Patent Application
20130074655
The present invention relates to gold and silver extraction with halogens. More precisely, it relates to a method and a system for gold extraction with halogens recycling.
It has been reported (U.S. Pat. No. 7,537,741) that gold/silver-bearing ores, after being deprived of most of their base metals such as Cu, Zn, Fe and chalcogens such as sulfur and tellurium, can be treated very efficiently with halogens for precious metals recovery. The ore is slurried in a brine of sodium chloride incorporating a minor portion of sodium bromide, and elemental chlorine is then admitted to the system at near ambient temperature (40-50° C.). The high oxidation potential of the chlorine leads to the formation of some bromine from the bromide in the slurry, and the mixed halogens (chlorine, bromine) lead to a fast (a few hours) and rather complete precious metals recovery. This process is a closed loop approach, which means that the brine, after separation from the barren solution and precious metal recovery, is used as a source of elemental chlorine. This production of chlorine is done by the electrolysis of the brine in a standard electrolytic cell with either a membrane or a diaphragm for the separation of the cathodic compartment from the anodic one.
This method is submitted to significant limitations when implemented. First, the brine collects many types of ions in the course of the gold extraction, particularly elements of the alkaline earth group, such as calcium and magnesium. As state of the art materials used as diaphragms or membranes are highly sensitive to these contaminants, extensive purification of the brine is thus required prior to electrolysis. Secondly, the solubility of chlorine in water is rather low, 0.091 mole/l at 25° C. (Advanced Inorganic Chemistry, A. Cotton and G. Wilkinson, Interscience Publishers, 1972, p. 476). This solubility is further decreased if a brine of NaCl rather than pure water is used. Chlorine addition requires periods of time counted in hours rather than minutes. In turn, finally, this long addition time leads to secondary reactions of chlorine and bromine with remaining base metals in the ore, mainly iron, and with sulfur as sulphide, thus increasing the overall consumption of halogens.
There thus remains a need for an improved method and system for precious metals extraction by the halogens allowing recycling halogens.
More specifically, in accordance with the present invention, there is provided a method for extracting precious metals from ore, comprising, in a reactor, slurrying the ore in the salt brine, acidifying the slurried ore and contacting the acidic slurried ore with halogens, said halogens being fed to the reactor in the form of hypohalites.
There is further provided a system for extracting precious metals from ore, comprising a diaphragm-less electrolytic cell; a leaching reactor; and a brine reservoir, the brine reservoir feeding the diaphragm-less electrolytic cell and the leaching reactor; and the leaching reactor receives the ore, brine from the brine reservoir, hypohalite generated in the diaphragm-less electrolytic cell, and an acid.
There is provided a method of gold and silver extraction from ore in a reactor, using diluted hypochlorites as a source of active chlorine, comprising controlling the pH of slurried ore in a range between 0.5 and 3, and adding hypochlorites in an amount sufficient to raise the oxido-reduction potential of the reactor in a range comprised between about 0.7 and about 1.2 V vs a Ag/AgCl reference electrode.
Other objects, advantages and features of the present invention will become more apparent upon reading of the following non-restrictive description of specific embodiments thereof, given by way of example only with reference to the accompanying drawings.
In the appended drawings:
There are known methods for the production of hypohalites, such as hypochorites (NaOCl) and hypobromites (NaOBr), by electrolysis of brine. For example, the company Siemens commercializes a system called OSEC® B-Pak generating a sodium hypochlorite solution through the electrolysis of brine, using an electrolytic cell devoid of membrane or diaphragm, and wherein the catolytic and anolytic solutions are mixed inside the cell to give corresponding hypohalites, NaOCl or NaOBr. These hypohalites are very soluble in water, and, in the case of NaOCl, they may be used at concentrations in the range of 0.5 to 1.0% for the purification of drinking water.
Surprisingly, it was found, in the present invention, that the use of diluted hypochlorites as a source of active chlorine was very efficient for gold and silver extraction, providing the pH of the slurried ore in the reactor is acidic, in a range between 0.5 and 3, and providing the added hypochlorites raised the oxido-reduction potential (ORP) of the system to about 0.85 V (Ag/AgCl reference). There is no need of complex, full-fledged compartmented electrolytic cells. Moreover, the rate of addition of active chlorine is greatly improved due to the high solubility of hypohalites, and secondary reactions with iron and sulfides are much decreased.
The production of hypochlorites (NaOCl) from salt brine can be described by the following equations (I):
Cathode 2Na++2e−→2Na
2Na+2H2O→2 NaOH+H2
Anode 2Cl−→Cl2+2e−
Mixing 2NaOH+Cl2→NaCl+NaOCl
Similar equations can be written for the production of hypobromites (NaOBr).
With a diaphragm-less cell, concentration of active chlorine, that is hypochlorites (NaOCl), at the level of 0.5 to 2.0% of active chlorine can be achieved, with equipment sold commercially for water purification for example.
The hypochlorite solution (NaOCl) can oxidize the bromide ion to elemental bromine (Oxidation Potential, W. M. Latimer, Prentice-Hall, 1952, pp. 56 and 62). Therefore, sodium hypochlorite can generate, in the reactor, the bromine required for gold extraction from the slurried ore. Also, the addition of the sodium hypochlorite is done in a slurry which is made acidic with an acid such as sulfuric acid, for example. Besides eliminating the carbonates that might be present in the ore, this acidic addition displaces the equilibrium of the hypochlorite/water system towards the liberation of free chlorine, as illustrated by the following equations (II):
H2SO4(excess)+2NaOCl→2HOCl+NA2SO4 pH 1.5-3.0
H2SO4+2 NaCl→2 HCl+Na2SO4
2HOCl+2H++2Cl−→2Cl2/2H2O
(Cotton and Wilkinson, Ibid., p. 476.)
In the present invention, very soluble hypochlorites are used as an intermediate form of active halogen used for recycling halogens, the free halogens being recovered in the reaction cell, under acidic conditions. The amount of hypohalite required to obtain a rapid and near-complete lixiviation of precious metals from the ore has been found to be of the order of one percent of the weight of the slurried ore, the corresponding ORP being in the range of 0.75 to 1.0 V, for example of 0.85 V.
This situation represents a very significant improvement over the direct chlorination with elemental chlorine, where the ratio of chlorine to ore was from 2% to 10%. Also, a significant decrease of the consumption of active chlorine by base metals in the ore, typically mostly iron, has been noted.
Those results are illustrated by the following examples.
A gold ore showing the following analysis: 2.6 g/t Au, 1.2 g/t Ag, 5.0% Fe, 0.4% S2− and ground to 80% minus 120 mesh was slurried (35% solid) in a brine 7% NaCl and 2% NaBr, the temperature being 40° C. The chlorination was done in two different ways: i) with direct chlorination with elemental chlorine, and ii) by addition of sodium hypochlorite as a source of active halogen.
The following Table I gives comparative results.
The same gold ore (200 g) as in Example 1 was slurried in a brine (100 g/L NaCl and 30 g/L NaBr) giving 30% solid content. The slurried ore was stirred at 40° C. for four hours and hypochlorite NaOCl 12% was added so as to have a 0.5% NaOCl concentration. Then, variable acidic (H2SO4) addition was done, yielding 5 different systems, with different ORP. Results are shown in the following Table II.
As clearly seen from these examples, an increase in acidity, as shown by pH decrease, corresponds to an accelerated halogen release and improved gold recovery.
A method according to an embodiment of an aspect of the present invention, as shown in the flowchart of
A system according to an embodiment of the present invention, as illustrated for example in
There is thus provided a system and a method for the extraction of precious metals by halogens (Cl2, Br2) where the halogens are recycled to the leaching reactor in the form of hypohalites. The formation of hypohalites is achieved by the electrolysis of brine in a diaphragm-less cell. The solution of recycled hypohalites is fed to an acidic slurry of the ore in the leaching reactor, the pH of the slurry being leached being between 0.5 and 3, with a preferred value of 1.5, and the ORP in the reactor is in the range of 0.7 to 1.2 V (Ag/AgCl reference electrode), with a preferred value of 0.85. The hypohalite may be NaOCl as active halogen, or NaOBr as active halogen, or a mixture of both hypohalites, in an amount between about 0.5 and 2 percent of the ore. A preferred concentration of NaOCl is 1.5%.
Although the present invention has been described hereinabove by way of embodiments thereof, it may be modified, without departing from the nature and teachings of the subject invention as recited herein.
This application claims benefit of U.S. provisional application Ser. No. 61/539,517, filed on Sep. 27, 2011. All documents cited herein are incorporated herein in their entirety by reference.
| Number | Date | Country | |
|---|---|---|---|
| 61539517 | Sep 2011 | US |
