T. V.
Volkova
a,
I. V.
Terekhova
a,
O. I.
Silyukov
a,
A. N.
Proshin
b,
A.
Bauer-Brandl
c and
G. L.
Perlovich
*a
aDepartment of Physical Chemistry of Drugs, Krestov's Institute of Solution Chemistry, Russian Academy of Sciences, 153045 Akademicheskaya str. 1, Ivanovo, Russia. E-mail: glp@isc-ras.ru
bInstitute of Physiologically Active Compounds, Russian Academy of Sciences, 142432, Chernogolovka, Russia
cDepartment of Physics, Chemistry and Pharmacy, University of Southern Denmark, 5230 Odense M, Denmark
First published on 28th October 2016
Novel 1,2,4-thiadiazole derivatives as potent neuroprotectors were synthesized and identified. Their ability to inhibit the glutamate stimulated Ca2+ uptake was investigated. The solubility of thiadiazoles was measured in a buffer solution (pH 7.4) at 298 K. The distribution coefficients in 1-octanol/buffer (pH 7.4) and 1-hexane/buffer (pH 7.4) immiscible phases as model systems imitating the gastrointestinal tract epithelium and the blood–brain barrier were determined. Permeation experiments the new Permeapad™ barrier using Franz diffusion cells were conducted and the apparent permeability coefficients were obtained. The influence of the compound structure on the physicochemical properties determining the bioavailability of drug-like substances was revealed. Solubility–permeability interplay has been assessed to evaluate potential bioavailability of the compounds studied.
The 1,2,4-thiadiazole derivatives are well known to have biologically active groups to specifically target different pathologies. Many of them reveal a wide spectrum of biological activity including antioxidant and neuroprotective ones.3–6 Analysis of the influence of 1,2,4-thiadiazole derivatives on the glutamate-induced calcium ion uptake into synaptosomes of the rat brain cortex is often used for primary evaluation of the biological activity of newly synthesized drug compounds.7 The glutamate receptors in the central nervous system are known to play an important role both in regular neurophysiological processes and pathogenesis of a series of neurodegenerative diseases.8 In this connection, the evaluation of a compound's ability to affect the calcium channels mediated by the glutamate receptors allows one to assess its common biological potential as a possible neuroprotector (in the case of inhibition) or activator of cognition functions (in the case of activation). Members of a newly discovered class of compounds, ampakines, boost the activity of glutamate and thus make it easier to form memories. The cognition enhancers work on the neural processes that underlie such mental activities as attention, perception, learning, memory, language, planning and decision-making, usually by altering the balance of the chemical neurotransmitters involved in these processes. At present, nootropics and some neuronotrophic agents represent the available approaches to symptomatic treatment of Alzheimer's disease.9 Attempts to improve cognitive function in patients with brain disorders have become the focus of intensive research efforts.10 The task of developing guidelines for creating effective modulators of brain cognitive functions based on the derivatives of 1,2,4-thiadiazole is relevant from the perspective of the creation of a new class of effective drugs for the treatment of Alzheimer's disease.
Lipophilicity is a property that has a major effect on in vivo processes of absorption, distribution, metabolism, excretion, and toxicity (ADMET) properties as well as pharmacological activity.11 The partition coefficient is accepted by most scientists to be one of the most relevant lipophilicity descriptors applied in pharmaceutical research.12 It can be measured by a rather simple experiment or calculated. Lipophilicity has been correlated to many other properties, such as solubility, permeability, metabolism, toxicity, protein binding, and distribution. 1-Octanol is the preferred organic solvent for phase-distribution investigations or partition coefficient determination of drugs. The 1-octanol/water partition coefficient is reported in drug handbooks and is commonly used in various types of analysis of drug properties.13 The logD7.4 (logDoct/buf in the present study) of a compound stands for its distribution coefficient at pH 7.4, and it is considered to be a property of utmost importance because of its high physiological relevance and its resemblance to real biological partitions in the body.14 As it has been emphasized in ref. 15, the implication of logD7.4 for drug development leads to a general rule for optimal intestinal absorption by passive diffusion permeability after oral dosing. Drug substances should have a moderate logD7.4. Namely, a good balance of permeability and solubility exists when logD7.4 = 0–3. At that, an optimum range for the CNS (central nervous system) narrows to logD7.4 = 1–3. Since all drug compounds for the prevention of Alzheimer's disease need to overcome the blood–brain barrier (BBB), the analysis of drug interactions with these barriers is an important objective in the design of effective drugs. As a rule, the water/alkane systems (usually 1-hexane/water distribution coefficients logDhex/w) are used for BBB simulation. Selecting the alkane phase is dictated by the fact that it is a good description of non-specific interactions occurring between the drug molecules and the rather tight and lipophilic BBB environment. A parameter describing the difference between the distribution coefficients in 1-octanol/water and 1-hexane/water phases is often used to account for specific interactions (donor–acceptor, hydrogen bonding) to drug transport properties.16
In the present study, we propose the synthesis of new 1,2,4-thiadiazole derivatives with different substitutions of the phenyl ring and replacement of the phenyl ring by cyclopropyl and isoxazole substituents. The aim focuses at investigating the biological activity of the synthesized 1,2,4-thiadiazoles and revealing correlations between the structures, solubilities, lipophilicities and membrane permeabilities of the respective substances. The present work is a continuation of our previous attempts to study the passive transport properties of 1,2,4-thiadiazoles17–23 and the relationship between the biological activity and transport characteristics of drugs and drug-like compounds.23,24
5-N-Monoaminosubstituted 5-amino-3-(2-aminopropyl)-[1,2,4]thiadiazoles (f) were synthesized in the following manner:
A solution of 3-amino-5-methylisoxazole (a) (0.01 M) in 10 mL of acetonitrile was added dropwise to a solution of isothiocyanate (0.01 M) in 10 mL of acetonitrile under stirring. At that, the obtained isoxazole thiourea (b) in situ is transformed to a [1,2,4]thiadiazole ring according to Boulton–Katritzky.25 Upon completion of the dropping, the mixture was brought to boiling and left at room temperature until the precipitation of 5-amino-3-(2-oxopropyl)-[1,2,4]thiadiazole (c) occurs. The precipitate was filtered off. If the crystallization did not take place, the reaction mixture was evaporated and the resultant oil was triturated in diethyl ether.
The resulting 5-amino-3-(2-oxopropyl)-[1,2,4]thiadiazole (c) (0.01 M) and primary amine (0.01 M) were dissolved in 10 ml of methanol and left one day at room temperature. The precipitate was filtered off. According to NMR spectroscopy, the imine (d) forming during the reaction was rearranged to the corresponding vinylamine 5-amino-3-(2-amino-1-propenyl)-[1,2,4]thiadiazole (e) which is introduced into the reduction reaction.
The resulting 5-amino-3-(2-amino-1-propenyl)-[1,2,4]thiadiazole (e) (0.01 M) was suspended in 30 mL of methanol, heated to 50 °C. Then sodium borohydride (0.01 M) was added portionwise under vigorous stirring. During the addition of sodium borohydride the precipitate was dissolved. Upon the completion of the reaction, methanol was evaporated, 50 mL of methylene chloride was added and washed with water (2 × 50 mL), and then the organic layer was separated, and dried over sodium sulfate. Sodium sulfate was filtered off, and the filtrate was evaporated to obtain 5-amino-3-(2-hydroxypropyl)-[1,2,4]thiadiazole (f).
NMR 1H [200 MHz] δ: 0.79 (2H, dt, J = 12.0, 21.2 Hz, C(3)H, C(5)H), 1.08 and 1.12 (both s, 6 H, 2 CH3), 1.15 (3H, d, J = 6.6 Hz, CH2CHC3), 1.84 (2H, dd, J = 3.3, 12.6 Hz, C(3)H, C(5)H), 2.84 (1H, dd, J = 6.0, 14.2 Hz, CHCHMe), 2.92 (1H, dd, J = 4.0, 14.2 Hz, CHCHMe), 3.00 (1H, m, C(4)H), 3.42 (1H, m, CH2CMe), 7.17 (1H, dd, J = 2.2, 8.6 Hz, Harom), 7.45 (1H, d, J = 8.6 Hz, Harom), 7.51 (1H, d, J = 2.2 Hz, Harom).
NMR 1H [200 MHz] δ: 0.65 (1H, t, J = 12.0 Hz, CHH), 0.75 (1H, t, J = 12.0 Hz, CHH), 1.00 (6H, s, (CH3)2), 1.06 (3H, d, J = 6.3 Hz, CCH3), 1.10 (6H, s, (CH3)2), 1.71 (2H, dd, J = 3.5, 12.3 Hz, 2CH), 2.31 (3H, s, Ph-CH3), 2.71 (2H, dd, J = 6.3, 14.2 Hz, CH2), 2.89 (1H, tt, J = 3.5, 11.6 Hz, NCH), 3.32 (1H, m, NCH), 7.17 (1H, d, J = 8.4 Hz, Harom), 7.29 (1H, dd, J = 2.2, 8.4 Hz, Harom), 7.71 (1H, d, J = 2.2 Hz, Harom).
NMR 1H [200 MHz,] δ: 0.77 (2H, dt, J = 12.1, 21.0 Hz, C(3)H, C(5)H), 1.06 and 1.14 (12H, c and c, 4 × CH3), 1.15 (3H, d, J = 6.6 Hz, CH2CHC3), 1.81 (2H, dd, J = 3.4, 12.6 Hz, C(3)H, C(5)H), 2.83 (1H, dd, J = 6.0, 14.0 Hz, CHCHMe), 2.97 (1H, dd, J = 4.1, 14.0 Hz, CHCHMe), 3.00 (1H, m, C(4)H), 3.40 (1H, m, CH2CMe), 7.16 (2H, m, Harom), 7.45 (1H, d, J = 8.0 Hz, Harom).
NMR 1H [200 MHz] δ: 0.71 (1H, t, J = 12.0 Hz, CHH), 0.85 (1H, t, J = 12.0 Hz, CHH), 1.12 (6H, s, (CH3)2), 1.14 (3H, d, J = 6.2 Hz, CCH3), 1.19 (6H, s, (CH3)2), 1.85 (2H, dd, J = 3.5, 12.3 Hz, 2CH), 2.32 (3H, s, Ph-CH3), 2.831 (2H, m, CH2), 2.99 (1H, tt, J = 3.5, 11.6 Hz, NCH), 3.41 (1H, m, NCH), 7.17 (2H, m, Harom), 7.52 (1H, s, Harom).
NMR 1H [200 MHz] δ: 0.86 (2H, m, C(3)H, C(5)H), 1.14 and 1.20 (12H, s and s, 4 × CH3), 1.27 (3H, d, J = 6.65 Hz, CH2CHC3), 1.87 (2H, d, J = 12.5 Hz, C(3)H, C(5)H), 2.84 (2H, d, J = 6.5 Hz, C2CHMe), 3.03 (1H, m, C(4)H), 3.45 (1H, m, CH2CMe), 7.40 and 7.50 (4H, d and d, J = 8.4 Hz, Harom).
NMR 1H [200 MHz] δ: 0.71 (2H, m, C(3)H, C(5)H), 1.02, 1.05 (6H, s + s, 2 × CH3), 1.07 (3H, d, J = 6.5 Hz, CH2CHC3), 1.12, 1.14 (6H, s + s, 2 × CH3), 1.75 (2H, dd, J = 3.1, 12.5 Hz, C(3)H, C(5)H), 2.73 (2H, dd, J = 2.3, 6.5 Hz, C2CHMe), 2.91 (1H, m, C(4)H), 3.32 (1H, m, CH2CMe), 7.09 and 7.38 (4H, d + d, J = 8.6 Hz, Harom), 10.56 (1H, br. s, ArNH).
NMR 1H [200 MHz] δ: 0.81 (2H, m, C(3)H, C(5)H), 1.13 and 1.20 (12H, s and s, 2 × CH3), 1.21 (3H, d, J = 6.5 Hz, CH2CHC3), 1.86 (2H, d, J = 12.4 Hz, C(3)H, C(5)H), 2.54 (3H, s, Ph-SCH3), 2.88 (2H, m, C2CHMe), 3.01 (1H, m, C(4)H), 3.47 (1H, m, CH2CMe), 7.01 (2H, m, Harom), 7.34 (2H, m, Harom).
NMR 1H [200 MHz] δ: 0.81 (2H, m, C(3)H, C(5)H), 1.09 and 1.17 (12H, c and c, 4 × CH3), 1.20 (3H, d, J = 6.2 Hz, CH2CHC3), 1.83 (2H, d, J = 12.2 Hz, C(3)H, C(5)H), 2.83 (2H, m, C2CHMe), 2.97 (1H, m, C(4)H), 3.39 (1H, m, CH2CMe), 3.81 (3H, c, Ph-OCH3), 6.73 (2H, m, Harom), 7.29 (2H, m, Harom).
NMR 1H [200 MHz] δ: 0.71 (2H, m, C(3)H, C(5)H), 1.02, 1.04 (12H, s, 4 × CH3), 1.07 (3H, d, J = 6.6 Hz, CH2CHC3), 1.72 (2H, dd, J = 3.0, 12.6 Hz, C(3)H, C(5)H), 2.72 (2H, dd, J = 2.3, 6.6 Hz, C2CHMe), 2.91 (1H, m, C(4)H), 3.34 (1H, m, CH2CMe), 7.04 (2H, t, J = 8.6 Hz, Harom), 7.58 (2H, dd, J = 4.7, 9.1 Hz, Harom).
NMR 1H [200 MHz] δ: 0.74 (2H, m, C(3)H, C(5)H), 1.00 and 1.10 (12H, c and c, 4 × CH3), 1.12 (3H, d, J = 6.2 Hz, CH2CHC3), 1.76 (2H, d, J = 12.2 Hz, C(3)H, C(5)H), 2.33 (1H, s, CCCH3), 2.83 (2H, m, C2CHMe), 3.00 (1H, m, C(4)H), 3.42 (1H, m, CH2CMe), 4.12 (2H, br. s, 2NH), 5.87 (1H, s, CCH).
NMR 1H [200 MHz] δ: 0.76 (6H, m, C(3)H, C(5)H, CH2CH2), 1.07 and 1.13 (12H, c and c, 4 × CH3), 1.13 (3H, d, J = 6.35 Hz, CH2CHC3), 1.79 (2H, m, C(3)H, C(5)H), 2.61 (1H, m, NCH), 2.75 (2H, m, C2CHMe), 2.91 (1H, m, C(4)H), 3.33 (1H, m, CH2CMe), 6.87 (1H, br. s, NH).
NMR 1H [200 MHz] δ: 0.73 (2H, m, C(3)H, C(5)H), 1.02 and 1.05 (12H, c and c, 4 × CH3), 1.08 (3H, d, J = 6.5 Hz, CH2CHC3), 1.72 (2H, dd, J = 3.1, 12.5 Hz, C(3)H, C(5)H), 2.75 (2H, dd, J = 2.3, 6.5 Hz, C2CHMe), 2.91 (1H, m, C(4)H), 3.33 (1H, m, CH2CMe), 7.40 and 7.52 (4H, d and d, J = 8.8 Hz, Harom).
Bidistilled water (with an electrical conductivity of 2.1 μS cm−1) was used for preparation of buffer solutions.
Phosphate buffer pH 7.4 (I = 0.15 mol L−1) for distribution and solubility experiments was prepared by combining a potassium dihydrogen phosphate solution (KH2PO4) (9.1 g in 1 L) and a disodium hydrogen phosphate dodecahydrate solution (Na2HPO4·12H2O) (23.6 g in 1 L).26 The pH values were measured by using a pH meter FG2-Kit (Mettler Toledo, Switzerland) standardized with pH 1.68, 6.86 and 9.22 solutions.
Phosphate buffer saline for permeation experiments was prepared as described in ref. 27 by mixing a 2.5% (weight/volume) sodium dihydrogen phosphate dehydrate solution with a 1.8% (weight/volume) disodium hydrogen phosphate dodecahydrate solution in a ratio of 1 to 4 in order to obtain a 74 mM phosphate solution.
The pH of the solution was measured using a pH meter FG2-Kit (Mettler Toledo, Switzerland) and adjusted to physiologic conditions (pH 7.3–7.4) by the addition of sodium hydroxide. The osmolality of the buffer solution was measured by a Semi-Micro Osmometer K-7400 (Herbert Knauer GmbH, Berlin, Germany) and adjusted to 280–290 mOsm by the addition of NaCl.
Permeapad™ barrier was prepared according to the description of di Cagno and Bauer-Brandl.27 In brief, a thin layer of phosphatidylcholine (S-100) was applied on a support sheet (Pütz GmbH, Taunusstein, Germany). The final barrier was composed of a support layer and a dried layer of lipid. The final barrier appears mechanically flexible and resistant, and can be cut to size by scissors or a punching tool.
(1) |
Secondly, the obtained flux was applied to calculate the apparent permeability coefficient (Papp) using the following equation:
(2) |
Lastly, based on the permeability coefficients measured through the Permeapad™ barrier (Papp) and the support layer (Psup), the permeability coefficient through the lipid layer (Plip) was determined by the following equation:29,30
(3) |
Standard deviation calculations and student's t-test were evaluated; P ≤ 0.05 was considered as significantly different. The Thomson Tau test was applied in order to identify possible outlier values.
Doct/buf = Coct/buf/Cbuf/oct | (4) |
mi = moct/buf + mbuf/oct | (5) |
In preliminary experiments, all the compounds were tested for their ability to inhibit glutamate stimulated Ca uptake at the concentration of 100 μM. If the inhibition of Glu-Ca-uptake was 50% and more, then further studies were carried out to determine the concentration dependence of inhibition. The amount of the 45Ca2+ uptake in the synaptosomes was determined by the difference of the label content with and without uptake stimulation and expressed in % control (control – 100%). The corresponding value of K43/21 was calculated according to the following equation:
K43/21 = [(Ca4 − Ca3)/(Ca2 − Ca1)] × 100% | (6) |
Equilibrium constants for the compounds synthesized were calculated by the ACD/ChemSketch program.36 Analysis of the equilibrium of the charged state of the molecules was conducted by using the program package presented in ref. 37.
S 2982/mol l−1 | X 2982/mol fract | D oct/buf | K oct/buf0 | D hex/buf | K hex/buf0 | K 43/21/% | T m/K | α | ∑(Ca) | ∑(Ca)/α | |
---|---|---|---|---|---|---|---|---|---|---|---|
a Relative standard uncertainty for solubility values ur(S2982) = 0.03; ur(X2982) = 0.03. b nd – not determined. c Ref. 23. d Ref. 20. e Ref. 19. f Ref. 17. g Ref. 18. | |||||||||||
1 | 7.45 × 10−3 | 1.35 × 10−4 | 12.60 ± 0.02 | 8.28 × 104 | 0.011 ± 0.003 | 72.3 | 305 ± 18 | 347.2 ± 0.5 | 47.113 | 7.68 | 0.163 |
2 | 5.57 × 10−3 | 1.00 × 10−4 | 11.01 ± 0.03 | 7.31 × 104 | 0.0031 ± 0.0002 | 20.6 | 214 ± 12 | 319.3 ± 0.5 | 47.02 | 7.75 | 0.165 |
3 | 9.24 × 10−3 | 1.67 × 10−4 | 5.0 ± 0.4 | 3.25 × 104 | 0.0064 ± 0.0005 | 42.0 | 189 ± 14 | 333.5 ± 0.5 | 45.094 | 7.76 | 0.172 |
4 | 4.86 × 10−3 | 8.77 × 10−5 | 6.9 ± 0.2 | 4.56 × 104 | 0.017 ± 0.004 | 112.8 | 177 ± 9 | 334.2 ± 0.5 | 47.02 | 7.83 | 0.166 |
5 | 3.72 × 10−3 | 6.71 × 10−5 | 1.83 ± 0.04 | 1.22 × 104 | 0.011 ± 0.005 | 73.0 | 172 ± 3 | 323.2 ± 0.5 | 45.185 | 7.69 | 0.17 |
6 | 8.37 × 10−3 | 1.51 × 10−4 | 6.6 ± 0.4 | 4.44 × 104 | 0.013 ± 0.001 | 89.3 | 128.0 ± 0.1 | 320.2 ± 0.5 | 45.092 | 7.73 | 0.171 |
7 | 1.20 × 10−2 | 2.17 × 10−4 | 4.4 ± 0.2 | 2.92 × 104 | 0.014 ± 0.002 | 92.9 | 117 ± 2 | 309.1 ± 0.5 | 47.792 | 8.16 | 0.171 |
8 | 2.13 × 10−2 | 3.87 × 10−4 | 3.5 ± 0.3 | 2.34 × 104 | 0.013 ± 0.003 | 86.3 | 112 ± 25 | 314.7 ± 0.5 | 45.366 | 8.33 | 0.184 |
9 | 1.82 × 10−2 | 3.30 × 10−4 | 7.6 ± 0.3 | 5.06 × 104 | 0.024 ± 0.003 | 158.0 | 112 ± 12 | 317.6 ± 0.5 | 43.166 | 7.66 | 0.177 |
10 | 1.41 × 10−2 | 2.55 × 10−4 | 0.375 ± 0.005 | 2.41 × 103 | 0.041 ± 0.002 | 258.6 | 108 ± 6 | 342.6 ± 0.5 | 41.113 | 8.48 | 0.206 |
11 | 3.10 × 10−1 | 6.19 × 10−3 | 1.21 ± 0.02 | 3.19 × 103 | 0.097 ± 0.004 | 655.5 | 86 ± 14 | 341.4 ± 0.5 | 38.328 | 7.32 | 0.191 |
12 | 3.49 × 10−3 | 6.29 × 10−5 | 2.041 ± 0.004 | 1.36 × 104 | 0.013 ± 0.001 | 85.0 | 82 ± 5 | 318.5 ± 0.5 | 45.883 | 7.69 | 0.168 |
13 | ndb | ndb | 610 ± 30c | 6.10 × 102 | 0.17 ± 0.01c | 0.17 | 51 ± 9c | nd | 29.307 | 5.21 | 0.178 |
14 | 4.83 × 10−4d | 8.70 × 10−6d | 1038 ± 10c | 1.038 × 103 | 1.68 ± 0.07c | 1.68 | 87 ± 2c | 402.3 ± 0.2e | 29.214 | 5.28 | 0.181 |
15 | nd | nd | 226 ± 5c | 2.26 × 102 | 0.16 ± 0.04c | 0.16 | 75 ± 6c | nd | 27.288 | 5.29 | 0.194 |
16 | 4.45 × 10−4d | 8.00 × 10−6d | 1049 ± 50c | 1.049 × 103 | 0.56 ± 0.01c | 0.56 | 88 ± 16c | 374.5 ± 0.2e | 29.214 | 5.35 | 0.183 |
17 | 4.836 × 10−4d | 8.30 × 10−6d | 380 ± 5c | 3.80 × 102 | 0.46 ± 0.05c | 0.46 | 89 ± 13c | 408.4 ± 0.2e | 27.379 | 5.22 | 0.191 |
18 | 2.19 × 10−3f | 3.95 × 10−5f | 445 ± 28c | 4.45 × 102 | 0.31 ± 0.02c | 0.31 | 85 ± 4c | 390.1 ± 0.2f | 27.286 | 5.26 | 0.193 |
19 | nd | nd | 94 ± 13c | 9.4 × 10 | 0.48 ± 0.02c | 0.48 | 86.7 ± 0.5c | nd | 29.986 | 5.68 | 0.19 |
20 | 3.04 × 10−3d | 5.48 × 10−5d | 205 ± 5c | 2.05 × 102 | 0.58 ± 0.03c | 0.58 | 108 ± 11c | 363.4 ± 0.2e | 27.56 | 5.93 | 0.215 |
21 | 3.40 × 10−3g | 6.13 × 10−4g | 316 ± 3c | 3.16 × 102 | 0.32 ± 0.02c | 0.32 | 88 ± 16c | 376.3 ± 0.2g | 25.36 | 5.18 | 0.204 |
22 | nd | nd | 45 ± 1c | 4.5 × 10 | 0.18 ± 0.01c | 0.18 | 109 ± 20c | nd | 23.307 | 6.01 | 0.258 |
We studied the trends between Doct/buf and selected physicochemical descriptors. The main purpose of such a search was connected with an idea to develop an algorithm for prediction of the experimental data on the basis of just molecular structure knowledge. The HYBOT35 descriptors were selected as independent parameters, because they describe the interaction of drug molecules with biological media. It should be noted that the access to obtain the correlation equation was complemented by Doct/buf-values for the related compounds which were prepared in the present work (group I) and those which have been published by us previously (group II)23 (Table 1). However, the compounds of group I are in the ionized state in buffer (pH 7.4), whereas drugs of group II are in the form of neutral entities. The appropriate calculation of the equilibrium forms of the compounds by using the approach described in ref. 37 and taking into account the calculated pKa (pKa1 = 14.01–14.04; pKa2 = 1.29–4.67)36 confirms the neutral forms of the compounds of group II. For this group of compounds, the equality is realized: Koct/buf0 = Doct/buf and Khex/buf0 = Dhex/buf.
In order to recalculate the distribution coefficients, the ionization state of the molecules was determined taking into account that the presently investigated thiadiazoles (group I) are bases and have several ionizable groups. The macroscopic dissociation constants were calculated according to ref. 36.
Based on the calculated pKa-values, we determined the content of a number of the forms with different degrees of protonation in aqueous solutions depending on the pH of the media by using ref. 37, taking into account the following ionization processes:
HL+ = H+ + L (pK1) | (7) |
H2L2+ = HL+ + H+ (pK2) | (8) |
H3L3+ = H2L+ + H+ (pK3) | (9) |
The pKa1 = 10.95 corresponds to the protonation process of the nitrogen atom of the NH-group of the bipyridine ring, pKa2 = 7.31–7.36 to the protonation of the bridge NH-group and pKa3 = 0.45–3.83 to the protonation process of a nitrogen atom of the thiadiazole ring. K1, K2 and K3 are equilibrium constants of the mentioned equations. The ionized/unionized particle distributions (%) as a function of pH for compound 2 (as an example) is presented in Fig. 1SI (ESI‡). It is found that all the compounds have similar dissociation constant values and, respectively, the protonation degree. As follows from Fig. 1SI,‡ all the compounds are completely ionized at pH 7.4 and their molecules exist as approximately equal shares in the form of mono- and di-cations.
For ionizable compounds, the distribution coefficient describing the overall lipophilicity of drugs is the ratio of the concentrations of all molecular forms of compounds existing in equilibrium in the aqueous phase and uncharged particles in 1-octanol. For the investigated thiadiazoles, the equilibrium distribution can be represented by an equation by which the apparent distribution coefficient (Doct/buf) can be experimentally determined:
Doct/buf = [L]o/([L]w + [HL+]w + [HL2+]w + [HL3+]w) | (10) |
Doct/buf = [L]o/[L]w + [L][H+]/K1 + [L][H+]2/K2 + [L][H+]3/K3 | (11) |
Further transformation leads to the following equation, which relates the intrinsic distribution coefficients to the experimentally determined apparent distribution coefficients, hydrogen ion concentration (H+) and the dissociation constants, K1, K2 and K3:
Koct/buf0 = Doct/buf(1 + [H+]/K1 + [H+]2/K2 + [H+]3/K3) | (12) |
To make the conditions of the distribution processes comparable, we recalculated the values of Doct/buf and Dhex/buf for the neutral forms of the compounds of group I by eqn (12) (in Table 2, these coefficients are designated as Koct/buf0 and Koct/buf0).
The data in Table 2 show that the calculated intrinsic distribution coefficients (normalized to neutral species) of the studied thiadiazoles significantly exceed (more than 4 times) the experimental apparent ones (belonging to the ionized forms of the molecules). The estimated ratios indicate greater lipophilicity of the neutral particles compared with the charged ones as expected.
The Koct/buf0-values have been analyzed concerning 32 descriptors. A suitable correlation was obtained for the independent variables which include polarizability (α) and the acceptor molecular ability to create hydrogen bonds (∑(Ca)). The results of the correlation analysis can be represented by the equation:
(13) |
(14) |
A comparison of eqn (13) and (14) shows that Khex/buf0 is approximately two times more sensitive to the variation of the ∑(Ca)-descriptor than Koct/buf0. Most probably, this phenomenon can be explained by the specific interactions of the dissolved molecule with the solvent both in 1-octanol and buffer phases in the 1-octanol/buffer system. Therefore, the contribution of the descriptor is partially equalized. As opposed to this, in the 1-hexane/buffer system the dissolved molecules interact specifically only with one phase (buffer) which leads to a higher regression coefficient value. Thus, the correlation of eqn (13) and (14) allow predicting the distribution coefficients for the studied class of compounds both in 1-octanol/water and 1-hexane/water systems. It is interesting to compare the distribution coefficients for the molecules of group I compounds (normalized to the neutral species) with those of group II which differ from each other by only one fragment (a tetramethylpiperidine fragment (group I) instead of a hydroxyl group (group II)) both in 1-octanol/water and 1-hexane/water systems. The results of the comparative analysis are given in Fig. 1. In the 1-octanol/water system, the difference in the distribution coefficients between group I and group II compounds is positive with an average ΔlogKoct/buf0-value of 2.58 ± 0.20 (excluding the pair of compounds 10/22). A similar tendency for the 1-hexane/water system with an average ΔlogKhex/buf0-value of 2.47 ± 0.23 (excluding the pair of compounds 2/14) is observed. The derived values of ΔlogK0 can be determined by: firstly, conformational differences of the molecules of groups I and II in water and 1-octanol and also water and 1-hexane phases; secondly, variation of the energy of the hydrogen bond forming by a hydroxyl-group in the considered phases.
Analysis of Doct/hex-values showed the existence of strong specific interactions of the drug molecules with the 1-octanol (1.5 < logDoct/hex < 3.6). On this ground, it may be assumed that the redistribution of molecules from blood plasma through the blood–brain barrier will be aggravated.
It is well known that the nature and position of the substituent may influence essentially the solubility of the compounds in a structure analogue series. In this connection, the comparative solubility analysis for the synthesized thiadiazoles was performed. It was found that the solubility among the investigated compounds with the tetramethylpiperidine fragment differs within two orders of magnitude. Compound (11) with a cyclopropyl substituent has the maximal solubility, and compounds (12) and (5) with 4-bromophenyl and 4-chlorophenyl substituents, respectively, have the minimal ones. The replacement of a chlorine atom in the para-position of the phenyl ring by a methyl group (compound 6) increases the solubility twice, and by a methoxy group (compound 8) or a fluorine atom (compound 9) – about 6 times. Changing a methylphenyl- to a methylisoxazole substituent slightly enhances the solubility (about 1.5 times). Interestingly, the introduction of the second chlorine atom in the meta-position of the phenyl ring of compound 5 (3,4-dichloro-derivative (1)) leads to double the solubility. At that, the solubility values of the structural isomers 3-chloro-4-methyl- (2) and 3-chloro-6-methyl- (4) are approximately equal. According to the solubility increase, the investigated thiadiazoles are arranged in the following order: 12 (4-bromophenyl-) ≤ 5 (4-chlorophenyl-) < 4 (3-chloro-6-methylphenyl-) ≤ 2 (3-chloro-4-methylphenyl-) ≤ 1 (3,4-dichlorophenyl-) ≤ 6 (4-methylphenyl-) ≤ 3 (3-chloro-4-fluorophenyl-) < 7 (3-methylthiaphenyl-) ≤ 10 (methylisoxazol-) < 9 (4-fluorophenyl-) ≤ 8 (4-methoxyphenyl-) < 11 (cyclopropyl-).
The solubility change regularities described above do not have a forecasting power. Therefore, it was important to obtain correlation equations between the solubility characteristics and any kinds of descriptors. HYBOT descriptors were used as physicochemical descriptors.25
Crystal lattice thermodynamic characteristics are important parameters in solid substance dissolution. To take this factor into account, Yalkowsky et al.38 introduced crystal melting temperature as a descriptor into the correlation equation (general solubility equation). Using this descriptor to analyze the solubility thermodynamics is justified by the fact that in many cases there is a correlation between the molecular crystal sublimation Gibbs energies and melting temperatures.39 Besides, Yalkowsky et al.38 described water solubility of the compounds using 1-octanol/water partitioning coefficients as descriptors (for imitation of the hydration term). The descriptor series suggested by Yalkowsky was used to describe the solubility of selected compounds. As a result, the correlation equation looks as follows:
(15) |
Thus, the solubility of this class of compounds decreases with an increase in the lipophilicity (due to reduction of the hydration term) and the melting temperature growth (crystal lattice energy strengthening).
We also tried to find a correlation equation using HYBOT descriptors. Analysis of all the available descriptors found that the best correlations were obtained with the polarizability (α) and the acceptor molecular ability to create hydrogen bonds (∑(Ca)):
(16) |
Thus, the solubility-values of this class of compounds in a buffer solution can be estimated based on the knowledge of the structural formula only.
Compound | Apparent permeability coefficients | ||
---|---|---|---|
Permeapad™ barrier | Support layer | Lipid layer | |
P app × 106/cm s−1 | P sup × 106/cm s−1 | P lip × 106/cm s−1 | |
1 | 9.8 ± 0.8 | 15.7 ± 1.2 | 26.1 ± 4.0 |
2 | 13.5 ± 0.4 | 20.6 ± 0.1 | 39.5 ± 3.1 |
3 | 13.9 ± 2.3 | 25.4 ± 1.5 | 30.9 ± 7.3 |
4 | 14.4 ± 0.1 | 30.8 ± 3.0 | 26.9 ± 4.8 |
5 | 8.6 ± 0.9 | 21.9 ± 1.4 | 14.1 ± 0.2 |
6 | 12.2 ± 2.7 | 26.3 ± 1.9 | 22.8 ± 7.7 |
7 | 10.1 ± 0.5 | 22.8 ± 1.4 | 18.2 ± 1.9 |
8 | 9.4 ± 1.1 | 16.5 ± 1.3 | 21.7 ± 0.7 |
9 | 8.7 ± 1.1 | 16.3 ± 1.1 | 18.6 ± 2.0 |
10 | 3.4 ± 0.3 | 31.7 ± 4.4 | 3.7 ± 0.4 |
11 | 5.4 ± 0.4 | 27.6 ± 1.3 | 6.8 ± 0.6 |
12 | 6.5 ± 0.7 | 25.8 ± 2.2 | 9.5 ± 0.6 |
The results showed in ref. 27 indicate that the permeability coefficients through the sheer support layer (Psup) were in all cases higher than the respective Papp measured for the entire Permeapad™ barrier. Our data in Table 3 confirmed these conclusions. This fact is a clear indication of a significant retention effect induced by the lipids present in the artificial barrier and that the lipid layer is the dominant impediment to drug permeation. From this it can be concluded that for all compounds investigated, the rate limiting step in permeability was represented by the lipid layer of the artificial barrier. Due to this fact it is proposed that for screening purposes, it is reasonable to go without measuring the Psup-value.
The values of the permeation coefficients vary depending on the nature and number of substituents in the molecule. The maximum permeability coefficient (Plip) is observed for the 3-chloro-4-methylphenylderivative (compound 2). Replacement of the methyl group in this compound by a chlorine atom (dichlorophenyl-substituted compound (1)) leads to a small reduction of permeability. Thus, the permeability coefficient of the 3-chloro-4-methylphenylsubstituted compound is about 1.5 times higher than that of its 3-chloro-6-methylisomer (4), indicating the effect of not only the nature but also the position of the substituent on the permeability of thiadiazoles. Significant reduction in permeability (minimum values among all compounds) occurs in substances with isoxazole (10) and cyclopropyl (11) substituents. According to the permeability values the investigated substances can be arranged in the following order: 3-chloro-4-methyl- (2) > 3-chloro-4-fluoro- (3) > 3-chloro-6-methyl- (4) ≥ 3,4-dichloro- (1) > 4-methyl- (6) ≥ 3-methyloxy- (8) > 4-fluoro- (9) ≥ 3-methylthia- (7) > 4-chloro- (5) > 4-bromo- (12).
Due to the fact that the distribution and permeability processes for the selected compounds were studied in the same buffer solution (pH 7.4) (i.e. ionization degree of the particles and their ratio remained the same for the two designated processes), we tried Doct/buf and Dhex/buf as descriptors for the permeability. In turn, logPapp, logPsup and logPlip were selected as the analyzed functions. It should be noted that there are no correlations between the selected functions and Dhex/buf (Fig. 2SI‡). In contrast, good correlations between logPapp and logDoct/buf, as well as between logPlip and logDoct/buf (Fig. 2), exist, which can be described by the following equations:
(17) |
(18) |
It is easy to see that logPlip is 1.7 times more sensitive to log(Doct/buf) changes than logPapp. Thus, the supporting layer contributes to the sensitivity of this coefficient, but, the correlation parameters are not much deteriorated. Consequently, logPapp can be used to analyze the lipid layer permeability. If we take into account that the logPlip-value is burdened with two experimental errors (sequential execution of two experiments: permeability of the Permeapad™ barrier and support layer), then the Papp value is more accurate (and the total time of the experiment is halved).
As the next step, it was interesting to analyze the relationships of the HYBOT physicochemical descriptors with the obtained permeability characteristics. Testing all the descriptors revealed that it is only for logPlip and logPapp (as in the previous cases for logDoct/buf) in which the correlation with the acceptor molecular ability to create hydrogen bonds normalized to molecular polarizability (∑(Ca)/α) was observed. The results of the analysis for logPlip and logPapp are presented in Fig. 3, whereas the relationship between logPsup and ∑(Ca)/α is shown in Fig. 3SI.‡ The received correlation can be described by the following equations:
(19) |
(20) |
Thus, the permeability coefficients of this class of compounds may be predicted based solely on their structural formulas. Due to the small number of data points, the paired correlation coefficients are not rather high. However, improvement should be expected if the number of data points would increase. Just as in the case of the distribution coefficients, the correlation equations for logPapp and logPlip retain the same trends on the selected descriptor.
logJlip = log(S2982·Plip) = logS2982 + logPlip | (21a) |
logJapp = log(S2982·Papp) = logS2982 + logPapp | (21b) |
Fig. 4 depicts the analyzed values. It is easy to see that according to the degree of decreasing diffusion flux value (a measure of absorption), the compounds can be placed in the following order: for the lipid layer – 11 > 8 > 9 > 3 > 2 > 7 > 1 ≈ 6 > 4 > 5 ≈ 10 > 12; for Permeapad – 11 > 8 > 9 > 3 > 7 ≈ 6 > 2 ≈ 1 ≈ 4 > 10 > 5 > 12.
With this range of changing the Plip and Papp-values, it turns out that the solubility values have the main contribution to the diffusion fluxes (Fig. 5).
The obtained results clearly indicate that the variation of the structure of the substituent in the phenyl ring as well as the replacement of the phenyl ring by the cyclopropyl- and isoxazole-one influences the ability of thiadiazole derivatives to inhibit calcium ion uptake. The biological activity (K43/21-values) of the investigated substances is presented in Fig. 6 as a histogram to compare the compounds of groups I and II with the same substituents.
The comparative analysis of the activity of thiadiazole derivatives newly synthesized and investigated by us before indicated that, on the whole, the presence of the tetramethylpiperidine ring and an additional NH-group instead of a hydroxyl group facilitates a considerable growth of K43/21-values (up to 6 times for the compounds with the dichlorophenyl substituent (compounds 1 and 13)). However, it is interesting to note that if the replacement of the phenyl ring by isoxazole substituent takes place, the activities of the respective structural analogues of groups I and II practically coincide. The analysis of the structure–activity relationship was conducted for thiadiazoles synthesized in the present study (group I – compounds 1–12). Compound 12 with a bromine atom as a substituent in the para-position of the phenyl ring, revealing maximal inhibiting activity (minimal K43/21), was chosen as a reference. As seen from the histogram data, replacing a bromophenyl substituent by a cyclopropyl- and methylisoxazole-one leads to a slight consistent increase in K43/21 (compounds 11 and 10). Further reduction of the inhibitory activity is observed for compounds with 4-fluorophenyl-, 3-methoxyphenyl- and 3-methylthiaphenyl-substituents, which have similar activity values (9 (112%) = 8 (112%) ≤ 7 (117%)). Introduction of the methyl group (compound 6) in the para-position of the phenyl ring contributes to a further increase of K43/21. At that, the inhibitory activity of the compound with a methylisoxazole fragment (10) is higher than that of the methylphenyl-substituted one (6).
The results presented in the histogram allowed us to evaluate the total biological potential of the compounds, not only as possible neuroprotectors, but also as cognitive stimulants (nootrops). Thus, for five of the compounds (1–5), the values of K43/21 > 150 suggest that they be subjected for further testing as stimulants of cognitive functions using a recognition test. It is interesting to note that these compounds have chlorine atoms as substituents in the phenyl ring. At the same time, di-substituted substances with a chlorine atom in the meta-position reveal the maximum K43/21-values and according to the reduction of the activation function of glutamate-dependent uptake of calcium ions, the thiadiazoles can be arranged in the following order: 1 (3-chloro-4-chloro) > 2 (3-chloro-4-methyl) > 3 (3-chloro-4-fluoro) > 4 (3-chloro-6-methyl) > 5 (4-chloro).
In order to describe graphically the activity–lipophilicity dependence, we applied an approach introduced in ref. 42 for compounds of a specific type of activity and a close chemical structure according to the equation:
log(1/Kba) = a0 + a1·logDoct/buf − a2·(logDoct/buf)2 + a3·σ + a4·Es | (22) |
Fig. 7 depicts the dependence of the biological activity of the investigated thiadiazoles on the lipophilicity of the molecules characterized by the distribution coefficient in the 1-octanol/buffer system.
The correlation equation, in which the biological activity acts as a dependent variable and the distribution coefficient in the 1-octanol/buffer system acts as an independent one, is as follows (compound 5 is excluded from the correlation):
(23) |
It should be noted that the obtained correlation is not high; this fact may be explained by the rather small number of the experimental points. Enhancement of the correlation can be expected at the extension of the number of the compounds investigated. However, the obtained regularities support the parabolic model to be an appropriate manner for describing the dependence of the specific activity of thiadiazoles synthesized in the present study on the lipophilicity expressed by the distribution coefficient in the 1-octanol/water system.
Footnotes |
† The authors declare no competing interests. |
‡ Electronic supplementary information (ESI) available: Dependence of the content of the ionized forms of the molecules on the pH of a buffer solution of compound 2 (Fig. 1SI); relationships of the permeability coefficients with the distribution coefficients (Fig. 2SI); relationship of the permeability coefficient with physicochemical descriptor HYBOT (Fig. 3SI). See DOI: 10.1039/c6md00545d |
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