Experimental Study on Preparation of Ferropericlase by Oxalate Coprecipitation

: It is always a goal of scientists to develop new techniques to identify the composition of mantle materials and understand geodynamic processes accurately. Ferropericlase (Mg,Fe)O is a prominent mineral in the lower mantel. It is a common practice in the research community to prepare ferropericlase using a solid-phase synthesis method or high-pressure experiment synthesis method. This conventional method contains a number of ambiguities a great deal of time is needed. In this paper, we have addressed the drawbacks of the conventional technique using a liquid-phase synthesis method to prepare ferropericlase. During the experiment, oxalic acid was added to a mixed solution of ferrous sulfate and magnesium chloride and mixed according to the molar ratio. The formed magnesium iron oxalate precipitate was sintered and reduced into the ﬁnal sample. Furthermore, the ﬁnal sample was analyzed using XRD and SEM. Compared to the solid-phase method, this coprecipitation method could produce ferropericlase with a shorter sintering time, lower sintering temperature, and a reduction in the amount of gas consumed. XRD and SEM results show that the liquid-phase method produced samples with better composition homogeneity.


Introduction
The depth of the lower mantle is 660-2890 km, the temperature range is 1600-2450 K, and the pressure range is 24-135 GPpa. Ferropericlase is the main mineral in the lower mantle (Manghnani, 1987 [1]; Ito and Takahashi, 1987 [2]; Irifune and Ringwood, 1987 [3]; Irifune, 1994 [4]; Murakami et al., 2005 [5]). Many researchers have studied the characterization of ferropericlase by simulating the temperature and pressure environment of the lower mantle through high-temperature and high-pressure experiments. Dubrovinsky et al. (2000) [6] simulated mantle conditions at 86 GPa and 1000 K to study the stability of (Mg 0.60 ,Fe 0.40 )O, and (Mg 0.50 ,Fe 0.50 )O. Kung, Li, and Liebermann (2004) [7] studied the rheological behavior of ferropericlase under high-temperature and high-pressure. Dubrovinsky et al. (2005) [8] studied the decomposition of magnesia under high-temperature and high-pressure. Demauchy, Mackwell, and Kohlstedt (2005) [9] studied the effect of water on the mutual diffusion of magnesium and iron in ferrites. Lin et al. (2006) [10] studied the sound velocity of ferropericlase in the earth's lower mantle. Skorikov et al. (2015) [11] studied the mechanism of the moment collapse of ferropericlase under pressure. Deng and Lee et al. (2017) [12] inferred the viscosity jump of the lower mantle from the melting curve of ferropericlase. Davies et al. (2018) [13] studied the oxygen distribution between the ferrite and the core.
High-pressure synthesis, solid-phase synthesis, and liquid-phase synthesis are the main methods to synthesize the ferropericlase solution. The majority of researchers use the solid-phase method to synthesize the (Mg,Fe)O solution, which is mainly to sinter the mixed powder of MgO and Fe 2 O 3 at a suitable precipitants. Supothina et al. (2007) [33] prepared tungsten oxide (WO 3 ) nanoparticles with an average particle size of 30 nm by controlling the precipitation of ammonium tungstate. Using copper nitrate (Cu(NO 3 ) 2 ) and copper chloride (CuCl 2 ) as precursors, Phiwdang et al. (2013) [34] prepared CuO nanoparticles by the precipitation method and compared the reaction before and after preparation. Ataie and Heshmati-Manesh (2001) [35] synthesized SrFe 12 O 19 hexaferrite strontium ultrafine particles with a particle size in the range of 0.1-0.2 µm by a modified coprecipitation method, with the mixture of iron and strontium nitrate as raw materials. Valenzuela et al. (2009) [36] synthesized superparamagnetic magnetite nanoparticles with an average diameter of 10 nm by coprecipitating Fe 2+ /Fe 3+ in an aqueous solution (molar ratio 1:2) and adding alkali at a mechanical stirring speed of 10,000 rpm. BiFeO 3 (BFO) nanoparticles were synthesized using the coprecipitation method at 353 K (Shami, Awan, and Anis-ur-Rehman (2011) [37]). Nejati-Moghadam et al. (2015) [38] prepared SnO 2 nanoparticles with ammonia as a precipitant and bis (acetylacetone) ethylenediamine as a capping agent by a rapid and simple coprecipitation method. Spiridigliozzi et al. (2016) [39] synthesized nanocrystalline 20 mol% samaria-doped ceria powders (Ce 0.8 Sm 0.2 O 1.9 ) by coprecipitation techniques with four precipitating agents in an aqueous solution: ammonia, ammonium carbonate, tetramethyl ammonium hydroxide, and urea. They found that the precipitant affected the morphology and sintering behavior of the powder. Ammonium carbonate and urea are the best precipitants to obtain the final dense products. Wu et al. (2018) [40] synthesized Sr 1-x Sm x Fe 12-x Cu x O 19 materials by a chemical coprecipitation technique, and they found that the grain size increased with the increase of Sm-Cu content. Rezaee, Chenari, and Ghodsi (2016) [41] prepared tungsten oxide nanoparticles by the precipitation method in a different calcinations temperature (773 K and 873 K), and they found that the nanoparticles calcined at 773 K exhibited a higher photocatalytic activity for methylene blue (MB) discoloration.
The phase diagram of ferropericlase is related to the Mg:Fe ratio, oxygen fugacity, and temperature (Figure 1a,b). According to the ferropericlase phase diagrams of different temperatures, oxygen fugacity, and Mg:Fe ratio, the sintering time of the solid-phase sintering method is longer, the sintering temperature is relatively high, and a large amount of reducing gas and energy is consumed in the experiment. Most people who study ferropericlase will synthesize the material with a solid-phase method that spends too much time and gas. From the previous studies, it is clearly identified that a conventional method takes 12-300 h to prepare ferropericlase and the synthesis temperature range is from 1350 K to 1873 K. The liquid-phase method would be a good way to reduce the synthesizing time. The liquid-phase method to synthesize ferropericlase is never used. Therefore, we propose a liquid-phase method to synthesize ferropericlase. In this paper, oxalic acid, magnesium chloride, ferrous sulfate, and sodium carbonate are used as raw materials, potassium hydroxide as a pH regulator, and the coprecipitation method is used to prepare magnesium iron oxalate precipitation. Magnesium iron oxalate precipitate is sintered at a suitable temperature with oxygen fugacity to produce ferropericlase (Mg 0.8 Fe 0.2 O).
Minerals 2020, 10, x FOR PEER REVIEW 3 of 10 aluminum nitrate as a precursor with different precipitants. Supothina et al. (2007) [33] prepared tungsten oxide (WO3) nanoparticles with an average particle size of 30 nm by controlling the precipitation of ammonium tungstate. Using copper nitrate (Cu(NO3)2) and copper chloride (CuCl2) as precursors, Phiwdang et al. (2013) [34] prepared CuO nanoparticles by the precipitation method and compared the reaction before and after preparation. Ataie and Heshmati-Manesh (2001) [35] synthesized SrFe12O19 hexaferrite strontium ultrafine particles with a particle size in the range of 0.1-0.2 μm by a modified coprecipitation method, with the mixture of iron and strontium nitrate as raw materials. Valenzuela et al. (2009) [36] synthesized superparamagnetic magnetite nanoparticles with an average diameter of 10 nm by coprecipitating Fe 2+ /Fe 3+ in an aqueous solution (molar ratio 1:2) and adding alkali at a mechanical stirring speed of 10,000 rpm. BiFeO3(BFO) nanoparticles were synthesized using the coprecipitation method at 353 K (Shami, Awan, and Anis-ur-Rehman (2011) [37] [39] synthesized nanocrystalline 20 mol% samaria-doped ceria powders (Ce0.8Sm0.2O1.9) by coprecipitation techniques with four precipitating agents in an aqueous solution: ammonia, ammonium carbonate, tetramethyl ammonium hydroxide, and urea. They found that the precipitant affected the morphology and sintering behavior of the powder. Ammonium carbonate and urea are the best precipitants to obtain the final dense products. Wu et al. (2018) [40] synthesized Sr1-xSmxFe12-xCuxO19 materials by a chemical coprecipitation technique, and they found that the grain size increased with the increase of Sm-Cu content. Rezaee, Chenari, and Ghodsi (2016) [41] prepared tungsten oxide nanoparticles by the precipitation method in a different calcinations temperature (773 K and 873 K), and they found that the nanoparticles calcined at 773 K exhibited a higher photocatalytic activity for methylene blue (MB) discoloration.
The phase diagram of ferropericlase is related to the Mg:Fe ratio, oxygen fugacity, and temperature (Figure 1a,b). According to the ferropericlase phase diagrams of different temperatures, oxygen fugacity, and Mg:Fe ratio, the sintering time of the solid-phase sintering method is longer, the sintering temperature is relatively high, and a large amount of reducing gas and energy is consumed in the experiment. Most people who study ferropericlase will synthesize the material with a solid-phase method that spends too much time and gas. From the previous studies, it is clearly identified that a conventional method takes 12-300 h to prepare ferropericlase and the synthesis temperature range is from 1350 K to 1873 K. The liquid-phase method would be a good way to reduce the synthesizing time. The liquid-phase method to synthesize ferropericlase is never used. Therefore, we propose a liquid-phase method to synthesize ferropericlase. In this paper, oxalic acid, magnesium chloride, ferrous sulfate, and sodium carbonate are used as raw materials, potassium hydroxide as a pH regulator, and the coprecipitation method is used to prepare magnesium iron oxalate precipitation. Magnesium iron oxalate precipitate is sintered at a suitable temperature with oxygen fugacity to produce ferropericlase (Mg0.8Fe0.2O).

Materials and Methods
In the experiment, the solid solution precipitation of magnesium iron oxalate (Mg 0.8 Fe 0.2 C 2 O 4 ) was obtained using the oxalate coprecipitation method, and then the ferropericlase (Mg 0.8 Fe 0.2 O) was further obtained by heat treatment. The reaction equation is given below: The experimental materials were oxalic acid (H 2 C 2 O 4 ), ferrous sulfate (FeSO 4 ), magnesium chloride (MgCl 2 ·6H 2 O), potassium hydroxide (KOH), and sodium carbonate (Na 2 CO 3 ). We weighed 3.25 g magnesium chloride hexahydrate and 0.61 g ferrous sulfate with an electronic balance (Table 1). In Table 1, the coefficient is the calculated materials' coefficient according to Equation (1): "n" means the amount of substance, "M" indicates the molecular weight, and "m" is the mass of the material weighed by an electronic balance. Furthermore, water-soluble magnesium salts and ferrous salts can also be used here to produce magnesium iron oxalate, which can be extracted by filtration or other methods after the precipitation reaction. A proper amount of distilled water was added to the beaker to dissolve the magnesium chloride and ferrous sulfate powder. The mixed solution of magnesium chloride and ferrous sulfate could realize the molecular level full mixing of magnesium ion and iron ion. Using an electronic balance to measure 3 g oxalic acid crystal, it was then dissolved in 50 mL distilled water. It was heated slightly to make it wholly dissolved to obtain the oxalic acid solution. A total of 2.5 g of sodium carbonate was weighed with an electronic balance and it was dissolved in 10 mL of distilled water to prepare the sodium carbonate solution. Slowly, oxalic acid solution was added into the prepared sodium carbonate solution, which generated a large amount of carbon dioxide gas and generated a sodium oxalate solution. We used a buret to slowly titrate the prepared sodium oxalate solution into the mixed solution of magnesium chloride and ferrous sulfate. The formation of yellowish precipitate (magnesium iron oxalate) is observed in Figure 2. Then, 0.01 mol (about 0.56 g) potassium hydroxide was weighed with an electronic balance and it was dissolved in 20 mL distilled water to prepare 0.5 mol/L potassium hydroxide solution, which was used to adjust the pH value of the final mixed solution. When the pH > 4, part of the ferrous oxalate was converted into green ferrous hydroxide, and then into brown ferric hydroxide, which created adverse effects on filtration and pre-combustion. In order to avoid the mixed coprecipitation of oxalate and hydroxide and facilitate the filtration and washing, the pH value was usually controlled to approximately 4.

Materials and Methods
In the experiment, the solid solution precipitation of magnesium iron oxalate (Mg0.8Fe0.2C2O4) was obtained using the oxalate coprecipitation method, and then the ferropericlase (Mg0.8Fe0.2O) was further obtained by heat treatment. The reaction equation is given below: The experimental materials were oxalic acid (H2C2O4), ferrous sulfate (FeSO4), magnesium chloride (MgCl2·6H2O), potassium hydroxide (KOH), and sodium carbonate (Na2CO3). We weighed 3.25 g magnesium chloride hexahydrate and 0.61 g ferrous sulfate with an electronic balance ( Table  1). In Table 1, the coefficient is the calculated materials' coefficient according to Equation (1): "n" means the amount of substance, "M" indicates the molecular weight, and "m" is the mass of the material weighed by an electronic balance. Furthermore, water-soluble magnesium salts and ferrous salts can also be used here to produce magnesium iron oxalate, which can be extracted by filtration or other methods after the precipitation reaction. A proper amount of distilled water was added to the beaker to dissolve the magnesium chloride and ferrous sulfate powder. The mixed solution of magnesium chloride and ferrous sulfate could realize the molecular level full mixing of magnesium ion and iron ion. Using an electronic balance to measure 3 g oxalic acid crystal, it was then dissolved in 50 mL distilled water. It was heated slightly to make it wholly dissolved to obtain the oxalic acid solution. A total of 2.5 g of sodium carbonate was weighed with an electronic balance and it was dissolved in 10 mL of distilled water to prepare the sodium carbonate solution. Slowly, oxalic acid solution was added into the prepared sodium carbonate solution, which generated a large amount of carbon dioxide gas and generated a sodium oxalate solution. We used a buret to slowly titrate the prepared sodium oxalate solution into the mixed solution of magnesium chloride and ferrous sulfate. The formation of yellowish precipitate (magnesium iron oxalate) is observed in Figure 2. Then, 0.01 mol (about 0.56 g) potassium hydroxide was weighed with an electronic balance and it was dissolved in 20 mL distilled water to prepare 0.5 mol/L potassium hydroxide solution, which was used to adjust the pH value of the final mixed solution. When the pH > 4, part of the ferrous oxalate was converted into green ferrous hydroxide, and then into brown ferric hydroxide, which created adverse effects on filtration and pre-combustion. In order to avoid the mixed coprecipitation of oxalate and hydroxide and facilitate the filtration and washing, the pH value was usually controlled to approximately 4.  The potassium hydroxide was dropped into the mixed solution to adjust the pH value to 3, and then the sodium oxalate solution was added until no new precipitation occurred. We filtered out the yellowish precipitate and washed it with distilled water 3 to 4 times. The magnesium iron oxalate precipitate that was washed with water was cleaned with acetone one or two times. Then, the final cleaned magnesium iron oxalate precipitate was placed in a dry place for a period of time to volatilize the water and acetone. Tin foil or other covers were used for the container containing precipitate and holes were drilled into the tin foil paper for ventilation to ensure the evaporation of water and acetone and to avoid the mixing of pollutants. The magnesium iron oxalate precipitate was allowed to dry fully in a dryer at 373 K for 3 h. The fully dried sample of magnesium iron oxalate powder was collected and put into a crucible, and then the magnesium iron oxalate powder was sintered in a vertical high-temperature furnace.
In the experimental heat treatment process (Figure 3), the temperature was first raised to 493 K for 1 h, then rapidly raised to 933 K for 10 min, kept for 5 h, and then cooled to room temperature. The gas used in the whole process was argon with 1% H 2 content. A Matheson #602 flow meter was used to measure the flow rate of the gas. The pressure reducing valve of the gas tank was 50 PSIG, the glass ball reading in the flow meter was 150, and the corresponding flow rate was 840 mL/min. The water in the magnesium iron oxalate evaporated at 493 K. In order to avoid oxidation of the ferrous oxide obtained from the decomposition of the magnesium iron oxalate by the evaporated water vapor, the temperature was kept at 493 K for 1 h to fully evaporate the water; at the same time, a large flow rate of gas was provided to remove the generated water vapor. Then, it was quickly heated to 933 K. At 773-873 K, the CO reducing gas obtained from the decomposition of magnesium iron oxalate and the reducing atmosphere introduced in the experiment provided a reducing environment to ensure that ferrous ions were not oxidized. Compared with the solid-phase method, there was no need to reduce the ferric ion. The requirement of reducing atmosphere in the experiment was to keep the existence of ferrous ion stable. In order to ensure the formation of (Mg 0.8 ,Fe 0.2 )O at 933 K, oxygen fugacity was about 10 −17 atm. In the experiment, argon containing 1% H 2 was used to provide the reducing atmosphere, and finally, the ferropericlase was obtained via sintering. The potassium hydroxide was dropped into the mixed solution to adjust the pH value to 3, and then the sodium oxalate solution was added until no new precipitation occurred. We filtered out the yellowish precipitate and washed it with distilled water 3 to 4 times. The magnesium iron oxalate precipitate that was washed with water was cleaned with acetone one or two times. Then, the final cleaned magnesium iron oxalate precipitate was placed in a dry place for a period of time to volatilize the water and acetone. Tin foil or other covers were used for the container containing precipitate and holes were drilled into the tin foil paper for ventilation to ensure the evaporation of water and acetone and to avoid the mixing of pollutants. The magnesium iron oxalate precipitate was allowed to dry fully in a dryer at 373 K for 3 h. The fully dried sample of magnesium iron oxalate powder was collected and put into a crucible, and then the magnesium iron oxalate powder was sintered in a vertical high-temperature furnace.
In the experimental heat treatment process (Figure 3), the temperature was first raised to 493 K for 1 h, then rapidly raised to 933 K for 10 min, kept for 5 h, and then cooled to room temperature. The gas used in the whole process was argon with 1% H2 content. A Matheson #602 flow meter was used to measure the flow rate of the gas. The pressure reducing valve of the gas tank was 50 PSIG, the glass ball reading in the flow meter was 150, and the corresponding flow rate was 840 mL/min. The water in the magnesium iron oxalate evaporated at 493 K. In order to avoid oxidation of the ferrous oxide obtained from the decomposition of the magnesium iron oxalate by the evaporated water vapor, the temperature was kept at 493 K for 1 h to fully evaporate the water; at the same time, a large flow rate of gas was provided to remove the generated water vapor. Then, it was quickly heated to 933 K. At 773-873 K, the CO reducing gas obtained from the decomposition of magnesium iron oxalate and the reducing atmosphere introduced in the experiment provided a reducing environment to ensure that ferrous ions were not oxidized. Compared with the solid-phase method, there was no need to reduce the ferric ion. The requirement of reducing atmosphere in the experiment was to keep the existence of ferrous ion stable. In order to ensure the formation of (Mg0.8,Fe0.2)O at 933 K, oxygen fugacity was about 10 −17 atm. In the experiment, argon containing 1% H2 was used to provide the reducing atmosphere, and finally, the ferropericlase was obtained via sintering. After heat treatment, the Mg0.8Fe0.2C2O4 formed Mg0.8Fe0.2O solid solution, CO2, and CO gas under a reducing environment (Equation (2)). XRD (X-ray diffraction), SEM (scanning electron microscope), and EDS (energy-dispersive X-ray spectroscopy) were used to analyze the structure and composition of the final material using a solution precipitation method.

Results
Now we will elaborate on the results step by step, which will give us a comprehensive understanding into the elaborate experimental results and help us to draw a conclusion.  (2)). XRD (X-ray diffraction), SEM (scanning electron microscope), and EDS (energy-dispersive X-ray spectroscopy) were used to analyze the structure and composition of the final material using a solution precipitation method.

Results
Now we will elaborate on the results step by step, which will give us a comprehensive understanding into the elaborate experimental results and help us to draw a conclusion.

XRD Result
XRD (X-ray diffraction) was used to analyze the structure of the synthesized material, ferropericlase. The analysis results are shown in Figure 4. The XRD spectrum was matched to the data of ferropericlase in the software database (Jade 6.0, MDI, Livermore, CA, USA). The XRD spectrum of the sample after oxalate coprecipitation and heat treatment is shown in Figure 4 in red color. The standard pattern was Mg 1−x Fe x O (JCPDS(ICDD) number 351393(00-035-1393)). The ferropericlase spectrum in the database is highlighted in green in Figure 4, and the sample name is shown in blue. By comparison, it was found that there were five peak spectra in the range of 3-90 • , and the spectral lines of ferropericlase in the database are consistent with those of XRD. The XRD results showed that the final product obtained by oxalate coprecipitation and heat treatment was ferropericlase.

XRD Result
XRD (X-ray diffraction) was used to analyze the structure of the synthesized material, ferropericlase. The analysis results are shown in Figure 4. The XRD spectrum was matched to the data of ferropericlase in the software database (Jade 6.0, MDI, Livermore, CA, USA). The XRD spectrum of the sample after oxalate coprecipitation and heat treatment is shown in Figure 4 in red color. The standard pattern was Mg1−xFexO (JCPDS(ICDD) number 351393(00-035-1393)). The ferropericlase spectrum in the database is highlighted in green in Figure 4, and the sample name is shown in blue. By comparison, it was found that there were five peak spectra in the range of 3-90°, and the spectral lines of ferropericlase in the database are consistent with those of XRD. The XRD results showed that the final product obtained by oxalate coprecipitation and heat treatment was ferropericlase.

SEM Result
The ferropericlase powder was obtained after heat treatment, and was a brownish-yellow powder. SEM (scanning electron microscope, phillips XL-30 SEM, F.E.I. Company, Hillsboro, OR, USA) analysis was performed for the final sample (ferropericlase) to analyze the microstructure. Figure 5 shows an SEM image for the surface of the original sample without polishing. According to the SEM image, the sample, which was obtained by oxalate coprecipitation and heat treatment, was a single-phase polycrystalline material with different grain sizes. Figure 5 shows the natural surface at different growth rates for the grain of the sintered material. It can be seen from Figure 5 that the synthesized sample was relatively dense, with small porosity and equiaxed grains. The diameters of the grains in the final sample ranged from 3 to 20 μm after sintering for 5 h. Moreover, we can also see that many ferropericlase particles were less than 10 μm on the natural surface of the sample.

SEM Result
The ferropericlase powder was obtained after heat treatment, and was a brownish-yellow powder. SEM (scanning electron microscope, phillips XL-30 SEM, F.E.I. Company, Hillsboro, OR, USA) analysis was performed for the final sample (ferropericlase) to analyze the microstructure. Figure 5 shows an SEM image for the surface of the original sample without polishing. According to the SEM image, the sample, which was obtained by oxalate coprecipitation and heat treatment, was a single-phase polycrystalline material with different grain sizes. Figure 5 shows the natural surface at different growth rates for the grain of the sintered material. It can be seen from Figure 5 that the synthesized sample was relatively dense, with small porosity and equiaxed grains. The diameters of the grains in the final sample ranged from 3 to 20 µm after sintering for 5 h. Moreover, we can also see that many ferropericlase particles were less than 10 µm on the natural surface of the sample.

XRD Result
XRD (X-ray diffraction) was used to analyze the structure of the synthesized material, ferropericlase. The analysis results are shown in Figure 4. The XRD spectrum was matched to the data of ferropericlase in the software database (Jade 6.0, MDI, Livermore, CA, USA). The XRD spectrum of the sample after oxalate coprecipitation and heat treatment is shown in Figure 4 in red color. The standard pattern was Mg1−xFexO (JCPDS(ICDD) number 351393(00-035-1393)). The ferropericlase spectrum in the database is highlighted in green in Figure 4, and the sample name is shown in blue. By comparison, it was found that there were five peak spectra in the range of 3-90°, and the spectral lines of ferropericlase in the database are consistent with those of XRD. The XRD results showed that the final product obtained by oxalate coprecipitation and heat treatment was ferropericlase.

SEM Result
The ferropericlase powder was obtained after heat treatment, and was a brownish-yellow powder. SEM (scanning electron microscope, phillips XL-30 SEM, F.E.I. Company, Hillsboro, OR, USA) analysis was performed for the final sample (ferropericlase) to analyze the microstructure. Figure 5 shows an SEM image for the surface of the original sample without polishing. According to the SEM image, the sample, which was obtained by oxalate coprecipitation and heat treatment, was a single-phase polycrystalline material with different grain sizes. Figure 5 shows the natural surface at different growth rates for the grain of the sintered material. It can be seen from Figure 5 that the synthesized sample was relatively dense, with small porosity and equiaxed grains. The diameters of the grains in the final sample ranged from 3 to 20 μm after sintering for 5 h. Moreover, we can also see that many ferropericlase particles were less than 10 μm on the natural surface of the sample.

EDS Result
EDS (energy dispersive spectrum) was used to measure the composition of ferropericlase, which was obtained by heat treatment after using the oxalate coprecipitation method. Table 2 shows the composition of the final sample. According to Table 2, there was 80.6 mol% MgO and 18.6 mol% FeO in the sample. The relative error of MgO and FeO content (wt. %) in EDS quantitative analysis was less than ±5%.

Discussion and Conclusions
Presently, the liquid-phase method is widely used in laboratories and factories to prepare ultrafine powder. For the preparation of ferropericlase, the solid-phase method is used in most experiments. Because the sintering time is long for the solid-phase synthesis method of preparing ferropericlase, large amounts of gases are needed to reduce Fe 3+ to Fe 2+ during the experimental process. Furthermore, the solid-phase method needs a higher temperature and longer time, which is a waste of energy. The liquid-phase method can achieve the molecular level mixing of magnesium ions and iron ions. At the same time, the ferrous ion salt solution is used without reducing from ferric iron ions. Compared with the solid-phase method, the liquid-phase method has the advantages of shorter preparation time, less atmosphere consumption, and better uniformity of composition.
In this paper, we proposed a liquid-phase oxalate coprecipitation method to synthesize ferropericlase (Mg 0.8 Fe 0.2 O). The ferropericlase obtained by the new method has been studied using characterization techniques, such as XRD (X-ray diffraction), EDS (energy dispersive spectrum), and SEM (scanning electron microscopy). The XRD and SEM results show that the liquid-phase method produces ferropericlase (Mg 0.8 Fe 0.2 O) as a single-phase polycrystalline material. The grain size is not uniform, which ranges from 3 to 20 µm. The morphology and grain size of ferropericlase (Mg 0.8 Fe 0.2 O) may be related to the precipitant and sintering time. The new method alleviates the roadblock's characteristic to a conventional "shake and bake" synthetic approach, and it is also advantageous because the decomposition of the oxalate intermediate provides a reducing atmosphere (CO) for the reduction of iron ions, stabilizing the ferropericlase phase. We also want to identify whether the CO gas is produced with the decomposition of magnesium iron oxalate in the heat treatment process, which will reduce the ferrous iron to metallic iron in our sampling process. The 1% H 2 is replaced with Ar gas with a purity of 99.99% during heat treatment. The SEM result also shows that there is no metallic iron formed, which means that the sample is still a solid solution of ferropericlase.
In this work, a dense and single-phase polycrystalline ferropericlase was successfully synthesized from precipitates obtained using the oxalate coprecipitation method. According to the oxalate coprecipitation method mentioned in this paper, polycrystalline ferropericlase with different iron-to-magnesium ratios can theoretically be synthesized. In the future, we will hope to study the effects of temperature, different precipitants, different iron-to-magnesium ratios, and sintering time on the growth rate and morphology of particles.