What's the initial concentraion of the Fe^2+ solution?

Question

a total of 17.34 mL of 0.122 M H2O2 titrant is required to completely neutralize 25.00mL of an unknown concerntarion of Fe2+ in basic aqueous solution according to the generalized redox formula:

_ H2O2 + _ Fe^2+ ---> _ OH- + _ Fe ^3+

Based on the balance form of this redox reaction formula, what is the initial concentraion of the Fe^2+ solution?

Answer 1

H2O2 + 2Fe^2+(aq) ---> 2OH-(aq) + 2Fe ^3+(aq)

is your balanced equation.

Then just use mole ratios to solve for your [Fe^2+]

#mol H2O2 reacted = 0.122M * 0.01734 = 0.00211548 mol

Therefore, using mole ratios, this means that 0.00211548*2 = 0.00423096 Fe^2+ reacted

[Fe^2+] = #mol/L = 0.00423096mol/0.025L = 0.17M

[Answer: see above]