Mole Fraction Of Ethanol Research Articles

Kinetic model for the ammoxidation of ethanol to acetonitrile

A comprehensive kinetic study, based on V-based catalysts (Vanadium Pyro-Phosphate, VPP, VOx/TiO2 and VOx/ZrO2), was modeled to retrieve the surface reaction mechanism and kinetic parameters for the ammoxidation of ethanol to acetonitrile. In all the cases, the catalysts showed a moderate to good acetonitrile selectivity, that in turn resulted correlated primarily to the reaction temperature, while the byproducts distribution was more influenced by the thermodynamic stability of the reacting mixture.A large and comprehensive collection of data on ammoxidation of C2 substrates for acetonitrile production was analysed and 5 groups of experiments on VOx-based catalysts (operating in the temperature range 250–450 °C) were selected. The base reactant was ethanol and ammonia and oxygen were fed in optimal ratios of 1:3–1:4 mol/mol.A kinetic model was then derived applying the Langmuir-Hinshelwood-Hougen-Watson (LHHW) approach to accepted catalytic oxidation mechanisms: for every catalytic material, eight to ten reactions with rates described by the Arrhenius formula were employed. Fixing the reaction orders according to the mechanistic assumption and adjusting only the kinetic and adsorption parameters, the calculated molar fractions of ethanol, ammonia, acetonitrile and ethylene resulted in good agreement with the extensive collection of experimental data available.

Solvent effect on solubility and preferential solvation analysis of buprofezin dissolved in aqueous co-solvent mixtures of N,N-dimethylformamide, ethanol, acetonitrile and isopropanol

The mole fraction solubility of buprofezin in aqueous co-solvent mixtures of N,N-dimethylformamide (DMF,1) + water (2), ethanol (1) + water (2), isopropanol (1) + water (2) and acetonitrile (1) + water (2) over the temperature range from (273.15 to 318.15) K was reported. At the same composition of DMF, ethanol, isopropanol or acetonitrile and temperature, the buprofezin solubility was highest in DMF (1) + water (2) mixtures. By using the Jouyban-Acree model, the buprofezin solubility was correlated obtaining RAD lower than 5.86% and RMSD lower than 15.60 × 10−4. Quantitative values for local mole fraction of DMF (ethanol, isopropanol or acetonitrile) and water nearby the buprofezin were calculated through the Inverse Kirkwood–Buff integrals method applied to the solubility. The values of preferential solvation parameters (δx1,3) were negative in water-rich mixtures but positive in co-solvent compositions from 0.19, 0.20 (0.25) or 0.25 to 1 in mole fraction of DMF, isopropanol, ethanol or acetonitrile, respectively. It was conjecturable that in water-rich mixtures, the hydrophobic hydration around the nonpolar methyl groups and aromatic ring group of buprofezin played a relevant important role in the solvation. The preference of buprofezin in water-rich mixtures could be explained in terms of the higher basic behaviour of buprofezin molecules interacting with the proton-donor functional groups of the water. In addition, solute-solvent and solvent-solvent interactions of buprofezin in the DMF (ethanol, isopropanol or acetonitrile) + water mixtures were investigated from the solubility data by using the linear solvation energy relationships concept. The variation of buprofezin solubility depended mainly upon the hydrogen bond acidity and cavity term for ethanol (isopropanol) + water mixtures, and the cavity term for DMF (acetonitrile) + water mixtures.

Isobaric Vapor–Liquid Equilibria for the Quaternary System Water + Ethanol + Ethylene Glycol + Choline Chloride and the Ternary System Water + Ethanol + Choline Chloride at 101.3 kPa

An organic salt choline chloride (ChCl) was introduced in ethylene glycol (EG) for improving the entrainer performance for ethanol dehydration by extractive distillation. The mixed solvent EG + ChCl with molar ratios of 8:1, 4:1, 2:1, and 4:3 were tested through vapor–liquid equilibrium (VLE) measurement for the quaternary system water + ethanol + EG + ChCl at 101.3 kPa. Data were also measured for the ternary system water + ethanol + ChCl. VLE behavior of the quaternary system was modeled successfully using the NRTL equation. The mean absolute deviations for the quaternary data were 0.24 K for equilibrium temperature and 0.0041 for vapor mole fraction of ethanol, while deviations for the ternary data were 0.15 K and 0.0032. As compared with EG alone, the existence of ChCl in the mixed solvent decreases the activity coefficient of water and increases the activity coefficient of ethanol, both leading to the enhancement of the relative volatility of ethanol to water. The azeotrope of water + ethanol can be removed with the addition of EG + ChCl 4:3 at a solvent mass fraction of 0.062, showing favorable entrainer performance for ethanol dehydration by extractive distillation.

Solubility and thermodynamic properties of azlocillin in pure and binary solvent systems

The solubility data of azlocillin (ALPC) in nine mono-solvents (methanol, ethanol, isopropanol, methyl acetate, ethyl acetate, isopropyl acetate, acetone, acetonitrile, tetrahydrofuran) and two different binary solvent systems (methanol + isopropanol, ethanol + isopropanol), under atmospheric pressure, were experimentally measured via a static gravimetric method in the temperature range from 278.15 K to 323.15 K. According to the experimental results, it could be found that the solubility of ALPC in all the tested pure and binary solvent systems increased with the rise of temperature at the measurable ranges. The solubility order of ALPC in the nine mono-solvents is generally ranked as: (ethanol or tetrahydrofuran) > acetone > (methanol or acetonitrile) > methyl acetate > ethyl acetate > isopropanol > isopropyl acetate. The solubility data of ALPC in both binary solvent systems increase with the increasing of mole fraction of methanol or ethanol. The modified Apelblat equation, λh equation, and NRTL model were applied to correlate the experimental solubility data of ALPC in pure and mixed solvent systems while the CNIBS/R-K model was also used for the mixed solvent systems. Finally, the mixing and dissolution thermodynamic properties of ALPC in the studied systems were calculated by the NRTL model and were analyzed. It was found that the mixing and dissolution processes of ALPC in the tested systems were spontaneous, endothermic and entropy-driven.

Low-temperature chemistry triggered by probe cooling in a low-pressure premixed flame

Previous studies on sampling probe effects in the premixed flat flame showed that the temperature in the preheat zone can be lowered down to low-temperature oxidation regime (e.g., 400–800 K). In order to investigate the contribution of the low-temperature chemistry in flame-sampling experiments, a stoichiometric laminar premixed flat flame of ethylene/oxygen/argon was investigated at 30 Torr using synchrotron vacuum ultraviolet photoionization mass spectrometry (SVUV-PIMS) in this work. Ethyl hydroperoxide (C2H5OOH) was identified and quantified in the present experiment, providing an experimental evidence for the existence of low-temperature chemistry in flame-sampling experiments. In addition to C2H5OOH, the formation of several other intermediates like ethanol and formaldehyde was also influenced by the low-temperature chemistry in the present flame-sampling experiment. A literature kinetic model (Hashemi et al., 2017) was used for predictions and analyses. The difference between the predicted maximum mole fractions of C2H5OOH with the perturbed and unperturbed temperature profiles can reach up to five orders of magnitude. The great improvement of the predictions with the perturbed temperature profiles indicates that the observed low-temperature chemistry in the present flame sampling experiment originates from the probe-induced perturbations, which lowers down the temperature window of the preheat zone and leads to a temperature drop of more than 400 K compared with the unperturbed temperature profile. Through modeling analysis, the low-temperature oxidation chemistry of ethylene involved in the present flame-sampling experiment was discussed. The influence of low-temperature chemistry in the present experiment has also been demonstrated by comparing the model predictions with/without key reactions at low temperatures. It is concluded that predicted maximum mole fractions of several low-temperature chemistry related intermediates, i.e. C2H5OOH, ethanol and formaldehyde, are strongly reduced without these reactions, while low-temperature chemistry only has negligible influence on the predictions of the fuel and the majority of flame intermediates. Furthermore, preliminary experiments were also conducted in ethane, propene and n-butane flames under similar conditions, where hydroperoxides can also be observed.

Spectroscopic Insight on Ethanol-Induced Aggregation of Papain.

In this contribution, the structural and dynamic changes occurring to papain in ethanol-water binary solvent mixtures have been investigated and compared with its denatured state. Steady-state fluorescence, solvation dynamics, time-resolved rotational anisotropy, circular dichroism (CD), and single molecular-level fluorescence correlation spectroscopic (FCS) studies were performed for this purpose. In ethanol-water mixtures with XEtOH = 0.6, N-(7-dimethylamino-4-methylcoumarin-3-yl)iodoacetamide (DACIA)-tagged papain was found to undergo a blue shift of 12 nm, while in the presence of 5 M GnHCl, a red shift of 5 nm was observed. Solvation dynamics of the system was also found to be different in the presence of these external agents. In ethanol-water mixtures, the average solvation time was found to increase almost 2-fold as compared to that in water, while in the presence of GnHCl, only a marginal increase could be observed. These changes of DACIA-tagged papain in ethanol-water mixtures are attributed to the aggregation of the protein in the presence of ethanol. The residual anisotropy was found to increase 14-fold, and the rotational time component corresponding to the rotation of the probe molecule was found to increase by 4-fold in the ethanol-water mixture which also gives a notion of the papain aggregation. Atomic force microscopy (AFM) confirms this aggregate formation, which is also quantified by the FCS study. The hydrodynamic radius of the protein aggregates in ethanol-water mixtures was calculated to be ∼155 Å as compared to the corresponding value of 18.4 Å in the case of native monomer papain. Also, it confirmed that the aggregate formation takes place even in the nanomolar concentration of papain. Analysis of circular dichroism spectra of papain showed that an increase in the β-sheet content of papain at the expense of α-helix and the random coil with an increase of the ethanol mole fraction may be responsible for this aggregation process.

Preferential Solvation of Vitamin C in Binary Solvent Mixtures Formed by Methanol, Ethanol, n-Propanol, Isopropanol and Water

The present work is an investigation of the preferential solvation of vitamin C in five solvent mixtures: ethanol (1) + methanol (2), isopropanol (1) + methanol (2), ethanol (1) + water (2), n-propanol (1) + water (2) and isopropanol (1) + water (2) from the reported solubility data by employing the method of inverse Kirkwood–Buff integrals. In the ethanol (1) + water (2) mixtures with compositions 0.25 < x1 < 1.00, and isopropanol (1) + water (2) and n-propanol (1) + water (2) mixtures with compositions 0.20 < x1 < 1.00, the local mole fractions of ethanol, isopropanol or n-propanol are smaller than those of the bulk solutions. Consequently, the values of preferential solvation parameter (δx1,3) are negative, which shows that vitamin C is preferentially solvated by water. Perhaps the structuring of water molecules near the vitamin C molecule contributes to lowering of the δx1,3 from the neat solvent water to negative values in the three solvent mixtures. Vitamin C acts as a Lewis base that interacts with the acidic hydrogen atoms of water. Nevertheless, in the ethanol (1) + methanol (2) and isopropanol (1) + methanol (2) mixtures, vitamin C is preferentially solvated neither by methanol nor by ethanol nor isopropanol.

Equilibrium solubility of dinitolmide in several neat solvents and binary aqueous co-solvent mixtures: Experimental determination and thermodynamic analysis

The dinitolmide solubility in twelve pure solvents such as methanol, ethanol, n-propanol, isopropanol, n-butanol, ethylene glycol (EG), ethyl acetate, dimethyl sulfoxide (DMSO), acetonitrile, cyclohexane, 1,4-dioxane and water and co-solvent mixtures of ethanol (1) + water (2), isopropanol (1) + water (2) and EG (1) + water (2) was studied by using a saturation shake-flask method over the temperatures from 283.15 K to 328.15 K under local atmospheric pressure p = 101.2 kPa. It was highest in solvent DMSO and lowest in solvent water. The achieved solubility data in monosolvents was mathematically described through the modified Apelblat equation; and in the binary mixtures, the Jouyban-Acree model. For the monosolvents, the maximum values of root-mean-square deviation and relative average deviation were 2.71 × 10−4 and 1.27%, respectively; and for the binary solvent mixtures, 0.276 × 10−4 and 1.46%. The solubility was correlated to KAT parameters and cavity term based on linear solvation energy relationships concept to investigate on the solvent effect. Results showed that the solubility in monosolvents depended significantly upon the Hildebrand parameter and nonspecific dipolarity/polarizability interactions. Quantitative values for the local mole fraction of ethanol (isopropanol or EG) and water around the dinitolmide were computed by using the Inverse Kirkwood–Buff integrals method. Dinitolmide was preferentially solvated by water in water-rich compositions; while in the intermediate and co-solvent-rich compositions for the aqueous mixtures of ethanol (isopropanol or EG), dinitolmide is preferentially solvated by the co-solvent. The preferential solvation magnitude of dinitolmide was higher in isopropanol mixtures than that in the other two solvent mixtures. Furthermore, transfer Gibbs free energy (ΔtrGo), enthalpy (ΔtrHo), and entropy (ΔtrSo) were deduced, demonstrating that the solubilization capacity was more favorable in the intermediate concentration of ethanol (isopropanol or EG).

Equilibrium solubility determination, modelling and preferential solvation of bioactive iminodibenzyl in aqueous co-solvent mixtures at various temperatures

The mole fraction solubility of bioactive iminodibenzyl in aqueous co-solvent mixtures of ethanol, ethylene glycol (EG), dimethyl sulfoxide (DMSO) and isopropanol was examined by the saturation shake-flask method over the temperature range from 283.15 K to 328.15 K at pressure of 101.2 kPa. The experimental solubility increased with increasing temperature at a given co-solvent composition and decreased with the increasing mass fraction of water in each binary system. The maximum solubility was found in pure co-solvent. Given the same temperature and mass fraction of the co-solvent, the solubility of iminodibenzyl was greater in (DMSO + water) than in the other three co-solvent systems. The solid crystal examples of iminodibenzyl was tested by X-ray power diffraction showing no polymorphic transformation, solvate formation or crystaltransition during entire experiments. The Jouyban-Acree model was employed to correlate the measured solubility. The calculated data were in alignment to measured values and RAD and RMSD data were no more than 3.08% and 10.37 × 10−4, respectively. Furthermore, quantitative values for the local mole fraction of ethanol (EG, DMSO or isopropanol) and water around the iminodibenzyl were acquired by using the Inverse Kirkwood–Buff integrals method. The preferential solvation parameters for ethanol, EG, DMSO or isopropanol were positive in the four co-solvent mixtures in intermediate and co-solvent-rich compositions, which indicated that iminodibenzyl was preferentially solvated by the co-solvent. iminodibenzyl could act mainly as a Lewis acid interacting with proton-acceptor functional groups of the co-solvents.

Thermodynamic and Theoretical solvation parameters for 2-amino-4,5-dimethylthiophene-3-carboxamide(ADTC) in Ethanol and Mixed EtOH-H2O solvents

The molar solubility for 2-amino-4,5-dimethylthiophene-3-carboxamide (ADTC) in pure ethanol and mixed ethanol (EtOH)- water solvents were measured at five different temperatures, 293.15, 298.15, 303.15, 308.15, and 313.15 K in the used mixed solvents, the solubility were increase by increase in the mole fraction of ethanol in the mixtures and increase of temperature due to more salvation parameters. All the solvation and thermodynamic parameters for ADTC in mixed EtOH+ H2O solvents were evaluated like solubility products, Gibbs free energies, enthalpies and entropies of solvation and discussed. Theoretical calculations for (ADTC) were done quantum mechanically by using Gaussian on set of calculations in ethanol for evaluating the different thermodynamic parameters.

Copolymer of m-phenylenediamine and anthranilic acid (P(mPDA-co-AA): new precursor of MnO Nanoparticles

ABSTRACTPoly(m-phenylenediamine-co-anthranilic acid) P(mPDA-co-ANTH) and their doped Mn, Ni, and Cu poly (m-phenylenediamine-co-anthranilic acid) have been synthesized and characterized. Mn P(mPDA-co- AA) has been used as a molecular precursor of MnO nanoparticles. The spectral, optical, refractive index, solubility and thermal properties of the synthesized polymers have been measured and discussed. The optical band gap (Eg) measurements indicated that Mn P(mPDA-co-AA) has wider optical band than the neat P(mPDA-co-AA). MnO nanoparticles have been synthesized from calcination of MnP(mPDA-co-AA) at 800oC. The obtained nanoparticles have been characterized by XRD and HR-TEM. The average size of MnO nanoparticles was found to be 71 nm. The refractive index measurements indicated slight change in the refractive index values of the polymer solution than that of the pure solvent. The solubility of the synthesized polymers in ethanol, dimethyl formamide (DMF)-aqueous mixed solvents was found to increase as the mole fractions of both ethanol and DMF increases. UV spectra of the synthesized polymers in ethanol, DMF-aqueous mixed solvents indicated blue shift and hyperchromic effect.

Novel computational tools based on bioinformatic and chemoinformatic data to complement zebrafish embryo teratogenicity test

The mole fraction solubility of buprofezin in aqueous co-solvent mixtures of N,N-dimethylformamide (DMF,1) + water (2), ethanol (1) + water (2), isopropanol (1) + water (2) and acetonitrile (1) + water (2) over the temperature range from (273.15 to 318.15) K was reported. At the same composition of DMF, ethanol, isopropanol or acetonitrile and temperature, the buprofezin solubility was highest in DMF (1) + water (2) mixtures. By using the Jouyban-Acree model, the buprofezin solubility was correlated obtaining RAD lower than 5.86% and RMSD lower than 15.60 × 10−4. Quantitative values for local mole fraction of DMF (ethanol, isopropanol or acetonitrile) and water nearby the buprofezin were calculated through the Inverse Kirkwood–Buff integrals method applied to the solubility. The values of preferential solvation parameters (δx1,3) were negative in water-rich mixtures but positive in co-solvent compositions from 0.19, 0.20 (0.25) or 0.25 to 1 in mole fraction of DMF, isopropanol, ethanol or acetonitrile, respectively. It was conjecturable that in water-rich mixtures, the hydrophobic hydration around the nonpolar methyl groups and aromatic ring group of buprofezin played a relevant important role in the solvation. The preference of buprofezin in water-rich mixtures could be explained in terms of the higher basic behaviour of buprofezin molecules interacting with the proton-donor functional groups of the water. In addition, solute-solvent and solvent-solvent interactions of buprofezin in the DMF (ethanol, isopropanol or acetonitrile) + water mixtures were investigated from the solubility data by using the linear solvation energy relationships concept. The variation of buprofezin solubility depended mainly upon the hydrogen bond acidity and cavity term for ethanol (isopropanol) + water mixtures, and the cavity term for DMF (acetonitrile) + water mixtures.

The validity of the potential model in predicting the structural, dynamical, thermodynamic properties of the unary and binary mixture of water-alcohol: Ethanol-water case

Thermodynamic, dynamical, and structural properties of ethanol are numerically studied using two ethanol models: TraPPE-UA and OPLS-AA. These properties are computed with temperatures ranging from 200K to 300K, with steps of 10K, and also with different mole fractions of ethanol at 300K. The TraPPE-UA and OPLS-AA models are mixed with two water models: SPCE and TIP4P. These models have been previously shown to be the best models of methanol among nine different models. In our previous paper on methanol-water mixtures, the OPLS-AA model showed superiority over the TraPPE-UA model in predicting most properties. In this study, we show that the TraPPE-UA has better predictions in all computed properties when compared to the experimental results, except for the total structure factor of mixing with respect to the second maximum.

Thermodynamics of R-(+)-2-(4-Hydroxyphenoxy)propanoic Acid Dissolution in Methanol, Ethanol, and Methanol-Ethanol Mixture

The solubilities of R-(+)-2-(4-hydroxyphenoxy)propanoic acid (D-HPPA) in methanol, ethanol and various methanol-ethanol mixtures are determined in the temperature range from 273.15 to 323.15 K at atmospheric pressure using a laser detecting system. The solubilities of D-HPPA increase with increasing mole fraction of ethanol in the methanol–ethanol mixtures. Experimental data were correlated with Buchowski-Ksiazczak λh equation and modified Apelblat equation; the first one gives better approximation for the experimental results. The enthalpy, entropy and Gibbs free energy of D-HPPA dissolution in methanol, ethanol and methanol-ethanol mixtures were also calculated from the solubility data.

Experimental Study and Thermodynamic Modeling of Methane Hydrate Dissociation Conditions in the Simultaneous Presence of BMIM-BF4 and Ethanol in Aqueous Solution

Experimental and thermodynamic results for methane hydrate dissociation conditions in the simultaneous presence of ethanol and 1-butyl-3-methylimidazolium tetrafluoroborate (BMIM-BF4) ionic liquid (IL) in aqueous solution are presented. Three different aqueous solutions including solution 1 (0.0142 mole fraction of ethanol, 0.0060 mole fraction of BMIM-BF4), solution 2 (0.0348 mole fraction of ethanol, 0.0059 mole fraction of BMIM-BF4) and solution 3 (0.0549 mole fraction of ethanol, 0.0058 mole fraction of BMIM-BF4) were used. An isochoric pressure-search method was used to perform the measurements. The experimental pressure and temperature ranges are (3.18 to 8.32) MPa and (273.6 to 283.3) K, respectively. The thermodynamic inhibition effects of these solutions on methane hydrate dissociation were observed and solution 3 leads to the strongest inhibition effect. The average hydrate dissociation temperature reduction for methane hydrate in the presence of solutions 1, 2, and 3 are approximately 1.0, 2.2,...

Experimental Data and New Binary Interaction Parameters for Ethanol-Water VLE at Low Pressures Using NRTL and UNIQUAC

Separation of ethanol from many sources, mainly renewable sources, is commonly achieved by atmospheric distillation. Even so, there is new technologies for ethanol separation and purification: pressure-swing distillation, extractive distillation, adsorption with molecular sieves and vacuum membrane distillation. The design, rating and optimization of these process technologies requires a reliable and universal thermodynamic modeling approach capable of represents the ethanol-water system properties, and in particular the vapor-liquid equilibrium (VLE) near the azeotropic point. This study resume experimental data of VLE for ethanol-water system at vacuum pressures (13.15-101.32 kPa) and its corresponding thermodynamic consistency test results using the Redlich-Kister method. The parameters and constants for the detailed thermodynamic modeling of the ethanol-water system using polar fluid Soave-Redlich-Kwong equation of state (polar-SRK) are resumed, as well as the standard binary interaction parameters for NRTL and UNIQUAC excess Gibbs energy models commonly used for the simulations involved in the chemical process engineering activities. This study contains the regression of new binary interaction parameters in a temperature dependent form compatible with the most process simulation software, for NRTL and UNIQUAC, and its validation using experimental data for azeotropic points at different low pressures with errors of less than 1% for temperature and ethanol molar fraction in vapor phase estimation. The new parameters were tested using isobaric experimental data for VLE at 3 under-atmospheric pressures obtaining correlation coefficient (R 2 ) values of about 1. The calculations were performed using python 3.4® codes developed and supplied by S&SE and Aspen properties® V8.6 provided by the Universidad Nacional de Colombia.

Solubility of Genistin in Ethanol/Acetone + Water and Daidzein in Ethanol + Water Co-solvent Mixtures Revisited: IBKI Preferential Solvation Method

The preferential solvation parameters (δx1,3) of genistin in ethanol/acetone (1) + water (2) and daidzein in ethanol (1) + water (2) co-solvent mixtures at elevated temperatures were derived from available solubility data using the inverse Kirkwood–Buff integral method. The values of δx1,3 varied non-linearly with the co-solvent (1) proportion in all the aqueous mixtures. For the three co-solvent mixtures, the values of δx1,3 were negative in water-rich mixtures, which indicated that daidzein or genistin was preferentially solvated by water and can act as Lewis bases to establish hydrogen bonds with the proton-donor functional groups of water (1). The same behavior was also observed for daidzein in ethanol (1) + water (2) and acetone (1) + water (2) mixtures with co-solvent-rich composition. For daidzein in ethanol (1) + water (2) mixtures with composition 0.24 < x1 < 1, and genistin in ethanol (1) + water (2) and acetone (1) + water (2) mixtures with intermediate compositions, the local mole fractions of ethanol or acetone were higher than those of the mixtures and therefore the δx1,3 values were positive, which indicated that genistin and daidzein were preferentially solvated by the co-solvent. In these regions, daidzein and genistin were acting as a Lewis acid with ethanol or acetone molecules.

Doped Poly(m-phenylenediamine-co-aniline) (P(mPD-co-ANI)): Synthesis, Characterization, Physical Properties, and Precursor for CuO Nanoparticles

ABSTRACTPoly(m-phenylenediamine-co-aniline) P(mPD-co-ANI) and Mn-, Ni-, and Cu-doped poly(m-phenylenediamine-co-aniline) (M-P(mPD-co-ANI)) have been synthesized and characterized. Cu-P(mPD-co-ANI) has been used as a molecular precursor of CuO nanoparticles. The spectral, optical, refractive index, solubility, and thermal properties of the synthesized polymers have been measured and discussed. The optical bandgap (Eg) measurements indicated that Ni(P(mPD-co-ANI)) has wider optical band than the pure (P(mPD-co-ANI)). Calcination of Cu-P(mPD-co-ANI) at 600°C produced (CuO) nanoparticles. The obtained nanoparticles have been characterized by XRD and TEM. The average size of CuO nanoparticles was found to be 42 nm. The refractive index measurements indicate slight change in the refractive index values of the polymer solution than that of pure solvent. The solubility of the synthesized polymers in ethanol, dimethyl formamide (DMF)–aqueous mixed solvents was found to increase as the mole fractions of both ethanol and DMF increase. The UV spectra of the synthesized polymers in ethanol, DMF–aqueous mixed solvents indicate blueshift and hyperchromic effect.

Solubility Determination and Modeling and Dissolution Thermodynamic Properties of Raspberry Ketone in Binary Solvent Mixtures of Ethanol and Water

The solubility and dissolution thermodynamic properties of raspberry ketone in a set of binary solvent mixtures (ethanol + water) with different compositions were experimentally determined by static gravimetrical method in the temperature range of 283.15–313.15 K at 0.10 MPa. The solubility of raspberry ketone in this series of ethanol/water binary solvent mixtures was found to increase with a rise in temperature and the rising mole fraction of ethanol in binary solvent mixtures. The van’t Hoff, modified Apelblat and 3D Jouyban–Acree–van’t Hoff equations were increasingly applied to correlate the solubility in ethanol/water binary solvent mixtures. The former two models could reach better fitting results with the solubility data, while the 3D model can be comprehensively used to estimate the solubility data in all the ratios of ethanol and water in binary solvent mixtures at random temperature. Furthermore, the changes of dissolution thermodynamic properties of raspberry ketone in experimental ethanol/water solvent mixtures were obtained by van’t Hoff equation. For all the above experiments, these dissolution processes of raspberry ketone in experimental ethanol/water binary solvent mixtures were estimated to be endothermic and enthalpy-driven.

Determination and Modeling of the Solubilities of Oleanolic Acid and Ursolic Acid in Ethanol + Sodium Hydroxide + Water Mixed Solvents from T = 283.2 to 323.2 K

The solubilities of oleanolic acid (OA) and ursolic acid (UA) in ethanol + sodium hydroxide + water mixed solvents were measured at different temperatures (283.2, 298.2, 293.2, 298.2, 303.2, 308.2, 313.2, 318.2, and 323.2 K). The solubility of OA in the mixed solvents increased with temperature. However, the solubility of UA in the mixed solvents first increased with temperature, and then decreased with temperature. The solubilities of both OA and UA increased with the initial mole fraction of ethanol in the mixed solvents. The addition of NaOH could improve the solubilities of OA and UA in the aqueous ethanol solution. The solubility of OA was correlated with temperature by the van’t Hoff model, the modified Apelblat model and the λh model, and the results indicated that the λh model had better correlation. The solubility of UA was correlated with temperature only by an empirical cubic equation.