Hydroxyl radical scavenging by ethyl gallate and related compounds: a method for rapid evaluation
Transcript of Hydroxyl radical scavenging by ethyl gallate and related compounds: a method for rapid evaluation
ELSEVIER Pharmaceutics Acta Helvetiae 7 I (1996) 22 I -224
Hydroxyl radical scavenging by ethyl gallate and related compounds: a method for rapid evaluation
G. Hall, T.T.T. Le, J.B. Stanford, J.K. Sugden *
Department of Pharmaceutical Sciences, School of Applied Scirnces, De Mowfort (/nicer.+?, The Gatewu~, Leicestrr LEl 9RH, l/K
Received 5 August 1995: accepted 13 September 1995
Abstract
Ethyl gallate and two related compounds, ethyl 4-hydroxybenzoate and ethyl 3,4-dihydroxybenzoate were evaluated as hydroxyl radical scavengers in a model system using dequalinium chloride and hydrogen peroxide irradiated with simulated sunlight to generate the radicals. All of the compounds showed some hydroxyl radical scavenging properties, with ethyl 3,4-dihydroxybenzoate being the most active under the conditions of test. The molecular implications of these results are considered. The potential radical scavengers were assessed individually for their reaction with photogenerated hydroxyl radicals and the results are discussed. The potential applications of this method for evaluating potential preservatives are also discussed.
Kewordst Hydroxyl radical: Hydroxybenaoate; Scavenger: Photogenerated
1. Introduction
Medicines, cosmetics and foods are all subject to oxida- tion, leading to the formation of unpleasant flavours, odours and the formation of toxic substances all of which consti-
tute product spoilage. It is normal good manufacturing practice to incorporate antioxidants to reduce the instance of these spoilage reactions (Scott, 1965; Stuckey, 1972).
Antioxidants can be classified as either reducing agents or free radical scavengers. In the latter case, the antioxidant acts as a chain breaking agent in the three stage process of
initiation, propagation and termination in which products are oxidised by a free radical reaction (Chamsi, 1986; Kirby, 1988). Antioxidants react with free radicals to form stable products which prevent the reaction progressing, a primary stage in the free radical mediated decomposition of fatty material is either electron or hydrogen donation
and that the antioxidant forms a loose complex with the
I Corresponding author.
fatty chain. Bollard and Ten Have (1947) reported that the reaction between hydroquinone and ethyl linoleate was a two stage process involving the formation of a semi- quinone radical, two of which combined to give quinone
and hydroquinone, thus acting as an antioxidant. The antioxidant effects of ring substituted phenols in
food oils have been investigated (Wu et al., 1993; Namiki
et al., 1993) leading to the conclusion that ring substitution with bulky alkyl groups yields products which are oil soluble, less volatile and toxic as well as being reasonably
effective antioxidants. Recent work has shown that pheno- lit acids are relatively ineffective at retarding the rates of
autoxidation at 100°C (Marinova and Yanishlieva, 1994). The objective of the present work is to extend the
investigation of ring substituted phenols to encompass aqueous systems with particular reference to hydroxyl radicals which can be generated in aqueous systems, par- ticularly in the presence of substances, which can act as
sensitizers. Hydroxyl radicals can also be generated in aqueous solutions in which there are transition metal ions, derived from manufacturing equipment. that could cause
003 I-6865/96/$15.00 Copyright 0 1996 Elsevier Science B.V. All rights reserved PII SOO31-6X65(96)00013-1
222 G. Hall et al. /Pharmaceutics Acta Helvetiae 71 (1996) 221-224
Fenton reactions (Fenton, 1894), which lead to product spoilage. Previous workers (Pate1 and Sugden, 1992; Ho et al., 1994; Allman et al., 1995) have shown that dequalin- ium chloride in the presence of hydrogen peroxide is decomposed in visible light by a hydroxyl radical mediated reaction. This reaction has been used as a model system in which to determine the effect of potential hydroxyl radical scavengers by measuring the rate constant of this reaction with and without the test compounds.
2. Procedures
2.1. Chemicals
Dequalinium chloride (Sigma Chemical Co., batch no.
124F06081, ethyl gallate (NIPA Co., batch no. 8001, ethyl 3,4_dihydroxybenzoate (Aldrich Chemical Co., batch no 5063), ethyl 4-hydroxybenzoate (Aldrich Chemical Co., batch no 44703) hydrogen peroxide (Aldrich Chemical Co., batch no. 28141). Ethyl N-methyl-4-hydroxy-5-oxo-
3-pyrroline-3-carboxylate (De Montfort University, Leices- ter).
Evans et al. (1975) and absorbance readings were taken at 326 nm at time zero and then every fifteen minutes for a further 2 h to measure the residual dequalinium chloride. The irradiated control solutions were used as the blank in the spectrophotometric assay of the residual dequalinium chloride. Another series of solutions of the hydroxyben- zoates was made in which each compound (30 mg) was dissolved in deionised water and made up to 250 ml. Aliquots of 220 ml were taken and hydrogen peroxide (1 ml, 30% v/v> added. A 1 in 10 dilution of these solutions was made and the diluted solutions irradiated as described
above; uv/visible scans being taken at time zero and at hourly intervals up to 7 h. Attempts to repeat this work
with more concentrated solutions were unsuccessful since the rate of reaction was too slow to be measured in reasonable time.
2.5. Treatment of results
2.2. Apparatus
Photoreactor Unit (Evans et al., 1975), Cecil Uv/visi- ble spectrophotometer Model CE 272, Beckman Uv/visi-
ble spectrophotometer Model DU 70.
Linear regression analyses were made of plots of the percentage residual dequalinium chloride, the log of the
percentage residual dequalinium chloride and the recipro- cal of the percentage residual dequalinium chloride against time. The plot giving the largest linear regression coeffi-
cient was deemed to represent the order of reaction (Pate1
and Sugden, 1992). The rate constants were calculated from the slopes of the graphs (Florence and Attwood,
1981).
2.3. Beer Lambert plot of dequalinium chloride 3. Results and discussion
A stock solution of dequalinium chloride (50 mg/lOO ml) was prepared in deionised water. Serial dilutions for
this solution were prepared (5, 10, 20, 30, 40, 50 mg/lOO ml> and the absorbance measured at 326 nm. Linear re- gression analysis of the mean of two sets of readings gave
a regression coefficient of 0.9994 (p = 0.0001).
The results of the irradiation of the solutions of de- qualinium chloride with the various substituted phenols are shown in Table 1.
Irradiation of the additives alone in deionised water gave no evidence of photochemical degradation.
2.4. Preparation and irradiation of solutions
Solutions of dequalinium chloride in deionised water (O.O25%w/v) were prepared and filled into Dreschel bot- tles (300 ml>. A second series of solutions was prepared and hydrogen peroxide (0.03% v/v> added before the Dreschel bottle was made up to volume. Separate solutions of dequalinium chloride (0.025% w/v> in deionised water were prepared containing selected amounts of the test compounds with respect to dequalinium chloride and hy- drogen peroxide (0.03% v/v>. A separate series of con- trols were prepared in which the dequalinium chloride was omitted. All the solutions were irradiated by the method of
Ethyl N-methyl-4-hydroxy-5-oxo-3-pyrroline-3-
carboxylate was used since it has a planar structure and an acidic hydroxy group like those of phenols. The evidence from the use of ethyl N-methyl-4-hydroxy-5-oxo-3-pyrro- line-3-carboxylate shows that this compound does not act as a hydroxyl radical scavenger which indicates that the presence of an aromatic ring rather than a n cloud of electrons in C=C and C =0 bonds incorporated in a ring system is essential for hydroxyl radical scavenging in the
test system. Examination of the results (Table 1) shows that of the
hydroxybenzoates tested ethyl 3,4_dihydroxybenzoate has the greatest effect in scavenging hydroxyl radicals, ethyl gallate (ethyl 3,4,5_trihydroxybenzoate) is less active which suggests that the hydroxyl radical scavenging effect is not
G. Hall et al. / Pharmaceutics Acta Helvetiae 71 (1996) 221-224 223
solely related to the number of hydroxyl groups on the
aromatic ring but also to their position with respect to the ester group
Raghaven and Steenken (1980) have reported that phe- nols are usually attacked by hydroxy radicals in the 2 and 4 positions in acid or neutral solutions (deionised water
used in this work had a pH of 6.1) to give a dihydroxy compound. Consideration of ethyl 4-hydroxybenzoate shows that hydroxylation can occur at C3 and C5 which
are activated by the phenolic hydroxy group. In the case of ethyl 3,4_dihydroxybenzoate (II) the 3-hydroxy group will activate C2 and C6, whilst the 4-hydroxy group will activate C5. In the case of ethyl gallate (III) only C2 and
C6 are available for hydroxylation and both of these are subject to steric hindrance from the ester group at Cl and also deactivation due to the ester carbonyl group. Conse- quently, some explanation of the greater hydroxyl scaveng- ing properties of (II) can be offered from consideration of
the availability of accessible hydroxylation sites. Examination of Table 2 shows that on irradiation with
hydrogen peroxide in deionised water the ethyl hydroxy- benzoates decompose, the reactions following first order
kinetics. The rate constants show that ethyl gallate decom- poses at the greatest rate, followed by that of ethyl 4-hy- droxybenzoate and the slowest reaction being that of ethyl
Table I Photodegradation of dequalinium chloride (DC) (0.025% w/v)
Table 2
Photodegradation of ethyl hydroxybenzoates (O.O012%‘c) + hydrogen per-
oxide
Compounds Reaction order Rate constant min-’
Ethyl 4-hydroxybenzoate 1st 4.82~ lo-’
Ethyl 3,4-dihydroxybenzoate 1st 2.12x lo-?
Ethyl gallate 1st 7.42~ lo-’
3,4-dihydroxybenzoate. Ethyl 4-hydroxybenzoate has been shown to be the least effective hydroxyl radical scavenger of those tested. The relative positions of ethyl 3,4-dihy- droxybenzoates and ethyl gallate do not relate precisely with the results from the tests on the model system with dequalinium chloride, which could be due to a number of
factors, including insensitivity of the analytical method. However, the uv/visible spectra of the mixtures showed considerable changes from those of the pure compounds in deionised water. In the case of ethyl 4-hydroxybenzoate
there were shifts in the primary aromatic peak from 216 nm to below 200 nm and in the wavelength maxima of the
second absorption band from 256 to 255 nm. The spectrum of ethyl 3,4_dihydroxybenzoate showed slight shifts in the primary aromatic band and in the wavelength maximum of
the other absorption band from 260 nm to 255 nm. The spectrum of ethyl gallate showed a slight shift of the primary aromatic band and in every case these changes in
wavelength were accompanied by increases in absorbance. During irradiation with simulated sunlight all of the ab-
sorption bands showed a progressive reduction in intensity. Raghaven and Steenken (1980) have shown that hydroxyl
radicals convert phenols to the corresponding phenoxy radical which has increased absorption in the uv/visible
spectrum. The phenoxy radical undergoes further reactions leading ultimately to dihydroxybenzenes. This would sug- gest that the rates of the reaction between the hydroxyben-
zoates and hydroxyl radicals would need to be faster than
Compounds Reaction order Rate constant min-’ d
DC alone
DC+H,O,
DC + H;O; + ethyl gallate (0.025% w/v)
DC+ H,O? +ethyl gallate (0.05% w/v)
DC + H,O, + ethyl 3,4_dihydroxybenzoate (0.025% w/v)
DC + H,O, +ethyl 3,4_dihydroxybenzoate (0.05% w/v)
DC + H;Oi + ethyl 4-hydroxybenzoate (0.025% w/v)
DC + HZOZ + ethyl 4-hydroxybenzoate (0.05% w/v)
DC + Hz02 + ethyl N-methyl-4-hydroxy-5-oxo-3-pyrroline-3-carboxylate (0.025% w/v)
DC + H202 + ethyl N-methy1-4-hydroxy-5-oxo-3-pyrroline-3-carboxylate (0.05% w/v)
li Mean of three sets of results
I St 1 St
1st
1st
I St
1st
1st
1st
1st
1 St
0.32~ IO-’
2.390x IO_’
0.392~ IO-’
0.191 x IO_ 1
0.186X IO_ J
0.160~ lo-’
0.560~ IO-’
0.520~ lo-’
1.48X lo-?
1.07x IF2 -
224 G. Hall et al. / Pharmaceutics Acta Heluetiae 71 (1996) 221-224
that between the dequalinium chloride and hydroxyl radi- cals for the hydroxybenzoates to act as antioxidants. The hydroxyl radical scavenging properties of ethyl gallate are in the system tested inferior to those of ethyl 3,4-dihy-
droxybenzoate but they show a much greater concentration
effect. In the cases of ethyl 3,4_dihydroxybenzoate and ethyl 4-hydroxybenzoate the effect of doubling the concen- tration is not nearly so marked as it is with ethyl gallate. The main advantage of using this technique is that results can be obtained within a working day and it can be used to
assess a number of potential antioxidants in an aqueous system using the same drugs and additives as are intended for the product formulation with consequent cost savings.
References
Allman, J., Ho, A.H.L., Ranson, C., and Sugden, J.K. (1995) Effect of
food dyes on radicals in aqueous media. Int. .I. Pharm., 115, 241-243.
Bollard, J.L. and Ten Have, P. (1947) Kinetic studies in the chemistry of
rubber and related materials IV Inhibitory effects of phenolic com-
pounds on the thermal oxidation of ethyl linoleate. Trans. Farad. Sot.,
43,201-210.
Chamsi, A.Y. (1986) Volumetric determination of antioxidants and other
species. Ph.D Thesis. Loughborough University, UK.
Evans, P.G.E., Sugden, J.K. and Van Abbe, N.J. (19751 Aspects of the
photochemical behaviour of I-hydroxypyridine-2-thione. Pharm. Acta.
Helv., 50, 94-99.
Fenton, H.J.H. (1894) Oxidation of tartaric acid in the presence of iron. J.
Chem. Sot., 899-910.
Florence, A.T. and Attwood, D (1981) Physico-Chemical Principles of
Pharmacy, Macmillan, London, P 459.
Ho, A.H.L., Popat, SC. and Sugden, J.K. (1994) Some effect of metal
ions on the photogeneration of hydroxyl radicals. Int. J. Pharm. 104,
247-251.
Kirby, R. (1988) Studies on the stability and antioxidant properties of
butylated hydroxyanisoles. M.Sc. Thesis. Loughborough University.
UK.
Marinova, E.M.M. and Yanishlieva, N.V. (1994) Effect of lipid unsatura-
tion on the antioxidative activity of some phenolic acids. J. Am. Oil.
Chem. Sot., 71, 421-434.
Namiki, M., Yamashita, K. and Osawa, T. (1993) Food related anti-
oxidants and their activities in vivo. Act. Oxygens Lipid Peroxides
Antioxid. 319-332.
Patel, R and Sugden, J.K. (1992) Photodegradation of aqueous solutions
of dequalinium chloride. Pharmazie, 47, H 2, 113- 115.
Raghaven, N.V. and Steenken, S. (1980) Electrophilic reactions of the
hydroxyl radical with phenols. Determination of the distribution of
isomeric dihydroxycyclohexadienyl radicals. J. Am. Chem. Sot.,
102(10), 3495-3499.
Scott, A.G. (1965) Atmospheric oxidation and antioxidants. Elsevier,
Amsterdam.
Stuckey, B.N. (1972) Antioxidants and food stabilisers, Handbook of
Food Additives, C.R.C., Boca Raton.
Wu, Z., Yan, L., Ma, S. and Qian, G. (1993) Gallic acid derivatives as
antioxidants for edible oils. Linchan Huaxue Yu Gongye, 13, 25-31.