Speleothem deposits are among the most valuable continental formations in paleoclimate research, as they can be dated using absolute dating methods, and they also provide valuable climate proxies. However, alteration processes such as post-depositional mineralogical transformations can significantly influence the paleoclimatic application of their geochemical data. An innovative sampling and measurement protocol combined with scanning and transmission electron microscopy, X-ray diffraction and Fourier transform infrared spectroscopy is presented, demonstrating that carbonate precipitating from drip water in caves at ~10 °C contains amorphous calcium carbonate (ACC) that later transforms to nanocrystalline calcite. Stable oxygen isotope fractionations among calcite, ACC and water were also determined, proving that ACC is 18O-depleted (by >2.4 ± 0.8‰) relative to calcite. This, in turn, has serious consequences for speleothem-based fluid inclusion research as closed system transformation of ACC to calcite may induce a negative oxygen isotope shift in fluid inclusion water, resulting in deterioration of the original compositions. ACC formation increases the speleothems’ sensitivity to alteration as its interaction with external solutions may result in the partial loss of original proxy signals. Mineralogical analysis of freshly precipitating carbonate at the studied speleothem site is suggested in order to determine the potential influence of ACC formation.
Speleothems (cave-hosted carbonate deposits) are among the most important climate archives, as their formation age, texture and geochemical composition provide information on temperature, amount of precipitation, and even seasonality, i.e. changes in the relative amount of precipitation during cold and warm seasons1. The preservation of the original climate-related signal (“proxy”) is therefore of crucial importance. The recrystallization and alteration of the original carbonate may significantly influence the commonly used U-Th age dating method, stable C and O isotope composition, as well as the distribution and isotope ratios of trace elements2,3,4,5.
A recent study6 has shown evidence for recrystallization-induced alteration processes that affected stable isotope compositions of inclusion-hosted water trapped in stalagmites. These were tentatively attributed to the formation of amorphous calcium carbonate (ACC) and its transformation to calcite. Potential effects of vaterite and aragonite formation has also been discussed and excluded by Demény et al.6 on the basis of available carbonate-water oxygen isotope fractionation relationships. Additionally, vaterite and aragonite has not been detected in the Baradla cave system, in spite of an extensive survey on different carbonate deposit types (freshly precipitated carbonate, stalagmites, flowstones, this study and Demény et al.6). As detected by the earlier study6, the stable hydrogen and oxygen isotope compositions (expressed as δD and δ18O values) of water trapped in the fluid inclusions of selected speleothems of the Baradla cave system shows that, whereas hydrogen isotope values reflect the composition of the cave drip water from which the carbonate precipitated, the oxygen isotope data of the inclusion-hosted water display increasingly negative shifts. The observed negative δ18O(water) shift starts from the stalagmite’s surface and increase inwards, towards the older layers. Although Demény et al.6 did not provide direct evidence for the presence of ACC in the stalagmites or on their surface, they did report the presence of nanocrystalline (<50 nm) calcite, from which ACC in the role of a precursor material may be inferred. According to experimental and empirical data, O isotope fractionation between ACC and water is smaller than that for crystalline carbonate7,8,9. Calcite crystallization could be responsible for driving the inclusion-hosted water in a negative direction, enabling it to reach the larger fractionation value, and thus could provide explanation for the observed negative δ18O shift6.
Detection of ACC is rather difficult in cave deposits, as ACC can undergo transformation to calcite in minutes in a hydrous environment, and even stabilizing compounds like Mg or organic matter10,11 are only capable of extending its stability to some weeks. Taking into consideration the general precipitation rate (0.1 to 1 mm per year), the collection of carbonate in appropriate amounts for mineralogical or geochemical analyses requires several months. Over the course of such a long collection time, however, the original ACC can be transformed into calcite. Although ACC preparation in the laboratory is a routine procedure12,13,14, its synthesis requires conditions distinctly different from those to be found in natural cave environments, e.g. mixing of CaCl2 and NaCO312,13 or (NH4)2CO314 solutions. Hence, the preparation conditions and characteristics of synthetic ACC render it inappropriate to function as an analogue of its natural counterpart, thus it cannot provide the information sought.
In the present paper, the issue of ACC vs. calcite precipitation was approached via the application of an innovative sample collection method in which transmission electron microscopy (TEM) grids and silica wool are placed directly under the dripping water in the studied caves. These sample holders were able to collect enough carbonate precipitate for mineralogical and isotopic analyses in relatively short times (24 hours and 2 weeks, respectively). This had the effect of allowing direct analyses without further sample concentration. Evidence is presented for ACC formation in natural cave environments and an estimate for calcite-ACC oxygen isotope fractionation at the studied cave temperature (10 ± 0.5 °C, the average temperature and its scatter of several sites in two caves) is provided.
Results and Discussion
The temperature, conductivity, pH values and stable isotope compositions of the drip water were recorded during sampling, as was the CO2 content of the cave air. These are listed in Table 1. Grids and silica wool samples were analysed for several sampling periods from the Baradla and the Pál-völgyi caves, but due to the very small amount of deposited material, only some of the grids yielded enough sample material to allow their study using a combination of methods. Grids that were placed under the drip waters for 24 hours could only be analysed using TEM, whereas the precipites collected for ~2 weeks could be studied employing a range of methods. Most of the grids showed traces of mainly clay minerals and idiomorphic calcite. However, CaCO3 was occasionally deposited in globular forms (Fig. 1) or thin films over lacey carbon (see later).
Fresh carbonate precipitate
FTIR spectroscopy, micro-focus XRD and TEM were used in order to characterize the structure of the carbonate precipitate. The FTIR spectra (Fig. 2) obtained for one of the grids (sample grid #2) were similar to that of the experimentally prepared ACC14. The splitting of peaks at 1393 and 1460 cm−1 wave numbers was observed, matching the data in the literature reported for ACC15 (1384 and 1472 cm−1). The wide peak centered on 1635 cm−1 indicates molecular water15, and the series of peaks between 800 and 1200 cm−1 is consistent with spectra obtained for clay minerals16.
The same grid that yielded the characteristic ACC FTIR spectrum was also analysed by means of micro-focus XRD. A 2Θ range of 20 to 50° was selected because this range is uniquely capable of defining ACC13. The sample showed no traces of calcite, but a broad hump with a maximum at ~31.6° 2Θ (Fig. 3), matching both the shape and the maximum of experimentally precipitated ACC11,13.
TEM analysis of the fresh precipitates showed either a thin (10–40 nm), commonly hollow, CaCO3 film consisting of 10–30 nm size rounded clusters (Fig. 4a,b) or 20–40 nm size particles (Fig. 4c), similar to published ACC TEM images17. The clusters contain <5 nm Cu nanocrystals, which probably originated from the alteration of the copper grid. The SAED patterns of the CaCO3 films showed poorly resolved diffuse rings, consistent with the diffraction characteristic of ACC. The SAED pattern of the small particles indicated the presence of CaO (lime). Lime may act as a proxy for ACC as interaction between the electron beam and ACC may release CO2, resulting in the formation of lime17. The upper particle size of the fresh precipitate matches with the average size (40 nm) of the calcite nanocrystals reported in the outermost layer of recently forming stalagmites6.
SEM pictures were taken of grids immediately after collection and again with the same samples after about 3 weeks’ storage in a refrigerator. The analysis of the fresh samples revealed the formation of globular CaCO3, while this form had disappeared after 3 weeks, being replaced by porous, crystalline carbonate (Fig. 5).
FTIR analyses of the stored grid with recrystallized carbonate match with that of calcite, no ACC-like spectra were observed. The formation of porous calcite is in accordance with the transformation of ACC to calcite. Since the ACC contains up to one H2O molecule per formula unit14, and the molar volume of ACC (73 cm−3 mol−1) exceeds the sum of molar volumes of calcite (36 cm−3 mol−1) and water (18 cm−3 mol−1)18, the transformation results in a significant porosity in the newly formed calcite. Intermediate CaCO3 polymorphs (line vaterite) may also be formed during the transformation process, depending on pH and Mg concentration in the parent solution11. In this study only the precursor ACC and the product calcite formations were detected. The occurrence of the precursor and the product phases allowed us to develop a new sampling and measurement protocol for the preservation of possible ACC fraction and to determine the ACC oxygen isotope composition compared to calcite. Although the formation of intermediate phases like vaterite11 may affect the crystallization process, the isotope fractionation values would not be influenced6, hence the simplified transformation model (from a precursor phase of ACC to a product phase of calcite) can be used for the evaluation of the isotope data.
In general, during stalagmite formation, ACC-calcite transformation may occur in a closed or open system. If the ACC particles are on the stalagmite surface in contact with drip water during the transformation, then we can assume a fully open system, and hence the calcite attains equilibrium with the ambient water through a dissolution-reprecipitation process. If the precipitated ACC particles are covered by the subsequent carbonate layers (containing ACC and calcite), then the transformation may proceed in a closed system, through solid phase recrystallization. The possibility of ACC entrapment can be evaluated in the light of ACC particle sizes and the rate of carbonate deposition. If the thickness of the carbonate layer formed during the period of ACC transformation significantly exceeds the size of ACC particles, then the latter can be – at least partially – embedded. As ACC was detected in the freshly precipitated carbonate several days after the collection, we can assume that the transformation period is extended to days. Carbonate deposition rates can be estimated from the sizes (5 and 7 cm in height) and formation ages (~50 and ~210 years, respectively) of actively forming stalagmites (NU-1 and NU-2) at the sampling site6, yielding 0.3 to 1 mm yr−1 deposition rates, i.e., deposition of 800 to 2700 nm thick carbonate layers per day. At such deposition rates 10–30 nm sized ACC particles can be trapped in the precipitated carbonate layer that precludes interaction with the ambient solution resulting in closed system ACC-calcite transformation. However, heterogeneous carbonate precipitation on the rugged stalagmite surface and temporal variation of the deposition rate produces spatially variable carbonate formation and hence can leave a part of the ACC uncovered. Hence, the most plausible assumption is that the ACC-calcite transformation during stalagmite formation at the study site takes place both in closed and open systems.
Calcite-ACC oxygen isotope fractionation
In order to evaluate the influence of ACC formation on the use of stable oxygen isotope compositions in speleothem research, calcite-ACC oxygen isotope fractionation was determined by measuring the carbonate content of grids and silica wool placed directly beneath dripping water. Since the carbonate precipitated on the copper grids and silica wool is a mixture of calcite and ACC, the oxygen isotope composition of the calcite component should be determined along with the measurement of water composition. Hence, the stable isotope composition of the outer, ~3 mm thick part of a recently forming stalagmite (sample NU-2) collected at the Baradla Cave6 study site was also measured. Based on XRD and FTIR analyses, this stalagmite’s carbonate is composed of calcite (Figs 2 and 3). Since the stalagmite was actively growing at the time of collection, the oxygen isotope compositions of the stalagmite and the drip water can provide the calcite-water isotope fractionation value for the study site. The current fractionation value depends on temperature, pH conditions, growth rate, degassing and drip rates19,20,21,22, resulting in site-specific carbonate-water oxygen isotope fractionation relationships. Kinetic fractionation due to CO2 degassing and H2O evaporation related to strong ventilation can significantly affect the stable C and O isotope compositions of the precipitating carbonate23. If the transforming carbonate is in contact with an ambient solution whose composition is subject to change due to degassing and evaporation, then this solution may influence the O isotope composition of the newly formed calcite by resulting in elevated δ18O values. The potential influence of degassing and evaporation at the study site can be determined by conducting the so-called Hendy test24 on recently forming stalagmites. The results (presented and discussed in the Supplementary Material) indicate that, although carbon isotope composition naturally records the degassing effect (which is inherent in the carbonate precipitation process), it is not associated with systematic δ18O shifts. This observation does not imply that the carbonate precipitated in thermodynamic equilibrium with the drip water, but it shows that the degassing/evaporation effect may be considered negligible at the site and hence its influence on the carbonate–water system can be excluded.
The δ18O values of the NU-2 stalagmite calcite (23.4‰) and the drip water (−9.5‰) yields a site-specific fractionation value of 32.7 for the longer term (about 2 years) cave temperature (9.7 °C). Slight variations in cave temperature and drip water composition at the sampling site, however, may influence the oxygen isotope composition of the precipitating carbonate, hence current conditions prevailing during sample collection should be used for the evaluation. The theoretical oxygen isotope composition of the calcite component of the carbonate sample can be calculated from formation temperature and drip water composition, provided that the calcite-water oxygen isotope fractionation equation is known. Although a pioneering experimental study determined the temperature-fractionation relationship for the calcite-water system almost 50 years ago25, the definition of the true equilibrium calcite-water fractionation equation is still a hotly-debated topic22. Fractionation equations have been obtained using three different approaches: theoretical calculations, experimental analyses and empirical observations. Statistical mechanical calculations based on internal vibration frequencies yielded theoretical fractionation equations26,27 that may represent thermodynamic equilibrium. Experimental studies provided different equations25,28,29 depending on the experimental conditions (temperature range, precipitation mechanism, pH, growth rate)19,22, which may be distinctly different from those prevailing in natural environments. The third approach is empirical observations, i.e., measurement of calcite-water oxygen isotope fractionation for actively precipitating calcite in different environments (e.g. caves or thermal water occurrences)30,31,32,33. This approach bears most uncertainties as the precipitation conditions are not controlled, but the obtained equations contain all the unknown factors that govern calcite precipitation and may be most effectively applied as environment-specific relationships. Due to the large differences between theoretical, experimental and empirical equations, two empirical equations were selected as most representative for the studied caves’ environment. The formation conditions of the Devil’s Hole calcite (very low deposition rate in a closed environment) may be considered a closest-to-natural equilibrium31. Although the Coplen equation30 is based only on one fractionation value at 33.7 °C and a slope acquired from earlier studies, its applicability to extension to lower temperatures has been verified by later studies22,34, therefore the Coplen equation30 was selected to represent calcite-water equilibrium:
The other selected study32 is based on a comprehensive collection of real speleothem data, representing general cave environments that collectively contain all the natural factors which may have an effect (see above):
Since the α fractionation factor is the ratio of 18O/16Occ/18O/16Owater, by definition:
where “cc” stands for calcite.
Weighting equations (1) and (2) by a factor of 65 and 35%, respectively, would yield the observed calcite-water fractionation value of 32.7‰ at 9.7 °C. Current cave air temperatures (10.42, 9.34 and 9.27 °C) detected at the time of sample collections (Table 1) were substituted in equations (1) and (2) followed by a 65–35% weighing of the calculated 1000 · lnα values, as described above. Then the theoretical calcite oxygen isotope compositions were calculated using equation (3) and the measured water compositions (−9.1, −9.3 and −9.8‰), yielding δ18Occ values of 23.8‰, 23.7‰ and 23.1‰ for the Baradla Cave grids, silica wool and the Pál-völgyi Cave silica wool samples, respectively. The composition of the ACC component in the sampled carbonate could be determined by simple mass balance calculation as follows, provided that the ACC amount in the precipitating carbonate is known.
The amount of the ACC component can be estimated on the basis of crystallinity data of actively forming stalagmites. Demény et al.6 presented XRD FWHM (full width at half maximum) data that showed a continuous decrease (from 0.16 to 0.12) from the stalagmite surface to the inner (older) layers for actively growing stalagmites collected in the close vicinity (within 50 m) of the sampling site of this study. FWHM values may depend on crystal domain size and lattice strain, but due to the absence of significant amounts of substituting ions or organic matter and physical deformation, the lattice strain effect can be excluded6. Attributing the observed peak broadening solely to domain size increase and using the classical Scherrer equation35 for the calculation, a domain size change from 55 nm to 70 nm would be obtained at the stalagmite surface and the innermost part of the NU-2 stalagmite, respectively. TEM analyses showed that the youngest layers contained nanocrystalline (<50 nm) calcite, whereas the oldest laminae were dominated by well crystallized carbonate6. As the presence of an amorphous carbonate fraction in the fresh precipitate has been proven by various methods, we suggest that the ACC fraction served as a precursor for the nanocrystalline calcite aggregates. Since ACC clusters are about 10–40 nm in size, a similar crystal size can be assumed for the initial nanocrystalline calcite. The 70 nm size can be attributed entirely to well crystallized calcite (Scc), whereas the 55 nm average size (Savg) at the stalagmite surface would be determined by the size and the amount of ACC-derived nanocrystalline calcite (SACC and XACC, respectively) according to a simple mass balance equation:
The size estimations (Scc = 70 nm, Savg = 55 nm, SACC = 10–40 nm) determine the amount of the nanocrystalline fraction (XACC) that ranges from 0.25 to 0.5. Since a part of this size fraction can be precipitated originally as nanocrystalline calcite, the 25–50% range represents an upper limit to the ACC amount estimation. The ACC amounts and the theoretical calcite composition (δ18Occ) can be used to calculate the isotopic composition of the ACC fraction (δ18OACC) using the equation
For the Baradla grid and silica wool samples, the calcite end-member composition calculations (using the calcite-water fractionation relationships and measured cave temperatures as described above) yielded 23.8 and 23.7‰, whereas the Pál-völgyi Cave site yielded 23.1‰. Substituting the 25–50% ACC amount in the carbonate mixture (XACC = 0.25 to 0.5) in equation (5), an average calcite-ACC δ18O difference of 2.4 ± 0.8‰ is obtained. As a part of the nanocrystalline fraction may also be precipitated originally as calcite, the XACC values are maximum estimations, and lower XACC values would yield larger calcite-ACC δ18O differences. An additional source of uncertainty derives from the partial transformation of ACC to calcite during the storage period between sample collection and isotope analyses. Although the low temperature in the refrigerator (2–5 °C) precludes solid-phase carbonate-water oxygen isotope exchange, structural reorganization during calcitization may also be associated with isotope exchange between the newly formed calcite and ambient water (containing the released hydration water and the ambient H2O vapor). At such low temperatures, calcite-water isotope fractionation is elevated relative to the studied cave’s temperature (~10 °C)25, leading to 18O-enrichment in the calcite. The presence of such newly formed calcite would mean that the original carbonate sample should have had lower δ18O value than measured, and consequently the calculated calcite-ACC difference should be larger. Transformation of ACC to calcite during sample storage also leads to the assumption that the calcite-ACC difference (~2.4‰) represents a lower limit.
Uncertainties in the estimation of ACC amount is a major weakness in the fractionation calculation, hence the verification of calcite-ACC fractionation estimation requires independent information provided either by experimental studies or by natural analogues. The experimental determination of ACC-water oxygen isotope fractionation representative for speleothem formation is challenging because (i) ACC rapidly transforms to calcite during the preparation and (ii) laboratory ACC synthesis requires physical and chemical conditions distinctly different from those found in a cave environment. Available estimations of δ18O differences between crystalline and amorphous carbonates formed in natural environments suggest that the crystalline carbonate is several ‰ more enriched in 18O than its amorphous counterpart (dolomite7, aragonite8, Mg-calcite9). These estimations are in agreement with the result of the present study, which suggests a >2.4‰ calcite-ACC δ18O difference at ~10 °C.
Implications for paleoclimate research
As a general rule, speleothems with well developed lamination and compact texture (non-porous texture with columnar or fibrous crystals) are selected for paleoclimate analyses36,37, as they are less prone to diagenetic alteration. The formation of a porous texture and late-stage re-crystallization both enhance post-depositional exchange with ambient solutions, leading to changes in the original stable isotope and trace element compositions2,3,4 during open system alteration. The formation of relatively 18O-depleted ACC and its subsequent transformation into calcite can also exercise an especially significant effect in fluid inclusion research, inducing oxygen isotope re-equilibration between the host carbonate and water trapped in fluid inclusions6 if the mineralogical transformation took place in a closed system. In general, primary fluid inclusions are thought to derive from entrapment of drip water solution during carbonate precipitation. However, in the present case hydration water released during ACC transformation to calcite may also be trapped, contributing to the inclusion-hosted water content. As pointed out above, fast deposition of primarily precipitated calcite may cover and enclose a part of ACC that is later transformed within the calcite host in a closed system. The fluid inclusions within or in contact with ACC would approach the calcite-water oxygen isotope equilibrium during the transformation and subsequent re-crystallization6. As the amount of water is negligible compared to the host carbonate, the inclusion water composition would be forced to shift to more negative δ18O values in order to achieve the larger calcite-water fractionation relative to the ACC-water value. As discussed by Demény et al.6, speleothems from warm/tropical regions frequently yield meaningful δ18O values for inclusion-hosted water, whereas the oxygen isotope compositions of inclusion-hosted water obtained for samples from cold/temperate regions are generally not appropriate for paleotemperature calculations6. A potential reason for this discrepancy is formation of ACC in cold/temperate caves whose transition to calcite induces δ18O shifts in the inclusion water6. The present study provides direct evidence for relatively 18O-depleted ACC formation in caves at about 10 °C. Since the δ18O value of inclusion-hosted water may carry significant paleoclimatic/paleohydrological information, it is important to note that its use is limited by the cave environment.
Demand for future studies
A number of experimental studies have shown that the formation and stability of ACC may be influenced by the physical parameters of the ambient environment and the chemical compositions of the parent solutions. In natural cave environments the most important factors might be the cave temperature, drip water pH, as well as concentrations of Mg, SO42− and organic compounds in the solution10,11,15,38,39,40. A comprehensive study is suggested to cover several cave environments with different temperatures, ventilation degree, soil characteristics, drip water chemistry and carbonate growth rates in order to determine the exact factors governing ACC formation. The transition from ACC to calcite has been shown to take place in several steps with intermediate hydration states and mineral phases like vaterite12,13,14,17,41. Investigations on the ACC-calcite transition and its governing factors require monitoring of mineralogical changes at high temporal resolution. Additionally to the inorganic factors, the role of microbial activity should also be investigated. Amorphous carbonates are ubiquitously secreted by living organisms in sedimentary environments42, hence microbial mediated carbonate precipitation is also a potentially important process in ACC formation, whose exploration requires systematic biological/biochemical investigations.
The formation of ACC was detected in carbonate samples precipitated from drip water in cave environments monitored for temperature, drip water pH, conductivity and stable isotope compositions. In order to capture and analyse very small amounts of carbonate without further sample concentration, Cu grids used for TEM and quartz wool were placed under drip water for times ranging between 24 hours and two weeks at two cave sites (the Baradla and Pál-völgyi Caves, Hungary). Globular forms of carbonate were observed on the copper grids using SEM; these then transformed into porous carbonate after several weeks. FTIR spectra, X-Ray powder diffraction and TEM analyses of freshly precipitated carbonates collected on TEM Cu grids showed the characteristic features reported for synthetic ACC precipitates. ACC occurred as films containing clusters 10–30 nm in size and as particles 10–40 nm in size. It may be assumed that this material is capable of serving as a precursor of nanocrystalline calcite found in the outermost layer of recently formed speleothems6.
The stable oxygen isotope compositions of the freshly precipitating carbonate, stalagmite calcite and host drip water were used to infer oxygen isotope fractionation between calcite and ACC. The calcite-ACC isotope fractionation estimation obtained in this study (>2.4 ± 0.8‰) is in agreement with those obtained from the data contained in earlier publications8,9. These observations further support the earlier hypothesis6 that closed-system transformation of ACC into calcite induces oxygen isotope changes in the fluid inclusion water of stalagmites as the carbonate-water system approaches calcite-water equilibrium fractionation. The further implication of our results is that ACC transformation into nanocrystalline carbonate and the recrystallization of the latter to well crystallized calcite increases the chance of late-stage interactions with infiltrating solutions. This open-system carbonate-water interaction during re-crystallization can lead to – at least a partial – loss of primary geochemical signals, affecting the speleothems’ sensitivity to diagenetic alteration and their applicability to paleoclimate research. As temperature rises, the extent of ACC precipitation decreases7, hence ACC formation may be of particular importance in cold-temperate caves. Besides cave monitoring, the mineralogical analysis of freshly precipitating carbonate at the location of speleothem collection is suggested in order to determine the potential influence of ACC formation in the cave site under study.
Fresh carbonate precipitate was collected in two caves, the Baradla Cave in the northeastern part of Hungary, and the Pál-völgyi Cave in Budapest, central Hungary. Temperature, pH, conductivity, and CO2 content in cave air were monitored at both locations and water samples were collected. Cave air and water temperatures were measured using a GMH-3710 type Pt-100 thermometer digital puncture (range from −199.99 to +199.99 °C, resolution: 0.01 °C) with a precision of ±0.03 °C. CO2 contents in cave air at 150 cm from the ground were determined using different NDIR instruments for low (TESTO-535, range 0 to 10 000 ppm, resolution: 1 ppm) and high (ANALOX ASPIDA, range 0 to 10 vol%, resolution: 0.01 vol%) levels. Electrical conductivity and pH values of dripping water and cave river waters were measured within 1 minute after sampling using a COMBO PH & EC instrument (EC range 0 to 3999 μS/cm, resolution: 1 μS/cm, pH range 0.00 to 14.00, resolution: 0.01) with precisions of 2% and 0.05, respectively. Plastic funnels holding Cu grids and silica wool over a filter were placed under the dripwater at both caves. Grids and silica wool samples were collected from 24 hours to two weeks. The samples were immediately placed in a cold box and transported to the laboratory, where they were stored in a refrigerator at 2–5 °C. According to literature data, low temperature can help stabilizing ACC38.
X-ray powder diffraction (XRD) analysis of stalagmite carbonate (sample NU-2/1) was performed using a Philips PW-1730 diffractometer (PW-1820/00 goniometer) equipped with a graphite monochromator using Cu-Kα radiation at 45 kV and 35 mA with 1° divergence slit and 1° receiving slit. Scanning rate was 0.05° 2Θ per minute from 3° to 70°. Micro-focus X-ray diffraction measurements were made by using D/MAX RAPIDII type diffractometer and RINTRAPID software at the Institute for Geological és Geochemical Research (IGGR), Budapest. Measurement conditions were 50 kV accelerating voltage, 0.6 mA current, using a 800 micrometer beam collimator. The analysed Cu grid (grid #2) was held in a fixed position during measurement. The 2DP software was applied to convert the Debye-rings into 2theta intensity values with 0.01 steps.
FT-IR (Fourier-transformation infrared) analyses were carried out using a Bruker Vertex 70 IR spectrometer equipped with a Hyperion 2000 microscope with video-controlled visualization and automatized sample stage operated by OPUS 7.2 software, at the IGGR, Budapest. The measurements were performed in transmittance mode using a 15X objective. For each sample 32 scans were recorded in the 4000–400 cm−1 spectral range with a resolution of 4 cm−1.
TEM studies of the samples collected on the Cu grids were carried out in a Philips CM20 (accelerating voltage: 200 kV, LaB6-filament) type transmission electron microscopes at Institute of Technical Physics and Materials Science of the Centre for Energy Research, Budapest. Bright-field images and selected area diffraction (SAED) patterns were recorded on CCD camera (Morgagni microscope) and image plates (Philips microscope). Radial distributions of intensities were generated from SAED patterns following the method described by Lábár43 and using the ProcessDiffraction software. Scanning electron microscope images were acquired by using a ZEISS EVO 40XVP Scanning Electron Microscope (accelerating voltage: 20 kV, W-filament, working distance 10 mm) at the Institute of Materials and Environmental Chemistry, Budapest.
Carbonate-bearing Cu grids and silica wool samples were divided to several sub-samples and placed in borosilicate exetainers, flushed with helium and reacted with pure H3PO4 at 70 °C in an automated GASBENCH II preparation unit44 attached to a Thermo Finnigan delta plus XP mass spectrometer at the IGGR, Budapest. Due to the accidental carbonate precipitation the CO2 yields were variable. The sample signals were monitored and samples below 50 μg and above 200 μg were excluded in order to match the standards’ signal (for about 150 μg calcite) and to avoid linearity related isotope shifts. Stable carbon and oxygen isotope compositions were determined on the evolved CO2 and are expressed as δ13C and δ18O in ‰ relative to V-PDB and V-SMOW, respectively. Precision and accuracy of stable carbon and oxygen isotope compositions were tested by analysing international standards that yielded the following compositions. NBS-18: δ13C = −5.03 ± 0.06‰, δ18O = −23.29 ± 0.07‰ (n = 16); NBS-19: δ13C = −1.92 ± 0.07‰, δ18O = −2.22 ± 0.04‰ (n = 16); LSVEC: δ13C = −46.60 ± 0.16‰, δ18O = −26.60 ± 0.08‰ (n =17), all of the values within 0.1‰ from the certified compositions reported by the International Atomic Energy Agency. Stable oxygen isotope compositions of drip water samples (δ18Ow values relative to V-SMOW) were determined using a liquid water isotope analyser (LWIA) manufactured by Los Gatos Research Ltd, model LWIA-24d with an analytical precision of 0.1‰6.
How to cite this article: Demény, A. et al. Formation of amorphous calcium carbonate in caves and its implications for speleothem research. Sci. Rep. 6, 39602; doi: 10.1038/srep39602 (2016).
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Fairchild, I. J. & Baker, A. Speleothem Science: From Process to Past Environments. 450 (Wiley-Blackwell, 2012).
Martín-García, R., Alonso-Zarza, A. M., Martín-Pérez, A., Schröder-Ritzrau, A. & Ludwig, T. Relationships between colour and diagenesis in the aragonite-calcite speleothems in Basajaún Etxea cave, Spain. Sed. Geol. 312, 63–75 (2014).
Scholz, D. et al. Diagenesis of speleothems and its effect on the accuracy of 230Th/U-ages. Chem. Geol. 387, 74–86 (2014).
Zhang, H., Cai, Y., Tana, L., Qina, S. & Ana, Z. Stable isotope composition alteration produced by the aragonite-to-calcite transformation in speleothems and implications for paleoclimate reconstructions. Sed. Geol. 309, 1–14 (2014).
Giuffre, A. J., Gagnon, A. C., De Yoreo, J. J. & Dove, P. M. Isotopic tracer evidence for the amorphous calcium carbonate to calcite transformation by dissolution–reprecipitation. Geochim. Cosmochim. Acta 165, 407–417 (2015).
Demény, A. et al. Recrystallization-induced oxygen isotope changes in inclusion-hosted water of speleothems – Paleoclimatological implications. Quaternary International 415, 25–32 (2016).
Schmidt, M., Xeflide, S., Botz, R. & Mann, S. Oxygen isotope fractionation during synthesis of CaMg-carbonate and implications for sedimentary dolomite formation. Geochim. Cosmochim. Acta 69, 4665–4674 (2005).
Rollion-Bard, C., Blamart, D., Cuif, J.-P. & Dauphin, Y. In situ measurements of oxygen isotopic composition in deep-sea coral, Lophelia pertusa: Re-examination of the current geochemical models of biomineralization. Geochim. Cosmochim. Acta 74, 1338–1349 (2010).
Mavromatis, V., Schmidt, M., Botz, R., Comas-Bru, L. & Oelkers, E. H. Experimental quantification of the effect of Mg on calcite-aqueous fluid oxygen isotope fractionation. Chem. Geol. 310–311, 97–105 (2012).
Bentov, S., Weil, S., Glazer, L., Sagi, A. & Berman, A. Stabilization of amorphous calcium carbonate by phosphate rich organic matrix proteins and by single phosphoamino acids. J. Struct. Biol. 171, 207–215 (2010).
Rodriguez-Blanco, J. D., Shaw, S., Bots, P., Roncal-Herrero, T. & Benning, L. G. The role of pH and Mg on the stability and crystallization of amorphous calcium carbonate. J. Alloys Compd. 536S, 477–479 (2012).
Shen, Q. et al. Properties of amorphous calcium carbonate and the template action of vaterite spheres. J. Phys. Chem. B 110, 2994–3000 (2006).
Rodriguez-Blanco, J. D., Shaw, S. & Benning, L. G. The kinetics and mechanisms of amorphous calcium carbonate (ACC) crystallization to calcite, via vaterite. Nanoscale 3, 265–271 (2011).
Ihli, J. et al. Dehydration and crystallization of amorphous calcium carbonate in solution and in air. Nat. Commun. 5, 3169 doi: 10.1038/ ncomms4169 (2014).
Loste, E., Wilson, R. M., Seshadri, R. & Meldrum, F. C. The role of magnesium in stabilising amorphous calcium carbonate and controlling calcite morphologies. J. Cryst. Growth 254, 206–218 (2003).
Madejová, J. FTIR techniques in clay mineral studies. Vib. Spectrosc. 31, 1–10 (2003).
Rodriguez-Navarro, C., Kudlacz, K., Cizer, Ö. & Ruiz-Agudo, E. Formation of amorphous calcium carbonate and its transformation into mesostructured calcite. CrystEngComm 17, 58–72 (2015).
Bolze, J., Peng, B., Dingenouts, N., Panine, P., Narayanan, T. & Ballauff, M. Formation and growth of amorphous colloidal CaCO3 precursor particles as detected by timeresolved SAXS. Langmuir 18, 8364–8369 (2002).
Dietzel, M., Tang, J., Leis, A. & Köhler, S. J. Oxygen isotopic fractionation during inorganic calcite precipitation — Effects of temperature, precipitation rate and pH. Chem. Geol. 268, 107–115 (2009).
Day, C. C. & Henderson, G. M. Oxygen isotopes in calcite grown under cave-analogue conditions. Geochim. Cosmochim. Acta 75, 3956–3972 (2011).
Feng, W., Banner, J. L., Guilfoyle, A. E., Musgrove, M. & James, E. W. Oxygen isotopic fractionation between drip water and speleothem calcite: A 10-year monitoring study, central Texas, USA. Chem. Geol. 304–305, 53–67 (2012).
Watkins, J. M., Hunt, J. D., Ryerson, F. J. & DePaolo, D. J. The influence of temperature, pH, and growth rate on the δ18O composition of inorganically precipitated calcite. Earth Planet. Sci. Lett. 404, 332–343 (2014).
Mickler, P. J., Stern, L. A. & Banner, J. L. Large kinetic isotope effects in modern speleothems. GSA Bull. 118, 65–81 (2006).
Hendy, C. H. The isotopic geochemistry of speleothems 1. The calculation of the effects of the different modes of formation on the isotopic composition of speleothems and their applicability as palaeoclimatic indicators. Geochim. Cosmochim. Acta 35, 801–824 (1971).
O’Neil, J. R., Clayton, R. & Mayeda, T. Oxygen isotopic fractionation in divalent metal carbonates. J. Chem. Phys. 51, 5547–5558 (1969).
Horita, J. & Clayton, R. N. Comment on the studies of oxygen isotopic fractionation between calcium carbonates and water at low temperatures by Zhou and Zheng (2003; 2005). Geochim. Cosmochim. Acta 71, 3131–3135 (2007).
Chacko, T. & Deines, P. Theoretical calculation of oxygen isotopic fractionation factors in carbonate systems. Geochim. Cosmochim. Acta 72, 3642–3660 (2008).
Kim, S.-T. & O’Neil, J. R. Equilibrium and nonequilibrium oxygen isotope effects in synthetic carbonates. Geochim. Cosmochim. Acta 61, 3461–3475 (1997).
Gabitov, R. I., Watson, E. B. & Sadekov, A. Oxygen isotope fractionation between calcite and fluid as a function of growth rate and temperature: An in situ study. Chem. Geol. 306–307, 92–102 (2012).
Coplen, T. B. Calibration of the calcite-water oxygen-isotope geothermometer at Devils Hole, Nevada, a natural laboratory. Geochim. Cosmochim. Acta 71, 3948–3957 (2007).
Demény, A., Kele, S. & Siklósy, Z. Empirical equations for the temperature dependence of calcite-water oxygen isotope fractionation from 10 to 70 °C. Rapid Commun. Mass Spectrom. 24, 3521–3526 (2010).
Tremaine, D. M., Froelich, P. N. & Wang, Y. Speleothem calcite farmed in situ: Modern calibration of δ18O and δ13C paleoclimate proxies in a continuously-monitored natural cave system. Geochim. Cosmochim. Acta 75, 4929–4950 (2011).
Kele, S. et al. Temperature dependence of oxygen- and clumped isotope fractionation in carbonates: A study of travertines and tufas in the 6–95 °C temperature range. Geochim. Cosmochim. Acta 168, 172–192 (2015).
Watkins, J. M., Nielsen, L. C., Ryerson, F. J. & DePaolo, D. J. The influence of kinetics on the oxygen isotope composition of calcium carbonate. Earth Planet. Sci. Lett. 375, 349–360 (2013).
Scherrer, P. Bestimmung der Grösse und der inneren Struktur von Kolloidteilchen mittels Röntgenstrahlen. Nachr. Ges. Wiss. Göttingen 26, 98–100 (1918).
Frisia, S., Borsato, A., Fairchild, I. J. & McDermott, F. Calcite fabrics, growth mechanisms, and environments of formation in speleothems from the Italian Alps and southwestern Ireland. J. Sediment. Res. 70, 1183–1196 (2000).
Boch, R., Spötl, C. & Frisia, S. Origin and palaeoenvironmental significance of lamination in stalagmites from Katerloch Cave, Austria. Sedimentology 58, 508–531 (2011).
Bots, P., Benning, L. G., Rodriguez Blanco, J. D., Roncal-Herrero, T. & Shaw, S. Mechanistic insights into the crystallization of amorphous calcium carbonate (ACC). Crystal Growth & Design 12, 3806–3814 (2012).
Wang, Y. W., Kim, Y. Y. & Stephens, C. J. In situ study of the precipitation and crystallization of amorphous calcium carbonate (ACC). Cryst. Growth Des. 12, 212–217 (2012).
Ihli, J., Kulak, A. N. & Meldrum, F. C. Freeze-drying yields stable and pure amorphous calcium carbonate (ACC). Chem. Commun. 49, 3134–3136 (2013).
Konrad, F., Gallien, F., Gerard, D. E. & Dietzel, M. Transformation of amorphous calcium carbonate in air. Cryst. Growth Des. 16, 6310–6317 (2016).
Diaz, M. R. et al. Geochemical evidence of microbial activity within ooids. Sedimentology 62, 2090–2112 (2015).
Lábár, J. L. Electron diffraction based analysis of phase fractions and texture in nanocrystalline thin film, Part I: Principles. Microscopy and Microanalysis 14, 287–295 (2008).
Spötl, C. & Vennemann, T. W. Continuous-flow IRMS analysis of carbonate minerals. Rapid Commun. Mass Spectrom. 17, 1004–1006 (2003).
Lively discussions with Prof. Martin Dietzel helped clarify our ideas and are gratefully acknowledged. This research was supported by the Hungarian Scientific Research Fund (OTKA CK 80661 and OTKA NK 101664). The Bolyai János research scholarships received by György Czuppon and Péter Németh greatly helped their work.
The authors declare no competing financial interests.
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Demény, A., Németh, P., Czuppon, G. et al. Formation of amorphous calcium carbonate in caves and its implications for speleothem research. Sci Rep 6, 39602 (2016). https://doi.org/10.1038/srep39602
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