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Crystallization of Salicylic Acid via Chemical Modification

Crystallization of Salicylic Acid via Chemical Modification


Source: Kerry M. Dooley and Michael G. Benton, Department of Chemical Engineering, Louisiana State University, Baton Rouge, LA

Processing of biochemicals involves unit operations such as crystallization, ultracentrifugation, membrane filtration, and preparative chromatography, all of which have in common the need to separate large from small molecules, or solid from liquid. Of these, crystallization is the most important from a tonnage standpoint. For that reason, it is commonly employed in the pharmaceutical, chemical and food processing industries. Important biochemical examples include chiral separations,1 purification of antibiotics,2 separation of amino acids from precursors,3 and many other pharmaceutical,4-5 food additive,6-7 and agrochemical purifications.8 The control of crystal morphology and size distribution is critical to process economics, as these factors affect the costs of downstream processing operations such as drying, filtration, and solids conveying. For more information about crystallization, consult a specialized textbook or a Unit Operations textbook.9

The crystallizer unit (Figure 1) enables study of: (a) the effects of key parameters, such as supersaturation and cooling/heating rates, on solids content, morphology and crystal size distribution; (b) and the on-line control of crystallization processes. Supersaturation can be controlled by altering conditions such as agitation rate and temperature. The different classifications of crystallization include cooling, evaporative, pH swing and chemical modification. In this experiment,an offline microscope will measure from crystals ranging in size from 10-1000 μm, a typical size range for biologicals.

Figure 1
Figure 1: P&ID schematic (left)and picture (right)of Crystallizer. Please click here to view a larger version of this figure.

This experiment will demonstrate a "chemical modification",or "pH-swing" crystallization, to generate salicylic acid (SAL) (precursor of aspirin) crystals from the rapid reaction of aqueous solutions of basic sodium salicylate (NaSAL), which are basic, and sulfuric acid (H2SO4) at anywhere from 40 - 80°C.11

Na+SAL + 0.5 H2SO4 SAL (ppt) + Na+ + 0.5 SO42-

The byproduct sodium sulfate remains soluble. The apparatus consists of two feed tanks, three variable speed (peristaltic) pumps, the crystallizer (stirred tank to approximate uniform temperature and concentration, ~5 L), a circulating bath for temperature control, power controller, product tank, and a makeup tank for feed regeneration with NaOH solution (if desired). Samples will be analyzed by a UV-Vis spectrometer for the residual soluble salicylate ion, and the salicylic acid crystal product will be dried and weighed.A pH probe can be used to determine steady-state when reaction conditions are altered.


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A mixed-suspension, mixed-product-removal (MSMPR) crystallizer is analogous to a continuous stirred-tank reactor - perfect mixing of both solid and liquid phases is assumed. Industrial crystallizers seldom (if ever) approach MSMPR behavior, but the concept is useful in bench- and pilot-scale units. This is because it provides an easy way to estimate key parameters such as growth rate, G, and nucleation rate, B0. Both existing crystals and other solid surfaces, such as the agitator, catalyze nucleation. The number density, n, of the crystals is a probability density with respect to L, the primary crystal dimension. Therefore, n dL/(Σn dL) represents the fraction of crystals oflength L to L+dL. In standard texts it is shown that for an MSMPR crystallizer, the solution of the general population balance model for n is:

Equation 1 (1)

where B0 is the crystalnucleation function in mols/vol/time, and G is the growth rate of crystals, dL/dt. Equation (1) predicts an exponential distribution for the number density produced in an MSMPR. Using the zeroth (related to crystal concentration) and first (related to crystal average size) moments of the distribution, B0 and G are:

Equation 2  (2)
Equation 3  (3)

where Cs is the concentration of solid crystals in the slurry, τ is residence time, which is approximately the liquid volume divided by the feed volumetric flow rate, and Equation 4 is the average length on a number basis, which is determined microscopically.

Therefore, for an MSMPR crystallizer, the growth and nucleation rates are determined by the normal control parameters (agitation rate, temperature, flow rates, etc.). However, the distribution should always be exponential, and any deviations from an exponential distribution represent imperfect mixing of either the solids or the liquid. The MSMPR (stirred tank) crystallizer is poorly suited to industrial crystallizations because it provides an exponential distribution of crystal sizes, whereas in most applications a relatively narrow, Gaussian, distribution is desired for product uniformity.Its study is relevant because: (a) it is almost always an element of a larger crystallizer design; (b) it is ideally suited for bench-scale and pilot-plant work because the degree of supersaturation and growth and nucleation rates can easily be extracted from the raw data; and (c) it is the easiest example for which geometry can be linked to crystal size distribution.

For constant temperature and agitator speed, both B0 and G are directly related to the supersaturation ΔC, which is the mass transfer driving force for crystallization:12

Equation 5 (4)

The powers b and g are system specific and can vary over a wide range (e.g., 1-7.2 for g).12

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Organic (sodium salicylate, NaSAL) and acid (sulfuric acid, 0.25 M = 0.50 N) solutions will be fed to the crystallizer. Make sure to wear latex gloves when handling NaSAL, salicylic acid or their solutions, and the 0.25 M sulfuric acid.

The entire system is controlled from a PC using a commercial distributed controller with an interface similar to the one in Figure 1. All on-off or 3-way solenoid valves and controller set points can be operated and changed using this interface. A schematic shows trends of the analog values (flow rates, temperature) associated with the unit.

1. Starting up the Crystallizer

At the start of a run, all continuous controllers should be in manual mode, and all solenoid valves should be either closed (on-off) or in recycle (3-way) mode.

  1. Be sure the crystallizer is full to the overflow level, (~4.15 L) indicated on the stirred tank, with water and salicylic acid slurry (in crystallization, the slurry is often called "magma"). If not full, add these through the addition port.
  2. Turn on the agitator for the crystallizer and thethermostated for the bath and pumps.
  3. Set the temperature controller for the bath temperature to AUTO and the setpoint to the desired temperature. The recommended temperature is ~53°C for a 50°C crystallizer.
  4. Set the pump speeds using the interface (e.g., 30% open). Knowing the concentrations of the feeds, set the flow rates for stoichiometric equivalence based on Equation (1).
  5. Confirm that the product tank is not full and that the drain valve is closed.
  6. Power up the spectrometer equipment and establish communication with a link provided in the control console. Spectrometer procedures are detailed in the operating manual (SpectraSuite). Calibration of the spectrometer is provided.

2. Operating the Crystallizer

  1. Raise the pump output as necessary to achieve the desired flow rates. For the acid solution, this is ~25-35 mL/min. For the NaSAL, it is determined by stoichiometric equivalence.
  2. Switch to feed mode on both 3-way valves. This is time zero for an experiment.
  3. Periodically check the overflow line. Under certain conditions it may block up. If so, use a piece of steel tubing to ream out the line entering the product tank.
  4. Collect five samples directly from the crystallizer through the sample port using a wide-mouth pipette and transfer them to 15 mL test or centrifuge tubes. Take two sets of samples about 10-15 min apart.
  5. Repeat at two other widely-spaced residence times, controlling tau (residence time) by varying the volumetric flow rates, but maintaining stoichiometric equivalence.

3. Shutting Down the Crystallizer

  1. To shut down the system, set the 3-way valves to recycle and the pump outputs to 0 %.
  2. Return the temperature controller to MANUAL at 0% output, and shut off the pumps, agitators and thermostated bath.
  3. If using the spectrophotometer, remember to shut off the lamps.

4. Analysis

Dissolved NaSAL and salicylic acid concentrations can be measured simultaneously by UV/Vis spectroscopy.The absorbances of dissolved salicylate and salicylic acid can be assumed additive because the same chromophore is observed. Further instructions are included in Appendix A. The salicylic acid concentration can also be determined gravimetrically in units of kg/m3 slurry.

  1. Centrifuge the 15 mL tubes for 5 min and record the volume of liquid sample retrieved by decanting. The decanted liquid can be used for NaSAL spectrophotometric analysis.
  2. Dry the test tubes containing the solids upright in the convection oven at 70ºC, for two days.
  3. Weigh, clean out the tubes, then re-dry briefly before re-weighing to get the weight of the crystals.

Industrial crystallization is applied for the separation and purification of compounds and mixtures. In order to design economical systems, various parameters have to be studied. Crystallization is used for the separation of chiral compounds and amino acids, or for purification of antibiotics, food additives and agrochemical compounds. Different means of crystallization include cooling, chemical modification, evaporation or pH swing. A crystallizer can be used to investigate key parameters affecting crystal development, such as cooling and rates or supersaturation. With the microscope, the crystal size and morphology can be monitored and dependencies of various factors observed. In this experiment, sodium salicylate is reacted with sulfuric acid, leading to precipitation of salicylic acid, which is a precursor of Aspirin. Samples are analyzed by UV vis, a gravimetric analysis and microscopy. This video will illustrate the concept, analysis and application of a crystallizer unit.

For a scale up of a crystallizer, it is important to estimate key parameters. These can be studied using an MSMPR unit. Although industrial crystallizers really behave like MSMPRs, the concept is still relevant for bench and pilot scale units. The MSMPR crystallizer is analogous to a continuous, stirred-tank reactor. It assumes perfect mixing of solid and liquid phases. MSMPRs are used to assess key crystallization parameters, such as the crystal nucleation rate, which is also known as the birth function and the crystal growth rate. The nucleation is catalyzed by existing crystals and solid surfaces such as the walls of the reactor. The general population balance model for a MSMPR crystallizer yields the number density N of the crystals, which is a probability density with respect to L, the primary crystal dimension. In an MSMPR, the number distribution is predicted to be an exponential distribution. The birth function and growth rate can be determined using the zeroth and first moments of this distribution. Most importantly, they can also be related to the supersaturation, which is the mass transfer driving force in crystallization, and which is, in turn, dependent on agitation rate and temperature. For a constant temperature and agitator speed, both the birth function and growth rate are directly related to supersaturation, and the powers B and G can be determined by linear regression. According to the MSMPR model, the number density of crystals decreases exponentially with length. A deviation from the exponential distribution would imply imperfect mixing of solids or liquids. In industrial applications, relatively narrow Gaussian distributions of crystal sizes are required, rather than exponential ones. Nevertheless, the MSMPR model is still useful, particularly in pilot plants, as it enables determination of growth and birth rates as well as the degree of supersaturation from raw data. Now that you are familiar with the MSMPR model, let's apply the concept to the experiment.

Wear proper PPE when handling sodium salicylate and sulfuric acid solutions. Write down the basic physical properties of the salicylic acid for later use. Before your start, familiarize yourself with the crystallization system. The apparatus consists of two feed tanks, variable speed pumps, a five liter crystallizer-stirred tank, a circulating bath for temperature control, power controller, product tank and a make-up tank for feed regeneration, using a sodium hydroxide solution. The system is operated using a distributed control system and a graphical interface, from which valves can be operated to control the temperature and flow. A schematic output providing trends of flow rate and temperature is also available.

Check that all continuous controllers are set to the manual mode, and that all solenoid valves are either in the closed, two-way or in the recycle, three-way mode. Make sure the crystallizer is full with water and some salicylic acid slurry to the overflow level of approximately 4.15 liters, as indicated on the stirred tank. Add water and salicylic acid using the addition port if tank is not full. Turn on the agitator for the crystallizer and the thermostated bath and pumps. Set the temperature controller for the bath temperature to auto, and the set point to the desired temperature, usually approximately 53 degrees Celsius for a 50 degree Celsius crystallizer. Set the pump speeds to give approximately 25 to 35 milliliters per minute for the acid solution. For the sodium salicylate, the flow rate is determined by stoichiometric equivalents. Using the known feed concentrations, set the flow rates for stoichiometric equivalents. Make sure that the product tank is not full and the drain valve is closed. Then, turn on the spectrometer, and use a provided link in the control console to check that communication between the apparatus is established.

Switch to feed mode on both three-way valves. This sets time zero for an experiment. Periodically check the overflow line for any blockage. Use a piece of steel tubing to remote the line entering the product tank using the hole provided if blockage is detected. After one hour, use a wide-mouthed pipette and insert it into the sample port of the crystallizer. Collect enough sample to fill enough five pre-weighed 15 milliliter centrifuge or test tubes. Take two sets of samples 10 to 15 minutes apart. Vary the volumetric flow rates to control TOW and adjust for two other widely-spaced residence times. Maintain the stoichiometric equivalents and collect samples as before. When finished, set the pump output to zero per cent, the three-way valves to recycle. Return the temperature controller to manual at zero per cent output and shut off the pumps, agitators and thermostated bath.

The salicylate ion concentration can be determined using UV vis and the solid salicylic acid concentration can be determined gravimetrically as kilograms per meter cubed slurry. Before the analysis, first centrifuge samples for five minutes and decant the liquid. Record the total volume of sample retrieved. Combine the liquid samples from a given set and dilute by 50 to 100 times. For the liquid, measure the absorbance of the sodium salicylate and the salicylic acid using the UV vis spectrometer. The absorbance is assumed to be additive, since the same chromophore is detected for both samples. For the gravimetric determination, use the solids remaining in the centrifuge or test tubes. Dry the tubes upright in the convection oven at 70 degrees Celsius for two days. Then reweigh the cooled test tubes to determine the weight of the crystals and the concentration in kilograms per liter. Lastly, using a microscope, determine the length distribution of the needle-shaped salicylic acid crystals.

Compute the solid crystal concentration for all runs via the gravimetric method. Generate a mass balance on salicylate. Then, calculate the supersaturation and residence time. Next, determine the crystal yields on a feed and product basis, using the moles of the product, feed, and the dissolved salicylate product. Use the crystal concentration, crystal dimension, and residence time to solve for the birth function and growth rate. Then estimate the powers G and B through linear regressions of the log functions. Here is an example of a crystallization at 50 degrees Celsius. The power of B is twice as large as G, indicating that supersaturation is affecting the birth rate more than the growth rate. These powers would be used for scale up if supersaturation is unchanged. Comparisons to other experiments can identify factors that influence the growth and birth functions, such as inadequate mixing, pH and ionic impurities in the make up water.

Industrial crystallization is widely applied in pharmaceutical, chemical and food-processing industries for separation and purification of various compounds. Danazol is synthetic steroid which is used for the treatment of endometriosis. As with many other pharmaceutical compounds, Danazol is hydrophobic and poorly soluble in water. Therefore, the raw Danazol product is initially dissolved in ethanol and then recrystallized by mixing it with some water, which produces pure, small particle sized product crystals. Industrialized crystallizers can be used in the production of lysosomes. The apparatus can be designed to produce a very narrow crystal sized distribution through the application of a pump around heat exchanger, which slightly raises the temperature to dissolve the smallest crystals. The size distribution can be regulated by separating the crystal particles on the basis of their terminal velocities. This concept also finds application in the crystallization of inorganic salts.

You've just watched Jove's introduction to industrial crystallization. You should now understand the MSMPR crystallizer model, how to operate the crystallization unit and how to analyze the results. Thanks for watching.

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Figure 2 presents representative data that suggests modest deviations from the crystal size distribution of the MSMPR ideal even at relatively high speeds and low feed concentrations.

Figure 2
Figure 2. Crystal size distribution for 0.16 M NaSAL feed, 540 rpm, 60 ° C

The crystals that form from this experiment are typically needle shaped, and the length distribution can be determined microscopically. Sample lengths with size dimensions (in microns) of typical crystals are shown in Figure 3. The normal and preferred range of crystals is 100-1000 microns.

Figure 3
Figure 3. Magnified salicylic acid crystals. The sizes are in microns. Please click here to view a larger version of this figure.

Assuming the equations of the MSMPR crystallizer (1-4), and using a mass balance on salicylate, runs the concentration of solid crystals in the magma (CSAL), the residence times (τ), growth rate functions G, amounts of supersaturation in the aqueous phase ΔC on a molar basis, nucleation function B0, and the crystal yields on both a product and a feed basis were determined. The G-function was computed from Equation (3) using the size distribution. And the supersaturation and mass balance equations are:

Equation 6 (5)

Equation 7 (6)

where Q1 is the volumetric flow rate of the NaSAL solution, Qt is total volumetric flow rate, (CNaSAL)0 is the feed concentration of NaSAL in Q1, and CNaSAL and CSAL are the product concentrations of soluble salicylate and crystals, respectively. Ceq is the equilibrium (interfacial) concentration of salicylate, which was ~2.2 g/L over the temperature range used in this demonstration.

The yield was defined on a feed basis as:

Equation 8 (7)

And on a product-only basis as:

Equation 9 (8)

If the % error in the mass balance on salicylate is large, then it is likely that either CSAL or CNaSAL are in error, as both are difficult to measure accurately. By looking at the values of Y1 and Y2 (at which gives a more reasonable trend), the primary source of the error can be determined.

From the values for G and B0, the powers "g" and "b" in Equation (4) were estimated using linear regression. Franck et al. reports a power "g" of ~3 and "b" of ~6 for this system11 using highly sterile conditions and high agitator speeds. Determining the differences between the experimental powers "g" and "b" and those of Franck et al. is useful in identifying factors that might be influencing the growth and nucleation functions. Representative data for a 50°C crystallization with feed concentrations of 0.35 M (NaSAL) and 0.25 M (H2SO4) are shown in Table 1.

Table 1. Crystallization Data

Flow rate, mL/min τ Equation 4 CNaSAL CSAL Y1 Y2
NaSAL H2SO4 min mm mol/L g/mL % %
119 59.5 23.3 700 0.063 0.022 69 72
85 42.5 32.6 876 0.059 0.026 81 76
51 25.5 54.3 1190 0.055 0.026 81 77

These data were also used to solve for G and B0 and linear regression was performed to determine the powers "g" and "b" using the linearized Equation (4). Linear regression of the log functions (an example is shown in Figure 4) gave g = 1.1 and b = 2.4. While the trend in the powers (b about twice as large as g) was the same as observed in Franck et al., the powers themselves differed significantly, and the dependences on supersaturation ΔC were much smaller. This suggests that factors other than ΔC could be affecting the growth and nucleation rates, such as inadequate mixing, the relatively high pH's (for equimolar feeds the pH's are between 2.2-2.4), and ionic impurities introduced in the water (the municipal supply). These experimental powers would be used in any scale-up calculations, because other than ΔC, these factors would presumably be present in both the pilot-scale and industrial designs.

Figure 4

Figure 4. Linear regression of growth rate G as a function of supersaturation ΔC

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Applications and Summary

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This experiment demonstrated how to take raw concentration, flow and temperature measurements and use MSMPR theory to estimate the key parameters needed to design a large, complex crystallizer system. The critical role that residence time plays in obtaining high crystal yields and in controlling the average size of the crystals, was explored. Often there is an optimal residence time because very large crystals are seldom desirable. The same is true for mixing - mixing must be sufficient to keep the solid crystals from settling to the bottom, but at the same time the agitator speed is often a significant operating cost.

Some of the problems often experienced with this unit - partial blockages due to particle agglomeration, difficulties in obtaining uniform supersaturation due to imperfect mixing, and long times to reach steady state - are common to even well designed industrial crystallizers. This is why crystallizer designs seen in the manufacturers' literature are often amazingly complex.

This process is similar to crystallizations of other biologicals, such as L-ornithine-L-aspartate, which is used to treat chronic liver failure.5 The precursor L-ornithine hydrochloride costs >$300/kg and is difficult to recycle, so design for high crystal yields is critical. An example of an antisolvent, as opposed to pH-swing, biological crystallization is the refinement of danazol, a synthetic steroid used to treat endometriosis.13 Many drugs are hydrophobic with poor solubility in water. By dissolving the raw danazol product in ethanol and then re-crystallizing it by mixing with water, a purer and smaller particle size crystal product can be obtained. Crystallization of proteins is another important application, one example being lysozyme production.14

Industrial crystallizers can be designed to produce very narrow crystal size distributions through the application of fines removal (e.g., a pumparound heat exchanger that slightly raises temperature to dissolve the smallest crystals) and size classification (e.g., an "elutriation leg" that separates particles on the basis of their terminal velocities, collecting only the largest in the population). These design concepts were developed for inorganic salt crystallization but are now moving into the biological realm.

Materials List

Name Company Catalog Number Comments
Agitator, 150 W Caframo BDC 3030 on reactor
Circulating heater Neslab RTE 110 0-100°C, for reactor
Peristaltic pumps (2) Cole-Parmer Masterflex L/S 7550-60, 1.6-100 rpm, 0.1 hp For both NaSAL and H2SO4 feeds
Centrifugal pump Cole-Parmer 7553-00, 6-600 rpm For product recycle
UV-Vis spectrophotometer Ocean Optics USB 2000 For soluble NaSAL analysis
UV-Vis power supply Ocean Optics DT1000 CE For use with USB 2000


  1. Open the SpectraSuite software. Switch on both the UV and VIS lamps on the source. Be sure to turn the lamps off after using. Set the acquisition mode to Scope (blue S button on toolbar).
  2. On the toolbar change the Integration Time to 250 ms, the Scans to Average to 25, and the Boxcar Width to 2. Check the boxes for Strobe/Lamp Enable, Electric Dark Correction, and Stray Light Correction.
  3. Prepare Dark Spectrum and Reference Spectrum files. The spectrometer requires the generation of a Dark Spectrum file and a Reference Spectrum file.
    1. Immerse the probe into a test tube filled with DI water.
    2. To create a Dark Spectrum file, unplug the probe from the light source (white box). The graph should nearly trace the x-axis. To save your newly created Dark Spectrum, click on the grey light bulb, then File -> Store -> Store Dark Spectrum.
    3. To create a Reference Spectrum file, plug the probe connection back into the light source. Some peaks should appear on the graph in SpectraSuite. To save this Reference Spectrum, click on the yellow light bulb, then File -> Store -> Store Reference Spectrum.
    4. If ANY settings are changed (e.g., Integration Time, etc.), both the Dark Spectrum and Reference Spectrum must be generated again.
    5. Switch from Scope to Absorbance (A) mode. For NaSAL solutions, the absorbance should be observed at ~300 - 330 nm.

Quantification is only possible if NaSAL/salicylic acid solutions follow the Beer-Lambert law (A is in the linear region). For the salicylate ion, this region is A < ~0.9 - 1. Given past results, this criterion suggests that NaSAL solutions MUST be diluted (with DI water) to 0.05 g/L or less for quantification. Then, the unknown solutions can be quantified by comparing to the absorbance of an appropriately diluted standard solution:

Equation 10

where C is concentration, A absorbance, “u” an unknown, and s a standard solution of NaSAL. Note that BOTH “u” and “s” must show absorbance inside the linear range.

In spectroscopy, the absorbance depends on two factors, the type of chemical and its concentration, and the path length in the fluid. Change the concentration by dilution.

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  1. C. Wibowo, L. OYoung and K.M. Ng, Chem. Eng. Prog., Jan. 2004, pp. 30-39.
  2. W.J. Genck, Chem. Eng. Prog., Oct. 2004, pp. 26-32.
  3. S. Takamatsu and D.D.Y. Ryu, Biotechnol. Bioeng., 32, 184-191 (1988).
  4. F. Wang and K.A. Berglund, Ind. Eng. Chem. Res., 39, 2101-2104 (2000).
  5. Y. Kim, S. Haam, Y.G. Shul, W.-S. Kim, J.K. Jung, H.-C. Eun and K.-K. Koo, Ind. Eng. Chem. Res., 42, 883-889 (2003).
  6. K. Hussain, G. Thorsen and D. Malthe-Sorenssen, Chem. Eng. Sci., 56, 2295-2304 (2001).
  7. H. Gron, A. Borissova and K.J. Roberts, Ind. Eng. Chem. Res., 42, 198-206 (2003).
  8. F. Lewiner, G. Fevotte, J.P. Klein and F. Puel, Ind. Eng. Chem. Res., 41, 1321-1328 (2002).
  9. For example:  W.L. McCabe, J.C. Smith, and P. Harriott, Unit Operations of Chemical Engineering, 7th Ed., McGraw-Hill, New York, 2005, Ch. 27, or C.J. Geankoplis, Transport Processes and Unit Operations, 3rd Ed., 1993, Ch. 12.
  10. P. Barrett, Chem. Eng. Prog., Aug. 2003, pp. 26-32.
  11. R. Franck, R. David, J. Villermaux and J.P. Klein, Chem. Eng. Sci., 43, 69-77 (1988).
  12. J. Garside, Chem. Eng. Sci., 40, 3-26 (1985).
  13. H. Zhao, J.-X. Wang, Qi-An Wang, J.-F. Chen and J. Yun, Ind. Eng. Chem. Res. 46, 8229-8235 (2007).
  14. J.S. Kwon, M. Nayhouse, G. Orkoulas and P.D. Christofides, Ind. Eng. Chem. Res., 53, 15538-15548 (2014).


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