Biomedical applications of calcium carbonate minerals have been receiving an increasing amount of attention. With a simple chemical composition, low production cost, and ease to produce in large quantities, this non-toxic (bio)mineral has been used preferentially in the pharmaceutical industry as a diluent, bulking or coating agent. Recently, novel products have been developed and amorphous calcium carbonate was successfully used as a hybrid carrier for drugs, proteins and genes. It is obvious that any impurities might have adverse effects in any of the aforementioned applications. However, the synthesis of impurity-free amorphous calcium carbonate often proves to be challenging due to its instability and rapid transformation to crystalline phases. Herein, we describe a novel, simple and scalable protocol for the synthesis of such impurity-free amorphous calcium carbonate nanoparticles that is potentially invaluable for critical health applications, improving the applicability of amorphous calcium carbonates in pharmaceutical and medical domains.


The crystallization of CaCO3 has been extensively investigated due to its technological applications and its importance in the formation of biogenic minerals. Calcium carbonate is a model system in which intermediate precursor phases such as pre-nucleation clusters, liquid and solid amorphous precursor phases were shown to occur prior to crystalline phases (Gebauer et al., 2008; Kellermeier et al., 2016; Sebastiani et al., 2017). Among these precursor phases, amorphous calcium carbonate (ACC) plays a pivotal role as an intermediate in the formation of crystalline calcium carbonate polymorphs (Politi et al., 2004; Weiner et al., 2005; Cartwright et al., 2012). Consequently, ACC has drawn a great deal of attention over the last decades resulting in many studies focussed on its formation, structural characterization, and transformation to different crystalline CaCO3 polymorphs. A wide variety of ACC species with diverse hydration level and/or characteristics of short-range order exists, which seems to play a decisive role on the resulting CaCO3 crystalline phase (Gebauer et al., 2008, 2010; Goodwin et al., 2010; Cartwright et al., 2012; Rez et al., 2014; Schmidt et al., 2014; Malini et al., 2016; Sun et al., 2016; Tobler et al., 2016). In the natural environment, species forming biominerals have exploited the tuneable features of amorphous phases and used them as un-differentiated material that will later undergo transformation and specialisation, ultimately forming their shells, teeth or skeleton (Addadi et al., 2003).

Because amorphous precursors can be modified and easily produced at industrial scales, amorphous calcium carbonate mineral phases, possessing intrinsic degradability at acidic pH values, are promising materials that can be used in many domains such as medicine, e.g., as novel cancer drug delivery systems, for the removal of heavy and toxic metal ions from water, or in materials science for the design of advanced hybrid and nano-composite materials possessing novel physical and optical properties (Cai et al., 2010; Meiron et al., 2011; Lee et al., 2012; Xue et al., 2012; Forsgren et al., 2013; Gebauer, 2013; Qi et al., 2014a and b; Farhadi-Khouzani et al., 2015; Tewes et al., 2016; Blue et al., 2017; Schmidt & Wagermaier, 2017; Wang et al., 2017, 2018; Xiao & Tang, 2017; Croitoru et al., 2018).

Given this wide range of applications, a need for an easy and reliable precipitation protocol is obvious. Many studies focussed on these issues and several precipitation protocols can be found in the literature using in- or outgassing diffusion methods, direct precipitation by rapid mixing of saturated solutions, hydrolysis of alkyl carbonate in presence of calcium ions, or direct bubbling of calcium chloride or calcium hydroxide solutions with gaseous CO2 (Becker et al., 2003; Loste et al., 2003; Faatz et al., 2004; Günther et al., 2005; Pouget et al., 2009; Bang et al., 2011; Wang & Xu, 2013; Gebauer et al., 2013; Ihli et al., 2013a and b, 2014; Rodriguez-Navarro et al., 2015; Farhadi-Khouzani et al., 2015, 2016). However, most of the amorphous precipitates obtained with the various protocols reported in the above cited publications are formed from sodium- or chloride-based reactants and hence present traces of impurities being incorporated during the crystallisation or quenching process. It has to be noted that the Kitano protocol based on the slow release of carbon dioxide from a saturated solution of calcium bicarbonate allows the preparation of impurity-fee amorphous or crystalline calcium carbonates (Kitano et al., 1962; Wolf et al., 2008); however, the accessible quantities are rather limited. Related protocols were adapted for the production of precipitated calcium carbonate (PCC) on industrial scales, but typically yield micrometre-sized crystalline particles with versatile use in a wide range of plastic and elastomeric applications (Vogel et al., 2012). Hence, a method for the preparation of impurity-free, nanoscale ACCs in large quantities is still missing. From a general point of view, impurities present a potential limitation and a major challenge as they can have pharmacological or toxicological relevance for the human body but also critically impact the quality of drug products. With the current development of calcium carbonate-based drug delivery systems, the necessity for developing impurity-free ACC phases appears to be essential and has the potential to enhance drug performances and bioavailability (Pan et al., 2011; Qi et al., 2014a and b; Tewes et al., 2016; Wang et al., 2017, 2018). Herein, we addressed these issues and present a novel protocol for the preparation of disordered, stable over several days in low humidity environment and several months in acetone, tuneable, chemical impurity-free, hydrated amorphous calcium carbonate possessing a size range of 155 ± 50 nm. The protocol is in principle scalable, allowing gram scale production.

Materials and methods


Amorphous calcium carbonate was precipitated by stepwise addition of water enriched in carbon dioxide to a saturated calcium hydroxide solution (KspCa(OH)2 = 5.5 × 10−6; Miller & Witt, 1928). For the preparation of the CO2-enriched solution, MilliQ water set at 7 °C was bubbled with CO2 for 30 min 50 mL of calcium hydroxide set at 7 °C were placed into a plastic beaker and the pH was monitored with a Metrohm pH electrode (model 6.0256.100). The CO2-saturated water was added drop-by-drop to the calcium hydroxide solution at a rate of 10 to 12 mL min−1 until the pH dropped from 12.43 (pH of the Ca(OH)2 saturated solution) to pH 10.00. The milky solution was poured into a mixture of 75% acetone and 25% absolute ethanol (initial calcium hydroxide to acetone/absolute ethanol volume ratio 1:20) contained in a plastic beaker that was afterwards sealed with ParafilmTM and stirred with a magnetic stirrer for 3 min. The solution was left to settle for half an hour after removing the magnetic stirrer. The sedimented amorphous calcium carbonates were then transferred into a falcon tube and centrifuged at 9000 r/min for 10 min in a benchtop centrifuge. The supernatant solution was carefully removed, the ACC nanoparticles re-suspended in acetone and centrifuged again. Half of the precipitated total particle weight was stored in acetone and the other half dried under dynamic vacuum conditions at 40 °C for further characterization. Different ratios of acetone and absolute ethanol for quenching were tested and the above-mentioned proportion proved to provide narrow size distribution of amorphous calcium carbonate nanoparticles (Fig. S1 in Supplementary Material linked to this article and freely available at A single synthesis procedure produced ~100 mg of pure amorphous calcium carbonate. Because this synthesis is essentially based on addition rates and volumes of reactants, it is obvious that this protocol can be up-scaled towards gram scales, if not industrial scales, if required.

Scanning electron microscopy

A Zeiss CrossBeam 1540 XB scanning electron microscope (SEM) was used to examine the samples in secondary-electron imaging mode. An accelerating voltage of 15 kV was used. Because calcium carbonate is not conductive, images quality is highly dependent on the size and morphology of the samples, therefore powders of ACC were sprinkled onto carbon adhesive tapes and coated with a thin layer of gold (approx. 10 nm). For elemental characterization, energy dispersive X-ray analysis (EDX) of calcium carbonate deposited on TEM grids was realised on a benchtop SEM (TM3000, Hitachi) at 15 kV.

Transmission electron microscopy

Transmission electron microscopy (TEM) images where acquired using an in-column Omega filter microscope Zeiss Libra 120 at 120 kV accelerating voltage, possessing a point resolution of 0.34 nm. Particles were collected for TEM observations by dipping carbon-film-coated copper grids into the ACC/acetone dispersions. Grids were dried in air and immediately analyzed by TEM.

Thermogravimetric analysis

Thermogravimetric analysis was performed on a NETZSCH STA 449 F3 Jupiter equipment under nitrogen atmosphere to limit crystallization of the samples when exposed to atmospheric conditions. Ten milligrams were positioned in the sample holder. The analysis was performed between room temperature and 900 °C with a heating rate of 10 K/min. Prior to all measurements, a calibration was performed using the calibration kit available with the instrument. All measurements were baseline corrected by the curves obtained by placing the empty crucible in the sample holder and heating in the same manner as during the actual measurement. For all measurements, the same starting mass of 10 mg was used. A stand-by mode was applied for 15 min in order to limit temperature fluctuations and accurately establish the initial weight values using the build-in microbalance under dry gas flow. The standard error associated with the apparatus is ±1.5 wt%.


ATR-FTIR spectra of the precipitated particles were recorded on a Perkin Elmer spectrometer 100 equipped with a diamond ATR crystal from 760 to 4000 cm−1 with a resolution of 1 cm−1, allowing the detection of the characteristic calcium carbonate bands denoted ν1, ν2, ν3 and ν4 according to the symmetric stretch, out-of-plane bending, asymmetric stretch and in-plane bending vibrational modes, respectively.

Heat treatment of amorphous calcium carbonate

Amorphous calcium carbonate was placed on a tube oven under N2 flow and heated up to 150 °C and 250 °C at a heating rate of 10 K/min into a Nabertherm oven equipped with a P320 controller, collected after cooling down and measured via ATR-FTIR. The FTIR scans were normalised based on the intensity of the ν3 band allowing direct comparison of FTIR spectra.

Results and discussion

The SEM, EDX and TEM analysis of the dried precipitates show spherical and amorphous CaCO3 particles. An estimation of the size distribution was performed by measuring the size of 120 spherical particles over five different SEM micrographs. The size distribution shows an average value of 155 ± 50 nm (Figs. 13). The diffuse rings in the selected-area electron diffraction (SAED) pattern confirm that the particles are truly amorphous. Within the limits of SEM and TEM techniques, no traces of crystalline calcium carbonate forms were seen. The EDX elemental analyses (Fig. 4) were realised on the same samples used for TEM analysis, confirming the presence of C, O, Ca (Al is present due to the SEM sample holder and Cu due to the TEM grid).

Characteristic infrared bands of carbonate are reported in the literature, the ν1 band corresponding to the symmetric stretching, the ν2 band to the out-of-plane bending, the ν3 band to the anti-symmetric stretching and the ν4 band to the in-plane bending vibrational modes. Such vibrational bands occur for the precipitated ACC samples between 1065 and 1075 cm−1 for the ν1 band, at 860 cm−1 for the ν2 band, between 1065 and 1075 cm−1 for the ν3 band and a broad band at ~700 cm−1 accounting for ν4 (Fig. 5). The last band is significantly broader in ACC than in crystalline polymorphs due to the superposition of the carbonate vibrational mode ν4 with a broad feature due to the hindered rotation of water molecules (Freda et al., 2005). The ν4 band is extremely sensitive to the absence of medium- to long-range order as typically found in amorphous calcium carbonates (Brečević & Nielsen, 1989; Loste et al., 2003; Günther et al., 2005; Gueta et al., 2007). Traces of structural water are observed at ~ 3300 cm−1, 1640 cm−1 and ~700 cm−1 (Fig. 6) corresponding to O–H stretching modes, HOH bending mode and hindered rotation of water molecules, respectively (Addadi et al., 2003; Gebauer et al., 2010; Farhadi-Khouzani et al., 2015). Quantitative discrimination between structural and absorbed water based only on band analysis is difficult, thus thermogravimetric analysis (TGA) was performed.

The TGA (Fig. 7) shows that the precipitated amorphous calcium carbonate contains approximately 1 mol of H2O per mol of CaCO3, which can be subdivided into 65% weakly and 35% strongly bound populations, as evident from the two steps of weight-loss between 30 °C and 350 °C (Radha et al., 2010; Bushuev et al., 2015; Jensen et al., 2018). The analysis of the mass ratio upon decomposition of anhydrous calcium carbonate into calcium oxide and calcium carbonate follows: 

Analysis of the residual mass from calcium carbonate decomposition into calcium oxide and gaseous carbon indicates that the analysed samples present statistically no impurities (outside of the potential one present in calcium hydroxide reactants). Consequently, the samples are initially composed of 100% hydrated calcium carbonate of the form CaCO3–H2O, which is consistent with the EDX analysis presented above (Fig. 4).

The dehydration capacity of the impurity-free ACC before crystallisation was tested by heating a few milligrams up to 150 °C and 250 °C. The FTIR spectra were normalised to the ν3 band intensities. Estimation of the water content upon dehydration was done by a systematic estimation of the water band intensity at 3300 cm−1aq) at the different temperatures. Dehydration is expressed in percentages and compared with the maximum intensity of the νaq band of freshly prepared ACC at room temperature (Figs. 5 and 6). Samples heated to 150 °C lost about 78% of their structural water and present no traces of crystals as apparent from the slight shift of the ν2 vibration band from 862 to 860 cm−1. Changes of the ν4 vibration band upon heating similarly reflect the change of hydrated water with the appearance and sharpening of the ν4 double band at 699 and 730 cm−1. A further increase in temperature, up to 250 °C, removed all structural water, weakly and strongly bound, but induced a partial crystallisation of ACC into calcite (Fig. 5).


The presented protocol has proven to produce high yield impurity-free amorphous calcium carbonate via cautious mixing of calcium hydroxide and carbon dioxide-enriched water. The presented alternative mineralisation pathway intrinsically prevents the incorporation of chemical impurities such as sodium and chloride ions, which are often observed in ACC, because they are not present as spectator ions. Essentially, the purity of the obtained ACC is thus governed by the quality of the used chemicals (calcium hydroxide, water, and organic solvents). Different water contents were tuneable upon heating up to 150 °C without significant changes towards crystalline structures. Based on the increasing number of publications using ACCs in hybrid materials in various fields, such as industry, medicine, or materials science, this protocol, optimised towards purity, can be upscaled and may allow the development of enhanced synthetic ACC materials for future applications in e.g., hybrid drugs or drug delivery with improved bioavailability.


The authors thank the Deutsche Forschungsgemeinschaft (SFB1214, A2 and A7) and the Zukunftskolleg of the University of Konstanz for support.

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Supplementary data