Determine the mass of BaSO₄ that is produced by the reaction of 45.0 mL of 0.155 M H₂SO₄ and 60.0 mL of 0.125 M BaCl₂. Assume that BaSO₄ is totally insoluble.

Question

Quizplus · Accepted Answer

First, we need to write the balanced chemical equation:

HSO4^- + BaCl2 → BaSO4↓ + 2HCl

From this equation, we can see that 1 mole of BaSO4 is produced for every 1 mole of HSO4^- reacted.

Next, we need to calculate the number of moles of HSO4^- and BaCl2 used in the reaction:

moles of HSO4^- = (0.155 M) x (0.045 L) = 0.006975 mol
moles of BaCl2 = (0.125 M) x (0.060 L) = 0.0075 mol

Since the mole ratio of HSO4^- to BaSO4 is 1:1, the number of moles of BaSO4 produced is also 0.006975 mol.

Finally, we can calculate the mass of BaSO4 produced using its molar mass:

mass of BaSO4 = (0.006975 mol) x (233.38 g/mol) = 1.626 g

Therefore, the answer is choice B, 1.62 g.

Determine the Mass of BaSO4 That Is Produced by the Reaction

Determine the Mass of BaSO₄ That Is Produced by the Reaction