Selective Oxidation of Furfural at Room Temperature on a TiO 2 -Supported Ag Catalyst

: The catalytic performance of the Ag/TiO 2 catalyst was evaluated in the oxidation of furfural (FF) to furoic acid (FA) in an alkaline aqueous solution under 15 bar of air in a batch reactor. The catalytic activity, yield, and stability of the catalyst were compared as a function of different reaction parameters including temperature (25–110 ◦ C), nature of the atmosphere, base equivalent (n base /n FF = 0.25–3), and nature of the inorganic bases used (NaOH, NaHCO 3 , and Na 2 CO 3 ). Under optimum conditions, the yield of FA (96%) was achieved at room temperature, with an excellent carbon balance (>98%). The recyclability of the catalyst was also studied and the catalytic activity of the Ag/TiO 2 catalyst slightly declined due to an increase in particle size as conﬁrmed by TEM studies.


Introduction
Over the last decades, society has tended towards the use of the lignocellulosic biomass as an interesting alternative for the production of biofuels and chemicals [1][2][3][4]. According to the US department of energy (DOE), furfural (FF) is considered as one of the ten most relevant building platform molecules among the lignocellulosic biomass derivatives [5][6][7]. Xylan-rich hemicelluloses are sources of FF which can be further valorized by different methods including hydrogenation, aldol condensation, and oxidation into various key products [7,8]. In particular, the production of furoic acid (FA) through the selective oxidation of FF (Scheme 1) has drawn attention due to its potential application in the polymer industries as a precursor of 2,5-furandicarboxylic acid (FDCA) [9,10]. It is also used as starting material in the pharmaceutical, fragrance, agrochemical, and flavor industries [11,12]. The industrial production of FA from FF is generally performed using strong oxidizing agents via a Cannizzaro reaction, followed by the addition of H 2 SO 4 as an acidification step [13]. This process is undesirable due to the corrosive and toxic nature of the employed reagents [12,14]. However, the application of heterogeneous catalysts in the presence of "green" oxidants such as H 2 O 2 , O 2 , or air to improve the efficiency of oxidation reaction has been investigated [15]. Various noble metals such as Au, Pd, and Pt have been considered for the catalytic oxidation of FF to FA. Au-based catalysts have been considered so far as the most efficient for the partial oxidation of FF under green conditions [11,[15][16][17][18]. Despite its high catalytic activity, the major drawback of gold in terms of cost and sustainability makes it attractive to search for alternative metals. There are few studies reporting the use of Ag, which has a much lower price than gold and its availability is confirmed by the huge world reserves. Sha et al. investigated the oxidation of FF into FA (92% yield) in an alkaline medium at 70 • C in the presence of a Ag 2 O/CuO catalyst [19]. Recently, the oxidation of 5-(hydroxymethyl) furfural (HMF) to 5-hydroxymethyl-2-furancarboxylic acid (HMFCA) over a Ag/ZrO 2 catalyst at 50 • C in the presence of air and NaOH as a base was studied. After 5 h and one equivalent of NaOH, 100% HMF conversion and 94% HMFCA yield was conversion and 94% HMFCA yield was obtained [20]. Commercial TiO2-P25 was used as a support with a non-basic character. It is stable in water under oxidation conditions [21].
Herein, a monometallic Ag/TiO2 catalyst was investigated for the selective oxidation of FF to FA at room temperature in an alkaline aqueous solution using air. The influence of the reaction parameters (e.g., temperature, atmosphere, ratio of base, and nature of base) on catalytic activity, yield, and carbon balance were also studied. Scheme 1. Oxidation of furfural (FF) into furoic acid (FA).

Results and Discussion
The physicochemical properties (chemical composition, specific surface area) of the synthesized Ag/TiO2 catalyst were studied. Using the ICP-OES analysis, 6 wt.% loading of Ag was confirmed. The specific surface area of the Ag/TiO2 catalyst was slightly lower (48 m 2 g −1 ) compared to that of the fresh TiO2 support (P25, 53 m 2 g −1 ). The XRD patterns Ag/TiO2 catalyst are compared to that of the pristine support in Figure 1. The XRD patterns of TiO2 support confirmed the presence of a mixture of two known anatase and rutile phase structures. Contrary to that, the Ag/TiO2 sample exhibited additional diffraction peaks (other than those of the supports) at 44°, 64°, and 77° which were attributed to silver in a metallic state. However, due to the overlapping of the main diffraction peak of metallic silver with the diffraction peak of TiO2 at 38° (Figure 1), the particle size was estimated through TEM analysis. The TEM image of the Ag/TiO2 catalyst and its corresponding particle size histogram are shown in (Figure 2). In order to estimate the average particle size, approximately 200 particles were measured. The average particle size in Ag/TiO2 was estimated to be 1.82 nm. This confirmed the obtention of a very good dispersion of silver nanoparticles on the support surface. Herein, a monometallic Ag/TiO 2 catalyst was investigated for the selective oxidation of FF to FA at room temperature in an alkaline aqueous solution using air. The influence of the reaction parameters (e.g., temperature, atmosphere, ratio of base, and nature of base) on catalytic activity, yield, and carbon balance were also studied.

Results and Discussion
The physicochemical properties (chemical composition, specific surface area) of the synthesized Ag/TiO 2 catalyst were studied. Using the ICP-OES analysis, 6 wt.% loading of Ag was confirmed. The specific surface area of the Ag/TiO 2 catalyst was slightly lower (48 m 2 g −1 ) compared to that of the fresh TiO 2 support (P25, 53 m 2 g −1 ). The XRD patterns Ag/TiO 2 catalyst are compared to that of the pristine support in Figure 1. The XRD patterns of TiO 2 support confirmed the presence of a mixture of two known anatase and rutile phase structures. Contrary to that, the Ag/TiO 2 sample exhibited additional diffraction peaks (other than those of the supports) at 44 • , 64 • , and 77 • which were attributed to silver in a metallic state. However, due to the overlapping of the main diffraction peak of metallic silver with the diffraction peak of TiO 2 at 38 • (Figure 1), the particle size was estimated through TEM analysis.
Catalysts 2022, 12, x FOR PEER REVIEW 2 of 10 conversion and 94% HMFCA yield was obtained [20]. Commercial TiO2-P25 was used as a support with a non-basic character. It is stable in water under oxidation conditions [21]. Herein, a monometallic Ag/TiO2 catalyst was investigated for the selective oxidation of FF to FA at room temperature in an alkaline aqueous solution using air. The influence of the reaction parameters (e.g., temperature, atmosphere, ratio of base, and nature of base) on catalytic activity, yield, and carbon balance were also studied.

Results and Discussion
The physicochemical properties (chemical composition, specific surface area) of the synthesized Ag/TiO2 catalyst were studied. Using the ICP-OES analysis, 6 wt.% loading of Ag was confirmed. The specific surface area of the Ag/TiO2 catalyst was slightly lower (48 m 2 g −1 ) compared to that of the fresh TiO2 support (P25, 53 m 2 g −1 ). The XRD patterns Ag/TiO2 catalyst are compared to that of the pristine support in Figure 1. The XRD patterns of TiO2 support confirmed the presence of a mixture of two known anatase and rutile phase structures. Contrary to that, the Ag/TiO2 sample exhibited additional diffraction peaks (other than those of the supports) at 44°, 64°, and 77° which were attributed to silver in a metallic state. However, due to the overlapping of the main diffraction peak of metallic silver with the diffraction peak of TiO2 at 38° (Figure 1), the particle size was estimated through TEM analysis. The TEM image of the Ag/TiO2 catalyst and its corresponding particle size histogram are shown in (Figure 2). In order to estimate the average particle size, approximately 200 particles were measured. The average particle size in Ag/TiO2 was estimated to be 1.82 nm. This confirmed the obtention of a very good dispersion of silver nanoparticles on the support surface. The TEM image of the Ag/TiO 2 catalyst and its corresponding particle size histogram are shown in (Figure 2). In order to estimate the average particle size, approximately 200 particles were measured. The average particle size in Ag/TiO 2 was estimated to be 1.82 nm. This confirmed the obtention of a very good dispersion of silver nanoparticles on the support surface.

Effect of the Temperature
The effect of reaction temperature was investigated over the 25-110 °C range un 15 bar of air in the presence of Ag/TiO2 catalyst. The evolution of FF concentration a function of time is presented in Figure 3a and the yield of FA accompanied with carb balance is shown in Figure 3b. At 25 °C, 96% conversion was achieved after 3 h of reacti As expected, the higher the reaction temperature, the faster the reaction rate. For examp at 50 °C, an FF conversion of 93% was attained after 2 h, whereas 1.7 and 1 h were need to reach the same conversion at 80 and 110 °C, respectively. When the reaction tempe ture was increased from 25 to 110 °C, the yield of FA significantly decreased from 96 45%, respectively ( Figure 3b). The degradation of furfural through the formation humins and humic acids occurred at a higher temperature (110 °C) resulting in a low c bon balance (45%) [15,17]. No leaching of silver was detected by ICP analysis of the liq solution at the end of the reaction over the 25-110 °C range of temperature. Finally temperature of 25 °C was chosen for further experiments to avoid the formation of products due to the degradation and to keep a high carbon balance (>98%).

Effect of the Temperature
The effect of reaction temperature was investigated over the 25-110 • C range under 15 bar of air in the presence of Ag/TiO 2 catalyst. The evolution of FF concentration as a function of time is presented in Figure 3a and the yield of FA accompanied with carbon balance is shown in Figure 3b. At 25 • C, 96% conversion was achieved after 3 h of reaction. As expected, the higher the reaction temperature, the faster the reaction rate. For example, at 50 • C, an FF conversion of 93% was attained after 2 h, whereas 1.7 and 1 h were needed to reach the same conversion at 80 and 110 • C, respectively. When the reaction temperature was increased from 25 to 110 • C, the yield of FA significantly decreased from 96 to 45%, respectively ( Figure 3b). The degradation of furfural through the formation of humins and humic acids occurred at a higher temperature (110 • C) resulting in a low carbon balance (45%) [15,17]. No leaching of silver was detected by ICP analysis of the liquid solution at the end of the reaction over the 25-110 • C range of temperature. Finally, a temperature of 25 • C was chosen for further experiments to avoid the formation of by-products due to the degradation and to keep a high carbon balance (>98%).

Effect of the Temperature
The effect of reaction temperature was investigated over the 25-110 °C range 15 bar of air in the presence of Ag/TiO2 catalyst. The evolution of FF concentrati function of time is presented in Figure 3a and the yield of FA accompanied with balance is shown in Figure 3b. At 25 °C, 96% conversion was achieved after 3 h of re As expected, the higher the reaction temperature, the faster the reaction rate. For ex at 50 °C, an FF conversion of 93% was attained after 2 h, whereas 1.7 and 1 h were to reach the same conversion at 80 and 110 °C, respectively. When the reaction te ture was increased from 25 to 110 °C, the yield of FA significantly decreased from 45%, respectively (Figure 3b). The degradation of furfural through the forma humins and humic acids occurred at a higher temperature (110 °C) resulting in a l bon balance (45%) [15,17]. No leaching of silver was detected by ICP analysis of th solution at the end of the reaction over the 25-110 °C range of temperature. Fi temperature of 25 °C was chosen for further experiments to avoid the formation products due to the degradation and to keep a high carbon balance (>98%).   Figure 4 shows the catalytic activity of a Ag/TiO2 catalyst under air and N2 phere at 25 °C with one equivalent of NaOH. It can be seen that oxygen strongl enced the furfural conversion. Under an inert gas atmosphere (N2, 15 bar), the ma conversion of furfural (14%) was rapidly reached after 1 h of reaction and it re constant (maximum of 17% after 3 h). In the presence of an oxidative atmospher furfural conversion was reached under 15 bar of air and 80% of furfural was con under atmospheric pressure after 3 h ( Figure 4). Selectivity remained optimal to acid (~96%) whatever the atmosphere used.  Figure 4 shows the catalytic activity of a Ag/TiO 2 catalyst under air and N 2 atmosphere at 25 • C with one equivalent of NaOH. It can be seen that oxygen strongly influenced the furfural conversion. Under an inert gas atmosphere (N 2 , 15 bar), the maximum conversion of furfural (14%) was rapidly reached after 1 h of reaction and it remained constant (maximum of 17% after 3 h). In the presence of an oxidative atmosphere, total furfural conversion was reached under 15 bar of air and 80% of furfural was converted under atmospheric pressure after 3 h ( Figure 4). Selectivity remained optimal to furoic acid (~96%) whatever the atmosphere used.  Figure 4 shows the catalytic activity of a Ag/TiO2 catalyst under air and N2 atmosphere at 25 °C with one equivalent of NaOH. It can be seen that oxygen strongly influenced the furfural conversion. Under an inert gas atmosphere (N2, 15 bar), the maximum conversion of furfural (14%) was rapidly reached after 1 h of reaction and it remained constant (maximum of 17% after 3 h). In the presence of an oxidative atmosphere, total furfural conversion was reached under 15 bar of air and 80% of furfural was converted under atmospheric pressure after 3 h (Figure 4). Selectivity remained optimal to furoic acid (~96%) whatever the atmosphere used.   A reaction mechanism was proposed in order to explain the difference in catalytic activity ( Figure 5). First, in an alkaline aqueous solution, the aldehyde group of furfural directly undergoes a reversible hydration through nucleophilic attack of a hydroxide ion (OH − ) to the carbonyl group followed by proton transfer (from water) to the alkoxide ion intermediate. In the second step, the intermediate diol is dehydrogenated on the surface of reduced silver particles and forms furoic acid. During the catalytic cycle, the surface of silver is covered with adsorbed H-species that are removed by oxygen leading to the regeneration of the silver catalyst [22].

Effect of the Atmosphere
Catalysts 2022, 12, x FOR PEER REVIEW 5 of 10 A reaction mechanism was proposed in order to explain the difference in catalytic activity ( Figure 5). First, in an alkaline aqueous solution, the aldehyde group of furfural directly undergoes a reversible hydration through nucleophilic attack of a hydroxide ion (OH -) to the carbonyl group followed by proton transfer (from water) to the alkoxide ion intermediate. In the second step, the intermediate diol is dehydrogenated on the surface of reduced silver particles and forms furoic acid. During the catalytic cycle, the surface of silver is covered with adsorbed H-species that are removed by oxygen leading to the regeneration of the silver catalyst [22]. Based on the mechanism proposed in Figure 5, the decrease in FF conversion from 100 to 80%, when atmospheric pressure was used instead of 15 bar air can be explained by the presence of hydrogen on the surface of silver which cannot be removed without oxygen. The catalytic cycle is closed by oxygen, which removes the hydrogen from the surface of Ag through the formation of water and regenerates the Ag catalyst by releasing the active sites to catalyze the further dehydrogenation step. A similar explanation can be concluded when 15 bar of N2 was used, which explains the lower conversion obtained (17% after 3 h, Figure 4). Without oxygen the surface of silver is covered by adsorbed Hspecies and the catalytic cycle is broken and further furfural conversion is stopped.
Finally, it is worth noting that for the first-time high yields to furoic acid were obtained at room temperature. Generally, this reaction is carried out on gold nanoparticles at higher temperature [15,17].

Effect of Base: Nature and Ratio
The effect of OH − :FF molar ratio (0.25-3) on FF conversion and FA yield (Table 1) was studied at 25 °C under 15 bar of air in the presence of a Ag/TiO2 catalyst. As expected, no furfural conversion was observed in the absence of a base. However, as the molar ratio OH − :FF increased from 0.25 up to 1, FF conversion and FA yield increased from 10 to 96%. In the whole OH − :FF range, the carbon balance was higher than 98 % and the only detected product was FA. By further increasing the amount of base from 1 to 3 equivalents, FF conversion remained constant (~100%) and the FA yield decreased from 96 to 70%. This result is consistent with the observations made during the aqueous phase oxidation of HMF (5-hydroxymethyl furfural) to HMFCA (5-hydroxymethyl-2-furan-carboxylic acid) over Ag/ZrO2 catalyst in the presence of NaOH [23]. The authors observed that at 50 °C, as the amount of NaOH increased from 0.5 to 1 equivalent, HMF conversion and HMFCA yield were also increased. The authors also showed that by increasing the amount of base Based on the mechanism proposed in Figure 5, the decrease in FF conversion from 100 to 80%, when atmospheric pressure was used instead of 15 bar air can be explained by the presence of hydrogen on the surface of silver which cannot be removed without oxygen. The catalytic cycle is closed by oxygen, which removes the hydrogen from the surface of Ag through the formation of water and regenerates the Ag catalyst by releasing the active sites to catalyze the further dehydrogenation step. A similar explanation can be concluded when 15 bar of N 2 was used, which explains the lower conversion obtained (17% after 3 h, Figure 4). Without oxygen the surface of silver is covered by adsorbed H-species and the catalytic cycle is broken and further furfural conversion is stopped.
Finally, it is worth noting that for the first-time high yields to furoic acid were obtained at room temperature. Generally, this reaction is carried out on gold nanoparticles at higher temperature [15,17].

Effect of Base: Nature and Ratio
The effect of OH − :FF molar ratio (0.25-3) on FF conversion and FA yield (Table 1) was studied at 25 • C under 15 bar of air in the presence of a Ag/TiO 2 catalyst. As expected, no furfural conversion was observed in the absence of a base. However, as the molar ratio OH − :FF increased from 0.25 up to 1, FF conversion and FA yield increased from 10 to 96%. In the whole OH − :FF range, the carbon balance was higher than 98 % and the only detected product was FA. By further increasing the amount of base from 1 to 3 equivalents, FF conversion remained constant (~100%) and the FA yield decreased from 96 to 70%. This result is consistent with the observations made during the aqueous phase oxidation of HMF (5-hydroxymethyl furfural) to HMFCA (5-hydroxymethyl-2-furan-carboxylic acid) over Ag/ZrO 2 catalyst in the presence of NaOH [23]. The authors observed that at 50 • C, as the amount of NaOH increased from 0.5 to 1 equivalent, HMF conversion and HMFCA yield were also increased. The authors also showed that by increasing the amount of base to two equivalents, the HMF conversion remained constant but the HMFCA yield decreased. In addition to NaOH, some mild bases were also examined in the selective oxidation of FF (Table 2). Almost no catalytic activity was observed in the presence of NaHCO 3 as in the case without the addition of a base. Na 2 CO 3 slightly accelerated the oxidation reaction resulting in 7% conversion of FF after 3 h. This is in agreement with observations made during the liquid phase oxidation of ethylene glycol to glycolic acid over Pt/CeO 2 catalyst in the presence of different bases [24]. It was shown that NaOH was the best base and the others (NaHCO 3 and Na 2 CO 3 ) had a poisoning effect caused by the introduction of HCO 3 − and CO 32 − in the reaction medium [24]. In addition, the increase in the base strength represents an increase in the overall concentration of HO − and, consequently, can explain the differences observed in the reaction rate. During the oxidation of aldehydes in basic aqueous solution, the reversible hydration of the aldehyde to germinal diols is a main step. This step is accelerated at a high pH. The germinal diols will adsorb in the metal surface to form an alkoxide that later undergoes a β-elimination to form carboxylic acid. Thus, the combination of high concentration of OH − and/or longer reaction times favours the oxidation of furfural to furoic acid [25]. Table 2. Effect of the nature of the base on FF conversion, FA yield, and carbon balance in the oxidation of FF over Ag/TiO 2 . Reaction conditions: C 0(FF) = 0.1 mol L −1 , n FF /n Ag = 300, n base /n FF = 1, 15 bar of air, T = 25 • C, 600 rpm, 3 h reaction.

Recyclability Tests
The recyclability of the Ag/TiO 2 catalyst was investigated at 25 • C under 15 bar of air using NaOH as a base ( Figure 6). In the first run, 83% conversion of FF was achieved with an 82% yield of FA after 2 h of reaction. Before the second and the third runs, the catalyst was recovered by centrifugation and dried overnight at 110 • C without any further activation. A decrease in the catalytic activity was observed and a conversion of 52% was observed during the third run. The carbon balance was always higher than 99% and FA was the only product analyzed by HPLC analysis. No leaching of Ag was detected by ICP analysis of the liquid solution at the end of each run, which does not explain the decrease in the catalytic activity over the Ag/TiO 2 catalyst. The average particle size measured by TEM on Ag/TiO 2 increased from 1.82 nm in the fresh catalyst ( Figure 2) to 5.29 nm in the spent catalyst (Figure 7) which could explain the deactivation of the silver catalyst after 3 runs of the reaction.  Another possibility was the re-oxidation of the catalyst during the drying step. The catalytic test with the calcined (AgO/TiO2) catalyst was performed and the activity of this catalyst was much lower than that of the reduced one (14% vs. 96% conversion after 3 h). This also demonstrated that the metallic silver was the active phase in this reaction.

Catalyst Preparation
Commercial TiO2-P25, (Sigma Aldrich, Saint Louis, MI, USA), was used as the support. Supported silver catalysts were prepared by a simple impregnation method. It was conducted by introducing the support and a solution of AgNO3 (50 mM, in water and ethanol at a volume ratio of 1:1) in a flask. The reducing agent sodium borohydride (NaBH4) was added in excess and the solution was stirred at 30 °C for 4 h. After filtration, the material was washed and dried overnight at 90 °C under static air.

Characterization of Catalysts
The elemental analysis of Ag and Ti in solutions was performed by ICP-OES (Inductively Coupled Plasma Optical Emission Spectrometry) analysis by using Agilent 720-ES ICP-OES equipment combined with Vulcan 42S automated digestion system (Agilent, Santa Clara, CA, USA). Powder X-ray diffraction patterns (XRD) of the samples were recorded in ambient conditions using a Bruker AXS D8 Advance diffractometer equipped  Another possibility was the re-oxidation of the catalyst during the drying step. The catalytic test with the calcined (AgO/TiO2) catalyst was performed and the activity of this catalyst was much lower than that of the reduced one (14% vs. 96% conversion after 3 h). This also demonstrated that the metallic silver was the active phase in this reaction.

Catalyst Preparation
Commercial TiO2-P25, (Sigma Aldrich, Saint Louis, MI, USA), was used as the support. Supported silver catalysts were prepared by a simple impregnation method. It was conducted by introducing the support and a solution of AgNO3 (50 mM, in water and ethanol at a volume ratio of 1:1) in a flask. The reducing agent sodium borohydride (NaBH4) was added in excess and the solution was stirred at 30 °C for 4 h. After filtration, the material was washed and dried overnight at 90 °C under static air.

Characterization of Catalysts
The elemental analysis of Ag and Ti in solutions was performed by ICP-OES (Inductively Coupled Plasma Optical Emission Spectrometry) analysis by using Agilent 720-ES ICP-OES equipment combined with Vulcan 42S automated digestion system (Agilent, Santa Clara, CA, USA). Powder X-ray diffraction patterns (XRD) of the samples were recorded in ambient conditions using a Bruker AXS D8 Advance diffractometer equipped Another possibility was the re-oxidation of the catalyst during the drying step. The catalytic test with the calcined (AgO/TiO 2 ) catalyst was performed and the activity of this catalyst was much lower than that of the reduced one (14% vs. 96% conversion after 3 h). This also demonstrated that the metallic silver was the active phase in this reaction.

Catalyst Preparation
Commercial TiO 2 -P25, (Sigma Aldrich, Saint Louis, MI, USA), was used as the support. Supported silver catalysts were prepared by a simple impregnation method. It was conducted by introducing the support and a solution of AgNO 3 (50 mM, in water and ethanol at a volume ratio of 1:1) in a flask. The reducing agent sodium borohydride (NaBH 4 ) was added in excess and the solution was stirred at 30 • C for 4 h. After filtration, the material was washed and dried overnight at 90 • C under static air.

Characterization of Catalysts
The elemental analysis of Ag and Ti in solutions was performed by ICP-OES (Inductively Coupled Plasma Optical Emission Spectrometry) analysis by using Agilent 720-ES ICP-OES equipment combined with Vulcan 42S automated digestion system (Agilent, Santa Clara, CA, USA). Powder X-ray diffraction patterns (XRD) of the samples were recorded in ambient conditions using a Bruker AXS D8 Advance diffractometer equipped with a nickel filter, a copper tube (λKα (Cu) = 1.54184 Å), and a multi-channel fast detector. Samples were scanned at 0.014 • s −1 over the range 5 ≤ 2θ ≤ 80 • (Bruker, Billerica, MA, USA). The BET specific surface area, pore volume, and pore size distribution were determined from the N 2 adsorption/desorption at −196 • C using a TriStar II Plus and 3Flex apparatus Micromeritics (Norcross, GA, USA). Before the measurements, catalysts were degassed at 110 • C for 2 h. Transmission electron microscopy (TEM) images were obtained by using a Tecnai G2 20 microscope equipped with a LaB 6 filament and operating at 200 kV (Tecnai, Hillsboro, OR, USA), also equipped with an EDX detector and a GATAN CCD camera (Orius SC1000A, Gatan Inc., Pleasanton, CA, USA). The images were acquired in the parallel beam TEM mode.

Catalytic Testing
The oxidation of FF (Merck, <99%) was carried out in a 30 mL Top Industry autoclave. A total of 20 mL of furfural aqueous solution (concentrations 100 mmol L −1 ) and 11.5 mg of catalyst were loaded into the reactor. The base (NaOH was added to the reactor (variable quantity depending on the performed test). In the nature of the base studies the OH to FF molar ratio was kept constant (equal to 1). After sealing, the autoclave was purged 3 times with air, pressurized with air to the required pressure (P air = 15 bar), and finally heated to the reaction temperature (T = 25-110 • C) under stirring (600 rpm). During the experiment, liquid samples were collected to follow the kinetics of the reaction. At the end of the reaction, air was released, the reactor was cooled, and the catalyst was collected by centrifugation. At the end of each reaction, the aqueous solution was analyzed by ICP to detect the leaching of metals expressed in ppm. A blank test was performed without a catalyst and no conversion of FF was observed.
The reaction products were analyzed by High Performance Liquid Chromatography (HPLC, Waters 2410 RJ, Waters, Milford, MA, USA) equipped with RI and UV (λ = 253 nm) detectors and a Rezex ROA-organic Acid H + column (Ø 7.8 mm × 300 mm) at 25 • C. Diluted H 2 SO 4 (5 mmol L −1 , 0.5 mL min −1 ) was used as the mobile phase. The products were identified by their retention times compared to available standards that were also used to determine the response factors.
The conversion of FF at time t was calculated from Equation (1): where C 0 FF is the initial concentration of FF and C t FF is the concentration of FF at time t. The yield and selectivity to FA were calculated using Equations (2) and (3), respectively.
in which C t FA is the concentration of FA at time t. The carbon balance (CB) at time t was calculated according to Equation (4).
where C 0 FF is the initial concentration of FF (in mol L −1 ) and C t FA is the concentration of FA at time t (in mol L −1 ).
At the end of each reaction, in order to detect the leaching of silver (in ppm), ICP analyses of the aqueous solution were performed.

Conclusions
The TiO 2 -supported Ag catalyst prepared by the simple impregnation method was proven to have an excellent activity in the oxidation of furfural. A high yield of furoic acid was obtained in an alkaline aqueous solution, under 15 bar of air and room temperature. The effect of different reaction parameters including temperature (25-110 • C), effect of atmosphere, base equivalent (n OH − /n FF = 0. , and nature of the inorganic base used (NaOH, NaHCO 3 , and Na 2 CO 3 ) on catalytic activity and yield were studied. Whatever the reaction conditions, furoic acid was the only product detected. The catalytic activity of Ag/TiO 2 catalyst however declined after three runs of the reaction which is associated with both an increase in the size and the re-oxidation of the silver particles.
Author Contributions: A.S.: conceptualization, data curation, formal analysis, writing-original draft, R.W.: conceptualization, project administration, supervision, writing-original draft, writing-review and editing, S.P.: reviewing. All authors have read and agreed to the published version of the manuscript.
Funding: This research received no external funding.

Data Availability Statement:
The data presented in this study are available on request from the corresponding author.