Why is calcite a strong phosphorus sink in freshwater? Investigating the adsorption mechanism using batch experiments and surface complexation modeling

Flower, Hilary; Rains, Mark; Taşcı, Yasemin; Zhang, Jia-Zhong; Trout, Kenneth; Lewis, David; Das, Arundhati; Dalton, Robert

doi:10.1016/j.chemosphere.2021.131596

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Why is calcite a strong phosphorus sink in freshwater? Investigating the adsorption mechanism using batch experiments and surface complexation modeling

2022
By Flower, Hilary ; Rains, Mark ; Taşcı, Yasemin ; ...
Source: Chemosphere, 286: 131596

[PDF-4.11 MB]

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Journal Title:

Chemosphere
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Flower, Hilary ; Rains, Mark ; Taşcı, Yasemin ; Zhang, Jia-Zhong ; Trout, Kenneth ; ... More +

Flower, Hilary ; Rains, Mark ; Taşcı, Yasemin ; Zhang, Jia-Zhong ; Trout, Kenneth ; Lewis, David ; Das, Arundhati ; Dalton, Robert Less -
NOAA Program & Office:

OAR (Oceanic and Atmospheric Research) ; AOML (Atlantic Oceanographic and Meteorological Laboratory)

OAR (Oceanic and Atmospheric Research) ; AOML (Atlantic Oceanographic and Meteorological Laboratory) Less -
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One of the primary drivers of Phosphorus (P) limitation in aquatic systems is P adsorption to sediments. Sediments adsorb more P in freshwater compared to other natural solutions, but the mechanism driving this difference is poorly understood. To provide insights into the mechanism, we conducted batch experiments of P adsorption to calcite in freshwater and seawater, and used computer software to develop complexation models. Our simulations revealed three main reasons that, combining together, may explain the greater P adsorption to calcite in freshwater vs. seawater. First, aqueous speciation of P makes a difference. The ion pair CaPO4− is much more abundant in freshwater; although seawater has more Ca2+ ions, MgHPO40 and NaHPO40 are more thermodynamically favored. Second, the adsorbing species of P make a difference. The ion pair CaPO4− (the preferred adsorbate in freshwater) is able to access adsorption sites that are not available to HPO42− (the preferred adsorbate in seawater), thereby raising the maximum concentration of P that can adsorb to the calcite surface in freshwater. Third, water chemistry affects the competition among ions for surface sites. Other ions (including P) compete more effectively against CO32− when immersed in freshwater vs. seawater, even when the concentration of HCO3−/CO32− is higher in freshwater vs. seawater. In addition, we found that under oligotrophic conditions, P adsorption is driven by the higher energy adsorption sites, and by the lower energy sites in eutrophic conditions. This study is the first to model P adsorption mechanisms to calcite in freshwater and seawater.
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Freshwater Phosphates
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Chemosphere, 286: 131596
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https://doi.org/10.1016/j.chemosphere.2021.131596
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Journal Article
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urn:sha256:cba5ee021b794fb217f8581593b51f7af7b1b54319eb7b7fcb467932d96816b6
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Why is calcite a strong phosphorus sink in freshwater? Investigating the adsorption mechanism using batch experiments and surface complexation modeling

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