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Titanium dioxide (TiO2) is used extensively as a white pigment. It is produced from an ore that contains ilmenite (FeTiO3) and ferric oxide (Fe2O3). The ore is digested with an aqueous sulfuric acid solution to produce an aqueous solution of titanyl sulfate [(TiOOSO4] and ferrous sulfate (FeSO4). Water is added to hydrolyze the titanyl sulfate to H2TiO3, which precipitates, and H2SO4. The precipitate is then roasted, driving off water and leaving a residue of pure titanium dioxide. (Several steps to remove iron from the intermediate solutions as iron sulfate have been omitted from this description.) Suppose an ore containing 23.3% Ti by mass is digested with an 75.0%H2SO4 solution, supplied in 50.0% excess of the amount needed to convert all the ilmenite to titanyl sulfate and all the ferric oxide to ferric sulfate [Fe2(SO4)3]. Further suppose that 92.0% of the ilmenite actually decomposes. Calculate the masses (kg) of ore and 75.0% sulfuric acid solution that must be fed to produce 1000kg of pure TiO2. kg ore kg75.0%H2SO4