Abstract
L-arabinose is widely used in food, medicine, chemistry, and biology fields; however, solubility and seeded metastable zone width (MSZW) of L-arabinose have not been reported in the literature. In this paper, solubility and MSZW of L-arabinose in aqueous solution were determined. Solubility of L-arabinose was measured in the range of 20-68 °C by a conventional equilibrium solubility method and quantitation was determined using the ion chromatography technique. Seeded MSZW was determined in the range of 51-73% by the calorimetric method. The effect of two salts (potassium chloride and calcium chloride) on the solubility and MSZW of L-arabinose were also evaluated. Results showed that both potassium chloride and calcium chloride increased the solubility of L-arabinose, and this increase was intensified with temperature rise. The MSZW of L-arabinose was not constant but a spread. Potassium chloride increased the MSZW of L-arabinose. However, the effect of calcium chloride on MSZW of L-arabinose was concentration dependent. Conclusion: the L-arabinose solubility increased with the increase in temperature, and both potassium chloride and calcium chloride increased the solubility of L-arabinose in aqueous solution. The seeded MSZW of L-arabinose is not a constant; it increases in the presence of potassium chloride and varies with the change in calcium chloride concentration.
sucrase; ion chromatography; potassium chloride; calcium chloride
1 Introduction
L-arabinose is a new functional low-caloric sugar with selective intestinal sucrase
inhibition effect (Seri et al., 1996Seri, K., Sanai, K., Matsuo, N., Kawakubo, K., Xue, C., & Inoue,
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Hygiene Research, 42(2), 295-297. PMid:23654110.). The taste of L-arabinose is quite similar to that of
sucrose, with approximately 50% the sweetness of sucrose. It can be used as a
functional additive for improving obesity and maintaining good health (Yoon et al., 2003Yoon, H. S., Kim, C. H., Kim, T. J., Keum, I., & Han, N. S.
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application status of L-arabinose. Food Research and Development, 1,
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al., 2010Fu-Yu, B., Ji-Cheng, D., & Zhao-Wei, Z. (2010). Application of
L-arabinose in processing chiffon cake. Food Engineering, 2010(1),
48-50.). L-arabinose is the critical agent in the synthesis of
antiviral drug clevudine (Choung et al.,
2012Choung, B. S., Kim, I. H., Jeon, B. J., Lee, S., Kim, S. H., Kim, S.
W., Lee, S. O., Lee, S. T., & Kim, D. G. (2012). Long-term treatment
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2014 Jia, J. D., Hou, J. L., Yin, Y. K., Tan, D. M., Xu, D., Niu, J. Q.,
Zhou, X. Q., Wang, Y. M., Zhu, L. M., Chen, C. W., He, Y. W., Ren, H., Wan, M.
B., Wu, S. M., Wang, Q. H., Wei, L., Bao, W., Dong, Y., & Trylesinski, A.
(2014). Two-year results of a randomized, phase III comparative trial of
telbivudine versus lamivudine in Chinese patients. Hepatology International,
8(1), 72-82.; Li et al., 2014Li, X., Wang, Y., Han, D., Zhang, W., Zhang, Z., Ye, X., Tian, L.,
Dong, Y., Zhu, Q., & Chen, Y. (2014). Correlation of hepatitis B surface
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potent anti-hepatitis B (HBV) agents. It also has great usage in tumor therapy
(Loessner et al., 2007Loessner, H., Endmann, A., Leschner, S., Westphal, K., Rohde, M.,
Miloud, T., Hämmerling, G., Neuhaus, K., & Weiss, S. (2007). Remote control
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& Choy, H. E. (2014). Anti-tumoral effect of the mitochondrial target domain
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I. L., Miniker, T. D., Shchyolkina, A. K., Strel’tsov, S. A., Chilov, G. G.,
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A., Borisova, O. F., & Shtil, A. A. (2009). Novel antitumor L-arabinose
derivative of indolocarbazole with high affinity to DNA. ChemMedChem, 4(10),
1641-1648. http://dx.doi.org/10.1002/cmdc.200900227.
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) and chemistry (Yamauchi & Kinoshita, 2001Yamauchi, S., & Kinoshita, Y. (2001). Synthesis of cis-lactone
lignan, cis-(2S,3R)-parabenzlactone, from L-arabinose. Bioscience,
Biotechnology, and Biochemistry, 65(7), 1669-1672.
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new C-nucleosides from L-arabinose and D-glucose. ARKIVOC, 2008(13), 278-285.
http://dx.doi.org/10.3998/ark.5550190.0009.d30.
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cerevisiae strain that consumes L-Arabinose and produces ethanol. Applied and
Environmental Microbiology, 69(7), 4144-4150.
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L-arabinose by epimerization and its purification by 3-zone simulated moving bed
chromatography. Bioprocess and Biosystems Engineering, 33(1), 87-95.
http://dx.doi.org/10.1007/s00449-009-0375-0. PMid:19714365
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). Although it has been known
for a long time, the solubility and metastable zone width of L-arabinose in aqueous
solution have not been reported before.
Solubility is a thermodynamic property of a material, and it depends on its chemical
composition, nature of the solvent(s), and temperature. The extent of the
supersaturation or supercooling is referred to the metastable zone width (MSZW). The
equilibrium and kinetic methods have usually been used for solubility determination
(Black et al., 2013Black, S., Dang, L., Liu, C., & Wei, H. (2013). On the
measurement of solubility. Organic Process Research & Development, 17(3),
486-492. http://dx.doi.org/10.1021/op300336n.
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Evaluation of the solubility of Copper and Zinc in a salty, watery vegetable
soup. Ciência e Tecnologia de Alimentos, 23(3), 386-388.
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; Elder & Holm, 2013Elder, D., & Holm, R. (2013). Aqueous solubility: simple
predictive methods (in silico, in vitro and bio-relevant approaches).
International Journal of Pharmaceutics, 453(1), 3-11.
http://dx.doi.org/10.1016/j.ijpharm.2012.10.041. PMid:23124107
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et al., 2007Três, M. V., Francheschi, E., Borges, G. R., Dariva, C., Corazza, F.
C., Oliveira, J. V., & Corazza, M. L. (2007). Influência da temperatura na
solubilidade de beta-caroteno em solventes orgânicos à pressão ambiente. Ciência
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2012Zhang, X., Wang, X., Hao, L., Yang, X., Dang, L., & Wei, H.
(2012). Solubility and metastable zone width of DL-tartaric acid in aqueous
solution. Crystal Research and Technology, 47(11), 1153-1163.
http://dx.doi.org/10.1002/crat.201200166.
http://dx.doi.org/10.1002/crat.201200166...
), while methods such as turbidity monitoring (Zhang et al., 2012Zhang, X., Wang, X., Hao, L., Yang, X., Dang, L., & Wei, H.
(2012). Solubility and metastable zone width of DL-tartaric acid in aqueous
solution. Crystal Research and Technology, 47(11), 1153-1163.
http://dx.doi.org/10.1002/crat.201200166.
http://dx.doi.org/10.1002/crat.201200166...
; Rabesiaka
et al., 2011Rabesiaka, M., Porte, C., Bonnin-Paris, J., & Havet, J.-L., and
the Rabesiaka (2011). An automatic method for the determination of
saturationcurve and matastable zone width of lysine monohydrochloride. Journal
of Crystal Growth, 332(1), 75-80.
http://dx.doi.org/10.1016/j.jcrysgro.2011.07.016.
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), Focused Beam Reflectance Measurement (FBRM), (Barrett & Glennon, 2002Barrett, P., & Glennon, B. (2002). Characterizing the metastable
zone width and solubility curve using Lasentec FBRM and PVM. Chemical
Engineering Research & Design, 80(7), 799-805.
http://dx.doi.org/10.1205/026387602320776876.
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; Sun et al.,2010Sun, Y., Song, X., Wang, J., Luo, Y., & Yu, J. (2010).
Determination of seeded supersolubility of lithium carbonate using FBRM. Journal
of Crystal Growth, 312(2), 294-300.
http://dx.doi.org/10.1016/j.jcrysgro.2009.10.036.
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), and electric conductivity
method (Wu et al., 2012Wu, S., Feng, F., Zhou, L., & Gong, J. (2012). Experimental
determination of the solid--liquid equilibrium, metastable zone, and nucleation
parameters of the flunixin meglumine-ethanol system. Journal of Crystal Growth,
354(1), 164-168.
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) have been used for
MSZW determination.
Crystallization is the phase transition of matter from the state of a supercooled or
supersaturated mother medium to a crystalline state with lower energy. Excess energy
dissipates in the form of the latent heat during the transformation (Salomatov, 1966Salomatov, V. V. (1966). Growth rate of a crystal dissipating latent
heat of crystallization by radiation. Soviet Physics Journal, 9(1), 38-39.
http://dx.doi.org/10.1007/BF00818488.
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latent heat of crystallization of water in cooled solutions. Chemical Physics
Letters, 121(6), 547-550.
http://dx.doi.org/10.1016/0009-2614(85)87138-4.
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). The dissipation of the latent heat
increases the temperature of the solution, which can be immediately recorded by a
real-time recording thermometer (Shiroishi et al.,
1999Shiroishi, A., Yoshida, M., Yamane, T., & Miyashita, H. (1999).
Flow and temperature fields under natural convection due to crystal growth in
supersaturated solution. Journal of Chemical Engineering of Japan, 32(4),
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). Thus, the calorimetric method can be an alternative method for
MSZW detection.
In the present study, solubility of L-arabinose in aqueous solution was measured in the temperature range of 20 °C to 68 °C, and the MSZW was detected by the calorimetric method from 51-73%. The effect of two salts on the solubility and seeded metastable zone width of L-arabinose were also evaluated. The findings obtained can be useful in the industrial production of L-arabinose.
2 Material and methods
2.1 Materials
L-arabinose (99.7% purity) was purchased from Shandong Futaste Co. Ltd. The purity of the L-arabinose was analyzed by ion chromatograph (Dionex, ICS5000). The measurement was performed using carbopac@ PA1 column with electrochemical detection under the following conditions: 100 mM NaOH, 1.0 mL/min; injection volume: 20 μL, and temperature: 30 °C. The chromatogram indicates presence only of a sharp peak at 2.9 minutes. X-ray diffraction (XRD) analyses confirmed that the purchased needle-like material is really the L-arabinose crystalline. The XRD spectrum (Figure 1) was obtained on a Bruker D8 Advance X-ray diffractometer (Bruker, Germany) using conventional Cu Kα radiation (λ=1.54 Å) at 33 kV, 45 mA. Data were collected between 2-theta degrees values of 8.0° and 60.0° with a step width of 0.02°. Impurities (Potassium chloride and Calcium chloride of analytical grade) were used without further purification. Deionized water was used in all experiments.
2.2 Experimental setup
Standard curve of L-arabinose
A standard curve of L-arabinose measured by ion chromatograph (Dionex, ICS5000) is shown in Figure 2. The measurement condition was consistent with that of L-arabinose purity determination. The relationship between the peak area and L-arabinose concentration was expressed by Equation 1.
Where A is the peak area and C is the concentration. The peak area and L- arabinose concentration showed an excellent linear relationship from 15.625 ppm to 700 ppm, indicating that ion chromatography is an effective analytic method for L-arabinose.
Solubility of L-arabinose in pure water system
An excess of L-arabinose was added to 20 mL water and kept in a water bath with a magnetic stirrer; it was stirred once every hour for 8h and kept still overnight. The supernatant was filtered with a 0.22 μm filter. An aliquot of 100 μL of filtered supernatant was drawn and diluted to 100 mL with water. By measuring the peak area of the diluted solution, it was possible to determine the solubility of L-arabinose at a certain temperature (Table 1).
Solubility of L-arabinose in impure water system
Potassium and calcium are ubiquitous inorganic ions. Determination of the L-arabinose solubility in the presence of these ions, therefore, is very instructive for L-arabinose production. The measurement of L-arabinose solubility in the presence of impurity was similar to that in pure water system, but 1.0-4.0% impurity was added. Figures 3a and b showed the L-arabinose solubility in the presence of Potassium chloride and Calcium chloride, respectively.
2.3 Seeded Metastable Zone Width in pure water system
All experiments were conducted using a simple experimental setup, as shown in Figure 4. Fifty grams of L-arabinose and a certain amount of water were first transferred to the crystallizer loaded with a thermocouple (K-type, Omega, USA) connecting to a USB TC-08 in-line temperature logger (Pico technology, England). After fully dissolved, the solution was cooled to room temperature. In the process of cooling, a seed crystal (about 2 mm×2 mm×10 mm) was added to the crystallizer when the solution reached the saturation temperature. The seed crystal was suspended by a fine nylon thread vertically into the crystallizer avoiding contact with the crystallizer wall, thermocouple wire, and the magnetic stirrer preventing collisions and breakage of the crystal.
Schematic of experimental setup: (1) rubble stopper; (2) crystallizer; (3) Thermocouple; (4) Crystal Seed; (5) Magnetic rotor; (6) heater (7) Water bath; (8) Data logging module; and (9) Computer.
The inflection point of the temperature curve is defined as Tm, as illustrated in Figure 5. The nucleation point was easily detected as the appearance of the inflection point of the solution temperature (Figure 5b). The temperature rise was about 0.5-2 °C; Tm of 51-73% L-arabinose solution is shown in Table 2. The crystallizer mentioned above was a 50 mL round-bottom flask with a rubber stopper. The stirring rate was 50 rpm.
Definition of MSZW and detection of Tm: 5a Schematic of MSZW definition and 5b Tm detection in a typical temperature profile of cooling process.
2.4 Metastable Zone Width in the presence of impurity
To evaluate the effect of impurity on the MSZW of L-arabinose, 2.0% and 4.0% of impurity were added to the L-arabinose solution before complete dissolution of the L-arabinose; results are shown in Figure 6.
3 Results and discussion
3.1 Solubility
Solubility of L-arabinose in pure water system
The solid–liquid equilibrium of a L-arabinose-water system over the temperature range from 20 °C to 68 °C was determined (Table 1). The relationship between solubility and temperature can be satisfactorily described by Equation 2.
Where W is saturated concentration (gram L-arabinose per 100 gram water), and T is temperature in Celsius.
Solubility of L-arabinose in Potassium chloride-water system
To analyze the effect of Potassium chloride on the solubility of L-arabinose in aqueous solution, 1.0-4.0% Potassium chloride was added. Results show that L-arabinose is more soluble in the Potassium chloride-water system (Figure 3a). The solubility increment increases with the increase in concentration from 1.0% to 4.0%. For example, at 35 °C, the solubility increments in 1%, 2%, and 4% (Potassium chloride) were 17.3%, 22.2%, and 24.5%, respectively. The solubility increment in the Potassium chloride-water system increases with temperature rise; take 4.0% for example, the increments were 9.0%, 11.4%, 13.4%, 15.1%, 16.5%, 17.7%, and 18.7%, respectively, at 30-60 °C (5 °C increments).
This could be explained by the melassigenic effect and salting-in effect. Some researches (Day-Lewis, 1993Day-Lewis, C. (1993). The effect of individual ash constituents on molasses exhaustion: A literature survey (Sugar Milling Research Institute Technical Report, No. 1656, pp. 10-12). Durban: Sugar Milling Research Institute.; Quentin, 1957Quentin, G. (1957). Der Einfluss der Kationen auf die Saccharoselöslichkeit in Melassen und die Möglichkeiten einer technologischen Auswertung der unterschiedlichen Loslichkeitsbeeinflussung. Zucker, 10, 408.) stated that the presence of salt can increase the sucrose solubility in molasses, and the relative solubility increment obtained was: potassium > sodium > calcium. Sahadeo (1998)Sahadeo, P. (1998). The Effect of some Impurities on Molasses Exhaustion. In Proceedings of the Annual Congress South African Sugar Technologists' Association (Vol. 72, pp. 285-289), Durban, South African., however, stated that the melassigenic effect of salt was: sodium > calcium > magnesium > potassium. No matter which cation has the greatest melassigenic effect, it cannot be denied that potassium ion has melassigenic effect, which increases the solubility of L-arabinose.
It is known that Potassium chloride has salting-in effect at low
concentration. Ferreira et al.
(2007)Ferreira, L. I. S. A., Macedo, E. E. N. A., & Pinho, S. A. O. P.
(2007). KCl effect on the solubility of five different amino acids in water.
Fluid Phase Equilibria, 255(2), 131-137.
http://dx.doi.org/10.1016/j.fluid.2007.04.004.
http://dx.doi.org/10.1016/j.fluid.2007.0...
stated that the solubility of five amino acids increased
with the increase in potassium chloride concentration from 0M to 1M (7.45%).
Accordingly, in the present study, it was found that the solubility of
L-arabinose in the potassium chloride-water system is higher than that in
the pure water system at all temperatures tested, and the increment was:
4.0% Potassium chloride > 2.0% Potassium chloride > 1.0% Potassium
chloride.
Solubility of L-arabinose in calcium chloride-water system
Figure 3b demonstrates the influence of calcium chloride on the solubility of L-arabinose in aqueous solution. Similar to the effect of potassium chloride, the solubility increases with the rise in temperature from 30-60 °C, and the solubility increment increases with temperature rise. For example, the solubility increments in the 1.0% calcium chloride-water system is 22.3%, 29.6%, 38.2%, 47.6%, 57.7%, 68.1%, and 78.6% at 30-60 °C (5 °C increments), respectively; it is 33.1%, 46.6%, 57.7%, 66.8%, 74.2%, 80.2% and 84.9% in a 2.0% calcium chloride-water system. It is observed that solubility increment in the calcium chloride-water system is higher than that of the Potassium chloride-water system under the same conditions. Take samples at 40 °C for example, the solubility increments were 38.2%, 57.7%, and 48.5% in 1.0%, 2.0%, 4.0% calcium chloride-water system, while in the potassium chloride-water system it were 7.7%, 11.5%, and 13.4%.
In addition to the melassigenic effect and salting-in effect, another
possible factor is that L-arabinose can react with calcium chloride to form
different types of compounds (Dale,
1934Dale, J. K. (1934). Crystalline compounds of d-Xylose and of
l-Arabinose with calcium chloride. Journal of the American Chemical Society,
56(4), 932-934. http://dx.doi.org/10.1021/ja01319a050.
http://dx.doi.org/10.1021/ja01319a050...
; Austin & Walsh,
1934Austin, W. C., & Walsh, J. P. (1934). A.; Walsh, J. P. A new
crystalline compound of α-l-Arabinose with calcium chloride and water. Journal
of the American Chemical Society, 56(4), 934-935.
http://dx.doi.org/10.1021/ja01319a051.
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), such as α-L-arabinose calcium chloride·4H2O,
(β-L-arabinose)2·calcium chloride·2H2O, and
(β-L-arabinose)2·calcium chloride·H2O. These
compounds might change the equilibrium of L-arabinose-water system, which
affects the solubility of L-arabinose. Among the systems evaluated, 2.0%
calcium chloride had the greatest solubility increment, which is in
accordance with Mendonca’s study, who found that low concentration of salt
had salting-in effect, while high concentration had more salting-out effect
(Mendonça et al., 2003Mendonça, Â. F. S. S., Pereira, S. N. R., & Lampreia, I. M. S.
(2003). Solubility of Triethylamine in Calcium Chloride Aqueous Solutions from
20 to 35 C. Journal of Solution Chemistry, 32(12), 1033-1044.
http://dx.doi.org/10.1023/B:JOSL.0000023919.48142.ee.
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).
Accordingly, in the present study, it was found that the solubility of
L-arabinose in the calcium chloride-water system increased compared with
that of the pure water system at 30-60 °C and that the solubility increment
in the calcium chloride-water system is higher than that of the potassium
chloride-water system under the same conditions.
3.2 MSZW detection
Detection of MSZW in pure water system
Detection of seeded MSZW was conducted using a simple experimental setup, as shown in Figure 4. The temperature of nucleation point is defined as Tm. The extent of supercooling is defined as MSZW, which is equal to the value between the temperature of saturation (T0) and nucleation point (Tm) (Figure 5). A typical temperature profile was illustrated in Figure 5b. The inflection point of the temperature profile is detected and termed as Tm, which represents the temperature of nucleation point.
Table 2 shows Tm at the concentrations of 51-73%. Ice was added to the water bath because the Tm measured was below room temperature at 51.0-55.0%. The relationship between supersaturation and temperature can be satisfactorily described by the following exponential Equation 3:
Where Ws is supersaturation (g /100g water) and T is temperature.
As can be seen in Table 2, the MSZW
(ΔTm) is not constant but a spread from
24.36-32.72 °C (Mean ± Std. Deviation = 27.11± 2.34), which might be
explained by the following reasons. Firstly, MSZW is a function of the
induction time of nucleation (tind) and cooling rate (Zhang et al., 2012Zhang, X., Wang, X., Hao, L., Yang, X., Dang, L., & Wei, H.
(2012). Solubility and metastable zone width of DL-tartaric acid in aqueous
solution. Crystal Research and Technology, 47(11), 1153-1163.
http://dx.doi.org/10.1002/crat.201200166.
http://dx.doi.org/10.1002/crat.201200166...
; Herden et al., 2001Herden, A., Mayer, C., Kuch, S., & Lacmann, R. (2001). About the
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; Kobari et al., 2010Kobari, M., Kubota, N., & Hirasawa, I. (2010). Simulation of
metastable zone width and induction time for a seeded aqueous solution of
potassium sulfate. Journal of Crystal Growth, 312(19), 2734-2739.
http://dx.doi.org/10.1016/j.jcrysgro.2010.05.042.
http://dx.doi.org/10.1016/j.jcrysgro.201...
; Kim & Mersmann, 2001Kim, K., & Mersmann, A. (2001). Estimation of metastable zone
width in different nucleation processes. Chemical Engineering Science, 56(7),
2315-2324. http://dx.doi.org/10.1016/S0009-2509(00)00450-4.
http://dx.doi.org/10.1016/S0009-2509(00)...
; Sangwal, 2011Sangwal, K. (2011). Recent developments in understanding of the
metastable zone width of different solute-solvent systems. Journal of Crystal
Growth, 318(1), 103-109.
http://dx.doi.org/10.1016/j.jcrysgro.2010.11.078.
http://dx.doi.org/10.1016/j.jcrysgro.201...
). It has been pointed
out that log (ΔTm) increased linearly with an
increase in log R (cooling rate). Therefore, the log R was not constant, but
it changed which resulting in the deflection of MSZW. Secondly, the size and
number of the seed crystals influences the MSZW of secondary nucleation
(Herden et al., 2001Herden, A., Mayer, C., Kuch, S., & Lacmann, R. (2001). About the
metastable zone width of primary and secondary nucleation. Chemical Engineering
& Technology, 24(12), 1248-1254.
http://dx.doi.org/10.1002/1521-4125(200112)24:12<1248::AID-CEAT1248>3.0.CO;2-W.
http://dx.doi.org/10.1002/1521-4125(2001...
). Thus, a
large crystal was suspended in the solution. However, the size of the seed
crystal is not identical, which might lead to the deflection of MSZW.
Thirdly, the volume of the crystallizer and the stirring rate also had great
influence on MSZW. It has been stated that the MSZW is not a reproducible
point at small volumes but a spread which increases roughly inversely
proportional to the volume (Kadam et al.,
2012Kadam, S. S., Kulkarni, S. A., Coloma Ribera, R., Stankiewicz, A.
I., ter Horst, J. H., & Kramer, H. J. M. (2012). A new view on the
metastable zone width during cooling crystallization. Chemical Engineering
Science, 72, 10-19.
http://dx.doi.org/10.1016/j.ces.2012.01.002.
http://dx.doi.org/10.1016/j.ces.2012.01....
). In addition, MSZW is influenced by the detection method
and sensitivity. To reach the detectable Tm, the
dissipated latent heat has to overcome the heat emission from solution to
environment, which means that there exists a time lag between nucleation
point and detection point (Kubota et al.,
2013Kubota, N., Kobari, M., & Hirasawa, I. (2013). Analytical and
numerical study of detector sensitivity and resolution effects on metastable
zone width. CrystEngComm, 15(11), 2091-2098.
http://dx.doi.org/10.1039/c2ce26968f.
http://dx.doi.org/10.1039/c2ce26968f...
).
Detection of MSZW in impure water system
In many instances, small amounts of impurities have dramatic effects on crystal growth, morphology, and nucleation. Therefore, the influence of Potassium chloride and calcium chloride on the seeded MSZW of L-arabinose was investigated. The seeded MSZW of L-arabinose in the Potassium chloride-water system and calcium chloride-water system are shown in Figures 6a and b, respectively.
The Tm in the 4.0% Potassium chloride-water
system is lower than that in the 2.0% Potassium chloride-water system, which
is slightly lower than that of the pure water system. In other words, the
MSZW increases in the potassium chloride-water system, and the higher the
potassium chloride concentration, the larger the MSZW. A possible reason is
that the solubility of L-arabinose increases due to the addition of
potassium chloride, which would reduce the effective supersaturation.
Another reason is that impurities can change the nucleation rate by
affecting both the kinetic factor and interfacial energy (Sangwal, 2009Sangwal, K. (2009). Effect of impurities on the metastable zone
width of solute--solvent systems. Journal of Crystal Growth, 311(16), 4050-4061.
http://dx.doi.org/10.1016/j.jcrysgro.2009.06.045.
http://dx.doi.org/10.1016/j.jcrysgro.200...
; Herden et al., 2001Herden, A., Mayer, C., Kuch, S., & Lacmann, R. (2001). About the
metastable zone width of primary and secondary nucleation. Chemical Engineering
& Technology, 24(12), 1248-1254.
http://dx.doi.org/10.1002/1521-4125(200112)24:12<1248::AID-CEAT1248>3.0.CO;2-W.
http://dx.doi.org/10.1002/1521-4125(2001...
). The findings obtained in the
present study are similar to those in Dhanaraj’s research, who found that
adding K+ ion increased the MSZW of KDP thus making the solution
more stable and inhibiting spontaneous nucleation (Dhanaraj et al., 2008Dhanaraj, P. V., Mahadevan, C. K., Bhagavannarayana, G., Ramasamy,
P., & Rajesh, N. P. (2008). Growth and characterization of KDP crystals with
potassium carbonate as additive. Journal of Crystal Growth, 310(24), 5341-5346.
http://dx.doi.org/10.1016/j.jcrysgro.2008.09.019.
http://dx.doi.org/10.1016/j.jcrysgro.200...
).
The Tm is sensitive to calcium chloride
concentration. The relationship of Tm in the
pure water system and calcium chloride-water system is:
Tm (2.0% calcium chloride) >
Tm (pure water)>
Tm (4.0% calcium chloride); this is
consistent with other studies that reported that there are solute–solvent
systems in which the MSZW either first increase then decrease or first
decrease then increase with the increasing of impurity (Haja Hameed et al., 2007Haja Hameed, A. S., Rohani, S., Yu, W. C., Tai, C. Y., & Lan, C.
W. (2007). Growth and characterization of a new chelating agent added
4-dimethylamino- N-methyl-4-stilbazolium tosylate (DAST) single crystals.
Materials Chemistry and Physics, 102(1), 60-66.
http://dx.doi.org/10.1016/j.matchemphys.2006.11.004.
http://dx.doi.org/10.1016/j.matchemphys....
). This could
be explained by the change in saturation temperature and nucleation rate. It
has been proved that addition of Ca2+ changes the saturation
temperature of borax decahydrate and boric acid and the effect is
concentration dependent (Gürbüz &
Özdemir, 2003Gürbüz, H., & Özdemir, B. (2003). Experimental determination of
the metastable zone width of borax decahydrate by ultrasonic velocity
measurement. Journal of Crystal Growth, 252(1-3), 343-349.
http://dx.doi.org/10.1016/S0022-0248(02)02519-8.
http://dx.doi.org/10.1016/S0022-0248(02)...
; Sayan &
Ulrich, 2001Sayan, P., & Ulrich, J. (2001). Effect of various impurities on
the metastable zone width of boric acid. Crystal Research and Technology,
36(4-5), 411-417.
http://dx.doi.org/10.1002/1521-4079(200106)36:4/5<411::AID-CRAT411>3.0.CO;2-L.
http://dx.doi.org/10.1002/1521-4079(2001...
). In the present study, it was proved that the
solubility increment in the 2.0% calcium chloride-water system was larger
than that in the 4.0% calcium chloride-water system. Thus, the addition of
calcium chloride would change the effective supersaturation, which leads to
the change of MSZW. Calcium chloride might also have an influence on MSZW by
acting as a nucleation enhancer or as a nucleation inhibitor, such as nickel
(Mielniczek & Sangwal,
2004Mielniczek-Brzóska, E., & Sangwal, K. (2004). Growth kinetics of
ammonium oxalate monohydrate single crystals from aqueous solutions containing
Co (II) and Ni (II) impurities. Crystal Research and Technology, 39(11),
993-1005. http://dx.doi.org/10.1002/crat.200410284.
http://dx.doi.org/10.1002/crat.200410284...
). By acting as a nucleation enhancer, it would decrease the MSZW
of the solute, whereas as a nucleation inhibitor, it would increase the MSZW
of the solute.
(Sangwal, 2009Sangwal, K. (2009). Effect of impurities on the metastable zone
width of solute--solvent systems. Journal of Crystal Growth, 311(16), 4050-4061.
http://dx.doi.org/10.1016/j.jcrysgro.2009.06.045.
http://dx.doi.org/10.1016/j.jcrysgro.200...
). However, the
influence of calcium chloride on the seeded MSZW of L-arabinose by modifying
the nucleation rate has not been proved yet. In this study, it was found
that the seeded MSZW of L-arabinose decreases in the 2.0% calcium
chloride-water system and increases in the 4.0% calcium chloride-water
system.
4 Conclusion
As a new functional sugar, L-arabinose can be used in many fields such as food and medicine industries and others. Detection of the solubility and seeded metastable zone width of L-arabinose in aqueous solution can be of great importance in the production and use of L-arabinose.
In this study, solubility and seeded MSZW of L-arabinose with and without impurity was determined. The following conclusions can be drawn:
-
1
The solid–liquid equilibrium of a L-arabinose-water system from 20-68 °C is determined, which can be described by W = 55.492 + 0.7637T + 0.0113T2 (R2 =0.995).
-
2
The solubility of L-arabinose in the potassium chloride-water system is higher than that of the pure water system, and the solubility increment at 4.0% potassium chloride > 2.0% potassium chloride > 1.0% Potassium chloride. Solubility increment in the calcium chloride-water system is higher than that of the potassium chloride-water system under the same conditions. Among all systems evaluated, the 2.0% calcium chloride system had the greatest solubility increment, while the 1.0% and 4.0% systems had almost the same solubility increment.
-
3
Calorimetric method is used to detect the temperature of nucleation. The MSZW (ΔTm) is not constant but a spread (Mean ± Std. Deviation = 27.11± 2.34) in the pure water system. The MSZW increased in the presence of potassium chloride, and the MSZW increment was 4.0% potassium chloride > 2.0% potassium chloride. However, The MSZW of L-arabinose increased in the 4.0% calcium chloride-water system and decreased in the 2.0% calcium chloride-water system.
Acknowledgements
This study was supported by the Ministry of Science and Technology through the Agriculture Science and Technology Achievements Transformation Fund (No. 2013GB23600669) and by The Science and Technology Planning Project of Guangzhou Municiplity, China (No. 2011Y2-00012).
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Publication Dates
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Publication in this collection
Jan-Mar 2015
History
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Received
26 July 2014 -
Accepted
22 Sept 2014