Volume 7, Issue 4, December 2018, Page: 63-72
An Experimental Investigation of Pristine Barite Adsorption on Sodium Oleate and Sodium Palmitate
Nwoko Christopher Ikpe Amadi, Department of Chemistry, School of Physical Sciences, Federal University of Technology, Owerri, Nigeria
Nkwoada Amarachi Udoka, Department of Chemistry, School of Physical Sciences, Federal University of Technology, Owerri, Nigeria
Okoji Josephine, Department of Chemistry, School of Physical Sciences, Federal University of Technology, Owerri, Nigeria
Opah Solomon, Department of Chemistry, School of Physical Sciences, Federal University of Technology, Owerri, Nigeria
Received: Dec. 15, 2018;       Accepted: Jan. 9, 2019;       Published: Jan. 28, 2019
DOI: 10.11648/j.ajpc.20180704.12      View  159      Downloads  23
Abstract
Characterization of the pristine barite mineral was established using a scanning electron microscope (SEM) and Fourier Transform Infra-Red (FTIR). Barite was applied for sodium oleate and sodium palmitate adsorption in aqueous solutions. Equilibrium adsorption data were fitted into two adsorption isotherms, three kinetic models and thermodynamic study. The concentration of the ion and pH in the solution proved to be a controlling factor in the adsorption process. Sodium oleate and sodium palmitate soaps adsorbed strongly onto the barite mineral at pH 9 and a temperature of 293k. They result was affected by the high bulk density and chemical resistance nature of barite indicated by successive increase in dosage amount. The effect of concentration and time typically gave a C-type adsorption isotherm. Adsorptive isotherm showed that sodium palmitate adsorption over natural barite was better described by the Langmuir adsorption isotherm while oleate desorption gave a good fitting with Freundlich isotherm. The adsorptive kinetics of sodium palmitate fitted well into pseudo 1 st order and 2nd order kinetics. Intra particle diffusion was not the rate-determining step. Thermodynamic study showed a physio-sorption that was exothermic. Hence the findings showed that pristine barite absorbs at optimum pH and temperature of 9 and 293K.
Keywords
Barite, Adsorption, Sodium Palmitate, Sodium Oleate
To cite this article
Nwoko Christopher Ikpe Amadi, Nkwoada Amarachi Udoka, Okoji Josephine, Opah Solomon, An Experimental Investigation of Pristine Barite Adsorption on Sodium Oleate and Sodium Palmitate, American Journal of Physical Chemistry. Vol. 7, No. 4, 2018, pp. 63-72. doi: 10.11648/j.ajpc.20180704.12
Copyright
Copyright © 2018 Authors retain the copyright of this article.
This article is an open access article distributed under the Creative Commons Attribution License (http://creativecommons.org/licenses/by/4.0/) which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Reference
[1]
Omar, A., and Azzam, E. (2004). Adsorption of Some Anionic Surfactants on Barite and at Solution/Air Interfaces. Journal of Surfactants and Detergents, 7(2), 141-145.
[2]
Labidi, N. (2018). Flotation of Barium Sulfate Contaminants Soils. Biodiversity International Journal, 2(1), 1-3. doi:10.15406/bij.2018.02.00049.
[3]
Ruiz-Agudo, C., Putnis, C., Ruiz-Agudo, E., and Putnis, A. (2015). The influence of pH on barite nucleation and growth. Chemical Geology, 391, 7-18. doi:10.1016/j.chemgeo.2014.10.023.
[4]
Bokern, D., Hunter, K., & McGrath, K. (2003). Charged Barite-Aqueous Solution Interface: Surface Potential and Atomically Resolved Visualization. Langmuir, 19, 10019-10027. doi:10.1021/la0269255.
[5]
Yoshihiro, K., and Masato, M. (2014). In situ AFM study on barite (001) surface dissolution in NaCl solutions at 30°C. Applied Geochemistry, 51, 246-254. doi:10.1016/j.apgeochem.2014.10.008.
[6]
Ganeshram, R., Francois, R., Commeau, J., and Brown-Leger, S. (2003). An Experimental Investigation of Barite Formation in Seawater. Geochimica et Cosmochimica Acta,, 67(14), 2599–2605. doi:10.1016/S0016-7037(03)00164-9.
[7]
Zuilen, V., Mueller, T., and Naegler, T. (2016). Experimental determination of barium isotope fractionation during diffusion and adsorption processes at low temperatures. Geochimica et Cosmochimica Acta, 186, 226-241. doi:10.1016/j.gca.2016.04.049.
[8]
Andrew, G., and Andrew, P. (1993). The kinetics of barite dissolution and precipitation in water and sodium chloride brines at 44-35°C. Geochimica et Cosmochimica Acta, 57, 2161-2168.
[9]
Sanchez-Pastor, N., Pina, C., Fernandez-Dı´az, L., and Astilleros, M. (2006). The effect of CO32- on the growth of barite (001) and (210) surfaces: An AFM study. Surface Science, 600, 1369-1381. doi:10.1016/j.susc.2006.01.042.
[10]
Omar, A., and El-adly, R. (2005). Mixed micelle formation and adsorption of anionic/nonionic surfactant mixture on barite for drilling fluids. Petroleum Science and Technology, 23(2), 209-217. doi:10.1081/LFT-200028190.
[11]
Xiong, C., Guohua, G, Donghui, L., and Renfeng, Z. (2017). The flotation separation of barite-calcite using sodium silicate as a depressant in the presence of sodium dodecyl sulfate. Physicochemical Problems of Mineral Processing, 10, 1-10. doi:10.5277/ppmp18136.
[12]
Pradip, and Fuerstenau. (1983). The adsorption of hydroxamate on semi soluble minerals. Part 1: adsorption on barite, calcite and bastnaesite. Colloids and Surfaces, 8, 103-119. doi:0166.6622/831S03.00.
[13]
Marinakis, K., and Shergold, H. (1985). The mechanism of fatty acid adsorption in the presence of fluorite, calcite and barite. International Journal of Mineral Processing, 14, 161-176.
[14]
Divya, B., and Tyagi, V. (2007). Laundry detergents: An overview. Journal of Oleo Science, 56(7), 327-340.
[15]
Cases, J., Villieras, F., Michot, L., and Bersillon, J. (2002). Long chain ionic surfactants: the understanding of adsorption mechanisms from the resolution of adsorption. Colloids and Surfaces, 205, 85-99.
[16]
Bokern, D., Hunter, K., and McGrath, K. (2003). Charged Barite-Aqueous Solution Interface: Surface Potential and Atomically Resolved Visualization. Langmuir, 19, 10019-10027. doi:10.1021/la0269255.
[17]
Prameena, B., Anbalagan, G., Sangeetha, V., Gunasekaran, S., and Ramkumaar, G. (2013). Behaviour of Indian natural Baryte mineral. International Journal of ChemTech Research, 5(1), 220-231.
[18]
Dimova, M., Panczer, G., and Gaft, M. (2006). Spectroscopic study of barite from the Kremikovtsi deposit (Bulgaria) with implication for its origin. Annales Géologiques De La Péninsule Balkanique, 67, 101-108.
[19]
Aroke, U., Abdulkarim, A., and Ogubunka, R. (2013). Fourier-transform infrared characterization of kaolin, granite, bentonite and barite. ABTU Journal of Environmental technology, 6(1), 42-53.
[20]
Femi, O., Ibrahim, Y., and Ekezue, J. (2015). Characterizing Barite from Bukkuyum local government area of Zamfara state of Nigeria, using Empyrean diffractometer DY 674 (2010) for XRD phase analysis of the powdered sample. World Academic Research in Environmental Protection and Sustainability Development, 1(12), 6-9.
[21]
Badr, S., Mohamed, A. R., and Abdulazeez, A. (2017). Evaluation of Barium Sulfate (Barite) Solubility Using Different Chelating Agents at a High Temperature. Journal of Petroleum Science and Technology, 7(1), 42-56.
[22]
Asuquo, J., Anusiem, A., and Etim, E. (2012). Effect of pH on the Adsorption of Metallic Soaps of Shea Butter Oil onto Hematite in Aqueous Medium. International Journal of Modern Chemistry, 2(2), 74-83.
[23]
Offor, O. (1995). Oleate adsorption at a Nigerian hematite-water interface: Effect of concetration, temperature and pH on adsorption density. Journal of Colloid and Interface Science, 174, 345-350.
[24]
Offor, O. (1996). Effect of Inorganic Ions on Oleate Adsorption at a Nigerian Hematite–Water Interface. Journal of colloud and interface science, 179, 323-328.
[25]
Offor, O., and Nwoko, C. (1997). Oleate Flotation of a Nigerian Baryte: The Relation between Flotation Recovery and Adsorption Density at Varying Oleate Concentrations, pH, and Temperatures. Journal of Colloud and Interface Science, 186, 225-233.
[26]
Alinnor, I., & Enenebeaku, C. (2014). Adsorption Characteristics of Sodium Oleate onto Calcite. International Research Journal of Pure & Applied Chemistry, 4(1), 88-96.
[27]
Agarry, S., and Ogunleye, O. (2014). Chemically treated kola nut pod as low-cost natural adsorbent for the removal of 2,4-dinitrophenol from synthetic wastewater: batch equilibrium, kinetic, and thermodynamic modelling studies. Turkish Journal of Engineering and Environmental solution, 38, 11-40. doi:0.3906/muh-1304-24.
[28]
Limousin, G., Gaudet, J., Charlet, L., Szenknect, S., Barthes, V., and Krismissa, M. (2007). Sorption isotherms: A review on physical bases, modeling and measurement. Applied Geochemistry, 22, 249-275. doi:10.1016/j.apgeochem.2006.09.010.
[29]
Foo, K., and Hameed, B. (2010). Insights into the modeling of adsorption isotherm systems. Chemical Engineering Journal, 156, 2-10. doi:10.1016/j.cej.2009.09.013.
[30]
Enenebeaku, K., Okorocha, J., and Akalezi, C. (2015). Adsorptive removal of methylene blue from aqueous solution using agricultural waste: equilibrium, kinetic and Thermodynamic Studies. American Journal of Chemistry and Materials Science, 2(3), 14-25.
[31]
Duong, D. (1998). Adsorption Analysis: Equilibria and kinetics (Vol. 2). (R. Yang, Ed.) London, United Kingdom: Imperial college press.
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