The Experts below are selected from a list of 246 Experts worldwide ranked by ideXlab platform
Teófilo A. Graber - One of the best experts on this subject based on the ideXlab platform.
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Thermodynamic modeling of the solubility of Boric Acid in the systems Boric Acid + lithium sulfate + water, Boric Acid + sodium sulfate + water and Boric Acid + potassium sulfate + water at 293.15–313.15 K
Fluid Phase Equilibria, 2015Co-Authors: Wilson Alavia, Jorge A. Lovera, Teófilo A. GraberAbstract:Abstract In this contribution the experimental solubility of Boric Acid in sodium sulfate aqueous solution was measured at different temperatures from (293.15 to 313.15) K, and Na2SO4 concentrations ranging from (0 to 3.3795) mol kg−1 H2O. The results were represented using an equation based on Pitzer model for the interactions of nonelectrolytes with electrolytes in aqueous solutions, given by Chanson and Millero (2006) [18]. The model parameter was estimated and validated estimating the solubility of Boric Acid in lithium sulfate, sodium sulfate and potassium sulfate aqueous solutions at different temperatures and salt concentrations. The model represented satisfactorily the data for the systems (SD = 0.033 mol kg−1 H2O for H3BO3 + Na2SO4 + H2O, SD = 0.020 mol kg−1 H2O for H3BO3 + Li2SO4 + H2O and SD = 0.030 mol kg−1 H2O for H3BO3 + K2SO4 + H2O). The model parameters are valid to maximum concentration of the salts, 3.380 mol kg−1 for Na2SO4, 3.149 mol kg−1 for Li2SO4 and 1.245 mol kg−1 for K2SO4 from 293.15 K to 313.15 K. Based on the results it was determined that lithium sulfate is a precipitant agent for Boric Acid and its behavior is attributed to the salting out effect of Li+ ion; sodium and potassium sulfates increase the Boric Acid solubility; this salting in effect is due to the presence of Na+ and K+ ions. The presence of these salts can be unfavorable for the crystallization of Boric Acid due to the increase of solubility which decreases the supersaturation, therefore the yield of the process. Comparing the parameters for the system H3BO3 + Na2SO4 + H2O, H3BO3 + Li2SO4 + H2O and H3BO3 + K2SO4 + H2O, it was found that effect of these ions on the decreasing of the solubilty of Boric Acid in aqueous sulfate solutions follows the order: Li+ > Na+ > K+, which can be attributed to the increase of their ionic radii, coordinated with 6 water molecules therefore the capacity to form hydration shells.
M. Bilen - One of the best experts on this subject based on the ideXlab platform.
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Fabrication of Boric Acid and sodium sulfate from Borax
Cfi-ceramic Forum International, 2004Co-Authors: Ayhan Mergen, M. Hamdi Demirhan, M. BilenAbstract:Boric Acid production was made from borax solutions with concentrations of 183 and 245 g/l B 2 O 3 . Sodium sulfate was recovered as a by-product during Boric Acid fabrication. 183 g/l B 2 O 3 was the optimum concentration for the Boric Acid production. Boric Acid production yield and Boric Acid purity were around 91 % and 96,7 % respectively for the concentration value of 183 g/l B 2 O 3 . Boric Acid fabrication can be carefully controlled by measuring the pH of the borax and Boric Acid solutions. Reaction times of between 5 and 90 min during Boric Acid production from borax solution of 183 g/l B 2 O 3 did not have significant impact on the Boric Acid production yield and Boric Acid purity. Rafinated Boric Acid and sodium sulfate crystals had purities of over 99%. Rafinated Boric Acid and sodium sulfate crystals were characterised using X-ray diffraction (XRD), differential thermal and thermogravimetric analysis (DTA-TG) and scanning electron microscopy (SEM).
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Processing of Boric Acid from borax by a wet chemical method
Advanced Powder Technology, 2003Co-Authors: Ayhan Mergen, M.h. Demirhan, M. BilenAbstract:Abstract Boric Acid crystals were obtained from borax (Na 2 B 4 O 7 · 10H 2 O) solutions which were prepared from borax ore. The concentration of borax solutions was varied from 1120 to 1240 kg/m 3 and 1180 kg/m 3 was determined to be the optimum concentration value for Boric Acid production from a relation between borax solution concentration and Boric Acid production yield and Boric Acid purity. Boric Acid production yield was around 91% for a borax solution of 1180 kg/m 3 . Boric Acid purity ranged from 94 to 97% for different concentrations before refining, and a high purity Boric Acid over 99.6% with low sulfate and sodium was obtained after refining. Boric Acid crystals were characterized by X-ray diffraction, differential thermal and thermograrimetric analysis, and scanning electron microscopy observation.
Wilson Alavia - One of the best experts on this subject based on the ideXlab platform.
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Thermodynamic modeling of the solubility of Boric Acid in the systems Boric Acid + lithium sulfate + water, Boric Acid + sodium sulfate + water and Boric Acid + potassium sulfate + water at 293.15–313.15 K
Fluid Phase Equilibria, 2015Co-Authors: Wilson Alavia, Jorge A. Lovera, Teófilo A. GraberAbstract:Abstract In this contribution the experimental solubility of Boric Acid in sodium sulfate aqueous solution was measured at different temperatures from (293.15 to 313.15) K, and Na2SO4 concentrations ranging from (0 to 3.3795) mol kg−1 H2O. The results were represented using an equation based on Pitzer model for the interactions of nonelectrolytes with electrolytes in aqueous solutions, given by Chanson and Millero (2006) [18]. The model parameter was estimated and validated estimating the solubility of Boric Acid in lithium sulfate, sodium sulfate and potassium sulfate aqueous solutions at different temperatures and salt concentrations. The model represented satisfactorily the data for the systems (SD = 0.033 mol kg−1 H2O for H3BO3 + Na2SO4 + H2O, SD = 0.020 mol kg−1 H2O for H3BO3 + Li2SO4 + H2O and SD = 0.030 mol kg−1 H2O for H3BO3 + K2SO4 + H2O). The model parameters are valid to maximum concentration of the salts, 3.380 mol kg−1 for Na2SO4, 3.149 mol kg−1 for Li2SO4 and 1.245 mol kg−1 for K2SO4 from 293.15 K to 313.15 K. Based on the results it was determined that lithium sulfate is a precipitant agent for Boric Acid and its behavior is attributed to the salting out effect of Li+ ion; sodium and potassium sulfates increase the Boric Acid solubility; this salting in effect is due to the presence of Na+ and K+ ions. The presence of these salts can be unfavorable for the crystallization of Boric Acid due to the increase of solubility which decreases the supersaturation, therefore the yield of the process. Comparing the parameters for the system H3BO3 + Na2SO4 + H2O, H3BO3 + Li2SO4 + H2O and H3BO3 + K2SO4 + H2O, it was found that effect of these ions on the decreasing of the solubilty of Boric Acid in aqueous sulfate solutions follows the order: Li+ > Na+ > K+, which can be attributed to the increase of their ionic radii, coordinated with 6 water molecules therefore the capacity to form hydration shells.
Ayhan Mergen - One of the best experts on this subject based on the ideXlab platform.
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Dissolution kinetics of probertite in Boric Acid solution
International Journal of Mineral Processing, 2009Co-Authors: Ayhan Mergen, M. Hamdi DemirhanAbstract:Abstract Probertite (NaCaB 5 O 9 ·5H 2 O) and ulexite (NaCaB 5 O 9 ·8H 2 O) posses identical chemical formula except for their water content. In this study, the dissolution of probertite in Boric Acid solution was investigated as a function of temperature and time. As the Boric Acid concentration increased, the dissolution of probertite also increased. However, the Boric Acid concentrations above 5 wt.% at 60 °C and 80 °C did not significantly affect the dissolution of probertite. The stirring speed had almost no effect on the dissolution of probertite. The dissolution kinetics of probertite in Boric Acid solution was controlled by first order pseudo homogeneous reaction. The activation energies for different probertite particle sizes varied from 25.25 kJ/mol K to 28.25 kJ/mol K, indicating that particle size had minor effect on the dissolution of probertite.
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Fabrication of Boric Acid and sodium sulfate from Borax
Cfi-ceramic Forum International, 2004Co-Authors: Ayhan Mergen, M. Hamdi Demirhan, M. BilenAbstract:Boric Acid production was made from borax solutions with concentrations of 183 and 245 g/l B 2 O 3 . Sodium sulfate was recovered as a by-product during Boric Acid fabrication. 183 g/l B 2 O 3 was the optimum concentration for the Boric Acid production. Boric Acid production yield and Boric Acid purity were around 91 % and 96,7 % respectively for the concentration value of 183 g/l B 2 O 3 . Boric Acid fabrication can be carefully controlled by measuring the pH of the borax and Boric Acid solutions. Reaction times of between 5 and 90 min during Boric Acid production from borax solution of 183 g/l B 2 O 3 did not have significant impact on the Boric Acid production yield and Boric Acid purity. Rafinated Boric Acid and sodium sulfate crystals had purities of over 99%. Rafinated Boric Acid and sodium sulfate crystals were characterised using X-ray diffraction (XRD), differential thermal and thermogravimetric analysis (DTA-TG) and scanning electron microscopy (SEM).
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Processing of Boric Acid from borax by a wet chemical method
Advanced Powder Technology, 2003Co-Authors: Ayhan Mergen, M.h. Demirhan, M. BilenAbstract:Abstract Boric Acid crystals were obtained from borax (Na 2 B 4 O 7 · 10H 2 O) solutions which were prepared from borax ore. The concentration of borax solutions was varied from 1120 to 1240 kg/m 3 and 1180 kg/m 3 was determined to be the optimum concentration value for Boric Acid production from a relation between borax solution concentration and Boric Acid production yield and Boric Acid purity. Boric Acid production yield was around 91% for a borax solution of 1180 kg/m 3 . Boric Acid purity ranged from 94 to 97% for different concentrations before refining, and a high purity Boric Acid over 99.6% with low sulfate and sodium was obtained after refining. Boric Acid crystals were characterized by X-ray diffraction, differential thermal and thermograrimetric analysis, and scanning electron microscopy observation.
Jorge A. Lovera - One of the best experts on this subject based on the ideXlab platform.
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Thermodynamic modeling of the solubility of Boric Acid in the systems Boric Acid + lithium sulfate + water, Boric Acid + sodium sulfate + water and Boric Acid + potassium sulfate + water at 293.15–313.15 K
Fluid Phase Equilibria, 2015Co-Authors: Wilson Alavia, Jorge A. Lovera, Teófilo A. GraberAbstract:Abstract In this contribution the experimental solubility of Boric Acid in sodium sulfate aqueous solution was measured at different temperatures from (293.15 to 313.15) K, and Na2SO4 concentrations ranging from (0 to 3.3795) mol kg−1 H2O. The results were represented using an equation based on Pitzer model for the interactions of nonelectrolytes with electrolytes in aqueous solutions, given by Chanson and Millero (2006) [18]. The model parameter was estimated and validated estimating the solubility of Boric Acid in lithium sulfate, sodium sulfate and potassium sulfate aqueous solutions at different temperatures and salt concentrations. The model represented satisfactorily the data for the systems (SD = 0.033 mol kg−1 H2O for H3BO3 + Na2SO4 + H2O, SD = 0.020 mol kg−1 H2O for H3BO3 + Li2SO4 + H2O and SD = 0.030 mol kg−1 H2O for H3BO3 + K2SO4 + H2O). The model parameters are valid to maximum concentration of the salts, 3.380 mol kg−1 for Na2SO4, 3.149 mol kg−1 for Li2SO4 and 1.245 mol kg−1 for K2SO4 from 293.15 K to 313.15 K. Based on the results it was determined that lithium sulfate is a precipitant agent for Boric Acid and its behavior is attributed to the salting out effect of Li+ ion; sodium and potassium sulfates increase the Boric Acid solubility; this salting in effect is due to the presence of Na+ and K+ ions. The presence of these salts can be unfavorable for the crystallization of Boric Acid due to the increase of solubility which decreases the supersaturation, therefore the yield of the process. Comparing the parameters for the system H3BO3 + Na2SO4 + H2O, H3BO3 + Li2SO4 + H2O and H3BO3 + K2SO4 + H2O, it was found that effect of these ions on the decreasing of the solubilty of Boric Acid in aqueous sulfate solutions follows the order: Li+ > Na+ > K+, which can be attributed to the increase of their ionic radii, coordinated with 6 water molecules therefore the capacity to form hydration shells.