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Separation and Purification Technology 52 (2006) 117
Review
Comparative assessment of downstream processing options for lactic acid
H.G. Joglekar , Imran Rahman, Suresh Babu, B.D. Kulkarni, Ajit Joshi
Chemical Engineering and Process Development Division, National Chemical Laboratory (NCL), Pune-411008, India
Received 14 October 2005; received in revised form 20 March 2006; accepted 20 March 2006
Abstract
The possibility of manufacturing a biodegradable polymer from lactic acid has led to extensive research in recovery of lactic acid produced
by fermentation, by different downstream processing routes. This paper assesses the suitability of different downstream processing options suchas reactive extraction, adsorption, electrodialysis, esterification and reactive distillation. It compares the costs of different process routes. The
assessment indicates that the conventional precipitation of calcium lactate, followed by acidification, esterification and hydrolysis will be the most
economical route although it generates large quantity of gypsum sludge.
2006 Elsevier B.V. All rights reserved.
Keywords: Lactic acid; Reactive extraction; Adsorption; Electrodialysis; Esterification; Reactive distillation
Contents
1. Introduction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
1.1. Objective . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
1.2. Global scenario . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 21.3. Polylactic acid/bio-degradable plastics . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
1.4. Lactic acid production . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
1.5. Source of carbohydrates for fermentation . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
1.6. Fermentation . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3
1.7. Downstream processing . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3
2. Reactive extraction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3
2.1. Extractant . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3
2.2. Diluents . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 4
2.2.1. Choice of diluents . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 4
2.3. Effect of extractants, diluents and pH on distribution coefficient . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 4
2.4. Third phase formation . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 5
2.5. Complex formation . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 5
2.6. Re-extraction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 6
2.6.1. Using NaOH . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 6
2.6.2. Using HCl . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 6
2.6.3. Temperature-swing regeneration . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 6
2.6.4. Using trimethyl amine (TMA) . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 7
2.6.5. Diluent swing . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 7
2.7. Choice of extraction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 7
3. Adsorption . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 8
3.1. Reported research . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 8
3.2. Choice of adsorption . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 11
Corresponding author. Tel.: +91 20 25902420; fax: +91 20 25902675.
E-mail address: [email protected] (H.G. Joglekar).
1383-5866/$ see front matter 2006 Elsevier B.V. All rights reserved.
doi:10.1016/j.seppur.2006.03.015
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2 H.G. Joglekar et al. / Separation and Purification Technology 52 (2006) 117
4. Electrodialysis . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 11
4.1. Reported research . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 11
4.2. Choice of electrodialysis . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 12
5. Esterification and reactive distillation . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 12
5.1. Reported research . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 12
5.2. Choice for esterification . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 146. Possible downstream process routes . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 14
7. Future direction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 15
8. Conclusion . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 15
References . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 16
1. Introduction
1.1. Objective
Lactic acid is a simple compound containing both the
hydroxyl and carboxylic acid groups, which permit it to par-ticipate in many interesting and valuable chemical reactions.
Among the known reactions of lactic acid the dehydration to
acrylic acid, the polymerization to poly(lactic acid) and conden-
sation to 2,3-pentanedione are potentially the most profitable
pathways. The viability of making an inexpensive biodegradable
polymer poly(lactic acid) from lactic acid has sparked exten-
sive interest andresearch in the area of producing andrecovering
relatively pure lactic acid. This paper is to assess various down-
stream processing options studied by researchers and identify
affordable process route for manufacturing lactic acid, which is
sufficiently pure for polymerization.
1.2. Global scenario
Lactic acid is currently being produced by number of compa-
nies around the world, but it is only used in limited applications
in the food, flavor as preservative, in cosmetics, leather process-
ing, and pharmaceuticals industries. Lactic acid of higher purity
or without certain impurities is required for polymerization.
The possibility of producing a high volume of inexpensive
lactic acid also has lead to research using lactic acid as an
alternative feedstock for the production of many speciality and
commodity chemicals such as acrylic acid, propionic acid, 2,3-
pentanedione, pyruvic acid and propylene glycol.
The world market of lactic acid is growing every year. Thelevel of production is around 350 millions kg per year [1] and the
worldwide growth is believed by some observers to be 1215%
per year [2].
1.3. Polylactic acid/bio-degradable plastics
The main application field of lactic acid polymer has been
medical applications, fibres, packaging materials and as sol-
vents. These medical applications include its usage utilizing
different properties in terms of tensile strength, viscosity, purity
etc. l-Lactic acid polymer exist in three different forms that can
be used for filling the gaps in bones, solid with tensile strengthto produce sutures (stitching material), and the glue form that
is mainly applied in joining membranes or thin skins in humans
[3]. Another important property of poly lactic acid is its high
strength against ultraviolet (UV) radiation [4].
Polylactic acid has a potential to provide a new product plat-
form to compete with hydrocarbon-based thermoplastic. Poly-
lactic acid polymers have barrier properties similar to polyethy-
lene terephthalate (PET) and gloss, clarity and processabilitysimilar to polystyrene (PS). In addition, they provide heat stabil-
ity at lower temperatures than polyolefins and can be processed
by most melt fabrication techniques, including fiber spinning.
The research on lactic acid related materials have attracted
several universities and institutes in Europe, Asia and USA.
There are a number of small-scale production facilities of poly-
lactic acid. Dow Chemicals and Cargill have the largest poly-
lactide (PLA) producing company with an annual capacity of
140,000 tonnes located in Blair, USA [5].
The future of the polylactic acid depends upon the technol-
ogy efforts of lactic acid manufacturers to develop Polylactic
acid modified with other co-monomers, so as to compete with
polymers such as PETand PS,both on cost andapplicationbasis.
1.4. Lactic acid production
Lactic acid can be manufactured by either chemical synthe-
sis or by fermentation of renewable carbohydrates. Both these
methods are used for commercial production. While chemical
synthesis route produces only a racemic mixture of lactic acid, a
fermentation process can produce a stereoisomer of lactic acid.
Therefore, fermentation process is preferred for the production
of lactic acid and about 90% of lactic acid is produced by fer-
mentation route. Currently the fermentation is carried out in
the batch mode. A large number of carbohydrate materials havebeen used, tested or proposed for manufacture of lactic acid by
fermentation.
1.5. Source of carbohydrates for fermentation
Sucrose from cane and beet, glucose, and whey contain-
ing lactose, maltose and dextrose from hydrolyzed starch are
presently used commercially. Molasses and whey are gener-
ally low-priced sources of sugars for fermentation. Sulfite waste
liquor and Jerusalem artichokes are potential sources of lactic
acid.
Sugar (or dextrose) is the most pure source, but is very costly.Molasses and other wastes are cheap but contain large number
of impurities in larger quantities, which affect downstream pro-
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cesses. Sugar cane juice can be a compromise between quality
and cost. Fermentation conditions also determine the quality of
broth and suitability of downstream processing options.
1.6. Fermentation
Carbohydrates are fermented to l-lactic acid by a number of
microorganisms. As lactic acid is formed and accumulated, pH
of the fermentor broth goes on lowering. This affects the produc-
tivity of microorganisms. Considerable research is being carried
out to develop strains, which canproduce lactic acid at lowerpH.
However it is still not a commercially viable preposition. In con-
ventional process pH of fermentor is continuously maintained
by addition of lime and thus converting lactic acid (partly) to
calcium lactate. Downstream processing of this broth includes
precipitation and acidification of calcium lactate to lactic acid.
This generates huge quantity of calcium sulphate, which poses
an environmental problem. Alternatively lactic acid can be con-tinuously removed from the fermentor by adsorption, extraction
or membrane separation. This is possible if fermentation is in
continuous mode. Alkalis other than calcium, such as ammo-
nium hydroxide, or sodium hydroxide (or carbonate) can also
be used. In that case alkalis need to be recovered and recycled
back.
1.7. Downstream processing
Conventionally two routes are followed: (i) the clarified fer-
mented liquor is concentrated to 32% well above crystallization
point and acidified with sulphuric acid to get the crude lactic
acid. (ii) The crude calcium salt which precipitates from the con-
centrated fermented liquor is crystallized, filtered, dissolved and
subsequently acidified with sulphuric acid according to process
described by Inskeep et al. [6] and Peckham [7]. In this route the
precipitated calcium lactate is separated from dissolved impu-
rities by filtration and washing. However, some impurities are
retained in the cake. There is a loss of calcium lactate along
with the washes. The conventional route generates huge quan-
tities of calcium sulphate cake. The cake with retained organic
impurities is difficult to dispose of.
Filtered fermented broth mainly contains impurities such as
residual sugar compounds, colour andother organic acids.These
impurities can be removed by reactive extraction, adsorption,electro dialysis and esterificationhydrolysis with distillation.
Research work done by various researchers on these purification
steps is reviewed and assessed here.
2. Reactive extraction
Lactic acid is poorly extractable by common organic solvent
due to their hydrophilic nature. Therefore, reactive extraction
has been considered for its recovery from aqueous solutions.
Reactive extraction of the lactic acid by a suitable extractant
has been found to be a promising alternative to the conventional
processes.Reactive extraction uses reaction between the extractant and
the material being extracted. The extractant in the organic phase
reacts with a material in aqueous phase and reaction complex is
solubilized into the organic phase. The lactic acid is recovered
from the organic layer by stripping. The prerequisite of an eco-
nomic recovery by extraction is a high distribution coefficient.
Reactive liquidliquid extraction has the advantage that lactic
acid can be removed easily from the fermentation broth (extrac-
tive fermentation), preventing the lowering of pH. Further, the
lactic acid can be re-extracted and the extractant and diluent
recycled to the fermentation process. However this implies that
extractant and diluent must not be toxic to the microorganism
used in fermentation. This can ideally be done for continuous
fermentation. Wasewar et al. [8], have reviewed and critically
analyzed the fermentation of glucose to lactic acid coupled with
reactive extraction.
Membrane extraction overcomes many drawbacks of the
extractive fermentation which have plagued us for long, and
offers other numerous advantages, such as (i) no fear of
back mixing, (ii) no direct exposure of microbes to extractionreagents, thereby ensuring biocompatibility, (iii) no need for
agitation, (iv) potentially high efficiency, etc. For the above rea-
sons, membrane extraction can be considered a very promising
alternative to the conventional solvent extraction for separation
and purification of lactic acid [9].
Huang et al. [10] and Tong et al. [11] successfully developed
an energy-efficient hollow-fiber membrane extraction process to
separate and recover lactic acid produced in fermentation.
2.1. Extractant
The extractant should have low water solubility, a high dis-tribution coefficient for the lactic acid and low distribution coef-
ficient for the impurities such as residual sugars [12].
The distribution coefficient is defined, as ratio of the concen-
tration of lactic acid in solvent phase to concentration of lactic
acid is aqueous phase. Organic bases or amine extractant can
provide much higher equilibrium distribution coefficient (Kd)
for the extraction of carboxylic acids than conventional solvents.
Kd =Cs
Cw, (1)
Cs is the total concentration of acid in solvent phase at equi-
librium, expressed as milliequivalent per milliliter; Cw the total
concentration of acid in water phase at equilibrium, expressedas milliequivalent per milliliter.
On account of its highly hydrophilic character, lactic acid
purification with solvent extraction by carbon bonded oxygen
donor extractants is not practical. Phosphorus-bonded, oxygen-
donor extractants contain a phosphoryl group which is a stronger
Lewis base than the carbon-bonded oxygen group. Further-
more, extractants belonging to this group coextract less water
and are less soluble in water than the extractants of the carbon-
bonded oxygen group.
It has been reported that long chain tertiary amines are suit-
able for the recovery of carboxylic acid from aqueous solution
[13]. Due to physical properties of aliphatic amines they mustalways be used in theform of solutionsin organic diluents.These
organic diluents affect the basicity of amines thereby, extraction
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behaviorof amineis significantly varied [14]. Recently, the influ-
ence of the chain length of tertiary amine on extractability has
been investigated in polar diluent and nonpolar diluent, respec-
tively [15]. In polar diluent such as 1-butanol, 1-hexanol, and
1-octanol, the extractability of tertiary amines increases with the
chain length of amines. However, the extractability of tertiary
amines decreases with the chain length of amines in nonpolar
diluent such as n-heptane [15].
Tertiary amines seem to be more suitable extractants for
organic acid removal compared to primary and secondary
amines [16].
2.2. Diluents
Long chain aliphatic amines are effective extractant for sep-
aration of carboxylic acid from dilute aqueous solution. Gen-
erally, the amine extractants are dissolved in diluent [17], an
organic solvent that dilutes the extractants to the desired concen-tration and controls the viscosity and density of solvent phase.
Solvents that contain functional group that interact strongly with
complex arecalled as theActive Diluent e.g. 1-octanoland that
of which interact inertly with complex are called Inert Diluent
e.g. n-hexane.
Diluents are classified as active diluents and inert diluents
depending on the interaction with the complex [18,19].
2.2.1. Choice of diluents
The choice of suitable diluents [20] for amine is not easy.
Polar diluents are more favorable than the nonpolar solvents
as shown in the extraction of lactic acid [12,18,21]. There areseveral important parameters, which must be taken into consid-
eration.
2.2.1.1. Distribution coefficient. The distribution coefficient
value in the extraction step should be greater than 1 at room
temperature and below 0.1 in the stripping step in order to obtain
a high concentration in the stripping raffinate.
2.2.1.2. Toxicity. Toxicity of the organic solvent and extractant
to microbes is the critical problem in extractive fermentation.
The degree of toxicity depends on the microbe and extractant
solution used [8]. Brink and Tramper [22] reported that theleast toxicity is expected from solvents of low polarity and high
molecular weight.
Toxic effect of extractants and diluents on microorganisms
can also be avoided by immobilization of cells. Yabannavar et
al. [23], reported that addition of soybean oil in immobilized
cells protects cells from toxic effects of extractants and diluents.
Tik et al. [24] obtained a maximum total lactic acid concen-
tration (2.5 times that without extraction) when 15% Alamine
336 in oleyl alcohol together with immobilized cell with 15%
sunflower oil was used.
Wasewar [8] concluded the Alamine 336 in oleyl alcohol,
which has the highest distribution coefficient, would serve as anideal extraction system unless the higher phase level toxicity of
octanol is reduced by using an immobilized enzyme system.
2.2.1.3. Solubility in water. This is important for several rea-
sons. One is economy and the diluents have to be recovered
from the raffinate phase by stripping. The physical properties
of fermentation broth make it desirable to avoid raffinate strip-
ping. A low concentration of some cheap hydrocarbon can be
acceptable for this consideration.
2.2.1.4. Viscosities and density. Low viscosity and low density
promote phase separation. These properties are best achieved
with paraffinic hydrocarbons.
2.2.1.5. Stability. Hydrocarbons are preferable to alcohol and
halogenated hydrocarbons as they are more stable.
2.3. Effect of extractants, diluents and pH on distribution
coefficient
Table 1 summarizes the reported results for various extractantin diluents and the Kd values. In general, the extraction power of
extractant is dictated by the basicity of the amine. The diluents
also affect the basicity of the amine and thus the stability of the
ion pair formed and its solvation power.
The use of tertiary amines including tri-n-octylamine (TOA),
triisooctylamine, and Alamine 336 for the extraction of
lactic acid from aqueous streams has been often reported
[12,1719,21,2527]. Tertiary amine extractants are effective,
with Kd strongly dependent upon the nature of the diluent [13].
The lactic acid extracted had to be stripped for the final
production of lactic acid. The reaction of amine and acid is
exothermic reaction, so the extraction efficiency of lactic acid
decreases with increasing temperature for active diluents where
as it shows little effect for inert diluents [16,18,19,27,28]. The
stripping efficiency does not change with the variation of inac-
tive diluent except for polar chlorobenzene [19,29].
The pH of the aqueous phase is an important parameter for
the reactive extraction of organic acids. Yang et al. [30], reported
that lower pH values result in good separation of lactic acid by
long chain tertiary amines. In the intermediate pH range (35),
Kd decreased with increasing equilibrium pH of the aqueous
phase. However, in the extremely high and low pH ranges, Kdremained insensitive to pH values. Similarly, Choudhury et al.
[32], reported that the distribution coefficient of lactic acid was
high at pH 2.0. In addition, these authors pointed out that theamount of amine in diluents affects the reactive extraction of
organic acids. Kd increased with increasing amount of aliquat
336, in their studies. They reported that increasing amine con-
centration might have a toxic effect on microorganisms in the in
situ extractive fermentation.
Temperature and initial organic acid concentration are also
important parameters for the extraction of organic acids. Yaban-
navar and Wang [33] investigatedthe extraction of aqueous lactic
acid by trioctylphosphineoxide in dodecane and Alamine 336
in oleyl alcohol. In their study, Kd decreased with increasing
initial lactic acid concentration and increased with increasing
concentration of Alamine 336 in oleyl alcohol. Martin et al.[21] studied the extraction of lactic acid from aqueous solu-
tions by Alamine 336 dissolved in toluene. They observed
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Table 1
Kd values reported in literature
Serial number Initial concentration Extractant Diluent Kd Reference
1 20% w/w TOAtripropylamine (TPA) (2:8w/w) 1 mol/kg 1-Octanol/ n-heptane
(3:7 w/w)
0.8 [15]
10% w/w TOATPA (2:8 w/w) 1 mol/kg 1.2
7.5% w/w TOATPA (2:8 w/w) 1 mol/kg 4
5% w/w TOATPA (2:8 w/w) 1 mol/kg 90
2 20% L.A. Tri-n-butyl phosphate (TBP) 0.95 [34]
TOA (0.8 M) Chloroform 9.44
TOA (0.8 M) Tributyl phosphate 7.42
Tributyl amine (TBA) Methylisobutylketone
(MIBK)
0.21
TOAmethylene chloride (0.6 M) Hexane 2.52
Chlorobenzene 0.2
Heptane 2.14
3 Model media
containing 90% l+
lactic acid
Cynex 923 (0.85 mol/l) Kerosene 2 [35]
Hostarex-327 (60% w/v) Xylene 4.44
Trioctylphosphine oxide (TOPO) Xylene 2.2
4 L.A. (2.3mol/l) TOA (1 M) Chlorobutane 1.4 [36]
L.A (2.6 mol/l) TOA (1.2 M) Methylene
chloriden-hexane
1.45
5 1.3 mol/l L.A. MIBK 0.13 [17]
Alamine 336 (0.3 mol/l) MIBK 8.3
Alamine 336 (0.3 mol/l) Chloroform 5.3
Trilauryl amine (1 mol/l) Xylene 8.3
6 0.0051.5 mol/l Alamine 336 940% MIBK decanol,
octanol
4.24 [37]
24.0
26.0
7 10 g/l L.A. 50% Alamine 336 Oleyl alcohol 13 [38]100 g/l L.A. 50% Alamine 336 Oleyl alcohol 4
8 1.6 mol/l L.A. Alamine 336 (40% v/v) MIBK 4.24 [39]
9 Calcium lactate Alamine (48%v/v) Octanol (30% v/v)
Isopar K Exxon
(22%) CO2 (300psig)
0.62 [40]
10 79 g/l lactate TOPO (30 wt.%) MIBK (70 wt.%) 1.05 [41]
Alamine 336 (82 wt.%) 10% Octanol 8%
isopar K
3.35
Alamine (100%) 0.36/5.9
Alamine 336 (89 wt.%) 9% Dodecanol 2%
isopar K
2.6
that the extraction of lactic acid decreased with increasing
temperature.
2.4. Third phase formation
In extraction of lactic acid with long chain tertiary amines
dissolved in organic diluents a third phase may form between
aqueous and organic phase. This phase is not broken by cen-
trifugation at high rpm. The third phase represents limiting
conditions for extraction, which must be avoided [42]. For best
separation of the emulsion that results from the third phase, a
phase modifier is being added to the organic solvent, represent-ing a long chain aliphatic alcohol, a component assuring a higher
solubility of the acid complex in the extract phase. Sometimes
mixed tertiary amine of short chain amine and long chain can
overcome the third phase formation. No cloudy, bubbly looking
phase was observed in this study. The prevention of third phase
makes the phase separation easy, thereby, the settling time gets
shortened.
2.5. Complex formation
Long-chain aliphatic amines are effective extractants for the
separation of carboxylic acids from dilute aqueous solution. The
specific chemical interactions between the amines and the acid
molecules to form acidamine complexesin the extractant phaseallow more acid to be extracted from the aqueous phase. Gen-
erally, the amine extractants are dissolved in a diluent such as
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a ketone, an alcohol, chloroform, etc., that is, an organic sol-
vent that dilutes the extractant to the desired concentration and
controls the viscosity and density of the solvent phase.
Many factors have been found to influence the equilibrium
extraction characteristicsof these systems. Three important vari-
ables are the nature of the acid extracted, the concentration of
the extractant, and the type of diluent. These factors have been
extensively studied for the extractions by tertiary amines of sev-
eral carboxylic acids, including lactic acid [31,43].
Eyal et al. [44], summarized the extraction of acid by amines
and proposed thatfour majormechanisms determine acid extrac-
tion by amine-based extractants: anion exchange, ion-pair for-
mation, H-bond formation, and solvation. These four mecha-
nisms depend on the strength of the amine-based extractant. For
amines of basicity similar to or higher than that of the anion
of the extracted acid, extraction is governed by ion-pair forma-
tion. H-bonding of undissociated acid becomes important only
for extractions of weak bases. Also, the specific basicity of theextractant (pKa,B), defined as follows, is suggested to express
the nature of extractant
R3NH+Ka,BR3N+H
+, (2)
Ka,B =[R3N][H
+]
[R3NH+]
, (3)
where R3N represents TOA. The species in the organic phase
are marked with an overbar, and all of the concentrations are
expressed in molar terms. pKa,B
depends on the amine concen-
tration and diluent type, representing the structure of the amine,
multiplied by coefficients for diluent solvation properties and
the properties of the anion of the extracted acid (hydrophobic
properties and steric hindrance).
The reactive extraction equilibrium for polar dilute solu-
tions of organic solutes can be described by the mass action
law in which the equilibrium behavior is modeled by postulat-
ing the formation of various stoichiometric complexes of acid
and amine. In addition, it is assumed that the carboxylic acid
is dissociated in water and extracted into the extractant phase
through the physical solubility of the solute in the diluent of
the extractant phase and the formation of 1:1, 2:1, 3:1, and
1:2 acidamine complexes, where the 2:1 and 3:1 complexesresult from the dimer and trimer, respectively, of the acid in the
extractant phase and the 1:2 complex results from hydrogen-
bond association between TOA and the hydroxyl and aldehyde
group on carboxylic acid. The physical extraction with diluent
and reactive extraction with TOA fit the simple additive model.
Although the stoichiometry of lactic acidamine extraction
systems has been studied there is no general agreement. The
formation of (1:1) acidamine complex has been commonly
suggested. Prochazka et al. [45] have indicated the forma-
tion of (1:1), (2:1) and (2:2) complexes for the extraction
of lactic acid by trialkylamine in mixtures of 1-octanol-n-
hexane. The quantitative description of the effect of amine andacid concentration on the change in complex composition is
unclear.
2.6. Re-extraction
In reactive extraction, the amine extractant recovers the acid
by reacting with it to form an acidamine complex that is sol-
ubilized into the extractant phase. A Second step, referred to
as regeneration, reverses this reaction to recover the acid into a
product phase and the acid free extractant, available for recycle.
The reported regeneration methods for lactic acid from a
loaded organic phase are described individually in the following:
Tamada and King [17] considered two approaches for regen-
eration through backextraction into an aqueous phase. These
involve changes in the equilibrium relationship through a swing
of temperature and a swing of diluent composition. Yabannavar
and Wang [23,33] suggested two methods for recovery of lactic
acid from a loaded solvent phase: using NaOH and using HCl.
2.6.1. Using NaOH
In the first recovery method, Yabannavar and Wang [23] sug-gested the backextraction of lactic acid from a loaded organic
phase (lactic acid + Alamine 336 + oleyl alcohol) with small vol-
ume of a sodium hydroxide solution [1:10 (v/v) NaOH-solvent].
NaOH in excess of stoichiometric amounts can be used to
ensure complete lactic acid recovery. Yabannavar and Wang [23]
obtained 100% recovery of lactate. The resultant high product
concentration is certainly desirable from the point of economic
product recovery.
However, the acid is then recovered as sodium lactate. One
must add an appropriate acid (e.g., sulfuric acid) to return it to
the free acid form. This approach has the same drawbacks as the
classical calcium precipitation process for direct recovery from
the aqueous feed. Both sulfuric acid and NaOH are consumed,
and a waste salt is formed, which requires disposal. The degree
of reextraction of lactate with 0.1 N NaOH is high (90%). The
degree of reextraction with water amounts to only 55%.
2.6.2. Using HCl
In the another recovery method suggested by Yabannavar and
Wang [33], concentrated HCl is used to essentially displace the
lactic acid from the loaded organic phase (lactic acid + Alamine
336 + oleyl alcohol). More than stoichiometric amounts of HCl
were necessary to recover most of the product from the solvent.
The lactic acid recovered through backextraction with HCl is in
the undissociated form. It is possible to regenerate the solvent bydistilling diluent in thedispersed organic phase. This methodhas
the drawbacks that aqueous HCl is highly corrosive and requires
special material of construction (glass lined/graphite).
Yabannavar and Wang [33], recommended the reextraction
of the free acid from Alamine 336/oleyl alcohol solution with
cone. HCI. The obtained yield was fairly high (83%), however,
the emulsion formed during the reextraction was very stable.
2.6.3. Temperature-swing regeneration
In a temperature-swing extraction/regeneration scheme [46],
the extraction is carried out at relatively low temperature, pro-
ducing an acid-loaded organic extract and an aqueous raffinatewaste stream containing the unwanted feed components. Dur-
ing regeneration, the extract is contacted with a fresh aqueous
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stream at a higher temperature to produce an acid-laden aqueous
product stream and an acid-free organic phase. The concentra-
tion of the acid achievable in this stream depends on the amount
of change in the extraction equilibrium between temperatures
and can be higher than that in the original aqueous feed stream
[46].
At low acid concentrations, a strong diluent effect can be
recognized. The Kd value is a function of the polarity of the
diluent and its ability to form hydrogen bonds. At higher acid
concentrations, however, this diluent effect diminishes consid-
erably. For highly complexed amines, the Kd value depends only
slightly on the acid concentration. The Kd value is considerably
reduced with increasingtemperature. This behavior ofKd is used
to reextract the citric acid into the aqueous phase by temperature
increase. Because of the lower enthalpy change, the extraction
efficiency of lactic acid by temperature-swing regeneration is
low [47].
2.6.4. Using trimethyl amine (TMA)
Lactic acid extracted in the organic phase can be back
extracted with a stronger volatile amine like TMA in aqueous
phase. It avoids consumption of chemicals and creation of salt
byproduct. The aqueous base, which is volatile, enables thermal
decomposition of the acidbase complex in the aqueous back-
extract. The decomposition forms lactic acid as a product and
freebase as a vapor that can be reabsorbed in water and recycled
for reuse in backextraction. The most obvious water-soluble,
volatile base is ammonia. However, ammonia and both primary
and secondary aminesform amides when they are heated in mix-
tures with carboxylic acids [4850]. The amides are sufficiently
stable so that it is difficult to reverse the process and recover the
amine.
The theory of extraction accompanied by chemical reaction
has been used to obtain the kinetics of back extraction of lactic
acid by aqueous TMA. In thermal regeneration of TMA, 99%
of TMA was removed at 200 mmHg from trimethylammonium
lactate aqueous solution.
An approach for regeneration and product recovery from
organic extracts (alamine, TPATOA in diluents) is to back
extract lactic acid with a water soluble, volatile tertiary
amine such as trimethyl amine. Equilibrium data presented by
researchers shows near stoichiometric recovery of lactic acid
from amine extract.The organic phase, which is recycled to the fermentor, may
contain residual dissolvedTMA,whichcan affect the bioactivity
of the enzyme.
2.6.5. Diluent swing
This is based on a shift of the equilibrium distribution of acid
from the aqueous phase to the organic phase between forward
and back extraction caused by a change in composition of the
diluent with which the extractant is mixed. This diluent compo-
sition swing facilitates back extraction of acid into an aqueous
product phase. The composition of the acid laden organic phase
leaving the extractor is altered, by either removal of the diluentor addition of another diluent, to produce a solvent system that
promotes distribution of the acid to the aqueous phase.
This altered organic phase is contacted with a fresh aque-
ous stream in the regenerator to produce the acid laden aqueous
product andthe acid-freesolvent for recycle to theextractor [47].
Adjustment of the diluent composition can also occur before
this solvent reenters the extractor. This approach involving more
than one diluent appears to be more complicated than the TMA
approach, where an easily removable volatile amine (TMA) is
the only externally introduced component. This process has the
disadvantage of diluting the extract stream and requiring dis-
tillation of large amounts of solvent (after the regeneration) to
obtain the same shift in the active/inert diluent ratio.
Tamada and King [47], suggested the diluent-swing regen-
eration process for lactic acid. Baniel et al. [40], also described
regeneration by back extraction following a changein thediluent
composition. In the diluent-swing process, extraction is carried
out in a solvent composed of the amine and a diluent that pro-
motes distribution of the acid in the organic phase.
To date, diluent systems have been composed of organic sol-vents that are liquids at room temperature. A drawback of such
systems is that changes in extractant-phase composition gen-
erally involve a distillation step to separate the active and inert
diluents.To avoid this energyexpense, a new process is proposed
that will replace the inert liquid diluent with a gas anti solvent.
Here, anti solvent is used to connote a substance that has a low
capacity to solubilize the extracted acid. In this process, the dilu-
ent composition change will be effected by pressurizing it with
a gaseous antisolvent (e.g., propane).
For carboxylic acids that exist as solids at room temperature,
this composition change might induce precipitation of the acid
product from the extractant phase. Alternatively, for acids that
are not solids at room temperature, this composition change will
be carried out while the extractant is in contact with an aqueous
product phase. Here, the antisolvent will shift the equilibrium
distribution of the acid to favor the aqueous product phase.
The idea for this process stems from previous work [51] on
extraction of carboxylic acids with amine extractants that indi-
cated that the chain length of liquid-phase aliphatic hydrocarbon
diluents (C7C12) has little effect on extractant loading. This
result is not surprising, since such diluents provide essentially no
stabilization of the acidamine complex. It is therefore expected
that gaseous aliphatic hydrocarbons (e.g., propane) will behave
similarly as inert diluents. Acid extraction power is expected
to decrease with increasing concentrations (i.e., higher partialpressures) of propane in the organic extractant phase. Thus,
a diluent-swing regeneration process will be devised whereby
pressurizing the system with propane gas will effect changes in
extractant composition. A benefit of this process over conven-
tional recovery techniques is that the diluent components can be
easily separated (e.g., by a flash operation) without involving a
distillation step.
2.7. Choice of extraction
The main parameters for selection of a diluent-extractant
system for extraction of lactic acid are distribution coefficient,toxicity, complexation constant and feasibility for back extrac-
tion. From the literature it is noted that Alamine 336 in proper
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8 H.G. Joglekar et al. / Separation and Purification Technology 52 (2006) 117
diluent is the best single extractant in terms of distribution coef-
ficient, toxicity and feasibility for back extraction. The oleyl
alcohol is a better diluent than octanol. However this system
forms a third layer, which is undesirable.
In reactive extraction by using mixed diluents such as 1-
octanol/n-heptane, the third layer formation is avoided, as well
as optimum extractability can be obtained by proper ratio of
short chain amine and long chain amine. Extraction efficiency
increases with decreasing initial lactic acid concentration in
aqueous phase. For 5 wt.% lactic acid concentration, the maxi-
mum extraction efficiency was obtained for TPA/TOA ratio in
the range of 6:48:2.
Regeneration of lactic acid-laden amine extractants by addi-
tion of a gas antisolvent appears to have advantages over more
traditional diluent swing or temperature swing methods. A
potential secondary benefit of regeneration by gas antisolvents
might be the ability to fractionate a mixture of carboxylic acids.
However this needs to be evaluated.Thus the best results can be obtained by employing reactive
extraction using a mixture of TPA and TOA as extractant, 1-
octanol and n-heptane as diluent and gas-antisolvent-induced
regeneration for reextraction. It is to be used advantageously
with continuous or semi continuous fermentation. Reactive
extraction does not totally separate other organic acids from
lactic acid and further purification is necessary.
3. Adsorption
Recovery of carboxylic acids from fermentation broths
presents a challenging separation problem, because of the dilute,
complex natureof fermentation broths. Methods of recovery that
utilize separatingagents, such as solidsorbents, that are selective
for carboxylic acids are attractive and reported by researchers
such as King [52], Tung and King [53]. Important characteristics
of extractants and solid sorbents are a high capacity for the acid,
a high selectivity for the acid as opposed to water and substrate
(e.g., glucose), regenerability, and, depending upon the process
configuration, the biocompatibility with microorganisms. Many
fermentations, such as that for lactic acid production, are subject
to end-product inhibition [23,54]. If a solid sorbent can be used
in situ or in an external recycle loop, higher overall yields can
be achieved.
3.1. Reported research
Many fermentations to produce carboxylicacids operate most
effectively at pH abovepKa of theacid product. Forexample, lac-
tic acid (pKa = 3.86) is typicallyproducedat pH 56[55,56].One
approach for recovering carboxylic acids from such solutions
is to use agents that are sufficiently basic to retain a substan-
tial capacity several pH units above the pKa of the carboxylic
acid. Tung and King [53] investigated extraction and sorption
of lactic and succinic acids using different basic extractants and
polymeric sorbents. The results showed that the uptake in the
pH range 56 varied substantially from one agent to another andwas strongly dependent upon the basicity and capacity of the
agent. Agents to be used in fermentation processes should pro-
vide high selectivity between the product carboxylic acid and
substrate sugars. In addition to conservation of substrate, one
reason why very high selectivitys are often sought is the ten-
dency for small amounts of sugars in a product such as lactic
acid to cause discoloration. Reported measurements of uptake
capacities for sugars and for selectivity achieved between car-
boxylic acids and sugars with extractants and/or solid sorbents
are few and fragmentary.
Kaufman et al. [57], screened a series of solid sorbents
preliminarily for possible utilization in biparticle fluidized-bed
fermentation to produce lactic acid from immobilized Lacto-
bacillus delbreuckii, measuring selectivity between acid and
sugar as well as other properties. Kaufman et al. [58], presented
selectivities between lactic acid and glucose obtained with a
fixed bed of the sorbent Amberlite IRA-35 under a particu-
lar set of operating conditions. Evangelista et al. [59], reported
breakthrough curves for lactic acid and glucose during fixed-bed
adsorption with actual fermentation broths.For typical lactic acid fermentations, the sorbent should
demonstrate substantial uptake in the pH 56 range [53,60].
Ion exchange technique is widely used in bio-separation
[61,62] and several different ion exchangers such as poly(4-
vinylpyridine) resin (PVP) [63], IRA-420 [64], IRA-400 [65,66]
have been studied on the recovery of lactic acid in the past
few years. However, little systematic research has been done
on the effect of different operating conditions on the separa-
tion efficiency of lactic acid and especially on the purification
performances of lactic acid.
Karl-Heinz et al. [67], discloses the separation of lactic acid
from a fermentation medium with an adsorbent comprising a
polymer with tertiary amino groups as described in US Patent
4,552,905 [68].
Kawabata et al. [69], separated carboxylic acid by using a
polymer adsorbent of pyridine skeletal structure and a cross-
linked structure.The polymer adsorbentshowed goodselectivity
and high adsorption capacity for carboxylic acids even in the
presence of inorganic salts. The selected eluants were aliphatic
alcohol, aliphatic ketone, and carboxylic ester.
Evangelista and Nikolov [70], recovered lactic acid from
fermentation broth by weak base polymer adsorbents MWA-
1, IRA-35, and VI-15. The pH for the adsorption of lactic acid
was below its pKa and fermentation broth was acidified by using
cation exchange resin instead of using inorganic acid to elim-inate possible competition between inorganic acid and lactate
in the subsequent adsorption steps. Methanol and 5% NH4OH
were used as elutants. Though 1.5 times of bed volume of 5%
NH4OH could recover all the adsorbed lactic acid from MWA-1
column, product purity was not high. However, 6.8 times of bed
volume of methanol could completely desorb lactic acid from
VI to 15 anion exchange resin with higher purity.
Simulated moving bed (SMB) chromatography is a continu-
ous separation process that has many important industrial appli-
cations [71]. An SMB consists of a circle of chromatographic
columns. The circle is typically divided into four zones by two
inlet ports and two outlet ports. The four ports move periodicallyby one column length along the mobile phase flow direction to
follow themigrating solute bands.The port movement maintains
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product purity and yield, while achieving simulated counter-
current movement between the adsorbent and the fluid [72].
In comparison to batch chromatography, SMB processes have
higher yield and product purity as well as lower solvent con-
sumption. SMB has been used, for instance, for hydrocarbon
and high fructose corn syrup purification [71]. Recently, SMB
has been developed for the separation of racemic mixtures or
isomers [73,74].
Lee et al. [75], explored the feasibility of developing a SMB
process for the separation of lactic acid from other organic
acids present in a fermentation broth. Poly(4-vinylpyridine)
resin (PVP), which was found to have a high capacity and selec-
tivity for organic acids in a previous study [76], was chosen as
the adsorbent. A systematic design method, which is based on
the standing wave analysis for Langmuir isotherm systems, was
tested for this separation [74]. Adsorption isotherms and mass
transfer parameters for the two organic acids were determined
from frontal chromatograms. These parameters were first vali-dated by comparing the single-column frontal chromatograms
with simulations based on a rate model [77]. The validated
parameters were applied in the standing wave design to find the
four zone flow rates and step time for a laboratory SMB unit.
High product purity (99.9%) and relatively high yield (>93%)
were achieved in the SMB experiments. SMB column profiles
and effluent histories can be better explained if the adsorption
isotherm of lactic acid is represented by a modified Lang-
muir equation. The standing wave design method was extended
to nonlinear systems with modified Langmuir isotherms. Rate
model simulations show that this method can achieve higher
purity and higher yield for this separation than the design based
on the Langmuir isotherms.
Chen et al. [78], examined polyvinyl pyridine (PVP) and
activated carbon for the adsorption characteristics pertinent to
their application in lactic acid fermentation. For PVP the lin-
ear adsorption constant, Kad, was between 0.7 and 1.0 for an
equilibrium pH range of 39. The pH was adjusted by acid/base
addition,similar to pH control in fermentation. Thevalues ofKadin the pH-adjusted systems were much lower than that reported
for pure lactic acid solutions, i.e., about 9.7. Furthermore, no
clear effect of pH was observed. These are attributed mainly to
the competition of anions (Cland lactate) for the adsorption
sites of protonated pyridinal N. Its adsorption capacity was also
found to decrease with the base regeneration (by about 14%
each time) after being contacted with the culture broth. These
factors limit its potential application in lactic acid fermentation.
Activated carbon was much more effective in lactic acid/lactate
adsorption than PVP. The adsorption further favored lower pH
under acid (HCI) addition. Activated carbon has been reported
to adsorb glucose. However, the presence of glucose in 070 g/l
was found in this study to have an insignificant effect on lac-
tate adsorption. Cells ofL. delbrueckii also adsorbed rapidly on
activated carbon. This cell adsorption had a negative effect on
lactate adsorption.
Kulprathipanja et al. [79], studied the separation of lactic acid
from a fermentation broth by using an adsorbent comprising
a water-insoluble macro-reticular gel or weakly basic anionic-
exchange resin possessing tertiary amine or pyridine functional
groups or a strongly basic anionic exchange resin possessing
quaternary functional groups. The resins are in sulphate form
and have a cross-linked acrylic or styrene resin matrix. Theadsorption mechanism is shown Fig. 1. For tertiary amine and
pyridine-function-containing ion exchange resins, the lone elec-
tron pair of the nitrogen atom enables nitrogen atom to form
hydrogen bond with sulfate ion. IRA-400, strongly basic qua-
ternary ammonium ion exchange resin has positive charge and
can form ionic bond with sulfate ion. The sulfate form of qua-
ternary ammonium of anion exchange resin has a weakly basic
property and can adsorb lactic acid through acidbase interac-
tion. Consequently, the adsorption of lactic acid is not affected
by inorganic salt in fermentation broth. Lactic acid is desorbed
with water or dilute inorganic acid. The pH of the feed is main-
tained below the ionization constant (pKa
) of the lactic acid to
obtain high selectivity.
Several different ion exchangers such as IRA-400, PVP,
and IRA-92, Amberlite were tested. IRA-92, a weakly basic
exchanger, is selected as the ion exchanger for the purification
of lactic acid because of its fair purity and recovery yield of
lactic acid comparable with other resins results.
Tong et al. [80], examined the capacity of IRA-92 to lactic
acid in the fermentation broth, and then, optimized the operating
conditions, and finally gained a fair product of lactic acid with a
higher purity, recovery yield and productivity with only one-step
chromatographic procedure from the supernatant of the fermen-
tation broth. The experimental results demonstrate that when the
Fig. 1. The mechanism of adsorption of lactic acid on the anion exchange resin.
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10 H.G. Joglekar et al. / Separation and Purification Technology 52 (2006) 117
pH of the fermentation broth is 6.0, the recovery yield, purity
and productivity in the lactic acid purification are the highest.
With the decrease of the sample volume loaded and of flow rate,
the recovery yield and the purity are improved but the productiv-
ity apparently reduced. In the experimental scale, the scale-up
of purification process exhibits little influence on the recovery
yield and the purity. Under the preliminary optimal conditions,
the yield, purity and specific productivity are 82.6%, 96.2% and
1.16 g LA/(g-resin day), respectively.
Raya-Tonetti et al. [81], studied the use of strong anionic
exchange resin (IRA-400) to recover lactic acid directly from
fermentation in an upflow fluidized bed column, resulting in
0.18 g lactic acid/g resin bound with a subsequent elution of
94%. When the culture broth was heated and adjusted pH to 8.0,
0.4 g lactic acid was bound per gram of resin, with a subsequent
elution of 90%. l (+) and d () lactic acid isomers distribution
was analyzed in the elution product resulting in an increase of
l (+) isomer concentration. The resin did not alter its bindingcapacity even after 23 cycles. The lactic acid recovery attained
was not dependent on the increase of the resin poured to the
columns but due to the increase in the hydraulic residence time
and back mixing which resulted in a high contact time between
lactate ions and resin particles.
Srivastava et al. [64], separated lactic acid by using IRA-
400 column coupled with fermentor. This study was focused on
improving fermentation yield, and the separation performance
of IRA-400 was not studied. The Amberlite IRA-400 resin has
proper pore size and high adsorption capacity for recovery of
lactic acid and it can adsorb lactic acid in wide pH range.
Cao, et al. [65], studied the application of Amberlite IRA-
400 anion exchange resin for the recovery ofl-(+)-lactic acid
from fermentation broth. Adsorption isotherm and breakthrough
curves for the separation of (l+)-lactic acid were obtained at pH
5.0 and 2.0, respectively. Recovery experiment coupled with
fermentor was carried out successfully by using a column with-
out autoclaving. Different types of adsorption isotherms were
found at pH above and below the pKa (3.86) of lactic acid. The
isotherm was found to be a Langmuir type at pH 5.0, whereas the
isotherm was type II (multilayer adsorption) at pH 2.0. At pH 5.0,
the maximum adsorption capacity of the resin, and dissociation
constant, were 222.46 mg/g wet resin and 60.7 mg/ml, respec-
tively. Breakthrough curve for the separation of lactic acid from
fermentation broth was also obtained. The maximum adsorptioncapacity (197.09 mg/g wet resin) at pH 5.0 was much higher
than that at pH 2.0 (106 mg/g wet resin). Proper elution and
washing conditions were sought by using H2SO4, methanol,
ammonia or their mixtures as eluant. When column separa-
tion was performed at pH 5.0 by using 50% (v/v) methanol
as washing solvent and 1.0 M H2SO4 as eluant, the total yield
was 86.21%. However, the total yield was 92.11% when the col-
umn separation was performed at pH 2.0 and water was used as
eluant.
IRA-400 was successfully applied for the separation of (l+)-
lactic acid from fermentation broth at pH above and below the
pKa (3.86). It shows different adsorption mechanisms in the sep-aration of lactic acid at pH above and below pKa. 1.0 M H2SO4could be used for the elution of lactic acid at pH 5.0 with high
recovery. Product loss in column washing step could be reduced
using methanol. The process is simple and feasible in lactic acid
industry and could be coupled with fermentation.
Salts ions in fermentation broth and inorganic acids used for
adjustment of pH did not affect the adsorption performance of
resin for lactic acid at pH 2.0. The elution of the IRA-400 anion
exchange resin could be easily performed using water as eluant.
Ionic exchange resins have been utilized by Vaccari, et al.
[82], Senthuran et al. [83] and Kaufman [84], obtaining 0.1, 0.18
and 0.2 g lactic acid/g resin, respectively. All purification tech-
niques mentioned earlier, need prior cell removal by filtration
or by centrifugation. Those steps mean increase in equipment
and energy costs, increase in total process time, and reduction
in total yield.
Lactic acid was recovered and purified by using a fluidized
bed column refilled with a strong anionic exchange resin:
Amberlite IRA-400 achieving 0.126 g LA/g resin [85]. This
methodology is more useful considering the fact that only con-trolling the ascensional velocity is sufficient to washout the
biological solids and to bind the lactate to the resin in only
one step. A very important advantage that this technique counts
with is the use of simple equipment, such as a glass column,
an anionic exchange resin, a peristaltic pump, and commercial
grade reagents, to carry out the early recovery process of lactic
acid from the culture [86].
Sosa, et al. [87], studied the influence of two design parame-
ters, bed-diameter (D) and bed-height (H), on lactic acid binding
capacity utilizing fluidized bed columns refilled with anionic
exchange resin. The binding capacity of the resin was constant
during the lactic acid downstream process when the columns
were scaled-up on diameter, keeping constant the bed height.
Substantial increase (50%) in lactic acid adsorption to Amberlite
IRA-400 was achieved in the case of scaling up the H parameter
maintaining the diameter of the columns constant.
The same ratio of grams of lactic acid to grams of resin was
fed to both columns in all experiments. Thus, the lactic acid
recovery attained was not dependent on the increase of the resin
poured to the columns but due to the increase in the hydraulic
residence time and back mixing which resulted in a high contact
time between lactate ions and resin particles. By changing the
settled bed height from 2.5 to 5cm for each diameter of column
analyzed, it was possible to obtain 50% increase in the binding
capacity of the resin in all experiments. This fact was attributedto a higher contact time between theculture broth andthe anionic
resin produced by the increase in back mixing and lactic acid
residence time.
There is a further need to study the effect of other parameters
on the performance of lactic acid purification process utilizing
fluidized bed columns, taking into account the developing of this
procedure on larger scale.
The uptake data for lactic acid with all three sorbents (Dowex
MWA-1, Reillex 425, Amberlite IRA-35) are well described by
1:1 complexation [88], which gives a functional form equivalent
to the Langmuir equation.
Qca
Qm=
KCa,f
(1+KCa,f), (4)
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H.G. Joglekar et al. / Separation and Purification Technology 52 (2006) 117 11
where Qca is thecomposite uptake of lacticacid (g of lacticacid/g
of sorbent); Qm the maximum value of sorbed lactic acid at high
concentration (g of lactic acid/g of sorbent); Ca,f the weight
fraction of lactic acid in the final solution; K the complexation
constant for sorption (g of resin/g of lactic acid).
Daietal. [89], has found that the uptakeof lacticacidfor sorp-
tion by Dowex MWA-1 is much higher than that for extraction
by Alamine 336. This advantage is more significant in the higher
pH range. On the other hand, the uptake capacity for water is
much higher for sorption than for extraction, and this results in a
substantially higher uptake of glucose onto the sorbent. Marked
swelling of the sorbent in the solution reduces the selectivities
for acid over water and glucose.
Sun et al. [90] demonstrated that the in situ product removal
process using the OH-form anion-exchange resin can be suc-
cessfully carried out for lactic acid fermentation. Both in the
shaking flasks and in the airlift bioreactor (ALB), the broth pH
was controlled at values higher than 6, and over 90% of the lacticacid produced by the bioconversion was recovered by the anion
exchanger. In addition, the mathematical model developed for
the in situ product removal (ISPR) process agreed well with the
experimental results.
3.2. Choice of adsorption
Adsorption or theion exchangeis a reliable technology. How-
ever, the process requires regeneration of an ion exchange resin
and adjustment of the feed pH to increase the sorption efficiency,
requiring large amounts of chemicals and needs to treat and dis-
pose of large quantities of salts/effluents.
Adsorption on ion exchange resin has the advantage that it
can be coupled with fermentation process. For lactic acid fer-
mentations, the sorbent should demonstrate substantial uptake
in the pH range of 56.
The uptake of lactic acid for sorption by Dowex MWA-
1 is much higher than that for extraction by Alamine 336.
This advantage is more significant in the higher pH range.
The capacity of IRA-92 to sorb lactic acid in the fermenta-
tion broth, at optimized operation conditions, is high with a
higher purity and recovery yield with only one-step chromato-
graphic procedure from the supernatant of the fermentation
broth.
The isotherm was found to be a Langmuir type at pH 5.0,whereas the isotherm was type II (multilayer adsorption) at pH
2.0. At pH 5.0, the maximum adsorption capacity of the resin,
qm and dissociation constant, Kd were 222.46 mg/g wet resin
and 60.7 mg/ml, respectively for recovery of l (+)-lactic acid
from fermentation broth using Amberlite IRA-400. The maxi-
mum adsorption capacity (197.09mg/g wet resin) at pH 5.0 was
much higher than that at pH 2.0 (106 mg/g wet resin). Proper
elution and washing conditions were sought by using H2SO4,
methanol, ammonia or their mixtures as eluant. When column
separation was performedat pH 5.0by using 50%(v/v) methanol
as washing solvent and 1.0 M H2SO4 as eluant, the total yield
was 86.21%. However, the total yield was 92.11% when the col-umn separation was performed at pH 2.0 and water was used as
eluant.
The Amberlite IRA-400 resin has proper pore size and high
adsorption capacity for recovery of lactic acid and it can adsorb
lactic acid in wide pH range.
To recover lactic acid from fermentation broth the most suit-
able adsorbent is found to be Amberlite IRA-400 resin with
methanol and 1.0 M H2SO4 as eluant. It has high adsorption
capacity to adsorb lactic acid in wide pH range. The elution
by methanol and 1.0 M H2SO4 is also advantageous to directly
esterify the recovered lactic acid in methanol. Thereby avoiding
the addition of alcohol and acid catalyst during esterification
to purify the lactic acid. Further purification by esterification
is necessary after adsorption, as it does not remove all other
organic acids.
4. Electrodialysis
Electrodialysis is one of very promising and perspective
methods provided by rapid development of the membrane pro-cesses, especially the membranes in the 80s and 90s [91].
Electrodialysis fermentation EDF is also studied by several
authors [9295]. Electrodialysis fermentation (EDF) is promis-
ing because it can remove product lactic acid continuously from
the fermentation and maintain the pH of the broth.
Most of the literature [9599], shows the feasible produc-
tion of lactic acid from lactate salts in two steps: conven-
tional electrodialysis (ED) for concentration and purification
and bipolar electrodialysis for conversion of lactate salts into
lactic acids with recovery of alkali. Bipolar membrane elec-
trodialysis also referred to as water splitting electrodialysis,
can convert aqueous salt solutions into acids. A water split-
ting stack is similar to a conventional (mono-polar) electro-
dialysis stack but incorporates a third type of membrane, the
bi-polar membrane, which is composed of a cation and anion
membrane layers laminated together. To meet the feed require-
ments of EDBM, clarification of the fermentation broth is first
performed by microfiltration. After the conversion of sodium
lactate into lactic acid, the product is purified by ion exchange
resins.
4.1. Reported research
Hongo et al. [91], proposed to use electrodialysis for in
situ lactate recovery to reduce the product inhibition. The mainobservation was fouling of anion exchange membranes by cells
in the electrodialysis fermentation(EDF). To solve this problem,
Nomura et al. [100], used immobilized growing cells entrapped
in calcium alginate. Theamount of lactic acid produced by semi-
continuous electrodialysis fermentation using immobilized cells
was eight-times higher than that produced by non-pH controlled
fermentation, but some free cells were found in the solution.
Czytko et al. [93], found that the electrodialysis unit could only
be operated with cell free solutions in order to prevent deposi-
tion of bacteria on the membranes. To increase the productivity
of the lactic acid fermentation and to reduce the amounts of
effluents, Boyaval et al. [94] combined the cell recycle systemwith electrodialysis and obtained a lactic acid concentration of
85 g l h and a productivity of 22g l h. Siebold et al. [95], showed
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12 H.G. Joglekar et al. / Separation and Purification Technology 52 (2006) 117
that lactic acid production with in situ electrodialysis without
ultrafiltratioon is also possible.
The two-stage electrodialysis method was described by
Glassner et al. [101]. Madzingaidzo et al. [96], presented a pro-
cess for sodium lactate purification by mono-polar electrodialy-
sis and recoveryof lactic acidby bi-polar electrodialysis. Sodium
lactate of feed concentration 125 g/l was concentrated by mono-
polar electrodialysis to a maximum of 150 g/l. A low incidence
of impurities was observed in the concentrated solutions with
less than 2 g/l glucose and 1.5g/l acetate detected. Bipolar elec-
trodialysis unit yielded 160 g/l free lactic acid while color and
otherchemicalimpuritieswere significantly reduced. The lactate
solution is passed through the bipolar electrodialysis unit to get
free lactic acid. Additional bleaching and de-ionization process
steps are followed to polish the free lactic acid for high-grade
applications.
Rathin Datta et al. [97], studied the various advantages of
bipolar electrodialysis to eliminate the salt or gypsum wasteproduced in the conventional processes in large scale lactic acid
production processes.
M. Bailly, et al. [102] suggested a complete production
scheme, targeted around membrane operations for clarification,
concentration and conversion. The fermentation broth is first
clarified by cross flow microfiltration. Divalent cations, that con-
stitute a poison in the configuration used, are then removed from
the clarified broth. Conventional electrodialysis (ED) is further
used prior to EDBM in order to increase the concentration of
ionic species, comprising the organic acid salt. In this manner,
the area of bipolar membrane required for the conversion is low-
ered so that the economical profitability of the EDBM step is
improved.
As described by Mathieu Bailly [98], electrodialysis with
bipolar membranes (EDBM) is used to prepare polymer grade
lactic acid. The process has to be simultaneously economically
attractive and have a low impact on the environment. In this con-
text, this article details the performance and cost related to an
industrial EDBM plant operated for the production of organic
acids. Over the past 15 years, not more than 12 commercial
plants totaling about 2400 m2 of Aqualytics and Tokuyamas
bipolar membranes have been installed throughout the world
for different chemicals. A complete downstream (from the fer-
mentation) process based on combined electrodialysis steps for
purification/concentrationand conversion is proposed in the caseof lactic acid.
Finally Bailly describes performances of a plant with a pro-
duction capacity 5000 tonnesof lactic acid peryear which makes
use of a two-stage electrodialysis process. An electricity con-
sumption of 1.8 kW/kg of produced acid is reported.
Habova et al. [99], confirmed that the two-stage electrodial-
ysis is a suitable and efficient technique for recovery of lactate
ions from the pretreated fermentation broth and subsequent
conversion into lactic acid. The pretreament consisted of ultra-
filtration, decolourisation and removing of multivalent metal
ions.
Several authors have carried out studies to improve the eletro-dialysis fermentation (EDF) method. [103105]. But commer-
cialization of EDF process has not been reported.
Kang, et al. [106] described nanofiltration (NF) as an alter-
native to desalting electrodialysis (ED) and ion exchange for the
recovery of ammonium lactate from fermentation broth.
Li et al. [107], developed a laboratory scale bioreactor com-
bining conventional electrodialysis and bipolar membrane elec-
trodialysis for in situ product removal and pH control in lactic
acid fermentation. The electrokinetic process enabled removal
of the biocatalytic product (lactic acid) directly from the biore-
actor system, in a concentrated form, as well as enabling good
pH control without generation of troublesome salts.
4.2. Choice of electrodialysis
Electrodialysis has been reported for sodium or ammo-
nium lactate broth. Ammonium lactate is preferred as it uses a
cheaper alkali. An electrodialysis fermentation(EDF) is promis-
ing because it can remove produced lactic acid continuously
from the fermentation and maintain the pH of the broth [103].Commercial exploitation of electrodialysis with bipolar
membranes (EDBM) is reported by Mathieu Bailly [98]. Broth
needs to be micro filtered prior to electrodialysis. Monopolar
electrodialysis is used to concentrate and purify the broth. How-
ever the output is in the form of ammonium lactate. Further
bipolar electrodialyis can convert ammonium lactate to lactic
acid. Recovered ammonium hydroxide can be reused in fer-
mentation. Addition of ammonium hydroxide in fermentation
is advantageous as it improves productivity of microorganisms.
Thus downstream process route will involve microfiltration,
monopolar electrodialysis and bipolar electrodialysis. However
this process also does not separate out other organic acids from
lactic acid.
5. Esterification and reactive distillation
High purity lactic acid can be prepared by esterification of
crude lactic acid with alcohols, distillation of ester, hydroly-
sis of the distillated lactate ester to yield the alcohol and lactic
acid. Esterification is the only downstream process, which sep-
arates other organic acids from lactic acid. Esterification gives
esters of lactic acid and further hydrolysis of esters is neces-
sary to get the product as lactic acid. Simultaneous distillation
with esterificationhydrolysis is called reactive distillation. Fer-
mented broth containing lactic acid needs to be pretreated toremove some impurities before reactive distillation using resin
beds as catalyst as well as bed for distillation column.
5.1. Reported research
Smith and Claborn [108], described methods for the prepara-
tion of purified lactic esters from crude lactic acid obtained from
fermentation. To obtain high yields of the pure lactic esters with
alcohol containing less than four carbons, it is necessary to use
a large excess of alcohol during esterification and then rapidly
remove water with excess alcohol from the ester at low temper-
ature, preferably in vacuum with aid of an efficient fractionatingcolumn. Calcium lactate is dissolved in methanol and equiva-
lent amount of sulphuric acid is added to liberate the lactic acid
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H.G. Joglekar et al. / Separation and Purification Technology 52 (2006) 117 13
to precipitate and separate calcium sulphate. Lactic acid solu-
tion is heated for 48 h at refluxing temperature to complete the
esterification. Similarly method for preparation of lactic esters
insoluble in water was also presented.
Filachione and Fisher [109], described a method for purifi-
cation of lactic acid by preparation of methyl lactate from crude
aqueous lactic acid. The method comprises of passing methanol
vapor through aqueous lactic acid and condensing the efflu-
ent vapors. The condensate, a mixture of methanol, water and
methyl lactate, can be distilled to recover the methyl lactate and
hydrolyzed to obtain purified lactic acid.
Schopmeyer et al. [110], suggested heating an esterification
mixture of lactic acid (4060 wt.%), a relatively low boiling
aliphatic alcohol, and an acidic catalyst (sulphuricacid) for ester-
ifiation in a jacketed kettle. The vapors from the esterification
kettle are continuously fed to a fractionating column, which may
contain alcohol, ester and water. Continuous hydrolysis of ester
in a fractionating column is done at atmospheric pressure. Alco-hol produced by hydrolysis is removed fromthe top and returned
to esterification kettle, and lactic acid along with water is drawn
from the bottom.
Recently reactive distillation has drawn considerable atten-
tion because of its striking advantages, especially for
equilibrium-limited reactions. Purification of lactic acid through
reactive batch distillation was investigated by several investi-
gators [111113]. The experimental setup used by the authors
consisted of two columns for separation of reactants from the
product and two reboilers for esterification reaction and hydrol-
ysis reaction. The feed consisted of only 1020% lactic acid by
weight.
Choi et al. [114], studied batch distillation of lactic acid with
simultaneous reactions. Lactic acid was reacted with methanol,
and methyl lactate was produced by the esterification reaction in
presence of cation exchange resin (Dowex 50W). The volatile
methyl lactate was distilledsimultaneouslywith hydrolysisreac-
tion forming lactic acid. To recover pure lactic acid through two
reactions and distillation, batch distillation system consisting of
two condensers, feed vessel, and reboiler was used. The yield of
recovered lactic acid was as high as 95%. When impure lactic
acid solution obtained from bacterial fermentation was used as
feed, highly pure lactic solution was obtained with yield of 92%
in reboiler.
Seo et al. [111], studied the feasibility of recovery of lacticacid by two batch reactive distillations using cation exchange
resin (Dowex 50 W) as a catalyst and glass packed column.
For the recovery of lactic acid, two reactions, esterification and
hydrolysis, are involved and hence, an apparatus with two dis-
tillation columns was developed and operated in a batch mode
to ensure enough residence time in the reboiler and column. The
effects of operating variables such as catalyst loading, mole ratio
of lactic acid to methanol, feed concentration, type of alcohols
and partial condenser temperature on yield were studied. The
reaction products of the esterification (methyl lactate and water)
were distilled to the hydrolysis part to recover into pure lactic
acid. The yield of lactic acid increased as catalyst loading in theesterification part was increased. The decrease in mole ratio of
lactic acid to methanol, and lactic acid feed also improved the
yield of lactic acid. Methanol as a reactant gave higher yield
than any other alcohol. The yield of lactic acid was as high as
90%.
Kim et al. [112], also carried out similar studies using Old-
ershaw columns and reboilers for fractionation and reactions.
Concentration and temperature profiles in the reboilers and on
each stage were investigated throughout the operation. Six hour
operating time was required for getting high purity lactic acid.
The effect of columns on the recovery yield was investigated.
The column improved the fractionation of the boilups from the
reboilers. More effective fractionation in columns allowed vapor
streamin columns to contain more methanol and liquid streamto
contain less methanol. Thereby, methanol-concentrated recycle
flow was obtained more effectively and methanol was prevented
to remain in hydrolysis part. That resulted in the more effective
reaction in both reboilers and improved the yield.
Kim et al. [113], studied reactive batch distillation similar to
Kim et al. [112]. Methanol recycle and feeding method wereinvestigated as the factors, which could control the component
boilup rate of each species and rate of esterification reaction.
The temperature of partial condenser controlled the flow rate
and composition of methanol recycle stream. Semi batch oper-
ation was compared with batch operation. Continuous feeding
of methanol enhanced the recovery system performance while
continuous feeding of lactic acid aqueous solution, deteriorated
the recovery compared with batch operation.
In continuous esterification, the mixture of an aqueous solu-
tion of lactic acid to be purified, a relatively low boiling aliphatic
alcohol, and an acidic catalyst of esterification is heated to pro-
duce mixture of vapors. Use of sulphuric acid as catalyst may
result in traces of acid in the product. In presence of impurities
with cation exchange resin catalyst it may be difficult to main-
tain the operation at steady state. Therefore it may be necessary
to purify the crude lactic acid from impurities like residual sugar
and protein before hand.
The two column reactive distillation scheme studied by Seo
et al. [111], Kim et al. [112], Kim et al. [113], is for upto 30%
crude lactic acid feed. And the catalyst used for the studies for
both esterification and hydrolysis is cation exchange resin i.e.
DOWEX 50W. This scheme with feed of 5060% lactic acid
concentration may reduce the size of equipment.
The reported yield of the ester vary from about 60 to 100%,
depending largely upon the method used for removing the wateras it is formed during the esterification reaction. It is more dif-
ficult to obtain a high yield of ester with methyl or isopropyl
alcohol than with a long chain alcohol such as butyl, amyl,
acetyl, lauryl, and stearyl, because the lower alcohols and the
corresponding lactic esters are soluble in water. It is necessary,
therefore, to resort to other methods for removing this water or
reducing the ratio of water to alcohol in the reacting mixture by
using a large excess of alcohol.
Recently, Sun at al.[115], studied conversion of LA or ammo-
nium lactate (NH4LA) into esters and subsequent hydrolysis
of the purified ester into LA to obtain highly pure LA. In this
study, using two reactors with a rectifying column were used torecover LA from the fermentation broth. NH4LA obtained by
fermentation was used directly to produce butyl lactate by react-
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