Upload
evelin-gonzalez-martinez
View
217
Download
0
Embed Size (px)
Citation preview
7/27/2019 Chandraprabha_2006_Hydrometallurgy
1/7
Surface chemical and flotation behaviour of chalcopyrite and pyrite
in the presence of Acidithiobacillus thiooxidans
M.N. Chandraprabha, K.A. Natarajan
Department of Metallurgy, Indian Institute of Science, Bangalore 560012, India
Available online 5 May 2006
Abstract
Extraction of valuable metals and removal of sulfide minerals from abandoned mines holds the key for environmental
protection. This paper discusses the utility ofAcidithiobacillus thiooxidansfor the selective removal of pyrite from chalcopyrite for
the economic extraction of valuable copper. Interaction of bacterial cells with the sulfide minerals altered the surface chemistry of
both the minerals and cells. The isoelectric point of both pyrite and chalcopyrite shifted to higher pH after interaction with cells.
Adhesion kinetics of the bacterial cells to both the minerals was similar, however, the adsorption density on pyrite was higher
compared to that on chalcopyrite. Interaction with cells rendered both the minerals hydrophilic. Flotation of minerals,
preconditioned with cells, with potassium isopropyl xanthate as collector resulted in depression of pyrite and good flotation of
chalcopyrite. The observed behaviour is discussed in detail. Poor selectivity achieved when the minerals were floated together was
overcome by conditioning the collector interacted minerals with the bacterial cells prior to flotation. Thus it was possible to
selectively depress pyrite from chalcopyrite at both acidic and neutral pH conditions.
2006 Elsevier B.V. All rights reserved.
Keywords: Acidithiobacillus thiooxidans; Pyrite; Chalcopyrite; Adhesion; Flotation
1. Introduction
Recent years have witnessed depletion of rich grade
ores resulting in the processing of more and more lean
grade ores. Economical extraction of valuable metals
from such ores requires selective separation of minerals
having high metal values from other associated miner-als. Chalcopyrite is often associated with pyrite and
economical extraction of copper demands selective
depression of pyrite from chalcopyrite. Conventionally
sodium cyanide is used as a depressant for the selective
depression of pyrite from chalcopyrite during the froth
flotation process, leading to potentially disastrous
environmental consequences [1]. Use of microbes or
bioreagents, on the other hand, would prove to be both
economically viable and an environmentally benign
process.
Thiobacillus sp., which are chemolithoautotrophs
and which thrives on either iron or sulfur, have been
successfully utilized for the bioleaching of sulfide
minerals and biooxidation of refractory gold ores[2,3]. Acidithiobacillus ferrooxidans are known to
adhere very tenaciously to sulfide mineral surfaces.
Such bacterial adhesion alters the surface chemistry of
the interacted minerals conferring either hydrophobicity
or hydrophilicity [4]. The role of A. ferrooxidans in
influencing the flotation behaviour of pyrite, chalcopy-
rite, sphalerite, galena, etc., has been studied in the past
[5,6]. The chemolithotrophic acidophilic thiobacilli
Acidithiobacillus thiooxidans and A. ferrooxidans both
grow on elemental sulfur, but only the latter uses ferrous
Hydrometallurgy 83 (2006) 146 152
www.elsevier.com/locate/hydromet
Corresponding author. Tel.: +9180 23600120;fax: +9180 23600472.
E-mail address:[email protected](K.A. Natarajan).
0304-386X/$ - see front matter 2006 Elsevier B.V. All rights reserved.doi:10.1016/j.hydromet.2006.03.021
mailto:[email protected]://dx.doi.org/10.1016/j.hydromet.2006.03.021http://dx.doi.org/10.1016/j.hydromet.2006.03.021mailto:[email protected]7/27/2019 Chandraprabha_2006_Hydrometallurgy
2/7
iron as an energy source. Thus A. thiooxidans has
similar applications asA. ferrooxidansin the processing
of sulfide minerals.
The oxidation of sulfur to sulfuric acid by A.
thiooxidans with sulfite as the key intermediate was
first proposed on the basis of the sulfur-oxidisingenzyme and sulfite-oxidising enzyme systems: S0 + O2+
H2OH2SO3 and H2SO3+(1/2)O2H2SO4 [79].
The mechanism of cell-sulfur adhesion process and
kinetics of sulfur oxidation is also well-established
[10].
However, the utility of this organism for bioflotation
is very limited. Recently Santhiya et al. [11] have
studied the surface chemical changes on galena and
sphalerite brought about by this organism and have
achieved selective separation of galena from sphalerite.
In the present study we investigate the surfacechemical changes on pyrite and chalcopyrite after
interaction with A. thiooxidans in view of selective
separation of pyrite from a mixture of pyrite and
chalcopyrite.
2. Materials and methods
2.1. Minerals
Pure handpicked mineral samples of pyrite were
obtained from Alminrock Indser Fabricks, Bangalore
and chalcopyrite from Gregory, Bottley and Lloyd, UK.The mineral samples were dry-ground with a porcelain
ball mill and dry-sieved to obtain different size fractions.
The 106+75 m fraction was used for flotation
studies. The 37 m fraction was further ground in a
Retsch mortar grinder. The particle size analysis of this
sample was done using a Malvern Mastersizer 3000-
model and the mean size was found to be 5 m. This
fraction was used for adsorption and electrokinetic
studies. The minerals were stored in a desiccator under
nitrogen atmosphere. The surface area was estimated by
BET nitrogen specific surface area method and wasfound to be 1.26 m2/g for pyrite and 1.61 m2/g for
chalcopyrite respectively. The purity of the mineral
samples were ascertained by mineralogical studies and
X-ray diffraction using a JDX-8030 X-ray diffractom-
eter system.
2.2. Microorganism
The bacterial culture used was a strain of A.
thiooxidans (MCM B41) obtained from MACS, Pune.
The bacteria were cultured in sterile modified 9K basal
medium containing 2 g/l ammonium sulfate, 0.25 g/
l dipotassium hydrogen phosphate, 0.5 g/l magnesium
sulfate and 10 g/l sulfur powder.
2.3. Growth of bacteria and preparation of cell pellet
The sterilized medium was inoculated with 10% (v/v) of active inoculum in 250 ml standard Erlenmeyer
flasks. The flasks were incubated at 30 C on a rotary
shaker at 200 rpm. The bacterial count was monitored
by a direct count method using a Petroff Hausser counter
viewed with a Leitz phase contrast microscope (Labro-
lux K Wild MPS12). The solution pH was also regularly
monitored using a Systronics digital pH meter.
The grown culture was initially filtered through
Whatman 42 filter paper to remove the precipitates. The
filtrate was then centrifuged at 12,000gfor 20 min in a
Sorvall RC-5B refrigerated high-speed centrifuge at5 C. The pellet obtained was resuspended in pH 2
H2SO4solution and then centrifuged as before to obtain
metabolite free cells.
2.4. Adsorption studies
Culture containing cells in the exponential growth
phase was centrifuged to obtain the cell pellet. This
pellet was washed twice with pH 2 H2SO4solution and
suspended in 100 ml 103 M KCl solution at the desired
pH in 250 ml standard Erlenmeyer flask. One gram of
the mineral sample was pulped in the cell suspensionand the resulting slurry was agitated on a rotary shaker at
200 rpm for 30 min for equilibration. After equilibra-
tion, the slurry was vortex mixed for 1 min to remove
loosely held cells, centrifuged at 500g for 5 min to
settle the mineral particles and the cell number in the
supernatant was recorded. For experiments on adhesion
kinetics, the above procedure was repeated at regular
intervals and the cell data with respect to time recorded.
2.5. Electrokinetic studies
The electrophoretic mobilities of the mineral samples
before and after interaction with the bacterial cells was
determined using a Malvern Zetasizer 3000 instrument.
KCl solution (103 M) was used as the base electrolyte
in all the experiments. One gram of the mineral sample
was interacted with the desired cell concentration and
pH for the required time. The slurry after interaction was
centrifuged at 500gfor 3 min to settle only the mineral
particles. The mineral sample was resuspended in KCl
solution, vortexed and washed two to three times to
remove loosely held cells. The mineral sample so
obtained was equilibrated in KCl solution that was
147M.N. Chandraprabha, K.A. Natarajan / Hydrometallurgy 83 (2006) 146152
7/27/2019 Chandraprabha_2006_Hydrometallurgy
3/7
preadjusted to the desired pH before taking the
measurements. Electrophoretic mobility of cells after
interaction with the minerals was also recorded by
equilibrating the interacted cells in 103 M KCl solution
at different pH. In all the experiments 5 readings were
recorded and the results reported represent the averagevalue. The standard deviation was
7/27/2019 Chandraprabha_2006_Hydrometallurgy
4/7
shifted to around pH 3 and 3.4 respectively. The
electronegative character of the mineral also reduced
after interaction with cells. The shift in iep and also the
reduction in the electrophoretic mobility for chalcopy-
rite was lower compared to that of pyrite.
Interaction of bacterial cells with minerals not onlyalters the surface properties of the minerals but also has
effect on the surface properties of the bacterial cells as
shown in Fig. 1(c). The iep of cells before interaction
with minerals is located around pH 2.9 and consequent
to interaction with the minerals the iep is shifted to
higher pH values. The magnitude of shift is higher for
pyrite-interacted cells compared to chalcopyrite-inter-
acted cells. The electrophoretic mobility of the cells is
also reduced consequent to interaction with the
minerals with the magnitude in reduction being higher
for the pyrite-interacted cells. This reduction in theelectrophoretic mobility can be attributed to the
proteinaceous secretion resulting from microbeminer-
al interaction and indicated specific adsorption of cells
on minerals due to chemical interaction [4]. The
observed difference in the electrokinetic behaviour of
the minerals and cells consequent to their mutual
interaction confirms that the cells exhibit selectivity
towards the minerals.
3.2. Adhesion studies
The adhesion kinetics ofA. thiooxidans at an initialcell concentration of about 6.25 108 cells/ml is
depicted inFig. 2. The kinetics of adsorption is similar
on both the minerals and the adsorption equilibrium is
attained in about 80 min. Presence of copper ions in the
chalcopyrite lattice does not seem to affect the kinetics
of adhesion of cells on its surface. However, the cell
density on the surface of chalcopyrite was lesser when
compared to that on pyrite, confirming that the bacteria
shows selectivity towards pyrite. This could be due to
the presence of toxic copper ions in the lattice of
chalcopyrite [12,13]. This explains the observed
difference in the electrokinetic behaviour of these
minerals consequent to their interaction with the
bacterial cells.
The adsorption isotherm ofA. thiooxidans for pyrite
and chalcopyrite at pH 2.5 is depicted in Fig. 3. The
adsorption density increases with increase in the
equilibrium number of cells up to about 2.2 1011
cells/100 ml and 71010 cells/100 ml respectively forpyrite and chalcopyrite and thereafter a plateau is
reached for both the minerals. The adsorption density is
higher on pyrite compared to chalcopyrite. The structure
of chalcopyrite is built up of copper, iron and sulfide
ions and presence of toxic copper ions may result in
lower adsorption density of A. thiooxidans cells on
chalcopyrite compared to pyrite.
Both the isotherms exhibit Langmuirian behaviour
confirming monolayer coverage of cells. Fig. 4 shows
the scanning electron micrograph ofA. thiooxidanscells
adhering onto pyrite after 1 h interaction. It is clear fromthe photograph that the cells form monolayer coverage
on the mineral surface.
3.3. Microflotation tests
Flotation recovery of pyrite and chalcopyrite as a
function of pH at different collector (potassium
isopropyl xanthate, PIPX) concentrations are shown in
Fig. 5a. Pyrite was most floatable under acidic
conditions and the recovery dropped with increase in
alkalinity. This is due to the changes in solubility of iron
hydroxides on the pyrite surface as the pH changes[14].
0 40 80 120 160
1010
1011
6.125x10
8
cells/ml
6.25x108cells/ml
Cellsadsorbed(cells/m
2)
Time (min)
PyriteChalcopyrite
Fig. 2. Adsorption kinetics of A. thiooxidans cells on pyrite andchalcopyrite.
107 108 109
1010
1011
pH 2.5
Cellsadsorbe
d(cells/m2)
Equilibrium concentration (cells/ml)
PyriteChalcopyrite
Fig. 3. Adsorption isotherm of A. thiooxidans cells on pyrite and
chalcopyrite.
149M.N. Chandraprabha, K.A. Natarajan / Hydrometallurgy 83 (2006) 146152
7/27/2019 Chandraprabha_2006_Hydrometallurgy
5/7
By contrast, the recovery of chalcopyrite remained
almost constant at all the pH studied.The flotation recovery of pyrite and chalcopyrite
after interaction with bacterial cells and further
conditioning with the collector are shown in Fig. 5b.
Both the minerals were completely depressed upon
interaction with cells. When pyrite, interacted with cells,
was further conditioned with collector, at higher
collector concentrations the mineral exhibited some
floatability in the acidic pH region. The maximum
recovery at 0.5 mM PIPX was about 30% and it
increased to 41% when the collector concentration was
increased to 1 mM. By contrast, conditioning with cells
did not significantly reduce the flotation recovery of
chalcopyrite. As seen from the figure, when the mineralinteracted with cells was further conditioned with
0.5 mM and 1 mM collector concentration, the recovery
obtained was 68% and 76% approximately at all pH
studied.
The alkylxanthate species formed when pyrite is
treated with an aqueous solution of potassium alkyl-
xanthate is dialkyl dixanthogen, which is hydrophobic,
and physisorbed to the surface in aqueous systems. In
case of chalcopyrite, the alkylxanthate ions are coordi-
nated to specific Cu ion sites on the mineral surface
forming solid copper (I) alkylxanthate, which is highlyhydrophobic and strongly chemisorbed to the surface
[15]. This explains the observed difference in the
floatability of the two minerals after interaction with
the cells and collector.
3.4. Differential flotation tests
Microflotation studies suggest possibility of selective
separation of pyrite from chalcopyrite consequent to
their interaction with A. ferrooxidans cells. Results of
the differential flotation studies of a 1:1 synthetic
mixture of pyrite and chalcopyrite is tabulated inTable1. Two conditions were tested. In the first case the
minerals were interacted with the cells and/or reagents
separately, and the interacted minerals were mixed
together and floated. In the second case, the minerals
were interacted together with the cells and/or collector
and floated together.
In the first condition, when the minerals were
conditioned individually and floated, consequent to
interaction with 4 108 cells/ml bacterial cells and
further conditioning with 0.5 mM collector, the recovery
of pyrite and chalcopyrite were 23.7% and 63.4% at pH
20
30
40
50
60
70
80
90
100 (a)
0.5 mM 1 mM PIPXFlotationrecovery(%
)
Pyrite Chalcopyrite
4 5 6 7 8 9 10
20
30
40
50
60
70
80 (b)
Pyrite Chalcopyrite
Flotationrecovery
(%)
pH
Cells (4x108 cells/ml)
Cells + 5x10-4M PIPX
Cells + 1x10-3M PIPX
Fig. 5. (a) Flotation behaviour of pyrite and chalcopyrite with respect
to pH at different collector (PIPX) concentration. (b) Effect of cells onxanthate-induced flotation of pyrite and chalcopyrite.
Table 1
Differential flotation of pyritechalcopyrite (1:1) mixture after
conditioning with cells followed by collector
Flotation
pH
Experimental
condition
Weight % in floated fraction
Pyrite Chalcopyrite
4.5 Individually 23.7 63.4
Together 41.3 69.1
6.5 Individually 25.2 66.2
Together 32.3 72.3
Conditions: PIPX: 0.5 mM (5 min).Cells (pH 4.5): 4 108 cells/ml (5 min).
Fig. 4. Scanning electron micrograph showing attachment of A.
thiooxidans cells on pyrite.
150 M.N. Chandraprabha, K.A. Natarajan / Hydrometallurgy 83 (2006) 146152
7/27/2019 Chandraprabha_2006_Hydrometallurgy
6/7
4.5 respectively. However, when the minerals were
conditioned together the recovery of pyrite increased to
41.3% and that of chalcopyrite increased to 69.1%.
Similar behaviour was observed at pH 6.5.
Galvanic interactions between a noble and an active
mineral reduce the floatability of the noble mineral, the
effect on the active mineral being minimal[16]. Blank
flotation tests carried out on pyrite
chalcopyrite mixtureafter preconditioning the minerals in distilled water
showed that the flotation of pyrite was slightly increased
when conditioned in the presence of chalcopyrite while
that of chalcopyrite remained almost the same [17].
Thus, the observed increase in the flotation of
chalcopyrite in Table 1 could be attributed to the
preferential adsorption of the cells onto pyrite surface,
i.e., due to the decrease in cell adhesion on the
chalcopyrite surface when both the minerals are present
together. However, the increase in the floatability of
pyrite could not be explained with this.
The effect of copper ions on the flotation behaviourof pyrite was studied earlier and it was observed that the
recovery of pyrite in the acidic pH region was increased
in the presence of copper [17]. The copper ions were
able to activate pyrite surface and increase its flotation.
Dissolution behaviour of chalcopyrite under different
conditions was tested and the results obtained are
tabulated in Table 2. The concentration of copper
recorded in the solution when chalcopyrite and pyrite
are conditioned together was less than that recorded
when chalcopyrite was conditioned alone. This indi-
cates that the copper released to the solution from thechalcopyrite surface might be migrating to the pyrite
surface. To test this, pyrite and chalcopyrite of two
different size fractions were conditioned together. The
conditioned minerals were separated by sieving and
acid digested for copper analysis. Presence of copper in
the pyrite-digested sample indicated that the copper
released from chalcopyrite surface was migrating to
pyrite surface (data not shown). As seen from the table,
there was dissolution of copper ions from the chal-
copyrite surface even in the presence of cells. Hence,
the observed increase in the recovery of pyrite was due
to copper dissolution from chalcopyrite resulting inpyrite activation [18]. Similar behaviour was observed
at pH 6.5.
When conditioned with the collector, copper disso-
lution from chalcopyrite was very low indicating that the
interaction of collector with the surface copper ions to
form stable Copper(I) alkylxanthate species was
Table 2
Dissolution behaviour of chalcopyrite under different conditions
(15 min conditioning)
Conditions Dissolved Cu (ppm)
Chalcopyrite (pH 4.5) 2.14
Chalcopyrite + pyrite (pH 4.5) 1.53Chalcopyrite + cells (pH 4.5) 1.73
Chalcopyrite+103 M xanthate (pH 6.5) 0.16
0
20
40
60
80
100
PIPX
Cells
Cells
+PIPX
PIPX+
cells
PIPX
Cells
Cells
+PIPX
PIPX+
cells
FlotationRecovery(%) Pyrite
Chalcopyrite
Fig. 6. Effect of sequence of conditioning with cells and collector on the flotation recovery of pyrite and chalcopyrite.
Table 3
Differential flotation of pyritechalcopyrite (1:1) mixture after
conditioning with collector followed by cells
Flotation
pH
Experimental
condition
Weight % in floated fraction
Pyrite Chalcopyrite
4.5 Individually 20.3 81.4Together 21.3 86.2
6.5 Individually 19.8 80.2
Together 19.3 84.6
Conditions: PIPX: 0.5 mM (5 min).
Cells (pH 4.5): 4 108 cells/ml (5 min).
151M.N. Chandraprabha, K.A. Natarajan / Hydrometallurgy 83 (2006) 146152
7/27/2019 Chandraprabha_2006_Hydrometallurgy
7/7
instantaneous thereby reducing the dissolution of copper
from the surface. This observation suggests that the
initial conditioning of the minerals with the collector
would suppress the activation of pyrite.
The effect of bacterial cells on the minerals
conditioned with the collector was further studied toascertain the flotation behaviour of the minerals. Fig. 6
shows the effect of the sequence of conditioning with
collector and cells on the flotation behaviour of pyrite
and chalcopyrite at pH 4.5. It was observed that the
bacterial cells were able to effectively depress xanthate-
interacted pyrite while having negligible effect on the
xanthate-induced floatability of chalcopyrite. It was also
interesting to note that the initial interaction with
collector followed by conditioning with cells improved
the flotation of chalcopyrite compared to the earlier
case. Thus, with this sequence of interaction betterseparation of the minerals can be obtained. Differential
flotation results of the 1:1 pyritechalcopyrite mixture
after conditioning with the collector followed by
interaction with cells are given inTable 3. Under these
conditions the selectivity was markedly improved, i.e.,
pyrite recovery was significantly reduced while chalco-
pyrite recovery was above 80%. The bacterial cells were
able to effectively depress collector interacted pyrite
even when the minerals were conditioned together.
Similar behaviour was observed when the minerals were
conditioned together with cells and collector simulta-
neously (data not shown). Thus it was possible toselectively float chalcopyrite with significant pyrite
depression at both acidic and alkaline pH.
References
[1] Ball, B., Rickard, R.S., in: Fuerstenau M.C. (Ed.), A. M. Gaudin
Memorial Volume. New York, American Institute of Mining
Metallurgical and Petroleum Engineers, 1976, p. 458.
[2] Brierley, C.L., Crit. Rev. Microbiol., 6 (1978), 207.
[3] Natarajan, K.A., Microbes Minerals and Environment, Banga-lore, Geological Survey of India, 1998.
[4] Devasia, P., Natarajan, K.A., Satyanarayana, D.N., Ramananda
Rao, G., Appl. Environ. Microbiol., 59 (1993), 4051.
[5] Yelloji Rao, M.K., Natarajan, K.A., Somasundaran, P., Miner.
Metall. Process., 9 (1992), 95.
[6] Nagaoka, T., Ohmura, N., Saiki, H., Appl. Environ. Microbiol.,
65 (1999), 3588.
[7] Suzuki, I., Chan, C.W., Takeuchi, T.L., Appl. Environ.
Microbiol., 58 (1992), 37673769.
[8] Suzuki, I., Biochim. Biophy. Acta, 104 (1965), 359371.
[9] Suzuki, I., Annu. Rev. Microbiol., 28 (1974), 85101.
[10] Takakuwa, S., Nishiwaki, T., Kayako, H., Tominaga, N.,
Iwasaki, H., J. Gen. Appl. Microbiol., 23 (1977), 163
173.[11] Santhiya, D., Subramanian, S., Natarajan, K.A., Min. Eng., 13
(2000), 747.
[12] Chen, Bor-Yann, Chen, Yun-Wen, Wu, Don-Jun, Cheng, Yang-
Chu, Environ. Eng. Sci., 20 (2003), 375.
[13] Das, A., Modak, J.M., Natarajan, K.A., Min. Eng., 10 (1997),
743.
[14] Gissinger, P.B., Ehrhardt, J.J., Behra, P., Environ. Sci. Technol.,
32 (1998), 2839.
[15] Mats, V., Persson, I., Colloids Surf., A Physicochem. Eng. Asp.,
83 (1994), 207.
[16] Yelloji Rao, M.K., Natarajan, K.A., Int. J. Miner. Process., 27
(1989), 279.
[17] Chandraprabha, M.N., Natarajan, K.A., Modak, J.M., Colloids
Surf., B Biointerfaces, 37 (2004), 93.[18] Wong, G., Lascelles, D., Finch, J.A., Min. Eng., 15 (2002), 573.
152 M.N. Chandraprabha, K.A. Natarajan / Hydrometallurgy 83 (2006) 146152