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Studies of volumetric and transport properties of ionic liquidwater mixtures and its viability to be used in absorption systems Pablo B Sánchez, Josefa García, Josefa Salgado, and Elisa Gonzalez-Romero ACS Sustainable Chem. Eng., Just Accepted Manuscript • DOI: 10.1021/ acssuschemeng.6b01541 • Publication Date (Web): 16 Aug 2016 Downloaded from http://pubs.acs.org on August 20, 2016
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Studies of volumetric and transport properties of
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ionic liquid-water mixtures and its viability to be
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used in absorption systems
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Pablo B. Sáncheza, Josefa Garcíaa,*, Josefa Salgadob, Elisa González-Romeroc,*
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a
8 9
b
10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31
Departamento de Física Aplicada, Universidad de Vigo-Campus Vigo, Lagoas-Marcosende s/n, 36310-Vigo, Spain
Departamento de Física Aplicada, Universidad de Santiago de Compostela-Campus Vida, 15782-Santiago de Compostela, Spain c
Departamento de Química Analítica y Alimentaria, Universidad de Vigo-Campus Vigo, Lagoas-Marcosende s/n, 36310-Vigo, Spain
Pablo B. Sánchez:
[email protected] Josefa García:
[email protected] Josefa Salgado:
[email protected] E. González-Romero:
[email protected] *
Corresponding authors: Dr. J. García Tel.: +34 986 818 753; Fax: +34 986 812 322 E-mail address:
[email protected] (J. García) Dr. E. González-Romero Tel.: +34 986 812 240; Fax: +34 986 812 322 E-mail address:
[email protected] (E. González-Romero, responsible of submission)
KEYWORDS: Ionic Liquid; density; viscosity; electrical conductivity; proton activity; absorbent
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ABSTRACT: Binary systems of two ionic liquids (ILs), 1-ethylpyridinium methanesulfonate
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[C2Py][MeSO3] and choline dihydrogenphosphate [Chol][H2PO4], and water have been experi-
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mentally studied. Density, viscosity, electrical conductivity and proton activity have been meas-
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ured at several temperatures covering all the miscibility range. From density data, isobaric coef-
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ficient of thermal expansion was calculated to study the volumetric behavior of the mixtures. All
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volumetric data were fit using polynomial equations. Vogel-Fulcher-Tamman (VFT) equation
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accurately describes the temperature dependence of viscosity for all systems. Systems based on
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[C2Py][MeSO3] are less dense and viscous than those involving [Chol][H2PO4], making
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[C2Py][MeSO3] more suitable for absorption systems where pumping cost has a significant im-
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portance. Electrical conductivity data were adjusted using Casteel-Amis equation. Similar trends
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were found for both systems, although ionic conductivity is higher for [C2Py][MeSO3] + H2O
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mixtures. The relation between viscosity and electrical conductivity was also explored. Accord-
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ing to Walden plots, ILs present low ionicity, however, internal friction and ionic concentration
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does not seem to be enough to explain the behavior of ionic conductivity and IL concentration.
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Proton activity measurements show different tendencies with molar fraction of each IL,
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[C2Py][MeSO3] leads to lower paH+ values than [Chol][H2PO4] in the binary mixtures. Results of
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ionic conductivity and proton activity suggest a higher corrosive potential of [C2Py][MeSO3] +
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H2O, however, a further analysis needs to be done to evaluate this risk in absorption systems.
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Finally, a composition analysis based on ionic chromatography (IC) was carried out to obtain
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insight about its effect on their physicochemical properties.
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INTRODUCTION
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Reducing the footprint of energy production systems is one of the main challenges for scien-
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tific and industrial communities. As a consequence, environmentally friendly technologies that
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may help reduce the use of natural resources are gaining presence and visibility over recent
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years. Among the consumption sectors, the heating and cooling industry occupies a considerable
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part of the overall numbers. In this field, one alternative to traditional heat pumps based on com-
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pression devices is absorption heat pumps1. In absorption systems, thermal energy works as a
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driving force instead of electric power used for mechanical compressors, thus, it brings the op-
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portunity of recovering heat disposal or using solar energy to satisfy heating and cooling de-
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mands. Nevertheless, commercial absorption systems based mainly on two working pairs (refrig-
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erant/absorbent), H2O/LiBr and NH3/H2O, present several drawbacks2; corrosion and crystalliza-
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tion problems in case of water and lithium bromide and low relative volatility and toxicity in
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case of ammonia and water. Therefore, the use of working pairs based on water and ionic liquid
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(H2O/IL) appears as a suitable option3–5 since their properties are expected to allow an efficient
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absorption/desorption process and to overcome the disadvantages of the commercial systems. It
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is important to define the target properties for a fluid to fit the requirements of the absorption
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process. i) Wide liquid range renders flexibility for temperatures in the absorber and the genera-
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tor, liquid-solid transitions and decomposition temperature provide the lower and upper limit of
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the liquid range.2 ii) Heat and mass transfer are crucial for absorption systems to work efficiently,
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thus, low viscosities and high thermal conductivities will improve the performance of the absorp-
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tion system.6 iii) Thermodynamics of the absorption process is also a critical issue for refrigera-
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tion systems, negative enthalpies of the mixture (H2O/IL), negative deviation of Raoult´s law and
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low water vapor pressure are target properties for absorption working pairs7. In addition, a low
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corrosive potential is also important to avoid the problem caused by H2O/LiBr.
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Ionic liquids (ILs) are salts melting under 100 ºC8. Despite there being no physical significance
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at that temperature9, it has become a commonly used definition. It is also very frequent to talk
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about room temperature ionic liquids (RTILs), when IL melting temperature is about 20-30 ºC. It
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is again a diffuse definition as there is no unique room temperature and melting points cannot be
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predicted with accuracy10. Since the ILs studied in this work, [C2Py][MeSO3] (1-ethylpyridinium
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methanesulfonate) and [Chol][H2PO4] (choline dihydrogenphosphate), are solid at room tem-
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perature, a definition based on the chemical structure and the physical and chemical properties
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was found to be more appropriate.
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ILs are usually based on an organic cation and an inorganic polyatomic anion11. It leads to
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unique properties, among them, their very low (but measurable) vapor pressure12; wide liquid
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range, caused by low melting points13,14 and high thermal stabilities15; wide electrochemical
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windows16 make ILs environmental friendly candidates for different applications17–19.
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Ionic liquids melting above room temperature present some drawbacks when physical charac-
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terization needs to be done. Difficulties during the drying process or possible damages in the
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experimental equipment caused by solidification are issues to deal with. Nevertheless, since in-
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dustrial applications very often involve mixtures of ILs with different solvents instead of pure
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components, we have chosen to study the behavior of water + IL mixtures. By doing so, we
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avoid the problem of manipulating solid ILs and we obtain useful information to evaluate wheth-
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er studied systems may work satisfactorily as working pairs for absorption heat pumps.
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Although the properties of water + IL mixtures have been broadly studied20–24, there is still a
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lack of data of water mixtures for many ILs. Hereby, mixtures of water with two ILs with a rela-
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tively high melting point have been studied in the concentration range that solubility allows.
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Thus, protic and aprotic ILs and water mixtures will be assessed, analyzing their volumetric and
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dynamic properties, as well as the proton activity of these solutions.
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In this work, density and viscosity of two water + IL mixtures, [C2Py][MeSO3] and
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[Chol][H2PO4], were measured. These properties provide very useful information for the devel-
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opment of industrial applications. While high densities are usually an advantage that ILs accom-
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plish very often, viscosity values are one the main barriers for the implementation of ILs at in-
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dustrial scale, mainly for low temperature applications. Nevertheless, it does not seem reliable to
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reach organic solvent viscosities due to ILs structures and interactions, alternatives such as high
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temperature applications or mixtures base on ILs together with different solvents may help to
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reduce the viscosity problem. For that reason, effects of temperature and water concentrations
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over the aforementioned properties will be discussed. Electrical conductivity, somehow related
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with other transport properties, is also a remarkable property for ILs, since electrochemical ap-
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plications usually demand a good ionic mobility. A quantitative analysis of the electrical conduc-
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tivity and pH (proton activity, aH+) have been carried out to explore the corrosive potential of the
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studied systems in absorption heat pumps. Moreover, the relationship between all transport prop-
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erties has been analyzed. Finally, a detailed study of the ILs impurities by ion chromatography
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has been also included.
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EXPERIMENTAL SECTION
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Materials and solutions
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Reagents of maximum purity available were purchased from IoLiTec Ionic Liquids Technolo-
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gies GmbH (Heilbronn, Germany). Some details of the compounds selected for this study are
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given in Table 1 and its structures in Scheme S1. Solutions were prepared gravimetrically using a
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digital balance Sartorius CPA225D with an uncertainty of 0.00001 g. The error on the mole frac-
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tion composition of the mixtures induced due to balance uncertainty was estimated to be 5.10−5.
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All reagents used in the chromatographic assays (H2SO4 as regenerating agent, NaHCO3 and
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Na2CO3 as mobile phase) and electrolytes as KH2PO4 were provided by Sigma-Aldrich. The rea-
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gents used as standard solution for the anion quantification by ionic chromatography (analytical
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grade sodium salts of F-, Cl-, Br-, NO3-, PO43- with 12 H2O and SO42-) were obtained from Pan-
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reac and used as received. All diluted solutions were prepared by using Milli-Q grade water. The
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molar fraction range studied for each ILs and the correlation to other concentration units (Molar,
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M, and Mass Percentage, %) are given in Table 2. Notice that the wide concentration range under
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study is for [C2Py][MeSO3] due to both higher solubility and hydroscopic properties observed in
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comparison with [Chol][H2PO4].
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Table 1. Name, Abbreviation, CAS number, purity, molecular weight and melting temperature of the compounds studied in this work Name
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Abbreviation
CAS Number
1-Ethylpyridinium [C2Py][MeSO3] 681481-41-4 methanesulfonate Choline [Chol][H2PO4] 83846-92-8 dihydrogenphosphate a Mass fraction. Information supplied by Iolitec
Puritya
MW (g mol-1)
tm (ºC)
>95%
203.26
6225
>99%
201.16
12626
135 136 137 138
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Table 2. Equivalence of the molar fraction, mass percentage and molar concentration for the systems studied. xIL 0.0039 0.0168 0.0317 0.0650 0.1842 0.3830 0.0400 0.0163 0.0316 0.0620 0.1651
%Mass [C2Py][MeSO3] 4.25 16.15 26.96 43.96 71.81 87.40 [Chol][H2PO4] 4.27 15.58 26.71 42.48 68.82
M /mol L-1 0.21 0.77 1.26 1.97 3.00 3.52 0.21 0.74 1.22 1.85 2.73
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APPARATUS AND PROCEDURES
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Density and viscosity measurements
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Density and dynamic viscosity measurements of the pure liquids and mixtures were performed
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with a rotational viscometer Anton Paar Stabinger SVM3000. The basic operating principles and
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schematic set up of the Stabinger Viscometer are described and laid down in a European Patent
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(EP 0 926 481 A2). The density cell is a glass u-tube, which is excited to produce mechanical
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resonant vibrations according to DIN 51757. The viscosity cell is based on a tube filled with the
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sample in which a hollow measuring rotor floats. The SVM 3000 uses Peltier elements for fast
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and efficient thermostatting. The temperature uncertainty (k = 2) is 0.02 K from T = (288.15 to
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378.15) K. Over the temperature range studied, the expanded viscosity uncertainty (k = 2, 95%
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confidence level) is estimated to be 2%.27 Following the methodology exposed in previous
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works28,29, these uncertainties were checked by means of the viscosity standard oil Cannon
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N350, with maximum deviations of 0.05% and 1.1%, for density and viscosity, respectively. This
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apparatus automatically corrects the influence of viscosity on the measured density.
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Electrical conductivity measurements
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The electrical conductivity was measured with a Crison CM35 conductivimeter at different
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temperatures. The electrodes (two platinum) were placed into the samples at a prefixed tempera-
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ture. Crison Standard solutions of 147 µS . cm-1, 1413 µS . cm-1 and 12.88 mS . cm-1 were used
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for calibration proposes. Further details of the calibration procedure can be found somewhere
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else.30. Electrical conductivity uncertainties are estimated to be 1. 10-2 mS . cm-1.
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Proton activity measurements
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The pH-meter 744 Metrohm was used to obtain the pH measurements. A thermopar is included
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into the electrode body. When it is not in use, the electrode is kept in KCl 3.5 M. The calibration
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with standard buffer solutions of pH 4 and 7 (Metrohm) was done prior to measurements, using
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the Nernst equation31:
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= − 0.059
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The 59.0-mV slope change in the electrode potential results from a 10-fold change in the pro-
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ton concentration of the monovalent ion, H+ (n = 1), and 2.303RT/nF where R is the universal
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gas constant, 8.134 JK−1 mol−1; F is the Faraday constant, 9.648×104 C mol−1; T is the absolute
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temperature in Kelvin and n is the ionic charge of the proton ion.
(1)
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Notice that the Nernst ions of opposite charge tend to associate into loosely bound ion pairs in
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more concentrated solutions, thus reducing the number of ions that are free to donate or accept
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electrons at an electrode. This is because ions in solution interact with each other and with H2O
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molecules. In this way, ions behave chemically like they are less concentrated than they really
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are (or measured). For this reason, the Nernst equation cannot accurately predict half-cell poten-
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tials for solutions in which the total ionic concentration exceeds about 10–3 M, such as is the case
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here (Table 2). Then, if the Nernst equation is applied to more concentrated solutions, the term in
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the equation pH must be expressed in "effective concentrations" or activities of the electroactive
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ionic species as proton activity, being the Nernst equation31 expressed as follows:
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= + 0.059 /
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where n is the ionic charge. The activity coefficient γ (gamma) relates the concentration of a
183 184 185
(2)
proton ion to its activity in a a given solution through the relation aH+ = γ CH+ In these experiments, the “effective” proton concentration (proton activity, aH+) is given by the IL and its interactions with water.
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Measurements by Ion Chromatography (IC)
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The ion chromatographic (IC) method is based on ion-exchange separation mechanisms and
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provides detailed anionic profiles including anionic counterions and impurities. This approach
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can be used for quality assurance, impurity analysis, and trace-level residue analysis. Therefore,
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IC system with conductimetric detection was used to analyze both ionic liquid (IL) anions, [Me-
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SO3]– and [H2PO4]–, which better suited the purpose of low-level quantification of anionic pro-
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files and gave us a better knowledge of the impurities content. The chromatographic system
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(Metrohm, Germany) can be operated with chemical suppression mode (regenerating agents are
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50 mM of H2SO4 and ultrapure water) with auto step when the loop sample is filled. The follow-
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ing components are included: 792 Basic IC chromatograph equipped with a 20 µL loop Rheo-
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dyne injection valve. The column system was a 250x4 mm Metrosep A supp 4 (column packing
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of polyvinyl alcohol with quaternary ammonium groups and particle size of 9 µm), guard col-
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umns and filters. The program used to record the chromatographic data and Data Acquisition
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System was the 792 PC Software Version 1.0 (Metrohm Ltd., Switzerland).The eluent was 1.8
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mM Na2CO3 and 1.7 mM NaHCO3 (standard flow 1 mL . min-1 and pH ≈ 10), freshly prepared,
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which was microfiltered (0.45 µm filter) and degassed (30 min in ultrasonic bath) before use.
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This mobile phase determined that the system peak appeared at a retention time of 9.97 min un-
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der the experimental conditions and column used. The ionic liquids were analyzed at a concen-
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tration of around 10 ppm and its solubility in the mobile phase was previously checked to the
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injection of 20 µL of sample into the chromatographic system.
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RESULTS AND DISCUSSION
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Volumetric properties: density
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Density measurements: density of [C2Py][MeSO3] + H2O and [Chol][H2PO4] + H2O mixtures
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at different temperatures are shown in Table S1. Range of concentrations is determined by the
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miscibility range of the solution, for [C2Py][MeSO3] it goes up to 0.3830 while for
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[Chol][H2PO4] it increases 0.1651, both referred to the molar fraction of IL. Vaporization of wa-
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ter has limited the upper limit of the temperature range. In all cases, density decreases as temper-
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ature goes up, as expected (Figure 1). Data were fit to either linear or to polynomial equations.
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Linear fittings describe the relation between density and temperature very accurately when the
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mixture is concentrated in IL, nevertheless, the accuracy of linear fittings decreases as water
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concentration grows, and thus, polynomial equations of second order were used. Brennecke et al.
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have already pointed out this pattern20 caused by the nonlinear behavior of water density with
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temperature. Fitting parameters together with the R-squared of the fitting are listed in Table S2
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(Supporting Information).
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Figure 1. Experimental density values: a) x [C2Py][MeSO3] + (1-x) H2O mixtures. x=0.0039 (),
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x=0.0168 (), x=0.0317 (●), x=0.0650 (), x=0.1842 (), x=0.3830 (). b) x [Chol][H2PO4] + (1-
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x) H2O mixtures. x=0.0040 (), x=0.0163 (), x=0.0316 (●), x=0.0620 (), x=0.1651 (), fitting
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lines ().
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Despite the concentrations of IL not being identical for both systems, from Figure 1 it is possi-
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ble to state that [Chol][H2PO4] mixtures are denser than mixtures based on [C2Py][MeSO3]. Alt-
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hough, higher densities are desirable for working pairs32, refrigerant/absorbent, it is not, in gen-
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eral, the key criteria to select working fluids for absorption heat pumps.
229 230
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Volumetric behavior can also be analyzed by calculating the isobaric coefficient of thermal expansion, αp, given by:
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= − ( )
232
Trends of αp with temperature are shown in Figure 2. It can be observed that αp increases with
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temperature for all IL concentrations. Note also that the effect of temperature over αp becomes
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smaller as IL concentration grows. It leads to a crossover at about 310 K, the explanation yields
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on the density dependence on temperature for different IL concentrations. Mixtures with higher
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concentrations in IL show linear dependence with temperature while those with higher water
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concentrations show a quadratic dependence. According to equation 3, the slope of trendlines
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shown in Figure 2 is expected to be higher as water concentration of the mixture rises. Even
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though this analysis is qualitatively consistent, to our view, further work needs to be done in or-
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der to establish a relationship between the crossover temperature and the components of the mix-
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ture.
(3)
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Thermal expansion coefficient (αp) shows values lower than 1.6 10-3 K-1 for both ILs. In the
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temperature range studied (from 293.15 K to 343.15 K), these ILs aqueous systems lead to nearly
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identical coefficients of thermal expansion. Thus, αp should not be a criterion to choose one IL
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over the other for some particular application, in this case, as absorbent for water refrigerant in
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an absorption cycle.
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Figure 2. Isobaric expansion coefficients: a) x [C2Py][MeSO3] + (1-x) H2O mixtures at several tempera-
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tures. x=0.0039 (), x=0.0168 (), x=0.0317 (●), x=0.0650 (), x=0.1842 (), x=0.3830 (). b) x
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[Chol][H2PO4] + (1-x) H2O mixtures. x=0.0040 (), x=0.0163 (), x=0.0316 (●), x=0.0620 (),
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x=0.1651 (). Fitting lines ().
252 253 254
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Transport properties: viscosity, electrical conductivity and proton activity
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Viscosity measurements: viscosity of [C2Py][MeSO3] + H2O and [Chol][H2PO4] + H2O mix-
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tures at different temperatures are shown in Table S1 (Supplementary Information). The three-
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parameter Vogel–Fulcher–Tammann (VFT) equation (4) was used to correlate experimental vis-
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cosities as a function of temperature:
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= . (
!
"#
)
(4)
261
being η the dynamic viscosity, and A, B and T0 the fitting parameters reported in Table S3 (Sup-
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porting Information) together with the R-squared of the fitting. Figure 3 illustrates that viscosity
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decreases drastically as temperature rises. Most ionic liquids have undesirable high viscosity; to
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deal with this problem one possible approach is lowering the viscosity by adding a molecular
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solvent. Thus, experimental measurements of both IL + H2O systems show how viscosity de-
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creases as the content of water increases for all temperatures.
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However, the effect of water over viscosity is more important at lower temperatures (Figure 3).
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This pattern was already found for [C2Py][OTf] + H2O systems 29. Dynamic studies at molecular
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scales have pointed out the lubricating action of molecular solvents over the dynamics of ionic
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liquids33,34 for different concentrations of water. A reliable explanation yield on the weakening of
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the coulombic interactions between ions would lead to a higher ionic mobility, and therefore to
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decrease the viscosity of systems.
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Both systems, IL + H2O, present very different solubility. While the most concentrated
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[C2Py][MeSO3] + H2O solution has a molar fraction x[C2Py][MeSO3] = 0.3830, for [Chol][H2PO4]
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the highest molar fraction is x[Chol][H2PO4] = 0.1651 (see Table 2 for concentration equivalences).
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However, by comparing all experimental data, it is possible to establish the viscosity sequence as
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follows, η[C2py][MeSO3] < η[Chol][H2PO4]. Thus, attending to viscosity, systems [C2Py][MeSO3] + H2O
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are found to be more suitable than [Chol][H2PO4] + H2O for absorption systems using water as
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refrigerant.
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Previously, the system [C2Py][OTf] was studied by us as a potential absorbent for absorption
281
heat pumps using water as refrigerant 29. Given that, [C2Py][OTf] and [C2Py][MeSO3] share the
282
same cationic structure, [C2Py]+, a detailed comparison of both systems could provide interesting
283
information about the effect of the anionic structure apart from their suitability to work as absor-
284
bents for absorption heat pumps. Trends of density and viscosity for IL + H2O systems are
285
ρ[C2py][OTf ] > ρ[C2Py][MeSO3] and η[C2py][OTf ] < η[C2py][MeSO3]. Inverse trends are found for both proper-
286
ties, in terms of atomic interactions, the larger charge delocalization caused by the trifluorome-
287
thyl group (CF3) group compared to methyl group (CH3) could explain this effect, since it would
288
smooth the electrostatic interactions and therefore improve ionic mobility, giving place to lower
289
viscosities. It would also lead to the formation of more compacted ionic networks and therefore
290
higher densities. This statement also agrees with their solid-liquid transition temperatures, 16 0C
291
and 620C for [C2Py][OTf] and [C2Py][MeSO3], respectively25.
292 293 294
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295 296 297
Figure 3. Experimental viscosity values: a) x [C2Py][MeSO3] + (1-x) H2O mixtures. x=0.0168 (),
298
x=0.0317 (), x=0.0650 (●), x=0.1842 (), x=0.3830 (). b) x [Chol][H2PO4] + (1-x) H2O mixtures.
299 300 301
x=0.0040 (), x=0.0163 (), x=0.0316 (●), x=0.0620 (), x=0.1651 (). Fitting lines ().
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302
Viscosity measurements show how different ionic structures lead to drastic differences in this
303
property when the mixtures are highly concentrated in IL, especially at low temperatures. These
304
differences become much smaller for diluted solutions where water concentration prevailed over
305
the IL or when temperature rises. Therefore, the addition of an organic solvent or the rising of the
306
working temperature represent two interesting strategies to overcome problems related to the
307
high viscosity of ILs.
308
Electrical conductivity measurements: Figure 4 shows dependence on electrical conductivity
309
(κ) with IL molar fraction (xIL) at several temperatures. Casteel-Amis35 equation (5) was used to
310
fit experimental data. Fitting parameters are given in Table S4 (Supporting Information).
311
$ = $%&' (
'()
'(),+,-
). /01
23
−
5 23,%&' 4
− (
'() "'(),+,'(),+,-
)6
(5)
312
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being κ the electrical conductivity, and κmax, m and n the fitting parameters reported in Table S4
314
(Supporting Information) together with the R-squared of the fitting.
315
A qualitative analysis of Figure 4a and 4b indicates that ionic mobility is higher for
316
[C2Py][MeSO3] than for [Chol][H2PO4] mixtures. Therefore, it is in agreement with the viscosity
317
values, η[C2Py][MeSO3] < η[Chol][H2PO4], since a lower internal friction is expected to improve IL dy-
318
namics and therefore it would favor charge transport. The comparison of the electrical conductiv-
319
ity between the ILs with same cation, [C2Py]+, and different anion, [MeSO3]- and [OTf]-, indi-
320
cates that the trend in conductivity is κ [C2py][OTf ] < κ [C2py][MeSO3], being around 5% lower for
321
[OTf]- counterion.
322
By comparing Figures 4a and 4b again, we observe similar tendencies of ionic conductivity
323
with IL molar fraction. For dilute solutions, κ grows drastically with xIL. Then, all curves reach a
324
maximum at molar fraction about 0.05 and 0.04 for [C2Py][MeSO3] and [Chol][H2PO4] respec-
325
tively, values for each temperature are provided in Table S1 (Supporting Information). After that
326
point, ionic conductivity decreases as concentration of IL grows. This pattern was already found
327
for other binary systems involving IL + H2O systems36–40. Two mechanisms are often mentioned
328
as responsible for this behavior. On one hand the increase in the ionic concentration should lead
329
to higher ionic conductivities since more charge is available to be transported. On the other, the
330
descent in ionic mobility, since interactions (electrostatic and dispersive) between cation-anion
331
and cation-cation become stronger, will have the opposite effect. Therefore, a balance between
332
mechanisms will bring maximum conductivity. To assess this hypothesis, measurements were
333
taken at three different temperatures, from 298 to 333 K. Linear tendencies with positive slope
334
were found in all cases. The effect of temperature over conductivity is more important as IL con-
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centration grows, for [C2Py][MeSO3] goes from 0.013 to 0.16 mScm-1 K-1 and for [Chol][H2PO4]
336
from 0.018 to 0.17 mScm-1 K-1 which is roughly an increase of ten times in the slope when xIL
337
moves from the most diluted solution to the most concentrated (Figure S1 in Supporting Infor-
338
mation).
339 340
Figure 4. Electrical conductivity versus xLI at several temperatures. T=298,15 K (), T=313,15 K
341 342
(), T=333.15 K (●), fitting lines (). a) [C2Py][MeSO3] + H2O. b) [Chol][H2PO4] + H2O.
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Since temperature has critical impact over ionic mobility, we will expect that κmax happens at
344
higher IL concentrations. Although this trend was found, its extent, smaller than expected, sug-
345
gests that other factors may also contribute to κ dependence with xIL33,41.
346
Viscosity and electrical conductivity relationship: The relation between these two properties is
347
often enlightened by Walden´s rule. From equation (6), where Λ is the molar conductivity, η the
348
viscosity and C is a constant; we have obtained the so-called Walden´s plot. Further details can
349
be found somewhere else 42. 8
350
Λ = 9
351
In Figure 5, IL + H2O mixtures with similar IL concentrations are represented. Deviation from
352
the ideal line21 (slope equals to 1) would provide, according to Ueno et al43, a measurement of
353
the ionicity of the IL. Both systems fall into the area of poor ILs, in terms of ionicity, no signifi-
354
cant differences between these systems were found since they show similar ratios between Λ and
355
1/η. Temperature effect is also shown in figure 5. As temperature rises, points are displaced to
356
the right. It is consistent with the fact that temperature effect over viscosity is stronger that its
357
effect over electric conductivity. Previously, several authors have analyzed the behavior of sev-
358
eral IL + H2O systems44,45, results indicate that aqueous solutions of ILs do not follow Walden´s
359
rule qualitatively, even though trends found suggest a physical background for the value of C45.
(6)
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360 361
Figure 5. Walden plot of the [C2Py][MeSO3] (x[C2Py][MeSO3] = 0.065) + H2O () and [Chol][H2PO4]
362
(x[Chol][H2PO4] = 0.062) + H2O mixtures (●) at 298.15, 313.15, 333.15 K. The straight solid line through the
363
origin with a slope of 1 represents the so-called ideal KCl line42
364 365
Proton activity measurements: Since the solvent is pure water, the experimental proton activi-
366
ty, aH+ or “effective” proton concentration (see experimental section) of these mixtures was also
367
determined, these measurements are representative rather than exhaustive, and its effect was
368
shown in Figure 6, together with the electrical conductivity data. The proton activity (expressed
369
as paH+) depends strongly on xII. Systems show different trends, depending mainly on the anion
370
structure, since the pKa´s values of both conjugated acid of aliphatic amines or unsatured pyri-
371
dines increase with the increasing alkylsubtitution and render the corresponding cations a basic
372
character (see structures in Scheme S1), although the charge and structure of these cations will
373
influence the polarity and the solvent properties of the ionic liquids.
374
For the [C2Py][MeSO3] (Fig. 6a), paH+ is 3.42 at x[C2Py][MeSO3] = 0.0039, this value decreases
375
drastically with the increase of x[C2Py][MeSO3] up to 0.0371, thus, [C2Py][MeSO3] plays the role of
376
an acidic species, where the minimum paH+ is close to the xIL where the conductivity presents its
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highest value (46.72 mS cm-1 at xIL 0.047). Afterwards, the paH+ values increase slightly with xIL,
378
reaching the value of 2.74 at xIL = 0.3830. Keeping in mind the structure for [C2Py][MeSO3],
379
that is a six-membered unsaturated ring that is more basic than the pyridinium and imidazolium
380
cations with a methanesulfonate (conjugated-base of a very strong methanesulfonic acid, Me-
381
SO3H, with a pKa = -1.8) as counteranion46,47, it should be expected to yield a “neutral” (in the
382
acidic/base sense) ionic liquid product48. This is the case of [C2Py][OTf] (note structures are sim-
383
ilar), with proton activities of paH+ 6.42 and 5.91 at xIL = 0.067 and xIL = 0.689, respectively,
384
where the weak acidity at high xIL can be attributed to the presence of free fluoride ion (conju-
385
gated-base of a weak fluorhydric, HF, with a pKa = 3.2). However, these [C2Py][MeSO3] mix-
386
tures exhibit a stronger acidity than expected, and this behavior, although we cannot yet offer an
387
conclusive explanation, seems to be, caused by some impurities from the acid used as precursor
388
in the synthesis. This hypothesis will be discussed later (next section and Fig.7a).
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389 390
Figure 6. Electrical conductivity () and paH+ () versus xIL at 298.15 K. a) [C2Py][MeSO3] + H2O b)
391
[Chol][H2PO4] + H2O. Notice that the points are joined for better following the trends in electrical con-
392
ductivity (Casteel-Amis fitting in Figure 4) and paH+
393 394
For [Chol][H2PO4] (Fig 6b), the most diluted solution, xIL = 0.0040, has a proton activity of
395
3.22, increasing with xIL during the whole concentration range, at xIL = 0.1651 the paH+ is 4.99
396
(see Table 2 for concentration equivalences). Furthermore, paH+ trend shows two straight lines
397
with the increasing of xIL, whose equations are as follows: paH+ = (3.168±0.004) + (13.4±0.2)
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x[Chol][H2PO4] for the first linear trend
(x[Chol][H2PO4] ≤ 0.0316) and paH+ = (3.29±0.05) +
399
(10.4±0.5) x[Chol][H2PO4] for the second linear trend (x[Chol][H2PO4] ≥ 0.0316), both with a good lin-
400
ear correlation (R² = 0.9999 and R² = 0.999, respectively), Fig. 6b()), and the crossing point
401
roughly coincides with the maximum of the conductivity value (28.34 mS cm-1 at xIL 0.0386).
402
According to its structure (Scheme S1), formed by an acyclic and saturated with a hydroxylfun-
403
tionalized side chain also on the cation-dependent degree of hydrogen bonding and an “ampho-
404
teric” counteranion, with the potential to both accept and donate protons depending on the other
405
substances present in the media47, these experimental results show that the dihydrogen phosphate
406
acts as Brønsted acid counteranion at diluted binary mixtures, being amphoteric at high IL con-
407
centration, where the paH+ tends to reach the theoretical value of 4.7 (semi-sum of pKa1 = 2.2
408
and pKa2 = 7.2 of phosphoric acid system) or experimental value of 4.36 for 1.845 M potassium
409
dihydrogenphosphate solution at the same concentration (Table 2) and it acts as second order
410
buffered solution.
411
Moreover, it should be noted that [Chol][H2PO4] gives a lower Brønsted acidity (higher paH+
412
values) than the observed for the [C2Py][MeSO3] at high molar fraction and probably, this is due
413
to the strong Brønsted acidity of the hydrogen sulfate counteranion or methanesulfonic acid that
414
can be present as impurities, in good agreement with what is found in the literature.49
415
Trends of electrical conductivity and proton activity for ILs + H2O systems are κ [Chol][H2PO4] < κ
416
[C2Py][OTf ]
κ ([Chol][H2PO4] + H2O)
485
•
paH+([C2Py][MeSO3]+H2O)