Process for selective separation of plutonium from uranium and other metals

Abstract

A process for selectively separating plutonium from uranium and other metals is disclosed wherein, in order to precipitate and remove the pertaining complexes, use is made of a sufficient quantity of a cationic compound containing at least one group adapted to assert affinity to polar surfaces and containing a radical which has little affinity to water, e.g. surface active agents and the like, and use is made of the capability of Pu.sup.4+ and U.sup.4+ to form nitrato-complexes and of the capability of Pu.sup.4+ and UO.sub.2.sup.2+ to form sulfato-complexes.

Description

BACKGROUND OF THE INVENTION

1. Field of the Invention

The present invention relates generally to improvements in or relating to processes for the selective separation of plutonium and uranium from one another and from other metals.

Nowadays, the processes of jointly separating plutonium and uranium from other metals and the separation of plutonium from uranium are almost always carried out using aqueous solutions. There are presently primarily two methods of particular interest, with each being used in several variations: the solvent extraction method and the ion exchange method. While both methods can, in general, be employed--also on a commercial scale--both still exhibit undesireable disadvantages.

Relative long residence times of organic solvents, agents adapted to form complexes, or resins, in higher radiation density ranges, lead to radiolytical destruction and, thereby, to losses in capacity and detrimental gas formation.

In the case of solvent extraction methods, the penetration of UO.sub.2.sup.2+ and Pu.sup.4+ through the phase boundary between water and organic solvent, as well as the concentration of precipitates at the phase boundary or interface, present kinetic problems.

When using the mixer-settler technique during solvent extraction, the stationary processing is rendered more difficult by density fluctuations in the organic and aqueous phases during successive extraction and re-extraction steps.

The reaction of ion exchange resins and complex-formers, e.g. tributylphosphate, with concentrated HNO.sub.3 presents an unnecessary danger potential.

The separation accuracy of solvent extraction processes, as well as ion exchange processes during the separation of uranium from plutonium, and in the separation of the two elements from one another, is of such a low extent that the separation is generally carried out in several successive steps.

These difficulties are already apparent in the case of relatively well defined solutions obtained, for example, by the dissolution of nuclear fuel elements in concentrated HNO.sub.3. Additional difficulties are encountered in such processing when nonuniform solutions are treated, which possibly also contain difficult to define organic materials of fluctuating composition. For such waste waters there have not been advanced fully satisfactory treatment processes so that also the recovery of nuclear fuel elements from such waste waters, the transport, and the storage of remaining residues have not been solved satisfactorily.

2. Description of the Prior Art

A flotation process for inorganic ions has been described in DE-AS No. 1 166 113 (DE-AS=German patent publication) in which process in conformity with the loading of the ion to be floated, there is added to the ion-containing solution an anionic or cationic collector and in which the so-formed insoluble reaction product is floated or slurried under introduction of a gas and removed as a foam or froth. In accordance with this prior art process the uranium may be separated from uranylsulfate solutions, albeit with poor yields.

In German Pat. No. 2 817 029 there is disclosed a process for selectively separating and recovering uranium from accompanying metals. In accordance with this prior art process hydrochloric acid is added to an aqueous solution containing uranium until the UO.sub.2.sup.2+ forms anionic chloro-complexes, a surface active agent is added, and the resultant precipitate is floated in a flotation cell. Uranium is recovered from the floated precipitate. While this prior art process allows recovery of uranium at a higher yield in comparison to the process of German patent publication No. 1 166 113, its particular drawbacks reside therein that it is based on the use of hydrochloric acid and, accordingly, can not be utilized on a larger scale without precautionary measures due to corrosion.

In accordance with German Pat. No. 2 902 516, the process of German Pat. No. 2 817 029 is extended to solutions containing sulfuric acid. This provides yields and concentrations of uranium which are superior in comparison with the process of German patent publication No. 1 166 113. However, the flotation time is longer and the concentration or enriching is lower than suggested by the process according to German Pat. No. 2 817 029; on the other hand, the corrosion dangers have been reduced.

In any event, the foregoing references do not provide a teaching of how to separate plutonium from uranium by means of particular organic compound-assisted precipitation.

SUMMARY OF THE INVENTION

There has continued to remain, therefore, a need to provide a new or improved process of separating uranium and plutonium which process does not exhibit the drawbacks indicated briefly in the foregoing, or only to a lesser extent.

In general terms, it was investigated whether plutonium could be precipitated from aqueous solutions as a substantially insoluble precipitate, either as a cation or as complex anion, using either anionic or cationic compounds containing at least one group adapted to assert affinity to polar surfaces and also containing a radical which has little affinity to water, whereby the plutonium could be separated, in this manner, selectively from uranium or other elements. It was further investigated whether plutonium precipitated in this manner would lead to hydrophobic precipitates which could be rapidly removed from the mother liquor by means of ionic flotation, or precipitation-flotation, respectively.

It is an object of the present invention to provide a process for separating plutonium and uranium which is simple, provides a method for the recovery of plutonium from nuclear-plant wastes and other radioactive wastes, and is devoid of the disadvantages of the prior art processes.

In accordance with one aspect of the present invention there is provided a process for selectively separating plutonium and uranium comprising the steps of: adding nitric acid in certain amounts to a solution containing Pu.sup.4+ and UO.sub.2.sup.2+, with the amount of nitric acid added being sufficient such that the Pu.sup.4+ forms anionic nitrato-complexes, adding, prior to, or with, or during, addition of the nitric acid, a compound containing at least one group adapted to assert affinity to polar surfaces and also containing a radical which has little affinity to water, separating the resultant precipitate from its mother liquor, and recovering the plutonium from the precipitate.

In accordance with another aspect of the present invention there is provided a process for selectively separating plutonium and uranium which comprises the steps of: adding, to a solution containing Pu.sup.4+ and UO.sub.2.sup.2+, sulfuric acid in such an amount that the uranium forms anionic sulfato-complexes, adding a sufficient amount of a cationic compound containing at least one group adapted to assert affinity to polar surfaces and also containing a radical which has little affinity to water, separating the resultant precipitate from its mother liquor, adjusting, after separation of the uranium-containing precipitate, the pH value in the remaining mother liquor in such a way that the Pu.sup.4+ forms anionic sulfato-complexes, adding a further amount of said cationic compound, separating the resultant precipitate from its mother liquor, and recovering plutonium from the precipitate.

In accordance with a further aspect of the invention there is provided a process for selectively separating plutonium and uranium which comprises the steps of: adding to a solution containing Pu.sup.4+ and UO.sub.2.sup.2+ such an amount of sulfuric acid that Pu.sup.4+ as well as UO.sub.2.sup.2+ form anionic sulfato-complexes, next adding iron(II)sulfate or other suitable reducing agents in such an amount the Pu.sup.4+ present is reduced to Pu.sup.3+, adding a cationic compound containing at least one group adapted to assert affinity to polar surfaces and also containing a radical which has little affinity to water, separating the resultant precipitate from its mother liquor, and recovering uranium from the precipitate. After separation of the uranium-containing precipitate, the process is continued by adding to the remaining mother liquor either sodium nitrite or peroxodisulfate, or other oxidizing agents, in such an amount that the Pu.sup.3+ is re-oxidized, adding a further amount of said cationic compound, separating the resulting plutonium-containing precipitate, and recovering the plutonium from the precipitate.

Electrolytic methods can be employed correspondingly instead of the reducing agents during the reduction and/or the oxidizing agents during the re-oxidation, respectively.

In accordance with yet another aspect of the present invention there is provided a process for selectively separating plutonium and uranium which process comprises the steps of: adjusting the sulfuric acid concentration and the pH of a solution containing Pu.sup.4+ and UO.sub.2.sup.2+ in such a way that both elements form anionic sulfato-complexes, adding a cationic compound containing at least one group adapted to assert affinity to polar surfaces and also containing a radical which has little affinity to water, separating the resultant precipitate from its mother liquor, suspending the precipitate in nitric acid for re-dissolution of the precipitated uranium, and isolating plutonium from the remaining precipitate and uranium from the uranium-containing solution.

In accordance with the present invention the exposure time of the utilized organic material is to be held at a minimum when exposed in ranges of high radiation densities or fluxes. Furthermore, the amount of the compound used is to be minimized. A process in accordance with the present invention is to be carried out exclusively in an aqueous environment so as to avoid problems of phase penetration kinetics (phase transfer kinetics) and density fluctuations of a two-phase system.

In continuation of the efforts of isolating, using flotation and enriching or concentration techniques, UO.sub.2.sup.2+ from homogeneous aqueous solutions by means of cationic compounds containing at least one group adapted to assert affinity to polar surfaces and also containing a radical having little affinity to water, as suggested in German Pat. No. 2 817 029, the possibility was examined to apply such technique in the isolation and enriching or concentration of Pu.sup.4+. In this context, there was utilized the known finding that Pu.sup.4+ and U.sup.4+ are capable of forming sulfato-complexes, as well as nitrato-complexes and, accordingly, satisfy the essential requirement for precipitation-flotation using such cationic compounds.

It was surprisingly found that Pu.sup.4+ and U.sup.4+ can be precipitated as nitrato-complexes using the cationic compounds referred to, with a preferred compound comprising cetylpyridinium, from nitric acid or nitrate-containing solutions at concentrations of NO.sub.3.sup.- of less than 10M, whereas UO.sub.2.sup.2+ would not be precipitated. This is even more surprising since one had to conclude, on the basis of the bonding capability of anionic exchange resins for uranium in nitric acid solutions, that UO.sub.2.sup.2+ would also be capable to form nitrato-complexes.

It was furthermore surprising that the cationic compounds used for precipitation, particularly the alkylpyridinium salts, exhibit a high stability under the influence of radioactive radiation. Thus, radiation doses of up to 10.sup.6 rad did not cause a detectable influence on the precipitation characteristics or capability of the cetylpyridinium cation. Only at 10.sup.8 rad could be noted a significant, approximately 30%, decrease of the precipitation capability.

Thus, in accordance with the invention there is provided a simple and highly selective process for the separation of Pu.sup.4+ and UO.sub.2.sup.2+ and for the recovery of both ions from aqueous solutions. In accordance with the present invention it is not required that organic solvents or ion exchange resins are used. Instead highly radiation-resistant reagents are used, and the residence time of these in the solution is, furthermore, relatively short. In accordance with the invention, one can separate Pu.sup.4+ from UO.sub.2.sup.2+ and associated metals, in nitric acid solutions, provided the associated metals do not form nitrato-complexes, or only form anionic nitrato-complexes less stable than Pu.sup.4+, and which do not precipitate an addition of said cationic compounds.

Pu.sup.4+ as well as UO.sub.2.sup.2+ form, in sulfuric acid solutions and in sulfate-containing solution, sustantially insoluble precipitates on addition of the cationic compounds mentioned before. Thus, Pu.sup.4+ and UO.sub.2.sup.2+ can either jointly or individually be separated from all associated metals in such solutions which do not form sulfato-complexes, or only sulfato-complexes which are less stable than Pu.sup.4+ and UO.sub.2.sup.2+ and which do not precipitate on addition of cationic compounds of the class described.

Thus, in accordance with the present invention there are indicated several methods for the separation of uranium and plutonium: Pu.sup.4+ is precipitated as a substantially insoluble complex from a solution containing Pu.sup.4+ and UO.sub.2.sup.2+ in the presence of nitric acid. The UO.sub.2.sup.2+ remains in solution and it can be precipitated either by the addition of sulfate ions as sulfato-complex, or upon reduction to U.sup.4+ as nitrato-complex.

Pu.sup.4+ and U.sup.4+ are together precipitated from nitric acid solution. The precipitate is subjected to a selective oxidation such that U.sup.4+ is converted to UO.sub.2.sup.2+ and is re-dissolved in the solution.

UO.sub.2.sup.2+ and Pu.sup.4+ are precipitated together from sulfate-containing solutions, and subsequently UO.sub.2.sup.2+ is redissolved from the precipitate by nitric acid.

In a sulfate-containing solution of both metals the Pu.sup.4+ is reduced to Pu.sup.3+, and the UO.sub.2.sup.2+ is precipitated as substantially insoluble complex by cationic compounds of the class indicated above. After re-oxidation of the Pu.sup.3+ to Pu.sup.4+, Pu.sup.4+ is then also precipitated.

In a sulfate-containing solution also containing Pu.sup.4+ and UO.sub.2.sup.2+ the pH value is adjusted in two steps in such a way that initially one element forms a substantially insoluble precipitate, and then the other, on addition of cationic compounds of the class indicated herein, followed by separation of the materials of interest.

In nitric acid solution, Pu.sup.4+ is reduced to Pu.sup.3+ and UO.sub.2.sup.2+ is reduced to U.sup.4+. The U.sup.4+ is then precipitated by use of a cationic compound. The Pu.sup.3+ is re-oxidized to Pu.sup.4+ and is also precipitated.

The lower limit of the concentration of nitric acid is from between 0.1 to 1.0N HNO.sub.3. An upper limit could not be determined to-date. It was found that one could use concentrations of 10N NHO.sub.3.

At concentrations of HNO.sub.3 of less than 10N, UO.sub.2.sup.2+ forms a complex UO.sub.2 NO.sub.3.sup.+. At a concentration of HNO.sub.3 of greater than 10N, there result anionic complexes (through adsorption of uranium on anionic exchangers), but the composition of these complexes is unknown. In HNO.sub.3, Pu.sup.4+ forms all complexes from Pu(NO.sub.3).sup.3+ to Pu(NO.sub.3).sub.6.sup.2- (compare: I. M. Cleveland, The Chemistry of Plutonium, American Nuclear Society). Pu.sup.3+ does not form anionic nitrato-complexes.

The cationic compound referred to herein is optimally added at slightly higher concentrations than stoichiometric concentrations, approximately at an excess of 1.01 to 1.05. When one adds a substantially greater amount of such cationic compound, of course, more metal enters the precipitate, however, unnecessary intensive foaming or frothing occurs, and the duration of the flotation process is extended. Furthermore, the flotation characteristics of the precipitate deteriorate.

If flotation is not desired, but instead centrifuging or filtration is used, the cationic compound may be used at higher concentrations, e.g. 1.01 to 1.50 equivalence.

U an Pu can be separated from the majority of radioactive fission products which are generated in a reactor. The separation is easy when the other metals do not form anionic complexes and/or anionic poly-acids, or heteropolyacids, respectively. The separation of anionic complexes and/or poly-acids is achieved in substantially all cases as well when one either somewhat varies ligand concentration (NO.sub.3.sup.-, SO.sub.4.sup.2-), or the pH, or U or Pu, respectively, or selectively oxidizes or reduces, respectively, the other metals. Thus, even the separation of Pu from Ce (which represents a simulate for Pu and also represents an important fission product) by selective reduction of the Ce.sup.4+ to Ce.sup.3+ can be achieved. The Ce.sup.3+ does not form precipitates on addition of cationic compounds as referred to.

Of primary importance is the separation of Pu and U from nitric acid or nitrate-containing solutions. On precipitation with appropriate cationic compounds as outlined herein, aside from Pu.sup.4+, only the ions Ce.sup.4+, Ru.sup.2+, Mo.sup.6+, U.sup.4+ and Th.sup.4+ precipitate. Depending on the given problem, these elements can either be separated by selecttivity in the precipitation conditions, or by a subsequent process, from the plutonium, or they may also be left with the plutonium.

The invention is generally applicable to the separation of U and Pu from any starting materials which contain U and Pu. Thus, both elements were removed from two types on non-specific, medium-active-waste waters (obtained from the Nuclear Research Center Karlsruhe, Germany):

1. From solutions which are collected in a central collecting tank and emanate from various laboratories. On average, the composition of such waste waters is somewhat constant. With good approximation this solution contains: Na.sup.+, Al.sup.3+, Ca.sup.2+, Cr.sup.3+, Cu.sup.2+, Fe.sup.3+, Mg.sup.2+, Mn.sup.2+, MoO.sub.4.sup.2-, Ni.sup.2+, Zn.sup.2+, and ZrO.sup.2+ in 1M NHO.sub.3, from which plutonium and, as required, also uranium are recovered.

2. From solutions which come from wet-incinerated Pu-containing wastes (rubber gloves, crucible tongs, towels, filter paper and the like) of the production of plutonium oxide. These are sulfuric acid solutions (1 to 2M H.sub.2 SO.sub.4) which, aside from plutonium and, possibly, uranium, also contain Al.sup.3+, Ca.sup.2+, Cr.sup.3+, Cu.sup.2+, Fe.sup.3+, Mg.sup.2+, Mn.sup.2+, Ni.sup.2+, Sn.sup.4+, TiO.sup.2+, and Zn.sup.2+.

With respect to other operating conditions and techniques reference may be had to German Pat. No. 2 817 029.

The following examples serve to further illustrate the invention.

EXAMPLE 1

Selective Precipitation of Pu.sup.4+ as Nitrato-Complex in the Presence of UO.sub.2.sup.2+

A solution was produced containing 625 mg UO.sub.2.sup.2+ and 25 mg Pu.sup.4+ in 100 ml of 7.0M HNO.sub.3. Solid cetylpyridinium chloride, 4 g, was dissolved in the solution. After several minutes a green precipitate of fine crystals was obtained. This was stirred for 30 minutes and subsequently filtered.

EXAMPLE 2

Joint Precipitation of Pu.sup.4+ and UO.sub.2.sup.2+ as Sulfato-Complexes and Separation in HNO.sub.3

In 75 mg of 1.3M H.sub.2 SO.sub.4 were dissolved 25 mg Pu.sup.4+, containing also Pu.sup.6+ and Pu.sup.3+, and 635 mg UO.sub.2.sup.2+, and 1 g solid NaNO.sub.2 was added. Upon dissolution of the salt, the pH of the solution was adjusted to 2.5 by the addition of aqueous ammonia, and water was added to bring the solution to 100 ml. In this solution 4 g solid cetylpyridinium chloride were dissolved. After several minutes a yellow precipitate of fine crystals was obtained which was filtered after stirring for 30 minutes.

The filtrate contained only 1.13% of the initially dissolved Pu.sup.4+ and 0.8% of the initially dissolved UO.sub.2.sup.2+. The recovery of plutonium in the precipitate was, accordingly, 98.78% and that of uranium 99.19%.

The precipitate was then suspended in 10 ml of 1.0M HNO.sub.3. The uranium-containing part of the precipitate was dissolved, while the plutonium-containing part remained in suspension. The precipitate was separated by centrifuging, and the uranium was removed from the mother liquor by neutralizing with aqueous ammonia, in the form of ammonium diuranate.

EXAMPLE 3

Selective Precipitation of UO.sub.2.sup.2+ as Sulfato-Complex in the Presence of Pu.sup.4+

In 75 ml of a 1.3M H.sub.2 SO.sub.4 solution were dissolved 24 mg Pu.sup.4+ and 632 mg UO.sub.2.sup.2+, and 152 mg solid FeSO.sub.4 was added. Upon dissolution of the salt the pH was adjusted to 2.5 by the addition of aqueous ammonia, and water was added to bring the solution to 100 ml. The solution was subsequently treated as described in EXAMPLE 2. The uranium reported at 99.46% in the precipitate, and the plutonium reported at 97.8% in the filtrate.

EXAMPLE 4

Selective Precipitation of Pu.sup.4+ as Nitrato-Complex in the Presence of UO.sub.2.sup.2+ and Am.sup.3+

A solution was produced containing 37.2 .mu.g Pu.sup.4+, 3.66 mg UO.sub.2.sup.2+, and an unknown but relatively small amount of Am.sup.3+, in 100 ml of 7.0M HNO.sub.3. To the solution was added 120 mg solid cetylpyridinium chloride which dissolved rapidly. The subsequent, green precipitate was stirred for 30 minutes and then filtered. The precipitate contained 91% plutonium, and uranium and americium reported at 97.7% each in the filtrate.

EXAMPLE 5

Fractionated Precipitation of UO.sub.2.sup.2+ and Pu.sup.4+ by Varying the pH Value

In 200 ml 1.0M H.sub.2 SO.sub.4 were dissolved 25 mg Pu.sup.4+ and 635 mg UO.sub.2.sup.2+, and the pH value was adjusted to 1.5 by the addition of aqueous ammonia. After addition of 3.8 g cetylpyridinium chloride and stirring for 30 minutes, the resultant precipitate was filtered and analyzed. It contained 98.2% of the initial uranium content and less than 1% of the entire Pu-activity. The pH of the filtrate was adjusted to 3.0 by the addition of aqueous ammonia. The plutonium was precipitated by a further addition of 100 mg cetylpyridinium chloride. The plutonium-containing precipitate was filtered and analyzed. It contained 97.9% of the initial Pu-activity and only traces of uranium.

EXAMPLE 6

Fractionated Precipitation of Plutonium and Uranium from Nitric Acid Solutions

A solution of 625 mg UO.sub.2.sup.2+ and 25 mg Pu.sup.4+ in 100 ml 4.3M HNO.sub.3 was prepared. To this solution was added a solution of 0.1 g cetylpyridinium chloride in 3 ml of 4.3N HNO.sub.3. After a few minutes a green precipitate of fine crystals was formed which was stirred for 30 minutes and then filtered. The filtrate was added to a sufficient amount of hydrazine, sufficient to produce a 0.2 molar hydrazine solution, and it was then introduced into a special electrolysis cell. The uranium was electrolytically reduced from UO.sub.2.sup.2+ to U.sup.4+. The reduction was carried out using a platinum screen as anode and mercury as cathode, at a voltage of 4.5 V. The 4-valent uranium was subsequently precipitated by addition of a further 4 g of cetylpyridinium chloride (dissolved in 10 ml 0.3N HNO.sub.3 at 60.degree. C.), and the suspension was again stirred for 30 minutes. Upon filtration of the uranium-containing precipitate, the filtrate was evaporated, and the residue as well as the two metal-containing precipitates, were analyzed. The plutonium precipitate contained 97.8% of the starting plutonium-activity and only trace amounts of uranium. The uranium precipitate contained 94.3% of the starting uranium content and less than 1% of the starting plutonium-activity.

In this invention, the terminology: a compound containing at least one group adapted to assert affinity to polar surfaces and also containing a radical having little affinity to water, is intended to convey the meaning of the German chemical expression TENSID. The expression is derived from the Latin and suggests `tensioned`. According to the 6th Edition of the German chemical encyclopedia `Rompp's Chemie Lexicon`, the definition given therein embraces at least portions of and all of the following terms and agents: surface active agents, phase[-surface-]-active agents, detergents, surfactants, syndets and the like. This definition of TENSID has been proposed at the session of the Commission Internationale de Terminologie des Comite International de la Detergence, on Feb. 24, 1960, in Luzern, Switzerland.

Reference in this disclosure to details of the specific embodiments is not intended to restrict the scope of the appended claims, which themselves recite those features regarded as essential to the invention.

Claims

1. A process for selectively separating plutonium an uranium comprising: a first, reduction, step; and a second, oxidation, step, said first step including: adding to a solution containing Pu.sup.4+ and UO.sub.2.sup.2+ such an amount of sulfuric acid that Pu.sup.4+ and UO.sub.2.sup.2+ form anionic sulfato-complexes, introducing a reducing agent in an amount sufficient to reduce Pu.sup.4+ present to Pu.sup.3+, adding a cationic compound containing at least one group adapted to assert affinity to polar surfaces and also containing a radical which has little affinity to water, separating the resultant, first, precipitate from its mother liquor, and recovering the uranium from said first precipitate; and said second step including: adding, after separating the uranium-containing precipitate, to remaining mother liquor such an effective amount of an oxidizing agent that Pu.sup.3+ is re-oxidized, introducing a further amount of said cationic compound, separating the resultant, second, precipitate, and recovering plutonium from said second precipitate.

2. A process according to claim 1 wherein said reducing agent comprises iron(II)sulfate.

3. A process according to claim 1 wherein said oxidizing agent is selected from the group consisting of sodium nitrate and peroxodisulfate.

4. A process according to claim 1 wherein said reduction step is carried out by electrolytic reduction.

5. A process according to claim 1 wherein said oxidation step is carried out by electrolytic oxidation.

6. A process according to claim 1 wherein said oxidation step and said reduction step are respectively carried out electrolytically.

7. A process according to claim 1 wherein during said first, reduction, step there is added such an amount of said cationic compound which is sufficient to effect precipitation of said first precipitate and said second precipitate.