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Synthesis and Characterization of a Novel Hydroquinone Sulfonate-Based Redox Active Ionic Liquid

Introducing redox-active moieties into an ionic liquid (IL) structure is an exciting and attractive approach that has received increasing interest over recent years for a various range of energy applications. The so-called redox-active ionic liquids (RAILs) provide a highly versatile platform to potentially create multifunctional electroactive materials. Ionic liquids are molten salts consisting of ionic species, often having a melting point lower than 100 °C. Such liquids are obtained by combining a bulky asymmetric organic cation and a small anion. Here, we report on the synthesis of a novel RAIL, namely 1-butyl-3-methylimidazolium hydroquinone sulfonate ((BMIM)(HQS)). (BMIM)(HQS) was synthesized in a two-step procedure, starting by the quaternization of methylimidazole using butylchloride to produce 1-butyl-3-methylimidazolium chloride ((BMIM)(Cl)), and followed by the anion exchange reaction, where the chloride anion is exchanged with hydroquinone sulfonate. The resulting product was characterized by 1H NMR, 13C NMR, FT-IR spectroscopy, themogravimetric analysis, and differential scanning calorimetry, and shows a high stability up to 340 °C. Its electrochemical behavior was investigated using cyclic voltammetry at different temperatures and its viscosity analysis was also performed at variable temperatures. The electrochemical response of the presented RAIL was found to be temperature dependent and diffusion controlled. Overall, our results demonstrated that (BMIM)(mix of HQS and HSQ) is redox active and possesses high stability and low volatility, leading to the employment of this RAIL without any additional supporting electrolyte or additives.


Introduction
Over the past two decades, ionic liquids (ILs) have received a great deal of attention, and extensive work has been devoted to developing their practical applications in various fields [1]. Many of the early studies have focused on the 'green' chemistry potential of these compounds, with a particular interest oriented towards replacing the organic solvents in homogeneous catalysis [2,3]. The unique property of ionic liquids that makes them environmentally suitable for these purposes is their intrinsic low vapor pressure, which has significant advantages when replacing highly volatile organic solvents [1]. Later on, ILs have been extensively studied in organic synthesis and materials chemistry [4,5], where they demonstrated their versatility and large range of applicability, not only as excellent solvents but, in many cases, in a more active role. For example, in the synthesis of porous materials (including zeolites and metal organic frameworks (MOFs)), ILs act as templates or structure directing agents, in addition to their principal role as reaction solvent [5]. Some physical and chemical key properties of ILs that make them attractive for many applications include their solubility and miscibility with water and many other solvents, intrinsic ionic conductivity, broad electrochemical potential window, good thermal stability, and very high boiling points [1].
However, the applicability of ILs is not limited only to the areas of catalysis and synthetic chemistry, as extensive research works have demonstrated their utility in diverse fields of technology, from energy applications, electropolishing, and electrodeposition to the use of supported ionic liquid as an electrocatalyst [6][7][8]. The application of ILs in the energy sector is likely the most appealing research area nowadays, especially for the development of energy conversion and storage materials and devices [9,10]. This is driven by the continuous need for the development of innovative systems in order to overcome the issues associated with the existing materials, and hence achieve the main goal of sustainable, safe, and cost-effective systems [9]. For example, lithium-ion batteries [11], despite their many advantages, still suffer from major safety issues, especially when they are employed on a large scale or high temperatures, due to the flammability of organic electrolytes. In this regard, ILs can serve as advanced materials to overcome these issues [12]. Another promising application could be represented by redox flow batteries (RFBs), which possess many attractive properties that make them excellent potential candidates for high energy density grid scale storage [13]. In this scenario, aqueous RFBs have limited cell voltage. While nonaqueous RFBs offer wider electrochemical windows, in exchange for the poor solubility of electroactive materials, which result in low energy density. In this context, the use of ILs for RFBs holds the potential to further advance this technology [14,15].
In addition to the many advantages of ILs previously described, the appeal of ILs in electrochemical applications is driven by their three key features, namely (i) their ionic conductivity, (ii) their large electrochemical potential window, and (iii) their thermal stability. The large electrochemical window may prevent side reactions, and the thermal stability allows for operation over wide ranges of temperatures. Another important feature of ILs that has attracted academic interest is the possibility of rationally altering their physical and chemical properties by varying the anion or the cation elements, or by introducing specific functionalities into the cation and/or anion, also known as task specific ILs (TSILs). This property stimulated the electrochemistry community to design novel ILs where the structure can be tailored to include redox active species; hence, they can be used not only as electrolytes but also as redox species or redox shuttles [16,17].
The concept of redox active IL (RAIL) is very intriguing, and research in this field is very promising, as this may pave the way for the development of new or improved electrochemical technologies [18,19].
ILs have widely been investigated as potential safe electrolytes for many electrochemical devices, and there are many reports on IL-based redox systems [20]. While some success was indeed achieved in terms of safety and increased cell voltages [21,22], the issue of solubility for these redox materials is still a major challenge [7]. In this context, RAILs present an elegant approach for increasing the concentration of redox active species in electrolytes, while overcoming the issue of poor solubility. This strategy extends the practicability of ILs beyond they mere role of inert electrolytes.
It is worth mentioning that ionic liquids with redox active moieties were know even before the modern definition of RAILs was introduced. This can be demonstrated by the work reported by Shreeve et al. [23], Kumar et al. [24] and Liu et al. [25] on the first ferrocenylmethylimidazolium and ferrocenylmethyltriazolium, the first viologen-based liquid crystalline containing "bis trifluromethylsulfonylimide" (TFSI)) as counter anion, and the first homogeneous mixture of vanadate, 2,2,6,6-tetramethyl-1-piperidinyloxy (TEMPO), acid functionalized ionic liquids, respectively. However, an enormous interest was devoted to the synthesis and application of these systems in energy in the past decade. This is driven by the need to achieve a liquid state system with high redox density. Some important recent studies on metal-and nonmetal-based RAILs are highlighted in Table 1, and a few selected examples are discussed below. Very recently, Sagara et al. [26] reported a charge transfer (CT) RAIL prepared by mixing carbazole-based and viologen-based RAILs. In their study, it was shown that mixing the two RAILs lead to unique properties that are distinct from those of the isolated components. Wang et al. [27] synthesized a RAIL bearing the redox active 2,2,6,6-tetramethyl-1-piperidinyloxy bis trifluromethylsulfonylimide (TFSI) for potential application in lithium oxygen batteries. It was demonstrated that adding this RAIL to diethylene glycol diethyl ether (DEGDME) leads to exceptional properties compared to pure DEGDME. A family of RAILs bearing the anthraquinone sulfonate (AQS) as anionic counterpart [28] were reported with different cations including phosphonium, ammonium, imidazolium, piperidinium, and pyrrolidinium. Among them only (P14,6,6,6) was found to be liquid at RT; this can be explained by the symmetry and planarity of the AQS core, coupled with the significant pi-pi intermolecular interaction between anthraquinone moieties, which favor a long-range order rather than liquefaction. In the attempt to achieve an ideal liquid system with a density of redox species close to the solid state, an excellent work has been reported by Fontaine et al. [29] on a bi-redox IL comprising a triflimide anion bearing the redox active anthraquinone (AQ-TFSI) and a methyl imidazolium cation bearing the redox active TEMPO. Rochford et al. [30] reported the synthesis of a RAIL based on 2,5-ditert-butyl-1,4-dimethoxybenzene (DDB) and a triflimide anion. This RAIL was highly soluble in carbonate-based electrolytes and holds the potential to be an excellent functional additive in Li-ion battery electrolytes, as it can act as redox shuttle for Li 4 Ti 5 O 12 /LiFePO 4 lithium-ion batteries.
Despite the significant advancements in the field of RAILs, the development of an optimized system in the liquid state offering a high density of redox species still remains very challenging.
While functionalizing ILs and introducing electroactive species is relatively straightforward, and might be easily accomplished using the common preparative methods for the synthesis of TSILs, [31] developing RAILs add other requirements, which make their preparation very challenging. As a matter of fact, it is well known that a fairly narrow range of ILs structures are liquids at RT, and only a very few of the reported RAILs are liquids at RT [15,19,23,25,32,33], as illustrated in Table 1.  Hydroquinone is a simple typical and important electroactive molecule well-known in fundamental electrochemistry research [36]. Despite being heavily studied, there is no report, to the best of our knowledge, of using this simple molecule as a component of RAIL. Although, and as mentioned above, some RAILs having bulkier molecules (such as viologen [28] and anthraquinone [37]) have been reported, the vast majority of the electrochemical studies of these RAILs were reported using an additional solvent such as acetonitrile [37,38]. The simplicity of the hydroquinone anion combined with a suitable cation may result in a RAILs that is liquid at room temperature (RT) with an optimum viscosity. This property is crucial in order to achieve solvent free electrochemical systems for many energy storage applications (such as redox flow batteries).
Recently, the topic of redox-active ionic liquids (RAILs) has resulted in a tremendous increase in terms of publications. Figure 1a displays the recent references related to the RAIL field from 2007 to 2021, showing a constant and continual increase. Looking to Figure 1b, one might notice that the most influential disciplines are Chemistry, Materials Science, and Chemical Engineering with emergence in other closely related fields such as Energy. While the scientific articles are dominating this publication domain, as shown in Figure 1c, only a small percentage of reviews articles are available so far (~3.6% of the published documents), and it would be interesting to contribute to filling this critical gap.
As part of our research interest in developing this burgeoning area further, we here report the synthesis and characterization of a new electrochemically active ionic liquid, 1-butyl-3-methyimidazolium hydroquinone sulfonate ((BMIM)(HQS)), having the redox species hydroquinone sulfonate as the anion. The studied RAIL result liquid at room temperature and characterized by a low water content. The electrochemical response of the developed RAIL was investigated at a wide range of temperatures, ranging from 20 to 70 • C, without any additional supporting electrolyte or additives. Viscosity and thermogravimetry analysis confirmed the high stability and low volatility of (BMIM)(HQS). All published languages were included. All document types, including journal and conference articles, report paper, conference proceeding, and monograph published chapters were recorded. Statistics are available from 2007 to April 2021, inclusively. Data were collected from Scopus Expertly curated abstract and citation database based information service.

Materials and Methods
All chemicals were purchased from Sigma Aldrich (Saint Luis, MO, USA) and used without further purification. All reactions were carried out under inert nitrogen atmosphere.
Products were characterized using 1 H NMR, 13 C NMR, FT-IR and TGA. Samples for NMR analyses were prepared by dissolving 20 mg of the product in about 0.5 mL of deutrated solvent (CDCl3/CD3OD). NMR spectra were recorded on a Bruker AVANCE III HD 800 MHz NMR spectrometer (Billerica, MA, USA) equipped with a 5 mm BBO H&F cryoprobe. NMR data were reported using the Aspin-NMR Data Reporting Tool (V 1.0). [39] FT-IR measurements were carried out using a Thermo Scientific Nicolet iS50 FTIR spectrometer (Waltham, MA, USA), via the KBr pellets method. The mass of the products was recorded using Thermo Scientific TSQ Quantitativa Quadrupole Mass Spectrometer (Waltham, MA, USA) by dissolving the samples in methanol.
The thermal stability of the products was examined by the thermogravimetric analyzer TA SDT Q600 TGA (New Castle, DE, USA). Samples were heated over temperatures between 20 to 600 °C under an oxygen atmosphere at a heating rate of 20 °C/min. In addition, melting point was measured with DSC-Q2000 (TA Instruments, New Castle, DE, USA) differential scanning calorimetry. The samples for DSC analysis were 10-20 mg; the heating and cooling rate was 10 °C min −1 over a temperature range of −70-+150 °C and the carrier gas was nitrogen. The samples were placed in an aluminum crucible. The DSC traces are reported in the ESI.
All electrochemical measurements were performed on SP-300 potentiostat controlled by EC-Lab software using a Three-electrode cell setup with a 5 mm diameter glassy carbon as working electrode, Ag/AgCl reference electrode and a platinum mesh counter electrode. Cyclic voltammetry was carried out using 10 mV/s scan rate and was performed at temperatures ranging from RT (21 °C) to 70 °C.
Viscosity was measured using Discovery HR-2 hybrid rheometer at temperatures ranging from 20 to 70 °C. All published languages were included. All document types, including journal and conference articles, report paper, conference proceeding, and monograph published chapters were recorded. Statistics are available from 2007 to April 2021, inclusively. Data were collected from Scopus Expertly curated abstract and citation database based information service.

Materials and Methods
All chemicals were purchased from Sigma Aldrich (Saint Luis, MO, USA) and used without further purification. All reactions were carried out under inert nitrogen atmosphere.
Products were characterized using 1 H NMR, 13 C NMR, FT-IR and TGA. Samples for NMR analyses were prepared by dissolving 20 mg of the product in about 0.5 mL of deutrated solvent (CDCl 3 /CD 3 OD). NMR spectra were recorded on a Bruker AVANCE III HD 800 MHz NMR spectrometer (Billerica, MA, USA) equipped with a 5 mm BBO H&F cryoprobe. NMR data were reported using the Aspin-NMR Data Reporting Tool (V 1.0). [39] FT-IR measurements were carried out using a Thermo Scientific Nicolet iS50 FTIR spectrometer (Waltham, MA, USA), via the KBr pellets method. The mass of the products was recorded using Thermo Scientific TSQ Quantitativa Quadrupole Mass Spectrometer (Waltham, MA, USA) by dissolving the samples in methanol.
The thermal stability of the products was examined by the thermogravimetric analyzer TA SDT Q600 TGA (New Castle, DE, USA). Samples were heated over temperatures between 20 to 600 • C under an oxygen atmosphere at a heating rate of 20 • C/min. In addition, melting point was measured with DSC-Q2000 (TA Instruments, New Castle, DE, USA) differential scanning calorimetry. The samples for DSC analysis were 10-20 mg; the heating and cooling rate was 10 • C min −1 over a temperature range of −70-+150 • C and the carrier gas was nitrogen. The samples were placed in an aluminum crucible. The DSC traces are reported in the ESI.
All electrochemical measurements were performed on SP-300 potentiostat controlled by EC-Lab software using a Three-electrode cell setup with a 5 mm diameter glassy carbon as working electrode, Ag/AgCl reference electrode and a platinum mesh counter electrode. Cyclic voltammetry was carried out using 10 mV/s scan rate and was performed at temperatures ranging from RT (21 • C) to 70 • C.
Viscosity was measured using Discovery HR-2 hybrid rheometer at temperatures ranging from 20 to 70 • C.

Results and Discussion
1 H NMR and 13 C NMR confirm the molecular structure of (BMIM)(Cl), and NMR data are comparable with the literature [40] (NMR spectra are reported in the ESI). The successful exchange of the chloride with hydroquinone sulfonate in (BMIM)(HQS) is clearly indicated in both 1 H NMR and 13 C NMR by the presence of the characteristic peaks of hydroquinone sulfonate with three additional peaks, observed in 1 H NMR of (BMIM)(HQS) in the range between 6.6-7.2 ppm, attributed to the aromatic protons in HQS. In addition to that, 13 C NMR spectrum illustrates the characteristic additional carbon peaks of hydroquinone sulfonate in the 110-160 ppm range. These results clearly demonstrate that the synthesis of (BMIM)(HQS) was successfully achieved. The 1 H NMR analysis for (BMIM)(HQS) revealed a strong attenuation of the NCHN peak (BMIM fragment) speculatively attributed to the acidity of this proton and accordingly a proton exchange with the HQS fragment or with the solvent.
The incorporation of hydroquinone sulfonate as an anion in (BMIM)(HQS) was further confirmed using FT-IR. In the FT-IR, when infrared photons hit the sample, some wavelengths are absorbed while other pass through (i.e., transmitted). The resulting signal spectrum represent a footprint of the sample, with typical fingerprint signal for specific molecular functional groups. As shown in Figure 2, the IR spectrum for (BMIM)(HQS) shows the clear characteristic (S=O) peak located in the range of 1322 −1149 cm −1 and (S-O) peak at around 1072 cm −1 . In addition to that, the large broad peak in the range of 3400-3300 cm −1 in (BMIM)(Cl) is not present in (BMIM)(HQS). The presence of this specific peak usually refers to an extensive H-bonding network between water molecules and the imidazolium cations [41]. As chloride ions are silent towards NMR analysis, and the FT-IR spectra of the ILs here reported do not provide quantitative information, to estimate the purity of (BMIM)(HQS) we have performed gravimetric silver nitrate test. This revealed the presence of 3.8% mol/mol of chloride traces with respect to BMIM HQS. (ii) Synthesis of (BMIM)(HQS) (BMIM)(Cl) (24 g, 0.137 mol) was dissolved in 40 mL of methanol. After that, an excess of potassium hydroquinone sulfonate (36 g, 0.157 mol) was added. The mixture was stirred at room temperature (21 • C) for 72 h, after which the KCl precipitate was removed by filtration. Then dry acetone was added, and the precipitate was removed via filtration. This last step was repeated 3-4 times until no further precipitation was observed. Solvents were removed using rotavapor and the resulting product was dried under high vacuum at 60 • C for 24 h. Yield: 70%.
The viscous liquid product was stored under inert atmosphere. 1

Results and Discussion
1 H NMR and 13 C NMR confirm the molecular structure of (BMIM)(Cl), and NMR data are comparable with the literature [40] (NMR spectra are reported in the ESI). The successful exchange of the chloride with hydroquinone sulfonate in (BMIM)(HQS) is clearly indicated in both 1 H NMR and 13 C NMR by the presence of the characteristic peaks of hydroquinone sulfonate with three additional peaks, observed in 1 H NMR of (BMIM)(HQS) in the range between 6.6-7.2 ppm, attributed to the aromatic protons in HQS. In addition to that, 13 C NMR spectrum illustrates the characteristic additional carbon peaks of hydroquinone sulfonate in the 110-160 ppm range. These results clearly demonstrate that the synthesis of (BMIM)(HQS) was successfully achieved. The 1 H NMR analysis for (BMIM)(HQS) revealed a strong attenuation of the NCHN peak (BMIM fragment) speculatively attributed to the acidity of this proton and accordingly a proton exchange with the HQS fragment or with the solvent.
The incorporation of hydroquinone sulfonate as an anion in (BMIM)(HQS) was further confirmed using FT-IR. In the FT-IR, when infrared photons hit the sample, some wavelengths are absorbed while other pass through (i.e., transmitted). The resulting signal spectrum represent a footprint of the sample, with typical fingerprint signal for specific molecular functional groups. As shown in Figure 2, the IR spectrum for (BMIM)(HQS) shows the clear characteristic (S=O) peak located in the range of 1322 −1149 cm −1 and (S-O) peak at around 1072 cm −1 . In addition to that, the large broad peak in the range of 3400-3300 cm −1 in (BMIM)(Cl) is not present in (BMIM)(HQS). The presence of this specific peak usually refers to an extensive H-bonding network between water molecules and the imidazolium cations [41]. As chloride ions are silent towards NMR analysis, and the FT-IR spectra of the ILs here reported do not provide quantitative information, to estimate the purity of (BMIM)(HQS) we have performed gravimetric silver nitrate test. This revealed the presence of 3.8% mol/mol of chloride traces with respect to (BMIM)(HQS).
Coulometric water content determination is primarily used for the determination of small amounts of water in the ppm range. In a coulometric titrator, electric current is used to generate the iodine needed for the Karl Fischer reaction. The current releases a stoichiometrically corresponding amount of iodine from the iodide-containing reagent. (BMIM)(Cl) is found to be highly hygroscopic and is more prone to quick hydration by absorbing moisture from the air. In contrast, (BMIM)(HQS) is more stable in air and does not absorb moisture, despite being soluble in water. This has been confirmed by the coulometric KF titration method. The moisture content in (BMIM)(HQS) was found to be 0.1% whereas (BMIM)(Cl) has been reported around 6.85% [42]. This is a relevant and representative example that demonstrates how changing the ILs anion can efficiently affect the final physical properties of the compound. Figure 3 shows the cyclic voltammogram for (BMIM)(HQS) recorded at different temperatures. At room temperature (21 • C) the potential difference between the anodic peak and its associated cathodic peak (∆E = 0.8 V) is high enough to indicate that the kinetic is fairly slow. Similar behavior was previously reported for the electrochemistry of hydroquinone dissolved in the non-active IL 1-butyl-3-methyimidazolium hexafluorophosphate (BMIM)(PF 6 ) and 1-butyl-3-methylimidazolium tetrafluroborate (BMIM)(BF 4 ) [37]. The same trend was also reported for the behavior of hydroquinone in acetonitrile [38]. Instead, reduction processes at the BMIM cationic fragment typically occur at more negative potentials, outside the electrochemical window here investigated [43]. Coulometric water content determination is primarily used for the determin small amounts of water in the ppm range. In a coulometric titrator, electric curren to generate the iodine needed for the Karl Fischer reaction. The current releases a ometrically corresponding amount of iodine from the iodide-containing (BMIM)(Cl) is found to be highly hygroscopic and is more prone to quick hydr absorbing moisture from the air. In contrast, (BMIM)(HSQ) is more stable in air a not absorb moisture, despite being soluble in water. This has been confirmed by lometric KF titration method. The moisture content in (BMIM)(HSQ) was found to whereas (BMIM)(Cl) has been reported around 6.85% [42]. This is a relevant an sentative example that demonstrates how changing the ILs anion can efficiently a final physical properties of the compound. Figure 3 shows the cyclic voltammogram for (BMIM)(HSQ) recorded at d temperatures. At room temperature (21 °C) the potential difference between the peak and its associated cathodic peak (ΔE = 0.8 V) is high enough to indicate tha netic is fairly slow. Similar behavior was previously reported for the electrochem hydroquinone dissolved in the non-active IL 1-butyl-3-methyimidazolium hex phosphate (BMIM)(PF6) and 1-butyl-3-methylimidazolium tetrafluroborate (BMI [37]. The same trend was also reported for the behavior of hydroquinone in ace [38]. Instead, reduction processes at the BMIM cationic fragment typically occur negative potentials, outside the electrochemical window here investigated [43]. The cyclic voltammograms depicted in Figure 4 show a clear dependence of the peak positions and peak current intensity on the temperature. It is clear that there is a significant reduction in peak potential separation (ΔE); hence, the kinetics were improved at The cyclic voltammograms depicted in Figure 4 show a clear dependence of the peak positions and peak current intensity on the temperature. It is clear that there is a significant reduction in peak potential separation (∆E); hence, the kinetics were improved at higher temperatures, together with a significant increase in the peak current intensity as shown in Figure 5. This indicates that increasing the temperature considerably reduces the viscosity of the IL, which allows for an increase in the diffusion rate of the active species.  As illustrated in Figure 6, the effect of increasing the temperature on the viscosity of (BMIM)(HSQ) was experimentally validated by measuring the viscosity of (BMIM)(HSQ) over the temperatures range 20-70 °C. The initial viscosity of 5640 mPa·s drastically dropped with increasing the temperature, reaching 186 mPa·s at 70 °C. This is a crucial factor to consider, since a redox flow battery is likely to be operated at different temperatures. The measured viscosities are anyway higher than those reported for imidazole-  As illustrated in Figure 6, the effect of increasing the temperature on the viscosity of (BMIM)(HSQ) was experimentally validated by measuring the viscosity of (BMIM)(HSQ) over the temperatures range 20-70 °C. The initial viscosity of 5640 mPa·s drastically In general, when ∆E is higher than 600 mV, the hydroquinone/quinone system is considered quasireversible or slow. However, in this system, the active species (HQ/Q) are in the form of ionic liquid and, as explained above, the viscosity can greatly affect the cyclic voltammetry behavior. This can be demonstrated from the electrode response upon increased temperature. As temperature increases, ∆E decreases. This indicates that the system is reversible, but its electrochemical behavior is being affected by the viscosity. Furthermore, the HQ/Q redox couple is well known for its reversibility; nevertheless, such reversibility (the degree of the anodic and cathodic peak) strongly depends on the nature of the working electrode and electrolyte (medium). Figure 4 shows the cyclic voltammograms of our system using various scan rate at 30 • C. It is evident that the peak current increases nonlinearly with an increasing the scan rate, suggesting a diffusion driven electrochemical redox process. This is not surprising, and a similar electrochemical behavior was reported on a family of metal-based ionic liquids [15].
As illustrated in Figure 6, the effect of increasing the temperature on the viscosity of (BMIM)(HSQ) was experimentally validated by measuring the viscosity of (BMIM)(HSQ) over the temperatures range 20-70 • C. The initial viscosity of 5640 mPa·s drastically dropped with increasing the temperature, reaching 186 mPa·s at 70 • C. This is a crucial factor to consider, since a redox flow battery is likely to be operated at different temperatures. The measured viscosities are anyway higher than those reported for imidazole-based ILs, which usually do not exceed the value of 160 mPa·s at 10 • C [42,44]. On the other hand, the high viscosity of (BMIM)(HQS) is counterbalanced by its low volatility and high thermal stability as discussed below. The thermal stability of (BMIM)(Cl) and (BMIM)(HQS) was determined by thermogravimetric analyzer in order to know their upper temperature limit. (BMIM)(HQS) resulted in a better thermal stability than (BMIM)(Cl), based on the TGA graph in Figure 7. The onset of thermal decomposition started at 261 °C for (BMIM)(Cl), as previously reported in the literature [45], whereas (BMIM)(HQS) started decomposing around 340 °C. This shows a high thermal stability for the RAIL here reported. It well established that anion type plays a major role in determining thermal stability, similar to determining the hydrophobicity of ILs [46,47]. Previous investigations have reported that the thermal stability of ILs with different anions decreases with the increase of the coordinating nature, nucleophilicity, and hydrophilicity of the corresponding anion [46]. This is in agreement with the difference of 80 °C in the onset temperature here measured in favor of HQS anion with respect to Cl. Indeed, it is well known that ILs properties can be tuned by varying The thermal stability of (BMIM)(Cl) and (BMIM)(HQS) was determined by thermogravimetric analyzer in order to know their upper temperature limit. (BMIM)(HQS) resulted in a better thermal stability than (BMIM)(Cl), based on the TGA graph in Figure 7. The onset of thermal decomposition started at 261 • C for (BMIM)(Cl), as previously reported in the literature [45], whereas (BMIM)(HQS) started decomposing around 340 • C. This shows a high thermal stability for the RAIL here reported. It well established that anion type plays a major role in determining thermal stability, similar to determining the hydrophobicity of ILs [46,47]. Previous investigations have reported that the thermal stability of ILs with different anions decreases with the increase of the coordinating nature, nucleophilicity, and hydrophilicity of the corresponding anion [46]. This is in agreement with the difference of 80 • C in the onset temperature here measured in favor of HQS anion with respect to Cl − . Indeed, it is well known that ILs properties can be tuned by varying the cation or the anion or both. This work and several other previous theoretical and experimental studies [48][49][50][51][52][53] clearly demonstrated that changing the ionic liquid anion greatly affects its physical properties (including viscosity, thermal stability, and melting point). As a matter of fact, in a study on several ionic liquids containing macrocyclic fragments [49], it was clearly demonstrated that replacing the halide anions by TFSI anions considerably decrease the melting point of the resulting IL. Similarly in another study [48], the ionic liquid 1-butyl-3-methylimidazolium bis(trifluoromethyl) phosphinate (BMIM (CF 3 )2PO 2 ) did not show a melting point in the temperature range −120 to 100 • C; in contrast, BMIM TFSI has a melting point of −3 • C [48].

Conclusions
The use of RTIL is supported by several crucial factors, which include low volatility, high concentration of redox-active species, high energy density, electrochemical and thermal stability so they can be used at moderate and even high temperatures. Here we reported the successful synthesis of (BMIM)(HSQ) bearing the electrochemically active hydroquinone sulfonate as an anion. The electrochemical characterization was performed on the sole RAIL with no other additives or solvents, revealing a diffusion driven electrochemical redox process, affected by a fairly slow kinetic. Replacement of the halide (chloride) anion with an organic (HSQ) anion resulted, as expected, in a lower water content of the final IL (higher hydrophobicity), together with a higher viscosity and higher thermal stability. This study demonstrates that ILs can be functionalized to include simple redox active species; thus, the RAILs can be used without any additional supporting electrolyte or additives. Of course, further studies are needed on the application of our system into electrochemical devices. For instance, studying the behavior of this novel RAIL with different electrode materials, including both carbonaceous and noncarbonaceous, will result in very useful findings. In this regard, we have already conducted an initial study using carbon paper as working electrode (JNTG carbon paper), which gave similar results compared to glassy carbon and the preliminary voltammograms are reported in the ESI.
In the future, the use of molecular engineering will add a further step to this study

Conclusions
The use of RTIL is supported by several crucial factors, which include low volatility, high concentration of redox-active species, high energy density, electrochemical and thermal stability so they can be used at moderate and even high temperatures. Here we reported the successful synthesis of (BMIM)(HSQ) bearing the electrochemically active hydroquinone sulfonate as an anion. The electrochemical characterization was performed on the sole RAIL with no other additives or solvents, revealing a diffusion driven electrochemical redox process, affected by a fairly slow kinetic. Replacement of the halide (chloride) anion with an organic (HSQ) anion resulted, as expected, in a lower water content of the final IL (higher hydrophobicity), together with a higher viscosity and higher thermal stability. This study demonstrates that ILs can be functionalized to include simple redox active species; thus, the RAILs can be used without any additional supporting electrolyte or additives. Of course, further studies are needed on the application of our system into electrochemical devices. For instance, studying the behavior of this novel RAIL with different electrode materials, including both carbonaceous and noncarbonaceous, will result in very useful findings. In this regard, we have already conducted an initial study using carbon paper as working electrode (JNTG carbon paper), which gave similar results compared to glassy carbon and the preliminary voltammograms are reported in the ESI.
In the future, the use of molecular engineering will add a further step to this study by modifying the anion/cation in order to achieve an optimum system with comparable stability but lower viscosity. Clearly, the flexibility and the possibility of designing a large number of hydroquinone-containing RTILs offer great opportunities for the development of new or improved electrochemical technologies, and the field is still widely open for further explorations and studies.