Measurement and Correlation of the Solubility of Enrofloxacin in Different Solvents from (303.15 to 321.05) K

Liu, Mengjiao; Fu, Hualin; Yin, Dai-ping; Lu, Chaocheng; Cao, Hongxin; Zhou, Jianyu

doi:10.1021/je5002158

Cited by 27 publications

(13 citation statements)

References 16 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…The apparatus for the solubility measurements was similar to that in our previous work, which has been described in detail in the literature. , Briefly, an excess amount of TMP and a known amount of pure solvent (ethanol, water, ethyl acetate, acetonitrile, or 2-propanol) or a binary mixture of ethanol + water or 2-propanol + water (the mass fraction of the organic solvent in the mixed solvent was varied by 0.1 from 0 to 0.5) were added into an Erlenmeyer flask with a stopper for each measurement. Then the Erlenmeyer flasks were placed into a constant-temperature shaker for 24 h to allow the contents reach solid–liquid equilibrium.…”

Section: Methodsmentioning

confidence: 99%

Solubility of Trimethoprim in Selected Pure Solvents and (Water + Ethanol/2-Propanol) Mixed-Solvent Systems

Yin

Liu

et al. 2015

J. Chem. Eng. Data

Self Cite

View full text Add to dashboard Cite

Trimethoprim (TMP) is an important antibacterial synergist in human and veterinary medicine. In this work, the solubilities of TMP in five pure solvents (ethanol, water, ethyl acetate, acetonitrile, and 2-propanol) and two binary mixtures (ethanol + water and 2-propanol + water) were measured by an equilibrium method over the temperature range from (293.15 to 322.65) K under atmospheric pressure. The experimental results show that in the pure solvents the solubility of TMP increases with increasing temperature, and the solubility decreases in the following order: ethanol > acetonitrile > 2-propanol > ethyl acetate > water. In the mixed solvents, the solubility of TMP increases with increasing temperature and mass fraction of the organic solvent. The mole-fraction solubility of TMP was observed to be the highest in the mixed solvent 50% ethanol/2-propanol, and the lowest mole-fraction solubility of TMP was found in water. Three correlating models (the modified Apelblat equation, the λh equation, and the ideal model) were used to correlate the experimental solubility values in the pure solvents, and four models (the modified Apelblat equation, the λh equation, the ideal model, and the CNIBS/R-K model) were applied to correlate the experimental solubilities in the mixed solvents. All of these thermodynamic models gave satisfactory correlation results, with the modified Apelblat equation showing better fitting degree than the other three equations. Furthermore, the standard molar enthalpy of the TMP during the dissolving process (ΔH sol °) was also determined in this work, and the results show that the dissolution process is endothermic.

show abstract

Section: Methodsmentioning

confidence: 99%

Solubility of Trimethoprim in Selected Pure Solvents and (Water + Ethanol/2-Propanol) Mixed-Solvent Systems

Yin

Liu

et al. 2015

J. Chem. Eng. Data

Self Cite

View full text Add to dashboard Cite

show abstract

“…The estimation of thermodynamic functions of solutions is a prerequisite for modeling SLE studies. The dissolution enthalpy (Δ d H °) vary according to interactions of solvent–solute, solvent–solvent, and solute–solute, whereas the entropy change (Δ d S °) is a function of the disorder degree or randomness of a system. , Thus, in order to interpret the solubility of para - tert -butylbenzoic acid in different pure solvents and mixed solvent systems better, the thermodynamic functions of solutions were evaluated. As all of the systems under consideration were nonideal, the enthalpy of dissolution (Δ d H °)), the entropy of dissolution (Δ d S °), and the Gibbs free energy of dissolution (Δ G d ) can be calculated as follows: where M represents either H , S , or G .…”

Section: Resultsmentioning

confidence: 99%

Measurement and Modeling of Solubility of para-tert-Butylbenzoic Acid in Pure and Mixed Organic Solvents at Different Temperatures

Aniya

Mohammed

et al. 2017

J. Chem. Eng. Data

View full text Add to dashboard Cite

The solid−liquid phase equilibrium of para-tertbutylbenzoic acid in methanol, ethanol acetic acid, propan-2-ol, hexane, toluene, 1-octanol, para-tert-butyltoluene, methyl 4-tert-butylbenzoate, and binary (methanol + methyl 4-tertbutylbenzoate) mixed solvent have been determined experimentally within the temperature range of 293.15−333.15 K at atmospheric pressure using a static equilibrium method. The solubility of para-tert-butylbenzoic acid increased with the increase in temperature for the pure solvents, while in the case of methanol + methyl 4-tert-butylbenzoate a maximum solubility effect is achieved at 0.6115 solute-free mole fraction of methanol. The experimental solubility data in pure and binary solvent system were correlated by the modified Apelbat equation, the λh (Buchowski) equation, and the NRTL model, among which the modified Apelbat equation provided better agreement than those with the other models. Furthermore, to understand the nature of interactions involved in a solute−solvent system, the dissolution thermodynamic properties, including enthalpy, entropy, and Gibbs free energy, were determined. This experimental data will be an aid for the design and optimization of the separation and purification processes involving para-tert-butylbenzoic acid.

show abstract

“…One characteristic feature of this work is underlining the correlation between the coefficient signs for each function, that is, when a 1 ; a 2 possessed the negative signs (a 0 ) adopts the positive sign and vice versa, which may also be present for other processes that are not addressed herein (e.g., the suggestion in [27] also according to Ref. [13] in Table 2 for acetonitrile). 2.…”

Section: Discussionmentioning

confidence: 98%

“…The Clarke-Glew equation has been used in various works for many other types of processes, for example, research on solubility [13] and phase balances [14,15].…”

Section: Significance Of Heat Capacity For the Reaction Processmentioning

confidence: 99%

Thermal dissociation in terms of the second law of chemical thermodynamics

Mianowski

Urbańczyk

2016

J Therm Anal Calorim

View full text Add to dashboard Cite

Starting from the relationship between Gibbs free energy and equilibrium constant of a chemical reaction (ECCR) and taking into account its temperature dependence according to Kirchhoff, Eq. (12), we arrive at the three-parametric Eq. (26). In going this way, we employ the relationship between the ECCR and the degree of conversion of the solid phase using Eqs. (20) and (21). We find that there is a compensating effect between the coefficients of the equation (i.e., a 1 ; a 2 ) in the form of a linear equation, which has been attributed to the enthalpy-entropy compensation. According to current state of knowledge, this result applies both to the chemical reactions resulting in individual chemical bond formation as well as in thermal decomposition. When the heat capacity of such chemical reactions decreases linearly along with temperature, it can adopt the value of the (arithmetic mean) average, and the negative sign determines the elements of the functional equations valid for theoretical (Eq. 26) and experimentally fit (Eq. 32) states. For calcite, several possibilities arising from equilibrium changes in the conversion rate vs. temperature are compared by taking into account the CDV L'vov theory.

show abstract

Measurement and Correlation of the Solubility of Enrofloxacin in Different Solvents from (303.15 to 321.05) K

Cited by 27 publications

References 16 publications

Solubility of Trimethoprim in Selected Pure Solvents and (Water + Ethanol/2-Propanol) Mixed-Solvent Systems

Solubility of Trimethoprim in Selected Pure Solvents and (Water + Ethanol/2-Propanol) Mixed-Solvent Systems

Measurement and Modeling of Solubility of para-tert-Butylbenzoic Acid in Pure and Mixed Organic Solvents at Different Temperatures

Thermal dissociation in terms of the second law of chemical thermodynamics

Contact Info

Product

Resources

About