Question

An ore of barium contains BaCO3. A 1.620 g sample of the ore was treated with HCl to dissolve the BaCO3. The resulting solution was filtered to remove insoluble material and then treated with H2SO4 to precipitate BaSO4. The precipitate was filtered, dried, and found to weigh 0.7766 g. What is the mass of barium in the sample?

Answer 1

0.453 g of barium (Ba)

Explanation:

We know that we have 0.7766 g of BaSO₄.

molecular weight of BaSO₄ = 137 + 96 = 233 g / moles

Considering 1 mole of BaSO₄ we devise the following reasoning:

if        233 g of BaSO₄ contains 136 g of Ba

then   0.7766 g of BaSO₄ contains X g of Ba

X = (0.7766 × 136) / 233 = 0.453 g of Ba

The 1.620 g sample of the ore contains 0.453 g of Ba.

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