Write the balanced net-ionic equation for the reaction of ferrous ion with perma

Question

Write the balanced net-ionic equation for the reaction of ferrous ion with permanganate in an acidic solution. (Show your work for full credit) Fe^2+ + MnO_4 rightarrow Fe^3+ Mn^2+ A 0.5585 g sample of ferrous ammonium sulfate hexahydrate, Fe(NH_4)2(H_2O)_6) requires 21.45 mL of a KMnO_4 solution to reach a pink endpoint. What is the molarity of the KMnO_4 solution? A 1.787 g sample containing some Fe^2+ requires 31.50 ml. of a 0.02188 M KMnO_4 solution to reach a stable pink endpoint. What is the percent by mass of Fe^2+ in the sample? Calculate the percent by mass of Fe^2+ in Mohr's salt (ferrous ammonium sulfate hexahydrate). Fe(NH_4)_(SO_4)_2(H_2O)_6 to four significant figures (This is the maximum percent of Fe^2+ you can have in your unknown in today's experiment).

Explanation / Answer

Question 1.

Balance the equation in acidic solution

First, split in two half cells

Fe+2 = Fe+3

MnO4- = Mn+2

balance O, adding H2O

Fe+2 = Fe+3

MnO4- = Mn+2 + 4H2O

balance H, adding H+

Fe+2 = Fe+3

8H+ + MnO4- = Mn+2 + 4H2O

Balance charges

Fe+2 = Fe+3 + e-

5e- + 8H+ + MnO4- = Mn+2 + 4H2O

Balance e-

5Fe+2 = 5Fe+3 + 5e-

5e- + 8H+ + MnO4- = Mn+2 + 4H2O

Add all

5Fe+2 + 5e- + 8H+ + MnO4- = Mn+2 + 4H2O + 5Fe+3 + 5e-

Cancel common terms

5Fe+2 +8H+ + MnO4- = Mn+2 + 4H2O + 5Fe+3

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