Dear Sir. Concerning your issue about whether the aluminum oxide is soluble or not in formic acid . A study of the atmospheric heterogeneous reactions of formic acid, acetic acid, and propionic acid on α-Al2O3 was performed at ambient condition by using a diffuse reflectance infrared Fourier transform spectroscopy (DRIFTS) reactor. From the analysis of the spectral features, observations of carboxylates formation provide strong evidence for an efficient reactive uptake process. Comparison of the calculated and experimental vibrational frequencies of adsorbed carboxylates establishes the bridging coordinated structures on the surface. The uptake coefficients of formic acid, acetic acid, and propionic acid on α-Al2O3 particles are (2.07±0.26)×10−3 or (2.37±0.30)×10−7 , (5.00±0.69)×10−3 or (5.99±0.78)×10−7 , and (3.04±0.63)×10−3 or (3.03±0.52)×10−7 , respectively (using geometric or BET surface area). Furthermore, the effect of varying relative humidity (RH) on these heterogeneous reactions was studied. The uptake coefficients of monocarboxylic acids on α-Al2O3 particles increase initially (RH20%) which was due to the effect of water on carboxylic acid solvation, particle surface hydroxylation, and competition for reactive sites. On the basis of the results of experimental simulation, the mechanism of heterogeneous reaction of α-Al2O3 with carboxylic acids at ambient RH was discussed. The loss of atmospheric monocarboxylic acids due to reactive uptake on available mineral dust particles may be competitive with homogeneous loss pathways, especially in dusty urban and desertified environments. I think the following below links may help you in your analysis:
https://www.atmos-chem-phys.net/10/7561/2010/acp-10-7561-2010.pdf
Thanks
This depends on the type of the alumina, alpha alumina especially if with large grain size low degree of impurities and calcined at high temperature will be practically insoluble. Nanoscale gamma alumina powders which are pporly crystallized may show considerable solubility.
Dear Sir. Concerning your issue about whether the aluminum oxide is soluble or not in formic acid . A study of the atmospheric heterogeneous reactions of formic acid, acetic acid, and propionic acid on α-Al2O3 was performed at ambient condition by using a diffuse reflectance infrared Fourier transform spectroscopy (DRIFTS) reactor. From the analysis of the spectral features, observations of carboxylates formation provide strong evidence for an efficient reactive uptake process. Comparison of the calculated and experimental vibrational frequencies of adsorbed carboxylates establishes the bridging coordinated structures on the surface. The uptake coefficients of formic acid, acetic acid, and propionic acid on α-Al2O3 particles are (2.07±0.26)×10−3 or (2.37±0.30)×10−7 , (5.00±0.69)×10−3 or (5.99±0.78)×10−7 , and (3.04±0.63)×10−3 or (3.03±0.52)×10−7 , respectively (using geometric or BET surface area). Furthermore, the effect of varying relative humidity (RH) on these heterogeneous reactions was studied. The uptake coefficients of monocarboxylic acids on α-Al2O3 particles increase initially (RH20%) which was due to the effect of water on carboxylic acid solvation, particle surface hydroxylation, and competition for reactive sites. On the basis of the results of experimental simulation, the mechanism of heterogeneous reaction of α-Al2O3 with carboxylic acids at ambient RH was discussed. The loss of atmospheric monocarboxylic acids due to reactive uptake on available mineral dust particles may be competitive with homogeneous loss pathways, especially in dusty urban and desertified environments. I think the following below links may help you in your analysis:
https://www.atmos-chem-phys.net/10/7561/2010/acp-10-7561-2010.pdf
Thanks
All metal (oxy-hydro) oxide minerals are typically insoluble in water. However, they are soluble in acid or alkali media irrespective of strong or weak acid or base and the extent of dissolution depends on several factors including concentration of acid or base. So I think aluminium oxide may be dissolved in formic acid.
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