Classifications

• • C—CHEMISTRY; METALLURGY
  • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
  • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
  • C22B23/00—Obtaining nickel or cobalt
  • C22B23/04—Obtaining nickel or cobalt by wet processes
  • C22B23/0453—Treatment or purification of solutions, e.g. obtained by leaching
  • C22B23/0461—Treatment or purification of solutions, e.g. obtained by leaching by chemical methods
• • C—CHEMISTRY; METALLURGY
  • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
  • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
  • C22B23/00—Obtaining nickel or cobalt
  • C22B23/04—Obtaining nickel or cobalt by wet processes
  • C22B23/0407—Leaching processes
  • C22B23/0415—Leaching processes with acids or salt solutions except ammonium salts solutions
• • C—CHEMISTRY; METALLURGY
  • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
  • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
  • C22B3/00—Extraction of metal compounds from ores or concentrates by wet processes
  • C22B3/20—Treatment or purification of solutions, e.g. obtained by leaching
  • C22B3/44—Treatment or purification of solutions, e.g. obtained by leaching by chemical processes
• • C—CHEMISTRY; METALLURGY
  • C22—METALLURGY; FERROUS OR NON-FERROUS ALLOYS; TREATMENT OF ALLOYS OR NON-FERROUS METALS
  • C22B—PRODUCTION AND REFINING OF METALS; PRETREATMENT OF RAW MATERIALS
  • C22B15/00—Obtaining copper
  • C22B15/0063—Hydrometallurgy
  • C22B15/0084—Treating solutions
  • C22B15/0089—Treating solutions by chemical methods
  • C22B15/0093—Treating solutions by chemical methods by gases, e.g. hydrogen or hydrogen sulfide
• • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
  • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
  • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
  • Y02P10/00—Technologies related to metal processing
  • Y02P10/20—Recycling

Definitions

• the present invention relates to a process for recovering valuable metals, such as nickel, from liquors obtained by processing laterite ores and concentrates of the ores that are contaminated with high levels of iron.
• processing laterite ores and concentrates is understood herein to include processing by any one or more of heap leaching, pressure leaching, bacterial oxidation leaching, and atmospheric tank leaching.
• the present invention relates particularly, although by no means exclusively, to a process for recovering nickel and cobalt from liquors obtained by acid leaching ores and concentrates of the ores that are contaminated with high levels of iron.
• high levels of iron is understood to mean levels of iron whereby the mole ratio of Fe:Ni is greater than 2:1.
• nickel can be recovered from such liquors containing nickel by contacting the liquors with H 2 S to precipitate nickel sulphides (and mixed sulphides in situations where nickel and other valuable metals such as cobalt are in the liquors) .
• iron can be removed from liquors prior to nickel (and cobalt) precipitation by using (a) high temperatures (180-220°C) to selectively precipitate iron as hematite (b) low temperatures (90-120°C) to precipitate iron as goethite, and low temperatures (70- 150°C) to precipitate iron as jarosite.
• high temperature precipitation is capital intensive, requiring autoclaves and flash vessels, and low temperature precipitation results in high nickel losses as a result of nickel adsorption onto iron species.
• the applicant has developed a process that is capable of recovering very high levels (greater than 99%) of nickel from nickel liquors with very low levels of co- precipitation of iron.
• the reduction step (a) includes reducing ferric ions to ferrous ions using the reductant in the presence of 40-90 g/1 free acid.
• the reductant may be any suitable reductant.
• One suitable reductant is NaHS.
• the reductant is a gaseous reductant.
• the gaseous reductant is H 2 S.
• the neutralisation step (b) increases the pH of the solution to 2.
• the neutralisation step (b) maintains iron in the ferrous state.
• the valuable metal is nickel.
• the valuable metals are nickel and cobalt.
• the laterite ores are ores that contain nickel in a chlorite mineral phase.
• the process conditions for the precipitation step (c) include operating at a partial pressure of the gaseous reductant of less, than 60 psi.
• gas partial pressure is less than 40 psi.
• the gas partial pressure is less than 30 psi. It is preferred particularly that the gas partial pressure be less than 25 psi.
• the process conditions for the precipitation step (c) include operating at a liquor temperature of at least 50°C.
• the liquor temperature is at least 60°C.
• the seed particles for the precipitation step (c) have a particle size of P 50 less than 100 micron.
• the particle size of the seed particles is P 50 less than 80 micron.
• the particle size of the seed particles be P 50 less than 60 micron.
• the seed particle concentration for the precipitation step (c) is greater than 30g/l.
• the seed particle concentration is greater than 40g/l.
• the ratio of iron and the valuable metal in the leach liquor supplied to step (a) is greater than 2:1.
• the ratio is greater than 3:1.
• the ratio is greater than 5:1.
• the present invention is based on extensive experimental work carried out by the applicant to recover nickel and cobalt from laterite ores.
• the experimental work included the following work.
• the initial test work included test work for optimal precipitation conditions using the synthetic liquor.
• the initial test work investigated the following precipitation parameters to determine their effect on nickel and cobalt recovery and nickel/iron separation:
• the kinetics of precipitation are also influenced by temperature .
• the surface area of seed particles can be increased by increasing the mass of seed in the reactor or by seeding with solids with a smaller average particle size. The influence of both factors was investigated. Detailed results are summarised in Figures 2 and 3.
• a second batch of liquors was generated and treated in the following sequence of process stages, as discussed below:
• the Fe(III) was effectively reduced to Fe(II) under the conditions employed.
• Nickel and cobalt precipitation were minimal. Nickel precipitation ranged from 0.083 to 0.67% while cobalt precipitation was less than 0.01%.
• the concentrations of the other elements assayed were not significantly altered by the pre-reduction stage with precipitation consistently being less than 0.5% and typically less than 0.1%.
• Residue assays showed sulphur as the main constituent (>80%) .
• the liquors generated from the pre-reduction stage were treated with limestone to increase the solution pH to ⁇ 2 in the neutralisation stage.
• the feed liquor compositions supplied to the neutralisation stage are given in Table 3.
• Nickel and cobalt losses by precipitation were low - ranging from 0.2 to 0.4% and 0.05% to 0.16%, respectively.
• the copper concentration in solution was reduced to below the copper detection limit of 0.1 mg/1.
• Mn, Cr, Fe and Zn was low, generally less than 1%.
• the iron essentially remained in the Fe(II) state enabling sulphide precipitation from the liquor to be undertaken.
• the residues were mainly composed of gypsum (indicated by high calcium and sulphur assays) .
• composition of the liquors used in the sulphide precipitation stage are summarised in Table 5,
• the solids contained between 4.0 and 5.0% Fe with the Ni:Fe mole ratio ranging between 9.0 and 11.2,
• aluminium concentration in the product generally increased with aluminium concentration in solution. Aluminium does not form stable sulphides in solution and the increase in aluminium concentration in the product appears to be through adsorption/entrainment with the sulphide.
• the chromium concentration in the product also increased with chromium concentration in solution. This effect is much stronger with the increase in chromium in the product increasing more steeply with chromium in the PLS compared to aluminium and could indicate that chromium precipitated as opposed to being adsorbed/entrained.
• Zinc concentration in solution was reduced to between 2 and 3 mg/1.
• the sulphide products were generally low in zinc (less than 0.03%) due to the relatively low zinc concentration in solution (3-5 mg/1) .
• Copper concentration in the products was low due to copper removal in previous unit operations with copper in the product ranging between 0.01 and 0.03%.
• Manganese and magnesium concentrations in the products were consistently low at less than 50 ppm and less than 500 ppm, respectively, reflecting the high selectivity of sulphide precipitation against these elements .
• Nickel and cobalt precipitation increased as liquor temperature increased from 40°C to 95°C.
• the Ni/Fe separation appeared to reach a maximum at 80°C.
• Aluminium, chromium, manganese and magnesium precipitation were not affected over the temperature range investigated.
• Liquors can be treated with H 2 S gas in a pre- reduction stage to reduce Fe(III) to Fe(II) with low nickel and cobalt losses (ranging from 0.08% - 0.67% and ⁇ 0.1%, respectively). Copper was the only impurity significantly removed during pre-reduction with copper concentration in solution being reduced below 1 mg/1.
• the neutralisation stage effectively increased the pH of the liquor from the pre-reduction stage to -2 while maintaining iron in the Fe(II) state.
• Nickel and cobalt losses during the neutralisation stage were 0.2%-0.4% and 0.05%-0.16%, respectively.
• the residues were mainly gypsum. Impurity removal during neutralisation was generally less than 1%.

Landscapes

• Chemical & Material Sciences (AREA)
• Engineering & Computer Science (AREA)
• Mechanical Engineering (AREA)
• Manufacturing & Machinery (AREA)
• Materials Engineering (AREA)
• Metallurgy (AREA)
• Organic Chemistry (AREA)
• General Chemical & Material Sciences (AREA)
• Chemical Kinetics & Catalysis (AREA)
• Life Sciences & Earth Sciences (AREA)
• Environmental & Geological Engineering (AREA)
• General Life Sciences & Earth Sciences (AREA)
• Geochemistry & Mineralogy (AREA)
• Geology (AREA)
• Manufacture And Refinement Of Metals (AREA)

Applications Claiming Priority (3)

Publications (2)

Family

ID=27809900

Family Applications (1)

Country Status (6)

Families Citing this family (5)

Citations (4)

Family Cites Families (11)

• 2002
  • 2002-08-15 AU AU2002950815A patent/AU2002950815A0/en not_active Abandoned
• 2003
  • 2003-08-15 EP EP03787516A patent/EP1546418A4/de not_active Withdrawn
  • 2003-08-15 US US10/524,574 patent/US20060169104A1/en not_active Abandoned
  • 2003-08-15 RS YUP-2005/0145A patent/RS20050145A/sr unknown
  • 2003-08-15 BR BR0313497-0A patent/BR0313497A/pt not_active Application Discontinuation
  • 2003-08-15 WO PCT/AU2003/001037 patent/WO2004016816A1/en not_active Application Discontinuation

Patent Citations (4)

Non-Patent Citations (5)

Also Published As

Similar Documents

Legal Events