Ambient temperature decontamination of nuclear power plant component surfaces containing radionuclides in a metal oxide

Abstract

This invention generally concerns radioactive decontamination of deposits on components in a nuclear power plant and is specifically concerned with improved compositions, systems and methods for disrupting, dissolving, removing and reducing at ambient temperature radionuclides formed on the primary side surfaces of components in a pressurized water reactor and the internal components of a boiling water reactor. The methods include identifying the structure, taking the structure out of operational service, contacting the structure with an aqueous solution (e.g., a recirculating flow or static immersion), and adding an effective amount of elemental metal in solid form to the aqueous solution.

Claims

1. A composition effective to at least partially disrupt and dissolve radioactive deposits formed on a surface of a structure in a nuclear water reactor when the composition is in contact with the surface of the structure during non-operational conditions, the composition consisting essentially of: an aqueous component at ambient temperature; from about 0.001 M to about 2 M based on the composition, of at least one elemental metal additive to the aqueous component, selected from the group consisting of zinc, beryllium, aluminum, magnesium, iron, lithium, and mixtures thereof, in particulate, powder or colloidal form; from about 0.025 weight percent to about 5.0 weight percent based on total weight of the composition, of an additive selected from the group consisting of a sequestering agent, a chelating agent, and mixtures thereof; optionally a dispersant; optionally an oxygen scavenger; optionally a pH adjustment agent; and optionally a reducing agent; wherein the radioactive deposits comprise oxide-containing radionuclides deposited on the surface, and wherein the surface is a primary side structure surface in the nuclear water reactor.

2. The composition of claim 1, wherein the elemental metal component is zinc.

3. The composition of claim 1, wherein the elemental metal is in colloidal form.

4. The composition of claim 3, wherein the colloidal form contains particles selected from the group consisting of micron-sized particles, nano-sized particles and combinations thereof.

5. The composition of claim 1, further comprising a dispersant.

6. The composition of claim 1, wherein the aqueous component has a pH in a range from about 3.0 to about 13.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

(1) A further understanding of the invention can be gained from the following description of the preferred embodiments when read in conjunction with the accompanying drawings in which:

(2) FIG. 1 is a plot showing the influence of elemental zinc on dissolution of nickel ferrite deposits under boric acid conditions; and

(3) FIG. 2 is a plot showing the influence of elemental zinc on dissolution of nickel ferrite deposits under reducing conditions.

DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS

(4) The invention relates to systems and methods for the at least partial disruption, dissolution, removal and reduction of radioactive deposits in nuclear water reactors at ambient temperature. The radioactive deposits include radionuclides, oxide scale, and corrosion products, deposited on primary side, e.g., reactor coolant system, component surfaces and associated piping in pressurized water reactors and from internal component surfaces in boiling water reactors. Deposits containing radionuclides can form and build-up on these surfaces as a result of reactor operation. In addition, other corrosion products can also be deposited on these surfaces during reactor operation. For instance, the deposits can include contaminants such as aluminum, manganese, magnesium, calcium, nickel, and/or silicon morphologies. Removal and reduction of these products can be effective to reduce the local dose rate in the system(s) surrounding the components, to prevent or preclude flow obstructions (which occur due to corrosion product build-up), and to inhibit corrosion caused by the presence of radioactive oxide scale. The methods of the invention employ electrochemical techniques at ambient temperature to at least partially disrupt, dissolve, remove and reduce the radioactive oxide scale. The composition of the radioactive oxide scale can vary and typically can include at least one of iron, nickel, cobalt, chromium and their radioisotopes.

(5) The invention employs an aqueous solution having an aqueous component and a solid metal component. The aqueous component includes water, e.g., reactor coolant water. The metal component includes elemental metal in solid form. The aqueous solution is effective to disassociate metal ions from an oxide lattice of radioactive deposits.

(6) The elemental metal is selected from known metals with standard electrochemical potentials anodic to low alloy steel. In certain embodiments, the electrochemical potential of the elemental metal is more active than the potential of low alloy steel in the galvanic series of metals and alloys. Suitable examples of elemental metal for use in the invention include, hut are not limited to, zinc, aluminum, magnesium, beryllium, lithium, iron or mixtures thereof. In certain embodiments, the elemental metal is zinc. The elemental metal can be in various solid or particulate forms, such as but not limited to, slab, granular, powder, colloidal, and combinations thereof. In certain embodiments, wherein the elemental metal is in colloidal form, it can include micron-sized particles, nano-sized particles and combinations thereof. The elemental metal can be present in varying amounts, and the amount can depend on the volume of the system, component and/or associated equipment intended for decontamination. In certain embodiments, the elemental metal concentration can be from about 0.001 M to about 2 NI based on volume of the aqueous solution.

(7) The of the aqueous solution can vary. In certain embodiments, the pH can be adjusted within a range from about 3.0 to about 13.0. Further, the aqueous solution may be borated and contain up to 6 ppm of lithium.

(8) The methods of the invention generally include addition of the elemental metal in solid, e.g., particulate, form to circulating coolant in an effective amount, an amount which is sufficient to at least partially disrupt, dissolve, remove or reduce the amount or level of radioactive deposits present on the surface of a structure located in the primary side of a pressurized water reactor or in a boiling water reactor. The methods of the invention can be conducted at ambient temperature and therefore, in the absence of system heat or an external heat source being applied to the structure or the system which contains the structure. Thus, the methods of the invention can be employed when the components and associated piping are taken out of operational service, e.g., during layup or shutdown conditions in a nuclear water reactor.

(9) Further, the methods of the invention generally include identifying a component and/or associated equipment, e.g., piping, to be electrochemically decontaminated, taking the component and/or associated equipment out of operational service, isolating the component and/or associated equipment from the remainder of the primary side, e.g., reactor coolant system, employing a recirculating flow of aqueous solution in contact with the component and/or associated equipment or a static immersion of the component and/or associated equipment in aqueous solution, and adding, e.g., injecting, an effective amount of elemental metal in solid or particulate form into the aqueous solution.

(10) Without intending to be bound by any particular theory, it is believed that the elemental metal releases one or more of its electrons which is/are accepted by the radioactive deposits, e.g., oxide scale film, present on the surface of the intended structure(s) for radioactive decontamination. A metal ion is released from the deposits and as a result, the surface charge of the deposits is modified, e.g., a charge imbalance occurs. The lattice of the radioactive deposits is destabilized and there is an increased rate of metal ion release, e.g., dissociated metal ions. In certain embodiments, elemental zinc reacts with iron oxide deposits causing the release of iron ions from the lattice.

(11) In certain embodiments, the elemental metal can be combined with a sequestering agent, a cheating agent or a mixture or blend thereof. The sequestering and/or chelating agent can be added to the aqueous solution prior to, in conjunction with, or following the addition of the elemental metal. Suitable sequestering and chelating agents can be selected from those known in the art. Non-limiting examples of sequestering agents include acids and salts of orthophosphates, polyphosphates, 1-hydroxy ethylidene-1, 1-diphosphonic acid, and mixtures thereof. Non-limiting examples of chelating agents include ligands selected from ethylenediamine tetraacetic acid (EDTA), hydroxyethyl ethylenediamine triacetic acid (HEDTA), lauryl substituted EDTA, polyaspartic acid, oxalic acid, glutamic acid, diacetic acid (GLDA), ethylenediamine-N,N′-disuccinic acid (EDDS), gluconic acid, glucoheptonic acid, N,N′-ethylenebis-[2-(o-hydroxyphenyl)]-glycine (EHPG), pyridine dicarboxcylic acid (PCDA), nitrilotriacetic acid (NTA), acids and salts thereof, and mixtures thereof.

(12) The sequestering and/or chelating agents can be utilized in varying amounts. In certain embodiments, the sequestering and/or chelating agents are present in an amount of from about 0.025 to about 5.0 weight percent based on weight of the solution composition.

(13) The use of one or more of these agents can be effective to complex ions released from the deposits, e.g., dissociated metal ions. In certain embodiments, iron, nickel, cobalt and their corresponding isotopes can be complexed from the lattice of radioactive deposits using a sequestering agent, chelating agent or a blend thereof. The dissociated metal ions can also be complexed by allowing the dissociated metal ions to precipitate and removing the colloidal precipitate using a dispersant. Suitable dispersants can be selected from those known in the art. Non-limiting examples of dispersants include polyacrylic acid, amine neutralized polyacrylic acid, polyacrylamide, polymethacrylate, and mixtures thereof. A non-limiting example of a suitable dispersant is commercially available under the trade name OptiSperse PWR 6600 from General Electric Company. The dissociated metal ion can be precipitated from the oxide deposits and the colloidal precipitate can be removed by employing filtration, reverse osmosis, or ion exchange.

(14) In certain embodiments, the aqueous solution may be circulated through a spectrophotometer to determine the concentration of complexed metals contained therein. Further, the expended aqueous solution may be drained through an in-line ion exchange bed, stacked filtration assembly or low micron size filter.

(15) Without intending to be bound by any particular theory, it is believed that hydrogen gas is generated in situ during the decontamination process and facilitates mixing and mechanical agitation of the solution and particulate.

(16) Further, the aqueous solution can be sparged with an inert gas or air for mixing, and the system which contains the intended component and/or associated equipment for decontamination can be under oxidizing or reducing conditions. For oxidizing conditions, an oxygen scavenger can be employed. Suitable oxygen scavengers can be selected from those known in the art. For reducing conditions, a reducing agent can be employed. Suitable reducing agents can be selected from those known in the art. Non-limiting examples of reducing agents include ascorbic acid, citric acid, hydrazine, carbohydrazide, catalyzed hydrazine, hydroquinone, methylethylketoxime, diethylhydroxylamine, erythorbate and mixtures thereof.

(17) In certain embodiments, the elemental metal can be added to a local area of the nuclear reactor. Non-limiting examples include adding the elemental metal to a local area containing a jet pump orifice or a reactor coolant pump.

(18) In certain embodiments, the deposits, e.g., radionuclides and/or radioactive oxide scale, can be conditioned with a noble metal. This conditioning step may be performed prior to adding the elemental metal to the aqueous solution.

(19) In certain embodiments, the system is adiabatic.

(20) The deposits, e.g., radionuclides and/or radioactive oxide scale, are at least partially disrupted and/or removed from a surface of a component and/or associated equipment, and are processed. The processing can include purifying the deposits generated by removing the particulate or transferring the deposits to a containment sump or adding the deposits to the radioactive waste system or transporting the deposits from the plant site to another location.

(21) Without intending to be bound by any particular theory, it is believed that in accordance with the invention, solid zinc in its elemental form can react with radioactive deposits to produce a byproduct containing zinc ions. In certain embodiments, zinc ions are used during normal operation as inhibitors to stress corrosion cracking. The byproduct zinc ions prevent excessive release of zinc from primary surface oxides which have formed as a result of on-line zinc addition, by the common ion effect.

(22) The methods of the invention do not require a rinsing step and may provide carbon molecules which may be beneficial for crud build-up on the nuclear fuel.

(23) The methods of the invention are effective to at least partially disrupt, dissolve, remove and reduce deposits in the absence of elevated temperatures, e.g., system heat and/or an external heat source is not required. Thus, the elemental metal in a colloidal or particulate form can be applied at ambient temperature when the system is in a shutdown or layup condition.

(24) While specific embodiments of the invention have been described in detail, it will be appreciated by those skilled in the art that various modifications and alternatives to those details could be developed in light of the overall teachings of the disclosure. Accordingly, the particular embodiments disclosed are meant to be illustrative only and not limiting as to the scope of the invention which is to be given the full breadth of the appended claims and any and all equivalents thereof.

EXAMPLE

(25) Nickel ferrite dissolution tests were performed in a laboratory under ambient dissolved oxygen boric acid conditions (at shutdown concentrations) and under alkaline non-borated conditions. Samples 1-4 were prepared as follows. Test volumes were 200 ml for each sample. Samples 1 and 2 included boric acid (approximately 2500 ppm boron), and Samples 3 and 4 were alkaline and did not include boric acid.

(26) Specifically, Samples 1 and 2 included approximately 1.84 grams of citric acid and 1.29 grams of boric acid. Approximately 0.78 grams of zinc were added to Sample 1, while Sample 2 did not contain any zinc.

(27) For Samples 3 and 4, an initial wet layup solution was prepared such that each sample contained approximately 0.009 grams of carbohydrazide and 0.2 mL of ethanolamine, and pH adjustment with added ammonium hydroxide. The final pH of the wet layup solution was approximately 10.2. Approximately 4 grams of EDTA was added to both Sample 3 and Sample 4. Subsequently, 0.8 grams of zinc was added to Sample 4, while Sample 3 did not contain any zinc.

(28) After the chemistries for each of Samples 1-4 were established, 2.5 grams of nickel ferrite was added to each and the bottles were capped. During testing, 2-3 samples were pulled from each of the Samples 1-4, and the time was recorded for each sample pull. The sample size was approximately 1 ml. The samples were filtered through a 0.45 μm-syringe filter. The tests were conducted for 23.5 hours. The pulled samples were then prepped with 100 μL of piranha bath solution containing sulfuric acid and hydrogen peroxide, diluted by a factor of 1:20, and analyzed for iron and nickel via inductively coupled plasma (ICP) spectroscopy. The results indicate a six-fold increase in the dissolution rate of corrosion products under both acidic borated conditions and alkaline non-borated conditions, as shown in FIG. 1 and FIG. 2. FIG. 1 shows the influence of elemental zinc on dissolution of nickel ferrite deposits under boric acid conditions, i.e., Samples 1 and 2. FIG. 2 shows the influence of elemental zinc on dissolution of nickel ferrite deposits under reducing conditions, i.e., Samples 3 and 4. The six-fold increase in the slope of measured iron concentration is indicative of the six-fold increase in dissolution rate under both chemistry regimes.