Cellulose

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Degradation of the cellulosic key chromophores 2,5- and 2,6-dihydroxyacetophenone by hydrogen peroxide under alkaline conditions. Chromophores in cellulosics, XVII

  • Nele S. Zwirchmayr
  • Ute Henniges
  • Markus Bacher
  • Takashi Hosoya
  • Heidemarie Reiter
  • Martin Spitzbart
  • Thomas Dietz
  • Klaus Eibinger
  • Wolfgang Kreiner
  • Arnulf Kai Mahler
  • Heribert Winter
  • Thomas Röder
  • Antje Potthast
  • Thomas Elder
  • Thomas Rosenau
Open Access
Original Paper
  • 101 Downloads

Abstract

The dihydroxyacetophenones 2,5-dihydroxyacetophenone (2,5-DHAP) and 2,6-dihydroxy-acetophenone (2,6-DHAP) belong to the key chromophores in cellulosic materials. The pulp and paper industry targets these key chromophores in their bleaching sequences to obtain brighter products. 2,5-DHAP and 2,6-DHAP were degraded with hydrogen peroxide in alkaline media, similar to conditions of peroxide bleaching (P stage) in industrial pulp bleaching. Degradation product analyses were performed by GC–MS and NMR. The degradation reaction starts by loss of acetic acid originating from the acetyl moiety of the dihydroxyacetophenones (Baeyer–Villiger rearrangement). Further reaction steps involve introduction of another hydroxyl group at C-1 (previously acetyl bearing), and further oxidation of the resulting trihydroxybenzene to quinone intermediates which are ultimately degraded to a mixture of low-molecular weight carboxylic acids.

Graphical Abstract

Keywords

Cellulose Chromophores Yellowing Brightness Bleaching Peroxide bleaching Quinones Dihydroxyacetophenones 

Introduction

Chromophores in cellulosic materials are survivors of pulp bleaching or are being (re)formed in aged samples. They are present in very low amounts, often as low as ppm to ppb values. Although the amounts are minute, the chromophores’ high extinction coefficient makes them immediately visible to the human eye (Schedl et al. 2016). For the pulp and paper industry this results in a need to improve bleaching sequences in order to obtain brighter products with little tendency toward discoloration or “brightness reversion” upon aging. At the same time, also the reduction of bleaching costs and chemical consumption is a crucial aspect of chromophore and bleaching research. The determination of well-defined cellulosic chromophores has been made possible by the CRI (chromophore release and identification) method (Rosenau et al. 2004; Korntner et al. 2015). Dihydroxyacetophenones form part of the key chromophores detected in aged pulp and cellulose. The two most important dihydroxyacetophenones in the key chromophore “family” are the constitutional isomers 2,5-dihydroxyacetophenone (2,5-DHAP, 1) (Schedl et al. 2016) and 2,6-dihydroxyacetophenone (2,6-DHAP, 2) (Rosenau et al. 2004). Of these two isomers, 2,5-DHAP is the stronger one by Vis absorption. Both 1 and 2 match the other key chromophores’—2,5-dihydroxy-1,4-benzoquinone (DHBQ) and 5,8-dihydroxy-[1,4]-naphthoquinone (DHNQ)—behavior in reaction conditions encountered in chemical pulp bleaching. Moderate solubility in aqueous environment and high stability towards oxidants are among the well-known characteristics of DHBQ, DHNQ, and the DHAP isomers (Hosoya et al. 2013a, b). The key chromophores’ characteristic passivity and easy reformation upon aging originates in their remarkable molecular structure. Hydroxyl groups in immediate proximity to carbonyl functions result in H-bonding in acidic and solid state. In alkaline media, deprotonation results in delocalized double bonds and increased stabilization, as depicted in Scheme 1. The ortho-quinoid forms 1′ and 2′ (Scheme 1), which in a way “anticipate” the quinoid state, are the reason why the compounds are much less prone to oxidation than one would reasonably expect from their structure as phenols. This stabilization effect is especially important when bleaching at alkaline pH, as in a peroxide stage (P stage). Traditional industrial bleaching agents attack localized double bonds, a reaction that is hindered in these chromophores due to precisely these attributes, delocalization of electrons and high symmetry (Rosenau et al. 2011).
Scheme 1

2,5-DHAP (1) and 2,6-DHAP (2) and their anions 1a-1b and 2a-2b: stabilization by H-bonds and by resonance

In this work, we address the chemical behavior of 1 and 2 under conditions of a P bleaching stage (alkaline hydrogen peroxide), with regard to the reaction mechanism of the degradation, and its products, by analogy to previous studies of DHBQ and DHNQ (Hosoya and Rosenau 2013a, b; Zwirchmayr et al. 2017). Kinetic experiments were performed at room temperature and at temperatures as high as 80 °C. This allowed reaction order determination and the construction of Arrhenius plots for the determination of activation energies. The final degradation products were analyzed by GC–MS and NMR experiments.

Experimental section

Kinetic analysis by UV/Vis measurements at 50 °C, varying excesses of H 2 O 2 . 2.5 mL of the chromophore solution (0.4 mM of 1 or 2) in borax buffer at pH 10 were put into a quartz cuvette. The spectra of 1 and 2 were recorded from 700 to 200 nm and the wavelengths of the highest absorption selected (380 nm for 1 and 388 nm for 2). Excess amounts of H2O2 (30%) of 100, 150, 250, 300, 500, 700, 900 and 1100 molar equivalents were added to the cuvette containing the chromophore solution and the degradation was followed at 50 °C for 5 min. The obtained data was plotted for kinetic analysis and determination of reaction order.

Kinetic analysis by UV/Vis measurements and temperature variation. 2.5 mL of the chromophore solution (0.4 mM of 1 or 2) in borax buffer at pH 10 were put into a quartz cuvette. H2O2 (30%, 300 molar equivalents) was added and the degradation was followed for 3 min at the wavelengths of 388 nm (1) and 380 nm (2) at constant temperature. The reaction temperatures were varied between 36 and 80 °C.

GCMS analysis of degradation products. 1 (12 mg, 0.081 mmol) and 2 (14 mg, 0.093 mmol) were dissolved in in 11.9 and 11.6 mL of borax buffer at pH 10, respectively. H2O2 (30%, 200 molar equivalents) was added. The degradation reaction was quenched with Na2S2O3 after 60 min of reaction time. For GC–MS analyses, the sample pH was adjusted to neutral by addition of aqueous HCl. 230 µL (1) and 235 µl (2) of the sample solution were added to a GC vial for freeze-drying. Standard addition, derivatization and sample analysis were performed according to the literature procedure, which also reports the GC–MS operating conditions (Liftinger et al. 2015) The NIST/Wiley 2008 database was used for compound identification.

NMR analyses of the degradation mixture. For NMR analysis, either 1 (2.61 mg, 0.017 mmol) or 2 (2.60 mg, 0.017 mmol) were dissolved 0.6 mL of borax buffer at pH 10. A few drops of D2O and 4,4-dimethyl-4-silapentane-1-sulfonic acid (DSS) as the internal standard were added and spectra recorded with the use of a solvent suppression technique. H2O2 (30%, 5 molar equivalents) was added and 1H, HSQC, and HMBC spectra were recorded 5 min after addition and again after 24 h. Peaks were assigned by NMR databases, by comparison with spectra of standards, and by comparison with the GC–MS results.

Isolation of pyrogallol. 2 (0.5 g, 3.29 mmol) was dissolved in 55 mL of borax buffer at pH 10. H2O2 (30%, 2 molar equivalents) was added and the solution stirred for 48 h. A peroxide test (Millipore Sigma, colorimetric test strips) showed no residual peroxide in the reaction solution. The aqueous solution was extracted first with CH2Cl2 and subsequently with ethyl acetate (EtOAc). The EtOAc extract was dried with Na2SO4, filtered and the solvent distilled off. The residue was used for column chromatography (solvent gradient: CH2Cl2/CH2Cl2+20% acetonitrile (ACN)/ACN+20% CH2Cl2/MeOH+5% acetic acid). The fractions were analyzed by TLC and the purest fraction used for NMR and GC–MS analysis. For GC–MS analyses, 1.4 mg of the substance were dissolved in 350 µL EtOAc. 100 µl of this solution were put in a GC vial and further diluted with 300 µl of EtOAc. Derivatization were performed according to the literature procedure, see above (Liftinger et al. 2015) Methyl α-D-galactopyranoside was used as an internal standard. The NIST/Wiley 2008 database was used for compound identification. Rf (EtOAc) = 0.81. 1H NMR δ(CD3CN/D2O): 6.64 (1H, t, 4-CH), 6.45 (2H, d, 3-CH and 5-CH). 13C NMR δ(CD3CN): 145.4 (2 and 6-C), 132.3 (1-C), 119.7 (4-C), 107.4 (3 and 5-C). MS (ESI, -), m/z (%): 133 (15), 239 (37), 342 (13, [M–H+]).

Results and discussion

Kinetic analyses of degradation reactions aim at determining reaction order and activation parameters, and thus allow conclusions as to a possible degradation reaction mechanism. For example, a reaction following pseudo-first order kinetics—with a linear correlation of ln[c] vs. time—represents one molecule bleaching agent reacting with one molecule chromophore, if the bleaching agent´s concentration can be considered constant throughout. To achieve this condition, the bleaching agent has to be present in large excess in relation to the chromophore. The reaction rate constant k of a pseudo-first order reaction can then be calculated from Eq. 1, where [DHAP]0 is the initial concentration of chromophore and [DHAP] is the concentration of chromophore at the time of measurement (Sandman 2006).
$$ \left[ {\text{DHAP}} \right]\, = \,\left[ {\text{DHAP}} \right]_{0} {\text{e}}^{{ - {\text{kt}}}} $$
(1)
Figure 1 summarizes the kinetic analyses of the degradation of 1 and 2 by alkaline H2O2, monitored by UV/Vis. The plots in the top row are constructed by variation of the H2O2 concentration over several orders of magnitude at a constant temperature of 323.15 K. The reaction rate constant k was calculated from the slope of the linear fit of the data points. The perfect linearity between ln[c] and the reaction time indicates pseudo-first order kinetics. The plots in the bottom row of Fig. 1 were obtained from temperature variation (313.15–353.15 K) at constant H2O2 concentrations of 300 molecular equivalents (arbitrarily set), these data being used for constructing the Arrhenius plots. All data were recorded at the wavelength of the highest Vis absorption, i.e. 380 nm for 1 and 388 nm in the case of 2.
Fig. 1

Kinetic analysis of the degradation of 1 and 2 by alkaline H2O2 at pH 10, followed by UV/Vis measurements. Top: Variation of the H2O2 concentration between 100 and 1100 molar equivalents at a constant temperature of 323.15 K for the determination of the reaction rate constant k from the slope of the linear fit of the data points. Bottom: Temperature variation (313.15–353.15 K) while the H2O2 concentration was kept constant at 300 molecular equivalents

The Arrhenius plots for the degradation of 1 and 2 are presented in Fig. 2, obtained by plotting ln(k) vs. 1/T [K]. The plots were used for the determination of the Arrhenius activation energy EA. The related activation parameters ΔH°, ΔS°, and ΔG° were determined according to the literature procedure from the Eyring plot, based on the thermodynamic formulation of the Eyring equation (Atkins and de Paula 2002). With the y-axis being ln(k/T) and the x-axis 1/T, ΔS° was calculated from the intercept. The Eyring plots for compounds 1 and 2 are depicted in Fig. 3.
Fig. 2

Arrhenius plots for the degradation of 2,5-DHAP (1) and 2,6-DHAP (2) by H2O2

Fig. 3

Eyring plots for the degradation of 2,5-DHAP (1) and 2,6-DHAP (2) by H2O2

The kinetic data for the alkaline-oxidative degradation of the chromophores 1 and 2 and the activation parameters calculated from the Arrhenius and Eyring plots are summarized in Tables 1 and 2, respectively.
Table 1

Kinetic data and activation parameters for the degradation of 2,5-DHAP (1) by alkaline hydrogen peroxide

T (K)

k (s−1)

Activation parameters

ΔH° (kcal/mol)

ΔS° (cal/K mol)

ΔG° (kcal/mol)

309.15

0.00112

8.18

− 45.65

22.29

313.15

0.00157

8.17

− 45.37

22.38

323.15

0.00225

8.15

− 45.58

22.88

333.15

0.00401

8.13

− 45.31

23.23

343.15

0.00602

8.11

− 45.33

23.67

EA(Arrhenius) = 8.79 kcal/mol

ΔS(Eyring)° = − 45.56 cal/K mol

Table 2

Kinetic data and activation parameters for the degradation of 2,6-DHAP (2) by alkaline hydrogen peroxide

T (K)

k (s−1)

activation parameters

ΔH° (kcal/mol)

ΔS° (cal/K·mol)

ΔG° (kcal/mol)

309.15

0.00339

9.99

− 37.59

21.61

313.15

0.00469

9.98

− 37.41

21.70

323.15

0.01050

9.96

− 36.92

21.89

333.15

0.01654

9.94

− 37.06

22.29

343.15

0.02453

9.92

− 37.27

22.71

EA(Arrhenius) = 10.60 kcal/mol

ΔS(Eyring)° = − 37.38 cal/K mol

The activation parameters were comparable for the two isomers 1 and 2. This was not necessarily to be expected because hydroquinone derivative 1 would be assumed to undergo oxidation much more readily than resorcinol derivative 2. The similarity of the activation parameters indicate that the rate determining step is not directly influenced by the substitution pattern and reactivity of the aromatic ring. This was confirmed by the mechanistic studies below. In similar experiments with DHNQ and DHBQ at 323.15 K, the reaction rate constant k was calculated to be twice as high for DHBQ compared to DHNQ and 2,6-DHAP (0.0261, 0.0115 and 0.0105, respectively) and the k value of compound 1 (0.00225) was only about a tenth of DHBQ´s. This behavior is reflected in the kinetics, with the slope of the curves for compound 1 being visibly less steep in the ln(A) vs. time graphs (Fig. 1). At 323.15 K, activation parameters were comparable between DHNQ, 2,6-DHAP, and 2,5-DHAP. DHBQ, however, had a higher (more positive) value for ΔH° (15.5 kcal/mol as compared to 11.1 kcal/mol for DHNQ, 8.15 kcal/mol for 2,5-DHAP), and 9.96 kcal/mol for 2,6-DHAP) and higher (more positive) values for ΔS° (− 23.6 cal/K mol compared to − 33.23 cal/K mol (DHNQ), − 45.58 cal/K mol (2,5-DHAP), and − 36.92 cal/K mol (2,6-DHAP)). ΔG° values were quite close to each other for all four chromophores (between 21.8 and 23.2 kcal/mol).

For both compounds 1 and 2, ΔG° was about twice as large as ΔH°, indicating a large entropic influence. The large negative value of ΔS° means a higher degree of order in the rate-determining transition state compared to the starting structures of this elemental step. This is highly indicative of an intermolecular process, involving both the chromophore and the co-reactant—in our case H2O2 or a derived species. A fragmentation reaction, i.e. an intramolecular process, as the rate-determining step would exhibit a positive activation entropy with a less-ordered transition state, which can be ruled out based on the experimental data (Zwirchmayr et al. 2017). The obtained results of a pseudo-first order reaction with similar activation parameters (and thus similar rate-determining steps) for the two chromophores were the base of the mechanistic considerations below.

Degradation reaction mechanism and degradation product analysis

The two chromophores 1 and 2 are constitutional isomers. The degradation kinetics of 1 and 2 were comparable, with k and activation parameters of the two compounds being in the same range. From a reaction mixture of the H2O2 degradation of 2, it was possible to isolate the intermediate pyrogallol (4,1,2,3-trihydroxybenzene), see Scheme 2. To form this compound, the acetyl function in 2 had evidently to be replaced by a hydroxyl group. Thus, a Baeyer–Villiger type oxidation reaction (BVO) had occurred. Literature offers many examples of acetophenones being oxidized according to this reaction type, with an OH-group being the newly introduced substituent (Grein et al. 2006). From the viewpoint of yield in organic synthesis, hydrogen peroxide is by no means the oxidant of choice in BVO reactions. Usually, peroxyacids are preferred, and H2O2 is known to require catalysts for efficient conversion. However, its reputation as an environmentally benign oxidizer has brought H2O2 more attention recently (Brink et al. 2004; Uyanik and Ishihara 2013). The fact that usually catalysts are involved in BVO reactions with H2O2 matches the observed kinetics of the chromophore degradation: the bleaching of 2,5-DHAP and 2,6-DHAP was slow compared to other key chromophores degraded under similar conditions (Hosoya and Rosenau 2013a, b, Zwirchmayr et al. 2017) and only elevated temperatures of 323.15 K made kinetic measurements possible at a reasonable time scale of several minutes until full decoloration of the solutions, compared to several hours at room temperature.
Scheme 2

Detailed mechanism of the Baeyer-Villiger oxidation/rearrangement as the initial step in the alkaline oxidation of 1 and 2 by hydrogen peroxide, followed by alkaline saponification of the formed phenyl acetate derivatives

Oxidation of pyrogallol on air is known to lead to the red chromophore purpurogallin (Barltrop and Nicholson 1948, Duerckheimer and Paulus 1985). We did not find any purpurogallin in the liquid reaction mixtures in our NMR experiments, but when isolating pyrogallol (4) as an intermediate, the formation of a black, inseparable precipitate in the column during fractionation was evident. From that it can be concluded that purpurogallin is not formed under the applied degradation conditions (alkaline, aqueous environment; large excess of H2O2). Instead, oxidation of pyrogallol leads to an ortho-quinone (3-hydroxy-1,2-benzoquinone, 6) (Corbett 1966, Juretic et al. 2013). An analogous BVO reaction in the degradation of 1 generates hydroxyhydroquinone (3, hydroxyquinol, 1,2,4-trihydroxybenzene). At pH 10, the degradation reaction starts by deprotonation and formation of the anions of 2,5-DHAP (1a) and 2,6-DHAP (2a), respectively. Deprotonation occurs always at the 5-OH group in 2,5-DHAP and at the 6-OH group in 2,6-DHAP. These phenolic hydroxyls are more acidic than the 2-OH of which the hydrogen is engaged in the strong hydrogen bond to the neighboring carbonyl oxygen.

The nucleophilic attack of the oxidant hydrogen peroxide at the carbonyl carbon is the rate-determining step, which is followed by the actual Baeyer–Villiger rearrangement into the Criegee intermediate, an ester (phenyl acetate derivative) that is immediately saponified under the alkaline reaction conditions. The outcome of this process is the loss of the acetyl group of the acetophenones as acetate, and a hydroxylation of the aromatic core at the position of the former acetyl moiety (C-1), see Scheme 2.

The isomeric benzenetriols 3 and 4, the primary oxidation products, were easily further oxidized into the corresponding intermediate quinones (Scheme 3), para-quinone 5 and ortho-quinone 6, which is in agreement with the literature (Corbett 1970a, b). Compound 5 can also be present in its tautomeric ortho-quinoid form 7, while 6 evidently has no para-quinoid tautomers due to its 1,2,3-substitution pattern. The ortho- and para-forms 5 and 7 are energetically very similar as concluded from computations at the M062X/6-311++g(d,p) level of theory. Their energy difference is only 3 × 10−6 kcal/mol and thus not within the accuracy of chemical determination methods (Cramer 2004).
Scheme 3

Formation of hydroxy-muconic acid derivatives 8 and 9 from the intermediate quinones 6 and 7. Further oxidation produces small carboxylic acids (shown as their anions) as final degradation products, which were confirmed in the reaction mixture

Degradation of the formed quinones continues by further oxidation by H2O2, hydrolysis and/or attack of hydroxyl ions. In any case, the muconic acid derivatives 2-hydroxy-muconic acid (8) and 3-hydroxymuconic acid (9) are obtained, a process which is well-known for the oxidative degradation of trihydroxybenzenes in alkaline media (Boeseken and Engelberts 1931; Corbett 1966a, b). The OH-substituent in 8 is able to undergo rearrangement from the position 2 to position 3, resulting in muconic acid derivative 9 (see Scheme 3).

The two muconic acids, in turn, are further degraded into small carboxylic acids according to a complex system of parallel and subsequent reactions. No aldehydes were observed. Although aldehydes could be primary intermediates of quinone-ring opening, their oxidation to carboxylic acids is very fast under the prevailing oxidative conditions (Criegee 1975). An overview of the final degradation products as analyzed by NMR and GC–MS can be found in Table 3 for the degradation of compound 1 and in Table 4 for its structural isomer 2.
Table 3

Final products of the degradation of 2,5-DHAP (1) by alkaline H2O2

2,5-DHAP (1) degrad. prod.

1H chemical shift (ppm)

13C chemical shift (ppm)

GC–MS m/z

rt (min)

MW (g/mol)

Acetic acid

s, 1.99

23.50, 181.54

60.05

Oxalic acid

b

 

190, 149, 148, 147, 133, 131, 117

13.03

90.03

Malonic acid

3.35

47.81, 177.29

233, 150, 149, 148, 147, 143, 133, 131, 117

15.16

104.06

Maleic acid (fumaric acid)

6.18

130.47, 175.42

247, 246, 245, 171, 157, 156, 155, 149, 148, 147, 144, 143, 133, 131, 128, 127, 126 117

19.18

116.07

Succinic acid

2.65

43.63a

247, 172, 147, 129

18.26

118.09

Formic acid

8.45

169.7

46.03

2,3-oxirane dicarboxylic acid

3.61

54.98, 174.1

132.07

Malic acid

Concentration too low

Concentration too low

245, 234, 233, 191, 190, 189, 175, 149, 148, 147, 133, 131, 117

23.22

134.09

The 1H and 13C chemical shifts are given in ppm. Wherever possible, 13C shifts were derived from 2D NMR spectra (HSQC, HMBC). GC–MS data is referring to the trimethylsilyl ester derivatives of the substances, minimum threshold 1%. Molecular weights are given for the non-derivatized substance in protonated (acid) form

a13C shifts were only partly obtained from 2D NMR spectra

bSubstance not detectable by 1H NMR in aqueous medium

Table 4

Final products of the degradation 2,6-DHAP (2) by alkaline H2O2

2,6-DHAP (2) degrad. prod.

1H chemical shift (ppm)

13C chemical shift (ppm)

GC–MS m/z

retention time (min)

MW (g/mol)

Acetic acid

1.93

25.43, 181.15

60.05

Oxalic acid

c

 

219, 190, 149, 148, 147, 133, 131, 117

13.04

90.03

Malonic acid

3.36

51.36b

233, 150, 148, 149, 147, 143, 133, 131, 117

15.16

104.06

Maleic acid (fumaric acid)

6.03

a

245, 155, 149, 148, 147, 143, 133, 131, 126, 117

18.03

116.07

Succinic acid

2.61

42.46b

247, 173, 172, 149, 148, 147, 133, 131, 129, 117, 116

18.26

118.09

Formic acid

8.46

a

   

2,3-Oxirane dicarboxylic acid

3.35

51.36

   

Malic acid

concentration too low

concentration too low

245, 234, 233, 191, 190, 189, 175, 148, 147, 133, 131, 117

23.22

134.09

The 1H and 13C chemical shifts are given in ppm. Wherever possible, 13C shifts were derived from 2D NMR spectra (HSQC, HMBC). GC–MS data is referring to the trimethylsilyl ester derivatives of the substances, minimum threshold 1%. Molecular weights are given for the non-derivatized substance in protonated (acid) form

a13C shift could not be derived from 2D NMR spectra

b13C shifts were only partly derived from 2D NMR spectra

cSubstance not detectable by 1H NMR in aqueous medium

Degradation product analysis

Products of the oxidative degradation of 1 and 2 were analyzed by GC–MS and NMR spectroscopy measurements. GC–MS used a previously developed analysis method for mixtures of acids, aldehydes, ketoacids and hydroxyacids in complex matrices that is based on oximation/trimethylsilylation. The analytical results agree largely with those from similar bleaching experiments (Juretic et al. 2013; Pillar et al. 2014, 2015). The products are the same for both chromophores, which is a result of the degradation pathway as delineated above, involving an initial Baeyer–Villiger type oxidation with acetic acid as the leaving group, subsequent oxidation of the resulting trihydroxybenzene isomers to the corresponding quinones and further oxidation under ring-fragmentation to muconic acids. The degradation of the latter results in acetic acid, oxalic acid, malonic acid, maleic acid, succinic acid, formic acid, and 2,3-oxiranedicarboxylic acid, with malic acid and oxalacetic acid as intermediates (Andreozzi et al. 2003). Under the prevailing reaction conditions all acids are deprotonated and present in the form of their anions. Apart from the organic low-molecular weight degradation products, carbonate was found as inorganic component. The total of organic degradation products and carbonate account for 66% of the carbon contained in the starting 2,6-DHAP, and 74% of starting 2,5-DHAP, respectively.

Except for oxalic acid that lacks NMR-active protons under aqueous conditions, and the short-lived intermediates malic acid and oxalacetic acid, all degradation products found in GC–MS were confirmed by in situ 1H NMR measurements, also by spiking with authentic samples. Acetic acid and formic acid were only found by NMR, as they were lost during the GC–MS derivatization process because of the high volatility of their trimethylsilyl derivatives. For details of GC–MS results and NMR shifts see Tables 3 and 4.

Conclusions

Oxidative degradation of 2,5-DHAP (1) and 2,6-DHAP (2) by alkaline H2O2 starts with an attack at the acetyl moiety and not at the aromatic ring. The degradation follows of pseudo-first order kinetics. It follows well-established pathways of acetophenone, polyhydroxybenzene and quinone degradation in alkaline and oxidative environments. Starting from the acetophenones, the loss of acetic acid and the introduction of an OH moiety in its place produces isomeric trihydroxybenzenes, which afford the corresponding quinones upon oxidation. Upon further oxidation and ring fragmentation, muconic acids are obtained which finally yielded mixtures of acetic acid, oxalic acid, malonic acid, maleic acid, succinic acid, formic acid, and 2,3-oxiranedicarboxylic acid, with malic acid and oxalacetic acid being intermediates, as well as carbonate. These products were confirmed by GC–MS and NMR, and their formation is in agreement with previous studies on hydroxybenzene oxidation (Andreozzi et al. 2003). We are reporting that the acetophenones 1 and 2 can be fully degraded by H2O2 to colorless products, but also that the bleaching reaction, in terms of faster consumption of the chromophores, greatly benefits from temperatures above r.t. Industrially, these conditions are already applied in P stage bleaching (Zwirchmayr et al. 2017). Especially for the key chromophores with acetophenone structure increased temperature is necessary. Albeit chromophoric intermediates were found (ortho- and para-quinones 5-7), it is positive for industrial bleaching that purpurogallin—a strongly colored compound formed from pyrogallol upon ambient oxidation (Barltrop and Nicholson 1948)—was not detected, neither by GC–MS nor in NMR spectra of our degradation analyses of 2. The colored quinones 5-7 are degraded quite easily in alkaline/oxidizing conditions since they lack the distinct stabilization of 1 and 2. With regard to cellulose bleaching, these results demonstrate that and how the highly stabilized acetophenone key chromophores can be fully degraded to colorless compounds under P stage conditions.

Notes

Acknowledgments

Open access funding provided by University of Natural Resources and Life Sciences Vienna (BOKU). The authors would like to thank the Austrian Research Promotion Society (FFG, project 829443) for financial support.

Supplementary material

10570_2018_1817_MOESM1_ESM.docx (583 kb)
Supplementary material 1 (DOCX 582 kb)

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© The Author(s) 2018

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors and Affiliations

  • Nele S. Zwirchmayr
    • 1
  • Ute Henniges
    • 1
  • Markus Bacher
    • 1
  • Takashi Hosoya
    • 2
  • Heidemarie Reiter
    • 3
  • Martin Spitzbart
    • 3
  • Thomas Dietz
    • 4
  • Klaus Eibinger
    • 5
  • Wolfgang Kreiner
    • 6
  • Arnulf Kai Mahler
    • 6
  • Heribert Winter
    • 6
  • Thomas Röder
    • 7
  • Antje Potthast
    • 1
  • Thomas Elder
    • 8
  • Thomas Rosenau
    • 1
    • 9
  1. 1.Division of Chemistry of Renewable Resources, Department of ChemistryUniversity of Natural Resources and Life SciencesViennaAustria
  2. 2.Graduate School of Life and Environmental SciencesKyoto Prefectural UniversityKyoto-shiJapan
  3. 3.Mondi Uncoated Fine & Kraft Paper GmbHViennaAustria
  4. 4.Evonik-DegussaHanau-WolfgangGermany
  5. 5.Zellstoff Pöls AGPölsAustria
  6. 6.SAPPI Papier Holding GmbHGratkornAustria
  7. 7.Lenzing AGLenzingAustria
  8. 8.USDA Forest Service, Southern Research StationAuburnUSA
  9. 9.Johan Gadolin Process Chemistry CentreÅbo Akademi UniversityÅbo, TurkuFinland

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