Question & Answer: II. Determination of Unknown Concentration Procedure: Add 1.2 mL of unknown Fe (II) solution…..

II. Determination of Unknown Concentration

Procedure:

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Add 1.2 mL of unknown Fe (II) solution into an Erlenmeyer flask along with 20.0 mL DI H₂O, 1.0 mL 9 M H₂SO₄, 2 drops 0.1 M MnSO₄, and 1 drop of 3 M phosphoric acid (H₃PO₄). Use a graduated pipet with 0.02 M KMnO₄ to titrate solution.

1. Volume of Fe(II) solution used- 1.2 mL

2. Volume of KMnO4 solution used- 1.28 mL —– this is the amount of KMnO₄ that was used to turn solution a pink color

*3. Balance the following chemical reaction

__MnO₄^– + __Fe⁺² + __H⁺ —–> __Mn⁺² + __Fe⁺³ + __H₂O

*4. Calculate the molarity of the Fe(II) solution. _________ M

Expert Answer

Answer

Moles of KMnO4 used = Molarity*Volume = 0.02*(1.28/1000) = 0.0000256

The balanced reaction is:

MnO₄^– + 5Fe²⁺ + 8H⁺ —–> Mn²⁺ + 5Fe³⁺ + 4H₂O

1 moles MnO4^– need 5 moles Fe²⁺

So,

0.0000256 moles need: 0.0000256*5 = 0.000128 moles Fe²⁺

So, unknown molarity = moles/volume = 0.000128/(1.2/1000) = 0.1067 M

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