Use the reaction: 2AgNO₃(aq) + H₂SO₄(aq) → Ag₂SO₄(s) + 2H₂O(l) What volume of 0.123 M AgNO₃(aq) is needed to form 0.657 g of Ag₂SO₄(s)?

Question

Quizplus · Accepted Answer

To solve this problem, we need to use stoichiometry and conversion of units. Firstly, we need to find the moles of Ag₂SO₄(s) formed: molar mass of Ag₂SO₄(s) = 311.8 g/mol moles of Ag₂SO₄(s) formed = 0.657 g / 311.8 g/mol = 0.0021073 mol The balanced chemical equation tells us that 2 moles of AgNO₃(aq) react with 1 mole of Ag₂SO₄(s). Therefore, we need: 0.0021073 mol Ag₂SO₄(s) x (2 mol AgNO₃ / 1 mol Ag₂SO₄(s)) = 0.0042146 mol AgNO₃(aq) Now we can use the definition of molarity to find the volume of 0.123 M AgNO₃(aq) needed: 0.0042146 mol AgNO₃(aq) x (1 L / 0.123 mol AgNO₃) = 0.0346 L = 34.2 mL Therefore, the best choice is C) 34.2 mL.

Use the Reaction: 2AgNO₃(aq) + H₂SO₄(aq) → Ag2SO₄(s) + 2H₂O(l)

Use the Reaction: 2AgNO₃(aq) + H₂SO₄(aq) → Ag₂SO₄(s) + 2H₂O(l)