you will synthesize iron (II) oxalate, a yellow precipitate, by reacting iron (I

Question

you will synthesize iron (II) oxalate, a yellow precipitate, by reacting iron (II) ammonium sulfate hexagydrate, Fe(NH4)2(SO4)2.6H2O, and saturated oxalic acid solution in a beaker. The compound containing the iron (II) ion will be dissoved in water.

1)List the predominant species in the Fe(NH4)2(SO4)2.6H2O solution

2)write the net ionic equation for the formation of iron (II) oxalate via the reaction of potassium oxalate and Fe(NH4)2(SO4)2.6H2O

3)Potassium oxalate solutionwill be added to the solid to provide the ligand for the complex ion. Is the cation or the anion the ligand? The formula of the ligand?

4)The oxidation number of the iron in the complex ion is +3. Is an oxidizer or a reducer required to change the oxidationnumber of the iron?

5)Write the balanced net ionic equation for the reaction of aqueous iron (II) ion reacting with H2O2 in acidic medium

Explanation / Answer

(a) Fe(NH4)2(SO4)2.6H2O(aq) => Fe2+(aq) + 2 NH4+(aq) + 2 (SO4)2-(aq) + 6 H2O(l)

The predominant species are Fe2+, NH4+, (SO4)2- and H2O


(b) Net ionic equation for precipitation:

Fe2+(aq) + (C2O4)2-(aq) => FeC2O4(s)


(c) K2C2O4(aq) => 2 K+(aq) + (C2O4)2-(aq)

The oxalate anion with negative charge is the ligand

Formula is (C2O4)2-


(d) Since oxidation state of Fe increases from +2 to +3

=> oxidation occurs

=> an oxidizer is required


(e) Net ionic equation for redox reaction:

2 Fe2+(aq) + H2O2(aq) + 2 H+(aq) => 2 Fe3+(aq) + 2 H2O(l)

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