before only the product could be detected. The chemical equation of the crystal violet method is as follows [27]:(3)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
C
V
+
+
H
2
P
M
o
12
O
40
-
⟶
C
V
H
2
P
M
o
12
O
40
+
C
V
+
C
V
+
+
C
V
H
2
P
M
o
12
O
40
+
H
+
⟶
C
V
H
2
P
M
o
12
O
40in which CV represents crystal violet compound.Figure 2
PA analysis from model PA compound solution. (a) Molybdenum blue method, (b) rhodamine B, and (c) crystal violet color reagent.
(a)
(b)
(c)The reaction with rhodamine B resulted in a distinct, light pink color. The chemical equation of the rhodamine B reaction is as follows [27]:(4)
12
M
o
O
3
+
H
2
P
O
4
-
⟶
H
2
P
M
o
12
O
40
R
h
B
+
+
H
2
P
M
o
12
O
40
-
⟶
R
h
B
H
2
P
M
o
12
O
40
+
R
h
B
+
R
h
B
+
+
R
h
B
H
2
P
M
o
12
O
40
+
N
a
O
C
l
⟶
R
h
B
H
2
P
M
o
12
O
40where RhB represents rhodamine B compound. In reaction (4), the concentration of rhodamine B and NaOCl had a critical impact on the color formation [27, 28]. The NaOCl bleached rhodamine B, but the optimized concentration of NaOCl required bleaching only the unreacted rhodamine B in the solution.


## 3.3. Spectrophotometric Measurement of PA Standard Solution

The PA concentration was determined by the absorption spectra in standard solution, molybdenum blue, crystal violet, and rhodamine B solution. Clear absorption peaks were observed in each color reagent as shown in Figure3. As mentioned above, since the heteropolyphosphoric acid, which is a colorific compound, was formed after the color developing reaction, the curves have more than one peak. In this case, the peak of maximum absorbance is chosen. The range of the absorption maxima of each reagent was as follows: 770 nm to 900 nm for molybdenum blue; 500 nm to 575 nm for crystal violet; and 550 nm to 700 nm for rhodamine B [26, 28]. The maximum absorbance was plotted against PA concentration, yielding a linear correlation. The degree of linearity was analyzed by the Least Mean Square method [35] and the residual value (R
2). The R
2-value was 0.99996 for molybdenum blue; 0.98768 for rhodamine B; and 0.99879 for the crystal violet solution. In addition to the residual value, a Lambert-Beer plot [36], obtained by standard solution PA concentration, and measured resulting absorbance are compared in Figure 4. The calibration curves in Figure 4 were plotted with apparent molar absorptivity data obtained from other investigators [28]. Linearity of the rhodamine B and crystal violet methods, Figures 4(b) and 4(c), respectively, was low. This revealed that the light pink rhodamine B has a low detection range and high potential error, crystal violet less so. Both color reagents required the decoloring of unreacted pigment through chemical reaction [28]. During the bleaching process, the pH of the decolorizing solution was a major factor that could destroy the desired, fully reacted product. Lastly, the detection limit for each color reagent was defined as a 1 : 1 signal to noise ratio, by which the noise was the maximum signal variance of the determined PA concentration. Upon analysis of all coloring reagents, molybdenum blue was best suited for the detection of PA concentration.Figure 3
Spectrometric measurement of standard solution reacted with (a) molybdenum blue, (b) rhodamine B, and (c) crystal violet color reagent.
(a)
(b)
(c)Figure 4
Relationship between PA concentration and the absorbance of standard solutions reacted with (a) molybdenum blue, (b) rhodamine B, and (c) crystal violet color reagent.
(a)
(b)
(c)


## 3.4. High-Temperature PEMFC Application

The molybdenum blue method was applied for quantitative analysis of leaked PA concentration from HT-PEMFCs (Figure5). After 100 hours of constant current density fuel cell operation, the exhaust water was removed from the anode and cathode side outlets. During constant current cell operation with a fixed current density of 1.1 A cm−2, the rate of water discharge was also constant as the oxygen reduction reaction produced water in the fuel cell at a constant rate. It is known that the PA is in the liquid state inside the fuel cell and is presumably moved out of the membrane by water, as the dominant leakage source was discharged water [19]. Figure 5(b) indicates the amount of phosphoric acid from cathode of the unit cell during constant current operation at 1.1 A cm−2 for 84 hours. The average PA leakage of the seven samples was 0.397 μg h−1 cm−2, which is a negligible amount when compared to the initial PA concentration in the HT-PEMFCs MEA. The reliability of the molybdenum blue method was confirmed through inductively coupled plasma atomic emission spectroscopy (ICP-OES). The accuracy of PA concentration from the molybdenum blue method was over 99.21%, which supported the computability and accuracy of the molybdenum blue method.Figure 5
Applicability of the colorimetric method to real device. (a) Photograph of operating real device. (b) Histogram of PA contents and discharged water as a function of operation time.
(a)
(b)


## 4. Conclusions

Recently, various investigation methods for PA concentration in the HT-PEMFCs have been studied and proposed; however, the spectrometric quantification with a color reagent solution is the most efficient method. Color reagents which have high apparent molecular absorptivity were selected and tested. The molybdenum blue and ascorbic acid method provided the most stable and reliable results, especially with respect to detecting speed and accuracy. The application of spectrometric quantification of PA leakage on the HT-PEMFCs is a competitive method.



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*Source: 5290510-2015-12-22.xml*