GB2181158A

GB2181158A - Electrolytic process for the manufacture of salts

Info

Publication number: GB2181158A
Application number: GB08524784A
Authority: GB
Inventors: Brian Surfleet
Original assignee: Electricity Council
Current assignee: Electricity Council
Priority date: 1985-10-08
Filing date: 1985-10-08
Publication date: 1987-04-15
Also published as: GB8524784D0; DE3684872D1; EP0221685A1; GB2181158B; EP0221685B1

Description

1 GB 2 181 158A 1

SPECIFICATION

Electrolytic process for the manufacture of salts The present invention relates to an electrolytic process for the manufacture of salts.

The production of salts, i.e. the chemical compounds formed by metal ions and acid/alkali anions, can be carried out in many ways. Traditionally the simplest routes have been selected, for example those metals which are readily and easily attacked by the acids or alkalis to form salts are well known, e.g. Zn+2HCI---ZnCI2+H2 For metals which are not readily attacked by the particular acids then synthetic routes via metal containing compounds are preferred, e.g. CuO+H2SolCuSO,+H20 It will be appreciated however, that the use of a compound containing a metal for salt formation is always more expensive than the use of the metal itself and a direct route is therefore economically preferable. However, in many cases the direct route is not thermodynamically favoured and aggresive reaction conditions such as high temperatures and pressures and long reaction times are often required. These processes become expensive in energy, time and capital costs.

We have now developed an economic electrolytic process for the manufacture of salts in which the energy involved is mainly that of an anodic corrosion process.

Accordingly, the present invention provides a process for the manufacture of a metal salt, which process comprises passing an electric current through an electrolytic cell comprising an anode formed from or containing the said metal, a cathode, an anolyte which will provide the anions to form the salt and a catholyte, the anode and the cathode being separated by a microporous plastics separator which has a pore size in the range of from 0.01 to 10 microns 30 and a pore volume in the range of from 45 to 55%.

In the process of the present invention, the metal which forms the anode loses electrons to give metal ions, e.g. M2+ by one reaction M-2e_M21 These ions exist either as totally ionised metal ions together with the corresponding anions A2or in an equilibrium MA;.tM2++A2- The position of this equilibrium depends upon the temperature, metal ion concentration, pH etc. The anode may comprise one of the following: a) an ingot of the metal whose salt is to be produced, 45 b) granulated metal or scrap pieces of the metal whose salt is to be produced contained in a 45 conductive basket or an insulated basket with an appropriate current feed, c) a non-soluble anode when the process is used to change the valency state of a metal ion and thus the nature of the salt which constitutes the anolyte, and d) granulated or particulate sampis of mixed metals where metal separation and salt production are required.

The cathode used in the process of the present invention remains inert and since in general some of the metal will pass through the separator and coat the cathode it is preferred to use a cathode of the metal concerned, although a cathode of another metal may also be used.

A cathodic reaction takes place at the cathode, for example the production of hydrogen by the reduction of the acid cation:

21-1++2e,H2 Other cathodic reactions can also be carried out.

The anolyte is an electrolyte which contains ions that will conduct electricity, which provides 60 the anions so as to form the metal salt, and in which the metal salt produced in the process of the invention is reasonably soluble. The anolyte may be an acid, such as sulphuric acid, hydro chloric acid, nitric acid, acetic acid, or an alkali, such as sodium or potassium hydroxide, or ammonium hydroxide.

The catholyte may comprise any electrolyte, but the preferred catholyte is an electrolyte which 65 2 GB 2 181 158A 2 is the same as the anolyte, but not necessarily at the same concentration.

The temperature, concentration and current density employed in the process of the invention depend upon the reaction which is being carried out.

The microporous plastics separator used in the process of the present invention preferably has a pore size in the range of from 0.0 1 to 0. 1 microns and a pore volume of about 50%. The porosity or pore volumne controls the electrical resistance of the separator, whilst the pore size influences the transport of ions across the separator. The microporous plastics separator should be chemically resistant to its environment at the operating temperature and the operating pH. It should also be made from a plastics material which is wettable, or which can be treated to render it wettable, and possesses sufficient mechanical strength so that it is capable of being 10 engineered into an appropriate support. It must be capable of transporting ions under an electrical and/or concentration gradient and it must also permit a reasonably high current density e.g. 50rnA/cm2 of separator surface. Examples of the microporous plastics separator are a filled polyethylene separator sold under the Trade Name DARAMIC (W.R. Grace & Co.), an irradiated polyethylene separator sold by Raychem, a microporous polyolefin manufactured by Schumacher, 15 a compound called GORTEX which is a microporous polytetrafluoroethylene and a product called WON/PORVAIR which is a microporous high density polyethylene. The separator is usually fabricated onto a support frame, for example by means of an adhesive or by thermal or ultrasonic welding. Such a frame enables the separator to be mounted in a cell and provides some support to the separator against bulging which is particularly important for those materials 20 which expand when wet and bulge.

It will be understood that any two or three compartment cell may be used in the present invention. However, it is generally more convenient to design a cell having the anode, cathode and separator planar to the walls of the vessel in which they are placed.. Similar considerations apply when using a granular anode since the baskets in which the material is held are usually 25 planar and rectangular baskets are easier to handle than circular ones. The cell should preferably have a symmetrical design so that the anode is attacked from both sides at an equal rate. The electrodes may be suspended in the cell from appropriate hooks e.g. of titanium, from lugs cast onto the electrode or by bolting the electrodes onto an appropriate bus bar.

The process of the present invention may be a continuous or a batch process. For continuous 30 operation some pumping of the electrolytes will be required but it is preferable to use external pumps so as not to interfere with the cell symmetry. Similarly if heating is required it is preferred that it is either external or that electrically controlled heating elements are positioned at the sides of the anode and cathode compartments of the cell.

Stirring is often beneficial in order to even the rate of corrosion of the anode. Gas stirring is 35 preferred as it leaves the cell uncluttered and is easily controlled.

The volume of the anolyte depends mainly upon the throughput required and thus is generally related to the product requirement, the stability of the product and the size of any ancillary equipment used for working up and extracting the product.

The volume of the catholyte is preferably the same as that of the anolyte since it is preferred 40 to use the catholyte to replace the anolyte on completion of the reaction.

In order to optimise the economics of the cell the anode area should be as large as possible, providing that the available area of microporous plastics separator can pass the current required having regard to the optimum current density required for the process. The cathode area is preferably chosen to be one of two extremes. Either the surface area is large and the current 45 density is kept low so that any metal ions penetrating to the cathode compartment are electro deposited onto the cathode, or the surfaces are small and the current density is kept high and hydrogen evolution prevents much of the metal being deposited on the cathode.

The process of the present invention will be further described with reference to the accom- panying Figure which shows a cell in which the reaction may be carried out.. - Referring to the drawing, anodes 1 are placed in the central- compartment 6 of a five compartment cell. The anodes are hung from the anode rail 2. On either side of the anode compartment 6 are middle compartments 6 which do not contain any electrodes. The middle compartments 8 are separated from the anode compartment by separators 5 of a microporous plastics material. On either side of the middle compartments 8 are cathode compartments 7 which are separated from the middle compartments by separators 5 of a microporous plastics material. The cathode compartments 7 contain cathodes 3 which are suspended from cathode rails 4. The compartments 6, 7 and 8 are filled with the appropriate electrolyte and the current switched on and adjusted to the required current density.

As the reaction proceeds the metal ion concentration in compartment 6 builds up and as the 60 anodes 1 corrode they are replaced by fresh anodes. The anodes are preferably replaced in sequence as this permits a realistic amount of the anode area to be used and hence a reasonable current density to be used- If an appreciable amount of the metal, say 7 to 10%, has been coated onto the cathode, then the cathode may be hung on the anode rail to function as an anode until the coating has redissolved.

3 GB 2 181158A 3 When the metal salt produced in compartment 6 reaches a level where extraction is viable, the anodes are removed from the compartment, the anolyte pumped out of the cell and the anolyte replaced either by fresh electrolyte which is generally the electrolyte from comprtments 7 or 8, if necessary augmented with further chemicals.

The anodes in compartment 6 are replaced, all of the compartments 6, 7, and 8 are topped 5 up with electrolyte, as necessary, and the cell switched on for the process to recommence.

The present invention will be further described with reference to the following Examples.

R Example 1 10 Production of Stannous Sulphate A tin anode was dissolved in 2N sulphuric acid in a two compartment cell having a microporous polyethylene separator separating the anode and cathode compartments which both had a volume of 2.51- (total cell volume 51---). The cell was operated under the following conditions:

Anode Current Density 15 mA/CM2 15 Cathode Current Density 60 mA/CM2 Temperature Ambient Initial Sulphuric Acid Concentration 2N Final Concentration of Tin as Stannous ion 1009/1 Weight loss of Tin Anode 270.59 20 Anode Current efficiency 98% Metal Transfer to Catholyte 15 9 Example 2 25 Production of Stannous Sulphate A tin anode was dissolved in 2N sulphuric acid in a two compartment cell having a filled microporous polyethylene separator separating the anode and cathode compartments. The cell had a total volume of 20L (71- anolyte and 13L catholyte). The cell was operated under the following conditions:

Anode Current Density 15 mA/cm2 Cathode Current Density 15 mA/CM2 Temperature Ambient Initial Sulphuric Acid Concentration 2N Final Concentration of Tin as Stannous ion 160 g/1 35 Weight loss of Tin Anode 1150 g Anode Current efficiency 98% Metal Transfer to Catholyte 30 g Final Sulphuric Acid Concentration 0.1 N 40 Example 3 Production of Silver Nitrate A silver anode was dissolved in 1N nitric acid in a three compartment cell having a filled microporous polyethylene separators separating the compartments thereof. The anode and cath ode compartments of the cell both had volumes of 0.51---. The cell was operated under the 45 following conditions:

Anode Current Density 40 mA/CM2 Cathode Current Density 10 mA/CM2 Temperature Ambient 50 Initial Nitric Acid Concentration 1N Final Concentration of Silver in Anolyte 409/1 Weight loss of Silver Anode 21 9 Anode Current efficiency 98% Final Concentration of free Nitric acid 0.52 N 55 Example 4

Production of Cobalt Chloride Cobalt chips were placed in a titanium anode basket in 5N hydrochloric acid in a two compartment cell having a filled microporous polyethylene separator separating the anode and 60 cathode compartments which both had a volume of 1.01- (total cell volume 21---). The cell was operated under the following conditions:

4 GB2181158A 4 Anode Current Density Cathode Current Density Temperature 5 Initial Sulphuric Acid Concentration Final Concentration of Cobalt in the Anolyte Weight loss of Cobalt Anode Anode Current efficiency Metal transfer to Catholyte mA/CM2 20 mA/CM2 350C 5N 192.3 g/1 196 9 98% 2.5 g Example 5 Production of Copper Acetate A copper anode was dissolved in 2N acetic acid in a two comprtment cell having a filled microporous polyethylene separator separating the anode and cathode compartments which both had a volume of 0.51---(total cell volume 11---). The cell was operated under the following condi- 15 tions:

Anode Current Density 20 mA/CM2 Cathode Current Density 20 mA/CM2 Temperature 1 OOC 20 Initial Acetic Acid Concentration 2N Final Concentration of Copper in the anolyte 41 9/1 Example 6 25 Production of Gold Chloride A gold anode was dissolved in 5N hydrochloric acid in a three compartment cell having a filling microporous polyethylene separator separating the cell compartments which all had a volume of 0.21---(total cell volume 0. 61---). The cell was operated under the following conditions:

Anode Current Density 40 mA/CM2 30 Cathode Current Density 20 mA/CM2 Temperature 600C Initial Hydrochloric Acid Concentration 5N Final Concentration of Gold in the anolyte 50 9/1 Weight loss of Gold Anode 10.2 g 35 Anode Current effeciency 98% Example 7

Production of Cuprammonium Salt A copper anode was dissolved in a mixture of 4M ammonium hydroxide and 1M ammonium 40 nitrate in a two compartment cell having a polyethylene separator sold under the Trade Name DARAMIC separating the anode and cathode compartments. The cell was operated under the following conditions:

Anode Current Density 25mA/CM2 45 Temperature 250C Initial pH of anolyte pH 10 Concentration of copper as cupric ion in anolyte 33 9/1 Anode Current Efficiency 98% 50 The above run was repeated under the same conditions using a microporous polytetrafluoroethylene separator which had been rendered wettable by immersion in methanol for about 1 hour. Similar results were obtained.

Example 8 Production of Copper Pyrophosphate A copper anode was dissolved in a mixture of 2M sodium pyrophosphate, 0. 5M sodium nitrate and 0.1M ammonium hydroxide in a two compartment cell having a filled microporous polyethylene separator separating the anode and cathode compartments. The cell was operated under the following conditions:

4 GB 2 181 158A 5 Anode Current Density 5mA/CM2 Temperature 250C Initial pH of anolyte pH 10 Concentration of copper as cupric ion in anolyte 25 9/1 5 Anode Current Efficiency 99% The above run was repeated under the same conditions using a microporous polytetrafluoroethylene separator sold under the name GORTEX which had been rendered wettable by immersion in methanol for about 1 hour. Similar results were obtained.

Example 9 Production of Sodium (or Potassium) Stannate A tin anode was dissolved in 3N sodium or potassium hydroxide in a two compartment cell having a microporous polytetrafluoroethylene separator sold under the name of GORTEX separating the anode and cathode compartments. The separator had previously been rendered wettable by immersion in methanol for about 1 hour. The cell was operated under the following conditions:

Final Anode Current Density 20rnA/CM2 20 Temperature 60-900C Initial pH of anolyte 13 Concentration of tin as stannous ion in anolyte 55 g/1 Anode Current Efficiency 99% 25 The above run was repeated under the same conditions using a similarly wetted microporous polytetrafluoroethylene manufactured by Doulton Industrial Products Limited. Similar results were obtained.

It will be understood by those skilled in the art that the process of the present invention cannot be used to produce salts where the acid/alkali starting material would attack the separa- 30 tor e.g. hydrogen fluoride would attack the microporous plastics separator. The process also cannot be used to produce insoluble salts unless other means, such as periodic renewal, rotation of the anode or mechanical clearing is carried out since the anode would rapidly become coated with the insoluble product thereby causing the cell voltage to rise and the process to stop. The process furthermore cannot be used where the product is thermodynamically unstable under the 35 cell operating conditions or where the anode is rendered passive by the acid/alkali starting material.

Claims

1. A process for the manufacture of a metal salt, which process comprises passing an 40 electric current through an electrolytic cell comprising an anode formed from or containing the said metal, a cathode, an anolyte which will provide the anions to form the salt and a catholyte, the anode and the cathode being separated by a microporous plastics separator which has a pore size in the range of from 0.01 to 10 microns and a pore volume in the range of from 45 to 55%.

2. A process as claimed in claim 1 wherein the anode is an ingot of the metal whose salt is to be produced.

3. A process as claimed in claim 1 wherein the anode is granulated metal or scrap pieces of the metal whose salt is to be produced.

4. A process as claimed in claim 1 wherein the anode is a non-soluble anode.

5. A process as claimed in claim 1 wherein the anode comprises granulated or particulate samples of mixed metals.

6. A process as claimed in any one of the preceding claims wherein the cathode is formed from the metal whose salt is to be produced.

7. A process as claimed in any one of the preceding claims wherein the anolyte is an acid. 55

8. A process as claimed in claim 7 wherein the acid is sulphuric acid, hydrochloric acid, nitric acid or acetic acid.

9. A process as claimed in any one of claims 1 to 6 wherein the anolyte is an alkali.

10. A process as claimed in claim 9 wherein the alkali is sodium hydroxide, potassium hydroxide or ammonium hydroxide.

11. A process as claimed in any one of the preceding claims wherein the catholyte is an electrolyte which is the same as the anolyte.

12. A process as claimed in any one of the preceding claims wherein the microporous plastics separator has a pore size in the range of from 0.01 to 0.1 microns and a pore volume of about 50%.

6 GB 2 181 158A 6

13. A process as claimed in any one of the preceding claims wherein the microporous plastics separator is made from a plastics material which is wettable or which can be treated to render it wettable.

14. A process as claimed in any one of the preceding claims which is carried out continu5 ously.

15. A process as claimed in claim 1 substantially as hereinbefore described with reference to the single figure of the accompanying drawings.

16. A process as claimed in claim 1 substantially as hereinbefore described with reference to any one of Examples 1 to 9.

17. A metal salt which has been produced by a process as claimed in any one of the 10 preceding claims.

Printed for Her Majesty's Stationery Office by Burgess & Son (Abingdon) Ltd, Dd 8991685, 1987. Published at The Patent Office, 25 Southampton Buildings, London, WC2A 1 AY, from which copies may be obtained.

i