Effect of ferrous iron on the nucleation and growth of CaCO<sub>3</sub>in slightly basic aqueous solutions

Lorenzo, Fulvio Di; Burgos-Cara, Alejandro; Ruíz-Agudo, Encarnación; Putnis, Christine V.; Prieto, M.

doi:10.1039/c6ce02290a

Cited by 19 publications

(29 citation statements)

References 48 publications

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“…For example, Kelland [71] found that iron ions concentrations below 25 ppm did not affect the CaCO 3 precipitation in high pressure dynamic tube blocking tests. Comparable results were found by Lorenzo et al [72] who studied the effect of ferrous iron ions on the CaCO 3 growth by the constant composition method. However, Herzog et al [73] found that, in magnetic water treatment devices, an excess of ferrous ions (5.6 ppm) strongly inhibits both calcite growth and the transformation of aragonite to calcite.…”

Section: Effect Of Iron Ionssupporting

confidence: 57%

Effect of Operating Parameters and Foreign Ions on the Crystal Growth of Calcium Carbonate during Scale Formation: An Overview

Korchef¹

2022

Crystallization and Applications

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Due to the insufficiency of freshwater resources and to supply the drinking water populations, many desalination processes such as reverse osmosis, electrodialysis and distillation are widely used. However, these processes are of large-scale consumers of energy and confronted with various problems such as corrosion and scale formation. In most cases, scales are made of calcium carbonate CaCO3. In the present chapter, an overview on the effect of operating parameters such as temperature, pH and supersaturation on the precipitation kinetics, microstructure, and polymorphism of CaCO3 is given. Additionally, I put special emphasis on the effect of foreign ions such as magnesium, sulphate, and iron ions on CaCO3 precipitation since they are present at significant concentrations in natural waters. Also, the mechanisms by which these ions affect the crystal growth of CaCO3 were pointed out. Knowledge about these operating parameters as well as the effects of foreign ions allow elucidating the polymorphs growth during water treatment. The control of these operating parameters allows reducing scale formation during drinking water and wastewater treatment. The economic impact is of greatest importance since this favorably affects the treatment costs, increases the equipment life, and allows enhanced product water recovery.

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Section: Effect Of Iron Ionssupporting

confidence: 57%

Effect of Operating Parameters and Foreign Ions on the Crystal Growth of Calcium Carbonate during Scale Formation: An Overview

Korchef¹

2022

Crystallization and Applications

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“…10, K Fe should be determined in advance. However, K Fe that specifically represents partition coefficient of benthic Fe 2+ incorporation into calcite has not been directly determined for modern limestone, although the factors affecting Fe 2+ incorporation into calcite in aqueous solution at equilibrium state have been investigated 55,56 . To constrain this unknown, we use Fe carb data of late Devonian-early Carboniferous shallow marine carbonate samples (Madao, Panlong and Dazhai sections), to calculate the K Fe .…”

Section: Discussionmentioning

confidence: 99%

Early animal evolution and highly oxygenated seafloor niches hosted by microbial mats

Ding

Dong

Sun

et al. 2019

Sci Rep

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The earliest unambiguous evidence for animals is represented by various trace fossils in the latest Ediacaran Period (550–541 Ma), suggesting that the earliest animals lived on or even penetrated into the seafloor. Yet, the O2 fugacity at the sediment-water interface (SWI) for the earliest animal proliferation is poorly defined. The preferential colonization of seafloor as a first step in animal evolution is also unusual. In order to understand the environmental background, we employed a new proxy, carbonate associated ferrous iron (Fecarb), to quantify the seafloor oxygenation. Fecarb of the latest Ediacaran Shibantan limestone in South China, which yields abundant animal traces, ranges from 2.27 to 85.43 ppm, corresponding to the seafloor O2 fugacity of 162 μmol/L to 297 μmol/L. These values are significantly higher than the oxygen saturation in seawater at the contemporary atmospheric pO2 levels. The highly oxygenated seafloor might be attributed to O2 production of the microbial mats. Despite the moderate atmospheric pO2 level, microbial mats possibly provided highly oxygenated niches for the evolution of benthic metazoans. Our model suggests that the O2 barrier could be locally overcome in the mat ground, questioning the long-held belief that atmospheric oxygenation was the key control of animal evolution.

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“…Thermodynamic data for nesquehonite (MgCO 3. 3H 2 O) (Robie and Hemingway, 1995), hydromagnesite (Mg 5 (CO 3 ) 4 (OH) 2 •4H 2 O) (Galvez-Martos et al, 2018), dolomite ((Ca 0.5 Mg 0.5 )CO 3 ) (Galvez-Martos et al, 2018), monohydrocalcite (CaCO 3 .H 2 O) (Robie and Hemingway, 1995), and an iron-calcium carbonate solid-solution model ((Ca,Fe)CO 3 ) (Di Lorenzo et al, 2017) were included in the simulations. Thermodynamic data for metastable nesquehonite and hydromagnesite were included as potential magnesium carbonate phases, opposed to "natural" mineral thermodynamic data to represent the short-term precipitation time.…”

Section: Thermodynamic Modeling Of Precipitation Productsmentioning

confidence: 99%

“…The dolomite phase was chosen to represent partial calcium replacement by magnesium within CaCO 3 . The (Ca,Fe)CO 3 non-ideal solution model was developed in a CaO-MgO-FeOOH-CO 2 system to represent iron (II) replacement within the CaCO 3 structure in the presence of magnesium (Di Lorenzo et al, 2017).…”

Section: Thermodynamic Modeling Of Precipitation Productsmentioning

confidence: 99%

“…For zeolitic solutions, aragonite formation is dominant between volume ratios of 0.2-0.6 because large [Ca]/[Fe] ratios are required to favor calcite formation (Di Lorenzo et al, 2017), with goethite as the primary contaminant. The reduction of the initial pH reduces goethite formation which decreases the [Ca]/ [Fe] in solution to a point where it enters the miscibility gap of the (Fe,Ca)CO 3 solid solution model used (Di Lorenzo et al, 2017). The FeCO 3 end-member forms preferentially but at low quantities which causes aragonite to form in place of calcite.…”

Section: Carbon Dioxide Mineralization Of Simulated Produced Water Anmentioning

confidence: 99%

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Implementation of Ion Exchange Processes for Carbon Dioxide Mineralization Using Industrial Waste Streams

et al. 2020

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Sequestration of CO2 within stable mineral carbonates (e.g., CaCO3) represents an attractive emission reduction strategy because it offers a leakage-free alternative to geological storage of CO2 in an environmentally benign form. However, the pH of aqueous streams equilibrated with gaseous streams containing CO2 (pH < 4) are typically lower than that which is required for carbonate precipitation (pH > 8). Traditionally, alkalinity is provided by a stoichiometric reagent (e.g., NaOH) which renders these processes environmentally hazardous and economically unfeasible. This work investigates the use of regenerable ion-exchange materials to induce alkalinity in CO2-saturated aqueous solutions such that the pH shift required for mineralization occurs without the need for stoichiometric reagents. Na+-H+ exchange isotherms (at [H+] = 10−8–10−1 M) and rates were measured for 13X and 4A zeolites and TP-207 and TP-260 organic exchange resins in batch equilibrium and fixed-bed exchange experiments, respectively. At solutions equilibrated with CO2 at 1.0 atm (pH = 3.9), H+ exchange capacities for the materials were similar (1.7–2.4 mmol H+/g material) and resulted in pH increases from 3.9 to greater than 8.0. Multi-component mixtures using Ca2+ and Mg2+ cations (at 10−3–10−1 M) in CO2-saturated water were used to probe competitive ion exchange. The presence of divalent cations in solution inhibited H+ exchange, reducing capacities to as low as 0.2 mmol H+/g for both resins and zeolites. Dynamic H+ exchange capacities in fixed-bed ion exchange columns were similar to equilibrium values for resins (∼1.5 mmol/g) and zeolites (∼0.8 mmol/g) using inlet solutions that were equilibrated with gaseous streams of CO2 at 1.0 atm. However, exchange kinetics were limited by intraparticle diffusion as indicated by the increased rate parameters with increasing inlet flow rates (20–160 cm3 min−1). Experimental calcite precipitation from mixing the alkaline CO32−-rich water solution obtained from the ion-exchange column with a simulated liquid waste stream solution achieved thermodynamic maximum yields. The results from these studies indicate that ion exchange processes can be used as an alternative to the addition of stoichiometric bases to induce alkalinity for the precipitation of CaCO3, thereby opening a pathway toward sustainable and economic mineralization processes.

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Effect of ferrous iron on the nucleation and growth of CaCO₃in slightly basic aqueous solutions

Cited by 19 publications

References 48 publications

Effect of Operating Parameters and Foreign Ions on the Crystal Growth of Calcium Carbonate during Scale Formation: An Overview

Effect of Operating Parameters and Foreign Ions on the Crystal Growth of Calcium Carbonate during Scale Formation: An Overview

Early animal evolution and highly oxygenated seafloor niches hosted by microbial mats

Implementation of Ion Exchange Processes for Carbon Dioxide Mineralization Using Industrial Waste Streams

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Effect of ferrous iron on the nucleation and growth of CaCO3in slightly basic aqueous solutions

Cited by 19 publications

References 48 publications

Effect of Operating Parameters and Foreign Ions on the Crystal Growth of Calcium Carbonate during Scale Formation: An Overview

Effect of Operating Parameters and Foreign Ions on the Crystal Growth of Calcium Carbonate during Scale Formation: An Overview

Early animal evolution and highly oxygenated seafloor niches hosted by microbial mats

Implementation of Ion Exchange Processes for Carbon Dioxide Mineralization Using Industrial Waste Streams

Contact Info

Product

Resources

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Effect of ferrous iron on the nucleation and growth of CaCO₃in slightly basic aqueous solutions