# Research on Enrichment of P2O5 from Low-Grade Carbonaceous Phosphate Ore via Organic Acid Solution

Authors: Fei Xie; Jie Zhang; Jiyan Chen; Jianrui Wang; Lin Wu
Journal: Journal of Analytical Methods in Chemistry
 (2019)

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## Abstract

The theory of using dilute organic acid solutions to leach the carbonaceous part from low-grade carbonaceous phosphate ore has been proposed by researchers as an effective approach to increase the proportion of P and to utilize the abundant low-grade resource. In this paper, a comprehensive experimental study was carried out to confirm the feasibility of organic acid leaching and investigate the optimized leaching conditions. Utilizing the low-grade carbonaceous phosphate ore produced in Zhijin, southwest of China, the effects of different types of acid, acid concentrations, reaction temperatures, reaction times, and liquid-solid ratios on leaching rate of P2O5 were evaluated using single-factor experiments and orthogonal experiments. The reaction mechanism, examined by SEM technique and the reaction thermodynamic analysis suggested that the leaching of P2O5 mainly resulted from the process of dissolution of dolomite (the main gangue mineral) in organic acid, consequently enriching the phosphate rock (the mineral of value). The effectiveness and impacts of different types of acid and reaction conditions were also studied. To conclude, this study first confirmed the viability of enriching P2O5 from low-grade ores through organic acid leaching the carbonaceous part by experimental data, and the experimental results will provide an essential scientific support for further upgrade of the technology to commercial scale utilization.


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## Body

## 1. Introduction

Although the phosphate resources in China are abundant, they mainly consist of low-grade phosphate rock. The beneficiation of low-grade phosphate ores is also a worldwide problem, and effective technologies to process such ores are yet to be developed. As a result, most low-grade phosphate rocks are currently unexploited. Low-grade phosphate rock exploitation has become one of the main topics in mineral research, with emphasis on developing a cheap and environmentally friendly method to take full advantage of such phosphate resources [1, 2]. In China, most of the low-grade phosphate mines obtain phosphorus concentrate through the beneficiation process to proceed follow-up production, and a few of them are used to produce phosphate rock powder as fertilizer after activation (Li et al., 2015) [3–5]. Depending on different factors including ore types, gangue mineral characteristics, as well as the dissemination relationship [8], flotation, dense medium beneficiation, roasting, calcination, washing, etc., are usually employed to beneficiate and process sedimentary phosphorous deposits. In the process of phosphorus enrichment, the low-grade phosphate ore is often calcined by a type of thermochemical beneficiation process, or leached by a strong acid such as sulfuric acid, hydrochloric acid, or phosphoric acid [9]. However, the current methods are not very economically efficient and environmentally friendly.Acid leaching of phosphate rock was first proposed in 1970s [10, 11], in the hope of avoiding beneficiation losses. In 1990s, some researchers begun to investigate the technique of leaching phosphate rock via organic acids solution [12–14], and since then some researchers have further studied approaches to utilize the low-grade ores [15–17]. Organic acids show an appreciable degree of selective leaching of calcareous material in low-grade phosphate ores and are proved to be effective and economical for the beneficiation of low-grade calcareous phosphate ores. Organic acid leaching is supposed to be very selective, environmentally friendly, and is able to generate products of high purity. However, the performance of this approach has not been comprehensively assessed by experimental studies, and hence its economic feasibility is not well understood. Gharabaghi et al. [17] also suggested that research studies about the leaching characteristics of specific phosphate ores and optimization of organic acid leaching techniques are needed.In this study, organic acid was used as a leaching agent for dolomite gangue minerals to enrich low-grade phosphorite. Single-factor experiments and orthogonal experiments were carried out to investigate main influence factors on enrichment of low-grade phosphate rock. Then, the mechanism of organic acid leaching and reaction thermodynamic was discussed to explain organic acid selectivity when leaching phosphate. The aim of this study is to confirm the viability of application of organic acid leaching in processing low-grade phosphorite and provide scientific support to develop a new effective method to utilize low-grade phosphate resources.


## 2. Materials and Methods

### 2.1. Materials

The sample was obtained from Zhijin Xinhua Phosphate Rock in Guizhou Province, China. The sample is sedimentary rock, and the sample number is GL2-3#. The results of the chemical analysis of the sample are listed in Table1. The chemical composition of the sample is 17.45% P2O5, 10.55% MgO, 889.76 × 10−4% ΣREE (total content of rare earth elements), and not particularly high levels of SiO2 and Al2O3.Table 1
Chemical analysis of phosphate rock (GL2-3#).
Chemical composition
Al2O3
CaO
Fe2O3
K2O
MgO
P2O5
SiO2
LOI
Others
REE
Content (%)
0.20
39.60
0.37
0.08
10.55
17.45
5.97
24.27
1.51
889.76 × 10−4There are three main types of phosphate rock in China, namely, magmatic phosphate rock, sedimentary phosphate rock, and sedimentary metamorphic phosphate rock, while 70% to 80% of which is sedimentary phosphate rock deposits. The composition of GL2-3# is typical of low-grade sedimentary dolomitic sedimentary phosphate rock containing rare earth. Due to the low phosphorus content in the rock, it is usually necessary to increase the content of P2O5 above to 25% by calcination or strong acid leaching before it can be utilized.The citric acid, lactic acid, acetic acid, and other reagents used in this experiment were all analytical reagents.


### 2.2. Analysis

The chemical composition of the sample was analyzed using X-ray fluorescence spectroscopy (XRF) (Axios mAx4KW, Panalytical, Netherlands) through melt samples. The microstructure of the phosphate rock’s surface was observed using scanning electron microscopy with an energy spectrometer (SEM-EDAX) (S-3400N, Hitachi, Japan).


### 2.3. Experiment Methods

Firstly, the sample was ground to 0.075 mm after drying at 105°C. Secondly, the water bath pot was heated to a preset temperature; about 10 g of the sample was poured slowly into a 500 cm3 beaker containing a certain concentration of dilute organic acid. Thirdly, the magnetic stirrer was started. After the sample reacted completely, the beaker was taken out, cooled, and filtered; the residue was washed, dried, and weighed.The content of P2O5 in phosphate rock was determined by the ammonium phosphomolybdate volumetric method. This method was specified by the national standard of China (GB 223.61-88 Steel and alloy chemical analysis methods), which is suitable for determining the content of P2O5 of phosphate rock when it is above 0.5%.The main operating parameters of dilute organic acid leaching are organic acid concentration, reaction temperature, and reaction time. The effect of stirring intensity on leaching was not so significant that it was not investigated in this study [21]. The stirring intensity was fixed at 300 rpm to ensure no sediment at the bottom of beaker. The parameter of liquid-solid ratio is tested by a single-factor experiment.


## 2.1. Materials

The sample was obtained from Zhijin Xinhua Phosphate Rock in Guizhou Province, China. The sample is sedimentary rock, and the sample number is GL2-3#. The results of the chemical analysis of the sample are listed in Table1. The chemical composition of the sample is 17.45% P2O5, 10.55% MgO, 889.76 × 10−4% ΣREE (total content of rare earth elements), and not particularly high levels of SiO2 and Al2O3.Table 1
Chemical analysis of phosphate rock (GL2-3#).
Chemical composition
Al2O3
CaO
Fe2O3
K2O
MgO
P2O5
SiO2
LOI
Others
REE
Content (%)
0.20
39.60
0.37
0.08
10.55
17.45
5.97
24.27
1.51
889.76 × 10−4There are three main types of phosphate rock in China, namely, magmatic phosphate rock, sedimentary phosphate rock, and sedimentary metamorphic phosphate rock, while 70% to 80% of which is sedimentary phosphate rock deposits. The composition of GL2-3# is typical of low-grade sedimentary dolomitic sedimentary phosphate rock containing rare earth. Due to the low phosphorus content in the rock, it is usually necessary to increase the content of P2O5 above to 25% by calcination or strong acid leaching before it can be utilized.The citric acid, lactic acid, acetic acid, and other reagents used in this experiment were all analytical reagents.


## 2.2. Analysis

The chemical composition of the sample was analyzed using X-ray fluorescence spectroscopy (XRF) (Axios mAx4KW, Panalytical, Netherlands) through melt samples. The microstructure of the phosphate rock’s surface was observed using scanning electron microscopy with an energy spectrometer (SEM-EDAX) (S-3400N, Hitachi, Japan).


## 2.3. Experiment Methods

Firstly, the sample was ground to 0.075 mm after drying at 105°C. Secondly, the water bath pot was heated to a preset temperature; about 10 g of the sample was poured slowly into a 500 cm3 beaker containing a certain concentration of dilute organic acid. Thirdly, the magnetic stirrer was started. After the sample reacted completely, the beaker was taken out, cooled, and filtered; the residue was washed, dried, and weighed.The content of P2O5 in phosphate rock was determined by the ammonium phosphomolybdate volumetric method. This method was specified by the national standard of China (GB 223.61-88 Steel and alloy chemical analysis methods), which is suitable for determining the content of P2O5 of phosphate rock when it is above 0.5%.The main operating parameters of dilute organic acid leaching are organic acid concentration, reaction temperature, and reaction time. The effect of stirring intensity on leaching was not so significant that it was not investigated in this study [21]. The stirring intensity was fixed at 300 rpm to ensure no sediment at the bottom of beaker. The parameter of liquid-solid ratio is tested by a single-factor experiment.


## 3. Results and Discussion

### 3.1. Results

The organic acids, as reported, are fully miscible with water and can be easily separated from the beneficiated solid phosphate product by filtration. It is reported that by dilution of the acid with water, the contact surface area between the dolomite and the acid increases [22]. Highly concentrated organic acid solution does not react with calcium and magnesium carbonate because of the high polarity of the O-H bond of the acid molecules. Also, it is necessary to use dilute solution for an effective reaction. In dilute solutions, water molecules tend to decrease the effect of polarity of the organic acids O-H bond [23]. Therefore, the research object of this paper was focused on dilute organic acid.Many types of organic acids had been reported to be used for the leaching of phosphate rock [24]. Among them, acetic acid had been proved to enhance dissolution of calcium carbonate [25], while other types of organic acid had also been proved to have the ability to dissolve the carbonate materials in low-grade phosphate rock, such as oxalic, citric, lactic, malic, succinic, and formic acids [15, 26–28]. The research studies above indicate that the effect of the enrichment rate of P2O5 is closely related to the type of organic acid. In this article, three types of acid had been chosen, listed in Table 2, to investigate the impact factors of acid type and other leaching conditions.Table 2
The types of organic acid studied in the article.
Type of organic acid
pKa
Citric acid
3.13
Lactic acid
3.86
Acetic acid
4.76


#### 3.1.1. Single-Factor Experiments

In dilute organic acids, acid concentration is one of the key factors in achieving good results in the selective removal of dolomite mineral in low-grade phosphate rocks. Table3 presents the results obtained from leaching tests under different concentrations of the three organic acids at room temperature. The results demonstrate that the three types of organic acids tested showed good selectivity for the leaching of dolomite. All three organic acids can improve the grade of P2O5, from the low level, which is 12% to 25%, to the higher level, which is above 30%. It is proved that the dilute organic acid is a promising leaching agent for the enrichment of P2O5 in low-grade phosphate ore. And it seems that the weaker the acidity, the higher the ability to improve the grade.Table 3
The leaching results of three kinds of organic acids at different acid concentrations.
Acid concentration (%)
Acid type
Grade of P2O5 (%)
Citric acid
Lactic acid
Acetic acid
1
17.72
18.94
23.46
3
20.66
22.87
27.34
5
23.58
24.14
33.78
7
25.46
28.42
32.62
9
27.36
28.88
28.22Furthermore, the effects of acid concentration, reaction temperature, reaction time, and liquid-solid ratio on the leaching rate of P2O5 were investigated using acetic acid as leaching reagent. Results are shown in Figure 1.Figure 1
Results of single-factor experiments (a) L/S = 40 : 1(vol./wt.),D = 0.075 mm, at 40°C; (b) L/S = 40 : 1(vol./wt.), 5% acetic acid; (c) 5% acetic acid, at 40°C; (d) 5% acetic acid, at 40°C, D = 0.075 mm.
(a)
(b)
(c)
(d)As seen in Figure1(a), at the beginning, the grade of P2O5 increases along with the intensity of acid concentration. When the concentration of acetic acid is 5%, the grade of P2O5 reaches to the maximum value.As shown in Figure1(b), raising reaction temperature can increase the grade of P2O5. When the temperature is higher than 40°C, the dissolution of dolomite does not increase. This indicates that a higher temperature can increase the evaporation of water and acetic acid.The P2O5 grade varies with the reaction time as shown in Figure 1(c). Firstly, as the leaching time lengthened, the P2O5 grade increases rapidly. At 30 minutes, the P2O5 rises up to 33.78%. After 30 minutes, the grade of P2O5 tends to fall and then rise but is lower than the value at 30 minutes. Within 60 minutes of the reaction, the grade of P2O5 experienced two increases; this phenomenon may indicate the following reaction. During the first 30 minutes, acetic acid selectively reacts with the exposed carbonate minerals in the sample particles. At the 30th minute, the first exposed carbonate minerals completely reacted with the acid. During the 30–40 minutes, the sample particles continued to dissolve in the acid solution, and some of the phosphorus-containing minerals were corroded by the solution, resulting in a decrease in the P2O5 grade. However, as time progressed, more carbonate mineral surfaces were exposed, and the acid in the solution reacted with it, resulting in an increase in P2O5 grade in 40–60 minutes.As seen in Figure1(d), it is found that the grade of P2O5 reaches the maximum value when liquid-solid ratio is 40 : 1(vol./wt.). When the liquid-solid ratio is low, the concentration of insoluble substance in the reaction becomes larger, and the insoluble substance is easily attached to the surface of the mineral to prevent hydrogen ions from further participating in the reaction. If the pulp is viscous, minerals do not fully react with acetic acid. Thus, the optimum liquid-solid ratio is 40 : 1(vol./wt).


#### 3.1.2. Orthogonal Experiments

Orthogonal experiments were designed to explore for effectiveness of different operating factors. The factors acid type, reaction temperature, acid concentration, and reaction time are listed in Table4, while the L/S is 40 : 1(vol./wt). So, the L9 (34) orthogonal experiments [29] were selected, and the results are shown in Tables 5 and 6.Table 4
The operating factors of orthogonal experiments.
Code
Factors’ name
Level 1
Level 2
Level 3
A
Acid type
Acetic acid
Citric acid
Lactic acid
B
Temperature (°C)
35
45
55
C
Concentration (%)
7
9
11
D
Reaction time (min)
60
120
180Table 5
The results of orthogonal experiments.
Level
Factor
A
B
C
D
Index
Acid type
Temperature (°C)
Concentration (%)
Reaction time (min)
P2O5 (%)
1
Acetic
35
7
60
28.43
2
Acetic
45
9
120
31.05
3
Acetic
55
11
180
32.43
4
Citric
35
9
180
32.75
5
Citric
45
11
60
31.74
6
Citric
55
7
120
32.83
7
Lactic
35
11
120
34.19
8
Lactic
45
7
180
32.54
9
Lactic
55
9
60
31.79Table 6
The range analysis of P2O5 grade.
Factor
Level
K1
K2
K3
Range analysis
Acid type
91.91
97.32
98.52
6.61
Temperature
95.37
95.33
97.05
1.72
Concentration
93.80
96.04
96.71
2.91
Reaction time
91.96
98.07
97.72
6.11Table6 shows that the R value of factor A (acid type) is the biggest, and the acid type has the most significant effect on the leaching. The R values of the other factors are A > D > C > B, which determine the effects of different operating factors on the P2O5 grade as follows:(1)acid type>reaction time>acid concentration>reaction temperature.The range analysis shows that the optimum condition is A3B3C3D2, which is 11% lactic acid concentration, 55°C temperature, and 120 min reaction time. From Table 6, it seems that the stronger acid has the higher grade of P2O5. Therefore, this result together with the result of the single-factor experiments indicates that more studies should be conducted to reveal the influence on the type of organic acid of the P2O5 enrichment effect.


### 3.2. Discussion

#### 3.2.1. Mechanism of Organic Acid Leaching

Take citric acid as an example to illustrate the reaction process. Under conditions of weak acidity, because the hydrophilicity of dolomite is higher than apatite, dolomite is decomposed by citric acid first. The main chemical reaction occurring in the leaching process between dolomite (CaMg(CO3)2) and citric acid is [30–32](2)4C6H8O7aq+3CaMgCO32s=Mg3C6H5O72aq+Ca3C6H5O72aq+6CO2g+6H2OlIn order to characterize the reaction between dolomite and citric acid, SEM-EDAX was used to analyze the thin sections of phosphate rock. The results are shown in Figure2 and Table 7.Figure 2
SEM-EDAX diagrams of phosphate rock after (a, b) and before (c) citric acid leaching. (Point 1, Point 3, and Point 6 are colloidal phosphate; Point 2, Point 4, and Point 5 are dolomite).
(a)
(b)
(c)Table 7
Spectral analysis of phosphate rock after citric acid leaching.
Content (%)
Element
C
O
Mg
P
Ca
1 wt.
8.40
20.60
0.37
18.45
52.17
2 wt.
18.41
33.82
10.26
—
37.51
3 wt.
—
23.45
—
20.74
55.80
4 wt.
9.64
38.62
12.02
—
39.71
5 wt.
19.97
44.53
15.77
—
19.72
6 wt.
27.50
34.10
—
24.24
14.15It can be seen from Figure2, before acid leaching, that the dolomite with the phosphate rock had a relatively smooth interface, and the colloidal phosphate was embedded between the dolomites’ gaps. The interface between them was not clear. The microscopic appearance of the dolomite after leaching had undergone a great change, and the original smooth surface was dissolved by acid, revealing a clear texture. At the same time, the phosphate rock maintained its original smooth surface, presenting a clear interface with the dolomite. It shows that citric acid can dissolve dolomite and dissociate dolomite from colloidal phosphate. The particle volumes of colloidal phosphate had got a little change during the leaching process, indicating that the citric acid showed good selectivity with dolomite and colloidal phosphate.


#### 3.2.2. Dissolution Thermodynamic Analysis

In order to judge the thermodynamic process direction of the interaction between organic acid (e.g., acetic acid) and phosphate rock, the main method used at present is the minimum free energy method to study the important thermodynamic parameter of Gibbs free energy change (ΔG). If Gibbs free energy of the reaction system is decreased, namely, negative Gibbs free energy change, the reaction would occur automatically. The larger the negative value, the easier the reaction is to proceed completely.The Gibbs free energy of the reaction in the standard state is(3)ΔGθ=ΔHθ−TΔSθ,where ΔGθ is the Gibbs free energy change in the standard state; ΔHθ is the enthalpy change in the standard state; ΔSθ is the entropy change in the standard state; and T is the thermodynamic temperature.In the experiment of leaching phosphate rock by acetic acid, the following formula is recommended for the calculation of reaction kinetics as an example for the discussion of the thermodynamic process direction of the interaction:(4)4CH3COOHaq+CaMgCO32s=2H2Ol+2CO2g+CaC2H3O22aq+MgCH3COO2aq10CH3COOHaq+Ca5PO43Fs=5CaC2H3O22aq+3H3PO4l+HFaqThe results listed in Table8 were carried out by the software HSC Chemistry v6.0. In the temperature range of 30°C to 70°C, ΔGθ of the reaction of acetic acid and dolomite is negative (Table 8). Thus, the reaction of acetic acid and dolomite can spontaneously proceed to the positive reaction direction. But, under the same circumstance, ΔGθ of the reaction of acetic acid and fluorapatite is positive (Table 9). This explains why the reaction of acetic acid and fluorapatite cannot spontaneously proceed to the positive reaction direction. Once more, this indicates that dolomite reacts with acetic acid prior to apatite.Table 8
ΔHθ, ΔSθ, and ΔGθ of the reaction of acetic acid and dolomite.
Temperature (oC)
ΔHθ (kJ/mol)
ΔSθ (J/mol·K)
ΔGθ (kJ/mol)
30
−60.598
−144.752
−16.716
40
−45.053
−94.292
−15.525
50
−30.436
−48.339
−14.815
60
−16.582
−6.112
−14.546
70
−3.302
33.166
−14.683Table 9
ΔHθ, ΔSθ, and ΔGθ of the reaction of acetic acid and fluorapatite.
Temperature (oC)
ΔHθ (kJ/mol)
ΔSθ (J/mol·K)
ΔGθ (kJ/mol)
30
52.182
−806.722
296.739
40
89.352
−686.064
304.193
50
124.269
−576.288
310.496
60
157.334
−475.505
315.748
70
189.003
−381.836
320.030


## 3.1. Results

The organic acids, as reported, are fully miscible with water and can be easily separated from the beneficiated solid phosphate product by filtration. It is reported that by dilution of the acid with water, the contact surface area between the dolomite and the acid increases [22]. Highly concentrated organic acid solution does not react with calcium and magnesium carbonate because of the high polarity of the O-H bond of the acid molecules. Also, it is necessary to use dilute solution for an effective reaction. In dilute solutions, water molecules tend to decrease the effect of polarity of the organic acids O-H bond [23]. Therefore, the research object of this paper was focused on dilute organic acid.Many types of organic acids had been reported to be used for the leaching of phosphate rock [24]. Among them, acetic acid had been proved to enhance dissolution of calcium carbonate [25], while other types of organic acid had also been proved to have the ability to dissolve the carbonate materials in low-grade phosphate rock, such as oxalic, citric, lactic, malic, succinic, and formic acids [15, 26–28]. The research studies above indicate that the effect of the enrichment rate of P2O5 is closely related to the type of organic acid. In this article, three types of acid had been chosen, listed in Table 2, to investigate the impact factors of acid type and other leaching conditions.Table 2
The types of organic acid studied in the article.
Type of organic acid
pKa
Citric acid
3.13
Lactic acid
3.86
Acetic acid
4.76


### 3.1.1. Single-Factor Experiments

In dilute organic acids, acid concentration is one of the key factors in achieving good results in the selective removal of dolomite mineral in low-grade phosphate rocks. Table3 presents the results obtained from leaching tests under different concentrations of the three organic acids at room temperature. The results demonstrate that the three types of organic acids tested showed good selectivity for the leaching of dolomite. All three organic acids can improve the grade of P2O5, from the low level, which is 12% to 25%, to the higher level, which is above 30%. It is proved that the dilute organic acid is a promising leaching agent for the enrichment of P2O5 in low-grade phosphate ore. And it seems that the weaker the acidity, the higher the ability to improve the grade.Table 3
The leaching results of three kinds of organic acids at different acid concentrations.
Acid concentration (%)
Acid type
Grade of P2O5 (%)
Citric acid
Lactic acid
Acetic acid
1
17.72
18.94
23.46
3
20.66
22.87
27.34
5
23.58
24.14
33.78
7
25.46
28.42
32.62
9
27.36
28.88
28.22Furthermore, the effects of acid concentration, reaction temperature, reaction time, and liquid-solid ratio on the leaching rate of P2O5 were investigated using acetic acid as leaching reagent. Results are shown in Figure 1.Figure 1
Results of single-factor experiments (a) L/S = 40 : 1(vol./wt.),D = 0.075 mm, at 40°C; (b) L/S = 40 : 1(vol./wt.), 5% acetic acid; (c) 5% acetic acid, at 40°C; (d) 5% acetic acid, at 40°C, D = 0.075 mm.
(a)
(b)
(c)
(d)As seen in Figure1(a), at the beginning, the grade of P2O5 increases along with the intensity of acid concentration. When the concentration of acetic acid is 5%, the grade of P2O5 reaches to the maximum value.As shown in Figure1(b), raising reaction temperature can increase the grade of P2O5. When the temperature is higher than 40°C, the dissolution of dolomite does not increase. This indicates that a higher temperature can increase the evaporation of water and acetic acid.The P2O5 grade varies with the reaction time as shown in Figure 1(c). Firstly, as the leaching time lengthened, the P2O5 grade increases rapidly. At 30 minutes, the P2O5 rises up to 33.78%. After 30 minutes, the grade of P2O5 tends to fall and then rise but is lower than the value at 30 minutes. Within 60 minutes of the reaction, the grade of P2O5 experienced two increases; this phenomenon may indicate the following reaction. During the first 30 minutes, acetic acid selectively reacts with the exposed carbonate minerals in the sample particles. At the 30th minute, the first exposed carbonate minerals completely reacted with the acid. During the 30–40 minutes, the sample particles continued to dissolve in the acid solution, and some of the phosphorus-containing minerals were corroded by the solution, resulting in a decrease in the P2O5 grade. However, as time progressed, more carbonate mineral surfaces were exposed, and the acid in the solution reacted with it, resulting in an increase in P2O5 grade in 40–60 minutes.As seen in Figure1(d), it is found that the grade of P2O5 reaches the maximum value when liquid-solid ratio is 40 : 1(vol./wt.). When the liquid-solid ratio is low, the concentration of insoluble substance in the reaction becomes larger, and the insoluble substance is easily attached to the surface of the mineral to prevent hydrogen ions from further participating in the reaction. If the pulp is viscous, minerals do not fully react with acetic acid. Thus, the optimum liquid-solid ratio is 40 : 1(vol./wt).


### 3.1.2. Orthogonal Experiments

Orthogonal experiments were designed to explore for effectiveness of different operating factors. The factors acid type, reaction temperature, acid concentration, and reaction time are listed in Table4, while the L/S is 40 : 1(vol./wt). So, the L9 (34) orthogonal experiments [29] were selected, and the results are shown in Tables 5 and 6.Table 4
The operating factors of orthogonal experiments.
Code
Factors’ name
Level 1
Level 2
Level 3
A
Acid type
Acetic acid
Citric acid
Lactic acid
B
Temperature (°C)
35
45
55
C
Concentration (%)
7
9
11
D
Reaction time (min)
60
120
180Table 5
The results of orthogonal experiments.
Level
Factor
A
B
C
D
Index
Acid type
Temperature (°C)
Concentration (%)
Reaction time (min)
P2O5 (%)
1
Acetic
35
7
60
28.43
2
Acetic
45
9
120
31.05
3
Acetic
55
11
180
32.43
4
Citric
35
9
180
32.75
5
Citric
45
11
60
31.74
6
Citric
55
7
120
32.83
7
Lactic
35
11
120
34.19
8
Lactic
45
7
180
32.54
9
Lactic
55
9
60
31.79Table 6
The range analysis of P2O5 grade.
Factor
Level
K1
K2
K3
Range analysis
Acid type
91.91
97.32
98.52
6.61
Temperature
95.37
95.33
97.05
1.72
Concentration
93.80
96.04
96.71
2.91
Reaction time
91.96
98.07
97.72
6.11Table6 shows that the R value of factor A (acid type) is the biggest, and the acid type has the most significant effect on the leaching. The R values of the other factors are A > D > C > B, which determine the effects of different operating factors on the P2O5 grade as follows:(1)acid type>reaction time>acid concentration>reaction temperature.The range analysis shows that the optimum condition is A3B3C3D2, which is 11% lactic acid concentration, 55°C temperature, and 120 min reaction time. From Table 6, it seems that the stronger acid has the higher grade of P2O5. Therefore, this result together with the result of the single-factor experiments indicates that more studies should be conducted to reveal the influence on the type of organic acid of the P2O5 enrichment effect.


## 3.1.1. Single-Factor Experiments

In dilute organic acids, acid concentration is one of the key factors in achieving good results in the selective removal of dolomite mineral in low-grade phosphate rocks. Table3 presents the results obtained from leaching tests under different concentrations of the three organic acids at room temperature. The results demonstrate that the three types of organic acids tested showed good selectivity for the leaching of dolomite. All three organic acids can improve the grade of P2O5, from the low level, which is 12% to 25%, to the higher level, which is above 30%. It is proved that the dilute organic acid is a promising leaching agent for the enrichment of P2O5 in low-grade phosphate ore. And it seems that the weaker the acidity, the higher the ability to improve the grade.Table 3
The leaching results of three kinds of organic acids at different acid concentrations.
Acid concentration (%)
Acid type
Grade of P2O5 (%)
Citric acid
Lactic acid
Acetic acid
1
17.72
18.94
23.46
3
20.66
22.87
27.34
5
23.58
24.14
33.78
7
25.46
28.42
32.62
9
27.36
28.88
28.22Furthermore, the effects of acid concentration, reaction temperature, reaction time, and liquid-solid ratio on the leaching rate of P2O5 were investigated using acetic acid as leaching reagent. Results are shown in Figure 1.Figure 1
Results of single-factor experiments (a) L/S = 40 : 1(vol./wt.),D = 0.075 mm, at 40°C; (b) L/S = 40 : 1(vol./wt.), 5% acetic acid; (c) 5% acetic acid, at 40°C; (d) 5% acetic acid, at 40°C, D = 0.075 mm.
(a)
(b)
(c)
(d)As seen in Figure1(a), at the beginning, the grade of P2O5 increases along with the intensity of acid concentration. When the concentration of acetic acid is 5%, the grade of P2O5 reaches to the maximum value.As shown in Figure1(b), raising reaction temperature can increase the grade of P2O5. When the temperature is higher than 40°C, the dissolution of dolomite does not increase. This indicates that a higher temperature can increase the evaporation of water and acetic acid.The P2O5 grade varies with the reaction time as shown in Figure 1(c). Firstly, as the leaching time lengthened, the P2O5 grade increases rapidly. At 30 minutes, the P2O5 rises up to 33.78%. After 30 minutes, the grade of P2O5 tends to fall and then rise but is lower than the value at 30 minutes. Within 60 minutes of the reaction, the grade of P2O5 experienced two increases; this phenomenon may indicate the following reaction. During the first 30 minutes, acetic acid selectively reacts with the exposed carbonate minerals in the sample particles. At the 30th minute, the first exposed carbonate minerals completely reacted with the acid. During the 30–40 minutes, the sample particles continued to dissolve in the acid solution, and some of the phosphorus-containing minerals were corroded by the solution, resulting in a decrease in the P2O5 grade. However, as time progressed, more carbonate mineral surfaces were exposed, and the acid in the solution reacted with it, resulting in an increase in P2O5 grade in 40–60 minutes.As seen in Figure1(d), it is found that the grade of P2O5 reaches the maximum value when liquid-solid ratio is 40 : 1(vol./wt.). When the liquid-solid ratio is low, the concentration of insoluble substance in the reaction becomes larger, and the insoluble substance is easily attached to the surface of the mineral to prevent hydrogen ions from further participating in the reaction. If the pulp is viscous, minerals do not fully react with acetic acid. Thus, the optimum liquid-solid ratio is 40 : 1(vol./wt).


## 3.1.2. Orthogonal Experiments

Orthogonal experiments were designed to explore for effectiveness of different operating factors. The factors acid type, reaction temperature, acid concentration, and reaction time are listed in Table4, while the L/S is 40 : 1(vol./wt). So, the L9 (34) orthogonal experiments [29] were selected, and the results are shown in Tables 5 and 6.Table 4
The operating factors of orthogonal experiments.
Code
Factors’ name
Level 1
Level 2
Level 3
A
Acid type
Acetic acid
Citric acid
Lactic acid
B
Temperature (°C)
35
45
55
C
Concentration (%)
7
9
11
D
Reaction time (min)
60
120
180Table 5
The results of orthogonal experiments.
Level
Factor
A
B
C
D
Index
Acid type
Temperature (°C)
Concentration (%)
Reaction time (min)
P2O5 (%)
1
Acetic
35
7
60
28.43
2
Acetic
45
9
120
31.05
3
Acetic
55
11
180
32.43
4
Citric
35
9
180
32.75
5
Citric
45
11
60
31.74
6
Citric
55
7
120
32.83
7
Lactic
35
11
120
34.19
8
Lactic
45
7
180
32.54
9
Lactic
55
9
60
31.79Table 6
The range analysis of P2O5 grade.
Factor
Level
K1
K2
K3
Range analysis
Acid type
91.91
97.32
98.52
6.61
Temperature
95.37
95.33
97.05
1.72
Concentration
93.80
96.04
96.71
2.91
Reaction time
91.96
98.07
97.72
6.11Table6 shows that the R value of factor A (acid type) is the biggest, and the acid type has the most significant effect on the leaching. The R values of the other factors are A > D > C > B, which determine the effects of different operating factors on the P2O5 grade as follows:(1)acid type>reaction time>acid concentration>reaction temperature.The range analysis shows that the optimum condition is A3B3C3D2, which is 11% lactic acid concentration, 55°C temperature, and 120 min reaction time. From Table 6, it seems that the stronger acid has the higher grade of P2O5. Therefore, this result together with the result of the single-factor experiments indicates that more studies should be conducted to reveal the influence on the type of organic acid of the P2O5 enrichment effect.


## 3.2. Discussion

### 3.2.1. Mechanism of Organic Acid Leaching

Take citric acid as an example to illustrate the reaction process. Under conditions of weak acidity, because the hydrophilicity of dolomite is higher than apatite, dolomite is decomposed by citric acid first. The main chemical reaction occurring in the leaching process between dolomite (CaMg(CO3)2) and citric acid is [30–32](2)4C6H8O7aq+3CaMgCO32s=Mg3C6H5O72aq+Ca3C6H5O72aq+6CO2g+6H2OlIn order to characterize the reaction between dolomite and citric acid, SEM-EDAX was used to analyze the thin sections of phosphate rock. The results are shown in Figure2 and Table 7.Figure 2
SEM-EDAX diagrams of phosphate rock after (a, b) and before (c) citric acid leaching. (Point 1, Point 3, and Point 6 are colloidal phosphate; Point 2, Point 4, and Point 5 are dolomite).
(a)
(b)
(c)Table 7
Spectral analysis of phosphate rock after citric acid leaching.
Content (%)
Element
C
O
Mg
P
Ca
1 wt.
8.40
20.60
0.37
18.45
52.17
2 wt.
18.41
33.82
10.26
—
37.51
3 wt.
—
23.45
—
20.74
55.80
4 wt.
9.64
38.62
12.02
—
39.71
5 wt.
19.97
44.53
15.77
—
19.72
6 wt.
27.50
34.10
—
24.24
14.15It can be seen from Figure2, before acid leaching, that the dolomite with the phosphate rock had a relatively smooth interface, and the colloidal phosphate was embedded between the dolomites’ gaps. The interface between them was not clear. The microscopic appearance of the dolomite after leaching had undergone a great change, and the original smooth surface was dissolved by acid, revealing a clear texture. At the same time, the phosphate rock maintained its original smooth surface, presenting a clear interface with the dolomite. It shows that citric acid can dissolve dolomite and dissociate dolomite from colloidal phosphate. The particle volumes of colloidal phosphate had got a little change during the leaching process, indicating that the citric acid showed good selectivity with dolomite and colloidal phosphate.


### 3.2.2. Dissolution Thermodynamic Analysis

In order to judge the thermodynamic process direction of the interaction between organic acid (e.g., acetic acid) and phosphate rock, the main method used at present is the minimum free energy method to study the important thermodynamic parameter of Gibbs free energy change (ΔG). If Gibbs free energy of the reaction system is decreased, namely, negative Gibbs free energy change, the reaction would occur automatically. The larger the negative value, the easier the reaction is to proceed completely.The Gibbs free energy of the reaction in the standard state is(3)ΔGθ=ΔHθ−TΔSθ,where ΔGθ is the Gibbs free energy change in the standard state; ΔHθ is the enthalpy change in the standard state; ΔSθ is the entropy change in the standard state; and T is the thermodynamic temperature.In the experiment of leaching phosphate rock by acetic acid, the following formula is recommended for the calculation of reaction kinetics as an example for the discussion of the thermodynamic process direction of the interaction:(4)4CH3COOHaq+CaMgCO32s=2H2Ol+2CO2g+CaC2H3O22aq+MgCH3COO2aq10CH3COOHaq+Ca5PO43Fs=5CaC2H3O22aq+3H3PO4l+HFaqThe results listed in Table8 were carried out by the software HSC Chemistry v6.0. In the temperature range of 30°C to 70°C, ΔGθ of the reaction of acetic acid and dolomite is negative (Table 8). Thus, the reaction of acetic acid and dolomite can spontaneously proceed to the positive reaction direction. But, under the same circumstance, ΔGθ of the reaction of acetic acid and fluorapatite is positive (Table 9). This explains why the reaction of acetic acid and fluorapatite cannot spontaneously proceed to the positive reaction direction. Once more, this indicates that dolomite reacts with acetic acid prior to apatite.Table 8
ΔHθ, ΔSθ, and ΔGθ of the reaction of acetic acid and dolomite.
Temperature (oC)
ΔHθ (kJ/mol)
ΔSθ (J/mol·K)
ΔGθ (kJ/mol)
30
−60.598
−144.752
−16.716
40
−45.053
−94.292
−15.525
50
−30.436
−48.339
−14.815
60
−16.582
−6.112
−14.546
70
−3.302
33.166
−14.683Table 9
ΔHθ, ΔSθ, and ΔGθ of the reaction of acetic acid and fluorapatite.
Temperature (oC)
ΔHθ (kJ/mol)
ΔSθ (J/mol·K)
ΔGθ (kJ/mol)
30
52.182
−806.722
296.739
40
89.352
−686.064
304.193
50
124.269
−576.288
310.496
60
157.334
−475.505
315.748
70
189.003
−381.836
320.030


## 3.2.1. Mechanism of Organic Acid Leaching

Take citric acid as an example to illustrate the reaction process. Under conditions of weak acidity, because the hydrophilicity of dolomite is higher than apatite, dolomite is decomposed by citric acid first. The main chemical reaction occurring in the leaching process between dolomite (CaMg(CO3)2) and citric acid is [30–32](2)4C6H8O7aq+3CaMgCO32s=Mg3C6H5O72aq+Ca3C6H5O72aq+6CO2g+6H2OlIn order to characterize the reaction between dolomite and citric acid, SEM-EDAX was used to analyze the thin sections of phosphate rock. The results are shown in Figure2 and Table 7.Figure 2
SEM-EDAX diagrams of phosphate rock after (a, b) and before (c) citric acid leaching. (Point 1, Point 3, and Point 6 are colloidal phosphate; Point 2, Point 4, and Point 5 are dolomite).
(a)
(b)
(c)Table 7
Spectral analysis of phosphate rock after citric acid leaching.
Content (%)
Element
C
O
Mg
P
Ca
1 wt.
8.40
20.60
0.37
18.45
52.17
2 wt.
18.41
33.82
10.26
—
37.51
3 wt.
—
23.45
—
20.74
55.80
4 wt.
9.64
38.62
12.02
—
39.71
5 wt.
19.97
44.53
15.77
—
19.72
6 wt.
27.50
34.10
—
24.24
14.15It can be seen from Figure2, before acid leaching, that the dolomite with the phosphate rock had a relatively smooth interface, and the colloidal phosphate was embedded between the dolomites’ gaps. The interface between them was not clear. The microscopic appearance of the dolomite after leaching had undergone a great change, and the original smooth surface was dissolved by acid, revealing a clear texture. At the same time, the phosphate rock maintained its original smooth surface, presenting a clear interface with the dolomite. It shows that citric acid can dissolve dolomite and dissociate dolomite from colloidal phosphate. The particle volumes of colloidal phosphate had got a little change during the leaching process, indicating that the citric acid showed good selectivity with dolomite and colloidal phosphate.


## 3.2.2. Dissolution Thermodynamic Analysis

In order to judge the thermodynamic process direction of the interaction between organic acid (e.g., acetic acid) and phosphate rock, the main method used at present is the minimum free energy method to study the important thermodynamic parameter of Gibbs free energy change (ΔG). If Gibbs free energy of the reaction system is decreased, namely, negative Gibbs free energy change, the reaction would occur automatically. The larger the negative value, the easier the reaction is to proceed completely.The Gibbs free energy of the reaction in the standard state is(3)ΔGθ=ΔHθ−TΔSθ,where ΔGθ is the Gibbs free energy change in the standard state; ΔHθ is the enthalpy change in the standard state; ΔSθ is the entropy change in the standard state; and T is the thermodynamic temperature.In the experiment of leaching phosphate rock by acetic acid, the following formula is recommended for the calculation of reaction kinetics as an example for the discussion of the thermodynamic process direction of the interaction:(4)4CH3COOHaq+CaMgCO32s=2H2Ol+2CO2g+CaC2H3O22aq+MgCH3COO2aq10CH3COOHaq+Ca5PO43Fs=5CaC2H3O22aq+3H3PO4l+HFaqThe results listed in Table8 were carried out by the software HSC Chemistry v6.0. In the temperature range of 30°C to 70°C, ΔGθ of the reaction of acetic acid and dolomite is negative (Table 8). Thus, the reaction of acetic acid and dolomite can spontaneously proceed to the positive reaction direction. But, under the same circumstance, ΔGθ of the reaction of acetic acid and fluorapatite is positive (Table 9). This explains why the reaction of acetic acid and fluorapatite cannot spontaneously proceed to the positive reaction direction. Once more, this indicates that dolomite reacts with acetic acid prior to apatite.Table 8
ΔHθ, ΔSθ, and ΔGθ of the reaction of acetic acid and dolomite.
Temperature (oC)
ΔHθ (kJ/mol)
ΔSθ (J/mol·K)
ΔGθ (kJ/mol)
30
−60.598
−144.752
−16.716
40
−45.053
−94.292
−15.525
50
−30.436
−48.339
−14.815
60
−16.582
−6.112
−14.546
70
−3.302
33.166
−14.683Table 9
ΔHθ, ΔSθ, and ΔGθ of the reaction of acetic acid and fluorapatite.
Temperature (oC)
ΔHθ (kJ/mol)
ΔSθ (J/mol·K)
ΔGθ (kJ/mol)
30
52.182
−806.722
296.739
40
89.352
−686.064
304.193
50
124.269
−576.288
310.496
60
157.334
−475.505
315.748
70
189.003
−381.836
320.030


## 4. Conclusions

It has been proposed by previous researchers that the grade of P2O5 of low-grade phosphate ore increases by leaching with organic acid. In this study, three organic acids have been studied through single-factor experiments and orthogonal experiments. The following conclusions can be drawn:(1)
Lactic, citric, and acetic acids all have the ability to improve the grade of P2O5 from a low level to a high level, which is above 30%.(2)
Acetic acid is more suitable for low temperature and fast, low concentration leaching, and the optimum parameters are 5% acid concentration, 40°C reaction temperature, and 30 min reaction time.(3)
Orthogonal experiments show that the impact order of various factors on enrichment of low-grade phosphate rock is organic acid type > reaction time > acid concentration > reaction temperature. And the best conditions are lactic acid concentration at 11%, reaction temperatures at 55°C, and reaction time at 120 min.(4)
SEM observations indicate that dolomite reacts with organic acid prior to apatite; the analysis results using thermodynamic theory also prove this.(5)
The unconformity with the results of single-factor experiments and orthogonal tests indicates that more studies should be conducted to reveal the influence on the type of organic acid of the P2O5 enrichment effect.



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*Source: 9859580-2019-02-03.xml*