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Research Article
Received: 9 August 2009 Revised: 5 December 2009 Accepted: 5 December 2009 Published onlinein Wiley Interscience: 25 January 2010
(www.interscience.wiley.com) DOI 10.1002/jctb.2348
Electro-membrane process for the separation
of amino acids by iso-electric focusingMahendra Kumar, Bijay P. Tripathi and Vinod K. Shahi
Abstract
BACKGROUND: Amino acids (AAs) are usually produced commercially using chemical, biochemical and microbiologicalfermentation methods. The product obtained from these methods undergoes various treatments involving extraction andelectrodialysis (ED) for salt removal and AA recovery. This paper describes an electro-membrane process (EMP) for the chargebased separation of amino acids.
RESULTS: Iso-electric separation of AAs (GLULYS) from their mixture, using ion- exchange membranes (IEMs) has beenachieved by an efficient and indigenous EMP. It was observed that electro-transport rate (flux) of glutamic acid (GLU) at pH 8.0(above its pI) was extremelyhigh, while that for lysine (LYS) (pH9.6) acrossthe anion-exchange membrane (AEM) was very low,under similar experimental conditions. Under optimum experimental conditions, separation of GLU from GLULYS mixturewasachievedwith moderate energyconsumption(12.9 kWhkg1), high current efficiency (CE) (65%) and 85% recovery of GLU.
CONCLUSIONS: On the basis of the electro-transport rate of AA and membrane selectivity, it was concluded that the separationof GLULYS mixture was possible at pH 8.0, because of the oppositely charged nature of the two amino acids due to theirdifferent pIvalues. Moreover, any type of membrane fouling and deterioration in membrane conductivity was ruled out underexperimental conditions. This work clearly demonstrates the great potential of EMP for industrial applications.c 2010 Society of Chemical Industry
Keywords: amino acid separation; iso-electric focusing; ion-exchange membrane; electro-membrane process
NOTATION
CE Current efficiencytmi Counter-ion transport number
m Specific membrane conductivity
Wd Weight of dry membrane
Ww Weight of wet membrane
R Gas constant (8.314 J mol1 K1)
a1 and a2 Activities of electrolyte solutions
T Absolute temperature (K)
F Faraday constant (96500 coulombs)
x, area Thickness of the wet membrane (cm)
A Electrode area (cm2)
V0F and Vtp Initial and final volume of the FC (cm3)
C0F and CtF Initial and final concentration of AA in PC(M)
W Energy consumption (kWh kg1)
V Cell voltage (V)
I Current (A)
t Time (s)
m Weight of GLU or LYS (g)
M Molecular weight of GLU or LYS, n t
n Stoichiometric number (n = 1 in this case)
Q Electric quantity passed (Coulombs; A s)
(J)GLU Flux of GLU (mol m2 s1)
(J)LYS Flux of LYS (mol m2 s1)
INTRODUCTION
Withthe advance in lifescience research,numbersof biomoleculeswith pharmaceutical characteristics have been discovered. In the
down-stream process, separation of amino acids (AA) (amphoteric
in nature with more than one ionizable group, fundamental
constituents of all proteins) was stimulated by an increasing
demand forhigh purity in orderto reduce the side effects induced
by impurities.1 5 During recent years, a noticeable growth of AA
production from molasses and raw sugar by a fermentation pro-
cess, andtheir utilization as an additive in food products, chemical
and pharmaceutical industries, has occurred.610 In particular,
glutamic acid (GLU) and lysine (LYS) have found a wide range
of applications in the food, pharmaceutical, biotechnology, bio-
chemistry and cosmetic industries.1113 Various membrane based
processes, such as ion-exchange, nanofiltration (NF), diafiltration,
ultrafiltration(UF), and electrodialysis (ED), were usedfor the sepa-ration of AAs fromfermentationbroths withoutprecipitation.1418
Use of acid and base to regenerate resins in the ion-exchange
process is a disadvantage because it increases the operational
cost. In addition, wastewater produced during resin regeneration
Correspondence to: Vinod K. Shahi, Electro-Membrane Processes Division,
Central Salt & Marine Chemicals Research Institute, Council of Scientific &
Industrial Research (CSIR), G. B. Marg, Bhavnagar-364002 (Gujarat) India.
E-mail: [email protected]; [email protected]
Electro-MembraneProcessesDivision,CentralSalt&MarineChemicalsResearch
Institute,CouncilofScientific&IndustrialResearch(CSIR),G.B.Marg,Bhavnagar-
364002 (Gujarat) India
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Electrode Wash
0.1M Na2SO4
GLU + LYS
in NaAC Buffer
NaAC Buffer
Electrode WashGLULYS
CEM CEMAEM
GLU-
LYS
FeedComp.(FC)
PermeateComp.(PC)
A
node
Ca
thode
Figure 1. Schematic of the EMP cell for separation of amino acids.
and washing causes serious environmental pollution. Membrane
processes such as NF and UF, are size based separation processes
andtheir separation performance is nothigh unless the molecular
weight (MW) ratio of the two components is larger than 10.17,19
In ED, ions are transported through ion-exchange membranes
(IEMs) under the influence of an applied potential to separate
ionic and nonionic constituents.20,21 Recently, bipolar membrane
electodialysis (BMED) processes have been developed for the
conversion of salts into corresponding acid and base.2224 BMED
processeshavealsobeenfoundtobesuitableandcosteffectiveforrecovering organic acid or AAs from their respective salt.2527 Salt
diffusion (co-ion leakage) through the bipolar membrane in BMED
is a serious problem, which affects the purity of the product and
enhances the process cost. There is no ion-exchange membrane
with100% selectivity. Thereis no electro-membrane process (EMP)
based on the principles of ED, used for the efficient separation of
amino acids, with close MWs and different iso-electric points.2831
Working principle of the electro-membrane process (EMP)
The iso-electric focusing technology has been used extensively in
separation of protein or AAs from fermentation broths with great
success. The performance is mainly determined by the net charge
of molecules at different pH and nature of the membranes.15,3234
A schematicdiagramof theEMP cell used forthe separation of AAs
from their mixture is illustrated in Fig. 1. The feed and permeate
chambers were partitioned by an anion-exchange membrane
(AEM) which only allows the passage of anions. Both electrode
chambers (catholyte, anolyte) were separated by cation-exchangemembranes (CEMs), which prevent the approach of AA molecules
to the electrode and further denaturation by electrode reaction.
Thus, at pHpI.
+H2N+H3NCC
(CH2)2
O
OH
COOH
H
CC
(CH2)2
O
O-
COOH
H
H2N CC
(CH2)2
O
O-
COOH
H
Cationic (pI)
C COO-H2N
H
CH2)4
NH3+
C COO-H2N
H
CH2)4
NH2
C COO-+H3N
H
CH2)4
NH3+
Cationic (pI)
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At pH 8.0, GLU existed in the GLU state and LYS in the LYS+
state. There was the possibility for migration of LYS+ towards
the catholyte through CEM. But, at pH 8.0 (near to its pI), due to
the small net positive charge on LYS, its electro-migration from
the feed compartment (FC) to the catholyte was not feasible.
Further, the presence of LYS+ in the catholyte was checked and
found to be negligible. Also, LYS+ remained in the FC due to
its electrical polarity and repulsion between positively charged
AEM. Also, this observation was validated by the mass balance
of LYS in FC before and after the experiments: mass balance was
found to be about 95%. GLU passed through the AEM from
the FC to the permeate compartment (PC), under the applied
electric potential. Thus, high-purity GLU may be obtained in the
PC. For high resolution AA separation, a stable and continuous
pH gradient with relatively constant conductivity and high buffer
capacity is required. Ampholyte was commonly used to provide a
stable pH gradient in the traditional iso-electric focusing system
due to various advantages, such as high buffer capacity, high
solubility, goodconductivity at pIofAAs, and absence of biological
effects.
Therefore, the purpose of this work is to investigate an EMP,
based on the principles of ED to achieve the separation of AAsabove or below the pI of one component in spite of their close
MW and thus molecular size. Herein, we report an EMP for the
separation of AAs from their mixture by iso-electricfocusing using
CEM and AEM as a separation media. A mixture of GLU and LYS in
solution was studied as a model case under similar experimental
conditions.
MATERIALS AND METHODSMaterials
Poly (ether sulfone) (PES) was obtained from Sigma-Aldrich
Chemicals (Mumbai, India) and all other reagents such as GLU,
LYS, H2SO4, NaCl, CdCl2.H2O, DMF, acetic acid, CH3COONa(NaAc), ninhydrine, of Analytical grade reagents (AR) grade were
obtained from S.D. Fine Chemicals, India,and used without further
purification.
Membranes preparation
Sulfonation of PES was carried out as reported earlier.35 CEM
was prepared using sulfonated poly (ether sulfone) (SPES) in
dimethylformamide (DMF) (20%, w/v) and further by casting onto
a cleaned glass plate. The prepared membrane was dried in
ambient condition for24 h, then at 60 C for 6 h ina vacuumoven.
The AEM used in this work was prepared in the laboratory by a
procedure reported earlier and used for various processes.
2831,36
Thus, the membranes obtained (CEM and AEM) were equilibrated
with 1.0 mol L1 HCl and 1.0 mol L1 NaOH solution before use.
The cleaned and equilibrated membranes were stored in double
distilled water.
Electrochemical properties of membranes
The thickness of the wet membrane was measured by micrometer
with 0.10 m accuracy. The membrane water content was
determinedfromtheweightofdryandwetmembrane.Theweight
of dry membrane was recorded after 24 h drying at 60 C, and the
weight of the wet membrane was determined after equilibrating
themembranein water for24 h, with surface water removed using
Table 1. Physicochemical and electrochemicalpropertiesof the CEMandAEM
Properties CEM AEM
Thickness1 (m) 150 150
Water content2 (%) 14.6 10.8
Ion-exchange capacity3
(mequiv./g of drymembrane)
1.03 1.28
Counter-ion transportnumbera,4 (tm )
0.96 0.91
Specific membraneconductivityb,5
(S cm1)
2.05 102 1.12 102
a Measuredby membrane potentialin equilibrationin with0.01 mol L1
and0.1 mol L1 NaCl solutions.b Measured in equilibration with 0.1 mol L1 NaCl solution.Uncertainty for measurements: 1: 1.0 m; 2: 0.1%; 3: 0.01 mequiv g1
of dry membrane; 4: 0.01; and 5: 0.01 103 S cm.
tissue paper. The water content was estimated from:
Water content(%) =WwWd
Wd 100 (1)
For estimation of the ion-exchange capacity (IEC), a piece of
the membrane was equilibrated in 1.0 mol L1 HCl or 1.0 mol L1
NaOH solution overnight to convert them into H+ or OH form.
The excess acid and base was removed by washing with distilled
water. The washed membranes were then equilibrated in 50 mL
of 0.50 mol L1 NaCl solutions to exchange the H+/OH by
Na+/Cl. The amount of H+ or OH ions liberated in solution
was determined by acidbase titration.37
tmi acrossthemembraneswasestimatedbymembranepotential
measurements in equilibration with 0.01 and 0.10 mol L1 NaClsolutions, according to following equation:31
Em = (2tm 1)RT
Fln
a1
a2(2)
The physicochemical and electrochemical properties of CEM
and AEM are presented in Table 1. Both membranes exhibited
good water content, IEC and counter-ion transport number in
the membrane phase under operating conditions. Properties of
these membranes are comparable with the best-known IEMs.38
The knowledge on membrane conductivity in an actual operating
environment is an essential parameter to assess the suitability of
membranes for an EMP.Membrane conductivity measurements for CEM and AEM were
carried out in equilibration with GLU, LYS and NaCl solution
of different concentrations using a potentiostat/galvanostat
frequency response analyzer (Auto Lab, Model PGSTAT 30,
EcoChemie, B.V. Utrecht, The Netherlands). The membrane was
sandwiched between two stainless steel circular electrodes
(4 cm2). Direct current (dc) and sinusoidal alternating currents
(ac) were supplied to the respective electrodes to record the
frequency at a scanning rate of 1.0 A s1 within a frequency
range 106 to103 Hz.39The membrane resistances were obtained
from Nyquist plots using a fit and simulation method. Membrane
conductivity was recorded in equilibration with NaCl, GLU and
LYS solutions of different concentrations. The specific membrane
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conductivity (m) was estimated by the given equation:
m =x
ARm(3)
The variation ofm for both type membranes (CEM and AEM)
in equilibration with NaCl, GLU, and LYS solutions of different
concentrations are shown in Fig. 2(A, B and C), respectively. m
values for both types of IEMs increased with concentration,and were highly dependent on the nature of equilibrating
environment and ionic concentration in the membrane/solution
interfacial zone.Both membranes exhibitedexcellentconductivity
in equilibration with NaCl solution, but m values were relatively
low in equilibration with GLU or LYS solutions of similar
concentration. This may be explained due to extremely low
dissociation constant of AAs and thus lower ionic concentration.40
Furthermore, conductivities values exhibited by CEM and AEM,
suggested their suitability for use in EMP under AAs environment.
Experimental procedure for separation of amino acids byiso-electric focusing
An experimental cell used for EMP was made up of poly vinylchloride (PVC), in which two pieces of CEM and one AEM
were used to separate the four compartments: two electrode
wash chambers (EW) (anolyte and catholyte), FC and PC as
depicted in Fig. 1. The parallel-cum-series flow arrangement
was used for the separation of AAs (GLU and LYS) from their
mixture. Expanded TiO2 sheets coated with a triple precious
metal oxide (titaniumrutheniumplatinum; 6.0 m thickness)
of 1.5 mm thickness and 8.0 103 m2 area, received from
Titanium Tantalum Products (TITAN, Chennai, India) were used
as cathode and anode. Space between each electrode and the
effective membrane area was 1.10 102 m and 8.0 103 m2,
respectively. Peristaltic pumps were used to feed the AA solution
(500 cm3) in a recirculationmode intothe respective compartment
with a constant flowrate (60 cm3 h1) to maintain the turbulence.The whole setup was operated in ambient conditions (303 K)
without any additional temperature control. The 0.1 mol L1
Na2SO4 solution was recirculated into the EW chambers. The
AA solution (GLU or LYS, separately or their mixture) of known
concentration (0.01 0.05 mol L1) in NaAc buffer (0.01 mol L1)
at known pH was fed into the FC, while NaAc buffer (0.01 mol L1)
wasfed into thePC. A dc power supply(Aplab, India, model L1285)
was used to apply constant potential across the electrodes and
the resulting current variations was recorded as a function of time
using a multimeter.
Under the influence of applied potential, amino acid with
negative net charge (AA ; depending on pH) was electro-
transported from FC to PC, across AEM. Solution conductivity and
pHchangesofeachcompartmentwereregularlymonitoredduring
all the experiments. For individual AA solution, concentration
of amino acid (GLU or LYS) was determined by UV-visible
spectrophotometer (Shimadzu, Japan) at max 504 nm fixed
wavelength.41 In a mixture case, AAconcentrationwasanalyzedby
high performance liquid chromatography (HPLC) after precolumn
derivitization using dansyl chloride. A mixture of acetonitrile and
acetate buffer (pH= 4.5; 0.045 mol L1) was used as the mobile
phase flowing through a C18 reverse phase column. The solvent
gradient was 20% to 60% acetonotrile over 30 min. In all cases
an equal volume of AAs solution (separately or their mixture) was
taken for simplicity and to study the feasibility of their separation,
above the iso-electric point of the AAs.
RESULTS AND DISCUSSIONElectro-transport of GLU or LYS
Electro-transport of GLU or LYS (individually) of 0.01 mol L1
concentration in acetate buffer at known pH was carried outin the EMP cell (Fig. 1) at different applied potential (4.06.0 V).
AA (GLU or LYS) solution of different concentrations in acetate
buffer was initially fed into the FC, while only acetate buffer was
fed to the PC. Both EW streams were reconnected and 0.1 mol L1
Na2SO4 solution was recirculated. Variation in current density with
time during electro-transport of AA from FC to PC across AEM
is presented in Fig. 3(A) and (B) for GLU and LYS, respectively, as
a representative case. Experiments were performed at constant
applied potential (4.06.0 V) and resulting variations in current
and concentrations of AA in both compartments (FC and PC)were
recorded as a function of time. At constant applied potential,
current density initially increased and then decreased with time
for both AA solutions. Initial feed concentration (0.01 mol L1 AA
+ 0.01 mol L1 NaAc) of FC and the electrode rinsing solution(0.1 mol L1 Na2SO4) were higher than the concentration of
permeate (0.01 mol L1 NaAc). In this case, buffer solution (NaAc)
and electrode rinsing solution (0.1 mol L1 Na2SO4) did not
influence the electro-migration of AA because the concentration
of NaAc was the same in FC and PC. Migration of Na2SO4was prohibited due to the electro-neutral conditions. Thus the
observed current of the EMP cell varied due to variation in the
electro-migration of AA. A schematic of the EMP for separation of
GLUorLYSor theirmixtureis shownin Fig. 1.Single step separation
was achieved by electro-transport of AA from FC to PC through
0
5
10
15
20
25
30
0 0.02 0.04 0.06
Conc. (M)
0 0.02 0.04 0.06
Conc. (M)
0 0.02 0.04 0.06
Conc. (M)
km
1
0-3
(Scm-1)
AEM
CEM
A
0
2
4
6
8
10
12
AEM
CEM
C
0
2
4
6
8
AEM
CEMB
Figure 2. Membrane conductivity (m) values for CEM and AEM in equilibration with: (A) NaCl; (B) GLU; and (C) LYS solutions of different concentrations.
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5
6
7
8
9
10
11
30 90 150 210
Time (min)
30 90 150 210
Currentdensity(mAcm-2)
4 V
5 V
6 V
A
2
6
10
14
18
4 V
5 V6 V
B
Figure 3. Variation of current density with time at different applied potential during electro-transport of: (A) GLU (0.01 mol L1; pH 8.0) (B) LYS(0.01 mol L1; pH 12) solutions, across the AEM.
2
4
6
8
10
12
14
FC
PC
B
2
4
6
8
10
12
0 50 100 150 200 0 50 100 150 200
Time (min) Time (min)
pH
FC
PC
A
Figure 4. pH variations of FC and PC with time in the EMP at 5.0V for (A) GLU (0.01 mol L1) (B) LYS (0.01 mol L1) solutions as feed for FC.
AEM under the influence of the applied potential. Since, AA was
separated from electrodes by CEMs; electro-migration of AA atspecific pH would not occur because of the strongly charged
nature of CEM. Electro-transport of AA at a particular pH was
further checked by regularly monitoring AA concentration in the
catholyte and anolyte using UV-visible spectrophotometer, and it
was found to be absent.
Under the influence of the applied potential (below limiting
current density), electro-transport of AA from FC to PC was also
verified by the variation of pH and solution conductivity for both
streams (FC and PC) with time, and is presented in Figs 4 and 5 forGLUandLYS,respectively.ThepHofPCdecreasedduetomigration
of AA from FC to PC. Increase in the pH of FC may be attributed
to depletion of GLU andLYS+ inFC.ThepIvalues of GLU and LYS
are3.22 and9.59,respectively. At pH 8.0; GLUexistedas negatively
charged ion (GLU), while at pH 12; LYS existed in the LYS state.
GLU or LYS was electro-transported from FC to PC across AEM
under the applied potential. Simultaneously, AA concentration
0
3
6
9
12
0 100 200 300
Time (min)
0 50 100 150 200
Conductivity(mS
)
FC
PC
A
3
8
13
18
23
FC
PC
B
Figure 5. Variation of conductivity in FC and PC with time at 5.0 V during electro-transport of: (A) GLU(0.01 mol L1 ; pH 8.0) (B) LYS (0.01 mol L1; pH12)solutions.
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in FC decreased, and increased in PC. This phenomenon resulted
in an increase in conductivity and AA concentration in PC. The
conductivity of FC decreased with the time due to depletion
of conducting species (AA). These observations confirmed the
electro-transport of AA across AEM from FC to PC in the EMP.
The electro-transport rate can be assessed on the basis of
GLU or LYS flux (J) in EMP. J values were estimated from the
change of GLU or LYS concentration in FC or PC, considering
negligiblemass(water)transportthroughAEM,usingthefollowing
equation:30,31
J=Va
A
Ct C0
t(4)
where C0 and Ct is the initial andfinal concentration of GLU/LYS
in compartment 1 (mol m3), t is the time allowed for EMP (s),
Va the total volume of solution in the permeate compartment
(0.50 103 m3), and A is the effective membrane area. GLU
and LYS flux during electro-transport are presented in Fig. 6(A)
and Fig. 7(A), respectively, as a function of electricity passed (i.e.
coulombs) at differentappliedpotentials. In bothcases at constant
applied potential, flux initially increased linearly with electricity
passed and then decreased, similarly to the variation of current
density (Fig. 3(A)). Initially, concentration of AA in the PC wasalmostzero. At the start of the process, the concentration of GLU
or LYS reduced in FC, and increased in PC with the amount of
electricity passed. Over time the concentration of AA in the FC
approached a minimum, while in the PC it was enhanced, which
further decreased flux value, similarly to the variation of current
density. Thus we can say that the amount of current (charge)
passed in the EMP at constant applied potential is also a measure
ofAA flux acrossthe AEM in the EMP.Here, itis important tonote
that GLU flux was extremely high, whereas LYS flux across the
AEM was very low under similar experimental conditions, in spite
of their almost equal molecular weight.
Recovery, current efficiency (CE) andenergyconsumption (W)
Recovery of product (GLU or LYS) is an important parameter
to examine the economic feasibility of any process, and may be
defined as:
Glu re covery(%) =CtpVtp
C0FV0F 100 (5)
GLU and LYS recovery (%) at different feed concentrations of
AA into PC is presented in Fig. 6(B) and Fig. 7(B), respectively, as a
function of electricity passed (coulombs). For both cases, recovery
increased with quantity of electricity passed, and decreased
with increasing concentration of AA in FC. Recovery of GLU
was greater than that of LYS, maybe due to the extremely
low migration velocity of LYS across the AEM because of itsbulkier size. It was found that at constant applied potential,
recovery of GLU decreased with increased concentration in FC
because flux becomes independent of feed concentrationabove a
certain minimum concentration.26 Under optimized experimental
0
2
4
6
8
10
12
800 2400 4000 5600 800 2400 4000 5600
Electricity passed (Coulombs)
J1
0-5
(molm-2
s-1)
4 V
5 V
6 V
5
25
45
65
85
Rec
overy(%) 0.01M
0.02M
0.05M
BA
Figure 6. Variation of: (A) flux (J) for GLU (0.01 mol L1; pH 8.0) through the AEM (from FC to PC) with electricity passed (coulombs) at different appliedpotentials; (B) recovery of GLU with electricity passed (coulombs) at 5.0V constant applied potential for different concentrations at pH 8.0; as feed of FC.
6
9
12
15
18
Recovery(%)
0.01M
0.02M
0.05M
B
2
4
6
8
10
800 1800 2800 3800
Electricity passed (Coulombs)
800 1800 2800 3800 4800
J1
0-6
(molm-2
s-1)
4 V
5 V
6 VA
Figure 7. Variation of (A) flux (J) for LYS solution (0.01 mol L1; pH 12) across the AEM with electricity passed (coulombs) at different applied potentials;(B) recovery of LYS with electricity passed (coulombs) at 5.0V constant applied potential for different concentrations at pH 12; as feed of FC.
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which increased steeply beyond pH 9.59 (pI of LYS) due to the
electro-transport of LYS across AEM in the EMP. On the basis
of the above observations, it was concluded that separation of a
GLULYS mixture was possible at pH 8.0, because of the existence
ofoppositely charged statesdue tothe difference in theirpIvalues.
Separation of amino acid (GLU-LYS) from their mixture in EMP
The separation of GLU and LYS (0.01 mol L1, each) from theirmixture was carried out using the EMP cell (Fig. 1) at constant
applied potential (5.0 V) and pH 8.0. Flux values for GLU and
LYS are presented in Fig. 9(A) as a function of electricity passed
(coulombs).GLU fluxwas high, while LYSfluxacross theAEM in the
EMP was extremely low (less than 1.0 mol m2 s1). The separation
factor (SF) can be defined as:
SF= (J)GLU
(J)LYS (8)
Initially the SF value was low, and reached about 7.5 after
passage of an appreciable amount of electricity (Fig. 9(B)). The
positively charged membrane (AEM) allowed GLU flux under
constant applied potential. Thus relatively high SF values reveal
the feasibility of separating GLU and LYS at pH 8.0. For AAs GLU
and LYS, transmission was strongly dependent on the nature of
the charge on the transmitting species (pH), the charge nature of
membranes and the electric gradient. Diffusion of LYS+ andGLU
from PC to anolyte and catholyte was also monitored and both
were found to be negligible.
The selective separation of GLU and LYS from their equi-molar
mixed solution (0.01 mol L1), was carried out at different pH
values from 2.011.0 at 5.0 V. The resulting flux variations are
presented as a function of pH in Fig. 10(A). Below pH 3.22, both
GLU and LYS existed in a positively charged state, and thus their
fluxes were very low and similar across the AEM under given a
electrical polarity. At pH 3.229.59, GLU existed in a negativelycharged (GLU) state, while LYS at pH 8.0 was in a positively
charged state (LYS+). Thus electro-transport and flux of GLU
across the AEM increased progressively, while the flux of LYS+
remained very low due to the diffusion through AEM. At pH 8.0
the difference in the fluxes of GLU and LYS+ was high. Beyond
pH 9.59, both AAsexisted in a negatively charged state (GLU and
LYS), and their flux across the AEM was high but very similar.
The SF values are presented as a function of pH in Fig. 10(B),
showing the optimum pH 8.0 for selective separation of the AA
mixture. The W, CE(%)andrecovery(%)data when separating GLU
at pH 8.0 from the equi-molar mixture of GLULYS at different
feed concentrations are presented in Table 4. Under optimized
experimental conditions (i.e. at 5.0 V applied potential, pH 8.0for 0.01 mol L1 GLU+LYS mixture), 12.9 kWh kg1 energy was
consumed for the separation of GLU from the equi-molar mixture
of GLULYS, CE(65%) and recovery (85%) of the product, showed
the economicfeasibility of the process for industrial exploitation. It
is clearly evident that separation of GLU and LYS can be efficiently
0
2
4
6
8
1000 2000 3000 4000
Electricity passed (Cuolombs)
1000 2000 3000 4000
J1
0-5(
molm-2
s-1)
Glu
Lys
A
3
4
5
6
7
8
Separationfactor(SF)
B
Figure 9. Variation of (A) J; (B) separation factor, with electricity passed (coulombs) at constant applied potential (5.0V) for GLU and LYS mixed solution(0.01 mol L1 each) at pH 8.0 as feed of FC.
0
1
2
3
4
5
6
7
0 2 4 6 8 10 12
J1
0-5
(molm-2
s-1)
pH
0 2 4 6 8 10 12
pH
GLU
LYS
A
0
2
4
6
8
10
Separationfactor(S
F)
B
Figure 10. Variation of (A) J; (B) separation factor, with pH of GLU and LYS mixed solution (0.01 mol L1 each) as feed into FC, after passage of 4000coulombs electricity at constant applied potential (5.0 V).
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www.soci.org M Kumar, BP Tripathi, VK Shahi
Table 4. Energy consumption (W), current efficiency (CE), andrecovery data for electro-transport of GLU from equi-molar GLU+LYSmixed solution (pH 8.0) across the AEM under different experimentalconditions
GLU+LYSconc. of each(mol L1)
Appliedvoltage
(V)W(kWh kg1GLU
separated) CE(%)Recovery of
GLU (%)
0.01 5.0 12.9 65.5 850.02 5.0 16.2 40.9 59
0.05 5.0 20.5 30.5 44
achieved using AEM under a constant applied potential in EMP
due to the difference in their pI values, in spite of very close
molecular weights and sizes. Thus the proposed EMP using IEM is
an importanttool forseparating AAswith close molecularweights
by focusing on their iso-electric values.
In this process no appreciable membrane fouling or AAs
denaturation was observed, while by focusing one component
at itsiso-electric point,and theothercomponent in theoppositely
charged state (depending on pH), they may be effectivelyseparated. In this particular case the difference in the p Ivalues of
GLU and LYS was quite high, but the method could be applied
in cases where pI values are very similar, by very careful control
of pH.
CONCLUSIONSIndigenously prepared CEM and AEM with good physicochemical
and electrochemical properties and stabilities were used to
develop an EMP for the separation of AAs with different pI
values but similar molecular weights. Relatively good membrane
conductivityvaluesforbothtypesofIEMinequilibrationwithNaCl,
GLU or LYS solutions suggested their suitability for application inanEMPundertheexperimentalenvironment.AnEMPcellwithfour
compartments (2-EWs, FC and PC)was fabricated, in whichelectro-
transport of GLU and LYS across the AEM towards the anode
side was studied to see the feasibility of their electro-transport
under given experimental conditions. This is due to the fact that
both the pH of AAs solutions and the electrostatic interaction
between the zwitterionic AA molecules and membrane surface
charge density play important roles in their electro-transport;
thus, demonstrating the importance of employing IEMs in the
EMP system to obtain AA separation by focusing their iso-electric
points with high throughput (flux), purity, recovery and CE. It was
observed that during electro-transport, GLU flux was extremely
high, whereas LYS
fluxes across the AEM were very low undersimilar experimental conditions, in spite of their almost equal
molecular weight and similar charged condition. Also, due to the
relatively high W and low CE and recovery, electro-transport of
LYS is not economically feasible, for the separation of GLULYS
mixture. It was concluded that separation of GLUfromthe mixture
of GLU LYS is possible at pH 8.0, because of the existence
of negatively charged state for both due to the difference in
their pI values. Under optimized experimental conditions (i.e. at
5.0V constant applied potential, pH 10 for 0.01 mol L1 GLU+LYS
mixture), 12.9 kWh kg1 energy was consumed for the separation
of GLU from an equi-molar mixture of GLULYS, CE (65%) and
recovery (85%) of the product, showed the economic feasibility of
the process for industrial exploitation.
Also from data it is clearly evident that separation of GLU
and LYS can be efficiently achieved by using AEM under applied
potential in EMPdue to difference in their pIvalues, in spite of very
close molecular weights. Membrane fouling and deterioration in
membrane conductivitywas notobservedunder the experimental
conditions tested. This work clearly demonstrates the great
potential of EMP for industrial applications.
ACKNOWLEDGEMENTSThe authors thank the Department of Atomic Energy, Government
of India for providing financial assistance by sanctioning project
no. 2007/35/35/BRNS. We also acknowledge the services of the
Analytical Science Division, CSMCRI, Bhavnagar for instrumental
support.
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