- Open Access
Carbonation of Portland Cement Studied by Diffuse Reflection Fourier Transform Infrared Spectroscopy
© The Author(s) 2013
- Received: 27 August 2012
- Accepted: 4 April 2013
- Published: 22 May 2013
Carbonation is a natural ageing process for cement. This study focuses on how the carbonation rate varies with selected hydration times and atmospheric conditions during the early stages of reacting dried cement paste. Diffuse reflection Fourier transform infrared spectroscopy is shown to be a suitable technique to monitor the formation of carbonates in cement. Combined with a previously developed freeze drying technique, carbonation can be studied at specific hydration stages. In ambient air both calcium hydroxide and calcium silicate hydrate (C–S–H) in cement are carbonated. Increased hydration time enhances the carbon dioxide uptake, which indicates that the calcium in the hydration products reacts more easily than the calcium in the clinker phase. In a humid CO2 atmosphere, the carbonation process is so pronounced that it decomposes C–S–H into calcium carbonate and silica. In a moist N2 atmosphere no carbonation occurs, but the sulfate chemistry of the cement seems to be affected due to the formation of ettringite.
- Portland cement
- infrared spectroscopy
- cement hydration
Portland cement is widely used for the construction of concrete buildings. The dry Portland cement powder reacts with water to form the matrix that binds the aggregates in concrete together. To be able to predict the properties of the final structure, it is vital to understand the water-cement interaction. However, during its time of service the concrete is exposed to an environment that will alter its properties and modify its structure, both physically and chemically. A very important chemical substance that reacts with the cement matrix in concrete is carbon dioxide. It can cause carbonation of both the clinker phases and the products formed during the hydration of the cement, such as calcium hydroxide and calcium silicate hydrate gel (C–S–H). It is therefore important to take the early carbonation of C–S–H into account when handling samples in the laboratory, since the studied properties may change and affect the results.
The carbonation of Portland cement is a naturally occurring process during the ageing of a concrete structure; it changes the physical and chemical properties of the cement. During the carbonation process CaCO3 is formed and other carbonate phases are expected to be negligible. The carbonation may also induce corrosion of steel reinforcing bars, due to the reduction of alkalinity, which may cause severe damage to a structure.
The objective of this study is to improve the understanding of the carbonation processes in cement by monitoring the changes in characteristic infrared vibration modes that are coupled to the process. This is done by monitoring the carbonation of all samples with diffuse reflection Fourier transform spectroscopy (DR-FTIR), a technique that is suited to determining initial cement chemistry (Ylmén et al. 2009).
By combining this with a freeze drying technique (Ylmén et al. 2008), carbonation can be studied at different quenched hydration stages. In this work short hydration times has been studied, from 10 min to 8 h.
This method of studying the carbonation of cement has previously not been applied.
It is well known that the carbonate ion has four characteristic vibration modes in the mid-IR region. There are three common polymorphs of anhydrous CaCO3: calcite, aragonite and vaterite. The characteristic vibration modes of the carbonate ion in these polymorphs lie approximately at 698–745 cm−1 (ν4), 842–910 cm−1 (ν2), 1,070–1,085 cm−1 (ν1) and 1,425–1,590 cm−1 (ν3) (Xyla and Koutsoukos 1989; Gunasekaran et al. 2006; Frech et al. 1980; Rutt and Nicola 1974; Vagenas et al. 2003). There are also combination bands such as ν4 + ν1 at 1,800 cm−1, ν4 + ν3 at 2,500 cm−1 and 2ν3 at 2,900 cm−1.
Water absorbs infrared radiation between 1,600 and 1,700 cm−1 due to its bending vibration ν2 (Trezza and Lavat 2001; Richard et al. 2006; Mollah et al. 2003). It also absorbs this radiation in the range 3,000–3,700 cm−1 as this corresponds to the O–H stretching region. The hydroxide containing compounds also absorb in this range, such as Ca(OH)2 at 3,643 cm−1 (Björnström 2005; Delgado et al. 1996; Yu et al. 1999).
In this study the samples were freeze-dried prior to exposure to quench the hydration process (Ylmén et al. 2008, 2009). A set of samples was exposed to ambient air for 19 days to simulate storage in open containers. The decision to stop the exposure to ambient air after 19 days was based on the observation that the carbonation had, more or less, ceased after 8 days.
Another set of samples was exposed to a highly carbonating environment with pure carbon dioxide of 75 % relative humidity. The exposure to pure carbon dioxide was stopped after 4 days since the samples showed carbonation equal to that of 19 days of exposure in ambient air. Reference samples were exposed to pure nitrogen gas with 75 % relative humidity to examine the effect of moisture. The 75 % relative humidity was chosen as it has been observed that the hydration of the cement is very slow, but the carbonation rate is high at this humidity (Mejlhede Jensen et al. 1999; Houst 1996).
The idea behind having a nitrogen atmosphere was to determine whether any of the observed changes during exposure to ambient air was only an effect of the presence of water in the air. The exposure to a nitrogen atmosphere was stopped after 3 days since the samples only showed small changes during this time, whereas the samples exposed to ambient air showed significant changes after only 3 h.
Ambient air with ~50 % humidity: The samples were scanned with DR-FTIR spectroscopy several times during a time period of 19 days. As a comparison, an unhydrated sample was also exposed at the same conditions.
N2 atmosphere with 75 % humidity: The samples were scanned with DR-FTIR after 3 days of exposure.
CO2 atmosphere with 75 % humidity: The samples were scanned with DR-FTIR spectroscopy after 4 days of exposure.
The 75 % atmospheric humidity was obtained by letting a small flow (~1 dm3/h) of pure CO2 gas or N2 gas pass through water, saturated with NaCl, into the chamber containing the samples. After exposure the samples were measured with diffuse reflection Fourier transform infrared spectroscopy using a Nicolet Magna-IR 560 with an insert cell for diffuse reflection spectroscopy. The measurement range lies between 400 and 4,000 cm−1 with a nominal resolution of 2 cm−1.
Wave number and assignment
842–910 cm−1: ν2—out of plane vibration of CO32−
1,070–1,085 cm−1: ν1—symmetric stretching of CO32−
1,200 cm−1 narrow peak: unknown, formed directly after addition of water to cement 1,200 cm−1 broad peak: Si–O stretching of condensed silica
1,425–1,590 cm−1: ν3—asymmetric stretching of CO32−
1,600–1,700 cm−1: bending mode of H2O
1,800 cm−1: ν4 + ν1 of CO32−
2,500 cm−1: ν4 + ν3 of CO32−
Broad band >3,000 cm−1: stretching of OH
3,643 cm−1: stretching of OH in Ca(OH)2
1,100–1,200 cm−1: S–O stretching of SO42−
3.1 Ambient Air
The DR-FTIR spectra are presented for unhydrated samples in Fig. 2a. Figure 2b–e shows samples hydrated during time intervals from 10 min to 8 h. All of the samples were exposed to ambient air. To remove all signatures that are not the result of exposure, the spectrum after 10 min of exposure, within each exposure series, was subtracted from all the other spectra. The peaks at 1,800 and 2,500 cm−1 and the three bands rising in the region of 1,300–1,700 cm−1 are related to the carbonation process. The peaks at 1,410 and 1,535 cm−1 increase initially, whereas the peak at 1,580 cm−1 starts to develop later. The humps at ~1,650 and 2,700–3,700 cm−1 are associated with an increase of water. There is also a dip at 3,643 cm−1 due to a decreased amount of Ca(OH)2.
3.2 N2 and CO2 Environment with 75 % Humidity
The peaks at 856, 875, 1080, 1410, 1540, 1795 and 2513 cm−1 can be observed in all of the spectra and were assigned to CaCO3. In a CO2 rich atmosphere there is a noticeable decline in Ca(OH)2, seen as a dip at 3,643 cm−1 in Fig. 6. It is interesting to note that for the 8-h hydration sample there is also a dip at ~950–1,100 cm−1 corresponding to the peaks for C–S–H (Ylmén et al. 2009). A decrease can also be seen in the OH-stretching region (3,000 cm−1) where a broad dip has formed, corresponding to the signature of C–S–H. The spectra for all hydration times also show a peak at 1,200 cm−1 with a narrow dip at the same position. The band at ~1,650 cm−1, together with the increased intensity in the OH-stretching region, indicates absorption of water for all hydration times.
It can be concluded from Figs. 3 and 7 that longer hydration times for the cement paste result in faster CaCO3 formation when the dried and ground paste is exposed to air. However, this relationship does not seem to be valid for the accelerated carbonation in a humid CO2 atmosphere.
The total amount of carbonates produced appears to increase for longer hydration durations, as indicated by the convergence limit of the curves in Fig. 3. At these experimental conditions it must therefore be easier for the carbon dioxide to react with the calcium in the hydrated cement than the calcium in the unhydrated clinker for short hydration times. This is reasonable, as the clinker is much denser and thus less accessible than the early formed hydration products. The absolute amount of carbonates formed was not determined. However, an estimate was made by integrating the peak areas in the interval 1,300–1,700 cm−1 in the original spectra without subtraction. The peak area is roughly doubled after 4 days of exposure to a humid CO2 atmosphere. A similar increase is also seen under ambient conditions after 19 days. Ideally, the integrated area is proportional to the concentration (Griffiths et al. 2007). This suggests that the original ~10 % by mass of CaCO3 in the cement investigated is approximately doubled. However, infrared spectroscopy is a surface technique that only penetrates a few wave lengths into the material, i.e. a few micrometers. If the limestone originally present in the cement consists of larger particles, and the carbonates formed during exposure is formed either as small particles or as shells around existing structures, then the total amount of carbonate is smaller. Since the small characteristic water peak at 1,650 cm−1 lies in the region 1,300–1,700 cm−1, it will also affect the result to some extent.
In all of the samples, except for the unhydrated cement, the carbonate is easily seen with DR-FTIR spectroscopy within an hour of exposure to ambient air. Consequently, freshly cast cement is sensitive to carbonation; to prevent interference of carbonate formation during analysis samples should be handled to minimize their exposure to carbon dioxide. However, as the samples are in powdered form their reactive surface area is very large. Indeed, samples in their cast form will probably be more resistant to carbonation as there is less exposed surface area and the carbon dioxide will have to diffuse into the sample.
The effect of the moist N2 atmosphere was small, and there was no sign of hydration of the clinker phases, which is consistent with previous results (Mejlhede Jensen et al. 1999). Some transformations of sulfates seem to occur, emphasized by a shift in absorbance of the S–O stretching between 1,100 and 1,200 cm−1. The spectrum of the product fits well with that of ettringite. However, it is interesting to note that the amount of ettringite does not uniformly increase or decrease with increased hydration time. The ettringite decreases during the first 2 h of hydration, after which it increases again for longer hydration times. This implies that there are only some sulfate species that can react with the moisture in the atmosphere, and that the amount of these species will vary during the early hydration of the cement.
In a moist atmosphere the CO2 reacts with calcium extracted from both the clinker and the calcium silica gel. Even though sulfate phases, such as ettringite, can be carbonated, this was not observed in this experiment. This can be concluded because there are no observable signatures of the calcium sulfate species, such as gypsum, formed as a by-product of the carbonation (Grounds et al. 1988; Xiantuo and Ruizhen 1994).
The consumption of C–S–H is seen as dips in the 8-h hydration spectrum in Fig. 6. This is apparent both in the OH-stretching region above 3,000 cm−1 and in the region 900–1,100 cm−1 (overlapping with the CaCO3 band at 1,080 cm−1). The remaining silica gives an absorption profile resembling condensed silica (Ylmén et al. 2008) with a broad band at 1,200 cm−1. The spectrum after 30 s of hydration, see Fig. 6, has no dips due to consumption of C–S–H, since the hydration time is too short to form C–S–H. Here condensed silica is formed as a by-product since calcium is extracted from the clinker by the CO2.
It was noted that there is also a narrow peak at 1,200 cm−1 for the unexposed samples in Fig. 4. The peak is larger in the 30-s hydrated sample than in the 8-h hydrated sample. Although the peak was not assigned in this work, the compound absorbing at this wavelength is probably crystalline since the peak is very narrow. This signature has been observed in earlier work (Ylmén et al. 2008) and was there found to be correlated with a broader peak at ~3,300 cm−1. This correlation is supported here, as there is a large peak centred at 3,310 cm−1 seen in the unexposed sample hydrated for 30 s in Fig. 4. When the hydrated samples are exposed to a humid N2 atmosphere there seems to be a slightly increased amount of this unidentified compound as the peak is visible in Fig. 5. However, the humid CO2 atmosphere seems to decompose the compound, since the signature is seen as a narrow dip at 1,200 cm−1 superimposed on the broader peak at the same position as a result of the formation of silica in Fig. 6.
It has previously been shown that the formation of CaCO3 in aqueous solution normally produces calcite and/or vaterite as final products (Shivkumara et al. 2006; Clarkson et al. 1992). However, the signature of the CaCO3 formed in this study does not exactly match any of the spectra of calcite, vaterite or aragonite (Xyla and Koutsoukos 1989). However, there are also hydrated forms of CaCO3, such as monohydrocalcite (CaCO3·H2O), ikaite (CaCO3·6H2O) and amorphous calcite (Lam et al. 2007; Andersen and Ljerka Brečević 1991; Coleyshaw et al. 2003). The shape of the large carbonate band, at 1,400–1,600 cm−1, with two distinct peaks and the increase of water at 1,650 cm−1 is similar to the infrared spectrum of both monohydrocalcite and amorphous calcium carbonate (Lam et al. 2007; Andersen and Ljerka Brečević 1991; Coleyshaw et al. 2003).
The formation of CaCO3 in cement is a complex process that can involve reactions at various particle surfaces. The mechanism of these reactions is not yet fully understood. In the early stages the carbonates formed could be considered amorphous, since the crystallites have not yet developed a well-defined structure. The broadening of the band observed at 1,080 cm−1 indicates a less ordered structure because the peak is expected to be narrow if the phases are crystalline. This is consistent with the infrared spectra of synthesized amorphous calcium carbonate (Lam et al. 2007; Andersen and Ljerka Brečević 1991). The broadening is a sign of a more varying environment for the carbonate ion than that present in the crystalline structures. At later stages a more crystalline product can be expected.
The DR-FTIR spectroscopy technique relies on the vibration modes of characteristic groups in a compound, i.e. not on the crystallinity of the sample. Consequently, the characteristic vibration peaks in the region 1,300–1,700 cm−1 are representative of all carbonate species irrespective of the chemical and physical form. Thus DR-FTIR spectroscopy is a very suitable method for monitoring the formation of compounds such as carbonates in cement. Complementary methods such as Raman spectroscopy, thermogravimetric analysis and scanning electron microscopy could be used to bring more detailed information about the formed carbonate species. Thermodynamic computer calculations may also be an important tool to understand the complex carbonation processes in cement. However, these techniques are not within the scope of this study, but is an interesting topic for future work.
A method combining DR-FTIR spectroscopy with a previously developed freeze drying technique was applied successfully to investigate the carbonation of cement samples during selected hydration stages. The method makes it possible to monitor the formation of carbonate phases during various carbonation conditions. Applying this method on cement, hydrated up to 8 h, it was found that in ambient air both the C–S–H and Ca(OH)2 show carbonation; longer hydration time leads to more carbonation. As cement samples are exposed in a humid CO2 atmosphere, the C–S–H carbonates to such an extent that it decomposes to CaCO3 and silica. When cement samples were exposed in a humid N2 atmosphere, no carbonation was observed with this technique. However, there was some ettringite formation.
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