Trans. Nonferrous Met. Soc. China 24(2014) 3716-3721

Preparation of electronic grade manganese sulfate from leaching solution of ferromanganese slag

Sheng YAN^1,2, Yun-ren QIU¹

1. School of Chemistry and Chemical Engineering, Central South University, Changsha 410083, China;

2. Innovation Base of Energy and Chemical Materials for Graduate Students Training of Hunan Province, Changsha 410083, China

Received 11 November 2013; accepted 6 June 2014

Abstract:

Preparation of electronic grade manganese sulfate from ferromanganese slag, including grinding, leaching and purification, was studied. The impurities, such as Fe³⁺, Al³⁺, Ca²⁺, Mg²⁺, heavy metal ions and Na⁺, K⁺, were removed from leaching solution by neutralized-hydrolysis, fluorination precipitation, sulfuration precipitation and re-crystallization. Effects of pH of reaction, temperature and dosage of the different additives on removal rates of the metallic ions in leaching solution were investigated, and the suitable temperature, pH and the added amount of precipitating agent were obtained. The prepared manganese sulfate product, of which the mass fractions of Ca²⁺, Mg²⁺, Na⁺, K⁺ are all smaller than 0.005%, the mass fractions of Fe³⁺, Al³⁺ and heavy metal ions are smaller than 0.001%, and the mass fraction of Mn²⁺ is greater than 32%, can meet the demand of anode materials of lithium-ion batteries.

Key words:

ferromanganese slag; leaching; purification; manganese sulfate; utilization of solid waste;

1 Introduction

With the development of lithium-ion battery industry, the electronic grade manganese sulfate for anode material of lithium-ion batteries is widely used in the production of new generation of environmentally friendly high-energy batteries [1-3].

Ferromanganese slag is a kind of blast furnace manganese slag from ferromanganese alloy smelting, a great amount of ferromanganese slag accounted for about 2-3 times as much as ferromanganese alloy each year [4,5]. The impurity categories included in ferro- manganese slag are the same as those of manganese ore, and the content of MnO is higher than that of ordinary manganese slag. Besides, there are no elements which have influence on the battery performance expect calcium, magnesium, iron, aluminum, potassium, sodium and heavy metal. However, these impurities can be removed by different purification technologies in order.

The preparation of electronic grade manganese sulfate from ferromanganese slag can lower the production cost of electronic grade manganese sulfate, bringing economic benefits and avoiding the environment pollution. WANG [6] reported that manganese was obtained through reduction method using sulfur dioxide as reducing agent and sintering method with ferromanganese slag as the raw material. SAFARIAN et al [7] studied the kinetics and mechanism of the simultaneous carbothermic reduction of FeO and MnO from high-carbon ferromanganese slag. However, no studies have been reported on the preparation of electronic grade manganese sulfate from ferromanganese slag due to it containing many impurities, such as iron, aluminum, potassium, sodium, calcium and magnesium, which makes it difficult to reduce the mass concentrations of Na⁺, K⁺, Ca²⁺ and Mg²⁺ smaller than 0.005%, and that of heavy metal is smaller than 0.001%.

In this work, preparation of electronic grade manganese sulfate from ferromanganese slag, including leaching and purification, was first studied, and the suitable condition was obtained. It can give guidance to the industrial production of the electronic grade manganese sulfate from ferromanganese slag.

2 Experimental

2.1 Material and analysis method

Manganese fluoride (MnF₂) and sulfuric acid (H₂SO₄) were of industrial grade, sodium sulfide (Na₂S) and manganese carbonate (MnCO₃) were of analytical purity. Ferromanganese slag used in the experiment was came from a smelter in Hunan, which was analyzed by XRD and the results were listed in Table 1. Mass concentrations of various ions were analyzed by an inductively coupled plasma-atomic emission spectrometer (ICP-AES)

Table 1 Major composition of ferromanganese slag (mass fraction, %)

2.2 Experimental procedure

The preparation of electronic grade manganese sulfate from ferromanganese slag is described as follows. 200 g of ferromanganese slag powder ground to 250 μm or less was added to 700 mL of 30% H₂SO₄ solution, and reacted for 3 h at 80 °C under stirring. The leaching solution with mass concentration of Mn²⁺ of about 35 g/L, was obtained by filtration. Solid MnCO₃ was added to the leaching solution to adjust pH so that the hydroxide precipitation of Fe³⁺ and Al³⁺ could be formed, and the precipitated hydroxides were removed by filtration. The obtained filtrate was evaporated till mass concentration of Mn²⁺ arrived at 92-94 g/L. Then, a certain amount of solid MnF₂ was added to the concentrated solution so that the fluoride precipitation of Ca²⁺ and Mg²⁺ could be formed, and the precipitated fluorides were removed by filtration. And then, a certain amount of solid Na₂S was added to the filtrate so that sulfide precipitation of heavy metal ions could be formed, and the precipitated sulfides were removed by filtration. Finally, the filtrate was evaporated, the crystal of MnSO₄ was obtained by filtration, then washed with deionized water. In order to further reduce the mass fraction of Na⁺ and K⁺, the obtained crystal was re-dissolved, and the target product was obtained by re-crystallization and drying. The flow chart is shown in Fig. 1.

3 Results and discussion

3.1 Removal of iron, aluminum and silicon ions

Iron, aluminum and silicon ions are the main associated elements of ferromanganese slag, so iron, aluminum and silicon ions should be removed at first. Elimination of iron and aluminum ions can be obtained by adjusting a certain pH and temperature to form the colloids of Fe³⁺ and Al³⁺ as Fe(OH)₃ and Al(OH)₃, respectively, and the colloid can adsorb silicate in leaching solution, while Mn²⁺ remains in solution.

Figure 2 exhibits the effect of temperature of reaction on mass concentration of silicon in filtrate under the conditions of stirring rate of 500 r/min, pH 5.5. With the increase of temperature from 20 to 95 °C, the mass concentration of silicon in filtrate continuously decreases. When the reaction temperature is greater than 80 °C, the mass concentration of silicon is smaller than 2 mg/L in filtrate, which can meet the production of electronic grade manganese sulfate. So the optimal temperature of reaction is 80-95 °C.

However, the pH needs to be controlled strictly to avoid the manganese loss due to precipitation of manganese hydroxide [7,8]. Figure 3 exhibits the effect of pH on mass concentration of Fe³⁺ and Al³⁺ in filtrate. The leaching solution was treated by adding solid MnCO₃ to adjust pH from 4 to 6 at 80-90 °C for 1.5 h.

Fig. 1 Flow chart of preparation of electronic grade manganese sulfate

Fig. 2 Effect of temperature on mass concentration of silicon

Fig. 3 Effect of pH on mass concentrations of Fe³⁺ and Al³⁺ in filtrate

The equation of metal hydroxide precipitation can be expressed as follows:

Mⁿ⁺+nOH^-M(OH)_n                           (1)

The equilibrium constant can be written as

                       (2)

where K_s is the solubility product, and M is Fe, Al or Mn.

Equation (2) can be written as

                         (3)

According to Eq. (3) and the practical concentrations of Fe³⁺, Al³⁺ and Mn²⁺ in leaching solution, the pH values of the starting precipitation of Fe³⁺, Al³⁺ and Mn²⁺ are 1.6, 2.8 and 6.5, respectively. Therefore, the pH is not greater than 6.5. Figure 3 shows that with the increase of the pH from 4 to 6, the mass concentration of Fe³⁺ decreases from 56 mg/L to 1.6 mg/L and that of Al³⁺ decreases from 112 mg/L to 1.8 mg/L. When pH is greater than 5.5, the mass concentrations of Fe³⁺ and Al³⁺ are smaller than 2 mg/L, which can meet the production of electronic grade manganese sulfate. Thus, the suitable pH is 5.5-6.0.

However, it is very difficult to filtrate for the formation of Fe(OH)₃ colloidal solution at room temperature. When the temperature is greater than 80 °C, the precipitation of Fe(OH)₃ is easily separated by filtration [9]. Thus, the suitable temperature is 80-90 °C.

3.2 Removal of calcium and magnesium ions

Generally, it gets difficult to remove calcium and magnesium ions from the solution containing manganese, because the chemical properties of Ca²⁺ and Mg²⁺ are similar to those of Mn²⁺ [10]. The different technologies of purification such as crystallization at high temperatures, solvent extraction and adsorption onto active carbon can remove about 90 % of Ca²⁺ and Mg²⁺ from manganese sulfate solution, but the mass concentrations of Ca²⁺ and Mg²⁺ in solution cannot meet the demand of the anode material of lithium-ion batteries. Thus, a suitable way needs to be found to effectively remove calcium and magnesium impurities from the solution containing manganese.

The filtrate, of which Fe³⁺ and Al³⁺ had been removed, was treated by adding solid MnF₂ and controlling the reaction condition to remove Ca²⁺ and Mg²⁺. Figure 4 exhibits the effect of pH of fluorination reaction on mass concentrations of Ca²⁺ and Mg²⁺ in filtrate under the condition of adding 1.3 times the theoretical amount of MnF₂, temperature 90 °C and time 1.5 h. With the increase of pH from 4.0 to 6.5, the mass concentration of Ca²⁺ decreases from 88 mg/L to 7 mg/L, and that of Mg²⁺ decreases from 96 mg/L to 10 mg/L. When the pH is smaller than 4, the precipitations of Ca²⁺ and Mg²⁺ as CaF₂ and MgF₂ respectively are not complete because F^- reacts with H⁺ to form HF and its dissociation constant (K_HF=7.4×10^-4) is relatively small [11]. When the pH is greater than 6, the mass concentrations of Ca²⁺ and Mg²⁺ are smaller than 14 mg/L in filtrate. But the excessively high pH could cause the loss of manganese. Thus, the optimal pH of fluorination reaction is 6.

Fig. 4 Effect of pH of fluorination reaction on mass concentrations of Ca²⁺ and Mg²⁺ in filtrate

Figure 5 exhibits the effect of fluorination reaction temperature on mass concentrations of Ca²⁺ and Mg²⁺ in filtrate under the condition of adding 1.3 times the theoretical amount of MnF₂, pH 6 and time 1.5 h. With the increase of fluorination reaction temperature from 60 °C to 95 °C, the mass concentration of Ca²⁺ decreases from 74 mg/L to 5 mg/L and Mg²⁺ from 92 mg/L to 8 mg/L, because the fluorination reactions are endothermic, heating is conducive to the generation of CaF₂ and MgF₂, and CaF₂ and MgF₂ have superior filter performance at higher temperatures [12,13]. When the fluorination reaction temperature is greater than 90 °C, the mass concentrations of Ca²⁺ and Mg²⁺ are smaller than 14 mg/L in filtrate, which can meet the production of electronic grade manganese sulfate. Thus, the optimal fluorination temperature is 90-95 °C.

Fig. 5 Effect of fluorination temperature on mass concentrations of Ca²⁺ and Mg²⁺ in filtrate

Figure 6 exhibits the effect of the added amount of MnF₂ on mass concentrations of Ca²⁺ and Mg²⁺ in filtrate under the condition of the pH 6.5, temperature 90 °C and time 1.5 h, where n_MnF2 is the mass ratio of practical amount of MnF₂ to theoretical amount by reaction equation. When n_MnF2 is smaller than 1.2, the precipitations of Ca²⁺ and Mg²⁺ as CaF₂ and MgF₂ respectively are not complete due to the lack of F^-. When n_MnF2 is 1.2-1.4, the mass concentrations of Ca²⁺ and Mg²⁺ are smaller than 14 mg/L, which can meet the production of electronic grade manganese sulfate. While, n_MnF2 is greater than 1.2, and the mass concentrations of Ca²⁺ and Mg²⁺ do not decrease. Thus, 1.2 times the theoretical amount of MnF₂ is suitable.

Fig. 6 Effect of added amount of MnF₂ on mass concentrations of Ca²⁺ and Mg²⁺ in filtrate

3.3 Removal of heavy metal ions

The filtrate, of which Ca²⁺ and Mg²⁺ had been removed, was treated by adding solid Na₂S to remove heavy metal ions based on the different sulfide solubilities of metals at a certain condition [14, 15]. The effect of pH on mass concentrations of heavy metal ions in filtrate is illustrated using Ni²⁺ as example because the solubility product of NiS is larger than that of other heavy metal sulfides such as CuS, CdS, PbS, ZnS and CoS. Figure 7 exhibits the effect of pH on mass concentration of Ni²⁺ in filtrate by adding 1.4 times the theoretical amount of Na₂S during reaction of 1.5 h at 90 °C.

Fig. 7 Effect of pH of sulphuration reaction on mass concentration of Ni²⁺ in filtrate

The thermodynamic equilibrium involved in the sulfide precipitation can be expressed as follows [16,17]:

M₂S_n2Mⁿ⁺+nS^2-, K_sp=[Mⁿ⁺]²[S^2-]ⁿ            (4)

H₂S(aq) H⁺+HS^-, K₁=10^-8                  (5)

HS^-H⁺+S^2-, K₂=10^-12.9                       (6)

H₂S(aq) 2H⁺+S^2-,      (7)

where K_sp is the solubility product of metals sulfide; K, K₁ and K₂ are dissociation equilibrium constants. These relationships can be written as

    (8)

According to Eq. (8), the pH of fluorination reaction relates to not only the solubility product of metal sulfides, but also the practical mass concentration of metal ions. The mass concentration of manganese is relatively greater than that of other heavy metal ions in solution, and the excessively high pH may cause the loss of manganese. Figure 7 shows that the mass concentration of Ni²⁺ decreases from 11 mg/L to 1.6 mg/L with the increase of pH from 3.5 to 6.0. When the pH is greater than 5.5, the mass concentration of Ni²⁺ is smaller than 2 mg/L, which can meet the production of electronic grade manganese sulfate. Thus, the optimal pH of fluorination is 5.5-6.0.

Figure 8 exhibits the effect of the added amount of Na₂S on the mass concentration of heavy metal ions in filtrate after reaction for 1.5 h under 90 °C and pH 6, where n_Na2S is the mass ratio of practical amount of Na₂S to theoretical amount by reaction equation. The mass concentration of Ni²⁺ decreases from 9 mg/L to 1.4 mg/L as n_Na2S increases from 1.1 to 1.5. When n_Na2S is smaller than 1.3, the precipitation of Ni²⁺ as NiS is not complete because a small part of S^2- reacts with H⁺ to form H₂S. When n_Na2S is greater than 1.3, and the mass concentration of Ni²⁺ is smaller than 2 mg/L, which can meet the production of electronic grade manganese sulfate. Thus, 1.3 times the theoretical amount of Na₂S is suitable.

Fig. 8 Effect of added amount of Na₂S on mass concentration of Ni²⁺ in filtrate

3.4 Removal of sodium and potassium ions

200 mL of filtrate, of which heavy metal ions had been removed and mass concentration of Mn²⁺ was 94 g/L, was evaporated till 10 mL or so under stirring at temperature from 95 °C to 100 °C; the concentrated suspension was filtered at 95-100 °C; the obtained crystal of MnSO₄·H₂O was washed with 95-100 °C deionized water and dried at 110 °C. The mass fractions of Na⁺ and K⁺ of the obtained product were greater than 0.005% (see Table 2). Thus, the obtained product was dissolved again with deionized water, the obtained solution was evaporated till 5 mL, the suspension was filtered at 95-100 °C and the obtained crystal of MnSO₄·H₂O was washed and dried at 110 °C. 51 g of MnSO₄·H₂O was obtained, and the recovery rate of manganese was 88%. The mass fractions of Na⁺ and K⁺ greatly decreased. The mass fractions of Na⁺ and K⁺ before and after re-crystallization are shown in Table 2, and the quality of prepared sample is shown in Table 3.

Table 2 Mass fractions of Na⁺ and K⁺

Table 3 Enterprise standard of electronic grade manganese sulfate (mass fraction, %)

4 Conclusions

1) Iron and aluminum ions in the leaching solution are removed with neutralization-hydrolysis by adjusting pH using solid MnCO₃, under suitable conditions of pH 5.5-6.0, temperature 85-90 °C and time 1.5 h. The mass concentrations of Fe³⁺ and Al³⁺ are smaller than 2 mg/L.

2) Calcium and magnesium ions in the leaching solution are removed with fluoride precipitation by adding solid MnF₂, under suitable conditions of 1.2 times theoretical amount of MnF₂, pH 6, temperature 90-95 °C and time 1.5 h. The mass concentrations of Ca²⁺ and Mg²⁺ are smaller than 14 mg/L.

3) Heavy metal ions are removed with sulfide precipitation by adding solid Na₂S, under suitable conditions of 1.3 times theoretical amount of Na₂S, pH 5.5-6.0, temperature 90-95 °C and time 1.5 h. The mass concentration of heavy metal ions is smaller than 2 mg/L.

4) Sodium and potassium ions are removed with re-crystallization at temperature of 95-100 °C, and the mass fractions of Na⁺ and K⁺ are all smaller than 0.005%.

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锰铁合金渣浸出液制备电子级硫酸锰

闫 升^1,2，邱运仁¹

1. 中南大学 化学化工学院，长沙 410083；

2. 湖南省能源与化工新材料研究生培养创新基地，长沙 410083

摘  要：以锰铁合金渣为原料，经研磨、硫酸浸出后，采用中和-水解、氟化沉淀、硫化沉淀和重结晶法去除浸出液中的铁、铝、钙、镁和重金属以及钠、钾等离子以制备电子级硫酸锰。研究反应pH、反应温度和不同添加剂的用量对硫酸锰产品中杂质含量的影响，并得到了较优的温度、pH、沉淀剂的用量等工艺条件。结果表明：在较优工艺条件下，所制备的碳酸锰中，Ca²⁺、Mg²⁺、Na⁺、K⁺杂质离子的含量小于0.005 %，Fe³⁺、Al³⁺和重金属离子的含量小于0.001%，Mn²⁺的含量大于32%，硫酸锰产品的质量满足锂离子电池正极材料的要求。

关键词：锰铁合金渣；浸出；纯化；硫酸锰；固废利用

(Edited by Xiang-qun LI)

Foundation item: Project (2013ZX0754-001) supported by China National Critical Project for Science and Technology on Water Pollution Prevention and Control

Corresponding author: Yun-ren QIU; Tel: +86-731-88879616; E-mail: qiuyunren@gmail.com; csu_tian@csu.edu.cn

DOI: 10.1016/S1003-6326(14)63520-2

Abstract: Preparation of electronic grade manganese sulfate from ferromanganese slag, including grinding, leaching and purification, was studied. The impurities, such as Fe³⁺, Al³⁺, Ca²⁺, Mg²⁺, heavy metal ions and Na⁺, K⁺, were removed from leaching solution by neutralized-hydrolysis, fluorination precipitation, sulfuration precipitation and re-crystallization. Effects of pH of reaction, temperature and dosage of the different additives on removal rates of the metallic ions in leaching solution were investigated, and the suitable temperature, pH and the added amount of precipitating agent were obtained. The prepared manganese sulfate product, of which the mass fractions of Ca²⁺, Mg²⁺, Na⁺, K⁺ are all smaller than 0.005%, the mass fractions of Fe³⁺, Al³⁺ and heavy metal ions are smaller than 0.001%, and the mass fraction of Mn²⁺ is greater than 32%, can meet the demand of anode materials of lithium-ion batteries.