JP5578750B1 - Amide derivatives - Google Patents

Abstract

Valuable metals are selectively extracted from an acidic solution containing impurities at a high concentration.
The amide derivative of the present invention is represented by the following general formula. In the formula, R ¹ and R ² each represent the same or different branched alkyl group, R ³ represents a hydrogen atom or an alkyl group, and R ⁴ is bonded to the α-carbon as a hydrogen atom or an amino acid. Represents any group other than an amino group. The following general formula preferably has a glycine unit, a histidine unit, a lysine unit, an aspartic acid unit or a normal-methylglycine unit. When extracting valuable metals, valuable metals can be selectively extracted by subjecting an acidic solution containing valuable metals and impurities to solvent extraction with the amide derivative.

[Selection] Figure 3

Description

  The present invention relates to amide derivatives.

  Cobalt and rare earth metals are known as valuable metals and are used for various purposes in industry. Cobalt is used in superalloys (high-strength heat-resistant alloys) used for aircraft jet engines and the like, in addition to positive electrode materials for secondary batteries. Rare earth metals are used in phosphor materials, negative electrodes for nickel metal hydride batteries, additives for magnets mounted on motors, abrasives for glass substrates used in liquid crystal panels and hard disk drives, and the like.

  In recent years, energy conservation has been strongly promoted, and in the automobile industry, a shift from a conventional gasoline vehicle to a hybrid vehicle or an electric vehicle equipped with a secondary battery using cobalt or a rare earth metal is rapidly progressing. In lighting fixtures, the transition from conventional fluorescent tubes to efficient three-wavelength fluorescent tubes using rare earth metals such as lanthanum, cerium, yttrium, terbium and europium is rapidly progressing. The above cobalt and rare earth metals are rare resources, and most of them depend on imports.

  However, although yttrium and europium were used as phosphors for CRT televisions for analog broadcasting, in recent years, a large amount of CRTs have been discarded as used products with the shift to liquid crystal televisions. In addition, rapidly spreading products such as secondary batteries and three-wavelength fluorescent tubes can easily be expected to become a large amount of waste as used products in the future. As described above, it is not preferable from the viewpoint of resource saving and resource security to use rare resources such as cobalt and rare earth metals as waste without recycling from used products. Recently, it has been strongly desired to establish a method for effectively recovering valuable metals such as cobalt and rare earth metals from such used products.

<Recovery of cobalt from secondary batteries>
By the way, as said secondary battery, a nickel metal hydride battery, a lithium ion battery, etc. are mentioned, Manganese other than cobalt which is a rare metal is used for these positive electrode agents. And in the positive electrode material of a lithium ion battery, it tends to increase the ratio of inexpensive manganese instead of expensive cobalt. Recently, recovery of valuable metals from used batteries has been attempted. As one of the recovery methods, there is a dry method in which used batteries are put into a furnace and dissolved, and separated into metal and slag to recover the metal. However, in this method, since manganese is transferred to slag, only cobalt can be recovered.

  In addition, a wet method is also known in which a used battery is dissolved in an acid, and a metal is recovered using a separation method such as a precipitation method, a solvent extraction method, or electrolytic collection. For example, in the precipitation method, there are a method of adjusting the pH of a solution containing cobalt and manganese, a method of obtaining a cobalt sulfide starch by adding a sulfurizing agent, and a method of obtaining a manganese oxide starch by adding an oxidizing agent. It is known (see Patent Document 1). However, this method has problems such as coprecipitation, and it is difficult to completely separate cobalt and manganese.

  Further, it is known that when cobalt is recovered as a metal by electrolytic collection, manganese oxide is deposited on the anode surface in a system in which a high concentration of manganese is present, and the deterioration of the anode is promoted. In addition, the specific colored fine manganese oxide floats in the electrolytic solution, and the filter cloth used for electrolytic collection is clogged, and the cobalt metal is contaminated with the manganese oxide, so that stable operation is difficult.

  Moreover, when trying to collect cobalt using a solvent extraction method, an acidic extractant is widely used. However, as described above, since a large amount of manganese is recently used in the positive electrode of lithium ion batteries, the battery solution contains a high concentration of manganese. There is no effective extractant to extract effectively.

  In addition to recycling used batteries, cobalt smelting currently used to produce cobalt is made of nickel ore such as nickel oxide ore, but nickel oxide ore has a manganese ratio compared to cobalt. It is high and the abundance ratio is about 5 to 10 times that of cobalt. In refining cobalt, separation from manganese has become a major issue.

<Recovery of rare earth metals from three-wavelength fluorescent tubes and CRTs>
In addition, a mixture of rare earth metals such as lanthanum, cerium, yttrium, terbium and europium is used for the phosphor used in the three-wavelength fluorescent tube mentioned above. Furthermore, the phosphor for a cathode ray tube contains yttrium and europium together with a high ratio of zinc.

  As a method for recovering a specific rare earth metal from a mixture of rare earth metals, a method of recovering by a solvent extraction method from a solution dissolved in an acid such as a mineral acid is generally used. For the mutual separation of rare earth metals, for example, there is an industrial example using a trade name PC88A (manufactured by Daihachi Chemical), which is a phosphorus-based extractant. However, because this extractant contains phosphorus in its structure, advanced wastewater treatment is required to prevent contamination of public water areas by extractants and their degradation products that migrate into wastewater when used industrially. It becomes. Depending on the specific area of the country, it is subject to the total amount regulation stipulated by the Water Pollution Law, which is a concern when used on an industrial scale.

  As an extractant that does not contain phosphorus, a carboxylic acid-based extractant (for example, 2-methyl-2-ethyl-1-heptanoic acid: neodecanoic acid) has been put into practical use. However, since this extraction agent can be extracted only in a pH range higher than neutrality, when targeting an acidic solution as described above, a large amount of neutralizing agent is required and there is a concern about an increase in cost. In addition, the extraction capacity of the carboxylic acid-based extractant is lower than that of the above-described phosphorus-based extractant, and excessive equipment is required, which increases the cost.

  In order to solve such problems, an extractant called DODGAA having a diglycolamide acid skeleton has been developed (see Patent Document 2). However, when this extractant is used, as shown in Non-Patent Document 1, among rare earth metals, yttrium (Y), lutetium (Lu), ytterbium (Yb), thulium (Tm), erbium (Er) called heavy rare earth metals are used. ), Holmium (Ho) tends to be extracted together with dysprosium (Dy), terbium (Tb), gadolinium (Gd), europium (Eu), and samarium (Sm), which are called middle rare earth metals. Not suitable for separation. Moreover, in DODGAA, the extraction rate of promethium (Pm), neodymium (Nd), praseodymium (Pr), cerium (Ce), and lanthanum (La) called light rare earth metals is low. In addition, europium (Eu), which is particularly low in production and expensive, cannot be selectively recovered from other rare earth metals. Thus, an extractant that can separate rare earth metals from each other and an extractant that can efficiently extract light rare earth metals have not been found.

JP 2000-234130 A JP 2007-327085 A

K. Shimojo, H. Naganawa, J. Noro, F. Kubota and M. Goto; Extraction behavior and separation of lanthanides with a diglycol amic acid derivative and a nitrogen-donor ligand; Anal. Sci., 23, 1427-30, 2007 Dec.

  An object of the present invention is to selectively extract valuable metals from an acidic solution containing impurities at a high concentration.

As a result of intensive studies to solve the above problems, the present inventors have found that the above object can be achieved by providing an amide derivative represented by the following general formula, and have completed the present invention. .

  Specifically, the present invention provides the following.

（式中、Ｃ _８ Ｈ _１７ は分鎖であり、Ｒは水素原子又はアルキル基を示す。） (1) The present invention is an amide derivative represented by the following general formula .

(In the formula , C ₈ H ₁₇ is a branched chain, and R represents a hydrogen atom or an alkyl group .)

  According to the present invention, valuable metals can be selectively extracted from an acidic solution containing impurities at a high concentration.

1 is a diagram showing a ¹ H-NMR spectrum of a glycinamide derivative synthesized in Example 1. FIG. 1 is a diagram showing a ¹³ C-NMR spectrum of a glycinamide derivative synthesized in Example 1. FIG. The result when cobalt is extracted from an acidic solution containing cobalt and manganese using the amide derivative of Example 1 is shown. The result when cobalt is extracted from an acidic solution containing cobalt and manganese using the amide derivative of Example 2 is shown. The result when cobalt is extracted from an acidic solution containing cobalt and manganese using the amide derivative of Reference Example 3 is shown. The result when cobalt is extracted from an acidic solution containing cobalt and manganese using a commercially available carboxylic acid-based cobalt extractant according to Comparative Example 1 is shown. The result when extracting europium from the acidic solution containing europium, yttrium, and zinc using the amide derivative of Example 1 is shown. The result when extracting europium from the acidic solution containing europium, yttrium, and zinc using N, N-dioctyl-3-oxapentane-1,5-amidic acid according to Comparative Example 2 is shown. The result when light rare earth metal is extracted from an acidic solution containing light rare earth metal and heavy rare earth metal using the amide derivative of Example 1 is shown.

  Hereinafter, specific embodiments of the present invention will be described in detail. However, the present invention is not limited to the following embodiments, and may be implemented with appropriate modifications within the scope of the object of the present invention. Can do.

<Amide derivatives>
The amide derivative of the present invention is represented by the following general formula .

In the formula, C ₈ H ₁₇ is a branched chain, and the substituent R represents a hydrogen atom or an alkyl group . In the present invention, by introducing an alkyl group into the amide skeleton, the lipophilicity can be increased and used as an extractant.

The above amide derivatives, glycine amide derived body及 beauty normal - is preferably any one or more of methyl glycine derivative. When the amide derivative is a glycinamide derivative, the above glycinamide derivative can be synthesized by the following method. First, 2-halogenated acetyl halide is added to an alkylamine having a structure represented by NH (C ₈ H ₁₇ ) ₂ , and the hydrogen atom of the amine is substituted with 2-halogenated acetyl by nucleophilic substitution reaction. -Halogenated (N, N-di) alkylacetamide is obtained.

  Next, the above-mentioned 2-halogenated (N, N-di) alkylacetamide is added to glycine or an N-alkylglycine derivative, and one of the hydrogen atoms of the glycine or N-alkylglycine derivative is (N, N) by a nucleophilic substitution reaction. Substitution with an N-di) alkylacetamide group. A glycine alkylamide derivative can be synthesized by these two-step reactions.

  Replacing glycine with histidine, lysine, and aspartic acid can synthesize histidine amide derivatives, lysine amide derivatives, and aspartic acid amide derivatives. From the constant, it is considered to be within the range of the results using the glycine derivative and the histidine amide derivative.

<Method for extracting valuable metals>
In order to extract valuable metal ions using the extractant synthesized by the above method, this acidic aqueous solution is added to and mixed with the organic solution of the extractant while adjusting the acidic aqueous solution containing the target valuable metal ions. Thereby, the target valuable metal ion can be selectively extracted into the organic phase.

  The organic solvent after extracting the valuable metal ions is separated, and the reverse extraction starting liquid whose pH is adjusted lower than that of the acidic aqueous solution is added thereto and stirred to extract the desired valuable metal ions into the organic solvent. The target valuable metal ions can be recovered in the aqueous solution by separating and further back extracting the target valuable metal ions from the organic solvent. As the back extraction solution, for example, an aqueous solution in which nitric acid, hydrochloric acid, or sulfuric acid is diluted is preferably used. Moreover, the objective valuable metal ion can also be concentrated by changing suitably the ratio of an organic phase and an aqueous phase.

  The organic solvent may be any solvent as long as the extractant and the metal extraction species are dissolved, for example, a chlorinated solvent such as chloroform and dichloromethane, an aromatic hydrocarbon such as benzene, toluene, and xylene, Examples thereof include aliphatic hydrocarbons such as hexane. These organic solvents may be used alone or in combination, and alcohols such as 1-octanol may be mixed.

  The concentration of the extractant can be appropriately set depending on the type and concentration of the valuable metal. The stirring time and extraction temperature are appropriately set according to the conditions of the acidic aqueous solution of valuable metal ions and the organic solution of the extractant because the equilibrium time varies depending on the type and concentration of the valuable metal and the amount of extractant added. do it. The pH of the acidic aqueous solution containing metal ions can also be adjusted as appropriate depending on the type of valuable metal.

[Extraction of cobalt]
When efficiently recovering cobalt from an acidic aqueous solution containing cobalt and manganese, any amino derivative may be used as an extractant as long as it is the above-described amino derivative, among which normal-methylglycine derivative or histidine amide derivative Is preferable because it has a wide pH range and is more convenient for cobalt extraction industrially. About pH, it is preferable to add the organic solution of an extractant, adjusting the pH of the acidic aqueous solution containing cobalt and manganese to 3.5 or more and 5.5 or less, and adjusting the said pH to 4.0 or more and 5.0 or less More preferably, an organic solution of the extractant is added. If the pH is less than 3.5, cobalt may not be sufficiently extracted depending on the type of the extractant. When pH exceeds 5.5, depending on the kind of extractant, not only cobalt but also manganese may be extracted.

[Extraction of europium]
In order to efficiently recover europium from an acidic aqueous solution containing multiple types of rare earth metals such as europium and yttrium, and zinc, extraction is performed while adjusting the pH of the acidic aqueous solution to 2.0 to 3.0. It is preferred to add an organic solution of the agent. If the pH is less than 2.0, europium cannot be sufficiently extracted, which is not preferable. If the pH exceeds 3.0, not only europium but also other rare earth metals such as yttrium are extracted, which is not preferable.

[Selective extraction of rare earth elements]
The extractant of the present invention is characterized in that light rare earth elements and medium rare earth elements are easier to extract than heavy rare earth elements, compared with the conventionally known extractant DODGAA. For this reason, after adjusting the pH of the solution containing both heavy rare earth elements and light rare earth elements, the light rare earth elements are extracted from the solution by contacting with the extractant of the present invention, and the heavy rare earth elements are extracted. Separation can be achieved by distributing the liquid. In the case of a solution that also contains medium rare earth elements, it is possible to separate light rare earth elements and medium rare earth elements by bringing DODGAA into contact again with the solution back-extracted from the above extractant. .

  In order to efficiently recover light rare earth elements from an acidic aqueous solution containing heavy rare earth elements and light rare earth elements, the pH of the acidic aqueous solution containing heavy rare earth elements and light rare earth elements is set to 1.7 or more and 2.7 or less. It is preferable to add an organic solution of the extractant while adjusting, more preferably, an organic solution of the extractant is added while adjusting the pH to 1.9 to 2.5, and the pH is adjusted to 2.1 to 2. More preferably, the organic solution of the extractant is added while adjusting to 4 or less. When the pH is less than 1.7, the separation of the heavy rare earth element and the light rare earth element is not complete, and as a result, the light rare earth element may not be sufficiently extracted. If the pH exceeds 2.7, not only light rare earth elements but also heavy rare earth elements are extracted, resulting in low selectivity of rare earth elements, which is not preferable.

  Although the mechanism by which the extractant of the present invention takes an extraction behavior different from that of the conventional extractant is not exactly known, it is considered that an effect that has not been obtained conventionally is obtained by the structural characteristics of the extractant of the present invention.

  EXAMPLES Hereinafter, although an Example demonstrates this invention further in detail, this invention does not receive a restriction | limiting at all in these description.

<Example 1> (Synthesis of glycinamide derivative)
As an example of an amide derivative used as an extractant, a glycinamide derivative represented by the following general formula (I), that is, N- [N, N-bis (2-ethylhexyl) aminocarbonyl into which two 2-ethylhexyl groups are introduced Methyl] glycine (N- [N, N-Bis (2-ethylhexyl) aminocarbonylmethyl] glycine) (or N, N-di (2-ethylhexyl) acetamido-2-glycine (N, N-di (2-ethylhexyl) acetamide) -2-glycine), hereinafter referred to as “D2EHAG”).

D2EHAG was synthesized as follows. First, as shown in the following reaction formula (II), 23.1 g (0.1 mol) of commercially available di (2-ethylhexyl) amine and 10.1 g (0.1 mol) of triethylamine were fractionated and mixed with chloroform. Then, 13.5 g (0.12 mol) of 2-chloroacetyl chloride was added dropwise, then washed once with 1 mol / l hydrochloric acid, then with ion-exchanged water, and the chloroform phase was separated. did.
Next, an appropriate amount (about 10 to 20 g) of anhydrous sodium sulfate was added and dehydrated, followed by filtration to obtain 29.1 g of a yellow liquid. When the structure of this yellow liquid (reaction product) was identified using a nuclear magnetic resonance analyzer (NMR), the yellow liquid was identified as 2-chloro-N, N-di (2-ethylhexyl) acetamide (hereinafter “ CDEHAA ”)). The yield of CDEHAA was 90% with respect to di (2-ethylhexyl) amine as a raw material.

Next, as shown in the following reaction formula (III), methanol is added to and dissolved in 8.0 g (0.2 mol) of sodium hydroxide, and the solution in which 15.01 g (0.2 mol) of glycine is further added is stirred. Then, 12.72 g (0.04 mol) of the above CDEHAA was slowly added dropwise and stirred. After completion of the stirring, the solvent in the reaction solution was distilled off, and chloroform was added to the residue to dissolve it. The solution was acidified by adding 1 mol / l sulfuric acid, washed with ion-exchanged water, and the chloroform phase was separated.
An appropriate amount of anhydrous magnesium sulfate was added to the chloroform phase for dehydration and filtration. The solvent was removed again under reduced pressure to obtain 12.5 g of a yellow paste. The yield based on the above CDEHAA amount was 87%. When the structure of the yellow paste was identified by NMR and elemental analysis, it was confirmed that it had a D2EHAG structure as shown in FIGS. The amide derivative of Example 1 was obtained through the above steps.

<Example 2> (Synthesis of normal-methylglycine derivative)
As another example of the amide derivative serving as an extractant, a normal-methylglycine derivative represented by the following general formula (I), that is, N- [N, N-bis (2- Ethylhexyl) aminocarbonylmethyl] sarcosine (N- [N, N-Bis (2-ethylhexyl) aminocarbonylmethyl) sarcosine) (or N, N-di (2-ethylhexyl) acetamido-2-sarcosine (N, N-di (2 -Ethylhexyl) acetamide-2-sarcosine), hereinafter referred to as "D2EHAS").

The synthesis of D2EHAS was performed as follows. As shown in the following reaction formula (IV), methanol is added to and dissolved in 5.3 g (0.132 mol) of sodium hydroxide, and 11.8 g (0.132 mol) of sarcosine (N-methylglycine) is further added. While stirring, 36.3 g (0.12 mol) of the above CDEHAA was slowly added dropwise and stirred. After completion of the stirring, the solvent in the reaction solution was distilled off, and chloroform was added to the residue to dissolve it. The solution was acidified by adding 1 mol / l sulfuric acid, washed with ion-exchanged water, and the chloroform phase was separated.
An appropriate amount of anhydrous magnesium sulfate was added to the chloroform phase for dehydration and filtration. The solvent was removed again under reduced pressure to obtain 26.8 g of a tan paste. The yield based on the above CDEHAA amount was 60%. When the structure of the yellow paste was identified by NMR and elemental analysis, it was confirmed to have a D2EHAS structure. The amide derivative of Example 2 was obtained through the above steps.

Reference Example 3 (Synthesis of histidine amide derivative)
As another example of an amide derivative serving as an extractant, a histidine amide derivative represented by the following general formula (I), that is, N- [N, N-bis (2-ethylhexyl) into which two 2-ethylhexyl groups are introduced Aminocarbonylmethyl] histidine (N- [N, N-Bis (2-ethylhexyl) aminocarbonylmethyl) histidine) (or N, N-di (2-ethylhexyl) acetamido-2-histidine (N, N-di (2-ethylhexyl)) ) Acetamide-2-histidine), hereinafter referred to as “D2EHAH”).

The synthesis of D2EHAH was performed as follows. As shown in the following reaction formula (V), methanol was added to 16 g (0.4 mol) of sodium hydroxide to dissolve it, and further, 31.0 g (0.2 mol) of histidine was further added, while stirring, the CDEHAA13. 2 g (0.04 mol) was slowly added dropwise. After completion of dropping, the mixture was stirred while maintaining alkaline conditions. After completion of the stirring, the solvent in the reaction solution was distilled off, and the residue was dissolved by adding ethyl acetate. This solution was washed and the ethyl acetate phase was separated.
An appropriate amount of anhydrous magnesium sulfate was added to the ethyl acetate phase for dehydration and filtration. The solvent was removed again under reduced pressure to obtain 9.9 g of a tan paste. The yield based on the above CDEHAA amount was 57%. When the structure of the yellowish brown paste was identified by NMR and elemental analysis, it was confirmed to have the structure of D2EHAH. The amide derivative of Reference Example 3 was obtained through the above steps.

<Comparative Example 1>
As Comparative Example 1, a commercially available carboxylic acid-based cobalt extractant (trade name: VA-10, neodecanoic acid, manufactured by Hexion Specialty Chemicals Japan) was used.

<Comparative example 2>
As Comparative Example 2, N, N-dioctyl-3-oxapentane-1,5-amidic acid (hereinafter referred to as “DODGAA”), which is a conventionally known europium extractant, was used.

The synthesis of DODGAA was performed as follows. First, as shown in the following reaction formula (VI), 4.2 g of diglycolic anhydride was placed in a round bottom flask and suspended in 40 ml of dichloromethane. Thereafter, 7 g of dioctylamine (purity 98%) was dissolved in 10 ml of dichloromethane and slowly added with a dropping funnel. While stirring at room temperature, it was confirmed that diglycolic anhydride reacted and the solution became transparent, and the reaction was terminated.

  Subsequently, the solution was washed with water to remove water-soluble impurities. Then, sodium sulfate was added as a dehydrating agent to the solution after washing with water. The solution was filtered with suction, and then the solvent was evaporated. And after recrystallizing (three times) using hexane, it vacuum-dried. The yield of the obtained substance was 9.57 g, and the yield based on the above diglycolic anhydride was 94.3%. And when the structure of the obtained substance was identified by NMR and elemental analysis, it was confirmed that it was DODGAA having a purity of 99% or more.

<Extraction of cobalt>
Using the compounds of Examples 1 and 2, Reference Example 3 and Comparative Example 1, cobalt was extracted and separated.

[Examples 1 and 2 and Reference Example 3 ]
Contains several kinds of sulfuric acid acidic solution containing 1 × 10 ⁻⁴ mol / l of cobalt and manganese and pH adjusted to 2.5 to 7.5, and 0.01 mol / l of valuable metal extractant with the same volume. The normal dodecane solution was added to a test tube, placed in a thermostatic chamber at 25 ° C., and shaken for 24 hours. At this time, the pH of the sulfuric acid solution was adjusted using sulfuric acid, ammonium sulfate and ammonia having a concentration of 0.1 mol / l.

After shaking, the aqueous phase was separated, and the cobalt concentration and the manganese concentration were measured using an induction plasma emission spectrometer (ICP-AES). The organic phase was back extracted with 1 mol / l sulfuric acid. And the cobalt concentration and manganese concentration in a back extraction phase were measured using ICP-AES. From these measurement results, the extraction rate of cobalt and manganese was defined by the quantity in the organic phase / (the quantity in the organic phase + the quantity in the aqueous phase). FIG. 3 shows the results when using the amide derivative of Example 1, FIG. 4 shows the results when using the amide derivative of Example 2, and shows the results when using the amide derivative of Reference Example 3. As shown in FIG. The horizontal axis of FIGS. 3-5 is pH of a sulfuric acid acidic solution, and a vertical axis | shaft is the extraction rate (unit:%) of cobalt or manganese. In the graph, squares indicate cobalt extraction rates, and circles indicate manganese extraction rates.

[Comparative Example 1]
Except that the pH of the sulfuric acid acidic solution was adjusted to 4.0 to 7.5 and that the concentration of the normal decane solution containing the amide derivative was 0.1 mol / l, which is 10 times that of the example, Cobalt was extracted by the same method. The results are shown in FIG. The horizontal axis of FIG. 6 is the pH of the sulfuric acid acidic solution, and the vertical axis is the extraction rate (unit:%) of cobalt or manganese. In the graph, the square indicates the extraction rate of cobalt, and the diamond shape indicates the extraction rate of manganese.

  When the amide derivative of the example was used, it was confirmed that cobalt could be extracted at an extraction rate exceeding 20% within a pH range of 3.0 to 5.5 (FIGS. 3 to 5). In particular, when a normal-methylglycine derivative or a histidine amide derivative was used, it was confirmed that the preferred pH range was wide and more convenient when industrially performing the cobalt extraction of the present invention (FIG. 4, FIG. 4). 5). Regardless of the type of derivative, it was confirmed that in the range of pH 4.0 to 5.0, cobalt can be extracted at an extraction rate exceeding 80%, and manganese is hardly extracted (FIG. 3). FIG. 5). On the other hand, when the amide derivative of Comparative Example 1 was used, it was confirmed that cobalt could be extracted only with an extraction rate of less than 20% even when the concentration of the extractant was 10 times that of the Example (FIG. 6).

<Extraction of Europium>
Europium was extracted and separated using the compounds of Example 1 and Comparative Example 2.

[Example 1]
A normal decane solution containing several kinds of acidic solutions each containing 1 × 10 ⁻⁴ mol / l of yttrium, europium and zinc and adjusting the pH to 1 to 4 and 0.01 mol / l of valuable metal extractant of the same volume Was added to a test tube, placed in a thermostatic chamber at 25 ° C., and shaken for 24 hours. At this time, the pH of the acidic solution was adjusted using nitric acid, acetic acid and sodium acetate having a concentration of 0.1 mol / l.

  After shaking, the aqueous phase was separated and the yttrium concentration, europium concentration and zinc concentration were measured using ICP-AES. The organic phase was back extracted with 1 mol / l nitric acid. And the yttrium density | concentration in the back extraction phase, the europium density | concentration, and the zinc density | concentration were measured using ICP-AES. From these measurement results, the extraction rates of yttrium, europium and zinc were defined and determined by the amount in the organic phase / (the amount in the organic phase + the amount in the aqueous phase). The results are shown in FIG. The horizontal axis in FIG. 7 is the pH of the acidic solution, and the vertical axis is the extraction rate of yttrium, europium, and zinc.

[Comparative Example 2]
Europium was extracted by the same method as in Example except that the pH of the sulfuric acid acidic solution was adjusted to 1.2 to 2.2. The results are shown in FIG.

When the amide derivative of Example 1 is used, europium can be extracted at an extraction rate exceeding 40% in the range of pH 2.0 to 3.0, and the extraction rate of europium and the extraction rate of yttrium It was confirmed that a significant difference was found between them (FIG. 7). On the other hand, when the compound of Comparative Example 2 was used, europium could be extracted at a high extraction rate, but yttrium was also extracted at a high extraction rate, so that it was confirmed that europium and yttrium could not be separated (FIG. 8).

（式中、Ｃ _８ Ｈ _１７ は分鎖であり、Ｒは水素原子又はアルキル基を示す。） Thus, by using a valuable metal extractant composed of an amide derivative represented by the following general formula, cobalt can be efficiently recovered from a used secondary battery, and europium and three-wavelength fluorescent tubes and It was confirmed that yttrium can be separated and recovered efficiently.

(In the formula , C ₈ H ₁₇ is a branched chain, and R represents a hydrogen atom or an alkyl group .)

<Extraction of light rare earth metals>
Using the amide derivative of Example 1, light rare earth metal was extracted and separated from an acidic solution containing a plurality of types of rare earth metals.
It contains 1 × 10 ⁻⁴ mol / l each of lanthanum (La) and cesium (Ce), which are light rare earth metals, and thulium (Tm) and ytterbium (Yb), which are heavy rare earth metals, and has a pH of 1.1 to 3. Four kinds of nitric acid acidic solution adjusted to .4 and a normal dodecane solution containing 0.01 mol / l of valuable metal extractant in the same volume were added to a test tube and placed in a thermostatic chamber at 25 ° C. and shaken for 24 hours. . At this time, the pH of the acidic solution was adjusted using nitric acid, ammonium nitrate and ammonia having a concentration of 0.1 mol / l.

  After shaking, the aqueous phase was separated and the concentration of each rare earth metal was measured using ICP-AES. The organic phase was back extracted with 2 mol / l nitric acid. And the density | concentration of each rare earth metal in a back extraction phase was measured using ICP-AES. From these measurement results, the extraction rate of each rare earth metal was defined by the quantity in the organic phase / (the quantity in the organic phase + the quantity in the aqueous phase). The results are shown in FIG. The horizontal axis in FIG. 9 is the pH of the acidic solution, and the vertical axis is the extraction rate of the rare earth metal.

  When the amide derivatives of the examples were used, it was confirmed that light rare earth metals can be selectively extracted from an acidic solution containing a plurality of types of rare earth metals within a pH range of 1.7 to 2.7 (FIG. 9). ). In particular, in the range of pH 1.9 or more and 2.5 or less, it was confirmed that light rare earth metals can be extracted with an extraction rate exceeding 30% and that heavy rare earth metals are hardly extracted (FIG. 9). In addition, when the pH is in the range of 2.1 to 2.4, light rare earth metals can be extracted with an extraction rate exceeding 50%, and the extraction rate of heavy rare earth metals is significantly small in view of the extraction rate of light rare earth metals. It was confirmed.

  When the compound of Comparative Example 2 is used, the heavy rare earth metal is extracted with priority over the light rare earth metal, and thus it cannot be said that the light rare earth metal can be extracted with higher efficiency than the amide derivatives of the examples.

Claims (1)

Amide derivatives represented by the following general formula .

(In the formula , C ₈ H ₁₇ is a branched chain, and R represents a hydrogen atom or an alkyl group .)

Images