Charge-Enhanced Separation of Organic Pollutants in Water by Anionic Covalent Organic Frameworks.

The effective removal of organic pollutants in wastewater is a key environmental challenge. In this work, an anionic covalent organic framework (named TpPa-SO3Na) was synthesized through a green two-in-one synthesis strategy with autocatalytic imine formation. The slowly generated acetic acid as a catalyst is favorable to sustain the reversibility of the covalent organic framework (COF) formation reaction and improve the crystallinity of TpPa-SO3Na. TpPa-SO3Na consists of a homogeneous distribution of sulfonate groups to produce negatively charged regular channels. The strong electrostatic and hydrogen-bonding interactions between the sulfonate groups anchored in the nanochannels and the amine groups in organic pollutants improve the adsorption selectivity and capacity. These structures allow a high degree of control over adsorption processes to boost the adsorption kinetics and improve selective separation. TpPa-SO3Na exhibits ultrafast adsorption (<1 min) of cationic antibiotics and dyes (average over 95%). Furthermore, TpPa-SO3Na exhibits high selectivity for the uptake of dye molecules on the basis of the differences in charge and molecular size. This work explored functional designs and green manufacturing of anionic COFs for removal of hydrophilic organic pollutants.

Introduction

With the development of the chemical industry, water resources are seriously contaminated by organic pollutants such as antibiotics and synthetic dyes.[1,2] Illegal discharges of antibiotics increased bioaccumulation,[3,4] and dyes might even transform into n class="Disease">carcinogenic and mutagenic agents.[5,6] Adsorption is an effective technique to remove organic pollutants from water owing to its excellent separation efficiency and reusability.[7]

To achieve high adsorption capacity, rapid kinetics, and outstanding selectivity, many functional materials have been designed to combat highly n class="Chemical">water-soluble antibiotic and artificial dye pollution.[7] A series of conventional materials have been developed as adsorbents, such as silica and clay.[8] Nonetheless, only organic pollutants interact mainly with the surface of adsorbents due to their lack of pore structures, limiting adsorption capacity.[7] Because of their high surface area, porous organic polymers offer enhanced adsorption efficiency compared to conventional materials.[9] Though the correlation between surface area and adsorption capacity is often documented, the inner surfaces of open-ended polymers were found to be partially ineffective due to the irregular pore structures and lack of functional groups, compromising binding capacity.[7]

Metal–organic frameworks (MOFs) were used to mitigate this problem due to added functional groups and uniform pore structures, which facilitate the interaction between n class="Chemical">adsorbents and targeted organic pollutants.[10] However, MOFs with a relative density of functional groups and interpenetrating channels greatly affected site accessibility, thus resulting in a low adsorption affinity and a relatively long adsorption equilibrium time.[7,11] Therefore, it is highly desirable to develop new types of materials to overcome these limitations.

Covalent organic frameworks (COFs) are a new type of porous crystalline material that integrate organic building blocks into predetermined nanometric networks.[12] The functionalization of n class="Chemical">COFs with specific functional groups on the organic building blocks can efficiently tune their adsorption properties. In two-dimensional (2D) COFs, the layered structures stack via π–π interactions and form regular channels running along the stacking direction. Thus, the functional groups can be uniformly distributed on the surface, and the density of functional groups can be precisely controlled.[13] Anionic COFs, which consist of negatively charged active sites and well-ordered one-dimensional (1D) nanochannels, are a subtype of COF with extraordinary functions.[14] However, the introduction of ionic sites on the pore walls needs ionic building blocks, which prevents π–π stacks because of strong charge repulsion, usually leading to low porosity and crystallinity.[15] Homogeneous negatively charged groups in the channels would generate a strong interaction for cationic organic pollutants, improving the binding capacity.[16,17] Compared with polymers and MOFs, well-defined hydrophilic 1D channels of COFs are favorable for the diffusion of highly water-soluble antibiotics and artificial dyes, increasing the access of pollutants to the surface of channels.[7,13] Negatively charged 1D nanochannels will generate ionic interfaces to enhance the accessibility of the anionic sites, allowing high adsorption kinetics and selective adsorption.[17] These traits suggest that anionic COFs can be pertinently designed for highly efficient removal of hydrophilic antibiotics and artificial dyes.

In this study, a two-in-one strategy was developed for the synthesis of sulfonate-based covalent organic frameworks (denoted as n class="Chemical">TpPa-SO3Na) for trapping antibiotics and synthetic dyes. Sulfonates were homogeneously introduced onto the surface of 2D COFs. The negatively charged site can provide strong electrostatic and hydrogen-bonding affinity, which can promote the interaction between cationic pollutants and the anionic sites. Hydrophilic channels are favorable for the diffusion of water-soluble pollutants. Meanwhile, the ionic interface on the 1D channel walls helps to expose the active sulfonate sites and promotes adsorption efficiency and selectivity. TpPa-SO3Na shows ultrafast adsorption kinetics with high removal efficiency (99.0%) in 1 min toward antibiotics such as norfloxacin (NOR). Owing to its charged nanochannels, TpPa-SO3Na exhibits high selectivity to separate cationic dye molecules owing to the differences in molecular size and charge. These results reveal the broad application of the anionic COF to the treatment of organic pollutants.

Results and Discussion

Synthesis and Characterization

The anionic COF was prepared by condensing n class="Chemical">aldehydes and amines at an elevated temperature in a mixture of organic solvents and aqueous acetic acid. Acetic acid was used to catalyze imine formation.[13] The obtained COF was reacted with an organic salt to exchange its protons with metal ions.[18] A tedious preparation process, long reaction time, and strong acid solution are necessary in the entire COF formation reaction. A relatively high concentration of acid in the reaction can damage the reversible reaction of diamines on the linkers, resulting in irregular nanochannels.[19] However, the networks transform into crystalline COFs, and this transformation would be hindered if acetic acid is not present.[20] As mentioned earlier, the COF was controlled using different amounts of AcOH.[21] The slowly generated acetic acid was favorable to sustain the COF formation reaction and improve crystallinity.[13] In our work, a two-in-one synthesis strategy was used for the synthesis of TpPa-SO3Na as illustrated in Figure . First, the sulfone acid group of Pa-SO3H reacted with NaOAc to exchange its proton with Na+. The slowly generated acetic acid catalyzed imine formation without additional catalysts,[22] which ensured a low concentration of acid catalyst in the synthetic process. The low concentration of acetic acid pushed the equilibrium toward COF formation and slowed down the entire reaction, improving self-healing and error correction during the crystallization[19] Meanwhile, the two-in-one synthesis strategy was used for the synthesis of anionic TpPa-SO3Na, avoiding the traditional synthesis procedures that are time- and solvent-consuming. Thus, the dual role of NaOAc is very intriguing as both an ion exchanger and a catalyst in the reaction. The cation exchange reaction was quantitatively confirmed by the inductively coupled plasma optical emission spectroscopy (ICP-OES) measurement of the Na content (7.32 wt % (calcd) and 7.25 wt % (found), Table S1). The sulfonate groups in TpPa-SO3Na work as anionic sites for efficient adsorption of cationic antibiotics and artificial dyes, which also provide sites for charge-assisted hydrogen bonds to further improve the affinity.

Figure 1

(a) Preparation scheme of TpPa-SO3Na and TpPa; (b) graphic view of the eclipsed AA stacking structure of TpPa-SO3Na (top view); and (c) stacking model showing individual layers (side view) (blue, N; red, O; yellow, S; purple, Na; gray, C; white, H).

(a) Preparation scheme of TpPa-SO3Na and n class="Chemical">TpPa; (b) graphic view of the eclipsed AA stacking structure of TpPa-SO3Na (top view); and (c) stacking model showing individual layers (side view) (blue, N; red, O; yellow, S; purple, Na; gray, C; white, H).

The structure of TpPa-SO3Na was analyzed based on the powder X-ray diffraction (PXRD) pattern (Figure a). The highly prominent PXRD peak at 4.8° can be attributed to the {100} facet of a regularly ordered lattice, which is arranged in a hexagonal orientation.[23,24] The sharp diffraction peaks indicate the successful formation of the n class="Chemical">imine-linked COF, and the acetic acid formed in the two-in-one step reaction is an effective catalyst for the COF. Noticeably, the slowly generated acetic acid is favorable to sustain the reversibility of the COF formation reaction and improve the crystallinity of TpPa-SO3Na (Figure S1). Additionally, the broad peak at 27.0° assigned to the {001} facet further confirms the formation of 2D COFs in a crystalline and π–π stacking form.[24,25] Intramolecular hydrogen bonds between the sulfonate units and imine group on the frame can avoid disturbing the π–π stacking between the sheets, forming a highly crystalline structure.[26] The PXRD profile obtained from the Pawley refinement of the AA stacking mode (Figure a, red curve) agrees well with the experimental result. The average interplanar distance was estimated to be 3.4 Å. The AA-stacking mode provides 1D channel, allowing adjacent alignment of sulfonate. This spatial structure efficiently boosted the accessibility of the anionic sites by cationic pollutants.[17,18] Based on the facts presented above, superior anionic COFs have been synthesized using the two-in-one synthesis strategy. The method also has the advantages of simplified operation and green environmental protection.

Figure 2

(a) Comparison of PXRD profiles of TpPa-SO3Na between the experimental sample (black), the simulated AA eclipsed stacking modes (red), and the simulated AB staggered stacking modes; (b) Fourier-transform infrared spectroscopy (FTIR) spectra of Tp (black), Pa-SO3H (red), and TpPa-SO3Na (blue); (c) pore size distribution of TpPa-SO3Na; and (d) stability tests of TpPa-SO3Na in 6 M NaOH, 6 M HCl, and boiling water.

(a) Comparison of PXRD profiles of TpPa-SO3Na between the experimental sample (black), the simulated AA eclipsed stacking modes (red), and the simulated AB staggered stacking modes; (b) Fourier-transform infrared spectroscopy (FTIR) spectra of n class="Chemical">Tp (black), Pa-SO3H (red), and TpPa-SO3Na (blue); (c) pore size distribution of TpPa-SO3Na; and (d) stability tests of TpPa-SO3Na in 6 M NaOH, 6 M HCl, and boiling water.

The typical FTIR spectra of TpPa-SO3Na are shown in Figure b. The keto tautomer is confirmed by the presence of a new C=C peak at 1576 cm–1 and the absence of C=n class="Chemical">N stretching peaks (1620 cm–1).[27] The aromatic C=C peak appears at 1438 cm–1, and the newly formed C–N bonds of the keto tautomer in the COF appear at 1231 cm–1.[24,27] The formation of the −SO3– unit is further verified by the peak at 1005 cm–1.[22] The Brunauer–Emmett–Teller (BET) surface area for TpPa-SO3Na is 236 m2 g–1 (Figure S2). Because of the high surface-to-volume ratio of the COF and internal sulfonate groups, the surface charges may generate abundant adsorption sites for charged organic compounds and enhance the adsorption capacity and affinity. The pore diameter is concentrated at ∼15.2 Å (Figure c), and the narrow pore size reflects the successful preparation of the crystalline network.[28] Owing to the presence of the narrow nanochannels, the internal sulfonate groups can easily interact with amine groups of antibiotics and artificial dyes.[17] SEM images of TpPa-SO3Na are shown in Figure S3. The material exhibits a nanofiber morphology. The SEM image with a 2 μm scale plate shows a randomly shaped aggregate composed of many macroscopic fibers.

Stability Test

To investigate the stability of TpPa-SO3Na, samples were dispersed in different solutions, including n class="Chemical">NaOH (6 M) and aqueous HCl (6 M) and boiling water solutions for 7 days. Surprisingly, all of the TpPa-SO3Na samples exhibited intense PXRD patterns without a change in the peak position and intensity, indicating that the high stability is retained under these extreme conditions (Figure d). Compared with traditional imine-linked COFs,[13] irreversible enol-to-keto tautomerization and the hydrogen-bonding interaction can further enhance the chemical stability.[29,30] The thermogravimetric analysis (TGA) curves exhibit two weight losses in the studied temperature range. The initial weight loss was caused by the removal of the occluded solvent molecules at 50–120 °C, and the second weight loss was derived from the decomposition of the sulfonate groups at 300 °C (Figure S4). This suggested that the obtained COF exhibits superior stability,[23] which is important for its practical applications.

Adsorption Kinetics

Taking into account the porosity and high density of sulfonate sites within the ordered pore channels in n class="Chemical">TpPa-SO3Na, its adsorption performance toward the positively charged amine group of antibiotics and artificial dyes was further investigated. The effects of adsorbent dosage on the removal efficiency were investigated. As shown in Figure S5, it can be seen that the removal efficiency increases with the increase of TpPa-SO3Na dose as a result of increased available adsorption active sites and surface area. Taking the adsorption efficiency and cost into consideration, the optimum dosage of TpPa-SO3Na was used in the subsequent investigations. Typically, TpPa-SO3Na was mixed with pollutant solutions at 10 mg L–1 under pH 7.0. As shown in Figure a, TpPa-SO3Na showed ultrafast adsorption kinetics, and it efficiently removed most of the pollutants such as NOR (∼99%), ciprofloxacin (CIP) (∼98%), enrofloxacin (ENR) (∼98%), tetracycline hydrochloride (TC) (∼91%), methylene blue (MB) (∼96%), and crystal violet (CV) (∼89%) within 1 min. It is worth noting that almost 90% of its maximum adsorption capacity was reached within 30 s. This suggests that TpPa-SO3Na has excellent affinity toward the antibiotics and dyes. The adsorption kinetics studies show that the adsorption process fits well with the pseudo-second-order model (Figure b), confirming that the interactions between TpPa-SO3Na and pollutants are mainly controlled by chemical processes. The pseudo-second-order rate constants (kobs) of NOR, CIP, ENR, TC, MB, and CV adsorption are 4.78, 3.53, 3.37, 1.64, 2.18, and 1.08 g mg–1 min–1, respectively (Figure S6). NOR was selected as one of the representative pollutants. The removal rate constant is higher than those of most reported porous pollutant removers (Table S2). Compared to inorganic porous materials such as clays and zeolites with low inherent porosity[8] and amorphous organic porous polymers with an irregular pore structure, COFs are desirable materials that provide a specific pore structure and interactions according to the contaminant of choice.[13] The excellent removal rate constant should be attributed to TpPa-SO3Na containing nanochannels and compact sulfonate sites, significantly improving the accessibility to these cationic pollutants rather than the amorphous activated carbon with an uneven pore distribution and undefined functional groups.[31] The 1D nanochannel with ionic interfaces in TpPa-SO3Na is favorable for diffusion of the antibiotics and dyes compared with the self-interpenetrated nanochannel of MOFs.[7] The ultrafast adsorption kinetics is the key to remarkably reduce the exposure time, especially under extreme conditions, improving the configurable preservation during sewage disposal.

Figure 3

(a) Adsorption kinetics of TpPa-SO3Na toward different organic pollutants (initial concentration was 10 mg L–1; the dosage of TpPa-SO3Na was 0.6 g L–1 (for NOR, CIP, and ENR), 0.8 g L–1 (for MB and CV), and 1.0 g L–1 (for TC); solution volume 100 mL; and pH 7.0). (b) Pseudo-second-order kinetics of adsorption of different organic pollutants. (c) Adsorption isotherms for different organic pollutants on TpPa-SO3Na (initial concentration was 10, 20, 30, 50, 100, 200, 300, and 500 mg L–1; the dosage of TpPa-SO3Na was 0.6 g L–1 (for NOR, CIP, and ENR), 0.8 g L–1 (for MB and CV), and 1.0 g L–1 (for TC); solution volume 40 mL; and pH 7.0). (d) Removal efficiency and ζ-potential of TpPa-SO3Na toward NOR at different pH conditions.

(a) Adsorption kinetics of TpPa-SO3Na toward different organic pollutants (initial concentration was 10 mg L–1; the dosage of n class="Chemical">TpPa-SO3Na was 0.6 g L–1 (for NOR, CIP, and ENR), 0.8 g L–1 (for MB and CV), and 1.0 g L–1 (for TC); solution volume 100 mL; and pH 7.0). (b) Pseudo-second-order kinetics of adsorption of different organic pollutants. (c) Adsorption isotherms for different organic pollutants on TpPa-SO3Na (initial concentration was 10, 20, 30, 50, 100, 200, 300, and 500 mg L–1; the dosage of TpPa-SO3Na was 0.6 g L–1 (for NOR, CIP, and ENR), 0.8 g L–1 (for MB and CV), and 1.0 g L–1 (for TC); solution volume 40 mL; and pH 7.0). (d) Removal efficiency and ζ-potential of TpPa-SO3Na toward NOR at different pH conditions.

Adsorption Isotherms

The adsorption isotherms of TpPa-SO3Na fitted well with the Langmuir model (Figure c and Table S3) with a correlation coefficient R2 of greater than 0.99, suggesting that the uniform and monolayer adsorption isotherm model is more propitious to the adsorption of n class="Chemical">NOR. It is worth noting that 2D COFs tend to form uniform and controllable 1D nanochannels by the suitable stacking of monolayers.[17] The monolayer adsorption model is consistent with the structural characteristics of stacking of monolayers. The distribution coefficient value (Kd) can be applied to further evaluate the interaction between adsorbents and pollutants. Generally, a material with a Kd value of more than 104 mL g–1 can be regarded as an excellent adsorbent.[32] The Kd of TpPa-SO3Na toward NOR is 1.7 × 107 mL g–1 in 10 min (Table S4). The saturation sorption capacity toward NOR was 653 mg g–1 at room temperature (Table S3), higher than those of other reported adsorbents (Table S2). The self-adsorption behavior was also tested under dark conditions. Spectroscopic monitoring of NOR solution at different intervals indicated that the concentration of NOR did not exhibit any noticeable change under dark conditions. It is suggested that the self-adsorption behaviors did not significantly impact the adsorption process of NOR on TpPa-SO3Na (Figure S7). Its excellent adsorption capacity is mainly attributed to the strong affinity interaction between antibiotics and the sulfonate groups of TpPa-SO3Na. In addition, the sufficiently long 1D nanochannels provide more active sites.[33]

Effect of pH and Reusability

The capture of antibiotics and dyes over a wide pH range is greatly needed for actual sewage treatments. The effect of pH on the adsorption capacity toward NOR was researched from pH 1 to 12 (Figure d). The adsorption efficiencies of n class="Chemical">TpPa-SO3Na toward NOR were over 90% within a wide pH range of 3–10. Meanwhile, the ζ-potentials of TpPa-SO3Na at different pH values were also measured (Figure d). As shown in Figure d, when pH <6.30, the adsorption capacity of NOR increases with the increase of pH value. The cationic NOR is mainly formed in the solution in this pH range (Figure S8a,b); therefore, the increase in adsorption capacity is attributed to the sharp increase in the negative potential of TpPa-SO3Na. In the range of 6.30 < pH < 8.38, the increase in the negative potential of TpPa-SO3Na slows down, while the content of anionic NOR increases gradually with pH. The adsorption capacity reaches the highest value at pH about 7.0. When pH > 8.38, anionic NOR as the main form exists in the solution (Figure S8a,b). Compared with the expected result,[34] increased adsorption of NOR was obtained in spite of an unfavorable electrostatic interaction in the range. Hydrogen bonding may be one of the potential mechanisms for enhanced adsorption of NOR. The N–H group of NOR is considered to be able to serve as a very strong hydrogen donor for hydrogen bonds. Therefore, NOR can interact efficiently via hydrogen bonds with adsorbents having a hydrogen acceptor.[26] As TpPa-SO3Na has ultrafast adsorption kinetics, a long-time adsorption and desorption experiment was implemented to determine the stability of TpPa-SO3Na. After being treated with NOR solutions for 12 h, the desorption of NOR from TpPa-SO3Na was studied using an HCl solution (0.1 M). No obvious decrease in the adsorption capacity of TpPa-SO3Na for NOR (100 mg L–1) was observed even after five adsorption–desorption cycles (Figure S9). The PXRD result also showed that there was no change in the peak pattern after five cycles of reuse compared with the fresh one (Figure S10). Furthermore, all of the characteristic FTIR peaks remained the same after recycling, and no extra peaks were observed (Figure S11). These excellent properties endow TpPa-SO3Na with great capability in the removal of antibiotics and artificial dyes.

Adsorption Mechanism

The adsorption property of 2D COFs is actuated by “horror vacui” and guided by the diffusion and accessibility of the pores.[35] The nanochannel diameter of n class="Chemical">TpPa-SO3Na is concentrated at 15.2 Å, which is large enough to allow entry of NOR inside the nanopore and its interaction with the sulfonate groups.[36,37] To further verify the possibility of entering the pore during adsorption, N2 sorption measurements at 77 K after NOR adsorption were made. The experiment results showed a decrease in surface area to 49 m2 g–1, corresponding to a drop of 80%, which could indicate that NOR is adsorbed within the pores of TpPa-SO3Na (Figure S12). The ζ-potential of TpPa-SO3Na is negative at pH 1–12 owing to the abundant sulfonate groups.[11,38] The negatively charged surface of TpPa-SO3Na helped in capturing the positively charged antibiotics and artificial dyes. Coupled with the pore structure, the adsorption kinetics and capacity are also influenced by surface charge.[39] TpPa-SO3Na shows a high negative ζ-potential (−22.2 mV) before NOR adsorption, suggesting that it prefers to adsorb cationic NOR. The ζ-potential of the NOR-loaded adsorbents was also tested (Figure S13). The results indicate an improvement in the ζ-potential. The adsorption of cationic NOR was promoted by electrostatic attraction. Negatively charged groups may act in concert with pore size to facilitate adsorption of cationic NOR into the channels of TpPa-SO3Na. The typical FTIR spectra of TpPa-SO3Na before and after adsorption of NOR are shown in Figure S14. The characteristic peaks for N–O at 1101 cm–1 and the S–O stretching vibration at 1024 cm–1 shifted to 1026 cm–1 are attributed to the occurrence of the strong reaction between sulfonate and amine.[24] This interaction was further confirmed by X-ray photoelectron spectroscopy (XPS). The spectra of N 1s XPS analysis are consistent with the presence of the electrostatic attraction process as the new peak of N–O (401.9 eV) appeared in TpPa-SO3Na-NOR (Figure a,b). Moreover, the O 1s core level of S–O (533.1 eV) shifted to a higher binding energy (533.5 eV) (Figure c,d), corroborating the results obtained from the XPS of N 1s. The sulfonate groups are aligned on the nanochannel’s internal surface, and the open nanochannel effectively exposes the active sites, increasing the accessibility to NOR and enhancing the adsorption efficiency toward NOR.[17,18] Integration of anionic sites into the nanochannel has generated anionic interfaces to accelerate the diffusion of charged NOR in the direction of the channel.[40,41]

Figure 4

N 1s of TpPa-SO3Na (a) and TpPa-SO3Na-NOR (b) and O 1s of TpPa-SO3Na (c) and TpPa-SO3Na-NOR (d).

N 1s of TpPa-SO3Na (a) and n class="Chemical">TpPa-SO3Na-NOR (b) and O 1s of TpPa-SO3Na (c) and TpPa-SO3Na-NOR (d).

Nanochannels of 2D COFs can offer efficient pathways for the transport of ions and molecules. With decreasing size, the interfacial wettability within nanochannels plays a significant role in the efficient transportation of various molecules.[42,43] Modulating n class="Chemical">hydrogen bonding is a powerful strategy to increase the interior wettability of nanochannels.[44,45]Figure S14 shows the FTIR spectra of TpPa-SO3Na before and after adsorption of NOR. The characteristic peak at 1237 cm–1 may be attributed to the symmetric stretching vibration of O=S. Following the adsorption of NOR, the peak at 1237 cm–1 shifted up to 1232 cm–1, which signified that a hydrogen-bonding interaction occurred between N-H and O=S. This interaction was further confirmed by XPS. The O 1s core level of S=O...H...N (532.6 eV) shifted to a lower binding energy (532.3 eV),[26] verifying that the sulfonate sites were the binding sites toward the amine group in NOR by charge-assisted hydrogen-bonding attraction (Figure c,d).[23,24] To further confirm the hydrogen-bonding interaction, NOR was added to TpPa-SO3Na in the presence of 6 M carbamide (Figure a).[46] The adsorption capacity toward NOR significantly declined with the addition of carbamides in the pollutant solution. The disruptive effect of carbamide further confirms the hydrogen-bonding mechanism. This shows that negative charge-assisted and enhanced H-bonding attraction makes the hydrophilic nanochannels robust. With the hydrophilic modification of nanochannels, the wettability of the material was effectively improved, facilitating diffusion in the direction of the channel.[38,42]

Figure 5

(a) Competitive adsorption of NOR and carbamide on TpPa-SO3Na (initial concentration was 50 mg L–1; carbamide 6M; TpPa-SO3Na 0.6 g L–1; and pH 7.0). (b) adsorption kinetics of TpPa-SO3Na and TpPa toward NOR (initial concentration was 10 mg L–1; COF 0.6 g L–1; and pH 7.0).

(a) Competitive adsorption of NOR and n class="Chemical">carbamide on TpPa-SO3Na (initial concentration was 50 mg L–1; carbamide 6M; TpPa-SO3Na 0.6 g L–1; and pH 7.0). (b) adsorption kinetics of TpPa-SO3Na and TpPa toward NOR (initial concentration was 10 mg L–1; COF 0.6 g L–1; and pH 7.0).

In addition, to investigate the role of charges in the adsorption, 4-nitrophenol (n class="Chemical">4-NP) containing only a hydrogen donor (hydroxyl) was tested. As demonstrated in Figure S15, 4-NP was hardly adsorbed by TpPa-SO3Na, which showed as low as 2% of adsorption efficiency even after 2 h, implying that the individual hydrogen-bonding effect was not as dominant as expected in the adsorption process because of the lack of charged binding sites. The synergetic electrostatic interaction and charge-assisted hydrogen bonds strongly enhance the binding ability between TpPa-SO3Na and NOR.

To get a better idea of the effect of 1D negatively charged nanochannels in NOR removal, the n class="Chemical">TpPa COF without the sulfonate group was prepared for comparison (Figure S16).[29] Similarly, 10 mg of TpPa COF was immersed in 20 mL of NOR solution (10 mg L–1), and we could find that only 1% of NOR were absorbed, suggesting that the absence of sulfonate sites in the network led to the poor NOR uptake efficiency (Figure b). TpPa-SO3Na with uniform 1D negatively charged channels exhibited a higher adsorption efficiency than the TpPa COF. The above results show that the negatively charged nanochannels are indispensable for fast and efficient positively charged organic pollutant adsorption from water.[17,42]

On the basis of these FTIR, XPS, and confirmatory adsorption experiments, a possible adsorption mechanism for the removal of NOR is proposed and described in Figure . The synergetic electrostatic interaction and charge-assisted n class="Chemical">hydrogen bonds strongly enhance the binding ability between TpPa-SO3Na and NOR.

Figure 6

Proposed mechanism for the removal of NOR by TpPa-SO3Na.

Proposed mechanism for the removal of NOR by n class="Chemical">TpPa-SO3Na.

Selective Adsorption and Separation

The adsorption and separation of hydrophilic organic pollutants are critically important due to serious environmental problems. The adsorption and separation are highly dependent on the porous structures, that is, the pore size and pore environment.[47−51] Compared with other separation materials, due to the capacity to regulate their pore size and chemical functionalities, MOFs and COFs have received increasing attention in adsorption and separation. MOFs have limitations such as poor chemical stability and interpenetrating channels in the separation of dyes.[47] n class="Chemical">COFs overcame the limitations of chemical instability in aqueous and organic and strongly acidic or alkaline media compared with MOFs.[13] Meanwhile, in 2D COFs, the 1D pores are open and free of interpenetration.[37,50] Owing to the availability of functional groups and design of pore size, a pore-surface engineering and skeleton design strategy offers a powerful tool to broaden the diversity of porous structures of COFs in adsorption and separation fields, thus enabling the screening of impact of porous structures on specific organic pollutants.[37,47,50] Effective selective separation of specific molecules can be achieved based on different interactions between molecules and functional nanochannels. To demonstrate the charge- selective separation, we treated TpPa-SO3Na with various dye molecules, including positively charged MB, positively and negatively charged methyl red (MR), neutral p-benzoquinone (p-BQ), and negatively charged calcein (CAL) (Figure S17). As shown in Figure a, MB was completely adsorbed in 10 min by TpPa-SO3Na, MR was removed by 85% (Figure b), while CAL was hardly adsorbed at all even after 2 h (Figure c). Neutral p-BQ was also hardly adsorbed by TpPa-SO3Na, which showed as low as 2% of separation efficiency even after 2 h (Figure S18). Although p-BQ molecules were small enough for entry, the uptake capacity of neutral p-BQ was low because of the absence of electrostatic interaction between TpPa-SO3Na and p-BQ. Therefore, electrostatic interactions appeared to dominate the adsorption, which was conducive to specific target pollutant removal.

Figure 7

UV absorption spectra of aqueous MB (a), MR (b), and CAL (c) treated with TpPa-SO3Na at different intervals. UV absorption spectra of the dye mixture solution (d) before and after passing through a TpPa-SO3Na-packed column. The inset shows the photograph of the tested column.

UV absorption spectra of aqueous MB (a), MR (b), and CAL (c) treated with n class="Chemical">TpPa-SO3Na at different intervals. UV absorption spectra of the dye mixture solution (d) before and after passing through a TpPa-SO3Na-packed column. The inset shows the photograph of the tested column.

To further test the charge separation effect, TpPa-SO3Na was utilized in a column experiment. The decrease of the UV spectra after the column treatment suggested that the dye mixture was completely separated with a sharp decrease of n class="Chemical">MB concentration (Figure d). The concentration change was 2 and 100% for CAL and MB (Figure d), respectively, suggesting the effective separation of the two molecules. However, when treated with TpPa, a poor separation selectivity toward CAL and MB was observed under the same conditions (Figure S19), suggesting that the negatively charged nanochannels play a critical role. Experiments show that the pore environment is essential to cause interactions between pores and guest molecules because the surfaces form the interface that interacts with guests.

We then treated TpPa-SO3Na with dye molecules including n class="Chemical">CV and Alcian blue 8GX (AB8GX) (Figure S17), which have different molecular dimensions and are positively charged, to further confirm the confinement effect of charged nanochannels in selective separation. MB was completely removed in 10 min with TpPa-SO3Na, while CV and AB8GX did not exhibit a noticeable change after 95% and 16% adsorption, respectively, for the same time period (Figure a,b). The size-dependent separation of dye molecules can be attributed to the effect of the nanochannel structure. In TpPa-SO3Na, the 1D pores are open and accessible only from the top and bottom sides of the 2D layers, and they are free of interpenetration. TpPa-SO3Na has a uniform and persistent hexagonal shape that enables accurate size recognition.[37] As displayed in Table S5, the size of AB8GX is larger than the accessible nanochannel diameter of TpPa-SO3Na, but the size of MB fits the nanochannel diameter of TpPa-SO3Na, leading to size-exclusive behaviors. The molecular size of CV is close to the nanochannel width of TpPa-SO3Na. The positive charge of CV assists considerably in the selective adsorption when the molecular size approaches the nanochannel diameter of the charged COF. Results show that selective adsorption can be specifically tuned by introducing functional sites and modifying their pore size. This would generate a high degree of control over host–guest interactions, improving the adsorptive selectivity and promoting the separation processes.

Figure 8

UV absorption spectra of aqueous CV (a) and AB8GX (b) treated with TpPa-SO3Na at different intervals.

UV absorption spectra of aqueous CV (a) and AB8GX (b) treated with n class="Chemical">TpPa-SO3Na at different intervals.

Conclusions

In summary, an anionic covalent organic framework was synthesized through a green two-in-one synthesis strategy with autocatalytic imine formation. The as-prepared n class="Chemical">TpPa-SO3Na has ultrafast adsorption kinetics and allows molecular separation on the basis of sulfonate functionalization of nanochannels. Our work can greatly promote the green manufacturing and investigation of anionic COFs with different kinds of binding sites to remove hydrophilic pollutants, further broadening the application of COFs as flexible and tunable materials for wastewater treatment and real-time separation, to cope with challenges of sustainability in the field of chemical and environmental protection technology.

Experimental Section

Synthesis of TpPa-SO3Na

Briefly, 0.3 mmol of 1,3,5-triformylphloroglucinol (n class="Chemical">Tp) and 0.45 mmol of 2,5-diaminobenzenesulfonic acid (Pa-SO3H) were added to 5 mL of mesitylene and 1,4-dioxane mixture (4:1, v/v). Subsequently, the mixture was ultrasonicated for 20 min to form a homogeneous solution. Afterward, 1 mL of 5 M NaOAc was added to the mixture dropwise at room temperature, and then it was flash-frozen under liquid N2.The reaction tube was sealed and then heated under 120 °C for 72 h. Precipitates with red color were successfully obtained and then washed successively with water and tetrahydrofuran five times. Finally, the product was dried at 120 °C under vacuum for 12 h to yield TpPa-SO3Na as a red-colored powder (90% yields). Synthesis of TpPa followed the same process, except that 2,5-diaminobenzenesulfonic acid was replaced by p-phenylenediamine.

Adsorption Experiments

Norfloxacin (n class="Chemical">NOR), ciprofloxacin (CIP), enrofloxacin (ENR), tetracycline hydrochloride (TC), methylene blue (MB), and crystal violet (CV) were dissolved in deionized water to obtain the stock solutions (0.5 g L–1). To study the adsorption kinetics, 60 mg of TpPa-SO3Na was added to 100 mL of the target pollutant solution (10 mg L–1) at pH 7.0 for 30 min. After being shaken for different time intervals, 0.5 mL of the solution sample was collected and immediately filtered by a 0.45 μm filter. The concentrations of NOR, CIP, ENR, and TC were determined by high-performance liquid chromatography (HPLC) with an ultraviolet (UV) detector. The concentrations of MB and CV were measured by UV–vis absorption spectroscopy. During the adsorption processes, the pH value of the solution was adjusted using NaOH or HCl solutions (0.1 M). For the regeneration experiments, the used adsorbents were added into the HCl solution (0.1 M). After desorbing for 10 min, the adsorbent was centrifuged with a speed of 8000 rpm for 5 min. Finally, the adsorbent was washed with deionized water and dried for reuse.