Review pubs.acs.org/jced
A Review of Sodium Fluoride Solubility in Water Jacob G. Reynolds* and Jeremy D. Belsher Washington River Protections, LLC, P.O. Box 850, Richland, Washington 99352, United States ABSTRACT: The solubility of NaF in water is important to a number of industries, but there is a limited review of the large amount of solubility data scattered throughout the literature. The present study collected all of the data on the NaF solubility in water that could be found in the peer-reviewed literature between the temperature 0 and 100.6 °C (the upper temperature being approximately the boiling point of a saturated solution). Fifty-five solubility data points were found, collected from 29 studies. There was a large amount of scatter among the data, both across and within most studies. After screening out suspect data, the solubility of NaF was found to be a linear function of temperature, with a change of solubility of 0.003 molal per °C. Averaging the data at 25 °C provides an estimated solubility of 0.987 molal at that temperature.
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cause someone to say “I will just use the most recent measurement, assuming that new data is better data than that from year 1930”. At the time the authors started this study, the newest data on NaF solubility in water was reported by Selvaraj et al., who report a NaF solubility of 4.31 wt %. at 25 °C.17 This same study reports a NaF solubility of 4.01 wt % at 50 °C, considerably lower than the value they report at 25 °C,17 making the data suspect. Clearly, these discrepancies indicate that a more detailed analysis of the solubility of NaF in water is needed. The commonly employed reference books Perry’s Chemical Engineers’ Handbook and Lange’s Handbook of Chemistry do not have any data on the solubility of NaF in water at any temperature.18,19 In 1991, The International Union of Pure and Applied Chemistry sponsored a review of the solubility of alkali chlorides in water, but not sodium fluoride.20 Balej evaluated the solubility of many inorganic electrolytes in water.21 In that evaluation, however, he simply took the NaF solubility data from a study modeling the activity of water in NaF solutions by Hamer and Wu.21,22 In turn, Hamer and Wu took the NaF solubility data from Ivett and De Vries without stating why this one study was favored over any other in the literature.22,23 Of note is that Ivett and De Vries report the same NaF solubility in water to three significant digits at three different temperatures.23 It seems suspect that measurements at three different temperatures resulted in the exact same value to three significant digits at all three temperatures. Therefore, it was concluded that a more thorough review of NaF was needed.
INTRODUCTION The solubility of sodium fluoride (NaF; CAS number 7681-494) in water is important to many industries. NaF is heavily used in organic synthesis and hydrometallurgy.1,2 The solubility of NaF is also important to the action of toothpaste.3 In nature, NaF is known as the mineral villiaumite and is found in alkaline rocks and evaporite deposits.4,5 The solubility of NaF is important to water treatment.6 Sodium fluoride salt is a nuisance chemical in the aqueous portion Bayer alumina refineries.7 The present work came out of interest in alkaline nuclear wastes at the Hanford site near Richland, WA, in the United States of America, where NaF as well as NaF-containing double salts have precipitated.8,9 Nuclear wastes are highly concentrated electrolyte solution containing NaNO2, NaNO3, NaOH, and NaAl(OH)4 as the most prevalent electrolytes, with many other electrolytes (including fluoride) being present. Given the complexity of the waste, solubility models are being developed10−12 to the support of the remediation effort. Weber et al. developed a Pitzer based model for NaF solubility that is being used for nuclear waste applications at Hanford.13 Weber et al., however, found that there is a large amount of scatter in the literature on the solubility of NaF solubility in water.13 Thus, their model for the temperature-dependent Gibbs free energy of NaF is somewhat sensitive to the data they selected for model fitting. Weber uses only a fraction of the data available in the literature. The limitations of the NaF solubility data encountered by Weber can be illustrated by discussing a few studies. Foote and Schairer are one of the few researchers who report the results of duplicate analysis of NaF solubility in water at 25 °C.14 Their measurements came to be 3.97 and 3.98 wt % NaF. This seems like reasonable evidence that the actual solubility of NaF in water at this temperature is between 3.97 and 3.98 wt % until you look at the solubility of NaF they reported at 35 °C. NaF solubility increases with temperature, as indicated by the NaF heat capacity,15,16 but Foote and Schairer report a lower solubility at 35 °C (3.97 wt %) than at 25 °C.14 This could then © XXXX American Chemical Society
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DATA A literature review was undertaken to find all of the available data on NaF solubility in water between 0 and 100.6 °C (Table 1), the upper temperature being approximately the boiling point of a saturated solution in water.24 Table 1 contains all of Received: January 26, 2017 Accepted: May 5, 2017
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Table 1. Bibliography of Studies Reporting NaF Solubility in Water between 0 and 100.6 °C authors Aghaie and Samaie29 Aghaie and Samaie29 Aghaie and Samaie29 Aghaie and Samaie29 Akerlof and Turck43 Belova and Mikailov44 Belova and Mikailova44 Campbell and Campbell30 Carter45 Chuvashev et al.46 Chuvashev et al.46 Faridi and El Guendouzi38 Faridi and El Guendouzi38 Faridi and El Guendouzi38 Faridi and El Guendouzi38 Foote and Schairer14 Foote and Schairer14 Foote and Schairer14 Foote and Schairer14 Foote and Schairer14 Foote and Schairer14 Foote and Schairer14 Foote and Schairer14 Hernandez-Luis et al.41 Ivett and De Vries23 Ivett and De Vries23 Ivett and De Vries23 Jehu and Hudleston47 Karov et al.48
T in °C
NaF solubility
original units
25 25 25 25 25 60 72.5 25
0.976 0.971 0.976 0.971 0.9989 4.57 4.93 37.7
mol/L mol/L mol/L mol/L molality wt % wt % g/L
0.985a 0.980a 0.985a 0.980a 0.9989 1.141 1.235 0.906
25 20 50 25
4.054 4.07 4.37 1.00
wt % wt % wt % molality
1.0065 1.011 1.089 1.00
40
1.03
molality
1.03
60
1.10
molality
1.10
80
1.20
molality
1.20
35 35 25 25 15 15 10 10 25 15 25 35 20 25
4.02 3.97 3.98 3.97 3.93 3.92 3.92 3.97 0.9851 0.983 0.983 0.983 3.96 4.01
wt % wt % wt % wt % wt % wt % wt % wt % molality molality molality molality wt % wt %
0.998 0.985 0.987 0.987 0.974 0.972 0.972 0.985 0.9851 0.983 0.983 0.983 0.982 0.995
solubility in molality units
authors Lopatkina33 Lopatkina33 Mason and Ashcraft49 Morales et al.50 Morkretskii and Portyannikova51 Morozova and Rzhechitskii52 Morrison and Jache53 Nagorskaya and Novoselova36 Nagorskaya and Novoselova36 Nagorskaya and Novoselova36 Nagorskaya and Novoselova36 Nagorskaya and Novoselova36 Payne37 Payne37 Payne37 Petrov et al.24 Roslyakova et al.31 Ryss54 Selvaraj et al.17 Selvaraj et al.17 Tananaev55 Tananaev55 Toghiani et al.56 Toghiani et al.56 Vlasov and Shishkina34 Zhikharev et al.32 a
the data used in this study, including temperature in °C, the solubility of NaF in water in the units of the original reference, and the solubility converted to molality. There are many studies in the literature focused on physical properties of NaF−H2O solutions that were not aimed at determining solubility, for example, the study of water activities by Hernandez-Luis et al.25 In many of those studies, they reported properties such as osmotic coefficient at NaF concentrations that are at or near saturation. We only included the NaF concentration from those type of studies if the authors specifically said that the solutions were at saturation with solid NaF. Data from Guiot26 were not included in Table 1 because these data were drastically different from any data set in Table 1 at every temperature. Lastly, we did not include data from Bekmuratov and Dobrynina, who only presented their data graphically.27
T in °C
NaF solubility
25 50 40 25 80
3.77 3.97 3.97 3.96 4.33
wt wt wt wt wt
% % % % %
0.933 0.985 0.985 0.982 1.078
0
3.70
wt %
0.915
0 0
3.42 3.99
wt % wt %
0.844 0.990
20
4.10
wt %
1.018
40
4.47
wt %
1.115
80
4.48
wt %
1.117
94
4.73
wt %
1.182667
0 25 35 100.6 25 25 25 50 0 40 25 50 25 25
0.871 0.983 0.989 4.80 3.77 3.86 4.31 4.01 3.95 4.35 3.929 4.171 3.75 3.77
molality molality molality wt % wt % wt % wt % wt % wt % wt % wt % wt % wt % wt %
0.871 0.983 0.989 1.20 0.933 0.956 1.07 0.995 0.980 1.08 0.9742 1.037 0.928 0.933
original units
solubility in molality units
Derived value; see the Discussion section.
was employed to get a simple relationship between the central tendency of the data and temperature. Most of the data sets in the literature reported the solubility of NaF in terms of wt % NaF in liquid, which could be readily converted to molality. All of the statistical analysis was performed in molality rather than wt %. The book by Aitchison explains that wt % is an undesirable unit for statistical analysis because all of the component percentages are constrained to sum up to 100%.28 This constraint invalidates the assumptions built into the statistics employed here.28 Aitchison explains that ratios of components, like molality (moles per kg of water), are a much more appropriate unit for performing statistical analysis.28 There were several data sets that we did not use in any of the statistical analysis. Two data sets reported the NaF solubility in units of molarity or g/L and did not provide a density or water content that could be used to convert to molality.29,30 Those two data sets were excluded from the statistical analysis but are discussed in the Discussion section. We did not use the data of Selvaraj et al.17 because this data set appeared to be a large outlier at both 25 and 50 °C. Lastly, we did not use the data from Roslyakova et al.31 because this same research group reported the exact same solubility value in a study less than one year earlier,32 and it is assumed that these two reported values were not two independent measurements.
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ANALYSIS A statistical analysis of the data found in the literature was performed. There were more data found at 25 °C than at any other temperature. Given the large amount of data available at this temperature, and the importance of this temperature as a common reference temperature in thermodynamics, a mean concentration and confidence interval around this mean were calculated. For the rest of the temperatures, a regression model B
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“Lower Cluster of Data Points Exclude” in Table 2, more likely represent the true solubility of NaF in water. Nonetheless, the estimated NaF molality at 25 °C is similar for both data sets. The data sets that were not included in the restricted data set are from refs 32−34. The uncertainty of NaF solubility at 25 °C can be compared to NaCl. Hefter35 used the standard deviation of 41 independent NaCl measurements complied by Cohen-Adad and Lorimer20 to conclude that ur(mNaCl) = 0.0026 at a 68% confidence interval and ur(mNaCl) = 0.0076 at a 95% confidence intervals. Using the same methodology for the data points selected for this study, the uncertainty in measured solubility at 25 °C for NaF is between ur(mNaF) = 0.013 at a 68% confidence interval and ur(mNaF) = 0.04 at a 95% confidence interval.
SOLUBILITY AT 25 °C Table 2 reports the summary statistics calculated here: estimated mean, the standard error of the estimated mean, as Table 2. Summary Statistics of the Solubility of NaF in Water at 25 °C statistic
full data
lower cluster of data excluded
estimated mean estimated standard deviation (s) standard error (SE) 95% confidence interval upper limit for μ̂ 95% confidence interval lower limit for μ̂ n (observations in data set)
0.976 0.0257 0.00662 0.999
0.987 0.0132 0.00381 0.995
0.961
0.978
15
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SOLUBILITY TRENDS BETWEEN 0 AND 100 °C Figure 2 is a plot of all of the data as a function of temperature, showing the large scatter in the data. There was a large spread between the lowest and the highest molalites at many temperatures, with 0, 40, and 80 °C all having a spread greater than 0.1 m. At 25 and 50 °C the spread was 0.1 m. The five data sets that had three or more data points are called out in the graphic. The data were fit with a simple linear model (eq 2)
12
well as the upper and lower 95% confidence interval of the estimated mean. The mean is the best estimate of the true NaF solubility in water at 25 °C. For the NaF data, the standard error, SE, is the variability (or standard deviation) associated with the estimated saturated NaF molality at 25 °C, and it can be used, along with the t-distribution, to construct a (1 − α)% confidence interval for the estimated NaF solubility per eq 1.
mNaF ± tα /2, n − 1SE
(1)
mNaF = β1T + β0
Here, n is the number of observations in the data set, and mNaF = the measured NaF solubility in molality. The “full dataset” column reported in Table 2 contains the calculated statistics when using all of the data that was not excluded in the Analysis section of this paper. After inspecting the data, it was observed that there was cluster of 11 data points around 0.98 molal and 3 points tightly clustered around 0.93 molal (Figure 1). Given that there was much more data around 0.98 molal and that 0.93 molal was below the lower 95% confidence interval of the estimated mean NaF concentration at 25 °C, the smaller clusters were assumed to be less accurate. A second set of summary statistics are provided in Table 2, where the statistics were recalculated with all of the data with values at 0.93 molal removed. These results, shown in the column
(2)
In eq 2, T is the temperature in Celsius, and β1 as well as β0 are empirically determined parameters. The results of the fit are shown in Table 3 and cover the central tendency of the data. Additional regression models and data transformation were explored, but they did not provide a better fit than the model in eq 2. The fitted model explains much of the variance in the measured molalities (r2 = 0.74), but there is clearly lots of noise in the data. It is possible that some solubility behavior is not perfectly captured by the simple linear model, but any nonlinearity is hidden by the scatter in the data. Therefore, this linear model represents the best empirical estimate of the solubility of NaF in water as a function of temperature currently available but should be re-evaluated as more data is collected.
Figure 1. Data density as a function of NaF solubility in water reported by the literature in Table 1. C
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Figure 2. Solubility of NaF in water as a function of temperature.
provide a reasonable estimate of NaF solubility as a function of temperature. In two studies, the original data were provided in either mass or moles per liter, and they did not provide a density or water content that could be used to convert the units to molality.29,30 Neither data set was used in any statistical analysis so that the regression was not biased by any inaccuracy in the estimated water content, but they are analyzed here. In those two cases, the Laliberte−Cooper model39 was used to estimate the water content needed to calculate molalities using the method described by Reynolds and Carter,40 with the results reported in Table 1. The molalities for the data reported by Aghaie and Samaie29 at 25 °C came to be 0.980 and 0.985, both of which are within the standard error reported in Table 2. The molality for the data reported by Campbell and Campbell30 came to be 0.91 at 25 °C, one of the farthest from the mean of any data set in Table 1 In the Introduction, we stated that the newest data point at 25 °C at the time we started this study seemed anomalous. Two new experimental studies have been published since we started this study in time to be included.38,41 The solubility of NaF at 25 °C reported in these two most recent studies (Table 1) are within the 95% confidence interval of the present statistical analysis, with one result being almost identical to the mean value in Table 2. We did not use the data from Selvaraj et al. in the development of the regression model because the data was an outlier, and their solubility reported at 50 °C was lower than their data reported at 25 °C.17 It is possible that their data is transposed in their paper, because their 50 °C data point was within the 95% confidence interval for the estimated solubility
Table 3. Regression Parameter for NaF Solubility in Water as a Function of Temperature (r2 = 0.74) parameter
value
standard error (SE)
β1 β0
2.87 × 10−3 0.918
2.53 × 10−4 1.05 × 10−2
lower 95% CI upper 95% CI 2.36 × 10−3 0.897
3.34 × 10−3 0.939
Most of the data sets consist of just one or two data points, so it is difficult to compare the trends of the individual sets against the eq 2, but we can look at the five data sets with three or more points. The Foote and Schairer as well as Ivett and De Vries data sets are the only two that have multiple data points between 10 and 35 °C, and neither seem consistent with eq 2 since both data sets exhibit minimal change in solubility over their reported temperature range.14,23 As noted in the Introduction, it seems odd that Ivett and De Vries found the exact same solubility to three significant digits at all three temperatures they investigated.23 In contrast, the Nagorskaya and Novoselova, Payne, as well as Faridi and El Guendouzi data sets cover a broader range of temperatures, and in general, the behavior of these data sets are broadly consistent with eq 2.36−38 Solving eq 2 at T = 25 °C calculates a NaF solubility of 0.990 m, which is within the standard error of the estimated solubility at 25 °C in reported in Table 2.
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DISCUSSION As noted in the Introduction, commonly used standard reference books have not provided a table of consensus solubility values for NaF in water as a function of temperature. Given the variability in the data in Figure 2, this lack of consensus in references books is understandable. Nonetheless, the regression equation and associated confidence interval can D
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of NaF in water at 25 °C, and their 25 °C data point is just 0.02 molal greater than the solubility predicted by eq 2 at 50 °C. From a nuclear waste management perspective, the present data can be used to estimate the minimum quantity of water required to dissolve NaF from sludge at the Hanford site. For instance, tank 241-AW-103 at the Hanford site has NaF as the dominate salt in the solid phase and is estimated to have 1.15 × 105 kg (6.06 × 106 moles) of fluoride.8,42 Once the sodiumbearing interstitial liquid is washed out, approximately 6.14 × 106 kg of water are required to dissolve the NaF out of this single tank at 25 °C. If the water is evaporated after the NaF is dissolved into it, the NaF will simply reprecipitate.
(12) Carter, R.; Pierson, K. L.; Reynolds, J. G. Binary Pitzer Model Parameters for Predicting the Solubility of Key Electrolytes in Hanford Waste. Proceedings of the Annual Waste Management Symposium, Phoenix, AZ, March 2−6, 2014. (13) Weber, C. F.; Beahm, E. C.; Lee, D. D.; Watson, J. S. A Solubility Model for Aqueous Solutions Containing Sodium, Fluoride, and Phosphate Ions. Ind. Eng. Chem. Res. 2000, 39, 518−526. (14) Foote, H. W.; Schairer, J. F. I. The Ternary Systems with Water and Two Salts. J. Am. Chem. Soc. 1930, 52, 4202−4209. (15) King, E. G. Low Temperature Heat Capacities and Entropies at 298.15 K. Of Cryolite, Anhydrous Aluminum Fluoride and Sodium Fluoride. J. Am. Chem. Soc. 1957, 79, 2056−2057. (16) O’Brien, C. J.; Kelley, K. K. High Temperature Heat Contents of Cryolite, Anhydrous Aluminum Fluoride and Sodium Fluoride. J. Am. Chem. Soc. 1957, 79, 5616−5618. (17) Selvaraj, D.; Toghiani, R. K.; Lindner, J. S. Solubility in the Na + F + NO3 and Na + PO4 + NO3 Systems in Water and in Sodium Hydroxide Solutions. J. Chem. Eng. Data 2008, 53, 1250−1255. (18) Green, D. W.; Perry, R. H. Perry’s Chemical Engineers’ Handbook, 8th ed.; McGraw-Hill, New York, NY, 2010. (19) Dean, J. A. Lange’s Handbook of Chemistry, 8th ed.; McGraw Hill: New York, NY, 1999. (20) Cohen-Adad, R.; Lorimer, J. W. Solubility Data Series: Alkali Metal and Ammonium Chlorides in Water and Heavy Water (Binary Systems); Pergman Press: New York, NY, 1991. (21) Balej, J. Verification of Accuracy of Standard Thermodynamic Data of Inorganic Electrolytes. Collect. Czech. Chem. Commun. 2010, 75, 21−31. (22) Hamer, W. J.; Wu, Y. C. Osmotic Coefficients and Mean Activity Coefficients of Uni-univalent Electrolytes in Water at 25°C. J. Phys. Chem. Ref. Data 1972, 1, 1047−1100. (23) Ivett, R. W.; De Vries, T. D. The Lead Amalgam-Lead Fluoride Electrode and Thermodynamic Properties of Aqueous Sodium Fluoride Solutions. J. Am. Chem. Soc. 1941, 63, 2821−2825. (24) Petrov, M. R.; Roslyakova, O. J.; Zhikharev, M. I. Solubility in the NaF-Na3PO4-H2O and NaF-NaNO3-H2O Systems at the Boiling Point. Russ. J. Inorg. Chem. 1982, 27, 900−901. (25) Hernandez-Luis, F.; Galleguillos, H. R.; Vazquez, M. V. Activity Coefficients of NaF in (Glucose + Water) and (Sucrose + Water) Mixtures at 298.15 K. J. Chem. Thermodyn. 2004, 36, 957−964. (26) Guiot, J. C. Etudes Sur le Syste’me H2O, Na+, F−, PO43−. Rev. Chim. Miner. 1967, 4, 85−127. (27) Bekmuratov, A.; Dobrynina, T. A. Solubility in the Ternary System NaF-H2O2-H2O. Bull. Acad. Sci. USSR, Div. Chem. Sci. 1971, 20, 2214−2216. (28) Aitchison, J. The Statistical Analysis of Compositional Data, 2nd ed.; Blackburn Press: Caldwell, NJ, 2003. (29) Aghaie, M.; Samaie, E. Non-ideality and Ion-Pairing in Saturated Aqueous Solution of Sodium Fluoride at 25°C. J. Mol. Liq. 2006, 126, 72−74. (30) Campbell, A. N.; Campbell, A. J. R. The Systems (a) BaCl2BaF2- H2O(b) SrCl2-SrF2- H2O (c) CaCl2-CaF2- H2O (d) NaCl-NaFH2O (e) KCl-KF-H2O at 25°C. Trans. Faraday Soc. 1939, 35, 241− 246. (31) Roslyakova, O. N.; Petrov, M. R.; Zhikharev, M. I. The NaFNa3PO4-H2O System at 25 °C. Russ. J. Inorg. Chem. 1979, 24, 115− 116. (32) Zhikharev, M. I.; Petrov, M. R.; Roslaykova, O. N. NaNO3-NaFH2O System at 25 °C. Russ. J. Inorg. Chem. 1978, 23, 785. (33) Lopatkina, G. A. A Study of Solubility in System NaF-NaClNa2CO3-H2O at 25 and 50 °C. J. Appl. Chem. USSR 1959, 32, 2722− 2727. (34) Vlasov, G. A.; Shishkina, L. A. Solubility of NaF in NaClO3 Solutions at 25 °C. Russ. J. Inorg. Chem. 1977, 22, 1250−1251. (35) Hefter, G. Some Highs and Lows (and in-betweens) of Solubility Measurements of Solid Electrolytes. Pure Appl. Chem. 2013, 85, 2077−2087. (36) Nagorskaya, N. D.; Novoselova, A. V. Solubility of NaF in Aqueous Solutions of NaOH. Zhur. Obs. Khimi 1935, 5, 182−185.
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CONCLUSION This study found a large amount of data on NaF solubility in water between 0 and 100.6 °C. There was a large amount of scatter in the values reported at all temperatures. The true solubility of NaF in water at 25 °C is likely between 0.97 and 1.00 molal, with the most likely value of 0.987 molal. The NaF solubility was a linear function of temperature. The change in NaF solubility in water with temperature is approximately 0.003 molal per °C.
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AUTHOR INFORMATION
Corresponding Author
*E-mail:
[email protected]. ORCID
Jacob G. Reynolds: 0000-0001-6091-8540 Notes
The authors declare no competing financial interest.
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REFERENCES
(1) Halpen, D. F. E-Eros Encyclopedia of Reagents for Organic Synthesis; Wiley Online Library, John Wiley & Sons, 2001. (2) Rodriguez, M. H.; Rosales, G. D.; Pinna, E. G.; Suarez, D. S. Effect of Na+ ion on the Dissolution of Ferrocolumbite in Autoclave. Hydrometallurgy 2016, 159, 60−64. (3) Cruz, R.; Ogaard, B.; Rolla, G. Acquisition of Alkali-Soluble Fluoride by Enamel Through Treatment with NaF-Containing Toothpastes in vitro. Eur. J. Oral Sci. 1992, 100, 81−87. (4) Stormer, J. C.; Carmichael, I. S. E. Villiaumite and the Occurrence of Fluoride Minerals in Igneous Rocks. Am. Mineral. 1970, 55, 126−134. (5) Nielsen, J. M. East African Magadi (trona): Fluoride Concentration and Mineralogical Composition. J. Afr. Earth Sci. 1999, 29, 423−428. (6) Jagtap, S.; Yenkie, M. K.; Labhsetwar, N.; Rayalu, S. Fluoride in Drinking Water and Defluoridation of Water. Chem. Rev. 2012, 112, 2454−2466. (7) Sovkilioglu, E.; Carton, C.; Ertugral, S.; Baygul, M.; Dinc, K.; Aveu, S. The Control of Fluoride Concentration in Eti Aluminyum Bayer Refinery Liquor. Light Metals 2013, 112, 2454−2466. (8) Reynolds, J. G.; Huber, H. J.; Cooke, G. A.; Pestovich, J. A. SolidPhase Speciation of Zirconium and Fluoride in Alkaline Zircaloy Cladding Waste at Hanford. J. Hazard. Mater. 2014, 278, 203−210. (9) Reynolds, J. G.; Cooke, G. A.; Herting, D. L.; Warrant, W. L. Salt Mineralogy of Hanford High-Level Waste Staged for Treatment. Ind. Eng. Chem. Res. 2013, 52, 9741−9751. (10) Reynolds, J. G.; Carter, R.; Felmy, A. R. A Pitzer Interaction Model for the NaNO3-NaNO2-NaOH-H2O System from 0°C to 100°C. Ind. Eng. Chem. Res. 2015, 54, 3062−3070. (11) Reynolds, J. G.; Carter, R. Pitzer Model Anion-Anion and Ternary Interaction Parameters for the Na2C2O4-NaOH-H2O and Na2C2O4-NaNO3−H2O Systems. J. Solution Chem. 2015, 44, 1358− 1366. E
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Journal of Chemical & Engineering Data
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DOI: 10.1021/acs.jced.7b00089 J. Chem. Eng. Data XXXX, XXX, XXX−XXX
