Density and Viscosity of Magnesium Chloride Solution in N

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Density and Viscosity of Magnesium Chloride Solution in N‑Methylacetamide over the Temperature Range from 308.15 to 328.15 K at Ambient Pressure Alexey A. Dyshin* and Michael G. Kiselev

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Laboratory of NMR-Spectroscopy and Computer Simulations, G.A. Krestov Institute of Solution Chemistry of the Russian Academy of Sciences, 1 Akademicheskaya Street, Ivanovo 153045, Russia ABSTRACT: The values of densities in N-methylacetamide solutions of magnesium chloride have been measured at atmospheric pressure using an Anton Paar DMA 5000M high-precision vibrating U-tube densimeter at temperatures ranging from 308.15 to 328.15 K, ΔT = 5 K, and in the concentration range from 0 to 0.083 mol·kg−1. The kinematic viscosity for these mixtures has been measured at the same thermodynamic conditions using an Ubbelohde viscometer. Partial molar volumes of N-methylacetamide, partial molar volumes of magnesium chloride, apparent molar volumes of magnesium chloride, and thermal expansion coefficients of solutions have been calculated from the experimental data. Dependences of these properties on the magnesium chloride concentrations have been discussed. Growth in the salt concentration increases the solution density and viscosity, and an increase in the temperature reduces the solution density and viscosity, at the same time. An increase in the temperature and salt concentration leads to a decrease in the magnesium chloride partial molar volume.

1. INTRODUCTION Inorganic single- and double-charged ions play an essential role in various cellular processes. Magnesium is one of the most important bioactive elements involved in metabolic processes in the human body, located in almost all cells. This substance is part of plasma substitutes, regulators of water and electrolyte balance, and parenteral nutrition. The most widely used magnesium salt is chloride. It is used in dermatology, dentistry, ophthalmology, etc., as well as in the manufacturing of various drugs. Magnesium chloride has antiedematous, regenerating, anti-inflammatory, and analgesic effects. It is also widely used in the food industry, labeled as food additive E511 and is used as a thickener and hardener. This compound is part of soft drinks, diet, and baby food. N-Methylacetamide (NMA) is a unique solvent that is characterized by a high dielectric constant and a high dipole moment. These characteristics allow it to dissolve many compounds well, and its small molecule is very convenient for studying the effect of hydrogen bonds of peptide groups, which are the basis of the protein structure. Being a mimetic of the structure of amino acids, NMA attracts the attention of many researchers.1−14 This is a good model compound for studying hydrogen bonds between groups of peptides and is widely used as a model of peptides and membranes during computer simulation.1,11−16 Based on these arguments, the study of density and viscosity of magnesium chloride and N-methylacetamide mixtures in a wide range of concentrations and temperatures is really important. In fact, viscometry and densimetry carry information about the structural changes occurring in solutions. In this work, the © XXXX American Chemical Society

density and viscosity of solutions of magnesium chloride in Nmethylacetamide were measured at temperatures ranging from 308.15 to 328.15 K.

2. EXPERIMENTAL SECTION 2.1. Chemicals and Preparation of Solutions. All of the chemicals used were received from Acros Organics and SigmaAldrich. All of the reagents were previously dehydrated. The initial N-methylacetamide was dried by the standard procedure described in ref 17. The first stage consisted in fractional crystallization of NMA. Then, calcium oxide was annealed for 8 h at 1373 K. After cooling in a dry box, calcium oxide was added to N-methylacetamide. The mixture was boiled for 3 h at the temperature of 358 K and then distilled under reduced pressure with the selection of the middle fraction. After distillation, NMA was stored in a flask under reduced pressure. The initial magnesium chloride was dried at 333 K under vacuum. All of the purified reagents were stored in a dry box with dry gaseous nitrogen. The moisture content of the used reagents after drying was determined by a Karl Fischer coulometer (MKC-710, Kyoto Electronics Manufacturing Co., Ltd.). The water content was found to be 0.001% for NMA and 0.003% for MgCl2. A summary of the used materials is presented in Table 1. The liquid mixtures were prepared by mass using a Sartorius Genius ME235S electronic analytical balance with the Received: January 15, 2019 Accepted: March 28, 2019

A

DOI: 10.1021/acs.jced.9b00046 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

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Table 1. Purity of Chemicals Used in This Study abbreviated name

IUPAC name

NMA

N-methylacetamide

79-16-3

Acros Organics

MgCl2

magnesium chloride

7786-30-3

Sigma-Aldrich

CASRN

source

initial water content, %

purification method

final water content, %

analysis method

>99

0.374

0.001

KFCa

99.99

0.120

fractional crystallization and distillation vacuum drying

0.003

KFCa

initial purity, %

a

Coulometric titration by the Karl Fischer method.

experimental uncertainty of ±1 × 10−5 g. The solutions were prepared from degassed solvents under the conditions that minimized the moisture uptake from the atmosphere air. After weighing in a dry box, the prepared mixtures in hermetically sealed flasks were placed in an ultrasonic bath in which the dissolution process was carried out. Depending on the magnesium chloride concentration, the process lasted from 30 to 60 min. 2.2. Experimental Apparatus. 2.2.1. Density Measurement. The densities of the initial NMA and N-methylacetamide−magnesium chloride solutions were measured using an Anton Paar DMA 5000M (Graz, Austria) high-precision densimeter with an oscillating U-tube. The device has automatic viscosity correction and is operated in the static mode. The experimental uncertainty provided by the manufacturer for density measurement is ±1 × 10−6 g·cm−3. The temperature was determined with an integrated platinum resistor thermometer together with Peltier elements provided by a high-precision thermostat. The temperature setting accuracy reached in the cell was ±0.001 K. The densimeter was calibrated by water (“liquid density standard” from Anton Paar, GmbH, that is in compliance with the NIST requirements) and dry air before each measurement. To prevent the formation of air bubbles in the solutions, all of the mixtures were preheated, to by 5 K above, and after that the solution was cooled step-by-step before carrying out the density measurements. The setup design and experimental procedure are detailed in refs 18, 19. All of the measurements were carried out at ambient pressure of 99.6 ± 0.8 kPa. 2.2.2. Kinematic Viscosity Measurement. The kinematic viscosity was measured using an automatic Ubbelohde capillary viscometer with a suspended level and optical detection of the liquid flow time. The measurement error was ±2 × 10−9 m2· s−1. The viscometer was always kept in a vertical position in a water thermostat. The precision of temperature maintenance in the viscosity measurements was ±0.01 K. Before the series of measurements, the viscosimeter was calibrated using bidistilled and degassed water at seven temperatures (303, 308, 313, 318, 323, 328 and 333 K). After calibration, the viscosimeter was tested for high-purity pentanol-1 at various temperatures. Pentanol has viscosity close to NMA and is well purified. The viscosimeter was filled without an atmospheric air access. After that, the pressure equalization was carried out by the air passing through the moisture absorbing tube. The experimental procedure is detailed in ref 20.

Table 2. Comparison of Measured N-Methylacetamide Densities (ρ) and Dynamic Viscosities (η) with Literature Values at Temperatures Ranging from 308.15 to 328.15 K ρ × 10−3/kg·m−3 solvent NMA

T/K

this work

308.15

0.94571

313.15

0.94153

318.15

0.93733

323.15

0.93316

328.15

0.92893

lit. 21,22

0.9459 0.9459123 0.941526 0.941722 0.937622 0.9387224 0.933243 0.933527 0.929073 0.929172

η × 103/Pa·s this work

lit.

3.4878

3.38024 3.6725 2.904121 3.01226 2.607221 2.67324 2.41128 2.49723 2.24472 2.24823

3.0734 2.7230 2.4377 2.1935

The experimental values of kinematic viscosity and densities for the N-methylacetamide−magnesium chloride system at the temperatures of 308.15, 313.15, 318.15, 323.15, and 328.15 K are reported in Table 3. The experimental data on the kinematic viscosity and densities were used to calculate the dynamic viscosity by the following equation24 η = ρ·ν (1) where η and ν are the dynamic (Pa·s) and kinematic (m2·s−1) viscosities of the solution, respectively, and ρ is the solution density (kg·m−3). The initial experimental data on the density were processed as a linear relationship. Then, these data were used to calculate the volumetric properties by eqs 2−5.29 The solutions thermal expansion coefficients were computed by the following equation30 1 i ∂ρ y αp = − ·jjj zzz ρ k ∂T { p

(2) −1

where αp is the thermal expansion coefficient (K ), T is the temperature (K), and ρ is the density of the solutions (kg· m−3). The partial molar volumes of N-methylacetamide were calculated by the following equation31 V1 =

3. RESULTS AND DISCUSSION The density values of the net solvent over the temperature range from 308.15 to 328.15 K and the comparison of these values with the literature data are presented in Table 2. The difference between the data on the density and viscosity of the solvent is due to different degrees and methods of solvent purification.

M1 mM1·(1000 + mM 2) ∂ρ + · ∂m ρ 1000·ρ2

(3)

where V1 is the partial molar volume of N-methylacetamide (m3·mol−1), ρ is the density of the solutions (kg·m−3), M1 is the molar mass of N-methylacetamide (kg·mol−1), M2 is the molar mass of MgCl2 (kg·mol−1), and m is the molality of magnesium chloride (mol·kg−1). The data on the densities were used to calculate the partial (eq 4) and apparent (eq 5) molar volumes of magnesium B

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Table 3. Densities (ρ), Kinematic (ν) and Dynamic (η) Viscosities, Partial Molar Volumes of N-Methylacetamide (V1), Partial Molar Volumes of MgCl2 (V2), Apparent Molar Volumes of MgCl2 (Vφ), and Thermal Expansion Coefficients (αp) for the NMethylacetamide−MgCl2 System at Temperatures Ranging from 308.15 to 328.15 K, ΔT = 5 K, and Pressure of 99.6 ± 0.8 kPaa m/mol·kg−1

ρ × 10−3/kg·m−3

ν × 106/m·2 s−1

η × 103/Pa·s

0 0.00111 0.00400 0.00479 0.00663 0.00734 0.00868 0.01179 0.01529 0.02124 0.02416 0.05144 0.08310

0.94571 0.94576 0.94590 0.94594 0.94603 0.94606 0.94613 0.94627 0.94645 0.94672 0.94686 0.94815 0.94960

3.688 3.692 3.703 3.705 3.713 3.715 3.720 3.731 3.744 3.767 3.777 3.882 4.000

3.488 3.491 3.502 3.505 3.512 3.514 3.520 3.531 3.544 3.566 3.577 3.681 3.798

0 0.00111 0.00400 0.00479 0.00663 0.00734 0.00868 0.01179 0.01529 0.02124 0.02416 0.05144 0.08310

0.94153 0.94157 0.94169 0.94173 0.94181 0.94185 0.94192 0.94207 0.94224 0.94253 0.94267 0.94394 0.94545

3.264 3.268 3.279 3.281 3.288 3.290 3.295 3.306 3.319 3.339 3.348 3.444 3.554

3.073 3.077 3.087 3.090 3.097 3.099 3.103 3.114 3.127 3.147 3.156 3.251 3.361

0 0.00111 0.00400 0.00479 0.00663 0.00734 0.00868 0.01179 0.01529 0.02124 0.02416 0.05144 0.08310

0.93733 0.93737 0.93751 0.93754 0.93763 0.93766 0.93773 0.93787 0.93804 0.93833 0.93847 0.93977 0.94126

2.905 2.907 2.918 2.919 2.926 2.929 2.933 2.943 2.954 2.975 2.985 3.075 3.181

2.723 2.725 2.735 2.737 2.743 2.747 2.750 2.760 2.771 2.792 2.801 2.890 2.994

0 0.00111 0.00400 0.00479 0.00663 0.00734 0.00868 0.01179 0.01529 0.02124 0.02416 0.05144 0.08310

0.93316 0.93320 0.93333 0.93337 0.93345 0.93348 0.93354 0.93370 0.93387 0.93415 0.93429 0.93560 0.93711

2.612 2.615 2.623 2.626 2.630 2.632 2.637 2.646 2.656 2.671 2.681 2.757 2.849

2.438 2.440 2.448 2.451 2.455 2.457 2.462 2.471 2.480 2.495 2.505 2.579 2.670

V1 × 106/m3·mol−1 T = 308.15 K 77.29 77.29 77.29 77.29 77.29 77.29 77.29 77.29 77.29 77.29 77.29 77.29 77.29 T = 313.15 K 77.63 77.63 77.63 77.63 77.63 77.63 77.63 77.63 77.63 77.63 77.63 77.63 77.64 T = 318.15 K 77.98 77.98 77.98 77.98 77.98 77.98 77.98 77.98 77.98 77.98 77.98 77.98 77.98 T = 323.15 K 78.33 78.33 78.33 78.33 78.33 78.33 78.33 78.33 78.33 78.33 78.33 78.33 78.33

C

V2 × 106/m3·mol−1

Vφ × 106/m3·mol−1

αp × 104/K−1

48.17 48.17 48.15 48.15 48.14 48.14 48.13 48.12 48.10 48.07 48.06 47.93 47.78

48.169 48.162 48.160 48.156 48.154 48.151 48.144 48.135 48.121 48.114 48.049 47.974

8.871 8.870 8.868 8.867 8.865 8.864 8.863 8.860 8.857 8.851 8.849 8.823 8.794

47.72 47.71 47.70 47.69 47.69 47.68 47.68 47.66 47.64 47.62 47.60 47.47 47.32

47.715 47.708 47.706 47.701 47.700 47.696 47.689 47.681 47.666 47.659 47.594 47.519

8.911 8.910 8.907 8.906 8.905 8.904 8.903 8.900 8.896 8.891 8.888 8.862 8.833

47.51 47.51 47.49 47.49 47.48 47.48 47.47 47.45 47.44 47.41 47.40 47.26 47.11

47.509 47.502 47.500 47.495 47.494 47.490 47.483 47.475 47.460 47.453 47.388 47.312

8.951 8.950 8.947 8.946 8.944 8.944 8.942 8.939 8.936 8.930 8.928 8.902 8.872

47.18 47.17 47.16 47.16 47.15 47.14 47.14 47.12 47.11 47.08 47.06 46.93 46.78

47.178 47.171 47.169 47.164 47.162 47.159 47.152 47.143 47.129 47.122 47.056 46.980

8.991 8.990 8.987 8.986 8.985 8.984 8.983 8.980 8.976 8.971 8.968 8.942 8.911

DOI: 10.1021/acs.jced.9b00046 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

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Table 3. continued m/mol·kg−1

ρ × 10−3/kg·m−3

ν × 106/m·2 s−1

η × 103/Pa·s

0 0.00111 0.00400 0.00479 0.00663 0.00734 0.00868 0.01179 0.01529 0.02124 0.02416 0.05144 0.08310

0.92893 0.92898 0.92912 0.92916 0.92924 0.92929 0.92935 0.92949 0.92968 0.92995 0.93009 0.93140 0.93291

2.361 2.364 2.370 2.373 2.377 2.379 2.382 2.390 2.399 2.413 2.420 2.487 2.563

2.194 2.196 2.203 2.204 2.208 2.211 2.214 2.221 2.230 2.244 2.251 2.317 2.391

V1 × 106/m3·mol−1 T = 328.15 K 78.69 78.69 78.69 78.69 78.69 78.69 78.69 78.69 78.69 78.69 78.69 78.69 78.69

V2 × 106/m3·mol−1

Vφ × 106/m3·mol−1

αp × 104/K−1

46.97 46.96 46.95 46.94 46.94 46.93 46.93 46.91 46.89 46.86 46.85 46.72 46.57

46.965 46.958 46.956 46.951 46.950 46.946 46.939 46.930 46.916 46.909 46.843 46.767

9.031 9.030 9.028 9.027 9.025 9.024 9.023 9.020 9.017 9.011 9.008 8.982 8.951

a m is the molality of MgCl2 in the MgCl2 + NMA solutions. The standard uncertainties (u) are u(T) = 0.01 K for the density and viscosity measurements, and the expanded uncertainties (U) are U(m) = 2 × 10−5 mol·kg−1, U(V1) = 3 × 10−8 m3·mol−1, U(V2) = 3 × 10−8 m3·mol−1, U(Vφ) = 2 × 10−9 m3·mol−1, U(αp) = 2 × 10−7 K−1, Ur(ρ) = 0.002, Ur(ν) = 0.01, and Ur(η) = 0.01 for the 0.95 level of confidence.

temperatures. From the figure, we can conclude that both the temperature and the concentration of the electrolyte affect the value of the partial molar volume of the solute. A temperature increase destroys the hydrogen bond network and, as a result, leads to an increase in the coefficient of thermal expansion (Figure 2) and a decrease in the solution density and the

chloride. The equations for the calculations were received from refs 32, 33, respectively. V2 =

Vφ =

M2 (1000 + mM 2) ∂ρ − · ∂m ρ ρ2 1000·(ρ0 − ρ) m ·ρ ·ρ0

+

(4)

M2 ρ

(5) −1

where V2 is the partial molar volume of MgCl2 (cm ·mol ), Vφ is the apparent molar volume of magnesium chloride (cm3· mol−1), ρ is the density of the solutions (g ·cm−3), ρ0 is the density of NMA (g·cm−3), M1 is the molar mass of Nmethylacetamide (g·mol−1), M2 is the molar mass of MgCl2 (g· mol−1), and m is the molality of magnesium chloride (mol· kg−1). The calculated values for the N-methylacetamide−magnesium chloride system are reported in Table 3. The experimental density values are linear and can be expressed as a function of temperature and concentration, and as expected, they decrease with a temperature increase and increase with MgCl2 concentration growth. Figure 1 shows the dependences of the partial molar volume of magnesium chloride in the NMA solution at various 3

Figure 2. Thermal expansion coefficients (α) for the Nmethylacetamide−magnesium chloride solutions as a function of molality (m). This work, black ■, 308.15 K; red ●, 313.15 K; green ▲, 318.15 K; blue ▼, 323.15 K; and aqua ◆, 328.15 K.

kinematic viscosity (Table 3). The growth in the salt molality leads to a decrease in the values of both the partial molar volume (Figure 1) and the coefficient of thermal expansion (Figure 2). A similar picture for lithium, zinc, and calcium chlorides was observed in refs 1−4. Apparently, this is due to the solvation processes occurring in the solutions. NMA has a high dielectric constant and a large dipole moment, and therefore the electrostriction may play an important role in the solvation processes of electrolytes.34 The phenomenon of electrostriction observed in solutions has a significant effect on their structure. This leads to changes in the bulk properties of the solutions. Due to electrostriction, magnesium ions bind the solvent molecules to solvates and, therefore, the partial molar volume of the solute and the thermal expansion coefficients of the mixtures decrease. Thus, a “denser” structure of the solution is formed. The temperature dependences are different.

Figure 1. Partial molar volumes (V2) of magnesium chloride as a function of molality (m). This work, black ■, 308.15 K; red ●, 313.15 K; green ▲, 318.15 K; blue ▼, 323.15 K; and aqua ◆, 328.15 K. D

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partially supported by the Russian Foundation for Basic Research (RFBR grant no. 17-03-00309 A).

As the temperature increases, the hydrogen bonds get partially broken and, as a consequence, the thermal expansion coefficients increase. However, this process is not dominant. A similar picture is observed in NMA solutions with lithium, calcium, and zinc chlorides.1−4 From the experimental data on the kinematic viscosity, we have calculated the dynamic viscosity values, which are presented in Figure 3. These dependences correspond to the

Notes

The authors declare no competing financial interest.

■

ACKNOWLEDGMENTS We would like to thank Dr Olga V. Eliseeva for help and suggestions during this study and comments on the various versions of the manuscripts. All of the densimetric studies were performed on an Anton Paar DMA 5000M vibrating tube densimeter at the Center for Joint Use of Scientific Equipment “The Upper Volga Region Center of Physico-Chemical Research”.

■

Figure 3. Dynamic viscosity (η) for the N-methylacetamide− magnesium chloride solutions at different temperatures as a function of molality (m). This work, black ■, 308.15 K; red ●, 313.15 K; green ▲, 318.15 K; blue ▼, 323.15 K; and aqua ◆, 328.15 K.

general concepts of the behavior of electrolytes in organic solvents. Since NMA can form hydrogen bonds through hydrogen bonding to nitrogen, and through the oxygen of the carbonyl group, it tends to form branched hydrogen-bonded clusters. As expected, the concentration dependences of the dynamic viscosity decrease with a temperature increase, and an increase in the salt concentration leads to viscosity growth.

4. CONCLUSIONS In this work, the density and viscosity of solutions of MgCl2 in N-methylacetamide have been measured. The dependences of the volumetric characteristics of solutions on temperature and concentration of components have been analyzed. An increase in temperature and concentration leads to a decrease in the partial molar volume of magnesium chloride. We explain this phenomenon by taking into account two factors. First, the increasing temperature destroys the hydrogen bond in N-methylacetamide. Second, the average distance between the cation and NMA in the first solvation shell of magnesium ions decreases as a result of their strong charge− dipole interaction. The effect of electrostriction is caused by the competition between the interaction of magnesium ions with NMA and the energy of the hydrogen bonds of the solvent molecules.

■

REFERENCES

(1) Manin, N.; da Silva, M. C.; Zdravkovic, I.; Eliseeva, O.; Dyshin, A.; Yasar, O.; Salahub, D. R.; Kolker, A. M.; Kiselev, M. G.; Noskov, S. Y. LiCl solvation in N-methyl-acetamide (NMA) as a model for understanding Li+ binding to an amide plane. Phys. Chem. Chem. Phys. 2016, 18, 4191−4200. (2) Dyshin, A. A.; Eliseeva, O. V.; Kiselev, M. G. Density and Viscosity of Zinc Chloride Solution in N-Methylacetamide over the Temperature Range from 308.15 to 328.15 K at Atmospheric Pressure. J. Chem. Eng. Data 2018, 63, 3130−3135. (3) Dyshin, A. A.; Eliseeva, O. V.; Kiselev, M. G. Density and Viscosity of N-Methylacetamide−Calcium Chloride Mixtures over the Temperature Range from 308.15 to 328.15 K at Atmospheric Pressure. J. Chem. Eng. Data 2017, 62, 4128−4132. (4) Dyshin, A. A.; Eliseeva, O. V.; Kiselev, M. G. Correction to “Density and Viscosity of N-Methylacetamide−Calcium Chloride Mixtures over the Temperature Range from 308.15 to 328.15 K at Atmospheric Pressure”. J. Chem. Eng. Data 2018, 63, 3167−3167. (5) Biernacki, K. A.; Kaczkowska, E.; Bruździak, P. Aqueous solutions of NMA, Na2HPO4, and NaH2PO4 as models for interaction studies in phosphate−protein systems. J. Mol. Liq. 2018, 265, 361− 371. (6) Cunha, A. V.; Salamatova, E.; Bloem, R.; Roeters, S. J.; Woutersen, S.; Pshenichnikov, M. S.; Jansen, T. L. C. Interplay between Hydrogen Bonding and Vibrational Coupling in Liquid NMethylacetamide. J. Phys. Chem. Lett. 2017, 8, 2438−2444. (7) Yu, H.; Mazzanti, C. L.; Whitfield, T. W.; Koeppe, R. E.; Andersen, O. S.; Roux, B. A Combined Experimental and Theoretical Study of Ion Solvation in Liquid N-Methylacetamide. J. Am. Chem. Soc. 2010, 132, 10847−10856. (8) Zhao, J.; Wang, J. Direct Anionic Effect on Water Structure and Indirect Anionic Effect on Peptide Backbone Hydration State Revealed by Thin-Layer Infrared Spectroscopy. J. Phys. Chem. B 2018, 122, 68−76. (9) Renugopalakrishnan, V.; Urry, D. W. A theoretical study of Na+ and Mg+2 binding to the carbonyl oxygen of N-methyl acetamide. Biophys. J. 1978, 24, 729−738. (10) Manin, N. G.; Kolker, A. M. Thermodynamic properties of LiCl solutions in N-methylacetamide at 308.15−328.15 K. Russ. J. Phys. Chem. A 2017, 91, 2293−2301. (11) Kang, N. S.; Kang, Y. K. Assessment of CCSD(T), MP2, and DFT methods for the calculations of structures and interaction energies of the peptide backbone with water molecules. Chem. Phys. Lett. 2017, 687, 23−30. (12) Dudev, T.; Mazmanian, K.; Lim, C. Competition between Li+ and Na+ in sodium transporters and receptors: Which Na+-Binding sites are “therapeutic” Li+ targets? Chem. Sci. 2018, 9, 4093−4103. (13) Torii, H. Strategy for Modeling the Electrostatic Responses of the Spectroscopic Properties of Proteins. J. Phys. Chem. B 2018, 122, 154−164. (14) Rubio-Martinez, J.; Tomas, M. S.; Perez, J. J. Effect of the solvent on the conformational behavior of the alanine dipeptide

AUTHOR INFORMATION

Corresponding Author

*E-mail: [email protected]. Tel: +7 4932 351869. Fax: +7 4932 336237. ORCID

Alexey A. Dyshin: 0000-0002-0263-642X Funding

This work was performed as part of the government contract (registration number 01201260481). This research was E

DOI: 10.1021/acs.jced.9b00046 J. Chem. Eng. Data XXXX, XXX, XXX−XXX

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deduced from MD simulations. J. Mol. Graphics Modell. 2017, 78, 118−128. (15) Paul, S.; Paul, S. Influence of temperature on the solvation of N-methylacetamide in aqueous trehalose solution: A molecular dynamics simulation study. J. Mol. Liq. 2015, 211, 986−999. (16) Zimmermann, M. O.; Boeckler, F. M. Targeting the protein backbone with aryl halides: systematic comparison of halogen bonding and π...π interactions using N-methylacetamide. Med. Chem. Commun. 2016, 7, 500−505. (17) Weissberger, A. Organic Solvents. Physical Properties and Method of Purification; Interscience Publishers, Inc.: New York, 1955; Vol. VII, p 519. (18) Ivanov, E. V.; Lebedeva, E. Y.; Petrovskaya, S. G.; Baranov, V. V.; Kravchenko, A. N.; Ivanova, N. G. Volume-related interaction parameters for dilute solutions of Mebicaret (2,4-dimethyl-6,8diethylglycoluril) in normal and heavy water between 278.15 K and 318.15 K. J. Mol. Liq. 2017, 242, 160−167. (19) Ivanov, E. V.; Lebedeva, E. Y.; Abrosimov, V. K. Standard Volumetric Properties of Tetra-N-ethylglycoluril (Bicaret) in Ordinary and Heavy Water at Temperatures from (278.15 to 318.15) K and Ambient Pressure. J. Chem. Eng. Data 2015, 60, 2079−2089. (20) Dyshin, A. A.; Eliseeva, O. V.; Kiselev, M. G. Dependence of Bulk and Viscosity Characteristics of Naphthalene Solutions in Methanol-Heptane Mixtures at 298.15 K. Russ. J. Phys. Chem. A 2013, 87, 336−339. (21) Boodida, S.; Bachu, R. K.; Patwari, M. K.; Nallani, S. Volumetric and transport properties of binary liquid mixtures of Nmethylacetamide with lactones at temperatures (303.15 to 318.15) K. J. Chem. Thermodyn. 2008, 40, 1422−1427. (22) Nain, A. K. Densities and volumetric properties of (acetonitrile + an amide) binary mixtures at temperatures between 293.15 K and 318.15 K. J. Chem. Thermodyn. 2006, 38, 1362−1370. (23) Nallani, S.; Boodida, S.; Tangeda, S. J. Density and Speed of Sound of Binary Mixtures of N-Methylacetamide with Ethyl Acetate, Ethyl Chloroacetate, and Ethyl Cyanoacetate in the Temperature Interval (303.15 to 318.15) K. J. Chem. Eng. Data 2007, 52, 405−409. (24) Victor, P. J.; Hazra, D. K. Excess Molar Volumes, Viscosity Deviations, and Isentropic Compressibility Changes in Binary Mixtures of N-Methylacetamide + 2-Methoxyethanol and NMethylacetamide + Water at (308.15, 313.15, and 318.15) K. J. Chem. Eng. Data 2002, 47, 79−82. (25) Vijaya Kumar Naidu, B.; Chowdoji Rao, K.; Subha, M. C. S. Densities, Viscosities, and Excess Properties for Binary Mixtures of Some Glycols and Polyglycols in N-Methylacetamide at 308.15 K. J. Chem. Eng. Data 2003, 48, 625−627. (26) Sears, P. G.; Stoeckinger, T. M.; Dawson, L. R. Dielectric constants, Viscosities, Fusion Point curves, and other properties of three nonaqueous binary systems. J. Chem. Eng. Data 1971, 16, 220− 222. (27) Pacák, P. Refractivity and density of some organic solvents. Chem. Papers 1991, 45, 227−232. (28) Dawson, L. R.; Sears, P. G.; Graves, R. H. Solvents Having High Dielectric Constants. II. Solutions of Alkali Halides in NMethylacetamide from 30 to 60°. J. Am. Chem. Soc. 1955, 77, 1986− 1989. (29) Harned, H. S.; Owen, B. B. The Physical Chemistry of Electrolytic Solution, 2nd ed.; Reinhold Publishing Corporation: New York, 1950. (30) Makowska, A.; Szydłowski, J. Densities, Viscosities, and Speeds of Sound of the Nitromethane + 1-Pentanol System near the Critical Demixing Temperature: Effect of Deuterium Substitution. J. Chem. Eng. Data 2005, 50, 1365−1369. (31) Ivlev, D. V.; Dyshin, A. A.; Eliseeva, O. V.; Kiselev, M. G. The Volume Characteristics and Molecular Dynamics Simulation of Nonaqueous Solutions of Aliphatic Alcohols. Russ. J. Phys. Chem. A 2009, 83, 209−213. (32) Eliseeva, O. V.; Golubev, V. V.; Dyshin, A. A.; Kiselev, M. G.; Al’per, G. A. A Volumetric Investigation of Solvophobic Effects in

Halide−n-Alkanol−n-Alkane Ternary Systems. Russ. J. Phys. Chem. 2006, 80, 205−209. (33) Dyshin, A. A.; Eliseeva, O. V.; Kiselev, M. G.; Al’per, G. A. The Volume Characteristics of Solution of Naphthalene in HeptaneEthanol Mixtures at 298.15 K. Russ. J. Phys. Chem. A 2008, 82, 1258− 1261. (34) Marcus, Y. Electrostriction in Electrolyte Solutions. Chem. Rev. 2011, 111, 2761−2783.

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DOI: 10.1021/acs.jced.9b00046 J. Chem. Eng. Data XXXX, XXX, XXX−XXX