VITAMIN C OXIDATION IN DRINKING WATER 857formation <strong>of</strong> dehydroascorbic acid. In the controlsample where ascorbic acid had been added toMilli-Q <strong>water</strong>, very low concentrations <strong>of</strong> dehydroascorbicacid could be detected. The amount <strong>of</strong>dehydroascorbic acid formed <strong>in</strong> four commerciallysold domestic bottled <strong>water</strong> samples, after ascorbicacid addition (15 m<strong>in</strong> <strong>in</strong>cubation), was <strong>in</strong> the range<strong>of</strong> 0–3 mM.FIGURE 1 Ascorbic acid degradation (A), and dehydroascorbicacid formation (B), <strong>in</strong> household dr<strong>in</strong>k<strong>in</strong>g <strong>water</strong> 2 mM ascorbicacid was added to two household tap <strong>water</strong> samples; sample 1 (A)and sample 2 (O), a Milli-Q <strong>water</strong> sample (X) and a Milli-Q <strong>water</strong>sample supplemented with 100 mg/l bicarbonate and 0.5 mg/lcopper (W). The concentration <strong>of</strong> ascorbic acid was measured at<strong>in</strong>dicated time po<strong>in</strong>ts by us<strong>in</strong>g HPLC analysis. Dehydroascorbicacid was measured by us<strong>in</strong>g the reagent o-phenylenediam<strong>in</strong>e.Data shown are mean ^ SD <strong>of</strong> triplicates from one representativeexperiment out <strong>of</strong> three conducted.be seen <strong>in</strong> Fig. 1B, dehydroascorbic acid wasrapidly formed <strong>in</strong> the tap <strong>water</strong> sample 2. After15 m<strong>in</strong> <strong>in</strong>cubation, 638 ^ 33 mM <strong>of</strong> dehydroascorbicacid had been formed. However, at 15 m<strong>in</strong>, only87 ^ 26 mM <strong>of</strong> dehydroascorbic acid had beenformed <strong>in</strong> sample 1. Addition <strong>of</strong> 2 mM ascorbicacid to Milli-Q <strong>water</strong> supplemented with 100 mg/lbicarbonate and 0.5 mg/l copper resulted <strong>in</strong> rapidDehydroascorbic Acid Reacts with HydrogenPeroxide and Generate Oxalic Acid and ThreonicAcidA typical chromatogram <strong>of</strong> a catalytic dr<strong>in</strong>k<strong>in</strong>g<strong>water</strong> sample <strong>in</strong>cubated with 2 mM ascorbic acidfor 3 h is shown <strong>in</strong> Fig. 2A. In this chromatogram,based on retention time, the peak that appeared at5.6 m<strong>in</strong> was identified as oxalic acid (peak 1).At 5.9 m<strong>in</strong>, a peak appeared that had a retentiontime similar to the hydrogen peroxide- andthreonic acid standards (peak 2). Dur<strong>in</strong>g the 3 h<strong>in</strong>cubation 2 mM ascorbic acid (rentention time7.9 m<strong>in</strong>, peak 4) had been oxidized, <strong>in</strong> thisbicarbonate rich and copper contam<strong>in</strong>ated dr<strong>in</strong>k<strong>in</strong>g<strong>water</strong> sample to 713 ^ 63 mM dehydroascorbicacid (o-phenylenediam<strong>in</strong>e assay), 488 ^ 28 mMoxalic acid and 77 ^ 14 mM threonic acid(quantitated by us<strong>in</strong>g an anion column). Thepeak for dehydroascorbic acid (peak 3) appeared<strong>in</strong> the chromatogram at 6.8 m<strong>in</strong> together with anunknown metabolite that had a retention time <strong>of</strong>7.1 m<strong>in</strong>. In a similar way, addition <strong>of</strong> 4 mMhydrogen peroxide to 2 mM ascorbic acid <strong>in</strong>Milli-Q <strong>water</strong> supplemented with 100 mg/lbicarbonate resulted <strong>in</strong> 839 ^ 72 mM oxalic acidand 192 ^ 24 mM threonic acid with<strong>in</strong> 3 h (Fig. 2B).Moreover, very rapid formation <strong>of</strong> oxalic acid andthreonic acid could be obta<strong>in</strong>ed when 4 mMhydrogen peroxide was added to 2 mM dehydroascorbicacid <strong>in</strong> Milli-Q <strong>water</strong> supplemented with100 mg/l bicarbonate. A 10-m<strong>in</strong> <strong>in</strong>cubation at roomtemperature resulted <strong>in</strong> 640 ^ 24 mM oxalic acidand 181 ^ 24 mM threonic acid (Fig. 2C). In controlexperiments, 2 mM dehydroascorbic acidwas added to Milli-Q <strong>water</strong> supplementedwith 100 mg/l bicarbonate. In the absence <strong>of</strong>hydrogen peroxide, 79% less oxalic acid wasformed (Fig. 2D).To verify that dehydroascorbic was formed <strong>in</strong> ourdr<strong>in</strong>k<strong>in</strong>g <strong>water</strong> samples, we used DTT, a reduc<strong>in</strong>gagent that can turn dehydroascorbic acid back <strong>in</strong>toascorbic acid. When DTT was added to copper andbicarbonate supplemented Milli-Q <strong>water</strong> that hadbeen <strong>in</strong>cubated with 2 mM ascorbic acid for 3 h, theascorbic acid peak reappeared <strong>in</strong> the chromatogram(approximately 680 mM ascorbic acid was formed).Dehydroascorbic acid has previously been shown tobe spontaneously decomposed to L-diketogulonate
858P.J. JANSSON et al.[18 – 20](2,3-DKG) or erythroascorbate. Our results<strong>in</strong>dicated that dehydroascorbic acid and not DKGwas present <strong>in</strong> the sample.DISCUSSIONFIGURE 2 HPLC analysis <strong>of</strong> ascorbic acid metabolites <strong>in</strong>dr<strong>in</strong>k<strong>in</strong>g <strong>water</strong>. (A) 2 mM ascorbic acid was added to a dr<strong>in</strong>k<strong>in</strong>g<strong>water</strong> sample and <strong>in</strong>cubated at room temperature for 3 h. (B) 2 mMascorbic acid and 4 mM hydrogen peroxide was added to a Milli-Q<strong>water</strong> sample supplemented with 100 mg/l bicarbonate and<strong>in</strong>cubated for 3 h at room temperature. (C) 2 mM dehydroascorbicacid and 4 mM hydrogen peroxide was added to a Milli-Q<strong>water</strong> sample supplemented with 100 mg/l bicarbonate and<strong>in</strong>cubated for 10 m<strong>in</strong> at room temperature. The <strong>in</strong>set show thepeaks for dehydroascorbic acid (at 6.8 m<strong>in</strong>) and an unknowncompound (at 7.1 m<strong>in</strong>). (D) 2 mM dehydroascorbic acid was addedto a Milli-Q <strong>water</strong> sample supplemented with 100 mg/lbicarbonate and <strong>in</strong>cubated for 10 m<strong>in</strong> at room temperature.(E) Oxalic acid standard (0.6 mM) <strong>in</strong> Milli-Q <strong>water</strong>. (F) Ascorbicacid standard (2 mM) <strong>in</strong> Milli-Q <strong>water</strong>. Please note the differentscal<strong>in</strong>g <strong>in</strong> chromatogram F.The dr<strong>in</strong>k<strong>in</strong>g <strong>water</strong> reach<strong>in</strong>g the consumer at theirhomes can easily be contam<strong>in</strong>ated by copper ionsdue to corrosion <strong>in</strong> the copper pipes <strong>in</strong> the house(build<strong>in</strong>g). Especially, the first-draw <strong>water</strong> used <strong>in</strong>the morn<strong>in</strong>g can readily be contam<strong>in</strong>ated by copperions. [21,22] In light <strong>of</strong> these facts, and our previousstudies show<strong>in</strong>g that ascorbic acid can drive ahydroxyl radical generat<strong>in</strong>g process <strong>in</strong> copper andbicarbonate conta<strong>in</strong><strong>in</strong>g dr<strong>in</strong>k<strong>in</strong>g <strong>water</strong> [11,15] wedecided to study how fast and to what extentascorbic acid is oxidized <strong>in</strong> a copper contam<strong>in</strong>ateddr<strong>in</strong>k<strong>in</strong>g <strong>water</strong> sample. Our results show thatascorbic acid is oxidized relatively fast <strong>in</strong> bicarbonaterich <strong>water</strong> samples that are contam<strong>in</strong>ated by copperions. Approximately 32% <strong>of</strong> the <strong>vitam<strong>in</strong></strong> C had beenoxidized after 15 m<strong>in</strong> and the <strong>vitam<strong>in</strong></strong> was almostcompletely oxidized with<strong>in</strong> 3 h (Fig. 1A and B). Theoxidation process could easily be mimicked byadd<strong>in</strong>g <strong>vitam<strong>in</strong></strong> C to Milli-Q <strong>water</strong> supplementedwith 100 mg/l HCO 2 3 and 0.5 mg/l Cu 2þ because,the oxidation process require copper ions and apH around 4–5. [15]When ascorbic acid is oxidized <strong>in</strong> the presence <strong>of</strong>copper ions, dehydroascorbic acid is formed (Fig. 1B).The dehydroascorbic acid formation, <strong>in</strong> the bicarbonaterich <strong>water</strong> sample contam<strong>in</strong>ated with copper,was very rapid and up to 650 mM dehydroascorbicacid could be formed with<strong>in</strong> 15 m<strong>in</strong>. The amount <strong>of</strong>dehydroascorbic acid formed with<strong>in</strong> 15 m<strong>in</strong> <strong>in</strong> thevarious tap <strong>water</strong> samples tested were <strong>in</strong> the range <strong>of</strong>100–650 mM. On the contrary, when commerciallysold domestic bottled <strong>water</strong> was used <strong>in</strong> the assayvery modest degradation <strong>of</strong> ascorbic acid took place.Some <strong>of</strong> the bottled <strong>water</strong> samples tested (m<strong>in</strong>eral<strong>water</strong>s) were buffered with bicarbonate. However, <strong>in</strong>the absence <strong>of</strong> copper ions, oxidation <strong>of</strong> <strong>vitam<strong>in</strong></strong> Ccannot take place. This reflects the importance <strong>of</strong>copper ions <strong>in</strong> the oxidation process.HPLC analysis, performed on the <strong>water</strong> samplesthat had been <strong>in</strong>cubated with 2 mM ascorbic acid for3 h at room temperature, clearly <strong>in</strong>dicated that the<strong>vitam<strong>in</strong></strong> had been oxidized <strong>in</strong>to dehydroascorbicacid and further decomposed <strong>in</strong>to two majormetabolites, oxalic acid and threonic acid. In the<strong>water</strong> sample 2, that was contam<strong>in</strong>ated with copperions and had high concentration <strong>of</strong> bicarbonate,only 131 ^ 13 mM <strong>of</strong> the added 2 mM ascorbic acidwas left after a 3 h <strong>in</strong>cubation. Dur<strong>in</strong>g the 3 h<strong>in</strong>cubation period, the added ascorbic acid had beenoxidized to 488 ^ 28 mM oxalic acid. High concentrations<strong>of</strong> oxalic acid (calcium oxalate) are toxic and
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Pro-oxidant activity of vitamin C i
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Supervised byDocent Tommy Nordströ
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ContentsCONTENTSLIST OF ORIGINAL PU
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List of original publicationsLIST O
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AcknowledgementsACKNOWLEDGEMENTSThi
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AbbreviationsABBREVIATIONSAsc …
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Review of the literatureREVIEW OF T
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Review of the literatureSince vitam
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Review of the literaturestill added
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Review of the literatureantioxidant
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Review of the literatureThe α-toco
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Review of the literatureCopper, wil
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Review of the literatureOH • + H
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Review of the literatureFormation o
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Review of the literature3.2. The ro
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Review of the literaturecopper conc
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Experimental proceduresEXPERIMENTAL
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Experimental procedures2.2. Measure
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Experimental procedurestetrahydrate
- Page 40 and 41: ResultsRESULTS1. Vitamin C induces
- Page 42 and 43: Results3. Oxidative decomposition o
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- Page 46 and 47: DiscussionDISCUSSIONNowadays, ascor
- Page 48 and 49: DiscussionCu 2+ + Asc → Cu + + As
- Page 50 and 51: Discussion3. Iron inhibits vitamin
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- Page 54 and 55: ConclusionsCONCLUSIONSThe main focu
- Page 56 and 57: ReferencesREFERENCES1. Arrigoni O,
- Page 58 and 59: References34. Padayatty SJ, Katz A,
- Page 60 and 61: References66. Sies H, Stahl W, Sund
- Page 62 and 63: References95. Halliwell B. Role of
- Page 64 and 65: References127. Park S, Han SS, Park
- Page 66 and 67: References157. Critchley MM, Cromar
- Page 68 and 69: References185. Liao CH, Kang SF, Wu
- Page 70 and 71: References214. Orr CW. Studies on a
- Page 72: References243. Miller C, Kennington
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