Schiff-Based Fluorescent-ON Sensor L Synthesis and Its Application for Selective Determination of Cerium in Aqueous Media

Sadia, Maria; Khan, Jehangir; Naz, Robina; Zahoor, Muhammad; Khan, Ezzat; Ullah, Riaz; Bari, Ahmed

doi:https://doi.org/10.1155/2020/2192584

Journal of Sensors

On this page

Abstract Introduction Experimental Results Conclusion Data Availability Conflicts of Interest Acknowledgments Supplementary Materials References Copyright Related Articles

Research Article | Open Access

Volume 2020 | Article ID 2192584 | https://doi.org/10.1155/2020/2192584

Schiff-Based Fluorescent-ON Sensor L Synthesis and Its Application for Selective Determination of Cerium in Aqueous Media

Maria Sadia,¹Jehangir Khan,¹Robina Naz,¹Muhammad Zahoor,¹Ezzat Khan,¹Riaz Ullah,²and Ahmed Bari³

Academic Editor: Giuseppe Quero

Received29 Dec 2019

Revised15 Mar 2020

Accepted28 Mar 2020

Published24 Apr 2020

Abstract

In the present study, a fluorescent sensor L for sensing of Ce³⁺ ion was designed and characterized by XRD, ¹HNMR, and FTIR. Its fluorescence behavior towards metal ion was examined by fluorescence spectroscopy. Chelation-enhanced fluorescence was shown by the sensor L upon interaction with Ce³⁺ ion. This fluorescent sensor exhibits high sensitivity and selectivity towards Ce³⁺ ion in acetonitrile solution, forming 2 : 1 (L : M) complex as determined by Job’s plot. Association constant was found to be estimated from the Benesi-Hildebrand plot. No significant interference was observed in the presence of other studied alkali, alkaline, and transition metal ions. A rapid response was observed when employed for the determination of Ce³⁺ ion in spiked water samples with a limit of detection equal to .

1. Introduction

Heavy metal contamination of water bodies is a severe concern of the modern era as it badly affects the natural environment and living beings [1, 2]. Even at a relatively low level of exposures, they are neurotoxic and carcinogenic [3]. Heavy metals are added to water sources due to industrial and anthropogenic activities [4]. Among the rare earth metal cations, cerium (being a heavy metal) is widely distributed in the earth crust. It has a variety of industrial applications in metallurgy, luminescence, microelectronics, agriculture, magnetism, nuclear energy, glass, and ceramics [5]. Cerium can also be found in fluorescent lamps, coloured televisions, arc lamps, and energy-saving lamps. Due to this wide range of usage, cerium concentration is gradually increasing in soils and water bodies. Cerium can cause severe systemic disorders in aquatic animal bodies including damage to the nervous system, reproduction system, and cell membranes. It also causes health problems in human especially in a working environment, e.g., lung embolisms, damage to the liver during long-term exposure, endomyocardial fibrosis, and dendriform pulmonary ossification [6, 7]. It also affects human metabolism, blood pressure, appetite, lowering cholesterol level, and risk of blood coagulation [8, 9]. Liu et al. developed thiophene-containing bis-pyridyl-bis-amide complexes having a good coordination ability for heavy metal ions, high stability in acids, and bases [10].

A number of techniques are in use to determine cerium in water samples like electrothermal atomization atomic absorption spectroscopy [11], inductively coupled plasma mass spectroscopy [12], and high-performance liquid chromatography. However, applicability of all these methods is a question mark due to expensive instrumentation, slow response time, lack of sensitivity/selectivity, and having limited portability [11]. In recent years, fluorescence technology for probing various environmental and biologically important analytes has become a powerful tool because of its rapid response, low cost, real-time monitoring, easy operation, high sensitivity, simplicity, potential for portability, and noninvasive properties [13].

Schiff base containing an azomethine group is the compound synthesized by condensation of carbonyl compounds with primary amines. Due to their structure flexibility and strong coordination capabilities, they are extensively used in the field of coordination chemistry. They coordinate through the nitrogen atom of the azomethine group and the oxygen atom of the deprotonated phenolic group [14]. Due to their multiple biological activities such as antibacterial, antitumor, insecticidal, anticancer, anticonvulsant, anti-inflammatory, and cytotoxicity, as prodrugs, in the strengthening of immune response against cancer, in HIV, and in leukemia, Schiff bases have been studied intensively over the past few decades [15]. They are also widely used in electrochemical and optical sensors [16]. The design of fluorescent sensors for the detection of heavy metal cations is a hot research subject that is under investigation these days. Only few sensors have been reported for the detection of lanthanide metal ions.

In the present research work, a Schiff base fluorescent material: [1-((pyrimidine-4-ylimino)methyl)-napthalene-2-ol] (sensor L), has been designed for the selective determination of cerium in water. Sensor L has naphthalene entity as the signalling site while imine and hydroxyl as the binding moieties. Sensor L was fluorescently silent in the absence of cerium but upon coordination with target analyte exhibited a significant chelation-enhanced fluorescence effect at .

2. Experimental

All experiments were performed in open air using analytical grade reagents, CH₃CN solvent, and distilled water. The chemical reagents (HCl, NaOH, CH₃CN, CH₃COOH, and DMSO) and other solvents (like ethyl acetate, n-hexane, and nitrate salt of lead, barium, cadmium, potassium, cerium, and mercury; sulphate salts of copper, magnesium, zinc, and manganese; and chloride salts of sodium, nickel, and arsenic, 2-hydroxy-1-napthaldehyde, and 2-aminopyrimidine) were from Sigma-Aldrich, Germany. For the determination of melting point, Stuart-SMP 10 was used. FTIR spectrum of sensor L was obtained using Prestige 21 Shimadzu Japan spectrophotometer. X-ray diffraction data was collected on a Bruker kappa APEXIICCD diffractometer. Refinements were carried out using full-matrix least squares techniques on F2 using the program SHELXL-97. UV-vis spectra were taken using a UV-vis 1800 spectrophotometer (Shimadzu, Japan). The ¹H-NMR of the sensor molecule was measured with the help of a JEOL 400 MHz spectrometer using deuterated DMSO as the solvent. The chemical shift of protons is given with reference to residual protons of the deuterated solvents . Fluorescence measurements were carried out using an RF-5301PC Spectrophotofluorometer (Shimadzu, Japan).

3. Synthesis of [1-((Pyrimidine-4-ylimino)methyl)-napthalene-2-ol]

The [1-((pyrimidine-4-ylimino)methyl)-napthalene-2-ol] referred as sensor L was synthesized by adopting the literature procedure [17]. To a methanolic solution of 2-hydroxy-1-napthaldehyde (10 mmol, 0.95 g) 3 drops of acetic acid were added to deprotonate it. An equimolar amount of 2-aminopyrimidine (10 mmol, 1.72 g) was then added dropwise over a period of 10 min followed by reflux at 80°C with vigorous stirring for a period of 14 h. Upon completion of the reaction, a light yellow product was formed. Reaction was continuously monitored by thin layer chromatographic (TLC) technique, using an appropriate solvent system, n-hexane : ethyl acetate (6 : 4), and the spots were recognized with the help of iodine chamber. After reaction completion, the product obtained was filtered, washed with excess of ethanol, dried, and recrystallized from hexane with 82% yield, having a melting point of 94-96°C (uncorrected). The IR (KBr, cm^-1): ν_C-OH 1298, 1207; ν_C=N, 1616, ν aromatic C=C, 1494, 1436; ν aromatic-C-H, 3036. ¹H-NMR (400 MHz, DMSO-d₆) δ ppm = 14.53 (br, 1H, HO), 10.81 (s, 1H, N=CH), 9.56, 9.53, 8.94, 8.92-6.52 (m, 9H, Aromatic without assignment). The structure and synthesis of sensor L are given in Figure 1.

4. Solution Preparation for Spectroscopic Measurement

Sensor L stock solution was prepared in acetonitrile as it was not soluble in water. Metal ion stock solutions were prepared in distilled water using nitrate salt of lead, barium, cadmium, potassium, cerium, and mercury; sulphate salts of copper, magnesium, zinc, and manganese; and chloride salts of sodium, nickel, and arsenic. Working solutions were prepared from stock solution by appropriate dilution. UV-visible and fluorescence spectra of sensor L were recorded in acetonitrile/water mixture (2 : 8). For spectroscopic analysis each time a fresh test sample was prepared by taking 7 mL of sensor L and 3 mL of metal ions in a beaker, equilibrated at room temperature. The pH of the test sample was adjusted using NaOH and HCl. Fluorescence analysis was performed with a slit width of 10 nm using quartz cuvettes of 1 cm path length.

5. UV-Visible Analysis

Owing to the weak water solubility of sensor L (5 μM), the spectra were taken in acetonitrile/water (2 : 8) mixture. The solution of cerium was prepared in the range 2-20 μM. Test solution containing a fixed amount of sensor L while increasing concentration of cerium was prepared, and spectra were recorded in the range 200-800 nm.

6. Metal Ion Binding Study by Fluorescence Titration

Sensor L (5 μM) was added with varied metal ion concentrations (up to 200 μM), and fluorescence spectra were recorded in the range 200-800 nm at 351 nm. Among the examined metal ions, only cerium was able to enhance the fluorescence of sensor L. Job’s plot experiment was conducted by plotting the fluorescence intensity at the -axis to determine the binding stoichiometry between sensor L and cerium. Association constants of sensor L-cerium complex were determined by the Benesi-Hildebrand equation.

7. Results and Discussions

7.1. IR Data

For the identification of functional groups present in the synthesized sensor L, FTIR spectroscopic analysis was performed. The peak details are presented in Table 1. The characteristic bands assigned to different functional groups were based on comparison with the available literature. The appearance of characteristic stretching band (C=N) in sensor L at 1612 cm⁻¹ and disappearance of aldehyde carbonyl (C=O) peak in the region of 1700 cm^-1 confirm the formation of sensor L (Figure 1S). Strong bands at 3,036 cm^-1 were assigned to the aromatic C–H group. The spectrum displayed absorption bands at 1491 and 1436 cm^-1 corresponding to the aromatic C=C group while at 1294 and 1210 cm^-1 representing phenolic (–OH) stretching vibration. In addition to the abovementioned IR band, it also exhibited bands at 1136 and 1035 cm^-1 for the aliphatic –C-O group [18].

7.2. Characterization by ¹H-NMR

The ¹HNMR spectrum of sensor L shows a number of characteristic peaks as expected for the proposed structure of the compound, sensor L. There are two characteristic peaks to elucidate the structure: one is azomethine (HC=N-) group which appears at 10.81 and the other one is proton at 14.53 as a result of zwitterion formation between OH protons with imine nitrogen which is a clear indication of the product formation (Figure 2S). Aromatic protons of other moieties appear as overlapping multiplets and cannot be precisely assigned. The data set obtained for sensor L is well comparable with the reported data for structurally analogous compounds [19, 20].

7.3. Characterization by X-Ray Diffraction

A single crystal of sensor L was grown from slow evaporation of its mother liquor. Single crystal X-ray diffraction analysis was used for the confirmation of solid-state structure of sensor L (CCDC No. 1987815). For data collection, scan and multiscan corrections were applied. Crystallographic analyses were carried out with the Bruker kappa APEXIICCD diffractometer, with a graphite monochromator (Mo-Kα radiation) () at ambient temperature. The crystal solution and refinements of sensor L were handled with SHELXL-97 [21] and publ CIF [22]. Full-matrix least squares techniques were used for final refinement on F2. Sensor L crystallizes in an orthorhombic system with the space group P2₁2₁2₁. The molecular view of sensor L with a partial numbering scheme is shown in Figure 2. The crystallographic data pertaining to crystal structure solution and refinement are given in Table 2. In the molecule, the naphthalene ring is regarded as the principal ring system. All atoms and ring system of the molecule are coplanar with negligible deviation. The characteristic bond lengths are C10-C11 1.381, C11-N11.340, N1-C12 1.397, and C1-O1 1.266 Å. Bond angles C12-N1-C11 124.51, N1-C11-C10 124.40, and O1-C1-C10 122.44° are well comparable with literature reports for structurally similar molecules [23]. The structure of sensor L indicates intramolecular hydrogen bonding as shown in Figure 3, since the molecule (L) contains electron-rich centres such as N, O, and π-bonds, which are involved in stabilizing the supramolecular structure of the compound. The O1 of each molecule interacts with CH function of neighbouring naphthalene moiety (separation distance is O1-C5 3.419 Å). C1 of the molecule is considerably polar, and it interacts with N3 of the neighbouring pyrimidine moiety with a separation distance of 3.247 Å. Similarly, pi-pi interaction between C2 and C11 can also be observed with a distance of 3.357 Å. These interactions collectively extend the structure in a 3D fashion (Figure 3).

7.4. UV-vis Absorption Spectroscopic Analysis

The UV-visible spectrum of sensor L showed characteristic main absorption band in the range 250-390 nm with a of 320 nm (Figure 3S). Upon addition of Ce³⁺ to sensor L, was shifted to 330 nm. The red shift of is an indication of coordination involving the hydroxyl and imine as a receptor and Ce³⁺ as an analyte. Upon addition of different concentrations of Ce³⁺ to sensor L solution, a marked enhancement in absorbance at 330 nm was noted. For absorbance analysis, test samples of sensor L, 5 μM, and different concentrations of Ce³⁺ ions were prepared. All the operations were performed at room temperature. The correlation coefficient value (; Figure 4S) obtained was in good agreement with that reported in the literature [24].

7.5. Fluorescence Studies

The fluorescence spectrum of sensor L was taken in the range of 200-800 nm with varying excitation wavelengths from 220 to 400 nm. The maximum fluorescence intensity for sensor L was observed at 351 nm as excitation wavelength as shown in Figure 5S.

7.6. Preliminary Study

The response of sensor L to fluorescence and UV radiation were evaluated through a titration method, and a good linear response has been observed (Figures 6S and 7S). Fluorescence response of sensor L (5 μM) was examined in CH₃CN/H₂O mixture (2 : 8) towards different metal ions (200 μM). First, the fluorescence emission of sensor L was studied in the range 250–800 nm with an excitation at 290 nm and an emission at 351 nm. Due to internal charge transfer phenomenon, very weak emission intensity was displayed at 351 nm by the free sensor L. To investigate metal ions sensing ability of sensor L, metal ions were separately added to the sensor L solution. The mixtures were equilibrated for 3 min at room temperature and transferred separately into cuvette, and the fluorescence of each test solution was monitored at 351 nm. Among the metal ions studied, only Ce³⁺ was able to enhance the fluorescence of sensor L (Figure 8S) which was due to combined effects of chelation, C=N isomerization, and intramolecular charge transfer mechanism [24].

7.7. Effect of Time

For fluorescent sensor, response time is one of the most important parameters to be measured. For this purpose, kinetic studies of fluorescent sensor L (10 μM) separately and in the presence of Ce³⁺ (3 μM) were studied from fluorescence spectra by measuring fluorescence emission intensities at different time intervals. The time range for this study was from 1 to 10 min. At 351 nm in the absence of Ce³⁺, no change in the fluorescence intensity occurred showing the stability of subject sensor L in the given conditions. In fluoremetric analysis, longer response time is undesired. The sensor L displayed instantaneous enhancement at 351 nm upon the addition of Ce³⁺ solution, indicating fast response of sensor L with Ce³⁺ (Figure 9S). The response time was less than 40 seconds even for high concentration of Ce³⁺. These results show that the determination of Ce³⁺ can be done immediately without any delay upon Ce³⁺ addition and sensor L is highly detectable in real samples with fast response (in terms of time).

7.8. Effect of Solvents

Changes in the fluorescence emission intensities of sensor L upon formation of complex with Ce³⁺ were investigated in a number of solvents including dimethyl sulfoxide (DMSO), methanol/water (2/8 ), N,N-dimethylformamide (DMF), acetone, chloroform, hexane, toluene, ethanol/water (2/8 ), and dichloromethane (Figure 10S). No solvent, other than the mixture of acetonitrile/water (2/8 ), showed good results in terms of fluorescence emission intensity [25].

7.9. Determination of Detection Limit

Free sensor L (5 μM) quenches fluorescence due to internal charge transfer phenomenon at 351 nm. Upon the addition of an equivalent of Ce³⁺ to sensor L solution (Figure 11S), enhancement at 351 nm occurred gradually by increasing Ce³⁺ concentration in the tested range (10-100 μM) which was due to the inhibition of internal charge transfer phenomenon. A best sensor is one which can detect even low concentration of metals. In the current study, the limit of detection of sensor L was found to be , determined from fluorescence spectra, which is much lower as compared to those of other reported sensors in the literature [26]. The limit of detection was calculated according to the formula: where is the standard deviation of blank measurements and is the slope of the plot of the fluorescence intensity versus sample concentration [27]. The mechanism of interaction can be explained as follows.

7.10. Association Constant and Binding Stoichiometry

For association constant and binding stoichiometric ratio determination, equimolar solutions (10 μM) of both sensor L and Ce³⁺ were used (Figure 12S). Job’s plot analysis was performed by continuous increase of one part and decrease of another part while keeping total concentration of both sensor L and Ce³⁺ constant at 10 μM (Figure 13S). Binding ratio was determined from their respective fluorescence emission intensities. Maximum fluorescence intensity was achieved at a molar fraction of 0.7 at 351 nm indicating 1 : 2 binding stoichiometry between sensor L and Ce³⁺ ion. It means that one Ce³⁺ ion binds to two units of sensor L.

There are four potential coordination cites in the ligand, including three N of guanidyl moiety and an oxygen of the hydroxyl group attached to the naphthyl group. The proposed structure of complex formed by mixing the ligand solution and Ce (NO₃)₃ salt is given in Scheme 1. The ligand is expected to act as bidentate and can also act as tridentate. In either case, the prosed structure as given in the Scheme 1 will be afforded. The coordination sphere of f-block elements like Ce can easily be expanded to 8 [28]. In several cases, the coordination number 6 [29] has also been reported. Since the bulk of our ligand is moderate and the bonding is expectedly strong, therefore, we expect that the proposed structure 2 in the scheme would be a probable complex with extra stability under the provided conditions of pH 7, at 60°C in methanol. The selectivity of the ligand regarding Ce was found to be excellent under these conditions while other metal ions were sensed up to negligible limit. Our investigations with respect to sensing of other metal ions as stated above are in progress, and it is hoped that conditions will be optimized soon to carry out the same with the given ligand.

Association constant was measured from the Benesi-Hildebraned plot from the increase in fluorescence intensities of sensor L as a function of Ce³⁺ ion concentration (Figure 14S). Based on equation (2), the association constant value was calculated.

In the given equation, (M^-2) is the association constant, is the fluorescence emission intensity of sensor L in the absence of Ce³⁺ ion, being the fluorescence intensity of sensor-L in excess of Ce³⁺ ion, and is the intensity noted at different concentrations of Ce³⁺ ion at 351 nm. The association constant was calculated graphically by plotting versus 1/[Ce³⁺]². A good liner relationship with slope () and intercept (1.399), respectively, were observed, confirming 2 : 1 binding stoichiometric ratio. The association constant (Ka) value was determined from the slope and intercept of the line as cited above and was found to be [30].

7.11. Effect of pH

In order to find out an appropriate pH for complexation of sensor L (5 μM) with Ce³⁺ (10 μM) pH analysis were conducted using NaOH and HCl solutions for pH adjustment (Figure 15S). Fluorescence intensity was monitored at 351 nm in the absence and presence of Ce³⁺ ion (10 μM) in the pH range 1-12. Upon change in pH of the test solution, change in fluorescence emission intensity of the complex was observed due to the presence of lone pairs of electrons on nitrogen and OH groups in sensor L. The fluorescence intensity of sensor L remained unaffected by varying the pH. On the other hand, the sensor L cerium complex showed a significant effect on its fluorescence emission intensity with change in pH. At low pH, the complex was found to be unstable and have low fluorescence emission intensity due to protonation of hydroxyl and amine moiety that acts as binding sites. With gradual increase of pH, drastic change in fluorescence emission intensity was observed. At pH 7, the complex was highly stable and maximum fluorescence emission intensity was observed. While at pH >7, a decrease in fluorescence emission intensity was observed due to Ce (OH)₃ formation thereby reducing the Ce³⁺ complex concentration. From these results, it can be deduced that sensor L can be employed at physiological pH range. The results obtained are in good agreement with respect to a comparative study performed on free sensor L [31].

7.12. Metal Ion Competition Study

Selectivity is one of the most important characteristics of a sensor, which is the relative response for the metal ion of interest over other competitive metal ions present in the samples. Therefore, to determine selectivity of sensor L toward Ce³⁺, 15 μM of sensor L and Ce³⁺ and 300 μM of other competitive metal ions were prepared in a acetonitrile/water mixture (2 : 8) and distilled water, respectively, and its fluorescence emission intensities at 351 nm were monitored. The result (Figure 4) shows that none of these metal ions interfere with Ce³⁺ ions showing high sensitivity and selectivity of sensor L with Ce³⁺ ions and can be successfully applied for Ce³⁺ ion determination in different water samples containing these competing metal ions [32].

7.13. Stability of Sensor L Solution

The stability of sensor L solution and its complex with cerium was determined up to 2 months by checking the fluorescence intensity at different intervals of time. The sensor L solution was stable up to 2 months as no change in fluorescence intensity was observed indicated in Figure 16S. The same stability was also observed for sensor L complex with cerium.

7.14. Comparison of Sensor L with Previous Works

Specific properties of the synthesized sensor L towards Ce³⁺ were compared with those of some previously reported sensors for Ce³⁺ determination (Table 3). Most of these sensors required arduous testing media that quenched fluorescence upon interaction with Ce³⁺. On the other hand, sensor L shows a number of attractive analytical features such as one-step easy synthesis, enhancement in fluorescence emission intensity, wide pH range, and its applications for rapid determination of Ce³⁺ in real water samples. The results obtained from the current study give ultra-high selectivity and sensitivity for the trace amount of Ce³⁺ ion determination as compared to other developed sensors [33].

7.15. Reversibility of Sensor L

The reversibility of sensor L was investigated using a common chelating agent ethylene diamine tetra acetic acid (EDTA). One equivalent of EDTA solution was added to a solution containing sensor L-Ce³⁺ complex. The fluorescence intensity was measured at 351 nm after EDTA interaction. The fluorescence emission signal was restored at 351 nm with the addition of EDTA thus showing that the process of chelation of sensor L with cerium is reversible as indicated in Figure 5.

7.16. Determination of Cerium in Different Water Samples

Application of the newly synthesized sensor L was assayed by analysing real water samples by collecting water samples from the outlet of our analytical Lab, Batkhela and Thana (areas located in Khyber Pakhtunkhwa, Pakistan). With a known concentration of Ce³⁺ (10-50 μM), all these samples were spiked, and its fluorescence emission intensity was noted at 351 nm as shown in Figure 6. The results showed that change in fluorescence intensity of L was directly proportional to Ce³⁺ ion concentration. Therefore, the sensor L could be applied for the determination of trace amount of Ce³⁺ ions in real water highlighting the applicability of sensor L in the control of environmental pollution with high sensitivity and selectivity [34].

8. Conclusion

In this study, a new fluorescent, sensor L for rapid, sensitive, and selective determination of Ce³⁺ in aqueous samples has been developed. The sensor was characterized by a number of instrumental techniques that confirmed the synthesis of sensor L and their sensing behavior toward Ce³⁺. The 2 : 1 stoichiometry of sensor L to Ce³⁺ was determined from Job’s plot based on UV-vis absorption and fluorescence analysis. Sensor L showed coordination with Ce³⁺ through the deprotonated phenolic group, azomethine nitrogen, and oxygen. Sensor L demonstrated high selectivity and ultrahigh sensitivity for Ce³⁺ among alkali, alkaline, and heavy and transition metals analysed, with limit of detection and association constant.

Data Availability

All the data associated with this research has been presented in this paper.

Conflicts of Interest

The authors declare that they have no conflicts of interest.

Acknowledgments

The authors extend their appreciation to the Deanship of Scientific Research at King Saud University for funding this work through research group no. RG-1440-009.

Supplementary Materials

CCDC No. 1987815 contains the supplementary crystallographic data for complex 1. These data can be obtained free of charge via http://www.ccdc.cam.ac.uk/conts/retrieving.html, or from the Cambridge Crystallographic Data Centre, 12 Union Road, Cambridge CB2 1EZ, UK; fax: (+44) 1223-336-033; or e-mail: [email protected]. (Supplementary Materials)

References

S. Elçin and H. Deligöz, “A versatile approach toward chemosensor for Hg2+ based on para-substituted phenylazocalix[4]arene containing mono ethyl ester unit,” Dyes and Pigments, vol. 107, article S0143720814001259, pp. 166–173, 2014.
View at: Publisher Site | Google Scholar
M. Jaishankar, T. Tseten, N. Anbalagan, B. B. Mathew, and K. N. Beeregowda, “Toxicity, mechanism and health effects of some heavy metals,” Interdisciplinary Toxicology, vol. 7, no. 2, pp. 60–72, 2015.
View at: Google Scholar
H. H. Haddad, “The effect of heavy metals cadimium, chromium and iron accumulation in human eyes,” American Journal of Analytical Chemistry, vol. 3, no. 10, pp. 710–713, 2012.
View at: Publisher Site | Google Scholar
D. Kar, P. Sur, S. K. Mandai, T. Saha, and R. K. Kole, “Assessment of heavy metal pollution in surface water,” International Journal of Environmental Science & Technology, vol. 5, no. 1, pp. 119–124, 2008.
View at: Publisher Site | Google Scholar
J. Dahle and Y. Arai, “Environmental geochemistry of cerium applications and toxicology of cerium oxide nanoparticles,” International Journal of Environmental Research and Public Health, vol. 12, no. 2, pp. 1253–1278, 2015.
View at: Publisher Site | Google Scholar
H. Moridi, S. A. Hosseini, H. Shateri et al., “Protective effect of cerium oxide nanoparticle on sperm quality and oxidative damage in malathioninduced testicular toxicity in rats,” International Journal of Reproductive Bio Medicine, vol. 16, pp. 261–266, 2018.
View at: Google Scholar
M. K. Rofouei, N. Tajarrod, M. Masteri-Farahani, and R. Zadmard, “A New fluorescence sensor for cerium (III) ion using glycine dithiocarbamate capped manganese doped ZnS quantum dots,” Journal of Fluorescence, vol. 25, no. 6, pp. 1855–1866, 2015.
View at: Publisher Site | Google Scholar
J. M. Dowding, T. Dosani, A. Kumar, S. Seal, and W. T. Self, “Cerium oxide nanoparticles scavenge nitric oxide radical (˙NO),” Chemical Communications, vol. 48, no. 40, pp. 4896–4898, 2012.
View at: Publisher Site | Google Scholar
R. Tang, K. Lei, K. Chen, H. Zhao, and J. Chen, “A rhodamine-based off–on fluorescent chemosensor for selectively sensing Cu(II) in aqueous solution,” Journal of Fluorescence, vol. 21, no. 1, pp. 141–148, 2011.
View at: Publisher Site | Google Scholar
G. C. Liu, X. Lu, X. W. Li et al., “Metal/carboxylate-induced versatile structures of nine 0D→ 3D complexes with different fluorescent and electrochemical behaviors,” ACS Omega, vol. 4, no. 17, pp. 17366–17378, 2019.
View at: Publisher Site | Google Scholar
T. Dai, Y.-Y. Huang, K. Sharma Sulbha, T. Hashmi Javad, B. Kurup Divya, and R. Hamblin Michael, “Topical antimicrobials for burn wound infections,” Recent patents on anti-infective drug discovery, vol. 5, no. 2, article 2, pp. 124–151, 2010.
View at: Publisher Site | Google Scholar
V. K. Gupta, A. K. Singh, M. R. Ganjali, P. Norouzi, F. Faridbod, and N. Mergu, “Comparative study of colorimetric sensors based on newly synthesized Schiff bases,” Sensors and Actuators B: Chemical, vol. 182, article S0925400513003432, pp. 642–651, 2013.
View at: Publisher Site | Google Scholar
T. A. Ali, A. L. Saber, G. G. Mohamed, and T. M. Bawazeer, “Determination of Cr (III) ions in different water samples using chromium (III)-sensor based on N-[4-(dimethylamino) benzylidene]-6-nitro-1, 3-benzothiazol-2-amine,” International Journal Electrochemical Science, vol. 9, no. 9, pp. 4932–4943, 2014.
View at: Google Scholar
C. Li, J. Qin, B. Wang, L. Fan, J. Yan, and Z. Yang, “A chromone-derived schiff-base ligand as Al³⁺ “Turn on” fluorescent Sensor: synthesis and spectroscopic properties,” Journal of Fluorescence, vol. 26, no. 1, pp. 345–353, 2016.
View at: Publisher Site | Google Scholar
A. Xavier and N. Srividhya, “Synthesis and study of schiff base ligands,” Journal of Applied Chemistry, vol. 7, 15 pages, 2014.
View at: Google Scholar
N. Mohamed, S. E. Ibrahim, and A. Sharif, “Synthesis, characterization and use of schiff bases as fluorimetric analytical reagents,” European Journal of Chemistry, vol. 4, pp. 531–535, 2007.
View at: Publisher Site | Google Scholar
Y. Tianzhi, Z. Kai, Z. Yuling et al., “Synthesis, crystal structure and photoluminescent properties of an aromatic bridged Schiff base ligand and its zinc complex,” Inorganic Chimica Acta, vol. 361, no. 1, pp. 233–240, 2018.
View at: Publisher Site | Google Scholar
S. Alghool, H. F. Abd el-Halim, M. S. Abd el-sadek, I. S. Yahia, and L. A. Wahab, “Synthesis, thermal characterization, and antimicrobial activity of lanthanum, cerium, and thorium complexes of amino acid Schiff base ligand,” Journal of Thermal Analysis and Calorimetry, vol. 112, no. 2, pp. 671–681, 2013.
View at: Publisher Site | Google Scholar
Jenisha, S. Theodore David, and J. P. Priyadharsini, “Schiff base ligand its complexes and their FTIR spectroscopy studies,” International Journal on Applied Bioengineering, vol. 9, no. 1, pp. 1–4, 2015.
View at: Publisher Site | Google Scholar
S. Jenisha, T. David, and B. Priyad, “Cd and Cu complexes of polydentate schiff base ligands: synthesis, characterization, properties and biological activity,” Journal of Bioscience and Bioengineering, vol. 9, pp. 135–145, 2015.
View at: Google Scholar
A. Golcu, T. Mehmet, H. Demirelli, and R. Alan, “A short history of SHELXL,” Inorganica Chemica Acta, vol. 8, pp. 1785–1797, 2015.
View at: Google Scholar
G. M. Sheldrick, “Publ CIF software for editing, validating and formatting crystallographic information files,” Acta Crystallographica Section A, vol. 4, pp. 112–122, 2013.
View at: Google Scholar
S. P. Westrip, “Synthesis of some Schiff base metal complexes involving para substituted aromatic aldehydes and glycylglycine spectral, electrochemical, thermal and surface morphology studies,” Journal of Molecular Structure, vol. 5, pp. 920–925, 2010.
View at: Google Scholar
D. Arish, M. Sivasankaran, and K. Nair, “Poly (1-amino-5-chloroanthraquinone): Highly selective and ultrasensitive fluorescent chemosensor For Ferric Ion,” Journal of Molecular Structure, vol. 8, pp. 112–121, 2016.
View at: Google Scholar
S. Devaraj and M. Kandaswamy, “Fluorescent chemosensing properties of new isoindoline based-receptors towards F^- and Cu²⁺ ions,” Optics and Photonics Journal, vol. 3, no. 1, pp. 32–39, 2013.
View at: Publisher Site | Google Scholar
Z. Zhao, L. Sheng, C. Su, K. Tao, and W. Jing, “Coumarin-based fluorescent probes for dual recognition of copper (II) and iron (III) ions and their application in bio-imaging,” Sensors, vol. 4, pp. 1145–1152, 2017.
View at: Google Scholar
G. B. Olimpo, K. Bruce, P. Claudio et al., “Coumarin-based fluorescent probes for dual recognition of copper (II) and iron (III) ions and their application in bio-imaging,” Sensors, vol. 14, no. 1, pp. 1358–1371, 2014.
View at: Google Scholar
X. Q. He, Q. Y. Lin, R. D. Hu, and X. H. Lu, “Synthesis, characterization and DNA-binding studies on La(III) and Ce(III) complexes containing ligand of N-phenyl-2-pyridinecarboxamide,” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 68, no. 1, article S1386142506006780, pp. 184–190, 2007.
View at: Publisher Site | Google Scholar
El-Wahab, Z. H. Abd, M. M. Mashaly, and A. A. Faheim, “Synthesis and characterization of Cobalt (II), Cerium (III) and dioxouranium (VI) complexes of 2, 3-dimethyl-1-phenyl-4-salicylidene-3-pyrazoline-5-one mixed ligand complexes, pyrolytic products and biological activities,” Chemical Papers, vol. 59, pp. 25–36, 2005.
View at: Google Scholar
K. Songzi, W. N. Seong, S. Wahhida, and M. H. Lee, “A new carbazole-based schiff-base as fluorescent chemosensor for selective detection of Fe³⁺ and Cu²,” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 13, pp. 1173–1178, 2009.
View at: Google Scholar
W.-K. Dong, S. F. Akogun, Y. Zhang, Y.-X. Sun, and X.-Y. Dong, “A reversible “turn-on” fluorescent sensor for selective detection of Zn2+,” Sensors and Actuators B: Chemical, vol. 238, article S0925400516310826, pp. 723–734, 2017.
View at: Publisher Site | Google Scholar
Z. Zhiyuan, S. Chunming, L. Aifeng, Z. Zhenyu, and Z. Dongmei, “Highly selective detection of Cr in water matrix by a simple 1, 8-naphthalene based turn on fluorescent sensor,” Journal of Fluorescence, vol. 5, pp. 335–340, 2015.
View at: Google Scholar
M. N. Gueye, M. Dieng, I. E. Thiam et al., “Lanthanide (III) complexes with tridentate Schiff base ligand, antioxidant activity and X-ray crystal structures of the Nd (III) and Sm (III) complexes,” South African Journal of Chemistry, vol. 70, pp. 8–15, 2017.
View at: Publisher Site | Google Scholar
S. Chahmana, S. Keraghel, F. Benghanem, R. Rosas, A. Ourari, and E. Morallón, “Synthesis, spectroscopic characterization, electrochemical properties and biological activity of 1-[(4Hydroxyanilino)- methylidene] naphthalen-2(1H)-one and its Mn (III) Complex,” International Journal of Electrochemical Science, vol. 13, pp. 175–195, 2018.
View at: Publisher Site | Google Scholar
X. Wang, M. Iqbal, and W. Huskens, “Turn-on fluorescent chemosensor for Hg²⁺ Based on multivalent rhodamine ligands,” International Journal of Molecular Sciences, vol. 13, no. 12, pp. 16822–16832, 2012.
View at: Publisher Site | Google Scholar
C. I. C. Esteves, M. M. M. Raposo, and S. P. G. Costa, “Novel highly emissive non-proteinogenic amino acids: synthesis of 1, 3, 4-thiadiazolyl asparagines and evaluation as fluorimetric chemosensors for biologically relevant transition metal cations,” Amino Acids, vol. 40, no. 4, pp. 1065–1075, 2011.
View at: Publisher Site | Google Scholar
Z. Lizhu, W. Jingyun, F. Jiangli, G. Kexing, and P. Xiaojun, “A highly selective, fluorescent chemosensor for bioimaging of Fe³⁺,” Bioorganic and Medicinal Chemistry Letters, vol. 21, no. 18, pp. 5413–5416, 2011.
View at: Publisher Site | Google Scholar
E. Elshehy, S. A. EL-Safty, and M. A. Shenashen, “Reproducible design for the optical screening and sensing of Hg (II) ions,” Chemosensors, vol. 2, no. 4, pp. 219–234, 2014.
View at: Publisher Site | Google Scholar

Copyright

Copyright © 2020 Maria Sadia et al. 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

2031

Downloads

1160

Citations

Journal of Sensors

Schiff-Based Fluorescent-ON Sensor L Synthesis and Its Application for Selective Determination of Cerium in Aqueous Media

Abstract

1. Introduction

2. Experimental

3. Synthesis of [1-((Pyrimidine-4-ylimino)methyl)-napthalene-2-ol]

4. Solution Preparation for Spectroscopic Measurement

5. UV-Visible Analysis

6. Metal Ion Binding Study by Fluorescence Titration

7. Results and Discussions

7.1. IR Data

7.2. Characterization by 1H-NMR

7.3. Characterization by X-Ray Diffraction

7.4. UV-vis Absorption Spectroscopic Analysis

7.5. Fluorescence Studies

7.6. Preliminary Study

7.7. Effect of Time

7.8. Effect of Solvents

7.9. Determination of Detection Limit

7.10. Association Constant and Binding Stoichiometry

7.11. Effect of pH

7.12. Metal Ion Competition Study

7.13. Stability of Sensor L Solution

7.14. Comparison of Sensor L with Previous Works

7.15. Reversibility of Sensor L

7.16. Determination of Cerium in Different Water Samples

8. Conclusion

Data Availability

Conflicts of Interest

Acknowledgments

Supplementary Materials

References

Copyright

7.2. Characterization by ¹H-NMR