Effects of fluoride and polymeric additives on the dissolution of calcite and the subsequent formation of fluorite

Yang, Taewook; Huh, Wansoo; Jho, Jae Young; Kim, Il Won

doi:10.1016/j.colsurfa.2014.03.040

Cited by 5 publications

(4 citation statements)

References 44 publications

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“…During the dissolution of calcite, the precipitation of several secondary minerals has been observed in the presence of aqueous cations (Pb 2+ , Cu 2+ , and ) 125 – 128 , oxyanions ( , , and ) 129 , 130 , and F − 131 due to the formation of less soluble phases. Sometimes, calcite might be entirely replaced by the secondary minerals, such as cerussite (PbCO 3 ) 132 , dolomite (CaMg(CO 3 ) 2 ) 133 – 135 , magnesite (MgCO 3 ) 134 , siderite (FeCO 3 ) 133 , gypsum (CaSO 4 ) 136 , 137 , whewellite (CaC 2 O 4 ·H 2 O) 138 and fluorite (CaF 2 ) 139 , 140 , via a coupled dissolution–precipitation mechanism.…”

Section: Discussionmentioning

confidence: 99%

Divalent heavy metals and uranyl cations incorporated in calcite change its dissolution process

Zhang

Guo

et al. 2020

Sci Rep

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Due to the high capacity of impurities in its structure, calcite is regarded as one of the most attractive minerals to trap heavy metals (HMs) and radionuclides via substitution during coprecipitation/crystal growth. As a high-reactivity mineral, calcite may release HMs via dissolution. However, the influence of the incorporated HMs and radionuclides in calcite on its dissolution is unclear. Herein, we reported the dissolution behavior of the synthesized calcite incorporated with cadmium (Cd), cobalt (Co), nickel (Ni), zinc (Zn), and uranium (U). Our findings indicated that the HMs and U in calcite could significantly change the dissolution process of calcite. The results demonstrated that the incorporated HMs and U had both inhibiting and enhancing effects on the solubility of calcite, depending on the type of metals and their content. Furthermore, secondary minerals such as smithsonite (ZnCO3), Co-poor aragonite, and U-rich calcite precipitated during dissolution. Thus, the incorporation of metals into calcite can control the behavior of HMs/uranium, calcite, and even carbon dioxide.

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Section: Discussionmentioning

confidence: 99%

Divalent heavy metals and uranyl cations incorporated in calcite change its dissolution process

Zhang

Guo

et al. 2020

Sci Rep

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“…This extra fluoride removal might be from adsorption of fluoride on the surface of both calcite nanoparticles and calcium fluoride. Yang et al [16] indicated that calcite dissolution to release calcium ions is the rate-determining step because the released calcium ions would rapidly form fluorite. Turner et al [15] indicated that equilibrium was reached within 24 h at pH < 8.0, and the slower rate of reaction at higher pH could reflect OH À competition with F À for surface adsorption sites or decreasing calcite dissolution rate.…”

Section: Kinetic Studymentioning

confidence: 99%

“…Direct evidence of calcium fluoride precipitation at fluoride concentration of 700 mg/L was found by XPS, and a conceptual model combining surface adsorption and precipitation was proposed. Yang et al [16] used X-ray diffraction (XRD) and AFM to examine dissolution of calcite and formation of fluorite at pH 3 and 7. Spherical fluorite rods formed around nucleation centers at pH 3.…”

Section: Introductionmentioning

confidence: 99%

Adsorption and precipitation of fluoride on calcite nanoparticles: A spectroscopic study

Budyanto

Kuo

Liu

2015

Separation and Purification Technology

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“…Both inhibition (e.g., organic acids, Fe 2+ , Mg 2+ , Sr 2+ , PO4 3-) and enhancement (e.g. chelators, Cl -, I -, F -, ) of dissolution kinetics have been observed [33][34][35][36][37][38][39][40][41][42], and in some cases enhancement changed to inhibition or vice versa as the concentration and/or molecular weight of structurally similar molecules changed (e.g., polyaspartate) [43,44]. Inhibition kinetic effects are often attributed to ion adsorption and pinning at step edges [33], as well as general competitive adsorption with Ca 2+ and/or CO3 2- [35].…”

Section: Introductionmentioning

confidence: 99%

Surfactant inhibition mechanisms of carbonate mineral dissolution in shale

Kim

Jagannath

et al. 2021

Colloids and Surfaces A: Physicochemical and Engineering Aspect

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Surfactants are common additives to hydraulic fracturing and enhanced oil recovery (EOR) fluids, and are under consideration for amendment to supercritical carbon dioxide for geological carbon sequestration (GCS). The effect of a common anionic surfactant, internal olefin sulfonate (IOS), on mineral dissolution from shale into brine was evaluated. When added to brine at concentrations exceeding the critical micelle concentration (94 mg/L), IOS inhibited carbonate mineral dissolution in an Eagle Ford shale, as well as dissolution of optical quality calcite (the dominant carbonate in the shale). Laser profilometry images provide spatial resolution across >3 orders of magnitude, and indicate that IOS addition to brine both enhances the formation of new etch pits in calcite, and impedes their further growth. Time-of-flight secondary ion mass spectrometry surface profiles show for the first time that IOS preferentially adsorbs at calcite pit edges versus flat calcite surfaces (i.e., terraces). Surface pressure calculations, sulfur K-edge near edge X-ray absorption fine structure (NEXAFS) spectroscopy results, and density functional theory (DFT) calculations support this observation; the DFT results indicate that the sulfonate head group of the IOS molecule binds strongly to the calcite step site as compared to the terrace site. The S K-edge NEXAFS results indicate that IOS adsorbed more to etched calcite surfaces compared to smooth calcite surfaces. Overall, the results indicate that weak adsorption on flat calcite surfaces (i.e., terraces) disrupts water structure and enhances mass transfer of dissolution, while strong adsorption on calcite pit edges displaces adsorbed water and inhibits further etch pit growth. This work provides the first direct evidence of preferential adsorption of IOS to etched calcite surfaces and links it to macroscopic dissolution kinetics. This work has implications for surfactantcontaining fluids used in hydraulic fracturing, EOR and potentially GCS for subsurface injection into carbonate rich reservoirs.

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Effects of fluoride and polymeric additives on the dissolution of calcite and the subsequent formation of fluorite

Cited by 5 publications

References 44 publications

Divalent heavy metals and uranyl cations incorporated in calcite change its dissolution process

Divalent heavy metals and uranyl cations incorporated in calcite change its dissolution process

Adsorption and precipitation of fluoride on calcite nanoparticles: A spectroscopic study

Surfactant inhibition mechanisms of carbonate mineral dissolution in shale

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