Iron(II) can be oxidized (not an oxidation problem) by an acidic Cr2O72- solution according to the net ionic equation.
Cr2O72- + 6 Fe2+ + 14 H+ 2 Cr3+ + 6 Fe3+ + 7 H2O
If it takes 50.0 mL of 0.0250 M Cr2O72- to titrate a solution containing Fe2+, what is the mass of Fe2+ recovered. The molar mass of Fe is =55.8 g/mol?

Question

Iron(II) can be oxidized (not an oxidation problem) by an acidic Cr2O72- solution according to the net ionic equation.
Cr2O72- + 6 Fe2+ + 14 H+ 2 Cr3+ + 6 Fe3+ + 7 H2O
If it takes 50.0 mL of 0.0250 M Cr2O72- to titrate a solution containing Fe2+, what is the mass of Fe2+ recovered. The molar mass of Fe is =55.8 g/mol?

aaronq · Answer

find the moles of Cr2O7^2- and use the stoichiometric ratio to find moles of Fe^2+ first, then convert to mass.