Multiple Choice
What is the concentration of chloride ions in the solution formed by mixing 3.50 g of NaCl with 40.9 mL of 0.407 M CaCl2 solution, assuming the volumes are additive?
6. Chemical Quantities & Aqueous Reactions
Solution Stoichiometry
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What volume of 0.305 M AgNO₃ is required to react exactly with 155.0 mL of 0.274 M Na₂SO₄ solution? (Hint: Write a balanced chemical equation for the reaction.)
A
139.0 mL
B
155.0 mL
C
278.0 mL
D
310.0 mL
Verified step by step guidance1
Write the balanced chemical equation for the reaction between AgNO₃ and Na₂SO₄: 2 AgNO₃ + Na₂SO₄ → 2 NaNO₃ + Ag₂SO₄.
Calculate the moles of Na₂SO₄ using its concentration and volume: \( \text{moles of Na}_2\text{SO}_4 = 0.274 \text{ M} \times 0.155 \text{ L} \).
Use the stoichiometry from the balanced equation to find the moles of AgNO₃ needed. According to the equation, 2 moles of AgNO₃ react with 1 mole of Na₂SO₄.
Calculate the volume of 0.305 M AgNO₃ solution required using the moles of AgNO₃ and its concentration: \( \text{Volume of AgNO}_3 = \frac{\text{moles of AgNO}_3}{0.305 \text{ M}} \).
Convert the volume from liters to milliliters by multiplying by 1000, as the final answer should be in milliliters.
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