Final answer:
Based on the provided moles of Al consumed and Pb formed, the expected stoichiometric ratio is not observed. Without additional information to reconcile this discrepancy, the concentration of Pb2+ in solution cannot be determined, making the correct answer A. Not enough information.
Step-by-step explanation:
To solve this problem, we need to use the reaction stoichiometry to relate the moles of Aluminum (Al) consumed to the moles of lead (Pb) formed. The balanced reaction is 2Al(s) + 3Pb2+(aq) → 2Al3+(aq) + 3Pb(s). This tells us that for every 2 moles of Al that react, 3 moles of Pb are produced. As the question states that 0.011 moles of Al are consumed, and 0.017 moles of Pb are formed, we can confirm the stoichiometric ratio.
However, we can immediately notice that the ratio between moles of Al consumed and Pb produced is off from the stoichiometric ratio. According to the balanced equation, the ratio of Al to Pb should be 2:3, but the given ratio would simplify to approximately 1:1.54, which does not match the expected 2:3 ratio. Without additional information or clarity on the reaction conditions, we cannot accurately calculate the concentration of Pb2+ ([Pb2+]) in solution.
Therefore, based on the provided data, the correct answer is A. Not enough information to calculate [Pb2+]. This is because the stoichiometry is not adhered to, which suggests that there might be an error or additional factors at play that were not accounted for in the problem.