Efficacies of sodium nitrite and sodium citrate–zinc acetate mixture to inhibit steel rebar corrosion in simulated concrete interstitial solution contaminated with NaCl

  • Binsi Paulson Maliekkal
  • Joby Thomas Kakkassery
  • Vinod Raphael Palayoor
Open Access
Research
  • 136 Downloads

Abstract

Investigations were carried out to compare the effectiveness of compounds such as sodium nitrite, trisodium citrate (TSC) and TSC–zinc acetate to inhibit the corrosion of steel rebar in simulated concrete interstitial solution contaminated with chloride and to explain the mechanism of corrosion inhibition on reinforcing steel by these systems. Inhibition efficiency of these systems was studied by electrochemical techniques such as potentiodynamic polarization and half cell potential measurements. Electronic spectral studies of simulated pore solution and FT-IR spectral investigations of the film deposited on steel surface were carried out for understanding the mechanism of corrosion inhibition. Microscopic surface analysis was conducted to obtain the surface morphological behaviour of steel rebar. TSC alone was not exhibited good corrosion inhibition at very low and high concentrations according to electrochemical studies. However, in the presence of zinc acetate, corrosion protection efficiency of TSC increased appreciably. When comparing with sodium nitrite, TSC in the presence and absence of zinc acetate displayed good corrosion inhibition efficiency. Among a number of samples, TSC 100 ppm-zinc acetate 50 ppm combination showed maximum corrosion inhibition efficiency on steel rebar in simulated concrete interstitial solution.

Keywords

Corrosion Inhibitor Trisodium citrate Reinforced concrete 

Introduction

Premature deterioration of concrete structures mainly occurs due to the ingress of chloride ions and carbon dioxide [1]. Chloride ions make local depassivation of the steel rebar leading to pitting corrosion [2, 3, 4, 5]. Carbon dioxide reacts with the alkaline compounds present in concrete leading to lower pH and consequent loss of passivation of the rebars [6, 7, 8, 9]. Among a few procedures available to minimize the corrosion of steel rebar in concrete, the use of corrosion inhibitors has been envisaged as the most practical solution [10, 11, 12, 13, 14]. An ideal corrosion inhibitor is a chemical substance which when added to concrete, prevent corrosion onset without making any adverse effects on the mechanical properties of the concrete. It has been generally accepted that inhibitors influence the kinetics of the electrochemical reactions involved in the corrosion process occurring in steel [15, 16, 17].

The mechanisms by which corrosion inhibitors are able to protect reinforcing steel have been discussed in the literature and include (1) decrease in the diffusion rate of the chloride ion (2) increase in the amount of bound chloride (3) increase in the chloride ion threshold value or (4) inhibition of the anodic, cathodic or both reactions [18, 19, 20, 21]. There are some controversies existing about the inhibition mechanism and protection efficiency of corrosion inhibitors. Some authors argue that those compounds which are used to protect concrete reinforcement are not effective [10] when the concrete is kept immersed in NaCl solution, whereas others report that some compounds are effective in reducing corrosion rate of steel rebar in concrete contaminated with chlorides [22, 23].

The inhibitors commonly used to control the reinforcement corrosion are usually classified in two: (1) inhibitors that can be mixed with fresh concrete mixture and applied in reinforced structures (admixture) and (2) inhibitors which are applied on the concrete surface during the rehabilitation procedures since they can diffuse into the hardened concrete (migrating corrosion inhibitors—MCI) [24, 25, 26]. Nowadays, some admixtures are available in the market, which are based on inorganic or organic compounds. Inorganic inhibitors are mainly consist of nitrites or sodium mono-fluoro-phosphate [27, 28, 29]. Effectiveness of nitrites as corrosion inhibitor has already been proved by various researchers [30, 31, 32]. Other organic corrosion inhibitors such as aminoethanols have also been studied; however, they are not as successful as nitrites [33, 34, 35]. Some organic water soluble admixtures are typically based on the mixtures of alkanolamines or organic acids. This kind of commercial inhibitors have been widely applied, but a very little is known about the mechanism of corrosion protection [36]. It is believed that these inhibitors are able to diffuse to the anodic or cathodic site (or both) on the steel surface and interfere the electrode reaction, and thus prevent corrosion initiation [37].

To investigate concrete rebar corrosion studies, researchers either depend upon actual concrete specimens or simulated concrete pore solution [38, 39]. Since first method is rather time consuming, many investigators adopt the second method as a quick procedure [40]. The choice of concrete pore solution gives an adequate support to study the corrosion behaviour of reinforcing steel in chemical conditions [33, 41].

In this work, corrosion inhibition efficacy of compounds such as trisodium citrate (TSC) and TSC–zinc acetate mixture on steel rebar in simulated concrete interstitial solution contaminated with NaCl was evaluated and compared with the corrosion inhibition efficacy of sodium nitrite on steel rebar in the same solution. The present investigation also aims to explain the behaviour of these chemical species on steel rebar in contaminated concrete pore solution.

Experimental

Materials

Chemicals such as trisodium citrate (98%), sodium chloride (> 99.9%), NaNO2 (EMSURE®) and zinc acetate (> 99%) were purchased from Merck Millipore. Portland cement (Malabar Cements Ltd, Kerala) used for the preparation of aqueous extract was procured from the market.

Steel rebar having approximate composition 0.62% Mn, 0.1% P, 0.04% S, 0.021% Si, and rest Fe (estimated by EDAX technique—SEM, Hitachi SU6600 model) was cut (10 cm) and pickled with 2 M HCl for 20 min. Steel specimens were washed with distilled water, degreased with acetone and dried in hot air oven for 5 min. The working solution (concrete pore solution) was prepared by mixing cement with water having a water/cement ratio 0.5 [42]. Temperature of the cement–water mixture gradually increased due to exothermic nature of hydration of cement. The mixture was continuously stirred for 15–20 min using mechanical stirrer for maintaining the homogeneity and temperature stabilisation. The mixture was filtered using vacuum pump to obtain clear concrete pore solution (CPS). The pH of the solution was between 12.5 and 13. Approximate chemical composition of this solution was determined by volumetric and photometric methods and is given in Table 1. To 100 ml of concrete pore solution, 3.5 g of NaCl was added to achieve 3.5% NaCl concentration. To this, trisodium citrate (TSC) was added to attain the concentrations 50, 100, 150, 200 and 1500 ppm. Similarly, NaNO2 solutions were prepared in CPS. Another set of sodium citrate solutions were also prepared (50–200 ppm) in CPS containing 50 ppm of zinc acetate (ZnAc).
Table 1

Composition of aqueous cement extract simulating the concrete interstitial electrolyte

Species

Ca2+

SO42−

Fe3+

PO43−

Cl

F

Mg2+

Conc. (ppm)

854

6642

1700

7.54

214

4.89

< 2

Potentiodynamic polarization studies

Steel specimens were immersed in CPS for 3 days in the presence and absence of added compounds. Potentiodynamic polarization studies were carried out using three electrode cell assembly consisting of steel rod as working electrode (exposed area 4 cm2), platinum electrode as counter electrode (1 cm2) and saturated calomel electrode (SCE) as reference electrode at 30 °C. A potential range of + 250 to − 250 mV with a sweep rate of 1 mV/s was used for the study. Slope analysis of Tafel curves gave the corrosion current densities, and the inhibition efficiency was calculated by the following equation [43, 44, 45]:
$$\eta_{\text{pol }} \% = \frac{{I_{\text{corr}} - I_{\text{corr}}^{\prime } }}{{I_{\text{corr}} }} \times 100,$$
where Icorr and \(I_{\text{corr}}^{\prime }\) are the corrosion current densities of exposed area steel rebar in the absence and presence of inhibitor, respectively.

Half cell potential measurements

For a quick examination of the corrosion behaviour of steel rebar in various medium, half cell potential measurements were carried out. After an equilibration period of 24 h, saturated calomel electrode (SCE) was immersed into solution containing steel rebar. The EMF of cell was measured using a high impedance voltmeter (HP E2378A). Half cell potential of steel electrode was obtained by subtracting the EMF from electrode potential of SCE at 30 °C.

Spectroscopic studies

To elucidate the mechanism of interaction of the added compounds on steel rebar immersed in simulated CPS, UV–visible spectroscopic study was performed (Schimadzu UV–visible-1800 spectrophotometer). The spectra of solutions were recorded after 3 days. The oxide film deposited on the steel rebar was carefully scratched with a stainless steel blade, dried and performed FT-IR spectral studies. KBr pellet method was employed to record IR spectra in the range 4000–400 cm−1 using Schimadzu IR Affinity-1 model FT-IR spectrophotometer.

Microscopic surface analysis

To investigate the surface morphological changes on the steel rod dipped in simulated concrete pore solution [46, 47], microscopic studies were performed using Leica Stereo Microscope (S8ACO).

Results and discussion

Potentiodynamic polarization studies

Interaction of sodium nitrite with steel rebar

The effect of sodium nitrite concentration on the corrosion of steel rebar in the simulated concrete interstitial solution was investigated using polarization experiments. Data obtained from polarization studies are represented in Table 2. Sodium nitrite solution having concentrations 50–1500 ppm was taken of the study. It is understandable from the polarization data that at very low concentration (50 ppm), sodium nitrite acted as a corrosion antagonist, i.e., the corrosion rate of steel rebar treated with nitrite was greater than that of the rebar immersed in CPS without nitrite (blank). This result warns that one must be very cautious regarding the concentration of the nitrite in concrete when it is employed as an admixture. But as the concentration of nitrite exceed 50 ppm in CPS, the corrosion inhibition efficiency increased. Sodium nitrite showed only 54.84% corrosion inhibition efficiency on steel rebar at a concentration of 1500 ppm in the simulated CPS.
Table 2

Potentiodynamic polarization data of steel rebar immersed in contaminated concrete pore solution in the presence and absence of various compounds at 30 °C

System

Icorr (μA/cm2)

ba (mV/dec1)

− bc (mV/dec1)

− Ecorr (mV)

ηpol%

Blank

45.6

136

222

777.7

NaNO2 50 ppm

52.79

156

192

752.5

− 15.76

NaNO2100 ppm

29.26

155

106

735.2

35.83

NaNO2 150 ppm

33.09

182

74

751.6

27.56

NaNO2 200 ppm

36.20

215

83

727.8

20.61

NaNO2 1500 ppm

20.59

407

176

472.7

54.84

TSC 50 ppm

34.24

142

97

746.1

24.91

TSC 100 ppm

20.01

156

112

742.9

56.11

TSC 150 ppm

15.50

146

81

746.9

66.01

TSC 200 ppm

22.17

177

82

756.2

51.38

TSC 500 ppm

52.92

247

137

723.8

− 16.05

TSC 1100 ppm

53.91

173

284

837.5

− 18.22

TSC 1500 ppm

170.20

254

451

889.1

− 272.0

ZnAc 50 ppm

20.09

167

71

714.9

55.94

ZnAc 100 ppm

22.14

164

78

700.4

51.44

ZnAc 50 ppm + TSC 50 ppm

39.13

160

145

709.0

14.18

ZnAc 50 ppm + TSC 100 ppm

9.021

105

63

789.9

80.23

ZnAc 50 ppm + TSC 150 ppm

10.27

101

95

782.8

77.47

ZnAc 50 ppm + TSC 200 ppm

11.99

104

87

774.8

73.70

From the Tafel plots (Fig. 1a), it is evident that at lower concentrations of nitrite, the cathodic slopes of polarization curves considerably changed when compared to that of blank steel rebar. But a drastic change in the anodic slopes of Tafel plots observed as the concentration increased. Thus, it can be concluded that at appreciable concentrations, nitrites mainly affect the anodic process of corrosion. It has been established by the earlier researchers that sodium nitrite, an anodic inhibitor, modifies the oxide film on the steel rebar to be more protective than the film that naturally forms in concrete. The inhibitive action of NaNO2 is due to reaction of nitrite ions with Fe2+ ions as shown in the following equation [48]:
$$2 {\text{Fe}}^{ 2+ } + 2 {\text{OH}}^{ - } + 2 {\text{NO}}_{ 2}^{ - } \to 2 {\text{NO}} \uparrow +\,{\text{Fe}}_{ 2} {\text{O}}_{ 3} + {\text{H}}_{ 2} {\text{O}}.$$
Fig. 1

Tafel curves of steel rebar in contaminated concrete pore solution containing a sodium nitrite, b TSC and c ZnAc and ZnAc + TSC at different concentrations

Sodium nitrite competes with the chloride ions for ferrous ions produced in concrete and incorporates them into a passive layer on the steel surface, and hence preventing further corrosion.

Interaction of trisodium citrate with steel rebar

Polarization experiments were conducted on steel rebar after an immersion period of 3 days in concrete pore solution containing TSC and 3.5% NaCl (Fig. 1b).

The corrosion protection capacity of TSC on steel rebar was ̴ 25% at 50 ppm concentration (Table 2). The inhibition efficiency (ηpol%) increased with the concentration and a maximum of 66% was reached at 150 ppm of TSC. After this concentration, ηpol% started to decrease. At a concentration of 1500 ppm, TSC showed corrosion antagonistic behaviour on steel rebar in CPS. This change of the behaviour of TSC on the steel rebar can be illustrated with the help of two competitive reactions. Citrate ions have a substantial capacity to adsorb on the steel surface from CPS, and hence at lower concentrations they can decrease the rate of corrosion. Simultaneously, citrate ions have a strong tendency to make coordinate bonds with Fe2+ ions. The strong complexation between Fe(II) with citrate ions has been well established by Krishnamurthy and Huang [49]. In other words, tendency of TSC to adsorb on steel surface leads to the corrosion inhibition behaviour of the molecule and the affinity of TSC towards ferrous ions favours corrosion antagonistic behaviour. As the concentration of TSC increases, the second process will predominate in the solution over first. This causes to dissolve more and more Fe atoms from the rebar surface to the solution. The mechanism of the interaction of citrate ions on steel rebar surface in CPS can be represented as shown in Fig. 2a. Some of the TSC molecules adsorb on steel surface through oxygen atoms. The species present in the bulk of the solution is Fe(II)–citrate complex. From the figure it can be realized that enhanced dissolution of Fe takes place due to the strong coordinating tendency of citrate ion with ferrous ions.
Fig. 2

Interaction of citrate ions on steel surface in simulated concrete pore solution a in the absence of zinc acetate and b in the presence of zinc acetate

The behaviour of sodium citrate on steel rebar in concrete pore solution was further verified by electronic spectroscopy. Two significant peaks appeared in the electronic spectrum of TSC in the simulated concrete pore solution at 340 and 217 nm can be explained due to n → π* and π → π* electronic transitions, respectively. CPS contains TSC (1500 ppm) when treated with steel rebar for 3 days, showed three peaks in addition to the above mentioned peaks in UV–visible spectrum. Additional peaks displayed at 682, 757 and 788 nm can be assigned to the electronic transitions of Fe(II)–citrate complex. Furthermore, it is noticed that the colour of the concrete pore solution containing TSC (1500 ppm) gradually changed into pale green when it was treated with steel rebar. This colour was persisted for ~ 10 days. This indicates the stability of Fe(II)–citrate complex in the alkaline CPS. All other concrete pore test solutions (including nitrite added CPS) were changed into brown colour during 2–3 days. This implies that the Fe(II) ions produced due to corrosion is converting to Fe(III) ions quickly. Hence it can be concluded that the reluctance of Fe(II) to convert into Fe(III) in CPS containing NaCl and TSC is definitely due to the strong complex formation between Fe(II) and citrate ions.

To improve the corrosion inhibition efficiency of TSC on steel rebar, zinc acetate (ZnAc) was added to the concrete pore solution. Table 2 describes the corrosion inhibition efficacy of TSC–ZnAc system and the potentiodynamic polarization parameters of steel rebar. Tafel plots are depicted in Fig. 1c. Data show that ηpol% of TSC enhanced appreciably in the presence of zinc acetate. Highest value of ηpol% (80.23%) was shown by TSC at 100 ppm in the presence of 50 ppm ZnAc, while it was only 56.11% in the absence of ZnAc. Thus, a drastic depletion in the rate of corrosion of steel rebar was noticed in the presence of TSC–ZnAc mixture in concrete pore solution. This is definitely due to the involvement of zinc ions which favours the strong adsorption of citrate ions on the steel rebar surface [50, 51]. TSC alone did not satisfactorily obey any adsorption isotherm on steel surface. But on the addition of ZnAc, it followed Langmuir adsorption isotherm for a concentration range of 100–200 ppm (Fig. 3).
Fig. 3

Langmuir adsorption isotherm for TSC–ZnAc system on steel surface in CPS contaminated with NaCl (TSC 100–200 ppm and ZnAc 50 ppm)

It can be assumed that affinity of Fe(II) ions to coordinate with citrate ions is minimized considerably in the presence of zinc acetate. This can be easily visualized with the help of Fig. 2b. Zinc ions attach on the steel surface first followed by the adsorption of citrate ions through zinc ions. But as the concentration of TSC increased, the corrosion inhibition efficiency began to decrease slowly. This can be illustrated by the same mechanism proposed for of Fe–citrate interaction without ZnAc.

On examination of the polarization data, it is understand that the citrate ion mainly acts on cathodic sites of corrosion. The cathodic slopes of polarization curves of steel rebar in TSC solution were considerably changed than that of blank experiment. Similar trend was observed for the polarization curves of steel rebar in TSC–ZnAc solution (Fig. 1c). The steel rebar treated with concrete pore solution containing 100 ppm of citrate and 50 ppm of zinc acetate displayed least value for cathodic slope in Tafel plot, suggesting that this particular combination has a great influence on the cathodic process of corrosion than any other combination. In alkaline medium, the main half cell reactions responsible for the corrosion are the oxidation of Fe into Fe2+ (anodic) and reduction of O2 into OH (cathodic). Citrates and citric acid are well known for its anti-oxidant property [52, 53]. The anti-oxidant property of citrate ion arises due to the scavenging of oxygen molecules. Since citrate ions mainly affect the cathodic sites of corrosion, it can be robustly believed that the oxygen molecules available for the reduction process are considerably reduced in the presence of citrate ions. Thus, it can be concluded that the ability of TSC and TSC–ZnAc systems to decrease the rate of corrosion of steel rebar in concrete pore solution is due to the combined action of adsorption and scavenging of oxygen molecules.

Comparison of ηpol% of various systems on steel rebar in CPS contaminated with 3.5% NaCl at 30 °C is shown in Fig. 4.
Fig. 4

Comparison of ηpol% of various systems on steel rebar in simulated concrete pore solution contaminated with 3.5% NaCl at 30 °C

Half cell potential measurements

Measurement of half cell potential of steel rebar gave a rough idea about the probability of corrosion. It has been generally accepted by the scientists that more negative the half cell potential, greater will be the possibility of corrosion. Half cell potentials of steel rebar immersed in concrete pore solution for a period of 24 h in the presence and absence of various compounds are given in Table 3 and compared with the help of a bar diagram (Fig. 5). According to the data, the steel rebar immersed in concrete pore solution (blank) showed a potential of − 460 mV against SCE. This is a clear indication of high corrosion rate of steel rebar. A regular increase of electrode potential (towards cathodic) was noted with the addition of TSC. But as the concentration reached to 200 ppm, electrode potential shifted to more anodic side. At 1500 ppm of TSC concentration, the electrode potential of the steel rebar was − 518 mV, indicating that the corrosion rate of steel rebar increased tremendously. Both half cell potential measurements and polarization studies revealed the similar corrosion behaviour of steel rebar in CPS solution. On comparing the potentials of steel rebars in CPS–NaNO2 solution with those rebars treated with CPS–TSC solution, it can be concluded that TSC is acting as a better corrosion inhibiting agent than nitrite at lower concentrations. The steel rebar treated with concrete pore solution containing 100 ppm TSC and 50 ppm ZnAc displayed very low anodic potential (− 283 mV), suggesting that this particular combination works well on the steel surface to reduce the corrosion. Similar result was obtained by potentiodynamic polarization studies.
Table 3

Half cell potential (mV) measured on steel rebar immersed in contaminated CPS-containing NaNO2, TSC and TSC–ZnAc systems at 24 h

C (ppm)

NaNO2

TSC

TSC + ZnAc (50 ppm)

0

− 460

− 460

− 460

50

− 358

− 333

− 349

100

− 338

− 314

− 283

150

− 328

− 307

− 304

200

− 346

− 316

− 307

1500

− 293

− 518

− 508

Fig. 5

Comparison of half cell potentials of steel rebar in simulated contaminated concrete pore containing NaNO2, TSC and TSC–ZnAc systems

FT-IR analysis

To investigate mechanism of molecular interaction on steel surface in simulated CPS, IR spectral studies were performed. Due to the presence of many species in the simulated concrete pore solution, it is rather difficult to interpret the spectrum of deposited products on steel rebar surface completely. However, on close inspection of the spectra, it is obvious that considerable shift in the frequencies occurred for the samples treated with and without ZnAc. Surface deposition of steel rebar is mainly consists of mixtures of compounds such as hydrated ferric oxide, ferrous and ferric hydroxides, ferrous chloride. In the IR spectrum of products on steel rebar surface (blank), a broad band appeared at 3375 cm−1 is due to –OH stretching frequency of Fe(OH)2 or amorphous hydrated ferric oxide (or both) [54]. The broadness of this peak is considerably reduced in the IR spectra of steel samples treated with TSC and TSC–ZnAc. This is due to the interaction of these species with Fe(OH)2. The bending frequency of –OH appeared in the spectrum of blank (at 1619 cm−1) was also shifted to lower frequency side in other two samples. Signals observed at ~ 440 cm−1 in the IR spectrum of blank and citrate-treated steel rebar are lowered to 401 cm−1 in TSC–ZnAc-treated steel rebar. This can be attributed to the change of lattice vibration of free OH ions due to the interaction O–H–Zn–citrate. Peaks displayed at 1392 and 1383 cm−1 in the IR spectra of two samples are due to the deformation of –CH2 group present in sodium citrate. A weak peak appeared at 1471 cm−1 in the IR spectrum of surface products of blank specimen is due to the existence of ferroxyhite phase associated with the amorphous ferric oxide on the steel surface. Figure 6 represents the IR spectrum of products deposited on steel rebar surface.
Fig. 6

IR spectrum of oxide film deposited on steel rebar in simulated concrete pore solution a contaminated with 3.5% NaCl, b containing 3.5% NaCl + 100 ppm TSC and 3.5% NaCl + 100 ppm TSC + 50 ppm ZnAc

Microscopic surface analysis

Visual examination of the micrographs showed that the ferric oxide layer formed on the steel rod immersed in the sample solutions was uneven, brittle, blistered and black in colour, quite different from the bare, where it was dark brown in colour. The removal of oxide film from the immersed steel rebars was easier due to the non-uniform distribution over the surface as compared to the bare where it was tightly adherent. The textures of immersed steel rods in CPS were different from each other and they also differed from the bare sample. The surface morphology of the steel sample treated with concrete pore solution containing TSC 1500 ppm got a unique appearance as its surface do not contains little or no oxide deposit. The complexing nature of citrate ions with Fe2+ enhanced the removal of more and more Fe atoms from the surface of rebar into the solution (Fig. 7).
Fig. 7

Optical micrographs of Fe rebar a bare surface, b immersed in concrete pore solution contaminated with 3.5% NaCl (blank) c with NaCl (3.5%) + TSC 100 ppm d with NaCl (3.5%) + TSC 100 ppm + ZnAc50 ppm e with NaCl (3.5%) + TSC 1500 ppm at 30 °C (samples be, immersed in CPS for 3 days)

Conclusions

Electrochemical studies of steel rebar in simulated concrete interstitial solution established the corrosion behaviour in the presence of various compounds. At low concentrations, NaNO2 acted as a corrosion accelerator. As the concentration of NaNO2 increased protection efficiency increased. Generally, trisodium citrate exhibited better protection capacity than NaNO2. However, in the presence of TSC–zinc acetate system very appreciable lowering of the corrosion rate was noticed. According to Tafel polarization studies, steel rebar is well protected in concrete pore solution contaminated with 3.5% NaCl by TSC 100 ppm–ZnAc 50 ppm system. Half cell potential measurements gave an idea about the probability of corrosion. Mainly, the rate of cathodic process of steel corrosion was suppressed by TSC and TSC–ZnAc systems in concrete pore solution. FT-IR and UV–visible spectral studies and optical microscopic investigations revealed the mechanism of interaction of compounds on steel rebar.

Notes

Supplementary material

40090_2018_142_MOESM1_ESM.doc (66 kb)
Supplementary material 1 (DOC 65 kb)

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© The Author(s) 2018

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors and Affiliations

  • Binsi Paulson Maliekkal
    • 1
  • Joby Thomas Kakkassery
    • 1
  • Vinod Raphael Palayoor
    • 2
  1. 1.Research Division, Department of ChemistrySt. Thomas’ College (Autonomous)ThrissurIndia
  2. 2.Department of ChemistryGovernment Engineering CollegeThrissurIndia

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