# The Influence of Calcium Chloride Salt Solution on the Transport Properties of Cementitious Materials

Authors: Yaghoob Farnam; Taylor Washington; Jason Weiss
Journal: Advances in Civil Engineering
 (2015)

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## Abstract

The chemical interaction between calcium chloride (CaCl2) and cementitious binder may alter the transport properties of concrete which are important in predicting the service life of infrastructure elements. This paper presents a series of fluid and gas transport measurements made on cementitious mortars before and after exposure to various solutions with concentrations ranging from 0% to 29.8% CaCl2 by mass. Fluid absorption, oxygen diffusivity, and oxygen permeability were measured on mortar samples prepared using Type I and Type V cements. Three primary factors influence the transport properties of mortar exposed to CaCl2: (1) changes in the degree of saturation, (2) calcium hydroxide leaching, and (3) formation of chemical reaction products (i.e., Friedel’s salt, Kuzel’s salt, and calcium oxychloride). It is shown that an increase in the degree of saturation decreases oxygen permeability. At lower concentrations (<~12% CaCl2 at room temperature), the addition of CaCl2 can increase calcium hydroxide leaching, thereby increasing mortar porosity (this is offset by the formation of Friedel’s salt and Kuzel’s salt that can block the pores). At higher concentrations (>~12%), the formation of chemical reaction products (mainly calcium oxychloride) is a dominant factor decreasing the fluid and gas transport in concrete.


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## Body

## 1. Introduction

The transport properties of cementitious materials are increasingly being used to predict the service life of infrastructure element [1, 2]. The importance of transport properties has been discussed for over six decades with pioneering work by Powers et al. [3]. Since that time, researchers have attempted to describe concrete durability [4, 5], concrete deterioration [5, 6], initiation of steel corrosion in reinforced concrete elements [1, 2], and concrete freeze-thaw resistance [7–12] using a variety of transport measurements.While we frequently assume that the fluid in the concrete pores is water, this may not always be true. Salts can alter the transport properties of cementitious materials in several different ways. First, salt can change the properties of a solution including the viscosity, surface tension, and density [13–15]. These variations in viscosity, density, and surface tension can alter the rate of solution ingress into concrete [16–18]. Second, exposure to salt can increase the saturation state of concrete pores due to increasing the equilibrium relative humidity of the solution (i.e., the relative humidity of the surrounding atmosphere when a solution neither gains nor losses moisture which is related to equilibrium water activity) [13, 19]. Third, salt can precipitate and crystallize inside concrete pores, thereby filling/blocking the pores [20, 21]. Finally, salt can react with the hydrated cementitious binder forming new chemical products which can reduce the porosity and further block the concrete pores [22–25].Different chloride based salts can influence the transport properties of cementitious materials in different ways as the copresent cations (e.g., Na+, Ca++, and Mg++) may play an important role in the rate of chloride ingress. Furthermore, chemical reactions can occur between salt and the hydrated cementitious binder. While NaCl appears to cause a relatively small change in transport properties, CaCl2 and MgCl2 can exhibit more dramatic change in comparison to NaCl [24, 26, 27]. Solution containing CaCl2 and MgCl2 may result in the formation of chemical phases (e.g., Friedel’s salt, Kuzel’s salt, calcium oxychloride, magnesium oxychloride, brucite, or magnesium silicate hydrate) [22, 23, 25].The formation of calcium oxychloride in addition to Friedel’s salt and Kuzel’s salt can block concrete pores and decrease fluid ingress into concrete samples [22, 27]. Figure 1 shows a phase diagram for a system containing calcium chloride, calcium hydroxide (CH), and water for two molar ratios, Rm (i.e., Rm<3 and Rm>3) [22]. This phase diagram can be used to interpret the formation of calcium oxychloride in a cementitious material when it is exposed to CaCl2 solution. Calcium oxychloride forms at room temperature (i.e., 23°C) for CaCl2 salt concentrations at or above ~12% by mass in the solution. For concentrations greater than ~12%, calcium oxychloride is stable (depending on the relative humidity and the temperature of the surrounding environment) [22, 26, 28] and the amount of calcium oxychloride increases as the salt concentration increases (in the presence of sufficient solution) [29]. These expansive products can fill in a large volume of pores and reduce solution transport in concrete.Figure 1
CaCl2-Ca(OH)2-H2O phase diagram for different Ca(OH)2/CaCl2 molar ratios (Rm) developed from [22].
(a)
(b)In previous studies [22, 26–28], it has been shown that CaCl2 solution ingress into mortar can substantially decrease when mortar samples are exposed to solutions with high concentrations of CaCl2 salt (greater than about 12% by mass). X-ray fluorescence examinations of mortar samples that were vacuum-saturated with solutions of varying CaCl2 concentrations greater than about 12% showed relatively no chloride ion ingress into the core of the samples presumably due to the blocking caused by calcium oxychloride formation [22].This paper uses different transport tests (fluid absorption, oxygen diffusivity, and oxygen permeability) to provide an improved understanding of how CaCl2 may change the transport properties of cementitious materials. Transport properties of cementitious materials are examined on mortar samples with varying cement compositions (Type I and Type V cements) while altering the CaCl2 salt concentrations in the solution and varying the degree of saturation.The main objective of this study is to determine whether the formation of reaction products (i.e., Friedel’s salt, Kuzel’s salt, and/or calcium oxychloride) is a significant factor contributing to the alteration of transport properties of cementitious materials. It is hypothesized that calcium oxychloride will not form in mortar samples exposed to CaCl2 solution with concentrations less than ~12% by mass at 23°C. It is expected that mortar samples prepared using Type V cement (with no tricalcium aluminate, i.e., C3A) will most likely produce no Friedel’s salt and/or Kuzel’s salt in the presence of CaCl2.


## 2. Experimental Program

Two series of experiments were performed in this study as shown in Table1. In the first series, mortar samples were prepared and exposed to solution with varying concentrations of CaCl2 before transport testing. In the second series, mortar samples were prepared of varying levels of saturation before transport testing. This section describes the material and mixture proportioning to prepare mortar sample, conditioning of the sample, and transport testing procedure.Table 1
Experimental program.
Experiment
Sample Type
Transport Testing
Conditioning
Series I: varying CaCl2 concentration
Mortar prepared using Type I and Type V cements
CaCl2 fluid absorption
(1) Being dried at 60°C for one week.(2) Performing test by exposing sample to CaCl2 solution with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% concentration by mass for two weeks.
Oxygen diffusivity
(1) Being dried at 60°C for one week.(2) Two-week exposure to CaCl2 solution with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% concentration by mass.(3) Being conditioned to reach 50% degree of saturation.
Oxygen permeability
(1) Being dried at 60°C for one week.(2) Two-week immersion in CaCl2 solution with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% concentration by mass.(3) Being conditioned at 50% ± 1% RH and 23°C ± 0.5°C for at least three months.
Series II:varying degree of saturation
Mortar prepared using Type I and Type V cements
Oxygen permeability
(1) Being dried at 60°C for one week.(2) Being conditioned with DI water to reach degrees of saturation between 0% and 100%.


### 2.1. Materials and Mixture Proportioning

Two types of ordinary Portland cement (OPC) were used: Type I and Type V with Blaine fineness of 375 m2/kg and 316 m2/kg, respectively. The chemical composition of the cements, as reported by the manufactures, is indicated in Table 2. Aggregates used to prepare mortar specimens consisted of a natural sand with a maximum size of 4.75 mm, specific gravity of 2.61, fineness modulus of 2.89, and an absorption value of 2.2% by mass. Mortar mixtures were prepared with a sand volume fraction of 55% and a water-to-cement ratio (w/c) of 0.42 by mass. Mortar was prepared in a standard mortar mixer in accordance with ASTM C305-12 [30]. The mortar was then cast in cylindrical molds (101 mm in diameter and 203 mm in height) and large beam molds (152 mm × 152 mm × 584 mm). Samples were demolded after 24 h and were double-sealed in plastic bags and then cured for 42 d at 23°C ± 0.5°C in these sealed conditions. Samples prepared using Type V cement were cured for an additional time (at 23°C ± 0.5°C in the sealed condition) until the porosity reached 19.6% (i.e., the porosity of samples prepared using Type I cement after 42 days). After reaching an equal total porosity, the curing was stopped for samples prepared using Type V cement. The porosity of samples was measured according to ASTM C642-13 [31] by measuring the oven-dried (at a temperature of 110 ± 5°C for two days) mass in air, the saturated surface-dry mass in air after vacuum saturation, and the apparent mass in water after vacuum saturation.Table 2
Properties of ordinary Portland cements (OPC).
Item
Percent by mass (%)
Type I
Type V
Silicon dioxide (SiO2)
19.43
21.3
Aluminum oxide (Al2O3)
5.39
2.6
Ferric oxide (Fe2O3)
3.18
4.2
Calcium oxide (CaO)
63.45
63.2
Magnesium oxide (MgO)
2.97
4.5
Sulfur trioxide (SO3)
3.38
2.8
Loss on ignition
0.88
1.20
Sodium oxide
0.35
NA∗
Potassium oxide
0.77
NA
Free lime
NA
0.38
Insoluble residue
0.25
0.18
Total equivalent alkali as Na2O
0.86
0.21
Tricalcium silicate (C3S)
60
64
Dicalcium silicate (C2S)
10
13
Tricalcium aluminate (C3A)
9
0
Tetracalcium aluminoferrite (C4AF)
10
13
∗Not available.


### 2.2. Transport Testing

Three transport tests were used in this study:(1) fluid absorption, (2) oxygen diffusivity, and (3) oxygen permeability as indicated in Figure 2. The following sections describe the sample preparation, sample conditioning, and testing procedure for each test.Figure 2
Experimental procedure: (a) fluid absorption test, (b) oxygen diffusivity test, and (c) oxygen permeability test.
(a)
(b)
(c)


#### 2.2.1. Fluid Absorption

After curing, cylindrical mortar samples (101 mm in diameter and 203 mm in height) were cut into smaller cylindrical samples using a wet saw (101 mm in diameter and 50 mm in height) for the fluid absorption test. Two smaller cylindrical samples were obtained from the center of each cylindrical mortar that was cast. Then, the outer circumference of the specimen was sealed with two layers of epoxy resin as shown in Figure2(a). Once the epoxy had hardened, the samples were then placed in an oven at 60°C ± 0.5°C for one week to remove the moisture and bring the samples to mass equilibrium.Fluid absorption testing was performed using procedure similar to ASTM C1585-11 [32], as shown in Figure 2(a). One circular face of a sample was exposed to a solution while the opposite face was covered by a loose plastic (Figure 2(a)). The mass change due to fluid absorption was then monitored over time. Solutions with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% CaCl2 salt concentration by mass were used. Three samples were exposed to each solution for 2 weeks. All fluid absorption tests were performed at room temperature (23°C ± 1°C).


#### 2.2.2. Oxygen Diffusivity

After completion of the fluid absorption experiment, samples were removed from the solutions and stored at a temperature and humidity controlled chamber at 50% ± 1% RH and at 23°C ± 0.5°C until mass equilibrium was reached (Δm<0.05%). After mass equilibrium was reached, the degree of saturation of samples was calculated using the average porosity of the mortar sample (19.6%) and the mass change from dry state. The degree of saturation for oxygen diffusivity samples was brought to 50% ± 1% by either drying or wetting the surface of the sample that had not been exposed to CaCl2 solution. All samples were then sealed in plastic bags for a minimum of one week to allow moisture to redistribute before oxygen diffusivity testing.The oxygen diffusivity was measured using an instrument that was modeled after that developed by Lawrence [33] as shown in Figure 2(b). The samples used for oxygen diffusivity testing were fitted in a rubber ring that is compressed to provide a condition that insures unidirectional flow. The test was performed by exposing the surface of the sample that had been exposed to CaCl2 solution to pure oxygen and the opposite face to pure nitrogen at the same pressure. The oxygen and nitrogen gasses counter diffused through the sample and the oxygen concentration in the outlet cell was measured at 0 and 60 minutes after starting the test. The oxygen diffusivity experiment is described in detail in [34].


#### 2.2.3. Oxygen Permeability

After curing and before exposure to salt, cylinders were cored from large cast beams (152 mm × 152 mm × 584 mm) using a 68 mm ± 2 mm diameter bit. These samples were then cut using a wet saw resulting in samples with a height of 25 mm ± 2 mm for oxygen permeability measurements. The outer circumference of the specimen was sealed with two layers of epoxy resin. After the epoxy hardened, the prepared samples were then placed in an oven at 60°C ± 0.5°C for a week to remove moisture and allow them to reach mass equilibrium.As shown in Table1, the oxygen permeability tests were performed on (a) samples exposed to solutions with varying CaCl2 concentration and (b) samples with varying degree of saturation. For samples exposed to solutions with varying CaCl2 concentration, the samples were completely submerged in CaCl2 solution with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% salt concentration by mass after having been dried for one week. The samples were then removed from the solutions and conditioned in a temperature and humidity controlled chamber at 50% ± 1% RH and at 23°C ± 0.5°C for at least three months until reaching mass equilibrium (Δm<0.05%). Oxygen permeability tests were then performed with these samples. The degree of saturation of each sample was detected before and after oxygen permeability test for samples exposed to solutions with varying CaCl2 concentration.For samples tested to determine the influence of varying degree of saturation, dry samples were vacuum-saturated to a degree of saturation of 100%. The vacuum saturation process was as follows:(1) samples were held under vacuum at a pressure of 10 mm Hg ± 5 mm Hg for 3 h, (2) while still under vacuum, deaerated deionized (DI) water was added to the container until the sample was completely submerged, (3) samples remained submerged in DI water under vacuum for 1 h, and (4) the samples remained submerged in the solution until they were tested, approximately 3 d. The samples intended for testing at lower degrees of saturation were removed from the solution and were allowed to air-dry while the mass was monitored every 15–30 min until the desired mass (i.e., degree of saturation) was obtained (Δm<0.05%). Samples were then double-sealed in bags where they were kept for one week before the oxygen permeability test was performed to encourage uniform distribution of moisture throughout the sample [20, 34]. To reach degrees of saturation below 60%, samples were dried in a vacuum oven at 50°C. To obtain degree of saturation equal to 0%, samples were dried in a normal oven at 105°C for two days.Oxygen permeability was measured using a falling head permeameter [35], whose principles are illustrated in Figure 2(c). A unidirectional flow of oxygen through the specimen was created due to the presence of a pressure gradient between the upper and the lower sides of the sample. The bottom surface of the sample was in contact with the pressurized oxygen (initially set to be 100 kPa as a gauge pressure) while the top surface was at atmospheric pressure (~101.4 kPa). The samples were placed inside a rubber collar which was compressed to insure unidirectional flow. The pressure of the oxygen in the chamber was monitored for a 24 hr period using a data acquisition system and data logger.


## 2.1. Materials and Mixture Proportioning

Two types of ordinary Portland cement (OPC) were used: Type I and Type V with Blaine fineness of 375 m2/kg and 316 m2/kg, respectively. The chemical composition of the cements, as reported by the manufactures, is indicated in Table 2. Aggregates used to prepare mortar specimens consisted of a natural sand with a maximum size of 4.75 mm, specific gravity of 2.61, fineness modulus of 2.89, and an absorption value of 2.2% by mass. Mortar mixtures were prepared with a sand volume fraction of 55% and a water-to-cement ratio (w/c) of 0.42 by mass. Mortar was prepared in a standard mortar mixer in accordance with ASTM C305-12 [30]. The mortar was then cast in cylindrical molds (101 mm in diameter and 203 mm in height) and large beam molds (152 mm × 152 mm × 584 mm). Samples were demolded after 24 h and were double-sealed in plastic bags and then cured for 42 d at 23°C ± 0.5°C in these sealed conditions. Samples prepared using Type V cement were cured for an additional time (at 23°C ± 0.5°C in the sealed condition) until the porosity reached 19.6% (i.e., the porosity of samples prepared using Type I cement after 42 days). After reaching an equal total porosity, the curing was stopped for samples prepared using Type V cement. The porosity of samples was measured according to ASTM C642-13 [31] by measuring the oven-dried (at a temperature of 110 ± 5°C for two days) mass in air, the saturated surface-dry mass in air after vacuum saturation, and the apparent mass in water after vacuum saturation.Table 2
Properties of ordinary Portland cements (OPC).
Item
Percent by mass (%)
Type I
Type V
Silicon dioxide (SiO2)
19.43
21.3
Aluminum oxide (Al2O3)
5.39
2.6
Ferric oxide (Fe2O3)
3.18
4.2
Calcium oxide (CaO)
63.45
63.2
Magnesium oxide (MgO)
2.97
4.5
Sulfur trioxide (SO3)
3.38
2.8
Loss on ignition
0.88
1.20
Sodium oxide
0.35
NA∗
Potassium oxide
0.77
NA
Free lime
NA
0.38
Insoluble residue
0.25
0.18
Total equivalent alkali as Na2O
0.86
0.21
Tricalcium silicate (C3S)
60
64
Dicalcium silicate (C2S)
10
13
Tricalcium aluminate (C3A)
9
0
Tetracalcium aluminoferrite (C4AF)
10
13
∗Not available.


## 2.2. Transport Testing

Three transport tests were used in this study:(1) fluid absorption, (2) oxygen diffusivity, and (3) oxygen permeability as indicated in Figure 2. The following sections describe the sample preparation, sample conditioning, and testing procedure for each test.Figure 2
Experimental procedure: (a) fluid absorption test, (b) oxygen diffusivity test, and (c) oxygen permeability test.
(a)
(b)
(c)


### 2.2.1. Fluid Absorption

After curing, cylindrical mortar samples (101 mm in diameter and 203 mm in height) were cut into smaller cylindrical samples using a wet saw (101 mm in diameter and 50 mm in height) for the fluid absorption test. Two smaller cylindrical samples were obtained from the center of each cylindrical mortar that was cast. Then, the outer circumference of the specimen was sealed with two layers of epoxy resin as shown in Figure2(a). Once the epoxy had hardened, the samples were then placed in an oven at 60°C ± 0.5°C for one week to remove the moisture and bring the samples to mass equilibrium.Fluid absorption testing was performed using procedure similar to ASTM C1585-11 [32], as shown in Figure 2(a). One circular face of a sample was exposed to a solution while the opposite face was covered by a loose plastic (Figure 2(a)). The mass change due to fluid absorption was then monitored over time. Solutions with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% CaCl2 salt concentration by mass were used. Three samples were exposed to each solution for 2 weeks. All fluid absorption tests were performed at room temperature (23°C ± 1°C).


### 2.2.2. Oxygen Diffusivity

After completion of the fluid absorption experiment, samples were removed from the solutions and stored at a temperature and humidity controlled chamber at 50% ± 1% RH and at 23°C ± 0.5°C until mass equilibrium was reached (Δm<0.05%). After mass equilibrium was reached, the degree of saturation of samples was calculated using the average porosity of the mortar sample (19.6%) and the mass change from dry state. The degree of saturation for oxygen diffusivity samples was brought to 50% ± 1% by either drying or wetting the surface of the sample that had not been exposed to CaCl2 solution. All samples were then sealed in plastic bags for a minimum of one week to allow moisture to redistribute before oxygen diffusivity testing.The oxygen diffusivity was measured using an instrument that was modeled after that developed by Lawrence [33] as shown in Figure 2(b). The samples used for oxygen diffusivity testing were fitted in a rubber ring that is compressed to provide a condition that insures unidirectional flow. The test was performed by exposing the surface of the sample that had been exposed to CaCl2 solution to pure oxygen and the opposite face to pure nitrogen at the same pressure. The oxygen and nitrogen gasses counter diffused through the sample and the oxygen concentration in the outlet cell was measured at 0 and 60 minutes after starting the test. The oxygen diffusivity experiment is described in detail in [34].


### 2.2.3. Oxygen Permeability

After curing and before exposure to salt, cylinders were cored from large cast beams (152 mm × 152 mm × 584 mm) using a 68 mm ± 2 mm diameter bit. These samples were then cut using a wet saw resulting in samples with a height of 25 mm ± 2 mm for oxygen permeability measurements. The outer circumference of the specimen was sealed with two layers of epoxy resin. After the epoxy hardened, the prepared samples were then placed in an oven at 60°C ± 0.5°C for a week to remove moisture and allow them to reach mass equilibrium.As shown in Table1, the oxygen permeability tests were performed on (a) samples exposed to solutions with varying CaCl2 concentration and (b) samples with varying degree of saturation. For samples exposed to solutions with varying CaCl2 concentration, the samples were completely submerged in CaCl2 solution with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% salt concentration by mass after having been dried for one week. The samples were then removed from the solutions and conditioned in a temperature and humidity controlled chamber at 50% ± 1% RH and at 23°C ± 0.5°C for at least three months until reaching mass equilibrium (Δm<0.05%). Oxygen permeability tests were then performed with these samples. The degree of saturation of each sample was detected before and after oxygen permeability test for samples exposed to solutions with varying CaCl2 concentration.For samples tested to determine the influence of varying degree of saturation, dry samples were vacuum-saturated to a degree of saturation of 100%. The vacuum saturation process was as follows:(1) samples were held under vacuum at a pressure of 10 mm Hg ± 5 mm Hg for 3 h, (2) while still under vacuum, deaerated deionized (DI) water was added to the container until the sample was completely submerged, (3) samples remained submerged in DI water under vacuum for 1 h, and (4) the samples remained submerged in the solution until they were tested, approximately 3 d. The samples intended for testing at lower degrees of saturation were removed from the solution and were allowed to air-dry while the mass was monitored every 15–30 min until the desired mass (i.e., degree of saturation) was obtained (Δm<0.05%). Samples were then double-sealed in bags where they were kept for one week before the oxygen permeability test was performed to encourage uniform distribution of moisture throughout the sample [20, 34]. To reach degrees of saturation below 60%, samples were dried in a vacuum oven at 50°C. To obtain degree of saturation equal to 0%, samples were dried in a normal oven at 105°C for two days.Oxygen permeability was measured using a falling head permeameter [35], whose principles are illustrated in Figure 2(c). A unidirectional flow of oxygen through the specimen was created due to the presence of a pressure gradient between the upper and the lower sides of the sample. The bottom surface of the sample was in contact with the pressurized oxygen (initially set to be 100 kPa as a gauge pressure) while the top surface was at atmospheric pressure (~101.4 kPa). The samples were placed inside a rubber collar which was compressed to insure unidirectional flow. The pressure of the oxygen in the chamber was monitored for a 24 hr period using a data acquisition system and data logger.


## 2.2.1. Fluid Absorption

After curing, cylindrical mortar samples (101 mm in diameter and 203 mm in height) were cut into smaller cylindrical samples using a wet saw (101 mm in diameter and 50 mm in height) for the fluid absorption test. Two smaller cylindrical samples were obtained from the center of each cylindrical mortar that was cast. Then, the outer circumference of the specimen was sealed with two layers of epoxy resin as shown in Figure2(a). Once the epoxy had hardened, the samples were then placed in an oven at 60°C ± 0.5°C for one week to remove the moisture and bring the samples to mass equilibrium.Fluid absorption testing was performed using procedure similar to ASTM C1585-11 [32], as shown in Figure 2(a). One circular face of a sample was exposed to a solution while the opposite face was covered by a loose plastic (Figure 2(a)). The mass change due to fluid absorption was then monitored over time. Solutions with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% CaCl2 salt concentration by mass were used. Three samples were exposed to each solution for 2 weeks. All fluid absorption tests were performed at room temperature (23°C ± 1°C).


## 2.2.2. Oxygen Diffusivity

After completion of the fluid absorption experiment, samples were removed from the solutions and stored at a temperature and humidity controlled chamber at 50% ± 1% RH and at 23°C ± 0.5°C until mass equilibrium was reached (Δm<0.05%). After mass equilibrium was reached, the degree of saturation of samples was calculated using the average porosity of the mortar sample (19.6%) and the mass change from dry state. The degree of saturation for oxygen diffusivity samples was brought to 50% ± 1% by either drying or wetting the surface of the sample that had not been exposed to CaCl2 solution. All samples were then sealed in plastic bags for a minimum of one week to allow moisture to redistribute before oxygen diffusivity testing.The oxygen diffusivity was measured using an instrument that was modeled after that developed by Lawrence [33] as shown in Figure 2(b). The samples used for oxygen diffusivity testing were fitted in a rubber ring that is compressed to provide a condition that insures unidirectional flow. The test was performed by exposing the surface of the sample that had been exposed to CaCl2 solution to pure oxygen and the opposite face to pure nitrogen at the same pressure. The oxygen and nitrogen gasses counter diffused through the sample and the oxygen concentration in the outlet cell was measured at 0 and 60 minutes after starting the test. The oxygen diffusivity experiment is described in detail in [34].


## 2.2.3. Oxygen Permeability

After curing and before exposure to salt, cylinders were cored from large cast beams (152 mm × 152 mm × 584 mm) using a 68 mm ± 2 mm diameter bit. These samples were then cut using a wet saw resulting in samples with a height of 25 mm ± 2 mm for oxygen permeability measurements. The outer circumference of the specimen was sealed with two layers of epoxy resin. After the epoxy hardened, the prepared samples were then placed in an oven at 60°C ± 0.5°C for a week to remove moisture and allow them to reach mass equilibrium.As shown in Table1, the oxygen permeability tests were performed on (a) samples exposed to solutions with varying CaCl2 concentration and (b) samples with varying degree of saturation. For samples exposed to solutions with varying CaCl2 concentration, the samples were completely submerged in CaCl2 solution with 0%, 5%, 10%, 15%, 20%, 25%, and 29.8% salt concentration by mass after having been dried for one week. The samples were then removed from the solutions and conditioned in a temperature and humidity controlled chamber at 50% ± 1% RH and at 23°C ± 0.5°C for at least three months until reaching mass equilibrium (Δm<0.05%). Oxygen permeability tests were then performed with these samples. The degree of saturation of each sample was detected before and after oxygen permeability test for samples exposed to solutions with varying CaCl2 concentration.For samples tested to determine the influence of varying degree of saturation, dry samples were vacuum-saturated to a degree of saturation of 100%. The vacuum saturation process was as follows:(1) samples were held under vacuum at a pressure of 10 mm Hg ± 5 mm Hg for 3 h, (2) while still under vacuum, deaerated deionized (DI) water was added to the container until the sample was completely submerged, (3) samples remained submerged in DI water under vacuum for 1 h, and (4) the samples remained submerged in the solution until they were tested, approximately 3 d. The samples intended for testing at lower degrees of saturation were removed from the solution and were allowed to air-dry while the mass was monitored every 15–30 min until the desired mass (i.e., degree of saturation) was obtained (Δm<0.05%). Samples were then double-sealed in bags where they were kept for one week before the oxygen permeability test was performed to encourage uniform distribution of moisture throughout the sample [20, 34]. To reach degrees of saturation below 60%, samples were dried in a vacuum oven at 50°C. To obtain degree of saturation equal to 0%, samples were dried in a normal oven at 105°C for two days.Oxygen permeability was measured using a falling head permeameter [35], whose principles are illustrated in Figure 2(c). A unidirectional flow of oxygen through the specimen was created due to the presence of a pressure gradient between the upper and the lower sides of the sample. The bottom surface of the sample was in contact with the pressurized oxygen (initially set to be 100 kPa as a gauge pressure) while the top surface was at atmospheric pressure (~101.4 kPa). The samples were placed inside a rubber collar which was compressed to insure unidirectional flow. The pressure of the oxygen in the chamber was monitored for a 24 hr period using a data acquisition system and data logger.


## 3. Results and Discussion

### 3.1. Intrinsic Fluid Absorption

ASTM C1585-11 [32] suggests the use of (1) to find the absorption for samples exposed to water: (1)absorptionmm3mm2=mt-moA·ρw,where mt is the mass of sample in grams at the time t after exposure to water, mo is the initial mass of sample before exposure, A is the exposed area of the specimen in mm2, and ρw is the density of water in g/mm3.One drawback of this method is that the absorption obtained by ASTM C1585-11 [32] is frequently interpreted as the depth of water penetration in the sample. This however is not correct as it does not account for the sample porosity. In addition, water is used as the fluid that is being absorbed and the equation from ASTM C1585-11 is not directly applicable to other fluids (e.g., salt solution). Increasing the salt concentration in a salt solution can increase viscosity, density, and surface tension in the solution [13–15].It has been suggested that the absorption and sorptivity are proportional to the square root of the ratio of surface tension and viscosity of the fluid in porous materials [13, 16–18]. An increase in viscosity/density or a decrease in surface tension can decrease solution ingress into a porous material [13, 16–18]. Equation (2) was developed to obtain an intrinsic absorption (i.e., depth of fluid penetration into the sample) of mortar sample exposed to CaCl2 solutions. The intrinsic absorption is independent of the properties of the solution (i.e., surface tension, viscosity, and density) and it represents the depth of fluid penetration into the sample:(2)intrinsic  absorption  (mm)=mt-moA·Φ·ρs1-Do∗γw·ηsγs·ηw,where γw and γs are the surface tensions for water and solution in N/mm, respectively; ηw and ηs are the viscosities for water and solution in Pa·s, respectively; Φ is the porosity of the sample in volume fraction; Do is the initial degree of saturation for sample in volume fraction; and ρs is the density of solution in g/mm3.Fluid absorption into a cementitious composite can be idealized as being divided into two regions (assuming no chemical reaction is occurring):(1) initial absorption (time between 0 and t1 in Figure 3) and (2) secondary absorption (time after t1 in Figure 3) [16, 18, 32, 36, 37]. The initial absorption is mainly related to the penetration of fluid into small pores (i.e., gel and capillary pores) [16, 18, 36–41]. Small pores generate a considerable amount of capillary suction which can help fluid to saturate small pores within a very short time. Once the small pores are saturated throughout the whole height of sample (time t1 in Figure 3), the large pores (i.e., entrapped or entrained pores) in the sample begin to be gradually saturated [16, 18, 36–41]. The portion of absorption which is related to saturating the large pores (after time t1 in Figure 3) is slow and is called secondary absorption.Figure 3
Schematic of intrinsic fluid absorption in a cementitious material with and without chemical reaction.Any reaction between a fluid and a hydrated cementitious composite can alter the intrinsic absorption which will be discussed in Section3.2.


### 3.2. The Effect of CaCl2 on Intrinsic Fluid Absorption

It has been reported that CaCl2 solution can react with hydrated cementitious binder and produce calcium chloroaluminate phases (such as Friedel’s salt and Kuzel’s salt) and calcium oxychloride phase [22, 24, 26–29, 42–45]. The calcium aluminate phases (e.g., C3A, monosulfate, and ettringite) from the hydrated cementitious binder gradually react with CaCl2 resulting in the production of Friedel’s salt and Kuzel’s salt. The amount of Friedel’s salt and Kuzel’s salt increases with exposure time, and an increase in salt concentration accelerates the formation of Friedel’s salt and Kuzel’s salt [24, 27, 42–45]. Calcium oxychloride is produced by the reaction between calcium hydroxide (CH) from the hydrated cementitious binder and CaCl2 solution [22, 26, 28, 29, 45]. Calcium oxychloride does not form at room temperature (i.e., ~23°C) until CaCl2 salt concentration reaches approximately 12% by mass in the solution (Figure 1). Beyond this concentration (concentrations greater than ~12%), the formation of calcium oxychloride is relatively rapid and its quantity increases as the salt concentration increases [22, 26, 28, 29, 45]. For samples prepared using Type V cement, no Friedel’s salt or Kuzel’s salt formation is expected (since Type V cement has relatively no C3A, see Table 2), while calcium oxychloride forms for samples prepared using both Type I and Type V cements as long as CaCl2 concentration is greater than ~12% by mass in the solution.The intrinsic absorption obtained for samples as a function of the square root of time is shown in Figure4. The addition of chemical reaction to the absorption appears to alter the shape of intrinsic absorption curve which is schematically illustrated in Figure 3. First, solution is absorbed into the small pores due to capillary suction during a very short time (time between 0 and t1′ in Figure 3). Beyond time t1′ in Figure 3, reaction begins and as a result chemical products precipitate in the pores blocking/filling the pore structure. Blocking/filling the pores continues over time and it gradually decreases the rate of intrinsic absorption (between t1′ and t2′ in Figure 3). At time t2′ in Figure 3, all the small pores are filled by either solution or chemical products and, after this time, big pores begin to be occupied. It is expected to have more reduction in fluid absorption as the amount of chemical products (Friedel’s salt, Kuzel’s salt, and calcium oxychloride) in the pores increases.Figure 4
The effect of CaCl2 concentration (% by mass) on intrinsic absorption for mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement.
(a)
(b)Figure4(a) illustrates the measured intrinsic absorption as a function of square root of time for samples prepared using Type I cement (with C3A). An increase in CaCl2 concentration results in a decrease in the intrinsic absorption for all of the samples prepared using Type I cement. As the salt concentration increases, the intrinsic absorption reduces primarily due to the fact that an increase in salt concentration increases the formation rate of Friedel’s salt and Kuzel’s salt [24, 27, 42–45]. A more significant reduction in intrinsic absorption can be seen at the salt concentration of ~12% or greater. At these concentrations, calcium oxychloride forms (in addition to Friedel’s salt and Kuzel’s salt) and further blocks/fills the pores.Figure4(b) illustrates the intrinsic absorption as a function of square root of time for samples prepared using Type V cement (with relatively no C3A). Samples exposed to CaCl2 concentrations less than or equal to ~12% by mass show a similar trend for intrinsic absorption since no reaction (Friedel’s salt and Kuzel’s salt formation) is expected to occur for these concentrations. For CaCl2 concentration beyond ~12%, a reduction in intrinsic absorption can be observed as the salt concentration increases, which is mainly due to calcium oxychloride formation in the pores.


### 3.3. The Effect of CaCl2 on Intrinsic Sorptivity

Intrinsic sorptivity is defined as the slope of the intrinsic absorption versus the square root of time curve. The derivative of intrinsic absorption (or intrinsic sorptivity) versus square root of time curve was obtained and is shown in Figure5 for the first 6 h. A linear trend line was also fitted for the intrinsic absorption versus square root of time curve during first 6 h and the slope of the linear trend line is reported in Figure 6 as an initial intrinsic sorptivity. For samples exposed to solutions with high concentrations (>15%), the obtained initial intrinsic sorptivity is not a proper indication of initial sorptivity since a nonliner trend can be seen in Figures 4 and 5 due to the presence of chemical reactions between cementitious matrix and CaCl2 solution.Figure 5
The effect of solution concentration on initial sorptivity of mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement.
(a)
(b)Figure 6
The initial intrinsic sorptivity as a function of CaCl2 concentrations for mortar samples prepared using (a) Type I cement containing C3A and (b) Type V cement containing approximately no C3A.
(a)
(b)As indicated in Figure5, the intrinsic sorptivity has a relatively similar value at the beginning of absorption test (0 to 1 min) for mortar samples saturated with different CaCl2 concentrations, which shows the rate of fluid ingress due to capillary suction. As the CaCl2 concentration increases, a reduction in intrinsic sorptivity over time can be observed in Figure 5. The reduction appears to be primary due to the formation of reaction products (Friedel’s/Kuzel’s salts and/or calcium oxychloride) in pores which can fill/block the pores (illustrated in Figure 3). The volume of the reaction products would be expected to increase as the exposure time increases. This can further fill/block the pores over time and cause continued reduction in the fluid absorption of the samples.The initial intrinsic sorptivity as a function of salt concentration is shown in Figure6. A reduction in initial intrinsic sorptivity can be seen as the CaCl2 concentration increases which may be again due to the chemical reaction products (Friedel’s/Kuzel’s salts and/or calcium oxychloride). The reduction in initial intrinsic sorptivity is relatively small for salt concentrations less than ~12%. A considerable reduction in initial intrinsic sorptivity can be observed in Figure 6 as the salt concentration becomes greater than ~12%. In general, samples prepared with Type I cement showed a greater reduction in initial intrinsic sorptivity in comparison to samples prepared with Type V cement. The difference in absorption behavior of samples prepared using different cements (i.e., Type I and Type V) may be twofold: (1) for lower CaCl2 concentrations (~<12% CaCl2), Friedel’s salts and Kuzel’s salts are the only chemical products for samples prepared using Type I cement while no reaction is expected for samples prepared using Type V cement; (2) for higher CaCl2 concentrations (~>12% CaCl2), both Friedel’s/Kuzel’s salts and calcium oxychloride are produced in the case of using Type I cement.


### 3.4. The Effect of CaCl2 on Oxygen Diffusivity

Oxygen diffusivity tests were performed on samples after being exposed to the solutions with different CaCl2 concentrations. Since the degree of saturation in mortar sample may have a substantial influence on oxygen diffusivity results, the degree of saturation was kept at 50% for all samples (described in Section 2.2.2) prior to performing the oxygen diffusivity experiments. The oxygen diffusivity results for mortar samples as a function of CaCl2 concentration in the exposed solution is shown in Figure 7. In general, the gas diffusivity for mortar samples prepared using Type V cement is higher than the one for mortar sample prepared using Type I cement; this may be due to the fact that different cements may create different pore structure that can influence the gas diffusivity result. As expected, for samples (prepared using either Type I or Type V cement) exposed to higher concentrations of CaCl2 solution (more than ~12%), a reduction in oxygen diffusivity can be seen due to the formation of calcium oxychloride which blocks the pores making the oxygen diffusion more difficult.Figure 7
The effect of salt concentration on oxygen diffusivity (degree of saturation = 50%) for mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement.
(a)
(b)An interesting observation is that, for lower concentrations (less than ~12%), the oxygen diffusivity increases as the salt concentration increases. This observation appears to be opposite to what one may expect as Friedel’s salt and Kuzel’s salt can fill/block the pores and reduce the oxygen diffusivity. This may be explained by competing mechanism of calcium hydroxide (CH) dissolution and leaching. Figure8 shows the solubility of lime (CaO) in CaCl2 solution as the CaCl2 concentration increases [46]. The solubility of lime increases as CaCl2 concentration increases until calcium oxychloride forms and precipitates in the solution. Therefore, mortar samples exposed to CaCl2 solution are susceptible to calcium hydroxide (so-called Portlandite in cement chemistry or CH) leaching from cementitious binder. An increase in CaCl2 concentration can result in an increase in leaching until the CaCl2 concentration reaches the point when calcium oxychloride forms. Calcium hydroxide leaching at lower CaCl2 concentration (less than ~12%) can increase the porosity in mortar sample and increase the oxygen diffusivity. This was not seen in the fluid absorption experiment (Section 3.1) where a decrease in fluid ingress was generally observed as the salt concentration increased. In fact, calcium hydroxide leaching outward of the sample may further reduce fluid ingress toward the sample for samples exposed to a lower concentration of CaCl2 (less than ~12%) since calcium hydroxide leaching occurs in the opposite direction of fluid ingress. As a result, calcium hydroxide leaching may be another factor in reducing fluid ingress into samples in addition to the formation of Friedel’s/Kuzel’s salts for samples exposed to lower concentration of CaCl2 (less than ~12%).Figure 8
Solubility of lime (CaO) in CaCl2 solution at different temperatures (for samples tested at 20°C and 40°C, precipitation of calcium oxychloride were reported for concentrations more than 15% and 20%, resp.) [46].


### 3.5. The Effect of Degree of Saturation on Oxygen Permeability

The oxygen permeability of mortar samples with different degrees of saturation was also tested. These tests were performed to determine the effect of the degree of saturation on the oxygen permeability. Figure9 shows the oxygen permeability results as a function of degree of saturation for all mortar samples. A change in the degree of saturation has a substantial influence on oxygen permeability in the degrees of saturation less than ~70%. The degree of saturation less than 70% approximately corresponds to removing water from small pores (i.e., gel pores with pore diameter less than 5 nm) [38–41]. At degrees of saturation that were greater than 70%, approximately all the small pores become saturated causing disconnection of open/empty pores [38–41]. As a result, oxygen can barely penetrate through the sample at degrees of saturation more than 70%.Figure 9
The effect of degree of saturation on oxygen permeability for mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement (notice that modified Gaussian function is only fitted for DI water points and the scale fory-axis is not identical).
(a)
(b)A Modified Gaussian Function, as shown in (3), is fitted empirically for the data points (oxygen permeability versus degree of saturation) obtained for samples saturated with DI water: (3)KP=a+b·exp⁡-0.5·Ds-cde,where KP is the oxygen permeability in m/s and Ds is the degree of saturation. a, b, c, d, and e are coefficients for Modified Gaussian Function. a, b, c, d, and e are obtained to be 1 × 10−15, 4.55 × 10−14, 0, 23, and 2.2, respectively, for mortar samples prepared using Type I cement and 5 × 10−15, 2.40 × 10−13, 0, 10, and 1.0, respectively, for mortar samples prepared using Type V cement.


### 3.6. The Effect of CaCl2 on Oxygen Permeability

Oxygen permeability was performed on samples that were exposed to solutions with varying CaCl2 concentrations. Exposure to the CaCl2 solution can alter the degree of saturation in mortar sample as shown in Figure 9. The disparity in the degree of saturation in each sample can substantially alter the transport response of the mortar sample as discussed in Section 3.5 and it is essential to minimize its effect to understand the effect of CaCl2 on the oxygen permeability result. Therefore, the oxygen permeability of mortar samples exposed to CaCl2 solution was modified for degree of saturation equal to 50% using (3).The modified oxygen permeabilty is calculated for the mortar samples exposed to CaCl2 solution and it is shown in Figure 10 as a function of CaCl2 concentration in the solution. A similar trend as was observed for oxygen diffusivity (Section 3.4) can be observed for oxygen permeability as well: (1) an increase in CaCl2 concentration increases the oxygen permeability until the salt concentration reaches ~12% due to calcium hydroxide leaching increasing the porosity of the mortar sample, and (2) beyond this point, the formation of calcium oxychloride in pores fills the pores, decreasing the oxygen permeability.Figure 10
The effect of salt concentration on modified oxygen permeability for 50% degree of saturation in mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement (notice that the scale fory-axis is not identical).
(a)
(b)


## 3.1. Intrinsic Fluid Absorption

ASTM C1585-11 [32] suggests the use of (1) to find the absorption for samples exposed to water: (1)absorptionmm3mm2=mt-moA·ρw,where mt is the mass of sample in grams at the time t after exposure to water, mo is the initial mass of sample before exposure, A is the exposed area of the specimen in mm2, and ρw is the density of water in g/mm3.One drawback of this method is that the absorption obtained by ASTM C1585-11 [32] is frequently interpreted as the depth of water penetration in the sample. This however is not correct as it does not account for the sample porosity. In addition, water is used as the fluid that is being absorbed and the equation from ASTM C1585-11 is not directly applicable to other fluids (e.g., salt solution). Increasing the salt concentration in a salt solution can increase viscosity, density, and surface tension in the solution [13–15].It has been suggested that the absorption and sorptivity are proportional to the square root of the ratio of surface tension and viscosity of the fluid in porous materials [13, 16–18]. An increase in viscosity/density or a decrease in surface tension can decrease solution ingress into a porous material [13, 16–18]. Equation (2) was developed to obtain an intrinsic absorption (i.e., depth of fluid penetration into the sample) of mortar sample exposed to CaCl2 solutions. The intrinsic absorption is independent of the properties of the solution (i.e., surface tension, viscosity, and density) and it represents the depth of fluid penetration into the sample:(2)intrinsic  absorption  (mm)=mt-moA·Φ·ρs1-Do∗γw·ηsγs·ηw,where γw and γs are the surface tensions for water and solution in N/mm, respectively; ηw and ηs are the viscosities for water and solution in Pa·s, respectively; Φ is the porosity of the sample in volume fraction; Do is the initial degree of saturation for sample in volume fraction; and ρs is the density of solution in g/mm3.Fluid absorption into a cementitious composite can be idealized as being divided into two regions (assuming no chemical reaction is occurring):(1) initial absorption (time between 0 and t1 in Figure 3) and (2) secondary absorption (time after t1 in Figure 3) [16, 18, 32, 36, 37]. The initial absorption is mainly related to the penetration of fluid into small pores (i.e., gel and capillary pores) [16, 18, 36–41]. Small pores generate a considerable amount of capillary suction which can help fluid to saturate small pores within a very short time. Once the small pores are saturated throughout the whole height of sample (time t1 in Figure 3), the large pores (i.e., entrapped or entrained pores) in the sample begin to be gradually saturated [16, 18, 36–41]. The portion of absorption which is related to saturating the large pores (after time t1 in Figure 3) is slow and is called secondary absorption.Figure 3
Schematic of intrinsic fluid absorption in a cementitious material with and without chemical reaction.Any reaction between a fluid and a hydrated cementitious composite can alter the intrinsic absorption which will be discussed in Section3.2.


## 3.2. The Effect of CaCl2 on Intrinsic Fluid Absorption

It has been reported that CaCl2 solution can react with hydrated cementitious binder and produce calcium chloroaluminate phases (such as Friedel’s salt and Kuzel’s salt) and calcium oxychloride phase [22, 24, 26–29, 42–45]. The calcium aluminate phases (e.g., C3A, monosulfate, and ettringite) from the hydrated cementitious binder gradually react with CaCl2 resulting in the production of Friedel’s salt and Kuzel’s salt. The amount of Friedel’s salt and Kuzel’s salt increases with exposure time, and an increase in salt concentration accelerates the formation of Friedel’s salt and Kuzel’s salt [24, 27, 42–45]. Calcium oxychloride is produced by the reaction between calcium hydroxide (CH) from the hydrated cementitious binder and CaCl2 solution [22, 26, 28, 29, 45]. Calcium oxychloride does not form at room temperature (i.e., ~23°C) until CaCl2 salt concentration reaches approximately 12% by mass in the solution (Figure 1). Beyond this concentration (concentrations greater than ~12%), the formation of calcium oxychloride is relatively rapid and its quantity increases as the salt concentration increases [22, 26, 28, 29, 45]. For samples prepared using Type V cement, no Friedel’s salt or Kuzel’s salt formation is expected (since Type V cement has relatively no C3A, see Table 2), while calcium oxychloride forms for samples prepared using both Type I and Type V cements as long as CaCl2 concentration is greater than ~12% by mass in the solution.The intrinsic absorption obtained for samples as a function of the square root of time is shown in Figure4. The addition of chemical reaction to the absorption appears to alter the shape of intrinsic absorption curve which is schematically illustrated in Figure 3. First, solution is absorbed into the small pores due to capillary suction during a very short time (time between 0 and t1′ in Figure 3). Beyond time t1′ in Figure 3, reaction begins and as a result chemical products precipitate in the pores blocking/filling the pore structure. Blocking/filling the pores continues over time and it gradually decreases the rate of intrinsic absorption (between t1′ and t2′ in Figure 3). At time t2′ in Figure 3, all the small pores are filled by either solution or chemical products and, after this time, big pores begin to be occupied. It is expected to have more reduction in fluid absorption as the amount of chemical products (Friedel’s salt, Kuzel’s salt, and calcium oxychloride) in the pores increases.Figure 4
The effect of CaCl2 concentration (% by mass) on intrinsic absorption for mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement.
(a)
(b)Figure4(a) illustrates the measured intrinsic absorption as a function of square root of time for samples prepared using Type I cement (with C3A). An increase in CaCl2 concentration results in a decrease in the intrinsic absorption for all of the samples prepared using Type I cement. As the salt concentration increases, the intrinsic absorption reduces primarily due to the fact that an increase in salt concentration increases the formation rate of Friedel’s salt and Kuzel’s salt [24, 27, 42–45]. A more significant reduction in intrinsic absorption can be seen at the salt concentration of ~12% or greater. At these concentrations, calcium oxychloride forms (in addition to Friedel’s salt and Kuzel’s salt) and further blocks/fills the pores.Figure4(b) illustrates the intrinsic absorption as a function of square root of time for samples prepared using Type V cement (with relatively no C3A). Samples exposed to CaCl2 concentrations less than or equal to ~12% by mass show a similar trend for intrinsic absorption since no reaction (Friedel’s salt and Kuzel’s salt formation) is expected to occur for these concentrations. For CaCl2 concentration beyond ~12%, a reduction in intrinsic absorption can be observed as the salt concentration increases, which is mainly due to calcium oxychloride formation in the pores.


## 3.3. The Effect of CaCl2 on Intrinsic Sorptivity

Intrinsic sorptivity is defined as the slope of the intrinsic absorption versus the square root of time curve. The derivative of intrinsic absorption (or intrinsic sorptivity) versus square root of time curve was obtained and is shown in Figure5 for the first 6 h. A linear trend line was also fitted for the intrinsic absorption versus square root of time curve during first 6 h and the slope of the linear trend line is reported in Figure 6 as an initial intrinsic sorptivity. For samples exposed to solutions with high concentrations (>15%), the obtained initial intrinsic sorptivity is not a proper indication of initial sorptivity since a nonliner trend can be seen in Figures 4 and 5 due to the presence of chemical reactions between cementitious matrix and CaCl2 solution.Figure 5
The effect of solution concentration on initial sorptivity of mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement.
(a)
(b)Figure 6
The initial intrinsic sorptivity as a function of CaCl2 concentrations for mortar samples prepared using (a) Type I cement containing C3A and (b) Type V cement containing approximately no C3A.
(a)
(b)As indicated in Figure5, the intrinsic sorptivity has a relatively similar value at the beginning of absorption test (0 to 1 min) for mortar samples saturated with different CaCl2 concentrations, which shows the rate of fluid ingress due to capillary suction. As the CaCl2 concentration increases, a reduction in intrinsic sorptivity over time can be observed in Figure 5. The reduction appears to be primary due to the formation of reaction products (Friedel’s/Kuzel’s salts and/or calcium oxychloride) in pores which can fill/block the pores (illustrated in Figure 3). The volume of the reaction products would be expected to increase as the exposure time increases. This can further fill/block the pores over time and cause continued reduction in the fluid absorption of the samples.The initial intrinsic sorptivity as a function of salt concentration is shown in Figure6. A reduction in initial intrinsic sorptivity can be seen as the CaCl2 concentration increases which may be again due to the chemical reaction products (Friedel’s/Kuzel’s salts and/or calcium oxychloride). The reduction in initial intrinsic sorptivity is relatively small for salt concentrations less than ~12%. A considerable reduction in initial intrinsic sorptivity can be observed in Figure 6 as the salt concentration becomes greater than ~12%. In general, samples prepared with Type I cement showed a greater reduction in initial intrinsic sorptivity in comparison to samples prepared with Type V cement. The difference in absorption behavior of samples prepared using different cements (i.e., Type I and Type V) may be twofold: (1) for lower CaCl2 concentrations (~<12% CaCl2), Friedel’s salts and Kuzel’s salts are the only chemical products for samples prepared using Type I cement while no reaction is expected for samples prepared using Type V cement; (2) for higher CaCl2 concentrations (~>12% CaCl2), both Friedel’s/Kuzel’s salts and calcium oxychloride are produced in the case of using Type I cement.


## 3.4. The Effect of CaCl2 on Oxygen Diffusivity

Oxygen diffusivity tests were performed on samples after being exposed to the solutions with different CaCl2 concentrations. Since the degree of saturation in mortar sample may have a substantial influence on oxygen diffusivity results, the degree of saturation was kept at 50% for all samples (described in Section 2.2.2) prior to performing the oxygen diffusivity experiments. The oxygen diffusivity results for mortar samples as a function of CaCl2 concentration in the exposed solution is shown in Figure 7. In general, the gas diffusivity for mortar samples prepared using Type V cement is higher than the one for mortar sample prepared using Type I cement; this may be due to the fact that different cements may create different pore structure that can influence the gas diffusivity result. As expected, for samples (prepared using either Type I or Type V cement) exposed to higher concentrations of CaCl2 solution (more than ~12%), a reduction in oxygen diffusivity can be seen due to the formation of calcium oxychloride which blocks the pores making the oxygen diffusion more difficult.Figure 7
The effect of salt concentration on oxygen diffusivity (degree of saturation = 50%) for mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement.
(a)
(b)An interesting observation is that, for lower concentrations (less than ~12%), the oxygen diffusivity increases as the salt concentration increases. This observation appears to be opposite to what one may expect as Friedel’s salt and Kuzel’s salt can fill/block the pores and reduce the oxygen diffusivity. This may be explained by competing mechanism of calcium hydroxide (CH) dissolution and leaching. Figure8 shows the solubility of lime (CaO) in CaCl2 solution as the CaCl2 concentration increases [46]. The solubility of lime increases as CaCl2 concentration increases until calcium oxychloride forms and precipitates in the solution. Therefore, mortar samples exposed to CaCl2 solution are susceptible to calcium hydroxide (so-called Portlandite in cement chemistry or CH) leaching from cementitious binder. An increase in CaCl2 concentration can result in an increase in leaching until the CaCl2 concentration reaches the point when calcium oxychloride forms. Calcium hydroxide leaching at lower CaCl2 concentration (less than ~12%) can increase the porosity in mortar sample and increase the oxygen diffusivity. This was not seen in the fluid absorption experiment (Section 3.1) where a decrease in fluid ingress was generally observed as the salt concentration increased. In fact, calcium hydroxide leaching outward of the sample may further reduce fluid ingress toward the sample for samples exposed to a lower concentration of CaCl2 (less than ~12%) since calcium hydroxide leaching occurs in the opposite direction of fluid ingress. As a result, calcium hydroxide leaching may be another factor in reducing fluid ingress into samples in addition to the formation of Friedel’s/Kuzel’s salts for samples exposed to lower concentration of CaCl2 (less than ~12%).Figure 8
Solubility of lime (CaO) in CaCl2 solution at different temperatures (for samples tested at 20°C and 40°C, precipitation of calcium oxychloride were reported for concentrations more than 15% and 20%, resp.) [46].


## 3.5. The Effect of Degree of Saturation on Oxygen Permeability

The oxygen permeability of mortar samples with different degrees of saturation was also tested. These tests were performed to determine the effect of the degree of saturation on the oxygen permeability. Figure9 shows the oxygen permeability results as a function of degree of saturation for all mortar samples. A change in the degree of saturation has a substantial influence on oxygen permeability in the degrees of saturation less than ~70%. The degree of saturation less than 70% approximately corresponds to removing water from small pores (i.e., gel pores with pore diameter less than 5 nm) [38–41]. At degrees of saturation that were greater than 70%, approximately all the small pores become saturated causing disconnection of open/empty pores [38–41]. As a result, oxygen can barely penetrate through the sample at degrees of saturation more than 70%.Figure 9
The effect of degree of saturation on oxygen permeability for mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement (notice that modified Gaussian function is only fitted for DI water points and the scale fory-axis is not identical).
(a)
(b)A Modified Gaussian Function, as shown in (3), is fitted empirically for the data points (oxygen permeability versus degree of saturation) obtained for samples saturated with DI water: (3)KP=a+b·exp⁡-0.5·Ds-cde,where KP is the oxygen permeability in m/s and Ds is the degree of saturation. a, b, c, d, and e are coefficients for Modified Gaussian Function. a, b, c, d, and e are obtained to be 1 × 10−15, 4.55 × 10−14, 0, 23, and 2.2, respectively, for mortar samples prepared using Type I cement and 5 × 10−15, 2.40 × 10−13, 0, 10, and 1.0, respectively, for mortar samples prepared using Type V cement.


## 3.6. The Effect of CaCl2 on Oxygen Permeability

Oxygen permeability was performed on samples that were exposed to solutions with varying CaCl2 concentrations. Exposure to the CaCl2 solution can alter the degree of saturation in mortar sample as shown in Figure 9. The disparity in the degree of saturation in each sample can substantially alter the transport response of the mortar sample as discussed in Section 3.5 and it is essential to minimize its effect to understand the effect of CaCl2 on the oxygen permeability result. Therefore, the oxygen permeability of mortar samples exposed to CaCl2 solution was modified for degree of saturation equal to 50% using (3).The modified oxygen permeabilty is calculated for the mortar samples exposed to CaCl2 solution and it is shown in Figure 10 as a function of CaCl2 concentration in the solution. A similar trend as was observed for oxygen diffusivity (Section 3.4) can be observed for oxygen permeability as well: (1) an increase in CaCl2 concentration increases the oxygen permeability until the salt concentration reaches ~12% due to calcium hydroxide leaching increasing the porosity of the mortar sample, and (2) beyond this point, the formation of calcium oxychloride in pores fills the pores, decreasing the oxygen permeability.Figure 10
The effect of salt concentration on modified oxygen permeability for 50% degree of saturation in mortar samples prepared using (a) Type I ordinary Portland cement and (b) Type V ordinary Portland cement (notice that the scale fory-axis is not identical).
(a)
(b)


## 4. Conclusion and Summary

This paper describes tests to measure the fluid absorption and gas transport (oxygen diffusivity/permeability) properties of mortars exposed to CaCl2 solutions. The mortars were prepared using two cements (Type I and Type V). The mortars were exposed to solutions with varying CaCl2 concentrations and with varying degrees of saturation. Based on the results of this study, the following conclusions can be drawn:(i)
Calcium oxychloride formation can substantially decrease fluid absorption and gas transport in cementitious materials. A substantial decrease in transport properties (i.e., absorption, oxygen diffusivity, and oxygen permeability) was observed for samples exposed to solutions of higher CaCl2 concentrations (solution with concentrations more than ~12% by mass). This is mainly due to the fact that, at concentrations greater than ~12%, calcium oxychloride is stable at room temperature (23°C ± 1°C) and can cause blocking or filling the pores.(ii)
Calcium hydroxide leaching influenced the gas transport properties of cementitious material exposed to CaCl2 solutions with low concentrations (~<12%). As the CaCl2 concentration increases, calcium hydroxide leaching also increases and can increase the concrete porosity. Any increase in concrete porosity can further increase gas and fluid ingress in cementitious materials.(iii)
Comparing samples prepared using Type I cement (with 9% C3A) and Type V cement (with approximately no C3A) shows that the formation of calcium chloroaluminate phases (e.g., Friedel’s salt and Kuzel’s salts) can also reduce the gas and fluid ingress properties in the mortar. The formation of Friedel’s salt and Kuzel’s salts (in addition to calcium oxychloride) in mortar samples prepared using Type I cement can further block or fill the concrete pores, thereby decreasing fluid and gas transport in mortar sample.(iv)
Deicing salts can increase the saturation state of cementitious materials resulting in an increase in the equilibrium relative humidity of the pore solution. The change in the saturation state of cementitious materials can substantially alter the transport properties of concrete. For degrees of saturation less than 70%, an increase in degree of saturation caused a considerable reduction in oxygen permeability. For degrees of saturation more than 70%, however, the change in oxygen permeability was relatively negligible since the small pores (i.e., gel pores with pore diameter less than 5 nm) become saturated causing disconnection of open/empty big pores. As a result, oxygen cannot easily penetrate through the sample at degrees of saturation more than 70%.(v)
Transport properties are often used in concrete to predict the time in which the chloride reaches its threshold value to initiate the corrosion of reinforcing steel or to estimate the time when the degree of saturation in concrete reaches its critical value to cause freeze-thaw damage. The results of this study show that, at high concentration of CaCl2 (more than 12%), the formation of chemical reactions may be a dominant factor in determination of service life (or damage development) rather than corrosion of reinforcement or freeze-thaw damage since fluid and gas ingress was not considerable at high concentrations due to pore blocking caused by chemical reactions. At low concentration (less than 12%), however, calcium hydroxide leaching due to CaCl2 solution exposure may increase the porosity, thereby decreasing the service life of concrete.



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*Source: 929864-2015-06-04.xml*