Comparison of dissolution and surface reactions between calcite and aragonite in L-glutamic and L-aspartic acid solutions

Article abstract of DOI:10.3390/molecules15010258

We have investigated dissolution and surface reaction of calcite and aragonite in amino acid solutions of L-glutamic (L-glu) and L-aspartic acid (L-asp) at weak acidity of above pH 3. The surface reactions of calcite and aragonite were related with the dissolution. Calcite was dissolved in both solutions but the dissolution was limited by an adsorption of Ca-carboxylate salt. Aragonite was neither dissolved nor reacted in amino acid solutions because the crystal surface consisted of a hard to dissolve structure.

Full text of DOI:10.3390/molecules15010258

Molecules 2010, 15, 258-269; doi:10.3390/molecules15010258
OPEN ACCESS
molecules
ISSN 1420-3049
www.mdpi.com/journal/molecules
Article
Comparison of Dissolution and Surface Reactions Between
Calcite and Aragonite in L-Glutamic and L-Aspartic Acid
Solutions
Miyoung Ryu 1,2, Hwan Kim 2, Mihee Lim 1, Kwangsuk You 1 and Jiwhan Ahn 1,*
1
Korea Institute of Geoscience and Mineral Resources, 92 Gahwangno, Yuseung-gu, Daejeon, 305-
350, Korea; E-Mails: miyung1@snu.ac.kr (M.R); limmh@paran.com (M.L); yks-30@hanmail.net
(K.Y); ahnjw@kigam.re.kr (J.A)
2
School of Materials Science and Engineering, Seoul National University, Sillim-dong, Gwanak-gu,
Seoul, 151-742, Korea; E-Mail: hwan94@snu.ac.kr (H.K)
* Author to whom correspondence should be addressed; E-Mail: ahnjw@kigam.re.kr.
Received: 17 November 2009; in revised form: 11 January 2010 / Accepted: 11 January 2010 /
Published: 11 January 2010
Abstract: We have investigated dissolution and surface reaction of calcite and aragonite in
amino acid solutions of L-glutamic (L-glu) and L-aspartic acid (L-asp) at weak acidity of
above pH 3. The surface reactions of calcite and aragonite were related with the
dissolution. Calcite was dissolved in both solutions but the dissolution was limited by an
adsorption of Ca-carboxylate salt. Aragonite was neither dissolved nor reacted in amino
acid solutions because the crystal surface consisted of a hard to dissolve structure.
Keywords: calcite; aragonite; dissolution; adsorption; amino acid solution
1. Introduction
The dissolution of calcium carbonate has been researched extensively for several decades because
calcium carbonate plays an important role in carbonate buffering in natural water. The dissolution
kinetics of calcium carbonate is related with the neutralization of acidic lakes, weathering processes
and elimination of scales in petroleum wells [1–5]. Calcite is the most stable phase among the various
calcium carbonate polymorphs (calcite, aragonite and vaterite), so that it has received the most

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attention from many researchers [6–8] and therefore, the dissolution kinetics of calcite has been widely
studied, but those of other phases have not been sufficiently studied yet.
In research on the dissolution of calcite in weak and strong acid solutions, the initial pH of the
solution was reported to be a critical factor in the determination of the dissolution rate [4,9]. In acetic
acid solution, the dissolution of calcite occurred by the transport of reactant to the surface, surface
reaction, and the transport of product from the surface. At pH values of below 2.9, the transport rates
of reactant and product affected the dissolution rate, and at pH of above 3.7, the surface reaction rate
also acted as a critical factor [9]. In nitric acid solutions, the initial pH was also reported as a
determinant. The dissolution amount of calcite increased drastically at the pH of below 2, but the
solution acidity did not affect the leaching of calcite above pH 3 [4].
Plummer et al. [10] have studied about the dissolution reaction of calcite and reported three
mechanisms according to pH range. At the pH of less than 3.5, the dissolution rate was directly
proportional to the hydrogen ion activity and was unrelated with the PCO2. In the pH region from 3.5 to
5.5, the dissolution rate depended on both pH and PCO2, so that the H2CO3 concentration was a
determinant. Above pH 6.5, H2O was involved in the dissolution reaction. The three dissolution
mechanisms are shown in the following reactions (1)–(3):
-
CaCO3 + H+ ↔ Ca2+ + HCO3
-------- pH < 3.5
(1)
(2)
(3)
0
-
CaCO3 + H2CO3 ↔ Ca2+ + 2HCO3
CaCO3 + H2O ↔ Ca2+ + HCO3 + OH-
-------- 3.5 < pH < 5.5
-------- pH > 6.5
-
The dissolution kinetics of calcite have been studied with various additives in the solutions such as
chelating agents, sodium dichromate, and polymaleic acid, phosphoric acid, or oxalic acid [9,11,12]. In
the presence of calcium chelating agents, calcite was dissolved even at pH 12. The hydrogen ion attack
of equation (1) did not occur, but the dissolution of calcite happened with the surface reaction between
the chelating agent and calcite. The Ca chelating agent was adsorbed and a Ca-complex was formed on
the surface of calcite. The Ca-complex resulted in weakening of the bonds between calcium and
carbonate, and desorption of the Ca-complex occurred at pH 12. Therefore, calcite could be dissolved
in a high pH region [9]. In the neutral pH region between 6 and 7, calcite was dissolved and the
dissolution rate was affected by the presence of carbon dioxide, which retards its dissolution [11].
When the surface of calcite was pretreated by acidic solutions such as polymaleic, phosphoric and
oxalic acids, the dissolution of calcite in acidic solutions was limited because the surface coating
hindered the dissolution reaction on the surface [12].
Among calcium carbonate polymorphs aragonite represents a meta-stable phase and is found in
certain living organisms such as oysters or abalones [13]. There are some results concerning the
synthesis of aragonite using additives, but the dissolution of aragonite has been less investigated
because of its instability. It has been reported that the dissolution of aragonite was controlled by the
diffusion in the bulk of the solution and was determined by the surface area [14,5]. All of the previous
research was focused on the dissolution of natural aragonite and bivalves in strong acid solutions, thus
the dissolution behavior of synthetic aragonite also needs to be studied.
The present study aims to compare dissolution and surface reactions of synthesized calcite and
aragonite in amino acids such as L-aspartic (L-asp) and L-glutamic (L-glu) acid. It is well known that
the dissolution behavior of calcite depends on the surface reaction in solution and in general, the

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carbonate mineral is hardly treated its surface with organic chemicals [12]. However, Demjén et al.
[15] have reported that the calcite could be treated by the silane coupling agent containing an amino
group. Based on the fact that the amino group has reactivity for the calcium carbonate surface, amino
acids were chosen as the solvent in this research. Calcite and aragonite were synthesized as
rhombohedra and needle-like particles, respectively, in our laboratory. Dissolution is related to surface
characters, thus we analyzed filtrates and the surface of solids after reactions.
2. Results and Discussion
2.1. Dissolution equilibrium of calcite in 0.02 M acetic acid solution
Ca concentrations after dissolution for four hours are described in Table 1, showing both
concentrations in mg/L and molarity (M). The dissolution of calcite resulted from the hydrogen attack
as shown in reaction (1) and the Ca concentration from dissolved calcite would be equal to a half of
the initial concentration of the acidic solution by charge balancing. Calcite was dissolved well in
0.02 M acetic acid solution and the Ca concentration from dissolved calcite was then 360 mg/L. It was
almost same as the concentration in mg/L converted from 0.01M of Ca and was also equal to a
theoretic value determined by the formula shown in the reaction (1). Therefore, the reaction for four
hours in which the dissolution reached equilibrium was thus determined as an optimal condition for
completely achieving calcite dissolution.
Table 1. Ca concentration at the dissolution for four hours. Ca concentrations by the
calcite dissolution depended on the initial concentration and acidic solutions. Ca molarity
(M) of in each filtrate was described in parenthesis. Ca concentrations in dissolution
filtrates of aragonite could be detected by AAS analysis.
0.002 M
0.005 M
0.01 M
0.02 M
360 mg/L
(0.01 M)
Calcite + acetic acid
Calcite + L-asp
-
-
-
13 mg/L
(0.0003 M)
16 mg/L
24 mg/L
(0.0006 M)
31 mg/L
60 mg/L
(0.0015 M)
65 mg/L
102 mg/L
(0.0025 M)
124 mg/L
(0.0031 M)
Calcite + L-glu
(0.0004 M)
(0.0008 M)
(0.0016 M)
Aragonite + each of
the solutions
Under 10 mg/L
2.2. Dissolution behavior of calcite in amino acid solutions
Calcite was dissolved less in amino acid solutions than in acetic acid solution as described in
Table 1. When the initial concentration was 0.02 M, the Ca concentrations in L-asp and L-glu solutions
were 102 mg/L and 124 mg/L, respectively, which could be converted to 0.0025 M and 0.003 M Ca.
Ca concentrations in 0.02 M amino acid solutions were much lower than that in acetic acid solution
under the same conditions. That is, the amount of calcite dissolved in amino acid solution did not reach
theoretical values. In addition, those in other solutions were lower than theoretical values as

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represented in Table 1. That is, the dissolution of calcite in amino acid solutions was extremely
inhibited in spite of the acidic conditions present.
The dissolution behavior of calcite according to the dissolution time was also investigated. Figure 2
shows Ca concentrations in L-asp and L-glu filtrates versus the dissolution time. Ca concentrations in
L-glu solutions [Figure 1(a)] were slightly higher than those in L-asp solutions [Figure 1(b)], but those
in both solutions were reduced with the dissolution time. After an hour, the dissolution reached an
equilibrium state. From the reduction of Ca concentration in amino acid solution, we could consider
that dissolved Ca ion adsorbed on calcite surface.
Figure 1. Ca concentrations in (a) L-glu and (b) L-asp solutions depending on the
dissolution time. Overall Ca concentrations in (a) L-glu solutions were slightly higher
overall compared with those in (b) L-asp solutions.
2.3. ATR-FTIR analysis of calcite surface
ATR-FTIR spectrums of calcite dissolved for four hours in L-glu and L-asp solutions are
represented in Figure 2. After the dissolution, a carbonate adsorption band at 1,419 cm-1 shifted to
1,411 cm-1 and new absorption bands appeared near 3,600 cm-1 and 1,589 cm-1. The absorption bands
appeared at about 3,500 cm-1 resulted from the existence of N-H bending vibrations [16]. Another
band at 1,589 cm-1 and the shift of the peak from 1,419 cm-1 to 1,411 cm-1 could be explained by
formation of a carboxylate salt. The characteristic pattern for carboxylate-metal ion complex (M-OOC-
R) is the result of the appearance of two bands near 1,400 cm-1 and 1,600 cm-1 [16]. Accordingly, we
could consider that a Ca-carboxylate salt existed on the surface of the calcite.
The carboxyl group reacts with the metal ions in solution and is adsorbed on the surface. The
adsorption mode of carboxylate salt could be determined by the shape of IR adsorption band. If the
carboxylate salt is adsorbed chemically on the surface, the adsorption band near 1,550 cm-1 appears as
a single one; if it is adsorbed physically or is precipitated on the surface, the adsorption band between
1,500 and 1,600 cm-1 appears a doublet [17,18]. In the cases of calcite dissolved in 0.02 M amino acid

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solutions, a single adsorption band appeared at 1,589 cm-1, as shown in Figure 3. Therefore, we could
consider that the Ca-carboxylate salt was chemically adsorbed on the surface.
Figure 2. ATR-FTIR spectrums of calcite before and after of the dissolution. From the top,
calcite, calcite dissolved in L-glu and calcite dissolved in L-asp.
The Ca concentration dissolved from calcite reduced with decrease in the initial concentration.
ATR-FTIR spectrums according to the initial concentration are shown in Figure 3. Absorption peaks at
1,589 cm-1 were intensified with an increase in the initial concentrations. The absorption peaks at
1,589 cm-1 were too weak to be detected on the surface of calcite reacted in 0.002 M of both amino
acid solutions. When the calcite was dissolved in L-asp solution, the adsorption peak did not appear in
0.01 M solution but appeared in 0.02 M solution, as shown in Figure 3(a). In the case of calcite
dissolved in L-glu solutions, however, the adsorption peak of Ca-carboxylate salt started appear from
0.01 M solution and became clearer with the increase to 0.02 M [see Figure 3(b)].
Figure 3. ATR-FTIR spectrums showing the carbonate stretching between 1,500 and
1,800 cm-1. From the top spectrum, the initial concentration of amino acid solution is 0.002,
0.01 and 0.02 M. (a) Calcite reacted with L-asp solutions and (b) reacted with L-glu solutions.

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From the Ca concentration and ATR-FTIR spectrum results, we could suppose that the adsorption
of Ca-carboxylate salt on the surface was related with the dissolution of calcite. The amount of
dissolved calcite increased with increasing initial concentration, and the adsorption peak of the
Ca-carboxylate salt was also intensified. On the contrary, adsorption peaks related with Ca-carboxylate
salt did not appear at low initial concentrations of both solutions. That is, Ca ion from calcite
dissolution reacted with ionized amino acid and Ca carboxylate salt was formed as a final product, as
shown in Scheme 1. And then, Ca-carboxylate salt was adsorbed on the surface of calcite.
Consequently, the inhibition of calcite dissolution in amino acid solutions resulted from the adsorption
of Ca-carboxylate salt.
Scheme 1. Chemical formula of the Ca-carboxylate salt formed by the reaction of Ca ion
and L-glu ion.
2.4. Insoluble aragonite in amino acid solutions
Ca concentrations from aragonite dissolution in all acidic solutions involving 0.02 M acetic acid
solution were below 10 mg/L, as represented in Table 1. That is, the needle-like aragonite was hardly
dissolved in weak acidic solutions and reaction conditions such as pH, initial concentration and the
reaction time did not affect its dissolution. Aragonite did not dissolve in amino acid solutions even
after four days.
Because needle-like aragonite was not dissolved in acidic solutions, no Ca-carboxylate salt could be
detected by ATR-FTIR, as shown in Figure 4. For the needle-like aragonite, a carbonate absorption
peak appeared at 1,473 cm-1 but it does not shift, although the aragonite was reacted with 0.02 M
amino acids for four hours. As aforementioned, the adsorption of Ca-carboxylate salt could occur after
the Ca ion was dissolved from calcium carbonate. It is reasonable that the adsorption of
Ca-carboxylate salt did not occur on the aragonite surface because aragonite was not dissolved at all.
The stability of the needle-like aragonite for the dissolution could be supposed to be the result of
the crystal structure. Figure 5(a) shows TEM image and Small Area Diffraction pattern of the needle-
like aragonite. One needle-like aragonite was composed of a single crystal and the lateral plane was
calculated as (110) and (010) with SAD in Figure 5(a) [19]. Especially, aragonite (010) has been
known as a cleavage plane. Vertical and parallel projections of aragonite (010) are shown in
Figure 5(b). Ca atoms and CO3 groups are located at different layers along the [010] and the stacking
sequence of layers is in the order of Ca-CO3-CO3-Ca-CO3 layers.
It was reported that the dissolution of calcium carbonate occurs with retention of charge balance [5].
2-
Each layer of aragonite (010) is formed by a single charge such as Ca2+ or CO3 , so that charge
balance hardly occurs on the surface during the dissolution. That is, aragonite could not be

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continuously dissolved even though a little amount of aragonite was dissolved at the beginning of the
reaction.
Figure 4. ATR-FTIR spectrums of aragonite. From the top, aragonite, aragonite dissolved
in L-glu and aragonite dissolved in L-asp.
Figure 5. Transmission Electron Microscopy (TEM) image of needle-like aragonite and
projection schemes of aragonite (010). (a) TEM image and Small Area Diffraction (SAD)
pattern showing a single crystalline aragonite. (b) Vertical and parallel projection of
aragonite (010).
2.5. Surface morphology change due to the dissolution
The surface morphology changes for the soluble calcite and the insoluble aragonite were different,
as shown Figures 6 and Figure 7. Before the dissolution, the surfaces of calcite and aragonite were
very clear and there were no defects or roughness on surfaces [see Figures 6(a) and 7(a)]. After the
dissolution in 0.02 M L-glu solution, dissolution pits were formed on calcite surface however they did
not appear on the aragonite surface [see Figures 6(b) and 7(c)]. During the dissolution of calcite, the

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shape of rhombic pit could appear on the surface due to its crystal symmetry [2]. In Figure 6(b), we
could see the rhombic pits which could be regarded as surface defects formed by the dissolution.
Though no surface defects were observed on the surface of aragonite, as shown in Figure 7(c), we
could note a surface crystallinity change. Crystallinity of the particle can be confirmed with Fast
Fourier Transformation (FFT) calculation of HRTEM image as shown in Figures 7(b) and (d). When
the HRTEM image of crystalline particle was transformed to FFT mode, we could observe spots in
FFT of Figure 7(b). After the dissolution, a bright circle appeared in FFT mode which indicated non-
crystalline phase was formed on the surface as in Figure 7(d). The surface of aragonite could be stable
on the dissolution in acid solution however the surface crystallinity could not be kept during the
dissolution. With this research, we have not defined the reason for the surface change and this needs to
be studied more in the future work.
Figure 6. Surface morphology change of calcite.TEM images of (a) raw calcite surface and
(b) dissolved calcite surface in 0.02 M L-glu solution for 4 hours.
Figure 7. HRTEM and corresponding FFT of aragonite surface. (a) HRTEM image and (b)
corresponding FFT before the dissolution of aragonite, and (c) HRTEM image and (d)
corresponding FFT After the dissolution.

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3. Experimental
3.1. Raw materials
Calcium carbonates were synthesized in our laboratory. Calcite was prepared by a carbonation
method which is synthetic process that involves blowing CO2 gas into a Ca(OH)2 slurry at room
temperature. The initial concentration of Ca(OH)2 slurry was 0.2 M and the injection rate of CO2 gas
was 50 mL/min. The carbonation process was determined by a pH change from pH 12.4 to 6.8. The
reaction was finished with the pH of the solution was below 6.8 [20]. Synthesized calcite was a single
phase and its specific surface area was 12 m2/g. Aragonite was synthesized with Na2CO3 and Ca(OH)2
solution at 80 °C and NaOH solution was used to control a dissolution rate of Ca(OH)2. Ca(OH)2
(0.5 mole) was mixed in 2.5 M NaOH solution (400 mL) and 0.5 M Na2CO3 solution (600 mL) was
injected into the Ca(OH)2-NaOH solution at 30 mL/min. Synthesized aragonite was also a single phase
and its specific surface area was 2 m2/g.
Synthesized calcite and aragonite were composed of a single phase and unreacted materials or
second phase was not detected in XRD analysis as shown in Figures 8 (a) and (b). Synthesized calcite
and aragonite were observed by the analysis of Scanning Electron Microscopy (SEM, JSM 6300,
JEOL; FESEM, S-4800, HITACHI) as represented in Figure 9. The particle size of calcite was just
below 1 μm and the shape appreared as rounded rhombohedra as in Figure 1(a), whereas that of
aragonite was very large and the length of the major axis was even above 10 μm and that of the minor
axis was almost 1 μm [Figure 1(b)]. In order to analyze the surface morphology, Transmission
Electron Microscopy (TEM, F20, Tecnai) image was taken, and Small Area Diffraction (SAD) was
analyzed.
Figure 8. XRD patterns of synthesized calcite and aragonite. (a) Rhombohedral calcite and
(b) needle-like aragonite.

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Figure 9. SEM images of synthesized calcite and aragonite. (a) Rhombohedral calcite of
less than 100 nm and (b) needle-like aragonite.
Acidic solutions were prepared using amino acids containing acidic side chains. The chosen amino
acids were L-aspartic (L-asp; HO2CCH(NH2)CH2CO2H) and L-glutamic (L-glu;
HO2C(CH2)2(NH2)CH2CO2H) acids which were ionized in aqueous solution, and solutions of pH 3.1
and pH 3.4 were formed. Acid solutions of amino acids were made to be 0.002, 0.005, 0.01 and 0.02 M,
respectively. In order to compare the dissolution behavior of calcium carbonate in amino acid solutions
and general weak acid solution, 0.02 M of acetic acid solution was used.
3.2. Experimental set-up
The dissolution reaction was performed using a one liter glass vessel and a mechanical stirrer (RW
20 DZM, IKA) equipped with a two-bladed Teflon propeller type impeller. Either calcite or aragonite
(15 g) was added into each acid solution (250 mL) as aforementioned. The agitation rate was fixed at
250 rpm and the dissolution was carried out at room temperature. Aliquots (40 mL each) were taken
out from the suspensions at 10 min, 30 min, 1 hour, 2 hour and 4 hour during the dissolution and
filtered using a membrane filter of 0.45 μm pore size. After the filtration, each solid residue on the
filter paper was dried at 60 °C for a day to be used for its surface analysis and each filtrate was
separately collected to be used for the analysis of its Ca concentration. Filtered solids were analyzed
with an ATR-FTIR (Nicolet 380, Thermo Instrument) which is a method to detect the IR spectrum
reflected from target materials. Ca concentration in the filtrate was measured using AAS (AA-6800,
Shimadzu). A Ca calibration curve was then made by three standard solutions of 10, 20 and 40 mg/L.
4. Conclusions
Surface reactions of calcite and aragonite were quite different in amino acid solutions. Calcite was
dissolved in amino acid solutions, whereas the adsorption of Ca-carboxylate salt limited the
dissolution behavior. Aragonite did not dissolve in amino acid solutions and no adsorption of
Ca-carboxylate salt appeared on its surface either. The lateral surface of needle-like aragonite
consisted of (010) on which its charge balance was hardly kept during the dissolution. In the future
study, it is necessary to investigate the surface morphology changes of calcite and aragonite caused by
the dissolution.

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Acknowledgements
This work was supported by the grant from the Energy Technology Innovation (ETI) R& D
program in the Ministry of Knowledge Economy, Republic of Korea and the Center for Iron and Steel
Research at Research Institute of Advanced Materials. We would like to acknowledge Seishi Goto for
his contribution to this article.
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