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Journal of the Mexican Chemical Society

Print version ISSN 1870-249X

J. Mex. Chem. Soc vol.58 n.1 México Jan./Mar. 2014

 

Article

 

Thermodynamic Studies of Ion Association of s-Acetylthiocholine Halides and Perchlorate in Methanol Solutions

 

Nasr Hussein El-Hammamy,*1 Marwa Nasr El-Hammamy,2 and Aida Ibrahim Kawana3

 

1 Chemistry Department, Faculty of Science, Alexandria University, Egypt. nasrelhammamy@yahoo.com

2 Physics Department, Faculty of Science, Damanhour University, Egypt.

3 Chemistry Department, Faculty of Education, Alexandria University, Egypt.

 

Received May 24, 2013.
Accepted August 21, 2013.

 

Abstract

Thermodynamic parameters (ΔH0, ΔG0, ΔS0) and the activation energy (ΔEs) were calculated to explain the limiting equivalent conductance (Λ0) and ion association constant (KA) of s-acetylthio-choline halides and perchlorate in methanol solutions at different temperatures by using conductance measurements. It has been evaluated by using Fuoss-Onsager equation. It is evident that the values of (Λ0) increase regularly with increase in temperature. For all salts of s-acetylthiocholine, (Λ0) indicates that higher mobility of the ions in all solvent systems studied. The free energy change ΔG0 values are negative for all salts (Br-, I- and ClO4-) in solvent systems studied. Clearly strengthening the interionic association at higher temperatures is largely caused by a decrease in the permitivity of the solvent. The positive values of (ΔH0) for three salts (Br-, I- and ClO4-) show that the association processes are endothermic in nature. Entropy change (ΔS 0) values were positive for all salts because of decrease in solvation of ion-pair compared to that of the free ion. This may be attributed to increase in the degree of freedom upon association, mainly due to the release of solvent molecules.

Keywords: s-acetylthiocholine salts, ion association, activation energy and thermodynamic functions.

 

Resumen

Los parámetros teimodinámicos (ΔH0, ΔG0, ΔS0) y la energía de activación (ΔEs) fueron calculados para explicar la conductancia equivalente límite (Λ0) y la constante de asociación (KA) a diferentes temperaturas, obtenidas con medidas de conductividad, de soluciones metanólicas de halogenuros y perclorato de s-acetiltio-colina. Estos parámetros fueron obtenidos utilizando la ecuación de Fuoss-Onsager. Los valores de (Λ0) se incrementan directamente con el incremento de la temperatura. Los valores obtenidos de (Λ0) para todas las sales de s-acetiltiocolina indican que existe una gran movilidad de los iones en todos los sistemas estudiados. Los valores para la variación de energía libre ΔG0 son negativos para todas las sales (Br-, I- y ClO4-) en las soluciones estudiadas. El notable incremento de la asociación interiónica a altas temperaturas está directamente relacionado con la disminución de la permitividad de las soluciones. Los valores positivos del (ΔH 0) para tres sales (Br-, I- y ClO4-) indican que los procesos de asociación son de naturaleza endotérmica. Los valores del cambio de entropía (ΔS0) son positivos debido a la disminución de la solvatación del par iónico en comparación con la del ion libre. Este comportamiento podría estar ocasionado por un incremento en los grados de libertad de la asociación, relacionado directamente por la liberación de moléculas del solvente.

Palabras clave: Sales de s-acetiltiocolina, asociación iónica, energía de activación, funciones termodinámicas.

 

Introduction

In a wide temperature range, conductivity measurements for electrolyte solution can give a detailed information for ion-ion and ion-solvent interactions [1, 2]. Primary alcohols (MeOH, EtOH, 1-PrOH and 1-BuOH) are polar solvents, having a lower relative permittivity than that of water. Alcohols associate in liquid by hydrogen bond. In the primary alcohols, ionic association is interpreted in terms of a multiple-step association process involving hydrogen bonded solvated of anions in the homologous series methanol through 1-pentanol by Matesich et al. [3]. Thus in this study, it was attempted to obtain some information on the association of s-acetylthiocholine halides and perchlorate in methanol solutions at different temperatures (25, 30, 35 and 40 °C) by conductometric measurements.

The limiting equivalent conductance and association constants for these salts in methanol solutions at (25, 30, 35 and 40 °C) were determined by analyzing conductivity data terms of Fuoss-Onsager equation [4]. The Thermodynamic functions (ΔH0, ΔG0, ΔS0) and activation energy (ΔEs) were calculated and compared according to interaction of solvent at different temperatures.

Fuoss and Onsager [4], used the sphere in continuum model and gave the following 3-parameter equation for the 1:1 associated electrolyte.

Where, Λ is the equivalent conductance ohm-1 equiv-1 cm2, C is the concentration (equiv/l) and ion association constant (KΑ) was determined using Fuoss and Onsager three parameter. γ is the degree of dissociation which can be calculated using the following equation:

S and E being the theoretically predicted constants, which depend on the dielectric constant D, the viscosity η, and the absolute temperature T of the medium. J is a term which includes the ion and ion-solvent interactions and is given by the equation

Where σ1 and σ2 are functions of the closest distance of approach α0 in addition to η and D.

s-acetylthiocholine is one of the acetylcholine families. Acetylcholine is a universal neurotransmitter in center nervous system. One of its hazards effect is accumulation. Accumulation will cause increased firing of neurons which lead to general hyper activity i.e. toxic to the nerve system.

 

Results and Discussion

It is evident from Tables 1, 2 and 3, that the values of Λ0 increase regularly with increase in temperature for salts of s-acetylthiocholine bromide, iodide and perchlorate, indicating less solvation or higher mobility of the ions in all solvent systems studied. This is due to the fact that the increased thermal energy results in greater bond breaking and also variation in vibrational, rotational and translational energy of molecules lead to higher frequency and higher mobility of ions [5]. Also, it is clear that the association constant (KA) values increase with increase in temperature and with increase in alcohol content and also with the increase of the -CH2- group in alcohol [5].

Since the conductance measurements of an ion depend on its mobility, it is quite reasonable to treat the conductance data similar to the one that employed for the processes taking place with change of temperature [6], i.e.

where A is the frequency factor, R is the ideal gas constant and ΔEs is the Arrhenius activation energy of transport processes. The ΔEs values have been computed from the slope (-ΔEs/2.303RT) of the plot of log Λ0 vs. 1/T and recorded in Tables 1, 2, 3 and Fig. 1.

 

From the tables, the activation energy ΔEs is positive value for the three salts in all solvents. Its values were decreased from Br- to ClO4- , indicating that higher mobility of the ions in solution and hence higher Λ0 values. The free energy change ΔGofor the association process is calculated from equation (2), [7]

Also it is evident from Tables 1, 2 and 3, that the free energy change (ΔG0) values are negative for the three salts (Br-, I- and ClO4- ) in all solvent systems studied. This means that the association process is favored over the dissociation process in all solvent systems.

According to the results of the calculated thermodynamic parameters as shown by Tables 1, 2, 3 and Fig. 2, the standard enthalpy changes, (ΔH 0), can be obtained from the slope (-ΔH0/2.303R) of the plot of log KΑ against. 1/T by using the Van’t Hoffs isochore equation

 

 

The positive values of (ΔH0) for the three salts (Br-, I- and ClO4-) show that the association processes are endothermic in nature and the calculated entropy change (ΔS0), from Gibbs equation;

The positive values of (ΔS0) for three salts (Br-, I- and ClO4-) indicates the randomness of ions in all solvent systems studied.

The values of ΔH0, ΔG0, ΔS0 are recorded in Tables 1, 2 and 3. For s-acetylthiocholine bromide, iodide and perchlorate in methanol at different temperatures (25, 30, 35 and 40 °C). (ΔG0) values decrease with increase in temperature. The decrease in (ΔG0) values for the (three salts) to more negative values at increasing temperature favors the transfer of the released solvent molecules into bulk solvent and leads to a smaller (ΔG0) values. It was observed that (ΔH0) values decrease in the order: I- > Br- > ClO4-. The (ΔH0) values were found to be positive in all alcohols. Positive and high (ΔH0) values can be attributed to the interaction between ions [8]. As presented in (Tables 1-3)(2) (ΔS0) values were positive because of decrease in the solvation of ion-pair compared to that of the free ion [2, 9, 10]. This may be attributed to increase in the degree of freedom upon association, mainly due to the release of solvent molecules.

The main factors which govern the standard entropy of ion association of electrolytes are (I) the size and shape of ions, (II) charge density on ions, III) électrostriction of the solvent molecules around the ions and (IV) the penetration of the solvent molecules inside the space of ions [11].

Bag et al. [12], measured the conductance of Co (III) complex monochloride in MeOH-H2O mixtures at different temperatures (25, 30, 35, 40 °C). It was found that, at a particular temperature ΔG0 becomes more negative. This indicates that ion-pair association is favored with lowering of dielectric constant of medium. A positive entropy change is explained on the assumption that iceberg structure around the cation is broken when association takes place leading to an increase in the degree of disorderness [13].

Dash et al. [5], measured the conductance of Co (III) complex of chloride and bromide in different composition of H2O-MeOH, H2O-EtOH and H2O in n-PrOH at different temperatures. It was found that the association constant KA values of Co (III) complexes of chloride and bromide increase with increase in temperature. It is evident that the activation energy Es is positive for both KA in all solvents, free energy change ΔGn 0 values are negative for both association constants in solvent with increasing the temperature. This indicates that the association process is favored over dissociation process in all solvent systems. The positive values of ΔH0 for both complexes show that the association processes are endothermic in nature. The positive value of ΔS0 indicates the randomness of ions in solvent system studied [5].

Pura [8], measured the conductance of ferric chloride (FeCl3 ) in primary alcohols at different temperatures. It was found that, at particular temperature ΔG0 values decrease with increase in temperature. The decrease in ΔG0 values for FeClto more negative values with increasing temperature favor the transfer of the released solvent molecules into the bulk solvent and lead to a smaller ΔG0 values. The experimental values of ΔG0 for FeCl3 varied in the order: MeOH > EtOH > 1-PrOH > 1-BuOH in thetemperature range studied in this work. It was observed that ΔH0 values of FeCl3 in alcoholic organic solvents decrease in the order of MeOH > EtOH > n-PrOH > n-BuOH. ΔH0 values were found to be positive in all alcohols. Positive and high ΔH0 can be attributed to the interaction between ions. ΔS0 values of FeCl3 in primary alcohols are found to decrease in the order MeOH < EtOH < n-PrOH < n-BuOH, indicating a weakening in the ion solvation due to the formation of ion pairs. The values of ΔS0 for all alcohols used in the study were positive because of the decrease in solvation of the ion pairs compared to that of the free ions. The positive ΔS0 values for FeCl3 in all alcohols may be attributed to the increase in the degree of freedom upon association mainly due to the release of solvent molecules. In other words, the solvation of ions weakens as soon as the ion pair formation occurs. The radii of solvent molecules and the degree of solvation decreases with of -CH2- groups of primary alcohols. For that reason, higher increase in entropy is observed, and the changes of entropy become more positive values from MeOH to «-BuOH. Positive values of ΔH0 and ΔS0 values for FeCl3 can be attributed to the counter balance entropy change resulting from both short- and long- term desolvation of ions. Positive (ΔS0) values attributed to desolvation of ions are also supported by the positive enthalpy values indicating a lack of the covalent bonds [8].

El-Hammamy et al. [14], measured the conductance of cobalt (III) the complex chloropentaammine chloride in water at different temperatures 40 ^ 60 °C and the data were analyzed using Fuoss-Edelson equation [15]. The obtained values of Λand Ka for complex at different temperatures was reported. It was found that Λ0 and KA increase with increasing temperatures. Thus from the plot of log Λ0 vs. 1/T for complex of in water at different temperatures, the ΔES (+ve) value has been evaluated, and also ΔH0, ΔG0 and ΔS0 for complex. It was found that ΔH0 and ΔS0 are positive at a particular temperatures but ΔG0 is negative, this is due to the solvation processes is less but association of ion increase with thermodynamic parameters. Endothermic solvation needs energy to break the bonds around free ion and ion-pairs, ΔS0 was constant but ΔG0 decreases the negativity with increasing the temperature.

El-Hammamy et al. [16], measured the conductance of 1:1 s-acetylthiocholine salts ( Cl-, Br-, I- and ClO4-) in water at different temperatures (25, 30, 35 °C) and the data were analyzed using Fuoss-Onsager equation. Values of Λ0, KA and α0 were obtained (solvation). It was found that Λ0 and α0 increase, while K decrease with increasing the temperatures for all salts of s-acetylthiocholine according to electrostatic attraction theory. Thus from the plot of log Λ0 vs. 1/T for s-acetylthiocholine halides and perchlorate in water at different temperatures, ΔES values have been evaluated, also ΔH0, ΔG0 and ΔS0 for salts. It was found that negative values of ΔH0, ΔG0 and ΔS0 in water at different temperatures; negative value of ΔH0 indicated that ion association processes were exothermic. The solvated radii were also increased with temperature indicating a higher solvation process due to increase in the electronic clouds around the solvated molecules as a result of an increase in their vibration and rotational motion. The limiting equivalent conductance and dissociation degree were also increased as the temperature increased, indicating higher solvation process [16]. The negative values of different thermodynamic parameters ΔH0, ΔG0 and ΔS0, for all salts under test in the used solvent, indicated exothermic association process with less energy-consuming and more stabilization [17]. While in [18], El-Hammamy et al. [18] measured the conductance of s-acetylthiocholine salts (Br-, I- and ClO4-) in acetonitrile at different temperatures (25, 30, 35, 40 °C) the data were analyzed using Fuoss-Onsager equation. The values of Λ0, KA and α0 (solvation) were obtained. It was found that Λ0 and KA increase with increasing the temperature. Thus from the plot of log Λ0 vs. 1/T for each salt in acetonitrile solutions at different temperatures, ΔEs(+ve) values have been evaluated, and also ΔH0, ΔG0 and ΔS0 all the salts. It was found that ΔH0 and ΔS0 are positive values at a particular temperatures but ΔG0 is negative. This is due to the solvation processes is less but association of ion increase with thermodynamic parameters. Endothermic solvation needs energy to break the bond around free ion and ion-pairs, i.e., endothermic solvation process was less energy consuming and more stabilized.

 

Experimental

The s-acetylthiocholine bromide, iodide and perchlorate were purified as reported in the literature [19], methanol (B.D.H) was purified previously as reported in refrence [20]. The specific conductance for purified methanol at different temperatures (25, 30, 35 and 40 °C) was found to be in the range (1.6 -7.3) x 10-7 Ω-1 cm-1. All solutions were reported by reducing weight to vacuo. Salts were weighed on microbalance which reads to ± 0.1 mg. Dilution was carried out successively into the cell by siphoning the solvent by means of weighing pipette. Conductivity Bridge was model Crison Cl P31 and the cell with bright platinum electrodes was used. The cell constant was 0.1 cm-1 for dilute solutions. The solvent constants used in all calculations were taken as reported [21-24], i.e., densities (d25°) = 0.78657 g . cm-3, (d30°) = 0.7862 g .cm-3, (d35°) = 0.7815 g . cm-3, (d40°) = 0.7765 g . cm-3, respectively, the viscosities (η25°) = 0.5448 x 10-2 P, (η30°) = 0.5030 x 10-2 P and (η35°) = 0.4620 x 10-2 P, (η40°) = 0.4220 x 10-2 P, respectively and the dielectric constants (D25°) = 32.63, (D30°) = 30.68, (D35°) = 29.90, (D40°) = 29.03, respectively.

 

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