# Properties of Calcium Acetate Manufactured with Etching Waste Solution and Limestone Sludge as a Cementitious High-Early-Strength Admixture

Authors: Deuck-Mo Kim; Hwa-Sung Ryu; Sang-Heon Shin; Won-Jun Park
Journal: Advances in Materials Science and Engineering
 (2016)

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## Abstract

Concrete is one of the most widely used construction materials. There are several methods available to improve its performance, with one of them being the use of high-early-strength admixtures (HESAs). Typical HESAs include calcium nitrate, calcium chloride, and calcium formate (CF). Industrial by-products, such as acetic acid and lime stone sludge (LSS), can be used together to produce calcium acetate (CA), which can subsequently be used as a cementitious HESA. In this study, calcium carbonate and LSS were mixed with cement in weight ratios of 1 : 1, 1 : 1.5, and 1 : 2, and the properties of the as-produced CA were evaluated. CA and CF were mixed with cement in different weight ratios (0, 1, 2, and 3 wt%) to obtain CA- and CF-mortars, respectively. The flow behavior, setting time, pH, and compressive strength of these mortars were evaluated, and their X-ray diffraction patterns were also analyzed. It was found that as the CF content in the CF-mortar increased, the initial strength of the mortar also increased. However, it impaired its long-term strength. On the other hand, when 1% CA was mixed with cement, satisfactory early and long-term strengths were achieved. Thus, CA, which is obtained from industrial by-products, can be an effective HESA.


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## Body

## 1. Introduction

Several methods such as accelerated curing and the use of precast concrete and construction robots are used for increasing the production rate in ferroconcrete construction [1–7]. In particular, it is important to reduce the concrete curing time to reduce the overall concrete construction period. The overall performance and development of concrete are significantly influenced by both the curing process and the subsequent cast removal. Some of the methods currently used to improve these characteristics include steam curing and the use of high-early-strength admixtures (HESAs) [8–13]. Accelerated curing however requires the use of costly equipment. On the other hand, in the case of HESAs, an admixture addition of just 1–3 wt% is required to enhance the concrete performance, rendering this method more cost-effective. In addition, with an increase in the use of blended cements and cementitious composites, the use of various HESAs as a supplement to low-early-strength cements such as the ground-granulated blast-furnace slag has increased to improve their performance [14–17]. The primary mechanisms for such HESAs include the enhancement of the production of calcium silicate hydrate (C-S-H) using highly soluble calcium ions or increasing the hydration of amphoteric aluminum ions [18–21]. Generally, calcium nitrate, calcium chloride, and highly soluble calcium formate (CF) are used as HESAs to produce calcium salts, and amine mixtures are used to enhance the hydration of aluminum ions [9, 22, 23].The semiconductor and steel industries produce a wide array of by-products including acetic acid and calcium salts. The amount of chemical substances used for etching thin film transistor-liquid crystal display boards in the semiconductor industry continues to increase. Etching is used to corrode a material with chemicals such as nitric acid and acetic acid to polish its surface and create a product with desired properties. The chemicals used for etching can be recycled by distillation [24]. Such substances have a lower solid content than the pure substances and use water as a solvent. According to the World Steel Association, the total global steel production in 2014 was over 12,700,000,000 tons [25]. The process of steelmaking commences by cleansing limestone, which is obtained by dehydration of the by-products produced during desulfurization, with water to produce quicklime. The quicklime so obtained is used as a raw material to produce steel. During this process, small limestone particles (<1 mm) are separated by precipitation and thus lime stone sludge (LSS) can be manufactured through a filter press process. LSS contains large quantities of water, which renders it uneconomical for recycling [26].In this study, we manufactured a calcium-containing HESA (calcium acetate, CA), which is a source of calcium ions, by reacting acetic acid with LSS, which is a by-product of various industrial processes and evaluated the performance of the admixture so obtained. For a thorough evaluation, we examined the viscosity, density, pH, calcium content, heavy metal content, and solid content of the resultant admixture. We also added this admixture in different weight ratios to cementitious composites or mortars and examined their fluidity, setting time, pH, and compressive strength. We also carried out an X-ray diffraction (XRD) analysis of the cementitious composites or mortars containing this admixture.


## 2. Materials and Methods

### 2.1. Materials

#### 2.1.1. Limestone Sludge

In this study, LSS, which is obtained from industrial by-products, was used to manufacture the calcium-containing HESAs. The XRD pattern and chemical composition analyses of LSS are shown in Figure1 and Table 1, respectively. The XRD patterns of both CaCO3 and LSS showed the presence of a CaCO3 peak at approximately 29°. The structure of LSS appears to be identical to that of CaCO3. However, considering the chemical composition, the CaO content in LSS was approximately 5.84% lesser than that in CaCO3. In addition, LSS also contained SiO2 and metallic salts such as Al2O3 and Fe2O3.Table 1
Chemical composition of CaCO3 and LSS (%).
CaO SiO2 MgO Al2O3 SO3 Fe2O3 P2O5 K2O Na2O CaCO3 96.08 0.98 2.06 0.39 0.02 0.36 0.00 0.11 0.00  Limestone sludge 90.46 3.81 1.06 2.06 0.08 1.35 0.70 0.45 0.04Figure 1
XRD patterns of CaCO3 and LSS.


#### 2.1.2. Recycled Acetic Acid

Recycled acetic acid (RAA) was obtained from the previous etching processes by extraction via an acid separation process. In this study, approximately 60% RAA was used. Figure2 shows the Fourier transform infrared (FT-IR) spectrum of RAA. In the FT-IR spectrum of RAA, the peaks in the range of 3300–2500 cm−1 correspond to organic acids containing carboxylic groups. The peaks associated with C=O groups (1760–1690 cm−1) and C-O groups (1320–1210 cm−1) can also be observed in this spectrum. Some examples of carboxylic acids include acetic acid, formic acid, gluconic acid, and propionic acid. Hence, it was confirmed that RAA contained carboxylic acid groups [27].Figure 2
FT-IR spectrum of RAA.


#### 2.1.3. Binder and Sand

A comparison between the properties of the conventional HESAs and the admixture produced in this study was performed by using mortar specimens. The mortar specimens consisted of class I ordinary Portland (OPC). The chemical compositions and physical properties of these materials are given in Tables2 and 3, respectively. A description of the sand used in this study is given in Table 4.Table 2
Chemical composition of binder (%).
CaO SiO2 MgO Al2O3 SO3 Fe2O3 P2O5 K2O Na2O 63.85 21.09 3.32 4.84 3.09 2.39 0.36 0.73 0.14Table 3
Physical properties of ordinary Portland cement (OPC).
Specific gravity Blaine specific surface (cm2/g) Setting time Compressive strength of mortar (MPa) Initial set (min) Final set (hour) 3 days 7 days 28 days 3.15 3400 400 7 20 23 38Table 4
Properties of fine aggregate.
Maximum size (mm) Unit weight (kg/l) Specific gravity Water absorption (%) Solid volume percentage (%) <1.2 1.5 2.62 0.40 58.1


### 2.2. Methods

#### 2.2.1. Overview

In this study, we manufactured both the CA and the mortars containing CA in different weight ratios (0, 1, 2, and 3 wt%) and evaluated the performance of these mortars. The viscosity, density, and pH of these mortars were evaluated. Their inductively coupled plasma mass spectroscopy (ICP-MS) analyses were also performed. In addition, an existing HESA (CF) was also added to mortar in different weight ratios (0, 1, 2, and 3 wt%) to obtain CF-mortars and their CF content, setting time, XRD patterns, and pH were also investigated. The flow behavior and compressive strength of the mortars were also measured. Table5 summarizes these experiments. The flow chart for the synthesis of CA is shown in Figure 3.Table 5
Measurements and methods.
Experiment Measurement sample Properties measured Standards Calcium acetate using limestone sludge and recycled acetate Calcium acetate Viscosity (cps) ASTM D 2196 [28] Density (kg/m3) ASTM D 4052-11 [29] pH — ICP-MS analysis ASTM D 6800-12 [30]  Cement matrix using accelerator Cement paste Setting time ASTM C 191 [31] pH — XRD — Cement mortar Flow ASTM C 230/230M-14 [32] Compressive strength ASTM C 109 [33]Figure 3
Flow diagram for CA synthesis.


#### 2.2.2. Manufacturing CA with LSS and RAA

Here, RAA and LSS reacted to yield CA in accordance with (1). The yield was maximum when the ratio of acetic acid to CaCO3 was 2 : 1 with 1 mol each of CA, water, and carbon dioxide per mol of CaCO3:(1)2CH3COOH+CaCO3=CaCH3COO2+H2O+CO2Calcium carbonate and RAA were used to compare the solubility of the LSS and acetic acid together. To 60% solid acetic acid, LSS was added in different weight ratios (1, 1.5, or 2) as shown in Table 6. This mix was reacted for 12 h. Upon mixing, the unreacted particles were removed via filtering and acetic acid was separated for future use.Table 6
Reaction ratio according to weight ratio of RAA : CaCO3.
RAA : CaCO3 1 : 0.5 1 : 1 1 : 1.5 1 : 2 Reaction yield (%) 52 42 31 24.97 Reacted acetic acid (%) 42.4 80.8 91.6 99.86


#### 2.2.3. Cementitious Composites with HESAs

The mix proportions of the cementitious composites (cement paste and mortar) that were mixed with HESAs are given in Table7. The CA (used as a HESA) was weighed such that the weight ratio of LSS to acetic acid was 2 : 1 and the pH of the overall mixture was 5.9. The manufactured specimen underwent steam curing at a temperature of 20°C and a relative humidity of 60%.Table 7
Mixtures for paste and mortar specimens.
Mixture number OPC Water Calcium acetate Calcium formate Sand OPC 100 32 0  135 OPC-A1(A) 100 32 1  135 OPC-A2 100 32 2  135 OPC-A3 100 32 3  135 OPC-F1(B) 100 32  1 135 OPC-F2 100 32  2 135 OPC-F3 100 32  3 135 ( A )A = calcium acetate, 1 = cement × 1 wt%. ( B )F = calcium formate, 1 = cement × 1 wt%.The paste specimens were produced by mixing 0, 1, 2, and 3% of CA and CF each with 100 g of OPC at a water to binder ratio of 0.32 for 3 min. The setting time and pH of these specimens were evaluated. Their XRD patterns were also analyzed. The setting time was measured according to ASTM C191. The pH measurements were performed by collecting 10 mL of each material after binding and subsequently immersing them in 100 g of distilled water. The results were recorded at 60 min and 24 h, in triplicate. For the XRD analysis, 30 g of the cured paste specimen was collected after 18 and 24 h, following which it was broken down into particles of <300μm diameter of the particles and finally immersed in acetone. The X-ray diffractometer was operated at 45 KV and 40 mA with Cu radiation. A scan rate of 5°/min was maintained over a range of 5–60°.The cement mortar was manufactured by adding 135 g of sand to the paste composites. The sand and paste composites were mixed for 3 min, allowed to rest for 2 min, and finally mixed for additional 2 min. The flow of the mixed specimen was measured according to ASTM C230. For each mixture, molds with the dimensions of 4 cm × 4 cm × 16 cm were formed, cured for 18 h, and were immediately removed. The compressive strength was measured according to ASTM C109 at the intervals of 1, 3, 7, and 28 days, in triplicate.


## 2.1. Materials

### 2.1.1. Limestone Sludge

In this study, LSS, which is obtained from industrial by-products, was used to manufacture the calcium-containing HESAs. The XRD pattern and chemical composition analyses of LSS are shown in Figure1 and Table 1, respectively. The XRD patterns of both CaCO3 and LSS showed the presence of a CaCO3 peak at approximately 29°. The structure of LSS appears to be identical to that of CaCO3. However, considering the chemical composition, the CaO content in LSS was approximately 5.84% lesser than that in CaCO3. In addition, LSS also contained SiO2 and metallic salts such as Al2O3 and Fe2O3.Table 1
Chemical composition of CaCO3 and LSS (%).
CaO SiO2 MgO Al2O3 SO3 Fe2O3 P2O5 K2O Na2O CaCO3 96.08 0.98 2.06 0.39 0.02 0.36 0.00 0.11 0.00  Limestone sludge 90.46 3.81 1.06 2.06 0.08 1.35 0.70 0.45 0.04Figure 1
XRD patterns of CaCO3 and LSS.


### 2.1.2. Recycled Acetic Acid

Recycled acetic acid (RAA) was obtained from the previous etching processes by extraction via an acid separation process. In this study, approximately 60% RAA was used. Figure2 shows the Fourier transform infrared (FT-IR) spectrum of RAA. In the FT-IR spectrum of RAA, the peaks in the range of 3300–2500 cm−1 correspond to organic acids containing carboxylic groups. The peaks associated with C=O groups (1760–1690 cm−1) and C-O groups (1320–1210 cm−1) can also be observed in this spectrum. Some examples of carboxylic acids include acetic acid, formic acid, gluconic acid, and propionic acid. Hence, it was confirmed that RAA contained carboxylic acid groups [27].Figure 2
FT-IR spectrum of RAA.


### 2.1.3. Binder and Sand

A comparison between the properties of the conventional HESAs and the admixture produced in this study was performed by using mortar specimens. The mortar specimens consisted of class I ordinary Portland (OPC). The chemical compositions and physical properties of these materials are given in Tables2 and 3, respectively. A description of the sand used in this study is given in Table 4.Table 2
Chemical composition of binder (%).
CaO SiO2 MgO Al2O3 SO3 Fe2O3 P2O5 K2O Na2O 63.85 21.09 3.32 4.84 3.09 2.39 0.36 0.73 0.14Table 3
Physical properties of ordinary Portland cement (OPC).
Specific gravity Blaine specific surface (cm2/g) Setting time Compressive strength of mortar (MPa) Initial set (min) Final set (hour) 3 days 7 days 28 days 3.15 3400 400 7 20 23 38Table 4
Properties of fine aggregate.
Maximum size (mm) Unit weight (kg/l) Specific gravity Water absorption (%) Solid volume percentage (%) <1.2 1.5 2.62 0.40 58.1


## 2.1.1. Limestone Sludge

In this study, LSS, which is obtained from industrial by-products, was used to manufacture the calcium-containing HESAs. The XRD pattern and chemical composition analyses of LSS are shown in Figure1 and Table 1, respectively. The XRD patterns of both CaCO3 and LSS showed the presence of a CaCO3 peak at approximately 29°. The structure of LSS appears to be identical to that of CaCO3. However, considering the chemical composition, the CaO content in LSS was approximately 5.84% lesser than that in CaCO3. In addition, LSS also contained SiO2 and metallic salts such as Al2O3 and Fe2O3.Table 1
Chemical composition of CaCO3 and LSS (%).
CaO SiO2 MgO Al2O3 SO3 Fe2O3 P2O5 K2O Na2O CaCO3 96.08 0.98 2.06 0.39 0.02 0.36 0.00 0.11 0.00  Limestone sludge 90.46 3.81 1.06 2.06 0.08 1.35 0.70 0.45 0.04Figure 1
XRD patterns of CaCO3 and LSS.


## 2.1.2. Recycled Acetic Acid

Recycled acetic acid (RAA) was obtained from the previous etching processes by extraction via an acid separation process. In this study, approximately 60% RAA was used. Figure2 shows the Fourier transform infrared (FT-IR) spectrum of RAA. In the FT-IR spectrum of RAA, the peaks in the range of 3300–2500 cm−1 correspond to organic acids containing carboxylic groups. The peaks associated with C=O groups (1760–1690 cm−1) and C-O groups (1320–1210 cm−1) can also be observed in this spectrum. Some examples of carboxylic acids include acetic acid, formic acid, gluconic acid, and propionic acid. Hence, it was confirmed that RAA contained carboxylic acid groups [27].Figure 2
FT-IR spectrum of RAA.


## 2.1.3. Binder and Sand

A comparison between the properties of the conventional HESAs and the admixture produced in this study was performed by using mortar specimens. The mortar specimens consisted of class I ordinary Portland (OPC). The chemical compositions and physical properties of these materials are given in Tables2 and 3, respectively. A description of the sand used in this study is given in Table 4.Table 2
Chemical composition of binder (%).
CaO SiO2 MgO Al2O3 SO3 Fe2O3 P2O5 K2O Na2O 63.85 21.09 3.32 4.84 3.09 2.39 0.36 0.73 0.14Table 3
Physical properties of ordinary Portland cement (OPC).
Specific gravity Blaine specific surface (cm2/g) Setting time Compressive strength of mortar (MPa) Initial set (min) Final set (hour) 3 days 7 days 28 days 3.15 3400 400 7 20 23 38Table 4
Properties of fine aggregate.
Maximum size (mm) Unit weight (kg/l) Specific gravity Water absorption (%) Solid volume percentage (%) <1.2 1.5 2.62 0.40 58.1


## 2.2. Methods

### 2.2.1. Overview

In this study, we manufactured both the CA and the mortars containing CA in different weight ratios (0, 1, 2, and 3 wt%) and evaluated the performance of these mortars. The viscosity, density, and pH of these mortars were evaluated. Their inductively coupled plasma mass spectroscopy (ICP-MS) analyses were also performed. In addition, an existing HESA (CF) was also added to mortar in different weight ratios (0, 1, 2, and 3 wt%) to obtain CF-mortars and their CF content, setting time, XRD patterns, and pH were also investigated. The flow behavior and compressive strength of the mortars were also measured. Table5 summarizes these experiments. The flow chart for the synthesis of CA is shown in Figure 3.Table 5
Measurements and methods.
Experiment Measurement sample Properties measured Standards Calcium acetate using limestone sludge and recycled acetate Calcium acetate Viscosity (cps) ASTM D 2196 [28] Density (kg/m3) ASTM D 4052-11 [29] pH — ICP-MS analysis ASTM D 6800-12 [30]  Cement matrix using accelerator Cement paste Setting time ASTM C 191 [31] pH — XRD — Cement mortar Flow ASTM C 230/230M-14 [32] Compressive strength ASTM C 109 [33]Figure 3
Flow diagram for CA synthesis.


### 2.2.2. Manufacturing CA with LSS and RAA

Here, RAA and LSS reacted to yield CA in accordance with (1). The yield was maximum when the ratio of acetic acid to CaCO3 was 2 : 1 with 1 mol each of CA, water, and carbon dioxide per mol of CaCO3:(1)2CH3COOH+CaCO3=CaCH3COO2+H2O+CO2Calcium carbonate and RAA were used to compare the solubility of the LSS and acetic acid together. To 60% solid acetic acid, LSS was added in different weight ratios (1, 1.5, or 2) as shown in Table 6. This mix was reacted for 12 h. Upon mixing, the unreacted particles were removed via filtering and acetic acid was separated for future use.Table 6
Reaction ratio according to weight ratio of RAA : CaCO3.
RAA : CaCO3 1 : 0.5 1 : 1 1 : 1.5 1 : 2 Reaction yield (%) 52 42 31 24.97 Reacted acetic acid (%) 42.4 80.8 91.6 99.86


### 2.2.3. Cementitious Composites with HESAs

The mix proportions of the cementitious composites (cement paste and mortar) that were mixed with HESAs are given in Table7. The CA (used as a HESA) was weighed such that the weight ratio of LSS to acetic acid was 2 : 1 and the pH of the overall mixture was 5.9. The manufactured specimen underwent steam curing at a temperature of 20°C and a relative humidity of 60%.Table 7
Mixtures for paste and mortar specimens.
Mixture number OPC Water Calcium acetate Calcium formate Sand OPC 100 32 0  135 OPC-A1(A) 100 32 1  135 OPC-A2 100 32 2  135 OPC-A3 100 32 3  135 OPC-F1(B) 100 32  1 135 OPC-F2 100 32  2 135 OPC-F3 100 32  3 135 ( A )A = calcium acetate, 1 = cement × 1 wt%. ( B )F = calcium formate, 1 = cement × 1 wt%.The paste specimens were produced by mixing 0, 1, 2, and 3% of CA and CF each with 100 g of OPC at a water to binder ratio of 0.32 for 3 min. The setting time and pH of these specimens were evaluated. Their XRD patterns were also analyzed. The setting time was measured according to ASTM C191. The pH measurements were performed by collecting 10 mL of each material after binding and subsequently immersing them in 100 g of distilled water. The results were recorded at 60 min and 24 h, in triplicate. For the XRD analysis, 30 g of the cured paste specimen was collected after 18 and 24 h, following which it was broken down into particles of <300μm diameter of the particles and finally immersed in acetone. The X-ray diffractometer was operated at 45 KV and 40 mA with Cu radiation. A scan rate of 5°/min was maintained over a range of 5–60°.The cement mortar was manufactured by adding 135 g of sand to the paste composites. The sand and paste composites were mixed for 3 min, allowed to rest for 2 min, and finally mixed for additional 2 min. The flow of the mixed specimen was measured according to ASTM C230. For each mixture, molds with the dimensions of 4 cm × 4 cm × 16 cm were formed, cured for 18 h, and were immediately removed. The compressive strength was measured according to ASTM C109 at the intervals of 1, 3, 7, and 28 days, in triplicate.


## 2.2.1. Overview

In this study, we manufactured both the CA and the mortars containing CA in different weight ratios (0, 1, 2, and 3 wt%) and evaluated the performance of these mortars. The viscosity, density, and pH of these mortars were evaluated. Their inductively coupled plasma mass spectroscopy (ICP-MS) analyses were also performed. In addition, an existing HESA (CF) was also added to mortar in different weight ratios (0, 1, 2, and 3 wt%) to obtain CF-mortars and their CF content, setting time, XRD patterns, and pH were also investigated. The flow behavior and compressive strength of the mortars were also measured. Table5 summarizes these experiments. The flow chart for the synthesis of CA is shown in Figure 3.Table 5
Measurements and methods.
Experiment Measurement sample Properties measured Standards Calcium acetate using limestone sludge and recycled acetate Calcium acetate Viscosity (cps) ASTM D 2196 [28] Density (kg/m3) ASTM D 4052-11 [29] pH — ICP-MS analysis ASTM D 6800-12 [30]  Cement matrix using accelerator Cement paste Setting time ASTM C 191 [31] pH — XRD — Cement mortar Flow ASTM C 230/230M-14 [32] Compressive strength ASTM C 109 [33]Figure 3
Flow diagram for CA synthesis.


## 2.2.2. Manufacturing CA with LSS and RAA

Here, RAA and LSS reacted to yield CA in accordance with (1). The yield was maximum when the ratio of acetic acid to CaCO3 was 2 : 1 with 1 mol each of CA, water, and carbon dioxide per mol of CaCO3:(1)2CH3COOH+CaCO3=CaCH3COO2+H2O+CO2Calcium carbonate and RAA were used to compare the solubility of the LSS and acetic acid together. To 60% solid acetic acid, LSS was added in different weight ratios (1, 1.5, or 2) as shown in Table 6. This mix was reacted for 12 h. Upon mixing, the unreacted particles were removed via filtering and acetic acid was separated for future use.Table 6
Reaction ratio according to weight ratio of RAA : CaCO3.
RAA : CaCO3 1 : 0.5 1 : 1 1 : 1.5 1 : 2 Reaction yield (%) 52 42 31 24.97 Reacted acetic acid (%) 42.4 80.8 91.6 99.86


## 2.2.3. Cementitious Composites with HESAs

The mix proportions of the cementitious composites (cement paste and mortar) that were mixed with HESAs are given in Table7. The CA (used as a HESA) was weighed such that the weight ratio of LSS to acetic acid was 2 : 1 and the pH of the overall mixture was 5.9. The manufactured specimen underwent steam curing at a temperature of 20°C and a relative humidity of 60%.Table 7
Mixtures for paste and mortar specimens.
Mixture number OPC Water Calcium acetate Calcium formate Sand OPC 100 32 0  135 OPC-A1(A) 100 32 1  135 OPC-A2 100 32 2  135 OPC-A3 100 32 3  135 OPC-F1(B) 100 32  1 135 OPC-F2 100 32  2 135 OPC-F3 100 32  3 135 ( A )A = calcium acetate, 1 = cement × 1 wt%. ( B )F = calcium formate, 1 = cement × 1 wt%.The paste specimens were produced by mixing 0, 1, 2, and 3% of CA and CF each with 100 g of OPC at a water to binder ratio of 0.32 for 3 min. The setting time and pH of these specimens were evaluated. Their XRD patterns were also analyzed. The setting time was measured according to ASTM C191. The pH measurements were performed by collecting 10 mL of each material after binding and subsequently immersing them in 100 g of distilled water. The results were recorded at 60 min and 24 h, in triplicate. For the XRD analysis, 30 g of the cured paste specimen was collected after 18 and 24 h, following which it was broken down into particles of <300μm diameter of the particles and finally immersed in acetone. The X-ray diffractometer was operated at 45 KV and 40 mA with Cu radiation. A scan rate of 5°/min was maintained over a range of 5–60°.The cement mortar was manufactured by adding 135 g of sand to the paste composites. The sand and paste composites were mixed for 3 min, allowed to rest for 2 min, and finally mixed for additional 2 min. The flow of the mixed specimen was measured according to ASTM C230. For each mixture, molds with the dimensions of 4 cm × 4 cm × 16 cm were formed, cured for 18 h, and were immediately removed. The compressive strength was measured according to ASTM C109 at the intervals of 1, 3, 7, and 28 days, in triplicate.


## 3. Results and Discussion

### 3.1. CA

#### 3.1.1. pH and Density of CA

The results of the viscosity and density measurements of the manufactured CA are shown in Figure4. The viscosity and density of the CA solutions (containing CaCO3 and LSS in weight ratios) showed similar trends. The viscosity and density of the CA solutions increased with an increase in the weight ratios of CaCO3 and LSS. The density of acetic acid is 1.049 g/cm3 and that of the CA is 1.509 g/cm3. Thus, as a greater quantity of acetic acid reacts with CaCO3 to produce the CA, the density of this reactant increases.Figure 4
Viscosity and density of calcium acetate.
(a)
CA made from CaCO3 and acetic acid (b)
CA made from sludge and acetic acid


#### 3.1.2. pH and Ca Ion-ICP Analysis

Figure5 shows the results of the pH measurement and Ca Ion-ICP analysis of the manufactured CA. The pH appeared to increase slightly when calcium carbonate was used. Conversely, the pH was low when LSS was used as it contains small quantities of Ca. However, when the weight ratio of LSS was greater than 2, the pH of the CA produced using CaCO3 was similar to that obtained when LSS was used for producing the CA.Figure 5
pH and Ca ion concentration of calcium acetate.
(a)
CA made from CaCO3 and acetic acid (b)
CA made from limestone sludge and acetic acid


#### 3.1.3. Microelement Analysis

Table8 shows the results of the ICP analysis of heavy metals of the manufactured CA. The microelements and solid contents of the manufactured CA are listed in Table 8. Heavy metals were not detected, indicating that the CA manufactured in this work is less hazardous to the environment than the other similar materials [34].Table 8
ICP Analysis of heavy metals (mg/l).
Recycled acetic acid Limestone sludge : recycled acetic acid Standard(A) 2 : 1 2 : 1.5 2 : 2 Cd Not detected Not detected Not detected Not detected <0.1 Cr Not detected Not detected Not detected Not detected <2 Cu 3 1.5 1.62 1.61 <3 Hg Not detected Not detected Not detected Not detected <0.005 Pb Not detected Not detected Not detected Not detected <1 Mn Not detected Not detected Not detected Not detected — Zn 3 1.5 1.7 1.9 <5 As Not detected Not detected Not detected Not detected <0.5 Solid contents 62% 22% 27% 29% ( A )Water quality standards of Japan.


### 3.2. Cement Composites

#### 3.2.1. Flow and Setting Time of Mortar

Figures6 and 7 display the flow and setting times, respectively, of the cement mortar obtained by mixing CA with cement. It was found that, for the CA-mortar, the fluidity increased with an increase in the CA content, as shown in Figure 6. However, in the case of the CF-mortar, the fluidity decreased with an increase in the CF content.Figure 6
Flow test results.Figure 7
Setting time tests results.
(a)
Initial setting time (b)
Final setting timeFrom Figure7, it can be observed that when CF was used and the mixing ratio was identical for the CA- and CF-mixed mortars, the initial and finish setting times were reduced. In the case of the CA-mortar, the initial setting time was reduced when the mixing ratio increased. At a CA content of 1%, a minimum final setting time was obtained, which increased as the mixing ratio increased. In case of the CF-mortar, no reversible change in the setting time was observed with a change in the mixing ratio, and the setting time decreased proportionally with a decrease in the mixture ratio.


#### 3.2.2. Change in pH of Cement Paste

The pH values of the cement pastes, as a function of time, are given in Table9. In the case of the paste containing the CA, the pH initially decreased with an increase in the CA content. On the other hand, in the case of the paste containing CF, the pH remained relatively constant regardless of the CF content. When the CA content exceeded 1%, the setting time was reduced. Bortoluzzi et al. reported that when CaCl2 (pH = 4.4) is mixed with cement, the pH of the cement decreases. The pH subsequently recovers because of the production of Ca2+, which reduces the setting time [35]. When 3% CA is mixed, the hydration time decreases to 24 h and a retarding phenomenon can be observed. When CA content is more than 2%, both initial pH decrease and setting time delay were observed because of the high solubility of CA and residual acetic acid.Table 9
pH of cement paste as a function of time.
HESA Admixture proportion (cement  ×  %) pH of cement paste as a function of time Immediate 60 minutes 24 hours OPC 12.2 12.4 12.4  Calcium acetate OPC-A1 11.8 12.2 12.3 OPC-A2 10.2 11.0 12.1 OPC-A3 9.0 10.2 11.9  Calcium formate OPC-F1 12.3 12.2 12.4 OPC-F2 12.2 12.3 12.3 OPC-F3 12.1 12.2 12.1


#### 3.2.3. Compressive Strength of Mortar

Figure8 shows the compressive strengths of the CA- and CF-mortar specimens at different curing times. When a CA content of 1% was used, the compressive strength of the resulting mixture was 22% greater than that obtained when no admixture was added (i.e., for a standard specimen). When the CF content in the mortar was 2%, similar strengths were obtained. When 3% CF was mixed and the mix was cured for seven days, the strength of the resulting mortar was found to be greater than that of the standard material. However, the strength started decreasing after 28 days. When 1% CA was mixed and the mix was cured for three days, the strength of the resulting mortar was over 40% greater than that of the standard specimen and was still 14% greater even after 28 days. However, when the CA content exceeded 2%, the compressive strength of the material diminished because of the reduction in both the pH of the cement paste and the hydration of acetic acid.Figure 8
Compressive strength of specimens.
(a)
Specimen incorporating calcium acetate (b)
Specimen incorporating calcium formate


#### 3.2.4. XRD

The XRD analysis was performed on the CA- and CF-mortars. Figure9 shows the XRD patterns of the CA-mortars with different CA contents after a curing period of one day. When 1% CA was mixed, the intensity of the Ca(OH)2 peak decreased, while that of the calcium aluminosilicate hydrate (C-A-S-H) and C-S-H peaks increased, indicating rapid hydration. The CA-mortar having a CA content of 3% showed a weaker Ca(OH)2 peak than that of the mortar containing no admixture. However, in the case of the CA-mortar containing 1% admixture, this peak was more intense, and the intensity of the C-A-S-H and C-S-H peaks was also lower. In contrast, the intensity of the ettringite peak increased as the CA content increased.Figure 9
Specimen incorporating calcium acetate (1 day).The XRD patterns of the CF-mortars with different CF contents after a curing period of one day are shown in Figure10. When 1% CF was mixed, the intensity of both the Ca(OH)2 and C-A-S-H peaks increased. When 3% CF was mixed, the intensity of both the Ca(OH)2 and C-A-S-H peaks decreased, while that of the ettringite and C-S-H peaks increased. As reported by Heikal [36], the diffusion rate of HCOO− ions is greater than that of Ca2+ ions. Therefore, it is possible for HCOO− ions to penetrate into the protective layer of C-S-H. As a result, the C-S-H decomposition is directly proportional to the deposition of Ca(OH)2. In addition, Ramachandran [37] stated that the presence of COOH− ions promotes the hydration of C3S by interfering with the protective layer of cement particles, which ultimately leads to the formation of ettringite. It was found that the structure of the CA- and CF-mortars containing 1% CA and CF, respectively, was similar, and both the mortars enhanced the production of C-A-S-H, ettringite, and C-S-H during the initial early stages of concrete formation [38].Figure 10
Specimen incorporating calcium formate (1 day).The XRD patterns of the CA- and CF-mortars cured for three days are shown in Figures11 and 12, respectively. In the case of the CA-mortar containing 1% CA, ettringite, the Ca(OH)2, and C-A-S-H peaks were more intense, as shown in Figure 11. When 3% CA was mixed, the intensity of the Ca(OH)2 and C-A-S-H peak decreased, while that of the ettringite and C-S-H peaks increased. In the case of the CA-mortar containing 1% CF, ettringite, the Ca(OH)2, and C-A-S-H peaks were more intense, as shown in Figure 11. When 3% CA was mixed, the intensity of the Ca(OH)2 and C-A-S-H peak decreased, while that of the ettringite peaks increased as shown in Figure 12.Figure 11
Specimen incorporating calcium acetate (3 days).Figure 12
Specimen incorporating calcium formate (3 days).When Al ion content is the same, Ca(OH)2 and C-A-S-H increase according to the increase of Ca ion [39]. Thus, when CA and CF contents are 1%, Ca(OH)2 and C-A-S-H increased. On the other hand, according to the increase of CA and CF contents, Ca(OH)2 and C-A-S-H peaks decreased. While the pH of CF is 7.0 and its solubility is 166 g/L, the pH of CA is about 5.9 and its density is 247 g/L. High solubility of CA affected both ettringite generation and decrease of Ca(OH)2 and C-A-S-H peaks [40].


## 3.1. CA

### 3.1.1. pH and Density of CA

The results of the viscosity and density measurements of the manufactured CA are shown in Figure4. The viscosity and density of the CA solutions (containing CaCO3 and LSS in weight ratios) showed similar trends. The viscosity and density of the CA solutions increased with an increase in the weight ratios of CaCO3 and LSS. The density of acetic acid is 1.049 g/cm3 and that of the CA is 1.509 g/cm3. Thus, as a greater quantity of acetic acid reacts with CaCO3 to produce the CA, the density of this reactant increases.Figure 4
Viscosity and density of calcium acetate.
(a)
CA made from CaCO3 and acetic acid (b)
CA made from sludge and acetic acid


### 3.1.2. pH and Ca Ion-ICP Analysis

Figure5 shows the results of the pH measurement and Ca Ion-ICP analysis of the manufactured CA. The pH appeared to increase slightly when calcium carbonate was used. Conversely, the pH was low when LSS was used as it contains small quantities of Ca. However, when the weight ratio of LSS was greater than 2, the pH of the CA produced using CaCO3 was similar to that obtained when LSS was used for producing the CA.Figure 5
pH and Ca ion concentration of calcium acetate.
(a)
CA made from CaCO3 and acetic acid (b)
CA made from limestone sludge and acetic acid


### 3.1.3. Microelement Analysis

Table8 shows the results of the ICP analysis of heavy metals of the manufactured CA. The microelements and solid contents of the manufactured CA are listed in Table 8. Heavy metals were not detected, indicating that the CA manufactured in this work is less hazardous to the environment than the other similar materials [34].Table 8
ICP Analysis of heavy metals (mg/l).
Recycled acetic acid Limestone sludge : recycled acetic acid Standard(A) 2 : 1 2 : 1.5 2 : 2 Cd Not detected Not detected Not detected Not detected <0.1 Cr Not detected Not detected Not detected Not detected <2 Cu 3 1.5 1.62 1.61 <3 Hg Not detected Not detected Not detected Not detected <0.005 Pb Not detected Not detected Not detected Not detected <1 Mn Not detected Not detected Not detected Not detected — Zn 3 1.5 1.7 1.9 <5 As Not detected Not detected Not detected Not detected <0.5 Solid contents 62% 22% 27% 29% ( A )Water quality standards of Japan.


## 3.1.1. pH and Density of CA

The results of the viscosity and density measurements of the manufactured CA are shown in Figure4. The viscosity and density of the CA solutions (containing CaCO3 and LSS in weight ratios) showed similar trends. The viscosity and density of the CA solutions increased with an increase in the weight ratios of CaCO3 and LSS. The density of acetic acid is 1.049 g/cm3 and that of the CA is 1.509 g/cm3. Thus, as a greater quantity of acetic acid reacts with CaCO3 to produce the CA, the density of this reactant increases.Figure 4
Viscosity and density of calcium acetate.
(a)
CA made from CaCO3 and acetic acid (b)
CA made from sludge and acetic acid


## 3.1.2. pH and Ca Ion-ICP Analysis

Figure5 shows the results of the pH measurement and Ca Ion-ICP analysis of the manufactured CA. The pH appeared to increase slightly when calcium carbonate was used. Conversely, the pH was low when LSS was used as it contains small quantities of Ca. However, when the weight ratio of LSS was greater than 2, the pH of the CA produced using CaCO3 was similar to that obtained when LSS was used for producing the CA.Figure 5
pH and Ca ion concentration of calcium acetate.
(a)
CA made from CaCO3 and acetic acid (b)
CA made from limestone sludge and acetic acid


## 3.1.3. Microelement Analysis

Table8 shows the results of the ICP analysis of heavy metals of the manufactured CA. The microelements and solid contents of the manufactured CA are listed in Table 8. Heavy metals were not detected, indicating that the CA manufactured in this work is less hazardous to the environment than the other similar materials [34].Table 8
ICP Analysis of heavy metals (mg/l).
Recycled acetic acid Limestone sludge : recycled acetic acid Standard(A) 2 : 1 2 : 1.5 2 : 2 Cd Not detected Not detected Not detected Not detected <0.1 Cr Not detected Not detected Not detected Not detected <2 Cu 3 1.5 1.62 1.61 <3 Hg Not detected Not detected Not detected Not detected <0.005 Pb Not detected Not detected Not detected Not detected <1 Mn Not detected Not detected Not detected Not detected — Zn 3 1.5 1.7 1.9 <5 As Not detected Not detected Not detected Not detected <0.5 Solid contents 62% 22% 27% 29% ( A )Water quality standards of Japan.


## 3.2. Cement Composites

### 3.2.1. Flow and Setting Time of Mortar

Figures6 and 7 display the flow and setting times, respectively, of the cement mortar obtained by mixing CA with cement. It was found that, for the CA-mortar, the fluidity increased with an increase in the CA content, as shown in Figure 6. However, in the case of the CF-mortar, the fluidity decreased with an increase in the CF content.Figure 6
Flow test results.Figure 7
Setting time tests results.
(a)
Initial setting time (b)
Final setting timeFrom Figure7, it can be observed that when CF was used and the mixing ratio was identical for the CA- and CF-mixed mortars, the initial and finish setting times were reduced. In the case of the CA-mortar, the initial setting time was reduced when the mixing ratio increased. At a CA content of 1%, a minimum final setting time was obtained, which increased as the mixing ratio increased. In case of the CF-mortar, no reversible change in the setting time was observed with a change in the mixing ratio, and the setting time decreased proportionally with a decrease in the mixture ratio.


### 3.2.2. Change in pH of Cement Paste

The pH values of the cement pastes, as a function of time, are given in Table9. In the case of the paste containing the CA, the pH initially decreased with an increase in the CA content. On the other hand, in the case of the paste containing CF, the pH remained relatively constant regardless of the CF content. When the CA content exceeded 1%, the setting time was reduced. Bortoluzzi et al. reported that when CaCl2 (pH = 4.4) is mixed with cement, the pH of the cement decreases. The pH subsequently recovers because of the production of Ca2+, which reduces the setting time [35]. When 3% CA is mixed, the hydration time decreases to 24 h and a retarding phenomenon can be observed. When CA content is more than 2%, both initial pH decrease and setting time delay were observed because of the high solubility of CA and residual acetic acid.Table 9
pH of cement paste as a function of time.
HESA Admixture proportion (cement  ×  %) pH of cement paste as a function of time Immediate 60 minutes 24 hours OPC 12.2 12.4 12.4  Calcium acetate OPC-A1 11.8 12.2 12.3 OPC-A2 10.2 11.0 12.1 OPC-A3 9.0 10.2 11.9  Calcium formate OPC-F1 12.3 12.2 12.4 OPC-F2 12.2 12.3 12.3 OPC-F3 12.1 12.2 12.1


### 3.2.3. Compressive Strength of Mortar

Figure8 shows the compressive strengths of the CA- and CF-mortar specimens at different curing times. When a CA content of 1% was used, the compressive strength of the resulting mixture was 22% greater than that obtained when no admixture was added (i.e., for a standard specimen). When the CF content in the mortar was 2%, similar strengths were obtained. When 3% CF was mixed and the mix was cured for seven days, the strength of the resulting mortar was found to be greater than that of the standard material. However, the strength started decreasing after 28 days. When 1% CA was mixed and the mix was cured for three days, the strength of the resulting mortar was over 40% greater than that of the standard specimen and was still 14% greater even after 28 days. However, when the CA content exceeded 2%, the compressive strength of the material diminished because of the reduction in both the pH of the cement paste and the hydration of acetic acid.Figure 8
Compressive strength of specimens.
(a)
Specimen incorporating calcium acetate (b)
Specimen incorporating calcium formate


### 3.2.4. XRD

The XRD analysis was performed on the CA- and CF-mortars. Figure9 shows the XRD patterns of the CA-mortars with different CA contents after a curing period of one day. When 1% CA was mixed, the intensity of the Ca(OH)2 peak decreased, while that of the calcium aluminosilicate hydrate (C-A-S-H) and C-S-H peaks increased, indicating rapid hydration. The CA-mortar having a CA content of 3% showed a weaker Ca(OH)2 peak than that of the mortar containing no admixture. However, in the case of the CA-mortar containing 1% admixture, this peak was more intense, and the intensity of the C-A-S-H and C-S-H peaks was also lower. In contrast, the intensity of the ettringite peak increased as the CA content increased.Figure 9
Specimen incorporating calcium acetate (1 day).The XRD patterns of the CF-mortars with different CF contents after a curing period of one day are shown in Figure10. When 1% CF was mixed, the intensity of both the Ca(OH)2 and C-A-S-H peaks increased. When 3% CF was mixed, the intensity of both the Ca(OH)2 and C-A-S-H peaks decreased, while that of the ettringite and C-S-H peaks increased. As reported by Heikal [36], the diffusion rate of HCOO− ions is greater than that of Ca2+ ions. Therefore, it is possible for HCOO− ions to penetrate into the protective layer of C-S-H. As a result, the C-S-H decomposition is directly proportional to the deposition of Ca(OH)2. In addition, Ramachandran [37] stated that the presence of COOH− ions promotes the hydration of C3S by interfering with the protective layer of cement particles, which ultimately leads to the formation of ettringite. It was found that the structure of the CA- and CF-mortars containing 1% CA and CF, respectively, was similar, and both the mortars enhanced the production of C-A-S-H, ettringite, and C-S-H during the initial early stages of concrete formation [38].Figure 10
Specimen incorporating calcium formate (1 day).The XRD patterns of the CA- and CF-mortars cured for three days are shown in Figures11 and 12, respectively. In the case of the CA-mortar containing 1% CA, ettringite, the Ca(OH)2, and C-A-S-H peaks were more intense, as shown in Figure 11. When 3% CA was mixed, the intensity of the Ca(OH)2 and C-A-S-H peak decreased, while that of the ettringite and C-S-H peaks increased. In the case of the CA-mortar containing 1% CF, ettringite, the Ca(OH)2, and C-A-S-H peaks were more intense, as shown in Figure 11. When 3% CA was mixed, the intensity of the Ca(OH)2 and C-A-S-H peak decreased, while that of the ettringite peaks increased as shown in Figure 12.Figure 11
Specimen incorporating calcium acetate (3 days).Figure 12
Specimen incorporating calcium formate (3 days).When Al ion content is the same, Ca(OH)2 and C-A-S-H increase according to the increase of Ca ion [39]. Thus, when CA and CF contents are 1%, Ca(OH)2 and C-A-S-H increased. On the other hand, according to the increase of CA and CF contents, Ca(OH)2 and C-A-S-H peaks decreased. While the pH of CF is 7.0 and its solubility is 166 g/L, the pH of CA is about 5.9 and its density is 247 g/L. High solubility of CA affected both ettringite generation and decrease of Ca(OH)2 and C-A-S-H peaks [40].


## 3.2.1. Flow and Setting Time of Mortar

Figures6 and 7 display the flow and setting times, respectively, of the cement mortar obtained by mixing CA with cement. It was found that, for the CA-mortar, the fluidity increased with an increase in the CA content, as shown in Figure 6. However, in the case of the CF-mortar, the fluidity decreased with an increase in the CF content.Figure 6
Flow test results.Figure 7
Setting time tests results.
(a)
Initial setting time (b)
Final setting timeFrom Figure7, it can be observed that when CF was used and the mixing ratio was identical for the CA- and CF-mixed mortars, the initial and finish setting times were reduced. In the case of the CA-mortar, the initial setting time was reduced when the mixing ratio increased. At a CA content of 1%, a minimum final setting time was obtained, which increased as the mixing ratio increased. In case of the CF-mortar, no reversible change in the setting time was observed with a change in the mixing ratio, and the setting time decreased proportionally with a decrease in the mixture ratio.


## 3.2.2. Change in pH of Cement Paste

The pH values of the cement pastes, as a function of time, are given in Table9. In the case of the paste containing the CA, the pH initially decreased with an increase in the CA content. On the other hand, in the case of the paste containing CF, the pH remained relatively constant regardless of the CF content. When the CA content exceeded 1%, the setting time was reduced. Bortoluzzi et al. reported that when CaCl2 (pH = 4.4) is mixed with cement, the pH of the cement decreases. The pH subsequently recovers because of the production of Ca2+, which reduces the setting time [35]. When 3% CA is mixed, the hydration time decreases to 24 h and a retarding phenomenon can be observed. When CA content is more than 2%, both initial pH decrease and setting time delay were observed because of the high solubility of CA and residual acetic acid.Table 9
pH of cement paste as a function of time.
HESA Admixture proportion (cement  ×  %) pH of cement paste as a function of time Immediate 60 minutes 24 hours OPC 12.2 12.4 12.4  Calcium acetate OPC-A1 11.8 12.2 12.3 OPC-A2 10.2 11.0 12.1 OPC-A3 9.0 10.2 11.9  Calcium formate OPC-F1 12.3 12.2 12.4 OPC-F2 12.2 12.3 12.3 OPC-F3 12.1 12.2 12.1


## 3.2.3. Compressive Strength of Mortar

Figure8 shows the compressive strengths of the CA- and CF-mortar specimens at different curing times. When a CA content of 1% was used, the compressive strength of the resulting mixture was 22% greater than that obtained when no admixture was added (i.e., for a standard specimen). When the CF content in the mortar was 2%, similar strengths were obtained. When 3% CF was mixed and the mix was cured for seven days, the strength of the resulting mortar was found to be greater than that of the standard material. However, the strength started decreasing after 28 days. When 1% CA was mixed and the mix was cured for three days, the strength of the resulting mortar was over 40% greater than that of the standard specimen and was still 14% greater even after 28 days. However, when the CA content exceeded 2%, the compressive strength of the material diminished because of the reduction in both the pH of the cement paste and the hydration of acetic acid.Figure 8
Compressive strength of specimens.
(a)
Specimen incorporating calcium acetate (b)
Specimen incorporating calcium formate


## 3.2.4. XRD

The XRD analysis was performed on the CA- and CF-mortars. Figure9 shows the XRD patterns of the CA-mortars with different CA contents after a curing period of one day. When 1% CA was mixed, the intensity of the Ca(OH)2 peak decreased, while that of the calcium aluminosilicate hydrate (C-A-S-H) and C-S-H peaks increased, indicating rapid hydration. The CA-mortar having a CA content of 3% showed a weaker Ca(OH)2 peak than that of the mortar containing no admixture. However, in the case of the CA-mortar containing 1% admixture, this peak was more intense, and the intensity of the C-A-S-H and C-S-H peaks was also lower. In contrast, the intensity of the ettringite peak increased as the CA content increased.Figure 9
Specimen incorporating calcium acetate (1 day).The XRD patterns of the CF-mortars with different CF contents after a curing period of one day are shown in Figure10. When 1% CF was mixed, the intensity of both the Ca(OH)2 and C-A-S-H peaks increased. When 3% CF was mixed, the intensity of both the Ca(OH)2 and C-A-S-H peaks decreased, while that of the ettringite and C-S-H peaks increased. As reported by Heikal [36], the diffusion rate of HCOO− ions is greater than that of Ca2+ ions. Therefore, it is possible for HCOO− ions to penetrate into the protective layer of C-S-H. As a result, the C-S-H decomposition is directly proportional to the deposition of Ca(OH)2. In addition, Ramachandran [37] stated that the presence of COOH− ions promotes the hydration of C3S by interfering with the protective layer of cement particles, which ultimately leads to the formation of ettringite. It was found that the structure of the CA- and CF-mortars containing 1% CA and CF, respectively, was similar, and both the mortars enhanced the production of C-A-S-H, ettringite, and C-S-H during the initial early stages of concrete formation [38].Figure 10
Specimen incorporating calcium formate (1 day).The XRD patterns of the CA- and CF-mortars cured for three days are shown in Figures11 and 12, respectively. In the case of the CA-mortar containing 1% CA, ettringite, the Ca(OH)2, and C-A-S-H peaks were more intense, as shown in Figure 11. When 3% CA was mixed, the intensity of the Ca(OH)2 and C-A-S-H peak decreased, while that of the ettringite and C-S-H peaks increased. In the case of the CA-mortar containing 1% CF, ettringite, the Ca(OH)2, and C-A-S-H peaks were more intense, as shown in Figure 11. When 3% CA was mixed, the intensity of the Ca(OH)2 and C-A-S-H peak decreased, while that of the ettringite peaks increased as shown in Figure 12.Figure 11
Specimen incorporating calcium acetate (3 days).Figure 12
Specimen incorporating calcium formate (3 days).When Al ion content is the same, Ca(OH)2 and C-A-S-H increase according to the increase of Ca ion [39]. Thus, when CA and CF contents are 1%, Ca(OH)2 and C-A-S-H increased. On the other hand, according to the increase of CA and CF contents, Ca(OH)2 and C-A-S-H peaks decreased. While the pH of CF is 7.0 and its solubility is 166 g/L, the pH of CA is about 5.9 and its density is 247 g/L. High solubility of CA affected both ettringite generation and decrease of Ca(OH)2 and C-A-S-H peaks [40].


## 4. Conclusions

CA was manufactured using acetic acid and LSS obtained from industrial by-products, and its characteristics were examined. The performances of the cementitious composites mixed with this manufactured CA were evaluated. On the basis of the results obtained, the following conclusions were made:(1)
The pH of the CA manufactured via the reaction of CaCO3 and LSS was found to be the same as that of the CA manufactured using CaCO3 (5.9). The microelemental analysis showed that the heavy metal content in the manufactured CA was lower than the detection limits.(2)
The compressive strength of the CA-mortars was maximum when 1% CA was mixed. This value of compressive strength was more than that obtained when no admixture was added even when the specimens were cured for 28 days. In particular, on the 28th day, the CA-mortar showed a higher compressive strength than that of the CF-mortar.(3)
For the cement pastes mixed with CF, the pH remained constant at all the mixing ratios. However, when the CF content exceeded 1%, CA, which is more acidic, had a greater influence on the mixture, leading to a reduction in the pH and strength of the cement, for the hydrates of the hardened cement pastes mixed with the CA and CF, which is advantageous for the enhancement of the C-S-H and ettringite.(4)
Finally, we can conclude that the CA is manufactured using the recycled industrial by-products functions as an effective HESA for cement composites.



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*Source: 2920370-2016-06-07.xml*