Based on the balanced chemical equation shown below,determine the molarity of a solution containing Fe²⁺(aq),if 40.00 mL of the Fe²⁺(aq)solution is required to completely react with 30.00 mL of a 0.500 M potassium bromate,KBrO₃(aq),solution.The chemical equation for the reaction is: 6 Fe²⁺(aq)+ BrO₃^-(aq)+ 6 H⁺(aq)→ 6 Fe³⁺(aq)+ Br^-(aq)+ 3 H₂O(l).

Question

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First, we need to use stoichiometry to determine the moles of KBrO3 that reacted with the Fe²⁺(aq) solution: 30.00 mL of 0.500 M KBrO3 = 0.0150 moles KBrO3 Using the balanced chemical equation, we can see that 6 moles of Fe²⁺(aq) react with 1 mole of KBrO3, so: 0.0150 moles KBrO3 * (6 moles Fe²⁺(aq) / 1 mole KBrO3) = 0.0900 moles Fe²⁺(aq) Now we can use the volume and moles of the Fe²⁺(aq) solution to determine its molarity: Molarity = moles of solute / volume of solution in liters Molarity = 0.0900 moles / 0.04000 L = 2.25 M Therefore, the correct answer is choice C, 2.25 M.

Based on the Balanced Chemical Equation Shown Below,determine the Molarity