Introduction

Hydrogen peroxide is a very useful oxidizer that has been employed in many different fields, such as chemistry of atmosphere [1], autodissociation dynamics [2, 3], and bleaching [4]. It is reasonably stable, readily available, inexpensive, and generates only water as a by-product [5]. Although its molecule is similar to water, it has not been much studied in a pure state because of its instability. However, like water, it forms hydrogen bonds with nitrogen- and oxygen-containing compounds [6, 7].

To avoid the stability issues, hydrogen peroxide can be transformed into a number of complexes with organic compounds. Urea–hydrogen peroxide complex (UHP) has already been used in many oxidation processes [8–11] as a source of anhydrous hydrogen peroxide. It is a stable and inexpensive solid that has been first prepared by Tanatar [12] and now is sold by a number of chemical manufacturers. Its crystals are composed of molecules of urea and hydrogen peroxide in 1:1 ratio, connected through multiple hydrogen bonds [13]. Hydrogen peroxide forms also complexes with melamine [14] and DABCO-di-N-oxide [15]. Some polymer-supported systems containing hydrogen peroxide are known as well. The most prominent among them is polyvinylpyrrolidone-hydrogen peroxide complex (PVP-H2O2), introduced by Pourali and Ghanei [16] that has already been successfully used for iodination of aromatic compounds as well as for oxidation of α,β-enones [17]. It can be easily prepared from 30 % aqueous solution of hydrogen peroxide and polyvinylpyrrolidone K-30, it contains up to 23 % of hydrogen peroxide by weight [18] and is insoluble in organic solvents [19]. It is stable for several months while stored in a refrigerator, without losing its weight or activity [16]. Hydrogen peroxide can also be encapsulated in different silica xerogel systems to serve as an oxidant in the presence of metal catalyst [20–22] or without it, with a hydrogen peroxide content up to 68 % [23].

Mesoporous materials developed in the 1990s, show numerous advantages: large surface area (~1,000 m2/g), uniform and controllable pore size, large pore volume (~1 cm3/g), narrow particle size, open pore structures [24], chemical and biological stability, and possibility of control of surface functionalization, which makes them very useful in a wide variety of applications such as adsorption, catalysis, ion exchange, sensing [25], chromatography [26], delivery carriers, and controlled drug/gene release [27]. There are three general paths to achieve surface functionalization of mesoporous silica surface [28]: postsynthetic functionalization (the so-called “grafting”) and two methods involved in the silica preparation process—co-condensation and condensation of bridged organosilica precursors forming periodic mesoporous organosilicas. The use of grafting method usually preserves the mesostructure of the starting silica phase, but the distribution of organic moieties anchored to the silica surface is solvent dependent [29] and sometimes leads to pores blockage [30]. Another advantage of this method is that it can be applied to a diversity of organic molecules, from small ones like aminopropyltrimethoxysilane [29] or compounds used in our experiment, to large moieties as dendrimers [31] and fullerenes [32]. Co-condensation is a convenient direct method of synthesis when the total amount of the organic part is supposed to be rather small. It provides better homogeneity of organic moieties, but can alter the matrix structure leading sometimes to totally disordered products [28]. It also allows the use of extraction as the only method for surfactant removal, as calcination could destroy organic compounds. After pioneering works of the groups of Mann and co-workers [33] and MacQuarrie [34], many different organically modified mesoporous silicas have been prepared by co-condensation, including those modified with alkyl, thiol, vinyl/allyl [35], amino, cyano/isocyano [36], alkoxy [37], organophosphine, and aromatic groups [38]. Periodic mesoporous organosilicas (PMOs) are materials with modified matrices but preserved organized pore system and narrow pore size distribution. They were first synthesized in 1999 by three groups working independently [39–41]. Until now, various PMOs are known: ethane- [39], ethene- [40], benzene- [42], bisphenyl-bridged [43], etc. They have found their application in chromatography [44] and catalysis [45].

The study was conducted to verify the ability of organic moieties grafted onto the mesoporous silicas of MCM-41 and MSU-H types to adsorb hydrogen peroxide from its aqueous solutions at different concentrations. Silica was chosen for the experiment, as it can be easily functionalized and has native silanol groups, able to form desired hydrogen bonds. Furthermore, both types of silica used differ in the pore diameter and noticeably in the surface area. We have used the method of postsynthetic modification to anchor nitrogen- and oxygen-containing groups that are able to form hydrogen bonds as grafting method offers higher coverage efficiency than direct synthesis methods and do not influence the order of mesoporous silica structure. Nitrogen-based compound (1-[3-(triethoxysilyl)propyl]urea) with urea-like moiety was chosen to permit comparison of the ability of hydrogen peroxide binding of this moiety and pure urea. Oxygen-based compound (N-(3-triethoxysilylpropyl)gluconamide) has many hydroxyl groups, and it was chosen to verify their influence on binding hydrogen peroxide.

This study is the first on hydrogen peroxide adsorption (not decomposition) on the surface of organically modified mesoporous silica. It is supposed to be the basis for future articles covering the presented issue.

Experimental details

Materials

Mesoporous silicas—MCM-41 (2.1–2.7 nm in diameter and 1,000 m2/g surface area) and MSU-H (~7.1 nm in diameter and 750 m2/g surface area), 30 % stock solution of hydrogen peroxide and 3-(triethoxysilyl)propyl isocyanate used for the synthesis of 1-[3-(triethoxysilyl)propyl]urea (1) were all purchased from Sigma-Aldrich, and N-(3-triethoxysilylpropyl)gluconamide (2) was purchased from ABCR GmbH & Co. KG. The structures of compounds used are presented in Fig. 1. Water used for the preparation of diluted hydrogen peroxide solutions had been degassed and deionized.

Fig. 1
figure 1

Molecules grafted on selected mesoporous silicas surface—1 stands for 1-[3-(triethoxysilyl)propyl]urea and 2 is N-(3-triethoxysilylpropyl)gluconamide

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Preparation of reagents

Both mesoporous silicas had been prepared for grafting by activation in boiling mixture of nitric acid and water (1:1) for a few hours, filtered off, washed by large amount of water, and dried in 60 °C for several hours.

A portion of 2 g of 3-(triethoxysilyl)propyl isocyanate was dissolved in 20 ml of acetonitrile and reacted with dry gaseous ammonia. The substrates reacted vigorously, so the solution was mixed and the flask was held in a cool water bath. After 1 h, the reaction was stopped, and both ammonia and acetonitrile were evacuated under vacuum. Gelatinous, quickly crystallizing solid, identified as N-[3-(triethoxysilyl)propyl]urea, was obtained. Figures 2, 3, and 4 present the spectra obtained for the isolated compound.

Fig. 2
figure 2

1H NMR spectrum of N-[3-(triethoxysilyl)propyl]urea

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Fig. 3
figure 3

ESI MS spectrum of N-[3-(triethoxysilyl)propyl]urea

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Fig. 4
figure 4

IR spectrum of N-[3-(triethoxysilyl)propyl]urea

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1H NMR spectrum was taken on an NMR Varian VNMR-S 400 MHz spectrometer at 298 K with TMS as a reference. 1H NMR(400 MHz, CDCl3), δ: 0.62–0.67 (t, 2H), 1.20–1.25 (t, 9H), 1.57–1.66 (quin, 2H), 3.11–3.17 (q, 2H), 3.79–3.85 (q, 6H), 4.74–4.77 (s, 2H), 5.20–5.28 (s, 1H).

ESI MS spectrum was obtained on a Waters/Micromass ZQ Mass Detector using 10−3 M methanol solution. ESI analysis parameters were the following: cone voltage—30 V, capillary voltage—3 kV, ion source temperature—393 K, desolvation temperature—573 K, and nitrogen was used as the nebulizing and desolving gas at flow rate of 80 l/min. ESI MS m/z: [M+H]+ 265, [M+Na]+ 287, [M+K]+ 303.

IR spectrum was obtained on a Bruker FT-IR IFS 66/s spectrometer using 1.2 mg of the compound mixed with 200 mg of KBr and formed into a pellet. IR: 3670–3440 cm−1 N–H amide stretching, 2975–2885 cm−1 C–H alkyl stretching, 1668 cm−1 C=O amide stretching, 1593, 1526 cm−1 N–H amide bending.

Preparation of modified silica

The procedure of modifying both silicas with each of grafting reagents used was as follows: 250 mg of the grafting reagent was dissolved in 10 ml of toluene, and then 250 mg of unmodified mesoporous silica was suspended. The mixture was stirred under reflux for 6 h, cooled to room temperature, filtered off, washed with pure toluene, and dried in 60 °C for several hours.

Hydrogen peroxide adsorption analysis

A series of hydrogen peroxide solutions with concentrations increasing from 5 to 30 % and pure, deionized, and degassed water were prepared for both unmodified and modified silica systems. Each system was composed of 35 mg of a selected silica suspended in 6 ml of hydrogen peroxide solution in a phial and stirred with a magnetic stirrer at room temperature for 24 h. Then, the phial contents were filtered off, washed with decent amount of water, and dried in 50 °C for 2 h to avoid hydrogen peroxide decomposition. The amount of hydrogen peroxide adsorbed was determined using the ferric thiocyanate method [46]. Before absorbance measurement on an UV–Vis Agilent 8453 Spectrophotometer, the silica suspensions were centrifuged to avoid disturbances caused by silica particles, and only clear solution from over the precipitate was taken for measurement.

Results and discussion

Elemental analysis

Elemental analysis for carbon, hydrogen, and nitrogen content allowed determination of the amounts of grafting reagents that had reacted with the silica surface. Results are presented in Table 1.

Table 1 Comparison of grafting efficiency for all obtained systems
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The presence of carbon in pure silicas can be a residue of surfactant used in the manufacturing process. Nitrogen observed in pure silica can be either adsorbed from the air or a surfactant residue, and hydrogen is a component of silanol groups densely covering the surface. The number of Si–O–Si bonds linking the grafted molecules to the surface could be easily calculated from the carbon:nitrogen ratio as hydrogen balance was more difficult to calculate. Hydrogen was removed from the surface silanol groups and added with grafted molecules in the amount depending on the total amount of the given compound grafted, hydrolysis of its alkoxy-groups, and the amount of Si–O–Si links formed.

The unbound 1-[3-(triethoxysilyl)propyl]urea of the molecular formula C10H24N2O4Si and the carbon:nitrogen ratio equal to 4.29:1 can be linked through one (with one ethoxy-group removed), two, or three Si–O–Si links with carbon:nitrogen ratios equal to 3.43:1, 2.57:1, and 1.71:1, respectively. The carbon:nitrogen ratios obtained for this compound suggest binding through two Si–O–Si links, when grafted on MCM-41, and through two or three (two links:three links ratio is 0.29:0.71) links, when grafted on MSU-H silica. Similar analysis conducted for binding of N-(3-triethoxysilylpropyl)gluconamide led to the following results: unbound compound of the molecular formula C15H33NO9Si and the carbon:nitrogen ratio equal to 12.86:1 can be linked through one, two, or all three links with carbon:nitrogen ratios equal to 11.14:1, 9.43:1, and 7.71:1, respectively. The carbon:nitrogen ratios for this compound suggest binding to the surface of both silicas through two or three Si–O–Si links (for MCM-41 two links:three links ratio is 0.21:0.79 and for MSU-H 0.45:0.55).

The silicas obtained contain large amounts of grafted compounds on their surface, comparable to those of simple organic compounds grafted in the previous studies on functionalization of mesoporous surfaces [47, 48], that could be estimated from the amount of nitrogen as its content is not dependent on the binding degree. 1-[3-(Triethoxysilyl)propyl]urea accounts for 32.11 % of total mass of modified MCM-41 and 41.71 % of MSU-H, which is 1.37 molecules/nm2 of MCM-41 surface and 3.09 molecules/nm2 of MSU-H surface. N-(3-Triethoxysilylpropyl)gluconamide accounts for 44.51 % of total mass of modified MCM-41 and 45.32 % of MSU-H, which is 1.51 molecules/nm2 of MCM-41 surface and 2.00 molecules/nm2 of MSU-H. These results show clearly that the pore size is an important factor, influencing the total amount of compounds grafted.

Hydrogen peroxide adsorption analysis

The graphs presented in Fig. 5 for different mesoporous silicas show clearly that surface modification influenced the amounts of hydrogen peroxide adsorbed on its surface, which after modification increased several times. The adsorption capacity of silicas modified with 1-[3-(triethoxysilyl)propyl]urea was increasing nonlinearly up to a hydrogen peroxide concentration of 25 %, and then it dropped to values similar to those obtained for unmodified silica, probably because of the destruction of organic moiety anchored to the silica surface (loss of the “urea” part makes it unable to form hydrogen bonds). The silicas modified with N-(3-triethoxysilylpropyl)gluconamide have their maximum adsorption at 5 % concentration of hydrogen peroxide, and then it decreases slightly to become almost equal to the adsorption of unmodified silica at 30 % hydrogen peroxide concentration. A large number of hydroxyl groups included in gluconamide moiety are oxidized, even at lower concentrations, and partially lose their ability to form hydrogen bonds (carbonyl group, without a hydrogen atom, can only be an electron donor). The average contents of carbon, hydrogen, and nitrogen for samples bathed in a 30 % solution of hydrogen peroxide are, respectively, 7.468, 2.261, and 3.897 %. The carbon:nitrogen ratio is much smaller than that for the unoxidized sample, which proves a major destruction to the organic part and the loss of ability to bind hydrogen peroxide. Small increase in the amount of hydrogen peroxide adsorbed at 25 and 30 % concentrations in comparison to that adsorbed from hydrogen peroxide solutions of concentrations 20 and 25 % may be caused by adsorption on the uncovered part of the silica surface.

Fig. 5
figure 5

Amount of hydrogen peroxide adsorbed on each functionalized silica as a function of hydrogen peroxide concentration in aqueous solution

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Also, MSU-H silica was found to adsorb much higher amounts of hydrogen peroxide, although it has smaller surface area. The influence of pore diameter on the amounts of hydrogen peroxide adsorbed is also indicated by the results obtained for each silica separately. The maximum amounts of hydrogen peroxide for MCM-41 are similar because of available space limitations. Grafted molecules occupy most of the pore volume, so there is not much space to bind H2O2 and its diffusion may be impaired. MSU-H provides much more space for both grafted organic moieties and hydrogen peroxide adsorbed as can be seen comparing Figs. 6 and 7, and the amount of H2O2 is only limited by the binding abilities of grafted molecules.

Fig. 6
figure 6

Cross-section of MSU-H silica, functionalized with N-(3-triethoxysilylpropyl)gluconamide, explaining the possible organization of grafted molecules and hydrogen peroxide adsorbed in the pores. Channel diameter and size of the molecules match

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Fig. 7
figure 7

Cross-section of MCM-41 silica, functionalized with N-(3-triethoxysilylpropyl)gluconamide, explaining the possible organization of grafted molecules and hydrogen peroxide adsorbed in the pores. Channel diameter and size of the molecules match

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The amount of hydrogen peroxide adsorbed on unmodified silica surface almost linearly increases with increasing hydrogen peroxide concentration. This phenomenon can be explained by formation of hydrogen bonds between free silanol groups and hydrogen peroxide. In the experimental conditions, almost all of silanol groups were ionized as mesoporous silanol groups existed in two forms, Si-(OH)2 and Si-(OH) with pK a values, respectively, 8.2 and 2.0 [49].

Conclusions

Two different molecules able to form hydrogen bonds were successfully grafted on the surface of two different mesoporous silicas of MCM-41 and MSU-H types. The amounts of hydrogen peroxide adsorbed on their surface were measured, and MSU-H sample was found to have a higher adsorption capacity, as about 2–3 times more hydrogen peroxide got adsorbed on its surface. Unmodified silica showed also some adsorption abilities dependent on the concentration of hydrogen peroxide solution. Functionalized surface was not resistant enough and the compounds deposited underwent oxidation, changing the silicas adsorption properties in higher hydrogen peroxide concentrations. Increased amount of hydroxyl groups introduced with N-(3-triethoxysilylpropyl)gluconamide indeed has enhanced the adsorption of hydrogen peroxide. Although the content of hydrogen peroxide bound by the systems obtained was small in comparison with that of PVP or urea complexes, results of this study can initiate further development in this field.