Introduction
Nitrite salts such as potassium nitrite (KNO2, E249) and sodium nitrite (NaNO2, E250) are commonly used food preservatives. They are employed in the production of “cured” meat products such as dry-cured ham, as part of a salting mixture that typically also contains sodium chloride and nitrate salts such as sodium nitrate (NaNO3, E251) and potassium nitrate (KNO3, E252) [1]. The “curing” process gives meat products a longer shelf-life, as the salts cause a barrier effect that retards microbial spoilage due to the reduced water activity (aW) that results [2]. Furthermore, the nitrite salts affect the color of the meat product and have a positive effect on its organoleptic properties. However, ingested nitrites are classified by the IARC as a group 2A carcinogen, i.e., “probably carcinogenic to humans, under conditions that result in endogenous nitrosation” [3]. This is due to the formation of nitrosating agents from nitrite in the low pH gastric environment. These in turn may react with amines or amides in vivo, leading to the production of N-nitrosamines and N-nitrosamides, some of which are known carcinogens. The World Health Organization (WHO) has specified an acceptable daily intake of 0‒0.06 mg/kg of body weight per day for nitrite ion [4]. Nitrite is also a regulated drinking water contaminant with maximum levels of 0.5 mg/L in the European Union and 1.0 mg/L in the United States and in WHO guidelines, respectively [5–7].
For the reasons outlined above, it is important to have methods for the quantitation of nitrite content of a given sample. The most commonly used method for determination of nitrite concentration in solution is a test that relies on the Griess reaction [8]. In this process, an aliquot of the sample is added to an acidic solution where protonation of nitrite (1) results in formation of nitrosonium cation 2 (NO+). This is then reacted with an appropriate aromatic amine, usually sulfanilamide 3, resulting first in the formation of the corresponding N-nitrosamine 4, and then, after further protonation, the corresponding diazonium salt 5. N-(1-Naphthyl)ethylenediamine 6 is then added, resulting in the formation of pink azo dye 7 (Scheme 1). Dye 7 has an absorption maximum at λmax = 535 nm, and the absorbance of the solution at this wavelength is measured spectrophotometrically.
In the above test, alternative arylamine and SEAr substrates have been studies in place of 3 and 7, but these have been found to be optimal [9]. The selectivity of the Griess test for nitrite over other anions derives from the fact that only nitrite is able to diazotize an arylamine under acidic conditions. Thus, other analytes, in particular nitrate ions, give a negative result. This key concept of nitrite-induced diazotization has been exploited in other nitrite probe designs. Gold nanoparticles have been surface-functionalized with covalently linked variants of 3 and 6—in the absence of nitrite, the colloidal nanoparticles are red due to a surface plasmon resonance, but addition of nitrite results in diazotization and crosslinking of the nanoparticles through the newly formed azo bonds, leading to aggregation and precipitation, and hence loss of color [10]. An alternative approach employing gold nanorods involves surface immobilization of arylamines, which are protonated under the acidic assay conditions, leading to a high positive surface charge. Nitrite induced diazotization followed by reduction (i.e., overall deamination) leads to neutral surface groups, and hence to a decreased surface charge. This in turn leads to aggregation and colour change [11]. Further variants employing gold nanostructures have also been described [12–14], as well as a system employing silver nanoparticles [15]. In addition, colorimetric nitrite probes that comprise aryl 1,2-diamine groups have been reported, the diazotization of an amine here leading to the formation of a benzotriazole instead of an azo linkage [16]. In the case of 2-arylethynylaniline colorimetric nitrite probes, diazotization leads to formation of a different heterocycle, 4(1H)-cinnolones [17,18]. An aza-BODIPY chromophore with conjugated arylamine substituents is reported to show a colorimetric response to nitrite as a result of diazotization [19]. Pyrrole has also been reported to be a colorimetric probe for nitrite, acting by a mechanism other than amine diazotization, although the exact mechanism was not disclosed [20]. Autocatalytic approaches to increase the sensitivity of colorimetric nitrite sensors have been developed [21]. Elsewhere, organometallic complexes have also been reported as colorimetric probes for nitrite [22,23].
The bicyclic aromatic compound azulene 8 (Fig. 1) has an intense blue colour, and both it and its derivatives have been extensively studied due to their unusual properties. For example, although azulene is isomeric with naphthalene, it possesses a dipole of 1.08 D, which is unexpectedly large for a hydrocarbon. In addition, its HOMO to LUMO transition lies in the visible region [24]. One characteristic of azulenes makes them especially suited to applications in colorimetric sensing. The absorption spectrum of azulene is very sensitive to the introduction of substituents onto the azulene ring, allowing access to the full visible spectrum [25,26]. Therefore, azulenes have been used in colorimetric probes for a variety of analytes [27–34]. As part of our ongoing work in the areas of azulene chemistry [35–37] and chemosensors [38], we wished to develop a probe for nitrite that exploited the diazotization of an azulenylamine to cause a visible colour change. Azulenes have been studied in the context of nitrite sensing previously: Sawicki and co-workers reported that the direct combination of azulene 8 and nitrite in acidic medium led to the formation of a species exhibiting an absorption at λmax = 617 nm, although the exact nature of this species was not determined [39]. Garcia employed azulene in a Griess test for nitrite, wherein para-nitroaniline (instead of 3) was diazotized by nitrite, then reacted with azulene 8 (instead of 6) to form the corresponding azo dye [40]. More recently, a report on a boron-containing azulene derivative describes a spectrophotometric response to nitrite [41], although nitrite sensing was not the focus of this work. Also of note, treatment of azulenes with nitrite salts has been reported to effect aromatic nitration [42,43] (as opposed to nitrosation) in certain specific cases.
Here, we report a selective colorimetric chemodosimeter for the detection of nitrite anion that relies on diazotization of an azulenylamine and subsequent formation of a diazoquinone. This is a conceptually distinct approach compared to the more common formation of an azo dye following diazotization; to the best of our knowledge, a colorimetric probe for nitrite with a diazoquinone as the end-point has not previously been reported. Crucially, our approach does not require a coupling reaction to occur between two separate reagents.
Results and discussion
Our nitrite probe, diethyl 2-amino-6-bromoazulene-1,3-dicarboxylate 9, may be synthesized in three steps from tropolone (Scheme S1), and in 71% overall yield, as previously reported by Nozoe [44,45]. Further details are given in the Electronic Supplementary Material (ESM). To evaluate the colorimetric response of 9, sodium nitrite was added to a solution of 9 in acetonitrile–water, acidified with HCl(aq) to pH 1. It is known that choice of solvent can influence both the sensitivity and selectivity of chemical probes [46–48] —in this instance the final solvent ratio MeCN/H2O was 1:1. A range of other conditions having different pH values were also assessed, but it was found that pH 1 was optimum (see ESM for details). A rapid color change was observed, with the solution changing from yellow to grey within 1 min. However, upon further standing of the test solution, a second color change was observed, with the grey color changing to orange after 10 min. These observations may be explained as shown in Scheme 2. Thus, formation of nitrosonium ion 2 from nitrite 1 in the acidic medium leads to diazotization of 9 to give azulenyldiazonium species 10, which we propose is the source of the grey color observed. Whereas in the traditional Griess test the diazonium intermediate reacts with an electron-rich arene to give a diazo product, in this instance (and in the absence of any such aryl nucleophile), 10 can instead react with the solvent. As first proposed by Nozoe [49], the presence of the electron-withdrawing diazonium group at the azulene 2-position renders the azulene 6-position electrophilic. Attack of water at this position, followed by loss of HBr, then affords stable diazoquinone 12.
In support of the above mechanism, the UV/vis spectrum of the test solution after 10 min was compared to that of an authentic sample of previously synthesised diazoquinone 12, and the two were found to exhibit the same absorption maxima (Fig. 2). Specifically, compared to unreacted probe 9, loss of the absorption maxima at λ = 320 nm and 332 nm (red line) and the appearance of new absorption maxima at λ = 318 nm and 395 nm (green line) confirm the formation of 12.
Fig.4 UV/Vis spectra of azulene 9 (S), azulene 9 and NaNO2 (S+NaNO2), and independently prepared 12 (DQ). Each vial contained the following. For S: MeCN (4.95 mL), DI water (2.00 mL), HCl(aq) (35%, 3.00 mL), and sensor 9 (50 µL, 5 mmol/L in MeCN). For S+NaNO2: MeCN (4.95 mL), DI water (1.95 mL), HCl(aq) (35%, 3.00 mL), NaNO2 (50 µL, 5 mol/L in DI water), and sensor 9 (50 µL, 5 mmol/L in MeCN). For DQ: MeCN (4.95 mL), DI water (2.00 mL), HCl(aq) (35%, 3.00 mL), and DQ 12 (50 µL, 5 mmol/L in MeCN) |
The dose-response characteristics of chemodosimeter 9 towards nitrite were then assessed (Fig. 3). It was observed that increasing equivalents of nitrite caused an increase in absorbance at λ = 318 nm, and a proportional increase in absorbance at λ = 395 nm (of diazoquinone 12), and a decrease in the absorbances at λ = 320 nm and 332 nm (of probe 9). The intensity of absorbances due to diazoquinone 12 showed no further increase once an excess of nitrite was present in solution (with respect to 9), suggestive of a 1:1 dose-response relationship. The 1:1 stoichiometry was further evidenced with a Job plot and calibration curve, the latter showing that the absorbance at 395 nm reaches a plateau once one equivalent of nitrite is added (See Fig. S1 and Fig. S2 of ESM).
Fig.5 Dose-response of probe 9 against increasing equivalence of NaNO2. Results taken after 20 min of nitrite addition to allow full conversion to diazoquinone 12. Titration was performed in a mixture of MeCN (4.95 mL), DI water (2.00 mL) and HCl(aq) (35%, 3.00 mL), with probe 9 (50 µL, 5 mmol/L in MeCN) and subsequent aliquots of analyte (10 µL, 5 mmol/L in DI water) |
We next examined the selectivity of probe 9 for nitrite over a variety of other anions. As shown in Figs. 4 and 5, 9 exhibited no response to chloride, bromide, iodide, hydrogen sulfate, bicarbonate and hydrogen phosphate under the same conditions. Most significantly, 9 also showed no response to nitrate; difficulty in discriminating between nitrite and nitrate is known to be a characteristic of certain probe designs [50].
An advantage of nitrite probe 9 is the rapidity of its response to nitrite under the assay conditions, and the speed with which the grey color of 10 develops. Achieving a color change visible to the naked eye within a minute compares favorably to most protocols based on Griess reactions. As 10 is not the end-point for this assay, the appearance of the grey color must be interpreted in a qualitative sense only, and quantitation of nitrite should be based on the absorbances arising from diazoquinone 12, which forms more slowly. Nevertheless, this feature of our probe provides additional information to the experimentalist. Quantitation of the probe’s response to the other potentially interfering anions was carried out by measuring the absorbance at the maximum at 395 nm, as shown in Fig. 6.
The detection limit of sensor 9 was also determined. For instrumental (spectrophotometric) detection, the limit of detection was determined to be 0.23 mg/L nitrite. A naked-eye detection limit experiment was also performed (see ESM for details), and sensor 9 was found to show a clear visible response to nitrite at concentrations of≥50 mg/L. In addition, kinetic studies were undertaken (see ESM for details) which indicated a relationship between analyte concentration and rate of color change.
To assess the feasibility of using sensor 9 in a practical scenario, the nitrite content of a sample of cured meat was assessed. Sodium nitrite was extracted from commercially available pepperoni using the methodology described by the British Standards ‘Method of test for meat and meat products—Determination of nitrite content’ (BS 4401-8) [51]. Assaying the extract with azulene probe 9, it was determined that the nitrite concentration in the pepperoni tested was 10.3 mg/kg (see ESM for details). For comparison, using the Griess methodology described by the British Standards procedure, a nitrite concentration of 10.8 mg/kg was determined.
Conclusions
Azulene probe 9 was synthesised over three steps with an overall yield of 72%. The compound was shown to change color rapidly in the presence of nitrite under acidic conditions, forming diazoquinone 12. This process was shown to be highly selective for nitrite over other common anionic analytes, allowing 9 to act as a selective, 1:1 colorimetric chemodosimeter for nitrite. The applicability of the sensor was demonstrated by testing nitrite content in cured meat, for which a result was obtained that was comparable to that acquired using the current British Standard of testing. Advantages of our method include the rapidity of the initial color change (formation of the diazonium intermediate) and the requirement to prepare only a single stock solution of the reagent, as opposed to the multiple stock solutions required for the Griess reagents.