# The Flotation Separation of Magnesite and Limonite Using an Amine Collector

Authors: Jiahong Han; Xiaoan Li; Shujuan Dai; Guozhen Liu
Journal: Adsorption Science & Technology
 (2021)

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## Abstract

In order to reduce the iron impurities in magnesite ore and improve the purity of magnesium products, the difference in floatability between magnesite and limonite has been studied by using mixtures with a collecting agent—KD (cationic amine collectors, containing soluble components). Sodium hexametaphosphate, pH, sodium silicate, and sodium carboxymethyl cellulose were used as regulators. Adsorption mechanisms of the reagents on minerals were analyzed by a zeta potential analyzer and infrared spectroscopy. Sodium silicate increased the floatability of both minerals at 11.6. All the three regulators reduced the zeta potential of both minerals, while KD increased the zeta potential of magnesite and decreased the zeta potential of limonite. All the three regulators were likely chemically adsorbed on the surface of both minerals; KD has electrostatic adsorption on the surface of the minerals.


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## Body

## 1. Introduction

Magnesite raw materials with iron impurities have a great impact on fire resistance. Iron impurities react with CaO, generating a low-melting point material, while iron oxide is reduced to the metallic iron, making refractory products in the formation of melting holes [1]. The presence of iron impurity degrades magnesite products [2]. The content of iron impurities in magnesite raw ore is low, but the existence of iron is more complicated. The observation by a polarization microscope shows that the primary iron minerals in the ore are pyrite, pyrrhotite, magnetite, and hematite and after weathering, the vast majority of iron sulfide minerals is converted into limonite with iron sulfide minerals only as a residue [3–6]. Limonite is a common impurity in magnesite ore, which is the main component of the natural mixture of ferrous oxides [7].At present, there are some reports about the technology of removing iron from magnesite at home and abroad. The iron in magnesite ore includes the iron in the raw ore and the iron impurities entrapped in the crushing process. The iron entrapped in the crushing and grinding can be partially removed by magnetic separation processes, but nonmagnetic iron and weak magnetic iron are difficult to be separated using a single magnetic separation method. The iron removal from magnesite is mainly carried out by strong magnetic separation. Besides, the content of iron is also reduced to a certain degree during the silicon removal purification of magnesite ore [8]. The DESCOS superconducting magnetic separator operating at a magnetic field intensity of 3.2 T at the Tutluca Magnesite Concentrator in Turkey processes a magnesite ore of a particle size of 100 to 4 mm with about 20% of SiO2 and 4% of Fe2O3. Dry roughing was conducted to obtain a product containing not more than 1.5% of SiO2 and not more than 0.3% of Fe2O3 [9]. Some research abroad focuses on magnetic separation of magnesite ore using magnetic seeds. At the appropriate pH level, the surfaces of serpentine and limonite are firstly modified with surfactants and the magnetic seeds are subsequently added to allow the magnetic seeds to selectively adhere to the serpentine and limonite surfaces, resulting in a large difference of magnetic susceptibility between the minerals for following magnetic separation [10]. Shenyang Aluminum and Magnesium Engineering and Research Institute conducted a beneficiation study on a low-grade magnesite ore with a TFe content of 1.20% in the Jiuquan area of Gansu Province. The iron-bearing minerals in the ore are mainly hematite, besides magnetite, limonite, and pyrite. An SHP-500 strong magnetic separator was used to remove the iron from the ore, followed by two stages of positive flotation. The resulting concentrate has a TFe content of 0.94% and a MgO content of 46.05% [11]. Mineral processing of the cryptocrystalline magnesite ore in Iran was carried out by Wuhan University of Science and Technology with an iron content of 1.05%. An XCSQ-50×70 wet magnetic separator was used to remove iron before flotation of the ore. It is shown that two stages of magnetic separation at 0.5 T reduced the iron down to 0.5% [12]. At present, most iron minerals with less magnetic susceptibilities such as limonite are strengthened to be magnetic by magnetization roasting [13–17]. Zhang et al. conducted flotation purification of magnesite with mechanism analysis [18]. The main impurities in magnesite ore were silicon, calcium, and iron. Cationic reverse flotation was usually used to remove silicon from magnesite ore; then, anion flotation was used to remove calcium and some silicon when the content of impurities was high [19]. It is necessary to remove iron during the removal of silicon by cationic reverse flotation.According to the characteristics of some high-iron magnesite resources in China, it is important to carry out a study on flotation separation and the mechanism of magnesite and limonite. Through a single-mineral flotation test, artificial mixed-mineral floating election test, potentiodynamic test, and infrared spectroscopy, the flotation behavior of magnesite and limonite and the effects of sodium hexametaphosphate, sodium silicate, and sodium carboxymethyl cellulose (CMC) on magnesite and limonite were investigated. The flotation behaviors of magnesite and limonite are analyzed. The research results are of guiding significance to the production of related enterprises, improving the comprehensive utilization of resources.


## 2. Materials and Methods

### 2.1. Material

#### 2.1.1. The Single-Magnesite Mineral

The single-magnesite sample was a stock from the mineral processing laboratory of Liaoning University of Science and Technology. After crushing, sorting, grinding (XMB−Ф200×240), and screening, the single-magnesite sample was washed and dried for experimental use at a particle size of 0.021–0.075 mm. Multielement analysis of the mineral sample is shown in Table 1, and X-ray diffraction test results are shown in Figure 1.Table 1
Chemical composition analysis of magnesite.
Chemical compositionCaOFe2O3Al2O3SiO2MgOContent (%)0.250.320.340.1947.20Figure 1
X-ray diffraction pattern of the magnesite sample.As can be seen in Table1, the single-magnesite sample contained 47.20% MgO and the MgCO3 content was 98.90%. The XRD results from Figure 1 also indicate that the major mineral is magnesite.


#### 2.1.2. The Single-Limonite Mineral

The single-limonite sample was a stock from the mineral processing laboratory of University of Science and Technology Liaoning. After crushing, sorting, grinding, and sieving, the limonite sample was washed and dried for the subsequent use with a particle size of 0.021–0.104 mm. As can be seen in Table2, the content of limonite reached more than 95%, with a small amount of other impurities, showing high purity of limonite in the sample, in good agreement with the XRF result in Figure 2.Table 2
Chemical composition analysis of limonite.
Chemical compositionFe2O3SiO2Al2O3MgOP2O5SO3TiO2Content (%)95.101.502.000.4020.130.2280.423Chemical compositionClK2OCaOMnOCuOCr2O3As2O3Content (%)0.0190.0110.0380.03770.0210.03490.0366Figure 2
X-ray diffraction pattern of the limonite sample.


#### 2.1.3. Test Methods

(1) The Flotation Test. The floatability difference between magnesite and limonite was investigated in a single-mineral flotation test using sodium hexametaphosphate, sodium silicate, and CMC as modification agents to the collector KD and by adjusting the pulp pH value with 1% HCl or 1% NaOH. The test was carried out on a 30 ml XFGC air-filled tank flotation machine, with 2 g of the mineral sample for each flotation test. In the flotation test, HCl or NaOH was added to adjust the pH value of the slurry, modification agents were added for 3 min stirring, and the collector was added for 3 min agitation before froth scraping. The single-mineral test process is shown in Figure 3. After flotation, foam products and unfloated products were filtered, dried, and weighed.Figure 3
Single-mineral flotation test flow chart.(2) The Electric Potential Test. Determination of electric potential was conducted using a JS94H-based microelectrophoresis apparatus to measure the surface potential of single minerals under different environments. The sample was ground to 5 μm or less using a ZXM-1 vibrating mill. A 250 mg sample was taken into 250 ml volumetric flask, to make the slurry. Take 30 ml pulp in a beaker, adjust the amount of each agent to be tested, and each time, place 0.5 ml liquid in the electrophoresis tank. A microelectrophoresis meter was used to measure the electrokinetic potential, each survey site was measured 5 times, and the remaining values were averaged after the number of interference was removed.(3) Infrared Spectrometry. Single minerals were tested by a certain percentage added to a certain dose of flotation reagents in aqueous solution at a varied pH value. The slurry was fully stirred and filtered, washed with distilled water, and air dried. KBr press was prepared with the appropriate proportion of KBr and minerals. The pressed tablet was placed in an infrared spectrometer (Nicolet 380 FT-IR, Thermo Electron Corporation) for measurement.(4) X-Ray Diffraction Measurement. The sample to be tested was ground to 45 μm or less and tested in an X-ray diffractometer (PW3040/60, Panalytical BV, the Netherlands) at ambient temperature. Diffraction pattern analysis was done according to the PDF2-2004 Card Version of the Joint Diffraction Data Standards Joint Commission International Diffraction Data Center (JCPDS-ICDD), and data analysis was performed using X’Pert HighScore Plus software.


## 2.1. Material

### 2.1.1. The Single-Magnesite Mineral

The single-magnesite sample was a stock from the mineral processing laboratory of Liaoning University of Science and Technology. After crushing, sorting, grinding (XMB−Ф200×240), and screening, the single-magnesite sample was washed and dried for experimental use at a particle size of 0.021–0.075 mm. Multielement analysis of the mineral sample is shown in Table 1, and X-ray diffraction test results are shown in Figure 1.Table 1
Chemical composition analysis of magnesite.
Chemical compositionCaOFe2O3Al2O3SiO2MgOContent (%)0.250.320.340.1947.20Figure 1
X-ray diffraction pattern of the magnesite sample.As can be seen in Table1, the single-magnesite sample contained 47.20% MgO and the MgCO3 content was 98.90%. The XRD results from Figure 1 also indicate that the major mineral is magnesite.


### 2.1.2. The Single-Limonite Mineral

The single-limonite sample was a stock from the mineral processing laboratory of University of Science and Technology Liaoning. After crushing, sorting, grinding, and sieving, the limonite sample was washed and dried for the subsequent use with a particle size of 0.021–0.104 mm. As can be seen in Table2, the content of limonite reached more than 95%, with a small amount of other impurities, showing high purity of limonite in the sample, in good agreement with the XRF result in Figure 2.Table 2
Chemical composition analysis of limonite.
Chemical compositionFe2O3SiO2Al2O3MgOP2O5SO3TiO2Content (%)95.101.502.000.4020.130.2280.423Chemical compositionClK2OCaOMnOCuOCr2O3As2O3Content (%)0.0190.0110.0380.03770.0210.03490.0366Figure 2
X-ray diffraction pattern of the limonite sample.


### 2.1.3. Test Methods

(1) The Flotation Test. The floatability difference between magnesite and limonite was investigated in a single-mineral flotation test using sodium hexametaphosphate, sodium silicate, and CMC as modification agents to the collector KD and by adjusting the pulp pH value with 1% HCl or 1% NaOH. The test was carried out on a 30 ml XFGC air-filled tank flotation machine, with 2 g of the mineral sample for each flotation test. In the flotation test, HCl or NaOH was added to adjust the pH value of the slurry, modification agents were added for 3 min stirring, and the collector was added for 3 min agitation before froth scraping. The single-mineral test process is shown in Figure 3. After flotation, foam products and unfloated products were filtered, dried, and weighed.Figure 3
Single-mineral flotation test flow chart.(2) The Electric Potential Test. Determination of electric potential was conducted using a JS94H-based microelectrophoresis apparatus to measure the surface potential of single minerals under different environments. The sample was ground to 5 μm or less using a ZXM-1 vibrating mill. A 250 mg sample was taken into 250 ml volumetric flask, to make the slurry. Take 30 ml pulp in a beaker, adjust the amount of each agent to be tested, and each time, place 0.5 ml liquid in the electrophoresis tank. A microelectrophoresis meter was used to measure the electrokinetic potential, each survey site was measured 5 times, and the remaining values were averaged after the number of interference was removed.(3) Infrared Spectrometry. Single minerals were tested by a certain percentage added to a certain dose of flotation reagents in aqueous solution at a varied pH value. The slurry was fully stirred and filtered, washed with distilled water, and air dried. KBr press was prepared with the appropriate proportion of KBr and minerals. The pressed tablet was placed in an infrared spectrometer (Nicolet 380 FT-IR, Thermo Electron Corporation) for measurement.(4) X-Ray Diffraction Measurement. The sample to be tested was ground to 45 μm or less and tested in an X-ray diffractometer (PW3040/60, Panalytical BV, the Netherlands) at ambient temperature. Diffraction pattern analysis was done according to the PDF2-2004 Card Version of the Joint Diffraction Data Standards Joint Commission International Diffraction Data Center (JCPDS-ICDD), and data analysis was performed using X’Pert HighScore Plus software.


## 2.1.1. The Single-Magnesite Mineral

The single-magnesite sample was a stock from the mineral processing laboratory of Liaoning University of Science and Technology. After crushing, sorting, grinding (XMB−Ф200×240), and screening, the single-magnesite sample was washed and dried for experimental use at a particle size of 0.021–0.075 mm. Multielement analysis of the mineral sample is shown in Table 1, and X-ray diffraction test results are shown in Figure 1.Table 1
Chemical composition analysis of magnesite.
Chemical compositionCaOFe2O3Al2O3SiO2MgOContent (%)0.250.320.340.1947.20Figure 1
X-ray diffraction pattern of the magnesite sample.As can be seen in Table1, the single-magnesite sample contained 47.20% MgO and the MgCO3 content was 98.90%. The XRD results from Figure 1 also indicate that the major mineral is magnesite.


## 2.1.2. The Single-Limonite Mineral

The single-limonite sample was a stock from the mineral processing laboratory of University of Science and Technology Liaoning. After crushing, sorting, grinding, and sieving, the limonite sample was washed and dried for the subsequent use with a particle size of 0.021–0.104 mm. As can be seen in Table2, the content of limonite reached more than 95%, with a small amount of other impurities, showing high purity of limonite in the sample, in good agreement with the XRF result in Figure 2.Table 2
Chemical composition analysis of limonite.
Chemical compositionFe2O3SiO2Al2O3MgOP2O5SO3TiO2Content (%)95.101.502.000.4020.130.2280.423Chemical compositionClK2OCaOMnOCuOCr2O3As2O3Content (%)0.0190.0110.0380.03770.0210.03490.0366Figure 2
X-ray diffraction pattern of the limonite sample.


## 2.1.3. Test Methods

(1) The Flotation Test. The floatability difference between magnesite and limonite was investigated in a single-mineral flotation test using sodium hexametaphosphate, sodium silicate, and CMC as modification agents to the collector KD and by adjusting the pulp pH value with 1% HCl or 1% NaOH. The test was carried out on a 30 ml XFGC air-filled tank flotation machine, with 2 g of the mineral sample for each flotation test. In the flotation test, HCl or NaOH was added to adjust the pH value of the slurry, modification agents were added for 3 min stirring, and the collector was added for 3 min agitation before froth scraping. The single-mineral test process is shown in Figure 3. After flotation, foam products and unfloated products were filtered, dried, and weighed.Figure 3
Single-mineral flotation test flow chart.(2) The Electric Potential Test. Determination of electric potential was conducted using a JS94H-based microelectrophoresis apparatus to measure the surface potential of single minerals under different environments. The sample was ground to 5 μm or less using a ZXM-1 vibrating mill. A 250 mg sample was taken into 250 ml volumetric flask, to make the slurry. Take 30 ml pulp in a beaker, adjust the amount of each agent to be tested, and each time, place 0.5 ml liquid in the electrophoresis tank. A microelectrophoresis meter was used to measure the electrokinetic potential, each survey site was measured 5 times, and the remaining values were averaged after the number of interference was removed.(3) Infrared Spectrometry. Single minerals were tested by a certain percentage added to a certain dose of flotation reagents in aqueous solution at a varied pH value. The slurry was fully stirred and filtered, washed with distilled water, and air dried. KBr press was prepared with the appropriate proportion of KBr and minerals. The pressed tablet was placed in an infrared spectrometer (Nicolet 380 FT-IR, Thermo Electron Corporation) for measurement.(4) X-Ray Diffraction Measurement. The sample to be tested was ground to 45 μm or less and tested in an X-ray diffractometer (PW3040/60, Panalytical BV, the Netherlands) at ambient temperature. Diffraction pattern analysis was done according to the PDF2-2004 Card Version of the Joint Diffraction Data Standards Joint Commission International Diffraction Data Center (JCPDS-ICDD), and data analysis was performed using X’Pert HighScore Plus software.


## 3. Results and Discussion

### 3.1. Flotation of Single Minerals Using Collector KD

#### 3.1.1. Influences of the pH Value on the Floatability of Magnesite and Limonite

The collector KD was 150 mg/l, and the pH value of pulp was adjusted. Flotation tests were carried out on single minerals of magnesite and limonite at different pH values, and the difference of the pH value of these two minerals in the system of the amine collector was studied. The test results are shown in Figure4.Figure 4
Effects of pH (a) and KD (b) on the flotation rate of magnesite and limonite.
(a)(b)As can be seen from Figure4, with the increase of the pH value, the recovery of magnesite appeared to have two peaks at pH of 5 and 11.6 at recovery rates 66.40% and 74.35%, respectively. When the pH value was 7.4, the floatation ratio of magnesite was 35.4%. While the rising rate of limonite showed a trend of initial increase and following decrease with the change of the pH value, the rising rate of limonite reached the maximum when the pH value was 7.9 and the maximum floatation ratio was 17.6%. At pH of 2.2 and 11.6, the floatation ratios were 2.35% and 3.25%, respectively, for limonite. In the KD amine collector system, the pH value influenced the floatation ratios of magnesite and limonite in the studied pH range. The flotation rate of magnesite was much higher than that of limonite. Thus, it is suggested to remove limonite by positive flotation of magnesite at the pH value of 5 or 11.6. According to the current technical process of the purification of a magnesite mine, it is reverse-positive combined flotation with the reverse flotation of silicon removal when the pH value is 5 [20, 21]. Thus, the following tests were used for flotation of iron at pH of 11.6.


#### 3.1.2. Influences of KD Dosage on the Floatability of Magnesite and Limonite

The pH value of the slurry was adjusted to 11.6 with NaOH, and the effect of the collector on the flotation effect of the two minerals was investigated. As can be seen in Figure4, with the increase of KD, the floatation ratio of magnesite increased continuously. When the KD dosage was increased to 150 mg/l, the floatation ratio of magnesite was 74.35% and that of limonite was 3.25%. When the dosage of KD was increased to 250 mg/l, the floatation ratio of magnesite reached 87.8% and the floatation ratio of limonite also increased with the increase of KD dosage at a maximum floatation ratio of only 4.55%. Considering the dosage and separation effects of flotation, at pH of 11.6 and KD dosage of 150 mg/l, the positive flotation magnesite was suggested to remove iron.


#### 3.1.3. Influence of the Adjustment Agent on the Floatability of Magnesite and Limonite

The addition of a modifier is beneficial to the effect of the collector on the mineral. In this study, the effects of sodium hexametaphosphate, sodium silicate, and CMC on the flotation of two minerals were studied in KD. The pulp pH value was adjusted to 11.6, the KD dosage was 150 mg/l, and the amounts of sodium hexametaphosphate, sodium silicate, and CMC were changed to study the effect of the flotation of the two minerals in the amine collector system. The test results are shown in Figure5.Figure 5
Effects of sodium hexametaphosphate (a), sodium silicate (b), and CMC (c) on the floatation ratios of magnesite and limonite.
(a)(b)(c)As can be seen in Figure5, with the amount of sodium hexametaphosphate being increased from 0 to 40 mg/l and then to 200 mg/l, the floatation ratio of magnesite decreased from 74.35% to 19.40% first and then slightly increased 21.90%. The floatation ratio showed a slight upward trend at first and then increased slightly. The floatation rate of limonite decreased from 3.25% to 0.05%, but the recovery of magnesite dropped more than that of limonite. The addition of sodium hexametaphosphate reduced the floatability difference between magnesite and limonite; there existed electrostatic adsorption which was not conducive to the flotation separation of two minerals, so the collector KD was not suitable for sodium hexametaphosphate as magnesite and limonite flotation-adjusting agents of the separation.With the amount of sodium silicate being increased from 0 to 150 mg/l and then increased to 250 mg/l, the floatation ratio of magnesite decreased from 74.35% to 61.65% and then to 67.85% and then decreased and finally increased slightly. The floatation rate of limonite fluctuated between 2.3% and 4.9%, with the increase of the sodium silicate content. Therefore, the addition of sodium silicate can still ensure the effective inhibition of limonite when magnesite is floated and the sodium silicate can be used as an adjusting agent for the flotation separation of two minerals.A small amount of CMC can strongly inhibit the floating rate of the magnesite; at a CMC dosage of 40 mg/l, the magma floatation ratio was only 9.45% and the limonite floatation ratio had little change with the carboxymethyl cellulose sodium being increased. The CMC dosage was 40 mg/l, and the maximum floatation ratio was 4.2%. This indicates that the addition of CMC did not reduce the floating difference between the two minerals and CMC was not a suitable adjusting agent for KD flotation of magnesite and limonite.In summary, less sodium hexametaphosphate and CMC dosage strongly inhibited the rise of magnesite. Thus, the magnesite floatation ratio was maintained at a relatively low level. Although sodium silicate also inhibited the floating of magnesite to a certain extent, its inhibitory effect was weak, with little impact on the flotation separation of these two minerals. Therefore, in the actual removal of iron from magnesite, sodium silicate was selected as an adjusting agent.


#### 3.1.4. Flotation Separation of the Artificial Mineral Mixture Using KD

In order to verify the effect of sodium silicate separation of two kinds of minerals, an artificial mixture of 2 g was made containing 99% magnesite and 1% limonite. The artificial mixed-ore grade was 0.92% iron, a test pH value of 11.6, and a KD dosage of 150 mg/l. The test results are shown in Figure6.Figure 6
Effect of sodium silicate on artificial mixed-ore test results.As can be seen in Figure6, when sodium silicate was 50 mg/l, the concentrate yield in the artificial mixed-ore was 76.97% and the iron grade was 0.33%. When the amount of sodium silicate was increased to 100 mg/l, the iron grade decreased down to 0.32%. The artificial mixed-flotation separation effect was better, showing the same trend of the two mineral floatation ratios in single-mineral flotation tests. Flotation of concentrate production decreased first, then there was a certain degree of recovery, and iron grade first declined and then tended to be stable. Compared with the single-mineral test, the floatation rate of limonite in the mixed-ore test further decreased, which is due to the preferential adsorption of KD to magnesite.


### 3.2. Reagents on the Mineral Surface Electrical Properties

#### 3.2.1. The Effect of pH on the Electrical Properties of Mineral Surfaces

Changes in mineral potential on the surface will affect the adsorption between the reagents and the mineral, thus affecting the mineral flotation separation. Studying electrical changes on the surface of minerals allows the analysis of the mechanism of action of reagents and minerals [22, 23]. Taking magnesite and limonite single minerals as research objects, the pH value was adjusted with HCl or NaOH and zeta potential of two minerals at different pH values were determined. The measurement results are shown in Figure 7.Figure 7
Magnesite and limonite zeta potential.With the increase of the pH value, the electric potential of the magnesite surface first decreased and then increased. When the pH value increased from 2.1 to 11, the electric potential of magnesite decreased from 15.05 mV to −13.91 mV. When the pH value was 6.0, the magnesite electrical potential is zero, consistent with references [24, 25]. When the medium pH is greater than the zero point of magnesite (pH=6.0), the surface of magnesite is negatively charged. When the pH is 12, the magnetization potential of magnesite is 6.68 eV and the kinetic potential starts to appear slightly, probably due to the larger ionic strength of the solution, which results in the compression of the electrical double layer on the mineral surface. It was assumed that the high ionic strength of the solution leads to the compression of the double electric layer on the surface of the mineral, thus reducing the absolute value of the electric potential on the surface of the mineral; it was also assumed that because the zero electric point of magnesium hydroxide is pH = 12.0, a number of hydroxide precipitates was generated on the surface of the mineral in the strong alkaline solution [26, 27]. The zeta potential of limonite decreases with the increase of the pH value. When the pH value increases from 2.0 to 11.9, the electromotive potential of limonite is reduced from 38.43 mV to −18.74 mV. When pH value is 7.5, the electromotive potential of limonite is zero, consistent with references [28, 29].


#### 3.2.2. The Effect of Sodium Hexametaphosphate on Electrical Properties of the Mineral Surface

The effects of adding different amounts of sodium hexametaphosphate on the zeta potential of magnesite and limonite surface were investigated. The results are shown in Figure8.Figure 8
Effect of sodium hexametaphosphate on the zeta potential of magnesite and limonite.It can be seen in Figure8 that sodium hexametaphosphate significantly reduced the zeta potential of the two minerals by electrostatic adsorption. When sodium hexametaphosphate concentration was 20 mg/l and the pH value increased from 2.0 to 11.0, the electromotive potential of magnesite reduced from −8.43 mV to −35.48 mV. When the pH was increased to 12.0, the magnetization potential of magnesite slightly increased to −25.07 mV. When the concentration of sodium hexametaphosphate was 40 mg/l and the pH was increased from 2.0 to 11, the electromotive potential of magnesite decreased from −19.28 mV to −37.48 mV and the pH value was further increased to 11.9 and the magnetron potential increased slightly to −26.87 mV. After the effect of sodium hexametaphosphate, the electric potential of magnesite in the same pH value was negative. The phosphate likely adsorbed on the magnesite surface, so that the magnesite potential dropped. The amount of sodium hexametaphosphate was further increased, the sodium potential increased further with the same tendency, and the electromotive potential decreased slightly. The electromotive potential of limonite decreased from −17.19 mV to −33.43 mV. When the concentration of sodium hexametaphosphate was 20 mg/l and the pH was increased from 2.2 to 11.2 mV, and further to a pH of 12, the limonite electromotive potential slightly increased to −25.75 mV. With an increased sodium hexametaphosphate concentration of 40 mg/l, the pH value increased from 2.2 to 11.2. The limonite electric potential decreased from −7.74 mV to −39.35 mV. When the pH value was further increased to 12, the electromotive potential of limonite increased to −28.80 mV, therefore adding a small amount of sodium hexametaphosphate could make the electromotive potential value of the two minerals in the pH range become a negative value and the greater the concentration, the greater the reduction in the electromotive potential value.


#### 3.2.3. The Effect of Sodium Silicate on the Electrical Properties of Mineral Surfaces

The effects of adding different amounts of sodium silicate on the zeta potential of magnesite and limonite were investigated. The results are shown in Figure9.Figure 9
Effect of sodium silicate dosage on the zeta potential of magnesite and limonite.As can be seen in Figure9, the addition of sodium silicate reduced the electromotive potential of magnesite by electrostatic adsorption, shifting its zero point to the left, and the greater the concentration of sodium silicate, the more the shifting to the left. When the sodium silicate dosage was 100 mg/l, the zero point of magnesite decreased from 6.0 to 4.0. When the amount of sodium silicate increased to 200 mg/l, the zero point of magnesite further decreased to 3.5. When the sodium silicate dosage was 100 mg/l, the electromotive potential value of limonite became negative within the measured pH range. With the further increase of sodium silicate, the change of electric potential becomes smaller.


#### 3.2.4. The Effect of CMC on the Electrical Properties of Mineral Surfaces

The effects of adding different amounts of CMC on the zeta potential of magnesite and limonite surface were investigated. The results are shown in Figure10.Figure 10
Effect of CMC on zeta potential of magnesite and limonite.As can be seen in Figure10, CMC significantly lowered the electric potential of magnesite by electrostatic adsorption under acidic conditions. When the CMC concentration was 20 mg/l, the magnesite magnetoelectricity potential value was negative and the increase of pH caused the electric potential value to slightly decline. In the alkaline region, the addition of CMC instead of magnetizing the electric potential value increased in carboxymethyl. The effect of CMC on the decrease of the electric potential value of limonite was also remarkable. When the CMC concentration was 20 mg/l, the electric potential value of limonite became negative.


#### 3.2.5. KD on the Electrical Properties of the Mineral Surface

The effect of adding KD with different dosages on the zeta potential of magnesite and limonite was investigated. The results are shown in Figure11.Figure 11
Effect of KD on zeta potential of magnesite and limonite.It can be seen in Figure11 that KD increased the magnetron potential of magnesite and increased with higher KD concentration. When the KD concentration was 100 mg/l, the zero point of magnesite was 6.0 to 9.0. When the KD concentration was increased to 200 mg/l, the zero point of magnesite further increased to 9.6. The electrokinetic potential of magnesite moves to positive in the pH range of 2.0–12.0, which indicated the existence of electrostatic adsorption after the interaction between KD and magnesite. The electric potential of limonite will decrease under the effect of KD, thus leading the zero electric point toward the acid zone. When the KD dosage was 100 mg/l, limonite was zero power. When the KD dosage was 200 mg/l, the zero point of limonite dropped to 3.2. With the increase of pH, the potential of limonite decreased gradually.


### 3.3. The Role of Reagents and Minerals by Infrared Spectroscopy

#### 3.3.1. Analysis of Sodium Hexametaphosphate and Mineral Adsorption by Infrared Spectroscopy

Infrared spectroscopy was used to analyze the chemisorption of minerals and chemicals [30]. A 2 g single-mineral ore sample was placed in a solution of sodium hexametaphosphate at a concentration of 50 mg/l, the pH value of the solution was adjusted to 11.6, and the solution was thoroughly stirred for 5 minutes. The mineral sample after being treated with the reagents was washed with distilled water three times, filtrated, and dried at room temperature for infrared spectroscopical analysis. The spectra of magnesite and limonite before and after interaction with sodium hexametaphosphate are shown in Figures 12 and 13, respectively.Figure 12
FTIR spectra of sodium hexametaphosphate and magnesite.Figure 13
FTIR spectra of limonite and sodium hexametaphosphate.As can be seen in Figures12 and 13, sodium hexametaphosphate shows a characteristic peak of P=O stretching vibration at 1207 cm−1 and a characteristic P−O−P at 882 cm−1. The peaks at 1095.15 cm−1 and 969.98 cm−1 were the P−O stretching vibration characteristic peaks of sodium hexametaphosphate [31]. After adding magnesite and sodium hexametaphosphate, the −OH stretching vibration absorption peak at 3351 cm−1 increased compared with that before sodium hexametaphosphate. This shows a chemical adsorption between sodium hexametaphosphate and magnesite. After the reaction of limonite and sodium hexametaphosphate, the characteristic peak of P−O−P in sodium hexametaphosphate appeared at 882 cm−1 in the spectrum and the peak of P=O stretching appeared to be at 1207 cm−1, indicating that sodium hexametaphosphate in brown chemical adsorption occurred on the surface of limonite [32].


#### 3.3.2. Analysis of Sodium Silicate and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of sodium silicate with a concentration of 200 mg/l. Hydrophilic silicas such as Si (OH)4 and SiO2(OH) 22− and acid micelles were selectively adsorbed on the mineral surface and changed its surface properties, thus changing the effect of the collector on the mineral surface. The adsorption mechanism was analyzed by infrared spectroscopy [33]. The spectra of magnesite and limonite before and after the action of sodium silicate are shown in Figures 14 and 15, respectively.Figure 14
FTIR spectra of magnesite and sodium silicate.Figure 15
FTIR spectra of limonite and sodium silicate.In Figures14 and 15, it can be seen that the asymmetric stretching vibration absorption peak of Si−O−Si appeared to be at 876 cm−1 [34] and CO32− showed a significant change in the characteristic peak at 1460 cm−1, indicating the chemical adsorption between magnesite and sodium silicate. The Si−O−Si stretching vibration peak of SiO32− in sodium silicate appeared to be at 1185 cm−1 in the limonite spectrum [35], reflecting chemisorption between sodium silicate and limonite.


#### 3.3.3. Analysis of CMC and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of CMC with a concentration of 50 mg/l. The IR spectra of CMC before and after the interaction with magnesite and limonite are shown in Figures16 and 17, respectively.Figure 16
FTIR spectra of magnesite and CMC.Figure 17
FTIR spectra of limonite and CMC.As can be seen in Figures16 and 17, the characteristic peaks in CMC appeared to be at 1372 cm−1 and 1256 cm−1 after magnesite was contacted with CMC, indicating chemical adsorption between CMC and magnesite. In the limonite and CMC system, infrared spectroscopy showed no significant difference before and after contact, indicating no chemical adsorption between CMC and limonite.


#### 3.3.4. Analysis of KD and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of KD with a concentration of 150 mg/l. The infrared spectra of magnesite and limonite before and after the action of the collector KD are shown in Figures18 and 19.Figure 18
FTIR spectra of magnesite and KD.Figure 19
FTIR spectra of limonite and KD.As can be seen in Figures18 and 19, the spectral peaks of magnesite and limonite were not displaced after the KD and no new characteristic peak was observed. However, in the single-mineral flotation test, magnesium ore had a catching effect, indicating no chemical adsorption between magnesite and KD, likely due to weak electrostatic force adsorption.


## 3.1. Flotation of Single Minerals Using Collector KD

### 3.1.1. Influences of the pH Value on the Floatability of Magnesite and Limonite

The collector KD was 150 mg/l, and the pH value of pulp was adjusted. Flotation tests were carried out on single minerals of magnesite and limonite at different pH values, and the difference of the pH value of these two minerals in the system of the amine collector was studied. The test results are shown in Figure4.Figure 4
Effects of pH (a) and KD (b) on the flotation rate of magnesite and limonite.
(a)(b)As can be seen from Figure4, with the increase of the pH value, the recovery of magnesite appeared to have two peaks at pH of 5 and 11.6 at recovery rates 66.40% and 74.35%, respectively. When the pH value was 7.4, the floatation ratio of magnesite was 35.4%. While the rising rate of limonite showed a trend of initial increase and following decrease with the change of the pH value, the rising rate of limonite reached the maximum when the pH value was 7.9 and the maximum floatation ratio was 17.6%. At pH of 2.2 and 11.6, the floatation ratios were 2.35% and 3.25%, respectively, for limonite. In the KD amine collector system, the pH value influenced the floatation ratios of magnesite and limonite in the studied pH range. The flotation rate of magnesite was much higher than that of limonite. Thus, it is suggested to remove limonite by positive flotation of magnesite at the pH value of 5 or 11.6. According to the current technical process of the purification of a magnesite mine, it is reverse-positive combined flotation with the reverse flotation of silicon removal when the pH value is 5 [20, 21]. Thus, the following tests were used for flotation of iron at pH of 11.6.


### 3.1.2. Influences of KD Dosage on the Floatability of Magnesite and Limonite

The pH value of the slurry was adjusted to 11.6 with NaOH, and the effect of the collector on the flotation effect of the two minerals was investigated. As can be seen in Figure4, with the increase of KD, the floatation ratio of magnesite increased continuously. When the KD dosage was increased to 150 mg/l, the floatation ratio of magnesite was 74.35% and that of limonite was 3.25%. When the dosage of KD was increased to 250 mg/l, the floatation ratio of magnesite reached 87.8% and the floatation ratio of limonite also increased with the increase of KD dosage at a maximum floatation ratio of only 4.55%. Considering the dosage and separation effects of flotation, at pH of 11.6 and KD dosage of 150 mg/l, the positive flotation magnesite was suggested to remove iron.


### 3.1.3. Influence of the Adjustment Agent on the Floatability of Magnesite and Limonite

The addition of a modifier is beneficial to the effect of the collector on the mineral. In this study, the effects of sodium hexametaphosphate, sodium silicate, and CMC on the flotation of two minerals were studied in KD. The pulp pH value was adjusted to 11.6, the KD dosage was 150 mg/l, and the amounts of sodium hexametaphosphate, sodium silicate, and CMC were changed to study the effect of the flotation of the two minerals in the amine collector system. The test results are shown in Figure5.Figure 5
Effects of sodium hexametaphosphate (a), sodium silicate (b), and CMC (c) on the floatation ratios of magnesite and limonite.
(a)(b)(c)As can be seen in Figure5, with the amount of sodium hexametaphosphate being increased from 0 to 40 mg/l and then to 200 mg/l, the floatation ratio of magnesite decreased from 74.35% to 19.40% first and then slightly increased 21.90%. The floatation ratio showed a slight upward trend at first and then increased slightly. The floatation rate of limonite decreased from 3.25% to 0.05%, but the recovery of magnesite dropped more than that of limonite. The addition of sodium hexametaphosphate reduced the floatability difference between magnesite and limonite; there existed electrostatic adsorption which was not conducive to the flotation separation of two minerals, so the collector KD was not suitable for sodium hexametaphosphate as magnesite and limonite flotation-adjusting agents of the separation.With the amount of sodium silicate being increased from 0 to 150 mg/l and then increased to 250 mg/l, the floatation ratio of magnesite decreased from 74.35% to 61.65% and then to 67.85% and then decreased and finally increased slightly. The floatation rate of limonite fluctuated between 2.3% and 4.9%, with the increase of the sodium silicate content. Therefore, the addition of sodium silicate can still ensure the effective inhibition of limonite when magnesite is floated and the sodium silicate can be used as an adjusting agent for the flotation separation of two minerals.A small amount of CMC can strongly inhibit the floating rate of the magnesite; at a CMC dosage of 40 mg/l, the magma floatation ratio was only 9.45% and the limonite floatation ratio had little change with the carboxymethyl cellulose sodium being increased. The CMC dosage was 40 mg/l, and the maximum floatation ratio was 4.2%. This indicates that the addition of CMC did not reduce the floating difference between the two minerals and CMC was not a suitable adjusting agent for KD flotation of magnesite and limonite.In summary, less sodium hexametaphosphate and CMC dosage strongly inhibited the rise of magnesite. Thus, the magnesite floatation ratio was maintained at a relatively low level. Although sodium silicate also inhibited the floating of magnesite to a certain extent, its inhibitory effect was weak, with little impact on the flotation separation of these two minerals. Therefore, in the actual removal of iron from magnesite, sodium silicate was selected as an adjusting agent.


### 3.1.4. Flotation Separation of the Artificial Mineral Mixture Using KD

In order to verify the effect of sodium silicate separation of two kinds of minerals, an artificial mixture of 2 g was made containing 99% magnesite and 1% limonite. The artificial mixed-ore grade was 0.92% iron, a test pH value of 11.6, and a KD dosage of 150 mg/l. The test results are shown in Figure6.Figure 6
Effect of sodium silicate on artificial mixed-ore test results.As can be seen in Figure6, when sodium silicate was 50 mg/l, the concentrate yield in the artificial mixed-ore was 76.97% and the iron grade was 0.33%. When the amount of sodium silicate was increased to 100 mg/l, the iron grade decreased down to 0.32%. The artificial mixed-flotation separation effect was better, showing the same trend of the two mineral floatation ratios in single-mineral flotation tests. Flotation of concentrate production decreased first, then there was a certain degree of recovery, and iron grade first declined and then tended to be stable. Compared with the single-mineral test, the floatation rate of limonite in the mixed-ore test further decreased, which is due to the preferential adsorption of KD to magnesite.


## 3.1.1. Influences of the pH Value on the Floatability of Magnesite and Limonite

The collector KD was 150 mg/l, and the pH value of pulp was adjusted. Flotation tests were carried out on single minerals of magnesite and limonite at different pH values, and the difference of the pH value of these two minerals in the system of the amine collector was studied. The test results are shown in Figure4.Figure 4
Effects of pH (a) and KD (b) on the flotation rate of magnesite and limonite.
(a)(b)As can be seen from Figure4, with the increase of the pH value, the recovery of magnesite appeared to have two peaks at pH of 5 and 11.6 at recovery rates 66.40% and 74.35%, respectively. When the pH value was 7.4, the floatation ratio of magnesite was 35.4%. While the rising rate of limonite showed a trend of initial increase and following decrease with the change of the pH value, the rising rate of limonite reached the maximum when the pH value was 7.9 and the maximum floatation ratio was 17.6%. At pH of 2.2 and 11.6, the floatation ratios were 2.35% and 3.25%, respectively, for limonite. In the KD amine collector system, the pH value influenced the floatation ratios of magnesite and limonite in the studied pH range. The flotation rate of magnesite was much higher than that of limonite. Thus, it is suggested to remove limonite by positive flotation of magnesite at the pH value of 5 or 11.6. According to the current technical process of the purification of a magnesite mine, it is reverse-positive combined flotation with the reverse flotation of silicon removal when the pH value is 5 [20, 21]. Thus, the following tests were used for flotation of iron at pH of 11.6.


## 3.1.2. Influences of KD Dosage on the Floatability of Magnesite and Limonite

The pH value of the slurry was adjusted to 11.6 with NaOH, and the effect of the collector on the flotation effect of the two minerals was investigated. As can be seen in Figure4, with the increase of KD, the floatation ratio of magnesite increased continuously. When the KD dosage was increased to 150 mg/l, the floatation ratio of magnesite was 74.35% and that of limonite was 3.25%. When the dosage of KD was increased to 250 mg/l, the floatation ratio of magnesite reached 87.8% and the floatation ratio of limonite also increased with the increase of KD dosage at a maximum floatation ratio of only 4.55%. Considering the dosage and separation effects of flotation, at pH of 11.6 and KD dosage of 150 mg/l, the positive flotation magnesite was suggested to remove iron.


## 3.1.3. Influence of the Adjustment Agent on the Floatability of Magnesite and Limonite

The addition of a modifier is beneficial to the effect of the collector on the mineral. In this study, the effects of sodium hexametaphosphate, sodium silicate, and CMC on the flotation of two minerals were studied in KD. The pulp pH value was adjusted to 11.6, the KD dosage was 150 mg/l, and the amounts of sodium hexametaphosphate, sodium silicate, and CMC were changed to study the effect of the flotation of the two minerals in the amine collector system. The test results are shown in Figure5.Figure 5
Effects of sodium hexametaphosphate (a), sodium silicate (b), and CMC (c) on the floatation ratios of magnesite and limonite.
(a)(b)(c)As can be seen in Figure5, with the amount of sodium hexametaphosphate being increased from 0 to 40 mg/l and then to 200 mg/l, the floatation ratio of magnesite decreased from 74.35% to 19.40% first and then slightly increased 21.90%. The floatation ratio showed a slight upward trend at first and then increased slightly. The floatation rate of limonite decreased from 3.25% to 0.05%, but the recovery of magnesite dropped more than that of limonite. The addition of sodium hexametaphosphate reduced the floatability difference between magnesite and limonite; there existed electrostatic adsorption which was not conducive to the flotation separation of two minerals, so the collector KD was not suitable for sodium hexametaphosphate as magnesite and limonite flotation-adjusting agents of the separation.With the amount of sodium silicate being increased from 0 to 150 mg/l and then increased to 250 mg/l, the floatation ratio of magnesite decreased from 74.35% to 61.65% and then to 67.85% and then decreased and finally increased slightly. The floatation rate of limonite fluctuated between 2.3% and 4.9%, with the increase of the sodium silicate content. Therefore, the addition of sodium silicate can still ensure the effective inhibition of limonite when magnesite is floated and the sodium silicate can be used as an adjusting agent for the flotation separation of two minerals.A small amount of CMC can strongly inhibit the floating rate of the magnesite; at a CMC dosage of 40 mg/l, the magma floatation ratio was only 9.45% and the limonite floatation ratio had little change with the carboxymethyl cellulose sodium being increased. The CMC dosage was 40 mg/l, and the maximum floatation ratio was 4.2%. This indicates that the addition of CMC did not reduce the floating difference between the two minerals and CMC was not a suitable adjusting agent for KD flotation of magnesite and limonite.In summary, less sodium hexametaphosphate and CMC dosage strongly inhibited the rise of magnesite. Thus, the magnesite floatation ratio was maintained at a relatively low level. Although sodium silicate also inhibited the floating of magnesite to a certain extent, its inhibitory effect was weak, with little impact on the flotation separation of these two minerals. Therefore, in the actual removal of iron from magnesite, sodium silicate was selected as an adjusting agent.


## 3.1.4. Flotation Separation of the Artificial Mineral Mixture Using KD

In order to verify the effect of sodium silicate separation of two kinds of minerals, an artificial mixture of 2 g was made containing 99% magnesite and 1% limonite. The artificial mixed-ore grade was 0.92% iron, a test pH value of 11.6, and a KD dosage of 150 mg/l. The test results are shown in Figure6.Figure 6
Effect of sodium silicate on artificial mixed-ore test results.As can be seen in Figure6, when sodium silicate was 50 mg/l, the concentrate yield in the artificial mixed-ore was 76.97% and the iron grade was 0.33%. When the amount of sodium silicate was increased to 100 mg/l, the iron grade decreased down to 0.32%. The artificial mixed-flotation separation effect was better, showing the same trend of the two mineral floatation ratios in single-mineral flotation tests. Flotation of concentrate production decreased first, then there was a certain degree of recovery, and iron grade first declined and then tended to be stable. Compared with the single-mineral test, the floatation rate of limonite in the mixed-ore test further decreased, which is due to the preferential adsorption of KD to magnesite.


## 3.2. Reagents on the Mineral Surface Electrical Properties

### 3.2.1. The Effect of pH on the Electrical Properties of Mineral Surfaces

Changes in mineral potential on the surface will affect the adsorption between the reagents and the mineral, thus affecting the mineral flotation separation. Studying electrical changes on the surface of minerals allows the analysis of the mechanism of action of reagents and minerals [22, 23]. Taking magnesite and limonite single minerals as research objects, the pH value was adjusted with HCl or NaOH and zeta potential of two minerals at different pH values were determined. The measurement results are shown in Figure 7.Figure 7
Magnesite and limonite zeta potential.With the increase of the pH value, the electric potential of the magnesite surface first decreased and then increased. When the pH value increased from 2.1 to 11, the electric potential of magnesite decreased from 15.05 mV to −13.91 mV. When the pH value was 6.0, the magnesite electrical potential is zero, consistent with references [24, 25]. When the medium pH is greater than the zero point of magnesite (pH=6.0), the surface of magnesite is negatively charged. When the pH is 12, the magnetization potential of magnesite is 6.68 eV and the kinetic potential starts to appear slightly, probably due to the larger ionic strength of the solution, which results in the compression of the electrical double layer on the mineral surface. It was assumed that the high ionic strength of the solution leads to the compression of the double electric layer on the surface of the mineral, thus reducing the absolute value of the electric potential on the surface of the mineral; it was also assumed that because the zero electric point of magnesium hydroxide is pH = 12.0, a number of hydroxide precipitates was generated on the surface of the mineral in the strong alkaline solution [26, 27]. The zeta potential of limonite decreases with the increase of the pH value. When the pH value increases from 2.0 to 11.9, the electromotive potential of limonite is reduced from 38.43 mV to −18.74 mV. When pH value is 7.5, the electromotive potential of limonite is zero, consistent with references [28, 29].


### 3.2.2. The Effect of Sodium Hexametaphosphate on Electrical Properties of the Mineral Surface

The effects of adding different amounts of sodium hexametaphosphate on the zeta potential of magnesite and limonite surface were investigated. The results are shown in Figure8.Figure 8
Effect of sodium hexametaphosphate on the zeta potential of magnesite and limonite.It can be seen in Figure8 that sodium hexametaphosphate significantly reduced the zeta potential of the two minerals by electrostatic adsorption. When sodium hexametaphosphate concentration was 20 mg/l and the pH value increased from 2.0 to 11.0, the electromotive potential of magnesite reduced from −8.43 mV to −35.48 mV. When the pH was increased to 12.0, the magnetization potential of magnesite slightly increased to −25.07 mV. When the concentration of sodium hexametaphosphate was 40 mg/l and the pH was increased from 2.0 to 11, the electromotive potential of magnesite decreased from −19.28 mV to −37.48 mV and the pH value was further increased to 11.9 and the magnetron potential increased slightly to −26.87 mV. After the effect of sodium hexametaphosphate, the electric potential of magnesite in the same pH value was negative. The phosphate likely adsorbed on the magnesite surface, so that the magnesite potential dropped. The amount of sodium hexametaphosphate was further increased, the sodium potential increased further with the same tendency, and the electromotive potential decreased slightly. The electromotive potential of limonite decreased from −17.19 mV to −33.43 mV. When the concentration of sodium hexametaphosphate was 20 mg/l and the pH was increased from 2.2 to 11.2 mV, and further to a pH of 12, the limonite electromotive potential slightly increased to −25.75 mV. With an increased sodium hexametaphosphate concentration of 40 mg/l, the pH value increased from 2.2 to 11.2. The limonite electric potential decreased from −7.74 mV to −39.35 mV. When the pH value was further increased to 12, the electromotive potential of limonite increased to −28.80 mV, therefore adding a small amount of sodium hexametaphosphate could make the electromotive potential value of the two minerals in the pH range become a negative value and the greater the concentration, the greater the reduction in the electromotive potential value.


### 3.2.3. The Effect of Sodium Silicate on the Electrical Properties of Mineral Surfaces

The effects of adding different amounts of sodium silicate on the zeta potential of magnesite and limonite were investigated. The results are shown in Figure9.Figure 9
Effect of sodium silicate dosage on the zeta potential of magnesite and limonite.As can be seen in Figure9, the addition of sodium silicate reduced the electromotive potential of magnesite by electrostatic adsorption, shifting its zero point to the left, and the greater the concentration of sodium silicate, the more the shifting to the left. When the sodium silicate dosage was 100 mg/l, the zero point of magnesite decreased from 6.0 to 4.0. When the amount of sodium silicate increased to 200 mg/l, the zero point of magnesite further decreased to 3.5. When the sodium silicate dosage was 100 mg/l, the electromotive potential value of limonite became negative within the measured pH range. With the further increase of sodium silicate, the change of electric potential becomes smaller.


### 3.2.4. The Effect of CMC on the Electrical Properties of Mineral Surfaces

The effects of adding different amounts of CMC on the zeta potential of magnesite and limonite surface were investigated. The results are shown in Figure10.Figure 10
Effect of CMC on zeta potential of magnesite and limonite.As can be seen in Figure10, CMC significantly lowered the electric potential of magnesite by electrostatic adsorption under acidic conditions. When the CMC concentration was 20 mg/l, the magnesite magnetoelectricity potential value was negative and the increase of pH caused the electric potential value to slightly decline. In the alkaline region, the addition of CMC instead of magnetizing the electric potential value increased in carboxymethyl. The effect of CMC on the decrease of the electric potential value of limonite was also remarkable. When the CMC concentration was 20 mg/l, the electric potential value of limonite became negative.


### 3.2.5. KD on the Electrical Properties of the Mineral Surface

The effect of adding KD with different dosages on the zeta potential of magnesite and limonite was investigated. The results are shown in Figure11.Figure 11
Effect of KD on zeta potential of magnesite and limonite.It can be seen in Figure11 that KD increased the magnetron potential of magnesite and increased with higher KD concentration. When the KD concentration was 100 mg/l, the zero point of magnesite was 6.0 to 9.0. When the KD concentration was increased to 200 mg/l, the zero point of magnesite further increased to 9.6. The electrokinetic potential of magnesite moves to positive in the pH range of 2.0–12.0, which indicated the existence of electrostatic adsorption after the interaction between KD and magnesite. The electric potential of limonite will decrease under the effect of KD, thus leading the zero electric point toward the acid zone. When the KD dosage was 100 mg/l, limonite was zero power. When the KD dosage was 200 mg/l, the zero point of limonite dropped to 3.2. With the increase of pH, the potential of limonite decreased gradually.


## 3.2.1. The Effect of pH on the Electrical Properties of Mineral Surfaces

Changes in mineral potential on the surface will affect the adsorption between the reagents and the mineral, thus affecting the mineral flotation separation. Studying electrical changes on the surface of minerals allows the analysis of the mechanism of action of reagents and minerals [22, 23]. Taking magnesite and limonite single minerals as research objects, the pH value was adjusted with HCl or NaOH and zeta potential of two minerals at different pH values were determined. The measurement results are shown in Figure 7.Figure 7
Magnesite and limonite zeta potential.With the increase of the pH value, the electric potential of the magnesite surface first decreased and then increased. When the pH value increased from 2.1 to 11, the electric potential of magnesite decreased from 15.05 mV to −13.91 mV. When the pH value was 6.0, the magnesite electrical potential is zero, consistent with references [24, 25]. When the medium pH is greater than the zero point of magnesite (pH=6.0), the surface of magnesite is negatively charged. When the pH is 12, the magnetization potential of magnesite is 6.68 eV and the kinetic potential starts to appear slightly, probably due to the larger ionic strength of the solution, which results in the compression of the electrical double layer on the mineral surface. It was assumed that the high ionic strength of the solution leads to the compression of the double electric layer on the surface of the mineral, thus reducing the absolute value of the electric potential on the surface of the mineral; it was also assumed that because the zero electric point of magnesium hydroxide is pH = 12.0, a number of hydroxide precipitates was generated on the surface of the mineral in the strong alkaline solution [26, 27]. The zeta potential of limonite decreases with the increase of the pH value. When the pH value increases from 2.0 to 11.9, the electromotive potential of limonite is reduced from 38.43 mV to −18.74 mV. When pH value is 7.5, the electromotive potential of limonite is zero, consistent with references [28, 29].


## 3.2.2. The Effect of Sodium Hexametaphosphate on Electrical Properties of the Mineral Surface

The effects of adding different amounts of sodium hexametaphosphate on the zeta potential of magnesite and limonite surface were investigated. The results are shown in Figure8.Figure 8
Effect of sodium hexametaphosphate on the zeta potential of magnesite and limonite.It can be seen in Figure8 that sodium hexametaphosphate significantly reduced the zeta potential of the two minerals by electrostatic adsorption. When sodium hexametaphosphate concentration was 20 mg/l and the pH value increased from 2.0 to 11.0, the electromotive potential of magnesite reduced from −8.43 mV to −35.48 mV. When the pH was increased to 12.0, the magnetization potential of magnesite slightly increased to −25.07 mV. When the concentration of sodium hexametaphosphate was 40 mg/l and the pH was increased from 2.0 to 11, the electromotive potential of magnesite decreased from −19.28 mV to −37.48 mV and the pH value was further increased to 11.9 and the magnetron potential increased slightly to −26.87 mV. After the effect of sodium hexametaphosphate, the electric potential of magnesite in the same pH value was negative. The phosphate likely adsorbed on the magnesite surface, so that the magnesite potential dropped. The amount of sodium hexametaphosphate was further increased, the sodium potential increased further with the same tendency, and the electromotive potential decreased slightly. The electromotive potential of limonite decreased from −17.19 mV to −33.43 mV. When the concentration of sodium hexametaphosphate was 20 mg/l and the pH was increased from 2.2 to 11.2 mV, and further to a pH of 12, the limonite electromotive potential slightly increased to −25.75 mV. With an increased sodium hexametaphosphate concentration of 40 mg/l, the pH value increased from 2.2 to 11.2. The limonite electric potential decreased from −7.74 mV to −39.35 mV. When the pH value was further increased to 12, the electromotive potential of limonite increased to −28.80 mV, therefore adding a small amount of sodium hexametaphosphate could make the electromotive potential value of the two minerals in the pH range become a negative value and the greater the concentration, the greater the reduction in the electromotive potential value.


## 3.2.3. The Effect of Sodium Silicate on the Electrical Properties of Mineral Surfaces

The effects of adding different amounts of sodium silicate on the zeta potential of magnesite and limonite were investigated. The results are shown in Figure9.Figure 9
Effect of sodium silicate dosage on the zeta potential of magnesite and limonite.As can be seen in Figure9, the addition of sodium silicate reduced the electromotive potential of magnesite by electrostatic adsorption, shifting its zero point to the left, and the greater the concentration of sodium silicate, the more the shifting to the left. When the sodium silicate dosage was 100 mg/l, the zero point of magnesite decreased from 6.0 to 4.0. When the amount of sodium silicate increased to 200 mg/l, the zero point of magnesite further decreased to 3.5. When the sodium silicate dosage was 100 mg/l, the electromotive potential value of limonite became negative within the measured pH range. With the further increase of sodium silicate, the change of electric potential becomes smaller.


## 3.2.4. The Effect of CMC on the Electrical Properties of Mineral Surfaces

The effects of adding different amounts of CMC on the zeta potential of magnesite and limonite surface were investigated. The results are shown in Figure10.Figure 10
Effect of CMC on zeta potential of magnesite and limonite.As can be seen in Figure10, CMC significantly lowered the electric potential of magnesite by electrostatic adsorption under acidic conditions. When the CMC concentration was 20 mg/l, the magnesite magnetoelectricity potential value was negative and the increase of pH caused the electric potential value to slightly decline. In the alkaline region, the addition of CMC instead of magnetizing the electric potential value increased in carboxymethyl. The effect of CMC on the decrease of the electric potential value of limonite was also remarkable. When the CMC concentration was 20 mg/l, the electric potential value of limonite became negative.


## 3.2.5. KD on the Electrical Properties of the Mineral Surface

The effect of adding KD with different dosages on the zeta potential of magnesite and limonite was investigated. The results are shown in Figure11.Figure 11
Effect of KD on zeta potential of magnesite and limonite.It can be seen in Figure11 that KD increased the magnetron potential of magnesite and increased with higher KD concentration. When the KD concentration was 100 mg/l, the zero point of magnesite was 6.0 to 9.0. When the KD concentration was increased to 200 mg/l, the zero point of magnesite further increased to 9.6. The electrokinetic potential of magnesite moves to positive in the pH range of 2.0–12.0, which indicated the existence of electrostatic adsorption after the interaction between KD and magnesite. The electric potential of limonite will decrease under the effect of KD, thus leading the zero electric point toward the acid zone. When the KD dosage was 100 mg/l, limonite was zero power. When the KD dosage was 200 mg/l, the zero point of limonite dropped to 3.2. With the increase of pH, the potential of limonite decreased gradually.


## 3.3. The Role of Reagents and Minerals by Infrared Spectroscopy

### 3.3.1. Analysis of Sodium Hexametaphosphate and Mineral Adsorption by Infrared Spectroscopy

Infrared spectroscopy was used to analyze the chemisorption of minerals and chemicals [30]. A 2 g single-mineral ore sample was placed in a solution of sodium hexametaphosphate at a concentration of 50 mg/l, the pH value of the solution was adjusted to 11.6, and the solution was thoroughly stirred for 5 minutes. The mineral sample after being treated with the reagents was washed with distilled water three times, filtrated, and dried at room temperature for infrared spectroscopical analysis. The spectra of magnesite and limonite before and after interaction with sodium hexametaphosphate are shown in Figures 12 and 13, respectively.Figure 12
FTIR spectra of sodium hexametaphosphate and magnesite.Figure 13
FTIR spectra of limonite and sodium hexametaphosphate.As can be seen in Figures12 and 13, sodium hexametaphosphate shows a characteristic peak of P=O stretching vibration at 1207 cm−1 and a characteristic P−O−P at 882 cm−1. The peaks at 1095.15 cm−1 and 969.98 cm−1 were the P−O stretching vibration characteristic peaks of sodium hexametaphosphate [31]. After adding magnesite and sodium hexametaphosphate, the −OH stretching vibration absorption peak at 3351 cm−1 increased compared with that before sodium hexametaphosphate. This shows a chemical adsorption between sodium hexametaphosphate and magnesite. After the reaction of limonite and sodium hexametaphosphate, the characteristic peak of P−O−P in sodium hexametaphosphate appeared at 882 cm−1 in the spectrum and the peak of P=O stretching appeared to be at 1207 cm−1, indicating that sodium hexametaphosphate in brown chemical adsorption occurred on the surface of limonite [32].


### 3.3.2. Analysis of Sodium Silicate and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of sodium silicate with a concentration of 200 mg/l. Hydrophilic silicas such as Si (OH)4 and SiO2(OH) 22− and acid micelles were selectively adsorbed on the mineral surface and changed its surface properties, thus changing the effect of the collector on the mineral surface. The adsorption mechanism was analyzed by infrared spectroscopy [33]. The spectra of magnesite and limonite before and after the action of sodium silicate are shown in Figures 14 and 15, respectively.Figure 14
FTIR spectra of magnesite and sodium silicate.Figure 15
FTIR spectra of limonite and sodium silicate.In Figures14 and 15, it can be seen that the asymmetric stretching vibration absorption peak of Si−O−Si appeared to be at 876 cm−1 [34] and CO32− showed a significant change in the characteristic peak at 1460 cm−1, indicating the chemical adsorption between magnesite and sodium silicate. The Si−O−Si stretching vibration peak of SiO32− in sodium silicate appeared to be at 1185 cm−1 in the limonite spectrum [35], reflecting chemisorption between sodium silicate and limonite.


### 3.3.3. Analysis of CMC and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of CMC with a concentration of 50 mg/l. The IR spectra of CMC before and after the interaction with magnesite and limonite are shown in Figures16 and 17, respectively.Figure 16
FTIR spectra of magnesite and CMC.Figure 17
FTIR spectra of limonite and CMC.As can be seen in Figures16 and 17, the characteristic peaks in CMC appeared to be at 1372 cm−1 and 1256 cm−1 after magnesite was contacted with CMC, indicating chemical adsorption between CMC and magnesite. In the limonite and CMC system, infrared spectroscopy showed no significant difference before and after contact, indicating no chemical adsorption between CMC and limonite.


### 3.3.4. Analysis of KD and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of KD with a concentration of 150 mg/l. The infrared spectra of magnesite and limonite before and after the action of the collector KD are shown in Figures18 and 19.Figure 18
FTIR spectra of magnesite and KD.Figure 19
FTIR spectra of limonite and KD.As can be seen in Figures18 and 19, the spectral peaks of magnesite and limonite were not displaced after the KD and no new characteristic peak was observed. However, in the single-mineral flotation test, magnesium ore had a catching effect, indicating no chemical adsorption between magnesite and KD, likely due to weak electrostatic force adsorption.


## 3.3.1. Analysis of Sodium Hexametaphosphate and Mineral Adsorption by Infrared Spectroscopy

Infrared spectroscopy was used to analyze the chemisorption of minerals and chemicals [30]. A 2 g single-mineral ore sample was placed in a solution of sodium hexametaphosphate at a concentration of 50 mg/l, the pH value of the solution was adjusted to 11.6, and the solution was thoroughly stirred for 5 minutes. The mineral sample after being treated with the reagents was washed with distilled water three times, filtrated, and dried at room temperature for infrared spectroscopical analysis. The spectra of magnesite and limonite before and after interaction with sodium hexametaphosphate are shown in Figures 12 and 13, respectively.Figure 12
FTIR spectra of sodium hexametaphosphate and magnesite.Figure 13
FTIR spectra of limonite and sodium hexametaphosphate.As can be seen in Figures12 and 13, sodium hexametaphosphate shows a characteristic peak of P=O stretching vibration at 1207 cm−1 and a characteristic P−O−P at 882 cm−1. The peaks at 1095.15 cm−1 and 969.98 cm−1 were the P−O stretching vibration characteristic peaks of sodium hexametaphosphate [31]. After adding magnesite and sodium hexametaphosphate, the −OH stretching vibration absorption peak at 3351 cm−1 increased compared with that before sodium hexametaphosphate. This shows a chemical adsorption between sodium hexametaphosphate and magnesite. After the reaction of limonite and sodium hexametaphosphate, the characteristic peak of P−O−P in sodium hexametaphosphate appeared at 882 cm−1 in the spectrum and the peak of P=O stretching appeared to be at 1207 cm−1, indicating that sodium hexametaphosphate in brown chemical adsorption occurred on the surface of limonite [32].


## 3.3.2. Analysis of Sodium Silicate and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of sodium silicate with a concentration of 200 mg/l. Hydrophilic silicas such as Si (OH)4 and SiO2(OH) 22− and acid micelles were selectively adsorbed on the mineral surface and changed its surface properties, thus changing the effect of the collector on the mineral surface. The adsorption mechanism was analyzed by infrared spectroscopy [33]. The spectra of magnesite and limonite before and after the action of sodium silicate are shown in Figures 14 and 15, respectively.Figure 14
FTIR spectra of magnesite and sodium silicate.Figure 15
FTIR spectra of limonite and sodium silicate.In Figures14 and 15, it can be seen that the asymmetric stretching vibration absorption peak of Si−O−Si appeared to be at 876 cm−1 [34] and CO32− showed a significant change in the characteristic peak at 1460 cm−1, indicating the chemical adsorption between magnesite and sodium silicate. The Si−O−Si stretching vibration peak of SiO32− in sodium silicate appeared to be at 1185 cm−1 in the limonite spectrum [35], reflecting chemisorption between sodium silicate and limonite.


## 3.3.3. Analysis of CMC and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of CMC with a concentration of 50 mg/l. The IR spectra of CMC before and after the interaction with magnesite and limonite are shown in Figures16 and 17, respectively.Figure 16
FTIR spectra of magnesite and CMC.Figure 17
FTIR spectra of limonite and CMC.As can be seen in Figures16 and 17, the characteristic peaks in CMC appeared to be at 1372 cm−1 and 1256 cm−1 after magnesite was contacted with CMC, indicating chemical adsorption between CMC and magnesite. In the limonite and CMC system, infrared spectroscopy showed no significant difference before and after contact, indicating no chemical adsorption between CMC and limonite.


## 3.3.4. Analysis of KD and Mineral Adsorption by Infrared Spectroscopy

The single-mineral sample was 2 g, mixed in a solution of KD with a concentration of 150 mg/l. The infrared spectra of magnesite and limonite before and after the action of the collector KD are shown in Figures18 and 19.Figure 18
FTIR spectra of magnesite and KD.Figure 19
FTIR spectra of limonite and KD.As can be seen in Figures18 and 19, the spectral peaks of magnesite and limonite were not displaced after the KD and no new characteristic peak was observed. However, in the single-mineral flotation test, magnesium ore had a catching effect, indicating no chemical adsorption between magnesite and KD, likely due to weak electrostatic force adsorption.


## 4. Conclusions

With KD as a collector, the maximum floatation ratio of magnesite was 74.35% at a pH value of 11.6 and the floatation ratio of limonite was 3.25%. There existed large floatability differences; magnesite and limonite increased the floatation ratio with the increase of collectors.Sodium hexametaphosphate inhibited both magnesite and limonite. A small amount of sodium silicate obviously inhibited the floatation ratio of limonite and had a little effect on the floatation ratio of magnesite. CMC had a significant inhibitory effect on magnesite and limonite flotation. The increase of the amount of CMC first inhibited reactivation. The addition of the three modifiers did not further increase this difference, but sodium silicate appeared to be the best to maintain the two types of mineral floatability differences. Mineral mixture tests showed that when sodium silicate was used as an inhibitor for flotation of magnesite and limonite, the collector was preferentially adsorbed on magnesite.The measured isoelectric points of magnesite and limonite were 6.0 and 7.5, respectively. Sodium hexametaphosphate significantly reduced the electromotive potential of the two minerals, the addition of sodium silicate reduced the electromotive potential of magnesite, with zero point moving to the left, and the greater concentration of sodium silicate, the more the moving to the left. Sodium silicate on the electric potential of limonite reduced the role more significantly. When the sodium silicate dosage was 100 mg/l, the limonite electric potential value became negative within the measured pH range; after CMC was added, the magnesite potential decreased with the increase of the pH value. The CMC caused the electromotive potential of limonite to decrease significantly, and a small amount of CMC turned the electromotive potential of limonite into negative. KD increased the electromotive potential of magnesite and reduced the zeta potential of limonite.The infrared spectroscopy test shows that all three kinds of modifiers chemically adsorbed on the magnesite surface. Sodium hexametaphosphate and sodium silicate chemically adsorbed the surface of limonite. CMC were not chemically adsorb limonite, and KD were not chemically adsorb on both mineral surfaces.



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*Source: 5534274-2021-03-08.xml*