Synthesis and Characterization of Ag<sub><b>2</b></sub>S Layers Formed on Polypropylene

Krylova, Valentina; Dukštienė, Nijolė

doi:https://doi.org/10.1155/2013/987879

Journal of Chemistry

On this page

Abstract Introduction Experimental Results and Discussion Conclusions References Copyright Related Articles

Research Article | Open Access

Volume 2013 | Article ID 987879 | https://doi.org/10.1155/2013/987879

Synthesis and Characterization of Ag₂S Layers Formed on Polypropylene

Valentina Krylova¹and Nijolė Dukštienė¹

Academic Editor: Peter Chang

Received29 Jun 2012

Revised20 Aug 2012

Accepted28 Aug 2012

Published16 Jan 2013

Abstract

Silver sulphide, Ag₂S, layers on the surface of polypropylene (PP) film was formed by chemical bath deposition method (CBD). Film samples were characterised by X-ray photoelectron spectroscopy (XPS), attenuated total reflection Fourier transform infrared (ATR-FTIR) spectroscopy, scanning electron microscopy (SEM), atomic force microscopy (AFM), and X-ray diffraction analysis (XRD). The surface morphology, texture, and uniformity of the silver sulphide layers were formed on PP surface dependent on the number of polymer immersions in the precursor solution. XPS analysis confirmed that on the surface of the polypropylene film, a layer of Ag₂S was formed. ATR-FTIR and FTIR spectra analysis showed that the surface of Ag₂S layers is slightly oxidized. All prepared layers gave multiple XRD reflections, corresponding to monoclinic Ag₂S (acanthite). The Ag₂S layer on polypropylene was characterized as an Ag⁺ ion selective electrode in terms of potential response and detection limit. The electrode was also tested as an end-point electrode for argentometric titration of thiamine hydrochloride.

1. Introduction

Polymers modified by thin electrically conductive or semiconductive films of binary inorganic compounds, particularly of metal chalcogenides [1–4] represent a new class of materials—composites. The application of these composites is determined by their properties, wheares the latter depend significantly on the preparation method, even the chemical composition and structure of composites slightly change [5, 6].

In the last few years, there is a growing interest in Ag₂S films because of their unique electrical [7, 8], optical [9], photovoltaic [10], and thermoelectric properties [11, 12].

These unique properties suggest potentially broad applications of Ag₂S films in various devices such as solar cells, super ionic conductors and semiconductors, photo detectors, photo thermal conversion, electroconductive electrodes, microwave shielding coating, gas sensors functioning at temperatures tending to room temperature, polarizer’s of infrared radiation, and active absorbents of radio waves [5, 6, 13–15].

The properties of Ag₂S films can be successfully utilized by deposition its layers (either by in situ or ex situ methods) onto polymer surface, since a polymer can be easily designed into almost any shape required by a particular application. Additionally, the polymer can also act as the controlled environment for the growth of the film layers. Furthermore, the Ag₂S/polymer composites may exhibit new properties that differ from those of single Ag₂S films, arising from the spatial orientation and network arrangement. Therefore, the ability to prepare such composites on a large scale is an important goal of materials science.

The properties of Ag₂S/polymer composites are very sensitive to preparation technique and significantly depend on the nature of polymer on which Ag₂S layers are formed. Recently, there have been a number of papers suggesting different methods for the incorporation of silver sulphide nanocrystals in different polymer matrices and their characterization. The well-dispersed Ag₂S nanoparticles incorporated in polyvinylpyrrolidone (PVP)/fibre matrices using the electrospinning technique [16]. Kumar et al. [17] have applied a sonochemical method for the preparation of Ag₂S nanoparticles in the presence of polyvinyl alcohol. Composite thin films consisting of nanosized Ag and Ag₂S particles dispersed in nylon 11 thin films have been prepared by using a thermal relaxation technique [18]. Wang et al. developed a gas/solid reaction method based on surface initiated atom transfer radical polymerization (ATRP) for fabricating nanoparticles/polymer composite thin films, while preventing the aggregation of nanoparticles; thus the reaction may happen on the surface of composite thin films [19].

This present study focuses on the deposition of Ag₂S layers on the polypropylene (PP) by the chemical bath deposition method (CBD). PP film is characterized by many excellent properties than other polymers. This is a low density, high thermal resistance, high strength at high flexibility, resistance to cracking under stress and a very good chemical stability [20].

The CBD method is relatively simple and inexpensive, and highly reproducible technique. The technology is based on slow controlled precipitation of the Ag₂S through the reaction between Ag⁺ and sulphur compounds as the sulphur source.

In the past decade, Ag₂S thin films by CBD method have been successfully prepared on silica [21], glass [22], biopolymer matrix [23], indium doted tin oxide (ITO) film [24], and polyamide (nylon) surfaces [25].

The sulphur precursors were usually thiourea [24], the elemental sulphur dissolved in a concentrated NaOH solution [26], thioacetamide [27], sodium sulphide [25], sodium thiosulphate [3], dimethylthiourea [6] and toxic carbon disulphide (CS₂) in ethanol [28]. The most pronounced role in the formation of the Ag₂S particles and consequently deposits has been played by the complexing agents. An ethylenediaminetetraacetate disodium salt (EDTA) [8] and ammonia solution [21] acting as a complexant for Ag ions or as a catalyst is usually employed to control the reaction rate. The commonly accepted underlying mechanism involves alkaline solution (pH 6−10) as ammonia for pH adjustment [8] and higher temperature 30−80°C [21].

However, the adding of complexing agent increases experimental parameters whereas the nonaqueous medium is expensive or toxic generally.

In this paper we report on the depositing of Ag₂S layers by CBD from an acidic aqueous solution containing silver nitrate and an excess of sodium thiosulphate at 20°C temperature. The replacement of complexing agents with excess of sodium thiosulphate results to the simpler reaction mechanism. A reaction mechanism for depositing continuous Ag₂S layer has been examined, and the optimal precursor’s concentrations in solution are suggested. The chemical composition, structural, and morphological properties of Ag₂S layer formed on polypropene surface have been investigated. The Ag₂S layer formed on polypropene was also tested as an indicator electrode for argentometric titration of thiamine hydrochloride (vitamin B₁).

2. Experimental

15 mm × 70 mm size samples of nonoriented isotactic polypropylene (PP) film of 150 μm thicknesses (Proline X998, KWH Plast, Finland) were used for the experiments.

Before Ag₂S formation process, the hydrophobic PP sample requires a previous surface treatment process in order to facilitate its adhesion properties. Polymer was treated for 25 min at 90°C with etching solution (H₂SO₄/H₃PO₄(1 : 1), saturated with CrO₃). The formation of Ag₂S layers on PP was carried out in the glass reactor. Etched PP films were immersed for 40 min in aqueous Na₂S₂O₃ (0.2 mol/dm³) and AgNO₃ (0.08 mol/dm³) solutions at 20°C with pH 2.3. Then obtained samples were removed from reaction solution, rinsed with distilled water and dried at room temperature. The Ag₂S/PP samples were subjected for repetitive immersions in order to increase Ag₂S amount. The Ag₂S/PP samples were repeatedly immersed in the freshly prepared reaction solution. The immersions procedure was repeated for 5 times.

Distilled water, and analytically pure Na₂S₂O₃·5H₂O, AgNO₃, reagents were used to prepare reaction solutions.

Solutions’ pH was measured by using pH-meter WTW330, with combinative glass and Ag/AgCl electrode and temperature meter WTW SenTix 41 (Germany).

Before the chemical analysis, samples of PP strips plated with Ag₂S films have been mineralized. Samples were treated under heating with 6 mol/dm³ nitric acid to oxidize sulphur compounds to sulphates. Heating with concentrated hydrochloric acid removed the excess of nitric acid. The resulting solution was poured into a 25 cm³ flask and made up to the mark with distilled water. Then the 5 cm³ of this solution was taken for the sulphur concentration determination, and remaining part was used to determine the silver concentration.

Sulphur concentration in the silver sulphide layer was determined turbidimetrically [29]. Sulphate ions in the range from 1 mg/dm³ to 15 mg/dm³ may be readily determined by utilising the reaction with barium chloride in a solution slightly acidified with hydrochloric acid to give barium sulphate. A glycerolethanol solution helped to stabilise the turbidity of the barium sulphate suspension. The measurement of the intensity of the transmitted light as a function of the concentration of the suspension of BaSO₄ was carried out with a GENESYS 20 spectrophotometer (Thermo Spectronic, UK), at a wavelength nm. The standard deviation of the method with the photometric procedure in the range of concentrations from 5 mg SO₄²⁻ dm³ to 10 mg SO₄²⁻ dm³ was ±8%.

Silver concentration was determined with an atomic Perkin-Elmer absorption meter 503 ( nm). The sensitivity of the method is 0.06 μg/cm³ for 1% Ag absorption.

The content of silver and sulphur was expressed as μmol/cm². Three samples of each PP strip plated with Ag₂S film have been used to determine the concentration of silver and sulphur.

The scanning electron microscope (SEM) Quantax 200 with a detector X Flash 4030 (Bruker AXS Microanalysis GmbH, Germany) was applied for the obtained Ag₂S layers surface analysis.

The surface morphology of the films was investigated using an atomic force microscope (NANOTOP-206, Microtestmachines, Belarus). An ULTRASHARP Si cantilever (force constant 5.0 N/m, curvature radius less than 10 nm) was used. The measurements were performed in the contact mode. The AFM characteristics: maximum scan field area up to microns, measurement matrix up to points. The image processing and the analysis of scanning probe microscopy data were performed using a Windows-based program (Surface View version 2.0).

XPS measurements were performed with a Vacuum Generator (VG) ESCALAB MKII spectrometer. The nonmonochromatic Al Kα X-ray radiation ( eV) was used for excitation. The Al twin anode was powered at 14 kV and 20 mA. The photoelectron takeoff angle with respect to the sample surface normal was 90°, and XPs spectra of Ag 3d_5/2, S 2p_3/2, and O 1s were taken at a constant analyzer energy mode (at 20 eV pass energy). The base pressure in the working chamber was kept bellow Pa. The spectrometer was calibrated relative to Ag 3d_5/2 at eV and Au 4f_7/2 at eV. The quantitative elemental analysis was done by estimating peak areas and taking into account empirical sensitivity factors for each element [30]. A standard program was used for data processing (XPS spectra were treated by a Shirley-type background subtraction and fitted with mixed Gaussian-Lorentzian functions). Binding energies were referenced to the C 1s (284.5 eV) on unsputtered surfaces. All samples were scanned as received—without ion beam surface cleaning procedure. Assignation of the signals to specific structures or given oxidation state of elements analysed was done by comparison with data reported by NIST Standard Reference Database 20, Version 3.5 [31] and to the literature references.

The changes in chemical structure and binding configuration of a thin layer were analyzed by attenuated total reflectance (ATR) spectroscopy, since ATR spectroscopy is an often chosen technique as it may be used to obtain the spectra of the surfaces of the adhesive sides of a sample. ATR-FTIR spectra were recorded in the wavenumber range 4000–600 cm⁻¹ by the compensation method. In the 600–100 cm⁻¹ spectral region, were recorded FT-IR spectra. Ag₂S deposits were scraped with a nonmetallic scraper, and then scrapings were solid mixed with CsI, modulated into pellets and subjected to FT-IR spectroscopy. Spectra were recorded on a Perkin Elmer FT-IR Spectrum GX spectrophotometer (USA) by averaging 64 scans with a wave number resolution of 1 cm⁻¹ (0.3 cm⁻¹) at room temperature.

X-ray diffractometry was carried out under a Brag Brendan circuit on a diffractometer (Dron-6, Russia) using Cu Kα ( nm) radiation, 30 kV voltage, and 30 μA current. The scanning range was 2θ = 22–60°. The scanning speed was 1°·min⁻¹. Results were registered in in situ mode with a computer, and X-ray diffractograms of samples were treated using the Search Match, Xfit, ConvX, Dplot95, and Photo Styler programs.

Potentials were measured by using modified microprocessor HI 2200 (Hanna Instruments USA) relative to the reference Ag, AgCl/KCl_(sat.) electrode. The indicator electrodes were Ag₂S/PP samples. The potentiometric measurements were made with the following electrochemical cell Ag/AgCl/KCl_(sat.)//sample solution/Ag₂S/PP/Ag. The Ag₂S/PP electrode was soaked in 0.01 mol/dm³ AgNO₃ solution for 2 h before each measurement.

The 0.100 g amount of vitamin B₁ (thiamine hydrochloride CAS RN67-03-8) powder was dissolved in 20 cm³ of water. The resulting solution was poured into a 100 cm³ volumetric flask and made up to the mark with distilled water. 50 cm³ of the sample solution containing 50 mg of thiamine was transferred into a beaker, 10 cm³ of distilled water or 10 cm³ of 1 mol/dm³ NaOH was added, and resulting solution was titrated with 0.01 mol/dm³ silver nitrate solution in 0.5 cm³ increments using Ag₂S/PP membrane electrode. The end point of the titration was determined from the Gran plots.

3. Results and Discussion

3.1. Ag₂S Layers Formation Mechanism on a PP Film in Chemical Bath Deposition Process

The silver sulphide layers may be deposited on the PP films by immersing polymer in aqueous solutions of silver nitrate (AgNO₃) and sodium thiosulphate (Na₂S₂O₃). When a soluble sodium thiosulphate reacts with a silver nitrate, insoluble silver thiosulphate, Ag₂S₂O₃, (the solubility product for Ag₂S₂O₃ is [32]) is formed by reaction

Ag₂S₂O₃ is comparatively unstable and hydrolyzes to release Ag₂S into the reaction solution:

The initial experiments indicated that the usage of 0.2–0.1 mol/dm³ AgNO₃ and 0.2–0.1 mol/dm³ Na₂S₂O₃ solutions for Ag₂S layers depositing on PP, results in quick settle of Ag₂S precipitates on reactor bottom and layers on polypropylene could not be formed. Therefore, the slow precipitation of silver sulphide particles is essential for the formation of the layers on polymer surface.

In order to diminish the rate of silver sulphide formation process, the silver ions were complexed by thiosulphate ions. When the sodium thiosulphate solution was added into the aqueous silver nitrate solution, silver ions were coordinating with some thiosulphate groups, resulting in the relatively high silver ions concentration around these groups. In the presence of thiosulphate excess, the soluble [Ag₂(S₂O₃)₂]²⁻, [Ag₂(S₂O₃)₃]⁴⁻ and [Ag₂(S₂O₃)₄]⁶⁻ complexes are formed.

In nitric acid solution, these complexes decomposed, and they slowly released S²⁻ ions combined with the Ag⁺ ions to form a very insoluble Ag₂S (the solubility product for Ag₂S is [32]) nuclei on some special sites of PP.

Simultaneously, the side reactions are also possible.

The thiosulphate can react with nitric acid forming thiosulphuric acid by reaction:

The formed thiosulphuric acid may slowly decompose, and the new structural units such as elemental sulphur appear:

Elemental sulphur can dissolve in nitric acid by reaction:

Silver nitrate and sulphur acid can react to form silver sulphate:

The incorporation of impurities such as a silver sulphate and sulphur is quite possible in the bulk Ag₂S layer.

It was found that the 0.08 mol/dm³ AgNO₃ and 0.20 mol/dm³ Na₂S₂O₃ solutions are the most suitable for the formation of silver sulphide layers on polypropylene surface at pH 2.3 and 20°C temperature.

3.2. Chemical Analysis of Ag₂S Layers

As mentioned above, the preparation method influences the composition and properties of sulphide layers. Therefore, the initial stage of the work was aimed to establish the chemical composition of the deposited silver sulphide.

The chemical composition of silver sulphide layer obtained for different PP film immersion time in 0.08 mol/dm³ AgNO₃ and 0.20 mol/dm³ Na₂S₂O₃ solutions at 20°C is presented in Table 1. The molar ratios of silver to sulphur show that the stoichiometric silver sulphide and nonsulphide sulphur can coexist in synthesised layers.

3.3. Morphology of Ag₂S Layers

Figure 1 shows the representative SEM images of an Ag₂S layers on PP surface formed after 5 immersions (40 min each) of polymer in precursor solution. The sulphide surface exhibits nonhomogeneous morphology. The irregularly shaped grains join to form different sized islands on PP surfaces. The maximum size of islands is μm and the smallest μm. The large number of micro bumps and irregularly spread clusters are also visible.

The AFM images of Ag₂S layers on PP surface are shown in Figures 2 and 3. The Ag₂S layer exhibits a grain-type surface morphology; however, the size of grains, like the roughness of layer depends on the number of polymer immersion time in precursor solution.

(a)

(b)

(a)

(b)

When the polymer was immersed for 1 cycle in precursor solution, the irregular growth of different shaped grains is observed (Figure 2). The height of grains changed from 36 nm to 108 nm, and the average width was about 148 nm. In the local regions of layer surface, some of grains coalescence forming aggregates. The width of aggregates changed from 0.54 to 0.97 μm. The maximum height of the aggregates was about 138 nm. The appreciable numbers of bumps is also observed on polymer surface (Figures 2(a) and 2(b)). The root mean square roughness () was 25.9 nm, while an average roughness () was about 20.2 nm. The value is greater than , which support the rough morphology of Ag₂S layer surface.

The increase of polymer immersions times of in precursor solution leads to PP surface fulfillment. When the number of immersions was increased up to 5 (Figure 3), the rather large agglomerates composed of the different size particles are observed on surface. The width of aggregates changed from 0.56 to 1.6 μm. The maximum height of the aggregates increased up to 162 nm. On the other hand, in the regions surrounding aggregates, the numerous grains are still observed. The width of grains varied from 28 to 200 nm, while the height of grains equaled to 46–48 nm. The parameters and are of higher magnitudes, namely, about 33.8 and 25.5 nm, respectively, suggesting a rather rough surface.

3.4. XPS Analysis of Thin Ag₂S Layers

Ag₂S layers deposited on PP surface were examined by XPS measurements. The core levels S 2p, Ag 3d_5/2, and O 1s spectra were measured. During formation of the Ag₂S layer on the surface of polypropylene, all processes proceed in an open medium; therefore, it is not possible to avoid ambient effects. Since the surface of this layer is active, it adsorbs oxygen, water, and other contaminants [33, 34]. The sulphide layer on the PP surface is non-homogeneous (Figure 1) enabling an easy contact of the atmospheric oxygen with silver and sulphur ions. Therefore, the composition of the Ag₂S layer on the surface can differ from the chemical composition of the entire layer. It is necessary to emphasize that the XPS method investigates a very thin (up to few nm) surface layers.

The analysis of experimental XPS data shows that the composition of Ag₂S layers formed at different immersions time is rather similar. They consist of silver, sulphur, and oxygen in various combinations (Table 2).

The S 2p_3/2 spectra for film samples show three peaks at about 160.8, 163.0, and 168.8 eV.

According to the NIST XPS date base [31], the S 2p_3/2 peak at 160.8 eV is assigned to Ag–S–Ag bonding of Ag₂S, and the S 2p_3/2 peak at 163.0 eV is assigned to –S–S–bonding. The latter is about from 13.77 to 23.66% of S 2p_3/2 peak (Table 2), depending on the immersion time. This peak probably resulted from the chemisorbed sulphide nanoparticles, rather than the incorporation of elemental sulphur, since the S 2p_3/2 peak occurs above 164.0 eV [35]. A spectral line at higher energies of about 168 eV originates from oxidized sulphur [36]. For all samples, the higher energy S 2p_3/2 peak position at 168.8 eV well coincides with the known Ag₂SO₄ position (168.6 eV) [31]; therefore, we assign this peak to sulphur(VI) bond to oxygen.

According to the literature data, Ag 3d_5/2 core level, located at 368.3 eV, corresponds to binding energy of metallic silver [37], while the line at lower energies of 367.8 eV indicates the presence of Ag⁺ [38, 39]. The peaks of Ag 3d_5/2 at 368 eV and S 2p_3/2 at 161.2 eV are the characteristic binding energies for the Ag₂S [26], whereas the Ag 3d_5/2 line for Ag bounded to sulphur has been reported at 368.9 eV [40]. The Ag 3d_5/2 component with binding energy of 367.9 eV was reported for Ag₂O [41], while for AgO, it shifted by 0.5 eV to value of 367.4 eV [42]. Summarising analysis data of experimental Ag 3d_5/2 peak detected in the range between 368.5 to 368.0 eV (Table 2), it is difficult to distinguish between Ag–O–Ag and Ag–S–Ag bond position. However, concerning the S 2p_3/2 core levels (Table 2), it can be noted that the majority of the sulphur is in the S²⁻ state, confirming that the obtained layers are indeed Ag₂S.

The XPS spectrum for O 1s can be deconvoluted into free different contributions with binding energies at around 531.0, 532.0, and 533.3 eV (Table 2). The peak at around 533.3 eV on the high binding energy side of the O 1s region was ascribed to the atmospheric oxygen adsorbed on the layer surface. The peak with binding energy of 529.5 eV was reported for Ag₂O [41]. Two peaks at 528.7 and 531.0 eV are observed in the O 1s spectrum of AgO [43]. The presence of component at 531.0 eV in all studied O 1s spectra confirms that the silver sulphide surface layer oxidized.

3.5. ATR-FTIR Analysis of Ag₂S Layers

Seeking to investigate the changes of the chemical composition of the untreated PP, etched PP, and PP samples, coated with a layer of silver sulphide, ATR-FTIR spectra (Figure 4) were recorded.

(a)

(b)

Figure 4(a) shows ATR-FTIR spectra of untreated (curve 1), etched polypropylene film (curve 2), and PP samples, coated with a layer of silver sulphide (curve 3) in the range of 4000 to 600 cm⁻¹, and Figure 4(b) displays FTIR spectrum of PP samples, coated with a layer of silver sulphide in the range of 600 to 100 cm⁻¹.

The PP sample ATR-FTIR spectrum (Figure 4(a), curve 1) displays absorption peaks which coincide well with the reported literature data [44]. In polypropylene spectrum, moderate absorption peaks of deformation vibrations of the plane methylene group arise in the spectral range of 1445 to 1485 cm⁻¹, and methyl groups vibrations are registered in range of 1430–1470 cm⁻¹ or 1365 to 1395 cm⁻¹. These peaks in our spectrum appear at 1451 cm⁻¹ and 1375 cm⁻¹, respectively. A broad and intense band at around 2915 cm⁻¹ was attributed to vibrations of CH bands. The absorption features at 840, 1000, and 1170 cm⁻¹ are characteristic vibrations of terminal unsaturated CH₂ groups present in isotactic PP [44]. These characteristic features in our experimental spectrum are observed at 840, 990, and 1165 cm⁻¹ (Figure 4(a), curve 1).

ATR-FTIR spectrum of etched PP sample (Figure 4(a), curve 2) shows some changes. The characteristic peaks sharply diminish, and a new signal appears at 1719 cm⁻¹. This signal is probably due to superposition of signals at 1710 and 1724 cm⁻¹, characteristic of carboxylic and carboxylic stretching vibrations, respectively [45]. The spectrum of etched PP confirms that the oxidizing pretreatment of polypropylene increases surface hydrophility. Better hydrophilic characteristics of PP surface induce electrostatic interactions between the charged sites of the polymer and the sulphide particles, providing its adhesion to the polymeric surface.

The ATR-FTIR spectrum of PP samples covered with Ag₂S layers (Figure 4(a), curve 3) shows that the intensity of peaks, characterising etched PP, decreased, and two new broad vibration bands at 1137 cm⁻¹ and 640 cm⁻¹ appeared. On the grounds of the literature data [46–48], the bands in the range of the wavenumbers 1000–1250 cm⁻¹ correspond to vibration frequencies of the S–O band: in the range of 1186–1224 cm⁻¹, it corresponds to the asymmetric valence S–O vibrations, (S–O), while the peaks corresponding to the symmetric valence S–O vibrations, (S–O), appear in the interval of 1018–1095 cm⁻¹. According to the reported data [47], the sulphates vibration modes arise in the wavenumber range of 1080–1130 cm⁻¹ and 610–680 cm⁻¹. The scissoring vibration mode of the O−S−O group occurs as a strong band between 400–650 cm⁻¹ [49].

Therefore, the peak of 640 cm⁻¹ to the symmetric deformation of O–S–O vibrations, (O–S–O), and the peak of 1137 cm⁻¹ corresponds to the asymmetric deformation of O−S−O vibrations, (O–S–O).

The broad absorption band maximum at 237 cm⁻¹ observed in FTIR spectrum (Figure 4(b)) corresponds to characteristic vibrations of Ag−S and is in good agreement with reported data for Ag₂S [48, 50].

3.6. XRD Analysis of Thin Ag₂S Film Layers

The deposited Ag₂S layers were subjected to X-ray diffractometry to investigate the crystallographic structure of these layers. Structural studies of the Ag₂S deposits on polypropylene are limited by the crystallinity of the PP film itself. The intensity of its peaks exceeds the intensity of silver sulphide peaks several times in . Therefore, XRD diffractograms of samples were recorded in the range between 22 and 60°.

Figure 5 presents the X-ray diffraction pattern of the as-prepared Ag₂S/PP composites. The phase composition was determined by comparing Ag₂S/PP composites XRD diffraction patterns with those of known minerals. Diffraction pattern gave dominant peaks at 26.189° (the crystallographic planes (111), 29.063°(012), 31.820°(120), 33.666°(121), 34.743°(112), 36.806°(022), 37.6°(200), 40.798°(031), 43.47°(130), 46.28°(202), and 53.21°(004)) and showed the polycrystalline nature of the prepared Ag₂S layer. The diffraction patters were indexed to the monoclinic Ag₂S phase and are in good agreement with the reported data for α-Ag₂S (acanthite) (JCPDS Card File: 00-014-0072).

3.7. Application of Ag₂S/PP Layers for Potentiometric Measurements

To assess the practical applicability of the prepared silver sulphide layer on polypropylene films, an attempt was made to test Ag₂S/PP composite as an Ag⁺ ion selective electrode.

For analytical applications, the response time of a sensor is an important factor. The average time to reach a potential within ±1 mV of its final equilibrium value was measured after successive immersion of the Ag₂S/PP composite electrode in a series of AgNO₃ solutions of different concentration, each having a 10-fold increase in Ag⁺ ion concentration from to mol/dm³. The ionic strength of solutions was 0.1 mol/dm³. The static response time for Ag₂S/PP composite electrode obtained was 20 s for mol/dm³ Ag⁺ ion concentration, while at lower concentrations the response time increased up to 60 s.

A linear potential response was obtained in the concentration range from to mol/dm³ (Figure 6). The change in slope per decade change in Ag⁺ ion concentration was found to be slightly lower than that of 25.6 mV decade for a theoretical Nernstian response, which is the expected value for a univalent ion. A potential deviation from linear behaviour was observed in the concentration range below mol/dm³.

The Ag₂S/PP composite electrode was also tested as an end-point indicator electrode in potentiometric titration involving Ag⁺ ions. The method can be applied for the determination of thiamine hydrochloride.

In highly alkaline medium, thiamine undergoes chemical transformation and loses two protons through two distinct dissociation steps. The reaction occurs through intramolecular addition of the amino group of thiamine to the thiazolium ring with loss of first proton, accompanied by opening of the thiazole ring and loss of a second proton [51]. These protons can be replaceable by Ag⁺ ions. In presence of sodium hydroxide, the silver ions do not react with free chloride but react with thiols only [52].(7)(8)

The solubility product of AgOH () is higher than that of AgCl (); therefore, the precipitation of AgCl would be suppressed by the addition of NaOH excess. In alkaline medium, Ag₂S/PP does not respond to HO⁻ ions; hence, this electrode can be used as an indicator electrode for the determination of thiamine content in vitamin B₁.

The potentiometric titration curves of 0.0024 mol/dm³ thiamine with 0.01 mol/dm³ silver nitrate in alkaline medium are shown in Figure 7. There is a clear potential break (Figure 7) corresponding to the consumption of 0.78 mole of silver nitrate per mole of thiamine.

4. Conclusions

Ag₂S layers were successfully prepared at 20° temperature on polypropylene (PP) immersed in a bath containing the aqueous solutions of 0.08 mol/dm³ silver nitrate and 0.2 mol/dm³ sodium thiosulphate solution. The surface morphology, texture, and uniformity of the silver sulphide layers formed on PP surface dependent on the number of polymer immersions in the precursor solution. Chemical and X-ray photoelectron spectroscopy analyses confirmed a formation of silver sulphide on polypropylene surface. ATR-FTIR and FTIR spectra analysis showed that the surface of Ag₂S layers is slightly oxidized. The XRD studies indicated that the deposited layers were polycrystalline with monoclinic (acanthite) crystal structure. The Ag₂S/PP sensor exhibited low detection limit and therefore, are promising as indicating electrode in argentometric titration of vitamin B₁ as well as a sensor for determination of silver ions.

References

V. Krylova and N. Dukštienė, “Characterization of Cu_xS layers obtained by adsorption-diffusion method on polycaproamide from K₂S₅O₆ solutions,” Polish Journal of Chemistry, vol. 80, no. 9, pp. 1435–1447, 2006.
View at: Google Scholar
V. Krylova, “Spectroscopic and diffraction studies of chemical deposition of copper sulfide films on polyamide surface using potassium pentathionate,” Materials Science—Poland, vol. 25, no. 4, pp. 933–945, 2007.
View at: Google Scholar
F. I. Eczema, P. U. Asogwa, A. B. C. Ekwealor, P. E. Ugwuoke, and R. U. Osuji, “Growth and optical properties of Ag₂S thin films deposited by chemical bath deposition technique,” Journal of the University of Chemical Technology and Metallurgy, vol. 42, no. 2, pp. 217–222, 2007.
View at: Google Scholar
V. Krylova and M. Andruleviçius, “Optical, XPS and XRD studies of semiconducting copper sulfide layers on a polyamide film,” International Journal of Photoenergy, vol. 2009, Article ID 304308, 8 pages, 2009.
View at: Publisher Site | Google Scholar
R. R. Pradhananga and L. K. Shrestha, “Application of Ag-ion selective electrode for the determination of solubility products of different sparingly soluble silver salts,” Analytical Sciences, vol. 17, pp. 395–396, 2001.
View at: Google Scholar
A. N. Rodríguez, M. T. S. Nair, and P. K. Nair, “Structural, optical and electrical properties of chemically deposited silver sulfide thin films,” Semiconductor Science and Technology, vol. 20, no. 6, pp. 576–585, 2005.
View at: Publisher Site | Google Scholar
B. R. Sankapal, R. S. Mane, and C. D. Lokhande, “New chemical method for the preparation of Ag₂S thin films,” Materials Chemistry and Physics, vol. 63, no. 3, pp. 226–229, 2000.
View at: Publisher Site | Google Scholar
S. S. Dhumure and C. D. Lokhande, “Studies on the preparation and characterization of chemically deposited Ag₂S films from an acidic bath,” Thin Solid Films, vol. 240, no. 1-2, pp. 1–6, 1994.
View at: Google Scholar
D. N. Okoli, G. C. Okeke, and A. J. Ekpunobi, “Optical properties of chemical bath deposited Ag₂S thin films,” Pacific Journal of Science and Technology, vol. 11, no. 1, pp. 411–415, 2010.
View at: Google Scholar
T. B. Nasrallah, H. Dlala, M. Amlouk, S. Belgacem, and J. C. Bernède, “Some physical investigations on Ag₂S thin films prepared by sequential thermal evaporation,” Synthetic Metals, vol. 151, no. 3, pp. 225–230, 2005.
View at: Publisher Site | Google Scholar
J. A. Muñoz, C. Gómez, A. Ballester, M. L. Blázquez, F. González, and M. Figueroa, “Electrochemical behaviour of chalcopyrite in the presence of silver and Sulfolobus bacteria,” Journal of Applied Electrochemistry, vol. 28, no. 1, pp. 49–56, 1997.
View at: Google Scholar
M. C. Brelle and J. Z. Zhang, “Femtosecond study of photo-induced electron dynamics in AgI and core/shell structured Agl/Ag₂S and AgBr/Ag₂S colloidal nanoparticles,” Journal of Chemical Physics, vol. 108, no. 8, pp. 3119–3126, 1998.
View at: Google Scholar
A. P. Yadav and R. R. Pradhananga, “Preparation and characterization of silver sulphide/silver iodide ion selective electrodes for the determination of I^-, S^2- and Ag⁺ ions,” Journal of Nepal Chemical Society, vol. 15, no. 9, pp. 19–26, 1996.
View at: Google Scholar
Y. Umezawa, P. Bühlmann, K. Umezawa, K. Tohda, and S. Amemiya, “Potentiometric selectivity coefficients of ion-selective electrodes part I. Inorganic cations,” Pure and Applied Chemistry, vol. 72, no. 10, pp. 1851–2082, 2000.
View at: Google Scholar
R. R. Pradhananga and A. Rajbhandari, “Low cost electrochemical sensors for silver, chloride, bromide and iodide ions,” Scientific World, vol. 6, no. 6, pp. 33–36, 2008.
View at: Publisher Site | Google Scholar
T. X. Liu, X. Z. Li, and F. B. Li, “AgNO₃-induced photocatalytic degradation of odorous methyl mercaptan in gaseous phase: mechanism of chemisorption and photocatalytic reaction,” Environmental Science and Technology, vol. 42, no. 12, pp. 4540–4545, 2008.
View at: Publisher Site | Google Scholar
R. V. Kumar, O. Palchik, Y. Koltypin, Y. Diamant, and A. Gedanken, “Sonochemical synthesis and characterization of Ag₂S/PVA and CuS/PVA nanocomposite,” Ultrasonics Sonochemistry, vol. 9, no. 2, pp. 65–70, 2002.
View at: Publisher Site | Google Scholar
K. Akamatsu, S. Takei, M. Mizuhata et al., “Preparation and characterization of polymer thin films containing silver and silver sulfide nanoparticles,” Thin Solid Films, vol. 359, no. 1, pp. 55–60, 2000.
View at: Publisher Site | Google Scholar
J. Y. Wang, W. Chen, A. H. Liu et al., “Controlled fabrication of cross-linked nanoparticles/polymer composite thin films through the combined use of surface-initiated atom transfer radical polymerization and gas/solid reaction,” Journal of the American Chemical Society, vol. 124, no. 45, pp. 13358–13359, 2002.
View at: Publisher Site | Google Scholar
C. Maier and T. Calafut, Polypropylene: The Definitive User's Guide and Databook, William Andrew, 1998.
R. S. Mane and C. D. Lokhande, “Chemical deposition method for metal chalcogenide thin films,” Materials Chemistry and Physics, vol. 65, no. 1, pp. 1–31, 2000.
View at: Publisher Site | Google Scholar
I. A. Ezenwa, N. A. Okereke, and N. J. Egwunyenga, “Optical properties of chemical bath deposited Ag₂S thin films,” International Journal of Science and Technology, vol. 2, no. 3, pp. 101–106, 2012.
View at: Google Scholar
D. K. Božanić, V. Djoković, J. Blanuša, P. S. Nair, M. K. Georges, and T. Radhakrishnan, “Preparation and properties of nano-sized Ag and Ag₂S particles in biopolymer matrix,” European Physical Journal E, vol. 22, no. 1, pp. 51–59, 2007.
View at: Publisher Site | Google Scholar
U. M. Jadhav, S. R. Gosavi, S. N. Patel, and R. S. Patil, “Studies on characterization of nanocrystalline silver sulphide thin films deposited by chemical bath deposition (CBD) and successive ionic layer adsorption and reaction (SILAR) method,” Archives of Physics Research, vol. 2, no. 2, pp. 27–35, 2011.
View at: Google Scholar
Y. Gotoh, T. Kanno, Y. Fujimori et al., “Introduction of Ag and Ag₂S nanoparticles into nylon 6 film and fiber,” Polymer Journal, vol. 35, no. 12, pp. 960–964, 2003.
View at: Publisher Site | Google Scholar
W. Zhang, L. Zhang, Z. Hui, X. Zhang, and Y. Qian, “Synthesis of nanocrystalline Ag₂S in aqueous solution,” Solid State Ionics, vol. 130, no. 1, pp. 111–114, 2000.
View at: Publisher Site | Google Scholar
S. S. Dhumure and C. D. Lokhande, “Chemical deposition of Ag₂S films from acidic bath,” Materials Chemistry and Physics, vol. 28, no. 1, pp. 141–144, 1991.
View at: Google Scholar
X. F. Qian, J. Yin, J. C. Huang, Y. F. Yang, X. X. Guo, and Z. K. Zhu, “Preparation and characterization of PVA/Ag₂S nanocomposite,” Materials Chemistry and Physics, vol. 68, no. 1–3, pp. 95–97, 2001.
View at: Publisher Site | Google Scholar
A. Vogel, Text Book of Guantitative Chemical Analysis I, Longman Scietific & Technical, London, UK, 1989.
D. Briggs and M. P. Seach, Analiz poverkhnosti metodami ozhe i rentgenovskoj fotoelektronnoj spectroskopii, Mir, Moscow, Russia, 1987.
National Institute of Standards and Technology, “NIST online databases, X-ray photoelectron spectroscopy database,” 2012, http://srdata.nist.gov/xps/.
View at: Google Scholar
R. A. Lidin, L. L. Andrejeva, and V. A. Molochko, Reference Book on Inorganic Chemistry, Khimiya, Moscow, Russia, 1987.
C. D. Wagner, W. M. Riggs, L. E. Davis, and J. F. Moulder, Handbook of X-Ray Photoelectron Spectroscopy, Perkin-Elmer, Waltham, Mass, USA, 1978.
J. Vinkevičius, I. Možginskiene, and V. Jasulaitiene, “Investigations of the interaction between Cu_2-xS coating and Ag(I) ions using cyclic voltammetry and X-ray photoelectron spectroscopy,” Journal of Electroanalytical Chemistry, vol. 442, no. 1-2, pp. 73–82, 1998.
View at: Google Scholar
R. Chen, N. T. Nuhfer, L. Moussa, H. R. Morris, and P. M. Whitmore, “Silver sulfide nanoparticle assembly obtained by reacting an assembled silver nanoparticle template with hydrogen sulfide gas,” Nanotechnology, vol. 19, no. 45, Article ID 455604, 11 pages, 2008.
View at: Publisher Site | Google Scholar
V. Djoković, R. Krsmanović, D. K. Božanić et al., “Adsorption of sulfur onto a surface of silver nanoparticles stabilized with sago starch biopolymer,” Colloids and Surfaces B, vol. 73, no. 1, pp. 30–35, 2009.
View at: Publisher Site | Google Scholar
C. J. Powell, “Elemental binding energies for X-ray photoelectron spectroscopy,” Applied Surface Science, vol. 89, no. 2, pp. 141–149, 1995.
View at: Google Scholar
G. Hota, S. B. Idage, and K. C. Khilar, “Characterization of nano-sized CdS–Ag₂S core-shell nanoparticles using XPS technique,” Colloids and Surfaces A, vol. 293, no. 1-3, pp. 5–12, 2007.
View at: Publisher Site | Google Scholar
D. J. Asunskis and L. Hanley, “Valence band and core level X-ray photoelectron spectroscopy of lead sulfide nanoparticle-polymer composites,” Surface Science, vol. 601, no. 19, pp. 4648–4656, 2007.
View at: Publisher Site | Google Scholar
X. Lu, L. Li, W. Zhang, and C. Wang, “Preparation and characterization of Ag₂S nanoparticlesembedded in polymer fibre matrices by electrospinning,” Nanotechnology, vol. 16, no. 10, pp. 2233–2237, 2005.
View at: Publisher Site | Google Scholar
J. S. Hammond, S. W. Gaarenstroom, and N. Winograd, “X-ray photoelectron spectroscopic studies of cadmium- and silver-oxygen surfaces,” Analytical Chemistry, vol. 47, no. 13, pp. 2193–2199, 1975.
View at: Google Scholar
B. J. Murray, Q. Li, J. T. Newberg, E. J. Menke, J. C. Hemminger, and R. M. Penner, “Shape- and size-selective electrochemical synthesis of dispersed silver(l) oxide colloids,” Nano Letters, vol. 5, no. 11, pp. 2319–2324, 2005.
View at: Publisher Site | Google Scholar
M. Bielmann, P. Schwaller, P. Ruffieux, O. Gröning, L. Schlapbach, and P. Gröning, “AgO investigated by photoelectron spectroscopy: evidence for mixed valence,” Physical Review B, vol. 65, no. 23, Article ID 235431, 5 pages, 2002.
View at: Google Scholar
B. H. Stuart, Infrared Spectroscopy: Fundamentals and Aplications, John Wiley & Sons, New York, NY, USA, 2002.
E. . Pretsch, P. Bühlmann, and M. Badertscher, Structure Determination of Organic Compounds: Tables of Spectral Data, Springer, Berlin, Germany, 4th edition, 2009.
G. Nickless, Inorganic Sulphur Chemistry, Elsevier, Amsterdam, The Netherlands, 1968.
L. J. Belamy, Infrared Spectra of Inorganic and Coordination Compounds, John Wiley & Sons, New York, NY, USA, 1963.
R. A. Nyquist and R. O. Kagel, Infrared Spectra of Inorganic Compounds, Academic Press, New York, NY, USA, 1971.
K. Nakamoto, Infrared and Raman Spectra of Inorganic and Coordination Compounds, Part A, John Wiley & Sons, New York, NY, USA, 5th edition, 1997.
J. C. Lindon, G. E. Tranter, and J. L. Holmes, Encyclopedia of Spectroscopy and Spectrometry, Academic Press, New York, NY, USA, 2000.
A. Rajbhandari, A. P. Yadav, K. Manandhar, and R. R. Pradhananga, “Characterization and applications of silver sulphide based membrane electrodes,” Scientific World, vol. 7, no. 7, pp. 19–23, 2009.
View at: Publisher Site | Google Scholar
S. S. M. Hassan and E. Elnemma, “Selective determination of thiamine (vitamin B1) in pharmaceutical preparations by direct potentiometric argentometric titration with use of the silver-silver sulphide ion-selective electrode,” Talanta, vol. 36, no. 10, pp. 1011–1015, 1989.
View at: Google Scholar

Copyright

Copyright © 2013 Valentina Krylova and Nijolė Dukštienė. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

PDF Download Citation

Download other formats

Order printed copies

Views

6375

Downloads

5591

Citations

Journal of Chemistry

Synthesis and Characterization of Ag2S Layers Formed on Polypropylene

Abstract

1. Introduction

2. Experimental

3. Results and Discussion

3.1. Ag2S Layers Formation Mechanism on a PP Film in Chemical Bath Deposition Process

3.2. Chemical Analysis of Ag2S Layers

3.3. Morphology of Ag2S Layers

3.4. XPS Analysis of Thin Ag2S Layers

3.5. ATR-FTIR Analysis of Ag2S Layers

3.6. XRD Analysis of Thin Ag2S Film Layers

3.7. Application of Ag2S/PP Layers for Potentiometric Measurements

4. Conclusions

References

Copyright

Synthesis and Characterization of Ag₂S Layers Formed on Polypropylene

3.1. Ag₂S Layers Formation Mechanism on a PP Film in Chemical Bath Deposition Process

3.2. Chemical Analysis of Ag₂S Layers

3.3. Morphology of Ag₂S Layers

3.4. XPS Analysis of Thin Ag₂S Layers

3.5. ATR-FTIR Analysis of Ag₂S Layers

3.6. XRD Analysis of Thin Ag₂S Film Layers

3.7. Application of Ag₂S/PP Layers for Potentiometric Measurements