# Ion-Exchange Membranes Based on Polynorbornenes with Fluorinated Imide Side Chain Groups

Authors: Arlette A. Santiago; Joel Vargas; Mikhail A. Tlenkopatchev; Mar López-González; Evaristo Riande
Journal: International Journal of Chemical Engineering
 (2012)

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## Abstract

The electrochemical characteristics of cation-exchange membranes based on polynorbornenes with fluorinated and sulfonated dicarboximide side chain groups were reported. This study was extended to a block copolymer containing structural units with phenyl and 4-oxybenzenesulfonic acid, 2,3,5,6-tetrafluorophenyl moieties replacing the hydrogen atom of the dicarboximide group. A thorough study on the electrochemical characteristics of the membranes involving electromotive forces of concentration cells and proton conductivity is reported. The proton permselectivity of the membranes is also discussed.


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## Body

## 1. Introduction

Ion-exchange membranes have received considerable attention for many applications. Thus, the desalination of sea-water and brackish-water, treatment of industrial effluents, concentration or separation of food and pharmaceutical products containing ionic species are some of the examples of these kinds of applications [1, 2].Ion-exchange membranes should exhibit high conductance, high permselectivity, low free diffusion of ionic species, low osmotic flow, good mechanical properties, and high chemical stability. Many polyelectrolytes based on perfluorinated polyimides, polyetherketones, polysulfones, polyphosphazenes; have been synthesized, and their electrochemical characteristics have been studied [3]. It is well known that norbornene monomers can be easily functionalized and membranes from functionalized polynorbornenes with adamantyl, phenyl, cyclohexyl, and pentafluorophenyl dicarboximide side groups have been prepared [4–6]. Taking into account these antecedents and searching for new ion-exchange membranes, a study was undertaken focused on the preparation of cation-exchange membranes based on modified polynorbornenes.In an earlier work, the preparation of hydrogenated and sulfonated poly(N-phenyl-exo-endo-norbornene-5,6-dicarboximide) has been reported [7]. A drawback of these membranes is that the sulfonation procedure does not guarantee a uniform sulfonation of the phenyl groups, and even it can produce degradative processes in the polymer chains. In order to circumvent these difficulties, we have synthesized poly(N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) and successfully replaced the fluorine atom in position 4 of the phenyl group by sulfonation in mild conditions [8].The fluorine atoms in the polyelectrolyte side chains can decrease attractive intermolecular interactions between phenyl groups thus avoiding the molecular piling of the phenyl rings. This behavior is a direct consequence of the high electronegativity of the fluorine atom which severely reduces the polarizability of theCar–F bond and as a result the formation of nonpermanent or flitting dipoles which are the basis of the London dispersion forces [9]. It should be noted that earlier studies on gas transport in polynorbornene-based membranes showed that fluorinated moieties in the polymer chains cause a significant increase in gas permeability as a consequence of the decrease in intramolecular interactions [10]. The cation-exchange membranes were also prepared from copolymers resulting from partially replacing the phenyl groups of poly(N-phenyl-exo-endo-norbornene-5,6-dicarboximide) by 4-oxybenzenesulfonic acid, 2,3,5,6-tetrafluorophenyl groups [11]. The aim of this study was to find out how the decrease of the density of sulfonic acid in the membranes affects their transport characteristics. The acronyms used for the homopolymeric and the copolymeric acidic membranes were, respectively, P5FNDIHS and C5FNDIHS, and the structural units of the respective chains are shown in Figure 1.Figure 1
Acid form structural units of hydrogenated-sulfonated poly(N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) (P5FNDIHS) and hydrogenated-sulfonated poly(N-phenyl-exo-endo-norbornene-5,6-dicarboximide-co-N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) (C5FNDIHS).


## 2. Experimental Part

### 2.1. Synthesis of the Monomer

By reaction of norbornene-5,6-dicarboxylic anhydride (NDA) with 2,3,4,5,6-pentafluoroaniline an amic acid (AA) that is obtained which further treated with anhydrous sodium acetate/acetic anhydride produces the monomerN-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide (5FNDI) (see Scheme 1). More details of the synthesis are given elsewhere [8].Scheme 1
Monomer synthesis and further polymerization.


### 2.2. Polymerization

Polymerization of 5FNDI was carried out by ring opening metathesis polymerization (ROMP) (Scheme1). The reaction was performed at 45°C for 2 h in glass vials, under nitrogen atmosphere. The polymerization was terminated by adding ethyl vinyl ether to the reaction medium which was further poured into methanol, solubilized with chloroform containing a few drops of 1 N HCl, and precipitated again into methanol. The product was dried in a vacuum oven at 40°C to constant weight. Then, the polymer was hydrogenated quantitatively at room temperature and 115 bar using a Wilkinson’s catalyst (Scheme 2).Scheme 2
Synthesis of sulfonated polymer and copolymer.


### 2.3. Sulfonation Procedure

Hydrogenated poly(N-pentafluorophenyl-norbornene-5,6-dicarboximide) (P5FNDIH) (0.5 g, 1.51 mmol), sodium 4-hydroxybenzenesulfonate dihydrate (0.70 g, 3.02 mmol), and potassium carbonate (0.52 g, 3.77 mmol) were mixed in a round flask equipped with a Dean-Stark trap and stirred in 15 mL of solvent (N,N-dimethylacetamide-toluene 2 : 1) at 120°C for 9 h (Scheme 2). Progressive precipitation overtime was observed. The product was then filtered off, washed several times with distilled water and dried in a vacuum oven at 40°C overnight. The resulting polymer P5FNDIHS, a pale-brown powder, was soluble in DMF and DMSO. Yield: 94%, Tg = 228°C, Td1 = 260°C (sulfonic group loss), Td2 = 430°C (main chain decomposition).1H NMR (300 MHz, DMF-d7): δ (ppm) = 7.80 (2H, s), 7.18 (2H, s), 3.56 (2H, s), 2.73, 2.31, 1.83, 1.58, 1.91.13C NMR (75 MHZ, DMF-d7): δ (ppm) = 175.0 (C=O), 145.5, 145.0, 140.4, 139.7, 128.2 (C–O), 115.1, 107.2, 49.0, 43.0.19F NMR (300 MHz, DMSO-d6, ref. TFA [−77 ppm]): δ (ppm) = −141.9, −143.0, −153.1.FT-IR (thin film, cm−1): 2926 (C-H asym str), 2860 (C–H sym str), 1787 (C=O), 1726, 1636, 1509, 1406, 1356, 1295 (C–F), 1140 (−SO3H, asym str), 1132, 1039 (−SO3H, sym str), 981, 833, 698, 561. The acronym for this polymer will be P5FNDIHS (Figure 1).


### 2.4. Copolymerization

The copolymer was prepared via ROMP in a block fashion [11]. Firstly, monomer PhNDI, synthesized according to literature [8] and catalyst I were stirred in 1,2-dichloroethane at 65°C for 0.33 h. Then, monomer 5FNDI dissolved in 1,2-dichloroethane was added to the polymer solution and stirred at 65°C for 0.66 h (Scheme 1). The obtained copolymer C5FNDI was soluble in chloroform and dichloroethane. The incorporation of 5FNDI in copolymer was 32 mol% as determined by 1H NMR. The block copolymer obtained was hydrogenated as mentioned above and the pentafluorophenyl moieties of hydrogenated poly(N-phenyl-exo-endo-norbornene-5,6-dicarboximide-co-N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) (C5FNDIH) were sulfonated with 4-hydroxybenzenesulfonate dihydrate using the procedure used for the sulfonation of hydrogenated poly(N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) (Scheme 2). The acronym for this copolymer will be C5FNDIHS and its composition is shown in Figure 1.


### 2.5. Membranes Preparation and Atomic Force Microscopy (AFM)

P5FNDIHS and C5FNDIHS membranes (in sodium salt form) were cast, respectively, from hotN,N-dimethylformamide solutions (~2 wt %) of P5FNDIHS and C5FNDIHS chains in a Teflon mold and dried at 70°C for 12 h. The films were immersed firstly in stirring methanol at room temperature for 3 h and secondly in deionized water for 1 h in order to remove the residual solvent. Afterwards, the membranes underwent a proton exchange treatment with 1.0 N hydrochloric acid during 12 h. Then, the films were washed repeatedly with deionized water until the rinse water became neutral. Finally, the membranes were dried under a vacuum at 120°C for 10 h.The surface morphology of the thin films was observed using tapping mode AFM (Multimode Nanoscope IVa, Digital Instrument/Veeco) under ambient conditions. In tapping mode, the stylus oscillates and touches the sample only at the end of its downward movement. The nominal resonance frequency for the tapping mode was between 265–309 kHz with a phosphorous (n) doped Si cantilever which had a spring constant that ranged from 20 to 80 N m−1. The set point in the AFM control program was adjusted to change the contact force between the tip and surface in order to detect the existence of morphologies.


### 2.6. Density, Water Uptake, and Ion-Exchange Capacity of the Membranes

The density of the dry membranes was measured by the flotation method using isooctane as solvent. The values of this parameter are shown in the first column of Table1.Table 1
Density in Kg m−3, ρ, water uptake in Kg H2O/Kg dry membrane, wu, IEC in equivalents of fixed anionic groups per Kg dry membrane obtained by titration, X-, and NMR, XNMR-, molecules of water per fixed ionic group, λ, and conductivity, σ, in S/m, at 30°C.
MembraneρwuX-XNMR-λx-λXNMR-σP5FNDIHS15000.6171.7502.06019.616.62.24C5FNDIHS13800.3730.2860.20472.5101.60.0134Weighed dry membranes were immersed in distilled water for several hours, removed from the solution, gently blotted with filter paper to remove superficial water, and weighed. From the weights of the dry membranes,md, and the membranes equilibrated with water, mw, the water uptake, wu, in g H2O/g dry membrane is obtained as wu=(mw/md)-1.The ion-exchange capacity (IEC) of a given membrane was measured by immersing the weighed dry membrane in a 1 N HCl solution for 1 h. Then the membrane was removed from the solution, washed several times with distilled water to eliminate the chloride acid absorbed, and finally immersed in a 1 N sodium chloride solution. The protons exchanged in the reaction(1)R-H+Na+⟶R-Na+H+
were estimated by titration with a very diluted NaOH solution. The values of IEC in equiv/Kg dry membrane were obtained as IEC=VN/md where V is the volume in L of the solution of NaOH of normality N (equiv/L) used in the titration, and md is the mass of the membrane in Kg.


### 2.7. Electromotive Forces of Concentration Cells

Electromotive forces of concentration cells made up of two semicells separated by the ion-exchange membrane were measured (Figure2). The configuration of the cells was Ag |AgCl| HCl solution (c1) |cation-exchangemembrane| HCl solution (c2)|AgCl|Ag, where c1 and c2 are the concentrations of the electrolyte in the left-hand and right-hand compartments of the concentration cells. Notice that the anion of the electrolyte must be reversible with that of the electrodes. The solution in each compartment was kept under strong stirring to minimize the formation of membrane-solution interface layers. The evolution of electromotive force, emf, of the cell with time was measured at 25°C with a 3645-20 Hioki voltage logger and recorded every second with a 3911-20 communication base apparatus via a PC. The emf of the concentration cell was taken as that one at which this quantity reaches a maximum.Figure 2
Concentration cell used to measure the electromotive force: (C) half cell, (E) electrodes, (M) ion-exchange membrane, and (S) magnetic stirrers.


### 2.8. Ohmic Resistance Measurements

The ohmic resistance of the membranes in the acid form was measured with a Novocontrol BDS system comprising a frequency response analyzer (Solartron Schlumberger FRA 1260) and a broadband dielectric converter with an active sample head. Gold disk electrodes were used in the impedance measurements carried out at several temperatures in the frequency window 4.9 × 10−2 – 1 × 107 Hz. The temperature was controlled by a nitrogen jet (QUATRO from Novocontrol) with a temperature error of 0.1 K during every single sweep in frequency (Figure 3). Measurements were carried out on molded disk-shaped samples of 60–100 μm thickness with diameters of 20 and 10 mm.Figure 3
Cell used to measure the ionic conductivity of the membranes.


## 2.1. Synthesis of the Monomer

By reaction of norbornene-5,6-dicarboxylic anhydride (NDA) with 2,3,4,5,6-pentafluoroaniline an amic acid (AA) that is obtained which further treated with anhydrous sodium acetate/acetic anhydride produces the monomerN-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide (5FNDI) (see Scheme 1). More details of the synthesis are given elsewhere [8].Scheme 1
Monomer synthesis and further polymerization.


## 2.2. Polymerization

Polymerization of 5FNDI was carried out by ring opening metathesis polymerization (ROMP) (Scheme1). The reaction was performed at 45°C for 2 h in glass vials, under nitrogen atmosphere. The polymerization was terminated by adding ethyl vinyl ether to the reaction medium which was further poured into methanol, solubilized with chloroform containing a few drops of 1 N HCl, and precipitated again into methanol. The product was dried in a vacuum oven at 40°C to constant weight. Then, the polymer was hydrogenated quantitatively at room temperature and 115 bar using a Wilkinson’s catalyst (Scheme 2).Scheme 2
Synthesis of sulfonated polymer and copolymer.


## 2.3. Sulfonation Procedure

Hydrogenated poly(N-pentafluorophenyl-norbornene-5,6-dicarboximide) (P5FNDIH) (0.5 g, 1.51 mmol), sodium 4-hydroxybenzenesulfonate dihydrate (0.70 g, 3.02 mmol), and potassium carbonate (0.52 g, 3.77 mmol) were mixed in a round flask equipped with a Dean-Stark trap and stirred in 15 mL of solvent (N,N-dimethylacetamide-toluene 2 : 1) at 120°C for 9 h (Scheme 2). Progressive precipitation overtime was observed. The product was then filtered off, washed several times with distilled water and dried in a vacuum oven at 40°C overnight. The resulting polymer P5FNDIHS, a pale-brown powder, was soluble in DMF and DMSO. Yield: 94%, Tg = 228°C, Td1 = 260°C (sulfonic group loss), Td2 = 430°C (main chain decomposition).1H NMR (300 MHz, DMF-d7): δ (ppm) = 7.80 (2H, s), 7.18 (2H, s), 3.56 (2H, s), 2.73, 2.31, 1.83, 1.58, 1.91.13C NMR (75 MHZ, DMF-d7): δ (ppm) = 175.0 (C=O), 145.5, 145.0, 140.4, 139.7, 128.2 (C–O), 115.1, 107.2, 49.0, 43.0.19F NMR (300 MHz, DMSO-d6, ref. TFA [−77 ppm]): δ (ppm) = −141.9, −143.0, −153.1.FT-IR (thin film, cm−1): 2926 (C-H asym str), 2860 (C–H sym str), 1787 (C=O), 1726, 1636, 1509, 1406, 1356, 1295 (C–F), 1140 (−SO3H, asym str), 1132, 1039 (−SO3H, sym str), 981, 833, 698, 561. The acronym for this polymer will be P5FNDIHS (Figure 1).


## 2.4. Copolymerization

The copolymer was prepared via ROMP in a block fashion [11]. Firstly, monomer PhNDI, synthesized according to literature [8] and catalyst I were stirred in 1,2-dichloroethane at 65°C for 0.33 h. Then, monomer 5FNDI dissolved in 1,2-dichloroethane was added to the polymer solution and stirred at 65°C for 0.66 h (Scheme 1). The obtained copolymer C5FNDI was soluble in chloroform and dichloroethane. The incorporation of 5FNDI in copolymer was 32 mol% as determined by 1H NMR. The block copolymer obtained was hydrogenated as mentioned above and the pentafluorophenyl moieties of hydrogenated poly(N-phenyl-exo-endo-norbornene-5,6-dicarboximide-co-N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) (C5FNDIH) were sulfonated with 4-hydroxybenzenesulfonate dihydrate using the procedure used for the sulfonation of hydrogenated poly(N-pentafluorophenyl-exo-endo-norbornene-5,6-dicarboximide) (Scheme 2). The acronym for this copolymer will be C5FNDIHS and its composition is shown in Figure 1.


## 2.5. Membranes Preparation and Atomic Force Microscopy (AFM)

P5FNDIHS and C5FNDIHS membranes (in sodium salt form) were cast, respectively, from hotN,N-dimethylformamide solutions (~2 wt %) of P5FNDIHS and C5FNDIHS chains in a Teflon mold and dried at 70°C for 12 h. The films were immersed firstly in stirring methanol at room temperature for 3 h and secondly in deionized water for 1 h in order to remove the residual solvent. Afterwards, the membranes underwent a proton exchange treatment with 1.0 N hydrochloric acid during 12 h. Then, the films were washed repeatedly with deionized water until the rinse water became neutral. Finally, the membranes were dried under a vacuum at 120°C for 10 h.The surface morphology of the thin films was observed using tapping mode AFM (Multimode Nanoscope IVa, Digital Instrument/Veeco) under ambient conditions. In tapping mode, the stylus oscillates and touches the sample only at the end of its downward movement. The nominal resonance frequency for the tapping mode was between 265–309 kHz with a phosphorous (n) doped Si cantilever which had a spring constant that ranged from 20 to 80 N m−1. The set point in the AFM control program was adjusted to change the contact force between the tip and surface in order to detect the existence of morphologies.


## 2.6. Density, Water Uptake, and Ion-Exchange Capacity of the Membranes

The density of the dry membranes was measured by the flotation method using isooctane as solvent. The values of this parameter are shown in the first column of Table1.Table 1
Density in Kg m−3, ρ, water uptake in Kg H2O/Kg dry membrane, wu, IEC in equivalents of fixed anionic groups per Kg dry membrane obtained by titration, X-, and NMR, XNMR-, molecules of water per fixed ionic group, λ, and conductivity, σ, in S/m, at 30°C.
MembraneρwuX-XNMR-λx-λXNMR-σP5FNDIHS15000.6171.7502.06019.616.62.24C5FNDIHS13800.3730.2860.20472.5101.60.0134Weighed dry membranes were immersed in distilled water for several hours, removed from the solution, gently blotted with filter paper to remove superficial water, and weighed. From the weights of the dry membranes,md, and the membranes equilibrated with water, mw, the water uptake, wu, in g H2O/g dry membrane is obtained as wu=(mw/md)-1.The ion-exchange capacity (IEC) of a given membrane was measured by immersing the weighed dry membrane in a 1 N HCl solution for 1 h. Then the membrane was removed from the solution, washed several times with distilled water to eliminate the chloride acid absorbed, and finally immersed in a 1 N sodium chloride solution. The protons exchanged in the reaction(1)R-H+Na+⟶R-Na+H+
were estimated by titration with a very diluted NaOH solution. The values of IEC in equiv/Kg dry membrane were obtained as IEC=VN/md where V is the volume in L of the solution of NaOH of normality N (equiv/L) used in the titration, and md is the mass of the membrane in Kg.


## 2.7. Electromotive Forces of Concentration Cells

Electromotive forces of concentration cells made up of two semicells separated by the ion-exchange membrane were measured (Figure2). The configuration of the cells was Ag |AgCl| HCl solution (c1) |cation-exchangemembrane| HCl solution (c2)|AgCl|Ag, where c1 and c2 are the concentrations of the electrolyte in the left-hand and right-hand compartments of the concentration cells. Notice that the anion of the electrolyte must be reversible with that of the electrodes. The solution in each compartment was kept under strong stirring to minimize the formation of membrane-solution interface layers. The evolution of electromotive force, emf, of the cell with time was measured at 25°C with a 3645-20 Hioki voltage logger and recorded every second with a 3911-20 communication base apparatus via a PC. The emf of the concentration cell was taken as that one at which this quantity reaches a maximum.Figure 2
Concentration cell used to measure the electromotive force: (C) half cell, (E) electrodes, (M) ion-exchange membrane, and (S) magnetic stirrers.


## 2.8. Ohmic Resistance Measurements

The ohmic resistance of the membranes in the acid form was measured with a Novocontrol BDS system comprising a frequency response analyzer (Solartron Schlumberger FRA 1260) and a broadband dielectric converter with an active sample head. Gold disk electrodes were used in the impedance measurements carried out at several temperatures in the frequency window 4.9 × 10−2 – 1 × 107 Hz. The temperature was controlled by a nitrogen jet (QUATRO from Novocontrol) with a temperature error of 0.1 K during every single sweep in frequency (Figure 3). Measurements were carried out on molded disk-shaped samples of 60–100 μm thickness with diameters of 20 and 10 mm.Figure 3
Cell used to measure the ionic conductivity of the membranes.


## 3. Results and Discussion

Values of the water uptake and the ion-exchange capacity (IEC) of the membranes measured by titration are given in Table1. The values of the IEC estimated from the NMR spectra, also given in Table 1, somewhat differ from those determined by titration. Moreover, the number of moles of water per –SO3- group anchored to the polymer chains of the membranes are also shown in Table 1. It is worth noting that in spite of its relatively low IEC, the C5FNDIHS membrane exhibits a rather large number of molecules of water per anionic fixed group.The variation of the electromotive force,emf, of the concentration cell with time for several HCl solutions flanking the membrane of interest is shown in Figures 4 and 5. The ratio between the concentrations of the solutions in the concentrated, c2, and diluted, c1, compartments lies in the vicinity of 2. In all cases, prior to each experiment, the membrane was washed several times with distilled water until exhausting the free electrolyte inside the membrane and then was equilibrated with the solution used in the dilute compartment of the concentration cell. An inspection of the evolution of the curves in the figures shows that the emf of the concentration cell increases with time needing nearly 3 h in most cases to reach the maximum value and then decreases as time increases. The emf at the maximum of the curves was taken as the apparent electromotive force of the concentration cell flanked by electrolyte solutions with concentration c2/c1.Figure 4
Evolution of theemf of the P5FNDIHS membrane for different c2/c1 ratios: (□) 0.01/0.005, (•) 0.02/0.01, (▵) 0.1/0.05, (▾) 0.2/0.1, (◃) 0.4/0.2, (▸) 0.8/0.4, and (◊) 1.0/0.5.Figure 5
Evolution of theemf of the C5FNDIHS membrane for different c2/c1 ratios: (□) 0.01/0.005, (•) 0.02/0.01, (▴) 0.1/0.05, (▾) 0.2/0.1, (◃) 0.4/0.2, (▸) 0.8/0.4, and (◊) 1.0/0.5.Theemf of a concentration for an electrolyte Aν+z+Bν-z-→ν+Az++ν-Bz- is given by [12](2)emf=νRTz+F∫a1a2t+(c)dln⁡a±=νRTF∫a1a2τ+(c)dln⁡a±,
where a1 and a2 are, respectively, the activities of the electrolyte solutions in the compartments 1 and 2 of the concentration cell, t+ and τ+ (=t+/z+) are, respectively, the number of equivalents and moles of cations transported across the membrane by a Faraday of current, F, and ν=ν++ν- is the total number of moles of ions proceeding from the dissociation of the electrolyte. For monovalent electrolytes, such as HCl, (2) becomes(3)emf=-2RTF∫a1a2t+(c)dln⁡a±.Notice that for monovalent electrolytes,t+=τ+. Since transport numbers depend on the concentration of electrolyte, solution of (3) requires measuring the t+(c) profile across the membrane using the Hirthoff method, that is, determining the variation of concentration of electrolyte in a concentration cell flanked by the electrolyte at the same concentration c after passing a known amount of dc current across the membrane. However, if the concentration ratio c2/c1 is 2 or lower, the average transport number of the cation can approximately be estimated as(4)t+=emfemfmax⁡,
where emfis the experimental value of the concentration cell and emfmax can be obtained doing  t+=1  in (3), that is,(5)emfmax⁡=-2RTFln⁡a2a1.Values of the apparent proton transport numbers for different concentrations flanking the membrane are shown in Figure6.Figure 6
Variation of the apparent proton transport number with the geometric average of the molality of the solutions flanking the membrane in P5FNDIHS (squares) and C5FNDIHS (circles).The response of cation-exchange membranes in acid form to an alternating electric field of angular frequencyω is modeled by an electric circuit consisting of an ohmic resistance RM accounting for proton transport in the membrane in series with a parallel RC circuit. The RC circuit represents a Debye relaxation process with a single relaxation time τ=RC. Strictly speaking, relaxation processes are described by a distribution of relaxation times and as a result it is more realistic to replace the capacitor by a constant phase element of admittance Y*(ω)=Y0(jωτ)n,0<n≤1 [13]. The impedance of the circuit is given by(6)Z*(ω)=RM+R1+Y1(jωτ)n,
where Y1=RY0 is a dimensionless parameter. The complex plane plot  Z′′(ω)versusZ′(ω), called Nyquist diagram [14], is an arc intersecting the abscissa axis at ω→∞ and ω→0. Taking into account that limω→∞Z′(ω)=RM and limω→∞Z′′(ω)=0, the intersection of the arc with the abscissa axis at high frequencies gives the ohmic resistance of the membrane to proton transport. However, Nyquist plots for the acidic P5FNDIHS and C5FNDIHS membranes presented in Figures 7 and 8, respectively, show in addition to the polarization arc another arc, at higher frequencies, that presumably intersects with the abscissa axis at the origin. The real impedance where the two arcs intersect with the abscissa axis at the same point is the resistance RM of the membrane. On the other hand, the polarization arc in the low-frequency region does not intersect with the abscissa axis as (6) predicts but both |Z′′| and Z′ increase as frequency decreases. This behavior is presumably associated with a charge-transfer resistance RCT and a double-layer capacitance Cdl. The Warburg impedance [13, 15, 16] nearly always exhibits these two characteristics in such a way that it is conditioned by the diffusion of charges in the membrane-electrode interface. The value of this impedance for an interface of infinite thickness is given by(7)ZW*(ω)=σω1/2-jσω1/2,
where σ is a constant that depends on Σi (1/CibDi1/2) where Cib and Di are, respectively, the bulk concentration and diffusion coefficients of the reactant species i. As a result the modulus of the impedance scales as |ZW*(ω)| ~ω-1/2, that is, the double logarithmic plot of the modulus of the complex impedance is a straight line of slope −1/2 in the case of a double layer of infinite thickness. Although the results seem to support the existence of a Warburg impedance, there are not enough data in the low-frequency region that allow to reach a definite conclusion concerning the membrane-electrode double layer thickness.Figure 7
Nyquist plots at 10 (■), 20 (•), 30 (▲), 40 (□) y 50°C (○) for the P5FNDIHS membrane in the acid form equilibrated with distilled water. Inset: zoom of the Nysquit plots at 20°C and 40°C in the high-frequency region.Figure 8
Nyquist plots at 20 (■), 30 (○), 50 (▲) y 70°C (∇) for the C5FNDIHS membrane in the acid form equilibrated with distilled water. Inset: zoom of the Nyquist plots at high frequencies.To account for the arc intersecting with the origin at high frequencies, the equivalent circuit of the membrane (ohmic resistance of the membrane in series with a circuit made up of constant phase element in parallel with the polarization resistance) should be in parallel with a capacitor, in the case of a semicircle, or a constant phase element for an arc.An alternative method to determine the resistance of the membranes is the Bode diagram [17] consisting in the plot of both the modulus of the impedance and tan-1(Z′′/Z′) against frequency. According to (6),(8)lim⁡ω⟶0⁡|Z*(ω)|=Rp+RM;lim⁡ω⟶0⁡|Z*(ω)|=RM,ϕ=lim⁡ω⟶∞⁡tan-1[Z′′(ω)Z′(ω)]=0.
Illustrative Bode plots for the P5FNDIHS and C5FNDIHS membranes are plotted in Figures 9 and 10, respectively. The curves show that the modulus of the impedance undergoes a sharp decrease reaching a plateau whereas ϕ reaches a maximum at the plateau. The resistance of the membrane is taken as the value of |Z*(ω)| at the maximum of ϕ. It can be seen at very high frequencies that the modulus drops as a result of the fact that the capacitor in parallel with RM governs the impedance of the circuit. The results obtained for RM by the two methods are in rather good agreement. For examples the value of RM for the P5FNDIHS membrane at 30°C estimated from Nyquist and Bode plots are, respectively, 1.79 and 1.70 Ω. These results are 20.24 and 20.41 Ω for the C5FNDIHS membrane (see Table 2). For consistency, the results of the Bode plots obtained for RM will be used in the analysis below.Table 2
Comparative and illustrative results for the ohmic resistance,RM, and conductivity, σ, of the membranes at 30°C obtained from Nyquist and Bode diagrams.
MembraneRM (Nyquist), ΩRM (Bode), Ωσ (Nyquist), S/mσ (Bode), S/mP5FNDIHS1.791.702.132.24C5FNDIHS20.2420.410.01350.0134Figure 9
Bode diagram showing the variation of the modulus of the impedance|Z*| (lines) and the out-of-phase angle (ϕ=tan-1/(Z′′/Z′) (symbols) with the frequency at 20°C (solid line and filled circles), 40°C (dash line and open squares) and 60°C (dot line and filled triangles) for the P5FNDIHS membrane in the acid form equilibrated with distilled water.Figure 10
Bode diagram showing the variation of the modulus of the impedance|Z*| (lines) and the out-of-phase angle (ϕ=tan-1/(Z′′/Z′) (symbols) with the frequency at 20°C (solid line and filled circles), 40°C (dash line and filled squares), 60°C (dot line and open triangles), and 80°C (dash dot line and filled circles) for the C5FNDIHS membrane in the acid form equilibrated with distilled water.The resistanceRM of the membranes was measured at different temperatures and the corresponding conductivities were obtained by means of the familiar expression(9)σ=lR0S,
where l and S are, respectively, thickness and area of the membrane in contact with the electrodes. For comparative purposes the values of the conductivity at 30°C are shown in Table 1. Illustrative Arrhenius plots showing the temperature dependence of the conductivity of the membranes obtained from the resistances of the membranes estimated from Bode plots are shown in Figure 11.Figure 11
Arrhenius plot showing the temperature dependence of the P5FNDIHS (squares) and C5FNDIHS (circles) membranes.Figure12 shows representative morphologies of the P5FNDIHS and C5FNDIHS membranes. The molecular chains of the latter membranes contain, respectively, 68% and 32% molar fractions of phenyl and 4-oxybenzenesulfonic acid, 2,3,5,6-tetrafluorophenyl moieties bonded to the dicarboximide side groups. It is expected that these moieties are mutually incompatible and therefore segregations occur giving rise to nanosize domains observed in the AMF of C5FNDIHS. It is worth noting that the AFM of P5FNDIHS suggests a much more homogeneous membrane surface than that of C5FNDIHS. Moreover, it is expected that the surface of the dry P5FNDIHS and C5FNDIHS membranes has significant surface fluorine content compared to the theoretical bulky fluorine content owing to the low-surface energy of the tetrafluorophenyl moieties which provide a thermodynamic-driving force for the self-assembly at the surface air-polymer interface [18, 19].AFM topographic image for C5FNDHIS (a) and P5FNDIHS (b) membranes.
(a)(b)In spite of the high water uptake of the P5FNDIHS membrane, the moles of water per anionic fixed group in the membrane,λ, are of the same order as that reported for Nafion [20] and copolyimide acid membranes [21, 22]. However, it is surprising that the value of λ for the low IEC C5FNDIHS membrane is nearly four times that of the P5FNDIHS. This fact suggests that microphases separation in the latter membrane serves to compartmentalize an excess of water into the hydrophilic polar side chain domains, specifically in the vicinity of the dicarboximide side groups. It is worth noting in this regard that apparently dried naphthalenic polyimides may contain up to 10% of water. Moreover, 1H NMR experiments carried out on acidic naphthalenic polyimide membranes heated at 130°C under vacuum show peaks at 0.7–1 ppm corresponding to water associated with imide groups [23]. This water may be absorbed by the membranes during the NMR experiments handling.An inspection of the dependence of the electromotive force on time for the C5FNDIHS and P5FNDIHS membranes shows that a certain time is required to reach a maximum value and then decreases as time increases. Theemf of the concentration cell containing the former membrane falls to zero. The change is not so dramatic for the concentration cell with the P5FNDIHS membrane. The drop of t+ to zero for the C5FNDIHS membrane at long times, even for dilute concentration solutions, suggests that the concentration of electrolyte equalizes in the two compartments of the concentration cell presumably as a consequence of strong electrolyte diffusion. The drop of t+ with increasing concentration is not so dramatic for the P5FNDIHS membrane at low concentrations, but the decrease of the transport parameter is still significant. To explain this behavior the membranes can be viewed formed by hydrophilic pores to the walls of which anionic SO3- groups are anchored. These groups prevent the diffusion of coions across the pores and therefore hinder electrolyte diffusion thus increasing the transport number of counterions. The strong dependence of the counterion transport on electrolyte concentration suggests that the number of anionic fixed groups in the walls is not large enough to prevent coins diffusion across the membranes. As a result, electrolyte diffusion from the high-to the low-concentration compartment occurs, c2/c1 decreases, and the electromotive force of the concentration goes down. Owing to the rather high time necessary to reach a maximum and the rather high free ionic diffusion taking place in that period of time, the ratio a2/a1 presumably undergoes a significant decrease for the more concentrated solutions. Therefore, the emf at the maximum is the lower bound of this quantity and the transport number corresponding to the nominal values of c2/c1 should be higher than those obtained by means of (4).The curves showing the variation of the transport number of protons with the geometrical average of the molality of the solutions flanking the membranes show that both membranes are ideally permselective for very dilute solutions, but the permselectivity undergoes a rather fast drop with increasing concentration. When the electrolyte solutions are flanking the membranes, protons in the concentrated HCl solution migrate to the side of the membrane facing the diluted HCl solution. Because fixed ions in the membrane hinder chloride anions transport across the membrane, the side of the membrane in contact with the concentrated HCl solution is negatively charged whereas that in contact with diluted HCl solution is positively charged. As a result an electric potential is created inside the membrane that drags the pore liquid positively charged toward the concentrated electrolyte solution compartment, enhancing the osmotic flow.As the concentrations of the electrolyte solutions increase, chloride anions are not totally rejected by the fixed anions of the membrane, and diffusion of hydrochloric acid from the concentrated HCl solution compartment to the diluted HCl solution compartment occurs. Both the ionic diffusion across the membranes and the osmotic flow may be responsible for the low permselectivity of the membranes at high electrolyte solution concentration.In an earlier work we carried out the synthesis of the nonfluorinated poly(N-phenyl-exo-endo-norbornene-5,6-dicarboximide) which underwent nonuniform sulfonation of the phenyl groups by using acetyl sulfate as sulfonating agent [7]. The IEC of the membrane prepared from this ionic polynorbornene dicarboximide was 0.82 eq/Kg dry membrane and in spite of having a higher IEC, in comparison with that of the fluorine-containing C5FNDIHS membrane, the former membrane exhibited a water uptake of 0.124 Kg H2O/Kg dry membrane, about one-third of the value in this latter obtained by titration; additionally, the conductivity of the sulfonated membrane equilibrated with water was 0.0414 S/m, of the same order of that found for the fluorine-containing C5FNDIHS membrane. These results suggest that the sulfonic acid groups have not relaxed the attractive interactions between phenyl groups and that molecular piling of the aromatic rings has taken place inhibiting the emergence of microphases separation in the non fluorinated membrane and therefore decreasing the storage of an excess of water into the polar side chain domains, specifically in the vicinity of the dicarboximide side groups. As it is seen, the chemical structure plays an important role in this kind of macromolecules since the more fluorine content in the polymer the more water uptake of the membrane. Indeed, an increase in the density of sulfonic acid affects directly the proportional transport properties in the membrane as it is shown in the fluorine-containing P5FNDIHS that exhibits the highest IEC, water uptake, and ionic conductivity of all the ionic polynorbornene dicarboximides we have discussed so far.The conductivity of membranes with high water uptake is strongly dependent on the fixed ions concentration. Thus the P5FNDIHS membrane (average IEC = 1.90 eq/Kg dry membrane) exhibits a conductivity of 2.24 S/m, at 30°C, of the same order of that reported for high-conductivity acidic membranes and about two orders of magnitude higher than that of the C5FNDIHS membrane (average IEC = 0.245 eq/Kg dry membrane). Despite the low permselectivity of the membranes at high electrolyte solution concentration, the rather high level of ionic conductivity as well as water content seems promising for low-temperature fuel cell applications. Arrhenius plots representing the temperature dependence of the membranes, presented in Figure11, show that the activation of energy associated with proton transport across the P5FNDIHS membrane (11.7±0.8 kJ/mol) is less than one half of that corresponding to the C5FNDIHS membrane (29.3±1.6 kJ/mol).The study of the mechanism governing proton transport in acidic ion-exchange membranes has drawn the attention of many researchers [24, 25]. Ab initio simulations suggest that the proton state in bulk water and in water clusters fluctuates between more localized hydronium ion-like states or Eigen ions and more delocalized H5O2+-like states or Zundel ions in such a way that forming and breaking hydrogen bonds in the neighborhood of the proton location (Grotthus like hoping) may be responsible for proton transport [26–30]. Proton diffusion involving this mechanism presumably takes place in high-conductivity membranes, such as, the P5FNDIHS membrane, is named structural diffusion. In low-conductivity membranes, such as, the C5FNDIHS membrane, water acts as a carrier of protons, and the transport is called vehicular diffusion.


## 4. Conclusions

The efficient segregation of hydrophilic from hydrophobic moieties, presumably favored by the low polarity ofCar–F bonds attached to the phenyl groups, gives rise to the formation of percolation paths responsible for the rather high proton conductivity of the homopolymeric membranes. The copolymeric membranes absorb an unusual quantity of water despite their low IEC. It seems that microphases separation in the membranes serves to compartmentalize an excess of water into the polar side chain domains, specifically in the vicinity of the dicarboximide side groups.The electromotive force of the concentration cells undergoes a strong decrease at long times in the case of the homopolymeric membrane dropping to zero for the copolymeric membranes. The performance of the membranes in separation processes in diluted solutions is rather poor, unless the concentrations of the solutions at both sides of the membranes are continuously renewed.



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*Source: 835378-2012-06-21.xml*