General analytical procedure for determination of acidity parameters of weak acids and bases.

The paper presents a new convenient, inexpensive, and reagent-saving general methodology for the determination of pK a values for components of the mixture of diverse chemical classes weak organic acids and bases in water solution, without the need to separate individual analytes. The data obtained from simple pH-metric microtitrations are numerically processed into reliable pK a values for each component of the mixture. Excellent agreement has been obtained between the determined pK a values and the reference literature data for compounds studied.

1. Introduction

Prediction or determination of pK a value is of great importance in chemistry, in particular in life and material sciences, pharmaceutical industry, and other R&D oriented enterprises. Important drug properties, such as lipophilicity, solubility, and transmembrane transfer, are all pH dependent. Also, rational drug formulation requires the knowledge of pK a. The proportion of drugs with an ionizable group has been estimated at 95% [1], but only 62.9% of drugs under analysis were ionizable at pH 2–12 [2]. According to Wells data 75% of drugs are weak bases and 20% weak acids and the remaining contain nonionics, ampholytes, and alcohols [1].

Recently, some theoretical approaches were employed to predict the pK a value, for example, ab initio quantum mechanical calculations [3, 4] or QSPR (quantitative structure-property relationship) modeling [5, 6] as well as QSPR models which employ partial atomic charges as descriptors [7, 8]. The theoretical models take into account electronic effects (induction, resonance), solvation of compounds of type HA, BH and their ionic forms, that is, A− and BH+, hydrogen bonding, and various stereochemical effects.

This report presents an application of pH-metric microtitration to determine standard pK a parameters of components of mixtures of various weak acids and bases by employing a technologically advanced potentiometer device and a software based on an algorithm straightforwardly accounting for complex acid-base equilibria (see below). A composition of the mixtures under study can be expressed as follows: where H3A1 + H2A2 + HA3 represents 3-H, 2-H, and 1-H protic carboxylic acids, B1 + B2 represents organic bases, (R1R2)CH2 represents the so-called C–H acids, R1R2N–H– represents the N–H acids, and ArOH denotes phenolic/enolic moiety (O–H acids). The C–H, N–H, and O–H acids are often reported as tautomeric forms of heterocyclic compounds with pharmacological activity and are identified within different groups of natural compounds (flavonoids, quinines, etc.).

Numerical Modelling. Numerical procedures are based on an original algorithm elaborated by Kostrowicki and Liwo [9] as well as the CVEQUID program, which was adopted in the Cerko Lab software within the Cerko Lab System microtitrator unit (Cerko, Gdynia, Poland). All details concerning Kostrowicki and Liwo algorithm were described previously [10]. The CVEQUID program is based on a least-square method for the determination of all parameters and takes into account all the sources of experimental errors considered in potentiometry, that is,

electrode calibration parameters (E 0, the standard potential (cell constant) and S, the standard Nernstian slope parameter);

composition of titrand D, its concentration C 0 (mol/L), and volume V 0 (mL);

composition of titrant T, its concentration (mol/L), and added volume (mL);

measured EMF (the electromotive force) in mV.

Within the Cerko Lab System software, the equilibrium is denoted as model. The model consists of a set of equations. Each equation is related to a particular pK value and to pK w. The model includes also information about the composition of titrant T and titrand D. The stoichiometric matrix, required for the numerical procedures, is generated from the model automatically. The representative models and the corresponding stoichiometric matrix for H2A (model 1) as well as H3A + H2A1 + HA2 (model 2) systems are given below.

Model 1. Reagents include titrand D = H2A and titrant T = OH. Individual equilibria that contribute to the overall equilibrium of the system are as follows:

H2A = H+1 + HA−1,  K 1 = [H+1][HA−1]/[H2A],

HA−1 = H+ + A−2,  K 2 = [H+1][A−2]/[HA−1],

0 = H+1 + OH−1,  K w = K[H2O] = [H+1][OH−1].

The stoichiometric matrix for the above model is presented in Table 1.

Table 1

Stoichiometric matrix for model 1.

	H+1	H2A	HA−1	A−2	OH−1
pK 1	1	−1	1	0	0
pK 2	1	0	−1	1	0
pK w	1	0	0	0	1

0 denotes a species that does not take part in equilibrium; −1 donates substrate (left side of equilibria equation); 1 donates product (right side of equilibria equation).

The concentration of titrand, D (C 0 = C 01 + C 02 + C 03⋯), and titrand volume (V 0 = V 01+ V 02 + V 03⋯), used in the potentiometric titration, result from mixing of various types of acid-base solutions.

Model 2. Reagents include titrand D = H3A + H2A1 + HA2 and titrant T = OH (Table 2). The model consists of a water solution of different types of acids. The equilibrium constants and stoichiometric matrix are as follows:

Table 2

Stoichiometric matrix for model 2.

	H+1	H3A	H2A−1	HA−2	A−3	H2A1	HA1 −1	A1 −2	HA2	A2 −1	OH−1
pK 1A	1	−1	1	0	0	0	0	0	0	0	0
pK 2A	1	0	−1	1	0	0	0	0	0	0	0
pK 3A	1	0	0	−1	1	0	0	0	0	0	0
pK 1A1	1	0	0	0	0	−1	1	0	0	0	0
pK 2A1	1	0	0	0	0	0	−1	1	0	0	0
pK 1A2	1	0	0	0	0	0	0	0	−1	1	0
pK w	1	0	0	0	0	0	0	0	0	0	1

H3A = H+1 + H2A−1,  K 1A = [H+1][H2A−1]/[H3A],

H2A−1 = H+1 + HA−2,  K 2A = [H+1][HA−2]/[H2A−1],

HA−2 = H+ + A−3,  K 3A = [H+1][A−3]/[HA−2],

H2A1 = H+1 + HA1 −1,  K 1A = [H+1][HA1 −1]/[H2A1],

HA1 −1 = H+ + A1 −2,  K 2A = [H+1][A1 −2]/[HA1 −1],

HA2 = H+1 + A2 −1,  K 1A = [H+1][A2 −1]/[HA2],

0 = H+1 + OH−1,  K w = K[H2O] = [H+1][OH−1].

General Model. Reagents include titrand D  =  H3A + H2A1 + HA2+ B + B1+ (R1R2)CH2 + R1R2NH+ Ar-OH + nHX (HX  as  a  strong  mineral  acid)…, and titrant T = OH. The presence of a strong mineral acid causes transformation of all the basic reagents into an acidic form—conjugate acid of amine.

The model consists of a water solution of different types of acids, bases, C–H, N–H, and O–H acids. The existing equilibria in solution are given below:

H3A = H+1 + H2A−1,  K 1A = [H+1][H2A−1]/[H3A],

H2A−1 = H+1 + HA−2,  K 2A = [H+1][HA−2]/[H2A−1],

HA−2 = H+ + A−3,  K 3A = [H+1][A−3]/[HA−2],

H2A1 = H+1 + HA1 −1,  K 1A = [H+1][HA1 −1]/[H2A1],

HA1 −1 = H+ + A1 −2,  K 2A = [H+1][A1 −2]/[HA1 −1],

HA2 = H+1 + A2 −1,  K 1A = [H+1][A2 −1]/[HA2],

BH+1 = H+1 + B,  K BH = [H+1][B]/[BH+1],

(R1R2)CH2 = H+1 + R1R2CH−1,  K (R = [H+1][(R1R2)CH−1]/[(R1R2)CH2],

see Scheme 1,

Scheme 1

ArOH = H+1 + ArO−1,  K OH = [H+1][ArO−1]/[ArOH],

H2O = H+1 + OH−1,  K w = K[H2O] = [H+1][OH−1].

2. Experimental

2.1. Apparatus and Reagents

The pH-metric titrations were performed in a 30 mL thermostated (25.0 ± 0.2°C) cell, using a Cerko Lab microtitration unit, fitted with a pH electrode (Hydromet ERH-13-6). The temperature was controlled using the Lauda E100 circulation thermostat. The electrode was calibrated with the use of buffer solutions: potassium hydrogen phthalate (pH 4.00), citric acid/Na2HPO4 (pH 7.00), and boric acid/KCl/NaOH (pH 10.00).

Titrant T (0.1 mol/L NaOH) was standardized according to the general analytical procedure and protected from carbon dioxide. Double distilled water of conductivity approximately 0.18 μS/cm was used throughout for the preparation of aqueous solutions of organic acids and bases under study. It was freshly produced in order to avoid carbon dioxide absorption. Other reagents together with their abbreviations used in the text are listed in Abbreviations section.

2.2. Analytical Procedure

Volume V 0 of 4.0 mL to 5.0 mL of titrand (D) was titrated with 0.1 mol·L−1 of titrant (T) using a Cerko Lab System, equipped with a syringe pump. Titrant (T) was added to titrand (D) in increments of 0.01 mL, with a pause of 7 s. The pK a values were calculated from the experimental data points {(V , pH)∣j = 1,…, N} according to the Kostrowicki and Liwo algorithm [9, 10].

3. Results and Discussion

3.1. Carboxylic Acids Mixture

The representative pH titration curves for the mixture of carboxylic acids PhA : Py-4CA : MA are presented in Figures 1 and 2. Compositions of titrand D for the mixture (PhA : Py-4CA : MA) were as follows: 1 : 1 : 1, 1 : 2 : 1, 1 : 2 : 2, and 1 : 1 : 1 with 0.5 mole ratio of HCl. The titration and fitted curves pH = f(V NaOH) obtained for mixture with molar ratio of the components 1 : 2 : 2 (PhA : Py-4CA : MA) are shown in Figure 2. The pK a data determined for the mixtures of carboxylic acids under study are listed in Tables 3 and 4.

Figure 1

Titration curves pH = f(V NaOH) obtained for the mixture of PhA, Py4CA, and MA with different mole ratio of acids and with excess of HCl.

Figure 2

Titration and fitted curves pH = f(V NaOH) obtained for mixture of PhA, Py-4CA, and MA with mole ratio of acids 1 : 2 : 2.

Table 3

The experimental pK a data obtained for the mixture of PhA, Py4CA, and MA at various compositions of titrand D.

Composition of D	pK n	pK aPhA ± s	pK aPy4CA ± s	pK aMA ± s
PhA + Py4CA + MA(1 : 1 : 1)	pK 1	2.97 ± 0.07	—	3.30 ± 0.03
	pK 2	5.31 ± 0.04	4.69 ± 0.03	—
PhA + Py4CA + MA(1 : 2 : 2)	pK 1	2.81 ± 0.06	—	3.12 ± 0.03
	pK 2	5.45 ± 0.03	4.71 ± 0.01	—
PhA + Py4CA + MA(1 : 2 : 1)	pK 1	2.78 ± 0.04	4.76 ± 0.02	3.4*
	pK 2	5.53 ± 0.04

  *pK a value const. taken from the literature [see Table 11].

Table 4

The experimental pK a data obtained for the mixture of A + MA + PhA + Py3CA and 2,6PyDCA + Py3CA.

Composition of D	pK n	pK aPhA ± s	pK aPy3CA ± s	pK aMA ± s	pK aA ± s
A + MA + PhA + Py3CA	pK 1	3.11 ± 0.05	—	3.74 ± 0.03	4.68 ± 0.02
	pK 2	5.62 ± 0.03	4.82*	—	—
Composition of D	pK n	pK a2,6PyDCA ± s	pK aPy3CA ± s	—	—
2,6PyDCA + Py3CA	pK 1	2.41 ± 0.04	—	—	—
	pK 2	4.72 ± 0.02	5.19 ± 0.04	—	—
Composition of D	pK n	pK aPhA ± s	pK aPy3CA ± s	pK aCA ± s	—
PhA + Py3CA + CA	pK 1	3.12 ± 0.03	—	3.04 ± 0.03	—
	pK 2	5.53 ± 0.03	4.82*	4.46 ± 0.05	—
	pK 3	—	—	6.05 ± 0.04	—

  *pK a value const. from the literature [see Table 11].

3.2. Organic Bases in Protonated Form (Cationic Acids)

The amino group is one of the most fundamental functional groups considered in organic and pharmaceutical chemistry and its pK a is an important and extensively studied property. The pK a value of the amino group can vary over several orders of magnitude (ammonia, pK a = 9.26; aniline, pK a = 4.63 [11]), depending on its chemical environment. In our study the pK a refers to the conjugate acid B + H+1 = BH+1 and dissociation according to the scheme: BH+1 = B + H+1.

We have tested a mixture of organic bases exemplified by aniline and pyridine derivatives (2- and 4-substituted aminopyridines and methylpyridine) at the presence of equimolar ratio of HCl. Organic bases exist in the system in the protonated form (cationic acids, BH+1) and dissociate according to the scheme: BH+1 = B + H+1, K BH + = [B][H+1]/[BH+1].

Based on the titration curve of mixture of amines (presented in the form of cationic acids), the pK a values were determined for aniline (B) and for 2- and 4-aminopyridine (2-NH2Py, 4-NH2Py). The heterocyclic five-membered ring systems of imidazole (Im), benzotriazole (Bt), and benzimidazole (Bi) were also investigated. We have applied a general procedure for the titration of mixtures of different types (and concentration) of organic acids and bases. The elaborated procedure was also tested in the presence of biological buffers exemplified by 2-(N-morpholino) ethane-sulfonic acid (Mes) [12].

The values of dissociation constants obtained for mixtures of different type of bases and acids are listed in Tables 5 and 6.

Table 5

The pK a's values of compounds determined in the multicomponent mixture of amines, heterocyclic moiety, and weak (Mes) and strong (HCl) acids at 25°C.

Composition of D	pK A ± s	pK 4NH2Py ± s	pK 2NH2Py ± s	pK FA ± s
A+ HCl	4.650 ± 0.02	—	—	—
A + 4NH2Py + HCl	4.53 ± 0.04	9.27 ± 0.18	—	—
A + 4NH2Py + 2NH2Py + HCl	5.13 ± 0.07	9.59 ± 0.07	7.18 ± 0.07	—
A + 2NH2Py + FA	4.7*	—	6.7*	3.05 ± 0.04
				4.26 ± 0.02
Composition of D	pK Mes ± s	pK 2NH2Py ± s	pK Py3CA ± s	pK Bt ± s
			or pK Py4CA ± s	or pK Bi ± s
Mes + Bt	6.24 ± 0.05	—	—	8.75 ± 0.59
Mes + 2NH2Py + Bi + HCl	6.28 ± 0.05	7.22 ± 0.05	—	5.36 ± 0.04
Mes + 2NH2Py + Py3CA	6.29 ± 0.03	7.22 ± 0.03	4.78 ± 0.03	—
Mes + 2NH2Py + Py4CA	6.29 ± 0.34	6.39 ± 0.34	4.76 ± 0.30	—
Composition of D	pK ASA ± s	pK 2NH2Py ± s	pK Py3CA ± s	pK AA ± s
				or pK 3MePy
ASA + Py3CA + AA	3.66 ± 0.05	—	5.02 ± 0.04	4.15 ± 0.05
ASA + 2NH2Py + 3MePy	3.61 ± 0.03	7.02 ± 0.03	—	5.82 ± 0.03

  *pK a value const. from the literature [see Table 11].

Table 6

The pK a's values of compounds determined in the mixture containing four-weak electrolytes (acids and bases) and a strong acid (HCl) at 25°C.

Composition of D	pK n	pK PhA ± s	pK MA ± s	pK Py3CA ± s	pK A ± s
PhA + MA + Py3CA + A + HCl	pK 1	3.11 ± 0.05	3.74 ± 0.03	4.8*	4.68 ± 0.02
	pK 2	5.62 ± 0.03	—	—	—
Composition of D	pK n	pK AA ± s	pK Bi ± s	pK ImH ± s	pK BtH ± s
AA + Bi + ImH + BtH + HCl	pK 1	4.29 ± 0.13	5.98 ± 0.14	7.55 ± 0.14	9.19 ± 0.14

  *pK a value const. from the literature [see Table 11].

3.3. Mixtures of Amino acids with Organic Acids and Bases

The presented general procedure was applied for studying the system consisting of amino acids, organic acids, and bases. The pK a values of this type of mixtures were calculated based on a single titration curve. Experimental results confirm the general application of the proposed procedure for the determination of pK a value for mixtures of any degree of complexity composed of weak acids and bases. The pK a values of weak acids (HA), bases (B), and amino acids (AB±) in the mixture of these types of components were determined. Composition of the tested mixtures (titrand D) and pK a values are listed in Table 7.

Table 7

The pK a's values of compounds determined in the multicomponent mixture of amino acid, heterocyclic moiety, and weak (Mes) and strong (HCl) acids at 25°C.

Composition of D	pK n	pK His ± s	pK Py3CA	pK Mes	pK ImH
L-His	pK 3	9.67 ± 0.01	—	—	—
L-His + HCl (1 : 1)	pK 2	6.28 ± 0.01	—	—	—
	pK 3	9.97 ± 0.01	—	—	—
L-His + HCl (1 : 2)	pK 1	1.54 ± 0.04	—	—	—
	pK 2	6.26 ± 0.01	—	—	—
	pK 2	9.66 ± 0.01	—	—	—
L-His + Py3CA++ Mes + ImH	pK 1	—	—	6.28*	7.56*
	pK 2	6.28*	4.68 ± 0.24	—	—
	pK 3	10.06 ± 0.55	—	—	—
L-His + Py3CA ++ Mes + ImH + HCl	pK 1	—	4.81 ± 0.28	6.07 ± 0.14	7.49 ± 0.05
	pK 2	6.43 ± 0.74	—	—	—
	pK 3	10.06 ± 0.37	—	—	—
Composition of D	pK n	pK Ala	—	—	—
L-Ala	pK 2	10.30 ± 0.01	—	—	—
L-Ala + HCl (1 : 1)	pK 1	2.25 ± 0.01	—	—	—
	pK 2	10.25 (0.07)	—	—	—

  *pK a value const. from the literature [see Table 11].

3.4. Phenol and Enol OH-Acids as Components of Titrand D

The acidity of the phenol group (OH-acid) depends on the substituent of the aromatic ring and its pK a ranges from 4 to 11 [8]. We have performed the titration and relevant calculations for several mixtures of phenolic compounds, exemplified by 4-NO2 phenol and a drug N-(4-hydroxyphenyl)acetamide (paracetamol) with different type of organic acids and bases as titrands D. The results are summarised in Table 8.

Table 8

The pK a's values of compounds determined in the multicomponent mixture of phenol and enol OH–acids together with other weak electrolytes at 25°C.

Composition of D	pK A ± s	pK FA ± s	pK 4NO2PhOH ± s	—
A + FA + 4NO2PhOH	4.87 ± 0.02	3.05 ± 0.034.06 ± 0.03	7.42 ± 0.04	—
Composition of D	pK MAL ± s	pK FA ± s	pK 4NO2PhOH ± s	—
FA + MAL + 4NO2PhOH	3.59 ± 0.045.14 ± 0.02	2.50 ± 0.044.06 ± 0.04	7.4 ± 0.03	—
Composition of D	pK AA ± s	pK Mes ± s	pK Pcm ± s	—
AA + Mes + Pcm	4.14 ± 0.03	6.24 ± 0.04	9.95 ± 0.05	—
Composition of D	pK ASA ± s	pK FA ± s	pK 4NO2PhOH ± s	pK Kpf
ASA + FA + 4NO2PhOH + Kpf	3.77 ± 0.05	2.91 ± 0.064.75 ± 0.37	7.52 ± 0.05	4.68 ± 0.36

3.5. Heterocyclic N–H-Acids as Components of Titrand D

The barbituric acid (BA) and a new class of 2(1H)-pyrazylidene acetonitrile derivatives (2(1H)PyAN), with marked pharmaceutical importance [13, 14], were tested at the presence of phthalic acid. Barbituric acid was also tested at the presence of different drugs (Table 9).

Table 9

The pK a's values of compounds determined in the multicomponent mixture which comprises barbituric acid, 2(1H)-pyrazylidene acetonitrile, and phthalic acid at 25°C.

Composition of D	pK n	pK 2(1H)PyAN ± s	pK BA ± s	pK PhA ± s
2(1H)PyAN + BA + PhA	pK 1	7.10 ± 0.09	4.01 ± 0.04	2.39 ± 0.08
	pK 2	—	—	5.76 ± 0.05

3.6. Determination of pK a Values for Different Drugs as a Components of Titrand D

For all tested compounds with pharmaceutical importance we confirmed that the elaborated method could be recommended as a general approach to the determination of pK a values for weak acids and bases in mixtures of any degree of complexity. The composition of titrand D and the pK a values determined for drugs under study are listed in Table 10.

Table 10

The pK a's values of compounds with pharmaceutical importance determined in the mixture containing other weak electrolytes 25°C.

Composition of D	pK AA ± s	pK Mes ± s	pK Pcm ± s	pK ASA	pK CA
AA + Mes + Pcm	4.14 ± 0.03	6.24 ± 0.04	9.95 ± 0.05	—	—
Composition of D	pK ASA ± s	pK ImH ± s	pK Eph ± s	—	—
ASA + ImH + Eph ∗ HCl	3.49 ± 0.03	7.21 ± 0.06	9.94 ± 0.05	—	—
Composition of D	pK Met ± s	pK ImH ± s	pK Mes ± s	—	—
Met + ImH + Mes	2.28 ± 0.04	7.35 ± 0.02	6.19 ± 0.01	—	—
Composition of D	pK ASA ± s	pK Mes ± s	pK L-His ± s	—	—
ASA + Mes + L-His	3.57 ± 0.03	6.29 ± 0.03	pK 1L-His  =  1.54*  pK 2L-His  =  5.96 ± 0.05pK 3L-His  =  9.67 ± 0.59	—	—
Composition of D	pK KTL ± s	pK Mes ± s	pK L-His ± s	—	—
KTL + Mes + L-His	pK 1 3.09 ± 0.05pK 2 6.15*	6.15*	pK 2L-His  =  6.15*  pK 3L-His  =  9.58 ± 0.06	—	—
Composition of D	pK AA ± s	pK Mes ± s	pK Ppv ± s	pK ASA	pK CA
AA + Mes + Ppv	4.24 ± 0.02	6.55 ± 0.03	6.02 ± 0.06	—	—
AA + Mes + ASA + CA	4.05 ± 0.16	—	—	3.90 ± 0.16	pK 1 = 2.53 ± 0.30pK 2 = 5.03 ± 0.33pK 3 = 6.5 ± 0.34

  *pK a value const. from the literature [see Table 11].

4. Conclusions

A new approach for studying equilibrium constants for the dissociation of different types of weak electrolytes present in a mixture of any degree of complexity has been proposed. Potentiometric titration technique and numerical procedure based on an original algorithm elaborated by Kostrowicki and Liwo and adopted in the Cerko Lab software have successfully been applied to obtain the pK a values of a variety of classes of compounds comprising of common organic acids and bases, amino acids, phenols and enols OH-acids, and heterocyclic N–H-acids as well as compounds of pharmaceutical importance. It was shown that the pK a values of the compound present in the mixture can be determined directly without the need to separate individual analytes. The obtained pK a values of the electrolytes under study are in a good agreement with those reported in the literature (Table 11, Figure 3). Thus, the presented methodology can be considered as a fast, simple, inexpensive, and reagents-saving way for studying equilibria in the mixture of electrolytes. Moreover, it does not require a highly trained personnel. The methodology described in this paper can be routinely used in a regular analytical practice.

Table 11

Experimental and literature pK a's values of the compounds under study.

No.	Compounds	pK exp⁡ *	pK literature	Reference
1	A	4.81	4.55–4.78	[11]
2	AA	4.17	4.10	[15]
3	ASA	3.67	3.30–3.74	[16]
4	BA	4.01	4.02	[17]
5	Bi	5.98	5.66	[18]
6	CA	2.53 5.03 6.50	3.134.766.40	[19]
7	Eph	9.94	9.56	[20]
8	FA	2.88 4.28	3.024.39	[21]
9	Im	7.43	6.95	[22]
10	KTL	3.09 6.15	2.90–3.296.39	[16]
11	Ktp	4.68	4.6	[23]
12	L-ala	2.25 10.28	2.26–2.549.7–9.9	[18]
13	L-his	1.67 6.22 9.79	1.546.079.34	[22]
14	MA	3.48	3.18–3.41	[18]
15	3-MePy	5.82	5.61–6.02	[18]
16	MAL	3.595.14	3.11–3.304.46–5.12	[18]
17	Mes	6.27	6.27	[22]
18	Met	2.28	2.38	[16]
19	2-NH2Py	7.04	6.72–6.76	[16]
20	4-NH2Py	9.43	9.02–9.29	[16]
21	4-NO2PhOH	7.44	7.02–7.15	[11]
22	PhA	2.86 5.53	2.955.41	[22]
23	Ppv	6.02	6.21–6.49	[16]
24	2(1H)PyAN	7.10	—	—
25	Py-3CA	4.85	4.82	[24]
26	Py-4CA	4.72	4.84	[24]
27	2.6-PyDCA	2.41 4.72	2.00–3.454.47–4.87	[18]

  *pK exp calculated as ∑pK /n.

Figure 3

Plot of experimental versus literature pK a's values for the compounds under study.