Not exactly. The pH of the solution affects the solubility of some oxides, but not all. The solubility of oxides also depends on the type of oxide and the type of metal or nonmetal it contains. For example, oxides of Group 1A metals are always soluble, regardless of the pH, because they are basic and react with water to form hydroxides. Oxides of nonmetals are usually soluble if they are acidic and form strong acids with water, such as SO 2 or CO 2 . Oxides of metals are usually insoluble, unless they are amphoteric and react with acids, such as Al 2 O 3 or ZnO. Does that make sense?
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