Measurement on Diffusion Coefficients and Isotope Fractionation Factors by a Through-Diffusion Experiment

For radioactive waste disposal, it is important that local groundwater flow is slow as groundwater flow is the main transport medium for radioactive nuclides in geological formations. When the groundwater flow is very slow, diffusion is the dominant transport mechanism (diffusiondominant domain). Key pieces of evidence indicating a diffusion-dominant domain are the separation of components and the fractionation of isotopes by diffusion. To prove this, it is necessary to investigate the different diffusion coefficients for each component and the related stable isotope fractionation factors. Thus, in this study, through-diffusion and effective-porosity experiments were conducted on selected artificial materials and natural rocks. We also undertook measurements relating to the isotope fractionation factors of Cl and Br isotopes for natural samples. For natural rock samples, the diffusion coefficients of water isotopes (HDO and H2O) were three to four times higher than those of monovalent anions (Cl−, Brand NO3), and the isotope fractionation factor of 37Cl (1.0017–1.0021) was slightly higher than that of free water. It was experimentally confirmed that the isotope fractionation factor of 81Br was approximately 1.0007–1.0010, which is equivalent to that of free water. The enrichment factor of 81Br was almost half that of 37Cl. The effective porosity ratios of HDO and Cl were slightly different, but the difference was not significant compared to the ratio of their diffusion coefficients. As a result, component separation was dominated by diffusion. For artificial samples, the diffusion coefficients and effective porosities of HDO and Cl were almost the same; it was thus difficult to assess the component separation by diffusion. However, isotope fractionation of Cl and Br was confirmed using a through-diffusion experiment. The results show that HDO and Cl separation and isotope fractionation of Cl and Br can be expected in diffusion-dominant domains in geological formations.


Introduction
Diffusion is the slowest transport mechanism in a geological formation. For this reason, in diffusion-dominant systems, groundwater flow is very slow and solute transport is limited. In general, the ratio between advection and diffusion is characterized by the Peclet number (=vL/D: v is velocity, L is the characteristic length, D is the diffusion coefficient); diffusion is dominant when the Peclet number is below one. Exploitation of diffusion-dominant domains is considered to be promising for radioactive waste disposal. Therefore, many studies have evaluated diffusion-dominant domains in natural systems. These studies have been summarized [1][2][3].
In this study, diffusion experiments were conducted to investigate component separation and isotope fractionation by diffusion. The diffusion coefficients of HDO and Cl in free water were investigated [4,5]. The diffusion coefficients of HDO and Cl were similar to that of free water. However, in natural rocks, the diffusion coefficient of HDO was about three times higher than those of anions such as Cl − and Br − . This was due to interactions 2 of 15 of the anions with negatively charged clay surfaces, which influence the anionic diffusion [2]. Anions are typically restricted to passing thorough pores by diffusion. By using this difference, the diffusion time and boundary condition changes was discussed [6][7][8].
Cl isotopes are fractionated by diffusion; therefore, δ 37 Cl is an important tool for the identification of a diffusion-dominant domain. Many studies have attempted to use isotope fractionation to estimate the diffusion time and boundary condition changes [9][10][11][12][13].
A combination of component separation and isotope fractionation is the most promising method to determine whether a system is diffusion-dominant. In Japan, it is common to find that marine sedimentary rock has been uplifted and flushed by meteoric water. This is a suitable condition under which to assess diffusion-dominant domains in which both component separation and isotope fractionation occur, as normally there is a large difference in HDO and Cl between seawater and meteoric water.
In this study, diffusion experiments were conducted with artificial and natural samples to measure the diffusion coefficients of HDO, Cl and Br, as well as the isotope fractionation factors of 37 Cl and 81 Br. This was the first attempt to determine Br isotope fractionation factors by diffusion for natural rocks in a laboratory. Effective porosity for each component was also measured. Effective porosity influences the progress of diffusion, which depends on D e /n e , where D e is the effective diffusion coefficient and n e is the effective porosity.
If D e /n e is the same for HDO and Cl, component separation does not occur. Therefore, effective porosity was also measured to estimate the progress of diffusion.

Samples
Porous stone, glass filters, and ceramic disks were used as the artificial samples. For the natural samples, the sedimentary rock of the confined layer of the Great Artesian Basin in Australia and siliceous mudstone from Horonobe in the north of Japan were used.
The artificial samples used were various types of filter for soil tests: the glass filters were sintered glass beads, and the porous stones and ceramic disks were sintered clay particles. The porous stones and glass filters were also bound to natural samples to prevent them from collapsing. Ceramic disks are normally used for soil testing. They are categorized by air entry value, which relates to pore radius. Here, air entry values of 1, 3, 5, and 15 Bar were used.
The confined layer of the Great Artesian Basin was from Richmond and Marree, which are the recharge and discharge areas of the Great Artesian Basin, respectively, that were previously drilled and cored [13]. These belong to the Rolling Down Group and are categorized as mudstone [14]. The formation at Richmond is more consolidated compared to Marree. The porosities of Richmond and Marree are about 25% and 40%, respectively.
The Horonobe siliceous mudstone that was used was from the Koetoi and Wakkanai Formation. The difference between these two geological formations lies in the diagenesis of the mudstone [15]. The Koetoi Formation has not undergone diagenesis, is mainly composed of Opal-A, and has a high porosity ratio of about 60%. The Wakkanai Formation has undergone diagenesis, is mainly composed of Opal-CT, and has a lower porosity ratio of about 40% relative to the Koetoi Formation. These rocks were sampled from the Horonobe Underground Research Laboratory (URL). The boundary between the Wakkanai and Koetoi Formations is at a depth of about 250 m in the Horonobe URL.

Through-Diffusion Experiment
A through-diffusion experiment was conducted as shown in Figure 1 [16]. The purpose of the experiment was to determine the diffusion coefficients for HDO, Cl, and Br and the fractionation factors for the Cl and Br isotopes. Occasionally, samples of sedimentary rocks crack due to swelling and unloading. In these cases, advection occurs due to densitydependent flow between the low-and high-concentration tanks, and the diffusion flux may be overestimated due to advection. Thus, reverse direction diffusion from the low-to high-concentration tank was also measured. In the experiment, the high-concentration tank contained HDO, Cl, Br, and NAP. NAP is a fluorescent dye-1-Naphthylamine-4-sulfonic Acid Sodium Salt Tetrahydrate. The low-concentration tank contained Na, NO 3 , and δ 18 O. NaNO 3 solution was used for the desalinization of rock samples, which was necessary as they contained high NaCl contents in their core. The concentrations of the high-and low-concentration tanks are shown in Table 1.
A through-diffusion experiment was conducted as shown in Figure 1 [16]. The purpose of the experiment was to determine the diffusion coefficients for HDO, Cl, and Br and the fractionation factors for the Cl and Br isotopes. Occasionally, samples of sedimentary rocks crack due to swelling and unloading. In these cases, advection occurs due to density-dependent flow between the low-and high-concentration tanks, and the diffusion flux may be overestimated due to advection. Thus, reverse direction diffusion from the low-to high-concentration tank was also measured. In the experiment, the high-concentration tank contained HDO, Cl, Br, and NAP. NAP is a fluorescent dye-1-Naphthylamine-4-sulfonic Acid Sodium Salt Tetrahydrate. The low-concentration tank contained Na, NO3, and δ 18 O. NaNO3 solution was used for the desalinization of rock samples, which was necessary as they contained high NaCl contents in their core. The concentrations of the high-and low-concentration tanks are shown in Table 1.   0  Cs  8300  0  Br  5000  0  NAP 10 0 The through-diffusion experiment was successful when the diffusion coefficients of δ 18 O and NO 3− were in agreement with those of HDO and the anions (Cl − and Br − ). The ceramic disks were the same as the samples tested [16]. Porous and glass filters have high conductivity and ager gel was thus used to prevent advective flow [17]. Sedimentary rock may become cracked by swelling. The sedimentary rock samples were thus bound by porous stones or porous glass for structural support, and the high-concentration solutions (Table 1) were used to prevent swelling.
The through-diffusion experiment was conducted as follows: (1) Form sample to dimensions of about φ50 mm × H 10 mm.
(3) Set the sample on the apparatus shown in Figure 1.  The through-diffusion experiment was successful when the diffusion coefficients of δ 18 O and NO 3− were in agreement with those of HDO and the anions (Cl − and Br − ). The ceramic disks were the same as the samples tested [16]. Porous and glass filters have high conductivity and ager gel was thus used to prevent advective flow [17]. Sedimentary rock may become cracked by swelling. The sedimentary rock samples were thus bound by porous stones or porous glass for structural support, and the high-concentration solutions ( Table 1) were used to prevent swelling.
The through-diffusion experiment was conducted as follows: (1) Form sample to dimensions of about ϕ50 mm × H 10 mm.
(3) Set the sample on the apparatus shown in Figure 1.  Step 2 took about four weeks and was repeated two or three times to confirm the low Cl concentrations.
Step 4 was performed to check for cracking by establishing if a flow was present.
Step 7 was to measure Cl isotopes, which require at least 3 mg Cl.

Effective Porosity Experiment
Effective porosity (n e ) is a measure of the accessible porosity of each component, such as HDO, Cl, Br, and NAP [2]. HDO can propagate better than Cl because clay surfaces are normally negatively charged and influence the progress of diffusion of negatively charged ions. Therefore, it is important to determine the effective porosity.
The effective porosity experiment was conducted as follows: (1) Dip the sample into the high-concentration solution containing HDO, Cl, Br, and NAP. The effective porosity was calculated as follows: where V C is the pore volume of each component, V L is the solution volume for the low-concentration solution, and C H and C L are the concentrations of the high-and lowconcentration solutions at Steps 2 and 4, respectively. n e is the effective porosity, and V S is the volume of the sample, which can be calculated from the diameter and width.
δD and δ 18 O were determined using cavity ring down spectroscopy (Los Gatos Research, San Jose, CA, USA). The Na + , Cl − , and NO 3 concentrations were determined using ion chromatography (Metrohm Co., Herisau, Switzerland). Inductively coupled plasma mass spectrometry (ICP-MS) was used to determine Br − content (Agilent Technology, California, US). NAP was determined by fluorescence spectrophotometry ( Nihonbunko, Tokyo, Japan).
δ 37 Cl and δ 81 Br were determined by gas chromatography continuous flow isotope ratio mass spectrometry (GC-CF-IRMS) at the University of Waterloo [18,19] (Agilent Technologies Inc., Santa Clara, CA, USA; Thermo Fisher Scientific, Bremen, Germany). These measurements required at least 3 mg of Cl and Br, respectively.    The results of the through-diffusion experiment are shown in Table 2. The ratios of the diffusion coefficients and isotope fractionation factors are shown in Table 3. The following equation, which transforms the solution for cumulative flux under constrained concentration boundaries [16,20] (pp. 49-53), was used to evaluate the diffusion coefficient:

Through-Diffusion Experiment
where C L,t is the concentration in the low-concentration tank at t, t is time, C H,0 is the initial concentration in the high-concentration tank, A is the cross-section area in the diffusion direction of sample, W is the sample width, n e is the effective porosity, and V is the tank volume. The following approximation can be applied when D e t/n e L 2 > 0.45 [20] (pp. 49-53): The diffusion coefficient can be calculated from the relationship between time and C L,t as follows: where s is the slope between C L,t and t. The results of the through-diffusion experiment are shown in Table 2. The ratios of the diffusion coefficients and isotope fractionation factors are shown in Table 3. The following equation, which transforms the solution for cumulative flux under constrained concentration boundaries [16,20] (49-53p), was used to evaluate the diffusion coefficient: Figure 3. Results of through-diffusion experiment for natural samples or (1) Horonobe URL 350 m and (2) Richmond 74 m, (a) concentration change, (b) isotope ratio change. δ is the difference in the isotope ratio between initial and time series measurements (δ = δ t=time − δ t=0 ). The absolute value of δ provides the enrichment factor ((α − 1) × 1000‰) if the concentration change effect is neglected.  For the ceramic discs, the diffusion coefficients were 6.5-9.3 × 10 −11 m 2 /s for HDO, 5.0-8.3 × 10 −11 m 2 /s for Cl and Br, and 0.97-2.1 × 10 −11 m 2 /s for NAP.
For the artificial samples, the diffusion coefficients of HDO and the anions (Cl and Br) were almost the same, as shown in Table 3 in which the ratio of the diffusion coefficient normalized by the diffusion coefficient for HDO is provided. The diffusion coefficient of NAP was 10-30% of the other components.
For the natural samples, the diffusion coefficient derived from Equation (5) should be corrected to account for the bound porous stone and porous glass. The correction methods will be discussed below.
For the Richmond samples, the diffusion coefficients were 2.3-3.6 × 10 −11 m 2 /s for HDO and 0.56-1.1 × 10 −11 m 2 /s for Cl and Br. For the Marree samples, the diffusion coefficients were 0.99-1.1 × 10 −10 m 2 /s for HDO and 2.7-3.3 × 10 −11 m 2 /s for Cl and Br. The diffusion coefficient of Richmond was smaller than that of Marree due to the higher porosity of Marree. The diffusion coefficient of HDO was three to four times higher than those of the anions. The diffusion coefficient of NAP could not be estimated because NAP could not be detected in the low-concentration tank.
For the Horonobe samples, the diffusion coefficients were 1.6-2.1 × 10 −10 m 2 /s for HDO, and 3.1-9.2 × 10 −11 m 2 /s for Cl and Br. The diffusion coefficient of HDO was similar for all Horonobe samples. On the contrary, the diffusion coefficients of the Koetoi Formation for Cl and Br were slightly larger than those of the Wakkanai Formation. The diffusion coefficient of HDO was two to five times higher than those of the anions. The diffusion coefficient of NAP could not be estimated, as mentioned before.

Effective Porosity Experiment
The results of the effective porosity experiments are shown in Table 4. This table shows the effective porosities for HDO, Cl, Br, and NAP and the porosities determined with the drying method. The ratios of the porosities divided by the drying porosities are also shown in Table 4. For the artificial samples, the porosity of HDO was slightly higher than that of Cl but within 12%, so the porosities of HDO and Cl can be considered to be similar. In contrast, for the Richmond and Marree samples, the porosity ratios of Cl and HDO were about 50% and 70%, respectively. For the Horonobe samples, it was 80-100%. The decreasing ratio was smaller than those for Richmond and Marree.

Corrections for Natural Samples Bound by Porous Stone and Glass Filters
Natural samples were bound by porous stones or glass filters to prevent cracking by swelling and unloading. Ceramic discs, glass filters, and porous stones were set onto the pedestal directly, without additional support. Thus, a correction had to be applied to accurately estimate the diffusion coefficients for natural rocks. Assuming a conceptual model of bound samples as shown in Figure 4, under a steady state, the relationship between flux and the diffusion coefficient is expressed as follows: where F is flux, D i is the diffusion coefficient of the i-th material, ∆C i is the concentration difference within the i-th material, and ∆L i is the length of the i-th material.
where F is flux, Di is the diffusion coefficient of the i-th material, ΔCi is the concentration difference within the i-th material, and ΔLi is the length of the i-th material.
Considering the experimental condition, D1 = D3 and ΔL2 = 2ΔL1 = 2ΔL3: where the apparent diffusion coefficient D' for length ΔL2 of the bound sample is as follows: Therefore, it becomes the following: Assuming that the diffusion coefficient for porous stone and glass filters is equivalent to approximately 3 × 10 −10 m 2 /s, which is the average of the diffusion coefficient for porous stone and glass filters, the relationship between D2 and D' is shown in Figure 5. When D1 is sufficiently larger than D' (D1 >> D'), D2 is equivalent to D' (D2≒D'). Considering the experimental condition, D 1 = D 3 and ∆L 2 = 2∆L 1 = 2∆L 3 : where the apparent diffusion coefficient D' for length ∆L 2 of the bound sample is as follows: Therefore, it becomes the following: Assuming that the diffusion coefficient for porous stone and glass filters is equivalent to approximately 3 × 10 −10 m 2 /s, which is the average of the diffusion coefficient for porous stone and glass filters, the relationship between D 2 and D is shown in Figure 5. When D 1 is sufficiently larger than D (D 1 >> D ), D 2 is equivalent to D (D 2 where F is flux, Di is the diffusion coefficient of the i-th material, ΔCi is the concentrati difference within the i-th material, and ΔLi is the length of the i-th material.
Considering the experimental condition, D1 = D3 and ΔL2 = 2ΔL1 = 2ΔL3: where the apparent diffusion coefficient D' for length ΔL2 of the bound sample is as f lows: Therefore, it becomes the following: Assuming that the diffusion coefficient for porous stone and glass filters is equivale to approximately 3 × 10 −10 m 2 /s, which is the average of the diffusion coefficient for poro stone and glass filters, the relationship between D2 and D' is shown in Figure 5. When is sufficiently larger than D' (D1 >> D'), D2 is equivalent to D' (D2≒D'). D ). To estimate the isotope fractionation, Dl and Dh are set as the diffusion coefficients for the light and heavy isotopes, respectively. Here, the isotope fractionation factor α is set as Dl/Dh. α' is the isotope fractionation factor of the bounded sample. α' can be expressed as follows:  (12) where Dh2/Dh1 and Dl2/Dl1 are equivalent to D2/D1.
As a result, the isotope fractionation factor of α2 can be solved as follows: Assuming that D1 and α1 are set to be 3 × 10 −10 m 2 /s and 1.0014, respectively, α2 can be calculated by using D' and α', as shown in Figure 6. When D1 is significantly larger than D' (D1 >> D'), α2 is equivalent to α' (α2≒α'). Therefore, if D1 is significantly larger than D', D' and α' are equivalent to the original value of D2 and α2. To estimate the isotope fractionation, D l and D h are set as the diffusion coefficients for the light and heavy isotopes, respectively. Here, the isotope fractionation factor α is set as D l /D h . α' is the isotope fractionation factor of the bounded sample. α' can be expressed as follows: where D h2 /D h1 and D l2 /D l1 are equivalent to D 2 /D 1 . As a result, the isotope fractionation factor of α 2 can be solved as follows: Assuming that D 1 and α 1 are set to be 3 × 10 −10 m 2 /s and 1.0014, respectively, α 2 can be calculated by using D and α , as shown in Figure 6. When D 1 is significantly larger than D (D 1 >> D ), α 2 is equivalent to α (α 2 where F is flux, Di is the diffusion coefficient of the i-th material, ΔCi is the concentration difference within the i-th material, and ΔLi is the length of the i-th material.
Considering the experimental condition, D1 = D3 and ΔL2 = 2ΔL1 = 2ΔL3: where the apparent diffusion coefficient D' for length ΔL2 of the bound sample is as follows: Therefore, it becomes the following: Assuming that the diffusion coefficient for porous stone and glass filters is equivalent to approximately 3 × 10 −10 m 2 /s, which is the average of the diffusion coefficient for porous stone and glass filters, the relationship between D2 and D' is shown in Figure 5. When D1 is sufficiently larger than D' (D1 >> D'), D2 is equivalent to D' (D2≒D'). α ). Therefore, if D 1 is significantly larger than D , D and α are equivalent to the original value of D 2 and α 2 .

Diffusion Coefficient
For the artificial samples consisting of ceramic discs, porous stones, and glass filters, the diffusion coefficients of HDO and Cl were similar. The diffusion coefficients of HDO were about 1.0-1.3 times higher than those of Cl.
On the contrary, for natural samples, the diffusion coefficients of HDO were three to four times higher than those of Cl. The differences in diffusion coefficients for natural samples were much higher than those of artificial samples. This may have been related to the influence of the negative charge of surfaces [21]. The diffusion coefficients of Br were similar to those of Cl. Anions were transported within small areas compared to the water isotopes (HDO an H 2 18 O). Thus, the ratio of the diffusion coefficients of HDO and Cl depends on the clay content and pore properties, including the porosity and tortuosity. Thus, a diffusion experiment was necessary to determine the difference in the diffusion coefficients.

Diffusion Coefficient
For the artificial samples consisting of ceramic discs, porous stones, and glass filters, the diffusion coefficients of HDO and Cl were similar. The diffusion coefficients of HDO were about 1.0-1.3 times higher than those of Cl.
On the contrary, for natural samples, the diffusion coefficients of HDO were three to four times higher than those of Cl. The differences in diffusion coefficients for natural samples were much higher than those of artificial samples. This may have been related to the influence of the negative charge of surfaces [21]. The diffusion coefficients of Br were similar to those of Cl. Anions were transported within small areas compared to the water isotopes (HDO an H2 18 O). Thus, the ratio of the diffusion coefficients of HDO and Cl depends on the clay content and pore properties, including the porosity and tortuosity. Thus, a diffusion experiment was necessary to determine the difference in the diffusion coefficients.
The diffusion coefficient of NAP was about one-fifth that of Cl for artificial samples. In comparison, the diffusion coefficient of natural samples could not be calculated because the NAP concentration in the low-concentration tank was below the analytical detection limit. NAP is organic matter, with a large molecular weight and structure compared to individual ions; thus, it has a very low diffusion coefficient and cannot pass thorough small pores. If organic matter can be transported by advection and not diffusion, the presence of remaining organic matter relative to other ions may be evidence of a diffusiondominant domain.
The effective porosity is shown in Table 4. With the exception of the Richmond and Marree samples, there was no significant difference between the effective porosities of HDO and Cl, and all were within 20%. In contrast, in the Richmond and Marree samples, the effective porosity of Cl decreased with a decreasing drying porosity. The ratio of the effective porosities of Cl and HDO was nearly 1.2. It is possible that the difference in the diffusion coefficient was counteracted by the effective porosity. Thus, measuring the effective porosity is important.
As shown above, the diffusion coefficient of HDO was about three to four times higher than that of Cl, and the difference in the effective porosity between HDO and Cl The diffusion coefficient of NAP was about one-fifth that of Cl for artificial samples. In comparison, the diffusion coefficient of natural samples could not be calculated because the NAP concentration in the low-concentration tank was below the analytical detection limit. NAP is organic matter, with a large molecular weight and structure compared to individual ions; thus, it has a very low diffusion coefficient and cannot pass thorough small pores. If organic matter can be transported by advection and not diffusion, the presence of remaining organic matter relative to other ions may be evidence of a diffusion-dominant domain.
The effective porosity is shown in Table 4. With the exception of the Richmond and Marree samples, there was no significant difference between the effective porosities of HDO and Cl, and all were within 20%. In contrast, in the Richmond and Marree samples, the effective porosity of Cl decreased with a decreasing drying porosity. The ratio of the effective porosities of Cl and HDO was nearly 1.2. It is possible that the difference in the diffusion coefficient was counteracted by the effective porosity. Thus, measuring the effective porosity is important.
As shown above, the diffusion coefficient of HDO was about three to four times higher than that of Cl, and the difference in the effective porosity between HDO and Cl was not significant compared to the difference in diffusion. Therefore, HDO and Cl were separated by diffusion for natural samples but separation did not occur for artificial samples.

Isotope Fractionation Factor
To estimate the isotope fractionation factor, it was necessary to correct for the initial influence and concentration change [16]. The initial influence could be negated because sampling was not conducted at the beginning of experiment. At least 3 mg of Cl and Br was required to measure these isotopes, so the required volume was too high when the concentration in the solution was low. The effect of concentration change increases with time, so it had to be accounted for. A standard curve was used to correct for this effect [16].
For the through-diffusion experiment, the concentration in the low-concentration tank can be expressed as follows [16], when the initial unsteady state is neglected: where C L,t is the concentration at time t in the low-concentration tank, C H,0 is the initial concentration in the high-concentration tank, β is the condition of the high-concentration tank, β = 1 when the concentration tank remains constant, β = 2 when the concentration changes (normal condition), D is the diffusion coefficient, A is the sample area, V is the sample volume, W is the sample width, and t is the time, as mentioned before.
Using the above equation, the isotope ratio in the low-concentration tank can be expressed as follows: where C l ,t and C h ,t are the concentration of light and heavy isotopes at t, respectively. α is the fractionation factor (= D L /D H ). α can be solved as follows: Then, the following approximation can be applied: where ∆ is the isotope ratio, subscripts L and H represent the low-and high-concentration tanks, respectively, and subscripts t and 0 represent the time and time = 0 (initial condition), respectively. α was calculated for each measured value. The α values and associated errors are listed in Table 2 as averages and standard deviations for measured values. For a bound sample, α' can be calculated by Equation (16) and α' can be transformed into α 2 using Equation (13). Here, α 1 is assumed to be the average for glass filters and porous stones. After this, the average and standard deviation can be calculated. α 2 is the fractionation factor of a natural sample.
For artificial samples, the fractionation factor of 37 Cl was 1.0016 ± 0.0007 for ceramic disks and 1.0015 ± 0.0001 for porous stone and glass filters. These values were slightly smaller than that of free water, which is 1.0016-1.0018 at 21 • C [17]. The fractionation factor of 81 Br was 1.0008 ± 0.0004 for ceramic disks and 1.0007 ± 0.00015 for porous stone and glass filters. These values were similar to that of free water, which is 1.00064 at 21 • C [17]. For the modular dynamics simulation, the fractionation factor was 1.0019 ± 0.0010 for 37 Cl [22] and 1.0008 ± 0.0002 for 81 Br [23]. The measured fractionation factors for artificial samples were similar to that of free water.
The enrichment factor of 81 Br, which was (ε = (α − 1) × 1000‰), was half of that of 37 Cl. This was in agreement with the measured value for free water [17].
For natural samples, the fractionation factor of 37 Cl was 10018 ± 0.00003 for the Koetoi Formation, 1.0020 ± 0.00008 for the Wakkanai Formation, and 1.0020 ± 0.0001 for the Richmond and Marree samples. These fractionation factors were higher than that of free water. The fractionation factors for the Wakkanai Formation were higher than those for the Koetoi Formation. Here, the fractionation factors increased with decreasing porosity. However, the fractionation factors for Richmond were smaller than those for Marree, which does not agree with the trend observed in the Koetoi and Wakkanai formations. This may have been due to influence from the variation in the isotope measurements. The fractionation factor of 81 Br was 1.0008 ± 0.00001 for the Koetoi Formation, 1.0009 ± 0.00001 for the Wakkanai Formation, and 1.0008 ± 0.0001 for the Marree and Richmond formations. These values were similar to that of free water and those of artificial samples. The enrichment factors of 81 Br were about half of 37 Cl, which also agreed with the artificial samples. There was no significant difference between an artificial and natural sample. The enrichment factor of 37 Cl was not as high and the enrichment factor of 81 Br did not show a distinct difference.

Summary
Through-diffusion experiments and effective porosity experiments were conducted to evaluate diffusion-dominant domains. For these experiments, ceramic discs, porous stones, and glass filters were used as artificial samples. For natural samples, the Koetoi and Wakkanai Formations, which are sedimentary rock formations in Horonobe, Japan, and confined layers sampled at Richmond and Marree in the Great Artesian Basin, Australia, were used.
For the through-diffusion experiments, HDO and H 2 18 O as water, Cl − , Brand NO 3 − as anions, and NAP as organic matter were used as tracers. It was found that for artificial samples, the diffusion coefficients of water isotopes were only slightly higher than those of the anions Cl − , Br − and NO 3 − . The fractionation factor of 37 Cl calculated for artificial samples was 1.0014-1.0017, which was equivalent to that of free water. On the contrary, for natural samples, the diffusion coefficient of water isotopes was three to five times higher than for the anions. The fractionation factor of 37 Cl calculated for natural samples was 1.0018-1.0021, which is higher than that of free water, as well as that of the artificial samples. This indicates that the negative charge at the surface of the natural samples influences the diffusion coefficient and fractionation factor. The fractionation factor of 81 Br was 1.007-1.009 for the artificial samples and 1.007-1.0010 for the natural samples. This was similar to the fractionation factor calculated for free water. The enrichment factor of 81 Br was almost half that of 37 Cl.
The effective porosity of HDO was larger than for anions, such as Cland Br -. For natural samples, the coefficient ratio of HDO and the anions was much larger than the effective porosity ratio of HDO and the anions. Therefore, HDO and the anions were separated by diffusion for natural samples. In contrast, HDO and the anions were not separated by diffusion for artificial samples because the diffusion coefficient and effective porosities of HDO and the anions were not so different. Isotope fractionation was observed for all samples; thus, the isotopes of Cl and Br were fractionated by diffusion. The separation of water isotopes and anions and the isotope fractionation of Cl and Br are useful parameters to evaluate whether a domain is diffusion-dominant. An investigation focused on the profile of δD (HDO), Cl, Br, δ 37 Cl and δ 81 Br can play an important role in assessing a diffusion-dominant domain. There are many locations where marine formations have been uplifted and exposed to meteoric water. If this marine formation is in a diffusion-dominant condition, this is a very suitable condition for applying the above method, as seawater and meteoric water have very different δD (HDO) and Cl values, causing a large diffusion gradient. Through-diffusion experiments to estimate the diffusion coefficient and fractionation factors and effective porosity experiments help to better understand diffusion-dominant domains and diffusion times.