2021
DOI: 10.37190/ppmp/139511
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On the use of Na<sub>2</sub>SO<sub>3</sub> as a pyrite depressant in saline systems and the presence of kaolinite

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Cited by 6 publications
(5 citation statements)
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“…Three main observations from this figure are (i) the zeta potential of kaolinite decrease with increasing pH in both solutions, (ii) in the presence of KCl, the isoelectric point (IEP) takes place at pH close to 6, and (iii) no significant effect on zeta potential is observed at alkaline pH values (pH > 7). At the working pH (pH = 8) in both working solutions, the typical values (−30 mV) are consistent with earlier reports, values that were reproduced by Zheng et al, among others [48,51,52].…”
Section: Effect Of Low Saline Concentration Electrolyte Over Ef Processsupporting
confidence: 92%
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“…Three main observations from this figure are (i) the zeta potential of kaolinite decrease with increasing pH in both solutions, (ii) in the presence of KCl, the isoelectric point (IEP) takes place at pH close to 6, and (iii) no significant effect on zeta potential is observed at alkaline pH values (pH > 7). At the working pH (pH = 8) in both working solutions, the typical values (−30 mV) are consistent with earlier reports, values that were reproduced by Zheng et al, among others [48,51,52].…”
Section: Effect Of Low Saline Concentration Electrolyte Over Ef Processsupporting
confidence: 92%
“…This is due to the nature of this type of ion, considered a breaker of water structures (breaker ion) [45]. On the other hand, the Na + ion promotes the hydrated layer on the kaolinite due to its tendency to generate aggregates with each other, probably negative, which promotes its tendency to stabilize in suspension in the medium [48].…”
Section: Zeta Potential Of Kaolinitementioning
confidence: 99%
“…The adjustments for copper recovery for Case 1 and Case 2 were 0.48 and 0.50, respectively (R 2 ). These results should not be surprising; in a previous study by the authors [89], similar results were obtained for the recovery of pure chalcopyrite in the presence of kaolinite and an aqueous solution of NaCl and KCl. In this case, it was not possible to represent copper recovery with a quadratic polynomial.…”
Section: Stage 2: Design and Experimentationsupporting
confidence: 84%
“…In this case, it was not possible to represent copper recovery with a quadratic polynomial. However, in a study with pure pyrite [89], it was possible to use a quadratic polynomial to adjust the recovery. In our case, for the real ore, the Fe recovery with the traditional method was not acceptable, with R 2 values of 0.54 and 0.79 for Case 1 and Case 2, respectively.…”
Section: Stage 2: Design and Experimentationmentioning
confidence: 99%
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