Solid–liquid equilibrium and thermodynamic research of 3-Thiophenecarboxylic acid in (water+acetic acid) binary solvent mixtures

Measurement, correlation of the solubility and solution thermodynamics of 2-cyanoguanidine in (methanol+water) binary solvent systems from T=(283.15 to 343.15)K

“…(2) As shown in figure 2, there is an apparent consistency between our solubility results at T = (283. 15 [29]) is only about 3.4%, which is lower than the claimed uncertainty of 4%. And their corresponding experimental temperature of other values reported in reference [29] are listed in The solubility of 2-cyanoguanidine in a binary (water + methanol) mixtures and the calculations of the parameters with models are listed in table 4.…”

“…The solubility of 2-cyanoguanidine in (water + methanol) mixed solvents with different mass fraction of methanol (0.100, 0.200, 0.300, 0.400, 0.500 and 0.600) on a solute-free basis was determined at T = (283. 15 The specific procedure used to measure the melting point of 2-cyanoguanidine is as follows: Based on method of measuring melting temperature in GB/T 617-2006, the sample was dried and ground into a fine powder according to the protocol of product standards, and then the sample was placed in a clean and dry [29]. b x is the solubility of 2-cyanoguanidine in reference [2]; x e is the experimental solubility of 2-cyanoguanidine was determined in this work; the standard uncertainties u are u(T) = 0.01 K, u(P) = 0.5 kPa, u r (x e ) = 0.04. melting point tube.…”

“…However, the solubility of 2-cyanoguanidine in various (methanol + water) mixed solvent systems has not been reported in the literature. In addition, It is necessary to understand the basic thermodynamics [13,14], such as solubility [15], dissolution enthalpy, dissolution entropy, and molar Gibbs free energy in the industrial crystallization process of 2-cyanoguanidine [16,17]. The modified Apelblat model and the semi-empirical Buchowski-Ksiazczak kh model are generally used to investigate the influence of temperature on mole fraction solubility of the solute [18,19].…”

KH2PO4 Production by Cooling Crystallization Using Its Phase Equilibrium in the KH2PO4‐KCl‐C2H5OH‐H2O System

“…1. To produce pure KH 2 PO 4 , it is necessary to understand the basic thermodynamics [3,4] such as accurate solubility [5] and physicochemical properties (viscosity m 1) , density r) for the design of the separation processes. Compared to other separation methods, cooling crystallization is normally regarded as having the apparent advantage of lower energy consumption [6][7][8].…”