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Relevant bibliographies by topics / Solubility

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Academic literature on the topic 'Solubility'

Author: Grafiati

Published: 4 June 2021

Last updated: 9 June 2025

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Journal articles on the topic "Solubility"

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Lajoie, Léo, Anne-Sylvie Fabiano-Tixier, and Farid Chemat. "Water as Green Solvent: Methods of Solubilisation and Extraction of Natural Products—Past, Present and Future Solutions." Pharmaceuticals 15, no. 12 (December 3, 2022): 1507. http://dx.doi.org/10.3390/ph15121507.

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Water is considered the greenest solvent. Nonetheless, the water solubility of natural products is still an incredibly challenging issue. Indeed, it is nearly impossible to solubilize or to extract many natural products properly using solely water due to their low solubility in this solvent. To address this issue, researchers have tried for decades to tune water properties to enhance its solvent potential in order to be able to solubilise or extract low-water solubility compounds. A few methods involving the use of solubilisers were described in the early 2000s. Since then, and particularly in recent years, additional methods have been described as useful to ensure the effective green extraction but also solubilisation of natural products using water as a solvent. Notably, combinations of these green methods unlock even higher extraction performances. This review aims to present, compare and analyse all promising methods and their relevant combinations to extract natural products from bioresources with water as solvent enhanced by green solubilisers and/or processes.

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Vaibhav, Gulabrao Bhamare, Ravindra Joshi Renuka, Sakharam Gangurde Mayur, and V. Pawar Vijay. "Theoretical consideration of solubility by Hildebrand solubility approach." World Journal of Advanced Research and Reviews 12, no. 3 (December 30, 2021): 528–41. https://doi.org/10.5281/zenodo.5813923.

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Pharmaceutical field is widely focusing on solubility parameter models to select solvent or non-solvent that can enhance solvency of drug. Solubility Parameter is very useful concept in understanding the mechanism of solvent and solvency behavior with their applications in pharmaceuticals to open the door of research having focus on theoretical considerations of solubility. Hildebrand and Hansen Solubility Parameter are frequently used to identify solvents.

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Van Dyk, John W., Harry L. Frisch, and Dao T. Wu. "Solubility, solvency, and solubility parameters." Industrial & Engineering Chemistry Product Research and Development 24, no. 3 (September 1985): 473–78. http://dx.doi.org/10.1021/i300019a028.

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Aghnatios, C., R. Losno, and F. Dulac. "A fine fraction of soil used as an aerosol analogue during the DUNE experiment: sequential solubility in water, decreasing pH step-by-step." Biogeosciences 11, no. 17 (September 2, 2014): 4627–33. http://dx.doi.org/10.5194/bg-11-4627-2014.

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Abstract. A soil sample collected in a desert aerosol source area near Douz (southern Tunisia) was dry-sieved at 20 μm in order to extract the fraction similar to a wind-generated aerosol, and was used to seed mesocosms during the DUNE experiment (a DUst experiment in a low Nutrient, low chlorophyll Ecosystem). In this work, said "aerosol-like" fine dust was sequentially leached by short contacts with water at initial pHs, decreasing from seven to one, representing various wet environmental conditions. For each step, the solubility of a given element is calculated as the amount of its dissolved fraction, relative to its total amount. The evolution of this fractional solubility from the highest to lowest pHs provides information on the chemical strength needed to solubilise a given element and its lability. The behaviour of the elemental solubility was sorted into two groups: (1) Ca, Sr, Ba, Mn, and P, with a solubility between 23% and 70%, and a maximum sequential solubility at pH 3; (2) Al and Fe, with a solubility of less than 2% and the highest release at pH 1. Similar solubility patterns in group 1 for Ca, P, and Mn suggest a possible association of the elements in the same minerals, most probably carbonates.

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O'Brien, Geoffrey G. "Solubility." Iowa Review 30, no. 3 (December 2000): 52–53. http://dx.doi.org/10.17077/0021-065x.5323.

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Azimullah, Stanekzai, ,. Vikrant, CK Sudhakar, Pankaj Kumar, Akshay Patil, Md Rageeb Md. Usman, and Mohammed Zuber Shaikh Usman. "Nanosuspensions as a promising approach to enhance bioavailability of poorly soluble drugs : An update." Journal of Drug Delivery and Therapeutics 9, no. 2 (March 20, 2019): 574–82. http://dx.doi.org/10.22270/jddt.v9i2.2436.

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Solubility is a vital factor for devloping drug delivery systems for poorly water soluble drugs. Several conventional approaches for enhancement of solubility have limited applicability, especially when the drugs are poorly water soluble. Nanosuspension technology can be used to enhance the solubilty, stability as well as the bioavailability of poorly water soluble drugs. Nanosuspensions are biphasic systems comperising of pure drug particles dispersed in an aqueous vehicle, stabilized by surfac active agents. Fabrication of nanosuspension is simple and more advantageous than other approaches. Techniques like high-pressure homogenization, wet milling, emulsification, solvent evaporation, bottom up technology and top down technology have been applicable in the fabrication of nanosuspensions. Nanosuspension delivery is possible by several routes, such as oral, pulmonary, parenteral and ocular routes. Nanosuspension not only solves solubility and bioavailability issue, but improve drug safety and efficacy. In this context, we reviewed the current techniques used to develop nanosuspensions and their recents studies application in drug delivery system. Keywords : Solubility, fabrication, Characterization, Applications, Nanosuspension.

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Benne, Darja, and Harald Behrens. "Water solubility in haplobasaltic melts." European Journal of Mineralogy 15, no. 5 (November 17, 2003): 803–14. http://dx.doi.org/10.1127/0935-1221/2003/0015-0803.

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Bajait, Manoj Gajanan. "IMPORTANCE OF SOLUBILITY AND SOLUBILITY ENHANCEMENT TECHNIQUES." Journal of Medical Pharmaceutical And Allied Sciences 8, no. 6 (December 15, 2019): 2403–16. http://dx.doi.org/10.22270/jmpas.v8i6.878.

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Carpenter, John H. "Solubility Products and Solubility: Plus Ca Change?" Journal of Chemical Education 66, no. 2 (February 1989): 184. http://dx.doi.org/10.1021/ed066p184.

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Redelius, Per. "Bitumen Solubility Model Using Hansen Solubility Parameter." Energy & Fuels 18, no. 4 (July 2004): 1087–92. http://dx.doi.org/10.1021/ef0400058.

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Dissertations / Theses on the topic "Solubility"

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Whiting, Gary Stephen. "Studies on solubility and solubility-related processes." Thesis, University College London (University of London), 1991. http://ethos.bl.uk/OrderDetails.do?uin=uk.bl.ethos.360561.

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Bouillot, Baptiste. "Approches thermodynamiques pour la prédiction de la solubilité de molécules d'intérêt pharmaceutique." Phd thesis, Toulouse, INPT, 2011. http://oatao.univ-toulouse.fr/6993/1/bouillot.pdf.

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La cristallisation est un procédé majeur de l’industrie pharmaceutique. Dans la mise au point d’un nouveau procédé de cristallisation, l’information essentielle est la solubilité de la molécule produite dans le solvant de cristallisation. Cette donnée n’est généralement pas connue lors de la phase de développement d’un nouveau principe actif. Elle doit donc être déterminée. L’objectif de cette thèse est d’étudier, et d’approfondir, l’utilisation de modèles thermodynamiques pour prédire la solubilité de molécules organiques complexes. Pour cela, six molécules sont prises pour référence : l’ibuprofène, le paracétamol, les acides salicylique, benzoïque et 4-aminobenzoïque et l’anthracène. Les modèles étudiés sont UNIFAC et ses modifications, COSMO-SAC, NRTL-SAC et PC-SAFT. Dans un premier temps, les potentialités de chaque modèle pour prédire la solubilité dans des solvants purs et des mélanges de solvants sont analysées. Dans un second temps, le modèle COSMO-SAC est approfondi et amélioré pour la prédiction des équilibres liquide-solide mettant en jeu des molécules complexes. Enfin, une nouvelle voie de mesure expérimentale de la solubilité dans de très faibles volumes est ouverte par l’intermédiaire de l’outil microfluidique.

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Evans, Lan Tuyet. "A simple solubility theory combining solubility parameter and Lewis acid-base concepts /." Online version of thesis, 1988. http://hdl.handle.net/1850/10940.

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Campanell, Frank Christopher. "The Modeling of Solubility." Wright State University / OhioLINK, 2006. http://rave.ohiolink.edu/etdc/view?acc_num=wright1169068854.

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Morris, Kenneth Robert. "Solubility of aromatic compounds in mixed solvents." Diss., The University of Arizona, 1988. http://hdl.handle.net/10150/184324.

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The solubilities of benzene, naphthalene and anthracene were measured in five binary solvent systems. These systems consised of water and one of the following water miscible organic solvents: acetone, acetonitrile, methanol, ethanol, and isopropanol. The measurements were made at intervals of 0.1 volume fractions of the organic cosolvent. Solubility data were also collected for the above solutes in mixed cosolvents. solvent systems containing three In addition, the solubilities of and six five other aromatic solutes were measured in the binary solvent systems of methanol/water and acetone/water. The data was used to test the log-linear solubility model of Yalkowsky (1981). The model predicts a linear relationship between the solubility of a solute in a binary solvent system (S(m)) and the volume fraction of cosolvent present (f(c)) log S(m) = σf(c) + log S(w) Where S(w) is the solubility of the solute in water and σ is the proportionality constant and slope of the curve. The model is easily extended to multiple mixed solvents by combining the σ values from the binary solvent systems. log (S(m)/S(w)) = Σ₁ (σ₁£₁) A method was developed to estimate σ in a given binary solvent system from the octanol-water partition coefficient of the solute. Combining this method with the generalized solubility equation of Yalkowsky to estimate S(w), allows a priori estimates of solubility in mixed solvents. Maximum deviations in the binary solvent systems studied were related to maxima in excess density. In the alcoholic binary solvent systems the minima were related to minima in the heats of mixing of the two cosolvents. The herbicide atrazine deviated dramatically from the model. The system was examined for possible changes in the crystal structure of atrazine. It was found that some crystal modification occured in the presence of mixed solvents. The rate of the change appears to be dependant on the concentration of the cosolvent. A change or modification in the crystal violates one of the basic assumptions of the log-linear model. The assumption is that the crystal contributes equally to the solubility behavior irrespective of the solvent system. It was determined that atrazine undergoes a polymorphic transition in the systems studied. It is postulated that this polymorphism is responsible for the anomolous solubility behavior observed for atrazine.

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Asatani, Haruki. "Solubility of gases in liquids." Thesis, University of Ottawa (Canada), 1986. http://hdl.handle.net/10393/4643.

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Montaseri, Hashem. "Taxol, solubility, stability, and bioavailability." Thesis, National Library of Canada = Bibliothèque nationale du Canada, 1997. http://www.collectionscanada.ca/obj/s4/f2/dsk3/ftp05/nq21604.pdf.

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Bondesson, Laban. "Microscopic Interpretations of Drug Solubility." Doctoral thesis, Stockholm : Skolan för Bioteknologi, Kungliga Tekniska högskolan, 2007. http://urn.kb.se/resolve?urn=urn:nbn:se:kth:diva-4388.

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Bondesson, Laban. "Microscopic views of drug solubility." Licentiate thesis, Stockholm, 2006. http://urn.kb.se/resolve?urn=urn:nbn:se:kth:diva-3940.

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Pitani, Lavanya. "SOLUBILITY ENHANCEMENT OF MODEL COMPOUNDS." Scholarly Commons, 2017. https://scholarlycommons.pacific.edu/uop_etds/2985.

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Solubility is the amount of solute in the solvent system at phase equilibrium with certain temperature and pressure. Many of the new chemical entities are lipophilic molecules that require techniques to enhance solubility. Solubility enhancement can be achieved by either physical and/or chemical modification of the drug. Various techniques are available for solubility enhancement of poorly soluble drugs include particle size reduction, salt formation, solid dispersions, use of surfactants, prodrug, crystal modification, etc. In this study, the three model drugs belong to BCS class II and IV having low solubility with a certain range of physicochemical properties were studies in solubility enhancement using fusion method, co-precipitation, nano-milling and spray drying techniques. The two different polymers employed for solubility enhancement are PEG 8000 and PVP 40,000. Solubility was determined by Shake Flask method at the temperature of 37±0.1 °C. The objective is to investigate the enhancement of solubility of the three model drugs namely Glipizide, Carvedilol and Furosemide in 1:1, 1:5 and 1:10 drug-polymer ratios and are characterized by Differential Scanning Calorimetry (DSC). The Solubility of Glipizide was enhanced from 11.18 ± 1.78 µg/ml to 35.73 ± 0.04 µg/ml by 219 % increase with nano-milling technique at 1:5 ratio with PEG 8000 as carrier whereas with PVP 40000 as carrier, 286 % increase in solubility to 43.26 ± 7.87 µg/ml was observed at 1:1 ratio by fusion method. The solubility of Carvedilol was enhanced from 5.04 ± 0.55 µg/ml to 17.51 ± 0.94 µg/ml by 246 % at 1:5 ratio by fusion method with PEG8000 as carrier and 2924 % enhancement in solubility to 152.70 ± 9.09 µg/ml at 1:10 ratio by nano-milling with PVP40000 as the carrier. Furosemide showed an increase in solubility from 55.94 ± 2.48 µg/ml to 164.11 ± 9.18 µg/ml by 193 % at 1:10 ratio by nano-milling technique with PEG8000 as carrier whereas with PVP40000 as carrier, 444 % increase was observed at 1:1 ratio by nano-milling technique with solubility of 304.52 ± 23.11 µg/ml. The data showed that the decrease in percentage crystallinity and enthalpy of fusion of the model drugs upon implementing solubility enhancement techniques with the effect of particle size and the carrier used resulted in the increase of aqueous solubility of the model drugs.

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Books on the topic "Solubility"

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1938-, Keith Lawrence H., Walters Douglas B, and National Toxicology Program (U.S.), eds. National Toxicology Program's chemical solubility compendium. Boca Raton: Lewis Publishers, 1992.

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2

James, Kenneth C. Solubility and related properties. New York: M. Dekker, 1986.

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Fogg, Peter G. T. Solubility of gases in liquids: A critical evaluation of gas/liquid systems in theory and practice. Chichester: J. Wiley, 1991.

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Letcher, Trevor M., ed. Developments and Applications in Solubility. Cambridge: Royal Society of Chemistry, 2007. http://dx.doi.org/10.1039/9781847557681.

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Knigsberger, Erich, and LanChi Knigsberger, eds. Biomineralization– Medical Aspects of Solubility. Chichester, UK: John Wiley & Sons, Ltd, 2006. http://dx.doi.org/10.1002/0470092122.

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Grant, David J. W. Solubility behavior of organic compounds. New York: John Wiley & Sons, 1990.

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Ferreira, Jardel Prata. Nitrogen solubility in molten slags. Ottawa: National Library of Canada, 1992.

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Grant, David J. W. Solubility behavior of organic compounds. New York: John Wiley & Sons, 1990.

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1970-, He Yan, and Jain Parijat, eds. Handbook of aqueous solubility data. 2nd ed. Boca Raton, FL: CRC Press, 2010.

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M, Letcher T., ed. Thermodynamics, solubility, and environmental issues. Amsterdam: Elsevier, 2007.

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Book chapters on the topic "Solubility"

1

Streng, William H. "Solubility." In Characterization of Compounds in Solution, 61–71. Boston, MA: Springer US, 2001. http://dx.doi.org/10.1007/978-1-4615-1345-2_6.

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Boily, Jean-François. "Solubility." In Encyclopedia of Earth Sciences Series, 1–9. Cham: Springer International Publishing, 2017. http://dx.doi.org/10.1007/978-3-319-39193-9_72-1.

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Boily, Jean-François. "Solubility." In Encyclopedia of Earth Sciences Series, 1359–67. Cham: Springer International Publishing, 2018. http://dx.doi.org/10.1007/978-3-319-39312-4_72.

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Rose, H. E. "Solubility." In Universitext, 229–47. London: Springer London, 2009. http://dx.doi.org/10.1007/978-1-84882-889-6_11.

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Gooch, Jan W. "Solubility." In Encyclopedic Dictionary of Polymers, 676. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_10868.

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Gooch, Jan W. "Solubility." In Encyclopedic Dictionary of Polymers, 676. New York, NY: Springer New York, 2011. http://dx.doi.org/10.1007/978-1-4419-6247-8_10869.

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De Angelis, Maria Grazia. "Solubility." In Encyclopedia of Membranes, 1788–89. Berlin, Heidelberg: Springer Berlin Heidelberg, 2016. http://dx.doi.org/10.1007/978-3-662-44324-8_357.

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De Angelis, Maria Grazia. "Solubility." In Encyclopedia of Membranes, 1–2. Berlin, Heidelberg: Springer Berlin Heidelberg, 2014. http://dx.doi.org/10.1007/978-3-642-40872-4_357-1.

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Vojdani, F. "Solubility." In Methods of Testing Protein Functionality, 11–60. Boston, MA: Springer US, 1996. http://dx.doi.org/10.1007/978-1-4613-1219-2_2.

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Kwon, Hyukjin, Bipin Rajpurohit, and Yonghui Li. "Solubility." In Methods and Protocols in Food Science, 307–14. New York, NY: Springer US, 2024. https://doi.org/10.1007/978-1-0716-4272-6_24.

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Conference papers on the topic "Solubility"

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Fu, Bob, Andrew J. McMahon, and Kevin Blakley. "The Controversy of CO2 Solubility in Water." In CORROSION 1998, 1–17. NACE International, 1998. https://doi.org/10.5006/c1998-98039.

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Abstract A study was conducted to measure the solubility of CO2 in water. The objective was to examine the effect of various experimental parameters on the CO2 solubility. The results confirmed that water vapour pressure must be considered when determining the dissolved CO2 concentration at elevated temperatures (&gt;30°C). The gas-sparging rate has no effect on the steady state CO2 solubility as long as the sparging time exceeds 1 hour. Indeed, the steady state concentration was established within the first 30 minutes of sparging at a rate of 100 mL/min. The evolution rate of dissolved CO2 was found to be considerably lower than the dissolution rate of CO2 gas. Although the solubility of CO2 measured at 80°C agreed reasonably well with the literature, the value obtained at room temperature was significantly lower. The steady state concentration of CO2 ranges from 265 to 320 ppm at 80°C and 1 bar total pressure, as compared to the calculated literature value of 307 ppm. Conversely, the concentration measured at 20°C (1125 – 1400 ppm) was significantly lower than the literature value (1720 ppm). Several measurement methods were attempted in order to resolve the difference; however, the results were consistently lower than those previously reported in the literature. The explanation to the discrepancy is yet to be identified.

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Tan, Yang, Jia Zheng, Liang Hong, and Bingxin Zhou. "PROTSOLM: Protein Solubility Prediction with Multi-modal Features." In 2024 IEEE International Conference on Bioinformatics and Biomedicine (BIBM), 223–32. IEEE, 2024. https://doi.org/10.1109/bibm62325.2024.10822310.

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Wang, Xin, Zhaoyi Dai, Yue Zhao, Chong Dai, Saebom Ko, Samridhdi Paudyal, Xuanzhu Yao, Cianna Leschied, Amy T. Kan, and Mason B. Tomson. "Zinc Sulfide Solubility Modeling in Aqueous Solution at High Temperature, Pressure, and Ionic Strength." In CONFERENCE 2022, 1–15. AMPP, 2022. https://doi.org/10.5006/c2022-17763.

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Abstract In this study, the solubility of zinc sulfide has been collected from the literature at pH 2 to 11, temperature 23 to 250 °C, pressure 0.6 to 150 bar, and ionic strength 0 to 4.6 m. A solubility model has been developed based on the combination of Pitzer theory calculated activity coefficient and speciation of the Zn-HS-OH-Cl aqueous system. In total, around 230 solubility data were collected as the input database, the model was fitted in Matalab 2020a with the particle-swarm optimization. The updated model is able to predict the ZnS solubility saturation index (SI) with 95% confidence interval 0.04 SI unit, which suggested good accuracy under model conditions. Due to the extremely low solubility of the ZnS itself, these errors correspond to only around 0.07 ppm of [Zn(II)], which is less than the error of measurement for field samples. For all pH conditions, Zn-HS complexes and Zn-Cl complexes have strong influence on the aqueous soluble zinc solubility. This new model with accurate ZnS solubility prediction will help field operators to better control the ZnS scaling and corrosion problem.

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Wang, Xin, Saebom Ko, Alex Yi-Tsung Lu, Guannan Deng, Yue Zhao, Chong Dai, Samridhdi Paudyal, Amy T. Kan, and Mason B. Tomson. "New Approach to Iron Sulfide Scale Modeling and Prediction at pH 4-7." In CORROSION 2020, 1–11. NACE International, 2020. https://doi.org/10.5006/c2020-14532.

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Abstract In this study, a plug flow reactor was built to investigate iron sulfide scale precipitation at various temperatures, pH and ionic strength conditions and two pieces of carbon steel C1018 coupons were put inside as reaction surfaces. The ferrous ion and total sulfide in collected effluent samples were measured to determine precipitation kinetics and solubility. The solid that formed on the steel surfaces were analyzed by Scanning Electron Microscopy (SEM/EDS) and X-ray Diffraction (XRD). The solubility data from this study and literature were collected and fitted by Matlab to build up a reliable FeS solubility prediction model. The experimental results show that mackinawite is the predominant precipitated scale and could be stable for a week at pH higher than 6.0. Iron sulfide precipitation is under diffusion control, accelerated by high temperature and ionic strength. At pH 6 – 7, the aqueous phase neutral species, such as FeSaq0, plays an important role in the solubility and precipitation kinetic. Based on this study, a new solubility model that combines Pitzer theory and ion-complexes (speciation of ferrous ion) has been developed for iron sulfide solubility calculation and scale prediction.

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Rahmi, Chusnur, Siti Katmiati, Wiji, and Sri Mulyani. "Students’ mental models on the solubility and solubility product concept." In MATHEMATICS, SCIENCE, AND COMPUTER SCIENCE EDUCATION (MSCEIS 2016): Proceedings of the 3rd International Seminar on Mathematics, Science, and Computer Science Education. Author(s), 2017. http://dx.doi.org/10.1063/1.4983933.

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Brady, J. L., L. L. Gantt, D. M. Fife, D. A. Rich, S. W. Almond, and D. A. Ross. "Cement Solubility in Acids." In Low Permeability Reservoirs Symposium. Society of Petroleum Engineers, 1989. http://dx.doi.org/10.2118/18986-ms.

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Osborne, Z. R., and J. B. Thomas. "TITANIUM SOLUBILITY IN COESITE." In GSA Annual Meeting in Seattle, Washington, USA - 2017. Geological Society of America, 2017. http://dx.doi.org/10.1130/abs/2017am-303998.

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Pongkendek, Jesi, John Parlindungan, and Novike Sumanik. "The Development of Direct Learning Strategies in Topic Solubility and Solubility Product." In Proceedings of the International Conference on Social Science 2019 (ICSS 2019). Paris, France: Atlantis Press, 2019. http://dx.doi.org/10.2991/icss-19.2019.211.

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Rogel, E., C. Ovalles, M. Moir, J. Vien, and H. Morazan. "Solubility Characterization of Asphaltene Deposits." In SPE International Symposium on Oilfield Chemistry. Society of Petroleum Engineers, 2015. http://dx.doi.org/10.2118/173757-ms.

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Zhang Yong-An and Xue He-Ru. "Online measurement solubility of CO." In International Conference on Advanced Infocomm Technology 2011 (ICAIT 2011). IET, 2011. http://dx.doi.org/10.1049/cp.2011.1075.

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Reports on the topic "Solubility"

1

Meyer, R. E., W. D. Arnold, and F. I. Case. Valence effects on solubility and sorption: the solubility of Tc(IV) oxides. Office of Scientific and Technical Information (OSTI), March 1986. http://dx.doi.org/10.2172/5954679.

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C. Stockman. Pure Phase Solubility Limits: LANL. Office of Scientific and Technical Information (OSTI), January 2001. http://dx.doi.org/10.2172/899942.

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Karakaya, P., M. Sidhoum, C. Christodoulatos, Wendy Balas, and Steven Nicolich. Aqueous Solubility of CL-20. Fort Belvoir, VA: Defense Technical Information Center, August 2005. http://dx.doi.org/10.21236/ada436626.

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Raman, S. V., R. Bopp, T. A. Batcheller, and Q. Yan. Zirconia solubility in boroaluminosilicate glass. Office of Scientific and Technical Information (OSTI), December 1995. http://dx.doi.org/10.2172/188530.

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Beahm, E. C. Comparative Calculations of Solubility Equilibria. Office of Scientific and Technical Information (OSTI), July 2000. http://dx.doi.org/10.2172/814615.

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McCabe, D. J. Carbollide solubility and chemical compatibility summary. Office of Scientific and Technical Information (OSTI), August 1993. http://dx.doi.org/10.2172/10105577.

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Barnes, M. J., R. A. Peterson, R. F. Swingle, and C. T. Reeves. Sodium tetraphenylborate solubility and dissolution rates. Office of Scientific and Technical Information (OSTI), December 1995. http://dx.doi.org/10.2172/383593.

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Karraker, D. G. Uranium solubility studies during waste evaporation. Office of Scientific and Technical Information (OSTI), August 1993. http://dx.doi.org/10.2172/10143240.

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Karraker, D. G. Solubility of plutonium and waste evaporation. Office of Scientific and Technical Information (OSTI), October 1993. http://dx.doi.org/10.2172/10158025.

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Davison, Brian H., and John W. Barton. Biofiltration of Volatile Pollutants: Solubility Effects. Office of Scientific and Technical Information (OSTI), June 2001. http://dx.doi.org/10.2172/834467.

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