A novel proton transfer salt of 2-amino-6-sulfamoylbenzothiazole and its metal complexes: the evaluation of their inhibition effects on human cytosolic carbonic anhydrases.

A novel proton transfer compound (SMHABT)+(HDPC)- (1) obtained from 2-amino-6-sulfamoylbenzothiazole (SMABT) and 2,6-pyridinedicarboxylic acid (H2DPC) and its Fe(III), Co(II), Ni(II) complexes (2-4), and Fe(II) complex of SMABT (5) have been prepared and characterized by spectroscopic techniques. Additionally, single crystal X-ray diffraction techniques were applied to complexes (2-4). All complexes (2-4) have distorted octahedral conformations and the structure of 5 might be proposed as octahedral according to spectral and analytical results. All compounds, including acetazolamide (AAZ) as the control compound, were also evaluated for their in vitro inhibition effects on human hCA I and hCA II for their hydratase and esterase activities. The synthesized compounds have remarkable inhibitory activities on hCA I and hCA II. Especially, the inhibition potentials of the salt and the metal complexes (1-5) are comparable with AAZ. Inhibition data have been analyzed by using a one-way analysis of variance for multiple comparisons (p < .0001).

Introduction

The sulfonamide and benzothiazole derivatives constitute an important class of drugs, with several types of pharmacological agents possessing, among others, antibacterial, anticonvulsant, antiinflammatory, antitubercular, therapeutic, protease, and carbonic anhydrase inhibitory effects [1,2]. Carbonic anhydrase (CA, EC 4.2.1.1) is a metalloenzyme containing Zn2+ ion in its active site to catalyze the simple but physiologically important reversible reaction of carbon dioxide to bicarbonate ion and proton [3-6]. This reaction also provides the equilibrium of some ions, such as sodium ion, calcium ion, and chloride ion [7,8]. Therefore, carbonic anhydrases take part in many physiological processes [9-11]. These isozymes are found in many organisms throughout the phylogenetic tree [12]. Sixteen of these isozymes are expressed in humans, and 13 of them are catalytically active [13,14]. Among the human CAs, hCA I, and hCA II are cytosolic, and hCA II is located in human eye, erythrocytes, gastrointestinal tract, and kidney [15]. Bicarbonate ion, which is produced by carbonic anhydrases, has an important role in the formation of aqueous humor. This fluid is produced in the eye’s posterior chamber and is transferred into anterior chamber through the space between lens and iris. Later, aqueous humor moves through trabecular meshwork and Schlemm’s canal. Thus, the cycle is completed, and the intraocular pressure is kept in balance. But some structural defects, such as blockage in trabecular meshwork and Schlemm’s canal, or the smoother of the iris, prevent the flow of aqueous humor resulting from incompletion of the cycle and accumulating of the liquid in the posterior chamber, and causing intraocular pressure (IOP) elevation [16]. Glaucoma is a group of diseases characterized by the gradual loss of visual field due to an elevation in intraocular pressure (IOP) [15,17,18] CA inhibitors (CAIs) decrease IOP by reducing the rate of bicarbonate formation and thus the secretion of the aqueous humor from ciliary body [18,19]. Some systemic and topical CAIs used clinically have effective inhibition effects on the enzyme, but they have also many side effects, such as weight loss, fatigue, blurred vision, depression, metallic taste, and burning of the eye [15,18,20,21]. This situation clearly demonstrates the need for the development of new carbonic anhydrase inhibitors. In the last years, 2-aminobenzothiazole derivatives and their proton transfer salts and metal complexes have been studied as carbonic anhydrase inhibitors by our group [22-25].

In this study, 2-amino-6-sulfamoylbenzothiazole (SMABT) according to literature [26] and proton transfer compound (SMHABT)+(HDPC)− (1) and its Fe(III), Co(II), and Ni(II) complexes (2–4) and Fe(II) complex of SMABT (5) have been prepared and characterized by elemental, spectral (1H-NMR, 13C-NMR, IR and UV-Vis), and thermal analyses, as well as using magnetic measurement and molar conductivity techniques. Single crystal X-ray diffraction techniques were applied to complexes 2–4. In order to compare the inhibition data of newly synthesized compounds, 1–4, the simple metal complexes of H2DPC [27] and Fe(II) complexes of SMABT (5) have been prepared. Furthermore, we have investigated the potential use of these compounds as new inhibitors of hCA isoenzymes in the treatment of glaucoma.

Experimental section

General methods and materials

All chemicals used were analytical reagents and were commercially purchased from Aldrich. Elemental analyses for C, H, N, and S were performed on Elementar Vario III EL (Hanau, Germany) and Fe, Co, and Ni were detected with Perkin Elmer Optima 4300 DV ICP-OES (Perkin Elmer Inc., Wellesley, MA). 1H and 13C-NMR spectra were recorded with Bruker DPX FT NMR (500 MHz) spectrometer (Karlsruhe, Germany) (SiMe4 as internal standard and 85% H3PO4 as an external standard). FT-IR spectra were recorded in the 4000–400 cm−1 region with Bruker Optics, Vertex 70 FT-IR spectrometer using ATR techniques (Ettlingen, Germany). Thermal analyses were performed on Pelkin Elmer SII Exstar 6000 TG/DTA 6300 model (SII Nanotechnology, Japan) using platinum crucible with 10-mg sample. Measurements were taken in the static air within a 30–900 °C temperature range. The UV–Vis spectra were obtained for DMSO solution of the compounds (10−3 M) with a SHIMADZU UV-2550 spectrometer (Shimadzu Co, Kyoto, Japan) in the range of 200–900 nm. Magnetic susceptibility measurements at room temperature were performed using a Sherwood Scientific Magway MSB MK1 model magnetic balance (Sherwood Scientific Ltd, Cambridge, UK) by the Gouy method using Hg[Co(SCN)4] as calibrant. The molar conductance of the compounds were determined in water/ethanol (1:1) and in DMSO (10−3 M) at room temperature using a WTW Cond 315i/SET Model conductivity meter (Weilheim, Germany).

Synthesis of 1 and metal complexes (2–5)

SMABT as the starting compound was synthesized from sulfanilamide (SA) and 4-thioureidobenzenesulfonamide (TBS) according to literature [27]. 1H NMR and 13C NMR of the compound are given in Supplementary Table S1 and other spectroscopic data can be found in Supplementary Tables S2 and S4 and Supplementary Figures S1 and S2.

A solution of SMABT (1.145 g, 5 mmol) in 25 mL ethanol was added to the solution of H2DPC (0.836 g, 5 mmol) in 25 mL ethanol. The mixture was refluxed for 3 h and then was cooled to room temperature. The reaction mixture was kept at room temperature for 3 h to give white solid of 1 (1.783 g, 90% yield).

A solution of 1 mmol metal(II) salt [0.278 g FeSO4.7H2O or 0.249 g Co(CH3COO)2.4H2O or 0.248 g Ni(CH3COO)2.4H2O] in water (10 mL) was added dropwise to the solution of 1 (0.519 g, 1 mmol) for 2–4 or was added dropwise to the solution of SMABT (0.229 g, 1 mmol) for 5 in water/ethanol (1:1) (20 mL) with stirring at room temperature for two hours to complete the reaction. On filtration the reaction mixture, the solution was kept at room temperature for 2 weeks to give yellow crystalline solid for 2 (0.275 g, %80 yield) or brown crystalline solid for 3 (0.399 g, %85 yield) or green crystalline solid for 4 (0.329 g, %70 yield) or orange amorphous solid for 5 (0.285 g, 62% yield) (Figure 1). The single crystals of complexes 2–4 suitable for X-ray diffraction were separated and washed with EtOH/water (1:1).

Figure 1.

Syntheses of all compounds (a for SMABT and b for 1 and c for 2–4 and d for 5).

Anal. Calcd. for 1 (C14H12N4O6S2): C, 42.42%; H, 3.05%; N, 14.13%; S, 16.18%. Found: C, 42.45%; H, 3.00%; N, 14.15%; S, 16.15%; for 2 (C21H22N5O14S2Fe): C, 36.64%; H, 3.22%; N, 10.17%; S, 9.32%; Fe, 8.11%. Found: C, 36.65%; H, 3.20%; N, 10.20%; S, 9.30%; Fe, 8.10%; for 3 (C28H32N8O17S2Co): C, 35.78%; H, 3.43%; N, 11.92%; S, 13.65%; Co, 6.27%. Found: C, 35.75%; H, 3.40%; N, 11.95%; S, 13.67%; Co, 6.25%.; for 4 (C28H32N8O17S2Ni): C, 35.79%; H, 3.43%; N, 11.93%; S, 13.65%; Ni, 6.25%. Found: C, 35.80%; H, 3.40%; N, 11.90%; S, 13.62%; Ni, 6.20%; for 5 (C21H29N9O11S6Fe): C, 30.32%; H, 3.51%; N, 15.16%; S, 23.13%; Fe, 9.71%. Found: C, 30.30%; H, 3.56%; N, 15.20%; S, 23.10%; Fe, 9.65%.

X-ray data collection and structure refinement

The crystal and instrumental parameters used in the unit-cell determination, and data collection are summarized in Table 1 for the compounds 2–4. Crystallographic data of 2–4 were recorded on a Bruker Kappa APEX II CCD area-detector X-ray diffractometer employing plane graphite monochromatized with MoKα radiation (λ = 0.71073 Å), using ω-2θ scan mode. The empirical absorption corrections were applied by multi-scan via Bruker, SADABS software [28]. The structures were solved by the direct methods and subsequently completed by difference Fourier recycling. All non-hydrogen atoms were refined anisotropically using the full-matrix least-squares techniques on F2. The SHELXS-97 and SHELXL-97 [29] programs were used for all the calculations. The H atoms were placed in idealized positions and constrained to ride on their parent atoms with distances in the range of N−H = 0.77(3)–1.03(8) Å, C−H = 0.93 Å and with Uiso(H) = 1.2Ueq(C,N). Hydrogen atoms of water molecules were located from difference Fourier maps and refined with isotropic thermal parameters with a distance of O−H = 0.72(7)–1.10(11) Å and with Uiso(H) = 1.2Ueq(O). The drawings of molecules were accomplished with the help of ORTEP-3 for Windows [30].

Table 1.

Crystal data and structure refinement details for compounds 2–4.

	2	3	4
Empirical formula	C21H22N5O14S2Fe	C28H32N8O17S4Co	C28H32N8O17S4Ni
Formula weight	688.41	939.79	939.55
T[K]	296(2)	296(2)	296(2)
Wavelength (Å)	0.71073	0.71073	0.71073
Crystal system, space group	Monoclinic, P21/c	Triclinic, P1	Triclinic, P1
Unit cell dimensions (Å, °)
a	13.287(3)	9.2195(3)	9.118(4)
b	28.417(6)	14.4582(4)	14.428(5)
c	7.5289(15)	14.6132(4)	14.614(5)
α		98.6100(10)	98.902(19)
β	102.199(4)	106.4460(10)	106.27(2)
γ		91.2240(10)	91.19(2)
V (Å3)	2778.6(10)	1842.97(9)	1819.1(11)
Z	4	2	2
Absorbtion coefficient (mm−1)	0.772	0.780	0.852
Dcalc (mg/m3)	1.646	1.694	1.715
F(000)	1412	966	968
Crystal dimensions (mm)	0.32 × 0.11 × 0.064	0.70 × 0.29 × 0.29	0.36 × 0.22 × 0.18
θ range for data collection (°)	1.43–28.83	1.43–28.56	1.43–28.46
Index ranges	−18≤ h ≤15−38≤ k ≤30−10≤ l ≤4	−12≤ h ≤12−19≤ k ≤19−19≤ l ≤19	−12≤ h ≤12−19≤ k ≤19−19≤ l ≤19
Reflections collected	7755	40682	36415
Independent reflections	7265	9410	9189
Data/parameters	5418/428	7932/579	6014/579
Max. and min. transmission	0.955, 0.903	0.798, 0.762	0.858, 0.799
Final R indices [I ≥ 2σ(I)]	R1 = 0.0583wR2 = 0.1107	R1 = 0.0374wR2 = 0.1052	R1 = 0.0606wR2 = 0.160
R indices (all data)	R1 = 0.1251wR2 = 0.179	R1 = 0.0448wR2 = 0.1111	R1 = 0.1022wR2 = 0.212
Goodness-of-fit on F2	1.203	1.077	0.997
Largest difference in peak and hole (e Å−3)	0.713, −0.544	0.539, −0.402	0.633, −0.568

Purification of carbonic anhydrase I and II isoenzymes from human erythrocytes

Erythrocytes were purified from human blood. The blood samples were centrifuged at 1500 rpm for 20 min, and plasma was removed. Later, red cells were washed with isotonic solution (0.9% NaCl), and the erythrocytes were hemolyzed with 1.5 volumes of ice-cold water. Cell membranes were removed by centrifugation at 4 °C, 20000 rpm for 30 min. The pH of hemolysate was adjusted to 8.7 with solid TRIS (tris(hydroxymethyl)aminomethane). The hemolysate was applied to affinity column (Sepharose®4B-L-tyrosine-p-aminobenzene sulfonamide) pre-equilibrated with 25.0 mM TRIS-HCl/0.1 M Na2SO4 (pH 8.7). After extensive washing with a solution of 25.0 mM TRIS-HCl/22.0 mM Na2SO4 (pH 8.7), the hCA I and hCA II isoenzymes were eluted with the solution of 1.0 M NaCl/25.0 mM Na2HPO4 (pH 6.3) and 0.1 M NaCH3COO/0.5 M NaClO4 (pH 5.6), respectively [31]. For quantitative protein determination, the Bradford method was used with bovine serum albumin as standard [32]. Also, the purity control of the isoenzymes was performed with SDS-PAGE after the purification [33].

Determination of hydratase and esterase activities of hCA I and hCA II

The CO2 hydratase activity of the enzyme was determined at 0 °C in a veronal buffer (pH 8.15) with the pH-stat method as the indicator and saturated carbon dioxide solution as the substrate in a final volume of 4.2 mL. The time (in seconds) taken for the solution to change from pH 8.15 to pH 6.50 was measured. The enzyme unit (EU) is the enzyme amount that reduces the non-enzymatic reaction time by 50%. The activity of an enzyme unit was calculated by using the equation ((t0−tc)/tc), where t0 and tc are times for pH change of the non-enzymatic and enzymatic reactions, respectively [34].

Esterase activity was examined by following the change in the absorbance at 348 nm of 4-nitrophenylacetate to 4-nitrophenolate ion over a period of 3 min at 25 °C using a spectrophotometer (SHIMADZU UV 1700 PharmaSpec) according to the method described in the literature [35]. The enzymatic reaction, in a total volume of 3.0 mL, contained 1.4 mL of 0.05 M TRIS–SO4 buffer (pH 7.4), 1.0 mL of 3.0 mM 4-nitrophenylacetate, 0.5 mL H2O, and 0.1 mL enzyme solution. A reference measurement was obtained by preparing the same cuvette without enzyme solution.

Determination of IC50 and Ki values of the compounds

To determine the IC50 values (the concentration of inhibitor producing a 50% inhibition of CA activity) of the simple ligands, proton transfer salt, metal complexes, and acetazolamide (AAZ), hydratase, and esterase activities of CA isoenzymes were examined in the presence of various inhibitor concentrations. Regression analysis graphs were drawn by plotting the percent enzyme activity versus inhibitor concentration and IC50 values were calculated [17].

To determine the Ki values as well as the inhibition type, three different inhibitor concentrations giving 30%, 50%, and 70% inhibition were selected. For each of these inhibitor concentrations, enzyme activity was measured in the presence of various substrate concentrations (0.3 mM, 0.4 mM, 0.5 mM, 0.6 mM, and 0.7 mM), and the data were linearized with Lineweaver–Burk plot for Vmax and the Ki determination. Enzyme activity was also measured in the presence of the same substrate concentrations but in the absence of any inhibitor to determine the Vmax (Supplementary Figure S3) [17].

Statistical analysis

All the presented data were confirmed by at least three independent experiments and are expressed as the mean ± SD. Data were analyzed by using a one-way analysis of variance for multiple comparisons (SPSS 13.0, SPSS Inc., Chicago, IL). p < .0001 was considered to be statistically significant.

Results and discussion

Crystal structures of 2–4

The molecular structures of 2–4, with the atom labeling of symmetric units, are shown in Figures 2–4. The details of the crystal structure solutions are summarized in Table 1, and the selected bond lengths and angles are listed in Table 2.

Table 2.

Selected bond distances [Å] and angles [°] of compounds 2–4.

Compound 2: (SMHABT)[Fe(DPC)2].4H2O
Fe1-N1	2.086(5)	Fe1-O1	2.034(5)	Fe1-O5	2.023(4)
Fe1-N2	2.068(5)	Fe1-O2	2.059(4)	Fe1-O6	2.004(5)
O1-Fe1-O2	150.62(18)	O1-Fe1-N2	115.50(19)	O2-Fe1-N1	74.96(17)
O1-Fe1-O5	90.02(19)	O5-Fe1-O2	94.58(19)	O2-Fe1-N2	93.71(17)
O1-Fe1-O6	95.6(2)	O6-Fe1-O2	94.14(19)	O5-Fe1-N1	103.62(18)
N1-Fe1-N2	168.6(2)	O1-Fe1-N1	75.76(18)	O5-Fe1-N2	75.68(18)
Compound 3: (SMHABT)2[Co(DPC)2].5H2O
Co1-N1	2.0239(14)	Co1-O1	2.1992(15)	Co1-O5	2.1251(14)
Co1-N2	2.0277(14)	Co1-O2	2.1148(14)	Co1-O6	2.1809(14)
N1-Co1-N2	178.57(6)	N2-Co1-O1	103.82(5)	O1-Co1-O5	92.53(6)
N1-Co1-O1	74.81(5)	N2-Co1-O2	104.12(6)	O1-Co1-O6	92.11(6)
N1-Co1-O2	77.21(6)	N2-Co1-O5	76.92(6)	O2-Co1-O5	98.43(6)
N1-Co1-O5	103.47(6)	N2-Co1-O6	75.10(5)	O2-Co1-O6	90.37(6)
N1-Co1-O6	104.45(5)	O1-Co1-O2	151.64(5)	O5-Co1-O6	151.94(5)
Compound 4: (SMHABT)2[Ni(DPC)2].5H2O
Ni1-N1	1.973(3)	Ni1-O1	2.151(3)	Ni1-O5	2.094(3)
Ni1-N2	1.970(3)	Ni1-O2	2.089(3)	Ni1-O6	2.161(3)
N2-Ni1-N1	178.67(12)	O2-Ni1-O5	95.30(11)	N2-Ni1-O6	76.67(11)
N2-Ni1-O2	101.98(11)	N2-Ni1-O1	103.13(11)	N1-Ni1-O6	102.49(11)
N1-Ni1-O2	79.04(11)	N1-Ni1-O1	75.82(11)	O2-Ni1-O6	91.95(11)
N2-Ni1-O5	78.59(11)	O2-Ni1-O1	154.83(10)	O5-Ni1-O6	155.16(10)
N1-Ni1-O5	102.20(11)	O5-Ni1-O1	91.26(11)	O1-Ni1-O6	92.19(11)

Intermolecular in the complexes, (2–4) hydrogen bonds play important roles in stabilizing the crystal structures. The ranges of the D-H…A angles and those of the H…A and D…A distances indicate the presence of strong and weak hydrogen bondings in the structures 2–4 (Table 3).

An ORTEP drawing of asymmetric unit of 2 with the atom-numbering scheme. Displacement ellipsoids are drawn at the 40% probability level.

An ORTEP drawing of asymmetric unit of 3 with the atom-numbering scheme. Displacement ellipsoids are drawn at the 40% probability level.

An ORTEP drawing of asymmetric unit of 4 with the atom-numbering scheme. Displacement ellipsoids are drawn at the 40% probability level.

Table 3.

Hydrogen bonds for compounds 2–4 (Å, °).

D-H···A	d(D-H)	d(H···A)	d(D···A)	<D-H···A
2
N3-H3B-O4W	0.86	2.08	2.899(12)	158.1
O1W-H14-O1	1.00(16)	2.17(16)	3.129(8)	161(12)
O1W-H14-O4	1.00(16)	2.28(15)	3.093(9)	138(12)
O3W-H32-O2	0.72(9)	2.21(10)	2.919(9)	166(10)
3
N4-H4’-O6	0.86	1.86	2.667(2)	155.1
O2w-H2A-O4	0.77(4)	2.60(4)	3.260(4)	146(3)
4
N3-H31-O2W	0.86	2.03	2.830(5)	155.4
N3-H32-O1W	0.86	2.02	2.811(6)	152.0
N4-H4-O6	0.86	1.89	2.627(4)	142.2
O2W-H2B-O7	0.831(10)	2.50(3)	3.238(6)	149(5)

The complex 2, (SMHABT)[Fe(DPC)2].4H2O, crystallizes in the monoclinic P21/c space group. The structure of 2 consists of one SMHABT+ cation, one [Fe(DPC)2]– anion, and four uncoordinated water molecules. All the other complexes, (SMHABT)2[M(DPC)2].5H2O [M = Co(II) for 3 and Ni(II) for 4], crystallize in the triclinic P1 space group. The structures of 3 and 4 consist of one [M(DPC)2]2− anion and two counter SMHABT+ cations and five uncoordinated water molecules.

In complexes 2–4, the metal ion coordinates to four oxygen atoms and two nitrogen atoms of two 2,6-pyridinedicarboxylate ions resulted with a distorted octahedral conformation. Both carboxylate oxygen atoms from DPC2− occupy the trans-apical positions of the metal, and define low trans-angle value around metal ion for all complexes within the range of 150.062(18)°–155.16(6)° for O1-M-O2 or O5-M-O6 which reveal a rather rigid structure of such tri-dentate ligands [M = Fe(III) for 2, Co(II) for 3 and Ni(II) for 4] (Table 2). In structures of 2–4, the N1-M-N2 trans-angles are closer to 180° [168.6(2)°, 178.57(6), and 178.67(12)°, respectively]. The dihedral angles for all complexes defined by the mean planes of two DPC2− ligands are 105.02(18)° for 2, 103.47(6)° for 3, and 101.98(11)° for 4, showing that they fall almost perpendicular. The M-N and M-O bond distances lie within expected range of 1.970(3)–2.086(5) Å and 2.004(5)–2.1992(15) Å, respectively (Table 2). In all essential details, the geometries of the molecules regarding bond lengths and angles of the compounds are in good agreement with the values observed in similar Fe(III) [22,23,25], Co(II) [22,23], and Ni(II) [22,24,25] complexes.

1H and 13C NMR studies of 1

The 1H-NMR and 13C-NMR spectra of the compound 1 were obtained in d6-DMSO with and without D2O at room temperature using TMS as internal Standard (Supplementary Figures S4 and S5). The 1H signals were assigned on the basis of chemical shifts, multiplicities, intensities of the signals, and coupling constants. Table 4 lists complete 1H-NMR and 13C-NMR spectra of the compound 1.

Table 4.

1H-NMR and 13C-NMR chemical shifts (ppm) with coupling constants and assignments for compound 1.

H3	–	C2	148 ppm
H4	7.44 (1H, d) [3JH4-H5 = 8.46 Hz]	C4	119 ppm
H5	7.67 (1H, dxd) [3JH5-H4 = 8.46 Hz, 4JH5-H7 = 1.96 Hz]	C5	132 ppm
H7	8.12 (1H, d) [4JH7-H5 = 1.87 Hz]	C6	156 ppm
H11	7.88 (2H, s)	C7	124 ppm
H12	7.20 (2H, s)	C8	137 ppm
H13	–	C9	140 ppm
H15	8.25 (2H, dxd) [3JH15-H16=7.67 Hz, 4JH15-H15’= 1.14 Hz]	C14, C14’	167 ppm
H16	8.18 (1H, d + d) [3JH16-H15/15’=7.70 Hz and 3JH16-H15’/15=7.69 Hz]	C15, C15’	128 ppm
		C16	118 ppm
		C17, C17’	170 ppm

In 1H NMR spectrum of 1 (Supplementary Figure S4a, Table 4), the H4, H5, and H7 protons of the ring of (SMHABT)+ are doublet, doublet–doublet, and doublet, respectively, with 1H intensity and they are observed at 7.44 ppm (H4, 3JH4-H5 = 8.46 Hz), 7.67 ppm (H5, 3JH5-H4 = 8.46 Hz, 4JH5-H7 = 1.96 Hz), and 8.12 ppm (H7, 4JH7-H5 = 1.87 Hz). H16 proton of the (HDPC)- ring is doublet and another doublet with 1H intensity and observed at 8.18 ppm (3JH16-H15 or H15’ = 7.70 Hz and 3JH16-H15’ or H15 = 7.69 Hz). Although the H16 seems to be symmetrical and is expected to give triplet, the tautomeric of H13 between O18 and O18’, H16 might be unsymmetrical and might give doublet with H15 and another doublet with H15’ [36]. H15 and H15’ protons are observed at 8.25 ppm as doublet–doublet with 2H intensity (3JH15-H16 =7.67 Hz, 4JH15-H15’ = 1.14 Hz or 3JH15’-H16 = 7.67 Hz, 4JH15’-H15 = 1.14 Hz) [36]. The hydrogen atoms (H3 and H13) in compound 1 were not observed in the 1H NMR spectrum. The H11 and H12 protons of NH2 are singlet with 2H intensity, and they are observed at 7.88 ppm and 7.20 ppm, respectively. These protons (H3, H11, H12 and H13) were not observed in the 1H NMR spectrum obtained in d6-DMSO with D2O due to deuterium exchange (Supplementary Figure S4b).

13C-NMR spectrum of 1 exhibits 13 resonances (Table 4, Supplementary Figure S5). Seven peaks of this spectrum [148 ppm (C2), 119 ppm (C4), 132 ppm (C5), 156 ppm (C6), 124 ppm (C7), 137 ppm (C8), and 140 ppm (C9)] could be assigned to the carbons of (SMHABT)+ moiety of compound 1. Four peaks at 167 ppm (C14), 128 ppm (C15), 118 ppm (C16), and 170 ppm (C17) could be assigned to the carbons of (HDPC)− ring moiety.

The room temperature NMR spectra for compound 1 indicate clearly the formation of the proton transfer compound with 1:1 ratio of SMABT and H2DPC (Supplementary Figures S4 and S5).

FT-IR measurements

The infrared spectral data of the starting compounds (SMABT and H2DPC) and compounds 1–5 are given in Supplementary Table S2. In the high frequency region, weak bands 3067–3098 cm−1 are attributed to the stretching vibrations of aromatic C-H for all compounds. There are also broad absorption bands at 3502–3529 cm−1, which are attributed to the ν(OH) vibrations of water molecules for compounds 2–5. The relatively weak and broad bands at 2508–2737 cm−1 are attributed to the ν(N+-H) vibration for 1–4 [37]. The absorption bands at 3423, 3324, 3293, and 3237 cm−1 of NH2 group of SMABT are slightly shifted from those found for 1 (3433, 3424, 3385, and 3229 cm−1), for 2 (3398, 3355, 3337, and 3326 cm−1), for 3 (3369, 3341, 3327, and 3297 cm−1), for 4 (3425, 3360, 3337, and 3235 cm−1), and for 5 (3422, 3319, 3297, and 3235 cm−1) due to the weak intermolecular interactions. The carboxylate groups for compounds H2DPC and 1–4 exhibit strong carbonyl bands in the region of 1705–1456 cm−1. These bands are reflected by IR spectrum of the asymmetric (νas) and symmetric (νs) stretching vibrations at 1701 and 1456 cm−1 for H2DPC, 1705 and 1465 cm−1 for 1, 1661 and 1474 cm−1 for 2, 1654 and 1475 cm−1 for 3, and 1632 and 1467 cm−1 for 4. The differences (Δυ) between the asymmetric and symmetric stretches of the carboxylate groups of 2–4 are 187, 179, and 165, respectively, which suggest monodentate binding of the carboxylate group to the metal ion in all complexes [38]. The strong absorption bands in the region of 1637–1445 cm−1 are attributed to the ν(C=N) and ν(C=C) vibrations for all compounds. The vibrations of the ν(S=O) are also observed in the 1430–1097 cm−1 region for compounds SMABT and 1–5. The C–O vibrations data for all compounds except SMABT are between 1375 and 1048 cm−1 as expected. The ring wagging vibrations of the pyridine groups are also observed in the 801–706 cm−1 region for compounds H2DPC and 1–5. The weak bands at 459–436 cm−1 and 591–575 cm−1 are from the M–N and M–O vibrations of the compounds 2–5.

Thermal analyses of all complexes

Supplementary Figures S6–S9 show the TG-DTG and DTA curves of compounds 2–5, and the thermal analyses results are given in Supplementary Table S3.

For the compounds 2–5, the first stage, an endothermic peak corresponds to the loss of water molecules, namely four moles for 2, five moles for 3, five moles for 4, and two moles for 5. The exothermic second stage is consistent to the loss of following units, that is, C5H5NO2S for 2, C14H16N6O4S4 for 3, C6H8N2O4S2 for 4, and C21H21N7O6S6 for 5. The following units are also decomposed exothermically in the third stage: C16H8N4O8S for 2, C15H6N2O8 for 3, C22H14N6O8S2 for 4, and N2H2O2 for 5. The final decomposition products are FeO for 2, CoO for 3, NiO for 4, and FeO for 5, and they are identified by IR spectroscopy (Supplementary Table S3).

UV/vis spectrum, magnetic susceptibility, and molar conductivity

The electronic spectra of compounds 1–5 and the free ligands SMABT and H2DPC were recorded in DMSO solution with 1 × 10−3 mol L−1 concentrations at room temperature (Supplementary Table S4 and Figure S10). The characteristic π–π* transitions in the spectrum of 1 are of 305 nm and 290 nm, 310 nm and 303 nm for 2, 288 nm and 271 nm for 3, 286 nm and 268 nm for 4, and 305 nm and 290 nm for 5, with the same profiles as the free ligands SMABT (305 nm and 290 nm) and H2DPC (303 nm). The bands for the d–d transitions in DMSO are observed at 796 nm for 3, 776 nm for 4, and 585 for 5. The d–d transition for complex 2 containing Fe(III) ion with d5 has not been observed.

The room temperature magnetic moment of the metal complexes is of 5.94 BM for 2, 3.82 BM for 3, 2.78 BM for 4, and 4.85 BM for 5 per metal ion, indicating the presence of five (Fe3+, d5), three (Co2+, d7), two (Ni2+, d8), and four (Fe2+, d6) unpaired electrons.

The molar conductivity data in DMSO are of 76.5 Ω−1 cm2 mol−1 for 2, 49.5 Ω−1 cm2 mol−1 for 3, 50.8 Ω−1 cm2 mol−1 for 4, and 3.2 Ω−1 cm2 mol−1 for 5, indicating that the complex 2 is ionic with a 1:1 ratio; the complexes 3 and 4 are ionic with a 2:1 ratio, and 5 is nonionic complex [39].

In vitro inhibition studies

In the present study, the inhibition effects on the hydratase and esterase activities of hCA I and hCA II isozymes of the proton transfer salt (1), its metal complexes (2–4), the starting compounds (SA, TBS, SMABT, H2DPC), Fe(II) complex of SMABT (5), the metal complexes of H2DPC, and the control compound AAZ have been investigated. H2DPC and its metal complexes have not inhibited the hydratase and esterase activities of hCA I and hCA II isoforms.

Hydratase activities of the isozymes have been inhibited by all synthesized compounds. The proton transfer salt and metal complexes have more potent inhibition effects than the starting compounds. However, 1–5 are slightly weaker inhibitors than AAZ. Only 4 has almost the same inhibition effect with AAZ (Table 5). The inhibition effect of SMABT is weaker than the proton transfer salt (1). Metal complexes of 1 are more powerful inhibitors than 1 for the hydratase activities of hCA I and hCA II. The structures of 2–4 are similar but their inhibition effects are different. Compound 4 is a more potent inhibitor than 2, 3, and 5 are. These differences in the inhibitory effects could be derived from different metal ions in the complexes for 2 and 3. However, it can be considered that the difference of the inhibitory effect of 5 is due to the differences in molecular structure. When the inhibition profiles of the synthesized compounds on the hydratase activity of isozymes are considered, hCA II has been inhibited almost twice stronger than hCA I. Inhibition levels of the compounds for the hydratase activities of hCA I and hCA II are in the order of AAZ ≈ 4 > 3 > 5 > 2 > 1 > SMABT > TBS > SA.

Table 5.

The inhibition data and Ki values of hCA I and hCA II isozymes for hydratase and esterase activity.

	Hydratase IC50 (μM)a,b		Esterase IC50 (μM)a,b		Ki (μM)a,b
Compound	hCA I	hCA II	hCA I	hCA II	hCA I	hCA II
AAZ	0.390 ± 0.008	0.200 ± 0.005	0.420 ± 0.004	0.310 ± 0.008	0.260 ± 0.003	0.140 ± 0.005
SA	30.44 ± 0.008	5.670 ± 0.003	28.14 ± 0.012	5.360 ± 0.005	26.32 ± 0.009	4.140 ± 0.011
TBS	7.846 ± 0.005	4.334 ± 0.021	0.499 ± 0.010	0.234 ± 0.006	0.268 ± 0.007	0.114 ± 0.003
H2DPC	No inhibition	No inhibition	No inhibition	No inhibition	No inhibition	No inhibition
MDPC	No inhibition	No inhibition	No inhibition	No inhibition	No inhibition	No inhibition
SMABT	6.348 ± 0.012	3.876 ± 0.014	0.567 ± 0.008	0.322 ± 0.006	0.306 ± 0.004	0.162 ± 0.010
1	4.075 ± 0.018	1.998 ± 0.009	0.258 ± 0.017	0.133 ± 0.015	0.149 ± 0.017	0.085 ± 0.019
2	2.533 ± 0.023	1.009 ± 0.013	0.409 ± 0.021	0.189 ± 0.005	0.192 ± 0.019	0.101 ± 0.005
3	1.601 ± 0.008	0.703 ± 0.014	0.066 ± 0.004	0.041 ± 0.003	0.028 ± 0.002	0.013 ± 0.006
4	0.397 ± 0.011	0.212 ± 0.006	0.136 ± 0.003	0.054 ± 0.001	0.043 ± 0.012	0.021 ± 0.004
5	1.751 ± 0.013	0.887 ± 0.011	0.149 ± 0.008	0.067 ± 0.008	0.068 ± 0.014	0.035 ± 0.013

AAZ was used as reference compound.

M = Fe(III), Co(II), and Ni(II).

Mean ± standard error, from three different assays.

p < 0.0001 for all analysis.

The esterase activities of the isozymes are similar to the inhibition of the hydratase activities. But a significant difference can be recognized immediately in the inhibition profiles of esterase activities of hCA I and hCA II as it follows: all of the newly synthesized compounds (1–5) are more powerful inhibitors than AAZ is. Only in terms of the inhibition of the esterase activity of hCA I, compound 2 has nearly same inhibition potential as AAZ. Also, the esterase activities of hCA I and hCA II were inhibited stronger than the hydratase activities of the isozymes. Another difference when compared to the inhibition profile of hydratase activity is that 2 has acted as weaker esterase inhibitor than the proton transfer salt (1). The inhibition effects of 1 are twice higher than SMABT. The inhibitory effects of the metal complexes (2–5) were in the range of 0.066 ± 0.004 µM–0.409 ± 0.021 µM for hCA I, and 0.041 ± 0.003 µM–0.189 ± 0.005 µM for hCA II. Compound 3 has the most effective inhibitor effect on the esterase activities of the isozymes. The inhibition potentials of 4 and 5 are close to each other. Similar to hydratase activity inhibition results, it is shown that hCA II has been inhibited twice stronger than hCA I, except for complex 3 which is 1.5fold. Inhibition levels of the compounds are in the order of 3 > 4 > 5 > 1 > 2 > AAZ > TBS > SMABT > SA for hCA I, and of 3 > 4 > 5 > 1 > 2 > TBS > AAZ > SMABT > SA for hCA II, respectively.

Ki values of the compounds have been determined by using esterase activity measurements (Table 5). Ki values clearly show that the compounds have remarkable inhibition effects on hCA I and hCA II isozymes for esterase activities. Especially 3–5 have effective inhibition constants with nearly nanomolar level. The inhibition potentials of these compounds (3–5) are 10 times, 4 times, and 6 times higher than AAZ, respectively. These results are quite remarkable in terms of further studies.

In our previous studies, we investigated the inhibition potentials of the proton transfer salts and the metal complexes derived from 2-aminobenzothiazole [23], 2-amino-6-methylbenzothiazole [22], 2-amino-6-methoxybenzothiazole [24], and 2-amino-6-chlorobenzothiazole [25]. These compounds have also shown remarkable inhibitory effects despite the fact that they do not contain sulfonamide moiety. In this study, the inhibitory effects of the compounds are further improved by using 2-amino-6-sulfamoylbenzothiazole. To summarize, carbonic anhydrase (hCA I and hCA II) inhibition profiles of non-sulfamoyl benzothiazole and sulfamoyl benzothiazole derivatives are imparted to the literature.

Conclusions

In the present work, five newly compounds (1–5) were prepared for the first time. The complexes crystallize in the monoclinic P21/c space group for 2 and the triclinic P1 space group for 3 and 4. In complexes 2–4, the metal ion coordinates to four oxygen atoms and two nitrogen atoms of two 2,6-pyridinedicarboxylate ions resulted with a distorted octahedral conformation. Intermolecular N-H···O and O-H···O hydrogen bonds and π–π stacking interactions seem to be effective in the stabilization of the crystal structure. Elemental analyses and all measurements show good agreement with the structures. The structure of 5 might be proposed as octahedral according to results of elemental, spectral, magnetic measurement, molar conductivity, and thermal analyses.

These five novel compounds possess significant inhibition effect on hCA I and on hCA II for hydratase and esterase activities with nearly nanomolar level. These results suggest that further inhibition studies are worthwhile in order to obtain correlation in such compounds and derivatives of such compounds should be subject to further inhibition in vivo tests. The order of the inhibition effects increasing through starting compounds and proton transfer salt and the complexes of these compounds might be due to the structural changes leading to an impressive difference of activity.

Disclosure statement

The authors declare no conflict of interest. The authors are solely responsible for the content and results presented in this paper.