JPS6221059B2 - - Google Patents

Description

[Detailed description of the invention]

The present invention relates to a method for separately recovering molybdenum, uranium, and vanadium from materials in which molybdenum, uranium, and vanadium coexist (for example, ores or chemical precipitates). Naturally occurring molybdenum and uranium ores often contain molybdenum, uranium, and vanadium, although the amounts vary. However, there are currently few reports on the separate recovery of molybdenum, uranium, and vanadium contained in the leachate obtained by leaching ores with sulfuric acid. Generally, coexisting molybdenum, uranium, and vanadium are leached out, and molybdenum, uranium, and vanadium are extracted from the leachate.
When separately recovering vanadium, it is better to separate and recover uranium first. The coprecipitation method, foaming separation method, adsorption method, and solvent extraction method are known as methods for fractional recovery of uranium, but these methods are extremely excellent methods for concentrating, separating, and purifying uranium. It is also used in uranium crude smelting plants. However, the form of molybdenum, uranium, and vanadium is Mo (~
Because they have many valences and similar properties, such as valence), U (~ valence), and V (~V valence), precipitation separation by direct neutralization is difficult. Furthermore, if the concentration of molybdenum is higher than that of uranium or vanadium, contamination of molybdenum with uranium cannot be avoided. For example, if a coexistence of molybdenum, uranium, and vanadium is leached with sulfuric acid and an alkaline agent is added to the leachate to neutralize it, uranium will almost completely precipitate at pH 6, but vanadium will also begin to precipitate slightly at pH 4. Molybdenum hardly precipitates, but if the molybdenum concentration is high, there will be a considerable amount of contamination. Furthermore, in a reduced state, molybdenum, uranium, and vanadium all precipitate, making separation difficult. Chemicals added for uranium co-precipitation include ferric salts such as ferric chloride or ferric ammonium sulfate, and aluminum salts such as aluminum sulfate or aluminum phosphate. In either case, molybdenum and vanadium may also precipitate due to pH adjustment, which is not appropriate. Furthermore, as a foaming separation method, foaming separation of uranium in seawater was attempted using surfactants such as soda soap, sodium lauryl sulfate, and laurylamine acetic acid. There have also been reports on the adsorption of uranium using ferric oxide, iron sulfide, titanic acid, or various metal soaps as organic adsorbents, but these methods are difficult to apply to sulfuric acid acidic solutions containing uranium, molybdenum, and vanadium. . On the other hand, direct separation using ion-exchange resins includes separation of uranium and vanadium in alkaline leaching, separation of molybdenum and vanadium from acidic solutions, etc., but separation of molybdenum, uranium, and vanadium-containing liquids using cation- and anion-exchange resins. This is difficult, especially for molybdenum and uranium. Uranium and molybdenum behave similarly when extracted and separated using organic solvents, and are extracted in the same way at pH values below 0.5, and although separation from vanadium is possible to some extent, it is difficult to completely separate them. There are examples of solvent extraction being used for crude separation; for example, after extracting molybdenum, uranium, and vanadium using a tertiary amine, uranium is back-extracted with sodium chloride, and then molybdenum is extracted with sodium carbonate. Although reverse extraction is performed, vanadium is mixed into the uranium cake, and uranium and vanadium are mixed into the molybdenum precipitate, making separation difficult. Particularly when the concentration of molybdenum in the leachate is 10 to 30 times higher than that of uranium or vanadium, it is difficult to separate uranium using any method for separating uranium alone due to the influence of molybdenum. Therefore, it is difficult to first separate and recover uranium from the above-mentioned three-component mixture, and there is currently no good method, so it is necessary to find another separation method. As a result of various studies, the present inventors discovered another method for separately recovering molybdenum, uranium, and vanadium dissolved in the sulfuric acid leachate. Through this method, molybdenum, uranium, and vanadium, which were conventionally difficult to separate, can be recovered as single raw materials or was made recoverable as a product, and the present invention was completed. That is, the present invention performs sulfuric acid leaching of coexisting molybdenum, uranium, and vanadium such as ores or chemical precipitates, and removes molybdenum, uranium, and vanadium dissolved in the leachate.
Of vanadium, molybdenum is first removed as sulfide, and then uranium is adsorbed using an ion exchange resin and separated from vanadium, thereby providing a method for recovering molybdenum, uranium, and vanadium. , A first step in which coexisting substances containing molybdenum, uranium, and vanadium are acid-leached using a mineral acid and the leaching residue is separated; A sulfiding agent is added to the leachate obtained in the first step and reacted, and the resulting precipitate is The second step is to collect items separately.
A third step of adding an oxidizing agent to the liquid obtained in the second step to oxidize it; Adding an alkaline agent to the oxidized liquid in the third step to neutralize it and adjusting the pH to 7 to 8. The fourth step is to separate the precipitate obtained in the fourth step. Mineral acid is added to the precipitate obtained in the fourth step, and the PH
The fifth step consists of dissolving in steps 1 and 2, a step of blowing hydrogen sulfide gas into the solution obtained in the fifth step to reduce it, a step of heating to drive out the hydrogen sulfide, and a step of separating the generated precipitate. 6th step, 7th step in which the liquid separated in the 6th step is passed through an ion exchange resin, an alkali agent is added to the liquid that has passed through the 7th step, and the pH is increased to 6th step.
7, and separately collect the generated precipitate; a ninth step, in which the adsorbed matter on the ion exchange resin in the seventh step is eluted using an alkaline salt solution; and the liquid eluted in the ninth step. A 10th step of adding mineral acid to make it acidic, adjusting the pH to 7 to 10 with an alkaline agent, and separately collecting the generated precipitate.Molybdenum, uranium,
This is a valuable metal recovery method that separates and recovers vanadium. The details of the present invention will be explained below. Regarding the first step. In this process of leaching crushed ores or chemical precipitates that coexist with molybdenum, uranium, and vanadium, sulfuric acid, which is common as a mineral acid and is inexpensive, is used, and the concentration of free sulfuric acid in the solution after leaching is 50 g/ One stage of leaching is carried out at normal temperature and pressure to achieve the above results, and after over-separation, if necessary, the entire amount of the residue is wet-pulverized (in this case, the pulp that has been sedimented and concentrated can also be wet-pulverized as it is without over-separation), and sulfuric acid is added. and perform the second leaching step. At this time, the sulfuric acid concentration as the leaching solution should be 300 g/min or more, and this solution, including the washing solution for the residue after the 2nd stage leaching, should be used as the leaching solution for the 1st stage leaching. Adjust the concentration and amount of cleaning solution. The reason why the free sulfuric acid concentration of the liquid after the first stage leaching is specified as 50 g/or more is to ensure the necessary acid concentration in the next second step. The above is the following:
This is because the leaching rate of each component, especially molybdenum and vanadium, decreases. Furthermore, precipitation of gypsum due to calcium contained in the coexisting substances and undissolved residues are removed, and if necessary, gypsum can be recovered by flotation. Regarding the second process. The free sulfuric acid concentration of the obtained leachate shall be 50 g/min or more. Figure 1 shows the relationship between free sulfuric acid concentration and molybdenum sulfide production rate. Further, the temperature is required to be 40°C or higher, and preferably after heating to 60 to 80°C, hydrogen sulfide gas is introduced to separate molybdenum in the liquid as molybdenum sulfide. At temperatures below 40°C, the amount of molybdenum sulfide produced is small, and higher temperatures are more advantageous in terms of transient properties. Figure 2 shows the relationship between reaction temperature and molybdenum sulfide production rate. The molybdenum eluted by sulfuric acid leaching in the first step is dissolved in a strong acidic solution with pH<1.
It exists as MoO ₂ SO ₄ in , and is thought to react with hydrogen sulfide to produce molybdenum sulfide in the following manner. MoO ₂ SO ₄ +3H ₂ S→MoS ₂ +H ₂ SO ₄ +2H ₂ O+S
...(1) A small amount of hydrogen sulfide exhibits a blue color and does not form a precipitate, so by supplying a sufficient amount of 3 equivalents or more as shown in reaction formula (1), a brown-black precipitate is gradually formed.
Further, vanadium ions in the leachate exist as VO ₂ ⁺ in a strongly acidic region and are colorless, but may be yellow to orange as polyacids, and are reduced by hydrogen sulfide to become VO ²⁺ and V ³⁺ . At this time, hydrogen sulfide is consumed, so if the vanadium concentration is high, the hydrogen sulfide gas is recovered in order to recover molybdenum as molybdenum sulfide, taking into account the amount of dissolved molybdenum and vanadium and the solubility of hydrogen sulfide gas in the liquid at the reaction temperature. Quantity is required. Naturally, in this case, the reactor should be highly airtight, and if the reaction is carried out under pressure, molybdenum sulfide can be quantitatively precipitated, and the recovery rate can be further improved. Note that instead of hydrogen sulfide gas, hydrogen sulfide water, sodium hydrogen sulfide, sodium sulfide, or other elemental sulfur, sulfide, etc. that react with free acid to generate hydrogen sulfide can be used. The molybdenum sulfide obtained in this process is purified,
It can be recovered as molybdenum trioxide. Regarding the third step. The liquid from which molybdenum was separated in the second step is in a reduced state, and when this liquid is neutralized with an alkaline agent,
At around pH 5, uranium and vanadium begin to precipitate, and even before the entire amount of uranium is precipitated, residual molybdenum also begins to precipitate. Figure 3 shows the relationship between the pH and the concentration remaining in the liquid when each hydroxide is precipitated in the neutralization of uranium, vanadium, and molybdenum in a reduced state. It is necessary to suppress the precipitation of this molybdenum, so hydrogen peroxide is added as an oxidizing agent to oxidize it. At this time, add an oxidizing agent until the standard monopolar potential reaches 500 mV or more to suppress precipitation of molybdenum. The relationship between the PH and the residual concentration in the liquid when precipitating each hydroxide during neutralization of uranium, vanadium, and molybdenum in a liquid with an oxidizing agent brought to 500 mV is shown in the fourth section.
As shown in the figure. Further, in place of hydrogen peroxide, persulfates, chlorine, hypochlorites, chlorates, and other compounds such as oxyrite, which produce hydrogen peroxide upon contact with water, can be used. Regarding the fourth step. In the third step, an alkaline agent is added to the oxidized solution and the pH is adjusted to 7 to 8, thereby forming uranium and vanadium precipitates and separating them. At this time, sodium hydroxide is used as the alkaline agent, but calcium hydroxide may be used instead. In the first step, sulfuric acid is used as the mineral acid in the leachate, and when calcium hydroxide is used, it is neutralized in two stages, and in the first stage, free sulfuric acid is separated as gypsum using calcium carbonate, and the separated liquid is Further, calcium hydroxide may be added to form a vanadium precipitate that co-precipitates all and a portion of uranium. Calcium hydroxide is further added to the separated liquid to recover residual molybdenum and vanadium. The collected precipitate can be repeated in the leaching process. This step can be omitted if the residual molybdenum concentration is 1g/or less, but if an ion exchange resin is used to separate uranium and vanadium in the seventh step, the amount of uranium concentration and liquid passing should be minimized. It is also a process for Regarding the fifth step. Dilute sulfuric acid is added to and dissolved in the uranium and vanadium hydroxide obtained in the fourth step. At that time, the dissolved pH
A value of 1 to 2 is selected because molybdenum sulfide is produced well at room temperature and uranium is adsorbed to the ion exchange resin. However, if there are undissolved components, the pH is adjusted using high-concentration sulfuric acid after dissolution. The relationship between PH at room temperature and the residual concentration due to the formation of molybdenum sulfide is shown in the fifth section.
As shown in the figure. Regarding the 6th step. Hydrogen sulfide gas is again introduced into the solution obtained in the fifth step to bring the solution into a reduced state, and the molybdenum in the solution adhering to the uranium precipitate separated in the fourth step is precipitated, and then the dissolved To remove the hydrogen sulfide present, heat to 60°C or higher, cool and separate. In this process, hydrogen sulfide gas is introduced again,
The reason for separating the precipitate is that pentavalent vanadium is adsorbed by the resin, so it must be reduced, and if a large amount of molybdenum remains,
This is because the amount of molybdenum in the liquid must be reduced as much as possible since the phenomenon of molybdenum being adsorbed by the resin occurs. In this case, a pH around 2 gives good results, but depending on the concentration of vanadium and uranium, these may precipitate, so it is desirable to feed hydrogen sulfide gas at a pH of 1.5. Furthermore, heating is necessary to release excess hydrogen sulfide dissolved in the liquid from the liquid, since this shortens the life of the ion exchange resin. Regarding the 7th process. The reduced solution obtained in the sixth step is passed through a strongly basic anion exchange resin. At this time, the amount of molybdenum in the solution is reduced to 0.1 g or less by the operations up to the sixth step, and the adsorption of uranium is not affected and vanadium passes through without being adsorbed. Furthermore, since an anion exchange resin is used, most divalent cations such as calcium and sodium are not adsorbed, which is very advantageous in increasing the purity of recovered uranium. The adsorption reaction of uranium by a strongly basic anion exchange resin is as follows. _{UO 2} ⁽ _{SO 4} ^{) 4− 3 +} _{4R + _} ^_ _{_ _} ^_ _{_} ^_ X ^- 〓 R ₂ ⁺ UO ₂ (SO ₄ ) ^2- ₂ + 2X ^- ... (3) However, R ⁺ is quaternary amine resin, X is NO ₃ ^- ,
Cl ^- , HSO ₄ ^- , 1/2SO ^2-4 Uranium is adsorbed on anion exchange resin regardless of its valence, but vanadium is adsorbed with a valence of 5 and not with other valences _, so sulfide is added to the solution. Hydrogen gas is blown in to reduce vanadium, and uranium is adsorbed 100% better at pH 1 to 2 than in strong acidity. If the pH is higher than 2, vanadium and uranium will precipitate, so this step is performed at a pH of 1.5. A strongly basic anion exchange resin is used as the SO ₄ type resin, and the resin is washed with 5 g of H ₂ SO ₄ before use. Regarding the 8th step. The liquid that passed through the resin in the seventh step exists as sky blue vanadium ions (VO ⁺⁺ or V ⁺⁺⁺ ), so by adding an alkali agent, vanadium is converted to VO (OH) at a pH of 6 to 7. ₂ and V
(OH) ₃ is precipitated and separated and collected. Since this precipitate contains divalent cations that are not adsorbed to the resin, further purification is required, but the recovered vanadium hydroxide can be made into a product as vanadium pentoxide by calcining. Regarding the 9th process. Elution of uranium adsorbed to ion exchange resin is normal.
Either 1M nitrate solution or 1M chloride solution is used. The reaction is as follows. R ₄ UO ₂ (SO ₄ ) ₃ +4X ^- 4RX + UO ^2- ₂ +3SO _{4 ...} (4) However, X = NO ₃ ^- or Cl ^- adsorbed uranium is eluted as shown in reaction formula (4). Therefore, in the seventh step, uranium adsorbed on the resin is eluted using a 1M sodium chloride solution. At this time, the addition of sodium carbonate allows uranium to be eluted in a short time, which is effective for concentrating and separating uranium. However, if molybdenum is present, the use of sodium carbonate is undesirable because it lowers the purity of uranium. Regarding the 10th process. If the uranium solution eluted with sodium chloride or sodium chloride and sodium carbonate has carbonate radicals, it will form a uranyl carbonate complex by adding an alkaline agent and will not completely precipitate. Therefore, use hydrochloric acid as a mineral acid to reduce the pH to 3 or less. Remove carbonate roots as
Figure 6 shows the relationship between pH and residual carbon dioxide concentration in the liquid.
Next, an alkali agent is added to adjust the pH to 7 to 10, and uranium is recovered as uranate. At this time, in addition to sodium hydroxide, aqueous ammonia and calcium hydroxide can be used as the alkaline agent. The precipitation form of uranium is U ₃ O ₈ when pH is 6 to 7.
(OH) ₂ is Na ₂ U ₂ O ₂₂ at pH 9.6 and Na ₆ O ₇ O ₂₄ at pH 10, and can be separated and recovered at pH 6 or higher. Uranate precipitation can occur at pH 6 or above, but as can be seen from the above precipitation forms by pH, U ₃ O ₈ (OH) ₂ is a desirable precipitation form.
It is advantageous to precipitate at pH 7-8 in order to obtain . As described above, the present invention is an extremely useful method that allows molybdenum, uranium, and vanadium to be separately recovered and manufactured into products more efficiently than coexisting molybdenum, uranium, and vanadium. The present invention will be explained in more detail below with reference to Examples. Example 1 Molybdenum, uranium,
A method for separately recovering vanadium will be shown.

[Table] Next, 500 g of the chemical precipitate was added to Solution 5 with a sulfuric acid concentration of 105 g/ml, and leaching was performed at room temperature for 1 hour. The composition of the leachate is shown in Table 2.

[Table] Next, the entire amount of the obtained residue was wet-pulverized, and then leached with Solution 5 having a free sulfuric acid concentration of 376 g/min, and the residue was washed after filtration. The residue after the two-stage leaching and cleaning is shown in Table 3.

【table】 Table 4 shows the overall leaching rates for the first and second stages.

[Table] Next, after heating the leachate 5 obtained in Table 2 to 80°C, flowing hydrogen sulfide gas at a flow rate of 2.0/min for 60 minutes, stopping the hydrogen sulfide gas and stirring until left to cool. I went there. The molybdenum sulfide thus produced was separated, washed and dried, and the composition is shown in Table 5. The weight of the molybdenum sulfide obtained is
It was 259g.

[Table] At this time, the recovery rate of molybdenum as molybdenum sulfide from the leachate was 78.9%. Next, the liquid composition of the liquid excluding molybdenum sulfide is shown in Table 6. Although the high concentration of molybdenum seems to be due to the airtightness of the reaction vessel, it was taken as a good example of the reaction process.

[Table] After adding hydrogen peroxide solution to the above Mo removal solution 5 and making the standard monopolar potential more than 500mV,
The solution after adding sodium hydroxide and adjusting the pH to 7 and separating the generated precipitate (including washing solution) 5.8
The composition of is shown in Table 7.

[Table] Further, sulfuric acid was added to the precipitate, and after dissolving it, hydrogen sulfide gas was blown into the solution to reduce it.Then, in order to remove excess hydrogen sulfide in the solution, it was heated to 70-80℃, and then cooled to remove the formed precipitate. Separated. The composition of the separated liquid 2 is shown in Table 8.

[Table] Table 9 shows the composition of the passing liquid 2 when the liquid shown in Table 8 was passed through a strong basic acid anion exchange resin. This liquid is used to recover vanadium.

[Table] As shown in Table 9, uranium was almost completely adsorbed, and vanadium remained unadsorbed. Next, uranium was eluted using 1M NaCl and 1M NaCO ₃ solutions, and the composition of the eluted solution 1 is shown in Table 10.

[Table] Next, add hydrochloric acid to the eluent in Table 10 to drive out the carbonate radicals, and then adjust the pH to 7 with sodium hydroxide.
Table 11 shows the composition of 8.3 g of uranate obtained when uranium was precipitated and separated.

[Table] On the other hand, the ion exchange resin permeate 2 shown in Table 9
Add calcium carbonate to the solution, precipitate 19g of gypsum at pH 2, and add calcium hydroxide after excessive separation.
Table 12 shows the composition of vanadium hydroxide when the pH was adjusted to 7 and 9.3 g of vanadium hydroxide was produced and separated separately.

[Table] As a result of analyzing the separately separated liquid, the metal component was not detected. Furthermore, after adding calcium hydroxide to the separately separated liquid in Table 11 and adjusting the pH to 10, the metal component was not detected in the separately separated liquid. As described above, molybdenum, uranium, and vanadium can be recovered and concentrated as precipitates, and each metal can be recovered from these precipitates.

[Brief explanation of the drawing]

Figure 1 shows the relationship between the concentration of free sulfuric acid and the production rate of molybdenum sulfide when hydrogen sulfide gas is blown into the leachate to precipitate molybdenum sulfide. Figure 3 shows the relationship between the reaction temperature and the production rate of molybdenum sulfide when precipitating molybdenum sulfide. Figure 4 shows the relationship between the residual concentration in the liquid and the PH when precipitating each hydroxide in the neutralization of uranium, vanadium, and molybdenum in the liquid after adding an oxidizing agent and setting the standard monopolar potential to 500 mV and the residual concentration in the liquid. Figure 5 is a diagram of the relationship between PH at room temperature and the residual concentration due to the formation of molybdenum sulfide, Figure 6 is a diagram of the relationship between PH and the residual carbonate concentration in the liquid, and Figure 7 is the diagram of the relationship between PH and the residual concentration of molybdenum sulfide in the liquid. This is a process diagram.

Claims (1)

[Claims] 1. A first step of acid leaching a coexisting substance containing molybdenum, uranium, and vanadium using a mineral acid and separating the leaching residue. A sulfiding agent is added to the leachate obtained in the first step. The second step is to react and separately collect the generated precipitate.
A third step of adding an oxidizing agent to the liquid obtained in the second step to oxidize it; Adding an alkaline agent to the oxidized liquid in the third step to neutralize it and adjusting the pH to 7 to 8. The fourth step is to separate the precipitate obtained in the fourth step. Mineral acid is added to the precipitate obtained in the fourth step, and the PH
The fifth step consists of dissolving in steps 1 and 2, a step of blowing hydrogen sulfide gas into the solution obtained in the fifth step to reduce it, a step of heating to drive out the hydrogen sulfide, and a step of separating the generated precipitate. 6th step, 7th step in which the liquid separated in the 6th step is passed through an ion exchange resin, an alkali agent is added to the liquid that has passed through the 7th step, and the pH is increased to 6th step.
7, and separately collect the generated precipitate; a ninth step, in which the adsorbed matter on the ion exchange resin in the seventh step is eluted using an alkaline salt solution; and the liquid eluted in the ninth step. A 10th step of adding mineral acid to make it acidic, adjusting the pH to 7 to 10 with an alkaline agent, and separately collecting the generated precipitate.Molybdenum, uranium,
A valuable metal recovery method that separates and recovers vanadium. 2. The method for separate recovery according to claim 1, wherein the mineral acid used in the first step is sulfuric acid. 3 The mineral acid concentration in the first step is reduced to free acid in the leaching solution.
50g/or more of the method for sorting and collecting according to claim 1 or 2. 4 The first step, leaching with mineral acid, consists of two stages.
The leaching residue from the first stage is wet-pulverized as necessary, and mineral acid is supplemented and adjusted to have a mineral acid concentration of 300 g/min or more, and the second stage is leached. After solid-liquid separation, the liquid and cleaning solution are separated. Claim 1, in which this is used as the first-stage leaching stock solution or a part thereof;
The separate collection method described in paragraph 2 or 3. 5 The sulfurizing agent in the second step is hydrogen sulfide gas,
The separate recovery method according to claim 1, in which the substance is one or more selected from the group of sodium hydrogen sulfide, sodium sulfide, and elemental sulfur and sulfides that react with free acids to generate hydrogen sulfide. . 6 Claims 1, 2, and 3 in which the reaction with hydrogen sulfide is carried out at 40°C or higher and under normal pressure in the second step.
4. The method for separate collection as described in Section 4, Section 4, or Section 5. 7 The oxidizing agent in the third step is one or two selected from the group of hydrogen peroxide, persulfates, hypochlorites, chlorates, and other compounds that generate hydrogen peroxide upon contact with water. 2. The method for separate recovery according to claim 1, wherein the amount of addition is such that the standard apparent potential is 500 mV or more. 8. The method for separate recovery according to claim 1, wherein the alkaline agent used in the fourth step is sodium hydroxide or calcium hydroxide. 9 When calcium hydroxide is used in the fourth step, neutralization is carried out in two stages, the first stage is neutralized with calcium carbonate and/or calcium hydroxide until the pH is 2, the generated gypsum is separated, and then the second stage is 3. The method for separation and recovery according to claim 2, wherein the pH is further adjusted to 7 to 8 with calcium hydroxide in the second stage to form a precipitate. 10. The separation and recovery method according to claim 1, wherein the mineral acid used in the fifth step is sulfuric acid. 11. The method for separate recovery according to claim 1, wherein the blowing of hydrogen sulfide gas in the sixth step is carried out at room temperature, and after the blowing and reduction, the hydrogen sulfide gas is heated to 60° C. or higher. 12. The method for fractional recovery according to claim 1, wherein the ion exchange resin used in the seventh step is a strongly basic anion exchange resin. 13. The method for separate recovery according to claim 1, wherein the alkaline agent used in the eighth step is one or more of sodium hydroxide, calcium carbonate, and calcium hydroxide. 14 When calcium carbonate or calcium hydroxide is used in the 8th step, neutralization is carried out in two stages, the first stage is to neutralize with calcium carbonate powder until the pH is 2, the gypsum component produced is separated, and then the carbonate is removed in the second stage. 11. The method for separation and recovery according to claim 2 or 10, wherein the pH is adjusted to 6 to 7 using calcium powder and/or calcium hydroxide powder to form a precipitate. 15. The method of fractional recovery according to claim 1, wherein the alkaline salt solution used in the ninth step is sodium chloride. 16. The method for fractional recovery according to claim 15, wherein sodium carbonate is further added to promote the elution of uranium in the ninth step. 17. The method for separate recovery according to claim 1, wherein the mineral acid used in the tenth step is hydrochloric acid, and the alkali agent is sodium hydroxide, aqueous ammonia, or calcium hydroxide. 18 The precipitate generated in the first step is gypsum,
A patent in which the precipitate produced in the second and sixth steps is molybdenum sulfide, the precipitate produced in the eighth step is vanadium hydroxide, and the precipitate produced in the tenth step is uranate. Claim 1
Term, 2nd term, 3rd term, 4th term, 5th term, 6th term,
Section 7, Section 8, Section 9, Section 10, Section 11,
Section 12, Section 13, Section 14, Section 15, Section 1
A method for separately recovering molybdenum, uranium, and vanadium from molybdenum, uranium, and vanadium coexisting materials according to item 6 or 17.