To 2 mL of aqueous iron(II) sulfate add about 2 mL of sodium hydroxide to make i

Question

To 2 mL of aqueous iron(II) sulfate add about 2 mL of sodium hydroxide to make it basic. Then add hydrogen peroxide to get a color change. (Bubbles are not part of the main reaction.) Complete and balance the double displacement reaction (not a redox reaction): FeSO_4(aq) + 2NaOH(aq) rightarrow Fe(OH)_2 + Na_2SO_4 The reactants in the redox reaction (when H_2O_2 is added) must be the compounds (or ions) actually in the solution at the start of the reaction. Since the Fe^2+ ions from the FeSO_4 solution precipitated upon addition of NaOH, the iron reactant in the redox reaction must be Fe(OH)_2(s). Fe(OH)_2 + H_2O_2 The iron product in the redox reaction is also in the form of a precipitate, and must be written as a precipitate. For the oxidation-reduction reaction. The oxidation product is___. The evidence is___. The reduction product is___. The evidence is___. Write and balance the oxidation-reduction equation (when hydrogen peroxide is added): Fe^2+ + H_2O_2 rightarrow Fe^3+ + OH^-

Explanation / Answer

1) the balanced reaction will be

FeSO4(aq) + 2NaOH(aq) --> Fe(OH)2 (s) + Na2SO4(aq)

2) The reaction between ferrous ion and peroxide will be

Fe2+ + H2O2 Fe3+ + HO• + OH

Oxidation product = Fe+3

Evidence is colour change

Reduction product = OH- and HO•

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