Removal of Metals by Sorption with Metal Concentration Colour Sensitive Azotized Polyethylene Terephthalate Adsorbent

doi:10.21203/rs.3.rs-2064128/v1

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Removal of Metals by Sorption with Metal Concentration Colour Sensitive Azotized Polyethylene Terephthalate Adsorbent

https://doi.org/10.21203/rs.3.rs-2064128/v1

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This paper reports on the preparation and modification of azotized polyethylene terephthalate (PET) as a stable and colour sensitive absorbent for metals in aqueous media and its application in the removal of heavy metal ions from water. This study successfully functionalized PET to produce an azotized material which was confirmed by FTIR (Fourier transform infrared) analysis and its metal adsorption property confirmed by FAAS (flame atomic absorption spectroscopic) analysis. The modified material exhibited colour variations upon interaction with metal ions. The material was capable of indicating when exhausted, and was then applied for the removal of the metals from water. Sorption parameters were investigated and optimized at fixed temperature (25°C). The optimum pH for the adsorption of copper, lead and chromium was 6.0 except that of cadmium was that was adsorbed at a pH value of 5.5. The uptake of the metals studied was found to be very fast as about 90% was adsorbed within the first 10 min of contact time. The adsorption of lead and cadmium prescribed to first order kinetics thus monolayer adsorption implying a chemisorption process while the adsorption of copper and chromium was of second order kinetics of multilayer adsorption. This could also be due to copper and chromium being smaller species hence being more interactive than lead and cadmium. The adsorption capacities of copper, lead, cadmium and chromium were found to be 46.47, 33.65, 70.93 and 59.06 mg g^− 1 respectively. The metal ions attached on the adsorbent were easily stripped of by the use of 1.0 M nitric acid, hence easily regeneratable. The results obtained confirmed that azotized PET has potential application as a colour sensitive sorbent for the removal of heavy metal pollutants from water.

Heavy metal pollutions

azotized Polyethylene terephthalate

pollution

Sorption

Despite the fact that water covers 71% of the surface of the earth, there exist a serious challenge in the availability of drinking water due to harmful dissolved species in the water [1]. Such stably dispersed species make it a serious concern on the health and wellbeing of man as a consumer of that vital commodity [2, 3]. Even when the levels of the dissolved species are at trace levels and regarded to be acceptable, there is danger in the consumption of such water due to bioaccumulation of metals that can eventually be incorporated in both hard and soft body tissues [2–4]. Such dissolved metal ions typically exist as positively-charged species and can bind to negatively charged organic moieties. In such a process, if the organic moiety are in the body fluid system, they act as Lewis base by donating electrons to the metal atom that becomes a Lewis acid or electron pair acceptor. Such a reaction ends up in the denaturation of the proteins and hence disruption of their activities ending to the eventual death of cells [5]. Such binding mechanism is usually by the formation of complexes which are difficult to retrieve safely from the bound metal.

To mitigate the metal denaturation poisoning process, the scarce insufficient clean and safe water has to be provided for human consumption. The best remedial method is to remove the metals from the water before consumption, to ensure its safety. This can be achieved by using the very same method of binding the metals from the water, using a similar mechanism that causes poisoning effect before the water is consumed, so that it can be presented safe for consumption.

Adsorption is a cost-effective methods capable of removing heavy metal ions in trace levels ranging from 1 mgL^− 1 to 20 mgL^− 1 in waste have been reported [6]. This has been achieved by the use of sorbents from biological origin in packed columns [7]. The bio sorption metal removal process has been found to be very effective as the exhausted biomaterial could be regenerated for re-use. The metals complexed with the sorbent functional groups of the biomaterial can easily be stripped using a dilute acid [8]. This excellent remedial method has its challenges in that the binding happens in certain specific stoichiometric ratios that cannot be quantified when using environmental samples [8]. Thus, it is difficult to determine when the biosorbent has been exhausted unless with the use of suitable instruments such as a conductivity meter or calorimeters. Such instruments can monitor the varying concentration of species being eluted. This renders the removal method out of reach to a vast majority of the needy cases due to the limiting facilities and resources. To address this challenge, the development of safe and affordable metal concentration colour sensitive material capable of removing heavy metals from water and render it safe for domestic consumption was considered. This study explored the use of aromatic compounds with azo (-N = N-) chromophores to treat the polluted water by removal of contaminants. This was achieved by using the property of a metal concentration colour sensitive self-indicating adsorbent material. The modified material is water insoluble, but capable of interacting with metals ions in water and holding them on its surface, thus removing them from water thus rendering the water safe for human consumption [9]. The mechanism is similar to stationery phase separation process as in chromatography. This enables a complete removal of dissolved metal ions from water by stripping them off from the liquid dispersing media.

We report the performance of azotized polyethylene terephthalate (PET) on adsorption of copper, lead, cadmium and chromium in aqueous solution. Azo compounds represent a class of coloured compounds used in textile-processing and other industries because of their colour. These compounds possess sites capable of forming metal-complexes by coordination to develop dye-metal complexes also called premetallized dyes despite being waster insoluble [10]. Such dyes could interact with metals in ratios of either 1:1 metal complexes or 1:2 metal complexes, to form metalized azo pigments that exhibit certain colours specific to the ratio [10]. The azo pigments in this study are similar in chemical structure to azo dyes, but they lack solubilizing groups. Below shows a presentation of a PET metalized azo pigment.

Scheme 1 Metalized azo pigment

The chromophores used in pigments are usually the same as those used in dyes, but the pigments are large molecules and do not have water solubilizing groups [11]. They contain groups that form intermolecular bonds that help to reduce water solubility. Such azo compounds are insoluble even in acidic conditions and therefore suitable for use in water treatment process [12]. Despite such azo being insoluble in water they have an affinity for hydrophobic metal ions (metallization) to produce a coloration specific to the metal. Metallization imparts a hypso or bathochromic shift to the colour of the material indicating the bonding of ligand to the metal ions through both azo nitrogen atoms [13]. Metal-complex dyes form strong coordination complexes and are an integral part of the chromophore [14]. Variation of the metal-azo ratio contribute to a variation of the colour. This is as reported by Chakraborty (2013) when he observed that the spectra of 1:1 metal-complex azo dyes displayed narrower curves, while that of 1:2 complex dyes show a broader curve exhibiting blueness and dullness [14]. That colour variation was exploited in this study to determine the exhaustion of the metallized azo material.

Although metal complexes do not have the same ligands, they are all anchored on the coordinating sites in a similar way irrespective of the electron donating group and its coordinating capacity [15]. Therefore, interaction of acids with metal complexes that include metallized azo material will result in protonation of the ligand and subsequent release of the metal similar to the corrosion process. This study exploited that property to regenerate the metal bound azo based adsorbent material for re-use by protonation of the metal pigment complex. This work presents the preparation and subsequent application of modified PET material for use in the remediation of metal laden water.

The polyethylene telephthalate material is a water insoluble chemically stable polymeric transparent solid material of high density (1.38 g cm^− 3) and a melting point of 260°C (500°F). This justifies its extensive use for shipping bulk food and packing of retail food products as well as a bottling material for water and soft drinks [16]. Structurally, PET contains no functional groups (sites) for metal ion sorption. For it to be applied as a metal adsorbent, a modification is required to create active sites for metal interaction. The modification process involves the attachment of an azo group that is able to chelate with metals and its colour will be influenced by the metal ion complexion. This is similar to metal complexometric indicators (pM) that undergoes a definite colour change upon interaction with some specific metal ions due to formation of weak complex with the ions present in the solution. This contributes to a significantly different colour change from the form existing outside the complex.

The PET material used in this study was from disposed bottles collected from dump sites in Nairobi. Environmental water samples were obtained from five different points in triplicates from Kipsonoi River in Sotik Sub-county of Bomet County.

The study aimed in exploiting the waste non-biodegradable synthetic material to offer a solution of remediation of water for domestic consumption. The waste PTE was used as a raw material to offer a solution to metal laden waters as well as put to good use the discarded waste that litters and affects negatively the aesthetic beauty of the environment. This study exploited the variation of colour of the modified material upon interaction metal ions. That colour variation confirms the presence of adsorbed metals or the absence of the metals upon regeneration when the material reverts to its original colour upon stripping the metal ions from the adsorbent.

2.1 Chemicals and reagents

All the solutions were prepared in double distilled de-ionized water and all the reagents were of analytical grade. Copper (II) sulphate, lead (II) nitrate, cadmium nitrate, potassium dichromate, sulphuric acid, sodium nitrite, hydrochloric acid, granulated tin, nitric acid, sodium hydroxide, sodium acetate, acetic acid and hydrochloric acid were obtained from Sigma-Aldrich through its outlet Kobian (K) in Nairobi. Metal standard stock solutions (1000 mg/L) were prepared in 0.1M sodium acetate solution.

2.2 Instrumentation

The metal ions content in solution was determined by flame atomic absorption spectrophotometer (FAAS), Shimadzu AA-62000 model, while the characterization of the raw and modified sorbent material was done using Fourier transform infrared spectrometer (Bruker Tensor 27- HTS-XT MIR model). The pH of the solutions in this study was adjusted using a 3505-JENWAY (UK) pH meter. The mechanical reciprocating shaker used for the agitation of the experimental sample mixtures was a DKZ-1 NO. 1007827 model.

2.3 Procedures

2.3a Azotization of polyethylene terephthalate

The waste non-biodegradable synthetic PET bottles were cleaned, dried, uncapped and their labels removed before being crushed to small flakes. The resultant PET flakes was then modified using the method proposed by Sliman and co-workers as the functionalized PET knitted fabrics [17]. This was achieved by transferring each time a mass of 5.00 g (PET flakes) into a 250 mL round bottomed flask containing 40 mL of concentrated nitric acid and 60 mL of concentrated sulphuric acid. The mixture was maintained at a temperature below 60 ^oC, for 1 hour [18]. The resultant mixture containing the nitrated product was transferred into a 1.0 liter beaker half filled with ice water. The mixture was then filtered and the residue washed with double distilled water until the solution obtained as the filtrate attained a pH of 4–5. The nitrated product was reduced by mixing it with concentrated hydrochloric acid-ethanol mixture (45:50, v/v) and 50.00g of tin granules and refluxed at 90 ^ºC for 24 hours. The product formed was then cooled to ambient temperature, filtered and washed with acid-ethanol mixture (45:50, v/v) followed by 2.0 M sodium hydroxide and then distilled water [19]. The amino product formed was diazotized by cooling it in an ice bath (0–3 ^ºC) and 75 mL of 1.0 M sodium nitrite added, followed by 100 mL of hydrochloric acid. The mixture was stirred and tested with iodide paper until the paper changed colour from white to violet due to formation of diazotized product. The product was then washed with ice-cold water, dried, then analyzed using FTIR and then applied for metal sorption [19].

The plausible mechanism for the modification process is given in Scheme 1.

Scheme 2: Azotization of the polyethylene terephthalate material

The reaction scheme 1 shows the products obtained in each respective step of the modification process.

2.3b Optimization of sorption parameters

Batches of 20.00 ml model solutions (20 ppm) were dispensed into 100 ml polyethylene bottles containing approximately 0.03g of the azotized PET material. The initial pH of the model solutions was adjusted to the appropriate pH value for each metal ion under study. The mixture was allowed to equilibrate and then removed from the shaker at different time intervals between 5-100 minutes. The resultant mixture was then filtered off by suction and the concentration of metal ions in the filtrate determined by FAAS.

The effects of various parameters such as pH, contact time, initial metal ion concentration and sorbent dose on metal ion removal from water were investigated at room temperature by varying the parameter under investigation while maintaining the others constant. All the experiments were carried out in triplicates. The pH of the medium was adjusted by using either sodium acetate solution or 0.1 M nitric acid dropwise. The content of the metal ions adsorbed were calculated using equations 1 and 2 for the adsorption capacity and removal efficiency respectively [20].

$${q_e}=\frac{{({C_o} - {C_e})V}}{m}$$

$$\% ~R=\frac{{({C_o} - {C_e})}}{{{C_o}}}x100$$

Where

m = mass of adsorbent (g)

q_e = Equilibrium adsorption capacity (mg/g)

C _o =Initial concentration (mg/L)

C _e = Concentration at unit time (mg/L)

% R = Percentage removal

V = Volume of solution (L)

2.3c Effect of pH on complexation modified and unmodified PET

The optimum pH value for the uptake of each heavy metal ion was determined by placing 0.03 g of azotized PET into 100 mL polythene bottles and adding 20 mL of solutions containing 20 mg/L of each analyte ion prepared in 0.1 M sodium acetate/acetic acid. The pH was adjusted to different values (2–7) using 0.1 M of nitric acid or 0.1M sodium hydroxide. The mixture was then equilibrated for 2 hours in a mechanical shaker at 180 rpm, filtered and the concentrations of the metal ions in the filtrate determined using flame atomic absorption spectroscopy (FAAS) [21, 22].

2.3d Effect of contact time on complexation

A sample containing 0.03 g of azotized PET was placed into 100 mL polyethylene bottles. Aliquots of 20 mL solutions of 20 mgL^− 1 concentrations initially adjusted to the optimum pH value for each metal ion under study was added into each of the bottles. The contents of the bottles were agitated on a mechanical reciprocating shaker at 180 rpm. Samples were removed at different time intervals and filtered by suction. The residual metal ion concentration in the filtrate was then determined by FAAS [22].

2.3e Effect of the initial metal ion concentration on complexation

The effect of concentration of the metal ion on the uptake by azotized PET was determined by placing 0.03 g of the adsorbent into a series of polyethylene bottles containing 20 mL of metal ions under study at different concentrations (10-100mg/L) buffered at optimum pH for each metal. The contents of the bottles were equilibrated on the mechanical shaker at 180 rpm for 50 minutes. After filtration, the residual concentration of the metal ions in the filtrate was determined by FAAS [21, 22].

2.3f Effect of adsorbent dose on removal of heavy metal ions

To determine the effect of the amount of azotized PET on the metal ions uptake, 20 mL of the model solutions containing 20 mgL^− 1 of metal ions buffered to optimum pH value for each metal ion were added to varying amounts (0.01–0.50 g) of the adsorbent in polyethylene bottles. They were then agitated in a mechanical shaker at 180 rpm for 50 minutes and then filtered. The concentration of metal ions in the filtrate were then determined using FAAS [21].

2.4 Adsorption kinetics

The uptake rate of metal ions and the mechanisms of binding by the adsorbents were evaluated by investigating their sorption kinetics. The kinetic models used in this study were the Lagergren’s Pseudo-first-order (Eq. 3) and the Ho’s pseudo-second-order (Eq. 4) [23, 24]. These models revealed the rate controlling steps and sorption mechanism.

$$l{\text{n}}\left( {{q_e} - {q_t}} \right)=\ln {q_{e~~}} - {k_1}t$$

${q_e}=\frac{1}{{{k_2}q_{e}^{2}}}+\frac{1}{{{q_o}}}t$ (4)

Where q_e and q_t (mg g^− 1) represents the amount of metal ions adsorbed on the adsorbent at equilibrium and time, t, respectively; k₁ (min^− 1) and k₂ (g mg^− 1min^− 1) are the adsorption rate constants of the pseudo-first-order and pseudo-second-order kinetics respectively. The approximate values of k₁ and k₂ can be obtained from the plots of ln(q_e-q_t) versus t and t/q_t versus t respectively.

The experimental results were fitted into adsorption models in order to determine the kinetics and mechanisms of adsorption.

2.5 Adsorption isotherms

Adsorption isotherms describe how the adsorbate interacts with adsorbents. The model isotherms applied in this study were Langmuir and Freundlich adsorption isotherms [25, 26]. They were applied to evaluate factors such as adsorption capacity and mechanism of adsorption. Adsorption equilibrium is attained when the capacity of the complexing agent is achieved and the rate of uptake of metal ions corresponds with the rate of desorption. The maximum adsorption capacity of an adsorbent was then determined using the Langmuir and Freundlich isotherms.

The Langmuir isotherm is based on the fact that all the binding sites of an adsorbent are identical and of equal energies. This model assumes that the adsorption process takes place at specific homogeneous sites on the adsorbent. This applies to the monolayer adsorption process [27]. The linear form Langmuir model is given by Eq. 5.

$$\frac{{{C_e}}}{{{q_e}}}=\frac{1}{{{k_{1~}}{q_m}}}+\frac{1}{{{q_m}~}}{C_e}$$

Where Ce (mg L^− 1) is the metal ion concentration at equilibrium, q_e (mg) is the adsorption capacity, q_𝑚 (mg g⁻¹) is the maximum adsorbate amount that forms a complete monolayer on the surface, and k_l (L mg⁻¹) is the Langmuir constant related to the rate of adsorption. The higher the value of k_l the much stronger the affinity of metal ion uptake. The values of q_m and k_l can be approximated from a plot of C_e/q_e versus C_e and determining its slope and intercept.

Freundlich isotherm is based on the equilibrium relationship between heterogeneous surfaces. This model assumes that the adsorption sites are distributed exponentially with respect to the heat of adsorption. Eq. 6 represents the linear form of Freundlich isotherm.

$$\ln {q_e}=\ln {k_F}+\frac{1}{n}\ln {C_e}$$

Where c_e, q_e have the same meaning as in Eq. 5; ${k_F}$ is the adsorption capacity while $\frac{{\text{1}}}{{\text{n}}}$denotes the energetic heterogeneity of adsorption sites. When a graph of lnq_e versus lnc_e is plotted, the values of ${k_F}$ and $\frac{{\text{1}}}{{\text{n}}}$ can be estimated. The values of n should be within the range 1–10 under normal adsorption conditions.

The data obtained in the effect of initial metal ion concentration was treated with the Freundlich and Langmuir adsorption models to determine the sorption mechanism and the best adsorption model for the uptake of each of the respective heavy metal ion dispersed in the solution.

2.6 Desorption studies

Desorption studies were carried out using separate transparent polyethylene columns of capacity 10 ml which had had a frit was inserted before packing the adsorbent material. In each of the columns, 0. 3 g of modified PET was packed and a frit was inserted after parking the adsorbent. The packed (tubes) columns were washed successively with water, preconditioned and buffered to the desired pH before use. After the conditioning, 10 mL of the different sample solutions containing 10 mgL^− 1 of copper, lead, cadmium and chromium ions were separately loaded in each respective column and each respective eluent collected. The retained metal ions were stripped using 5 mL of 1.0 M nitric acid. The concentrations of each of the desorbed metal ions were then determined using FAAS. The demetalization of the metalized azo material can be regarded as acid treatment of the azo-metal complex as presented below.

$ML+{H^+} \to HL+{M^+}$

The reusability of the azotized PET was determined by repeating the adsorption-desorption cycles five times under the same experimental conditions [22, 26].

2.7 Analysis of environmental water samples

Samples of water from River Kipsonoi (Bomet County, Kenya) were collected using 1 L polyethylene bottles. They were filtered and the concentration of copper, lead, cadmium and chromium ions determined. Portions (50 mL) of water were separately spiked with known concentrations of copper, lead, cadmium and chromium ions. Each of the resulting solution was then added to a 0.03 g of azotized PET adsorbent in a 100 mL polyethylene bottle and agitated for 50 minutes on a mechanical reciprocating shaker at 180 rpm. The retained metal ions were then stripped with 10.0 mL of 1.0 M nitric acid and their concentrations determined by FAAS [21].

3.1 Characterization of the adsorbent material

Characterization of the parent PET and its chemically modified forms were done using FTIR. The results are discussed in the following sub-sections.

3.1a Parent PET

The FTIR spectrum of the parent PET is given by Fig. 1.

Figure 1: FTIR sperctrum of the parent PET

The spectrum (Fig. 1) shows a peak at 3642.9 cm^− 1 which may be attributed to the terminal O-H stretching [22, 29]. A peak which appeared at 3085.6 cm^− 1 may be due to aromatic C-H stretching [4, 27, 31, 32]. The peak observed at 2973.7 cm^− 1 could be as a result of the aliphatic methylene asymmetric C-H stretching while the one appearing at 2910.1 cm^− 1 could be assigned to methylene symmetric C-H stretching [22, 27, 31–33].. The sharp peak at 1745.3 cm^− 1 corresponds to C = O stretching while the peak at 1616.1 cm^− 1 may be assigned to aromatic C = C stretching [22, 29, 31–33]. The methylene C-H bending bands were observed at the frequencies of 1459.9 cm^− 1 (scissoring), 1346.1 cm^− 1 (wagging), 1299.8 cm^− 1 (twisting) and 732.8 cm^− 1 (rocking) [31, 33]. The aromatic in-plane C-H and out-of-plane bending peaks occurred at 1216.9 cm^− 1 and 680.8 cm^− 1 respectively [331]. The peak at 1137.8 cm^− 1 could be as a result of C-O stretching [33]. The parent material was then chemically modified by anchoring the required functional groups within its structure.

3.1b Nitrated PET

Below shows the spectrum of the nitrated PET.

Figure 2: FTIR sperctrum of the nitrated PET

The FTIR results as in Fig. 2, show a band at 3102.9 cm^− 1 which could be due to aromatic C-H stretching [4, 27, 29]. Aliphatic C-H stretching band appeared at 2971.8 cm^− 1 [22, 33–35]. The band at 1756 cm^− 1 could be due to aromatic C = O stretching, while the one observed at 1556.3 cm^− 1 could be due to aromatic C = C stretching [22, 27–29]. The peaks appearing at 1162.9 cm^− 1 and 1114.7 cm^− 1 may be attributed to aromatic in-plane C-H bending bands, while those observed at 885.2 cm^− 1, 769.5 cm^− 1, 725.1 cm^− 1 and 702.0 cm^− 1 may be assigned to aromatic out-of- plane C-H bending bands [31, 33].

The additional peaks observed at the frequencies 1554.4 cm^− 1 and 1359.6 cm^− 1 may be due to aromatic nitro, NO_{2 ,} asymmetric and symmetric stretching frequncies respectively [21, 31, 38]. This indicates a successful nitration of the aromatic ring of PET.

The nitro functional group in the nitrated material was then chemically reduced to produce an amino functional group within the structure.

3.1c Aminated PET

Below shows the spectrum of the aminated PET

Figure 3: FTIR spectrum of the aminated PET

The results (Fig. 3) shows the appearance of two sharp peaks at the frequencies 3484.8cm^− 1 and 3363.3 cm^− 1. These correspond to signals of N-H stretching [31, 38]. A peak observed at 2989.2 cm^− 1 may be assigned to aromatic C-H stretching [4, 28, 32]. Aromatic C = O stretching occurred at 1729.9 cm^− 1 while C = C stretching appeared at 1450.2 cm^− 1 [22, 29–38]. The bands at 1137.8 cm^− 1 may be due to aromatic in-plane C-H bending while those at 900.6 cm^− 1 and 767 cm^− 1 could have been as a result of aromatic out-of-plane C-H bending [26, 31, 39].

The signal observed at 1554.5 cm^− 1 for the nitrated PET (Fig. 2) disappeared and a new one appeared at 1598.0 cm^− 1. This may be attributed to signals of N-H vibrations [29, 34]. These observations can be ascribed to the successful reduction of the nitro group to amino group in the aromatic ring of PET. The amino group was then azotized to produce an adsorbent whose colour was sensitive to metal ion concentrations.

3.1d Azotized PET

Below shows the spectrum of the azotized PET

Figure 4: FTIR sperctrum of the azotized PET

The results presented in Fig. 4 indicate that the signal which was at a 3300 cm^− 1 and a shoulder at 3400 cm^− 1 corresponding to 1^o amine (-NH₂) stretching observed in aminated PET (Fig. 3) disappeared. This may be attributed to the diazotization of aminated PET. The bands corresponding to aromatic C-H stretching was observed at 3035.4 cm^− 1 [4, 29–32]. Aromatic C = O stretching band occurred at 1733.7 cm^− 1 [22, 29–33]. Aromatic in-plane C-H bending bands appeared at 1143.6 cm^− 1 and 1031.7 cm^− 1, while aromatic out-of-plane bending band was noted at 771.4 cm^− 1 [22]. The C = C stretching band occurred at 1569.8 cm^− 1 [22, 29–33]. The peak corresponding to an azo (-N = N-) stretching was observed at 1532.9 cm^− 1 [31, 35]. Signals with frequencies between 1500–1600 cm^− 1 are evidence of the azo group [36]. This signifies a successful azotization of the aminated PET. Below shows the combined results of FTIR analysis

Figure 5: FTIR sperctrum of the parent and modified forms of PET

Figure 5 is presents results obtained from the FTIR analysis. The results analysis show that the findings was in agreement with the expected products in each step of the modification process as presented in the reaction scheme [31, 35]. The final product was then applied for optimization of metal ions sorption parameters from water.

3.2 Optimization experiments

Optimization experiments were done in order to determine the most suitable conditions which favour the maximum removal of the heavy metal ions from aqueous solution. The results are highlighted in the following sub-sections.

3.2a Effect of pH

The metal binding efficiency of nitrogen-containing ligand is greatly influenced by the pH. This is due to the fact that pH affects the charge on the surface of the electron donating group (nitrogen), the degree of ionization, the speciation of metal ions and the level of precipitation [36, 37].

The binding of metals by a chelating polymer is based on the Lewis acid-base theory. Nitrogen atom on the coordinating group acts as a Lewis base by donating electrons to metal cations which act as Lewis acids [38]. For the adsorption process to occur, the binding sites in the adsorbent dissociates according to Eq. 7.

$${\text{H}\text{L}}_{\left(aq\right)}\rightleftharpoons { H}_{\left(aq\right)}^{+} + { L}_{\left(aq\right)}^{-}$$

Where HL is the adsorbent which on dissociation yields a proton, H⁺ and conjugate base of the acid, L⁻. This implies that the pH of a solution has a significant effect on the dissociation of the adsorbent functional groups and hence the uptake of metal ions. The dissociation of azotized PET may thus be given by the equation.

$${PET}-N={N}^{+}+{H}_{2}O\rightleftharpoons PET-N={N-OH+H}^{+}$$

Figure 6 shows effect of pH on sorption of metal ions by azotized PET.

Figure 6: Effect of pH on sorption of metal ions by azotized PET

The results show that at low pH values, the uptake of metal ions was low. This may be attributed to the high concentration and mobility of H⁺ ions which favours the adsorption of H⁺ ions over the metal ions. [38]. This leads to the competition between the metal ions and the H⁺ ions resulting in the protonation of the chelating polymer which enhances the electrostatic repulsion of metal ions in solution [38]. The adsorption of heavy metal ions increased with the increase in pH and reached optimal values of 6.0 for copper lead and chromium while 5.5 for cadmium. Increase in the pH causes the deprotonation of the binding sites and make the surface functional groups of the complexing agents to be negatively charged. This consequently leads to in an increase in the uptake of metal ions due to electrostatic forces of attraction [21, 35–37]. It also reduces the competition between H⁺ ions and adsorbate cations for the binding sites on the adsorbent [21]. Beyond that optimal pH region, precipitation of the metal ions results [21, 36–38].

3.2b Effect of contact time on metal uptake

The rate of metal ion uptake by the azotized adsorbent was investigated when the mixture was buffered at their respective optimum pH values obtained experimentally. This was intended to monitor the efficiency of the sorbent binding sites to hold the metal, as well as the activity of the metal, thus controlling the residence time of sorbate at the solid-solution interface [39, 40]. The contact time required for adsorption to be completed is critical in designing the adsorption process since it gives the minimum time needed for the uptake of metal ions. [36]. The results obtained were presented in Fig. 7.

Figure 7 Effect of contact time on the adsorption of metal ions

The results show that the general rate of metal uptake up take was very high as 90% within the first 10 minutes of interaction. That rapid uptake may be attributed to the availability of numerous binding sites in the surface of the azotized PET adsorbent [38, 39]. This implies that a contact time of 10 minutes is sufficient to achieve maximum adsorption. However, in this study, sorption experiments were carried out at an equilibration time of 40 minutes. The decline in the rate of the uptake of metal ions after the equilibrium time for each metal cation could be as a result of the saturation of the coordination sites of the adsorbents [41].

3.2c Effect of the initial metal ion concentration on the uptake of metal ions

The adsorption capacity of azotized PET was determined by adding 10 mL model solutions of concentrations ranging between 2 mg L^− 1 and 100 mg L^− 1 and buffered to the optimum pH for each metal ion to 0.03 g of the adsorbent in polystyrene screw-cap bottles. The mixtures were then agitated on a mechanical shaker for 40 minutes, then filtered and the resulting filtrate analyzed for the metal ion concentration, using FAAS. The amount of metal ion adsorbed (q_e) was plotted against the initial metal ion concentration (C_o) and the results obtained are presented in Fig. 8.

Figure 8: Effect of initial metal ion concentration on the sorption of metal ions

The results show that the metal ions uptake increased almost linearly with the increase in the concentration of the metal ions up to 80, 60, 70 and 80 mg/L for copper, lead cadmium and chromium ions respectively, then levels off. This observation could be due to the exhaustion of available binding sites [36, 37]. Further increase in the concentration beyond the equilibrium concentration, leads to slower uptake of metal ions since the available active sites in the adsorbent have become saturated [42–47]. The uptake capacities were found to be: copper (48.49 mg/g), lead (33.65 mg/g), cadmium (70.93 mg/g) and chromium (59.06 mg/g).

It was also observed that as the metal ion concentration was increased, the colour of the azotized PET changed from yellow to orange. This can be attributed to the bathochromic shift to a long-wavelength absorption band as a result of the metal azo dye complexation [39]. These colour changes show that nitrogen in the azo (-N = N) group is responsible for the adsorption of metal ions by complexation. This is in agreement with studies reported earlier [35,47–49].

3.3 Sorption Kinetics

The kinetic data obtained was analyzed using Lagergren [23, 24] first-order and Ho’s second-order kinetics. This was to investigate the molecularity of the sorption mechanism and the rate controlling steps [23, 24]. The results obtained are as presented in the Fig. 9 below.

Figure 9: Kinetic data on the sorption of metal ions

The pseudo-first- and pseudo-second-order kinetic models for the binding of the considered heavy metal ions onto azotized PET are presented in Figs. 9–11, while the values of the parameters are given in Table 1. The results indicate that pseudo-second-order best describe the kinetics of binding of all the metal ions studied onto the complexing agent since the R² are closer to one. This is similar to the results obtained in several studies [37]. The pseudo-second-order rate constant (k₂) followed a decreasing sequence of Cu (0.1616) > Pb (0.1457) > Cr (-0.1960) > Cd (0.00108) in mg min^− 1. This suggests that the chemical interaction is dependent on the affinity of metal ions to interact with the azo group (- N = N) of azotized PET.

Table 1

Sorption kinetics for the uptake of selected heavy metals by azotized PET
Metal ion	Pseudo-First-Order			Pseudo-Second-Order
Metal ion	q_e(mg/g)	k₁(min^− 1)	R²	q_e(mg/g)	k₂(g/mg min^− 1)	R²	Best model
Cu²⁺	0.9936	0.0331	0.3257	24.75	0.1616	0.9998	2nd order
Pb²⁺	1.0543	0.0055	0.4492	25.45	0.1457	1.0000	2nd order
Cd²⁺	2.8766	0.0143	0.0331	32.05	1.081 x 10^− 3	0.8354	2nd order
Cr⁶⁺	0.0102	-0.0491	0.1544	20.45	-0.1960	0.9998	2nd order

A summary of the calculated factors from kinetic data for each metal uptake at their respective optimum parameters is as presented in a tabular form as shown in Table 1. From that information, the sorption kinetics prescribed by each respective metal is obtained based on their respective linear correlation coefficient, R², values.

Table 1: Sorption kinetics for the uptake of selected heavy metals by azotized PET

The results show that the sorption for all the metal was of pseudo second order of multisite. This could be as a result of the metals being multivalent and the adsorbent having more than one active site [40].

3.4 Effect of adsorbent on the uptake of heavy metal ions

The type of the complexing agent and the functional groups it contains has intense effect on the binding of metal ions. The effect of adsorbent dose on the adsorption of metal ions was investigated at room temperature by varying the quantity of the adsorbents from 0.015 g to 0.5 g. Model solutions containing 40 mg L^− 1 of metal ions buffered at optimum pH value were added to the adsorbents and agitated in the mechanical shaker for 40 minutes. The mixture was then filtered and the concentration of the metal ions in the filtrate determined by FAAS [36]. The effect of the amount of the adsorbent on the % adsorption of metal ions is given by Fig. 10 below.

Figure 10: Effect of sorbent dose on the sorption of metal ions

The results show that an increase in the amount of azotized PET resulted in an increase metal removal observed to be copper from 86.58–98.10%, lead from 82.17–95.44%, cadmium from 81.22–95.77% and chromium ions from 68.71–89.57%. The amount of the adsorbent required for the maximum uptake of copper, lead, cadmium and chromium were found to be 0.15 g, 0.4 g, 0.25 g and 0.4 g respectively. This could be as a result of an increase in the number of binding sites for metal sorption of the porous material[36, 37, 45–46]. An excessive increase in the amount of the adsorbent did not result in any significant changes in the % uptake of metal ions. This is probably because of the establishment of an equilibrium between the metal ions bounded to the azotized PET and those remaining in the aqueous solution [37].

The experimental data obtained for the adsorbed metal against equilibrium concentration, was analysed using Langmuir and Freundlich equations.

3.5 Adsorption isotherms

The results from the optimization experiments were subjected to Langmuir and Freundlich isotherms. The results obtained are as presented in Fig. 11.

Figure 11: Adsorption isotherms for some selected metal by azotized PET

A summary of the calculated factors from linearized Langmuir and Freundlich adsorption models for each metal uptake at their respective optimum parameters is as presented in tabular form as shown in Table 2. From that information, the model prescribed by each respective metal is obtained.

Table 2

Langmuir and Freundlich isotherm parameters for the binding of metal ions
	Langmuir			Freundlich
Metal ion	Q_max (mg/g)	k_l (L/mg)	R²	1/n	k_F (mg/g)	R²	Best model
Cu²⁺	149.25	0.0633	0.9088	0.6724	10.04	0.9110	Freundlich
Pb²⁺	172.41	1.0000	0.9470	0.3445	34.12	0.9217	Langmuir
Cd²⁺	175.44	0.0490	0.9837	0.6437	10.48	0.9786	Langmuir
Cr⁶⁺	476.19	0.0004	0.4349	0.8951	2.472	0.9859	Freundlich

The best model for the complexation of each metal ion considered is the one whose linear correlation coefficient, R², value is closest to one. Table 2 represents the parameters of the adsorption isotherms.

Table 2: Langmuir and Freundlich isotherm parameters for the binding of metal ions

The complexation of lead and cadmium ions are best described by the Langmuir isotherm model with R² values > 0.94. This indicates that azotized PET provided the homogenous surface for monolayer adsorption of lead and cadmium ions. The values of k_l which determines the affinity of binding indicates that the binding sites of azotized PET had greater affinity for lead ions as compared to cadmium ions. This can be attributed to electronegativity of metal ions, since the binding of the metal ions on the adsorbent is also due to ion exchange at the surface [37]. The more electronegative the metal ions the higher the uptake by the adsorbent. According to Pauling’s scale, the electro negativities of lead and cadmium are 1.87 and 1.7 respectively [37].

Freundlich isotherm suited best in describing the binding of copper and chromium ions with R² values of 0.9110 and 0.9859 respectively. The Freundlich isotherm can be applied in heterogeneous systems, especially for adsorbents with interactive species such as copper and chromium. These metal ions are small and also have multiple oxidation states, thus capable of causing polarizing effects leading to heterogeneity [37]. The behavior of and character metal ions species in solution depends on many parameters, such as the composition of dispersed complexing agents particulate matter, mineral content and pH of the dispersing media [37]. An example is the reduction of copper (II) ions in solution is distorted by nitrogen containing ligands in the presence of other functional groups. This is due to the electrostatic repulsions between copper ions and positively charged molecules at certain pH values [37]. The reason for that behaviour is existence of dissolved Cu (II) and Cu (I) oxidation states due to stabilization by the electron donation complexing agent. In that case, both species of copper are attracted by the nitrogen containing azo adsorbent. The same phenomenon is experienced in the analysis of chromium. The distortion due to electrostatic repulsions between the chromium ions and positively charged molecules of the azo adsorbent result to the metal having more one oxidation state attracted on the azo adsorbent. That contribute to the two metals prescribing to the multilayer adsorption as prescribed by the Freundlich model.

This was supported by the ${k_F}$ values for copper and chromium ions are 10.04 and 2.472 mg/g respectively. The values of $\frac{{\text{1}}}{{\text{n}}}$being in the Freundlich model were observed to be less than 1 indicating that the adsorption of copper and chromium ions by azotized PET was heterogeneous thus multisite. The sorption of lead ions with modified azo adsorbent gave an R² value of 0.947 for Langmuir and 0.9217 for the Freundlich model. These values have reasonably high correlation however, the sorption mechanism of lead can best prescribe to the Langmuir model. Langmuir model describes a monolayer adsorption and it indicates a chemisorption mechanism. Lead is a relatively bulky ion with low polarizing ability.

3.6 Regeneration of used adsorbent

Desorption studies were undertaken in order to ascertain the reusability of azotized PET adsorbent and thus the cost effectiveness of the treatment method. It is also useful in the recovery of valuable metals from water. This was done by loading 0.03 g of the adsorbent with 10 mL of 40 ppm metal ions [33]. The metal ions retained by azotized PET were stripped with 50 mL of 1.0 M nitric acid and determined using FAAS [22, 30]. The adsorption-desorption studies were repeated five times under the same experimental conditions, and the fraction recovered for each cycle was determined using Eq. 9.

$$\% R=\frac{{{C_e}}}{{{C_o}}}100$$

Where C_e is the concentration of the metal ions retained while C_o is the initial metal ion concentration. Figure 12 shows the adsorption-desorption cycles of the adsorbents for the metal ions.

Figure 12: Adsorption cycles of the azotized PET for the metal ions.

From the results in Fig. 11, it can be observed that azotized PET adsorbent could be used up to 5 cycles for the removal of copper, lead and cadmium with still over 80% sorption efficiency. However, the adsorption efficiency of chromium ions by azotized PET declined to 66.81% by the 5th cycle. This indicate that the attached azo group is resistant to leaching and hence the regeneration ability and reusability of the azotized adsorbent. These results are in agreement with those obtained by Tharanitharan and Srinivasan as they removed Ni (II) ions from water and waste water using modified Duolite XAD-761 resin [31].

3.7 Analysis of environmental water samples

The azotized PET adsorbent was applied in real water samples obtained from Kipsonoi River. This was done by adding a 50 mL water sample previously spiked with known concentration of individual heavy metal ion to 0.03 g of the adsorbent and equilibrating for 50 minutes in a mechanical shaker. The retained metal ions were then stripped with 10.0 mL of 1.0 M nitric acid and their concentrations determined by FAAS [21, 35]. The results are given in Table 3.

Table 3

Langmuir and Freundlich isotherm parameters for the binding of metal ions
Metal ion	Added (mg L^− 1)	Azotized PET
		Found (mg L^− 1)	% recovered
Cu²⁺	0		-
	2	1.985 ± 0.010	92.00 ± 0.459
	4	3.851 ± 0.020	92.62 ± 0.476
Pb²⁺	0		-
	2	1.936 ± 0.018	91.16 ± 0.830
	4	3.923 ± 0.018	95.13 ± 0.446
Cd²⁺	0		-
	2	1.978 ± 0.018	98.63 ± 0.887
	4	3.613 ± 0.027	90.21 ± 0.664
Cr⁶⁺	0		-
	2	1.513 ± 0.016	75.42 ± 0.799
	4	2.576 ± 0.018	64.29 ± 0.450

Table 3: Langmuir and Freundlich isotherm parameters for the binding of metal ions

The results (Table 3) obtained when the adsorbent was applied to real water sample are comparable to those obtained using the model solutions. The recovery values obtained were over 90% for copper, lead and cadmium. However, the adsorption of chromium was found to be relatively lower for the environmental water samples. The recovery was not 100% due to the effect of interferences by species in the samples with an environmental matrix [47]. Despite that, the results indicate that there is reliability of the present method in the recovery of heavy metal ions from environmental water samples without significant interference by various matrices [35].

This study successfully functionalized PET to produce an azotized material which was confirmed by FTIR analysis. The modified material exhibited colour variations upon interaction with metal ions. That colour indicating metallization process was applied for the removal of the metals from water with the synthesized adsorbent that was capable of indicating when it was exhausted. Sorption parameters such as the effect of contact time, sorbent dose, pH of the sample and the adsorption capacity were investigated and optimized at fixed temperature (25°C). The optimum pH for the adsorption of copper, lead and chromium was found to be 6.0 and that of cadmium was 5.5, thus within the physiological pH of water. The uptake of metal ions was more than 90% within the first 10 min of contact time. The adsorption of lead and cadmium prescribed to Langmuir isotherm model of monolayer adsorption implying a chemisorption process while the adsorption of copper and chromium conformed to Freundlich isotherm model. The adsorption capacities of copper, lead, cadmium and chromium were found to be 46.47, 33.65, 70.93 and 59.06 mg g^− 1 respectively. The metal ions attached on the adsorbent were easily stripped of by the use of a dilute acid, hence easily regeneratable. The results obtained confirmed that azotized PET has the potential to be applied as an efficient and effective colour sensitive sorbent for the removal of heavy metal pollutants from water.

Acknowledgements

The authors appreciate Ministry of Education Science and Technology (MOEST) through African Development Bank (ADB) grant for the tuition fees.

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Scheme 1 and 2 are available in the Supplementary Files section.

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scheme1.png
Scheme 1 Metalized azo pigment
scheme2.png
Scheme 2: Azotization of the polyethylene terephthalate material

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Removal of Metals by Sorption with Metal Concentration Colour Sensitive Azotized Polyethylene Terephthalate Adsorbent

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Abstract

Figures

1. Introduction

2. Material And Methods

2.1 Chemicals and reagents

2.2 Instrumentation

2.3 Procedures

2.4 Adsorption kinetics

2.5 Adsorption isotherms

2.6 Desorption studies

2.7 Analysis of environmental water samples

3. Results And Discussions

3.1 Characterization of the adsorbent material

3.2 Optimization experiments

3.3 Sorption Kinetics

3.4 Effect of adsorbent on the uptake of heavy metal ions

3.5 Adsorption isotherms

3.6 Regeneration of used adsorbent

3.7 Analysis of environmental water samples

4. Conclusions

Declarations

Acknowledgements

References

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Additional Declarations

Supplementary Files

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