Synthesis of Heterostructure of ZnO@MOF-46(Zn) to Improve the Photocatalytic Performance in Methylene Blue Degradation

The heterostructure of ZnO and MOF-46(Zn) was synthesized to improve the photocatalytic performance of ZnO and prove the synergistic theory that presented the coexistence of ZnO and MOF-46(Zn), providing better efficiency than pure ZnO. The heterostructure material was synthesized by using prepared ZnO as a Zn2+ source, which was reacted with 2-aminoterephthalic acid (2-ATP) as a ligand to cover the surface of ZnO with MOF-46(Zn). The ZnO reactant materials were modified by pyrolysis of various morphologies of IRMOF-3 (Zn-MOF) prepared by using CTAB as a morphology controller. The octahedral ZnO obtained at 150 mg of CTAB shows better efficiency for photodegradation, with 85.79% within 3 h and a band gap energy of 3.11 eV. It acts as a starting material for synthesis of ZnO@MOF-46(Zn). The ZnO/MOF-46(Zn) composite was further used as a photocatalyst material in the dye (methylene blue: MB) degradation process, and the performance was compared with that of pure prepared ZnO. The results show that the photocatalytic efficiency with 61.20% in the MB degradation of the heterostructure is higher than that of pure ZnO within 60 min (90.09% within 180 min). The reason for this result may be that the coexistence of ZnO and MOF-46(Zn) can absorb a larger range of energy and reduce the possibility of the electron–hole recombination process.

ZnO is an N-type semiconductor that possesses a wide energy band gap, as 3.37 eV is emitted in the near-UV region of the spectrum. Several methods have been used for ZnO synthesis, including precipitation [9], electrochemical [10], sol-gel [11], microwave [12], mechano-chemical [13], and hydro/solvothermal [14] methods, and the pyrolysis of metalorganic frameworks based on Zn(II) ions (Zn-MOFs) [15]. Different syntheses can provide different properties that affect the efficient performance. Not only does the synthesis method affect the performance, but the different morphologies also affect the efficiency of ZnO. Elamin and Elsanousi [16] synthesized different morphologies of ZnO by hydrothermal methods with different treatment durations. The obtained products comprising nanosheets and nanotubes were used as photocatalysts in the methyl orange degradation process. The results showed that the photocatalytic efficiency depended on the morphology, and ZnO nanosheets were more effective than nanotubes due to their larger surface area. Although ZnO is used in extensive work, its wide band gap restriction leads to its use in high-energy and low harvesting of light. Many previous studies have focused on ZnO modification, such as morphology and size modification by adding other materials to reduce the operating energy and increase the light harvesting ability [17] for material performance improvement. In previous reports, ZnO nanostructures were codoped with Al/Ni by Reddy's group [18]. This work presented that the coexistence of Al/Ni in the ZnO site provided great photocatalytic performance in dye removal activity. In another work, Nguyen's [19] group improved the photocatalytic efficiency of ZnO by synthesizing a composite of ZnO nanorods/CuO. The performance of the composite exhibited excellent photodegradation efficiency. Recently, biomimetics and bioinspiration concepts [20] were adopted as an idea for shape modification. Serra and a collaborator [21] synthesized a novel photocatalyst material based on using helical microalgae as a biotemplate; namely, Ni@ZnO@ZnS-Spirulina. The photocatalyst presented higher efficiency, minimal photocorrosion, excellent reusability, and ecofriendliness. ZnO nanorod arrays were synthesized hydrothermally with various amounts of CTAB (cetyltrimethylammonium bromide) to control exposure of the {0001} facet [22]. The photocatalytic activities measured by photodegradation of RhB reveal that they depended on the morphology of the prepared ZnO. From the reviews of ZnO modification, one interesting material is the metal-organic framework (MOFs), which is a good choice for ZnO to obtain a ZnO/MOF heterostructure.
MOF, a kind of porous material, is a functional material that comprises metal ions/ clusters and organic ligands with functionality that are linked together by strong bonds to form one, two, or three dimensionalities. MOFs possess extraordinary properties, such as a large surface area and thermal stability, a particular porosity, a tunable topology and functionality, light absorption ability in the UV-Vis range, rich host-guest chemistry, well-developed pores to make high accessibility of active sites, and Lewis acid sites that they can be tuned by the formation of missing ligand defects. These attractive properties have led to numerous fields of work in recent decades in luminescence sensors [23], adsorption/desorption [23], gas storage [24], molecular separation [25], drug delivery [26], and catalysis from the last two properties [27][28][29].
To date, many studies on the photodegradation of methylene blue using ZnO-based photocatalysts have been reported. For this research, we adopted the outstanding properties of MOFs (large surface area, light absorption ability, specific pore site) with the semiconductor property of ZnO to improve the photocatalytic performance. First, ZnO was modified on the outer surface by covering the MOF. MOF-46(Zn), as a Zn-MOF type, was chosen by Yagki's group for the first time to cover ZnO surfaces synthesized from Zn(II) ions and 2-aminoteraphalic acid (2-ATP) [30]. In this work, not only was the MOF covered on the surface of ZnO to obtain a core-shell heterostructure, but it was also used as a starting precursor to prepare ZnO by the pyrolysis of Zn-MOF to easily control the shape and obtain a high yield. Since we hypothesized that the ZnO morphologies affected the photocatalytic performance, three different morphologies of ZnO were produced by controlling the starting material morphology (IRMOF-3). IRMOF-3, a kind of Zn-MOF with three different shapes, was synthesized in the first step by Zn(II) ions, 2-ATP, and various amounts of CTAB surfactant as a shape controller. IRMOF-3 was transformed by calcination. The prepared ZnO was used as a Zn(II) ion source instead of zinc salts, which are environmentally unfriendly. The partial Zn(II) ions dissolving from ZnO interact with 2-ATP ligands to form a core-shell ZnO@MOF-46(Zn) composite. To prove the synergistic properties of the ZnO and MOF-46(Zn) composite and prove that it exhibits better performance than pure ZnO, ZnO@MOF-46(Zn) was used as a photocatalyst for the degradation of dye (methylene blue: MB), and the performance was compared with that of pure ZnO in the aqueous phase with UV irradiation. IRMOF-3 was used as the starting material and prepared by a modified procedure [31]. First, 0.3 mmol of Zn(NO 3 ) 2 6H 2 O and 0.15 mmol of 2-ATP were dissolved in a mixed solvent (30 mL) of DMF and C 2 H 5 OH(7:3). Various amounts of CTAB (0, 80, and 150 mg) were then added to a mixture solution. The mixture was further transferred into an autoclave and heated at 115 • C for 4 h. Subsequently, the reactor was cooled to room temperature, then the products were washed with DMF and C 2 H 5 OH. The three different morphologies of the products of IRMOF-3 from each addition of CTAB were dried at 60 • C for 4 h.

Experiment
To prepare ZnO, the obtained IRMOF-3 was placed in a muffle furnace and heated in air at a rate of 5 • C/min in a stepwise manner from room temperature to 500 • C and kept at this temperature for 2 h.

Synthesis of ZnO@MOF-46(Zn)
To synthesize the composite material, MOF-46(Zn) was chosen to cover the ZnO surface. MOF-46(Zn) can be synthesized by the reaction of Zn 2+ ions with 2-ATP as the ligand. In this work, ZnO was prepared by the pyrolysis of IRMOF3 with different morphologies from the previous step. The prepared ZnO was used as a Zn 2+ source by dissolving ZnO in a solvent. ZnO@MOF-46(Zn) was prepared by adding 1 mmol of obtained ZnO and 1 mmol of 2-ATP into a flask containing 48 mL of a mixed solvent of DMF/H 2 O (3:1 v/v). The mixture was sonicated for 30 min and then left at room temperature for 48 h. The product was filtered and washed several times with DMF and EtOH to obtain ZnO@MOF-46(Zn). To investigate the effect of sonication and treatment times, the mixture solution was sonicated for 10 and 20 min under the same conditions for a treatment time of 48 h. The treatment was also carried out for 6 and 24 h with the same synthetic procedure.

Synthesis of MOF-46(Zn) as a Reference Material
To synthesize pure MOF-46(Zn) for use as a reference material, commercial-grade ZnO was used as the starting precursor for the Zn 2+ source to prepare pure MOF-46(Zn) with 2-ATP. In this experiment, MOF-46(Zn) was synthesized via the slow diffusion method at room temperature. First, 1 mmol of both ZnO and 2-ATP were added to the flask comprising a mixed solvent of DMF/H 2 O (48 mL; 3/1 v/v). The mixture was continuously stirred for 24 h, and afterward, the cream product was filtered and washed with DMF and ethanol several times. To study the synthesis factor, the reactants were added in different solvent ratios (1/2 v/v, only H 2 O, and only DMF) with the same procedure for 24 h or 48 h.

Characterization of Samples
All products were characterized by powder X-ray diffraction (XRD) (D8 Advance Bruker X-ray diffractometer, Billerica, MA, USA) using Cu-Kα radiation (λ = 1.54060 Å) and Fourier-transformed infrared (FT-IR) spectrophotometry (Bruker Model Vertex70) with a KBr pellet sampler in the 400-4000 cm −1 region. Thermogravimetric analysis (TGA) was performed by a Perkin Elmer TGA7 system (Waltham, MA, USA) with a heating rate of 10 • C per min under N 2 . The morphologies of the samples were monitored by scanning electron microscopy (SEM) on a Quanta 450 FEI (Graz, Austria) instrument with a tungsten filament electron source operated at 25 kV and transmission electron microscopy (TEM) on a TEM-Hitachi HT7700 system (Tokyo, Japan). The BET surface area of the obtained ZnO was calculated by N 2 adsorption. UV/Vis spectra were obtained by UV-Vis spectrophotometry on a Shimadzu UV-1800 (Kyoto, Japan) model in solid-state mode. Fluorescence spectra were examined on a Perkin-Elmer LS55 (Waltham, MA, USA) luminescence spectrometer in solid-state mode to investigate the photoelectron transfer of the samples. The amount of MOF-46(Zn) sample was equal to the quantity of MOF-46(Zn) in the ZnO/MOF-46(Zn) heterostructure sample, which was calculated to be 47.22% w/w (from the TGA result).

Photocatalytic Activity
The obtained samples (ZnO and ZnO@MOF-46(Zn)) were used as photocatalysts for the MB degradation process with UV irradiation. First, 70 mg of photocatalyst was suspended in 5 ppm MB aqueous solution (150 mL) and was then consistently stirred in the dark for 60 min to reach adsorption/desorption equilibrium. Afterward, the mixture was exposed to UV irradiation with continuous stirring. An amount of 3 mL of the solution was collected from the mixture every 30 min for 3 h to determine the absorption intensity of MB by UV-visible spectroscopy (Perkin-Elmer Lambda 35) at a maximum wavelength of 664 nm. The absorbance was calculated and reported for the photocatalytic performance of the samples. To ensure adsorption/desorption equilibrium, the mixture was treated in the dark for 30, 45, 60, and 75 min before examining the photocatalytic process. Furthermore, the inorganic products from the photocatalytic degradation of MB were determined by using ion chromatography (Metrohm 940 Professional IC Vario with a 5 µm particle size and 150 × 4 mm column dimension). Eluents NaHCO 3 /Na 2 CO 3 and HNO 3 /dipicolinic acid were introduced at 0.7 and 0.9 mL/min, respectively, for anions and cations, respectively.

Results and Discussion
Overall synthesized materials can be seen in Scheme 1. IRMOF-3 starting material for synthesis of ZnO can be prepared by various amounts of surfactant CTAB to control morphology. To synthesize ZnO, IRMOF3 was calcined. Prepared ZnO was used as the Zn 2+ source, which reacted with 2ATP by the sonication method to obtain ZnO@MOF-46(Zn).
transmission electron microscopy (TEM) on a TEM-Hitachi HT7700 system. The BET surface area of the obtained ZnO was calculated by N2 adsorption. UV/Vis spectra were obtained by UV-Vis spectrophotometry on a Shimadzu UV-1800 model in solid-state mode. Fluorescence spectra were examined on a Perkin-Elmer LS55 luminescence spectrometer in solid-state mode to investigate the photoelectron transfer of the samples. The amount of MOF-46(Zn) sample was equal to the quantity of MOF-46(Zn) in the ZnO/MOF-46(Zn) heterostructure sample, which was calculated to be 47.22% w/w (from the TGA result).

Photocatalytic Activity
The obtained samples (ZnO and ZnO@MOF-46(Zn)) were used as photocatalysts for the MB degradation process with UV irradiation. First, 70 mg of photocatalyst was suspended in 5 ppm MB aqueous solution (150 mL) and was then consistently stirred in the dark for 60 min to reach adsorption/desorption equilibrium. Afterward, the mixture was exposed to UV irradiation with continuous stirring. An amount of 3 mL of the solution was collected from the mixture every 30 min for 3 h to determine the absorption intensity of MB by UV-visible spectroscopy (Perkin-Elmer Lambda 35) at a maximum wavelength of 664 nm. The absorbance was calculated and reported for the photocatalytic performance of the samples. To ensure adsorption/desorption equilibrium, the mixture was treated in the dark for 30, 45, 60, and 75 min before examining the photocatalytic process. Furthermore, the inorganic products from the photocatalytic degradation of MB were determined by using ion chromatography (Metrohm 940 Professional IC Vario with a 5 μm particle size and 150 × 4 mm column dimension). Eluents NaHCO3/Na2CO3 and HNO3/dipicolinic acid were introduced at 0.7 and 0.9 mL/min, respectively, for anions and cations, respectively.

Results and Discussion
Overall synthesized materials can be seen in Scheme 1. IRMOF-3 starting material for synthesis of ZnO can be prepared by various amounts of surfactant CTAB to control morphology. To synthesize ZnO, IRMOF3 was calcined. Prepared ZnO was used as the Zn 2+ source, which reacted with 2ATP by the sonication method to obtain ZnO@MOF-46(Zn).

Phase of Samples
IRMOF-3 was chosen as the precursor for the preparation of the ZnO photocatalyst, and it was synthesized in three morphologies by adding different amounts of CTAB: no adding (0 mg), 80, and 150 mg. To confirm the product phase, synthesized IRMOF-3 was investigated by powder X-ray diffraction (XRD), and the results are shown in Figure 1. The XRD patterns of synthesized IRMOF-3 are in good agreement with the simulated phase of IRMOF-3. After heating at 500 °C for 2 h, the ZnO phase was obtained. The complete preparation and highly crystalline phase corresponding to wurtzite ZnO can be confirmed with JCPDS number 36-1451, as revealed in Figure 2.  IRMOF-3 was chosen as the precursor for the preparation of the ZnO photocatalyst, and it was synthesized in three morphologies by adding different amounts of CTAB: no adding (0 mg), 80, and 150 mg. To confirm the product phase, synthesized IRMOF-3 was investigated by powder X-ray diffraction (XRD), and the results are shown in Figure 1. The XRD patterns of synthesized IRMOF-3 are in good agreement with the simulated phase of IRMOF-3. After heating at 500 • C for 2 h, the ZnO phase was obtained. The complete preparation and highly crystalline phase corresponding to wurtzite ZnO can be confirmed with JCPDS number 36-1451, as revealed in Figure 2.

Morphologies of Samples
The morphologies of prepared IRMOF-3 were determined by scanning electron microscopy (SEM), and the SEM image in Figure 3 presents the different morphologies of IRMOF-3. In the absence of CTAB, the synthesized IRMOF-3 showed a typical cubic shape, became cuboctahedral, and finally became octahedral when the amount of CTAB was increased, as shown in Figure 3a-c, respectively. The BFDH (Bravais, Friedel, Donnay, and Harker) law reported that the crystal growth process depends on the relative growth rate of each facet. The facet with the slowest rate becomes the final shape. The initial shape of the obtained IRMOF-3 without CTAB is a cubic shape with six {100} facets. When the amount of CTAB in the reaction is increased, triangular facets of {111} appear in the eight corners of the cubic shape. CTAB extremely affects the {111} facet, resulting in the slow growth rate of the facet. A suitable amount of CTAB (80 mg) affects the rate of

Morphologies of Samples
The morphologies of prepared IRMOF-3 were determined by scanning electron mi croscopy (SEM), and the SEM image in Figure 3 presents the different morphologies o IRMOF-3. In the absence of CTAB, the synthesized IRMOF-3 showed a typical cubi shape, became cuboctahedral, and finally became octahedral when the amount of CTAB was increased, as shown in Figure 3a-c, respectively. The BFDH (Bravais, Friedel, Don nay, and Harker) law reported that the crystal growth process depends on the relativ growth rate of each facet. The facet with the slowest rate becomes the final shape. Th initial shape of the obtained IRMOF-3 without CTAB is a cubic shape with six {100} facets When the amount of CTAB in the reaction is increased, triangular facets of {111} appea in the eight corners of the cubic shape. CTAB extremely affects the {111} facet, resulting in the slow growth rate of the facet. A suitable amount of CTAB (80 mg) affects the rate o

Morphologies of Samples
The morphologies of prepared IRMOF-3 were determined by scanning electron microscopy (SEM), and the SEM image in Figure 3 presents the different morphologies of IRMOF-3. In the absence of CTAB, the synthesized IRMOF-3 showed a typical cubic shape, became cuboctahedral, and finally became octahedral when the amount of CTAB was increased, as shown in Figure 3a-c, respectively. The BFDH (Bravais, Friedel, Donnay, and Harker) law reported that the crystal growth process depends on the relative growth rate of each facet. The facet with the slowest rate becomes the final shape. The initial shape of the obtained IRMOF-3 without CTAB is a cubic shape with six {100} facets. When the amount of CTAB in the reaction is increased, triangular facets of {111} appear in the eight corners of the cubic shape. CTAB extremely affects the {111} facet, resulting in the slow growth rate of the facet. A suitable amount of CTAB (80 mg) affects the rate of {100} and {111} growth, presenting a cuboctahedral shape as an intermediate shape. Increasing the amount of CTAB in the reaction system enhances the growth rate ratio of {100} to {111} and finally reveals an octahedral shape (150 mg of CTAB).  The calcined products of IRMOF-3 were monitored by SEM, as shown in Figure 4. The SEM images reveal the morphologies of ZnO (ZnO(1), ZnO(2), and ZnO (3)), which maintained the original morphologies of the precursor IRMOF-3 (cube, cuboctahedron, and octahedron, respectively). However, the size of the synthesized ZnO was reduced, and increasing the ratio of surface area to volume led to a large surface area. In addition, the surfaces of cuboctahedral and octahedral ZnO were rough and contained a large amount of defects.

Synthesis of ZnO@MOF-46(Zn) Composite Materials for Use as Photocatalysts
ZnO(1) (cube), ZnO(2) (cuboctahedron), and ZnO(3) (octahedron) were used as Zn 2+ sources for the formation of MOF-46(Zn). By mixing ZnO and 2-ATP in the presence of a mixing solvent under ultrasonication and by allowing the reaction to proceed, MOF-46(Zn) production was expected. Under the same synthetic conditions, including the same sonication time, reaction time, and solvent system, ZnO(1), ZnO(2) and ZnO(3) yielded products whose XRD patterns are shown in Figure 5. The product obtained from ZnO (1) consists of ZnO and an unknown phase, while the materials produced from ZnO(2) and ZnO (3) show the presence of ZnO, MOF-46(Zn), and a small amount of the same unknown material. The calcined products of IRMOF-3 were monitored by SEM, as shown in Figure 4. The SEM images reveal the morphologies of ZnO (ZnO(1), ZnO(2), and ZnO (3)), which maintained the original morphologies of the precursor IRMOF-3 (cube, cuboctahedron, and octahedron, respectively). However, the size of the synthesized ZnO was reduced, and increasing the ratio of surface area to volume led to a large surface area. In addition, the surfaces of cuboctahedral and octahedral ZnO were rough and contained a large amount of defects.

Synthesis of ZnO@MOF-46(Zn) Composite Materials for Use as Photocatalysts
ZnO(1) (cube), ZnO(2) (cuboctahedron), and ZnO(3) (octahedron) were used as Zn 2+ sources for the formation of MOF-46(Zn). By mixing ZnO and 2-ATP in the presence of a mixing solvent under ultrasonication and by allowing the reaction to proceed, MOF-46(Zn) production was expected. Under the same synthetic conditions, including the same sonication time, reaction time, and solvent system, ZnO(1), ZnO(2) and ZnO(3) yielded products whose XRD patterns are shown in Figure 5. The product obtained from ZnO(1) consists of ZnO and an unknown phase, while the materials produced from ZnO(2) and ZnO (3) show the presence of ZnO, MOF-46(Zn), and a small amount of the same unknown material. The cuboctahedral and octahedral ZnO morphologies comprise several {111} facets. These planes drag through an array of Zn and O atoms, resulting in increased exposure of ZnO on the surface ( Figure S1). It is possible that Zn 2+ ions can be dissolved easily in the solution. Therefore, cuboctahedral and octahedral ZnO can be efficient starting materials for the synthesis of MOF-46(Zn) because the concentration of Zn 2+ is high enough. In particular, the octahedral ZnO that occupied only the facet of {111} can produce more MOF-46(Zn) phases. SEM images of ZnO@MOF-46(Zn) synthesized by each ZnO morphology are shown in Figure 6. They reveal different morphologies. ZnO(2)@MOF-46(Zn) and ZnO(3)@MOF-46(Zn) are spherical due to the aggregation of thin plates, while ZnO(1)@MOF-46(Zn) is random. The cuboctahedral and octahedral ZnO morphologies comprise several {111} facets. These planes drag through an array of Zn and O atoms, resulting in increased exposure of ZnO on the surface ( Figure S1). It is possible that Zn 2+ ions can be dissolved easily in the solution. Therefore, cuboctahedral and octahedral ZnO can be efficient starting materials for the synthesis of MOF-46(Zn) because the concentration of Zn 2+ is high enough. In particular, the octahedral ZnO that occupied only the facet of {111} can produce more MOF-46(Zn) phases. SEM images of ZnO@MOF-46(Zn) synthesized by each ZnO morphology are shown in Figure 6. They reveal different morphologies. ZnO(2)@MOF-46(Zn) and ZnO(3)@MOF-46(Zn) are spherical due to the aggregation of thin plates, while ZnO(1)@MOF-46(Zn) is random.

Sonication Time
MOF-46(Zn) was found in a significant amount when ZnO(3) was used. Therefore, the synthetic factors that might affect the formation of MOF-46(Zn) were studied by using ZnO(3) as a precursor. Considering that ZnO can be dissolved during sonication to give zinc ions, different sonication times of 10, 20, and 30 min could result in a different number of zinc ions for MOF-46(Zn) formation. The effects of ultrasonication times are shown in Figures 7 and 8. The XRD patterns in Figure 7 show that after 10 min of sonication, the main phase belongs to the unknown compound found in Figure 5, and the MOF-46(Zn) phase is barely observed. When the sonication time increases to 20 and 30 min, the MOF-46(Zn) phase can be assigned easily but with a small amount of the same unknown material present. Since the sonication time contributed to the degree of the dissolution of zinc ions from the zinc oxide surface, it is possible that at sonication times less than 20 min, the concentration of zinc ions was too low for MOF-46(Zn) formation. Instead, the low zinc ion content might favor the formation of the unknown phase. As a result, an unknown phase was still obtained with increasing sonication time, and the content of dissolved Zn 2+ ions in the solution increased. Although certain zinc ions were used to form the unknown phase, once the concentration ratio between zinc ions and 2-ATP was sufficient, MOF-46(Zn) could form. phase is barely observed. When the sonication time increases to 20 and 30 min, the MOF 46(Zn) phase can be assigned easily but with a small amount of the same unknown mate rial present. Since the sonication time contributed to the degree of the dissolution of zin ions from the zinc oxide surface, it is possible that at sonication times less than 20 min, the concentration of zinc ions was too low for MOF-46(Zn) formation. Instead, the low zin ion content might favor the formation of the unknown phase. As a result, an unknown phase was still obtained with increasing sonication time, and the content of dissolved Zn 2 ions in the solution increased. Although certain zinc ions were used to form the unknown phase, once the concentration ratio between zinc ions and 2-ATP was sufficient, MOF 46(Zn) could form.

Treatment Time
The effect of reaction time on the formation of MOF-46(Zn) was also studied. Afte 30 min of sonication, the reactions were allowed to proceed for 6, 24, and 48 h. As seen in

Treatment Time
The effect of reaction time on the formation of MOF-46(Zn) was also studied. After 30 min of sonication, the reactions were allowed to proceed for 6, 24, and 48 h. As seen in the XRD patterns (Figure 9) of the composites reacted for 6 and 24 h, only an unknown phase was presented as a product, while for the composite reacted for 48 h, both MOF-

Treatment Time
The effect of reaction time on the formation of MOF-46(Zn) was also studied. After 30 min of sonication, the reactions were allowed to proceed for 6, 24, and 48 h. As seen in the XRD patterns (Figure 9) of the composites reacted for 6 and 24 h, only an unknown phase was presented as a product, while for the composite reacted for 48 h, both MOF-46(Zn) and the unknown phase coexisted. This indicates that the reaction time also plays a significant role in governing the nucleation and growth of MOF-46(Zn) on the surface of ZnO. It is possible that to form MOF-46(Zn), the concentration of zinc ions in the solution needs to be high enough. This can be achieved by allowing the reaction to proceed for as long as 48 h so that the amount of Zn 2+ ions can reach the required value. Based on the results presented here, the proper sonication and reaction times were 30 min and 48 h, respectively.  The nanosheets assembled into spherical agglomerated particles regardless of sonication time. XRD analysis indicates that both the unknown phase and MOF-46(Zn) were produced in nanosheet form. The effect of reaction time as studied by SEM is displayed in Figure 10. The results reveal that for the composites reacted for 6 h, small nanosheets of the unknown phase with a size of approximately 0.37 nm assembled to form agglomerated particles with sizes varying from 1.9 to 3.5 nm. As the reaction time increased to 24 h, the agglomerated particles became larger in size than those produced in 6 h.  The nanosheets assembled into spherical agglomerated particles regardless of sonication time. XRD analysis indicates that both the unknown phase and MOF-46(Zn) were produced in nanosheet form. The effect of reaction time as studied by SEM is displayed in Figure 10. The results reveal that for the composites reacted for 6 h, small nanosheets of the unknown phase with a size of approximately 0.37 nm assembled to form agglomerated particles with sizes varying from 1.9 to 3.5 nm. As the reaction time increased to 24 h, the agglomerated particles became larger in size than those produced in 6 h.  The nanosheets assembled into spherical agglomerated particles regardless of sonication time. XRD analysis indicates that both the unknown phase and MOF-46(Zn) were produced in nanosheet form. The effect of reaction time as studied by SEM is displayed in Figure 10. The results reveal that for the composites reacted for 6 h, small nanosheets of the unknown phase with a size of approximately 0.37 nm assembled to form agglomerated particles with sizes varying from 1.9 to 3.5 nm. As the reaction time increased to 24 h, the agglomerated particles became larger in size than those produced in 6 h.  After 48 h of reaction, spherically agglomerated particles formed by the assembly of MOF-46(Zn) nanosheets. The sizes of the spheres are quite uniform, indicating that the nucleation and growth of MOF-46(Zn) on the surface of ZnO were homogeneous throughout the solution. From the results, we conclude that MOF-46(Zn) can be synthesized when the sonication time is 20-30 min and that the appropriate time for the synthesis of MOF-46(Zn) on the ZnO surface is 48 h.
The morphology of the products was investigated by SEM, and the results are exhibited in Figures 6, 8 and 10. After 48 h of the reaction, we observed the loss of the initial shape of ZnO precursors. Cubic ZnO(1) yielded aggregated rhombus shapes of the unknown phase and ZnO. The use of cuboctahedralZnO(2) and octahedral ZnO(3) led to the formation of microspheres assembled by MOF-46(Zn) rhombus shapes. TEM and HRTEM, as shown in Figure 11, reveal a spherical morphology, with ZnO in the core shell and MOF-46(Zn) covering the outer shell, which can be confirmed by SAED. The core shell shows the diffraction of electrons, with a d-spacing of 0.288 nm, which corresponds to the (100) plane of ZnO.

Preparation of MOF-46(Zn) as a Reference Material
The samples were also prepared with different ratios of solvent and DMF, with DMF/H2O = 1:2 and 3:1. The XRD patterns of the samples are shown in Figure 12. After stirring ZnO in DMF for 24 h, the original ZnO phase was observed in the XRD pattern. This suggests that no reaction takes place because ZnO cannot dissolve in pure DMF, while when using H2O instead, only the unknown phase appears. After stirring the mixture in the solvent with DMF/H2O of 3:1 for 24 h, MOF-46(Zn) was obtained. When the reaction time was extended to 48 h, diffraction peaks due to the unknown phase became apparent, while other peaks still existed, which suggested the existence of MOF-46(Zn). However, the use of a 1:2 ratio of DMF/H2O with stirring for 24 h is just obtained the unknown phase. These phenomena imply that the formation of MOF-46 requires using mixed DMF and H2O as a solvent and that the quantity of DMF is crucial to successfully prepare MOF-46(Zn).
Thermal gravimetric analysis was conducted to obtain information on the thermal stability of the unknown phase and MOF-46(Zn) prepared by DMF/H2O ratios of 1:2 and 3:1, respectively ( Figure 13). MOF-46(Zn) shows significant weight loss from 200 to 300 °C, corresponding to the decomposition of DMF ligands. This loss is not found in the unknown phase, implying that the unknown phase does not contain DMF. This can be correlated to the small amount of DMF present in the synthetic system when 1:2 DMF/H2O is used. In contrast, the DMF/H2O 3:1 solvent system provides enough DMF, and a large quantity of DMF favors MOF-46(Zn) synthesis. Therefore, the unknown phase could be

Preparation of MOF-46(Zn) as a Reference Material
The samples were also prepared with different ratios of solvent and DMF, with DMF/H 2 O = 1:2 and 3:1. The XRD patterns of the samples are shown in Figure 12. After stirring ZnO in DMF for 24 h, the original ZnO phase was observed in the XRD pattern. This suggests that no reaction takes place because ZnO cannot dissolve in pure DMF, while when using H 2 O instead, only the unknown phase appears. After stirring the mixture in the solvent with DMF/H 2 O of 3:1 for 24 h, MOF-46(Zn) was obtained. When the reaction time was extended to 48 h, diffraction peaks due to the unknown phase became apparent, while other peaks still existed, which suggested the existence of MOF-46(Zn). However, the use of a 1:2 ratio of DMF/H 2 O with stirring for 24 h is just obtained the unknown phase. These phenomena imply that the formation of MOF-46 requires using mixed DMF and H 2 O as a solvent and that the quantity of DMF is crucial to successfully prepare MOF-46(Zn).
Thermal gravimetric analysis was conducted to obtain information on the thermal stability of the unknown phase and MOF-46(Zn) prepared by DMF/H 2 O ratios of 1:2 and 3:1, respectively ( Figure 13). MOF-46(Zn) shows significant weight loss from 200 to 300 • C, corresponding to the decomposition of DMF ligands. This loss is not found in the unknown phase, implying that the unknown phase does not contain DMF. This can be correlated to the small amount of DMF present in the synthetic system when 1:2 DMF/H 2 O is used. In contrast, the DMF/H 2 O 3:1 solvent system provides enough DMF, and a large quantity of DMF favors MOF-46(Zn) synthesis. Therefore, the unknown phase could be called MOF-46(Zn)-H 2 O.  To study the relationship between MOF-46(Zn) and MOF-46(Zn)-H2O (unknown), the obtained MOF-46(Zn)-H2O was dehydrated at 220 °C for 30 min and then immersed in DMF with consistent stirring for 24 h to produce MOF-46(Zn). The XRD pattern in Figure S2 shows that the obtained product cannot transform to MOF-46(Zn) because of the strong coordination of aqua ligands with Zn(II) ions, resulting in aqua ligands that could not be removed from the structure. The obtained MOF-46(Zn) from a previous experiment was also immersed in aqueous solution and continuously stirred for 24 h to produce an unknown phase. The XRD pattern in Figure S3 exhibits the obtained product in an unknown phase without the MOF-46(Zn) phase. These results confirm that MOF-46(Zn)-H2O can be more easily formed than MOF-46(Zn), leading to the mixture phase of products MOF-46(Zn) and MOF-46(Zn)-H2O, which we call MOF-46(Zn)-DW.   To study the relationship between MOF-46(Zn) and MOF-46(Zn)-H2O (unknown), the obtained MOF-46(Zn)-H2O was dehydrated at 220 °C for 30 min and then immersed in DMF with consistent stirring for 24 h to produce MOF-46(Zn). The XRD pattern in Figure S2 shows that the obtained product cannot transform to MOF-46(Zn) because of the strong coordination of aqua ligands with Zn(II) ions, resulting in aqua ligands that could not be removed from the structure. The obtained MOF-46(Zn) from a previous experiment was also immersed in aqueous solution and continuously stirred for 24 h to produce an unknown phase. The XRD pattern in Figure S3 exhibits the obtained product in an unknown phase without the MOF-46(Zn) phase. These results confirm that MOF-46(Zn)-H2O can be more easily formed than MOF-46(Zn), leading to the mixture phase of products MOF-46(Zn) and MOF-46(Zn)-H2O, which we call MOF-46(Zn)-DW. To study the relationship between MOF-46(Zn) and MOF-46(Zn)-H 2 O (unknown), the obtained MOF-46(Zn)-H 2 O was dehydrated at 220 • C for 30 min and then immersed in DMF with consistent stirring for 24 h to produce MOF-46(Zn). The XRD pattern in Figure S2 shows that the obtained product cannot transform to MOF-46(Zn) because of the strong coordination of aqua ligands with Zn(II) ions, resulting in aqua ligands that could not be removed from the structure. The obtained MOF-46(Zn) from a previous experiment was also immersed in aqueous solution and continuously stirred for 24 h to produce an unknown phase. The XRD pattern in Figure S3 exhibits the obtained product in an unknown phase without the MOF-46(Zn) phase. These results confirm that MOF-46(Zn)-H 2 O can be more easily formed than MOF-46(Zn), leading to the mixture phase of products MOF-46(Zn) and MOF-46(Zn)-H 2 O, which we call MOF-46(Zn)-DW.

Structural Confirmation of Samples
To confirm the presence of ZnO and MOF-46(Zn) in the obtained products, the samples were investigated by FT-IR spectroscopy and thermal analysis. Because the product obtained from 30 min of sonication consists of both MOF-46(Zn) and MOF-46(Zn)-H 2 O, it could be called ZnO@MOF-46(Zn)-DW. The FT-IR spectrum in Figure 14 reveals the vibration band of ZnO at 441 cm −1 , but it is not obvious in the obtained products. To confirm the presence of ZnO and MOF-46(Zn) in the obtained products, the sam ples were investigated by FT-IR spectroscopy and thermal analysis. Because the produc obtained from 30 min of sonication consists of both MOF-46(Zn) and MOF-46(Zn)-H2O, i could be called ZnO@MOF-46(Zn)-DW. The FT-IR spectrum in Figure 14 reveals the vi bration band of ZnO at 441 cm −1 , but it is not obvious in the obtained products. The FT-IR spectra of the obtained products compared with the FT-IR spectrum o MOF-46(Zn) are presented in Figure 14. The vibration peaks at 1395 and 1558 cm −1 were symmetric, and the asymmetric vibration energy of the carboxylate group (-COO-) in the products shifted from 1381 and 1576 cm −1 in MOF-46(Zn). The vibration peak at approximately 1430-1630 cm −1 is displayed in MOF-46(Zn), MOF-46(Zn)-H2O (10 min of soni cation), and ZnO@MOF-46(Zn)-DW (sonicated for 20 and 30 min), contributing to the (C=C and C=N) aromatic vibration band. The vibration peak at 1668 cm −1 was also found in the ZnO@MOF-46(Zn)-DW spectra, which was expected to be the carbonyl vibration ( CO) of the DMF ligand, but it was not clear in MOF-46(Zn)-H2O sonicated for 10 min. Figure 15 shows the TGA spectrum of ZnO@MOF-46(Zn)-DW sonicated for 30 min and left to stand for 48 h under a nitrogen atmosphere. Slight degradation was observed at 70-180 °C due to the decomposition of humidity and aqua ligands of 7.68%. The temperature range of 180-300 °C presents a % weight loss of the DMF ligand of 10.80%, indi cating that the content of MOF-46(Zn) in the structure was approximately 47.22% (MOF 46(Zn) contains 22.87% of DMF in the structure). The next decomposition range of 300-460 °C is attributed to the cleavage of coordination linkages in the MOF-46(Zn) and MOF-46(Zn)-H2O phases. At 500 °C and upwards, no decomposition is found. The final produc was ZnO(30%), which was thermally stable at temperatures over 500 °C. The difference between the MOF-46(Zn) and MOF-46(Zn)-H2O phases is the DMF ligand. From a previ ous study, the structure of MOF-46(Zn)-H2O includes none of the DMF ligands. However the TGA curve indicated that MOF-46(Zn) was truly formed at ZnO@MOF-46(Zn)-DW. The FT-IR spectra of the obtained products compared with the FT-IR spectrum of MOF-46(Zn) are presented in Figure 14. The vibration peaks at 1395 and 1558 cm −1 were symmetric, and the asymmetric vibration energy of the carboxylate group (-COO-) in the products shifted from 1381 and 1576 cm −1 in MOF-46(Zn). The vibration peak at approximately 1430-1630 cm −1 is displayed in MOF-46(Zn), MOF-46(Zn)-H 2 O (10 min of sonication), and ZnO@MOF-46(Zn)-DW (sonicated for 20 and 30 min), contributing to the (C=C and C=N) aromatic vibration band. The vibration peak at 1668 cm −1 was also found in the ZnO@MOF-46(Zn)-DW spectra, which was expected to be the carbonyl vibration (-CO) of the DMF ligand, but it was not clear in MOF-46(Zn)-H 2 O sonicated for 10 min. Figure 15 shows the TGA spectrum of ZnO@MOF-46(Zn)-DW sonicated for 30 min and left to stand for 48 h under a nitrogen atmosphere. Slight degradation was observed at 70-180 • C due to the decomposition of humidity and aqua ligands of 7.68%. The temperature range of 180-300 • C presents a % weight loss of the DMF ligand of 10.80%, indicating that the content of MOF-46(Zn) in the structure was approximately 47.22% (MOF-46(Zn) contains 22.87% of DMF in the structure). The next decomposition range of 300-460 • C is attributed to the cleavage of coordination linkages in the MOF-46(Zn) and MOF-46(Zn)-H 2 O phases. At 500 • C and upwards, no decomposition is found. The final product was ZnO(30%), which was thermally stable at temperatures over 500 • C. The difference between the MOF-46(Zn) and MOF-46(Zn)-H 2 O phases is the DMF ligand. From a previous study, the structure of MOF-46(Zn)-H 2 O includes none of the DMF ligands. However, the TGA curve indicated that MOF-46(Zn) was truly formed at ZnO@MOF-46(Zn)-DW.

Photocatalytic Activity of Prepared ZnO and ZnO@MOF-46(Zn)-DW
The photocatalytic activities of the three morphologies of ZnO were studied by monitoring the photodegradation of methylene blue via UV-Vis spectroscopy. To investigate the proper time for reaching adsorption-desorption equilibrium, ZnO(3) was used as a substitute for all prepared ZnO to treat MB aqueous solutions (5 ppm) in the dark for 30, 45, 60, and 75 min. The result in Figure S4 shows that adsorption-desorption equilibrium was reached after 30 min. To verify the equilibrium of the system, the photocatalysts were treated without UV irradiation for 60 min before measuring the photodegradation process. As shown in Figure 16 and Table 1, the photodegradation efficiency of three ZnO samples was examined after UV light irradiation every 30 min for 3 h in three trials. The results show that the efficiency of ZnO photocatalysts with different ZnO cube, cuboctahedron, and octahedron morphologies are 72.70%, 82.38%, and 85.79%, respectively. The octahedral shape of ZnO presents the highest efficiency in dye photodegradation. The BET surface areas and pore volume of the synthesized ZnO were measured, as shown in Table  2.

Photocatalytic Activity of Prepared ZnO and ZnO@MOF-46(Zn)-DW
The photocatalytic activities of the three morphologies of ZnO were studied by monitoring the photodegradation of methylene blue via UV-Vis spectroscopy. To investigate the proper time for reaching adsorption-desorption equilibrium, ZnO(3) was used as a substitute for all prepared ZnO to treat MB aqueous solutions (5 ppm) in the dark for 30, 45, 60, and 75 min. The result in Figure S4 shows that adsorption-desorption equilibrium was reached after 30 min. To verify the equilibrium of the system, the photocatalysts were treated without UV irradiation for 60 min before measuring the photodegradation process. As shown in Figure 16 and Table 1, the photodegradation efficiency of three ZnO samples was examined after UV light irradiation every 30 min for 3 h in three trials. The results show that the efficiency of ZnO photocatalysts with different ZnO cube, cuboctahedron, and octahedron morphologies are 72.70%, 82.38%, and 85.79%, respectively. The octahedral shape of ZnO presents the highest efficiency in dye photodegradation. The BET surface areas and pore volume of the synthesized ZnO were measured, as shown in Table 2. Cubic ZnO presents a larger BET surface area and pore volume than cuboctahedral and octahedral ZnO. The photocatalytic efficiency is not related to the surface area but depends on the morphology. The different morphologies could affect the exposed sur-  Cubic ZnO presents a larger BET surface area and pore volume than cuboctahedral and octahedral ZnO. The photocatalytic efficiency is not related to the surface area but depends on the morphology. The different morphologies could affect the exposed surfaces. From the result of synthesized ZnO, cubic ZnO(1) consists of only the exposed {100} facet, cuboctahedral ZnO(2) presents both the exposed facets {100} and {111}, and octahedral ZnO(3) reveals only the exposed {100} facet. From Figure S1, the {111} plane drags through an array of Zn and O atoms, resulting in increased exposure of ZnO on its surface. This {111} plane can be called the active site. It is possible that the octahedral ZnO(3) that occupied only {111} facets could be exposed more to the reaction medium. Therefore, octahedral ZnO(3) exhibits a higher photocatalytic efficiency than the other ZnO morphologies.
Another explanation that describes the photodegradation efficiency is the optical properties. All the synthesized ZnO show UV-visible spectra in the UV region ( Figure  17a), which are related to the energy for the transition of electrons. Octahedral ZnO shows the largest absorption intensity, but it is slightly more intense than that of cubic ZnO. In addition, UV-visible spectra measurements were used to determine the band gap energy of ZnO (Figure 17b) by the Kubelka-Munk method [32] as follows.
(αhν) 2 where hν is the photon energy (eV), K is a constant related to the material, α is the absorption coefficient, and Eg is the band gap energy (eV). The band gaps of cubic ZnO(1), cuboctahedral ZnO (2), and octahedral ZnO(3) are 3.28, 3.15, and 3.11 eV, respectively. Therefore, the morphologies of synthesized ZnO affect the absorption range and band gap energy [22]. Octahedral ZnO reveals the lowest band gap energy, which is related to the highest photocatalytic efficiency. After completely preparing the ZnO@MOF-46(Zn)-DW composite, it was tested as a photocatalyst in the photodegradation of MB, and its efficiency was compared to that of the prepared ZnO by using the same weight (70 mg). Figure 16 and Figure S5 reveal dye photodegradation at various times. In the results, the photodegradation of ZnO@MOF-46(Zn)-DW shows better efficiency than that of prepared ZnO. A photograph of degraded MB solutions with the elapsed time of the ZnO@MOF-46(Zn)-DW photocatalysis also shown in Figure S5.
The evidence shows that ZnO@MOF-46(Zn)-DW exhibits better photocatalytic efficiency than ZnO within 60 min, and the optical and fluorescent properties were determined. Solid-state UV-vis spectroscopy was used to analyze the absorption properties of the samples. Figure 18 displays the absorption spectra of ZnO@MOF-46(Zn)-DW compared with those of ZnO and MOF-46(Zn), which resulted in a wider UV-visible range and enhanced intensity in the composite. In this study, not only does the coexistence of ZnO and MOF-46(Zn) provide extensive absorption regions, but it also leads to more absorption ability. After completely preparing the ZnO@MOF-46(Zn)-DW composite, it was tested as a photocatalyst in the photodegradation of MB, and its efficiency was compared to that of the prepared ZnO by using the same weight (70 mg). Figures 16 and S5 reveal dye photodegradation at various times. In the results, the photodegradation of ZnO@MOF-46(Zn)-DW shows better efficiency than that of prepared ZnO. A photograph of degraded MB solutions with the elapsed time of the ZnO@MOF-46(Zn)-DW photocatalysis also shown in Figure S5.
The evidence shows that ZnO@MOF-46(Zn)-DW exhibits better photocatalytic efficiency than ZnO within 60 min, and the optical and fluorescent properties were determined. Solid-state UV-vis spectroscopy was used to analyze the absorption properties of the samples. Figure 18 displays the absorption spectra of ZnO@MOF-46(Zn)-DW compared with those of ZnO and MOF-46(Zn), which resulted in a wider UV-visible range and enhanced intensity in the composite. In this study, not only does the coexistence of ZnO and MOF-46(Zn) provide extensive absorption regions, but it also leads to more absorption ability. Furthermore, the photoluminescence (PL) property of the synthesized ZnO@MOF-46(Zn)-DW was examined and related to that of MOF-46(Zn) in solid-state mode. The emission spectra in Figure 19 show the emissive position (λem) at 429 nm for MOF-46(Zn), which is near that of ZnO@MOF-46(Zn)-DW at 433 nm when excited at 385 nm. The het- Furthermore, the photoluminescence (PL) property of the synthesized ZnO@MOF-46(Zn)-DW was examined and related to that of MOF-46(Zn) in solid-state mode. The emission spectra in Figure 19 show the emissive position (λ em ) at 429 nm for MOF-46(Zn), which is near that of ZnO@MOF-46(Zn)-DW at 433 nm when excited at 385 nm. The heterostructured material exhibits a hypochromic shift and quenching intensity compared with bare MOF-46(Zn). It could be indirectly consumed by the photoelectron transfer (PET) process between ZnO and MOF-46(Zn). When ZnO@MOF-46(Zn)-DW was excited at 385 nm, electrons (e − ) in MOF-46 were also excited and jumped to the LUMO of MOF-46(Zn). Subsequently, ecan transfer to the conduction band (CB) of ZnO, resulting in a lower intensity in ZnO@MOF-46(Zn)-DW than in bare MOF-46(Zn). Furthermore, the photoluminescence (PL) property of the synthesized ZnO@MOF-46(Zn)-DW was examined and related to that of MOF-46(Zn) in solid-state mode. The emission spectra in Figure 19 show the emissive position (λem) at 429 nm for MOF-46(Zn), which is near that of ZnO@MOF-46(Zn)-DW at 433 nm when excited at 385 nm. The heterostructured material exhibits a hypochromic shift and quenching intensity compared with bare MOF-46(Zn). It could be indirectly consumed by the photoelectron transfer (PET) process between ZnO and MOF-46(Zn). When ZnO@MOF-46(Zn)-DW was excited at 385 nm, electrons (e − ) in MOF-46 were also excited and jumped to the LUMO of MOF-46(Zn). Subsequently, ecan transfer to the conduction band (CB) of ZnO, resulting in a lower intensity in ZnO@MOF-46(Zn)-DW than in bare MOF-46(Zn). The result from the photoluminescence (PL) studies mimicked the diagram shown in Figure 20, which could explain why the ZnO@MOF-46(Zn)-DW heterostructure exhibited higher photocatalytic efficiency. Usually, MOFs can absorb energy in visible light, resulting in a larger absorption energy range. Moreover, covering the ZnO surface with the MOF may reduce the recombination process between eand holes (h + ), providing a more efficient photocatalytic process than pure ZnO. In the diagram, during UV irradiation, both the electrons of ZnO and MOF are excited from the valence band (VB) to their conduction band (CB) to obtain h + at the VB. The eof the MOF in the CB can evacuate to the CB of ZnO and react with O2 in the atmosphere to create oxygen superoxide species and further convert to hydroxyl radicals (OH • ) entering the degradation process. Meanwhile, The result from the photoluminescence (PL) studies mimicked the diagram shown in Figure 20, which could explain why the ZnO@MOF-46(Zn)-DW heterostructure exhibited higher photocatalytic efficiency. Usually, MOFs can absorb energy in visible light, resulting in a larger absorption energy range. Moreover, covering the ZnO surface with the MOF may reduce the recombination process between eand holes (h + ), providing a more efficient photocatalytic process than pure ZnO. In the diagram, during UV irradiation, both the electrons of ZnO and MOF are excited from the valence band (VB) to their conduction band (CB) to obtain h + at the VB. The eof the MOF in the CB can evacuate to the CB of ZnO and react with O 2 in the atmosphere to create oxygen superoxide species and further convert to hydroxyl radicals (OH • ) entering the degradation process. Meanwhile, h + also appeared in the VB of the MOF and reacted with water (H 2 O) or hydroxide anions (OH − ) on the surface of the MOF to introduce OH • into the degradation process.
To determine the role of specific active species in the photocatalytic process, a control experiment was performed by adding 0.1 M isopropanol, which acted as a chemical selective radical scavenger for hydroxyl radicals in the MB solution. The result is shown in Figure S6, which shows that the photocatalytic activity of ZnO@MOF-46(Zn)-DW is significantly decreased in the control experiment. This indicated that OH • is the key specific active radical for the photocatalytic degradation of MB.
Ion chromatography analysis was used to determine the concentrations of inorganic products, ammonium, sulfate, and nitrate ions (NH + 4 , SO 2− 4 , and NO − 3 , respectively) obtained during MB photodegradation for a radiation time of 600 min (10 h). NH + 4 and SO 2− 4 ions are obtained in the first hour of the process, while NO − 3 ions are detected after more than six hours of photodegradation. This reveals the evolution of MB photodegradation because the concentration of these ions increases with increasing time [33] as shown in Figure S7. h + also appeared in the VB of the MOF and reacted with water (H2O) or hydroxide anions (OH − ) on the surface of the MOF to introduce OH • into the degradation process.
To determine the role of specific active species in the photocatalytic process, a control experiment was performed by adding 0.1 M isopropanol, which acted as a chemical selective radical scavenger for hydroxyl radicals in the MB solution. The result is shown in Figure S6, which shows that the photocatalytic activity of ZnO@MOF-46(Zn)-DW is significantly decreased in the control experiment. This indicated that OH • is the key specific active radical for the photocatalytic degradation of MB.
Ion chromatography analysis was used to determine the concentrations of inorganic products, ammonium, sulfate, and nitrate ions (NH , SO , and NO , respectively) obtained during MB photodegradation for a radiation time of 600 min (10 h). NH and SO ions are obtained in the first hour of the process, while NO ions are detected after more than six hours of photodegradation. This reveals the evolution of MB photodegradation because the concentration of these ions increases with increasing time [33] as shown in Figure S7.
To investigate the stability of the ZnO@MOF-46(Zn)-DW photocatalyst, the recycling procedure was performed five times by performing the photodegradation of MB and regenerating the photocatalyst with ethanol through centrifugation and drying at 75 °C before the next cycle under the same conditions ( Figure S8a). The results show that the photocatalyst can be readily regenerated with a negligible intensity change after recycling five times. After the final test, ZnO@MOF-46(Zn)-DW was subjected to XRD and SEM analysis for structural and shape evaluations ( Figure S8b,c). The XRD pattern of ZnO@MOF-46(Zn) after the degradation process exhibited both the MOF-46(Zn)-H2O and ZnO phases but not the MOF-46(Zn) phase. MOF-46(Zn) can easily transform to MOF-46(Zn)-H2O in aqueous systems. These results demonstrate that ZnO@MOF-46(Zn)-DW can serve as the greatest photocatalyst in the photodegradation of MB and possesses recyclable properties.

Conclusions
To date, many new ZnO-based photocatalysts have been synthesized. This work has demonstrated that the morphology of ZnO affects the photocatalytic efficiency performance. The octahedral ZnO shows better efficiency than the others, with 85.79% within 180 min, because it possesses more active sites and low band gap energy. The synergistic To investigate the stability of the ZnO@MOF-46(Zn)-DW photocatalyst, the recycling procedure was performed five times by performing the photodegradation of MB and regenerating the photocatalyst with ethanol through centrifugation and drying at 75 • C before the next cycle under the same conditions ( Figure S8a). The results show that the photocatalyst can be readily regenerated with a negligible intensity change after recycling five times. After the final test, ZnO@MOF-46(Zn)-DW was subjected to XRD and SEM analysis for structural and shape evaluations ( Figure S8b

Conclusions
To date, many new ZnO-based photocatalysts have been synthesized. This work has demonstrated that the morphology of ZnO affects the photocatalytic efficiency performance. The octahedral ZnO shows better efficiency than the others, with 85.79% within 180 min, because it possesses more active sites and low band gap energy. The synergistic effect on the MB photodegradation of the ZnO@MOF-46(Zn) composite was determined. A simple low-cost method was shown for preparing ZnO@MOF-46(Zn). Octahedral ZnO (higher provided phase of MOF-46(Zn) than the others) acts as a Zn 2+ source combined with 2-ATP as a ligand. The effects of sonication and reaction times were found to be essential factors for the complete synthesis of ZnO@MOF-46(Zn)-DW. Meanwhile, the appearance of an unknown phase in the products was also investigated and identified as MOF-46(Zn)-H 2 O. MOF-46(Zn) is an aqua ligand instead of a DMF ligand. ZnO@MOF-46(Zn)-DW was further used as a photocatalyst to degrade MB and compared with pure ZnO. Photocatalysis of the heterostructure exhibits higher efficiency within 60 min with 61.20% (90.09% within 180 min). The coexistence of ZnO and MOF can reduce the energy band gap, prevent the recombination process of electrons and holes, enhance the light absorption capacity from UV to visible regions, and increase the adsorption of dye due to the outstanding properties of both components, resulting in better photocatalytic efficiency. These results confirm that the synergistic effect of ZnO and MOF-46(Zn) that make ZnO@MOF-46(Zn)-DW a good photocatalyst in MB degradation.

Supplementary Materials:
The following are available online at https://www.mdpi.com/article/ 10.3390/cryst11111379/s1: Figure S1: View of {111} plane of hexagonal ZnO; Figures S2 and S3: XRD pattern of related MOF-46(Zn); Figure S4: Adsorption-desorption equilibrium experiment; Figure S5: Photograph of degraded MB solutions; Figure S6: Photocatalytic degradation of MB during present and absent isopropanol as OH • scavenger; Figure S7: Concentration of anions during the photocatalytic degradation of MB; Figure S8: Photodegradation efficiency after recycling five times, comparison of the XRD patterns before and after five recycling tests and SEM image of the photocatalyst after five cycles.