Next Article in Journal
Correction: Toda, K., et al. Key Factors Affecting Strength Development of Steel Slag-Dredged Soil Mixtures. Minerals 2018, 8(5), 174
Previous Article in Journal
Helium and Argon Isotopes in the Fe-Mn Polymetallic Crusts and Nodules from the South China Sea: Constraints on Their Genetic Sources and Origins
Previous Article in Special Issue
Oxidative Depression of Arsenopyrite by Using Calcium Hypochlorite and Sodium Humate
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Minerals
Volume 8
Issue 10
10.3390/min8100472
minerals-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Separation of Oxidized Pyrrhotite from Fine Fraction Serpentine

by
Jian Zhou
,
Yiping Lu
* and
Guozhi Mao
*
School of Minerals Processing and Bioengineering, Central South University, Changsha 410083, China
*
Authors to whom correspondence should be addressed.
Minerals 2018, 8(10), 472; https://doi.org/10.3390/min8100472
Submission received: 29 August 2018 / Revised: 12 October 2018 / Accepted: 19 October 2018 / Published: 22 October 2018
(This article belongs to the Special Issue Sustainable Mineral Processing Technologies)
Browse Figures
Versions Notes

Abstract

:
The valuable minerals in copper-nickel sulfide ore can easily be oxidized, leading to the reduction of their flotation recovery and a difficulty in separating them from gangue. In order to solve the problem, the reaction mechanism of the octanohydroxamic acid (OHA) on oxidized pyrrhotite was revealed through micro-flotation, adsorption tests, zeta potential measurements, and X-ray photoelectron spectroscopy (XPS) analysis. The results show that this is a feasible way to find a suitable collector that can directly react to oxidation products on the surface of pyrrhotite. OHA can efficiently reclaim oxidized pyrrhotite and achieve the selective separation of a pyrrhotite-serpentine mixture in a weak alkaline environment. The adsorption tests, zeta potential measurements, and XPS analyses show that OHA can interact with an oxidized pyrrhotite surface, and the interaction between OHA and serpentine is very weak. The XPS analyses indicate that the OHA collector can chelate with Fe(OH)3 on the surface of oxidized pyrrhotite and form an “O, O” five-ring chelate. At the same time, the OHA collector may compete with the hydroxyl groups of hydrophilic substances on the mineral surface to produce hydrophobic products and reduce the hydrophilic substances on the mineral surface.

1. Introduction

Froth flotation, a widely-used treatment of base metal sulfides, relies on the differences in surface properties between sulfide minerals and non-sulfide minerals. However, these differences become increasingly marginal as the sulfide mineral surface becomes oxidized [1,2,3,4]. Oxidation of the sulfide mineral surface is an important phenomenon, which represents one of the central issues in the flotation practice of complex sulfide ores, as the floatability of sulfide particles is controlled by the level of surface oxidation [5,6,7,8,9,10,11]. A moderate surface oxidation of sulfide minerals is known to be beneficial for the adsorption of collectors and the formation of a hydrophobic surface, i.e., slight surface oxidation can increase the floatability of sulfide minerals [6]. However, once sulfide minerals are heavily oxidized, the floatability of sulfide minerals decreases sharply, which may be mainly due to the formation of metal hydroxide species on the surface of sulfide minerals [12,13]. As a result, a collector cannot effectively collect the valuable sulfide minerals unless the dosage is significantly increased [1].
Jinchuan Nickel Mine is the largest nickel producer in China [14]. The valuable minerals in the ore of this mine are mainly pentlandite, chalcopyrite, violarite, and pyrrhotite. Pyrrhotite is a complex iron sulfide mineral that can be found in many base metal sulfide ores. It is an iron-deficient mineral with the formula Fe(1−x)S (0 < x ≤ 0.125), which results in numerous compositions with different Fe/S ratios, commonly referred to as pyrrhotite superstructures [15]. Pyrrhotite is one of the most abundant iron sulfide minerals. It is found in nature and is commonly associated with pentlandite, quartz, ankerite (CaFe(CO3)2), pyrite, chalcopyrite, and other sulfide minerals [16]. In many flotation plants, pyrrhotite is often discharged to the flotation tailings as a waste product. However, a strong interest in pyrrhotite recovery arises when pyrrhotite contains Ni, platinum group metals (PGM), and other precious metals [16,17]. In addition, pyrrhotite is also one of the most reactive sulfide minerals. It is well established that the flotation recovery of pyrrhotite is highly influenced by the level of oxidation; the oxidation of the pyrrhotite may occur during all stages of the process, from milling to flotation [18,19]. Moreover, the oxidation products, such as iron hydroxides, oxyhydroxides, and oxides, form a coating on the mineral surfaces of pyrrhotite [2], which can interfere with the flotation. Serpentine is the dominant gangue in sulfide mineral flotation and is often associated with many metal sulfide ore deposits [14,20]. The gangue can also interfere with flotation by forming a coating on the sulfide mineral surface, which has two consequences: The dilution of the concentrate when the partially coated sulfide remains floatable, and the lowering of sulfide recovery when the extensively coated sulfide becomes hydrophilic [14,21].
Xanthates are some of the most commonly used collectors for the flotation of sulfide minerals and are capable of recovering pyrrhotite well when the surface of the pyrrhotite is not oxidized in the weak alkaline environment. As the degree of oxidation of pyrrhotite increases, the ability of xanthate to collect pyrrhotite decreases sharply [5,17,22]. The time during which the samples were exposed to air, counted from the end of milling, is denoted as the exposure time (ET), and the degree of oxidation is measured by the exposure time (ET) of minerals. There is a significant decrease in the recovery of pyrrhotite using sodium butyl xanthate (SBX) as a collector when ET = 24 h [19,23]. Hydroxamic acids, R-CO-NHOH (R, alkyl/aryl group), are much weaker acids than the corresponding carboxylic acids, in the identical carbon chain, but possess stronger abilities in selectively chelating metal ions [24]. Hydroxamic acids can chelate with metal cations (e.g., Cu2+, Fe3+, Al3+) to form hydrophobic metal chelates [24,25], and the chelation reaction for hydroximic acids to metal cation can form an “O, N” four-ring chelate and/or an “O, O” five-ring chelate (the chelate products are shown in Figure 1). Since the tension of the four-ring chelate is relatively high, and the stability is poor, the chelate product is mainly a five-ring chelate.
In this paper, the Octanohydroxamic acid (OHA) was introduced as a flotation collector to solve the problem that oxidized pyrrhotite and serpentine are difficult to separate. Micro-flotation tests were performed to reveal the selective flotation of pyrrhotite by OHA. In addition, the underlying mechanism was investigated through adsorption tests, zeta potential measurements, and XPS analysis.

2. Materials and Methods

2.1. Materials

2.1.1. Minerals

The pyrrhotite specimen in this work was obtained from Tongling in the Anhui Province of China. It was handpicked to ensure a high purity specimen for this test work. The specimen was then milled in a ceramic ball mill, followed by dry sieving to extract the −74 μm size fraction used in this study. The XRD quantitative analysis showed that the purity of pyrrhotite was above 95%. The results of the elemental analysis of a pyrrhotite single mineral (mass fraction) are presented in Table 1. The serpentine was obtained from Donghai, Jiangsu Province, China, and was chosen as the gangue mineral. The particle size analysis and elemental analysis results of a serpentine single mineral (mass fraction) of serpentine are presented in Table 2 and Table 3, respectively. The artificially mixed ore was prepared by mixing pyrrhotite and serpentine samples at a weight ratio of 1:1. For Zeta potential measurements, the finer fraction (−5 μm) was used. In order to oxidize the pyrrhotite samples used in the experiment, the samples were exposed to air for 24 h (denoted as ET = 24 h), counted from the end of milling.

2.1.2. Reagents

Octanohydroxamic acid (OHA) was bought from a commercial company, and its purity was above 98%. Sodium butyl xanthate (SBX) with 93% purity was used as the collector and was obtained from Zhuzhou Flotation Reagent Company. Methyl Isobutyl Carbinol (MIBC) acts as the frother and was an industrial product. Sodium hexametaphosphate (SHMP, AR) was used as the dispersant in this study, and hydrochloric acid (HCl) and sodium hydroxide (NaOH) of analytical grade were both used as pH regulators and were added to the micro-flotation tests.

2.2. Experimental

2.2.1. Micro-Flotation Tests

Micro-flotation tests were conducted in a micro-flotation cell with a volume of 40 mL, and the contents of the cell were stirred at 1650 rpm by a four-bladed impeller. A PHS-3C acidometer, built by Shanghai Leici Company (Shanghai, China), was used to measure the pH value. The micro-flotation tests involved the following procedures: (1) Wetting the single minerals (2 g) or mineral mixture (1 g pyrrhotite plus 1 g serpentine) with 40 mL de-ionized water for 1 min; (2) adding the pH regulator for the required pH and agitating for 2 min; (3) if necessary, adding the depressant and agitating for 3 min; (4) adding the collector and agitating for 3 min; (5) after adding the frother, collecting the floating materials for 3 min; and (6) filtering the collected materials, and drying and weighing them for recovery calculation and chemical analyses. Micro-flotation tests were only used for assessing the flotation of single pure minerals and the separation of the artificial mixture of pyrrhotite-serpentine. For single mineral flotation, the flotation recovery was calculated based on the dry weight of the products obtained. For mixed minerals (the ratio of pyrrhotite and serpentine was 1:1) flotation, the flotation recovery was calculated based on S and MgO grades between the concentrates and tailings. Each flotation experiment was repeated at least three times, and the average flotation recovery value was calculated. The error of the recovery was found to be within 3.0%.
In the weakly alkaline pH range, where sulfide mineral flotation was commonly used, the serpentine surface is positively charged, and the sulfide mineral surface is negatively charged. Strong electrostatic attraction exists between the two minerals, which resulted in heterogeneous agglomeration. Heterogeneous agglomeration leads to the formation of a serpentine slime coating on the sulfide mineral surfaces and depresses the flotation of sulfide minerals [26].
In the field of mineral processing, polyphosphates have been used as depressants, which disperse agents for slimes, stabilizers for mineral suspensions, which precipitate agents for some metal ions, and as a water-softening agent. SHMP (Sodium hexametaphosphate) is one of the most important polyphosphates with these functions [27]. SHMP usually has a mean molecular weight of 12,000 to 18,000 and up to 200 PO3 units in the chain [28]. In the flotation process, it was widely used to disperse slime that might attach to valuable mineral surfaces by increasing the repulsive energy between particles. Thus, here, SHMP was chosen as the dispersant for the separation of pyrrhotite from the pyrrhotite-serpentine mixture in combination with the OHA as the collector.

2.2.2. Adsorption Studies

In this study, the collector adsorption amount on the mineral particle surface was calculated by the residual concentration method. For each adsorption test, 2 g of the mineral was added into an 80 mL conical flask with a 40 mL collector solution, which was prepared at the desired concentration. The total volume was 40 mL, and the pH value was adjusted to the desired pH. Then, the suspension in the sealed conical flask was performed with the SHZ-82A thermostatic oscillator at 298 (±1) K for 30 min. Centrifugation was used to separate the solid and liquid, with a set speed of 9000 rpm for 20 min, and the supernatant was used for the following tests. The concentration of OHA in the aqueous solutions was determined by a Shimadzu TOC-LCPH analyzer (Shimadzu, Kyoto, Japan). The equilibrium concentration of SBX in the solution was measured by UV spectrophotometry, and the value was calculated from the standard curve of SBX, which was obtained by different concentrations of SBX (absorbance at 301 nm). The adsorption of collectors was calculated by the difference between the initial and the residual concentrations of the solutions. The specific surface area of the two minerals was measured with an automatic specific surface analyzer (Monosorb, Quantachrome Corp., Boynton Beach, FL, USA). The BET surface areas of pyrrhotite and serpentine were measured at 1.26 and 1.34 m2/g, respectively.

2.2.3. Zeta Potential Measurements

The zeta potentials of pyrrhotite and serpentine samples were measured using the Coulter Delsa440sx Zeta Potential & Size Analyzer (Beckman Coulter, Inc., Brea, CA, USA). Next, 50 mg of samples (−5 μm) was added to 40 mL 0.01 mol/L KCl solutions, in the absence or presence of 5 × 10−5 mol/L OHA, after the pulp was stirred with a magnetic stirrer for 5 min. Then, the pH values were adjusted with hydrochloric or sodium hydroxide solutions and measured, and the agitated suspension was sampled to record the zeta potentials. The average value of at least three independent measurements of zeta potential was reported as the zeta potential of a point.

2.2.4. XPS Analysis

X-ray photoelectron spectroscopy (XPS) was used to detect the changes of the mineral surface, in the absence or presence of 5 × 10−4 mol/L OHA. The measurements were performed using an ESCALAB 250Xi X-ray photoelectron spectrometer, manufactured by Thermo Fisher Scientific Inc, Waltham, MA, USA. For the measurements, 2 g of the mineral sample was agitated in the flotation cell at pH 8, according to the corresponding reagent condition, for 30 min. Centrifugation was used to separate the solid and liquid, with a set speed of 9000 rpm, for 10 min. Additionally, the solid mineral, after centrifugation, was washed with ultrapure water twice, then dried in a vacuum drying oven, at a temperature of 298 K, for XPS analysis.

3. Results and Discussion

3.1. Flotation of Pyrrhotite and Serpentine with Two Collectors

The effect of pulp pH values on the flotation recovery of pyrrhotite (ET = 24 h), using OHA (OHA concentration: 4 × 10−5 mol/L) or SBX (SBX concentration: 1 × 10−3 mol/L) as collectors, was studied, and the results are shown in Figure 2. It can be seen, from Figure 2, that the favorable pH values for the recovery of pyrrhotite (using OHA as a collector) were 4–10, and pulp pH values of less than 4 or above 10 would decrease the flotation recovery of pyrrhotite. At pH 8, the pyrrhotite has a very good floatability, with a flotation recovery of above 95%. However, the flotation recovery of pyrrhotite (ET = 24 h) decreased sharply as the pH increased, using SBX as a collector. The maximum recovery of pyrrhotite was about 85% at pH 2.
The results of the micro-flotation of the single pyrrhotite (ET = 24 h) and serpentine minerals, as a function of the OHA dosage at pH 8.0, are summarized in Figure 3. It can be seen, from Figure 3a, that the flotation recovery of pyrrhotite increased rapidly with the increase in the OHA concentration. The recovery of pyrrhotite, at 4 × 10−5 mol/L OHA, was almost 90%. At the same time, in the same OHA concentration range, the recovery of fine serpentine remained low as the concentration was increased, and the maximum recovery of serpentine was only about 15%. However, as can be observed from Figure 3b, the recovery of pyrrhotite slowly increased with the increasing collector concentration and reached 68.74% at a 1 × 10−3 mol/L SBX dosage. It can be inferred from the results of the micro-flotation tests that the OHA has an excellent ability to collect the surface-oxidized pyrrhotite under a weakly alkaline condition and has a poor ability to capture the serpentine. Therefore, the OHA has good selectivity.

3.2. Separation of Pyrrhotite from Pyrrhotite–Serpentine Mixture

The single mineral flotation tests indicate a large separation window at pH 8.0. Hence, the mixed-mineral flotation tests were carried out to examine the possibility of using OHA as a collector in the flotation separation of the pyrrhotite-serpentine mixture.
The results of the chemical analysis and the recovery of the flotation of pyrrhotite-serpentine mixture concentrates (OHA concentration: 4 × 10−5 mol/L) at pH 8.0, are shown in Table 4. It can be seen from Table 4 that OHA has good selectivity when separating oxidized pyrrhotite and fine-grained serpentine by flotation; the recoveries of pyrrhotite (ET = 24 h) and serpentine at an 8 mg/L dosage of SHMP were 87.32% and 13.03%, respectively.
As the dosage of SHMP increased from 0 mg/L to 20 mg/L, the yield and recovery of pyrrhotite (ET = 24 h) increased at first and then decreased, and the maximum value of the yield and recovery of pyrrhotite (ET = 24 h) reached 50% and 87.32%, respectively. Meanwhile, the recovery of serpentine gradually decreased from 16.64% to 8.60%. Therefore, with an appropriate dosage of SHMP, the OHA can collect oxidized pyrrhotite (ET = 24 h) from a pyrrhotite-serpentine mixture very well, but its ability to collect serpentine is weak.

3.3. Adsorption Studies

The adsorbed amount of OHA (OHA concentration: 1 × 10−4 mol/L) or SBX (SBX concentration: 1 × 10−3 mol/L) on the surfaces of pyrrhotite (ET = 24 h), as a function of pH values, is shown in Figure 4. As can be seen from Figure 4, the optimum adsorption range of OHA is pH = 6–10, and pH values of less than 6 or above 10 would decrease the adsorption amount of OHA on the surface of pyrrhotite. The adsorbed amount of SBX on the surface of pyrrhotite (ET = 24 h) decreased sharply as the pH values increased.
The adsorbed amount of OHA on the surfaces of both pyrrhotite (ET = 24 h) and serpentine, as a function of the collector dosage at pH 8.0, is shown in Figure 5. The result of Figure 5 illustrated that, at pH 8.0, the adsorption amount of OHA on pyrrhotite (ET = 24 h) and serpentine both increased with the increase of the OHA concentration, and pyrrhotite (ET = 24 h) showed a high adsorption capacity, while the amount of adsorption for serpentine was consistently low.
By comparing the flotation tests, the effect of pH on the adsorption amount of the two collectors is consistent with the flotation results. The adsorbed amount of the two collectors on the surface of pyrrhotite (ET = 24 h) is quite similar within the collector concentration range of 5 × 10−5 mol/L–5 × 10−4 mol/L. However, the collector ability of OHA is much stronger than that of SBX. In addition, the adsorbed amount of OHA on the surfaces of both pyrrhotite (ET = 24 h) and serpentine became more dissimilar as the amount of OHA increased in the collector concentration range experiments at pH 8.0. The adsorption of OHA on the surfaces of both pyrrhotite (ET = 24 h) and serpentine has good selectivity.

3.4. Zeta Potential Measurements

In order to investigate the adsorption mechanism of OHA on the surfaces of the two minerals, zeta potential measurements were carried out. The zeta potentials of pyrrhotite (ET = 24 h) and serpentine, as a function of the suspension of pH values, in the absence and presence of OHA, are listed in Figure 6. As can be seen in Figure 6a, the surface zeta potential of pyrrhotite (ET = 24 h), in the absence of OHA, gradually decreased and changed from positive to negative at pH 6.5, as the pH value increased, indicating that the point of zero charge (PZC) of pyrrhotite is pH 6.5. When OHA was added, the zeta potentials of pyrrhotite (ET = 24 h) shifted, to some extent, to more negative values in the whole examined pH range. It was understandable that the zeta potential became more negative because the anionic collector, OHA, adsorbed on the surface of pyrrhotite.
It can be seen from Figure 6b that the surface zeta potential of serpentine was insensitive to the addition of OHA and remained almost the same as that without OHA. The surface zeta potential of serpentine gradually decreased and changed from positive to negative at pH 11.5, before and after the addition of OHA, as the pH value increased, indicating that the PZC of serpentine is pH 11.5. After the action of the OHA collector, the zeta potential of serpentine changed very little. It can be concluded that the anionic collector, OHA, had a slight effect on the zeta potential of serpentine.
By comparing the changes of zeta potential, before and after the interaction of pyrrhotite (ET = 24 h) and serpentine with OHA, it can be concluded that the adsorption effect of the anionic collector, OHA, on the surface of pyrrhotite (ET = 24 h) is good and on the surface of serpentine is weak. The results obtained from the zeta potential measurements are in agreement with the previous adsorption results. From the perspective of the molecular structure, in which the OHA is considered an anionic collector, it is understandable that the zeta potential became more negative, due to ionization of the anionic OHA, once the anionic collector OHA adsorbed on the surface of pyrrhotite. However, that the anionic collector OHA adsorbed on the negative surface of pyrrhotite cannot be fully explained by an electrostatic attraction, and specific adsorption or/and some chemically based compounds may be involved [27].

3.5. XPS Analysis

X-ray photoelectron spectroscopy (XPS) analysis was utilized to investigate the adsorption mechanism of OHA on pyrrhotite (ET = 24 h) and serpentine. The shift energies of valence electrons on the surfaces of pyrrhotite (ET = 24 h) and serpentine, before and after treatment with OHA (OHA concentration: 5 × 10−4 mol/L, pH = 8.0), are shown in Table 5, and the O1s and N1s spectra of pyrrhotite (ET = 24 h) and pyrrhotite (ET = 24 h) treated with OHA (OHA concentration: 5 × 10−4 mol/L, pH = 8.0) are shown in Figure 7 and Figure 8, respectively.
The binding energy of O1s and Fe2p of pyrrhotite (ET = 24 h) underwent a change of 0.15 eV and 0.18 eV after OHA treatment, respectively, which indicated that the chemical environment of Fe and O atoms experienced changes, and OHA was chemically adsorbed on the surface of pyrrhotite (ET = 24 h) [25]. However, the binding energy of the O1s of serpentine had not changed in the presence of OHA. At the same time, the binding energy of the Mg1s of serpentine had only changed by 0.04 eV, which indicated that the chemical environment of O and Mg atoms did not change.
With reference to the data from the United States National Institute of Standards and Technology (NIST) [29], the binding energy of 531.35 eV corresponds to Fe(OH)3, which indicates that a hydrophilic substance on the surface of oxidized pyrrhotite (ET = 24 h) is mainly Fe(OH)3. As can be seen from Figure 7, a new peak (529.27 eV) has been observed after OHA treatment, which may be consistent with the result, presented in Table 5, that the peak corresponding to the “O, O” five-ring chelate, in which Fe(III) chelates with OHA [24,30,31], as well as the peak area of O1s, were reduced by 20.93%, from 128,494.2 (a.u.), in the absence of OHA, to 101,602.7 (a.u.), in the presence of OHA. Thus, the OHA collector may compete with the hydroxyl groups of hydrophilic substances on the mineral surface to produce hydrophobic products and reduce the hydrophilic substances on the mineral surface (the mechanism is shown in Figure 9 [32,33]). Moreover, the Fe-OHA complexes are adsorbed onto the pyrrhotite (ET = 24 h) surface via a monodentate covalent bond between Fe3+ in the Fe-OHA complex, one O atom of the surface and two hydrogen bonds [32]. Meanwhile, a new peak (398.88 eV) was observed after OHA treatment, as shown in Figure 8, which may correspond to an “O, N” four-ring chelate [30].

4. Conclusions

This paper indicates that copper-nickel sulfide ore can easily be oxidized, and the reaction mechanism of OHA on the surface-oxidized pyrrhotite was revealed through micro-flotation, adsorption tests, zeta potential measurements, and X-ray photoelectron spectroscopy (XPS) analyses. The following conclusions can be drawn:
  • This is a feasible way to find a suitable collector that can directly react with oxidation products on the surface of pyrrhotite. OHA can efficiently reclaim oxidized pyrrhotite and achieve the selective separation of pyrrhotite-serpentine artificially mixed minerals in a weak alkaline environment.
  • Adsorption tests, zeta potential measurements, and XPS analyses show that the selective adsorption of OHA on the surface of oxidized pyrrhotite (ET = 24 h) and serpentine is obvious.
  • The XPS analyses indicate that the OHA collector can chelate with Fe(OH)3 on the surface of oxidized pyrrhotite and form an “O, O” five-membered ring, and at the same time, the OHA collector may compete with the hydroxyl groups of hydrophilic substances on the mineral surface to produce hydrophobic products and reduce the hydrophilic substances on the mineral surface.

Author Contributions

Y.L., J.Z. and G.M. conceived and designed the experiments; J.Z. and G.M. performed the experiments and analyzed the data; Y.L. and G.M. contributed the reagents and materials; and J.Z. and G.M. wrote and revised the paper.

Funding

This research is supported by the National Basic Research Program of China (973 Program) (2014CB643402).

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Yin, W.; Xue, J.; Li, D.; Sun, Q.; Yao, J.; Huang, S. Flotation of heavily oxidized pyrite in the presence of fine digenite particles. Miner. Eng. 2018, 115, 142–149. [Google Scholar] [CrossRef]
  2. Newell, A.J.H.; Bradshaw, D.J.; Harris, P.J. The effect of heavy oxidation upon flotation and potential remedies for Merensky type sulfides. Miner. Eng. 2006, 19, 675–686. [Google Scholar] [CrossRef]
  3. Xian, Y.; Wang, Y.; Wen, S.; Nie, Q.; Deng, J. Floatability and oxidation of pyrite with different spatial symmetry. Miner. Eng. 2015, 72, 94–100. [Google Scholar] [CrossRef]
  4. Ejtemaei, M.; Nguyen, A.V. Characterisation of sphalerite and pyrite surfaces activated by copper sulphate. Miner. Eng. 2017, 100, 223–232. [Google Scholar] [CrossRef]
  5. Nanthakumar, B.; Kelebek, S.; Katsabanis, P.D. Impact of oxidation on flotation of Ni–Cu sulphide ore with respect to grinding. Miner. Process. Extr. Metall. 2013, 116, 197–206. [Google Scholar] [CrossRef]
  6. Tayebi-Khorami, M.; Manlapig, E.; Forbes, E.; Edraki, M.; Bradshaw, D. Effect of surface oxidation on the flotation response of enargite in a complex ore system. Miner. Eng. 2018, 119, 149–155. [Google Scholar] [CrossRef]
  7. Peng, Y.; Zhao, S. The effect of surface oxidation of copper sulfide minerals on clay slime coating in flotation. Miner. Eng. 2011, 24, 1687–1693. [Google Scholar] [CrossRef]
  8. Jacques, S.; Greet, C.J.; Bastin, D. Oxidative weathering of a copper sulphide ore and its influence on pulp chemistry and flotation. Miner. Eng. 2016, 99, 52–59. [Google Scholar] [CrossRef] [Green Version]
  9. Fullston, D.; Fornasiero, D.; Ralston, J. Zeta potential study of the oxidation of copper sulfide minerals. Colloids Surf. A Phys. Eng. Asp. 1999, 146, 113–121. [Google Scholar] [CrossRef]
  10. Raichur, A.M.; Wang, X.H.; Parekh, B.K. Quantifying pyrite surface oxidation kinetics by contact angle measurements. Colloids Surf. A Phys. Eng. Asp. 2000, 167, 245–251. [Google Scholar] [CrossRef]
  11. Murphy, R.; Strongin, D.R. Surface reactivity of pyrite and related sulfides. Surf. Sci. Rep. 2009, 64, 1–45. [Google Scholar] [CrossRef]
  12. Mavros, P.; Matis, K.A. Innovations in Flotation Technology; Springer: Heidelberg, Germany, 1992; Volume 208, p. 538. [Google Scholar]
  13. Legrand, D.L.; Bancroft, G.M.; Nesbitt, H.W. Surface characterization of pentlandite, (Fe,Ni)9S8, by X-ray photoelectron spectroscopy. Int. J Miner. Process. 1997, 51, 217–228. [Google Scholar] [CrossRef]
  14. Feng, B.; Peng, J.; Zhang, W.; Luo, G.; Wang, H. Removal behavior of slime from pentlandite surfaces and its effect on flotation. Miner. Eng. 2018, 125, 150–154. [Google Scholar] [CrossRef]
  15. Multani, R.S.; Williams, H.; Johnson, B.; Li, R.; Waters, K.E. The effect of superstructure on the zeta potential, xanthate adsorption, and flotation response of pyrrhotite. Colloids Surf. A Phys. Eng. Asp. 2018, 551, 108–116. [Google Scholar] [CrossRef]
  16. Miller, J.D.; Li, J.; Davidtz, J.C.; Vos, F. A review of pyrrhotite flotation chemistry in the processing of PGM ores. Miner. Eng. 2005, 18, 855–865. [Google Scholar] [CrossRef]
  17. Khan, A.; Kelebek, S. Electrochemical Aspects of Pyrrhotite and Pentlandite in Relation to their Flotation with Xanthate. Part-I: Cyclic Voltammetry and Rest Potential Measurements. J. Appl. Electrochem. 2004, 34, 849–856. [Google Scholar] [CrossRef]
  18. Bunkholt, I.; Kleiv, R.A. Flotation of pyrrhotite and pyrite in saturated CaCO3 solution using a quaternary amine collector. Miner. Eng. 2015, 70, 55–63. [Google Scholar] [CrossRef]
  19. Bunkholt, I.; Kleiv, R.A. Pyrrhotite oxidation and its influence on alkaline amine flotation. Miner. Eng. 2015, 71, 65–72. [Google Scholar] [CrossRef]
  20. Zhang, C.; Liu, C.; Feng, Q.; Chen, Y. Utilization of N-carboxymethyl chitosan as selective depressants for serpentine on the flotation of pyrite. Int. J. Miner. Process. 2017, 163, 45–47. [Google Scholar] [CrossRef]
  21. Bremmell, K.E.; Fornasiero, D.; Ralston, J. Pentlandite-lizardite interactions and implications for their separation by flotation. Colloids Surf. A Phys. Eng. Asp. 2005, 252, 207–212. [Google Scholar] [CrossRef]
  22. Buswell, A.M.; Nicol, M.J. Some aspects of the electrochemistry of the flotation of pyrrhotite. J. Appl. Electrochem. 2002, 32, 1321–1329. [Google Scholar] [CrossRef]
  23. Buckley, A.N.; Woods, R. Surface composition of pentlandite under flotation-related conditions. Surf. Interface Anal. 1991, 17, 675–680. [Google Scholar] [CrossRef]
  24. Xu, H.; Zhong, H.; Tang, Q.; Wang, S.; Zhao, G.; Liu, G. A novel collector 2-ethyl-2-hexenoic hydroxamic acid: Flotation performance and adsorption mechanism to ilmenite. Appl. Surf. Sci. 2015, 353, 882–889. [Google Scholar] [CrossRef]
  25. Natarajan, R.; Sharma, J.; Nirdosh, I. Adsorption of N-hydrocinnamoyl-N-phenylhydroxylamine on pure minerals. Adsorption 2010, 16, 541–548. [Google Scholar] [CrossRef]
  26. Chen, G.; Grano, S.; Sobieraj, S.; Ralston, J. The effect of high intensity conditioning on the flotation of a nickel ore, part 2: Mechanisms. Miner. Eng. 1999, 12, 1359–1373. [Google Scholar] [CrossRef]
  27. Wu, X.Q.; Zhu, J.G. Selective flotation of cassiterite with benzohydroxamic acid. Miner. Eng. 2006, 19, 1410–1417. [Google Scholar] [CrossRef]
  28. Rashchi, F.; Finch, J.A. Polyphosphates: A review, their chemistry and application with particular reference to mineral processing. Miner. Eng. 2000, 10–11, 1019–1035. [Google Scholar] [CrossRef]
  29. Chen, Y.; Feng, Q.; Zhang, G.; Liu, D.; Liu, R. Effect of Sodium Pyrophosphate on the Reverse Flotation of Dolomite from Apatite. Minerals 2018, 8, 278. [Google Scholar] [CrossRef]
  30. Wang, P.; Qin, W.; Ren, L.; Wei, Q.; Liu, R.; Yang, C.; Zhong, S. Solution chemistry and utilization of alkyl hydroxamic acid in flotation of fine cassiterite. Trans. Nonferr. Met. Soc. China 2013, 23, 1789–1796. [Google Scholar] [CrossRef]
  31. Sreenivas, T.; Padmanabhan, N.P.H. Surface chemistry and flotation of cassiterite with alkyl hydroxamates. Colloids Surf. A Phys. Eng. Asp. 2002, 205, 47–59. [Google Scholar] [CrossRef]
  32. Tian, M.; Zhang, C.; Han, H.; Liu, R.; Gao, Z.; Chen, P.; Wang, L.; Li, Y.; Ji, B.; Hu, Y.; et al. Effects of the preassembly of benzohydroxamic acid with Fe (III) ions on its adsorption on cassiterite surface. Miner. Eng. 2018, 127, 32–41. [Google Scholar] [CrossRef]
  33. Griffith, D.M.; Szőcs, B.; Keogh, T.; Suponitsky, K.Y.; Farkas, E.; Buglyó, P.; Marmion, C.J. Suberoylanilide hydroxamic acid, a potent histone deacetylase inhibitor; its X-ray crystal structure and solid state and solution studies of its Zn(II), Ni(II), Cu(II) and Fe(III) complexes. J. Inorg. Biochem. 2011, 105, 763–769. [Google Scholar] [CrossRef] [PubMed]
Minerals 08 00472 g001 550
Figure 1. Chelate products of hydroximic acid with metal cations.
Figure 1. Chelate products of hydroximic acid with metal cations.
Minerals 08 00472 g001
Minerals 08 00472 g002 550
Figure 2. Effect of pulp pH values on the flotation of pyrrhotite (ET = 24 h).
Figure 2. Effect of pulp pH values on the flotation of pyrrhotite (ET = 24 h).
Minerals 08 00472 g002
Minerals 08 00472 g003 550
Figure 3. Effect of the collector dosage ((a): OHA, (b): SBX) on the flotation of pyrrhotite (ET = 24 h).
Figure 3. Effect of the collector dosage ((a): OHA, (b): SBX) on the flotation of pyrrhotite (ET = 24 h).
Minerals 08 00472 g003
Minerals 08 00472 g004 550
Figure 4. The adsorbed amount of the two collectors on the surfaces of pyrrhotite (ET = 24 h), as a function of pH values (octanohydroxamic acid (OHA) concentration: 1 × 10−4 mol/L, SBX concentration: 1 × 10−3 mol/L).
Figure 4. The adsorbed amount of the two collectors on the surfaces of pyrrhotite (ET = 24 h), as a function of pH values (octanohydroxamic acid (OHA) concentration: 1 × 10−4 mol/L, SBX concentration: 1 × 10−3 mol/L).
Minerals 08 00472 g004
Minerals 08 00472 g005 550
Figure 5. The adsorbed amount of the two collectors on the surfaces of pyrrhotite (ET = 24 h), as a function of the collector dosage (pH = 8.0).
Figure 5. The adsorbed amount of the two collectors on the surfaces of pyrrhotite (ET = 24 h), as a function of the collector dosage (pH = 8.0).
Minerals 08 00472 g005
Minerals 08 00472 g006 550
Figure 6. Effect of OHA on the zeta potentials of pyrrhotite (a) and serpentine (b).
Figure 6. Effect of OHA on the zeta potentials of pyrrhotite (a) and serpentine (b).
Minerals 08 00472 g006
Minerals 08 00472 g007 550
Figure 7. O1s narrow region scan of (a) pyrrhotite (ET = 24 h) and (b) pyrrhotite (ET = 24 h) treated with OHA (OHA concentration: 5 × 10−4 mol/L, pH = 8.0).
Figure 7. O1s narrow region scan of (a) pyrrhotite (ET = 24 h) and (b) pyrrhotite (ET = 24 h) treated with OHA (OHA concentration: 5 × 10−4 mol/L, pH = 8.0).
Minerals 08 00472 g007
Minerals 08 00472 g008 550
Figure 8. N1s narrow region scan of (a) OHA and (b) pyrrhotite (ET = 24 h) treated with OHA (OHA concentration: 5 × 10−4 mol/L, pH = 8.0).
Figure 8. N1s narrow region scan of (a) OHA and (b) pyrrhotite (ET = 24 h) treated with OHA (OHA concentration: 5 × 10−4 mol/L, pH = 8.0).
Minerals 08 00472 g008
Minerals 08 00472 g009 550
Figure 9. The reaction mechanism of OHA with iron (III) hydroxide on the oxidized pyrrhotite surface.
Figure 9. The reaction mechanism of OHA with iron (III) hydroxide on the oxidized pyrrhotite surface.
Minerals 08 00472 g009
Table
Table 1. Chemical compositions of the pyrrhotite single mineral (mass fraction/%).
Table 1. Chemical compositions of the pyrrhotite single mineral (mass fraction/%).
TFeSPSiO2MgOCaOCu
58.6839.340.0010.410.050.210.06
Table
Table 2. The particle size analysis of serpentine (μm).
Table 2. The particle size analysis of serpentine (μm).
Sampled10d50d90Average Size
Serpentine1.7115.1048.7320.70
Table
Table 3. Chemical compositions of the serpentine single mineral (mass fraction/%).
Table 3. Chemical compositions of the serpentine single mineral (mass fraction/%).
MgOSiO2Fe2O3NiOAl2O3CaOK2OOthers
32.9237.107.390.370.800.210.0621.15
Table
Table 4. Results of the chemical analysis and the recovery of artificially mixed minerals.
Table 4. Results of the chemical analysis and the recovery of artificially mixed minerals.
NumberSHMP (mg/L)Yield (%)S grade (%)MgO Grade (%)Recovery of Pyrrhotite (%)Recovery of Serpentine (%)
1048.5131.275.9977.1216.64
2550.0033.495.3485.1315.29
3849.4734.724.6087.3213.03
41048.4334.954.1086.0511.37
51544.4435.294.0179.7310.21
62041.0235.913.6674.958.60
Table
Table 5. The shift energies of valence electrons on the surfaces of pyrrhotite (ET = 24 h) and serpentine, before and after treatment with OHA (Binding Energy/ΔE: eV).
Table 5. The shift energies of valence electrons on the surfaces of pyrrhotite (ET = 24 h) and serpentine, before and after treatment with OHA (Binding Energy/ΔE: eV).
Electronic Orbital PyrrhotiteSerpentinePyrrhotite + OHASerpentine + OHA
Binding EnergyBinding EnergyBinding Energy ΔEBinding Energy ΔE
C1s284.80284.80284.80
0		284.80
0
O1s531.50531.41531.35
0.15		531.41
0
Fe2p710.68-710.50
0.18		-
Mg1s-1303.00-1303.04
0.04

Share and Cite

MDPI and ACS Style

Zhou, J.; Lu, Y.; Mao, G. Separation of Oxidized Pyrrhotite from Fine Fraction Serpentine. Minerals 2018, 8, 472. https://doi.org/10.3390/min8100472

AMA Style

Zhou J, Lu Y, Mao G. Separation of Oxidized Pyrrhotite from Fine Fraction Serpentine. Minerals. 2018; 8(10):472. https://doi.org/10.3390/min8100472

Chicago/Turabian Style

Zhou, Jian, Yiping Lu, and Guozhi Mao. 2018. "Separation of Oxidized Pyrrhotite from Fine Fraction Serpentine" Minerals 8, no. 10: 472. https://doi.org/10.3390/min8100472

APA Style

Zhou, J., Lu, Y., & Mao, G. (2018). Separation of Oxidized Pyrrhotite from Fine Fraction Serpentine. Minerals, 8(10), 472. https://doi.org/10.3390/min8100472

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop