# CaCO3–Polymer Nanocomposite Prepared with Supercritical CO2

Authors: Hiroaki Wakayama
Journal: International Journal of Polymer Science
 (2018)

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## Abstract

A novel process for generation of a CaCO3–polymer nanocomposite with a controlled three-dimensional shape was developed. Specifically, a nanocomposite with a high CaCO3 content was produced by introducing supercritical CO2 into a polymer matrix containing Ca ions. A mixture of poly(vinyl alcohol), Ca acetate, and poly(acrylic acid) was poured into a mold, the mold was placed in an autoclave, and CO2 was introduced to precipitate CaCO3 within the polymer matrix. Laser Raman spectroscopy and transmission electron microscopy showed that this process produced a nanocomposite containing highly dispersed CaCO3 (aragonite) nanoparticles. The flexural strength of the nanocomposite was larger than the flexural strengths of limestone and CaCO3 produced by hydrothermal hot pressing. The use of supercritical CO2 facilitated CO2 dissolution, which resulted in rapid precipitation of CaCO3 in the polymer matrix. The above-described process has potential utility for fixation of CO2.


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## Body

## 1. Introduction

The adverse environmental effects of human activities are becoming increasingly problematic. Minimizing energy consumption and waste generation during material production is therefore an important goal in the field of material engineering. One potential strategy for achieving this goal is to mimic processes and simulate materials found in living organisms.Organisms synthesize inorganic substances such as hydroxyapatite, calcium carbonate (CaCO3), and silica and organic substances such as cellulose and chitin at ambient temperature and atmospheric pressure [1]. These substances are eventually returned to the natural environment and are transformed into resources such as limestone and phosphate ores [2]. In addition, living organisms also serve as sources of materials, such as wood and tree lacquers, that can be used and reused by humans over the course of many centuries [3].The highly controlled microstructures of living organisms are constructed from various molecular building blocks, and the organisms themselves can therefore be thought of as aggregates of sophisticated nanodevices [4]. By combining multiple types of organic molecules or by combining organic and inorganic molecules at the nanometer scale, organisms can carry out an astonishing array of functions that cannot be achieved with artificial devices.Biomaterials represent a treasure trove of functional materials, and mimicking biological functions and effectively using biomaterials are major challenges in the field of materials engineering. Biomaterials such as bones, teeth, shells, and pearls are good models for the development of novel functional materials with minimal environmental loads and energy consumption. Designing and creating new functional materials based on substances, structures, functions, and processes of living things are called biomimetic materials processing, and functional materials generated by such processing are referred to as biomimetic functional materials [5]. One biological process that is of particular interest is biomineralization (i.e., biological synthesis of minerals). Because this process consumes little energy and emits little waste into the environment, it has an extremely low environmental burden. Therefore, imitation of biomineralization might lead to an environmentally friendly process for synthesis of ceramics.Biominerals are not simple inorganic crystals but composites of inorganic and organic materials [6]. For example, shells consist of 95% CaCO3 and 5% protein, a composition that imparts flexibility and structural anisotropy not found in pure CaCO3 crystals. Several attempts to produce composite materials by mimicking biomineralization have been reported [7–10]. However, in most cases, the CaCO3 products obtained are powders with particle sizes of no more than a few micrometers. Although there have been a few reports of the formation of CaCO3 thin films, the process takes several days [11]. More research is necessary for the development of versatile, industrially practical routes to bioinspired materials, such as the production of bulk CaCO3 nanocomposite materials via rapid CO2 fixation.In this study, a novel process for producing CaCO3 nanocomposite materials was developed. Specifically, glossy CaCO3–polymer nanocomposites were produced by introducing supercritical CO2 into aqueous Ca2+ in the presence of a polymer. In the work described in this paper, supercritical CO2 was used to facilitate mineralization of CaCO3 for production of a CaCO3–polymer nanocomposite with a controlled three-dimensional shape. Specifically, a mixture of poly(vinyl alcohol) (PVA), Ca acetate, and poly(acrylic acid) (PAA) was poured into a mold, the mold was placed in an autoclave, and CO2 was introduced to precipitate CaCO3 within the polymer matrix. Laser Raman spectroscopy and transmission electron microscopy revealed that the resulting nanocomposite was composed of highly dispersed CaCO3 (aragonite) nanoparticles and had excellent mechanical properties; its flexural strength was larger than the flexural strengths of limestone and CaCO3 produced by hydrothermal hot pressing.


## 2. Experimental

### 2.1. Materials

PVA (100 g,MW=2×103) was dissolved in 500 mL of 1.42 M aqueous Ca acetate along with 2.4 × 10−3 wt% of PAA (MW=2×103). The mixture was stirred for 10 min, heated at 90°C for 3 h, and then poured into a mold. The mold was placed in an autoclave, CO2 was introduced, and the autoclave was heated at 50°C and 10 MPa for 2 h. The sample was removed from the mold and cut into a rectangular parallelepiped in order to measure mechanical properties.


### 2.2. Analysis

X-ray diffraction patterns (Cu Kα) were collected on a diffractometer (RINT-TTR, Rigaku, Japan) operated at 40 kV and 50 mA. Scanning electron microscopy images and energy-dispersive X-ray spectra were obtained with a scanning electron microscope (S-3600N, Hitachi, Japan). Scanning transmission electron microscopy images were obtained with a transmission electron microscope (JEM-2010 FEF [HR], JEOL, Japan). Thermal decomposition of the samples up to 1273 K was measured with a thermogravimetric analysis instrument (Thermo Plus, Rigaku) under an air atmosphere. Raman spectra were recorded with a Raman spectrometer (NRS-3300, JASCO, Japan). Three-point bending tests were conducted with a testing machine (universal testing machine type 5966, Instron, USA).


## 2.1. Materials

PVA (100 g,MW=2×103) was dissolved in 500 mL of 1.42 M aqueous Ca acetate along with 2.4 × 10−3 wt% of PAA (MW=2×103). The mixture was stirred for 10 min, heated at 90°C for 3 h, and then poured into a mold. The mold was placed in an autoclave, CO2 was introduced, and the autoclave was heated at 50°C and 10 MPa for 2 h. The sample was removed from the mold and cut into a rectangular parallelepiped in order to measure mechanical properties.


## 2.2. Analysis

X-ray diffraction patterns (Cu Kα) were collected on a diffractometer (RINT-TTR, Rigaku, Japan) operated at 40 kV and 50 mA. Scanning electron microscopy images and energy-dispersive X-ray spectra were obtained with a scanning electron microscope (S-3600N, Hitachi, Japan). Scanning transmission electron microscopy images were obtained with a transmission electron microscope (JEM-2010 FEF [HR], JEOL, Japan). Thermal decomposition of the samples up to 1273 K was measured with a thermogravimetric analysis instrument (Thermo Plus, Rigaku) under an air atmosphere. Raman spectra were recorded with a Raman spectrometer (NRS-3300, JASCO, Japan). Three-point bending tests were conducted with a testing machine (universal testing machine type 5966, Instron, USA).


## 3. Results and Discussion

A CaCO3–polymer nanocomposite sample was prepared (Figure 1) via the procedure described in Section 2.1.Figure 1
An external view of the CaCO3–polymer nanocomposite sample.The CaCO3–polymer nanocomposite sample was subjected to thermogravimetric analysis (TGA) (Figure 2). The TGA trace revealed successive mass losses due to the removal of absorbed water and acetic acid, PVA degradation [12], and CaCO3 decomposition [13] (Figure 2). The weight loss from 200 to 500°C was due to the dehydration reaction of –OH groups in the PVA chains and subsequent release of CO2 gas due to degradation of PVA [12]. The amounts of CaO and ash produced were calculated from the weight loss of CaCO3 (corresponding to the amount of CO2 produced) when CaCO3 decomposed into CaO and CO2 at 600–700°C [13]. The attribution of the weight loss in each temperature range and the percentages of the total weight contributed by each component are shown in the TGA results (Figure 2). The overall percentage of CaCO3 in the nanocomposite was estimated to be 57.3 wt%; that is, the CaCO3 content was high. Producing nanocomposites containing large amounts of inorganic materials is difficult via conventional mixing processes [14].Figure 2
Thermal weight change of the CaCO3–polymer nanocomposite sample.The X-ray diffraction pattern of the nanocomposite sample showed only reflections corresponding to aragonite (Figure3), which is less stable than calcite, the most stable CaCO3 polymorph [15]. The production of aragonite was attributed to the templating effect of the hydroxyl groups of the PVA [16]. That is, the aragonite polymorph formed because the hydroxyl groups bonded to Ca2+ via PAA, and the arrangement of the hydroxyl groups was very similar to the arrangement of the atoms of aragonite. When PAA was adsorbed onto the crystalline form of PVA, a locally aligned two-dimensional structure formed in the PVA matrix. The templating effect of the PVA matrix resulted in the formation of aragonite crystals on this two-dimensional structure.Figure 3
X-ray diffraction pattern of the CaCO3–polymer nanocomposite sample.Electron micrographs of the CaCO3–polymer nanocomposite sample were obtained (Figures 4(a) and 4(b)). The image shown in Figure 4(a) confirmed that ~3 μm CaCO3 particles were embedded firmly in the polymer matrix. The columnar crystals that are characteristic of aragonite [17] were clearly observed in the magnified image shown in Figure 4(b). Surprisingly, calcium was detected at locations both on and near the particles. Specifically, in the energy-dispersive X-ray spectra, calcium was detected both in the smooth areas of the sample and in the areas with CaCO3 particles (Figures 4(c) and 4(d)). This result suggested the formation of a nanocomposite structure consisting of fine CaCO3 particles precipitated in a polymer matrix.Figure 4
Scanning electron microscopy photographs of the CaCO3–polymer nanocomposite sample (a and b) and corresponding energy-dispersive X-ray spectra (c and d).
(a)
(b)
(c)
(d)Figure5 shows the microscopic laser Raman spectrum of the CaCO3–polymer nanocomposite sample. Peaks for CaCO3 (aragonite) [18] were detected both in the parts of the sample corresponding to CaCO3 particles and in the parts considered to consist mainly of PVA. This result suggested a nanocomposite structure of extremely fine CaCO3 particles precipitated in the polymer matrix and was consistent with the energy-dispersive X-ray analysis result.Figure 5
Laser Raman spectrum on (a) and near the CaCO3 microparticle (b).In the transmission electron microscopy image (Figure6), the presence of fine particles (<10 nm) confirmed that the nanocomposite consisted of highly dispersed CaCO3 nanoparticles in a polymer matrix. The image showed that CaCO3 nanoparticles were dispersed in the PVA matrix (Figure 6). In contrast, as shown in the scanning electron microscopy images (Figures 4(a) and 4(b)), CaCO3 microparticles with dimensions of several micrometers were also present in the samples. The TGA result showed that the content of CaCO3 in the whole sample was relatively high. Even though CaCO3 nanocomposites have previously been synthesized [14, 19, 20], synthesizing nanocomposites with a high CaCO3 content remains challenging. For example, in a previous synthesis of CaCO3 nanocomposites, CaCO3 particles with dimensions of several tens of nanometers, synthesized in advance, were mixed with polymers, but when high concentrations of these CaCO3 particles were mixed with the polymers, CaCO3 aggregated [21]. In contrast, in this study, the use of supercritical CO2 facilitated CO2 dissolution, which resulted in rapid precipitation of CaCO3 within the polymer matrix. That is, CaCO3-containing nanoparticles with diameters of several nanometers formed in the polymer matrix, and these nanoparticles were finer than previously reported CaCO3 nanoparticles. The functional groups in the polymer molecules probably acted as templates for the crystallization of CaCO3 in the aragonite crystal structure, and even though the CaCO3 content was high, CaCO3 was highly dispersed in the polymer.Figure 6
Transmission electron microscopy image of the CaCO3–polymer nanocomposite sample.The flexural strength of the CaCO3–polymer nanocomposite sample was 12 MPa, which is larger than the corresponding values for limestone and CaCO3 produced by hydrothermal hot pressing (Figure 7). The strength of the nanocomposite was likely due to the existence of a nanocomposite structure in which CaCO3 nanoparticles were more firmly attached to the polymer matrix than the particles in limestone or hot-pressed CaCO3. Limestone and hot-pressed CaCO3 consist of calcite, whereas the process reported herein produced aragonite, which is mechanically stronger than calcite [22].Figure 7
Flexural strength of the CaCO3–polymer nanocomposite sample compared with strengths of limestone and CaCO3 produced by hydrothermal hot pressing.


## 4. Conclusion

A novel process for generation of a CaCO3–polymer nanocomposite with a controlled three-dimensional shape was developed. The nanocomposite consisted of large amounts of CaCO3 (aragonite) dispersed in a polymer matrix at the nanometer scale. The nanocomposite had excellent mechanical properties; its flexural strength was larger than the flexural strengths of limestone and CaCO3 produced by hydrothermal hot pressing. The use of supercritical CO2 facilitated CO2 dissolution, which resulted in rapid precipitation of CaCO3 in the polymer matrix. This process has potential utility for fixation of CO2.



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*Source: 9783941-2018-08-01.xml*