This document summarizes research determining ion-specific equation coefficients for the Abraham solvation parameter model for several ionic liquid solvents. The researchers compiled partition coefficient data for solutes dissolved in five ionic liquids and correlated the data using the Abraham model. They were able to describe the partition coefficients within 0.13 log units. Cation-specific coefficients were then calculated for each ionic liquid, allowing predictions of solute partitioning in 76 ionic liquid solvents using previously reported anion coefficients.
Complex-formation reactions are widely used in analytical chemistry. One of the first uses of these reagents was for titrating cations. In addition, many complexes are colored or absorb ultraviolet radiation; the formation of these complexes is often the basis for spectrophotometric determinations. Some complexes are sparingly soluble and can be used in gravimetric analysis. Complexes are also widely used for extracting cations from one solvent to another and for dissolving insoluble precipitates. The most useful complex forming reagents are organic compounds that contain several electron donor groups that form multiple covalent bonds with metal ions.
FORMING COMPLEXES
Most metal ions react with electron-pair donors to form coordination compounds or complexes. The donor species, or ligand is an ion or a molecule that forms a covalent bond with a cation or a neutral metal atom by donating a pair of electrons that are then shared by the two.
The number of covalent bonds that a cation tends to form with electron donors is its coordination number. Typical values for coordination numbers are two, four, and six. The species formed as a result of coordination can be electrically positive, neutral, or negative.
A ligand that has a single donor group, such as ammonia, is called unidentate(single-toothed), whereas one such as glycine, which has two groups available for covalent bonding, is called bidenate. Tridentate, tetradentate, pentadentate, and hexadentate chelating agents are also known.
Another important type of complex, a macrocycle, is formed between a metal ion and a cyclic organic compound. The selectivity of a ligand for one metal ion over another relates to the stability of the complexes formed. The higher the formation constant of a metal-ligand complex, the better the selectivity of the ligand for the metal relative to similar complexes formed with other metals.
Kinetics of Ruthenium(III) Catalyzed and Uncatalyzed Oxidation of Monoethanol...Ratnakaram Venkata Nadh
Kinetics of uncatalyzed and ruthenium(III) catalyzed oxidation of monoethanolamine by N-bromosuccinimide
(NBS) has been studied in an aqueous acetic acid medium in the presence of sodium acetate
and perchloric acid, respectively. In the uncatalyzed oxidation the kinetic orders are: the first order in NBS,
a fractional order in the substrate. The rate of the reaction increased with an increase in the sodium acetate
concentration and decreased with an increase in the perchloric acid concentration. This indicates that free
amine molecules are the reactive species. Addition of halide ions results in a decrease in the kinetic rate,
which is noteworthy. Both in absence and presence of a catalyst, a decrease in the dielectric constant of the
medium decreases the kinetic rate pointing out that these are dipole—dipole reactions. A relatively higher
oxidation state of ruthenium i.e., Ru(V) was found to be the active species in Ru(III) catalyzed reactions. A
suitable mechanism consistent with the observations has been proposed and a rate law has been derived to
explain the kinetic orders.
This short presentation describes the principles of measuring lipophilicty and bio-mimetic properties, such as protein and phospholipid binding by HPLC. These data can be used to model compound's in vivo distribution.
The branch of chemistry, which deals with the study of reaction rates and their mechanisms, called chemical kinetics.
Thermodynamics tells only about the feasibility of a reaction whereas chemical kinetics tells about the rate of a reaction.
For example, thermodynamic data indicate that diamond shall convert to graphite but in reality the conversion rate is so slow that the change is not perceptible at all.
Mannich Synthesis Under Ionic Liquid [Et3NH][HSO4] CatalysisIOSRJAC
Ionic liquid [Et3NH][HSO4] was found to be a particularly efficient catalyst for the synthesis of β- amino carbonyl pyrimidines through the Mannich condensation reaction of substituted pyrimidin-2(1H)-ones, cyclohexanone and 4-fluro/chlorobenzaldehyde under ultrasonic irradiation at room temperature. The present methodology offers several advantages such as excellent yields, simple procedure and mild conditions.
Partial Molar Volumes of Tetra alkyl ammonium salts in 10%(W/W) 2-(Ethoxy) et...Premier Publishers
In this article densities and apparent molar volumes of Tetra alkyl ammonium bromide salts ( ) in 10% (W/W) 2-(Ethoxy) ethanol-water mixture is studied at 30o, 35o and 40oC. Partial molar volumes are divided into ionic components using different methods such as Conway et al. and Jolicoeur et al. The results are compared with the values of partial molar volumes of ions reported in literature for pure water. Decrease in hydrophobic hydration is noticed. This may be due to the addition of co-solvent 2-(Ethoxy) ethanol (confirming the conclusions drawn from our viscosity studies that in 2-(Ethoxy) ethanol-water mixture, the structuredness of water is reduced by the breaking of hydrogen bonds). The values are divided into and . Making use of the Padova’s equation values of salts are calculated. These are also divided into ionic contributions. Dimensions of ions have been calculated to understand solvation behavior. It is shown that the classification of salts into structure makers and structure breakers on the basis of the sign of is not valid for the present water rich mixed solvent system.
International Journal of Engineering Research and Applications (IJERA) is an open access online peer reviewed international journal that publishes research and review articles in the fields of Computer Science, Neural Networks, Electrical Engineering, Software Engineering, Information Technology, Mechanical Engineering, Chemical Engineering, Plastic Engineering, Food Technology, Textile Engineering, Nano Technology & science, Power Electronics, Electronics & Communication Engineering, Computational mathematics, Image processing, Civil Engineering, Structural Engineering, Environmental Engineering, VLSI Testing & Low Power VLSI Design etc.
A poor solubility in water limits in a drastic way the effi cacy of a drug, because the absorption phenomenon requires the drugs be in dissolution. The therapeutic activity of a drug is depending of its acid-base dissociation constant (pKa) and solubility, the knowledge of pKa values being thus of great worth. The solubility method can be very useful in spite of their limitations if an appropriate method is available to carry out the solubility measurements of scarce solubility compounds. Some examples taken from the bibliography whose behaviour is well adapted to conventional acid-base dissociation equilibria without further complications are selected for study: Calcein blue, butaperazine, sulfadiazine, tyrosine, 8-hydroxiquinoleine and nifl umic acid. The pKa values have been recalculated applying the single least squares method and the classic monoprotic acid bilogarithmic model. A slope-intercept procedure is also applied to get the evaluation of acidity constants of overlapping equilibria (pKa2 and pKa3 of tyrosine). Results obtained in all cases are compared with literature data.
Kinetic And Mechanism of Oxidation of Cobalt Metal Complex By Acidic Potassiu...IJMERJOURNAL
ABSTRACT: The Kinetic of oxidation of Cobalt derived from 8-hydroxy quinolone and salicylaldehyde by potassium permanganate has been studied in the presence of acidic medium. The overall reaction is first order with respect to KMnO4, Substrate acid and temperature. No effect of salts has been found suitable mechanism is given.
this presentation describes ways to enantiomeric product synthesis, hence introducing to chiral catalysts. the temperature effects are discussed with relation to soai autocatalysis. it shows introduction to stereocartography.
Complex-formation reactions are widely used in analytical chemistry. One of the first uses of these reagents was for titrating cations. In addition, many complexes are colored or absorb ultraviolet radiation; the formation of these complexes is often the basis for spectrophotometric determinations. Some complexes are sparingly soluble and can be used in gravimetric analysis. Complexes are also widely used for extracting cations from one solvent to another and for dissolving insoluble precipitates. The most useful complex forming reagents are organic compounds that contain several electron donor groups that form multiple covalent bonds with metal ions.
FORMING COMPLEXES
Most metal ions react with electron-pair donors to form coordination compounds or complexes. The donor species, or ligand is an ion or a molecule that forms a covalent bond with a cation or a neutral metal atom by donating a pair of electrons that are then shared by the two.
The number of covalent bonds that a cation tends to form with electron donors is its coordination number. Typical values for coordination numbers are two, four, and six. The species formed as a result of coordination can be electrically positive, neutral, or negative.
A ligand that has a single donor group, such as ammonia, is called unidentate(single-toothed), whereas one such as glycine, which has two groups available for covalent bonding, is called bidenate. Tridentate, tetradentate, pentadentate, and hexadentate chelating agents are also known.
Another important type of complex, a macrocycle, is formed between a metal ion and a cyclic organic compound. The selectivity of a ligand for one metal ion over another relates to the stability of the complexes formed. The higher the formation constant of a metal-ligand complex, the better the selectivity of the ligand for the metal relative to similar complexes formed with other metals.
Kinetics of Ruthenium(III) Catalyzed and Uncatalyzed Oxidation of Monoethanol...Ratnakaram Venkata Nadh
Kinetics of uncatalyzed and ruthenium(III) catalyzed oxidation of monoethanolamine by N-bromosuccinimide
(NBS) has been studied in an aqueous acetic acid medium in the presence of sodium acetate
and perchloric acid, respectively. In the uncatalyzed oxidation the kinetic orders are: the first order in NBS,
a fractional order in the substrate. The rate of the reaction increased with an increase in the sodium acetate
concentration and decreased with an increase in the perchloric acid concentration. This indicates that free
amine molecules are the reactive species. Addition of halide ions results in a decrease in the kinetic rate,
which is noteworthy. Both in absence and presence of a catalyst, a decrease in the dielectric constant of the
medium decreases the kinetic rate pointing out that these are dipole—dipole reactions. A relatively higher
oxidation state of ruthenium i.e., Ru(V) was found to be the active species in Ru(III) catalyzed reactions. A
suitable mechanism consistent with the observations has been proposed and a rate law has been derived to
explain the kinetic orders.
This short presentation describes the principles of measuring lipophilicty and bio-mimetic properties, such as protein and phospholipid binding by HPLC. These data can be used to model compound's in vivo distribution.
The branch of chemistry, which deals with the study of reaction rates and their mechanisms, called chemical kinetics.
Thermodynamics tells only about the feasibility of a reaction whereas chemical kinetics tells about the rate of a reaction.
For example, thermodynamic data indicate that diamond shall convert to graphite but in reality the conversion rate is so slow that the change is not perceptible at all.
Mannich Synthesis Under Ionic Liquid [Et3NH][HSO4] CatalysisIOSRJAC
Ionic liquid [Et3NH][HSO4] was found to be a particularly efficient catalyst for the synthesis of β- amino carbonyl pyrimidines through the Mannich condensation reaction of substituted pyrimidin-2(1H)-ones, cyclohexanone and 4-fluro/chlorobenzaldehyde under ultrasonic irradiation at room temperature. The present methodology offers several advantages such as excellent yields, simple procedure and mild conditions.
Partial Molar Volumes of Tetra alkyl ammonium salts in 10%(W/W) 2-(Ethoxy) et...Premier Publishers
In this article densities and apparent molar volumes of Tetra alkyl ammonium bromide salts ( ) in 10% (W/W) 2-(Ethoxy) ethanol-water mixture is studied at 30o, 35o and 40oC. Partial molar volumes are divided into ionic components using different methods such as Conway et al. and Jolicoeur et al. The results are compared with the values of partial molar volumes of ions reported in literature for pure water. Decrease in hydrophobic hydration is noticed. This may be due to the addition of co-solvent 2-(Ethoxy) ethanol (confirming the conclusions drawn from our viscosity studies that in 2-(Ethoxy) ethanol-water mixture, the structuredness of water is reduced by the breaking of hydrogen bonds). The values are divided into and . Making use of the Padova’s equation values of salts are calculated. These are also divided into ionic contributions. Dimensions of ions have been calculated to understand solvation behavior. It is shown that the classification of salts into structure makers and structure breakers on the basis of the sign of is not valid for the present water rich mixed solvent system.
International Journal of Engineering Research and Applications (IJERA) is an open access online peer reviewed international journal that publishes research and review articles in the fields of Computer Science, Neural Networks, Electrical Engineering, Software Engineering, Information Technology, Mechanical Engineering, Chemical Engineering, Plastic Engineering, Food Technology, Textile Engineering, Nano Technology & science, Power Electronics, Electronics & Communication Engineering, Computational mathematics, Image processing, Civil Engineering, Structural Engineering, Environmental Engineering, VLSI Testing & Low Power VLSI Design etc.
A poor solubility in water limits in a drastic way the effi cacy of a drug, because the absorption phenomenon requires the drugs be in dissolution. The therapeutic activity of a drug is depending of its acid-base dissociation constant (pKa) and solubility, the knowledge of pKa values being thus of great worth. The solubility method can be very useful in spite of their limitations if an appropriate method is available to carry out the solubility measurements of scarce solubility compounds. Some examples taken from the bibliography whose behaviour is well adapted to conventional acid-base dissociation equilibria without further complications are selected for study: Calcein blue, butaperazine, sulfadiazine, tyrosine, 8-hydroxiquinoleine and nifl umic acid. The pKa values have been recalculated applying the single least squares method and the classic monoprotic acid bilogarithmic model. A slope-intercept procedure is also applied to get the evaluation of acidity constants of overlapping equilibria (pKa2 and pKa3 of tyrosine). Results obtained in all cases are compared with literature data.
Kinetic And Mechanism of Oxidation of Cobalt Metal Complex By Acidic Potassiu...IJMERJOURNAL
ABSTRACT: The Kinetic of oxidation of Cobalt derived from 8-hydroxy quinolone and salicylaldehyde by potassium permanganate has been studied in the presence of acidic medium. The overall reaction is first order with respect to KMnO4, Substrate acid and temperature. No effect of salts has been found suitable mechanism is given.
this presentation describes ways to enantiomeric product synthesis, hence introducing to chiral catalysts. the temperature effects are discussed with relation to soai autocatalysis. it shows introduction to stereocartography.
Similar to Ion specific equation coefficient version of the Abraham model for ionic liquid solvents determination of coefficients for tributylethylphosphonium 1
Development of Dynamic Models for a Reactive Packed Distillation ColumnCSCJournals
This work has been carried out to develop dynamic models for a reactive packed distillation column using the production of ethyl acetate as the case study. The experimental setup for the production of ethyl acetate was a pilot scale packed column divided into condenser, rectification, acetic acid feed, reaction, ethanol feed, stripping and reboiler sections. The reaction section was filled with Amberlyst 15 catalyst while the rectification and the stripping sections were both filled raschig rings. The theoretical models for each of the sections of the column were developed from first principles and solved with the aid of MATLAB R2011a. Comparisons were made between the experimental and theoretical results by calculating the percentage residuals for the top and bottom segment temperatures of the column. The results obtained showed that there were good agreements between the experimental and theoretical top and bottom segment temperatures because the calculated percentage residuals were small. Therefore, the developed dynamic models can be used to represent the reactive packed distillation column.
These slides may be used for a part of Advanced level course in Chemical Reaction Engineering. I taught this course to Masters level students covering 1.5 credit hours.
Previously published technical article giving a new vapor pressure equation that is thermodynamically consistent, as well as including EOS and BIP's for chlorosilanes and impurities
The International Journal of Engineering & Science is aimed at providing a platform for researchers, engineers, scientists, or educators to publish their original research results, to exchange new ideas, to disseminate information in innovative designs, engineering experiences and technological skills. It is also the Journal's objective to promote engineering and technology education. All papers submitted to the Journal will be blind peer-reviewed. Only original articles will be published.
The papers for publication in The International Journal of Engineering& Science are selected through rigorous peer reviews to ensure originality, timeliness, relevance, and readability.
Shortcut Design Method for Multistage Binary Distillation via MS-ExceIJERA Editor
Multistage distillation is most widely used industrial method for separating chemical mixtures with high energy consumptions especially when relative volatility of key components is lower than 1.5. The McCabe Thiele is considered to be the simplest and perhaps most instructive method for the conceptual design of binary distillation column which is still widely used, mainly for quick preliminary calculations. In this present work, we provide a numerical solution to a McCabe-Thiele method to find out theoretical number of stages for ideal and non-ideal binary system, reflux ratio, condenser duty, reboiler duty, each plate composition inside the column. Each and every point related to McCabe-Thiele in MS-Excel to give quick column dimensions are discussed in details
Classification either on quality or type based for groundwater can offer great advantages especially in regional groundwater management. It provides a short, quick processing, interpretation for a lot of complete hydro-chemical data sets and concise presentation of the results. There is a demonstrable need for a quality assurance, with the advanced usage of world's largest fresh water storage i.e Ground water. Its getting depleted over the years and the quality of the same degrading with a rapid pace. Ground water Quality is assessed mainly by the chemical analysis of samples. The data obtained from the chemical analysis is key for the further classification, analysis, correlation etc. Graphical and Numerical interpretation of the data is the main source for Hydro-chemical studies. In this paper we test the performance of the many available graphical and statistical methodologies used to classify water samples including: Collins bar diagram, Stiff pattern diagram, Schoeller plot, Piper diagram, Durov's Double Triangular Diagram, Gibbs's Diagram, Stuyfzand Classification. This paper explains various models which classify, correlate etc., summarizing the water quality data. The basic graphs and diagrams in each category are explained by sample diagrams. In addition to the diagrams an overall characterization of hydro-chemical facies of the water can be carried out by using plots which represents a water type and hardness domain. The combination of graphical and statistical techniques provides a consistent and objective means to classify large numbers of samples while retaining the ease of classic graphical presentation.
Liquid-Liquid Equilibria of Nitrobenzene-Inorganic Acid Systems at 298.15 KReddysuresh Kolavali
Similar to Ion specific equation coefficient version of the Abraham model for ionic liquid solvents determination of coefficients for tributylethylphosphonium 1 (20)
Liquid-Liquid Equilibria of Nitrobenzene-Inorganic Acid Systems at 298.15 K
Ion specific equation coefficient version of the Abraham model for ionic liquid solvents determination of coefficients for tributylethylphosphonium 1
1. Full Terms & Conditions of access and use can be found at
http://www.tandfonline.com/action/journalInformation?journalCode=gpch20
Download by: [University of North Texas] Date: 15 November 2016, At: 10:15
Physics and Chemistry of Liquids
An International Journal
ISSN: 0031-9104 (Print) 1029-0451 (Online) Journal homepage: http://www.tandfonline.com/loi/gpch20
Ion-specific equation coefficient version
of the Abraham model for ionic liquid
solvents: determination of coefficients
for tributylethylphosphonium, 1-butyl-1-
methylmorpholinium, 1-allyl-3-methylimidazolium
and octyltriethylammonium cations
Bihan Jiang, Melissa Y. Horton, William E. Acree Jr. & Michael H. Abraham
To cite this article: Bihan Jiang, Melissa Y. Horton, William E. Acree Jr. & Michael H. Abraham
(2016): Ion-specific equation coefficient version of the Abraham model for ionic liquid solvents:
determination of coefficients for tributylethylphosphonium, 1-butyl-1-methylmorpholinium,
1-allyl-3-methylimidazolium and octyltriethylammonium cations, Physics and Chemistry of
Liquids, DOI: 10.1080/00319104.2016.1218009
To link to this article: http://dx.doi.org/10.1080/00319104.2016.1218009
Published online: 08 Aug 2016. Submit your article to this journal
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3. solvents studied, it is not practical to perform measurements for every organic solute pair dissolved
in every IL solvent. It is estimated that the number of possible IL solvents may exceed 1014
[23]
when one considers all of the different cation–anion pair combinations.
To facilitate the use of ILs in industrial processes involving separations, researchers have
turned to predictive methods to generate activity coefficients of solutes dissolved in IL solvents,
as well as to estimate other physical properties of IL solvents that may be needed in process design
computations. Predictive methods have involved both theoretical and semi-theoretical treatments,
as well as approaches based on group contribution and molecular fragment schemes, linear free
energy relationships (LFERs) and quantitative structure–property relationships (QSPRs). Group
contribution methods have been proposed, which enable one to predict infinite dilution activity
coefficients and gas–to-liquid partition coefficients of solutes dissolved in ILs,[24–26] to predict
enthalpies of solvation of organic solutes dissolved in ILs,[27] and to estimate viscosities,[28,29]
thermal conductivities,[30,31] isobaric heat capacities,[32–34] surface tensions [35] and densities
[36] of ILs at both 298 K and as a function of temperature. In several of the above methods the
entire cation was defined as one functional group and the entire counter-anion was defined as a
second functional group.
Our contribution towards facilitating the use of IL solvents in chemical separation processes
has been to develop mathematical correlations based on the Abraham model that enable one to
predict infinite dilution activity coefficients and chemical separation factors. The Abraham model
[37] is an LFER approach that can describe solute transfer between two condensed phases:
log P ¼ cp;il þ ep;ilÁE þ sp;ilÁS þ ap;ilÁA þ bp;ilÁB þ vp;ilÁV (1)
or solute transfer to a condensed phase from the vapour phase:
log K ¼ ck;il þ ek;ilÁE þ sk;ilÁS þ ak;ilÁA þ bk;ilÁB þ lk;ilÁL (2)
In the present study one of the condensed phases is the IL solvent. Equation (1) will thus describe
the water-to-IL solvent partition coefficient, log P, while Equation (2) will describe the gas-to-IL
partition coefficient, log K. Uppercase alphabetic letters on the right-hand side of Equations (1)
and (2) represent the properties of the dissolved solute and are called solute descriptors, which are
unique to a given solute molecule. Solute descriptors are defined as follows: the solute excess
molar refractivity in units of (cm3
mol–1
)/10 (E), the solute dipolarity/polarisability (S), the overall
or summation hydrogen-bond acidity and basicity (A and B, respectively), the McGowan volume
in units of (cm3
mol–1
)/100 (V), and the logarithm of the gas-to-hexadecane partition coefficient
at 298 K (L). Once calculated, the solute descriptors can be used to predict log K and log P values
for the solute in any IL solvent for which the lowercase equation coefficients (cp,il, ep,il, sp,il, ap,il,
bp,il, vp,il, ck,il, ek,il, sk,il, ak,il, bk,il and lk,il) are known. The equation coefficients are unique to the IL
solvent, and provide information regarding the IL properties, such as polarity, polarisability and
hydrogen-bonding character. To date IL-specific equation coefficients have been calculated for
more than 70 ILs. See Table 1 for a list of the published equation coefficients for the various IL
solvents that have been studied thus far. Included in the tabulation is the statistical information
associated with each Abraham model correlation expression, which includes: the standard devia-
tion (SD) and the number of experimental data points used in the regression analysis (N) to
calculate the equation coefficients. The ionic liquids are listed according to the cation and anion
abbreviation (see Table 2 for the names that correspond to the different abbreviations).
The predictive ability of the IL-specific version of the Abraham model (Equations (1) and (2))
is limited in applicability to only those IL solvents for which equation coefficients have been
determined. The model’s predictive ability can be increased by recognising that each term in the
log P and log K correlations corresponds to a different type of solute–IL interaction. Sprunger and
co-workers [38–40] split each type of molecular interaction into a cation contribution and anion
contribution:
2 B. JIANG ET AL.
9. log P ¼ cp;cation þ cp;anion þ ep;cation þ ep;anion
À Á
E þ sp;cation þ sp;anion
À Á
S
þ ap;cation þ ap;anion
À Á
A þ bp;cation þ bp;anion
À Á
B þ vp;cation þ vp;anion
À Á
V
(3)
log K ¼ ck;cation þ ck;anion þ ek;cation þ ek;anion
À Á
E þ sk;cation þ sk;anion
À Á
S
þ ak;cation þ ak;anion
À Á
A þ bk;cation þ bk;anion
À Á
B þ lk;cation þ lk;anion
À Á
L (4)
In other words, the lowercase equation coefficients now become cation-specific and anion-specific
numerical values, which can then be combined as a cation–anion sum to yield Abraham model
equation coefficients that would be specific for the one IL solvent containing the given cation–
anion pair combination. In some respects the treatment proposed by Sprunger and co-workers is
analogous to estimating each of the different Abraham model equation coefficients by a group
contribution or fragment group method, where the entire cation serves as one functional group in
the IL and the entire counter-anion defines the second functional group.
To date we have reported ion-specific equation coefficients for 45 different cations and 19
different anions. The most updated set of ion-specific equation coefficients was published
approximately 2 years ago.[41] Since the last update was published, we have calculated ion-
specific equation coefficients for five additional cations: 1-butyl-2,3-dimethylimidazolium,[42] 4-
cyano-1-butylpyridinium,[42] 2-methoxyethyl(dimethyl)ethylammonium,[43] 1-hexylquinuclidi-
nium,[21] 1-octylquinuclidinium [21] and for three additional anions: L-lactate,[44] (1S)-(+)-10-
camphorsulphonate,[44] and 4,5-dicyano-2-(trifluoromethyl)imidazolide.[45] The 45 different
cation and 19 different anion equation coefficients that we have determined can be combined
to give Abraham model correlations for predicting log K and log P values for 855 (45 × 19)
different IL solvents. This is significantly more IL solvents than the 76 IL solvents listed in Table 1
for which we have IL-specific Abraham model correlations. Through standard thermodynamic
relationships, the predicted log K and log P values can be converted first to infinite dilution
activity coefficients, γ1
solute:
log K ¼ log P þ log KW ¼ log
RT
γ1
solutePo
soluteVsolvent
(5)
and then to separation factors, S1
1;2:
S1
1;2 ¼
γ1
solute1
γ1
solute2
(6)
that can be used to determine whether or not a desired chemical separation can be achieved using a
particular IL solvent. In Equation (5), R is the universal gas constant, Vsolvent is the molar volume of the
IL solvent, Po
soluteis the vapour pressure of the solute at the system temperature, T is the system
temperature, and log Kw is the logarithm of the solute’s gas-to-water partition coefficient. In the
present communication we have determined Abraham model correlations from published γ1
solute and
log K data for solutes dissolved in 1-allyl-3-methylimidazolium dicyanamide ([AllMIm]+
[N(CN)2]–
),
Table 2. (Continued).
Ion abbreviation Ion name
[B(CN)4]–
tetracyanoborate
[MeSO3]–
methanesulfonate
[BETI]–
bis(pentafluoroethylsulfonyl)imide
[Tos]–
tosylate
[C(CN)3]–
tricyanomethanide
[L-Lact]–
L-lactate
[+CS]–
(1S)-(+)-10-camphorsulfonate
[TDI]–
4,5-dicyano-2-(trifluoromethyl)imidazolide
8 B. JIANG ET AL.
10. [46] 1-allyl-3-methylimidazolium bis(trifluoromethylsulphonyl)imide ([AllMIm]+
[Tf2N]–
),[47] octyl-
triethylammonium bis(trifluomethylsulphonyl)imide ([OE3Am]+
[Tf2N]–
),[48] tributylethyl-
phosphonium diethylphosphate ([B3EP]+
[E2PO4]–
)[49] and 1-butyl-1-methylmorpholinium
tricyanomethanide ([BMMorp]+
[C(CN)3]–
).[50] Also calculated as part of this study are the ion-
specific equation coefficients for [AllMIm]+
, [OE3Am]+
, [B3EP]+
and [BMMorp]+
cations.
2. Computation methodology and the partition coefficient data sets
The Abraham model has been successfully used to correlate solute transfer processes. The transfer
process might involve solute partitioning between two immiscible (or partly immiscible) phases as
would be the case for solvent extractions, or might involve solute transfer where the two phases
are physically separated from each other. The latter would be referred to as a hypothetical
partition coefficient where the numerical value would be calculable as either a solubility ratio or
through a thermodynamic cycle, such as water-to-organic solvent partition coefficient equals the
gas-to-organic solvent partition coefficient divided by the gas-to-water partition coefficient
(P = K/Kw). A major difference between the two types of solute transfer processes is that first
involves mutually saturated phases, while the second involves the ‘neat’ liquid solvents. The water-
to-IL solvent partitioning systems that are listed in Table 1 all pertain to solute transfer into neat
IL solvents that are not saturated with water.
The data sets for ([AllMIm]+
[N(CN)2]–
), ([AllMIm]+
[Tf2N]–
), ([OE3Am]+
[Tf2N]–
),
([B3EP]+
[E2PO4]–
) and ([BMMorp]+
[C(CN)3]–
) were constructed from published partition coeffi-
cient data for solutes dissolved in the anhydrous IL solvents. For each IL solvent the partition
coefficient measurements were performed at several temperatures slightly higher than 298.15 K. The
numerical log K (at 298.15 K) values used in the present study were calculated from the standard
thermodynamic log K vs. 1/T linear relationship based on the measured values at either 318.15 and
328,15 K for ([AllMIm]+
[Tf2N]–
), ([OE3Am]+
[Tf2N]–
) and ([BMMorp]+
[C(CN)3]–
), or 328.15 and
338.15 K for ([B3EP]+
[E2PO4]–
), or 308.15 and 318.15 K for ([AllMIm]+
[N(CN)2]–
). The foremen-
tioned temperatures were the two lowest temperatures that were studied for each of the four IL
solvents. The linear extrapolation should be valid as the measurements were performed at tempera-
tures not too far removed from the desired temperature of 298.15 K (about 40 K in the worst case).
The respective log P values for each solute–IL combination were calculated by subtracting log Kw
from the extrapolated log K values as indicated in Equation (5).
The calculated log K and log P values at 298.15 K are assembled in Tables 3–7 for solutes
dissolved in ([AllMIm]+
[N(CN)2]–
), ([AllMIm]+
[Tf2N]–
), ([B3EP]+
[E2PO4]–
), ([OE3Am]+
[Tf2N]–
)
and ([BMMorp]+
[C(CN)3]–
), respectively. Each data set contains between 49 and 63 chemically
diverse organic liquid solutes. The list of organic solutes includes alkanes, alkenes, alkynes,
aromatic and heterocyclic compounds, primary and secondary alcohols, dialkyl ethers and cyclic
ethers, alkanones, alkyl alkanoates, and nitroalkanes. We searched the published literature but was
unable to find partition coefficient or solubility data for gaseous or solid solutes in the five IL
solvents. Also collected in Tables 3–7 are the numerical solute descriptors for the organic
compounds studied in the present investigation. Numerical values of the solute descriptors in
our database are of experimental origin and are based on observed solubility data and Henry’s law
constants,[51–54] on measured gas–liquid and high-performance liquid chromatographic reten-
tion times and retention factors,[55,56] and on experimental practical partition coefficient mea-
surements for the equilibrium solute distribution between water and an immiscible (or partially
miscible) organic solvent.[57]
Calculation of the Abraham model IL-specific equation coefficients is relatively straightforward
and begins with writing a log K and log P equation for each solute–IL solvent pair. For each
equation the measured log K and log P values, as well as the five solute descriptors that appear on
the right-hand side of Equations (1) and (2), are known. This leaves only the six unknown
equation coefficients that must be calculated. The resulting set of log K equations are solved
PHYSICS AND CHEMISTRY OF LIQUIDS 9
21. simultaneously to give the numerical values of ck,il, ek,il, sk,il, ak,il, bk,il and lk,il that best describe the
observed gas-to-IL partition coefficient data. The equation coefficients for the set of log P
equations are solved in similar fashion to yield the numerical values of cp,il, ep,il, sp,il, ap,il, bp,il,
vp,il. The Abraham model IL-specific equation coefficients for all derived correlations were
obtained by regression analysis using the IBM SPSS Statistics Package, Version 22. The statistical
information for each derived correlation equation was also determined using the statistical soft-
ware package. Ion-specific equation coefficients for the [AllMIm]+
, [OE3Am]+
, [B3EP]+
and
[BMMorp]+
cations were calculated simply by subtracting the known anion-specific values from
the IL-specific equation coefficients (e.g. ccation = cIL – canion; ecation = eIL – eanion, etc.). The
computational procedure will be illustrated in the next section.
3. Results and discussion
The ([AllMIm]+
[N(CN)2]–
) and ([AllMIm]+
[Tf2N]–
) data sets are the two largest of the five data sets and
contain partition coefficients for 65 and 64 organic solutes, respectively. An analysis of the experimental
log P and log K values in Tables 3 and 4 yielded the following four Abraham model IL-specific
correlations:
For ([AllMIm]+
[N(CN)2]–
):
log P 298Kð Þ¼ À0:202 0:087ð Þ þ 0:360 0:083ð ÞE þ 0:780 0:099ð ÞS þ 0:790 0:122ð ÞA
À 4:475 0:095ð ÞB þ 2:621 0:076ð ÞV
with N ¼ 65; SD ¼ 0:102; R2
¼ 0:994; F ¼ 1890
À Á
(7)
log K 298Kð Þ¼ À0:815 0:060ð Þ þ 0:534 0:076ð ÞE þ 2:719 0:076ð ÞS þ 4:550 0:100ð ÞA
þ 0:450 0:079ð ÞB þ 0:514 0:018ð ÞL
with N ¼ 65; SD ¼ 0:084; R2
¼ 0:993; F ¼ 1706
À Á
(8)
For ([AllMIm]+
[Tf2N]–
):
log P 298Kð Þ¼ 0:058 0:090ð ÞE þ 0:703 0:096ð ÞS À 1:301 0:115ð ÞA À 4:343 0:103ð ÞB
þ 3:159 0:025ð ÞV
with N ¼ 64; SD ¼ 0:112; R2
¼ 0:998; F ¼ 5328
À Á
(9)
log K 298Kð Þ ¼ À0:420 0:058ð Þþ0:081 0:071ð ÞE þ 2:493 0:072ð ÞS þ 2:369 0:094ð ÞA
þ 0:599 0:074ð ÞB þ 0:643 0:017ð ÞL
with N ¼ 64; SD ¼ 0:079; R2
¼ 0:990; F ¼ 1160
À Á
(10)
The standard errors in each of the calculated equation coefficients are given in parentheses
immediately after the respective coefficient. An examination of the associated statistical informa-
tion reveals that the derived correlations provide a very good mathematical description of solute
transfer into ([AllMIm]+
[N(CN)2]–
) and ([AllMIm]+
[Tf2N]–
) as evidenced by the small standard
deviations, SD = 0.079 to 0.112 log units, near-unity squared correlation coefficients, R2
= 0.990 to
0.998, and large Fisher F-statistical values, F = 1160 to 5328, for Equations (7)–(10). Figures 1 and
2 depict a graphical comparison of the experimental log P data vs. back-calculated values based on
our derived Abraham model correlations for solutes dissolved in ([AllMIm]+
[N(CN)2]–
) and
([AllMIm]+
[Tf2N]–
), respectively. Similar comparisons of the log K values are shown in Figures
3 and 4. There are insufficient experimental data to permit a training set and test set assessment of
the predictive ability of Equations (7)–(10) by randomly splitting the entire databases in half.
The four mathematical correlations that have been obtained thus far should enable one to
predict log P and log K values for additional organic solutes dissolved in ([AllMIm]+
[N(CN)2]–
)
20 B. JIANG ET AL.
22. and ([AllMIm]+
[Tf2N]–
), provided of course that the solute’s descriptor values fall within the in
range of numerical values used in deriving Equations (7)–(10) above. Greater predictive ability
can be obtained through the ion-specific equation coefficient version of the Abraham model. The
[AllMIm]+
-specific equation coefficients can be determined using the derived correlations for
either IL solvent. From a purely mathematical standpoint it is easier to perform the calculations
using the correlations for ([AllMIm]+
[Tf2N]–
). In developing the ion-specific model, Sprunger
and co-workers [38–40] needed a reference point for calculating the numerical values for
individual ions. In an IL solvent the ions come as a cation–anion pair, and to calculate the values
for the cation one must know the values for the anion, and vice versa. To get around this problem,
the authors set all of the equation coefficients for the [Tf2N]–
anion equal to zero. Hence, the
Figure 1. Comparison of the experimental log P data and back-calculated values based on Equation (7) for solutes dissolved in
([AllMIm]+
[N(CN)2]–
).
Figure 2. Comparison of the experimental log P data and back-calculated values based on Equation (9) for solutes dissolved in
([AllMIm]+
[Tf2N]–
).
PHYSICS AND CHEMISTRY OF LIQUIDS 21
23. coefficients in Equations (9) and (10) are not only the IL-specific equation coefficients for the
entire ([AllMIm]+
[Tf2N]–
) IL solvent, but also the ion-specific equation coefficients for the
[AllMIm]+
cation.
Alternatively, one can calculate the ion-specific equation coefficients for the [AllMIm]+
cation
from Equations (7) and (8) as log P and log K equation coefficients for the [N(CN)2]] –
anion are
known: (cp,anion = –0.257; ep,anion = 0.164; sp,anion = 0.446; ap,anion = 2.217; bp,anion = –0.256 and
vp,anion = –0.243) and (ck,anion = –0.372; ek,anion = 0.345; sk,anion = 0.476; ak,anion = 2.270; bk,anion =
–0.198 and lk,anion = –0.055).[41] We have summarised in Table 8 the results of this computation.
We have taken the average of the two sets of calculations as the [AllMIm]+
-specific equation
Figure 3. Comparison of the experimental log K data and back-calculated values based on Equation (8) for solutes dissolved in
([AllMIm]+
[N(CN)2]–
).
Figure 4. Comparison of the experimental log K data and back-calculated values based on Equation (10) for solutes dissolved
in ([AllMIm]+
[Tf2N]–
).
22 B. JIANG ET AL.
24. coefficients for the log P and log K correlations. The average [AllMIm]+
-specific equation
coefficients have been summed with the respective [Tf2N]–
-specific and [N(CN)2]–
-specific
equation coefficients to constructive predictive Abraham model correlations for both
([AllMIm]+
[N(CN)2]–
) and ([AllMIm]+
[Tf2N]–
). The log K correlations predicted the experimen-
tal values in Tables 3 and 4 to within standard errors (SE) of 0.179 log units and 0.177 log units,
respectively. Standard errors corresponding to the log P predictions were SE = 0.183 log units and
SE = 0.189 log units for ([AllMIm]+
[N(CN)2]–
) and ([AllMIm]+
[Tf2N]–
), respectively. Standard
errors are slightly larger for the log P predictions because of the added uncertainties in the log Kw
values that were used to convert the experimentally determined gas-to-IL partition coefficients to
water-to-IL partition coefficients. The computations are in accord with our earlier observations in
that the best predictions are obtained using the IL-specific Abraham model correlations, which for
these two ILs would be Equations (7)–(10).
We suspect that we can improve on the predictions by recalculating the equation coefficients
for the [N(CN)2]–
anion. Recently published experimental data for solutes dissolved in 1-butyl-3-
methylimidazolium dicyanamide [19] and 1-butyl-4-methylpyridiniun dicyanamide [58] would
nearly double the number of data points for IL solvents containing the [N(CN)2]–
anion.
Reanalysis would be a massive computation task, however, as it would require regression analysis
on our entire IL database. The last regression analysis of the entire IL database was done just over
2 years ago,[41] and at the time there were 3731 experimental log P values and 3786 experimental
log K values. It is not computationally feasible to perform a complete reanalysis every time that a
new cation or anion is added to the database. A complete reanalysis will change most (if not all) of
the existing values that have been calculated for the 40 cations and 16 anions that were in the
database when the values were last updated. It will be difficult for readers to keep track of the
latest set of equation coefficients. We prefer to update values every few years whenever there has
been sufficient new experimental values added to the large database to warrant the computational
effort.
The ([B3EP]+
[E2PO4]–
) data set is the smallest of the five IL data sets, and it contains
experimental partition coefficients for only 49 solutes. Preliminary regression analysis of the
experimental data in Table 5 gave an Abraham model log K correlation:
log K 298Kð Þ¼ À0:279 0:074ð Þ À 0:441 0:097ð ÞE þ 1:952 0:104ð ÞS þ 5:698 0:190ð ÞA
À 0:382 0:105ð ÞB þ 0:823 0:022ð ÞL
with N ¼ 49; SD ¼ 0:089; R2
¼ 0:984; F ¼ 543:2
À Á
(11)
which had a negative numerical value for the bk,il coefficient. A negative bk,il coefficient is not
realistic as this would indicate that the H-bond acidity of ([B3EP]+
[E2PO4]–
) is less than that of
Table 8. Summary of determination of the ion-specific equation coefficients for the [AllMIm]+
cation.
IL Solvent/ion Property c e s a b v l
([AllMIm]+
[Tf2N]–
) log P 0.000 0.058 0.703 −1.301 −4.344 3.159
[AllMIm]+
log P 0.000 0.058 0.703 −1.301 −4.344 3.159
([AllMIm]+
[N(CN)2]–
) log P −0.202 0.360 0.780 0.789 −4.475 2.621
[N(CN)2]–
log P −0.257 0.164 0.446 2.217 −0.256 −0.243
[AllMIm]+
log P 0.055 0.196 0.334 −1.428 −4.219 2.864
Average for [AllMIm]+
log P 0.028 0.127 0.519 −1.365 −4.282 3.012
([AllMIm]+
[Tf2N]–
) log K −0.420 0.081 2.493 2.368 0.599 0.643
[AllMIm]+
log K −0.420 0.081 2.493 2.368 0.599 0.643
([AllMIm]+
[N(CN)2]–
) log K −0.815 0.534 2.719 4.550 0.450 0.514
[N(CN)2]–
log K −0.372 0.345 0.476 2.270 −0.198 −0.055
[AllMIm]+
log K −0.443 0.189 2.243 2.280 0.648 0.569
Average for [AllMIm]+
log K −0.432 0.135 2.368 2.324 0.624 0.606
PHYSICS AND CHEMISTRY OF LIQUIDS 23
25. the gas phase. We removed the bk,il·B from Equation (11), and re-analysed all of the experimental
data in Table 5. The final Abraham model correlations,
log P 298Kð Þ ¼ 0:120 0:127ð Þ À 0:242 0:137ð ÞE þ 0:309 0:153ð ÞS þ 1:899 0:269ð ÞA
À 5:345 0:150ð ÞB þ 3:723 0:110ð ÞV
with N ¼ 49; SD ¼ 0:128; R2
¼ 0:994; F ¼ 1389
À Á
(12)
log K 298Kð Þ ¼ À0:357 0:080ð Þ À 0:224 0:086ð ÞE þ 1:663 0:073ð ÞS þ 5:859 0:209ð ÞA
þ 0:844 0:025ð ÞL
with N ¼ 49; SD ¼ 0:102; R2
¼ 0:980; F ¼ 527:8
À Á
(13)
describe the partitioning behaviour of 49 organic solutes into ([B3EP]+
[E2PO4]–
) to within a
standard deviation of 0.128 log units. As an informational note, there was very little loss in
descriptive ability by removing the bk,il·B term from the log K equation. The standard deviation
was SD = 0.089 log units with the term included in the correlation vs. SD = 0.102 log units
without the term. Ion-specific equation coefficients are available in the published literature [41]
for the [E2PO4]–
anion: (cp,anion = 0.071; ep,anion = 0.073; sp,anion = 0.006; ap,anion = 5.089; bp,anion
= –0.832 and vp,anion = 0.184) and (ck,anion = 0.093; ek,anion = 0.107; sk,anion = –0.068; ak,anion = 5.071;
bk,anion = –0.774 and lk,anion = 0.061). Subtraction of the anion-specific equation coefficients from
the respective coefficients in Equations (12) and (13) results in the following set of coefficients for
the [B3EP]+
cation: (cp,cation = 0.049; ep,cation = –0.315; sp,cation = 0.303; ap,cation = –3.190; bp,cation
= –4.513 and vp,cation = 3.539) and (ck,cation = –0.450; ek,cation = –0.331; sk,cation = 1.731; ak,cation
= 0.788; bk,cation = 0.774 and lk,cation = 0.783).
The experimental partition coefficient data in Tables 6 and 7 were analysed in a similar fashion
to yield the following two sets of Abraham model IL-specific correlations:
For ([OE3Am]+
[Tf2N]–
):
log P 298Kð Þ ¼ À0:044 0:096ð Þ þ 0:111 0:091ð ÞE þ 0:398 0:108ð ÞS À 1:298 0:133ð ÞA
À 4:815 0:103ð ÞB þ 3:667 0:085ð ÞV
with N ¼ 63; SD ¼ 0:110; R2
¼ 0:996; F ¼ 3022
À Á
(14)
log K 298Kð Þ ¼ À0:378 0:053ð Þ À 0:074 0:066ð ÞE þ 2:088 0:066ð ÞS þ 2:368 0:087ð ÞA
þ 0:166 0:068ð ÞB þ 0:792 0:016ð ÞL
with N ¼ 63; SD ¼ 0:073; R2
¼ 0:990; F ¼ 1075
À Á
(15)
For ([BMMorp]+
[C(CN)3]–
):
log P 298Kð Þ ¼ À0:318 0:088ð Þ þ 0:374 0:093ð ÞE þ 0:951 0:104ð ÞS À 4:484 0:101ð ÞB
þ 3:122 0:076ð ÞV
with N ¼ 61; SD ¼ 0:114; R2
¼ 0:994; F ¼ 2243
À Á
(16)
log K 298Kð Þ ¼ À0:774 0:067ð Þ þ 0:371 0:078ð ÞE þ 2:762 0:078ð ÞS þ 3:707 0:109ð ÞA
þ 0:452 0:080ð ÞB þ 0:643 0:020ð ÞL
with N ¼ 61; SD ¼ 0:086; R2
¼ 0:991; F ¼ 1269
À Á
(17)
As an informational note, the ap,il·A term made a negligible contribution to the overall log P
correlation. The calculated ap,il coefficient was very small (0.021) and the standard error in the
coefficient was approximately seven times larger than the coefficient itself. Equations (14)–(17)
provide reasonably accurate mathematical descriptions of the observed log P and log K values for
solute transfer into both ([OE3Am]+
[Tf2N]–
) and ([BMMorp]+
[C(CN)3]–
). There is insufficient
24 B. JIANG ET AL.
26. experimental data to perform training set and test set analyses by splitting the data sets in half.
Based on our past experience in deriving and using Abraham model correlations for IL solvents,
however, we fully expect that Equations (14)–(17) will allow one to predict log P and log K values
for additional organic solutes to within approximately 0.13 log units of the observed values.
As noted above, for IL solvents that contain the [Tf2N]–
anion the calculated equation
coefficients pertain not only the entire IL solvent, but to the cation as well. The coefficients that
are given in Equations (14) and (15) are the ion-specific equation coefficients for the [OE3Am]+
cation. Determination of the ion-specific equation coefficients for [BMMorp]+
is slightly more
involved and requires knowledge of the equation coefficients for the [C(CN)3]–
anion, which are
available in the published tabulations in the paper by Stephens and co-workers.[41] The equation
coefficients for the [C(CN)3]–
anion are: (cp,anion = –0.079; ep,anion = 0.056; sp,anion = 0.276; ap,anion
= 1.223; bp,anion = –0.070 and vp,anion = –0.008) and (ck,anion = –0.098; ek,anion = 0.094; sk,anion
= 0.290; ak,anion = 1.338; bk,anion = –0.145 and lk,anion = 0.005). Subtraction of the anion-specific
equation coefficients from the respective coefficients in Equations (16) and (17) results in the
following set of coefficients for the [BMMorp]+
cation: (cp,cation = –0.239; ep,cation = 0.318; sp,cation
= 0.675; ap,cation = –1.223; bp,cation = –4.414 and vp,cation = 3.130) and (ck,cation = –0.676; ek,cation
= 0.277; sk,cation = 2.472; ak,cation = 2.369; bk,cation = 0.597 and lk,cation = 0.638). The calculated
cation-specific equation coefficients can be combined with the 19 anion-specific equation coeffi-
cients that we have previously determined.[41,44,45] For each of the four cations that we have
studied in the present communication, we can build log K and log P Abraham model predictive
correlations for an additional 19 different IL solvents. This increases the Abraham model’s
predictive capability by an additional 76 different IL solvents.
4. Conclusion
The Abraham model has been shown to provide very good mathematical descriptions of the
water-to-anhydrous IL and gas-to-anhydrous IL partition coefficients for solutes dissolved in
([AllMIm]+
[N(CN)2]–
), ([AllMIm]+
[Tf2N]–
), ([B3EP]+
[E2PO4]–
), ([OE3Am]+
[Tf2N]–
) and
([BMMorp]+
[C(CN)3]–
). The derived correlations back-calculate the observed partition coefficient
data to within standard deviations from SD = 0.073 log units to SD = 0.128 log units. As part of
the present communication, cation-specific equation coefficients have been calculated for
[AllMIm]+
, [OE3Am]+
, [B3EP]+
and [BMMorp]+
. For each of the four cations that we have
studied in the present communication, we can build log K and log P Abraham model predictive
correlations for an additional 19 different IL solvents. This increases the Abraham model’s
predictive capability by an additional 76 different IL solvents.
Acknowledgements
Bihan Jiang and Melissa Horton thank the University of North Texas’s Texas Academy of Math and Science
(TAMS) program for a summer research award.
Disclosure statement
No potential conflict of interest was reported by the authors.
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28 B. JIANG ET AL.