Boron Adsorption on Muscovite Mineral as a Function of pH, Ionic strength of Solution and Kinds of Cation

آب و خاک

Article 9, Volume 29, Issue 1, March 2015, Pages 188-197   

Document Type: Research Article

DOI: 10.22067/jsw.v0i0.32794

Authors

F. Zareapour Rafsanjani; M. Hamidpour^* ; Hossein Shirani; M. Heshmati; seyed javad hosseinifard

Vali-e Asr University of Rafsanjan

Abstract

Introduction: Boron is one of the eight essential micronutrients required for plant growth and development. The optimal concentration range (between deficiency and phytotoxicity) for boron is narrower than for other plant essential nutrients. Generally, irrigating water containing concentrations of B greater than 1 mg L-1 would be detrimental for most plants. Although, there are a large number of different studies on the removal of B ions from aqueous solutions using different adsorbents, every special adsorbent material requires individual research. Information about the chemical behavior of muscovite for boron is very limited. Therefore, the objective of this study was to investigate boron adsorption on muscovite as a function of solution pH, ionic strength of the background electrolyte, kinds of cation, and initial boron concentration.
Materials and Methods: The muscovite sample was obtained from a mine near Hamadan city in western Iran. It was powdered in a mortar and sieved before sorption experiment. Boron adsorption experiments were performed in batch systems using 15 mL polyethylene (PE) bottles in 0.01 M Ca(NO3)2 electrolyte solution at a adsorbent concentrations of 10 g L-1, and at room temperature (23±2 ◦C). All samples were prepared in duplicate. Blank samples (without adsorbent) were prepared for all experiments. For pH dependent B adsorption, aliquots of B stock solution (1000 mg L−1) were added to obtain initial B concentrations of 5 and 15 mg L-1. The pH of the solutions were adjusted to values of 6.8, 7.7 and 8.8 by adding negligible predetermined volumes of 0.03M NaOH or 0.03M HNO3 solution. To study the effects of kinds of cation on boron adsorption, samples of adsorbent (0.1 g) were mixed with 10 mL background electrolyte solutions (0.01M Ca(NO3)2, Mg(NO3)2 and NaNO3) in 15 mL centrifuge tubes. Then, predetermined amount of B were added to the centrifuge tubes to obtain final concentrations of 5 mg L-1 B. For determination of boron adsorption isotherm, after 10 ml 0.01 M of Ca(NO3)2 was transferred into 15 ml centrifuge tubes, 0.1 g sample of muscovite was added to obtain adsorbent concentration of 10 g L-1. Then a predetermined amount of boron from the stock solution was added to give final concentration range between 1 and 15 mg B per liter. Initial pH of the solution was adjusted to 8.2 ± 0.1 by predetermined amount of 0.03 M NaOH solution. Suspensions were then shaken for 24h. At the end of equilibrium time, final pH was measured in the suspensions and the tubes were then centrifuged for 10 min at 5000 g. Half of the supernatant volume (5 mL) was pipetted out from each tube and then B in the supernatants were measured using the colorimetric Azomethin-H method. The amount of B adsorbed on the adsorbent was calculated as the difference between the B concentration in the blanks and the concentration in the solution after equilibration. Chemical species in the solutions were also predicted using Visual MINTEQ, a chemical speciation program developed to simulate equilibrium processes in aqueous systems.
Results and Discussion: The effect of pH on the amount of B retained depended on the initial B concentration. The amount of boron adsorption increased with increasing equilibrium pH. Boron adsorption on muscovite increased with increasing ionic strength. Greater adsorption was observed in the presence of Mg2+ as compared with Ca2+ at the same ionic strength. Calculations using Vminteq showed that the concentration of Mg-borate ion pairs (MgH2BO3+) were higher than the concentration of Ca and Na-borate ion pairs (CaH2BO3+ and NaH2BO3°). It thus seems that the much greater loss of B from solution observed in the Mg system was caused by Mg-borate ion pair adsorption. Sorption isotherm of B were well described by the Freundlich, Langmuir and Sips models but the Sips sorption model describes the interaction between B and the mineral better than the Langmuir model. On the basis of n value of Freundlich model, adsorption isotherm of boron on muscovite was classified as L-type (n≤ 1). This kind of adsorption behavior could be explained by the high affinity of the adsorbent for the adsorptive at low concentrations, which then decreases as concentration increases. Maximum sorption capacity (qmax) was obtained to be 13.98 mmol kg-1 for muscovite.
Conclusion: The experimental data showed that less than 5% of initial boron concentration was adsorbed by muscovite, thus this mineral has not a reasonable adsorption capacity for B.

Keywords: Boron, Adsorption, Muscovite, Speciation.

Keywords

Boron; adsorption; Muscovite; Speciation

References

- Hosseinifard S.J., Sedaghat N., Mohammadi Mohammad Abadi A., Heidarinejad A. 2009. Survey on boron position on water, soil and pistachio in pistachio growing area in Iran.Pajohesh and Sazandegi, 81:9-19. (in Persian with English abstract).

2- Hosseinifard S.J., Khademi H., Kalbasi M. 2010. Nonexchangeable K Release from Three Micaceous Minerals Using Sequential Extraction and Different Extracting Solutions. Journal of Science and Technology of Agricultural and Natural Resources, Water and Soil Sciences, 13: 105-118. (in Persian with English abstract).

3- Pais I., and Jones J.B. 1997. The Handbook of Trace Elements. Boca Raton, Fla: St. Lucie Press, Chicago.

4- Chen W.T., Ho S.B., and Lee D.Y. 2009. Effect of pH on boron adsorption-desorption hysteresis of soils. Soil Science, 174:330-338.

5- Demircivi P., and Nasun-Saygili G. 2010. Removal of boron from wastewaters using HDTMA- modified zeolites. Desalination and Water Treatment, 23:110–117.

6- Elrashidi M.A., and O,Connor G.A. 1982. Boron sorption and desorption soils. Soil Science Society of America Journal, 46:27-31.

7- Freundlich H.M.F. 1906. Over the adsorption in solution, Journal of Physical Chemistry, 57:385-470.

8- Giles C.H., Silva A.P., and Easton I.A. 1974. A general treatment and classification of the solute adsorption isotherm part. II. Experimental interpretation. Journal of Colloid and Interface Sciences, 47:766-778.

9- Goldberg S. 2005. Inconsistency in the triple layer model description of ionic strength dependent boron adsorption. Journal of Colloid Interface Science, 285:509-517.

10- Goldberg S., and Suarez D.L. 2011. Influence of soil solution cation composition on boron adsorption by soils. Soil Science, 75:80-83.

11- Goli E., Hiemstar T., Van Riemsdijk W.H., Rahnemaie R.M., and Malakouti M.J. 2011. The interaction of boron with goethite: experiments and CD-MUSIC modeling. Chemosphere, 82:1475-1481.

12- Hamidpour M., Afyuni M.,Kalbasi H., and Shariatmadari H. 2010. Kinetic and isothermal studies of cadmium sorption onto bentonite and zeolite. International-Agrophysics, 24:253-259.

13- Inam D. 2005. Organocly preparation for anionic contaminant removal from water. MSC. Thesis. Natural and applied Sciences. Middle East Technical University.

14- Karahan S.,Yurdakoc M., Seki Y., and Yurdakoc K. 2007. Removal of boron from aqueous solution by clays and modified clays. Journal of Colloid and Interface Science, 293:36–42.

15- Keren R., and Bingham F.T. 1985. Boron in water, soils and plants. Advanced Soil Science, 1:229-276.

16- Keren R., Bingham F.T., and Rhoades J.D. 1985. Plant uptake of boron as affected by boron distribution between liquid and solid phases in soil. Soil Science Society of America Journal, 49:279-302.

17- Keren, R., and Sparks D.L. 1994. Effect of pH and ionic strength on boron adsorption pyrophyllite. Soil Science Society of America Journal, 58:1095-1095

18- Kumar K.V., and Sivanesan, S. 2006. Pseudo second order kinetic models for safranin onto rice husk: Comparison of linear and non-linear regression analysis. Process Biochemistry, 41:1198-1202.

19- Langmuir I. 1918. Adsorption of gas on plane surfaces of glass mica and platinum. Journal of the American Chemical Society, 40:1361-1403.

20-Lemarchand E., Schott J., and Gaillardet J. 2007. How surface complexes impact boron isotope fractionation: Evidence from Fe and Mn oxides sorption experiments. Earth and Planetary Science Letters, 260:277-296.

21- Limousin G., Gaudet J.P.,Charlet L., Szenknect S., Barthes V., and Krimissa M. 2007. Sorption isotherms: A review on physical bases Modeling and measurement. Applied Geochemistry, 22:249-275.

22- Mahjoory R.A. 1975. Clay mineralogy, physical and chemical properties of some soils in arid regions of Iran. Soil Science Society of America, Proc. Vol. 39:1157-1164.

23- Sahin S. 2002. A mathematical relationship for the explanation of ion exchange for boron adsorption. Desalination, 143:35-43.

24- Seyhan S., Seki Y.,Yurdakoc M., and Merdivan M. 2007. Application of iron-rich natural clays in C amlica, Turkey for boron sorption from water and its determination by fluorimetric-azomethine-H method. Journal of Hazardous Materials, 146:180–185.

25- Sips R. 1948. On the structure of a catalyst surface. Journal of the Chemical Physics, 16:490-495.

26- Sparks D. l. 2003. Environmental Soil Chemistry. Academic Press San Diego, Califonia.

27- Xu D., and Peak D. 2007. Adsorption of boric acid on pure and humic acid coated am-Al(OH)3: A boron K-edge XANES study. Environmental Science and Technology, 41:903-908.