Precipitated calcium carbonate

Abstract

The present invention relates to crystalline and stable amorphous CaCO.sub.3 precipitated on lignocellulosic fibers.

Claims

1. A method for preparing stable amorphous calcium carbonate precipitated on natural fibers comprising the steps of: a. mixing water, 0 to 120 wt-% (based on the fiber weight) of at least one highly charged anionic polymer in solution, 1-99.9 wt-% (based on the total dry weight of the batch) Ca(OH).sub.2, and 0.1 to 95 wt-% (based on the total dry weight of the batch) of natural fibers; b. feeding CO.sub.2 to the mixture of step a) while stirring to obtain a precipitation; and c. drying or filtering the mixture to obtain the stable amorphous calcium carbonate, wherein 60-80 wt-% of Ca(OH)2 and 40-120 wt-% of highly charged anionic polymer is used in step a).

2. The method according to claim 1, wherein the highly charged anionic polymer is polyacrylic acid or a salt thereof.

3. The method according to claim 1, wherein 0.5 to 5 wt-% of lignocellulosic fibers is used as natural fibers.

4. The method according to claim 3, wherein 0.5 to 1.5 wt-% of lignocellulosic fibers is used as the natural fibers.

5. The method according to claim 3, wherein 2.5 to 3.5 wt-% of lignocellulosic fibers is used as natural fibers.

6. The method according to claim 1, wherein the fibers used are native or a byproduct from pulping.

7. The method according to claim 1, wherein said fiber is selected from microcrystalline cellulose, microfibrillated cellulose, nanocellulose, bacteria cellulose, cellulose nanocrystals or a mixture thereof.

8. A method for preparing stable amorphous calcium carbonate precipitated on natural fibers comprising the steps of: a. mixing water, 40 to 120 wt-% (based on the fiber weight) of at least one highly charged anionic polymer in solution, 1-99.9 wt-% (based on the total dry weight of the batch) Ca(OH).sub.2, and 0.1 to 95 wt-% (based on the total dry weight of the batch) of natural fibers; b. feeding CO.sub.2 to the mixture of step a) while stirring to obtain a precipitation; and c. drying or filtering the mixture.

9. The method according to claim 8, wherein the highly charged anionic polymer is polyacrylic acid or a salt thereof.

10. The method according to claim 8, wherein 0.5 to 5 wt-% of lignocellulosic fibers is used as natural fibers.

11. The method according to claim 10, wherein 0.5 to 1.5 wt-% of lignocellulosic fibers is used as the natural fibers.

12. The method according to claim 10, wherein 2.5 to 3.5 wt-% of lignocellulosic fibers is used as natural fibers.

13. The method according to claim 8, wherein the fibers used are native or a byproduct from pulping.

14. The method according to claim 8, wherein said fiber is selected from microcrystalline cellulose, microfibrillated cellulose, nanocellulose, bacteria cellulose, cellulose nanocrystals or a mixture thereof.

Description

BRIEF DESCRIPTION OF THE FIGURES

(1) FIG. 1: CaCO.sub.3 precipitated on microfiber with targeted ash of 48.2% using A) 1.0 wt-% fiber concentration and 0.5 l/min CO.sub.2 feed, B) 3.0 wt-% fiber concentration and 0.5 l/min CO.sub.2 feed, C) 3.0 wt-% fiber concentration and 1.5 l/min CO.sub.2 feed.

(2) FIG. 2: SEM micrographs of the ash

(3) FIG. 3: pH as a function of time during carbonation of samples having different fiber concentrations

(4) FIG. 4: CaCO.sub.3 precipitated on microfiber in presence of PAA concentration: A) 100.0 wt-% B) 3.0 wt-% and C) 1.0 wt-%. The microfiber concentration was 1.0 wt-% (A), 1.0 wt-% (B), and 3.0 wt-% (C), respectively. Note that PAA concentration is given as wt-% of fiber addition (g).

DETAILED DESCRIPTION

(5) Materials and Methods

(6) The calcium carbonate was precipitated at ambient temperature (20-23 C.) using Ca(OH).sub.2 as lime milk and CO.sub.2 (AGA, purity 99.7%). A dry cellulosic microfiber (Arbocel UFC100, JRS), with a mean particle size of 8 m according to the manufacturer was dispersed in water with strong mixing. Sodium polyacrylic acid, Na-PAA (Sigma-Aldrich, M 1800 g/mol) was dissolved in water (2, 5 and 8 wt-%, using a concentration as low as possible to reach the targeted concentration in the reaction batch) and diluted with water immediately prior use.

(7) The batches were prepared by mixing water, PAA solution (if used), Ca(OH).sub.2 and fibers, in this order. The contents of the solutions and suspensions were determined gravimetrically with an accuracy of 0.5 g. The precipitation was performed in an open batch reactor equipped with mixer and inlet for CO.sub.2. The stirring speed was set to a constant 800 rpm and the initial batch temperature was ca. 20 C. Changes in temperature and pH were monitored during the experiments, and the experiments were terminated when the pH began to stabilize at a low level, usually at ca. pH 6.5.

(8) Most of the samples were dried in oven without filtration, but some samples made using PAA as an additive were filtered using a polycarbonate membrane (Whatman, 0.6 m) and rinsed with distilled water (ca. 30 C.) before drying. The dried PCC-cellulose composite samples were studied using a Scanning Electron Microscope (FEI Nova NanoSEM 450 field emission (Schottky emitter) with a 10.0 kV accelerating voltage, 8 mm working distance and retractable concentric back scatter detector (CBS)). Ash contents were determined according to TAPPI standards T 211 om-02 and T 413 om-11, and thermogravimetric analysis (Mettler Toledo TGA/DSC 2) was performed on selected samples.

(9) The morphology of the cellulose microfiber-PCC agglomerates and the size of PCC crystal on the cellulose were determined from the SEM images. The CaCO.sub.3 polymorphs and the crystallinity of the cellulose-PCC complexes were characterized using x-ray diffraction (XRD measurements on a Bruker Discover D8 diffractometer (Karlsruhe, Germany) using Cu(K) radiation (=1.54184 nm). The XRD diffractograms were collected in the 2 range of 13-48. The X-ray tube was operated at 40 kV and 40 mA. For phase identification, a PDF-2 database (2012) was used.

(10) The variables relevant for the precipitating nanoclusters and crystals on the microfibers are listed and explained in Table I. Although the fiber appears to be a non-reactive component in the precipitation reaction, it plays an important but indirect role in the supersaturation of the solution, in addition to its ability to assist nucleation. This is explained as follows:

(11) The Ca(OH).sub.2/fiber ratio at a given ash content and a given amount of fiber is decided by the targeted filler content of the fiber-PCC composite material according to the following equation, derived from the T 211 om-02 ash definition in TAPPI.

(12) $m_{{\mathrm{Ca}\left(\mathrm{OH}\right)}_2}=\frac{\mathrm{Ash},\%.Math.\left(B-A\right)}{100-\mathrm{Ash},\%}.Math.0.7402$

(13) Where A is the weight of ash targeted PCC ash, and B is the weight of the test specimen so that B-A is the weight of fiber. The constant 0.7402 is the ratio of the molar masses of Ca(OH).sub.2 and CaCO.sub.3, to translate the targeted weight of PCC ash to the weight of Ca(OH).sub.2.

(14) In the batch system used, increasing fiber concentration increases Ca(OH).sub.2 concentration when the targeted ash content is kept at constant. An increase in Ca(OH).sub.2 concentration can in turn affect the degree of supersaturation and the ratio of ionic species by offering reactive material for the precipitation. An important consequence is that when the same batch process is used for different targeted filler ash contents by simply changing the amount of added Ca(OH).sub.2 and perhaps the CO.sub.2 feed, the PCC properties and thus the fiber furnish properties may change. Even if all the process parameters were changed so that the ratios were truly fixed, the precipitation process would still change with a change in the amount of Ca(OH).sub.2 added, as the driving force for precipitation is supersaturation that under given conditions depends on the concentration of the precipitating species. Changing the fiber concentration in order to fix the Ca(OH).sub.2 concentration would, instead, change the surface area of fiber per volume unit.

(15) TABLE-US-00001 TABLE I Variables investigated and units used. Ratios are calculated using the units given in the table. Variable Clarification Ca(OH).sub.2 concentration Calcium hydroxide concentration in reaction mixture (wt-%, of batch before precipitation) Microfiber concentration Microfiber concentration in reaction mixture (wt-%, of batch before precipitation) CO.sub.2 feed Carbon dioxide feed (l/min, at 20 C.) PAA concentration Concentration of additive (PAA) (wt-%, of fiber) Ca(OH).sub.2/CO.sub.2 Ratio of calcium hydroxide concentration to carbon dioxide feed (wt-%/l/min) Ca(OH).sub.2/fiber Ratio of calcium hydroxide concentration and fiber concentration, (wt-%/wt-%) PAA/Ca(OH).sub.2 Ratio of additive concentration to calcium hydroxide concentration (wt- %/wt-%)

(16) Results

(17) Effect of Microfiber Concentration and CO.sub.2 Feed

(18) CaCO.sub.3 was precipitated onto microfibers without polymeric additives at 5 different fiber concentrations, viz. 0.5, 1.0, 2.0, 3.0 and 6.0 wt-%. The targeted Ca(OH).sub.2 concentration was 69 wt-% based on oven-dry fiber. The precipitation gave on average 46.3 wt-% ash (mineral filler) content measured on unfiltered samples. In this case, mineral filler content and ash content are synonym, since microfiber gave no ash. The obtained ash gave a 91 mol-% conversion efficiency of Ca(OH).sub.2, based on weight loss (TAPPI standards T 211 om-02 and T 413 om-11 in conjunction) assuming that the lime milk was essentially free from impurities or reaction products such as CaCO.sub.3.

(19) FIG. 1 shows relatively large PCC particles precipitated onto the at 1.0 and 3.0 wt-% microfiber concentrations. The size of the deposited PCC particles was found to decrease with decreasing ratio of fiber (wt-%) to carbon dioxide (l/min), and with increasing fiber concentration at constant ratio. FIG. 1C shows that a substantially larger fraction of nanoparticles were nucleated and grown on the surface of the cellulose microfibers (instead of ellipsoidal CaCO.sub.3 particles) at the higher fiber concentration and greater carbon dioxide feed, presumably because of the larger surface area of fiber per unit volume and the higher degree of supersaturation in the system.

(20) Much of the difference in observed PCC particle sizes was due to aggregation and agglomeration of nano-sized crystals that form ellipsoidal particles at low microfiber concentrations, rather than to the size of individual crystals. When the fiber concentration was increased from 1.0 wt-% to 3.0 wt-% at a constant CO.sub.2 feed (0.5 l/min), the morphology of the PCC particles was slightly altered and many of the particles precipitated onto the microfibers were larger (see FIG. 1B), which is attributed to more intensive agglomeration. Moreover, increasing the CO.sub.2 feed from 0.5 l/min to 6.0 l/min for the suspension containing 0.5 or 1.0 wt-% microfiber did not lead to any detectable change in the morphology of the PCC particles. Instead, when the CO.sub.2 feed was increased in batches containing 3.0 wt-% or more fiber, the crystal size decreased as can be seen in FIGS. 1B and 1C. Changes in aggregation and agglomeration resulted in a more even PCC distribution on the fiber surface and a better coverage of the fiber. FIG. 2 shows SEM images of ash (52525 C.) of sample precipitated using 3.0 wt-% fiber concentration and 1.5 l/min CO.sub.2 feed, with irregular PCC agglomerates.

(21) In experiments conducted by Subramanian et al. (2007), ellipsoidal PCC structures were obtained, which are in agreement with FIGS. 1A and 1B. These ellipsoidal PCC structures, denoted colloidal PCC (c-PCC) by Subramanian et al. (2007), were obtained with a low concentration of cellulosic fines and were ascribed to the intermediate formation of ACC and its decomposition. This nucleation and crystal growth process led to a steep drop in pH (formation of ACC), immediately following by a rapid increase in pH (decomposition of ACC), and this was also observed in the present case.

(22) FIG. 2 shows SEM micrographs of the ash obtained from the microfiber-PCC-PAA samples combusted at 52525 C. The PCC particle morphology was similar to that of PCC precipitated onto microfiber in the absence of PAA. At low PAA/Ca(OH).sub.2 ratios, PCC particles were uniform in size with a symmetrical, spherical or ellipsoid morphology. With increasing PAA/Ca(OH).sub.2 ratio, the particles became non-uniform, developing a molten appearance linked with liquid precursors of CaCO.sub.3 (Gower & Odom, 2000). Especially at 50 and 100 wt-% PAA concentrations, the particles formed large polycrystalline aggregates with curved shapes, also linked with the formation of crystals via PILPs and ACC (Gower & Odom, 2000).

(23) When, at a PAA concentration of 3.0 wt-%, and the addition of Ca(OH).sub.2 was increased from 32 to 69 wt-%, no obvious differences were seen in the PCC particles on the microfibers. The morphology of the particles determined after combustion, on the other hand, showed an increase in particle regularity with increasing Ca(OH).sub.2 concentration above 41 wt-%. The particle irregularity increased when the PAA/Ca(OH).sub.2 ratio increased, which agrees with results presented by e.g. Yu et al. (2004) who concluded that PAA/CaCO.sub.3 ratio has a more pronounced effect on the CaCO.sub.3 morphology than on the concentration of the CaCO.sub.3 formed.

(24) FIG. 3 shows the pH as function of time upon CO.sub.2 dosage and subsequent carbonation and its dependence on the fiber concentrations. At low fiber concentration, the pH dropped quite rapidly with a constant CO.sub.2 feed at the beginning of the experiment, followed by an immediate increase. The inflection point occurred later with increasing fiber concentration (when the targeted ash content was kept at constant).

(25) The Effect of Sodium Polyacrylic Acid (PAA) as Precursor Stabilizer

(26) The use of PAA to control CaCO.sub.3 crystal morphology has been previously demonstrated (Huang et. al., 2007; Ouhenia et. al., 2008; Yu et. al., 2004), and also when CaCO.sub.3 crystals were deposited on a cellulosic substrate (Hosoda & Kato, 2001; Matahwa et. al., 2008), but, to our knowledge, effect of PAA in a cellulosic fiber-Ca(OH).sub.2-CO.sub.2 system has not been investigated before.

(27) Experiments with PAA carried on using three different fiber concentrations, viz. 1.0 wt-%, 3.0 wt-% and 6.0 wt-%, with a fixed ratio of fiber to CO.sub.2 of 0.5. The effects of PAA and Ca(OH).sub.2 concentration were thus varied in order to determine their impact on the complexes obtained.

(28) The results, summarized in Table II and FIG. 4, show that at a microfiber concentration of 1.0 wt-% and a Ca(OH).sub.2 concentration of 69 wt-%, an increase in PAA concentration initially resulted in an increase in PCC particle size. The SEM images (FIG. 4) show that this was due to increased agglomeration and nanoparticle cluster formation. The ability of PAA to inhibit nucleation in bulk solution may have contributed to this process by supporting aggregate growth. The PCC particles formed were elongated and had a rice-like shape (PAA concentration 0.5 wt-%), similar to those seen in FIG. 4 C, but slightly larger. At PAA concentrations 1.0 and 3.0 wt-%, the PCC crystals were rounder, see FIG. 4B. The difference was probably caused by temporary ACC stabilization by PAA, but this was not confirmed. Matahva et al. (2008) obtained similar CaCO.sub.3 particles when precipitating in presence of PAA, and these were ascribed to an ACC-PAA gel similar to that obtained by Ulinas et al (2007). They describe the formation of a viscous ACC gel temporarily stabilized by PAA, which precipitates into more stable polymorphs after losing its stability.

(29) Surprisingly, the effect of PAA at a microfiber concentration of 3.0 wt-% was opposite to that at 1.0 wt-%. With increasing dosage of PAA from 0.3 to 3.3 wt-%, the PCC crystal size increased, and crystals became elongated. The crystals retained their elongated shape but the crystal size increased when the PAA concentration was increased further. At very low and fixed PAA concentrations (0.06 wt-%) and a microfiber concentration of 3.0 wt-% an increase in Ca(OH).sub.2 from 32 wt-% to 69 wt-% led to a significant decrease in the PCC crystal particle size. A clear crystal phase transition region was seen at a Ca(OH).sub.2 concentration between 51 wt-% and 69 wt-%, where the particle morphology changed from approximately 1 micron roundish crystals to more elongated PCC crystals with a greater aspect ratio (length ca. 1 m and width 0.2 m). At 32 wt-% Ca(OH).sub.2 addition, the crystals were more elongated at a microfiber concentration of 6.0 wt-% than at 3.0 wt-%. An increase in microfiber concentration from 3.0 to 6.0 wt-% resulted in a crystal phase transition region between 32 wt-% and 51 wt-% of Ca(OH).sub.2 addition.

(30) However, when the concentration of PAA was increased to 10.0 wt-%, it was found that the particle size and amounts of large PCC crystals and clustered PCC agglomerates deposited on the microfibers decreased significantly, but that a few individual nano-sized PCC crystal particles were still formed and present on the microfiber surface (not shown here). FIG. 4A shows that when the PAA concentration was increased further to 100.0 wt-%, crystal formation of PCC on the surface of the microfiber was inhibited, which was confirmed by a lower ash content in samples rinsed before drying.

(31) The ash contents of some of the microfiber-PAA-CaCO.sub.3 complexes (rinsed before drying) were clearly lower than unreacted Ca(OH).sub.2 should yield. This can only be explained by the removal of soluble compounds or nanocrystals in bulk solution during filtering of the samples through the 0.6 m membrane and subsequent rinsing. A pronounced loss of crystalline material during filtration should mean that an increased dose of PAA would facilitate bulk solution precipitation, instead of decreasing it as stated frequently in the literature (Hosoda & Kato, 2001; Huang et. al., 2007; Watamura et. al., 2014).

(32) A possible alternative is heterogeneous nucleation in bulk solution, improved by PAA addition in a manner similar to that in which the addition of PAA can improve crystallization on cellulosic fibers, i.e. via electrostatic interaction between calcium ions and anionic groups of the polyelectrolyte (PAA) and foreign particles. Bulk solution precipitation is not, however, supported by the filtrate collected in these experiments, since the filtrate was transparent, which suggests an absence of crystalline material and the presence of amorphous transparent ACC as reported in the literature (Gower & Odom, 2000; Saghavaz et. al., 2013), or a complex. The formation of an electrostatic complex between carboxyl groups and calcium ions is frequently described in the literature (Hosoda & Kato, 2001; Huang et. al., 2007; Ouhenia et. al., 2008; Ulinas et. al., 2007; Watamura et. al., 2014), and ascribed to the formation of an ACC-containing gel (Matahwa et. al., 2008; Ulinas et. al., 2007), suggesting that role of the PAA in the system is the stabilization of ACC or the formation of a precursor or complex, or both.

(33) TABLE-US-00002 TABLE II Results of the PCC-PAA-Microfiber experiments. PAA concentration is given as wt-% of the fiber content. Microfiber Ca(OH).sub.2 PAA PCC morphology and size concentration addition concentration Low PAA High PAA [wt-%] [wt-%] [wt-%] conc. conc. 1 69 0.1; 0.5; 1.0; Elongated. Round, 3.0; 10.0; irregular 50.0; 100.0 Reduced particle size 32; 41; 51; 3.0 Elongated Elongated- 60; 69 irregular 3 69 0.3; 1.0; 2.0; Round Elongated 3.3 Increased particle size 32; 51; 69 6.0 Slightly Elongated elongated Reduced particle size 6 32; 51 1.0 Elongated Reduced particle size

(34) XRD and TGA

(35) Ten Microfiber-PCC samples, with and without precipitated calcium carbonate, were characterized using XRD. Diffractograms were collected in the 2 range of 13-48.

(36) The XRD results show different crystalline forms of cellulose, with slight peak shifts between some of them. The main peak for cellulose located at 20-22 (Haleem et. al., 2014; Obi et. al., 2014; Tibolla et. al., 2014) was found in samples 0, 5 and 6, where it is quite sharp, but the calcite peak located at the same angle makes it difficult to reliably determine the presence of crystalline cellulose in the samples. However, a smaller peak originating from cellulose at 34.6 was clearly observed in all the diffractograms except those for samples 1 and 3. The presence of cellulose I in these two samples was therefore considered as possible. In the case of the fiber reference sample, the co-existence of cellulose I and cellulose I was suspected.

(37) The only CaCO.sub.3 polymorph observed in the samples was calcite, although some PAA with different molecular weights have been linked with the formation of aragonite in the literature (Ouhenia et. al., 2008; Watamura et. al., 2014). Calcite peaks (Kim, et. al., 2013; Kirboga et. al., 2014; Lpez-Periago et. al., 2010) were observed in all samples except for the 0 (the fiber reference) and 5 and 6 (Ca(OH).sub.2 69 wt-%, CO.sub.2 feed 0.5 l/min and PAA concentrations 50.0 and 100.0 wt-%). The ash contents (52525 C.) for samples 5 and 6 were 8.2 and 4.0%, respectively, confirming that samples 5 and 6 clearly contained sufficient ash to be detectable in the XRD measurement, i.e. if it were crystalline.

(38) For sample 5 and 6, the absence of both crystalline Ca(OH).sub.2 and crystalline CaCO.sub.3 suggests that the high PAA concentration in the samples led to the formation and stabilization of amorphous CaCO.sub.3. The unstable character of amorphous ACC is well known, but no phase transition to a crystalline material detectable with XRD was observed, despite the long delay time between the precipitation experiments and the XRD measurements, even though particulate matter residing on the fibers was observed with SEM and the ash content of the samples showed that the concentration of inorganics was detectable with XRD, if crystalline.

(39) TABLE-US-00003 TABLE III XRD results. Sample number and description Cellulose I PCC Fiber reference 0 - Microfiber, , untreated No PAA 1 - fiber 1 wt-% (possible) Calcite CO.sub.2 feed 0.5 l/min 2 - fiber 3 wt-% Calcite CO.sub.2 feed 0.5 l/min 3 - fiber 3 wt-% (possible) Calcite CO.sub.2 feed 1.5 l/min Ca(OH).sub.2 69 wt-% 4 - PAA 1.0 wt-% Calcite CO.sub.2 feed 0.5 l/min 5 - PAA 50.0 wt-% 6 - PAA 100.0 wt-% PAA 3.3 wt-% 7 - Ca(OH).sub.2 32 wt-% Calcite CO.sub.2 feed 0.5 l/min 8 - Ca(OH).sub.2 51 wt-% Calcite 9 - Ca(OH).sub.2 69 wt-% Calcite

(40) Table IV shows the results of the Thermogravimetric measurements. The data at 550 C. and 925 C. were used to estimate the conversion yield and possible residual Ca(OH).sub.2.

(41) TABLE-US-00004 TABLE IV TGA results Property Method/basis Unit 1.sup.1 2 3 5 Dry TGA (105 C.) % 98.2 97.72 97.97 94.87 matter (105 C.) Ash TGA (550 C.) % 43.4 29.8 44.5 7.4 content (550 C.) Ash TGA (550 C.) %, 44.2 30.5 45.5 7.8 content dry basis (550 C.) Ash TGA (925 C.) % 25.9 17.3 25.8 4.6 content (925 C.) Ash TGA (925 C.) %, 26.4 17.7 26.4 4.9 content dry basis (925 C.) [CaCO3] Theoretical %, 40.6 29.0 43.4 6.6 (TGA 550 and dry basis 925 C.) [CaCO3] Theoretical % of ash 91.8 95.3 95.5 85.2 (TGA 550 and (550 C.) 925 C.) [Ca(OH)2] Theoretical % 4.8 1.9 2.7 1.5 (TGA 550 and dry basis 925 C.) [Ca(OH)2] Theoretical % 10.6 6.2 5.9 18.7 inorganic species Property Method/basis Unit 6 10.sup.2 11.sup.3 Dry TGA (105 C.) % 97.48 98.02 98.06 matter (105 C.) Ash TGA (550 C.) % 35.9 43.9 44.7 content (550 C.) Ash TGA (550 C.) %, 36.9 44.8 45.6 content dry basis (550 C.) Ash TGA (925 C.) % 20.5 25.4 25.9 content (925 C.) Ash TGA (925 C.) %, 21.0 25.9 26.4 content dry basis (925 C.) [CaCO3] Theoretical %, 36.0 43.0 43.8 (TGA 550 and dry basis 925 C.) [CaCO3] Theoretical % of ash 97.6 96.1 96.0 (TGA 550 and (550 C.) 925 C.) [Ca(OH)2] Theoretical % 1.2 2.3 2.4 (TGA 550 and dry basis 925 C.) [Ca(OH)2] Theoretical % 3.1 5.1 5.2 inorganic species .sup.1Not taken at the end of the process and therefore holds a larger proportion of Ca(OH).sub.2 .sup.2Microfiber concentration 3 wt-%, PAA concentration 1.0 wt-% .sup.3Microfiber concentration 3 wt-%, PAA concentration 0.3 wt-%

(42) The results indicate that all the samples contained unreacted Ca(OH).sub.2, the amount of Ca(OH).sub.2 in the samples being typically ca. 5 wt-% of the inorganic species, with the notable exception of sample 5 which was formed in the presence of a high PAA concentration of 50 wt-%. The result is approximately in line with the conversion estimate from the TAPPI ash content measurements. The remaining Ca(OH).sub.2 was not, however, identified in the XRD analysis, suggesting either that the material was not crystalline or that it resided in CaCO.sub.3 particles or microfibers, too far from the particle surfaces to be determined by the method. On the other hand, the TGA results may also interfere with the release of physisorbed water at 525 C. and at higher temperature the possible dihydroxylation of Ca(OH).sub.2 (Renaudina et. al., 2008).

(43) In view of the above detailed description of the present invention, other modifications and variations will become apparent to those skilled in the art. However, it should be apparent that such other modifications and variations may be effected without departing from the spirit and scope of the invention.

REFERENCES

(44) Butler M. F, Glaser N, Weaver A. C, Kirkland M, Heppenstall-Butler M, 2006. Calcium Carbonate Crystallization in the Presence of Biopolymers. Crystal growth & design, 6(3), 781-794. Cai, G-B, Zhao G-X, Wang X-K, Yu S-H, 2010. Synthesis of Polyacrylic Acid Stabilized Amorphous Calcium Carbonate Nanoparticles and Their Application for Removal of Toxic Heavy Metal Ions in Water. Journal of Physical Chemistry C, 144, 12948-12954. Ciobanu M, Bobu E, Ciolacu F., 2010. In-situ cellulose fibres loading with calcium carbonate precipitated by different methods. Cellulose Chemical Technology, 44, 379-387. Cfen H, Antonietti M. Mesocrystals and Nonclassical Crystallization. England: Chichester; 2008. Gower L. B, Odom D. J, 2000. Deposition of calcium carbonate films by a polymer-induced liquid-precursor (PILP) process. Journal of Crystal Growth, 210, 719-734. Haleem N, Arshadm M, Shahid M., Tahir M. A, 2014. Synthesis of Carboxymethyl cellulose from waste of cotton ginning industry. Carbohydrate Polymers, 113, 249-255. Hardikar V. V, Matijevi E, 2001. Influence of ionic and nonionic dextrans on the formation of calcium hydroxide and calcium carbonate particles. Colloids and Surfaces, 186, 23-31. Hosoda N, Kato T, 2001. Thin-Film Formation of Calcium Carbonate Crystals: Effects of Functional Groups of Matrix Polymers. Chemistry of Materials, 13, 688-693. Hu Z, Deng Y, 2004. Synthesis of needle-like aragonite from calcium chloride and sparingly soluble magnesium carbonate. Powder technology, 140, 10-16. Huang S-C, Naka K, Chujo Y, 2007. A Carbonate Controlled-Addition Method for Amorphous Calcium Carbonate Spheres Stabilized by Poly(acrylic acid)s, Langmuir, 23, 12086-12095. Huang S-C, Naka K, Chujo Y, 2008. Effect of Molecular Weights of Poly(acrylic acid) on Crystallization of Calcium Carbonate by the Delayed Addition Method, 2008. Polymer Journal, 40(2) 154-162. Jada A., Ait Akbour R, Jacquemet C, Suau J. M, Guerret O, 2007. Effect of sodium polyacrylate molecular weight on the crystallogenesis of calcium carbonate. Journal of Crystal Growth, 306, 373-382. Kellermeier M., Melero-Garca E, Glaab F, Klein R, Drechsler M, Rachel R, Garci-Ruiz J, Kunz W, 2010. Stabilization of Amorphous Calcium Carbonate in Inorganic Silica-Rich Environments. Journal of the American Chemical Society, 132, 17859-17866. Kim H. K, Park S. J, Han J. I, Lee H. K, 2013. Microbially mediated calcium carbonate precipitation on normal and lightweight concrete. Construction and Building Materials, 38, 1073-1082. Kirboga S, Oner M, Akoyl E, 2014. The effect of ultrasonication on calcium carbonate crystallization in the presence of biopolymer. Journal of Crystal Growth, 401, 266-270. Kitamura M, Konno H, Yasu A, Masuoka H, 2002. Controlling factors and mechanism of reactive crystallization of calcium carbonate polymorphs from calcium hydroxide suspensions. Journal of crystal growth, 2002, 323-332. Klungness J. H, Ahmed A, Ross-Sutherla N, AbuBakr S, 2000. Lightweight, high-opacity paper by fiber loading: filler comparison. Nordic Pulp and Paper Research Journal (15)5, 345-350. Klungness J. H, Caulfield D, Sachs I., Tan F, Sykes M, Shilts R, 1994. Fiber-loading: a progress report. Tappi Recycling symposium (pp. 283-290). Boston: Tappi Press. Klungness J. H, Sykes M. S, Tan F, Abubakr S, Eisenwasser, J. D, 1996. Effect of fiber loading on paper properties. Tappi Journal, 79(3), 297-301. Klungness J. H, Tan F, Aziz S. Sykes M. S. Retention of calcium carbonate during recycling: direct loading versus fiber loading. In: Environmental Conference & Exhibit Book 1: 1997 May 5-7th; Minneapolis. Atlanta: Tappi Press; 1997. Kumar P, Gautam S. K, Kumar V, Singh S. P, 2009. Enhancement of optical properties of bagasse pulp by in-situ filler precipitation. BioResources, 4(4), 1635-1646. Kumar P, Singh Negi Y, Pal Singh S, 2011. Filler loading in the lumen or/and cell wall of fibersa literature review. BioResources 6(3) 3526-3546. Lpez-Periago A. M, Pacciani R, Craca-Gonzlez C, Vega L. F, Domingo C, 2010. A Breakthrough technique for the preparation of high-yield precipitated calcium carbonate. Journal of Supercritical Fluids, 52, 298-305. Malkaj P, Dalas E, Kanellopoulou D. G, Chrissanthopoulos A, Sevastos D, 2007. Calcite particles formation, in the presence of soluble polyvinyl-alcohol matrix. Powder Technology, 177, 71-76. Matahwa H, Ramiah V, Sanderson R. D, 2008. Calcium carbonate crystallization in the presence of modified polysaccharides and linear polymeric additives. Journal of Crystal Growth, 310, 4561-4569. Mohamadzadeh-Saghavaz K, Resalati H, & Ghasemian A., 2014. Cellulose-precipitated calcium carbonate composites and their effect on paper properties. Chemical Papers, 68(6) 774-781. Nielsen J. W, Sand K. K, Pedersen C. S, Lakshtanov L. Z, Winther J. R, Willemos M, Stipp S. L. S, 2012. Polysaccharide Effects on Calcite Growth: The Influence of Composition and Branching. Crystal Growth & Design, 12, 4906-4910. Obi Reddy K, Zhang J, Zhang, J, Varada Rajulu A, 2014. Preparation and properties of self-reinforced cellulose composite films from Agave microfibrils using an ionic liquid. Carbohydrate polymers, 144, 537-545. Ouhenia S, Chateigner D, Blekhir M. A, Guilmeau E, Krauss C, 2008. Synthesis of calcium carbonate polymorhs in the presence of polyacrylic acid. Journal of Crystal Growth, 310, 2832-2841. Park W. K, Ko S-J, Lee S. W, Cho K-H, Ahn J-W, Han C, 2008. Effects of magnesium chloride and organic additives on the synthesis of aragonite precipitated calcium carbonate. Journal of crystal growth, 310, 2593-2601. Payne S. R, Heppenstall-Butler M., Butler M. F, 2007. Formation of Thin Calcium Carbonate Films on Chitosan Biopolymer Substrates. Crystal Growth & Design, 7(7), 1262-1276. Renaudin G, Bertrand A, Dubois M, Gomes S, Chevalier P, Labrosse P, 2008. A study of water releases in ground (GCC) and precipitated (PCC) calcium carbonates. Journal of Physics and Chemistry of Solids, 69, 1603-1614. Saghavaz K. M, Resalati H, Mehrabi E, 2013. Characterization of cellulose-PCC composite filler synthesized from CMC and BSKP fibrils by hydrolysis of ammonium carbonate, Powder Technology, 246, 93-97. Saito T, Oaki Y, Nishimura T, Isogai A, Kato T, 2014. Bioinspired stiff and flexible composites of nanocellulose-reinforced amorphous CaCO3. Material Horizons, 1, 321-325. Silenius P. Preparation of filler containing papermaking materials by precipitating calcium carbonate in-situ in the presence of cellulosic material [Licentiate thesis]. Lappeenranta: Lappeenranta University of Technology; 1996. Subramanian R, Fordsmand H, Paulapuro H, 2007. Precipitated calcium carbonate (PCC)-cellulose composite fillers; effect of PCC particle structure on the production and properties of uncoated fine paper. BioResources, 2(1), 91-105. Tibolla H, Franciele M. P, Florencia C. M, 2014. Cellulose nanofibers produced from banana peel by chemical and enzymatic treatment. LWTFood Science and Technology, 59, 1311-1318. Ulinas A, Butler M. F, Heppenstall-Butler M, Singleton S, Miles M. J, 2007. Direct observation of spherulitic growth stages of CaCO3 in a poly(acrylic acid)-chitosan system: In situ SPM study. Journal of Crystal Growth, 307, 378-385. Watamura H, Sonobe Y, Hirasawa I, 2014. Polyacrylic Acid-Assisted Crystallization Phenomena of Carbonate Crystals, Chemical Engineering & Technology, 37(8), 1422-1426. Vdovi N, Kralj D, 2000. Electrokinetic properties of spontaneously precipitated calcium carbonate polymorphs: the influence of organic substances. Colloids and Surfaces, 161 499-505. Wei H, Shen Q, Zhao Y, Zhou Y, Wang D, Xu D, 2005. On the crystallization of calciumcarbonate modulated by anionic surfactants. Journal of Crystal Growth, 279, 439-446. Volkmer D, Harms M, Gower L, Ziegler A, 2005. Morphosynthesis of Nacre-Type Laminated CaCO3 Thin Films and Coatings. Angewandte Chemie International Edition, 44, 639-644. Yu J, Lei M, Cheng B, Zhao X, 2004. Effects of PAA additive and temperature on morphology of calcium carbonate particles. Journal of Solid State Chemistry, 177, 681-689.