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The equation coefficients reported by Li and co-workers measuring the solubility of 1,6-Hexanediamine in binary solvents (1-butanol + cyclohexane) using the Jouyban-Acree equation are found to be wrong. The back-calculated values according to Jouyban-Acree equation published by Li and co-workers are inconsistent with the mole fraction solubility in the reported paper, and there is a big difference between the calculated values and the values reported by the author. The equation coefficients listed in Table 6 calculated by author are in error.

A polemic is given in terms of the equation that Shen et al. used to calculate the molar entropy of dissolution of tylosin tartrate in methanol + (tetrahydrofuran or acetone). The equations of the molar enthalpy and molar entropy used in the calculation combine to give a numerical value of zero for the Gibbs energy of dissolution at all temperatures, which is inconsistent with the mathematical expression used for the molar entropy of dissolution.

Information regarding relevant solid–liquid balance pertaining to 3-nitro-1H-pyrazole (3-NP) within a range of solvents is of a high significance to the preliminary analysis of industry-related uses. Here, through the gravimetric approach, 3-NP dissolvability in various clean solvents, i.e., n-butyl acetate (NBAC), isopropyl acetate (IPAC), n-propyl acetate (NPAC), ethyl acetate (EAC), methyl acetate (MAC), n-propanol (Pro-OH), ethanol (EtOH), methanol (MeOH), toluene (PhMe), acetonitrile (AN), tetrahydrofuran (THF), acetone (DMK), water and benzene (Ph), was explored under an atmosphere pressure of 0.1 MPa and within a range of temperature (T = 283.15 K to 323.15 K). In accordance with the outcomes, with the rise of the temperature, 3-NP dissolvability increased in fourteen solvents taken. Among all the solvents, water exhibiting the maximum polarity had the minimum dissolvability, while methanol exhibited the maximum quality of solubility. At a particular temperature, 3-NP’s quality of solubility followed that of MeOH (8.54 × 10-2, 323.15 K) > EtOH (6.46 × 10-2, 323.15 K) > Pro-OH (6.27 × 10-2, 323.15 K) > AN (4.18 × 10-2, 323.15 K) > DMK (3.76 × 10-2, 323.15 K) > MAC (3.20 × 10-2, 323.15 K) > EAC (2.82 × 10-2, 323.15 K) > NPAC (2.25 × 10-2, 323.15 K) > NBAC (1.91 × 10-2, 323.15 K) > IPAC (1.25 × 10-2, 323.15 K) > THF (1.07 × 10-2, 323.15 K) > PhMe (7.29 × 10-3, 323.15 K) > Ph (3.23 × 10-3, 323.15 K) > water (2.16 × 10-3, 323.15 K). The experimental data of 3-NP had a correlation according to Wilson approach, NRTL model, λh equation and the modified Apelblat equation. As was revealed from the fitting outcomes, the optimal correlative result of the experimental information was given through NRTL model. The relative average deviation (102ARD) and the root-mean-square deviation (104RMSD) achieved were lower than 9.44 and 23.75 separately. Moreover, 3-NP dissolvability characteristics in solvents studied were analyzed with the use of the Hansen dissolvability coefficient (δd, δp, δh, δt, and Δδt) here. This study determined the effect exerted by interacting processes pertaining to solvent–solute and solvent–solvent molecules upon the 3-NP’s quality of solubility with the association of linear solving energy in accordance with the descriptors of the solvents. Moreover, the mixing characteristics of 3-NP in 14 pure solvents, including the mixing Gibbs energy (ΔmixG), mixing enthalpy (ΔmixH) and mixing entropy (ΔmixS), were determined and analyzed through Wilson approach. The result of ΔmixG

Errors are found in the listed thermodynamics-related characteristics reported by Zheng and colleagues. The authors' determined thermodynamics-related characteristics of Table 5 were discovered to be inconsistent, and do not abide by the thermodynamics-related association that ∆G = ∆H - T∆S.

On the basis of the references, we checked our article carefully and discussed in depth the corresponding section. We found a mistake that Eq. (5) was written incorrectly, and the values of root-mean-square deviation (RMSD) calculated were incorrect. The errors should be corrected and in this comment the values of RMSD calculated with the corrected equation of Eq. (1) are presented.

The comments regarding “Solid-liquid equilibrium solubility, thermodynamic properties and solvent effect of 3,4-dinitro-1H-pyrazole in different pure solvents” helps to improve the quality of the article published by the authors recently. According to the comments, the article of the authors was checked in depth again. Such discrepancy was because the thermodynamic mixing properties in the our original work of the authors were calculated incorrectly, and did not comply with the standard thermodynamic relationship, i.e., ∆mixG = ∆mixH - T∆mixS. The errors should be corrected and in this reply the values of the ∆mixG, ∆mixH and ∆mixS were recalculated.

Errors are discovered in the tabulated thermodynamic mixing properties reported by Li and coworkers. The authors' calculated thermodynamic mixing properties were found to be internally inconsistent, and do not obey the standard thermodynamic relationship that ∆mixG = ∆mixH - T∆mixS.

In the present study, the solubility of 1-methyl-3,4,5-trinitropyrazole (MTNP) was determined by a dynamic laser monitoring at T = (283.15, 288.15, 293.15, 298.15, 303.15, 308.15, 313.15, 318.15 and 323.15) K in twelve pure solvents, including water, benzene (Ph), dimethyl sulfate (DMS), methylbenzene (PhMe), tetrahydrofuran (THF), methanol (MeOH), ethanol (EtOH), 1,2-dichloroethane (DCE), nitromethane (NM), acetonitrile (ACN), ethyl acetate (EA) and formic acid (FA), at atmospheric pressure (P = 0.1 MPa). In the temperature range from 283.15 K to 323.15 K, the mole fraction solubility values of MTNP in water, Ph, DMS, PhMe, THF, MeOH, EtOH, DCE, NM, ACN, EA and FA were 0.000008–0.000072, 0.003495–0.025271, 0.002153–0.037197, 0.001602–0.012304, 0.002103–0.074525, 0.000318–0.001625, 0.003752–0.048205, 0.017836–0.047105, 0.008408–0.016783, 0.003579–0.012367, 0.004460–0.022006 and 0.220917–0.443206. As revealed from the experimental results, the solubility of MTNP in twelve pure solvents increased with the increase in the temperature. The solubility behaviors of MTNP in investigated solvents were analyzed with the Hansen solubility parameter (δd, δp, δh, δt, δv and Δδt). The Kamlet-Taft parameters were calculated to delve into the solvent effect. Subsequently, the measured solubility data was correlated with five thermodynamic models, i.e., the modified Apelblat equation, λh equation, NRTL model, Wilson model and Two-Suffix Margules model. Overall, the NRTL model provided the most satisfactory fitting results. As revealed from the results, the minimum average values of relative mean deviation (102ARD) and root-mean square deviation (104RMSD) were determined with the NRTL model that achieved the values of 2.06 and 1.49. Furthermore, the dissolution thermodynamic parameters, including mixing enthalpy (ΔmixH), mixing entropy (ΔmixS) and mixing Gibbs energy (ΔmixG) were calculated according to the Wilson model, and the relative contributions of enthalpy %ζH and entropy %ζS were also calculated. It can be seen that the dissolution of MTNP in a given solvent is spontaneous and entropy driven.

In this paper, the solubility of 5,5′-bis(2,4,6-trinitrophenyl)-2,2′-bis(1,3,4-oxadiazole) (TKX-55) was first determined by a dynamic laser monitoring at T = (293.15, 298.15, 303.15, 308.15, 313.15, 318.15, 323.15, 328.15 and 333.15) K in fourteen pure solvents, including nitrobenzene (NB), methylethylketone (MEK), dimethyl carbonate (DMC), N,N-dimethylformamide (DMF), methoxybenzene (MOB), ethenyl acetate (VAC), 1,2-propanediol (PDO), cyclohexanone (CYC), epichlorohydrin (ECH), 1-butanol (NBA), n-butyl acrylate (BA), dimethyl sulfoxide (DMSO), tributyl phosphate (TBP) and 2-butanol (IBA), under atmospheric pressure (P = 0.1 MPa). Besides, supersolubility as well as the metastable zone width of TKX-55 in PDO, BA, DMSO and IBA was determined by the dynamic laser monitoring method. The experimental results showed that the solubility of TKX-55 in fourteen pure solvents increases with increasing temperature and the metastable zone width decreases with increasing temperature. The metastable zone width is approximately 2.49 K–43.26 K. In addition, in order to improve the applicability of the solubility, the modified Apelblat equation, λh equation, the polynomial empirical equation, van't Hoff equation and NRTL equation were used to correlate the solubility data of TKX-55, and the results showed that all models can give a satisfactory correlation. The average root-mean-square deviation (102RMSD) values were 1.71, 8.91, 2.33, 6.12 and 3.30, respectively. Moreover, Hansen solubility parameter was used for explaining the solubility order of TKX-55 in selected solvents, the consequences showed that solubility order of TKX-55 resulted from the comprehensive function of several solubility parameters. The solubility parameter of Δδt between TKX-55 and solvents reached from 1.27 MPa0.5 to 15.28 MPa0.5. Furthermore, three kinds of thermodynamic properties of the mixing enthalpy (ΔmixH), the mixing entropy (ΔmixS) and the mixing Gibbs energy (ΔmixG) of TKX-55 in selected solvents were calculated by NRTL equation and the results turned out that the dissolution process was spontaneous. Besides, thermal properties of TKX-55 were measured by differential scanning calorimetry (DSC). The results showed that the melting temperature and the fusion enthalpy were 640.65 K and 19.60 kJ·mol−1, respectively. Finally, solubility values and thermodynamic relations of TKX-55 in fourteen pure solvents would be invoked as fundamental data and models regarding the purification process.