Question

Question 1: Hydrogen peroxide will be used to oxidize the iron(II) in the complex ion to iron(III). Several things happen in this reaction:

Iron(II) is oxidized to iron(III)

The oxalate ions that were attached to the iron(II) in the complex ion return to the solution (as oxalate ions)

Each hydrogen peroxide molecule is reduced to form two hydroxide ions

Part A - Oxidation of iron(II) to iron(III).

Write a balanced net ionic equation for the oxidation of the iron(II) complex ion with hydrogen peroxide. Make certain that your equation depicts all three things described in the introduction and that is it blanced for nujmber of electrons transferred (charge) as well as for atoms.

Question 2:Part A - The dissolution of iron(II) ammonium sulfate

In the first step of experiment #9, iron(II) ammonium sulafte is desolved in water. Write the equation for this process.

Write the equation for the dissolution of Fe(NH4)2(SO4)2. Include the phases in your equation

Answer 1

1. oxidation of the iron(II) complex ion with hydrogen peroxide:

The half−reactions are:

oxidation: Fe²⁺ → Fe³⁺

reduction: H₂O₂ → H₂O

Balancing the second equation for O and H gives:

2H⁺ + H₂O₂ → 2H₂O

Balance both equations for charge with electrons:

Fe²⁺ → Fe³⁺ + e⁻

2H⁺ + H₂O₂ + 2e⁻ → 2H₂O

Now, multiply the first half−reaction by 2 to equalize charge

2Fe²⁺ → 2Fe³⁺ + 2e⁻

add, and cancel electrons

2Fe²⁺ + 2H⁺ + H₂O₂ → 2Fe³⁺ + 2H₂O

2. Dissociation of ferrous ammonium sulfate:

(NH₄)₂Fe(SO₄)₂ (s) --> 2 NH4⁺_(aq) + Fe⁺²_(aq) + 2 (SO₄)^-2_(aq)