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The effect of a copolymer inhibitor on baryte precipitation

Published online by Cambridge University Press:  05 July 2018

Cristina Ruiz-Agudo ,
Christine V. Putnis  and
Andrew Putnis
Cristina Ruiz-Agudo*
Affiliation:
Institut für Mineralogie, University of Münster, 48149 Münster, Germany
Christine V. Putnis
Affiliation:
Institut für Mineralogie, University of Münster, 48149 Münster, Germany
Andrew Putnis
Affiliation:
Institut für Mineralogie, University of Münster, 48149 Münster, Germany
*
* E-mail: [email protected]
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Abstract

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In situ atomic force microscopy (AFM) experiments were used to study the effect of trace amounts of a commercial inhibitor on the (001) baryte surface during growth. The additive tested was a copolymer, used as a scale inhibitor in oil recovery (maleic acid/allyl sulfonic acid copolymer with phosphonate groups, partial sodium salt). The morphology of the growth was used to gain a better understanding of the inhibition mechanism. Without an inhibitor, barium sulfate growth occurred by 2D island nucleation and spreading. The addition of a small amount (0.1 ppm and 0.5 ppm) of copolymer inhibitor enhances 2D nucleation but blocks growth. Just 1 ppm of inhibitor blocks nucleation and growth by adsorption of a copolymer layer onto the baryte surface. Similarly in 3D studies, small amounts of inhibitor seem to act on growth and not on nucleation and larger amounts of copolymer act on both by adsorption of the copolymer to all baryte surfaces keeping the particles in their embryo stage.

Keywords

AFMbarytescale inhibitor
Type
Research Article
Information
Mineralogical Magazine , Volume 78 , Issue 6 , November 2014 , pp. 1423 - 1430
Creative Commons
Creative Common License - CCCreative Common License - BY
© [2014] The Mineralogical Society of Great Britain and Ireland. This is an open access article distributed under the terms of the Creative Commons Attribution (CC BY) licence (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
Copyright
Copyright © The Mineralogical Society of Great Britain and Ireland 2014

References

Baynton, A., Chandler, B.D., Jones, F., Nealon, G., Ogden, M.I., Radomirovic, T., Shimizu, G.K.H. and Taylor, J.M. (2011) Phosphonate additives do not always inhibit crystallization. CrystEngComm, 13, 1090–1095.CrossRefGoogle Scholar
Baynton, A., Ogden, M.I., Raston, C.L. and Jones, F. (2012) Barium sulfate crystallization dependence on upper rim calix[4]arene functional groups. CrystEngComm, 14, 1057–1062.CrossRefGoogle Scholar
Benton, W.J., Collins, I.R., Grimsey, I.M., Parkinson, G.M. and Rodger, S.A. (1993) Nucleation, growth and inhibition of barium sulfate-controlled modification with organic and inorganic additives. Faraday Discussions, 95, 281–297.CrossRefGoogle Scholar
Blount, C.W. (1977) Barite solubilities and thermodynamic quantities up to 300ºC and 1400 bars. American Mineralogist, 62, 942–957.Google Scholar
Coveney, P.V., Davey, R., Griffin, J.L.W., He, Y., Hamlin, J.D., Stackhouse, S. and Whiting, A. (2000) A new design strategy for molecular recognition in heterogeneous systems: A universal crystal-face growth inhibitor for barium sulfate. Journal of the American Chemical Society, 122, 11557–11558.CrossRefGoogle Scholar
Fernandez-Diaz, L., Putnis, A. and Cumberbatch, T.J. (1990) Barite nucleation kinetics and the effect of additives. European Journal of Mineralogy, 2, 495–501.CrossRefGoogle Scholar
Jones, F., Oliveira, A., Rohl, A.L., Parkinson, G.M., Ogden, M.I. and Reyhani, M.M. (2002) Investigation into the effect of phosphonate inhibitors on barium sulfate precipitation. Journal of Crystal Growth, 237–239, 424–429.CrossRefGoogle Scholar
Judat, B. and Kind, M. (2004) Morphology and internal structure of barium sulfate – derivation of a new growth mechanism. Journal of Colloid and Interface Science, 269, 341–353.CrossRefGoogle ScholarPubMed
Kowacz, M., Putnis, C.V. and Putnis, A. (2007) The effect of cation:anion ratio in solution on the mechanism of barite growth at constant supersaturation: Role of the desolvation process on the growth kinetics. Geochimica et Cosmochimica Acta, 71, 5168–5179.CrossRefGoogle Scholar
Long, X., Ma, Y., Cho, K.R., Li, D., De Yoreo, J.J. and Qi, L. (2013) Oriented calcite micropillars and prisms formed through aggregation and recrystallization of poly(acrylic acid) stabilized nanoparticles. Crystal Growth and Design, 13, 3856–3863.CrossRefGoogle Scholar
Mavredaki, E., Neville, A. and Sorbie, K. (2011) Assessment of barium sulphate formation and inhibition at surfaces with synchrotron X-ray diffraction (SXRD). Applied Surface Science, 257, 4264–4271.CrossRefGoogle Scholar
Mavredaki, E., Neville, A. and Sorbie, K.S. (2011) Initial stages of barium sulfate formation at surfaces in the presence of inhibitors. Crystal Growth and Design, 11, 4751–4758.CrossRefGoogle Scholar
Parkhurst, D.L. and Appelo, C.A.J. (1999) Users guide to PHREEQC (version 2) – a computer program for speciation, b.t.h reaction, o.e.dimensional transport, a.d.inverse geochemical calculations. U.S. Geological Survey Water-Resources Investigation Report, 99–4259.Google Scholar
Piana, S., Jones, F. and Gale, J.D. (2006) Assisted desolvation as a key kinetic step for crystal growth. Journal of the American Chemical Society, 128, 13568–13574.CrossRefGoogle ScholarPubMed
Pina, C.M., Becker, U., Risthaus, P., Bosbach, D. and Putnis, A. (1998) Molecular-scale mechanisms of crystal growth in barite. Nature, 395, 483–486.CrossRefGoogle Scholar
Pina, C.M., Putnis, C.V., Becker, U., Biswas, S., Carroll, E.C., Bosbach, D. and Putnis, A. (2004) The inhibition of barite growth by phosphonates: Determination of adsorption isotherms by atomic force microscopy. Surface Science, 553, 61–74.CrossRefGoogle Scholar
Putnis, C.V., Kowacz, M. and Putnis, A. (2008) The mechanism and kinetics of DTPA-promoted dissolution of barite. Applied Geochemistry, 23, 2278–2788.CrossRefGoogle Scholar
Qi, L., Coelfen, H. and Antonietti, M. (2000) Control of barite morphology by double-hydrophilic block copolymers. Chemistry of Materials, 12, 2392–2403.CrossRefGoogle Scholar
Sangwal, K. (1998) Growth kinetics and surface morphology of crystals grown from solutions: recent observations and their interpretations. Progress in Crystal Growth and Characterization of Materials, 36, 163–248.CrossRefGoogle Scholar
Shakkthivel, P., Sathiyamoorthi, R. and Vasudevan, T. (2006) Acrylic acid-diphenylamine sulphonic acid copolymer threshold inhibitor for sulphate and carbonate scales in cooling water systems. Desalination, 197, 179–189.CrossRefGoogle Scholar
Sorbie, K.S. and Mackay, E.J. (2000) Mixing of1 injected connate and aquifer brines in waterflooding and its relevance to oilfield scaling. Journal of Petroleum Science and Engineering, 27, 85–106.CrossRefGoogle Scholar
Teng, H.H., Dove, P.M., Orme, C. and De Yoreo, J.J. (1998) Thermodynamics of calcite growth: baseline for understanding biomineral formation. Science, 282, 724–727.CrossRefGoogle ScholarPubMed
Van der Leeden, M.C. and Van Rosmalen, G.M. (1995) Adsorption behaviour of polyelectrolytes on barium sulfate crystals. Journal of Colloid and Interface Science, 171, 142–149.CrossRefGoogle Scholar
Van Rosmalen, G.M. (1983) Scale prevention with special reference to threshold treatment. Chemical Engineering Communications, 20, 209–23.CrossRefGoogle Scholar