A sample of technical iron sulfide weighing 9.8 g (impurity content 10%) was treated with hydrochloric acid. A gas with an unpleasant

A sample of technical iron sulfide weighing 9.8 g (impurity content 10%) was treated with hydrochloric acid. A gas with an unpleasant odor was released, which was passed through concentrated sulfuric acid. The resulting new gas with a pungent odor was completely absorbed by the concentrated barium hydroxide solution. This resulted in a white precipitate. Determine the composition and weight (g) of the sediment.

FeS + 2HCl → FeCl2 + H2S ↑
H2S + 3H2SO4conc → 4SO2 ↑ + 4H2O
SO2 + Ba (OH) 2conc → BaSO3 ↓ + H2O
m (FeS) pure = 9.8 x 0.9 = 8.82 g
n (FeS) = 8.82 / 88 = 0.1 mol
n (FeS) = n (H2S) = 0.1 mol
n (SO2) = n (H2S) x 4 = 0.4 mol = n (BaSO3)
⇒ m (BaSO3) = 0.4 x (137 + 32 + 48) = 86.8 g
Answer: the precipitate is barium sulfite, its mass is 86.8 g.

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