Introduction 

Investigation of Magnetic Field (MF) effects on properties of water and aqueous solutions are still of interest although they have been studied for at least 50 years. Hundreds of papers have been published where magnetic fields effects and application of MF in industry, agriculture, medicine, and others are described. Nevertheless, some of the results are debatable or even incompatible. Initially MF studies were focused to eliminate the hard scale formation at elevated temperatures in industrial pipes or house heating installations. If MF would successfully protect against deposition of the carbonates this could be beneficial elimination of chemicals used for water softening which are expensive and harmful for the environment. Later studies of MF effects in many systems and applications were carried out. Generally, using the classical magnetic field theory it is hardly to explain the observed effects which, however, often are well documented and statistically validated. The latest theories claim that to obtain an MF effect more important is the field gradient than its strength [1-3]. Also, the non-classical theory of nucleation mechanism and formation of dynamically ordered, so called liquid like oxyanion polymers, are used to explain the magnetic field action [4,5].

However, to our knowledge only in few papers the investigations of MF effects in different systems where a surfactant was present are reported [6-10]. However, no paper describes any MF effects on pure surfactant solutions. On the other hand, surfactants are present in the surface and waste waters, soil, and many industrial waters, sewage treatment plants, laundry, etc. [11,12]. Therefore, it seemed us interesting to carry out study in a natural room environment to learn whether some MF effects will appear in pure anionic or cationic surfactant aqueous solutions, and if so, whether the effects are reproducible qualitatively and/or quantitatively. In this paper first the MF effects on the rate of water evaporation from a surfactant solution was studied. The enhanced water evaporation from pure water was already reported in some papers [13-20].

For this purpose static MF (max. 0.5 T) originating from ring Nd magnets (MP 86 x 58 x 35 mm) was applied in which the sample of 10^-3 M anionic Sodium Dodecyl Sulfate (SDS) or cationic Dodecyl Trimethylamonium Bromide (DoTAB) solutions were placed in the magnet for up to 2-3h in an open plastic vessel. Simultaneously, another vessel as a reference with the same surfactant solution was placed ca.1.5 m apart from that with the MF and the samples were separated by a wooden board. All the experiments were carried out at room temperature and humidity. Every 30 min the vessels were weighed with the accuracy 0.1 mg, and the evaporated amount of water was calculated. For the reference purposes evaporation of water from the surfactant solution and pure Milli-Q water without MF presence were investigated too. In the previous paper similar studies have been conducted on MF effects on evaporation rate of pure water and water surface tension [21]. These are preliminary studies and depending on the obtained results further systematic investigations in aspect of possible practical applications will be continued. Application of MF for enhancing or hindering water evaporation, depending on the need of the process, would be beneficial.

Experimental 

Materials

Sodium dodecyl sulfate >99.0% was purchased from Fluka and dodecyl trimethylammonium bromide approx. 99% was from Sigma. Both were used without further purification. For preparation of their 10^-3M aqueous solutions water from Milli-Q Plus system was used and the solutions were prepared a day before their first usage.

Methods

For the experiments of evaporation rate 65 mL (in some cases 50 mL, see Figure 8) samples of the surfactant solution or water from Milli-Q Plus system (resistivity 18.2 MΩcm) were used. The magnetic field originated from a neodymium ring magnet 86 mm (outer diameter) x 58 (inner dimeter) x 35 mm (height) directed with its north N­ or south S­ pole upward. The solution or water surface in the vessel was exactly on the level of the magnet edge and the vessel outer diameter was 53.6 mm while the inner one was 52 mm. Figure 1a shows the magnet used and Figures 1b and 1c present changes of the magnetic field strength perpendicularly from the solution surface at the inner edge and at the center of magnet. In Figure 1c the changes of MF gradients at the same places as in Figure 1b are plotted respectively.

Figure 1a: The used magnet and the magnetic field strength change across the radial distribution.

Figure 1b: Changes of MF in the perpendicular direction z from the water surface. Curves: 1-from the magnet top inside wall and curve 2-from the top center of the magnet [21].

Figure 1c: The product of magnetic field and its gradient along the direction z perpendicular to the water surface from the top of inner magnet wall (curve 1) and from the magnet top center (curve 2) [21].

In Figure 2 the setup for the evaporation experiments is shown. The same setup and procedure were used in the study of MF effects on pure water published earlier [21]. As it is seen in Figure 2 during the evaporation experiments the MF-treated and MF-untreated samples evaporated simultaneously at the room temperature (23 ± 1°C) and the relative humidity was 32-38%. The surface area of the sample on which the MF acted was 21.24 cm2 and the circular surface radius was 26 mm. Therefore the meniscus curvature effect on the vapor pressure (Kelvin equation) did not play any role at this sample diameter. From Figures 1b and 1c it is seen that the strongest MF effect in vertical direction appears at the sample vessel walls and it vanishes toward the sample center. In the surface radial direction it decreases from 0.35T to 0.05T. After every 30 min the closed samples were weighed and then their location together with the magnet was replaced. To avoid any possible influence of air fluctuations in the room the samples were placed in plastic tubes (Figure 2). The samples were weighed using a high precision balance Sartorius with an accuracy of 0.1 mg. The amounts of evaporated water were calculated by subtracting from the initial weight of the MF-treated or MF-untreated sample its weight after given time of the evaporating experiment, respectively. Then the difference between these two amounts was calculated and plotted versus time. 

Figure 2: Setup for the solution evaporation experiments.

Results and Discussion

Anionic sodium dodecylsulfate, SDS, solution

First to learn whether water evaporation rate is different from aqueous surfactant solutions than that from pure water experiments without MF were performed using 10-3M SDS solution and pure water. In Figure 3 are shown the results where it can be seen that more water evaporates from pure water than from 10-3M SDS solution (the negative differences in mg). However, the differences obtained in these three separate experiments differ between themselves. The room temperature was the same 22oC and the relative humidity did not differ much. The plateau on the curve indicates that the rate of water evaporation is the same from MF treated and untreated samples and an extremum show the greatest difference in the evaporation rate. The difference in the evaporated amounts can be also presented as the relative percentage taking the evaporated amount from the pure water (or MF-untreated sample) as the reference 100%. In Figure 3 are shown these relative negative percentages calculated after 150 min of the experiment duration. Thus, the reduced evaporation of water from the SDS solution amounts to 2.0%, 10.8% and 14.3%, respectively which gives mean reduction percentage 9%. In experiment 1 (Figure 3, curve 1) the 2.0% relative decrease after 150 min results from 511.2 mg and 521.4 mg evaporated water from the SDS solution and pure water. However, after 30 min of the MF treatment in this experiment the percentage reduction amounted to 18.7% (Figure 3). It is because during this time 94.1 mg and 115.8 mg of water evaporated from the SDS solution and pure water, respectively. Therefore to better depict the changes in the next figures, presenting the differences in amounts of evaporated water in mg, also the relative percentage values are given for 150 min of the experiment duration. As can be seen in Figure 3 in next two experiments much larger difference in the evaporated amounts of water has been obtained. Hence, the mean relative smaller amount of the evaporated water from the SDS solution after 2h is 9.0%. These results show that even without MF presence it is difficult to reproduce exactly the evaporation rate of water in a typical room environment using the same experimental setup, the surfactant lot and water. Nevertheless, an important finding is that water evaporates faster from pure water than 10-3 M SDS solution. However, one would expect an opposite relationship, i.e. faster and enhanced evaporation of water from the SDS solution whose surface tension is lower than pure water, 49.01 ± 0.26 mN/m (10-3 M SDS) and 72.30 ± 0.22 mN/m, respectively. This indicates that the cohesion forces between water molecules are stronger on the surface in pure water (2 × 72.8=145.6 mN/m) than in the SDS solution. Despite that 10-3 M SDS solution concentration is less than its critical micelle concentration, CMC=8.2 ×10-3 M at 25°C, there is already significant amount of SDS molecules adsorbed on this solution surface (compare the surface tensions). The molecules are oriented with their hydrocarbon chains toward the air and the ionic heads are located between the water molecules. The -SO4- head of SDS posseses oxygen atoms which interact with water molecules by hydrogen bonds. They are much stonger than the London dispersion and Keesom dipole-dipole forces, i.e. the strength of hydrogen bonds in water is ca. 20 kJ/mol while that of London and Keesom is 0.4-4 kJ/mol [22]. Van Oss and Constanzo [23] reported surface tension for SDS molecules immersed in water to be 23.8 mN/m for the hydrocarbon tail and 34.6 mN/m for the electron-donor parameter due to the presence of -SO4- head responsible for the hydrogen bonds formation. The average distance between the -SO4- groups in water was evaluated to be 0.907 nm. While between two alkyl chains the attraction amounts to102.1 mJ/m2 so strong repulsion of the electrostatic and polar nature exists between the sulfate heads. Therefore, they have to diverge with at least one -CH2- to which -SO4- is attached. From the surface tension values of SDS solution cited above it results that the interactions are responsible for SDS surface tension to a great degree.

Figure 3: Differences in the amounts of evaporated water from MF-untreated 10^-3M SDS solutions and MF-untreated pure water. 

In the next series of experiments the effect of static MF on the evaporation rate of water from 10^-3 M solution of SDS was studied using the setup shown in Figure 2. The obtained results of five individual experiments performed during different timespan are plotted in Figure 4. In the all cases, except for one, more water evaporated from magnetized solutions. In one experiment during first 2h water evaporated faster from MF-untreated solution. However, at a longer MF treatment time the evaporation rate from magnetized solution significantly increased and after next 2h the difference in the evaporated amount of water from MF-treated sample was similar to the two others MF-treated samples (Figure 4, curves 3 and 5). Interestingly no clear relationship between the MF direction (north N or south S pole directed upward) and the evaporation rate has been observed. Hypothesizing similarly as above for the MF-untreated SDS samples, the observed faster evaporation of water from the MF-treated samples would result from a smaller number of SDS molecules adsorbed on the surface after the treatment. However, it is probably not the case because the surface tension of MF treated10^-3M solution decreases by ca. 4 mN (to be published in the Part II of this paper) and hence according to the Gibbs adsorption equation it means that the surface excess concentration has increased.

For Equation 1 refer PDF

Where: is the surface excess concentration of component 2  (surfactant) relative to its concentration in the bulk solution at zero excess concentration of main component 1(water).
a2 - is the surfactant activity in the bulk solution  (concentration in the case of diluted solutions). 

Figure 4: Differences in the amounts of evaporated water from MF treated and untreated 10^-3M SDS solutions at room temperature 22-24^oCand relative humidity RH = 30-35% obtained for 5 individual experiments on different date as shown in the figure. The final relative differences in the evaporated amounts are given in percentage.

Therefore, the reason of increased water evaporation from MF treated solution might be due to weakening of Van der Waals interactions and hydrogen bonds in water intra-clusters [24,25] and formation of hydrogen bonds of water with the oxygen atoms from -SO3^- groups. The average increase in the evaporated water after 150 min MF treatment amounts to 4.5% but it changes between 1.0% and 8.5% depending on the experiment run (Figure 4). To better depict the MF effects and compare water evaporation from the SDS solution and from pure water the differences are plotted in Figure 5 where curve 1 is that 1 N from Figure 4 (these values are about the mean ones) and the curves 2 and 3 were calculated using the values obtained for pure water on the same day as those of curve 1. As can be seen in Figure 5 during 1h less water evaporated from the MF-untreated 10^-3 M SDS solution than from pure water (1.7%, curve 2). From the MF-treated SDS solution more water evaporated from this solution than the MF-untreated one (1.6 %, curve 1). After timespan 150 min the differences increased to 4.8% (curves 2) and 4.2% (curves 1), respectively. However, within 2h the evaporation rates of water from MF-treated SDS and pure water appeared to be practically the same and decreased by 0.8% only after 150 min (curve 3).

Figure 5: Differences between evaporated water amounts from MF-treated and MF-untreated SDS solutions and pure water.

Curves: 1- between magnetized and non-magnetized solutions; 2-between non-magnetized solution and pure water; 3-between magnetized solution and pure water. The relative differences in the evaporated amounts are given in percentage.

Cationic dodecyltrimethylammonium bromide, DoTAB, solution

Analogous experiments to those with the anionic SDS surfactant were carried out with 10^-3M cationic dodecyltrimethyl ammonium bromide, DoTAB, solution. Similarly as in the case of SDS solution first it was interesting to compare water evaporation rate from 10^-3 M DoTAB aqueous solution and pure water without MF presence. Two series of experiments have been carried out and the results are plotted in Figure 6. While from the anionic SDS solution water evaporated faster from pure water samples, so in the case of cationic DoTAB solution water evaporated faster from its solution than from pure water. In other words, at the same experiment duration more water evaporated from MF-untreated DoTAB sample than pure water, hence the differences in Figure 6 are positive. Also the percentage changes of evaporated water amounts are calculated for 150 min experiment duration and also at the end of particular experiment. The mean value from 7 experiments amounts 5.1% of the increased amount of evaporated water from DoTAB while in the case of SDS solution 9% less of water evaporated from the solution than from pure water (Figure 3). In the room environment at a slightly changing humidity and temperature obtained differences vary from run to run of the experiment but no doubt each time the evaporated amount of water from the solution is larger than from pure water.

Figure 6: Differences between amounts of evaporated water from 10^-3M DoTAB and pure water. Two series of the experiments without MF. Curves: 1-3-t=23^oC, RH=31%; 4-t = 23^oC, RH = 36%; 5-t = 22^oC, RH = 30%; 6-t =21^oC, RH = 23%, 7-t = 24^oC, RH = 36%. The relative differences are given in percentage.

Next the DoTAB sample was MF treated during water evaporation and simultaneously water from a reference untreated sample evaporated too (Figure 2). The results of differences in the amounts of evaporated water from MF treated and untreated solutions are presented in Figure 7 for four individual experiments. It can be seen in the figure that the MF causes increase in the evaporated amount of water in comparison to the MF-untreated solution. The relative percentage from 150 min experiment duration lies between 1.9-9.3%, giving mean value 4.6% which is practically the same as the mean value for SDS MF-treated solutions (4.5%, Figure 4). Similarly as in the case of SDS solution the MF field direction (north or south pole upward) does not make any visible difference. Also it looks that the small changes in relative humidity (32% and 36%) do not influence significantly the evaporation. The surface tension of 10^-3 M DoTAB solution after 60 min MF treatment decreased by 11.4 mN/m from 60.7 mN/m to 49.3 mN/m, i.e. more than in SDS solution, by 5.7 mN/m (to be published in the Part II of the paper). Taking again into account the Gibbs adsorption equation (Equation 1) for binary solutions a decreasing surface tension with the increasing bulk concentration (activity) of a surfactant means an increase in the surface excess concentration of this surfactant G₂⁽¹⁾. Therefore, it can be concluded that MF causes an increased adsorption of these two surfactant molecules on the surface, especially that of cationic DoTAB. In other words, it can be concluded that MF affects the structure of surfactants surface layer in a similar way as it occurs during the increasing bulk concentration of surfactant.

Figure 7: Differences between amounts of evaporated water from MF-treated and MF-untreated 10^-3M DoTAB solutions (65 mL, t = 23^oC, RH=32%, except for curve 4 where RH = 36%).The relative differences are given in percentage.

Then, an evaporation experiment was carried out using simultaneously three samples, i.e. MF-treated DoTAB sample, another MF-untreated sample and pure water. Thus obtained results are plotted in Figure 8. Additionally, for comparison curve 1b shows the biggest differences obtained after MF treatment (curve 3 from Figure 7). The 150-min MF treatment enhances water evaporation from the DoTBA solution between 2.6 % (curve 1a) and 9.3% in the extreme case (curve 1b). This extreme effect is comparable with the differences between evaporating water from the MF-untreated DoTAB solution and pure water (curve 2). In comparison to pure water the 150 min MF treatment enhances evaporation of water by 12.5% (curve 3). Comparing these results with those for SDS solutions (Figure 5) much stronger MF effect is clearly seen in the case of cationic surfactant.

Figure 8: Differences between evaporated water amounts from MF-treated and MF-untreated DoTAB solutions and pure water.
Curves: 1a and 1b-between magnetized and non-magnetized solutions, maximum and minimum differences obtained; 2-between non-magnetized solution and pure water; 3-between magnetized solution and pure water.

Comparison of the MF effects on the surfactant solutions

To compare the observed MF effects on the two kinds of surfactants, first the differences in their ionic heads should be discussed. This is because both surfactants have the same hydrocarbon chain length, C₁₂, therefore the different behaviour can be ascribed to drastic differences in the head group properties. They possess completely different ionic heads, i.e. -OSO₃^-Na⁺ and -N⁺(CH₃)₃Br^–:
First of all, the size of these groups is different which is 0.17 nm² for SDS and 0.54 nm² for the hard-core area of DoTAB. These areas were estimated from knowledge of the bond lengths, bond angles and atomic volumes using a molecular model of the headgroup [26]. Also the distance from the hydrophobic core surface to the centre of the counterion location is 0.545 nm and 0.345 nm, respectively [26]. Therefore the Na⁺ counterions are at a larger distance from the -O-SO₃^- headgroup than Br^- from the -N⁺(CH₃)₃. The Critical Micelle Concentration (CMC) of these surfactants at 25^°C amounts to 8.2 mM and 11.0 mM, respectively. Moreover, the SDS molecules -O-SO₃^- group can form hydrogen bonds with water molecule oxygen atom but this is not the case for DoTAB whose head is more hydrophobic because of the presence of three methyl -CH₃ groups and only a weak N--H hydrogen bond the -N⁺(CH₃)₃ group can form [27]. The determined surface tension of 10^-3 M DoTAB is 60.7 mN/m while that of SDS was 49.0 mN/m (will be publish in Part II of the paper). Because the DoTAB head group is much larger than the SDS therefore it can be expected that the same surface area occupies less DoTAB head groups -N⁺(CH₃)₃ than -O-SO₃^- of SDS. Moreover, the Br^- counterions are located closer to the head [26] and hence at the solution surface the interactions between water molecules and the head group are much weaker than those at the SDS solution surface. Therefore this cationic surfactant can also reduce some of the hydrogen water-water molecules bonding. In consequence evaporation of water from the 10^-3 M DoTAB solution is easier than from pure water (Figure 8), contrary to the SDS solution (Figure 4).

The surface activity of surfactants can be described by Sprow and Prausnitz equation [20].

For Equation 2 refer PDF

Analogical equation can be written for water molecules in the surface layer.

For Equation 3 refer PDF

In Equations 2 and 3 the activity a of the components are defined in symmetrical system, i.e. a_w, a_s ®1 if x_w, x_s ® 1. On the basis of the above equations Zdziennicka et al. [28] found for many surfactant solutions the maximum reduction of water surface tension to be ca. 41 mN/m, what indicated that the chains are oriented parallel toward the surface. This value is smaller than the values of our SDS and DoTAB solutions measured after MF treatment. The bigger decrease in surface tension of the cationic surfactant than the anionic after MF treatment can be ascribed to the presence of three -CH₃ groups in the DoTAB head group whose surface tension is lower than -CH₂- group present in the hydrocarbon tail [29,30]. Hence the decrease in surface tension after MF treatment can be due to the molecules reorientation. More detailed discussion will be given in the paper to follow (in Part II) on the MF effect on the surface tension of these two surfactants. Basing on the above results it can be concluded that the magnetic field causes changes in the structure of the surface layer of adsorbed surfactant molecules and because of different surface properties of -N⁺(CH₃)₃ and -O-SO₃^– groups the former causes water evaporation easier while the later harder.

Possible mechanisms of MF action

It is important to recognize possible mechanisms of the MF force action. Some approaches were discussed in the previous paper dealing with water evaporation from pure water surface [21]. Nakagawa et al. [13] and others [2-5,18] found that for water evaporation in the MF field more important is the field gradient B×dB/dx than the field itself. Moreover, oxygen present in the air can cause a susceptibility gradient in the direction normal to evaporating water surface which can enhance magnetic convection and in consequence a decrease in the water vapor density. This is because volume susceptibility c of oxygen is much greater than that of water and nitrogen. The bulk magnetic force was calculated by the authors [13] from Equation (4).

For Equation 4 refer PDF

In the magnetic field B = 8 T and the field gradient B·dB/dx = 320 T²/m the force corresponded to as much as 17% of the gravitational force acting on the air which can be compared to the thermal convection effect that would be caused by 50K temperature increase from 293K [13]. In the case of our experiment at the water surface close to the inner magnet wall the gradient B·dB/dz amounted to 15 T²/m but only 0.42 T²/m at the magnet centre (Figures 1b and 1c) [21]. Hence the maximum force difference (Equation 4) amounted to 0.089 N/kg which is only 0.91% of the gravitational force and its contribution in the magnetic convection is rather minimal. Then the Lorentz force acting on the ionic surfactant solutions can be analyzed.

For Equation 5refer PDF

In the case of electrolyte solution first term in Equation (5) equals zero because the electric field density E = 0. The second term expresses the magnetic force whose direction is perpendicular both to velocity v of the charge q and to magnetic field B. The force action depends upon the charge and the magnitude of so called cross product of v × B, i.e. the velocity and flux density vectors, where the relative directions of these two vectors are taken into account. The magnitude of the force equals qvB sinϕ, where ϕ is the angle between v and B. If the angle ϕ = 90^o, i.e. v is perpendicular to B, the particle trajectory is circular with a radius of r = mv/qB. For angles ϕ smaller than 90° the charge moves along a helix with the axis parallel to the field lines. Obviously, if ϕ= 0^o no action of magnetic force is observed. Silva et al. [31] taking v @ 0.992 m/s (determined experimentally) and q = 3.2 ×10⁻¹⁹ C (divalent cation) in the field B = 1T calculated the Lorentz force to be 3.17×10^-19 N. Because the ion mass is equal to 10^-25-10^-26 kg, the acceleration (F/m) can be as large as 10⁶-10⁷ m/s² which can cause the ion polarization.

In our experiments the MF in the ring magnet changes radially from the top inner edge to its center from 0.347 T to 0.053 T, which occurs on the distance of 19 mm. Hence ¶B/¶x on the sample surface level equals to 43.2 T/m and 7.9 T/m, respectively. Then the MF gradient changes from 14.96 T²/m to 0.42 T²/m, respectively [13]. Because of the field gradient and some mixing during the samples weighing every 30 min, the ions moves in the solution. Let us assume a v value 0.5 m/s and if some of the ions cross perpendicularly the field lines, the Lorentz force F = qvB for a monovalent ion amounts to (1.6×10^-19 C × 0.5 m/s × 0.347 T) = 0.278×10^-19 N. Hence the acceleration force F/m acting on the dodecylsufate ion C₁₂-O-SO₃^- (4.406×10^-25 kg/ion) would be 6.3×10⁴ m/s² and that acting on C₁₂-N(CH₃)₃⁺ (3.79 ×10^-25 kg/ion) would amount to 7.3 ´ 10⁴ m/s². The force at the magnet center is ca. 6.5 times lower than those at the edge. Although above calculations are very rough ones they show possible way to understand the observed MF effects.

Conclusions

These preliminary experiments showed for the first time that in a common laboratory environment preserving comparable conditions of temperature and humidity the static MF effects on the evaporation of water from both cationic and anionic surfactant solutions are present. Although they are not quantitatively reproducible, they are reproducible qualitatively. Nevertheless the amount of experiments is too small to be evaluated statistically the obtained changes can be assumed as significant because in each experiment simultaneously with MF- treated sample the reference MF-untreated sample was present. Thus in most carried out experiments the MF affects evaporation of water from cationic and anionic surfactant solutions. Water from the MF-treated samples evaporates faster than that from the untreated ones thus leading to a larger evaporated amount of water during the same time. Larger MF effect observed in the experiments for the cationic than anionic surfactant solutions can be understood by taking into account the different properties of the two head groups, the anionic -O-SO₃^-Na⁺ and cationic -N⁺(CH₃)Br^-. The cationic group is over 3 times larger than the anionic and possesses three hydrophobic methyl groups -CH₃. Also the Na⁺ counterions are located at a larger distance from the head than Br^-. The sulfate group can form relatively strong hydrogen bonds with water molecules while the hydrogen bond with the ammonium group is weak, if ever. These differences reflect in the observed differences of the MF effects on these surfactant solutions. Generally, MF increases evaporated amount of water from both surfactant solutions and the mean relative values from several experiments are comparable for up to 150 min of their duration. The rough calculations indicate that MF can interact both perpendicularly to the liquid surface as the bulk magnetic force, as well as horizontally as the Lorentz force. In the Part II of this paper the MF effects on the surface tension of these two surfactants solutions will be described. To our knowledge such MF effects on the surfactant solutions are published for the first time in the literature although a number of papers have been published on the MF effects on water evaporation from pure water. These results suggest that more systematic study at well-defined conditions are needed to better recognized these effects and the MF mechanisms causing their appearance. Such study will be conducted next. Potentially these MF effects may have a practical meaning in the processes where water is evaporated from surfactant solutions.

Acknowledgements 

This work was supported by Polish National Centre of Science, grant 2016/21 B/ST4/00987, which is greatly appreciated.

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Keywords

Magnetic field effects, Anionic and cationic surfactant, Water evaporation