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The Electrolytic Dissociation of Aryl Derivatives of Succinic Acid

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^{-3}) solutions was carried out with the aid of a new method of determination of the dissociation parameters of weak multibasic organic acids with the “overlapping equilibria” effect previously described by authors. Values of the usual and “partial” degrees of dissociation, the concentrations of all anions, hydrogen ions and undissociated acid molecules, the activity coefficients of all charged dissociation products were calculated. Together with the accurate equations, the simple empirical equations for fast approximate determination of the various dissociation parameters were also suggested.

KEYWORDS

1. Introduction

Succinic acid and its various derivatives are widely used in the organic synthesis and polymer industry; participate in the biologically important Krebs cycle. Ben- zylsuccinic acid was described to be the most potent inhibitor of carboxypeptidase A. It is a by-product analog and is proposed to bind to the active site of carboxypeptidase A via the succinyl carboxyl group and a carbonyl group. It was established that benzylsuccinic acid was bound at a single locus at the active site of carboxypeptidase A. The useful properties of these acids are directly connected with the peculiarities of their electrolytic dissociation.

Previously we described the original method for determination of various dissociation parameters of weak multibasic organic acids with the close values of stepwise dissociation constants (the effect of “overlapping equilibria”) [1] [2] [3] [4] . This method was widely used for an analysis of various weak organic acids with different basicity in their dilute solutions [5] - [14] . The term of the “partial” degree of dissociation was also suggested [2] and used for a more detailed analysis of the complex equilibria existing in the processes of dissociation of such acids. In this work, our method is applied for the study of the peculiarities of electrolytic dissociation of the aryl derivatives of succinic acid: phenylsuccinic, benzylsuccinic, dibenzylsuccinic and phenyl-2-benzylsuccinic acids in their dilute (0.0001 - 0.01 mol・dm^{-3}) solutions.

2. The Equations

All acids studied in this work are the vivid examples of weak dibasic organic acids with the “overlapping equilibria” effect. This fact is confirmed by the values of the dissociation constants of these acids presented in Table 1.

The law of dilution equations for weak dibasic organic acid with the effect of “overlapping equilibria” may be expressed as follows [1] [2] [3] [4] :

(1)

(2)

where K_{1} and K_{2} are the thermodynamic dissociation constants for first and second steps, α_{1} and α_{2} are the usual degrees of dissociation for corresponding steps, is the “partial” degree of dissociation for the second step, x_{1} and x_{2} are the contributions of first and second steps to the [H^{+}] value ([H^{+}] = x_{1} + x_{2}), c is the total (analytical) concentration of acid, F_{1} and F_{2} are the quotients of the activity coefficients:

(3)

(4)

The α_{1}, α_{2}, , x_{1} and x_{2} values are connected by the following equation:

(5)

(6)

(7)

Table 1. The dissociation constants of aryl derivatives of succinic acid.

The concentrations of hydrogen ions, mono and dianions and undissociated acid molecules can be expressed as follows:

(8)

(9)

(10)

(11)

The values of the activity coefficients can be approximated by the Debye- Huckel equation:

(12)

where a_{i} is the cation-anion distance of closest approach, A and B are constants depending on the properties of water at given temperature, z_{i} is the charge of ion. The ionic strength. The values of a_{i}, A and B at 25˚C were taken from [17] , the a_{i} values for studied acids were estimated according to the data also presented in [17] . The activity coefficient of undissociated acid is assumed to be unity. The values of the dissociation constants presented in Table 1 were used in calculations.

According to the Equations ((1) and (2)), the α_{1}, α_{2}, , x_{1} and x_{2} values can be evaluated successively by iterative solution of following equations:

(13)

(14)

(15)

(16)

(17)

When the [H^{+}] value is known, these parameters may be calculated with the aid of the following equations:

(18)

(19)

(20)

(21)

(22)

3. Results and Discussion

In Tables 2-5, the values of the usual and “partial” degrees of dissociation and pH for the dilute (0.0001 - 0.01 mol∙dm^{-3}) solutions of the studied aryl derivatives of succinic acid are presented. The corresponding x_{1} and x_{2} values may be determined with the aid of the Equations ((6) and (7)).

The comparison of the α_{2} and values show that the values of the “partial” degree of dissociation (which more correctly characterize the completeness of dissociation at second step) exceed appreciably the values of the usual degree of dissociation (especially in case of the low K_{1} values and higher acid concentrations).

The values of the activity coefficients of hydrogen ions and mono and dianions determined by the Debye-Huckel equation change within the following limits in the acid concentration interval 0.0001 - 0.01 mol・dm^{-3}: 0.9911 - 0.9223 (H^{+} ion), 0.9909 - 0.9118 (monoanion); 0.9643 - 0.7007 (dianion).

The Equations (8)-(11) give the opportunity to determine the regions of the acid concentration in which the various charged and uncharged forms of acid prevail. The conditions of equality of the concentrations of these particles are:

Table 2. The values of the dissociation parameters for the dilute solutions of methylsuccinic acid at 25˚C.

Table 3. The values of the dissociation parameters for the dilute solutions of benzylsuccinic acid at 25˚C.

Table 4. The values of the dissociation parameters for the dilute solutions of dibenzylsuccinic acid at 20˚C.

Table 5. The values of the dissociation parameters for the dilute solutions of 2-phenyl- 2-benzylsuccinic acid at 25˚C.

(23)

(24)

(25)

(26)

(27)

(28)

(29)

(30)

(31)

The calculations show that the monoanion concentration exceeds the [H_{2}A] value when c ≤ 0.0002 mol・dm^{-3} (benzyl and dibenzylsuccinic acids), c ≤ 0.0003 mol・dm^{-3} (phenylsuccinic acid) and c ≤ 0.0004 mol・dm^{-3} (2-phenyl-2-benzylsuccinic

acid). In all these cases the inequalities:, and are fulfilled. The regions of prevailing [H^{+}] values in comparison with the [H_{2}A] values are: c < 0.0002 mol・dm^{-3} (benzyl and dibenzylsuccinic acids) and c ≤ 0.0004 mol・dm^{-3} (phenyl and 2-phenyl-2-benzylsuccinic acid). In all these cases, the inequalities, and are fulfilled.

4. The Empirical Equations

In conclusion, taking into account the comparatively complexity of the calculations with the aid of the Equations (13)-(22), we suggest also the simple empirical equations for fast approximate determination of the values of usual and “partial” degrees of dissociation and pH in the dilute solutions of all studied derivatives of succinic acid.

Phenylsuccinic acid

(32)

(up to c = 0.001 mol・dm^{-3})

(33)

(up to c = 0.01 mol・dm^{-3})

(34)

(up to c = 0.002 mol・dm^{-3})

(35)

(up to c = 0.01 mol・dm^{-3})

Benzylsuccinic acid

(36)

(up to c = 0.002 mol・dm^{-3})

(37)

(up to c = 0.01 mol・dm^{-3})

(38)

(up to c = 0.002 mol・dm^{-3})

(39)

(up to c = 0.01 mol・dm^{-3})

Dibenzylsuccinic acid

(40)

(up to c = 0.001 mol・dm^{-3})

(41)

(up to c = 0.01 mol・dm^{-3})

(42)

(up to c = 0.001 mol・dm^{-3})

(43)

(up to c = 0.01 mol・dm^{-3})

2-Phenyl-2-benzylsuccinic acid

(44)

(up to c = 0.001 mol・dm^{-3})

(45)

(up to c = 0.01 mol・dm^{-3})

(46)

(up to c = 0.001 mol・dm^{-3})

(47)

(up to c = 0.01 mol・dm^{-3})

For all described empirical equations the values of the relative error do not exceed 5% - 7% (the relative error is the ratio of the difference between the approximate and accurate values, divided by the approximate value, and converted to percent).

In [18] , we considered also the possibility of obtaining of the general empirical equations for α_{1}, α_{2} and pH values in which these parameters were connected with the dissociation constants and acid concentration. Such equations were obtained as a result of the investigation of dependence of the constants of empirical equations on the dissociation constants values of various weak dibasic organic acids.

For the α_{1} value we suggest two general empirical equations. The first equation corresponds to the pK_{1} values range 2.5 - 3.75:

(48)

For the pK_{1} values range 3.8 - 4.7, we suggest the following equation:

(49)

The pK_{1} values of the studied in this work derivatives of succinic acid are within the range 3.54 - 3.69 (2-phenyl-2-benzylsuccinic acid) and 3.77 - 4.13 (phenyl, benzyl and dibenzylsuccinic acids). Consequently, corresponding calculations were carried out using both general Equations (48) and (49). Our calculations show that Equations ((48) and (49)) can be used (taking into account the pK_{1} values) in the following concentration interval: c = 0.0001 - 0.01 mol・dm^{-3}.

For the pH values of the dilute solutions of the aryl derivatives of succinic acid can be used suggested by us following general empirical equation:

(50)

This equation may be used in all studied interval of the acid concentration. For all acids the values of relative error in this interval do not exceed 5%.

For the α_{2} value we suggest the following general empirical equation:

(51)

where m values for studied acids are within the range 0.16603 - 0.17954. This equation may be used in the concentration interval c = 0.0001 - 0.001 mol・dm^{-3} (dibenzyl and 2-phenyl-2-benzyl derivatives) and in all studied concentration interval in case of phenyl and benzyl derivatives. In all these cases the values of the relative error do not exceed 14%.

5. Conclusion

With the aid of the method previously described by the authors, an analysis of the regularities of electrolytic dissociation of the aryl derivatives of succinic acid: phenylsuccinic, benzylsuccinic, dibenzylsuccinic and phenyl-2-benzylsuccinic acids was carried out. Values of the degrees of dissociation of both steps, the “partial” degrees of dissociation of second step, concentrations of hydrogen ion, monoanion and dianion and undissociated acid were determined for the dilute (0.0001 - 0.01 mol・dm^{-3}) solutions of above mentioned acids. The concentration intervals of domination of various charged and uncharged forms of these acids were established. Simple empirical equations were suggested for the fast approximate calculation of α_{1}, α_{2}, and pH values for all studied acids.

Conflicts of Interest

The authors declare no conflicts of interest.

Cite this paper

*Journal of Biomedical Science and Engineering*,

**10**, 163-171. doi: 10.4236/jbise.2017.104013.

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