U.S. patent application number 11/878110 was filed with the patent office on 2008-01-31 for method of leaching copper sulfide ores containing chalcopyrite.
This patent application is currently assigned to NIPPON MINING & METALS CO., LTD.. Invention is credited to Tsuyoshi Mitarai, Norimasa Ohtsuka.
Application Number | 20080026450 11/878110 |
Document ID | / |
Family ID | 38986792 |
Filed Date | 2008-01-31 |
United States Patent
Application |
20080026450 |
Kind Code |
A1 |
Ohtsuka; Norimasa ; et
al. |
January 31, 2008 |
Method of leaching copper sulfide ores containing chalcopyrite
Abstract
An object of the present invention is to provide a method of
efficiently leaching copper from copper sulfide ores containing
chalcopyrite at room temperature. A method of recovering copper
from copper sulfide ores, characterized by comprising: using a
sulfuric acid solution having a chloride ion concentration adjusted
to 6 g/L or more but less than 18 g/L and a pH adjusted to 1.6 or
more but less than 2.5 as a leaching solution; and carrying out
copper leaching with the addition of a chloride ion-resistant
sulfur-oxidizing bacterium to the leaching solution, when
recovering copper from copper sulfide ores containing chalcopyrite,
is provided.
Inventors: |
Ohtsuka; Norimasa; (Ibaraki,
JP) ; Mitarai; Tsuyoshi; (Ibaraki, JP) |
Correspondence
Address: |
BIRCH STEWART KOLASCH & BIRCH
PO BOX 747
FALLS CHURCH
VA
22040-0747
US
|
Assignee: |
NIPPON MINING & METALS CO.,
LTD.
|
Family ID: |
38986792 |
Appl. No.: |
11/878110 |
Filed: |
July 20, 2007 |
Current U.S.
Class: |
435/262 |
Current CPC
Class: |
C22B 3/18 20130101; Y02P
10/236 20151101; C22B 15/0071 20130101; Y02P 10/20 20151101; Y02P
10/234 20151101; C22B 15/0069 20130101 |
Class at
Publication: |
435/262 |
International
Class: |
C22B 15/00 20060101
C22B015/00 |
Foreign Application Data
Date |
Code |
Application Number |
Jul 27, 2006 |
JP |
2006-204454 |
Claims
1. A method of recovering copper from copper sulfide ores,
characterized by comprising: using a sulfuric acid solution having
a chloride ion concentration adjusted to 6 g/L or more but less
than 18 g/L and a pH adjusted to 1.6 or more but less than 2.5 as a
leaching solution; and carrying out copper leaching with the
addition of a chloride ion-resistant sulfur-oxidizing bacterium to
the leaching solution, when recovering copper from copper sulfide
ores containing chalcopyrite.
2. The method according to claim 1, wherein the initial copper (II)
ion concentration and the initial iron (II) ion concentration are
adjusted to 0.5 g/L or more but less than 5 g/L.
3. The method according to claim 1 or 2, wherein the chloride
ion-resistant sulfur-oxidizing bacterium is of an Acidithiobacillus
sp. TTH-19A strain (NITE P-164).
Description
TECHNICAL FIELD
[0001] The present invention relates to a method of efficiently
recovering copper from copper sulfide ores and particularly from
primary copper sulfide ores such as chalcopyrite.
BACKGROUND ART
[0002] Hitherto, copper metallurgy has been carried out mainly by
pyrometallurgy whereby copper metal is obtained by electrolyzing
crude copper that is obtained via concentrate smelting. However, in
view of energy saving and influences upon the environment,
hydrometallurgy (SX-EW: solvent extraction-electrowinning) not
involving smelting has been rapidly adopted in recent years.
Hydrometallurgy is regarded as a technology to replace
pyrometallurgy. In the SX-EW method, copper is dissolved from
copper ores with the use of sulfuric acid, copper is removed from
the leach solution with the use of an organic solvent, and
electrolytic copper is obtained via electrolysis. A typical solvent
used for hydrometallurgy of copper ores is sulfuric acid. Thus,
target ores used for hydrometallurgy have been limited to copper
oxide ores that are readily dissolved in sulfuric acid. However, in
general, there are fewer copper oxide ore reserves that can be used
are than copper sulfide ore reserves. Thus, the use of copper
sulfide ores with large ore reserves as target ores for
hydrometallurgy has been examined.
[0003] Examples of known leaching operations for copper sulfide
ores via hydrometallurgy include a leaching operation performing an
agitated batch reaction with the use of sulfuric acid or
hydrochloric acid and a leaching operation (heap leaching method):
forming ore heaps, supplying sulfuric acid or hydrochloric acid to
the tops of the ore heaps, and recovering liquid dripping therefrom
due to the force of gravity. However, with such heap leaching
method, leaching takes several years. In addition, leaching rate of
copper is extremely low, resulting in poor efficiency. Further, a
method of efficiently leaching copper with the use of
microorganisms such as an iron-oxidizing bacterium and recovering
copper (bacterial leaching method) has also been used. According to
such bacterial leaching method, iron (II) ions in a leaching
solution are oxidized into iron (III) ions that functions as
powerful oxidants with the use of an iron-oxidizing bacterium. At
such time, sulfur contained in ores is oxidized by iron (III) ions
so that sulfuric acid is produced. Thereafter, copper in ores is
eluted in the form of copper sulfate due to the presence of the
produced sulfuric acid.
[0004] The aforementioned bacterial leaching method has been
applied in practice with the use of secondary copper sulfide ores
containing chalcocite (Cu.sub.2S), covellite (CuS), or the like,
which have been found in secondary enriched zones of porphyry
copper deposits. However, such technology has been developed mainly
for the purpose of using primary copper sulfide ores containing
copper chalcopyrite (CuFeS.sub.2), which most abundantly exist as
copper resources.
[0005] However, chalcopyrite is substantially insoluble in sulfuric
acid. In addition, the copper leaching rate is extremely slow.
Therefore, a variety of techniques in addition to the addition of
an oxidant in order to improve the leaching rate have been
suggested.
[0006] For instance, high temperature-pressure treatments (JP
Patent No. 3046986, JP Patent Publication (Kokai) No. 2001-515145
A, and JP Patent Publication (Kokai) No. 2003-328050 A), the
maintenance of a certain redox potential (of a Ag/AgCl reference
electrode) by adjusting iron content and the ratio of trivalent
irons to divalent irons (JP Patent Publication (Kokai) No.
10-265864 A (1998)), the maintenance of a certain redox potential
by adding activated carbon and iron to a leaching solution (JP
Patent Publication (Kokai) No. 2005-15864 A), and other techniques
have been reported. Although all of the aforementioned methods are
effective for improving leaching rate to some extent, such methods
are problematic because of the high costs of energy and reagents
used. Further, at an advanced stage of a leaching reaction, the
leaching rate is significantly lowered due to a leaching inhibition
phenomenon caused by residual sulfur on the surface of a
sulfur-containing concentrate, which is also problematic.
Therefore, in practice, there is no practicable technology
involving hydrometallurgy with the use of primary copper sulfide
ores containing chalcopyrite.
DISCLOSURE OF THE INVENTION
[0007] In view of the aforementioned reasons, it is an objective of
the present invention to provide a method of recovering copper from
primary copper sulfide ores containing chalcopyrite as a main
constituent under versatile conditions for real operation in an
efficient and cost-effective manner.
[0008] As a result of intensive studies to achieve above
objectives, the inventors of the present invention have found that
the copper leaching rate can be promoted at room temperature when
recovering copper from primary copper sulfide ores containing
chalcopyrite via hydrometallurgy in a manner such that the chloride
ion concentration of a leaching solution is adjusted and a chloride
ion-resistant sulfur-oxidizing bacterium is added to the leaching
solution. Also, they have found that such leaching-promoting effect
is enhanced by adjusting the initial copper (II) ion concentration
and the initial iron (II) ion concentration in the leaching
solution. These have led to the completion of the present
invention.
[0009] Specifically, the present invention encompasses the
following inventions.
(1) A method of recovering copper from copper sulfide ores,
characterized by comprising: using a sulfuric acid solution having
a chloride ion concentration adjusted to 6 g/L or more but less
than 18 g/L and a pH adjusted to 1.6 or more but less than 2.5 as a
leaching solution; and carrying out copper leaching with the
addition of a chloride ion-resistant sulfur-oxidizing bacterium to
the leaching solution, when recovering copper from copper sulfide
ores containing chalcopyrite.
(2) The method according to (1), wherein the initial copper (II)
ion concentration and the initial iron (II) ion concentration are
adjusted to 0.5 g/L or more but less than 5 g/L.
[0010] (3) The method according to (1) or (2), wherein the chloride
ion-resistant sulfur-oxidizing bacterium is of an Acidithiobacillus
sp. TTH-19A strain (NITE P-164).
BRIEF DESCRIPTION OF THE DRAWINGS
[0011] FIG. 1 is a graph showing time course changes in the
bacterial density of a leaching solution (pH 1.8) upon copper
leaching with the use of leaching solutions of Examples 1 and 2 and
Comparative Examples 1 to 4 with the addition of a chloride
ion-resistant sulfur-oxidizing bacterium (1.times.10.sup.7
cells/mL) (Example 1: chloride ion concentration=6 g/L; Example 2:
chloride ion concentration=12 g/L; Comparative Example 1: chloride
ion concentration=0 g/L; Comparative Example 2: chloride ion
concentration=3 g/L; Comparative Example 3: chloride ion
concentration=18 g/L; and Comparative Example 4: chloride ion
concentration=30 g/L).
[0012] FIG. 2 is a graph showing time course changes in the pH of a
leaching solution (pH 1.8) upon copper leaching with the use of
leaching solutions of Examples 1 and 2 and Comparative Examples 1
to 4 with the addition of a chloride ion-resistant sulfur-oxidizing
bacterium (1.times.10.sup.7 cells/mL) (Example 1: chloride ion
concentration=6 g/L; Example 2: chloride ion concentration=12 g/L;
Comparative Example 1: chloride ion concentration=0 g/L;
Comparative Example 2: chloride ion concentration=3 g/L;
Comparative Example 3: chloride ion concentration=18 g/L; and
Comparative Example 4: chloride ion concentration=30 g/L).
[0013] FIG. 3 is a graph showing time course changes in the copper
concentration of a leaching solution (pH 1.8) upon copper leaching
with the use of leaching solutions of Examples 1 and 2 and
Comparative Examples 1 to 4 with the addition of a chloride
ion-resistant sulfur-oxidizing bacterium (1.times.10.sup.7
cells/mL) (Example 1: chloride ion concentration=6 g/L; Example 2:
chloride ion concentration=12 g/L; Comparative Example 1: chloride
ion concentration=0 g/L; Comparative Example 2: chloride ion
concentration=3 g/L; Comparative Example 3: chloride ion
concentration=18 g/L; and Comparative Example 4: chloride ion
concentration=30 g/L).
[0014] FIG. 4 is a graph showing time course changes in the
bacterial density of a leaching solution upon copper leaching with
the use of leaching solutions of Examples 1, 3, and 4 and
Comparative Examples 5 and 6 with the addition of a chloride
ion-resistant sulfur-oxidizing bacterium (1.times.10.sup.7
cells/mL) (Example 1: pH=1.8; Example 3: pH=1.6; Example 4: pH=2.0;
Comparative Example 5: pH=1.4; and Comparative Example 6:
pH=2.5).
[0015] FIG. 5 is a graph showing time course changes in the copper
concentration of a leaching solution upon copper leaching with the
use of leaching solutions of Examples 1, 3, and 4 and Comparative
Examples 5 and 6 with the addition of a chloride ion-resistant
sulfur-oxidizing bacterium (1.times.10.sup.7 cells/mL) (Example 1:
pH=1.8; Example 3: pH=1.6; Example 4: pH=2.0; Comparative Example
5: pH=1.4; and Comparative Example 6: pH=2.5).
[0016] FIG. 6 is a graph showing time course changes in increase in
copper concentration of a leaching solution upon copper leaching
with the use of leaching solutions of Examples 1, 5, and 6 and
Comparative Examples 7 and 8 with the addition of a chloride
ion-resistant sulfur-oxidizing bacterium (1.times.10.sup.7
cells/mL) (Example 1: initial copper (II) ion concentration=0 g/L,
initial iron (II) ion concentration=0 g/L; Example 5: initial
copper (II) ion concentration=0.5 g/L, initial iron (II) ion
concentration=0.5 g/L; Example 6: initial copper (II) ion
concentration=1.0 g/L, initial iron (II) ion concentration=1.0 g/L;
Comparative Example 7: initial copper (II) ion concentration=0.1
g/L, initial iron (II) ion concentration=0.1 g/L; and Comparative
Example 8: initial copper (II) ion concentration=5.0 g/L, initial
iron (II) ion concentration=5.0 g/L).
[0017] Hereinafter the present invention will be described in
detail. The present application claims the priority of Japanese
Patent Application No. 2006-204454 filed on Jul. 27, 2006 and
encompasses contents described in the specification and/or drawings
of the patent application.
[0018] The method of recovering copper from copper sulfide ores of
the present invention characterized by comprising: using a sulfuric
acid solution having a chloride ion concentration adjusted to 6 g/L
or more but less than 18 g/L and a pH adjusted to 1.6 or more but
less than 2.5 as a leaching solution; and carrying out copper
leaching with the addition of a chloride ion-resistant
sulfur-oxidizing bacterium to the leaching solution, when
recovering copper from copper sulfide ores containing
chalcopyrite.
[0019] Copper sulfide ores containing chalcopyrite as target ores
of the present invention may be copper sulfide ores containing
chalcopyrite as a main constituent or copper sulfide ores that
partially contain chalcopyrite, for example. The chalcopyrite
content is not particularly limited.
[0020] Further, when it comes to hydrometallurgy of copper using a
sulfuric acid solution as a leaching solution, the method of the
present invention can be used in any types of leaching operations.
For example, not only agitated batch leaching but also heap
leaching and dump leaching where copper is leached into sulfuric
acid by sprinkling sulfuric acid over ore heaps may be optionally
adopted.
[0021] Dissolution and leaching of copper sulfide ores proceed
through a series of reactions shown in Equation 1 to Equation 3
below.
Cu.sup.2++Fe.sup.2+Cu.sup.++Fe.sup.3+ (Equation 1)
CuFeS.sub.2+Cu.sup.++Fe.sup.3+.fwdarw.Cu.sub.2S+2Fe.sup.2++S
(Equation 2)
Cu.sub.2S+4Fe.sup.3+.fwdarw.2Cu.sup.2++4Fe.sup.2++S (Equation
3)
[0022] According to the method of the present invention, the
equilibrium of the above Equation 1 is shifted toward the right by
increasing chloride ion concentration in the leaching solution (D.
M. Muir, M. D. Benari, B. W. Clare et al, Hydrometallurgy, 9, 257,
1981). As a result, the reaction in Equation 2 can be
accelerated.
[0023] According to the method of the present invention, the
chloride ion concentration of a leaching solution is adjusted to 6
g/L or more but less than 18 g/L. The chloride ion concentration of
a leaching solution may be optionally adjusted with the addition
of, for example, sodium chloride. When the chloride ion
concentration of a leaching solution is less than 6 g/L, a small
leaching-promoting effect is obtained. Meanwhile, when the
concentration exceeds 18 g/L, growth inhibition is induced even
with the use of a chloride ion-resistant sulfur-oxidizing
bacterium, which is undesirable.
[0024] Elemental sulfur that is produced in the above reactions
(Equations 2 and 3) and causes a coating phenomenon is removed in
the reaction described below (Equation 4) with the addition of a
chloride ion-resistant sulfur-oxidizing bacterium. As a result,
deceleration of the leaching rate is prevented so that efficient
leaching can be realized.
S+1.5O.sub.2+H.sub.2O sulfur-oxidizing
bacterium.fwdarw.H.sub.2SO.sub.4 (Equation 4)
[0025] Herein, the term "chloride ion-resistant sulfur-oxidizing
bacterium" indicates any sulfur-oxidizing bacterium without
particular limitation as long as such sulfur-oxidizing bacterium is
not inhibited in terms of growth or ability to oxidize sulfur at a
high chloride ion concentration of a leaching solution (6 g/L or
more but less than 18 g/L) as described above.
[0026] A preferred example of such sulfur-oxidizing bacterium that
can be used is the Acidithiobacillus sp. TTH-19A strain that was
deposited under accession number NITE P-164 at the Patent
Microorganisms Depositary, National Institute of Technology and
Evaluation (NPMD) (2-5-8 Kazusakamatari, Kisarazu-shi, Chiba), an
Independent Administrative Institution, on Jan. 13, 2006.
[0027] Meanwhile, Cu.sub.2S produced above (Equation 2) is
dissolved by the reaction described below (Equation 5). Thus, it is
advantageous to set the pH at a low level for leaching. Although
sulfuric acid produced above (Equation 4) accelerates leaching, the
growth of a sulfur-oxidizing bacterium is inhibited when the pH is
less than 1.6.
[0028] Further, in a case of a pH of more than 2.5, the leaching
reaction is inhibited due to production of jarosite and the like.
Thus, the pH of a leaching solution is preferably 1.6 or more but
less than 2.5.
Cu.sub.2S+4H.sup.++O.sub.2.fwdarw.2Cu.sup.2++2H.sub.2O+S (Equation
5)
[0029] The amount of the aforementioned sulfur-oxidizing bacterium
added to a leaching solution is not particularly limited. However,
in general, such bacterium is added so as to result in a bacterial
density of 1.times.10.sup.6 to 1.times.10.sup.7 cells/mL. It is not
necessary to adjust a bacterial density that varies in a
time-dependent manner to a specific level.
[0030] Furthermore, in another preferred embodiment of the method
of the present invention, in addition to the adjustment of the
chloride ion concentration of a leaching solution described above,
the initial copper (II) ion concentration and the initial iron (II)
ion concentration are adjusted. As a result, the above reaction
(Equation 1) is further promoted so that it becomes possible to
accelerate the leaching rate.
[0031] Preferably, the initial copper (II) ion concentration of a
leaching solution is adjusted to 0.5 g/L or more but less than 5
g/L. The initial copper (II) ion concentration of a leaching
solution is adjusted with the addition of, for example, copper (II)
sulfate. Alternatively, when pregnant leach solution (PLS) is
subjected to solvent extraction, such as via the SX-EW method for
recovering copper, a raffinate obtained after solvent extraction is
repeatedly used as a lixivant. Accordingly, the copper (II) ion
concentration of such raffinate may be adjusted to a certain
concentration. When the initial concentration is less than 0.5 g/L,
a small leaching-promoting effect is obtained. On the other hand,
when the initial concentration exceeds 5 g/L, the amount of reagent
added is increased and the solvent extraction yield declines,
resulting in undesirable poor cost-effectiveness.
[0032] In addition, preferably, the initial iron (II) ion
concentration of a leaching solution is adjusted to 0.5 g/L or more
but less than 5 g/L. The iron (II) ion concentration of a leaching
solution may be adjusted with the addition of, for example, iron
(II) sulfate. When the iron (II) ion concentration of a leaching
solution is less than 0.5 g/L, a small leaching-promoting effect is
obtained. On the other hand, when the concentration exceeds 5 g/L,
the amount of reagent added is increased, resulting in undesirable
poor cost-effectiveness.
BEST MODES FOR CARRYING OUT THE INVENTION
[0033] Hereinafter, the present invention is more specifically
described by way of examples and comparative examples. However, the
present invention is not limited thereto.
EXAMPLES 1 AND 2
[0034] Concentrate (mined in Candelaria) containing chalcopyrite as
a main constituent was used as a target ore. The quality of the
concentrate was as follows: Cu=28% by mass; Fe=28% by mass; and
S=32% by mass.
[0035] Three grams of the above concentrate was mixed with 300 mL
of a leaching solution (containing: ammonium sulfate=3 g/L;
potassium hydrogen phosphate=0.5 g/L; magnesium sulfate
heptahydrate=0.5 g/L; and potassium chloride=0.1 g/L) that had been
adjusted to a pH of 1.8 with sulfuric acid and poured into a 500 mL
Shaking flask. To the leaching solution in the flask, sodium
chloride was added so that the chloride ion concentration became 6
g/L (Example 1) or 12 g/L (Example 2), and a chloride ion-resistant
sulfur-oxidizing bacterium (Acidithiobacillus sp. TTH-19A strain:
accession no. NITE P-164) was further added at a density of
1.times.10.sup.7 cells/mL. Then the flask was shaken at room
temperature for a certain period of time. The bacterial density,
pH, and copper concentration of the supernatant of the resulting
leaching solution were measured. Then, time course changes in the
measurement results were examined.
COMPARATIVE EXAMPLES 1 TO 4
[0036] Shaking leaching (Comparative Example 1) was performed at
room temperature in the same manner as in Example 1, except that
sodium chloride was not added to the leaching solution described in
Example 1. In addition, shaking leaching was performed at room
temperature in the same manner as in Example 1 except that sodium
chloride was added to the leaching solution described in Example 1
so that the chloride ion concentration became 3 g/L (Comparative
Example 2), 18 g/L (Comparative Example 3), or 30 g/L (Comparative
Example 4).
[0037] The experimental results of Examples 1 and 2 and Comparative
Examples 1 to 4 are shown in FIG. 1 (changes in bacterial density),
FIG. 2 (changes in pH), and FIG. 3 (changes in copper
concentration).
[0038] As shown in FIG. 1, in the cases of Examples 1 and 2 and
Comparative Examples 1 and 2, bacterial growth was observed.
However, in the cases of Comparative Examples 3 and 4, bacterial
growth was not observed. This is because the levels of chloride ion
concentrate in Comparative Examples 3 and 4 exceeded the upper
level of the growth conditions for the chloride ion-resistant
sulfur-oxidizing bacterium (Acidithiobacillus sp. TTH-19A strain:
accession no. NITE P-164).
[0039] As shown in FIG. 2, in the cases of Comparative Examples 3
and 4 in which bacterial growth was not observed, production of
sulfuric acid due to oxidation of sulfur represented by Equation 4
did not take place, resulting in increases in pH. Simultaneously,
concentrate particles were floating on the surface of the leaching
solution due to a coating phenomenon caused by elemental
sulfur.
[0040] As shown in FIG. 3, the copper concentration of Example 1
(Day 34: 1.0 g/L) was higher than that of Comparative Example 1
(Day 30: 0.74 g/L). Thus, it was confirmed that the copper leaching
rate was fast in the case of Example 1. In the case of Example 2,
the copper leaching rate became faster (Day 34: 1.4 g/L).
[0041] Meanwhile, in the case of Comparative Example 2, the
increase in copper leaching rate was small (Day 34: 0.84 g/L).
Thus, the effect of the addition of sodium chloride was not
observed.
[0042] Based on the above results, it has been found that efficient
copper leaching can be carried out by adding chloride ions (6 g/L
or more but less than 18 g/L) and chloride ion-resistant
sulfur-oxidizing bacteria to a leaching solution at a pH of
1.8.
EXAMPLES 3 AND 4
[0043] Shaking leaching was performed at room temperature in the
same manner as in Example 1 except that sulfuric acid was added to
the leaching solution described in Example 1 so that the leaching
solution was adjusted to a pH of 1.6 (Example 3) or a pH of 2.0
(Example 4). The bacterial density and copper concentration of the
supernatant of the leaching solution were measured. Then, time
course changes in measurement results were examined.
COMPARATIVE EXAMPLES 5 AND 6
[0044] Shaking leaching was performed at room temperature in the
same manner as in Example 1 except that sulfuric acid was added to
the leaching solution described in Example 1 so that the leaching
solution was adjusted to a pH of 1.4 (Comparative Example 5) or a
pH of 2.5 (Comparative Example 6). The bacterial density and copper
concentration of the supernatant of the leaching solution were
measured. Then, time course changes in the measurement results were
examined.
[0045] The experimental results of Examples 1, 3, and 4 and
Comparative Examples 5 and 6 are shown in FIG. 4 (changes in
bacterial density) and FIG. 5 (changes in copper
concentration).
[0046] As shown in FIG. 4, in the cases of Examples 1, 3, and 4 and
Comparative Example 6, bacterial growth was observed. However, in
the case of Comparative Example 5, bacterial growth was not
observed. This is because the growth of the chloride ion-resistant
sulfur-oxidizing bacterium (Acidithiobacillus sp. TTH-19A strain:
accession no. NITE P-164) was inhibited at a low pH.
[0047] As shown in FIG. 5, the copper concentration in the case of
Example 3 (Day 30: 1.2 g/L) and the copper concentration in the
case of Example 4 (Day 30: 0.96 g/L) were almost equivalent to or
exceeded the copper concentration in the case of Example 1 (Day 34:
1.0 g/L). However, in the case of Comparative Example 6 (Day 30:
0.82 g/L), a leaching reaction was inhibited due to production of
jarosite and the like so that it was confirmed that the copper
leaching rate was slow.
EXAMPLES 5 AND 6
[0048] Shaking leaching was performed at room temperature in the
same manner as in Example 1 except that the initial copper (II) ion
concentration and the initial iron (II) ion concentration in the
leaching solution were adjusted to 0.5 g/L (Example 5) or 1.0 g/L
(Example 6). An increase in the copper concentration in the
supernatant of the leaching solution was measured. Then, time
course changes in the measurement results were examined.
COMPARATIVE EXAMPLES 7 AND 8
[0049] Shaking leaching was performed at room temperature in the
same manner as in Example 1 except that the initial copper (II) ion
concentration and the initial iron (II) ion concentration in the
leaching solution were adjusted to 0.1 g/L (Comparative Example 7)
or 5.0 g/L (Comparative Example 8). An increase in the copper
concentration in the supernatant of the leaching solution was
measured. Then, time course changes in the measurement results were
examined.
[0050] FIG. 6 shows changes in increases in copper concentrations
in the cases of Examples 1, 5, and 6 and Comparative Examples 7 and
8. Increases in the copper concentrations in the cases of Example 5
(Day 30: 1.1 g/L) and Example 6 (Day 30: 1.2 g/L) exceeded the
increase in the copper concentration in the case of Example 1 (Day
34: 1.0 g/L). However, it was impossible to confirm the effect of
adjusting the initial copper (II) ion concentration and the initial
iron (II) ion concentration in the leaching solution in the case of
Comparative Example 7 (Day 30: 0.98 g/L). In the case of
Comparative Example 8, a large increase in the copper concentration
was obtained. However, when the initial copper (II) ion
concentration and the initial iron (II) ion concentration in the
leaching solution exceeded 5 g/L, the amount of reagent added was
increased and the yield of solvent extraction declined, resulting
in undesirable poor cost-effectiveness.
[0051] All publications, patents, and patent applications cited
herein are incorporated herein by reference in their entirety.
INDUSTRIAL APPLICABILITY
[0052] According to the present invention, efficient leaching of
copper from copper sulfide ores containing chalcopyrite can be
achieved at room temperature. A high temperature-pressure treatment
is not necessary for the method of the present invention. Thus, it
is possible to promote a copper leaching rate by merely adjusting
the chloride ion concentration of a leaching solution with sodium
chloride, for example. Therefore, the method of the present
invention is simple and highly cost-effective. In addition, with
the addition of a chloride ion-resistant sulfur-oxidizing bacterium
to a leaching solution, sulfur can be changed into sulfuric acid,
such sulfur being produced as a by-product during a leaching
reaction for copper sulfide ores so as to adhere to ore surfaces,
causing deterioration in leaching performance. Accordingly, it
becomes possible to prevent a coating phenomenon caused by sulfur
by-products on ore surfaces and to perform efficient leaching of
copper as a result of the consumption of the sulfuric acid produced
during copper leaching.
* * * * *