K4Nb6O17,15 KLaNb2O7,16 RbCa2Ta3O10,17 LiTaO3,18 NaTaO3 18 and KTaO3 18 were prepared by a solid-state reaction, as previously reported. The starting materials used were as follows: Li2CO3 (Wako Pure Chemical; 99.0%), Na2CO3 (Kanto Chemical; 99.0%), K2CO3 (Kanto Chemical; 99.5%), Rb2CO3 (Kojundo Chemical; 99%), CaCO3 (Kanto Chemical; 99.5%), La2O3 (Kanto Chemical; 99.99%), Nb2O5 (Kojundo Chemical; 99.95%) and Ta2O5 (Rare Metallic; 99.99%). K2La2Ti3O10 19 was prepared using a polymerized complex method. The precursor was obtained from K2CO3 (Kanto Chemical; 99.5%), Ti(OC4H9)4 (Kanto Chemical; 97%), La(NO3)3 (Kanto Chemical; 99.99%), ethylene glycol (Kanto Chemical; 99.5%) and citric acid (Sigma Aldrich; 99.5%) by pyrolysis and was calcined at 1173 K for 2 h in air using an alumina crucible. CuCl was freshly prepared by reduction of CuCl2 (Wako Pure Chemical; 99.0%) with metallic Cu in boiling dilute hydrochloric acid. The molten CuCl treatment was carried out by immersing the prepared photocatalysts in molten CuCl at 773 K for 10 h in a quartz ampoule tube under vacuum. After the molten salt treatment, the excess CuCl was removed using an aqueous NH3 solution.
Na2co3
Manufactured by Kanto Chemical
Sourced in Japan
Sodium carbonate (Na2CO3) is a chemical compound that is commonly used in various laboratory applications. It is a white, crystalline solid that is soluble in water. Sodium carbonate serves as a buffer, pH regulator, and desiccant in various experimental and analytical procedures.
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Lab products found in correlation
K2co3, by Kanto Chemical (2 mentions)
Cacl2, by Fujifilm (2 mentions)
Nahco3, by Kanto Chemical (2 mentions)
Caco3, by Kanto Chemical (1 mentions)
Li2co3, by Fujifilm (1 mentions)
Citric acid, by Merck Group (1 mentions)
Casio3, by Fujifilm (1 mentions)
Metrosep a supp 4 250 4.0 column, by Metrohm (1 mentions)
Li2co3, by Thermo Fisher Scientific (1 mentions)
Mn2o3, by Merck Group (1 mentions)
Nb2o5, by Kanto Chemical (1 mentions)
Rh 2 o 3, by Fujifilm (1 mentions)
Baco3, by Kanto Chemical (1 mentions)
V 570, by Jasco (1 mentions)
Jsm 6700f, by JEOL (1 mentions)
Miniflex, by Rigaku (1 mentions)
8 protocols using na2co3
1
Synthesis and Photocatalytic Treatment
2
Synthesis of CaCO3 Crystals
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All chemical reagents used for syntheses of CaCO3 crystals were obtained from commercial sources. PAA (Mw = 2.0 × 103) was purchased from Sigma-Aldrich. CaCl2 was obtained from Wako. Na2CO3 was obtained from Kanto Chemical. All reagents were used without purification. Deionized water, obtained by using an Auto Pure WT100 purification system (Yamato), was employed as the solvent for syntheses of CaCO3 crystals.
3
Calcium Carbonate Production from Calcium Silicate
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GLDA tetrasodium salt (GLDA-4Na, C9H9NNa4O8) solutions with different concentrations were prepared by mixing the initial GLDA-4Na solution (40 wt% in water, Tokyo Chemical Industry, Japan) with Milli-Q water, and pH was adjusted from an initial value of 13.8–~9.0 through the addition of aqueous HNO3 (60–61%, Kanto Chemical, Japan). This weakly alkaline pH was used at the beginning of the Ca extraction process to minimize the cost of pH regulation, as subsequent CaCO3 precipitation requires alkaline environments (pH > 8)32 (link),33 (link). High-purity commercial calcium silicate powders (Fig. 2 , < 30 µm) with a general composition of CaSiO3 (Wako Pure Chemical Industries, Japan) were used as a Ca source to represent silicate minerals. Na2CO3 (>99.0%, Kanto Chemical, Japan), NaHCO3 (> 99.0%, Kanto Chemical, Japan), and CO2 gas (> 99.995 vol.%, Taiyo Nippon Sanso, Japan) were used as CO2 sources to optimize the CaCO3 production system.![]()
Representative X-ray diffraction (XRD) pattern of the employed calcium silicate.
4
Ion Chromatography Analysis of Anions and Cations
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After the extraction processes, the anion and cation concentrations of each fraction were measured by ion chromatography (IC), using the Metrohm 930 Compact IC Flex system (Metrohm AG, Herisau, Switzerland). For cations, the samples were eluted through a Metrohm Metrosep C6-250/4.0 column with 8 mM ultrapure HNO3 (TAMAPURE AA-100, Tama Chemical, Kawasaki, Japan) at a flow rate of 0.9 mL·min−1. Anions were measured with a Metrohm Metrosep A Supp4-250/4.0 column with a chemical suppressor module. The mobile phase consisted of a mixture of 1.8 mM Na2CO3 and 1.7 mM NaHCO3 (Kanto Chemical, Tokyo, Japan) at a flow rate of 0.9 mL·min−1. A chemical suppressor module (Metrohm MSM) was used to decrease the background conductivity of the eluent and to transform the analytes into free anions. The column temperature was set at 35 °C throughout the analysis. Detection of cations and anions was accomplished by measuring electrical conductivity.
5
Characterization of SiO2-Al2O3-Na2CO3-K2CO3 Glass
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The glass samples were prepared using SiO2 (MORIMURA, 99.5%), Al2O3 (Kanto Chemical, 99.0%), Na2CO3 (Kanto Chemical, 99.8%) and K2CO3 (Kanto Chemical, 99.5%) reagents. After mixing the ingredients, it was melted in a platinum crucible at 1823 K for an hour at air condition using a heating rate of 10 K/min. The sample was annealed at temperature higher than the glass transition temperature in 50 K for an hour, followed by a cooling to room temperature with a quenching rate of 1 K/min.
The density of the obtained glass sample was measured by Archimedes method and the glass transition temperature was determined by measuring the thermal expansion using a thermo-mechanical analyzer (TMA; TD5000SA). For the electrical resistivity measurement, an aluminum deposited glass sample with 50 × 50 × 4 mm size was prepared, then the resistance was measured at 323 to 473 K. According to the resistance-temperature dependence, the resistivity was determined by assuming the Arrhenius equation.
The density of the obtained glass sample was measured by Archimedes method and the glass transition temperature was determined by measuring the thermal expansion using a thermo-mechanical analyzer (TMA; TD5000SA). For the electrical resistivity measurement, an aluminum deposited glass sample with 50 × 50 × 4 mm size was prepared, then the resistance was measured at 323 to 473 K. According to the resistance-temperature dependence, the resistivity was determined by assuming the Arrhenius equation.
6
Synthesis of P2-type Na-Li-Mn Oxide
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P2‐type Na0.6Li0.2Mn0.8O2 powder was synthesized through a solid‐state reaction with Na2CO3 (Kanto chemical), Li2CO3 (Alfa Aesar), and Mn2O3 (Sigma Aldrich) as the metallic precursors. Accurate stoichiometric amounts of the precursor powders, without excess Na or Li sources, were homogeneously mixed via ball milling with acetone. After drying at 65 °C for 2 h, the powder mixture was heat‐treated in air at 900 °C for 10 h and was naturally allowed to cool to room temperature. To avoid unfavorable side reactions with the ambient atmosphere and moisture, the synthesized powder was transferred to an argon‐filled glove box after the heat treatment.
7
Synthesis of Calcium Carbonate Crystals
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All chemical reagents used to synthesize CaCO3 crystals were obtained from commercial sources. PAA (Mw = 2.0 × 103) was purchased from Polysciences, Inc. (Warrington, PA, USA). CaCl2 was obtained from Wako Pure Chemicals Industries, Ltd. (Osaka, Japan). Na2CO3 was purchased from Kanto Chemical (Tokyo, Japan). All reagents were used as received.
8
Synthesis of Doped Metal Oxide Photocatalysts
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Preparation of Rh-or Ir-doped metal oxide photocatalysts SrTiO 3 :Rh(1%), 29 SrTiO 3 :Ir(0.2%), 22 TiO 2 :Rh(x%),Sb(2x%) (x ¼ 0.5 or 1.3), 25 NaTaO 3 :Ir(1%),La(2%), 24 BaTa 2 O 6 :Ir(1%),La(2%) 23 and BiVO 4 26, 27 were prepared by a solid-state reaction, a borate-ux method, and a liquid-solid reaction according to previous reports. In addition to them, NaNbO 3 :Rh(x%),Ba(y%) (x, y) ¼ (1.2, 1.44) or (1.0, 2.0) was newly prepared by a solid-state reaction. The starting materials, Na 2 CO 3 (Kanto Chemical; 99.5 or 99.8%), Nb 2 O 5 (Kanto Chemical; 99.99% or Kojundo Chemical; 99.99%), Rh 2 O 3 (Wako Chemical; 98%), and BaCO 3 (Kanto Chemical; 99%), were mixed at a molar ratio of Na/Nb/Rh/Ba ¼ 1.05-1.05y : 1 À x : x : y. An excess of sodium was added in the starting materials to compensate for volatilization. The starting materials mixture was calcined at 1173 K for 1 h, and then 1423-1473 K for 10 h once or twice. The excess sodium was washed out with water aer the calcination. The obtained powders had nonspecic shapes with aggregations, judging from the SEM images (Jeol; JSM-6700F) (Fig. S1 †). The obtained samples were identied using X-ray diffraction (Rigaku; MiniFlex, Cu Ka). Diffuse reectance spectra were obtained by a UV-vis-NIR spectrometer (JASCO, V-570) equipped with an integrator sphere and were converted to absorbance measurements via the Kubelka-Munk method.
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