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Article

Pyridinyl Conjugate of UiO-66-NH2 as Chemosensor for the Sequential Detection of Iron and Pyrophosphate Ion in Aqueous Media

by
Aasif Helal
1,*,
Md. Eyasin Arafat
1 and
Mohammad Mizanur Rahman
2
1
Center of Research Excellence in Nanotechnology, King Fahd University of Petroleum and Minerals, Dhahran 31261, Saudi Arabia
2
Center of Research Excellence in Corrosion, King Fahd University of Petroleum and Minerals, Dhahran 31261, Saudi Arabia
*
Author to whom correspondence should be addressed.
Chemosensors 2020, 8(4), 122; https://doi.org/10.3390/chemosensors8040122
Submission received: 7 October 2020 / Revised: 21 November 2020 / Accepted: 23 November 2020 / Published: 30 November 2020
(This article belongs to the Section Optical Chemical Sensors)
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Abstract

:
A new chemosensor UiO-66-N-Py (Py = 2-methinepyridine, N = imine nitrogen) based on isoreticular UiO-66 (University of Oslo) Metal–Organic Framework (MOF) containing 2-methinepyridine functionalized organic linker was solvothermally synthesized and characterized. This UiO-66-N-Py was very selective and sensitive for detecting the Fe3+ ion and sequential detection of the pyrophosphate (PPi) anion. The limits of detection for the Fe3+ ion and PPi were calculated to be 10 ppb (0.19 μM) and 50 ppb (0.3 μM), respectively. The quenching constant Ksv for Fe3+ and the binding constant for PPi were 1.4 × 105 M−1 and 1.7 × 105 M−1, respectively. The functionalization of UiO-66-NH2 with 2-methinepyridine enhanced its fluorescence emission properties and introduced more binding sites for the analytes. We additionally studied the interaction of the sensor and the analytes with Fourier-transform infrared spectroscopy (FTIR), X-ray photoelectron spectroscopy (XPS), and Inductively Coupled Plasma Mass Spectrometry (ICP-MS). This chemosensor also demonstrated a regenerative emission property without loss in the detection ability for six consecutive cycles.

1. Introduction

The selective sensing of heavy and transitional metals has attracted immense interest due to their considerably important structural, regulatory, and catalytic role in different biological systems. Among them, iron is vital, as it plays a very significant role in biological systems such as oxygen transport, synthesis of DNA and RNA, hemoglobin formation, and brain and muscle function [1,2,3]. A deficiency of iron can lead to various biological disorders such as skin alignment, insomnia, anemia, and endotoxemia [4,5]. Moreover, due to the acceleration in industrialization, a lot of iron ion has been emitted in the environment, which is consumed by the human body through edible materials. Thus, iron overload can lead to hepatic cirrhosis, hereditary hemochromatosis leading to neuroinflammation, diabetes, heart failure, and Alzheimer’s disease progression [6,7,8]. This has prompted the development of different methods for detecting Fe3+ ion, such as inductively coupled plasma atomic emission spectrometry, spectrophotometry, atomic absorption spectrophotometry, and electrochemical methods [9]. However, these traditional methods are expensive, less selective, complicated, time consuming, and less sensitive.
Pyrophosphate (PPi) is the dimeric form of the inorganic phosphate and an essential by-product of ATP’s cellular hydrolysis. The concentration of PPi in the cellular system helps us to detect a large number of diseases [10]. The amount of PPi in the cell acts as an indicator of cancer research [11]. A high concentration of PPi is detected in patients with calcium pyrophosphate dihydrate crystal deposition disease (CPPD) [12]. Detection of the PPi has additionally been used for the real-time DNA sequencing. Thus, the detection and imaging of PPi are of vital importance in the case of human beings. Compared to the conventional detection methods for both the ions, fluorescence chemosensors offer a more straightforward and economical method with immense accuracy, sensitivity, and selectivity for the ions’ online monitoring.
Metal–Organic Frameworks (MOFs) are extended crystalline structures with high, tunable porosity and surface area that have been widely used for the capture and storage of different gases such as hydrogen, carbon dioxide, and methane [13,14]. Fluorescent chemosensors based on luminescent MOFs have been extensively used for the highly sensitive detection of analytes. The extensive surface area and open avenues in the MOFs allow the fast diffusion of specific analytes for highly sensitive fluorescence detection. These pore environments can be easily tuned using functionalized linkers that provide highly accessible interactional sites and enclosed environments for the highly selective recognition of specific analytes [15,16]. Moreover, the MOF’s profound crystalline nature helps understand the host–guest interaction within the MOF and the mechanism of fluorescence [17]. The high oxidation state of Zirconium (IV) leads to enhanced charge density and bond polarization. That results in a robust metal–ligand bond in all the Zirconium-based MOFs leading to high thermal and chemical stability [18,19]. Moreover, the organic linker (benzene ring) of the UiO-66 can be readily derivatized without disturbing the crystalline structure, the thermal property, or the chemical property of the MOF. This particular characteristic of UiO-66 makes it appropriate for different post and pre synthetic modifications. The primary fluorescence in the UiO-66-NH2 arises from the linker, but due to the zirconium clusters’ presence, the emission of the linker is quenched. So, the amino group can be derivatized with different heteroaromatic groups to produce strong emission and strong binding moieties [20,21].
This paper reports the synthesis and characterization of a pyridinyl imine appended UiO-66-NH2 MOF (UiO-66-N-Py) (Figure 1) and its application in the sequential detection of cation and anion in the aqueous media. A pyridine-imine appended 2-aminoterephthalic acid linker (H2L) was used to prepare UiO-66-N-Py by the hydrothermal method. Then, the newly synthesized MOF was characterized with powdered XRD, surface area analysis (BET), FTIR, SEM, thermogravimetric analysis (TGA), and the digestion NMR. The fluorescence emission studies with different cations showed that the MOF was highly selective for Fe3+, leading to the complete quenching of the fluorescence. Then, this Fe3+-incorporated UiO-66-N-Py was used in the same aqueous media for the sequential detection of pyrophosphate anion.

2. Experimental

2.1. Materials and General Methods

2.1.1. Chemicals Used in this Work

First, 2 aminoterephthalic acid (98% purity), 2-pyridinecarboxaldehyde (99% purity), methanol (99.9% purity), ethanol (97.2% purity), N,N-dimethylformamide (DMF; 99.8% purity), dichloromethane (99.8% extra dry grade), all other nitrates or chlorides of the metal salts, and the tetrabutylammonium or potassium salts of the anions were purchased from Sigma Aldrich (USA) Corporation. NMR solvents: dimethyl sulfoxide-d6 (DMSO-d6; 99.9% purity) were purchased from Cambridge Isotope. All chemicals were used without further purification. Water used in this work was double distilled and filtered through a Millipore membrane. The solutions of metal ions were prepared from their nitrate, and chloride salts and anions were prepared from their tetrabutylammonium or potassium salts (analytical grade) followed by subsequent dilution of the working solutions.

2.1.2. Instrumentation

1H and 13C NMR spectra were recorded on a Bruker AM-400 spectrometer (Billerica, MA, USA) using Me4Si as the internal standard. Elemental microanalyses (EA) were performed using a PerkinElmer-EA 2400 elemental analyzer (Waltham, MA, USA). Powdered X-ray diffraction patterns of the samples were recorded using a Rigaku MiniFlex diffractometer (Tokyo, Japan), which was equipped with Cu-Kα radiation. The data were acquired over the 2θ range of 5° and 30°. The FTIR spectra of UiO-66-N-Py were obtained using a Nicolet 6700 Thermo Scientific instrument (Waltham, MA, USA) in the range of 400–4000 cm−1, using KBr. Thermogravimetric analysis (TGA) of the samples were performed using a TA Q500. In this study, an activated UiO-66-N-Py (10 mg) sample was heated in an alumina pan under airflow (60 mL min−1) with a gradient of 10 °C min−1 in the temperature range of 30–800 °C. The BET surface areas of the MOFs were calculated by using Micromeritics ASAP 2020 instrument (Norcross, GA, USA). These materials’ surface morphology was discerned using a field emission scanning electron microscope (FESEM, LYRA 3 Dual Beam, Tescan), which operated at 30 kV. The FESEM samples were prepared from suspension in ethanol. The surface chemical analyses were performed using an XPS equipped with an Al-Kα micro-focusing X-ray monochromator (ESCALAB 250Xi XPS Microprobe, Thermo Scientific, Waltham, MA, USA). Inductively Coupled Plasma Mass Spectrometry (ICP-MS) of the iron ion-treated samples of UiO-66-N-Py were carried in Thermo Scientific X Series 2 ICP-MS. The absorption spectra of the MOF were studied using a Jasco V-670 spectrophotometer (Tokyo, Japan). Fluorescence spectra were measured using a Jasco, FP-8500ST fluorescence spectrophotometer, which was equipped with a xenon discharge lamp and 1 cm quartz cells with slit width 2 nm for both the source and the detector. The quantum yield and chromaticity studies were done using an integration sphere (Jasco FP-8500ST) by using a liquid sample holder at room temperature. The excitation wavelength used in the absolute emission quantum yield measurement is 340 nm, which does not interfere with the emission spectrum, and the concentration is adjusted so that the optical density is 0.1 at the excitation wavelength.

2.1.3. Sample Preparation for Photophysical Studies

In a typical luminescence-sensing experimental setup, 1 mg of UiO-66-N-Py powder was dispersed in 1 mL of water. In a 1 cm quartz cuvette, 3 mL of dispersed aqueous solution of UiO-66-N-Py was placed, and the absorption and emission responses were measured in situ after an incremental addition of freshly prepared analyte solutions. The mixtures were sonicated for 5 min after each incremental addition of the analytes for uniform dispersion during the luminescent measurements. All of the measurements were performed at 298 K. All the optical sensing experiments were carried out using 10−2 M aqueous solution of the analyte salt.

2.2. Synthesis

2.2.1. Synthesis of the Linker

The synthesis of the Linker is shown in Scheme 1.

2.2.2. Synthesis of Compound H2L

To a solution of 2-aminoterephthalic acid (500 mg, 2.8 mmol) in ethanol (10 mL), 2-pyridinecarboxaldehyde (450 mg, 4.2 mmol) was added and refluxed for 6 h. The reaction mixture was cooled down, and the precipitate was filtered and washed with ethanol to give H2L as yellow solid in 91% yield. 1H NMR (DMSO-d6) δ7.22–7.31 (m, 3H), 7.51 (s, 1H), 7.65 (d, J = 7.6 Hz, 1H), 7.76 (d, J = 8.4 Hz, 1H), 7.93 (d, J = 3.2 Hz, 1H), 8.82 (s, 1H); 13C NMR (DMSO-d6) δ108.35, 110.44, 113.03, 113.39, 115.30, 118.09, 125.07, 127.28, 130.99, 132.26, 147.04, 156.57, 162.96, 164.94; Anal. Calcd for C14H10N2O4: C, 62.22; H, 3.73; N, 10.37; Found: C, 62.18; H, 3.66; N, 10.30 (Figures S1 and S2, in Supplementary Materials).

2.2.3. UiO-66-NH2

UiO-66-NH2 was synthesized by dissolving ZrCl4 (250 mg, 1.08 mmol) and 2-amino-1,4-benzenedicarboxylic acid (268 mg, 1.5 mmol) in DMF (40 mL) with ultrasonic vibration for 30 min; then, 0.3 mL of acetic acid was added. The as-obtained mixture was transferred to a 50 mL vial and heated at 393 K for 24 h. Then, the vial was cooled in the air to room temperature. The resulting UiO-66-NH2 was washed three times with DMF (5–10 mL) using a centrifuge (10,000 rpm for 30 min), and then sequentially immersed in methanol (5–10 mL three times per day) for three 24 h periods. Finally, UiO-66-NH2 was activated by removing the solvent under vacuum for 24 h at 100 °C. FTIR (KBr, cm−1): 3429, 1663, 1569, 1437, 1382, 1258, and 1094 (Figure S3, Supplementary Materials). Anal. Calcd for C54H52N8O36Zr6 (Zr6O4(OH)4(2-NH2BDC)6(DMF)2(H2O)2): C, 33.49; H, 2.71; N, 5.79; Zr, 28.27; Found: C, 33.61; H, 2.99; N, 6.05; Zr, 28.54.

2.2.4. UiO-66-N-Py

UiO-66-N-Py was synthesized in a similar way as above by dissolving ZrCl4 (250 mg, 1.08 mmol) and H2L (405 mg, 1.5 mmol) in DMF (20 mL) with ultrasonic vibration for 30 min; then, 0.3 mL of acetic acid was added. The as-obtained mixture was transferred to a 50 mL vial and heated at 393 K for 24 h. Then, the vial was cooled in the air to room temperature. The resulting UiO-66-N-Py was washed in the same way as the previous method by three times with DMF (5–10 mL) using a centrifuge (10,000 rpm for 30 min) and then sequentially immersed in methanol (5–10 mL three times per day) for three 24 h periods. Finally, UiO-66-N-Py was activated by removing the solvent under vacuum for 24 h at 110 °C. FTIR (KBr, cm−1): 3093, 1671, 1596, 1521, 1408, 1295, 1227, 1160, and 851 (Figure S3, Supplementary Materials). Anal. Calcd for C90H70N14O36Zr6 (Zr6O4(OH)4(2-N-Py-BDC)6(DMF)2(H2O)2): C, 43.75; H, 2.86; N, 7.94; Zr, 22.15; Found: C, 43.91; H, 2.56; N, 8.17; Zr, 22.55.

3. Results and Discussion

3.1. Characterization of H2L

In a covalent post-synthetic modification (PSM), there are chances that all the linkers are not completely functionalized within the MOF framework; hence, in this paper, we presynthetically modified the linker 2 amino-terephthalic acid with 2-pyridinylcarboxyaldehyde to give the imine conjugate H2L (Scheme 1). The structure of H2L was confirmed with 1H NMR, 13C NMR, (Figures S1 and S2, in Supplementary Materials), and elemental analysis data. The 1H NMR spectra of H2L exhibited a singlet peak at 8.82 ppm, which corresponds to the imine (–CH=) proton, and another doublet peak was noticed at 7.93 ppm that is assigned to the proton adjacent to the nitrogen of the pyridine ring.

3.2. Characterization of UiO-66-N-Py and UiO-66-NH2

The powdered XRD of UiO-66-NH2 was consistent with that reported in the literature (Figure 2) [18]. The high crystalline nature and the peaks of UiO-66-N-Py at 2θ = 7.78°, 8.92° (Figure 2) were found to be consistent with the characteristic peaks of UiO-66-NH2. This establishes that appending 2-aminoterephthalic acid with 2-pyridinylcarboxyaldehyde does not disrupt the framework and connectivity present in UiO-66-NH2.
In the IR spectrum of UiO-66-N-Py, the peaks at 1408 cm−1 and 1295 cm−1 correspond to the carbon–nitrogen bond’s vibration in the 2-aminoterephthalate. Similarly, the peaks at 1671 cm−1 and 1521 cm−1 are assigned to the −COO asymmetrical and symmetrical stretching. The presence of the imine bond in UiO-66-N-Py exhibits a sharp enhanced peak at 1596 cm−1 with the disappearance of the N-H stretching peak, which is found in UiO-66-NH2 at the 3429 cm−1 (Figure S3, in Supplementary Materials).
The alkaline digestion 1H NMR of UiO-66-N-Py confirmed the presence of the linker H2L in the framework. The 1H NMR spectrum obtained after the digestion of UiO-66-N-Py has peaks at the chemical shifts analogous to H2L (Figure S1, in Supplementary Materials).
The N2 adsorption isotherm of UiO-66-N-Py indicated Type I behavior with a sharp uptake at a very low relative pressure (P/P0) of 0 to 0.05, which signifies its microporous nature similar to the UiO-66-NH2. From the isotherm of UiO-66-N-Py, the BET surface area and pore volume were found to be 573 m2g−1 and 0.381 cm3g−1, respectively, which is diminished significantly from the pristine UiO-66-NH2 (BET surface area = 1032 m2g−1 pore volume = 0.517 cm3g−1) due to the presence of the functionalized pyridine moieties (Figure 3). Furthermore, the DFT adsorption pore-size distribution affirmed a pore diameter of 10.2 Å for UiO-66-N-Py, which is much more reduced than the UiO-66-NH2 (11.5 Å), indicating the presence of conjugated pyridine groups (Figure S4, in Supplementary Materials).
The thermogravimetric analysis (TGA) was used to study the thermal stability of UiO-66-N-Py and UiO-66-NH2 materials under an airflow with a heating rate of 5 °C min−1 (Figure 4).
Both the materials show analogous thermal behavior with an initial mass loss of 5.0% between 200 and 250 °C due to the removal of the trapped solvents molecules from the framework’s pores. The maximum weight loss in UiO-66-N-Py is 64.5% at a temperature of 375 °C, indicating the decomposition of the framework. In UiO-66-NH2, the maximum weight loss of 56.4% occurs at a temperature of 410 °C. It signifies that UiO-66-NH2 and UiO-66-N-Py are stable up to 375 °C and 410 °C, respectively. The remaining residue of 30.5% for UiO-66-N-Py and 38.6% for UiO-66-NH2 corresponds to zirconium oxide. Thus, the TGA of the materials illustrates that functionalization with 2-pyridinecarboxaldehyde does not affect the stability of the MOF. The thermal stability of UiO-66-N-Py has also been confirmed by powdered XRD (Figure S5, in Supplementary Materials).
The SEM study of UiO-66-N-Py confirmed that it has uniformly distributed bipyramidal morphology with the particle size ranging from 130 to 150 nm (Figure S6, in Supplementary Materials).

3.3. Optical Properties of UiO-66-N-Py

The photophysical properties of UiO-66-N-Py were investigated as emulsion in an aqueous medium. The comparative absorption spectroscopy of all the linkers, UiO-66-NH2, and UiO-66-N-Py, indicates that conjugation with pyridine redshifts the absorption peak of UiO-66-NH2 from 360 to 370 nm in UiO-66-N-Py (Figure S7, in Supplementary Materials). In general, 2-aminoterphthalate is luminescent, but in case of UiO-66-NH2 (λem = 449 nm), due to coordination with the Zr-O clusters, ligand-to-metal charge transfer (LMCT) takes place, and the luminescence is abated [20]. However, in case of UiO-66-N-Py, the emission peak appears at 485 nm on excitation at 341 nm wavelength (Figure S8, in Supplementary Materials). Thus, an enhanced 36 nm redshift in the emission peak of UiO-66-N-Py is produced due to the pyridine ring’s conjugation to the 2-aminobenzene ring of the main framework of UiO-66-NH2. Furthermore, the pyridine group’s nitrogen and the imine bond contribute selective binding sites for transitional metal ions. The absolute quantum yield of UiO-66-N-Py, which was calculated from the integrated sphere, was found to be 0.43. The CIE coordinates obtained from the chromaticity diagram were commensurate with the experimentally derived emission peak values (Figure S9, in Supplementary Materials).

3.4. Cation Sensing Properties of UiO-66-N-Py

The cation sensing properties of UiO-66-N-Py were studied by screening with various cations, and the transition in their photophysical properties was noted. It was observed that on the addition of different cations to the aqueous solution of the UiO-66-N-Py, only the Fe3+ ion produce a change in the absorbance of UiO-66-N-Py (Figure S10, in Supplementary Materials). On the gradual addition of Fe3+ ion to a suspension of UiO-66-N-Py, the absorbance peak at 370 nm diminishes with the formation of a new peak at 315 nm and isobestic point 341 nm (Figure S11, in Supplementary Materials). This formation of a new peak at 315 nm indicates the coordination of the Fe3+ with the imine N and the nitrogen of the pyridine. The stoichiometric ratio of binding between the Fe3+ and UiO-66-N-Py was validated by Job’s plot, which indicated that the complexation between Fe3+ and UiO-66-N-Py has a 1:1 stoichiometric ratio (Figure S12, in Supplementary Materials) [22,23].
The chemosensing behavior of UiO-66-N-Py was interpreted by studying the change in fluorescence emission of this MOF with an increasing concentration of Fe3+ at an excitation wavelength of 341 nm. The fluorescence emission was significantly quenched with the increasing concentration of Fe3+, and a complete quenching was accomplished when the molar ratio of UiO-66-N-Py: Fe3+ was 1:1 (Figure 5). This quenching of emission indicates that complete complexation has occurred between the Fe3+, imine linkage, and the pyridine moiety. Fe3+ being paramagnetic impedes the intramolecular charge transfer from the pyridine ring to the benzene ring of the main structural framework of UiO-66 (Scheme 2), leading to the complete emission suppression. The quenching efficiency indicated by the Stern–Volmer constant (Ksv), which is calculated from the fluorescence titration experiment shown in Figure 5, was found to be 1.4 × 105 M−1 (Figure S13, in Supplementary Materials) [24].
The sensitivity of UiO-66-N-Py for Fe3+ was established from the limit of detection, which was calculated to be 10 ppb (0.19 μM) by the ratio of 3σ/k (Section S6, Table S1, and Figure S24, in Supplementary Materials). The selectivity and the tolerance of UiO-66-N-Py for Fe3+ as compared to other metal pollutants was examined by immersion of the MOF into aqueous solution of various metal ions (e.g., Fe2+, Fe3+, Co2+, Cu2+, Ni2+, Zn2+, Cd2+, Hg2+, Ag+, Pd2+, Al3+, Ga3+, Pb2+ Na+, K+, Ca2+, Mg2+, Sr2+, Rb2+, and Cs2+) (Figure 6, and Figure S14 in Supplementary Materials). It was observed that complete emission suppression occurs only in the case of Fe3+ due to its paramagnetic nature, and proximity of the pyridine nitrogen with the imine group helps in selective binding of the Fe3+ as compared to the other cations [25]. PXRD of UiO-66-N-Py bounded with Fe3+ indicated that the framework’s crystallinity is not disturbed (Figure 2). Competitive binding experiments with 200 μL of various metal ions along with 200 μL of Fe3+ was performed, and it showed that complete quenching of UiO-66-N-Py by Fe3+ was not hindered by any of the metal ions (Figure S15, in Supplementary Materials).
The complexation of Fe3+ with UiO-66-N-Py was further confirmed by ICP, FTIR, and the XPS studies of the washed and dried samples. The ICP analysis of the sample confirmed Fe along with the metal of the MOF framework. It was analyzed that 11.891 mg of Fe3+ was obtained per 100 mg of the zirconium. The FTIR study of the UiO-66-N-Py samples collected after the sensing experiments provided us essential insight into the nature of the complexation between the guest (Fe3+) and the host framework. The Fe3+ ion’s complexation with the pyridine nitrogen of UiO-66-N-Py is depicted by the change of the –C=N– stretching vibration from 1296 to 1282 cm−1. The Fe3+ ion also interacts with the imine linkage of UiO-66-N-Py, which is mirrored by the change in –C=N– stretching vibration from 1595 to 1583 cm−1 (Figure S16, in Supplementary Materials). In addition, the interaction with Fe3+ changes the pyridine’s C-H vibration from 3100 to 3067 cm−1 (Figure S17, in Supplementary Materials). The XPS of the pristine MOF sample and after complexation with the Fe3+ were also analyzed. It was observed that both the MOF indicates the characteristic peaks for C, N, and Zr at 283, 398, and 181 eV, respectively. In UiO-66-N-Py and the Fe3+ complex, we can detect peaks for iron at 712 and 726 eV, which emphasized the complexation of UiO-66-N-Py with Fe3+ (Figure S18, in Supplementary Materials).

3.5. Anion Sensing Properties of UiO-66-N-Py

It has already been reported that many metal complexes have an affinity toward selective anions such as Ni-CN, Al-F, or Cu-S [26,27,28,29,30]. Thus, we also tried to check the selectivity of different anions F−, Cl−, Br−, I−, CH3COO−, NO3−, SO42−, HSO4−, PO43−, ATP, ADP, MnO4−, CrO42−, Cr2O72−, and PPi toward the complex of UiO-66-N-Py + Fe3+ (Figure 7). Upon the addition of aqueous solution (10−2 M) of each anion, there was no change in the emission of UiO-66-N-Py + Fe3+ complex except in the case of PPi, where the emission peak of the pristine UiO-66-N-Py was restored at the 485 nm at an excitation wavelength of 341 nm (Figure S19, in Supplementary Materials). The absorbance study also shows that the peak at 315 nm due to Fe3+ complexation gradually reduces, and the peak of UiO-66-N-Py is restored at 370 nm (Figure S20, in Supplementary Materials).
Fluorescence titration of the UiO-66-N-Py + Fe3+ complex with the incremental addition of PPi resulted in the enhancement of the emission at 485 nm (Figure 8), with a binding constant of 1.7 × 105 M−1 (Figure S21, in Supplementary Materials). The limit of detection for PPi calculated from the ratio 3σ/k was estimated to be 50 ppb (0.3 μM) (Section S6, Table S1, and Figure S25 in Supplementary Materials). Job’s method, obtained from the fluorescence emission, established that the stoichiometry of binding of PPi with UiO-66-N-Py + Fe3+ is 1:1 (Figure S22, in Supplementary Materials). To delve into the possibility of using UiO-66-N-Py + Fe3+ for the practical detection of PPi, competitive binding experiments with different anions (10−2 M) in the presence of PPi were carried out. This study showed that the fluorescence enhancement of UiO-66-N-Py + Fe3+ by PPi was not interfered by any of the anions (Figure S23, in Supplementary Materials). The FTIR data also show that the interaction of UiO-66-N-Py + Fe3+ with PPi shifts the peak of imine stretching and C-H vibration of pyridine from 3067 to 3100 cm−1 (Figures S16 and S17, in Supplementary Materials). An efficient chemosensor for successful practical applications should be effective in aqueous media within a broad pH range. The fluorescence emission of UiO-66-N-Py remained impervious within a pH range of 4.0–8.0 (Figure S26, in Supplementary Materials), even after its regeneration with PPi. Beyond this range, the fluorescence emission properties were lost, which was probably due to breaking the imine linkage or destruction of the UiO-66-N-Py framework.
The fluorescent enhancement mechanism was due to the release of Fe3+ from the UiO-66-N-Py + Fe3+ complex by the metal–MOF displacement method by PPi (Scheme 2) [31,32,33]. This was confirmed by the restoration of the emission peak of the pristine UiO-66-N-Py at 485 nm after interaction with PPi. The PXRD data also confirmed that the crystallinity of the UiO-66-N-Py is intact after the interaction with the PPi (Figure 2).
For this sensor’s practical application, a fluorescence test paper was prepared for the portable and straightforward optical sensing of Fe3+. A filter paper of the size 4.0 × 2.0 cm2 was immersed in an emulsion of UiO-66-N-Py and water and then dried to get the test paper. As shown in Figure 9, the test paper containing UiO-66-N-Py produces a blue fluorescence that can be seen with the naked eye when placed under UV light irradiation of 365 nm (Figure 9A).
When this test paper is immersed in Fe3+ solution and then irradiated by UV light of 365 nm, the fluorescence is completely quenched (Figure 9B). After further immersion of the same quenched test paper into a PPi solution, the blue fluorescence emission is restored (Figure 9C).

3.6. Reusable Properties of UiO-66-N-Py

The recyclable sensing ability of UiO-66-N-Py was measured by repeating the fluorescence sensing experiments with Fe3+ and PPi sequentially. The material obtained after the first experiment was washed with water and methanol and then dried at 110 °C for 5 h. The recovered UiO-66-N-Py showed an identical change in the emission intensities and sensitivities toward the detection of analytes for six consecutive cycles (Figure 10).

4. Conclusions

In summary, we synthesized an isoreticular MOF UiO-66-N-Py by using a pyridine appended new linker H2L. This presynthetic incorporation of pyridine moiety through imine linkage enhanced the MOF’s intrinsic emission property and introduced additional coordinating sites for selective and sensitive binding of Fe3+. All the experimental data highlight that UiO-66-N-Py can be used to detect Fe3+ ion and the sequential detection of PPi with high efficiency, sensitivity, and selectivity. The detection limits for Fe3+ ion and PPi were found to be 10 ppb and 50 ppb, respectively. We investigated the nature of the interaction between the analytes and the functionalized linker of the framework. We also discovered that UiO-66-N-Py has good recyclability for six consecutive cycles without decreasing its sensing performance. Further work related to the sensing of Fe3+ in wastewater and the biological application of this sensor is currently being carried out in our lab.

Supplementary Materials

The following are available online at https://www.mdpi.com/2227-9040/8/4/122/s1, Figure S1. 1H NMR spectrum of H2L in DMSO-d6 solution at 400 MHz, Figure S2. 13C NMR spectrum of H2L in DMSO-d6 solution at 400 MHz, Figure S3. FTIR spectra of UiO-66-N-Py and UiO-66-NH2, Figure S4. DFT adsorption pore-size distribution of UiO-66-N-Py and UiO-66-NH2, Figure S5. Thermal stability of UiO-66-N-Py at different temperatures, Figure S6. SEM image of UiO-66-N-Py, Figure S7. UV-vis spectra of UiO-66-N-Py, UiO-66-NH2, linkers, and FeCl3 in water, Figure S8. The fluorescence emission spectra of UiO-66-NH2 and UiO-66-N-Py. (λex = 341 nm), Figure S9. Chromaticity diagram of UiO-66-N-Py dispersion in water, Figure S10. Change in the normalized absorbance of UiO-66-N-Py at 315 in water upon addition of 200 μL of different metal cations (10−2 M), Figure S11. Changes in UV-vis spectra of UiO-66-N-Py with the incremental addition of FeCl3 (10−2 M) in water, Figure S12. Job’s plot for UiO-66-N-Py with FeCl3 in water, Figure S13. Stern-Volmer plot of UiO-66-N-Py quenched by FeCl3 in water, Figure S14. Changes in emission spectra of UiO-66-N-Py upon addition of 200 μL of different metal cations (10−2 M) in water. (λex = 341 nm), Figure S15. Competitive metal ion selectivity of UiO-66-N-Py: Bars indicate the fluorescence intensity (341 nm excitation, 485 nm emission). Salts of various metal ions (10−2 M) were added to UiO-66-N-Py and Fe3+ (10−2 M) (a) UiO-66-N-Py only, (b) Ag+ + Fe3+, (c) Pb2+ + Fe3+, (d) Zn2+ + Fe3+, (e) Mg2+ + Fe3+, (f) Fe3+ + Cu2+, (g) K+ + Fe3+, (h) Co2+ + Fe3+, (i) Al3+ + Fe3+, (j) Fe2+ + Fe3+, (k) Na+ + Fe3+, (l) Cd2+ + Fe3+, (m) Sr2+ + Fe3+, (n) Rb+ + Fe3+, (o) Pd2+ + Fe3+ (p) Ni2+ + Fe3+, (q) Hg2+ + Fe3+, (r) Ga3+ + Fe3+, (s) Cs+ + Fe3+, (t) Ca2+ + Fe3+ in water., Figure S16. Part of FTIR spectra for UiO-66-N-Py before and after sensing experiments with Fe3+, Figure S17. Part of FTIR spectra for UiO-66-N-Py before and after sensing experiments with Fe3+ and PPi, Figure S18. XPS of UiO-66-N-Py and UiO-66-N-Py + Fe3+, Figure S19. Changes in emission spectra of UiO-66-N-Py − Fe3+ upon addition of 200 μL of different anionic species (10−2 M) in water. (λex = 341 nm), Figure S20. Changes in UV-vis spectra of UiO-66-N-Py + Fe3+ with the incremental addition of PPi (10−2 M) in water, Figure S21. Binding constant calculation of UiO-66-N-Py + Fe3+ with PPi in water, Figure S22. Job’s plot for UiO-66-N-Py + Fe3+ with PPi in water, Figure S23. Competitive anion selectivity of UiO-66-N-Py + Fe3+: Bars indicate the fluorescence intensity (341 nm excitation, 485 nm emission). Various anions (10−2 M) were added to UiO-66-N-Py + Fe3+and PPi (10−2 M) (a) UiO-66-N-Py + Fe3+ only, (b) F− + PPi, (c) Cl− + PPi, (d) Br− + PPi, (e) I− + PPi, (f) CH3CO2− + PPi, (g) MnO4− + PPi, (h) NO32− + PPi, (i) PO42− + PPi, (j) SO42− + PPi, (k) HSO4− + PPi, (l) Cr2O72− + PPi, (m) CrO42− + PPi, (n) ADP + PPi, (o) ATP + PPi in water, Figure S24. Linear region of fluorescence intensity (λx = 341 nm and λem = 485 nm) for UiO-66-N-Py suspensions in water upon incremental addition of Fe3+ solutions, Figure S25. Linear region of fluorescence intensity (λex = 341 nm and λem = 485 nm) for UiO-66-N-Py+Fe3+ suspensions in water upon incremental addition of PPi solutions, Table S1. Calculation of the Limit of Detection (LOD), Figure S26. Effect of pH on the emission intensities at 485 nm of UiO-66-N-Py, in H2O (λex = 341 nm).

Author Contributions

Conceptualization, A.H.; methodology, A.H.; formal analysis, A.H., M.E.A., and M.M.R.; investigation, A.H., M.E.A., and M.M.R.; resources, A.H., M.E.A., and M.M.R.; data curation, A.H., and M.E.A.; writing—original draft preparation, A.H.; writing—review and editing, A.H., and M.M.R.; visualization, A.H. and M.M.R.; supervision, A.H.; project administration, A.H.; funding acquisition, A.H. All authors have read and agreed to the published version of the manuscript.

Funding

This research was supported by King Abdulaziz City for Science and Technology—National Science, Technology, and Innovation Plan (NSTIP No. 15-NAN4601-04).

Acknowledgments

We acknowledge King Abdulaziz City for Science and Technology—National Science, Technology, and Innovation Plan (NSTIP No. 15-NAN4601-04) for supporting this research.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Schematic representation of UiO-66-NH2 and UiO-66-N-Py.
Figure 1. Schematic representation of UiO-66-NH2 and UiO-66-N-Py.
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Scheme 1. Synthesis of the linker H2L.
Scheme 1. Synthesis of the linker H2L.
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Figure 2. Powered XRD patterns of UiO-66-NH2 obtained from cif file, UiO-66-NH2 as synthesized, UiO-66-N-Py as synthesized, UiO-66-N-Py after addition of iron, and UiO-66-N-Py + Fe3+ after addition of pyrophosphate (PPi).
Figure 2. Powered XRD patterns of UiO-66-NH2 obtained from cif file, UiO-66-NH2 as synthesized, UiO-66-N-Py as synthesized, UiO-66-N-Py after addition of iron, and UiO-66-N-Py + Fe3+ after addition of pyrophosphate (PPi).
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Figure 3. N2 adsorption isotherms of UiO-66-N-Py and UiO-66-NH2. The filled and open circles represent the adsorption and desorption branches, respectively.
Figure 3. N2 adsorption isotherms of UiO-66-N-Py and UiO-66-NH2. The filled and open circles represent the adsorption and desorption branches, respectively.
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Figure 4. Thermogravimetric analysis (TGA) of UiO-66-N-Py and UiO-66-NH2.
Figure 4. Thermogravimetric analysis (TGA) of UiO-66-N-Py and UiO-66-NH2.
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Figure 5. Changes in fluorescence emission spectra of UiO-66-N-Py with the incremental addition of FeCl3 (10−2 M) in water (λexe = 341 nm). Inset: Fluorogenic changes in UiO-66-N-Py upon addition of Fe3+ in water upon illumination at 365 nm.
Figure 5. Changes in fluorescence emission spectra of UiO-66-N-Py with the incremental addition of FeCl3 (10−2 M) in water (λexe = 341 nm). Inset: Fluorogenic changes in UiO-66-N-Py upon addition of Fe3+ in water upon illumination at 365 nm.
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Scheme 2. Schematic illustration of the mechanism of sequential detection of Fe3+ and PPi by UiO-66-N-Py.
Scheme 2. Schematic illustration of the mechanism of sequential detection of Fe3+ and PPi by UiO-66-N-Py.
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Figure 6. Change in the normalized fluorescence emission of UiO-66-N-Py in water upon the addition of 200 μL of different metal cations (10−2 M).
Figure 6. Change in the normalized fluorescence emission of UiO-66-N-Py in water upon the addition of 200 μL of different metal cations (10−2 M).
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Figure 7. Change in the normalized fluorescence emission of UiO-66-N-Py + Fe3+ in water upon addition of 200 μL of different anionic species (10−2 M).
Figure 7. Change in the normalized fluorescence emission of UiO-66-N-Py + Fe3+ in water upon addition of 200 μL of different anionic species (10−2 M).
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Figure 8. Changes in fluorescence emission spectra of UiO-66-N-Py + Fe3+ with the incremental addition of PPi (10−2 M) in water (λexe = 341 nm).
Figure 8. Changes in fluorescence emission spectra of UiO-66-N-Py + Fe3+ with the incremental addition of PPi (10−2 M) in water (λexe = 341 nm).
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Figure 9. Luminescence picture of the UiO-66-N-Py test paper: (A) UiO-66-N-Py, (B) UiO-66-N-Py + Fe3+ (10−2 M), (C) UiO-66-N-Py + Fe3+ + PPi under UV-light irradiation of 365 nm.
Figure 9. Luminescence picture of the UiO-66-N-Py test paper: (A) UiO-66-N-Py, (B) UiO-66-N-Py + Fe3+ (10−2 M), (C) UiO-66-N-Py + Fe3+ + PPi under UV-light irradiation of 365 nm.
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Figure 10. Bar diagram depicting the recyclability of UiO-66-N-Py, fluorescence quenching with UiO-66-N-Py + Fe3+, regeneration of fluorescence with UiO-66-N-Py + Fe3+ + PPi up to 6 cycles.
Figure 10. Bar diagram depicting the recyclability of UiO-66-N-Py, fluorescence quenching with UiO-66-N-Py + Fe3+, regeneration of fluorescence with UiO-66-N-Py + Fe3+ + PPi up to 6 cycles.
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Helal, A.; Arafat, M.E.; Rahman, M.M. Pyridinyl Conjugate of UiO-66-NH2 as Chemosensor for the Sequential Detection of Iron and Pyrophosphate Ion in Aqueous Media. Chemosensors 2020, 8, 122. https://doi.org/10.3390/chemosensors8040122

AMA Style

Helal A, Arafat ME, Rahman MM. Pyridinyl Conjugate of UiO-66-NH2 as Chemosensor for the Sequential Detection of Iron and Pyrophosphate Ion in Aqueous Media. Chemosensors. 2020; 8(4):122. https://doi.org/10.3390/chemosensors8040122

Chicago/Turabian Style

Helal, Aasif, Md. Eyasin Arafat, and Mohammad Mizanur Rahman. 2020. "Pyridinyl Conjugate of UiO-66-NH2 as Chemosensor for the Sequential Detection of Iron and Pyrophosphate Ion in Aqueous Media" Chemosensors 8, no. 4: 122. https://doi.org/10.3390/chemosensors8040122

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