Ramato Ashu
Tufa
a,
Efrem
Curcio
*ab,
Willem
van Baak
c,
Joost
Veerman
d,
Simon
Grasman
d,
Enrica
Fontananova
b and
Gianluca
Di Profio
b
aDepartment of Environmental and Chemical Engineering, University of Calabria (DIATIC-UNICAL), via P. Bucci CUBO 45A, 87036 Rende, CS, Italy. E-mail: e.curcio@unical.it; Fax: +39 0984 496655; Tel: +39 0984 494013
bInstitute on Membrane Technology of the National Research Council (ITM-CNR), c/o University of Calabria, via P. Bucci, cubo 17/C, 87036 Rende, CS, Italy
cFujifilm Manufacturing Europe B.V., Oudenstaart 1, 5047 TK, Tilburg, The Netherlands
dREDstack B.V., Pieter Zeemanstraat 6, 8606 JR, Sneek, The Netherlands
First published on 13th August 2014
In the present work, a salinity gradient power-reverse electrodialysis (SGP-RE) unit was tested for the production of electrical energy by exploiting the chemical potential of real brackish water and exhaust brine from a solar pond. A cross-flow SGP-RE module (REDstack B.V.), equipped with AEM-80045 and CEM-80050 membranes specifically developed by Fujifilm Manufacturing Europe B.V. within the EU-funded project REAPOWER (“Reverse Electrodialysis Alternative Power Production”), was able to generate a maximum power density (expressed in W m−2 membrane pair – MP) of 3.04 W m−2 MP when operated with pure NaCl aqueous solutions (0.1 M in low concentration compartment – LCC, 5 M in high concentration compartment – HCC) at 20 °C and at a recirculation rate of 20 L h−1. However, a drastic reduction to 1.13 W m−2 (−63%) was observed when feeding the SGP-RE unit with artificial multi-ion solutions mimicking real brackish water and exhaust brine. Further experimental activity allowed to identify Mg2+ ion as responsible for the significant increase in stack resistance and consequent depletion in SGP-RE performance. Therefore, specific softening treatments of the real solutions should be considered in order to maintain the process efficiency at practical level.
(1) |
Previous investigations carried out on aqueous NaCl solutions, which mimic seawater and river water salinity, reached a power density around 2 W m−2 of membrane3–7 and energy efficiency around 50%.8 Vermaas et al. (2013) showed that the theoretically obtained Gibbs free energy of mixing seawater (30 g L−1 NaCl) and river water (1 g L−1 NaCl), both at a flow rate of 1 m3 s−1 is 1.39 MW.8
Advantages of SGP-RE operations carried out at high concentration in the HCC have been clearly envisaged in the work of Post et al. (2007); if LCC and HCC are fed with 0.05 M and 5 M NaCl, respectively, the theoretically available amount of energy from mixing 1 m3 of diluted and 1 m3 of a concentrated solution at 293 K increases to 15 MJ.9
At present, literature works on RE systems operated under high concentrated solutions like brine are less in number and, most of the work, refer to pure NaCl aqueous solutions. A power density up to 0.87 W m−2 (all data are referred to total membrane area, unless otherwise specified) has been reported for a RE system operated with a standard grade electrodialysis membrane compartments filled with a coal-mine brine and fresh water.10 Theoretical models predict that a power density up to 8.5 W m−2 is achievable by appropriate optimization and use of specially developed AEM and CEM membranes in contact with brine and seawater solutions.1 However, the behaviour of a RE system might vary significantly when operated with real solutions. From eqn (1) it is possible to roughly envisage the different levels of influence of the monovalent and multivalent ions on the open circuit voltage generated by SGP-RE. Assuming apparent membrane permselectivity and activity coefficients constant, the electrochemical potential generated by monovalent ions (almost all investigations in literature focus on Na+ and Cl−) is about twice as large as the one produced by divalent ions (Mg2+ and Ca2+ are among the most abundant ions in natural water) when operating at equal ion concentration ratio. Therefore, the sensitivity of a SGP-RE system to real feed conditions is crucial for practical applications.
To date, literature lacks systematic and adequate information on the effect of the simultaneous presence of ions other than sodium and chloride on SGP-RE performance. Vermaas et al. (2014) observed that, when using a mixture with a molar fraction of 10% MgSO4 and 90% of NaCl in both LCC and HCC, experimentally obtained power density in steady state decreased from 29% to 50% compared to the case, in which the feed solutions contained only NaCl as a salt.11 An increase in stack resistance because of the addition of Mg2+ ions into sodium chloride solution was also noticed by Post et al. (2009).12 Further experimental investigation is needed in order to define clearly the potentialities of the SGP-RE technology and to take a decisive step towards real applications.
In the present work, with the aim to investigate realistic high-salinity conditions, in which sodium, magnesium, calcium, chloride, sulfate, and bicarbonate are the most common and abundant salt ions in natural waters, experiments have been carried out using brackish water and brine from solar ponds (Sicily, Italy) as a sources for low concentration compartment (LCC) and high concentration compartment (HCC) of a SGP-RE unit, respectively. The effect of ionic composition on SGP-RE was evaluated by the measurement of current, voltage and power density.
Membrane code | Thicknessa (μm) | Ion exchange capacity (mmol g−1 membrane) | Density of fixed chargesa (mol L−1) | Membrane area resistanceb (Ω cm2) |
---|---|---|---|---|
a Measurement conditions: NaCl 0.5 M, 20 C. b Measurement conditions: NaCl 0.5 M, 20 °C, 2.8 cm s−1. | ||||
Fuji-AEM-80045 | 129 ± 2 | 1.4 ± 0.1 | 3.8 ± 0.2 | 1.551 ± 0.001 |
Fuji-CEM-80050 | 114 ± 2 | 1.1 ± 0.1 | 2.4 ± 0.2 | 2.974 ± 0.001 |
Testing solutions (composition in Table 2) were prepared by dissolving the following reagent grade salts: NaHCO3, KCl and Na2SO4 purchased from Sigma Aldrich S.r.l. (Italy); NaCl, CaCl2·2H2O and MgCl2·6H2O from Carlo Erba Reagenti (Italy) in deionized water.
Na+ | K+ | Ca2+ | Mg2+ | Cl− | HCO3− | SO42− | ||
---|---|---|---|---|---|---|---|---|
a Calculated from eqn (1). Activity coefficients calculated by PHREEQC v. 2.18.00 software.15 | ||||||||
Brackish water | Concentration (mg L−1) | 1520 | 49.7 | 101 | 323 | 3560 | 0.523 | 335 |
Molar ratio | [Na+]/[K+] = 52.1 | [Na+]/[Ca2+] = 26.4 | [Na+]/[Mg2+] = 4.99 | [Cl−]/[HCO3−] = 11717 | [Cl−]/[SO42−] = 28.8 | |||
Brine from solar pond | Concentration (mg L−1) | 66000 | 7740 | 242 | 37400 | 170000 | 50.0 | 64400 |
Molar ratio | [Na+]/[K+] = 14.5 | [Na+]/[Ca2+] = 474 | [Na+]/[Mg2+] = 1.86 | [Cl−]/[HCO3−] = 5841 | [Cl−]/[SO42−] = 7.15 | |||
Theoretical voltage over membranea (mV) | 84 | 117 | 5 | 61 | 80 | 122 | 42 |
Salt solutions were recirculated throughout the SGP-RE system at a flow rate of 20 L h−1 by Masterflex L/S digital peristaltic pumps Mod. no. 7528-10 6–600 rpm (Cole-Palmer, US). Heated circulating baths (PolyScience, US) were used to control the temperature of recirculating streams; temperature at the six inlets of the module was monitored by Multichannel data logging thermometers type K 800024 with high full scale accuracy of ±0.5% rdg (Sper Scientific, US). The conductivity of the solutions was measured by YSI (US) model 3200 Conductivity Instrument.
V(I) = OCV − RstackI | (2) |
It is noteworthy to mention that power density is equal to zero when the current is equal to zero (open circuit condition) or when the voltage is equal to zero (shortcut current condition).
Ion chromatography (IC) was used to evaluate the variation in the composition of LCC dilute solutions after one hour of SGP-RE operation in batch mode.
Cation and anion analysis were performed by 861 Advanced compact ion chromatograph (Metrohom Italiana SrL, Italy) and data processed by ICNet 2.3 software. For cation analysis, Metrosep A Supp 5 250/4.0 column and Metrosep A Supp 4/5 Guard precolumn were used with eluent solution 2 mM HNO3/0.25 mM oxalic acid. For anion analysis, Metrostep C4-250/4.0 column and Metrostep C 4 Guard precolumns were used, with 3.2 mM Na2CO3/1 mM NaHCO3 as the eluent solution.
Fig. 2 a) Voltage vs. current; (b) gross power density vs. current density. Data collected under reference conditions: NaCl solution (0.1 M/0.5 M). Temperature: 20 °C. Margin of error within 10%. |
Kim and Logan (2011) showed an innovative microbial reverse-electrodialysis unit (5-cells stack), when operated with typical seawater (600 mM NaCl) and river water (12 mM NaCl) solutions at 0.85 mL min−1, produced up to 3.6 W m−2 (cathode surface area) and 1.2–1.3 V with acetate as a substrate; a higher flow rate (1.55 mL min−1) resulted in power densities up to 4.3 W m−2.16
In a comparative study between reverse electrodialysis and pressure retarded osmosis, both considered for applications on seawater and river water, Post et al. (2007) calculated a potential maximum power density for SGP-RE in the range of 2–4 W m−2.9
Using a 50-cells stack, a power density of 0.93 W m−2 was obtained by Veerman and colleagues (2009) with artificial river water (1 g L−1 NaCl) and artificial sea water (30 g L−1 NaCl).4
Daniilidis et al. (2014) achieved a power density of 6.7 W m−2 of total membrane area using 0.01 M NaCl solution against 5 M at 60 °C, in general, the power density was found to increase monotonically for highly concentrated feed solutions.17
Theoretical predictions on a 12-cells stack equipped with Fujifilm ion exchange membranes and operated with 0.5 M/5.4 M NaCl diluate/concentrate solutions resulted in a maximum gross power density of 2.4 W m−2.4 A maximum gross power density of 2.2 W m−2 was measured in a stack having an intermembrane distance of 100 μm using 0.507 M NaCl as artificial seawater and 0.017 M NaCl as artificial river water.7
LCC solution composition | HCC solution composition | Parameters in eqn (2) | |
---|---|---|---|
OCV (V) | R stack (Ω) | ||
0.1 M NaCl | 5 M NaCl | 3.40 | 3.83 |
0.0999975 M NaCl + 8.5 × 10−6 M NaHCO3 [Cl−]/[HCO3−] = 11717 | 4.99915 M NaCl + 8.5 × 10−4 M NaHCO3 [Cl−]/[HCO3−] = 5841 | 3.39 | 3.79 |
0.098 M NaCl + 0.002 M KCl [Na+]/[K+] = 52.1 | 4.68 M NaCl + 0.32 M KCl [Na+]/[K+] = 14.5 | 3.40 | 4.08 |
0.096 M NaCl + 0.004 M CaCl2 [Na+]/[Ca2+] = 26.4 | 4.99 M NaCl + 0.01 M CaCl2 [Na+]/[Ca2+] = 474 | 3.27 | 3.84 |
0.0966 M NaCl + 0.0034 M Na2SO4 [Cl−]/[SO42−] = 28.8 | 4.39 M NaCl + 0.61 M Na2SO4 [Cl−]/[SO42−] = 7.15 | 3.40 | 4.15 |
NaCl 0.083 M + MgCl2 0.017 M [Na+]/[Mg2+] = 4.99 | NaCl 3.25 M + MgCl2 1.75 M [Na+]/[Mg2+] = 1.86 | 2.73 | 6.69 |
Fig. 3 a) Voltage vs. current; (b) gross power density vs. current density for multi-ion solutions. Compositions are detailed in Table 3. Temperature: 20 °C. Margin of error within 10% (average of 3 tests). |
Despite its significant concentration in the brine (0.32 M), the impact of K+ on the power density was quite limited because of the similar electrochemical properties of Na+ and K+ ions, listed as follows: ionic radii of unhydrated Na+ and K+ are 1.17 Å and 1.64 Å, respectively; ionic radii of hydrated Na+ and K+ are 3.58 Å and 3.32 Å, respectively;18 ion diffusion coefficients in water for Na+ and K+ are 1.334 × 10−9 m2 s−1 and 1.957 × 10−9 m2 s−1, respectively.19 Although no appreciable difference in OCV was observed, Ishortcut moderately decreased to 0.83 A (−6.7%) and Rstack increased to 4.08 Ω (+6.5%). The maximum power density (2.84 W m−2) was reached at a current density of 41.8 A m−2.
Because of its propensity to form sparingly soluble CaSO4 and to precipitate from solution, Ca2+ is generally present in natural waters only at relatively low concentration. As a consequence, for the investigated LCC/HCC composition of 0.004 M/0.096 M CaCl2, both OCV and power density were affected in a limited extent (−4% and −6.6% with respect to pure NaCl, respectively). The concentration of sulphate and magnesium ions is typically highest after Na+ and Cl− in brine, seawater and brackish water. However, the presence of SO42− did not significantly change OCV and resulted in a moderate decrease of Ishortcut (0.82 A) and Pd,max (2.79 W m−2, −8.2% with respect to pure NaCl).
On the other hand, the presence of magnesium drastically decreased both OCV (2.73 V, −20% with respect to pure NaCl) and power density (1.11 W m−2, −64% with respect to pure NaCl). The measured value of iPd,max = 20.2 A m−2 was lowest. The effect of magnesium valence on the reduced electrical potential difference has been already anticipated when introducing eqn (1).
Moreover, the significant enhancement of the cell resistance may be attributed to an increase in membrane resistance in the presence of Mg2+. Sata (2004) reported a two- to three-fold increase in electrical resistance for different commercial cation exchange membranes (NEOSEPTA CL-25T, AMFion C-310, Ionac MC-3470) when using MgCl2 instead of NaCl. An enhancement in the electrical resistance of the membranes with the concentration of the electrolyte solution was also because of the increase in Donnan adsorbed salts and shrinking of the membranes.20
A systematic investigation of this aspect, based on the electrochemical impedance spectroscopy,13,14 will be the objective of future communications.
Fig. 4 Internal area resistance per cell for the binary solutions investigated (single membrane area: 100 cm2; number of cell pairs: 25). |
These results show a lower IAR per cell of SGP-RE stack (below 26.8 Ω cm2) compared to previous investigations on RE operated with a river water/seawater solutions pair, which was above 50 Ω cm2 in most cases.3,4,18 With respect to the reference NaCl solutions (Rstack = 3.83 Ω, IAR = 15.32 Ω cm2), significant variations in electrical resistance were observed only for NaCl + MgCl2 solutions. In this case, the presence of magnesium increased the resistance of the stack (6.69 Ω) and IAR (26.8 Ω cm2) by 75%, resulting in a drastic decrease of 64% in power density.
Only the solution flowing in the low concentration compartment was analyzed because of the large measurement errors related to the small variations in the highly concentrated brine.
Results reported in Table 4 show an increase in the overall concentration of LCC in the investigated interval of time, and the total mass of the dissolved ions increases by 164% from 6970 to 18400 mg L−1. Within a narrow margin of measurement error (2%), the charge balance after migration of ions is satisfied (total positive charge = 329 meq L−1. Total negative charge = 323 meq L−1).
HCC | LCC | |||
---|---|---|---|---|
Ion | Initial concentration (mg L−1) | Initial concentration (mg L−1) | Concentration after 1 hour (mg L−1) | Concentration increase (mmol L−1) |
a Volume of low conc. compartment: 5 L; volume of high conc. compartment: 5 L. Solutions recirculated at 20 L h−1. Temperature: 20 °C. Data averaged on 3 measurements. | ||||
Na+ | 66000 | 1520 | 3870 | 102 |
K+ | 7740 | 49.7 | 478 | 11 |
Mg2+ | 37400 | 323 | 1740 | 58 |
Ca2+ | 242 | 101 | 115 | 0.35 |
Cl− | 170000 | 3560 | 8960 | 152 |
SO42− | 64400 | 335 | 3380 | 32 |
Fig. 5 illustrates the transport rate of each ion as a function of its concentration in HCC compartment.
Because of the nonideal behavior of the membranes, having perselectivity lower than 100%, a combined transport of both cations and anions can occur. It is interesting to compare transport rate and theoretical voltage over membrane for each ion reported in Table 2. The measured OCV for the SGP-RE stack operated with brackish water/solar pond brine was 2.77 V (Fig. 2a), thus implying a membrane voltage of 55 mV. Most of the voltages reported in Table 2 are higher than 55 mV, indicating a forward transport. Exceptions are for divalent ions Ca2+ and SO42−, in which expected back-transport is not observed because of the effect of multiple co-ion transport. When considering all ions, the overall electrochemical balance is satisfied within an acceptable confidence interval (7%).
The diffusion of Na+ resulted in a concentration increase of 155% for an initial HCC/LCC Na+ concentration ratio of 34; a similar concentration increase (+152%) was found for chlorine with an initial HCC/LCC Cl− concentration ratio of 47.8. These data seem to confirm that ion migration through ion exchange membranes is substantially driven by a concentration gradient. In highlighting the experiments on ion transport carried out by Post et al. (2009), in which the LCC solution consisted of 3 mM NaCl + 2 mM MgSO4 and the HCC of 0.45 M NaCl + 0.05 M MgSO4, an almost two-fold increase of sodium and chloride content in the LCC was observed after one hour when operating with standard-grade ion-exchange membranes.12
Moreover, our measurements indicate that sodium and magnesium are transported across CEM with a flux of 2.84 and 3.24 meq m−2 s−1, respectively, whereas chlorine and sulfate diffuse across AEM with rates of 4.23 and 1.76 meq m−2 s−1, respectively.
Moreover, an urgent need for developing specific ion exchange membranes not suffering from magnesium effects is envisaged.
This journal is © The Royal Society of Chemistry 2014 |