The controlled oxidative precipitation of manganese oxides from Mn(II) leach liquors using SO2/air gas mixtures

Bello-Teodoro, S.; Pérez‐Garibay, R.; Uribe‐Salas, A.

doi:10.1016/j.mineng.2011.09.002

Cited by 12 publications

(9 citation statements)

References 5 publications

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“…The leaching experiments were conducted at atmospheric pressure using SO 2 gas as the reducing agent, as previously proposed Bello-Teodoro et al 20 At pH 2.1, the leach liquor contained 0.5 M Mn(II) combined with a small amount of iron (∼90 ppm). Iron in solution was precipitated by increasing the pH from 2.1 to 6 and removed from the solution before initiating the Mn(II) oxidation treatment.…”

Section: Sampling and Analysismentioning

confidence: 99%

Synthesis of Mn₂O₃ from Manganese Sulfated Leaching Solutions

Pérez‐Garibay

González-García

Fuentes-Aceituno

et al. 2016

Ind. Eng. Chem. Res.

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Manganese trioxide (Mn2O3) is one of the most important manganese compounds for the electronic industry. It is widely used for preparing the cathode component in primary and secondary batteries and electronic devices employed for electrocatalysis. There is a lack of information regarding the feasibility of employing a manganese mineral feedstock for the synthesis of Mn2O3. Hence, in the present work, research efforts were devoted to investigating a new processing route to obtain Mn2O3, which involved the leaching of pyrolusite mineral to first obtain a manganese sulfate solution. Subsequently, Mn(OH)2 was produced by adding an alkaline solution of NaOH. The Mn3O4 particles were successfully produced by aging the Mn(OH)2 precursor gel at 25 °C for 24 h in air. Finally, the precursor Mn3O4 was treated with acetic acid solutions resulting in the formation the oxy-hydroxide of manganese (α-MnO(OH)) and manganese acetate (Mn(CH3COO)2). The precipitated solid was then successfully transformed to manganese trioxide (Mn2O3) by thermal decomposition, which was conducted at temperatures between 600 and 700 °C in air.

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Section: Sampling and Analysismentioning

confidence: 99%

Synthesis of Mn₂O₃ from Manganese Sulfated Leaching Solutions

Pérez‐Garibay

González-García

Fuentes-Aceituno

et al. 2016

Ind. Eng. Chem. Res.

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“…Increasing the temperature to 80 °C did not reveal to be successful for improving the crystallinity of the precipitate. Bello-Teodoro et al observed the production of amorphous MnO 2 at room temperature. However, increasing the temperature promoted the apparition of species with a lower oxidation levels and high crystallinity, i.e., MnO·OH at 50 °C, and of Mn 3 O 4 at 75 °C.…”

Section: Current Status Of Understandingmentioning

confidence: 99%

“…Most of them were focused on the manganese removal of the solution, as it is considered as an impurity in leach liquors of several metals (Zhang et al, , Mulaudzi and Mahlangu, Menard and Demopoulos), or on the treatment of the waste stream of hydrometallurgical processes to comply with the environmental discharge regulations . In almost all these studies, the formation of MnO 2 as a reaction product has been reported; however, Bello-Teodoro et al recently observed that other oxidized manganese species precipitate as well when the oxidation temperature is increased above 50 °C. However, the authors specified neither the temperature range of formation, nor the kinetics of each reaction.…”

Section: Introductionmentioning

confidence: 99%

Synthesis of Different Manganese Oxides Using SO₂/O₂ Gas Mixtures at Different Temperatures

Bello-Teodoro

Pérez‐Garibay

Bouchard

2014

Ind. Eng. Chem. Res.

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The aim of this work is to study the kinetics and required operation conditions for the formation of various manganese oxides using the SO2/O2 gas mixture as the oxidant agent. This promising approach presents some obvious economical advantages over traditional pyrometallurgical routes. Experimental evidence demonstrate that increasing the temperature of the reaction allows modifying the oxidation potential, thus facilitating the oxidation product synthesis. However, at 25 °C by varying the SO2/O2 ratio and the gas mixture flow rate, it was not possible to modify this potential. It was also observed that manganese dioxide (MnO2) is formed between 20 and 50 °C (activation energy (E a) = 14.33 kJ/mol), oxy-hydroxide of manganese (MnO·OH) is obtained between 55 and 65 °C (E a = 25.14 kJ/mol), and manganese(II, III) oxide (Mn3O4) is produced between 70 and 90 °C (E a = 12.44 kJ/mol). The magnitude of these activation energy values is characteristic of processes controlled by the diffusion of the gaseous reagents.

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“…Many authors have studied different ways of separation and recovery of Mn from solutions containing one or more metals such as copper (Cu), cobalt (Co), zinc (Zn), iron (Fe), and nickel (Ni) (Zhang et al, 2002;Zhang and Cheng, 2007 b;Bello-Teodoro, 2011). Some other authors have studied the separation of Mn from Ca and Mg by hydroxide precipitation, carbonate precipitation, or oxidative precipitation Zhang et al, 2010;.…”

Section: Introductionmentioning

confidence: 99%

Modeling and Optimization of Manganese Carbonate Precipitation Using Response Surface Methodology and Central Composite Rotatable Design

Muanda

Omalanga²

2021

J. Eng. Exact Sci.

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A sulfate solution containing 1773.965 mg/L Mn2+, 3216.178 mg/L Mg2+ and 566.254 mg/L Ca2+ was used to perform the maximum recovery of manganese and minimum recovery of magnesium. Carbonate precipitation was used due to the better selectivity for manganese over magnesium and other impurities recovery compared to hydroxide precipitation. Four factors were studied: solution pH value, contact time, reaction temperature and sodium carbonate consumption. Analysis of variance (ANOVA) and response surface methodology (RSM) were used to determine the optimum. Under the optimum conditions, the manganese and magnesium recoveries were the highest and the lowest respectively, while the pH, the time, the temperature and the volume of Na2CO3 were the lowest. The values of the four factors were found as followed: 8.9293, 60.69 min, 77.95°F, and 50.7650 mL respectively. Moreover, the recoveries of manganese and magnesium were 99.9799% and 4.3045% respectively. The results show that optimization using RSM is effective in improving carbonate precipitation of manganese.

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The controlled oxidative precipitation of manganese oxides from Mn(II) leach liquors using SO2/air gas mixtures

Cited by 12 publications

References 5 publications

Synthesis of Mn₂O₃ from Manganese Sulfated Leaching Solutions

Synthesis of Mn₂O₃ from Manganese Sulfated Leaching Solutions

Synthesis of Different Manganese Oxides Using SO₂/O₂ Gas Mixtures at Different Temperatures

Modeling and Optimization of Manganese Carbonate Precipitation Using Response Surface Methodology and Central Composite Rotatable Design

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The controlled oxidative precipitation of manganese oxides from Mn(II) leach liquors using SO2/air gas mixtures

Cited by 12 publications

References 5 publications

Synthesis of Mn2O3 from Manganese Sulfated Leaching Solutions

Synthesis of Mn2O3 from Manganese Sulfated Leaching Solutions

Synthesis of Different Manganese Oxides Using SO2/O2 Gas Mixtures at Different Temperatures

Modeling and Optimization of Manganese Carbonate Precipitation Using Response Surface Methodology and Central Composite Rotatable Design

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Synthesis of Mn₂O₃ from Manganese Sulfated Leaching Solutions

Synthesis of Mn₂O₃ from Manganese Sulfated Leaching Solutions

Synthesis of Different Manganese Oxides Using SO₂/O₂ Gas Mixtures at Different Temperatures