CA1065143A - Recovery of copper from chalcopyrite utilizing copper sulfate leach - Google Patents
Recovery of copper from chalcopyrite utilizing copper sulfate leachInfo
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- CA1065143A CA1065143A CA243,025A CA243025A CA1065143A CA 1065143 A CA1065143 A CA 1065143A CA 243025 A CA243025 A CA 243025A CA 1065143 A CA1065143 A CA 1065143A
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- chalcopyrite
- sulfate
- copper sulfate
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Abstract
RECOVERY OF COPPER FROM CHALCOPYRITE
UTILIZING COPPER SULFATE LEACH
ABSTRACT OF THE INVENTION
Copper is recovered from chalcopyrite by means of a pollution-free hydrometallurgical process which entails leaching and converting the chalcopyrite with copper sulfate in order to produce an insoluble copper sulfide, a soluble iron sulfate and sulfuric acid. A secondary leach is then conducted in order to react the copper sulfide with oxygen in the presence of a jarosite-forming cation to produce a soluble copper sulfate and an insoluble iron bearing jarosite.
This copper sulfate is separated from the jarosite and sent to a copper recovery process and/or recycled. Alternatively, the copper sulfide from the initial leach may be separated from the iron sulfate solution immediately after the initial leach, and this copper sulfide can be treated with other processes to produce elemental copper and sulfur.
UTILIZING COPPER SULFATE LEACH
ABSTRACT OF THE INVENTION
Copper is recovered from chalcopyrite by means of a pollution-free hydrometallurgical process which entails leaching and converting the chalcopyrite with copper sulfate in order to produce an insoluble copper sulfide, a soluble iron sulfate and sulfuric acid. A secondary leach is then conducted in order to react the copper sulfide with oxygen in the presence of a jarosite-forming cation to produce a soluble copper sulfate and an insoluble iron bearing jarosite.
This copper sulfate is separated from the jarosite and sent to a copper recovery process and/or recycled. Alternatively, the copper sulfide from the initial leach may be separated from the iron sulfate solution immediately after the initial leach, and this copper sulfide can be treated with other processes to produce elemental copper and sulfur.
Description
BACKGRO~IND OF THE INVENT ON
Field o~ the In~ention This invention relates to the hydrometallurgical.
- recovery of copper from chalcopyrite by means of a copper :~ sul~ate leaching process.
The Prior Art - Processes have long been disclosed describing the reco~ery o copper from its sulfide and mixed sulfide forms.
Most of the economic copper recovery processes are classified :as pyrometallurgical, with the ore being smelted to oxidize the sul~ide to sulfur dioxide. This sulfur dioxide is now o~ course recognized as a major air pollutant, and means must be used in conjunction with pyrometallurgical plants to eliminate this contaminant. As a result considerable :
-,..., ............ - - , ~
, : ~065143 development is now being undertaken to formulate hydro-metallurgical processes in order to circumvent the production of the byproauct sulfur dio~ide. Much of the hydrometallurgical development centers around chloride and ammoniacal leaching processes, some of which may prove to ultimately be beneficial.
Copper sulfate leaching agents have ~een proposed to be used in conjunction with a number of metal sulfides, including zinc sulfide. U.S. Patent 3,655,538 to Renken discloses such a process whereby the zinc sulfide is leached with copper sulfate in order to produce copper sulfide and a zinc sulfate solution, the zinc sulfate solution being easily separated for the ultimate recovery of zinc. Another similar process discloses the utilization of a copper sulfake leach to recover nickel from a nickel-copper matte, this process being set forth by Llanos et al in a paper presented at the Third Annual Meeting of the Hydrometallurgical Section of the Metallurgical Society of C.I.N., Edmonton, October 19, 1973.
Heretofore the value of leaching chalcopyrite with copper sul~ate has not been recognized, and it has commonly been believed that chalcopyrite does not react with copper .~ - , sulfate. This is borne out by the Renken patent, cited above, which specifically sets forth at column 3 that chalcopyrite does not react with copper sulfate.
It has now been recognized that under the proper processing conditions, as hereinafter set forth, copper sulfate can be used as a beneficial leaching agent for chalcopyrite, and such a process results in a number of advantages including providing an effecti~e means for sepa~at-ing coppe- sulfide from many other metal sulfides and other impurities, as well as greatly facilitating any secondary leaching o~ the copper sulfides.
,' . ' .' ' .
Field o~ the In~ention This invention relates to the hydrometallurgical.
- recovery of copper from chalcopyrite by means of a copper :~ sul~ate leaching process.
The Prior Art - Processes have long been disclosed describing the reco~ery o copper from its sulfide and mixed sulfide forms.
Most of the economic copper recovery processes are classified :as pyrometallurgical, with the ore being smelted to oxidize the sul~ide to sulfur dioxide. This sulfur dioxide is now o~ course recognized as a major air pollutant, and means must be used in conjunction with pyrometallurgical plants to eliminate this contaminant. As a result considerable :
-,..., ............ - - , ~
, : ~065143 development is now being undertaken to formulate hydro-metallurgical processes in order to circumvent the production of the byproauct sulfur dio~ide. Much of the hydrometallurgical development centers around chloride and ammoniacal leaching processes, some of which may prove to ultimately be beneficial.
Copper sulfate leaching agents have ~een proposed to be used in conjunction with a number of metal sulfides, including zinc sulfide. U.S. Patent 3,655,538 to Renken discloses such a process whereby the zinc sulfide is leached with copper sulfate in order to produce copper sulfide and a zinc sulfate solution, the zinc sulfate solution being easily separated for the ultimate recovery of zinc. Another similar process discloses the utilization of a copper sulfake leach to recover nickel from a nickel-copper matte, this process being set forth by Llanos et al in a paper presented at the Third Annual Meeting of the Hydrometallurgical Section of the Metallurgical Society of C.I.N., Edmonton, October 19, 1973.
Heretofore the value of leaching chalcopyrite with copper sul~ate has not been recognized, and it has commonly been believed that chalcopyrite does not react with copper .~ - , sulfate. This is borne out by the Renken patent, cited above, which specifically sets forth at column 3 that chalcopyrite does not react with copper sulfate.
It has now been recognized that under the proper processing conditions, as hereinafter set forth, copper sulfate can be used as a beneficial leaching agent for chalcopyrite, and such a process results in a number of advantages including providing an effecti~e means for sepa~at-ing coppe- sulfide from many other metal sulfides and other impurities, as well as greatly facilitating any secondary leaching o~ the copper sulfides.
,' . ' .' ' .
- 2 -- ( ~065i43 SUMMARY OF THE INVENTIO~I
~ pollution-free hydrometallurgical copper recovery process rcsults from the leaching of chalcopyrite with copper sulfate .in o.rder to form insoluble copper sul~ides, a soluble iron sulfate solution and sulfuric acid. The copper sulfides can then be separated from the product mixture and further treated in order to recover the copper v~lues.
Also, the products from the initial leach may be immediately - subjected to a secondary oxidation leach reaction wherein the copper sulfides are converted to a soluble copper sulfate solution and the iron is converted to an insoluble state such that the copper sulfate solution is easily separated from the residual insoluble iron cons.~ituents along with any other insoluble impurities~ The copper may then be conventionally recovered from the isolated copper sulate solution, and if , desired a portion of the copper sulfate solution may be recycled for reaction and conversion with fresh chalcopyrite feed.
. DESCRIPTION OF THE PREFERRED EMBODIMæNTS
The basic chemical reaction with which this process :. is concerned is as follows: -3CuFeS2 ~ 6CuS04 ~ 4H20 ~ Cugss + 3FeSO~ + 4H2S04 Along with the digenité (CugS5) some chalcocite (Cu2S) and covellite (CuS) in minor amounts may also be produced.
. In addition to chalcopyrite the starting materials may contain other copper sulfides, such as chalcocite and covelli~e, and also may contain sul~ides of other metals.
For example, copper may be recovered from mixed sulfides containing chalcopyrite and zinc sulfide according to the above set forth reaction since the zinc will go into solution as zinc sulfate, permitting the insoluble digenite to be easily separated from the solution cont~ining zinc sulfate, ~ 065143 iron sul~ate and sulfuric acid. Examples of okher metal sulfides which would similarly react in the presence of chalcopyrite includo nickel and co~alt.
This .ini~ial leach reaction may be opexated in accoxdcnce with convention~l leaching techniques, with a reaction tempe-cature preerably maintained at greater than about 100C, moxc preferably from about 150 to about 250C, and most preferably from about 180 to about 200C. As is comlmon in leaching operations the raw ~eed material is crushed and ground to a sufficiently small particle size in order ~o con~eniently per~orm concentration operations such as flotation. When leaching mixed sulfides containing chalcopyrite the copper sulrate concentration is preferably maintained from about 1 gram per liter of copper to saturation concentration, more preferably from about 30 to about 100, and most preferably from about 40 to about ~0 grams per liter. When proce~sing chalcopyrite alone, thi~ concentration preerably approaches the copper sulfate saturation concen~
tration. The mole ra'cio of copper sul~ate to chalcopyrite is as shown in the above set forth reaction, i.e., two rnoles of copper sulfate per mole of chalcopyrite. This i~ of course ; the stoichiome'cric amount required, and an excess amount of copper sulfate ma~ be maintained.
The reaction time is inversely proportional to temperature, the amount of time decreasing with increased~
temperatures.
As is conventional in chemical leaching, this initial leach reaction may be perfoxmed in more than one stage in order to e~editiously carry out the reaction, and may be conducted cocurrently or countercurrently.
Following the initial leach reaction the copper sulfide product may be immediately separated from the soluble - ~ ( sul~ates and sulfuric acid Such a separation is accomplished -by conventional means in the art, as for example by thickening and filtration. ~ separation at t'nis stage of the process may be preferred in some instances, however, a further separation will be necessitated at a later stage of the process since the gangue material will also be separated with the copper sulfides. Separation immediately following the initial leach reaction is therefore dictated by the particular copper sulfide reaction employed to recover the elemental copper ln values and also the composition of the initial feed material.
One preferable technique is therefore to subject the products of the initial leach and conversion reaction directly to a secondary leach reaction in,conjunction with a jarosite orming cation to convert the copper sulfides to a copper sulate solution while precipitating the iron sulfate as j jarosite. Due to the nature of this reaction it is apparent that this secondary leach will immediately follow the initial leac~h in those cases when the sulfides initially fed to ~he reaction are basically copper or iron s~lfides with only - 20 relatively small proportions of other metal sulfides. If :: , the products of the initial leach include substantial amounts of metal sulfates other than iron sulfates, it will then be preferable to separate the copper sulfides prior to the initiation of this secondary leach.
~ pollution-free hydrometallurgical copper recovery process rcsults from the leaching of chalcopyrite with copper sulfate .in o.rder to form insoluble copper sul~ides, a soluble iron sulfate solution and sulfuric acid. The copper sulfides can then be separated from the product mixture and further treated in order to recover the copper v~lues.
Also, the products from the initial leach may be immediately - subjected to a secondary oxidation leach reaction wherein the copper sulfides are converted to a soluble copper sulfate solution and the iron is converted to an insoluble state such that the copper sulfate solution is easily separated from the residual insoluble iron cons.~ituents along with any other insoluble impurities~ The copper may then be conventionally recovered from the isolated copper sulate solution, and if , desired a portion of the copper sulfate solution may be recycled for reaction and conversion with fresh chalcopyrite feed.
. DESCRIPTION OF THE PREFERRED EMBODIMæNTS
The basic chemical reaction with which this process :. is concerned is as follows: -3CuFeS2 ~ 6CuS04 ~ 4H20 ~ Cugss + 3FeSO~ + 4H2S04 Along with the digenité (CugS5) some chalcocite (Cu2S) and covellite (CuS) in minor amounts may also be produced.
. In addition to chalcopyrite the starting materials may contain other copper sulfides, such as chalcocite and covelli~e, and also may contain sul~ides of other metals.
For example, copper may be recovered from mixed sulfides containing chalcopyrite and zinc sulfide according to the above set forth reaction since the zinc will go into solution as zinc sulfate, permitting the insoluble digenite to be easily separated from the solution cont~ining zinc sulfate, ~ 065143 iron sul~ate and sulfuric acid. Examples of okher metal sulfides which would similarly react in the presence of chalcopyrite includo nickel and co~alt.
This .ini~ial leach reaction may be opexated in accoxdcnce with convention~l leaching techniques, with a reaction tempe-cature preerably maintained at greater than about 100C, moxc preferably from about 150 to about 250C, and most preferably from about 180 to about 200C. As is comlmon in leaching operations the raw ~eed material is crushed and ground to a sufficiently small particle size in order ~o con~eniently per~orm concentration operations such as flotation. When leaching mixed sulfides containing chalcopyrite the copper sulrate concentration is preferably maintained from about 1 gram per liter of copper to saturation concentration, more preferably from about 30 to about 100, and most preferably from about 40 to about ~0 grams per liter. When proce~sing chalcopyrite alone, thi~ concentration preerably approaches the copper sulfate saturation concen~
tration. The mole ra'cio of copper sul~ate to chalcopyrite is as shown in the above set forth reaction, i.e., two rnoles of copper sulfate per mole of chalcopyrite. This i~ of course ; the stoichiome'cric amount required, and an excess amount of copper sulfate ma~ be maintained.
The reaction time is inversely proportional to temperature, the amount of time decreasing with increased~
temperatures.
As is conventional in chemical leaching, this initial leach reaction may be perfoxmed in more than one stage in order to e~editiously carry out the reaction, and may be conducted cocurrently or countercurrently.
Following the initial leach reaction the copper sulfide product may be immediately separated from the soluble - ~ ( sul~ates and sulfuric acid Such a separation is accomplished -by conventional means in the art, as for example by thickening and filtration. ~ separation at t'nis stage of the process may be preferred in some instances, however, a further separation will be necessitated at a later stage of the process since the gangue material will also be separated with the copper sulfides. Separation immediately following the initial leach reaction is therefore dictated by the particular copper sulfide reaction employed to recover the elemental copper ln values and also the composition of the initial feed material.
One preferable technique is therefore to subject the products of the initial leach and conversion reaction directly to a secondary leach reaction in,conjunction with a jarosite orming cation to convert the copper sulfides to a copper sulate solution while precipitating the iron sulfate as j jarosite. Due to the nature of this reaction it is apparent that this secondary leach will immediately follow the initial leac~h in those cases when the sulfides initially fed to ~he reaction are basically copper or iron s~lfides with only - 20 relatively small proportions of other metal sulfides. If :: , the products of the initial leach include substantial amounts of metal sulfates other than iron sulfates, it will then be preferable to separate the copper sulfides prior to the initiation of this secondary leach.
3 A preferable secondary leach reaction is an oxygen leach in an acid media in the presence of a jarosite forming cation. As mentioned the products of this leach reaction are copper sulfate and jarosite. This oxygen leach is operated in accordance with known techniques, as for example set forth in U. S. Pat. 3,642,435. Partial oxygen pressures for such a reaction are well below the comparable necessary values required in the absence of the initial copper sulfate leach.
- _ 5 _ ~065143 In performing the secondary oxy~en leach in the presence of iron sulfates it is preferred to add a su~ficient amount oE a jarosite-formin~ cation in order that the iron may be precipitated from the solution. These jarosite-forming cations are discussed in U. S. Pat. 3,684,490 and are preferably potassium, sodium and ammonium. The amount added need only be sufficient to prècipitate the ixon from solution.
Other secondary techniques may also be employed to recover the copper values from the copper sulfide products of the primary leach reaction. For example, chloride leaching techniques as described in U. S. Pat. 3,767,543 may be utilized.
Preferable chloride leaching agents include ferric chloride and cupric chloride. Also the copper sulfides may be modi-fied by techniques kn~wn in the art in order to ernploy elec-trolytic dis~olution processes, as set forth for example in U. S. Patents 3,673,061 and 3,736,238. Other suitable secondary leach operations include ammoniacal leaching and - cyanide leaching. It is therefore understood that while the following discussion assumes the utilization of a secondary oxygen leach in an acid media, the artisan can determine from the present state of the art the necessary modifications to be made should one of these alternative processes be em-ployed.
Following the secondary oxidation leach it is necessary to separate the copper sulfate from the remaining solids, including the jarosite and the gangue material. This separation is conveniently made by thickening and filtration or other means known in the art.
Qnce the copper sulfate is isolated the copper may be recovered. This recovery is conveniently made by means known in the art, preferably by electrolysis or cementation. A
portion of the copper sulfate can also be recycled in order ( 1065~43 to treat new chalcopyrire feed matc~ial. The amount of copper sulfate recycled is dependent upon the fresh sulfide feed characteristics.
The following examples are illustrati~e of some of t~e aspects encompassed by this process.
EX~PL~ NO. 1 A commercial copper concentrate assaying 34.5%
C copper, 22.~% iron, 32~ total sulfur, 4.9~ silica di~'d~, 1.7 ounces per ton silver, 0.01 ounces per ton gold, 0.12~
calcium, 0.27~ molybdenum, 0.01% lead and 0.02~ nickel and being comprised of the approximate mineral percentages of 40%
chalcopyrite, 23~ chalcocite, 23~ pyrite, 3% covellite, 1%
~!,, bornite, less than 1% hematite and 9% gangue was gxound to a mesh ~ze of -270 and reacted with copper sul~ate in a r~t~o of 0.84 pounds o~ coppex as copper sulfate per pound of copp~r ini~ially in the concentrate: The temperaturé was maintained at 180C and the reaction was permitted to take place under normal agitatlon for three hours. The initial pulp density was 192 grams of solids per liter of solution and the c~pper , . . .
sulfate concentration was 55 grams per liter of copper. The s~ 20 product analysis indicated that 0.74 pounds o~ copper was precipitated, mostly as digenite, per pound of copper initially in the concentrate, representing a substantial conversion o .: .
chalcopyrite copper to digenite copper. Iron sulfate and ` sulfuric acid were also produced.
!'! EXAMPLE NO. 2 ., , The process of Example No. 1 was followed in all respects except that the reaction temperature was maintained at 210C and the total time o~ the reaction was one hour.
., .
;
. . .
~0651~3 The results showed 0.8 pounds of copper precipita~ed as di~enite per pound of cop~r in the initial concentrate.
.
FX~PL~ ~IO. 3 Two identical acld pressuxe leaches were performed on copper concentrates of identical composition as that set forth in Example 1, one pressure leach being performed directly on the concentrates ~7hile the other pressure leach was performed subsequent to a copper sulfate leach reaction.
The concentrate was ground to -325 mesh and a pulp density C of 4.7% solids was formPd. The leach~ solution contained 13 grams per liter of copper, 33 grams per liter o~ sulfuric acid, and 11 yrams per liter of sodium sulfate. In both ca~es the r~action temperature was maintained at 95C, the vapor and oxygen total pxe~ure at 125 psig and the ~olukion was agitaked at a turbine tip speed of 525 feet per minute.
Ater an elapsed time of three and one-half hours, th~Q
results showed 82% of the copper was extracted from the sampLe that was not treated with copper sulfate, ~7hile ~
grams per liter o~ iron remained in solution. On the other hand, the sample that was initially treated with ~he copper sulfate leach reaction yielded a 95% copper extraction, with only 1.3 grams o iron in each liter OL solution, the remaining iron being precipitated as sodium jarosi~e.
fi EXP~LE NO. ~
Ano~her comparative test simil~r to Examp?e No. 3 was performed with two samples or a commercial concentrate of identical co~position as that set forth in Example No. 1.
One sample was directly leached under ammoniac~l conditions while the other sample was initially leached with copper sulfate followed by the ammoniacal leach reaction. The
- _ 5 _ ~065143 In performing the secondary oxy~en leach in the presence of iron sulfates it is preferred to add a su~ficient amount oE a jarosite-formin~ cation in order that the iron may be precipitated from the solution. These jarosite-forming cations are discussed in U. S. Pat. 3,684,490 and are preferably potassium, sodium and ammonium. The amount added need only be sufficient to prècipitate the ixon from solution.
Other secondary techniques may also be employed to recover the copper values from the copper sulfide products of the primary leach reaction. For example, chloride leaching techniques as described in U. S. Pat. 3,767,543 may be utilized.
Preferable chloride leaching agents include ferric chloride and cupric chloride. Also the copper sulfides may be modi-fied by techniques kn~wn in the art in order to ernploy elec-trolytic dis~olution processes, as set forth for example in U. S. Patents 3,673,061 and 3,736,238. Other suitable secondary leach operations include ammoniacal leaching and - cyanide leaching. It is therefore understood that while the following discussion assumes the utilization of a secondary oxygen leach in an acid media, the artisan can determine from the present state of the art the necessary modifications to be made should one of these alternative processes be em-ployed.
Following the secondary oxidation leach it is necessary to separate the copper sulfate from the remaining solids, including the jarosite and the gangue material. This separation is conveniently made by thickening and filtration or other means known in the art.
Qnce the copper sulfate is isolated the copper may be recovered. This recovery is conveniently made by means known in the art, preferably by electrolysis or cementation. A
portion of the copper sulfate can also be recycled in order ( 1065~43 to treat new chalcopyrire feed matc~ial. The amount of copper sulfate recycled is dependent upon the fresh sulfide feed characteristics.
The following examples are illustrati~e of some of t~e aspects encompassed by this process.
EX~PL~ NO. 1 A commercial copper concentrate assaying 34.5%
C copper, 22.~% iron, 32~ total sulfur, 4.9~ silica di~'d~, 1.7 ounces per ton silver, 0.01 ounces per ton gold, 0.12~
calcium, 0.27~ molybdenum, 0.01% lead and 0.02~ nickel and being comprised of the approximate mineral percentages of 40%
chalcopyrite, 23~ chalcocite, 23~ pyrite, 3% covellite, 1%
~!,, bornite, less than 1% hematite and 9% gangue was gxound to a mesh ~ze of -270 and reacted with copper sul~ate in a r~t~o of 0.84 pounds o~ coppex as copper sulfate per pound of copp~r ini~ially in the concentrate: The temperaturé was maintained at 180C and the reaction was permitted to take place under normal agitatlon for three hours. The initial pulp density was 192 grams of solids per liter of solution and the c~pper , . . .
sulfate concentration was 55 grams per liter of copper. The s~ 20 product analysis indicated that 0.74 pounds o~ copper was precipitated, mostly as digenite, per pound of copper initially in the concentrate, representing a substantial conversion o .: .
chalcopyrite copper to digenite copper. Iron sulfate and ` sulfuric acid were also produced.
!'! EXAMPLE NO. 2 ., , The process of Example No. 1 was followed in all respects except that the reaction temperature was maintained at 210C and the total time o~ the reaction was one hour.
., .
;
. . .
~0651~3 The results showed 0.8 pounds of copper precipita~ed as di~enite per pound of cop~r in the initial concentrate.
.
FX~PL~ ~IO. 3 Two identical acld pressuxe leaches were performed on copper concentrates of identical composition as that set forth in Example 1, one pressure leach being performed directly on the concentrates ~7hile the other pressure leach was performed subsequent to a copper sulfate leach reaction.
The concentrate was ground to -325 mesh and a pulp density C of 4.7% solids was formPd. The leach~ solution contained 13 grams per liter of copper, 33 grams per liter o~ sulfuric acid, and 11 yrams per liter of sodium sulfate. In both ca~es the r~action temperature was maintained at 95C, the vapor and oxygen total pxe~ure at 125 psig and the ~olukion was agitaked at a turbine tip speed of 525 feet per minute.
Ater an elapsed time of three and one-half hours, th~Q
results showed 82% of the copper was extracted from the sampLe that was not treated with copper sulfate, ~7hile ~
grams per liter o~ iron remained in solution. On the other hand, the sample that was initially treated with ~he copper sulfate leach reaction yielded a 95% copper extraction, with only 1.3 grams o iron in each liter OL solution, the remaining iron being precipitated as sodium jarosi~e.
fi EXP~LE NO. ~
Ano~her comparative test simil~r to Examp?e No. 3 was performed with two samples or a commercial concentrate of identical co~position as that set forth in Example No. 1.
One sample was directly leached under ammoniac~l conditions while the other sample was initially leached with copper sulfate followed by the ammoniacal leach reaction. The
4 ,~ leache~ solution had a concentration o 80 yrams per liter 1~ of ammonium sulfate and 75 grams per liter of alNmonia as ammonium hydroxide. The temperature was maintained at 81C
for both tests, and the oxygen and ammonia total pressure was kept at 20 psig. After an ~lapsed time of two hour.s, the sample which had not been treat~d with the copper slllfate solution showed a 93% coppe~ recovery, while the sample which had initially been treated showed a 98% copper extraction.
In both Examples 3 and 4 the copper sulfate leach xeaction was performed in similar fashion to that described in Example 1.
EXAMPI,E NO. 5 A commercial copper concentrate consisting of about 75%
chalcopyrite and assaying 26.1% copper, 27.5% iron and 31.4% total sulfur was reacted with ~.2 moles of copper as copper sulfate per mole o copper in the chalcop~rite concentrate at 180C for three hour~. Th~ product analysi~ indicatea that two moles of copp~r as copper sul~a te r~acted with one mole of copper in the chalcopyrite concentrate to yiela three moles o~ copper as digenite, this analysis being ~erified by Y-ray diffraction. Essentially all of the iron from the chalcopyrite entered into solution as ferrou~
sulfate.
for both tests, and the oxygen and ammonia total pressure was kept at 20 psig. After an ~lapsed time of two hour.s, the sample which had not been treat~d with the copper slllfate solution showed a 93% coppe~ recovery, while the sample which had initially been treated showed a 98% copper extraction.
In both Examples 3 and 4 the copper sulfate leach xeaction was performed in similar fashion to that described in Example 1.
EXAMPI,E NO. 5 A commercial copper concentrate consisting of about 75%
chalcopyrite and assaying 26.1% copper, 27.5% iron and 31.4% total sulfur was reacted with ~.2 moles of copper as copper sulfate per mole o copper in the chalcop~rite concentrate at 180C for three hour~. Th~ product analysi~ indicatea that two moles of copp~r as copper sul~a te r~acted with one mole of copper in the chalcopyrite concentrate to yiela three moles o~ copper as digenite, this analysis being ~erified by Y-ray diffraction. Essentially all of the iron from the chalcopyrite entered into solution as ferrou~
sulfate.
Claims (25)
PROPERTY OR PRIVILEGE IS CLAIMED ARE DEFINED AS FOLLOWS:
1. A process for hydrometallurgically recovering ele-mental copper from chalcopyrite comprising:
reacting the chalcopyrite with a copper sulfate solu-tion at a temperature and mole ratio sufficient to form an insoluble copper sulfide consisting essen-tially of digenite, a soluble iron sulfate and sulfuric acid;
separating the copper sulfide from the iron sulfate; and recovering the elemental copper from the copper sulfide.
reacting the chalcopyrite with a copper sulfate solu-tion at a temperature and mole ratio sufficient to form an insoluble copper sulfide consisting essen-tially of digenite, a soluble iron sulfate and sulfuric acid;
separating the copper sulfide from the iron sulfate; and recovering the elemental copper from the copper sulfide.
2. The process of claim 1 wherein the concentration of the copper sulfate solution is from about 30 to about 100 grams per liter of copper.
3. The process of claim 1 wherein the chalcopyrite reaction is conducted from about 180°C to about 200°C.
4. The process of claim 1 wherein the mole ratio of copper sulfate to chalcopyrite reactants is at least about two to one.
5. The process of claim 4 wherein the temperature of the copper sulfate reaction is maintained from about 180°C to about 200°C.
6. A process for hydrometallurgically recovering copper from chalcopyrite comprising:
initially leaching the chalcopyrite with a copper sul-fate solution at a temperature and mole ratio sufficient to form insoluble digenite, minor amounts of other insoluble copper sulfides and a soluble iron sulfate;
separating the insoluble copper sulfides from the soluble iron sulfate;
secondarily leaching the copper sulfides with oxygen in an acid medium and in the presence of a jarosite form-ing cation to form a soluble copper sulfate solution and an insoluble jarosite; and recovering a portion of the copper from the copper sulfate solution and recycling the remainder of the copper sulfate solution to the initial leach reaction.
initially leaching the chalcopyrite with a copper sul-fate solution at a temperature and mole ratio sufficient to form insoluble digenite, minor amounts of other insoluble copper sulfides and a soluble iron sulfate;
separating the insoluble copper sulfides from the soluble iron sulfate;
secondarily leaching the copper sulfides with oxygen in an acid medium and in the presence of a jarosite form-ing cation to form a soluble copper sulfate solution and an insoluble jarosite; and recovering a portion of the copper from the copper sulfate solution and recycling the remainder of the copper sulfate solution to the initial leach reaction.
7. The process of claim 6 wherein the mole ratio of copper sulfate to chalcopyrite reactants is at least about two to one.
8. The process of claim 6 wherein the temperature of the copper sulfate reaction is maintained from about 180°C to 200°C.
9. A process for hydrometallurgically recovering copper from chalcopyrite comprising:
leaching and converting the chalcopyrite with a copper sulfate solution at a temperature and mole ratio sufficient to concurrently form a mixture of an insoluble copper sulfide consisting essentially of digenite, a soluble iron sulfate and sulfuric acid;
subjecting said concurrently formed mixture to a secondary treatment including leaching with oxygen and addition of a jarosite-forming cation, to produce from said concurrently formed mixture a soluble copper sulfate solu-tion and an insoluble jarosite;
separating the soluble copper sulfate solution from the insoluble jarosite; and recovering elemental copper from the copper sulfate solution.
leaching and converting the chalcopyrite with a copper sulfate solution at a temperature and mole ratio sufficient to concurrently form a mixture of an insoluble copper sulfide consisting essentially of digenite, a soluble iron sulfate and sulfuric acid;
subjecting said concurrently formed mixture to a secondary treatment including leaching with oxygen and addition of a jarosite-forming cation, to produce from said concurrently formed mixture a soluble copper sulfate solu-tion and an insoluble jarosite;
separating the soluble copper sulfate solution from the insoluble jarosite; and recovering elemental copper from the copper sulfate solution.
10. The process of claim 9 wherein a portion of the copper sulfate solution produced from the secondary leaching operation is recycled to treat fresh chalcopyrite feed material.
11. The process of claim 9 wherein the leaching of the chalcopyrite with copper sulfate is performed at a temper-ature of from about 180°C to about 200°C.
12. The process of claim 9 wherein elemental copper is recovered by means of electrolysis.
13. The process of claim 9 wherein the jarosite-forming cation is sodium.
14. The process of claim 9 wherein the jarosite-forming cation is potassium.
15. The process of claim 9 wherein the jarosite-forming cation is an ammonium ion.
16. The process of claim 9 wherein the chalcopyrite initially treated with the copper sulfate solution is in the presence of other mixed sulfides.
17. The process of claim 9 wherein the mole ratio of copper sulfate to chalcopyrite reactants is at least about two to one.
18. The process of claim 9 wherein the temperature of the copper sulfate reaction is maintained from about 180°C to 200°C.
19. A process for hydrometallurgically recovering elemental copper from chalcopyrite comprising:
reacting the chalcopyrite with a copper sulfate solu-tion at a temperature and mole ratio sufficient to form an insoluble copper sulfide consisting essentially of digenite, a soluble iron sulfate and sulfuric acid;
separating the copper sulfide from the iron sulfate;
leaching the separated copper sulfide with a chloride selected from the group consisting of ferric chloride and cupric chloride in order to produce a solution comprising cuprous chloride, cupric chloride and ferrous chloride;
and reducing at least a portion of the cuprous chloride to elemental copper.
reacting the chalcopyrite with a copper sulfate solu-tion at a temperature and mole ratio sufficient to form an insoluble copper sulfide consisting essentially of digenite, a soluble iron sulfate and sulfuric acid;
separating the copper sulfide from the iron sulfate;
leaching the separated copper sulfide with a chloride selected from the group consisting of ferric chloride and cupric chloride in order to produce a solution comprising cuprous chloride, cupric chloride and ferrous chloride;
and reducing at least a portion of the cuprous chloride to elemental copper.
20. The process of claim 19 wherein the chalcopyrite re-action is conducted from about 180°C to about 200°C.
21. The process of claim 20 wherein the mole ratio of copper sulfate to chalcopyrite reactants is at least about two to one.
22. The process of claim 19 wherein the solution comprising cuprous chloride, cupric chloride and ferrous chloride is subjected to electrolysis to produce elemental copper.
23. A process for hydrometallurgically recovering elemental copper from chalcopyrite comprising:
reacting the chalcopyrite with copper sulfate solution at a temperature and mole ratio sufficient to form an insoluble copper sulfide consisting essentially of digenite, a soluble iron sulfate and sulfuric acid;
separating the copper sulfide from the iron sulfate;
leaching the separated copper sulfide with an ammoniacal leach solution; and recovering copper from the ammoniacal leached solution.
reacting the chalcopyrite with copper sulfate solution at a temperature and mole ratio sufficient to form an insoluble copper sulfide consisting essentially of digenite, a soluble iron sulfate and sulfuric acid;
separating the copper sulfide from the iron sulfate;
leaching the separated copper sulfide with an ammoniacal leach solution; and recovering copper from the ammoniacal leached solution.
24. The process of claim 23 wherein the chalcopyrite reaction is conducted from about 180°C to about 200°C.
25. The process of claim 24 wherein the mole ratio of copper sulfate to chalcopyrite reactants is at least about two to one.
Priority Applications (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CA243,025A CA1065143A (en) | 1976-01-06 | 1976-01-06 | Recovery of copper from chalcopyrite utilizing copper sulfate leach |
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CA243,025A CA1065143A (en) | 1976-01-06 | 1976-01-06 | Recovery of copper from chalcopyrite utilizing copper sulfate leach |
Publications (1)
| Publication Number | Publication Date |
|---|---|
| CA1065143A true CA1065143A (en) | 1979-10-30 |
Family
ID=4104909
Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CA243,025A Expired CA1065143A (en) | 1976-01-06 | 1976-01-06 | Recovery of copper from chalcopyrite utilizing copper sulfate leach |
Country Status (1)
| Country | Link |
|---|---|
| CA (1) | CA1065143A (en) |
-
1976
- 1976-01-06 CA CA243,025A patent/CA1065143A/en not_active Expired
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