Hydrogen peroxide is an effective oxidizing agent, accepting two electrons. It will oxidizediron(II) to iron(III). This process strips some of the oxalate ion from the iron, so the productis a mixture of Fe3+ (aq), FeC2O4+(aq), and Fe(C2O4)2¯(aq). Assume that the predominantproduct is Fe3+ (aq). This is a redox reaction; therefore you must balance the electrons(charge) as well as the atoms.Fill in the blank: The resulting solution is basic, causing some or all of the iron to precipitate as iron (III)hydroxide, a reddish-brown precipitate.__________ (aq) + ____ OH-(aq) → ________________ ( )

Question
Asked Oct 31, 2019

Hydrogen peroxide is an effective oxidizing agent, accepting two electrons. It will oxidized
iron(II) to iron(III). This process strips some of the oxalate ion from the iron, so the product
is a mixture of Fe3+ (aq), FeC2O4
+
(aq), and Fe(C2O4)2
¯
(aq). Assume that the predominant
product is Fe3+ (aq). This is a redox reaction; therefore you must balance the electrons
(charge) as well as the atoms.

Fill in the blank: The resulting solution is basic, causing some or all of the iron to precipitate as iron (III)
hydroxide, a reddish-brown precipitate.
__________ (aq) + ____ OH-
(aq) → ________________ ( )

check_circleExpert Solution
Step 1

Reaction of Fe(C2O4)2- with Hydrogen peroxide...

2-
Fe(C,0),(aq)H,02(aq)> Fe(C,01), (aq) +C,0,2(aq)+3OH
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2- Fe(C,0),(aq)H,02(aq)> Fe(C,01), (aq) +C,0,2(aq)+3OH

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