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Interaction between Dissolved Organic Matter and Long-Chain Ionic Liquids: A Microstructural and Spectroscopic Correlation Study Xiao-Yang Liu, Wei Chen, Chen Qian, and Han-Qing Yu Environ. Sci. Technol., Just Accepted Manuscript • DOI: 10.1021/acs.est.6b05228 • Publication Date (Web): 13 Apr 2017 Downloaded from http://pubs.acs.org on April 13, 2017

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Interaction between Dissolved Organic Matter and Long-Chain Ionic Liquids: A Microstructural and Spectroscopic Correlation Study

Xiao-Yang Liu*, Wei Chen*, Chen Qian, Han-Qing Yu** CAS Key Laboratory of Urban Pollutant Conversion, Department of Chemistry, University of Science and Technology of China, Hefei, 230026, China

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ABSTRACT

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The production and use of ionic liquids (ILs) increase the potential risk after their

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emission into the environment. After entering the environment, ILs will readily interact

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with dissolved organic matter (DOM), and their environmental behavior will be impacted

5

by DOM, which is abundant in the environment and has various functional groups.

6

However, to date, the interaction between DOM and ILs, especially long-chain ILs,

7

remains unclear. In this work, the interaction between long-chain ILs and humic acid

8

(HA), a representative DOM, was investigated using synchronous fluorescence, Fourier

9

transform infrared spectroscopy, dynamic light scattering and zeta potential techniques,

10

which were integrated with two-dimensional correlation spectroscopy (2DCOS), hetero-

11

2DCOS and perturbation-correlation moving-window analyses. The results show that

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cation exchange by the carboxylic groups in humic-like fractions was primarily

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responsible for interaction at low IL concentrations. As a result, the decrease in

14

electrostatic repulsion and the increase in hydrophobicity facilitated the loose aggregation

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of HA. With an increase in IL concentration, the aromatic and carbonyl groups were

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involved in the interaction via the π-π interaction and dipole-dipole interaction

17

respectively, which resulted in the disruption of intra-molecular hydrogen bond and

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promoted the compaction of HA under the hydrophobic effect. The intensity transition

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sequence of various groups in HA was elucidated more specifically by 2DCOS. With

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these results, a comprehensive view of the structural changes of DOM in its IL-binding

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process was obtained, and the fate and environmental impact of ILs could be better

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understood. Furthermore, the superior potential of such an integrated approach in

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investigating the complex interactions in the environment was also demonstrated.

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INTRODUCTION

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Ionic liquids (ILs), composed of organic cations and organic/inorganic anions, are

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generally liquid at room temperatures. Recently, ILs have received considerable attention

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due to their unique physical and chemical properties, such as their inherent

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amphiphilicity, negligible volatility, good thermal stability and good extraction

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capability.1,

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including catalysis, organic synthesis, oils, electrochemistry and liquid/liquid extraction,

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etc.3, 4 Considering these applications and their potential use in large-scale production

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processes, ILs will inevitably be released into the environment.5 Although their low vapor

35

pressure minimizes the atmospheric pollution, the impacts of ILs on aquatic and

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terrestrial ecosystems cannot be ignored or underestimated.6

2

Therefore, the commercial applications of ILs are rapidly increasing,

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Dissolved organic matter (DOM), which is ubiquitous in aquatic and terrestrial

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environments, is composed of aromatic and aliphatic hydrocarbon structures and contains

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amide, carboxyl, hydroxyl, ketone and various minor functional groups.7, 8 The presence

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of DOM is able to influence the mobility, retention, transformation and environmental

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toxicity of ILs.1, 2, 9 Previous studies have proven that ILs can interact with various soils

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via cation-exchange mechanism and the absorption strength increases with the increasing

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organic carbon content.2 It is also found that the dispersive interaction occurs with the

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excess cation exchange capacity of soils.10 Several driving forces in the interaction of ILs

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and DOM, i.e. ionic binding, ion-dipole interaction, dipole-dipole interaction and π-π

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interactions, were proposed.10 In extraction experiments, a high affinity of humic acid

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(HA) towards ILs in aqueous solutions was reported.11 Although this interaction

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significantly reduces the freely dissolved concentration and bioavailability of ILs, another

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study indicates that DOM and coexisting organic contaminants could be released from

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soils after addition of ILs, suggesting that DOM could facilitate the transportation of ILs

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in soils and groundwater and thereby increase their sub-surface mobility.9,

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influence of DOM is reported, but there is no molecular-level study to probe such an

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interaction process in detail. Furthermore, previous studies on DOM-ILs interaction focus

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on the absorption behavior only. Therefore, elucidating the interaction between ILs and

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DOM at a molecular level is essential and will lead to a better understanding of the fate

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and environmental impacts of ILs.

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The

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Current approaches, e.g., binding isotherm and conductivity titration, which can be

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used to explore the interaction between ILs and DOM, are limited, and little is known

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about the binding mechanism between DOM and ILs and the behavior of DOM after

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binding with ILs at a molecular level.12,

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dimensional correlation spectroscopy (2DCOS) analysis could remedy this defect and

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offer a deep insight into the variations of molecular structure. Recently, hetero-2DCOS

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receives growing attention due to the capability of integrating complementary

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information from the two different types of spectroscopy.7,

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two methods shows detailed information along the perturbation direction. Therefore, it is

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difficult to connect changes in the functional group of analytes with the macroscopic

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properties, such as the morphology, zeta potential and so on. To solve this problem, an

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emerging technique called perturbation-correlation moving-window (PCMW) is derived

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from the correlation between the spectral intensities and perturbation changes. This

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Optical spectroscopy coupled with two-

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approach can monitor the complicated spectral variations along the perturbation direction

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and determine the transition points and regions.16, 17

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In this work, by using FTIR, synchronous fluorescence, dynamic light scattering

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(DLS) and zeta potential techniques, we aim to provide a comprehensive understanding

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of the interaction between DOM and ILs from both the microstructural and spectroscopic

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perspectives. 2DCOS was used to analyze the subtle changes in the optical spectroscopy,

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while hetero-2DCOS and PCMW were employed to integrate the results, including the

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functional groups, fluorophore variations and macroscopic characteristics, i.e., the zeta

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potential and hydrodynamic size. To the best of our knowledge, this might be the first

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report about using a combination of macroscopic and microscopic approaches to

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investigate the DOM-related interaction. HA was used as a representative DOM, and a

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typical long-chain imidazolium-based IL, 1-dodecyl-3-methylimidazolium bromide

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[C12mim]Br, was used to represent the ILs due to its good surface activity, hard

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degradation and wide application in various areas.7, 18-22

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MATERIALS AND METHODS

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Sample Preparation. Analytical reagent-grade NaOH and HCl were purchased from

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Sinopharm Chemical Reagent Co., China. [C12mim]Br was obtained from Shanghai

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Cheng Jie Chemical Co., China with a purity of over 99%. Commercial HA (Sigma-

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Aldrich Co., USA) was purified prior to use (details in Supporting Information, SI). The

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purified HA was dissolved to a final concentration of 100 mg/L at pH=7.0 with 1 M

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NaOH and 1 M HCl. The [C12mim]Br powder was dissolved to a final concentration of

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25 mM as a stock solution. A series of solutions containing 24 mg C/L HA and

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[C12mim]Br with concentrations ranging from 0 to 0.65 mM were prepared, and the

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background ionic strength was maintained by 0.03 M KBr. The concentrations of IL used

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were far below the critical micelle concentration (10.9 mM).23 The mixed solutions were

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shaken for 30 h at room temperature (25 °C) to ensure the binding equilibrium.11 Then,

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the solutions were agitated gently using a vortex mixer for 5 s and analyzed by DLS, zeta

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potential and synchronous fluorescence spectroscopy. A 35-mL aliquot of each sample

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was freeze-dried for further analysis by FTIR spectroscopy.

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DLS and Zeta Potential Measurements. The DLS and zeta potential

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measurements of HA solutions with different IL concentrations were performed using a

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Malvern Zetasizer ZS instrument (Malvern Instruments Co., UK). During the DLS

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measurement, a He-Ne laser beam operated at λ = 633 nm was incident on the samples,

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and then scattered light was detected and collected by a photodetector at an angle of 173°

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to utilize the backscattering mode. The DLS instrument could be used to measure

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particles ranging from 0.6 nm to 6 µm. In the DLS and zeta potential measurements, three

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parallel tests were conducted at 25 °C, and the data were presented as the mean ±

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standard deviation. In addition, after the reaction the pH values of all the solutions were

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measured to be 6.14 ± 0.07. Such a slight change of pH should have negligible impact on

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the zeta potential.24

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Spectroscopy Measurements. Synchronous fluorescence spectra of HA solutions

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with various IL concentrations were analyzed with a luminescence spectrometer (LS-55,

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Perkin-Elmer Inc., USA). The synchronous scans were performed over a range from 250

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to 550 nm with a constant offset △λ of 60 nm.7 The excitation and emission slits were

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both 10 nm, and the scan rate was 1000 nm/min. The background synchronous

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fluorescence spectra of water and IL are shown in Figure S1.

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The freeze-dried HA samples with various IL concentrations were ground and

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homogenized. Afterwards, 50 mg of each sample was pressed under the irradiation of an

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infrared lamp to eliminate the influence of moisture. Their transmission IR spectra were

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recorded on a Vertex 70 spectrometer (Bruker Co., Germany) with a deuterated triglycine

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sulfate detector, and each spectrum was obtained after 64 scans with a 4 cm-1 resolution

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and finally transformed to absorbance spectra using OPUS 5.5 software for the

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subsequent analysis. The IL samples at different concentrations in the absence of HA

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were treated by the same procedure referring to literature.7, 25 No extra KBr was added as

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ground KBr powder was added into the solution (30 mM) before freeze drying. The FTIR

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spectra of the purified HA and IL are shown in Figure S2.

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Data Analysis. To probe the structural variation in the interaction between HA and

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the IL, 2DCOS, hetero-2DCOS and PCMW analyses were performed using the

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synchronous fluorescence and FTIR spectra (details in SI). The concentration of the IL

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was used as an external variable. Prior to the analysis, the spectra of each sample were

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baseline-corrected and smoothed, and the background signal (without the addition of HA)

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was subtracted with the peak at 860 cm-1 as a reference band (Figure S2). 2DCOS,

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hetero-2DCOS and PCMW maps were calculated and plotted by 2D Shige (Kwansei-

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Gakuin University, Japan) and Origin 8.5 software.

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RESULTS

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Change of HA Stability with the IL. HA is a complex mixture of negatively charged

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organic compounds present in the environment. The impact of the tested IL on the

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stability of HA was evaluated by examining the hydrodynamic radii Rh and zeta

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potentials of HA at variable IL concentrations (Figure 1). Three steps of aggregation

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could be distinguished from Figure 1a: (i) Rh of the HA-IL complexes rapidly increased

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from 236.4 ± 2.1 nm at [IL] = 0.05 mM to 3275.8 ± 234.3 nm at [IL] = 0.20 mM; (ii) Rh

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slightly decreased from 0.20 to 0.30 mM IL; and (iii) the mean size of the HA-IL

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complexes remained almost unchanged at approximately 2500 nm. The three distinct

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steps were designated Periods 1, 2 and 3. There was significant difference between the

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sizes of HA in the IL concentration ranges (0.15 mM, 0.20 mM), (0.20 mM, 0.25 mM)

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and (0.25 mM, 0.30 mM) (p < 0.05, Table S1). The difference was not significant at IL

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concentrations higher than 0.30 mM. These results further confirm that there were three

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periods when the IL with increasing concentrations bound to HA, and the turning points

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were around 0.20 and 0.30 mM. The increase in the HA size in Period 1 likely resulted

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from the decrease in electrostatic repulsion and the increase in hydrophobicity.26 Then,

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the aggregates became dense and compact in Periods 2 and 3, which was attributed to the

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hydrophobic effect of IL as well as the disruption of intramolecular hydrogen bond in HA,

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which will be discussed later with the spectroscopy results.8, 11, 27

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The zeta potential profiles of HA in the presence of the IL are shown in Figure 1b.

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With the addition of the IL, the zeta potential of HA became less negative, indicating that

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the IL imparted positive charges to HA and decreased the absolute surface potential.28

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Moreover, according to the DLVO theory, the decrease in surface potential would reduce

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the repulsive forces between HA molecules, and subsequently, large aggregates were

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formed, which is exactly in agreement with the DLS results. In Period 2, the zeta

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potentials of the HA-IL complexes remained almost unchanged, which was likely related

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to the constriction and rearrangement of HA. There was significant difference for the zeta

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potentials at IL concentrations of 0-0.10 mM and 0.40-0.55 mM (p < 0.05, Table S1) due

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to the absorption of IL, while the difference was not significant at 0.10-0.40 mM.

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Although Na+, K+ and IL+ are all mono-valent cations, the absorption energy of ILs

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with HA is much higher than that of Na+ and K+ due to the hydrophobicity of the alkyl

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chain.11 Thus, IL+ could be absorbed closer to the HA surface, leading to the less negative

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zeta potential. Previous studies have shown that Na+ forms very weak outer-sphere

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complexes with DOM.29 By calculating the occupancy of the Stern layer with ionic

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surfactant and Na+ in the sorption on glass, Dimov et al. also found that, although cation

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exchange took place, the increase in the occupancy of Stern layer with ionic surfactant

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was larger than the decreased amount of occupancy with Na+.30 Considering the similarity

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between ILs and ionic surfactants, the ion replacement ratio of IL+ and Na+ or K+ in the

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Stern layer should also be larger than 1:1.10

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Spectral Response of HA to the IL. There are abundant functional groups in HA,

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including carboxyl, phenol, hydroxyl, quinone, ester, ketone and amino groups. Thus,

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synchronous fluorescence and FTIR spectroscopies were used to probe the spectral

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changes of HA during interaction with the IL (Figure 2). In order to show the changes of

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synchronous fluorescence spectra with the dose of IL more clearly, the contour map is

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shown in Figure 2a and the corresponding spectra are shown in Figure S3. There were

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three fluorescence regions at 250-300, 300-380 and 380-550 nm, which could be assigned

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to the protein-, fulvic- and humic-like fluorescence fractions of HA, respectively.

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Compared to the fulvic- and humic-like regions, the fluorescence intensity of the protein-

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like fraction was relatively low. After dosing the IL, the fluorescence intensity in the

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humic-like fraction decreased remarkably, which suggests that the interaction sites were

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mainly from the humic-like fraction, and the decrease is probably due to the charge-

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transfer effect. Numerous studies show that the fluorescence properties of DOM result

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from the intra-molecular charge-transfer interactions between hydroxy-aromatic donors

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and quinoid or other acceptors formed by the partial oxidation of lignin precursors.31

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Especially, in the wavelength region where the local donor states should no longer absorb

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(beyond λex 375-400 nm), the fluorescence emission is primarily attributed to an

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ensemble of the charge-transfer states of differing energies.32

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The dominant infrared spectral characteristics of HA with the addition of the IL are

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presented in Figure 2b. At low IL concentrations, the characteristic peak at 1385 cm-1

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assigned to the symmetric stretching vibrations of COO- or phenolic C-O-H was shifted

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to approximately 1408 cm-1. The drastic blue-shift might be attributed to the breaking of

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hydrogen bonding. The structural changes of HA upon IL addition are illustrated more

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clearly in the differential IR absorbance spectra, in which the spectrum of HA without IL

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addition was subtracted from each other spectrum (Figure 2c). For example, the peak

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intensity at 1200 cm-1 attributed to the stretching vibrations of C-O of aromatic acid and

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aliphatic acid ester gradually increased with IL addition. Even so, some of the IR bands

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remained overlapped and could hardly be distinguished owing to the diverse groups of

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HA. Thus, to determine the conformational changes of HA in the binding process with

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the IL, 2DCOS, hetero-2DCOS and PCMW analyses were performed using the

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synchronous fluorescence and FTIR spectra.

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Correlation Analysis of the Structural Change in the HA-IL Interaction.

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2DCOS enables the decomposition of overlapping peaks and enhances the spectral

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resolution by spreading the spectra in a second dimension.14 When two or more

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overlapping peaks behave differently under perturbation, the cross-peaks, which are

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located in the off-diagonal region, could provide clues that aid the assignment of their

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frequencies and components. In addition, 2DCOS may reveal the trend of intensity

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changes that are not evident in the original spectra.14 The synchronous 2DCOS map for

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the synchronous fluorescence spectra of HA in the 280-550 nm region (Figure 3a) shows

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that two predominant autopeaks centered at 450 and 320 nm along the diagonal line, and

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a small peak at 266 nm can be identified from the cross-peaks, which indicates that the

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fluorescence of fulvic- and humic-like fractions were readily affected by IL addition.

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Moreover, the intensity at 450 nm changed in the opposite direction compared to those at

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266 and 320 nm, considering the negative cross-peaks of (450, 266) and (450, 320). The

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asynchronous map provided the sequential relationship among these fractions (Figure 3b).

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The cross-peaks (450, 266) and (450, 320) exhibited positive and negative signs,

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respectively, which implies that the intensity variation followed the order: 266 nm > 450

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nm > 320 nm, i.e., protein- → humic- → fulvic-like fractions.

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Overlapping IR peaks are major obstacles to assigning bands and analyzing the

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conformational changes of HA, but 2DCOS could effectively resolve this problem.

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Figure 3c and d shows the 2D IR COS of the interaction between HA and the IL at

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various concentrations. The sign and assignment of each cross-peak are listed in Tables

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S2 and S3, respectively.33 There were eight autopeaks in the synchronous map, centered

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at 1730, 1600, 1570, 1490, 1408, 1375, 1201 and 1060 cm-1 (Figure 3c). The band

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centered at 1600 cm-1 changed most significantly, which was attributed to the asymmetric

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stretching of the carboxylate group. The smallest changes were at 1730 and 1060 cm-1,

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which was assigned to the stretching of C=O of the carboxylic group and C-O of

234

polysaccharides, respectively. The autopeak at 1644 cm-1 corresponding to the C=O

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stretching of amide, quinone or ketone could be overlapped by the peak at 1600 cm-1,

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according to the cross-peaks. Most of the cross-peaks in the synchronous map were

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positive, except for those associated with 1570 and 1375 cm-1. This indicates that most IR

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bands changed in the same direction, whereas the bands at 1570 and 1375 cm-1 changed

239

in the reverse direction. The 1570 and 1375 cm-1 bands could be assigned to the

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stretching of imidazole C=C and C-N-C as well as the wagging vibration of CH2 of the

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IL, suggesting the formation of HA and IL complexes. Combined with the asynchronous

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map in Figure 3d, the final sequence order of HA conformational changes could be

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concluded on the basis of Noda’s rule: 1570, 1375 > 1730 > 1490 > 1201 > 1644 >

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1060 > 1600 > 1408 cm-1 or ν(C=C of imidazole), νas(C=C of imidazole) or ω(CH2 of IL)

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→ ν(C=O of COOH) → ν(C=C of aromatic ring) → ν(C-O of aromatic acid, aliphatic

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acid ester) → ν(C=O of amide, quinone or ketone) → ν(C-O of polysaccharide) →

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νas(COO-) → νs(COO-) or phenolic ν(C-O), δ(O-H).

248

To determine the IR band assignments and the correlation between the fluorescence

249

and FTIR spectra, fluorescence/IR hetero-2DCOS analysis was performed (Figure S4a

250

and b). In the synchronous map, six cross-peaks were located remarkably in the IR

251

regions 1644, 1600, 1570, 1490, 1375, and 1201 cm-1 and the corresponding fluorescence

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region 450 nm (Figure S4a). The cross-peaks of 1570 and 1375 cm-1 with 450 nm were

253

positive, while the others were negative. These results indicate that the carbonyl and

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aromatic groups are the basic fluorescent units for the humic-like fraction of HA, and

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their IR intensities increased after the IL addition. In the asynchronous map, two new

256

cross-peaks were observed at 1730 and 1010 cm-1 with the fluorescence peak at 450 nm,

257

which indicates that carboxylic groups and some polysaccharide groups were also related

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to the humic-like fraction (Figure S4b). In addition, the fulvic-like fraction had a higher

259

content of carboxylate and phenolic groups due to the two cross-peaks at 1600 and 1408

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cm-1 with the fluorescence region at 380-300 nm.34

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Because the IR and fluorescence spectra reflect the different aspects of molecular

262

responses towards an identical stimulation, asynchrony was observed between the

263

spectroscopic data of the same species. Five positive signs at coordinates (1644, 450),

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(1600, 450), (1201, 450), (1600, 380-300) and (1408, 380-300) appeared in the

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asynchronous map, which implies that the fluorescence response of the fulvic-like

266

fraction occurred before the carboxylate groups, and the fluorescence response of the

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humic-like fraction occurred before the carboxylate groups, C-O of aromatic acid and

268

aliphatic acid ester, and C=O of amide, quinone or ketone. In addition, the cross-peaks

269

(1490, 450), (1570, 450) and (1375, 450) indicate that the fluorescence response of the

270

humic-like fraction changed after the addition of IL and C=C groups. The order of IR

271

intensity changes was in good agreement with the 2DCOS results.

272

Correlation between the Spectral Variable and the IL Concentration. Although

273

the spectral resolution was enhanced greatly by 2DCOS, the correlation between the

274

characteristic spectral variable and the IL concentration remained unclear. Thus, PCMW

275

was used to determine the transition point and monitor the complicated spectral variations

276

along the perturbation. Furthermore, the changes of the HA functional groups observed

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by the PCMW method could be readily related to other data, such as the DLS and zeta

278

potential.

279

Figure 4a and b shows the PCMW synchronous and asynchronous maps based on

280

the FTIR spectra of HA with the IL at various concentrations. A window size of 2m + 1 =

281

7 was applied for the calculation. For convenience, the transition concentrations and

282

transition regions of HA that can be read from these maps are plotted in Figure 4c. The

283

transition concentrations of various functional groups, which are the local maximum

284

gradient of the spectral intensity change along the concentration, were determined by the

285

synchronous peaks: carboxylic (1730 cm-1) and IL functional groups (1375, 1570 cm-1)

286

below 0.15 mM IL→ aromatic groups (1490, 1201 cm-1) at 0.35 mM IL→ carboxylate

287

groups (1600, 1408 cm-1) and C-OH of polysaccharide (1060 cm-1) at 0.4 mM IL. These

288

transition concentrations were mostly gathered around 0.35-0.4 mM, indicating that the

289

changes of the functional groups slowed down after the size of HA-IL reached a limit

290

(Period 3).

291

Combining the signs of the PCMW synchronous and asynchronous spectra, the

292

spectral variations along the concentration perturbation could be probed by the signs of

293

correlation peaks.16 The transition concentration region could be determined by the peak

294

positions in the asynchronous spectra, which are all the turning points of the curves.17

295

Based on these rules, it was concluded that, with the IL addition, the aromatic, COO- and

296

C-O of the polysaccharide groups exhibited S-shaped spectral changes. These groups are

297

related to the hydrogen bonding capability of HA, and the onset concentrations were

298

focused in the region of 0.2-0.35 mM, in which the HA-IL complexes became compact.

299

This result suggests that the constriction of HA might be related to the hydrogen bonds

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and hydrophobic environment.8 In addition, at an [IL] of less than 0.15 mM, the peaks at

301

1570 and 1375 cm-1 decreased, while the intensity of the peak at 1730 cm-1 increased.

302

This confirms that the carboxylic group of HA was the main group that interacted with

303

the IL at low concentrations.

304 305

DISCUSSION

306 307

Evolution of the Binding between ILs and DOM. DOM has a great impact on the

308

absorption, transport and transfer of ILs, as demonstrated by various binding

309

experiments.2,

310

interaction between DOM and ILs. HA, a representative DOM, is generally considered as

311

a supramolecular association of self-assembling heterogeneous and relatively small

312

molecules stabilized by weak dispersive forces, such as hydrophobic (i.e., van der Waals,

313

π-π and CH-π) forces and hydrogen bonds. Thus, the structure of HA could be readily

314

destroyed and reconstructed by ILs. The interaction between HA and the IL can be

315

divided into three periods based on the DLS results. The hydrodynamic size of the HA-IL

316

complexes underwent a rapid increase, experienced condensation and was almost

317

constant in Periods 1, 2, and 3, respectively.

11, 12

However, robust evidence is still required to further elucidate the

318

In Period 1 (0-0.2 mM IL), the increased size and zeta potential indicate the loose

319

aggregation of HA. These structural changes of HA have also been observed when HA

320

interacts with other cations.26 According to the non-ideal competitive adsorption (NICA)-

321

Donnan model, carboxylic and phenolic groups of HA are the low and high proton-

322

affinity sites, respectively. The low proton-affinity carboxylic sites tend to interact with

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cations, as reported in a recent study related to clarithromycin.35 In addition, upon

324

interaction with HA, the critical aggregation concentration of the IL-HA complexes was

325

approximately 0.10 mM, which is equivalent to the average amount of carboxylic groups

326

(3.17 mol/kg) in HA.36 Therefore, the carboxylic groups are supposed to dominate the

327

initial binding process of ILs with HA. In Period 2 (0.2-0.3 mM IL), ILs continued to be

328

bound to HA in the compression of the HA-IL complexes; otherwise, the absolute zeta

329

potential value would increase. In Period 3 (0.3-0.65 mM IL), although the size of the

330

HA-IL complexes remained constant, the ILs still tended to be close to HA, as evidenced

331

by the zeta potential results.

332

The combination of further experimental data and previous literature findings allows

333

us to examine the detailed HA-IL interaction. By combining the DLS and zeta potential

334

results with PCMW analysis, the interaction process can be elucidated from the point of

335

view of structural change of HA. In Period 1, the carboxylic groups of the humic-like

336

fraction are bound to the cationic head of the IL, which is consistent with the proposed

337

conjecture obtained from the DLS results. In Period 2, C=C of aromatic ring, C-O of

338

aromatic acid and aliphatic acid ester, C=O of amide, quinone or ketone, and C-O of

339

polysaccharides related to the humic-like fraction changed in succession, implying that π-

340

π and dipole-dipole interactions occurred and made IL close to HA. A previous study

341

demonstrates that intra-molecular hydrogen bonds helped to stabilize the structure of HA

342

and hinder its compaction, with carboxylic acids and phenols as proton donors, while

343

carbonyl groups (carboxylic acids and ketones) and π-electrons in aromatic rings as

344

proton acceptors.8, 37 The π-hydrogen bonds in HA, which resulted from stereochemical

345

arrangements in primary structures, were rather weaker (< 4 kcal/mol) compared to the π-

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π interaction (4-17 kcal/mol).10, 38 Thus, the π-π interaction could readily destroy the π-

347

hydrogen bond. As a result, the decreased stability of HA and the increased

348

hydrophobicity led to the compression of HA, which is supported by the DLS and zeta

349

potential results. The π-π and dipole-dipole interaction are also reported to be involved in

350

the interaction between ILs and soil.10, 39

351

In addition, intra-molecular π-hydrogen bonds formed by the aromatic ring and

352

electron acceptors in HA were more readily destroyed by imidazole ring of IL than those

353

formed by the C=O groups.8, 40 The fluorescence of the humic-like fraction, which has a

354

higher aromatic degree, was quenched due to the increased charge-transfer effect

355

resulting from the π-π interaction and the decreased distance between donors and

356

acceptors because of contraction, according to the sequence derived from hetero-2DCOS

357

and PCMW analyses.31, 41 Furthermore, due to the increased synchronous fluorescence

358

intensity of the fulvic-like fraction after the change of the humic-like fraction in Period 3,

359

the constriction may lead to the release of the low molecular weight and relatively

360

hydrophilic HA fraction, i.e., the fulvic-like fraction, from the supermolecular structure.42,

361

43

362

eliminate self-quenching because of the charge-transfer interactions.31 On the other hand,

363

the aggregation of HA mainly takes place in the hydrophobic region under the influence

364

of dilution or the addition of metal cations.44, 45 It is reported that the hydrated humic

365

components could be hardly incorporated in aggregates.45 Thus, the release of fulvic-like

366

fraction could occur in the HA-IL interaction process. In addition, the release of the small

367

molecular weight and hydrophilic fraction has also been observed in the interaction

368

between HA and the cationic surfactant dodecylpyridinium chloride.46 As a result, the

On the one hand, the release of fulvic-like fraction from the HA aggregate could

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369

carboxylate groups related to the fulvic-like fraction were changed. Owing to the

370

similarity in basic chemical structure, it is reasonable to assume that the mechanism for

371

the fulvic acid (FA)-IL interaction is similar to that for the HA-ILs interaction. The

372

binding affinity between FA and IL is weaker, as the structure of FA is less hydrophobic.

373

Inter- and Intra- Molecular Interactions of DOM with the IL at Various

374

Concentrations. The interaction between ILs and mineral surfaces or organic matter has

375

been studied, and various mechanisms have been proposed, e.g., cation exchange,

376

hydrophobic force and van der Waals interaction.1, 2 The interaction mechanisms depend

377

on the physicochemical properties of ILs and soils/sediments/mineral surfaces. The

378

cation exchange was primarily responsible for the initial binding process, as confirmed

379

by our DLS, zeta potential and FTIR results.1 HA became destabilized and formed loose

380

aggregates due to the reduced intermolecular electrostatic repulsion and the increased

381

hydrophobicity in Period 1. Furthermore, our results suggest that the breaking of intra-

382

molecular hydrogen bonds and hydrophobic forces might drive the structural changes of

383

the HA-IL complexes in Periods 2 and 3 (Figure 1). The condensation of fulvic acid by

384

the hydrophobic effect of long alkyl chains was also reported for the interaction between

385

fulvic acid and cation surfactants.47 The transition and turning concentrations of the

386

groups were distinct, which indicates that the energy of hydrogen bonds varied with the

387

functional groups in HA.8 Afterwards, the rearrangement of HA might lead to the release

388

of the small molecular weight fraction in Period 3, because the HA structure is soft and

389

permeable and the aggregation mainly takes place in the hydrophobic region.37, 45

390

In order to understand the effect of alkyl chain length, the interaction between

391

[C6mim]Br and HA in the same concentration region (0-0.65 mM) was investigated, and

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392

the results are shown in Figures S5 and S6. With an increase in IL concentration, the

393

hydrodynamic size of HA increased slightly, but far less significantly compared with

394

[C12mim]Br. Meanwhile, the zeta potential and synchronous fluorescence spectra of HA

395

remained almost unchanged. According to the p value in Table S4, there was almost no

396

significant difference for the hydrodynamic size and zeta potential with [C6mim]Br

397

addition (p > 0.05). Due to the hydrophobicity of the alkyl chain, long-chain IL+ could be

398

absorbed closer to the HA surface, which makes the zeta potential less negative.11, 30 As a

399

result, the decrease in electrostatic repulsion and the increase in hydrophobicity promotes

400

the aggregation of HA. However, as for the short-chain ILs, their absorption energies are

401

lowered, thus, cation exchange may not effectively occur. Therefore, compared to long-

402

chain ILs, the interaction between short-chain IL and HA was much weaker. This could

403

be used to explain the observation that long-chain ILs would be more readily extracted

404

from aqueous solutions by HA than the short-chain ones.12 Koopal et al. also found that

405

the phase separation of HA-surfactant induced by compaction became stronger with the

406

increase in hydrophobicity.46

407

Significance of This Work. To date, staple ILs are manufactured at the metric ton

408

scale, and big chemical companies (e.g., BASF, Degussa, and IoLiTec/Wandres) are

409

using ILs in various processes, implying that the production volumes and demand of ILs

410

continue increasing. As a result, the emission of ILs into aqueous environments is

411

inevitable. Therefore, insight into the interaction between ILs and DOM is essential,

412

because the widespread DOM in aqueous environments will remarkably affect the

413

mobility, retention, transformation and environmental toxicity of ILs. Combining various

414

correlation analyses with DLS and zeta potential results, this study reveals that DOM

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415

could interact with IL through cation-exchange, π-π and dipole-dipole interactions. The

416

disruption of intra-molecular hydrogen bond and the hydrophobic effect of ILs promoted

417

the compression of the HA-IL complex. These findings suggest that, the mobility of long-

418

chain ILs will likely be reduced and sedimentation may occur in the presence of high-

419

hydrophobicity DOM and at high ionic strengths, e.g., in estuaries. DOM can obviously

420

diminish the environmental impact and even toxicity of ILs. In addition, relatively

421

hydrophilic fulvic-like fraction in DOM could be released after compression. Likewise,

422

the other coexisting contaminants in DOM may also occur, as the release of polycyclic

423

aromatic hydrocarbons from soil under the IL addition has already been reported.11 The

424

in-depth elucidation of such an interaction process will enable better understanding of the

425

fate and transformation of ILs in environments and even promote the design of more

426

environmentally friendly IL products. Furthermore, such an integrated approach could

427

also be applied to probe other complicated interaction processes in natural and engineered

428

environments.

429 430

AUTHOR INFORMATION

431

*These authors contributed equally to this work.

432

**Corresponding author: Prof. Han-Qing Yu, Fax: +86 551 63601592; E-mail:

433

[email protected]

434 435

ACKNOWLEDGEMENTS

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436

We thank the National Natural Science Foundation of China (21261160489, 21590812

437

and 51538011) and the Collaborative Innovation Center of Suzhou Nano Science and

438

Technology of the Ministry of Education of China for the support of this study.

439 440

ASSOCIATED CONTENT

441

Supporting Information Available. Experiment details, p values of hydrodynamic size

442

and zeta potential with [C12mim]Br addition (Table S1), sign and assignment of

443

characteristic bands in the 2DCOS maps (Tables S2 and S3), p values of hydrodynamic

444

size and zeta potential with [C6mim]Br addition (Table S4), synchronous fluorescence

445

spectra of water and ILs (Figure S1), FTIR spectra of purified HA and IL (Figure S2),

446

synchronous fluorescence spectra of HA with the dose of ILs at various concentrations

447

(Figure S3), synchronous (a) and asynchronous (b) hetero-2DCOS maps calculated from

448

the FTIR spectra of HA interacting with the IL at various concentrations (Figure S4),

449

average particle size, zeta potential (Figure S5) and synchronous fluorescence spectra of

450

HA with the addition of [C6mim]Br (Figure S6). This information is available free of

451

charge via the Internet at http://pubs.acs.org/.

452 453

REFERENCES

454 455

1.

of ionic liquids: A review. Environ. Sci. Technol. 2015, 49 (21), 12611-12627.

456 457 458

Amde, M.; Liu, J. F.; Pang, L. Environmental application, fate, effects, and concerns

2.

Pham, T. P. T.; Cho, C. W.; Yun, Y. S. Environmental fate and toxicity of ionic liquids: A review. Water Res. 2010, 44, 352-372.

21 ACS Paragon Plus Environment

Environmental Science & Technology

459

3.

industry. Chem. Soc. Rev. 2008, 37 (1), 123-150.

460 461

4.

5.

Richardson, S. D.; Ternes, T. A. Water analysis: emerging contaminants and current issues. Anal. Chem. 2014, 86 (6), 2813-2848.

464 465

Zhang, S.; Sun, J.; Zhang, X.; Xin, J.; Miao, Q.; Wang, J. Ionic liquid-based green processes for energy production. Chem. Soc. Rev. 2014, 43 (22), 7838-7869.

462 463

Plechkova, N. V.; Seddon, K. R. Applications of ionic liquids in the chemical

6.

Ruokonen, S. K.; Sanwald, C.; Sundvik, M.; Polnick, S.; Vyavaharkar, K.; Dusa, F.;

466

Holding, A. J.; King, A. W.; Kilpelainen, I.; Lammerhofer, M.; Panula, P.; Wiedmer,

467

S. K. Effect of ionic liquids on zebrafish (Danio rerio) viability, behavior, and

468

histology; correlation between toxicity and ionic liquid aggregation. Environ. Sci.

469

Technol. 2016, 50 (13), 7116-7125.

470

7.

Chen, W.; Habibul, N.; Liu, X. Y.; Sheng, G. P.; Yu, H. Q. FTIR and synchronous

471

fluorescence heterospectral two-dimensional correlation analyses on the binding

472

characteristics of copper onto dissolved organic matter. Environ. Sci. Technol. 2015,

473

49 (4), 2052-2058.

474

8.

Cao, X.; Drosos, M.; Leenheer, J. A.; Mao, J. Secondary Structures in a freeze-dried

475

lignite humic acid fraction caused by hydrogen-bonding of acidic protons with

476

aromatic rings. Environ. Sci. Technol. 2016, 50 (4), 1663-1669.

477

9.

Zhang, Z.; Liu, J. F.; Cai, X. Q.; Jiang, W. W.; Luo, W. R.; Jiang, G. B. Sorption to

478

dissolved humic acid and its impacts on the toxicity of imidazolium based ionic

479

liquids. Environ. Sci. Technol. 2011, 45 (4), 1688-1694.

480 481

10. Jungnickel, C.; Mrozik, W.; Markiewicz, M.; Luczak, J. Fate of ionic liquids in soils and sediments. Curr. Org. Chem. 2011, 15 (12), 1928-1945.

22 ACS Paragon Plus Environment

Page 22 of 33

Page 23 of 33

Environmental Science & Technology

482

11. Wang, H.; Wang, J.; Fan, M. Extraction of ionic liquids from aqueous solutions by

483

humic acid: an environmentally benign, inexpensive and simple procedure. Chem.

484

Commun. 2012, 48 (3), 392-394.

485

12. Markiewicz, M.; Jungnickel, C.; Arp, H. P. Ionic liquid assisted dissolution of

486

dissolved organic matter and PAHs from soil below the critical micelle concentration.

487

Environ. Sci. Technol. 2013, 47 (13), 6951-6958.

488

13. Mrozik, W.; Kotlowska, A.; Kamysz, W.; Stepnowski, P. Sorption of ionic liquids

489

onto soils: experimental and chemometric studies. Chemosphere 2012, 88 (10),

490

1202-1207.

491 492

14. Noda, I. Close-up view on the inner workings of two-dimensional correlation spectroscopy. Vib. Spectrosc. 2012, 60, 146-153.

493

15. Mecozzi, M.; Tudino, M. B.; Finoia, M. G.; Conti, M. E. Uncommon multivariate

494

statistical methods for environmental studies: A review. Trend. Environ. Anal. Chem.

495

2015, 6, 31-38.

496

16. Chen, Z.; Zhou, T.; Hui, J.; Li, L.; Li, Y.; Zhang, A.; Yuan, T. Tracing the

497

crystallization

498

crystalline/crystalline

499

spectroscopy. Vib. Spectrosc. 2012, 62, 299-309.

500

process

of

blends

polyoxymethylene/poly by

two-dimensional

(ethylene infrared

oxide) correlation

17. Lai, H.; Wu, P. A infrared spectroscopic study on the mechanism of temperature-

501

induced

phase

transition

of

concentrated

aqueous

502

isopropylacrylamide) and N-isopropylpropionamide. Polymer 2010, 51 (6), 1404-

503

1412.

23 ACS Paragon Plus Environment

solutions

of

poly(N-

Environmental Science & Technology

504

18. Sharma, R.; Kamal, A.; Kang, T. S.; Mahajan, R. K. Interactional behavior of the

505

polyelectrolyte poly sodium 4-styrene sulphonate (NaPSS) with imidazolium based

506

surface active ionic liquids in an aqueous medium. Phys. Chem. Chem. Phys. 2015,

507

17 (36), 23582-23594.

508

19. He, Y.; Shang, Y.; Liu, Z.; Shao, S.; Liu, H.; Hu, Y. Interactions between ionic

509

liquid surfactant [C12mim]Br and DNA in dilute brine. Colloids Surf. B 2013, 101,

510

398-404.

511

20. Gu, B.; Bian, Y.; Miller, C. L.; Dong, W.; Jiang, X.; Liang, L. Mercury reduction

512

and complexation by natural organic matter in anoxic environments. Proc. Natl.

513

Acad. Sci. U.S.A. 2011, 108 (4), 1479-1483.

514

21. Yan, L.; Fitzgerald, M.; Khov, C.; Schafermeyer, A.; Kupferle, M. J.; Sorial, G. A.

515

Elucidating the role of phenolic compounds in the effectiveness of DOM adsorption

516

on novel tailored activated carbon. J. Hazard. Mater. 2013, 262, 100-105.

517

22. Liu, G.; Cai, Y. Complexation of arsenite with dissolved organic matter: conditional

518

distribution coefficients and apparent stability constants. Chemosphere, 2010, 81 (7),

519

890-896.

520

23. Wang, X.; Liu, J.; Yu, L.; Jiao, J.; Wang, R.; Sun, L. Surface adsorption and micelle

521

formation of imidazolium-based zwitterionic surface active ionic liquids in aqueous

522

solution. J. Colloid Interface Sci. 2013, 391, 103-110.

523

24. Omar, F. M.; Aziz, H. A.; Stoll, S. Aggregation and disaggregation of ZnO

524

nanoparticles: influence of pH and adsorption of Suwannee River humic acid. Sci.

525

Total Environ. 2014, 468, 195-201.

24 ACS Paragon Plus Environment

Page 24 of 33

Page 25 of 33

Environmental Science & Technology

526

25. Chen, W.; Qian, C.; Liu, X. Y.; Yu, H. Q. Two-dimensional correlation

527

spectroscopic analysis on the interaction between humic acids and TiO2

528

nanoparticles. Environ. Sci. Technol. 2014, 48 (19), 11119-11126.

529

26. Zhou, M.; Meng, F. Aluminum-induced changes in properties and fouling propensity

530

of DOM solutions revealed by UV-vis absorbance spectral parameters. Water Res.

531

2016, 93, 153-162.

532 533

27. Matzke, M.; Thiele, K.; Muller, A.; Filser, J. Sorption and desorption of imidazolium based ionic liquids in different soil types. Chemosphere 2009, 74 (4), 568-574.

534

28. Zhang, Y.; Chen, Y.; Westerhoff, P.; Crittenden, J. Impact of natural organic matter

535

and divalent cations on the stability of aqueous nanoparticles. Water Res. 2009, 43

536

(17), 4249-4257.

537

29. Kalinichev, A.; Kirkpatrick, R. Molecular dynamics simulation of cationic

538

complexation with natural organic matter. Eur. J. Soil Sci. 2007, 58 (4), 909-917.

539

30. Dimov, N.; Kolev, V.; Kralchevsky, P.; Lyutov, L.; Broze, G.; Mehreteab, A.

540

Adsorption of ionic Surfactants on solid particles determined by zeta-potential

541

measurements: competitive binding of counterions. J. Colloid Interface Sci. 2002,

542

256 (1), 23-32.

543

31. Sharpless, C. M.; Blough, N. V. The importance of charge-transfer interactions in

544

determining chromophoric dissolved organic matter (CDOM) optical and

545

photochemical properties. Environ. Sci. Process Impacts 2014, 16 (4), 654-671.

546

32. Boyle, E. S.; Guerriero, N.; Thiallet, A.; Vecchio, R. D.; Blough, N. V. Optical

547

properties of humic substances and CDOM: relation to structure. Environ. Sci.

548

Technol. 2009, 43 (7), 2262-2268.

25 ACS Paragon Plus Environment

Environmental Science & Technology

549

33. Vergnoux, A.; Guiliano, M.; Di Rocco, R.; Domeizel, M.; Theraulaz, F.; Doumenq,

550

P. Quantitative and mid-infrared changes of humic substances from burned soils.

551

Environ. Res. 2011, 111 (2), 205-214.

552

34. Fujii, M.; Imaoka, A.; Yoshimura, C.; Waite, T. D. Effects of molecular composition

553

of natural organic matter on ferric iron complexation at circumneutral pH. Environ.

554

Sci. Technol. 2014, 48 (8), 4414-4424.

555

35. Christl, I.; Ruiz, M.; Schmidt, J. R.; Pedersen, J. A. Clarithromycin and tetracycline

556

binding to soil humic acid in the absence and presence of calcium. Environ. Sci.

557

Technol. 2016, 50 (18), 9933-9942.

558

36. Wang, L. F.; Habibul, N.; He, D. Q.; Li, W. W.; Zhang, X.; Jiang, H.; Yu, H. Q.

559

Copper release from copper nanoparticles in the presence of natural organic matter.

560

Water Res. 2015, 68, 12-23.

561

37. Town, R. M.; Van Leeuwen, H. P. Intraparticulate metal speciation analysis of soft

562

complexing nanoparticles. The intrinsic chemical heterogeneity of metal-humic acid

563

complexes. J. Phys. Chem. A 2016, 120 (43), 8637-8644.

564

38. Saggu, M.; Levinson, N. M.; Boxer, S. G. Experimental quantification of

565

electrostatics in X-H··· π hydrogen bonds. J. Am. Chem. Soc. 2012, 134 (46), 18986-

566

18997.

567

39. Markiewicz, M.; Mrozik, W.; Rezwan, K.; Thöming, J.; Hupka, J.; Jungnickel, C.

568

Changes in zeta potential of imidazolium ionic liquids modified minerals-

569

implications for determining mechanism of adsorption. Chemosphere 2013, 90 (2),

570

706-712.

26 ACS Paragon Plus Environment

Page 26 of 33

Page 27 of 33

571 572

Environmental Science & Technology

40. Schneider, G.; Baringhaus, K. H. Molecular design: concepts and applications; Wiley-VCH: Weinheim, 2008.

573

41. Zielińska, K.; Town, R. M.; Yasadi, K.; van Leeuwen, H. P. Partitioning of humic

574

acids between aqueous solution and hydrogel. 2. Impact of physicochemical

575

conditions. Langmuir 2014, 31 (1), 283-291.

576

42. Zhu, G.; Yin, J.; Zhang, P.; Wang, X.; Fan, G.; Hua, B.; Deng, B. DOM removal by

577

flocculation process: fluorescence excitation-emission matrix spectroscopy (EEMs)

578

characterization. Desalination 2014, 346, 38-45.

579

43. Jung, A. V.; Frochot, C.; Bersillon, J. L. Fluorescence spectroscopy as a specific tool

580

for the interaction study of two surfactants with natural and synthetic organic

581

compounds. Colloid Surface A. 2015, 481, 567-576.

582

44. Kučerík, J.; Šmejkalová, D.; Čechlovská, H.; Pekař, M. New insights into

583

aggregation and conformational behaviour of humic substances: application of high

584

resolution ultrasonic spectroscopy. Org. Geochem. 2007, 38 (12), 2098-2110.

585

45. Nebbioso, A.; Piccolo, A. Molecular rigidity and diffusivity of Al3+ and Ca2+

586

humates as revealed by NMR spectroscopy. Environ. Sci. Technol. 2009, 43 (7),

587

2417-2424.

588 589

46. Koopal, L. K.; Goloub, T. P.; Davis, T. A. Binding of ionic surfactants to purified humic acid. J Colloid Interface Sci. 2004, 275 (2), 360-367.

590

47. Chaaban, A. A.; Lartiges, B.; Kazpard, V.; Plisson-Chastang, C.; Michot, L.;

591

Bihannic, I.; Caillet, C.; Prelot, B. Probing the organization of fulvic acid using a

592

cationic surfactant. Colloid Surface A. 2016, 504, 252-259.

593

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Figure captions

594 595 596 597

Figure 1. Effect of IL concentrations on (a) average particle size; and (b) zeta potential of HA

598 599

Figure 2. Spectral responses of HA to ILs: (a) synchronous fluorescence contour maps of

600

HA in the 250-550 nm region; (b) FTIR absorbance spectra; and (c) differential

601

IR absorbance spectra of the freeze-dried HA

602 603 604

Figure 3. Synchronous and asynchronous 2DCOS maps generated from the synchronous fluorescence (a, b) and FTIR (c, d) analysis of HA with IL binding

605 606

Figure 4. PCMW analysis generated from the IL concentration-dependent FTIR spectra

607

of HA (a) synchronous map; (b) asynchronous map; and (c) transition

608

concentration (□) as well as the onset and end concentrations (▲, ▼) of

609

various groups of HA

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Figure 1

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Figure 2

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Figure 3

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Figure 4

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