Assessing the effect of on scale formation–bulk precipitation and surface deposition

Chen, Tao; Neville, Anne; Yuan, Mingdong

doi:10.1016/j.jcrysgro.2004.11.169

Cited by 112 publications

(81 citation statements)

References 18 publications

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“…Calcite did not appear during the experiments (Table 1), although it is the most stable CaCO 3 polymorph. Both the nucleation and the growth of calcite were inhibited by the presence of Mg 2+ in the solution (Chen et al, 2004). Because synthesized MHC contains a small amount of magnesium, the amount of magnesium present in MHC will be released to the solution during the dissolution of MHC.…”

Section: Resultsmentioning

confidence: 99%

Transformation kinetics of monohydrocalcite to aragonite in aqueous solutions

Munemoto

Fukushi

2008

Journal of Mineralogical and Petrological Sciences

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Monohydrocalcite (CaCO 3 ·H 2 O; MHC) is a rare mineral in geological settings. It is metastable with respect to calcite and aragonite. This metastability of MHC is considered to make it a rare mineral in geological settings. Alteration experiments of MHC in aqueous solutions in a closed system were conducted at temperatures between 10 and 50 °C in order to measure its metastability quantitatively. In the present study, monohydrocalcite transformed to aragonite with time. There are two rate -limiting steps in the transformation of monohydrocalcite to aragonite: the nucleation and crystal growth of aragonite. On the other hand, the dissolution of monohydrocalcite is a faster process than the nucleation and crystal growth of aragonite. The amounts of aragonite were calculated from the X -ray diffraction (XRD) intensity to evaluate the rate of both the processes at different temperatures. The induction times for the nucleation of aragonite were estimated to be 2.7 ± 0.9×10 , and 1.6 ± 0.3×10 -6 mmol·s -1 at 10, 25, 40, and 50 °C, respectively. From Arrhenius plots, the apparent activation energies were estimated to be 108.1 kJ·mol -1 and 80.7 kJ·mol -1 for the nucleation and crystal growth steps, respectively.

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Section: Resultsmentioning

confidence: 99%

Transformation kinetics of monohydrocalcite to aragonite in aqueous solutions

Munemoto

Fukushi

2008

Journal of Mineralogical and Petrological Sciences

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“…13 The scaling tendency for a given solution can be quantified by its saturation ratio (SR) which is the excess of the actual concentration of dissolved ions over the solubility product. [14][15][16][17] In many laboratory tests, the saturation ratio decreases with time as a result of reduction in ionic species as scale formation proceed, thereby making the development of a suitable surface kinetic model very difficult. To be able to predict scaling kinetics accurately, it is necessary to be able to quantify scaling as a function of the saturation ratio which should remain fairly constant at one point in the system.…”

Section: Introductionmentioning

confidence: 99%

Development of a novel once-through flow visualization technique for kinetic study of bulk and surface scaling

Sanni

Bukuaghangin

Huggan

et al. 2017

Review of Scientific Instruments

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There is a considerable interest to investigate surface crystallization in order to have a full mechanistic understanding of how layers of sparingly soluble salts (scale) build on component surfaces. Despite much recent attention, a suitable methodology to improve on the understanding of the precipitation/deposition systems to enable the construction of an accurate surface deposition kinetic model is still needed. In this work, an experimental flow rig and associated methodology to study mineral scale deposition is developed. The once-through flow rig allows us to follow mineral scale precipitation and surface deposition in situ and in real time. The rig enables us to assess the effects of various parameters such as brine chemistry and scaling indices, temperature, flow rates, and scale inhibitor concentrations on scaling kinetics. Calcium carbonate (CaCO3) scaling at different values of the saturation ratio (SR) is evaluated using image analysis procedures that enable the assessment of surface coverage, nucleation, and growth of the particles with time. The result for turbidity values measured in the flow cell is zero for all the SR considered. The residence time from the mixing point to the sample is shorter than the induction time for bulk precipitation; therefore, there are no crystals in the bulk solution as the flow passes through the sample. The study shows that surface scaling is not always a result of pre-precipitated crystals in the bulk solution. The technique enables both precipitation and surface deposition of scale to be decoupled and for the surface deposition process to be studied in real time and assessed under constant condition.

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“…This is in contrast to the ROSA modelling which is based on equilibrium solubility data alone, which showed an LSI of 4.8 for the concentrate, which is conducive for precipitation [21]. This may be attributable to the large quantities of magnesium present, which can act as a powerful inhibitor of calcium carbonate precipitation [22]. The magnesium concentration (Figure 2c) also does not deviate from the noprecipitation line at water recoveries less than 80%.…”

Section: Scaling Potential Of Rocmentioning

confidence: 59%

Silica scale mitigation for high recovery reverse osmosis of groundwater for a mining process

Sartipy

Milne

Taylor³

et al. 2014

Desalination

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Abstract:The feasibility of silica removal in RO treatment of groundwater from a Western Australian mining and processing operation to prevent scaling and enhance water recovery was investigated. This study has shown that it is possible to decrease the silica concentration in RO concentrate to levels that would allow an overall water recovery of 90% to 95% using 10 g/L of regenerable activated alumina adsorbent. Regeneration of the adsorbent using 2% NaOH was found to be effective for at least three regeneration cycles. A preliminary costing of the high water recovery RO process using silica removal by adsorption indicated product water (permeate) costs of $5.6/kL and savings due to a reduction in brine volume from the current 40% of feed volume to 5-10% of feed volume. It also allows better utilization of a scarce groundwater resource, allowing the production of up to 1.6 times more low salt water from a given volume of groundwater. These results warrant larger scale investigation of silica removal and adsorbent regeneration for high recovery RO processing for mining operations, and application of silica removal to RO treatment of other silica laden waters such as coal seam gas produced water.

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Assessing the effect of on scale formation–bulk precipitation and surface deposition

Cited by 112 publications

References 18 publications

Transformation kinetics of monohydrocalcite to aragonite in aqueous solutions

Transformation kinetics of monohydrocalcite to aragonite in aqueous solutions

Development of a novel once-through flow visualization technique for kinetic study of bulk and surface scaling

Silica scale mitigation for high recovery reverse osmosis of groundwater for a mining process

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