# Recovery and Then Individual Separation of Platinum, Palladium, and Rhodium from Spent Car Catalytic Converters Using Hydrometallurgical Technique followed by Successive Precipitation Methods

Authors: Ahmed M. Yousif
Journal: Journal of Chemistry
 (2019)

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## Abstract

Recovery of PGMs (especially rhodium, platinum, and palladium) from different spent manufactured products (like catalytic converters) is considered as an important task as they are rarely found in nature, and they possess high economic value. In this work, the honeycomb of a car catalytic converter was primarily processed by crushing, grinding, and then treating in a hydrogen atmosphere. In order to establish an economic and ecofriendly method for the recovery of studied PGMs, different experimental conditions of changing HCl/H2O2 (as a leaching solution) ratio, temperature, and contact time were studied through batch experiments to obtain the optimum leaching conditions. The use of 0.8 vol% H2O2 and 9.0 M HCl mixture at 60°C for a contact time of 2.5 hours during the leaching process may be considered as the best conditions to be followed to save chemicals, energy, and time (about 86%, 96%, and 98% of Rh, Pt, and Pd were recovered, respectively). Individual separation of PGM ions from each other using precipitation technique from their leaching liquor was performed where % purity values of 99.5, 99.3, and 95.5 were obtained for Pt, Pd, and Rh, respectively.


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## Body

## 1. Introduction

In order to reduce the nitrogen oxide, hydrocarbon, and carbon monoxide emissions (they are considered as harmful gases) produced by different vehicle engines, it has been a must for all vehicles produced since 1993 to be fitted with catalytic converters. A catalytic converter contains precious metals (as active components) such as palladium, platinum, and rhodium (referred to as PGMs) in order to convert harmful gases emitted from vehicle engines to relatively harmless ones by both the reduction of nitrogen oxides (NOx) into nitrogen N2 and the oxidation of hydrocarbons and CO to CO2 [1].Catalytic converters consist of honeycomb skeleton units which possess PGMs on its large surface (as the honeycomb skeleton of each unit increases the contact area between the unit and the vehicle exhaust emissions) [2]. During the manufacturing process, salts of PGMs are impregnated into the surface of honeycomb skeleton using their solutions and then they are reduced to their metallic form [3]. Depending on the manufacturer, the concentrations of PGMs in the unit vary widely. In recent car catalytic converters, Pt concentration ranges from 300 to 1000 μg·g−1; for Pd, the concentration ranges from 200 to 800 μg·g−1; and for rhodium, they vary from 50 to 120 μg·g−1. Therefore, in all cases, the percentage of total content of PGMs in the samples should always be smaller than 0.1% [4].Because of the production of PGMs by limited quantities and their high value, there is an increasing demand for their recovery from different spent manufactured products as a secondary source. Besides, from an environmental point of view, such a recovery process should be correctly managed to avoid health and environmental risks [5, 6].Spent catalytic converters are good candidates for such requirement. Several works have been conducted to recover PGMs from spent catalytic converters using different metallurgical and refining methods through the use of smelting furnaces, hydrogen pretreatment, and/or direct leaching of PGMs [4, 7–9]. Several leaching processes have been developed based on the selective dissolution of the honeycomb unit consisting of PGMs after its crushing and milling [10]. One of the obstacles faces the dissolution process is the fact that PGMs are inert. Therefore, they are hardly dissolved in ordinary acids. Instead, a mixture of a strong acid (mainly HCl) and a suitable strong oxidizing agent (such as nitric acid, chlorate, hypochlorite, perchloric acid, bromated, nitrate, and cupric ions) is required in relatively large amounts to dissolve PGMs during a long period of time estimated in hours [11–13].Since the leaching processes are usually performed by the use of strong oxidizing agents, their potential effects must be taken into consideration regarding their environmental and safety issues. The use of chlorine compounds requires special care because of their poisoning effect. The use of aqua regia and other HCl/HNO3 mixtures produces nitrous vapors emission, due to several intermediate and final species generation such as NOCl, NO, NO2, and HNO2, besides Cl2 generation, as mentioned elsewhere. The use of cupric ions leaves behind copper compounds in the leaching liquor which are themselves considered as contaminants hardly separated from leached PGMs [12, 14]. Therefore, these facts lead us to think about the use of efficient and ecofriendly leaching processes.In the present study, efforts were directed to recover PGMs from processed spent catalytic converters (after pretreatment in a hydrogen atmosphere) using harmless leaching mixtures of hydrochloric acid and hydrogen peroxide as an oxidant (without any harmful gas emission or a residual byproduct generation during the process). Different experimental conditions of changing HCl/H2O2 ratio, temperature, and contact time were studied for the leaching processes to obtain the optimum leaching conditions. Other experiments were conducted to individually separate PGMs from each other in the leaching liquor using the precipitation technique.


## 2. Experimental

### 2.1. Chemicals and Materials

Reagents used in the experiments (36% HCl (12 M) and 30% H2O2 (w/w) solutions) were Sigma-Aldrich products and used as received. All other chemicals were purchased from Prolabo and Merck and used as received. Double distilled water was used throughout the experimental work. The catalyst used in this study is of honeycomb supports (found in a spent three-way gasoline catalytic converter brought from an end-of-life car management company), which are formed by a cylindrical body traversed by many straight channels and coated with a wash coat on which the PGMs are located.


### 2.2. Preparation of the Catalyst Powder and Hydrogen Pretreatment

The honeycomb unit was crushed and then ground using a cutting mill (IKA MF10) until the powder size reached 0.3 mm. The obtained powder was mixed well (to make it more homogeneous to reduce misleading results during analysis) and then was stored in a desiccator to avoid side reactions. 1 gram of the powder is used in the elemental analysis after digestion with an acid mixture (firstly with HCl/HNO3 = 3/1 (v/v) and then HF) in a Teflon vessel at 110 psi relative pressure, using a microwave digester.Hydrogen pretreatment for obtained powder stabilizes the PGMs in their metallic form in order to be easy to dissolve with the studied leaching mixtures [1]. Accordingly, the powder was treated with a constant hydrogen gas flow (8% H2) for 20 hours at 100°C.


### 2.3. Leaching and Experimental Techniques

Different experimental conditions of HCl/H2O2 ratio, contact time, and temperature were studied for the leaching processes to obtain the optimum leaching conditions through the following batch techniques.For each experiment, solid powder and working leaching solution (solid/solution ratio is 1 : 20 w/v, respectively) were put in a 250 mL flask. The flask was conditioned on a vibromatic shaker at 250 rpm and was immersed in an oil bath at the working temperature and pH for 3 hours (several preliminary experiments were performed to conclude that the contact time of 3 hours was sufficient for an experiment to reach the optimum leaching capacity). At the end of the experiment, leached PGM ion concentrations in the solution were calculated quantitatively (after clarifying a small portion of the leaching solution through centrifugation) and were compared with the PGM content in the solid powder. Each measurement reading was an average of three replicates.For monitoring the effect of contact time for the leaching experiment, small portions of the leaching solution were collected throughout the experiment at different time intervals and then centrifuged. Then, the clarified solutions were sent to analysis to record the leaching efficiency as a function of the contact time.After applying the optimum leaching conditions for a batch experiment, leaching solution containing PGM ions was directed to another treatment to individually separate PGM ions from each other using precipitation technique as illustrated in the following section.


### 2.4. Individual Separation of PGM Ions from Each Other Using Precipitation Method

This method is based on selecting suitable precipitating agents to be successively added to PGM ions found in their pretreated leaching solution in order to separate them individually as insoluble substances which may be treated after filtration to obtain their pure metallic form as illustrated in the forthcoming section (Section3.1.).


### 2.5. Instruments

The elemental analysis, as well as concentration measurements, was performed by using inductively coupled plasma-atomic emission spectrometry (ICP-AES, Horiba Jobin-Yvon Ultima).


## 2.1. Chemicals and Materials

Reagents used in the experiments (36% HCl (12 M) and 30% H2O2 (w/w) solutions) were Sigma-Aldrich products and used as received. All other chemicals were purchased from Prolabo and Merck and used as received. Double distilled water was used throughout the experimental work. The catalyst used in this study is of honeycomb supports (found in a spent three-way gasoline catalytic converter brought from an end-of-life car management company), which are formed by a cylindrical body traversed by many straight channels and coated with a wash coat on which the PGMs are located.


## 2.2. Preparation of the Catalyst Powder and Hydrogen Pretreatment

The honeycomb unit was crushed and then ground using a cutting mill (IKA MF10) until the powder size reached 0.3 mm. The obtained powder was mixed well (to make it more homogeneous to reduce misleading results during analysis) and then was stored in a desiccator to avoid side reactions. 1 gram of the powder is used in the elemental analysis after digestion with an acid mixture (firstly with HCl/HNO3 = 3/1 (v/v) and then HF) in a Teflon vessel at 110 psi relative pressure, using a microwave digester.Hydrogen pretreatment for obtained powder stabilizes the PGMs in their metallic form in order to be easy to dissolve with the studied leaching mixtures [1]. Accordingly, the powder was treated with a constant hydrogen gas flow (8% H2) for 20 hours at 100°C.


## 2.3. Leaching and Experimental Techniques

Different experimental conditions of HCl/H2O2 ratio, contact time, and temperature were studied for the leaching processes to obtain the optimum leaching conditions through the following batch techniques.For each experiment, solid powder and working leaching solution (solid/solution ratio is 1 : 20 w/v, respectively) were put in a 250 mL flask. The flask was conditioned on a vibromatic shaker at 250 rpm and was immersed in an oil bath at the working temperature and pH for 3 hours (several preliminary experiments were performed to conclude that the contact time of 3 hours was sufficient for an experiment to reach the optimum leaching capacity). At the end of the experiment, leached PGM ion concentrations in the solution were calculated quantitatively (after clarifying a small portion of the leaching solution through centrifugation) and were compared with the PGM content in the solid powder. Each measurement reading was an average of three replicates.For monitoring the effect of contact time for the leaching experiment, small portions of the leaching solution were collected throughout the experiment at different time intervals and then centrifuged. Then, the clarified solutions were sent to analysis to record the leaching efficiency as a function of the contact time.After applying the optimum leaching conditions for a batch experiment, leaching solution containing PGM ions was directed to another treatment to individually separate PGM ions from each other using precipitation technique as illustrated in the following section.


## 2.4. Individual Separation of PGM Ions from Each Other Using Precipitation Method

This method is based on selecting suitable precipitating agents to be successively added to PGM ions found in their pretreated leaching solution in order to separate them individually as insoluble substances which may be treated after filtration to obtain their pure metallic form as illustrated in the forthcoming section (Section3.1.).


## 2.5. Instruments

The elemental analysis, as well as concentration measurements, was performed by using inductively coupled plasma-atomic emission spectrometry (ICP-AES, Horiba Jobin-Yvon Ultima).


## 3. Results and Discussion

Elemental analysis of Pd, Pt, and Rh in the powder is listed in Table1. The difference in readings for the same metal in the analysis may be attributed to the heterogeneity of samples. Therefore, in all cases, the percentage of total content of PGMs in the samples was found to be smaller than 0.1% as mentioned in the literature [4].Table 1
Elemental analysis of Pt, Pd, and Rh of the spent catalyst unit under study.
Content (μg·g−1)
Pt
Pd
Rh
Range
251–277
391–419
112–126
Average
264
405
119Conditioning of HCl/H2O2 mixture with different compositions to the powder during the batch experiment yields a leaching solution of reddish color. This color is considered as a primary evidence of the existence of PGMs in the powder that they form colored chlorocomplexes as illustrated in the following equations [11]:(1)Pts+2H2O2aq+6HClaq⟷PtCl62−aq+2H+aq+4H2O(2)Pds+H2O2aq+4HClaq⟷PdCl42−aq+2H+aq+2H2O(3)2Rhs+3H2O2aq+12HClaq⟷2RhCl63−aq+6H+aq+6H2OTo study the effect of changing HCl/H2O2 ratio on the leaching efficiency, 30% H2O2 was added to 12°M HCl of ratios up to 2.4 : 100 v/v, respectively, and the leaching efficiencies were recorded through batch experiments and are shown in Figure 1. It is obvious that by increasing H2O2/HCl ratio up to 0.8 : 100 v/v, the leaching efficiency increased dramatically. Afterwards, there was no significant increase observed. Gas bubbles were observed after the addition of H2O2 to the leaching solutions which were considered as a primary evidence of the formation of chlorine gas active species (which react with PGMs to produce their chlorocomplexes in acid solutions) as illustrated in the following equation:(4)H2O2aq+2HClaq⟷Cl2g+2H2OFigure 1
Effect of changing H2O2/HCl volume percentage on PGM leaching efficiencies at 60°C for 3 hours.Based on the facts listed above, the following experiments were conditioned by holding 0.8 vol% H2O2 as a constant ratio during a series of experiments through which HCl concentration was varied from 1 to 12 M using distilled water. The obtained leaching efficiencies are shown in Figure 2. As illustrated in the figure, PGM dissolution efficiencies increased dramatically with increasing HCl concentration till reaching the value of 9.0 M. Afterwards, slight increases of the leaching efficiencies were observed. For all experiments, the observed leaching efficiencies order of PGMs was Pd > Pt > Rh. By using 11.7 M HCl, the leaching efficiencies of Pd, Pt, and Rh were 100, 96, and 88, respectively.Figure 2
Effect of changing HCl concentration with addition of 0.8 vol% H2O2 on PGM leaching efficiencies at 60°C for 3 hours.Figure3 illustrates the effect of changing the temperature on the leaching efficiencies of PGMs from the powder samples using optimum conditions of H2O2 volume ratio and HCl concentration (0.8 vol% H2O2 and 9.0 M HCl). The temperature was varied in a wide range from 20°C to 80°C. The batch experiments were conducted using well-sealed 250 mL flasks to avoid evaporation of liquids at high temperatures to maintain the constant solid/solution ratio for all experiments. The results obtained showed that, at all temperatures, the leaching efficiencies followed the order Pd > Pt > Rh. For Pt and Pd curves, the leaching efficiencies increased significantly till reaching a temperature of 60°C. Afterwards, there was no observable increase in the efficiency values. For Rh curve, the leaching efficiencies increased constantly till reaching a temperature of 60°C after which there were no considerable increases in recorded efficiencies.Figure 3
Effect of changing temperature on PGM leaching efficiencies using 0.8 vol% H2O2 and 9.0 M HCl for 3 hours.Figure4 illustrates the effect of contact time of the batch experiments on the leaching efficiencies of PGMs from the powder sample using optimum conditions of H2O2 volume ratio, HCl concentration, and temperature (0.8 vol% H2O2, 9.0 M HCl, and 60°C). The leaching processes possessed high kinetics. Pd and Pt reached equilibrium leaching values after 2 hours, while Rh reached that value after 2.5 hours. More than the mentioned equilibrium times, leaching time gave no effect to the PGM dissolution.Figure 4
Effect of contact time on the PGM leaching efficiencies using 0.8 vol% H2O2 and 9.0 M HCl at 60°C for 3 hours.A comparison between the various variables examined during the leaching experiments is tabulated in Table2. In terms of an economic feasibility study based on the best conditions that save chemicals, energy, and time, selectively the use of 0.8 vol% H2O2 and 9.0 M HCl mixture in the leaching process at 60°C for a contact time of 2.5 hours, respectively may be considered as the best conditions to be followed in the leaching process as about 86%, 96%, and 98% of Rh, Pt, and Pd were recovered, respectively.Table 2
Effect of the various variables examined during leaching process on the PGM leaching efficiencies.
Variables studied
Leaching efficiency (%)
Temp. (°C)
H2O2 (vol%)
[HCl] (M)
Time (hours)
Rh
Pt
Pd
60
0.2
11.92
3.0
48
53
67
60
0.3
11.88
3.0
61
67
78
60
0.4
11.84
3.0
71
76
87
60
0.5
11.80
3.0
80
89
93
60
0.8–2.4
11.68–11.36
3.0
88-89
96-97
100
60
0.8
1.00
3.0
20
30
60
60
0.8
2.00
3.0
38
47
69
60
0.8
3.00
3.0
52
63
77
60
0.8
5.00
3.0
64
76
85
60
0.8
6.00
3.0
73
83
90
60
0.8
7.00
3.0
80
90
95
60
0.8
9.00–11.68
3.0
86–88
96
98–100
20
0.8
9.00
3.0
40
70
75
30
0.8
9.00
3.0
54
79
83
40
0.8
9.00
3.0
66
86
89
50
0.8
9.00
3.0
77
92
94
60–80
0.8
9.00
3.0
86–90
96
98-99
60
0.8
9.00
0.5
35
50
60
60
0.8
9.00
1.0
60
73
76
60
0.8
9.00
1.5
75
90
93
60
0.8
9.00
2.0
80
95
98
60
0.8
9.00
2.5–3.0
86
96
98


### 3.1. Individual Separation of PGM Ions from Each Other Using Precipitation Method

A simplified flow sheet of the followed leaching and precipitation techniques is shown in Scheme1. Primarily, the leaching solution is directed to some treatments before being suitable for individual separation of PGMs from each other. The first step was the distillation of the excess HCl by evaporation at 190°C. Then, the dilution of the hot solution with water until a solution of 200 mg/L Pt was obtained (a suitable precipitation concentration for Pt species) [15]. During dilution, hydrolysis of metal species occurred. The complexes formed remained dissolved in the mother liquor as these species possess high solubility. The hydrolysis probability seemed to be higher for Pd and Rh than Pt, which is the reason for their complete separation from Pt at the precipitation step mentioned in the following section [16]. It is important to say that the distillation temperature must be high enough (not below 190°C) to ensure effective hydrolysis of Pd and Rh species.Scheme 1
Simplified flow sheet of the followed leaching and precipitation techniques.The individual precipitation of Pt over Pd and Rh from each other was performed by adding NH4Cl (290 g/L) at 40°C to their solution under vigorous stirring. A yellowish Pt precipitate of (NH4)2[PtCl6] was obtained. The precipitate was filtered and then washed with a dilute NH4Cl solution (140 g/L). The filtrate was set aside for later use. The contact time between the mother liquor and the precipitate was kept small to avoid coprecipitation of the impurities with Pt to ensure high purity of the precipitate. Pt precipitate was calcined at 800°C, washed several times with hot distilled water, and then dried to obtain a fine Pt powder of more than 99.5% purity. The calcination process may be summarized as follows:(5)3NH42PtCl6⟶800°C3Pts+2NH4Cl+16HCl+2N2To precipitate Pd individually from Rh found in the filtrate, it was evaporated to concentrate the solution. To the hot solution below boiling temperature was slowly added about 3 grams of sodium chlorate (NaClO3) crystals (as they vigorously reacted to the solution due to the presence of organic materials in the solution) with continuous stirring until the bright red precipitate of insoluble (NH4)2[PdCl6] was completely formed instead of the former soluble form of (NH4)2[PdCl4]. The precipitate was filtered and then washed thoroughly with distilled water, and the filtrate was set aside to extract remaining Rh as a next step. The dried precipitate was calcined at 900°C where a Pd powder of more than 99.3% purity was obtained and stored in a closed vessel. The calcination process may be illustrated as follows:(6)3NH42PdCl6⟶900°C3Pds+2NH4Cl+16HCl+2N2Remaining dissolved rhodium species in the filtrate was precipitated as a lemon yellow rhodium hydroxide (Rh(OH)3) precipitate using KOH solution by slow addition with stirring until complete precipitation occurred. The precipitate was filtered, washed thoroughly with distilled water, and then dried in air. The complete decomposition in the air for Rh(OH)3 to Rh2O3 and then Rh metal was performed by ignition at 1150°C to produce a grey Rh metal powder of 95.4% purity. Other refining processes may be followed in a forthcoming work (low purity percentage of Rh may be due to some impurities found in the leaching solution or due to various treatments performed to the individual separation process).


## 3.1. Individual Separation of PGM Ions from Each Other Using Precipitation Method

A simplified flow sheet of the followed leaching and precipitation techniques is shown in Scheme1. Primarily, the leaching solution is directed to some treatments before being suitable for individual separation of PGMs from each other. The first step was the distillation of the excess HCl by evaporation at 190°C. Then, the dilution of the hot solution with water until a solution of 200 mg/L Pt was obtained (a suitable precipitation concentration for Pt species) [15]. During dilution, hydrolysis of metal species occurred. The complexes formed remained dissolved in the mother liquor as these species possess high solubility. The hydrolysis probability seemed to be higher for Pd and Rh than Pt, which is the reason for their complete separation from Pt at the precipitation step mentioned in the following section [16]. It is important to say that the distillation temperature must be high enough (not below 190°C) to ensure effective hydrolysis of Pd and Rh species.Scheme 1
Simplified flow sheet of the followed leaching and precipitation techniques.The individual precipitation of Pt over Pd and Rh from each other was performed by adding NH4Cl (290 g/L) at 40°C to their solution under vigorous stirring. A yellowish Pt precipitate of (NH4)2[PtCl6] was obtained. The precipitate was filtered and then washed with a dilute NH4Cl solution (140 g/L). The filtrate was set aside for later use. The contact time between the mother liquor and the precipitate was kept small to avoid coprecipitation of the impurities with Pt to ensure high purity of the precipitate. Pt precipitate was calcined at 800°C, washed several times with hot distilled water, and then dried to obtain a fine Pt powder of more than 99.5% purity. The calcination process may be summarized as follows:(5)3NH42PtCl6⟶800°C3Pts+2NH4Cl+16HCl+2N2To precipitate Pd individually from Rh found in the filtrate, it was evaporated to concentrate the solution. To the hot solution below boiling temperature was slowly added about 3 grams of sodium chlorate (NaClO3) crystals (as they vigorously reacted to the solution due to the presence of organic materials in the solution) with continuous stirring until the bright red precipitate of insoluble (NH4)2[PdCl6] was completely formed instead of the former soluble form of (NH4)2[PdCl4]. The precipitate was filtered and then washed thoroughly with distilled water, and the filtrate was set aside to extract remaining Rh as a next step. The dried precipitate was calcined at 900°C where a Pd powder of more than 99.3% purity was obtained and stored in a closed vessel. The calcination process may be illustrated as follows:(6)3NH42PdCl6⟶900°C3Pds+2NH4Cl+16HCl+2N2Remaining dissolved rhodium species in the filtrate was precipitated as a lemon yellow rhodium hydroxide (Rh(OH)3) precipitate using KOH solution by slow addition with stirring until complete precipitation occurred. The precipitate was filtered, washed thoroughly with distilled water, and then dried in air. The complete decomposition in the air for Rh(OH)3 to Rh2O3 and then Rh metal was performed by ignition at 1150°C to produce a grey Rh metal powder of 95.4% purity. Other refining processes may be followed in a forthcoming work (low purity percentage of Rh may be due to some impurities found in the leaching solution or due to various treatments performed to the individual separation process).


## 4. Conclusions

Selectively, the HCl/H2O2 mixture was used as a suitable leaching mixture as it did not cause any harmful gas emission or any residual byproduct generation during the leaching process of PGMs from catalytic converters. Different experimental conditions of changing HCl/H2O2 ratio, temperature, and contact time were studied for the leaching processes to obtain the optimum leaching conditions. The use of 0.8 vol% H2O2, and 9.0 M HCl mixture at 60°C for a contact time of 2.5 hours during the leaching process may be considered as the best conditions to be followed in order to save chemicals, energy, and time (about 86%, 96%, and 98% of Rh, Pt, and Pd were recovered, respectively). Pt, Pd, and Rh were separated individually from the leaching liquor with % purity values of 99.5, 99.3, and 95, respectively, by using the precipitation technique.



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