Question

Close Problem Tutored Practice Problem 9.5.10 OUNTS TOWARDS GRADE Determine an unknown volume or concentration using an oxidation-reduction titration The concentration of a Fe solution is determined by titrating it with a 0.1138 M solution of permanganate. The balanced net ionic equation for the reaction is shown below Mn (aq)+5 Fe (aq)+12 H200) MnO(aq)+5 Fe (aq)+8 H3o (aq) In one experiment, 18.41 mL of the 0.1138 M MnO4 solution is required to react completely with 40.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2 solution. Show Approach Check&Submit Answer

Answer 1

concentration Fe²⁺ = 0.2619 M

Explanation

concentration MnO₄^- = 0.1138 M

volume MnO₄^- = 18.41 mL

moles MnO₄^- = (concentration MnO₄^-) * (volume MnO₄^-)

moles MnO₄^- = (0.1138 M) * (18.41 mL)

moles MnO₄^- = 2.095 mmol

moles Fe²⁺ = (moles MnO₄^-) * (5 moles Fe²⁺ / 1 mole MnO₄^-)

moles Fe²⁺ = (2.095 mmol) * (5 / 1)

moles Fe²⁺ = (2.095 mmol) * (5)

moles Fe²⁺ = 10.475 mmol

concentration Fe²⁺ = (moles Fe²⁺) / (volume Fe²⁺)

concentration Fe²⁺ = (10.475 mmol) / (40.00 mL)

concentration Fe²⁺ = 0.2619 M