Direct Effects and Interactions Involving Iron and Humic Acid During Formation of Colloidal Phosphorus

  • Thomas C. Young
  • W. Gregg Comstock

Abstract

Precipitation and complexation reactions involving factorial treatment combinations of iron (Fe), phosphorus (P), and humic acid (HA) in aerobic, slightly alkaline (pH 8.65) media permitted differentiation of direct effects and interactions among these factors, which result in formation of colloidal (nondialyzable) P. The range of concentrations studied were 0.05 to 0.2 mg total P/1, 0.1 to 100 mg total Fe/1, and 0.05 to 50.0 mg HA (Aldrich)/1. The data showed that HA, in contrast to Fe, had no capacity to bind inorganic P directly to form a colloidal phase. However, the extent of formation of colloidal P by Fe varied inversely with the amount of HA and inorganic P added to the experimental systems. Adsorption isotherms grouped according to the Fe/HA ratio (w/w) of the treatment combinations indicated occurrence of a maximum adsorption density of 0.1 mg P/mg Fe at a ratio of approximately 0.2:1. The results suggested that HA in increasing amounts decreased the polynuclear nature of the colloidal Fe and, coincidently, changed the number of sites for adsorption of P.

Keywords

Humic Substance Humic Acid American Public Health Association Flame Atomic Absorption Spectrometry Outer Solution 
These keywords were added by machine and not by the authors. This process is experimental and the keywords may be updated as the learning algorithm improves.

Preview

Unable to display preview. Download preview PDF.

Unable to display preview. Download preview PDF.

References

  1. American Public Health Association (APHA), 1975. Standard Methods, ed. 14. American Public Health Association, New York, 1193 pp.Google Scholar
  2. Bache, B., 1964. Aluminum and iron phosphate studies relating to soils. J. Soil Sci., 15: 110–116.CrossRefGoogle Scholar
  3. Comstock, W.G., 1982. The Direct and Interactive Effects of Iron and Humic Acid on the Partitioning of Inorganic Phosphorus Between Dissolved and Colloidal States, M.S. Thesis. Department of Civil and Environmental Engineering, Clarkson University, Potsdam, NY, 225 pp.Google Scholar
  4. Cowen, W.F. and Lee, G.F., 1976. Phosphorus availability in particulate materials transported in urban runoff. J. Water Poll. Control Fed., 48: 580–591.Google Scholar
  5. De Pinto, J.V., Young, T.C. and Martin, S.C., 1981. Algal- available phosphorus in suspended sediments of lower Great Lakes tributaries. J. Great Lakes Res., 7: 311–325.CrossRefGoogle Scholar
  6. Dorich, R.A., Nelson, D.W. and Sommers, L.E., 1980. Algal availability of sediment phosphorus in drainage water of the Black Creek watershed. J. Environ. Qual., 9: 557–563.CrossRefGoogle Scholar
  7. Dousma, J. and de Bruyn, PC., 1976. Hydrolysis- precipitation studies of iron solutions. I. Model for hydrolysis and precipitation from Fe(III) nitrate solutions. J. Colloid Internatl. Sci., 56: 527–539.Google Scholar
  8. Eisenreich, S.J. and Armstrong, D.E., 1980. Association of organic matter, iron, and inorganic phosphorus in lake water. Environ. Internatl, 3: 485–490.CrossRefGoogle Scholar
  9. Koenigs, J. P. and Hooper, F.F., 1976. The influence of colloidal organic matter on iron and iron-phosphorus cycling in an acid bog lake. Limnol Oceanogr., 21: 674–696.CrossRefGoogle Scholar
  10. Lijklema, L., 1980. Interaction of orthophosphate with iron (III) and aluminum hydroxides. Environ. Sci. Tech- nol., 14: 537-541.Google Scholar
  11. Rast, W. and Lee, G.F., 1978. Summary Analysis of the North American (U.S. Portion) OECD Eutrophication Project: Nutrient Loading—Lake Responses, Relationships and Trophic State Indices. Ecological Research Series, EPA-600/3-78-008, USEPA-ORD, ERL, Corvallis, OR, 455 pp.Google Scholar
  12. Stumm, W. and Morgan, J.J., 1981. Aquatic Chemistry. Wiley-Interscience, New York, 780 pp.Google Scholar
  13. Swenson, R.M., Cole, C.V. andSieling, D.H., 1949. Fixation of phosphate by iron and aluminum and replacement by organic and inorganic ions. J. Soil Sci., 67: 3–22.CrossRefGoogle Scholar
  14. Syers, J.K., Harris, R.R. and Armstrong, D.R., 1973. Phosphate chemistry in lake sediments. J. Environ. Qual., 2: 1–14.CrossRefGoogle Scholar
  15. Westall, J.C., Zachary, J.L. and Morel, F.M.M., undated. MINEQL: A Computer Program for the Calculation of Chemical Equilibrium Composition of Aqueous Systems (MINEQL User’s Guide). Department of Civil Engineering, Massachusetts Institute of Technology, Boston, MA, 91 pp.Google Scholar
  16. Williams, J.D.H., Syers, J.K., Shukla, S.S. and Harris, R.R., 1971. Levels of inorganic and total phosphorus in lake sediments as related to other sediment parameters. Environ. Sci. Technol., 5: 1113–1120.CrossRefGoogle Scholar
  17. Williams, J.D.H., Shear, H. and Thomas, R.L., 1980. Availability to Scenedesmus quadricauda of different forms of phosphorus in sedimentary materials in the Great Lakes. Limnol. Oceanogr., 25: 1–11.CrossRefGoogle Scholar
  18. Young, T.C. and De Pinto, J.V., 1982. Algal-availability of particulate phosphorus from diffuse and point sources in the lower Great Lakes basin. Hydrobiologia, 94: 111–119.Google Scholar

Copyright information

© Springer-Verlag New York Inc. 1986

Authors and Affiliations

  • Thomas C. Young
  • W. Gregg Comstock

There are no affiliations available

Personalised recommendations