SOHIO process legacy waste treatment: Uranium recovery using ion exchange

Foster, Richard I.; Amphlett, James; Kim, Kwang‐Wook; Kerry, Timothy; Lee, Keun‐Young; Sharrad, Clint A.

doi:10.1016/j.jiec.2019.09.001

Cited by 59 publications

(19 citation statements)

References 36 publications

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“…It is noted also that similar performance was evidenced for 2 cm column tests, where the volume of ion exchange was conserved rather than the height (given in the Electronic Supplementary Materials, Figure S5), highlighting a good consistency in the scale-up parameterisation. In general, for the scale-up tests the MDR model was found to give a better fit to the collected breakthrough data compared to the Thomas model (from R 2 values in Table 1), which is a similar finding to that of other works [77,79,80], although differences between the models were minor.…”

Section: Static Column Studiessupporting

confidence: 85%

“…The fitted equilibrium adsorption capacity (qe) values were also correspondingly similar between both models, where, importantly, the qe values for caesium are considerably higher than for strontium (at 171.90 or 170.44 mg/g for caesium against 15.31 or 16.67 mg/g for strontium using the Thomas and MDR models, respectively). There is also a direct correlation between the qe values and the number of bed volumes processed to breakthrough, which is expected to follow a linear trend following previous research [9,25,29,76,77].…”

Section: Static Column Studiessupporting

confidence: 69%

“…By reducing the residence time, the breakthrough curve is shifted to lower bed volumes, where the 50% breakthrough point (Ce/C0 = 0.5) is decreased to around 100 bed volumes. Testing column residence time limits is industrially important, as obviously, reducing residence times will also increase the effluent flowrate of solution (and increase process capacity) while at the same time it will lower the contact time between the adsorbent and contaminants [29,30,77]. In this case, the contact time is far too small at 15 min for efficient material performance.…”

Section: Static Column Studiesmentioning

confidence: 99%

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Kinetic Studies of Cs+ and Sr2+ Ion Exchange Using Clinoptilolite in Static Columns and an Agitated Tubular Reactor (ATR)

et al. 2021

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Natural clinoptilolite was studied to assess its performance in removing caesium and strontium ions, using both static columns and an agitated tube reactor (ATR) for process intensification. Kinetic breakthrough curves were fitted using the Thomas and Modified Dose Response (MDR) models. In the static columns, the clinoptilolite adsorption capacity (qe) for 200 ppm ion concentrations was found to be ~171 and 16 mg/g for caesium and strontium, respectively, highlighting the poor material ability to exchange strontium. Reducing the concentration of strontium to 100 ppm, however, led to a higher strontium qe of ~48 mg/g (close to the maximum adsorption capacity). Conversely, halving the column residence time to 15 min decreased the qe for 100 ppm strontium solutions to 13–14 mg/g. All the kinetic breakthrough data correlated well with the maximum adsorption capacities found in previous batch studies, where, in particular, the influence of concentration on the slow uptake kinetics of strontium was evidenced. For the ATR studies, two column lengths were investigated (of 25 and 34 cm) with the clinoptilolite embedded directly into the agitator bar. The 34 cm-length system significantly outperformed the static vertical columns, where the adsorption capacity and breakthrough time were enhanced by ~30%, which was assumed to be due to the heightened kinetics from shear mixing. Critically, the increase in performance was achieved with a relative process flow rate over twice that of the static columns.

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Section: Static Column Studiessupporting

confidence: 85%

Section: Static Column Studiessupporting

confidence: 69%

Section: Static Column Studiesmentioning

confidence: 99%

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Kinetic Studies of Cs+ and Sr2+ Ion Exchange Using Clinoptilolite in Static Columns and an Agitated Tubular Reactor (ATR)

et al. 2021

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“…However, sorption processes have retained more attention for the treatment of low-concentration effluents. Uranium sorption was reported using biosorbents [13][14][15][16], chelating resins [17][18][19][20], and ion-exchange resins [21][22][23][24][25][26], and functionalized inorganic supports [27][28][29][30][31][32][33][34].…”

Section: Introductionmentioning

confidence: 99%

Quaternization of Composite Algal/PEI Beads for Enhanced Uranium Sorption—Application to Ore Acidic Leachate

Hamza

Mubark

Wei

et al. 2020

Gels

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The necessity to recover uranium from dilute solutions (for environmental/safety and resource management) is driving research towards developing new sorbents. This study focuses on the enhancement of U(VI) sorption properties of composite algal/Polyethylenimine beads through the quaternization of the support (by reaction with glycidyltrimethylammonium chloride). The sorbent is fully characterized by FTIR, XPS for confirming the contribution of protonated amine and quaternary ammonium groups on U(VI) binding (with possible contribution of hydroxyl and carboxyl groups, depending on the pH). The sorption properties are investigated in batch with reference to pH effect (optimum value: pH 4), uptake kinetics (equilibrium: 40 min) and sorption isotherms (maximum sorption capacity: 0.86 mmol U g−1). Metal desorption (with 0.5 M NaCl/0.5 M HCl) is highly efficient and the sorbent can be reused for five cycles with limited decrease in performance. The sorbent is successfully applied to the selective recovery of U(VI) from acidic leachate of uranium ore, after pre-treatment (cementation of copper, precipitation of rare earth elements with oxalate, and precipitation of iron). A pure yellow cake is obtained after precipitation of the eluate.

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“…The pH plays a critical role in the adsorption of UO 2 2+ as pH can affect the solution chemistry of uranium ions and the properties of the active sites of the adsorbent [31] . The adsorption of U(VI) on Duolite ES‐467 resin was examined in the pH values from 1 to 5 using 30 mL of 250 mg/L U(VI) standard solution and 0.1 g resin at room temperature (Figure 9).…”

Section: Resultsmentioning

confidence: 99%

Recovery of uranium from ferruginous Shale mineralization from Um Bogma formation, Egypt, via Duolite ES‐467 chelating resin

Radwan

Gado

El–Wahab

et al. 2021

Zeitschrift anorg allge chemie

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The ferruginous shale iron content (27.5 %) is a serious problem that prevents the separation of uranium. Chemical dissolution of the ferruginous shale from Um Bogma Formation, Egypt, has been studied for the recovery of uranium using the acidic leaching method. Um Bogma representative sample assays 700 ppm of uranium as the element of interest. The effective dissolution parameters such as acid concentrations, solid/liquid addition ratio, leaching time, and leaching temperature were planned to investigate. It was found that The dissolution rate was greatly influenced by the studied dissolution factors. Analysis of the kinetic data showed that the dissolution mechanism is fitted well to shrinking core model within chemical reaction as a rate determining step. It was found that the recorded activation energy (Ea) of uranium dissolution is 205 kJ/mol. The uranium dissolution efficiency of 95.2 % has been achieved with optimized conditions of 250 g/L H2SO4; 1 : 7 (S/L) phase ratio; 250 °C for 7 hours. Finally, the best‐controlling factors were applied for uranium separation from Um Bogma leach liquor to produce a uranium concentrate with 69.985 % uranium purity.

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SOHIO process legacy waste treatment: Uranium recovery using ion exchange

Cited by 59 publications

References 36 publications

Kinetic Studies of Cs+ and Sr2+ Ion Exchange Using Clinoptilolite in Static Columns and an Agitated Tubular Reactor (ATR)

Kinetic Studies of Cs+ and Sr2+ Ion Exchange Using Clinoptilolite in Static Columns and an Agitated Tubular Reactor (ATR)

Quaternization of Composite Algal/PEI Beads for Enhanced Uranium Sorption—Application to Ore Acidic Leachate

Recovery of uranium from ferruginous Shale mineralization from Um Bogma formation, Egypt, via Duolite ES‐467 chelating resin

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