Answer :
Final answer:
The molarity of Pb2+ ions in the solution when 4.00 moles of PbCl2 are dissolved in 1.00 liter of solution is 4.00 M (option a).
Explanation:
The molarity of Pb2+ ions in a solution can be found by first determining the number of moles of Pb2+ in the solution and then dividing that quantity by the volume of the solution in liters. When 4.00 moles of PbCl2 are dissolved in 1.00 liters of solution, this means that 4.00 moles of Pb2+ ions are present since each molecule of PbCl2 releases one Pb2+ ion into solution. The molarity (M) is calculated as the number of moles of solute (Pb2+) divided by the volume of the solution in liters. Therefore, the molarity of the Pb2+ ions in the solution is 4.00 M (option a).
