Abstract
Chemical reactions in soils largely determine the availability of Fe to plants. The solubility of Fe in soils can best be expressed as: Fe(OH)3(soil-Fe) + 3H+ ⇌ Fe3+ + 3H2O having a log K° value of 2.70. This solubility constant is 0.84 log units less than that of freshly precipitated amorphous Fe(OH)3, and approximately 2.7 log units more soluble than goethite and hematite. Hydrolysis species of Fe3+ raise total soluble Fe to approximately 10-10.4 M in calcareous soils, but plants growing in soils require approximately 10-8 M soluble Fe. Without some modifying mechanism, most plants would show Fe deficiencies when growing in media above pH 5.0.
Some plants are capable of lowering redox next to respiring roots to the pe + pH range of 4 to 7. This highly reducing environment is capable of supplying available Fe2+ through the dissolution and reduction of Fe(III) oxides.
Chelating agents in the rhizosphere are beneficial because they raise total Fe in solution, increase diffusion gradients, and eliminate Fe depletion zones next to absorbing roots. Strong chelating agents such as FeEDDHA generally correct Fe deficiency, but in hydroponic solutions, they sometimes cause Fe deficiency. As plants absorb Fe, chelating agent is left behind and depresses Fe3+ activity making it less available to plants. Adding extra Fe to a nutrient media, keeps the chelating agent saturated with Fe and available to plants.
Both synthetic and natural chelating agents act as carriers to transport Fe to plant roots. The enriched electron environment of respiring roots reduces Fe3+ to Fe2+ thus decreasing Fe3+ and causing ferric chelate (FeL-) to dissociate. The newly formed Fe2+ is available for absorption by roots while the released chelating agent diffuses away from the root and becomes resaturated with Fe3+. Chelation and reduction are important mechanisms that take place near roots which affect the availability of Fe to plants.
Chemical speciation models such as MINTEQA2 and GEOCHEM-PC are useful for predicting and interpreting complex equilibrium relationships involving chelation, Fe solubility, redox, and nutrient uptake. Computer models are useful for examining equilibrium relationships that simulate root environments.
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References
Allison J D, Brown D S and Novo-Gradac K J 1990 MINTE-QA2/PRODEFA2 — a geochemical assessment model for environmental systems, Version 3.0 User’s Manual. Environmental Res. Lab., U S EPA, Athens, GA 30613.
Arden T V 1950 The solubility products of ferrous and ferrosic hydroxides. J. Chem. Soc. XX, 882–885.
Barber S A 1984 Soil Nutrient Bioavailability — A Mechanistic Approach. John Wiley and Sons, New York. 398p.
Bell P F, Chaney R L and Angel J S 1991 Determination of the copper activity required by maize using chelator-buffered nutrient solutions. Soil Sci. Soc. Am. J. 55, 1366–1374.
Brennan E W 1994 Effect of redox on the solubility and mineral transformations of Fe, Zn, Pb, and Cd in soils. Ph.D. Dissertation, Department of Agronomy, Colorado State University, Fort Collins, CO.
Elgawhary S M, Lindsay W L and Kemper W D 1970 Effect of complexing agents and acids on the diffusion of zinc to a simulated root. Soil Sci. Soc. Am. Proc. 34, 211–214.
Halvorson A D 1971 Chelation and availability of metal ions in nutrient solutions. Ph.D. Dissertation, Department of Agronomy, Colorado State University, Fort Collins, CO. 134 p.
Lindsay W L 1974 Role of chelation in micronutrient availability. In The Plant Root and its Environment. Ed. E W Carson, pp 507–524. University Press of Virginia, Charlottesville.
Lindsay W L 1979 Chemical Equilibria in Soils. Wiley-Interscience, New York. 449 p.
Lindsay W L 1981 Solid phase-solution equilibria in soils. In Chemistry in the Soil Environment. Eds. R H Dowdy, J A Ryan, V V Volk and D E Baker, pp 183–202. ASA Special Pub. 40. Am. Soc. Agronomy, Madison, WI.
Lindsay W L and Ajwa H A 1994 Use of MINTEQA2 for teaching soil chemistry. In Chemical Equilibrium Reaction Models. Eds. R H Loeppert, S Goldberg and A P Schwab. Soil Science Society of America, Madison, WI. (In press).
Lindsay W L and Sadiq M 1983 Use of pe + pH to predict and interpret metal solubility relationships in soils. Sci. Total Environ. 28, 169–178.
Lindsay W L and Schwab A P 1982 The chemistry of iron in soils and its availability to plants. J. Plant Nutr. 5(4–7), 821–840.
Marschner H, Römheld V and Ossenberg-Neuhaus H 1982 Rapid method for measuring changes in pH and reducing processes along roots of intact plants. Z. Pflanzenphysiol. 105, 407–416.
Norvell W A and Lindsay W L 1982a Estimation of the concentration of Fe3+ and the (Fe3+) (OH-)3 ion product from equilibria of EDTA in soil. Soil Sci. Soc. Am. J. 46, 710–715.
Norvell W A and Lindsay W L 1982b Effect of ferric chloride additions on the solubility of ferric ion in a near-neutral soil. J. Plant Nutr. 5, 1285–1295.
O’Connor G A, Lindsay W L and Olsen S R 1970 Diffusion of iron and iron chelates in soil. Soil Sci. Soc. Am. Proc. 34, 407–410.
Parker D R, Norvell W A and Chaney R L 1993 GEOCHEM-PC: a chemical speciation program for IBM compatible. In Chemical Equilibrium Reaction Models. Eds. R H Leoppert, S Goldberg and A P Schwab. Soil Science Society of America, Madison, WI. (In press).
Ponnamperuma F N, Tianco E M and Loy T 1967 Redox equilibria in flooded soils: I. The iron hydroxide systems. Soil Sci. 103, 374–382.
Powell P E, Szaniszlo P J, Cline G R and Reid C P P 1982 Hydrox-amate siderophores in the iron nutrition of plants. J. Plant Nutr. 5, 653–673.
Römheld V 1991 The role of phytosiderophores in acquisition of iron and other micronutrients in graminaceous species: An ecological approach. In Iron Nutrition and Interactions in Plants. Eds. Y Chen and Y Hadar. pp 159–166. Kluwer Academic Publishers, Dordrecht.
Römheld V and Marschner H 1990 Genotypical differences among graminaceous species in release of phytosiderophores and uptake of iron phytosiderophores. Plant and Soil 123, 147–153.
Schwab A P and Lindsay W L 1983 Effect of redox on the solubility and availability of iron. Soil Sci. Soc. Am. J. 47, 201–205.
Schwab A P and Lindsay W L 1989a A computer simulation of Fe(III) and Fe(II) complexation in limited nutrient solution: I. Program development and testing. Soil Sci. Soc. Am. J. 53, 29–34.
Schwab A P and Lindsay W L 1989b A computer simulation of Fe(III) and Fe(II) complexation in nutrient solutions: II. Application to growing plants. Soil Sci. Soc. Am. J. 53, 34–38.
Schwertmann U and Taylor R M 1989 Iron oxides. Minerals in Soil Environments. Second Edition. Eds. J B Dixon and S B Weed. Soil Sci. Soc. Am., Book Series 1, 379–438.
Simeoni L A, Lindsay W L and Baker R 1987 Critical iron level associated with biological control of fusarium wilt. Ecol. Epidemiol. 77, 1057–1061.
Thorne D W, Wann F B and Robinson W 1951 Hypotheses concerning lime-induced chlorosis. Soil Sci. Soc. Am. Proc. 15, 254–258.
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Lindsay, W. (1995). Chemical reactions in soils that affect iron availability to plants. A quantative approach. In: Abadía, J. (eds) Iron Nutrition in Soils and Plants. Developments in Plant and Soil Sciences, vol 59. Springer, Dordrecht. https://doi.org/10.1007/978-94-011-0503-3_2
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DOI: https://doi.org/10.1007/978-94-011-0503-3_2
Publisher Name: Springer, Dordrecht
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