Figures
Abstract
Poly(o-anisidine) molybdophosphate was expediently obtained by sol-gel mixing of Poly(o-anisidine) into the inorganic matrices of molybdophosphate, which was allowed to react with silver nitrate to the formation of poly(o-anisidine) molybdophosphate embedded silver nano composite. The composite was characterized by Fourier Transform Infrared Spectroscopy, X-ray powder diffraction, UV-Vis Spectrophotometry, Fluorescence Spectroscopy, Scanning Electron Microscopy/Energy-dispersive X-ray Spectroscopy and Thermogravimertic Analysis. Ion exchange capacity and distribution studies were carried out to understand the ion-exchange capabilities of the nano composite. On the basis of highest distribution studies, this nano composite cation exchanger was used as preparation of heavy metal ion selective membrane. Membrane was characterized for its performance as porosity and swelling later on was used for the preparation of membrane electrode for Hg(II), having better linear range, wide working pH range (2–4.5) with fast response in the real environment.
Citation: Khan A, Khan AAP, Asiri AM, Rub MA (2014) Synthesis of Silver Embedded Poly(o-Anisidine) Molybdophosphate Nano Hybrid Cation-Exchanger Applicable for Membrane Electrode. PLoS ONE 9(5): e96897. https://doi.org/10.1371/journal.pone.0096897
Editor: Dariush Hinderberger, Martin-Luther-Universität Halle-Wittenberg, Germany
Received: September 26, 2013; Accepted: April 14, 2014; Published: May 7, 2014
Copyright: © 2014 Khan et al. This is an open-access article distributed under the terms of the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original author and source are credited.
Funding: This paper was funded by King Abdulaziz University, under grant No. (D- 004/431). The authors, therefore, acknowledge technical and financial support of KAU. The funders had no role in study design, data collection and analysis, decision to publish, or preparation of the manuscript.
Competing interests: The authors have declared that no competing interests exist.
Introduction
Organic-inorganic hybrid materials, based on interactions between organic and inorganic components, have been extensively developed in the past decades [1]–[4]. The inorganic components include zeolite [5], layered structures [6]–[7], sometimes one dimensional polymers [8]; and the organic component could be small organic molecules, organometallics or organic polymers. The resultant hybrids may exhibit properties synergistically derived from the two components [9]. Molybdophosphate has interesting properties and practical applications, such as catalysts and cathode materials. Van der Waals bonds connect the nearest layers. Inserting guests (Ag) into the host will modify the properties of MoP and have interesting applications. Due to their anisotropic optical and electrical properties, electrochemical and electrochromic behaviors, conjugated polymers such as polypyrrole, polyaniline and polythiophene [10] have been used.
Generally, the synthetic methodology of a nanocomposite depends on the chemical and physical properties of the host inorganic materials and the guest organic polymers [11], [12]. It has been believed that the guest species needs to be soluble in some solvent system, whether miscible or immiscible with water. To date, most of polymer nanocomposites have been achieved through the direct insertion approach, where the polymers are first dispersed in water or organic solvent and then inserted into the layered structure. Another synthetic approach involves insertion of monomer first, followed by treatment with an oxidant. In this paper, this approach has been developed to prepare the intercalation of poly(ortho-methoxy aniline) POMA into MoP.
Design, fabrication and application of novel electrochemical sensors have been a topic of research in recent years [13], [14]. For this aspect, modification of membranes with suitable functionalities is an ongoing task among researchers world-wide because of its ability to improve the ion transfer rate from substrates to the membrane [15], [16]. In this topic of research, modification of membrane with heteropolyacids (HPAs) has received much attention [17], [18] owing to their attractive electronic and molecular properties, which results in novel applications in catalysis, materials science [19] and energy storage devices [20], [21] etc. However, the high solubility of heteropolyacids in aqueous media limits the stability of those modified membranes, as it leads to leaching of hetero polycation from the membrane surface and to the consequent drop of their electrochemical features. Composite prepared of inorganic matrix and conducting polymer have reduced leaching of exchanger due to its interactions with the polymer matrix and the poor solubility of the conducting polymer in water. In addition, inorganic clusters keep their integrity and activity while benefiting from the conducting properties and polymeric nature of the hybrid structure. Further incorporation of metal nanoparticles into the organic-inorganic hybrid materials offers enhanced performance due to the increase in conductivity and surface area. In this regard, we made an attempt to fabricate membranes with metal-incorporated organic-inorganic hybrid material for ion selective electrode, i.e. silver-incorporated POMA-MoP. Hence in the present paper, we developed a facile method to fabricate a metal-incorporated organic–inorganic composite-embedded membrane and its electrochemical properties.
Experimental
Reagents
The main reagents used for the synthesis of the material were obtained from CDH, Loba Chemie, E-merck and Qualigens (used as received). All other reagents and chemicals were of analytical grade.
Preparation of POMA-MoP/Ag
The polymerization of the monomer ortho-anisidine was initiated by the addition of oxidizing agent, i.e., ammonium persulfate in 1∶1 ratio under constant stirring at 5°C for 6 h. After 6 h a greenish color poly-o-anisidine polymer obtained [22]. The method of preparation of the inorganic precipitate of MoP ion-exchanger was very similar to that of Alberty and co-author [23] and Constantino [24] with slight modification.
The composite was prepared by the sol-gel mixing of POMA, an organic polymer into the inorganic matrices of MoP. In this process when the gels of POMA were added to the inorganic MoP with a constant stirring, the resultant mixture was turned slowly into brown colored slurries and kept for 24 hours at room temperature.
Now the resultant composite gels were filtered off, washed thoroughly with demineralized water (DMW) to remove excess acid and any adhering trace of oxidant. The washed material was dried over P4O10 at 45°C in an oven. The dried products were immersed in DMW to obtain small granules. They were converted to the H+ form by keeping them into 1 M HNO3 solution for 24 hours with occasionally shaking intermittently replacing the supernatant liquid. The excess acid was removed after several washing with DMW. The material was finally dried at 45°C and sieving to obtain particles of particular size range (∼125 µm). Hence a number of POMA-MoP/Ag nanocomposite cation-exchanger samples were prepared and on the basis of Na+ ion-exchange capacity (i.e.c.), and physical appearance, best one sample was selected for further studies.
Ion-exchange Capacity (i.e.c.)
The ion-exchange capacity, which is generally taken as a measure of the hydrogen ion liberated by neutral salt to flow through the composite cation-exchanger was determined by standard column process.
Thermal Studies
Simultaneous thermogravimetric analysis (TGA) studies of the composite cation-exchanger (POMA-MoP/Ag) in original form were carried out by an automatic thermo balance on heating the material from 10°C to 600°C at a constant rate (10°C per min) in the air atmosphere (air flow rate of 400 mL min−1).
Characterization
The FT-IR (Spectrum-100 FT-IR) spectrum of POMA-MoP/Ag in original form, dried at 40°C, was taken by KBr disc method at room temperature. UV-visible studies were carried out by Lamda-950, Perkin Elmer, Germany. Powder X-ray diffraction (XRD) pattern was obtained in an aluminum sample holder in original form using a PW 1148/89 based diffractometer with Cu Kα radiations. Microphotographs of the original form of POMA-MoP/Ag were obtained by the FE-SEM (FESEM; JSM-7600F, Japan) at various magnifications.
Selectivity (Sorption) Studies
The distribution coefficient (Kd values) of various metal ions on POMA-MoP/Ag nano-composite were determined by batch method in various solvent systems [25]. The distribution coefficient (Kd) was determined by using the following equation:(1)
(2)where, I is the initial amount of metal ion in the aqueous phase, F is the final amount of metal ion in the aqueous phase, V is the volume of the solution (mL) and M is the amount of cation-exchanger (g).
Preparation of POMA-MoP/Ag Cation-exchange Membrane
Ion-exchange membrane of POMA-MoP/Ag was prepared as the method reported by A.A. Khan and A. Khan [26] in earlier studies. To find out the optimum membrane composition, different amount of the composite (M-1 = 0.2 g, M-2 = 0.4 g, M-3 = 0.6 g) material was grounded to a fine powder and mixed thoroughly with a fixed amount of PVC (25%) dissolved in 10 mL tetrahydrofuran with one drop of plasticizers (Dioctyl Phthalate (DAP)). The resultant slurries were poured to cast in glass tube having 10 cm in length 5 mm in diameter. These glass tubes were left for slow evaporation for several hours. In this way, three sheets of different thicknesses 0.37, 0.39 and 0.40 mm were obtained. A fixed area of the membranes was cutted using sharp edge blade.
Characterization of Membrane
For the characterization of membrane, three important parameters such as water content, porosity and thickness of membrane are determined as previously described in the literatures [27], [28].
Water content (% total wet weight).
First, the membranes were soaked in water to elute diffusible salt, blotted quickly with Whatmann filter paper to remove surface moisture and immediately weighted. These were further dried to a constant weight in a vacuum over P2O5 for 24 h. The water content (total wet weight) was calculated as:(3)where Wd = weight of the dry membrane and Ww = weight of the soaked/wet membrane.
Porosity.
Porosity (ε) was determined as the volume of water incorporated in the cavities per unit membrane volume from the water content data:(4)where Ww = weight of the soaked/wet membrane, Wd = weight of the dry membrane, A = area of the membrane, L = thickness of the membrane and ρw = density of water.
Fabrication of Ion-selective Membrane Electrode
The membrane sheet of 0.40 mm thickness (M-3) as obtained by the above procedure was cut in the shape of disc and mounted at the lower end of a pyrex glass tube (o.d. 0.8 cm, i.d. 0.6) with araldite. Finally, the assembly was allowed to dry in air for 24 h. The glass tube was filled with 0.1 M mercuric nitrate solution. A saturated calomel electrode was inserted in the tube for electrical contact and another saturated calomel electrode was used as external reference electrode. The whole arrangement can be shown as:
Following parameters were evaluated to study the characteristics of the membrane such as lower detection limit, response curve, response time and working pH range.
Electrode Membrane Potential
To determine the membrane response, a series of standard solutions of varying concentrations ranging from 10−1 M to 10−10 M were prepared. External electrode and ion selective membrane electrode are plugged in digital potentiometer and the potentials were recorded.
For the determination of membrane potentials, the membrane electrode was conditioned by soaking in 0.1 M Hg(NO3)2 solution for 5–7 days and for 1 h before use. When membrane electrode was not in use it must be kept in 0.1 M Hg(NO3)2 solution. Potential measurement was plotted against selected concentration of the respective ion in aqueous solution.
Effect of pH
pH solution ranging from 1–10 were prepared at constant ion concentration i.e (1×10−2 M). The value of membrane potential at each pH was recorded and plot of membrane potential versus pH was plotted.
The Response Time
The membrane is first dipped in a 1×10−3 M solution of Hg(NO3)2 and then 10 fold higher concentration (1×10−2 M). The potential of the solution was read at zero second; just after dipping of the membrane electrode in the second solution and subsequently recorded at the intervals of 30 s. The value of electrode potential at each pH was recorded and electrode potential was plotted vs. pH.
Determination of Hg2+ by Potentiometric Titration using POMA-MoP/Ag Nano Composite Membrane Electrode
The practical utility of the proposed membrane electrode assembly was tested by its use as an indicator membrane electrode in the potentiometric titration of Hg(II) with ethylenediaminetetraaceticacid (EDTA).
Results and Discussion
New and novel nano Ag embedded composite material has been synthesized by the incorporation of electrically conducting POMA into the inorganic matrices of MoP, responsible for cation exchange selectivity. Schematic representation for the preparation is given in Fig. 1. Due to the high percentage of yield, better ion-exchange capacity, reproducible behavior, chemical and thermal stabilities, best sample was chosen for detail studies. The composite cation-exchange material possessed a good Na+ ion-exchange capacity (1.25 meq g−1).
Characterization
It is clear from the TGA curve of the composite cation-exchanger that upto 125°C only 3% weight loss was observed, which may be due to the removal of external H2O molecules present at the surface of the composite [29]. Further continuous loss of mass approximately between 125 to 600°C may be due to the slight conversion of inorganic phosphate into pyrophosphate (Fig. 2) and may be due to the slight decomposition of organic part of the material.
The FTIR spectrum of the composite cation-exchanger (Fig. 3) indicates the presence of external water molecule in addition to the –OH groups and metal oxides present internally in the material. The peak at the 1610 cm−1 may be due to interstitial water present in the composite material [30]. The peak at 1000 cm−1 may represent the presence of ionic phosphate groups [31] in the material. The additional band at between 1440 cm−1 can be ascribed to stretching vibration of C–N [32]. The characteristic peaks at around 1490 cm−1 and 1598 cm−1 are attributed to the stretching vibrations of N-B-N and N = Q = N rings respectively (where Q refers to Quinoid and B refers to Benzenoid ring).This indicates that the material contains considerable amount of OMA. The out of plane bending deformations of C-H in the substituted benzene ring are attributed to the band at 817 cm−1 that becomes stronger peaks due to the presence of metal effect.
The phase identification for the prepared hybrid material was carried out using powder X-ray diffraction shown in Fig. 4. The observed XRD pattern of POMA-MoP/Ag hybrid semi crystalline and low resolved diffraction peaks (2θ) characteristic of silver. Diffraction peak at about 25° shows the characteristic formation of POMA which is clearly visible in the case of hybrid material whereas the observed intensity of the peak was very low in the case of POMA-MoP/Ag hybrid material. Reason for such low intensity is due to the presence of silver in POMA-MoP/Ag hybrid material which modified the relative ratio between the crystalline and amorphous structures. Further, no XRD diffraction patterns are noticed for bulk POMA-MoP/Ag phase indicates that the MoP is finely dispersed in the POMA matrix. The presence of nanosized silver particles in the hybrid material induces lattice strain which contributes broadening of XRD peaks. However, the crystallite size and strain contributions to line broadening are independent of each other [33]. Hence, the total peak broadening is represented by sum of the crystallite size and strain contributions and it is calculated from the X-ray diffraction pattern using Williamson–Hall equation as follows(5)
The SEM was employed to investigate the morphology and size of the nanoparticles in the hybrid materials. Fig. 5a shows the representative FE-SEM image of POMA-MoP/Ag. The formed silver nanoparticles are polydisperse and of irregular morphology with two size. Fig. 5b shows the high resolution FE-SEM image of one of the silver nanoparticles. The grey shadow present in the image may be due the MoP layer covered on the silver nanoparticles. Thus, the FE-SEM images provide further evidence for the presence of silver nanoparticles in the polymer hybrid matrix.
In order to explore the potential of the composite material in the separation of metal ions, distribution studies for different metal ions were performed in different solvent systems. It was observed that the Kd- values vary with the nature of the contacting solvents. It was also observed from the (Kd) values (Table 1) that Hg2+ was strongly adsorbed and Zn2+, Ba2+, Ca2+ and Al3+ are significantly adsorbed while the remaining are partially adsorbed on the surface of ion-exchange material.
The optical property of the POMA-MoP/Ag was examined using UV–vis spectrophotometer at room-temperature and shown in Fig. 6. To measure the UV–vis absorption, the POMA-MoP/Ag were dispersed in distilled water and measured. The obtained UV absorption exhibits a well-defined exciton band at 300 nm, a characteristic and corresponding peak to single bulk compound and other peak related with impurities were not observed in the spectrum which confirms that the synthesized compound is in pure form.
Preparation of Hg2+ Ion-selective Membrane
In this study, POMA-MoP/Ag cation-exchanger was also used for the preparation of heterogeneous ion-selective membrane electrode. Sensitivity and selectivity of the ion-selective membranes electrode depend upon the nature of electro-active material, membrane composition and physico-chemical properties of the membranes employed. A number of samples of the POMA-MoP/Ag nanocomposite membrane were prepared (Table 2) with different amount of composite material and PVC and checked for the mechanical stability, surface uniformity, materials distribution, cracks and thickness, etc. But the membranes obtained with 25% PVC (w/w) were found suitable.
The heterogeneous precipitate Hg(II) ion-selective membrane electrode obtained from POMA-MoP/Ag material gives linear response in the range 1 ×10−1 M to 1×10−6 M. Suitable concentration were chosen for sloping portion of the linear curve. The limit of detection determined from the intersection of the two extrapolated segments of the calibration graph [34] was found to be 8 ×10−6 M, and thus the working concentration range is found to be 1 ×10−1 M to 8 ×10−6 M (Fig. 7.) for Hg2+ ions with a Nernstian slope of 28.5 mV per decade change in Hg2+ion concentration. The slope value is near to Nernstian value, 29.6 mV per concentration decade for divalent cation [35].
pH effect on the potential response of the membrane electrode were measured for a fixed (1×10−2 M) concentration of Hg2+ ions in different pH values. It is clear that membrane potential remains unchanged with in the pH range 2.0–4.5 (Fig. 8), known as working pH for this membrane electrode in acidic medium.
Another important factor is the promptness of the response of the ion-selective membrane electrode. The average response time is defined as the time required for the membrane to reach a stable potential. It is clear that the response time of the membrane sensor is found to be ∼10 s (Fig. 9).
The membrane electrode could be successfully used upto 3×1/2 months without any notable drift in potential during which the potential slope is reproducible within ±1 mV per concentration decade. Whenever a drift in the potential is observed, the membrane is re-equilibrated with 0.1 M metal nitrate solution for 4–5 days.
The selectivity coefficients, of various differing cations for the Hg(II) ion selective POMA-MoP/Ag nanocomposite membrane were determined by the mixed solution method [36]. The selectivity coefficient indicates the extent to which a foreign ion (Mn+) interferes with the response of the membrane towards its primary ions (Hg2+). By examine the selectivity coefficient data given in Table 3, it is clear that the membrane is selective for Hg(II) in presence of interfering cations.
The practical utility of the proposed membrane sensor assembly was tested by its use as an indicator electrode in the potentiometric titrations of Hg(II) with EDTA. The mercury selective membrane electrodes was employed as indicator electrodes in the titration of 1.0×10−2 M Hg(NO3)2 solutions against 1.0×10−2 M EDTA solution as a titrant. For this, 5 ml of Hg(NO3)2 solution was pipette out in a beaker. The volume of beaker was raised upto 20 mL by DMW. The solution was titrated with EDTA solution and electrode potential was measured after each addition of 0.5 ml of EDTA solution. The necessary adjustment of pH was made before adding the titrant. The addition of EDTA causes a decrease in potential as a result of the decrease in the free Hg(II) ions concentration due to its complexation with EDTA. The amount of Hg(II) ions in solution can be accurately determined from the resulting neat titration curve providing a sharp rise in the titration curve at the equivalence points. Some parameters of ion selective membrane electrode reported in literature compared with present studies given in Table 4 [37]–[41].
Conclusions
In this study, a novel silver embedded nano composite cation-exchanger POMA-MoP/Ag, having good ion-exchange capacity and thermal stability had been prepared successfully. This composite material was also utilized as an electro active component for the preparation of ion-selective membrane for the determination of Hg(II) ions in aqueous solution. The membrane showed a working concentration range 1×10−1–8×10−6 M, response time 10s, pH range 2–4.5, and selectivity in presence of other metal ions. The practical utility was determined as potentiometric sensor for the titration of Hg(II) using EDTA as a titrant. This is a material of interests for removal of water pollution in heavy metal ion source of Hg. Conductivity studies will be continuing in the next part of study.
Acknowledgments
This paper was funded by King Abdulaziz University, under grant No. (D- 004/431). The authors, therefore, acknowledge technical and financial support of KAU.
Author Contributions
Conceived and designed the experiments: AK AAPK AMA MAR. Performed the experiments: AK AAPK AMA MAR. Analyzed the data: AK AAPK AMA MAR. Contributed reagents/materials/analysis tools: AK AAPK AMA MAR. Wrote the paper: AK.
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