Introduction

Since the first report of 3,6-bis(dimethylamino)acridine or acridine orange (AO) as a fluorochromatic stain1, acridinediamines have become one of the most investigated class of fluorescent dyes owing to their multifunctional properties. It exhibits affinity for nucleic acids and can be used to fluorometrically differentiate between DNA and RNA2,3,4. Moreover, AO shows marked accumulation in the acidic lysosomes of cancer cells, shows stronger cytotoxic effects under blue light or UV-C illumination making it a promising candidate for effective anti-cancer therapy5,6. As a weak basic dye (pKa = 10.5) AO is used as an intracellular pH indicator due to its low molecular weight and hydrophobic nature. Precise measurement of intracellular pH can provide critical information for studying physiological and pathological processes, such as cell death, cancers, and cell proliferation7. For quantitative pH measurements, the use of luminescent sensors is desired8,9. The most commonly used cellular pH-sensitive stains are BCECF10,11,12, carboxySNARF-113,14, BODIPYs15 and 8-Hydroxypyrene-1,3,6-trisulfonic acid (HPTS)16,17,18,19. Because of their cheapness and easy preparation fluorescein and fluorescein derivatives20,21 are also still used. Although being excellent physiological pH probes, a few of the dyes listed above have serious drawbacks such as cell impermeability, leakage through the membranes, suboptimal properties in terms of photostabilities or quantum yields, complex structure, therefore complicated synthesis and high price. In addition to pH-sensing, AO is extensively used for the mapping of microenvironments, such as the interior or Stern layer of reverse or normal micelles and water in oil microemulsions22,23,24,25,26,27. Moreover, very recently Yeasmin et al. showed28 by utilizing a spiro-rhodamine pH-probe, which selectively interacted with the anionic interfacial Stern layer, that it is possible that a defined curvature at the membrane interface controls its pH/polarity to exhibit specific bioactivity. We assume that an AO like smart dye would also be able to detect pH deviation in artificial and/or natural membranes.

A possible solution to prepare a “smarter” fluorescent dye could be the exchange of one of the dimethylamino groups of AO to a multifunctional electron withdrawing group, such as isocyanide. Despite the versatile chemistry of isonitriles, the field of isocyanoacridines remained completely unexplored until now. The incorporation of the isocyano group has many advantages: it can lower the pKa of AO from 10.5 to around 7.0 yielding a powerful physiological pH probe, the reactive C-N bond can serve as a versatile base for many organic reactions, such as the Ugi reaction29, isonitriles easily form complexes with transition metal ions30 and the related isonitrile complexes of silver(I) are much less studied, in spite of interesting properties such as liquid crystalline behaviour31,32.

Recently, we developed a novel amino-isocyanonaphthalene (ICAN) based solvatochromic fluorophore family33,34. We assumed that by combining the best properties of our ICAN derivatives with those of AO we can obtain a novel dye family, amino-isocyanoacridines (ICAAcs) with significantly extended multifunctionality. 3-amino-6-isocyanoacridine (ICAAc) can be obtained by the treatment of proflavine with dichlorocarbene resulting the conversion of one of the amino groups to isonitrile (Fig. 1).

Figure 1
figure 1

The structures and names of the dyes used in this study. 3-amino-6-isocyanoacridine (ICAAc), 3-N-methylamino-6-isocyanoacridine (monoMICAAc), 3-N,N-dimethylamino-6-isocyanoacridine (diMICAAc).

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Hereby we report the development of a multifunctional isocyanoacridine based solvatochromic family with tunable properties. The photophysical behavior of the dyes, their applicability as physiological pH probes, their behavior in the micellar environment, their complexation with Ag(I) were investigated in detail and was backed by quantum chemical calculations. In addition, the cell staining ability of the ICAAc derivatives was also studied.

Results and Discussion

Steady-state fluorescence properties

All the quantum chemical (DFT) calculations, steady-state emission, absorption and excitation spectra in various solvents are presented in the Supporting Information (SI) for all the substances as separate chapters.

The UV-vis and fluorescence properties of ICAAc, monoMICAAc, and diMICAAc for solvents of different polarity are summarized in Fig. 2a and Table 1. Independently of solvent polarity, similarly for all three compounds, a broad long wavelength absorption band is seen in the range of ~370–540 nm (Fig. 2a inset), which can be attributed to the internal charge transfer transition (ICT) between the donor amino and the acceptor isocyano groups. This ICT band is accompanied by overlapping structured absorption bands belonging to the locally excited state (LE) characteristic for the aromatic acridine ring in the region of ~300–370 nm. These structured bands are also present in the UV-vis spectrum of 2-aminoacridine35, however they are completely missing from the spectrum of both proflavine and acridine orange. The reappearance of the structured bands may be explained by the presence of the rigid electron withdrawing isocyanide group, which breaks the symmetry of the molecule compared to AO. While the position of the LE bands remains unaffected by changing the solvent polarity, the longer wavelength (ICT) absorption bands show a considerable redshift with increasing solvent polarity. Increasing the electron donating ability of the amino group by methylation also results in a bathochromic shift of the higher wavelength absorption bands. These shifts are greater than those observed when changing solvent polarity. That is, the higher the electron donating ability of the amino group the higher wavelength the ICT absorption peak is located at. As it is evident from Fig. 2 and Table 1, all three dyes have a considerable emission range spanning from green to orange. The emission maximum of diMICAAc in water is the highest of the three dyes with λem = 576 nm, which is 50 nm higher than that of AO (λem = 526 nm). In addition, AO has a solvatochromic range of approximately 30 nm, while in the case of monoMICAAc and diMICAAc this value is doubled to more than 60 nm.

Figure 2
figure 2

(a) The normalized emission spectra of the isocyanoacridine dyes recorded in hexane (blue) and water (red). The inset shows the excitation spectra recorded only in hexane. (b) Demonstration of the fluorescence properties of the ICAAc derivatives in different solvents (λex = 365 nm). Solvents from left to the right are hexane (1), toluene (2), 1,4-dioxane (3), CH2Cl2 (4), CHCl3 (5), THF (6), MeCN (7), acetone (8), pyridine (9), methanol (10), DMF (11), DMSO (12), water (13).

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Table 1 Comparison of the optical properties of the dyes in solvents of different polarity.
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To get a better understanding of the solvatochromic behavior of the ICAAc derivatives Lippert-Mataga plots (Figs S14, 15) were constructed based on Eqs S1, S2 in the SI. As solvent polarity increases the emission maximum shifts bathochromically (Fig. S14b), due to the solvent reorientation around the excited dye, reducing the energy gap between the ground and excited state and as a result the energy of the emitted photon also decreases. Additionally, the quantum yields (ΦF) show a linear decrease with increasing solvent polarity parameter ET(30) values, which is in line with the data of Fig. 2 and Table 1. All our dyes have very low quantum yields (ΦF = 2.9–0.4%) in water, that of diMICAAc being the lowest. The low ΦF may be advantageously used in cell staining applications where the suppression of background fluorescence is essential. The extended solvatochromic range of the ICAAc derivatives can be explained by their increased dipole moment difference between the ground (μg) and excited state (μe) due to the the electron withdrawing isocyano group, which makes the dyes more polar. The dipole moment difference was determined experimentally from the slope of the Lippert-Mataga plot (Fig. S14a) and by DFT calculations. As it is evident from the data of Table 1, the μe-μg values of the ICAAc derivatives are at least 3 times higher than that of AO and are increasing with the methylation of the amino group.

The behavior of ICAAc derivatives in water

It is known that acridine based dyes such as AO can be present in different forms in aqueous media22. To characterize the acid-base properties of our ICAAc derivatives UV-vis and steady-state fluorescence measurements were carried out in the pH range of 2–12 in the same Britton–Robinson “universal” buffer (BRB). The results are presented for diMICAAc in Fig. 3 and in Figs S16, 17 for ICAAc and monoMICAAc and are summarized in Table 2.

Figure 3
figure 3

Demonstration of the changes in the UV-vis absorption (a) and emission (b) spectrum of diMICAAc in BRB at different pH. The insets show Eq. 1 fitted on the experimental absorbance or PL intensity data. (T = 20 °C. ([dye] = 4.58 × 10−5 M), V = 3.00 cm3).

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Table 2 Absorption (λabs,max) and emission (λem,max) maxima of the ICAAc derivatives at pH = 3 and pH = 11, respectively, in aqueous buffer.
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The absorption spectrum of all three compounds contains a broad CT band with a maximum of λabs,max = 470 nm for ICAAc, 475 nm for monoMICAAc and 502 nm for diMICAAc at pH = 3. This maximum suffers a hypsochromic shift upon increasing the pH of the medium to λabs,max = 428 nm for ICAAc, 446 nm for monoMICAAc and 470 nm for diMICAAc at pH = 11.

The base (DB) and protonated (DBH+) forms (Fig. 4) can be distinguished by the shape of the minor acridine-like absorption bands located between λabs = 320 nm and 400 nm. It should be noted that these bands are completely absent from the absorption spectrum of AO, making our dyes more suitable for pH sensing. The UV-vis spectrum of the free base in the same region exhibits a more structured absorption pattern consisting of three moderate bands of different intensity, while the spectrum of the protonated species contains only two broader and higher intensity peaks. This low intensity three-band structure is characteristic for all solvents investigated except water. Therefore, to further support our assignation, UV-vis spectra of diMICAAc were recorded in acetonitrile in the presence of water, ammonia and acetic acid (Fig. 5).

Figure 4
figure 4

The protonation equilibrium between the free base form DB and the protonated form DBH+ of the dyes.

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Figure 5
figure 5

Demonstration of the changes in the UV-vis absorption spectrum of diMICAAc dissolved in MeCN upon the addition of water, base (NH3) and acid (CH3COOH). The inset picture demonstrates the color change of diMICAAc upon the addition of acid. Yellow (left, base form), red (right, protonated form).

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According to Fig. 5 the absorption spectra do not change either upon the addition of small amounts of water or base (NH3). After the addition of acetic acid in ~7 molar excess, a new band starts to appear at ~375 nm and a broad double band structure only appears after the addition of a large excess (~35x molar) of acetic acid. After recording the absorption spectra in the concentration range of 10−6–10−4 M in water and in buffers too, no deviation from the Lambert-Beer law was observed, which excludes the presence of dimers.

Assuming a simple equilibrium between DB and DBH+ (Fig. 4) and denoting the pH-dependent property (absorbance or PL intensity) by Y(λ,pH), the acid dissociation constant (Ka) can be determined by fitting Eq. 1. to the Abs(502)-pH experimental plots as presented in the inset of Fig. 6.

$$Y(\lambda ,pH)=\frac{{Y}_{B}(\lambda )}{1+{10}^{p{K}_{a}-pH}}+\frac{{Y}_{BH+}(\lambda )\cdot {10}^{p{K}_{a}-pH}}{1+{10}^{p{K}_{a}-pH}}$$
(1)
Figure 6
figure 6

UV-vis titration curves of diMICAAc in BRB buffer at different pHs. The lines were fitted using Eq. 2. The bottom left inset shows the absorbance ratios as a function of the molar fraction of the protonated form αHA+. The top right inset shows the correlation between the absorbance ratios calculated at the ICT and acridine like absorption wavelengths. (T = 20 °C, [dye] = 1.14 × 10−5 M, V = 3.00 cm3).

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The obtained pKa values show only a slight variation between pKa = 7.05 and 7.58 (UV-vis) and pKa = 6.96 and 7.71 (Fluorescence). These pKa values make the ICAAc derivatives three orders of magnitude weaker bases than AO (pKa = 10.5)22. The fluorescence intensity also shows strong pH dependence, it increases in the more acidic medium in the case of ICAAc, and monoMICAAc. The PL intensity ratio I3/I11 calculated from the intensities measured at pH = 3 and pH = 11 is 2.25 and 1.69 for ICAAc, and monoMICAAc, respectively. The situation is completely different for diMICAAc, where PL intensity increases at higher pH and I3/I11 is only 0.58.

Investigation of the applicability of diMICAAc for pH determination

Favorably, the pKa value of diMICAAc is 7.5, which falls in the physiological pH range making it a possible candidate for a fluorescent biosensor. For the precise determination of the pH, calibration curves were constructed based on Eq. 2.

$$r=\frac{{b}_{1}+{10}^{-pH}}{{b}_{2}+{b}_{3}{10}^{-pH}}$$
(2)

where r is the ratio of the absorbances (PL intensities) measured at different wavelengths, b1, b2, and b3 are parameters used for fitting. The UV-vis titration curves are presented in Fig. 6 and the fluorescence titration curves in Fig. S18.

As it is evident from Fig. 6 both curves have a very similar run. The A502/A470 ratio varies between 1.43–0.73, while the A375/A359 between 1.05–0.34 in the pH range of 5.5–10.0. The majority of the change happens between pH = 6.5–8.5, making it the most useful region for pH determination. In addition, it should be noted that there is a perfect correlation between the two absorbance ratios as is presented in Fig. 6 inset. Unlike UV-vis, the fluorescence (excitation) titration curve is shifted approximately 1 pH unit to the left, that is the drop in the curve is located between pH = 5.5–8.0, extending the useful section more in the acidic region. To test the practical applicability of our dye and the reproducibility of the method, that is its dependence on the dissolved chemical species and ionic strength, buffer media of different pH and concentration were prepared and their absorption and fluorescence spectra were recorded after the addition of diMICAAc. The results are summarized in Table 3.

Table 3 Reproducibility of the spectroscopic pH sensing method using different buffers.
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The spectroscopically measured pH values for both the phosphate and borate buffers agree well with the previously set values in the 6.00–9.00 pH region. No selectivity for different chemical species could be detected. The largest errors 2–4% can be observed on the edges of the range, whereas between pH = 7.00–8.50 the errors are well below 1% for both the UV-vis and the fluorescence methods, which is important for biological applications. The method was also tested on a 0.10 M NaHCO3 solution with a pH of 8.50 and the measured values were pH = 8.53 ± 0.07 (UV-vis) and pH = 8.59 ± 0.01 (PL). The stability of the method was also tested in phosphate buffer at pH = 6 and 8 respectively for an hour. No significant change (the relative errors were 0.6% at pH = 6 and 0.4% at pH = 8) could be observed during this period as can be seen in Figs S19, 20. To investigate the salt effect, samples in BRB buffer at pH = 6 and 8, respectively were titrated with saturated KCl solution. As Fig. S21 shows the ionic strength has no significant effect on the method, the errors are below 1–2% even at 0.5 M KCl concentrations. Hence, we can conclude that the method is stable and can be used as soon as 5 minutes after mixing the dye with the medium.

Critical micelle concentration (CMC) studies

It has been shown previously that the pH in the Stern layer of micelles formed from anionic surfactants such as sodium lauryl sulfate (SLS) can significantly differ from that of the bulk28. It is known that AO interacts with SLS micelles through both hydrophobic and electrostatic interactions. Since our dyes are highly dipolar and the intracyclic imino group gets easily charged through protonation, it is more likely that the dyes will reside in the Stern layer instead of penetrating into the nonpolar core. In order to investigate the behavior of our dyes in the micellar medium, we have studied diMICAAc in SLS solutions prepared in 50 mM BRB buffer at pH = 7 (to keep the bulk pH constant). The pH values were calculated from the excitation spectra using the ratio of I376/I362 and the fluorescence intensities were read at 575 nm (peak maximum). The results are summarized in Fig. 7. As it is evident from Fig. 7 the pH of the microenvironment of diMICAAc starts to decrease in the first four steps by increasing the SLS concentration. This linear decrease is followed by a sharp drop to pH = 6 and then fluctuates around this value. Since ΦF = 0.4% for diMICAAc, the interaction with micelles results in a sharp increase in fluorescence intensity at 575 nm. The change in pH and PL intensity vs concentration curves correlate perfectly, the sharp drop (jump) happens at approximately 4 mM which can be considered the critical micelle concentration (CMC) in this medium. However, this value is a bit lower than the one reported in pure water, it is known that the use of a buffer solution, therefore the elevated ionic strength results in a lower CMC36.

Figure 7
figure 7

Calculated pH of the microenvironment of diMICAAc versus SLS concentration in BRB (pH = 7). The inset shows the fluorescence intensities measured at λ = 575 nm versus SLS concentration (T = 20 °C, [dye] = 4.58 × 10−6 M, V = 3.00 cm3).

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The experiments were repeated using deionized water and diMICAAc and the results are presented in Fig. S22. Similarly to the buffered solution, below CMC the PL intensity decreases until a minimum is reached followed by a sudden increase after which the PL intensity runs into saturation above CMC. It is evident from Fig. S22b. that the run of the intensity vs SLS concentration curves are identical and no matter which wavelength we use the same CMC value of approximately 7 mM is obtained, which is in good agreement with the values found in the literature for SLS. When looking at Fig. S22a. we can see the variation of the excitation spectrum as a function of SLS concentration. It should be emphasized that independently from the wavelengths used, the CMC of SLS can be very well guessed from the excitation spectra too. At 5.74 and 6.54 mM SLS concentrations (indicated by thick lines) we can see the shape of the spectra alter, that is a shoulder at 530 nm appears on the ICT band and it almost becomes a double band. This change can be assigned to the start of the increasing part of the intensity curve in the premicellar region of SLS concentration. Above CMC the 530 nm shoulder remains, but the 503 nm band becomes dominant. It should be noted that λem,max does not change above or below CMC with respect to the one recorded in pure water. Therefore the dye is not likely to penetrate to the nonpolar core of the micelles and it most likely resides in the Stern layer of the micelles where the interaction is of electrostatic character. For comparison, the CMC was also determined using the more sophisticated method of Pineiro et al.37, where the CMC is defined as the total surfactant concentration [S]0 at which the change in the gradient of the monomer concentration [S1] with respect to [S]0 is maximum, that is where the third derivative of [S1] is zero. Consequently, we describe the second derivative of [S1] with respect to [S]0 by a Gaussian function centered at the CMC as is presented in Fig. S23. The CMC obtained by this method is 7.5 mM which is very close to the literature value of 8.2 mM. In summary, diMICAAc is well applicable for both CMC determination and microenvironment pH mapping.

Complexation of diMICAAc with Ag(I) ions

We have shown earlier34 that aromatic amino-isocyano compounds tend to form complexes in the presence of Ag(I) ions and the process is accompanied by significant spectral changes. Steady-state fluorescence titration of diMICAAc in dioxane revealed a sharp decrease of PL intensity (to one-third of the original) with increasing silver(I) concentration as is presented in Fig. 8. In addition, a 20 nm bathochromic shift of the emission maximum occurs from λem,max = 548 nm to λem,max = 568 nm, which manifests in a color change from greenish-yellow to red in visible light and from neon green to orange when excited with λex = 365 nm UV light (Fig. 8 insets a and b respectively). The shape of the inset graph in Fig. 8 indicates the formation of a 1:1 complex, which was also detected under ESI-MS conditions. The first isotopic mass of the complex with a formula of [Ag(C16H13N3)]+ is 354.015 Da as can be seen in Fig. S24 and no additional mass corresponding to other Ag:diMICAAc composition could be observed. The equilibrium constant of complexation was determined using non-linear regression analysis described in ref.34 and turned out to be K = (4.5 ± 0.9) × 105 M −1. However, this equilibrium constant is lower than those obtained for ICAN derivatives (K = 106 M−1 and 107 M−1) it still indicates high binding affinity of silver(I) towards diMICAAc. The formation of a 1:1 complex is further backed by quantum chemical (DFT) calculations since the calculated PL spectrum agrees very well with the measured one as can be seen in Fig. S25. DFT calculations also revealed that Ag+ is attached to the isocyano moiety instead of the imino nitrogen in the ring (Fig. S26).

Figure 8
figure 8

The change of fluorescence as a function of metal (Ag+) concentration in the dioxane solution of diMICAAc (4.58  ×  10−5 M). Picture (a) diMICAAc in dioxane (left) and in the presence of 130 μM Ag+ (right) under visible light. Picture (b) the same compositions as in (a) illuminated by λex = 365 nm UV-light.

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Computational results

The calculated absorption and emission spectra of the three amino-isocyanoacridine molecules are shown in Figs S27–32. In nonpolar solvents, the calculated and experimental spectra show very good agreement. Considering polar solvents, however, it seems that additional effects, other than simple dielectric interactions play an important role. First, we investigated whether the observed fluorescence quenching is due to the decoupling of either the amino or the isocyano group from the acridine ring by simply replacing the two functional groups with a hydrogen atom. As Fig. S33 shows, both spectra are blue-shifted compared to the unmodified ICAAc but no dark states or lower oscillator strengths are calculated. The TICT (Twisted Intramolecular Charge Transfer) mechanism is unlikely because the planarization of the amino group in the excited state is not hindered by nearby hydrogens according to geometry optimization in the excited state. Another commonly reported quenching mechanism, the dimerization is also not expected to play a role because dimer formation of ICAAc is endergonic by 3.3–5.0 kcal mol−1. Since these molecules can be used as pH sensors, we also explored the possible sites of protonation, as well as the optical properties of these protonated species using DFT. We considered three protonation modes, as shown in Fig. 9a,b. It can be seen, that in both the ground and S1 states, the protonation of the acridine nitrogen is by far the most favored case. Protonation of the amino group is also interesting because it gives rise to the observed double peak structure below 400 nm in the absorption spectrum but the low energy band disappears. The change in the experimental fluorescence spectrum of ICAAc upon protonation is reproduced by the calculations well, however, the emission behavior of diMICAAc remains an open question. As Fig. 9c shows, the frontier orbitals barely change upon protonation which is reflected by the very small change in the calculated emission spectra. We also considered another approach where an excited state proton transfer was modeled using an explicit water molecule. The spectral changes following the gradual decrease of the N-H distance are shown in Fig. 9d. This shows the experimentally observed behavior of a minimal red shift together with a nearly twofold increase in intensity. Correlation between the protonation coordinate and change in emission wavelength for the protonation and deprotonation of the amino group is shown in Figs S34, 35. The calculated wavelength shift is in the opposite direction which further strengthens the view that protonation takes place on the acridine nitrogen.

Figure 9
figure 9

(a) The calculated UV-Vis absorption spectra of the three different protonation modes of diMICAAc in water. The relative Gibbs free energies in the ground state are the following: 0, +17.4 and +26.7 kcal mol−1 for the acridine N and amino N, and isocyano C protonated states, respectively. (b) The calculated emission spectra of the amino and acridine N protonation modes of diMICAAc in water. The aminomethyl groups are perpendicular to the acridine ring. The relative electronic energies in the excited state are the following: 0, +17.3 for the acridine N, amino N protonated states, respectively. (c) The frontier orbitals of diMICAAc (left) and its acridine N protonated (right) form. (d) Change in the emission spectrum when the acridine nitrogen gets protonated along a relaxed potential energy scan of the Hwater and Nacridine distance. The protonated state is not reached in the end.

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Overview of the staining capacity of the new dyes for fluorescence microscopy and cytometry in live human cells

The biological applicability of the dyes as supravital cell stains (Laser-Scanning Cytometry and microscopy) and the investigation of their toxicity (MTT cell viability assay) are presented in the Supporting Information as Chapter VII. Biological studies.

Conclusions

Novel, multifunctional, amino-isocyanoacridines (ICAAc, monoMICAAc and diMICAAc) were prepared by the reaction of 3,6-diaminoacridine with dichlorocarbene. The resulting dyes showed tunable solvatochromic behavior (Δλem = 53–63 nm) owing to the dipolar nature (μe-μg varies between 5.6–8.9 Debye) of the molecules. The introduction of the electron withdrawing isonitrile group, resulted in a reduced basicity (pKa = 7.05–7.58), which in combination with their unique pH-sensitive vibronic absorption bands make them promising pH-probes in the physiological pH range. It was demonstrated using UV-vis and fluorescence spectroscopy that the pH of different buffer solutions could be recovered with great precision (2–3% error) between pH = 6–8 and the method is stable for at least an hour. The dyes were shown to be able to sense pH change in different microenvironments such as the lowered pH in the Stern layer as it was demonstrated on SLS micelles. Furthermore, the isocyano group is an excellent ligand for complexation with Ag(I), this way the optical behavior of our dyes can be fine-tuned by ions too. 24 hour MTT assays on HeLa cells revealed LD50 values of 7.27, 5.78, and 7.50 μM for ICAAc, monoMICAAc and diMICAAc dyes, respectively. The applicability of ICAAc, monoMICAAc, and diMICAAc dyes for live cell imaging was demonstrated on HeLa cells at 0.3 μg/ml dye concentration. diMICAAc stained cells demonstrated the best-preserved morphology. DiMICAAc probably binds cell membranes, some unknown intracellular vesicular structures, probably the DNA slightly, and possible binds to some extent to the RNA. All the three dyes are well-applicable with conventional epifluorescence imaging at the UV excitation. Furthermore, at the blue excitation, diMICAAc is optimally suited as a whole-cell probe for both the conventional microscopic and the laser-illumination studies, like flow- and imaging cytometric, or confocal laser-scanning microscopic examinations.

Methods

Materials

Acetone, dichloromethane (DCM), hexane, 2-propanol (iPrOH), toluene, ethyl-acetate (EtOAc) (reagent grade, Molar Chemicals, Hungary) were purified by distillation. Acetonitrile (MeCN), tetrahydrofuran (THF), methanol (MeOH), dimethyl formamide (DMF), dimethyl sulfoxide (DMSO), pyridine (HPLC grade, VWR, Germany), cyclohexane, 1,4-dioxane (reagent grade, Reanal, Hungary), chloroform, 3,6-diaminoacridine hydrochloride (Sigma-Aldrich, Germany), sodium lauryl sulfate (SLS) (Biosolve, France) were used without further purification.

Synthesis

The preparation and characterization of the ICAAc derivatives are detailed in the SI.

Methods

UV-vis

The UV-vis spectra were recorded on an Agilent Cary 60 spectrophotometer (Agilent, Santa Clara, CA, USA) in a quartz cuvette of 1.00 cm optical length. 3.00 cm3 solution was prepared from the sample.

Fluorescence measurements

Steady-state fluorescence measurements were carried out using a Jasco FP-8200 fluorescence spectrophotometer equipped with a Xe lamp light source. The excitation and emission spectra were recorded at 20 °C, using 2.5 nm excitation, 5.0 nm emission bandwith, and 200 nm/min scanning speed. Fluorescence quantum yields (Φ) were calculated by using quinine-sulfate as the reference, using the following equation:

$${\rm{\Phi }}={\rm{\Phi }}r\,\ast \,\frac{I}{{I}_{ref}}\,\ast \,\frac{{A}_{ref}}{A}\,\ast \,\frac{{n}^{2}}{{n}_{ref}^{2}}$$
(3)

where Φr is the quantum yield of the reference compound (quinine-sulfate in 0.1 mol/L sulfuric acid, absolute quantum efficiency (Φr = 55%)), n is the refractive index of the solvent, I is the integrated fluorescence intensity and A is the absorbance at the excitation wavelength. The absorbances at the wavelength of excitation were kept below A = 0.1 in order to avoid inner filter effects. For UV-vis and fluorescence measurements the investigated compounds were dissolved in acetonitrile at a concentration of 1.2 mM and was diluted to 2.4 × 10−5 M and 4.8 × 10−6 M in the solvents in interest.

Measurements on the pH-dependence of the optical properties

Britton-Robinson buffer (BRB) was prepared by mixing 100–100 cm3 0.04 M H3BO3, 0.04 M H3PO4 and 0.04 M acetic acid solution, then titrated to the desired pH with 2.0 M NaOH solution. The cuvette was charged with 3.00 cm3 buffer solution, and 30 μl stock solution of the dye in acetonitrile was added. NaH2PO4/Na2HPO4 and NaH2BO3/Na2HBO3 buffers were prepared by the titration of 0.05 M Na2HPO4 or Na2B4O7 solution with 1.0 M NaOH or HCl to set the desired pH.

CMC studies

A stock solution of sodium lauryl sulfate (SLS) was prepared in water or 0.004 M pH = 7.01 BRB buffer at a concentration of 0.082 M, and was diluted to the given concentration. The cuvette was charged with 3.00 cm3 SLS solution, and 12 μl stock solution of the dye in acetonitrile was added. Optical properties were measured after 1 hour equilibration.

Complexation of diMICAAc with Ag(I) ions

The cuvette was charged with 3.00 cm3 dioxane and 120 μl stock solution of the dye in acetonitrile, then silver trifluoroacetate stock solution (3.4 mM in dioxane) was added in 10 μl portions.

Laser-Scanning Cytometry and microscopy and MTT cell viability assay are presented in the Supporting Information.