Submit an Article
Become a reviewer
Vol 237
Pages:
307
Download volume:

Thermodynamic Model of Ion-Exchange Process as Exemplified by Cerium Sorption from Multisalt Solutions

Authors:
O. V. Cheremisina1
J. Schenk2
E. A. Cheremisina3
M. A. Ponomareva4
About authors
  • 1 — Saint-Petersburg Mining University
  • 2 — Montan Universität Leoben
  • 3 — K1-Met GmbH
  • 4 — Saint-Petersburg Mining University
Date submitted:
2019-01-13
Date accepted:
2019-03-04
Date published:
2019-06-25

Abstract

A complex heterogeneous process of ion exchange can be defined with an isotherm-isobar equation of the chemical reaction, which describes differential affinity between the process and its effect – the law of mass action. Ion exchange includes processes accompanied by changes in the charge of ions and functional groups caused by the passing of ionic bond into covalent one. Hence isotherm equations of ion exchange for such processes must differ from conventional stoichiometric equations, but they can be obtained by classical study approaches to ion exchange equilibrium. The paper describes a new thermodynamic model, based on linearization of mass action law, modified for the ion exchange equation. The application of this model allows to define stoichiometry of ion exchange and the shape of ions adsorbed by the solid phase of ion-exchange resins, as well as to estimate equilibrium constant and Gibbs free energy of the process. Comparative analysis has been carried out for the thermodynamic model of cerium sorption in the form of anionic complex with Trilon B from a multisalt solution with ionic strength of 1 mol/kg (NaNO 3 ) under рН = 3 and temperature 298 K on a test sample of weak-base anion-exchange resin Cybber EV009. Experimental isotherm of the sorption has been obtained. Calculations of thermodynamic parameters have been performed using Langmuir, Freundlich, Dubinin – Radushkevich, Temkin and Flory – Huggins models, as well as thermodynamic model of linearized mass action law, proposed by the authors. Calculated values of the equilibrium constant and Gibbs energy – K = 9.0±0.5 and ΔrG 0 298  = –5.54±0.27 kJ/mol – characterize the sorption of EDTA cerate ions by ion-exchange resin. The shape of adsorbed ions has been defined in Stern-Helmholtz layer of CeTr, and total capacity of anion resin EV009 for EDTA cerate ions has been estimated as q ∞  = 2.0±0.1 mol/kg.

10.31897/pmi.2019.3.307
Go to volume 237

References

  1. Arlyuk B.I., Veprikova T.B. Dependency of Hydrargyllite Solubility on Concentration of Sodium Alkali and Temperature. Tsvetnye metally. 1981. N 6, p. 59-60 (in Russian).
  2. Druzhinina N.K. Diaspore Solubility in Aluminate Solutions. Tsvetnye metally. 1955. N 1, p. 54-56 (in Russian).
  3. Kuznetsov S.I., Derevyankin V.A. Physical Chemistry of Alumina Production Using Bayer Method. Мoscow: Metallurgizdat. 1964, p. 353 (in Russian).
  4. Lainer Yu.A., Kitler I.N. Metallurgy of Non-Ferrous and Rare Metals. Мoscow: Nauka. 1967, p. 194-199 (in Russian).
  5. Lyapunov A.N., Khodakova A.G., Galkina Zh.G. Hydrargyllite Solubility in Alkali Solutions of Sodium Hydroxide, Containing Soda and Sodium Chloride, under 60 and 95 °С. Tsvetnye metally. 1964. Vol. 37, p. 48-51 (in Russian).
  6. Magarshak G.K. Polytherms in the System Al2O3–Na2O–H2O under 30-200 °С. Legkie metally. 1938. Vol. 7. N 2,
  7. p. 12-16 (in Russian).
  8. Mazel' V.A. Alumina Production. Мoscow: Metallurgizdat. 1955, p. 430 (in Russian).
  9. Lainer A.I., Eremin N.I., Lainer Yu.A., Pevzner I.Z. Alumina Production. Мoscow: Metallurgiya. 1978, p. 344 (in Russian).
  10. Sizyakov V.M., Korneev V.I., Andreev V.V. Increasing the Quality of Alumina and Co-Products During Nepheline Processing. Мoscow: Metallurgiya. 1986, p. 118 (in Russian).
  11. Sizyakov V.M. Chemical and Engineering Patterns of Sintering Processes in Alkali Alumosilicates and Hydrochemical Processing of Sintered Material. Zapiski Gornogo instituta. 2016. Vol. 217, p. 102-112 (in Russian).
  12. Metallurgist’s Guidelines on Non-Ferrous Metals. Alumina Production. Ed. by Yu.V.Baimakova, Ya.E.Kantorovich. Мoscow: Metallurgiya, 1970, p. 320 (in Russian).
  13. Abramov V.Ya., Stel'makova G.D., Nikolaev I.V. et al. Physico-Chemical Outlines of Complex Processing of Aluminum Raw Materials (Alkali Methods). Мoscow: Metallurgiya, 1985, p. 288 (in Russian).
  14. Chizhikov D.M., Kitler I.N., Lainer Yu.A. Chemistry and Alumina Technology. NTISNKh Arm. SSR. Erevan, 1964, p. 233-342 (in Russian).
  15. Tsyrlina S.M. Solubility of Aluminum Hydroxide in Caustic Soda Solutions (System Al(OH)3–NaOH–H2O). Legkie metally. 1936. № 7, p. 28-37 (in Russian).
  16. Chen N.Y. Physical Chemistry of Alumina Production. Shanghai: Scientific and Technical Publishers. 1962, p. 325.
  17. Du C., Zheng S., Zhang Y. Phase equilibria in the K2O–Al2O3–H2O system at 40 C. Fluid Phase Equilibria. 2005. Vol. 238, p. 239-241.
  18. Fricke R., Jucaitis P. Untersuchungen über die Gleichgewichte in den Systemen Al2O3–Na2O–H2O und Al2O3–K2O–H2O. Zeitschrift für anorganische und allgemeine Chemie. 1930. Band 191, p. 129-149.
  19. Ikkatai T., Okada N. Viscosity, specific gravity and equilibrium concentration of sodium aluminate solutions. Extractive Metallurgy of Aluminum. 1963. Vol. 1, p. 159-173.
  20. Israelachvili J.N. Intermolecular and Surface Forces. London: Academic Press. 2011, p. 706.
  21. Pál Sipos. The structure of Al(III) in strongly alkaline aluminate solutions A review. Journal of Molecular Liquids. 2009. Vol. 146. Iss. 1, 2, p. 1-14.
  22. Ma S., Zheng S., Zhang Y., Zhang Yi. Phase Diagram for the Na2O−Al2O3−H2O System at 130 °C. Journal of Chemical and Engineering Data. 2007. Vol. 52. Iss. 1, p. 77-79.
  23. Wei J., Zheng S., Du H., Xu H., Wang S., Zhang Yi. Phase Diagrams for the Ternary Na2O−Al2O3−H2O System at 150 and 180 °C. Journal of Chemical and Engineering Data. 2010. Vol. 55. Iss. 7, р. 2470-2473.
  24. Qiu G., Chen N. Phase study of the system Na2O-Al2O3-H2O. Canadian Metallurgical Quarterly. 1997. Vol. 36. Iss. 2, p. 111-114.
  25. Russell A.S., Edwards J.D., Taylor C.S. A solubility and Density of Hydrate Alumina in Sodium solutions. Journal of Metals. 1955. Vol. 7, p. 1123-1128.
  26. Sprauer J.W., Pearce D.W. Equilibria in the Systems Na2O–SiO2–H2O and Na2O–Al2O3–H2O at 25 °C. Journal of Physical Chemistry. 1940. Vol. 44. Iss. 7, p. 909-911.
  27. Zhang Y., Li Y., Zhang Yi. Phase Diagram for the System Na2O−Al2O3−H2O at High Alkali Concentration. Journal of Chemical and Engineering Data. 2003. Vol. 48. Iss. 3, p. 617-620.

Similar articles

Improving Methodological Approach to Measures Planning for Hydraulic Fracturing in Oil Fields
2019 I. V. Burenina, L. A. Avdeeva, I. A. Solovjeva, M. A. Khalikova, M. V. Gerasimova
Geological and Geomechanical Model of the Verkhnekamsk Potash Deposit Site
2019 Yu. A. Kashnikov, A. O. Ermashov, A. A. Efimov
Modern Physicochemical Equilibrium Description in Na2O–Al2O3–H2O System and Its Analogues
2019 V. M. Sizyakov, T. E. Litvinova, V. N. Brichkin, A. T. Fedorov
Strategic approach to assessing economic sustainability objects of mineral resources sector of Russia
2019 A. O. Nedosekin, E. I. Rejshahrit, A. N. Kozlovskij
Modeling of the Welding Process of Flat Sheet Parts by an Explosion
2019 M. A. Marinin, S. V. Khokhlov, V. A. Isheyskiy
Key Factors of Public Perception of Carbon Dioxide Capture and Storage Projects
2019 S. V. Fedoseev; Pavel S. Tcvetkov