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Soil Solution and Mobility Characterization of Imazaquin

Published online by Cambridge University Press:  12 June 2017

Andrew J. Goetz ,
Glenn Wehtje ,
Robert H. Walker  and
Ben Hajek
Andrew J. Goetz
Affiliation:
Dep. Agron. and Soils, Alabama Agric. Exp. Stn., Auburn Univ., AL 36849
Glenn Wehtje
Affiliation:
Dep. Agron. and Soils, Alabama Agric. Exp. Stn., Auburn Univ., AL 36849
Robert H. Walker
Affiliation:
Dep. Agron. and Soils, Alabama Agric. Exp. Stn., Auburn Univ., AL 36849
Ben Hajek
Affiliation:
Dep. Agron. and Soils, Alabama Agric. Exp. Stn., Auburn Univ., AL 36849
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Abstract

Imazaquin {2-[4,5-dihydro-4-methyl-4-(1-methylethyl)-5-oxo-1H-imidazol-2-yl]-3-quinolinecarboxylic acid} sorption and mobility were studied in five Alabama soils ranging from sandy loam to clay. Techniques included thinlayer soil chromatography, batch equilibrium, and soil solution recovery. Imazaquin was mobile in all soils with Rf values of 0.8 to 0.9. Sorption based on batch equilibrium was minimal with Kd values ranging from 0.001 to 0.21. The soil solution recovery technique was used to evaluate imazaquin sorption in each soil as influenced by imazaquin concentration, wetting and drying, and pH. As herbicide concentration added to the soils was increased from 0.1 to 10 mg/kg, the amount of 14C-imazaquin in soil solution increased. Temporarily drying each soil to 25 or 50% of field capacity resulted in maximum sorption of imazaquin. Lowering the pH enhanced sorption in all soils such that the amount of imazaquin in solution ranged from 38 (low pH) to 100% (high pH). Soil sorption appeared to be governed by the pH-dependent charge surfaces from aluminum and iron oxyhydroxides (specifically hematite and gibbsite) and kaolinite.

Keywords

Herbicide mobilityanion sorptionsoil sorption
Type
Soil, Air, and Water
Information
Weed Science , Volume 34 , Issue 5 , September 1986 , pp. 788 - 793
Copyright
Copyright © 1986 by the Weed Science Society of America 

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References

Literatur Cited

1. Adams, F., Bumester, C., Hue, N. V., and Long, L. F. 1982. A comparison of column displacement and centrifuge methods of obtaining soil solution. Soil Sci. Soc. Am. Proc. 44:733–735.CrossRefGoogle Scholar
2. Arnold, P. W. 1981. Surface-electrolyte interactions. Pages 355–404 in Greenland, D. J. and Hayes, M. B., eds. The Chemistry of Soil Constituents. John Wiley and Sons, New York.Google Scholar
3. Atkinson, R. J., Posner, A. M., and Quirk, J. P. 1967. Adsorption of potential-determining ions at the ferric oxide-aqueous electrolyte. J. Phys. Chem. 71:550–558.Google Scholar
4. Basham, G. W. and Lavy, T. L. 1985. Imazaquin disappearance in two Arkansas soils. South. Weed Sci. Soc. Proc. 38:477.Google Scholar
5. Bohn, H., McNeal, B., and O'Connor, G. 1979. Soil Chemistry. John Wiley and Sons, New York. 172 pp.Google Scholar
6. Breeuwsma, A. and Lyklema, J. 1973. Physical and chemical adsorption of ions in electrical double layer on hematite (Fe2O3). J. Coll. Int. Sci. 43:437–448.Google Scholar
7. Dickens, R. and Hiltbold, A. E. 1967. Movement and persistence of methanearsonates in soil. Weed Sci. 15:299–304.Google Scholar
8. Fischer, W. R. and Schwertmann, U. 1975. The formation of hematite from amorphous iron (III) hydroxide. Clay Miner. 23:33–37.Google Scholar
9. Gast, R. G. 1977. Surface and colloid chemistry. Pages 22–73 in Dixon, J. B. and Weed, S. B., eds. Minerals in Soil Environments. Soil Sci. Soc. Am., Madison, WI.Google Scholar
10. Green, R. E. and Obien, S. R. 1969. Herbicide equilibrium in soils in relation to soil water content. Weed Sci. 17:514–519.CrossRefGoogle Scholar
11. Greenland, D. J. and Mott, C.J.B. 1978. Surfaces of soil particles. Pages 321–354 in Greenland, D. J. and Hayes, M. B., eds. The Chemistry of Soil Constituents. John Wiley and Sons, New York.Google Scholar
12. Hammaker, F. J., Goring, C.A.I., and Youngson, C. R. 1966. Sorption and leaching of 4-amino-3,5,6-trichloropicolinic acid in soil. Adv. Chem. Ser. 60:23–37.Google Scholar
13. Helling, C. S. 1971. Pesticide mobility in soils. I. Parameters of thin-layer chromatography. Soil Sci. Soc. Am. Proc. 35: 732–737.CrossRefGoogle Scholar
14. Hingston, F. J., Atkinson, R. J., Posner, A. M., and Quirk, J. P. 1967. The specific adsorption of anions. Nature 215:1459–1461.CrossRefGoogle Scholar
15. Hingston, F. J., Atkinson, R. J., Posner, A. M., and Quirk, J. P. 1968. Specific adsorption of anions on goethite. Int. Congr. Soil Sci. Trans. 9th (Adelade) III: 677–699.Google Scholar
16. Hsu, P. H. 1977. Aluminum hydroxides and oxyhydroxides. Pages 99–143 in Dixon, J. B. and Weed, S. B., ed. Minerals in Soil Environments. Soil Sci. Soc. Am., Madison, WI.Google Scholar
17. Karathanasis, A. D. and Hajek, B. F. 1982. Revised methods for rapid quantitative determination of minerals in soil clays. J. Soil Sci. Soc. Am. 46:419–425.CrossRefGoogle Scholar
18. Majka, J. T. and Lavy, T. L. 1977. Adsorption, mobility, and degradation of cyananzine and diuron in soils. Weed Sci. 25: 401–406.CrossRefGoogle Scholar
19. Morrill, L. G., Mahlium, B. C., and Mohiuddin, S. H. 1982. Pages 1–93 in Organic compounds in soils: sorption, degradation, and persistence. Ann Arbor Sci., MI.Google Scholar
20. Mott, C.J.B. 1981. Anion and ligand exchange. Pages 179–218 in Greenland, D. J. and Hayes, M. B., eds. The Chemistry of Soil Processes. John Wiley and Sons, New York.Google Scholar
21. Muljadi, D. A., Posner, M., and Quirk, J. P. 1966. The mechanisms of phosphate adsorption by kaolinite, gibbsite, and pseudo boehmite, Part I. The adsorption isotherms and effect of pH on adsorption. J. Soil Sci. 17:212–228.Google Scholar
22. O'Connor, G. A. and Anderson, J. U. 1974. Soil factors affecting the adsorption of 2,4,5-T. Soil Sci. Soc. Am. Proc. 38:433–436.Google Scholar
23. Parfitt, R. L. 1978. Anion adsorption by soils and soil materials. Adv. Agron. 30:1–50.Google Scholar
24. Parks, G. A. and DeBruyn, P. L. 1962. The zero point of charge of oxides. J. Phys. Chem. 66:967–972.CrossRefGoogle Scholar
25. Patterson, M. G., Buchanan, G. A., Walker, R. H., and Patterson, R. M. 1982. Fluometuron in soil solution as an indicator of its efficacy in three soils. Weed Sci. 30:688–691.CrossRefGoogle Scholar
26. Reyes, E. D. and Jurinak, J. J. 1967. A mechanism of molybdate adsorption on Fe2O3 . Soil Sci. Soc. Am. Proc. 31:637–640.Google Scholar
27. Russell, E. W. 1973. Soil Conditions and Plant Growth. Page 545. William Clowes and Sons, London, England.Google Scholar
28. Schofield, R. K. and Samson, H. R. 1953. The deflocculation of kaolinite suspensions and the accompanying change-over from positive to negative chloride adsorption. Clay Min. Bull. 2:45–50.Google Scholar
29. Schwertmann, U. and Taylor, R. M. 1977. Iron Oxides. Pages 145–180 in Dixon, J. B. and Weed, S. B., eds. Minerals in Soil Environments. Soil Sci. Soc. Am., Madison, WI.Google Scholar
30. Talbert, R. E. and Fletchall, O. R. 1965. The adsorption of some s-triazines in soils. Weeds 13:46–52.Google Scholar
31. Wanchopr, R. D. 1975. Fixation of arsenicals herbicides, phosphate arsenicals in alluvial soils. J. Environ. Qual. 4:355–358.Google Scholar
32. Wang, C. H., Willis, D. J., and Loveland, W. D. 1975. Pages 181–232 in Radiotracer Methodology in the Biological, Environmental, and Physical Sciences. Prentice-Hall, Inc., New Jersey.Google Scholar
33. Weber, J. B. 1970. Mechanisms of adsorption of s-triazines by clay colloids and factors affecting plant availability. Residue Rev. 32:93–130.Google ScholarPubMed