Titration and stoichiometry

A solution of hydrogen peroxide, H(2)O(2), is titrated with potassium permanganate, KMnO(4), according to the following equation:

5H(2)O(2) + 2KMnO(4) + 3H(2)SO(4) ---> 5O(2) + 2MnSO(4) + 8H(2)O + K(2)SO(4)

It requires 46.9mL of 0.145 mol/L KMnO(4) to titrate 50.0 mL of the solution of H(2)O(2).

What is the moles per liter concentration of H(2)O(2)?

I appreciate any help. Please show as many steps as possible. I'm trying to learn this stuff, but I have very limited resources. (I don't even know what titration is)
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STep 1: balanced equation: 5H2O2 + 2KMnO4 + 3H2SO4 ---> 5O2 + 2MnSO4 + 8H2O + K2SO4

Step 2: Convert your concentration and volume of KMnO4 into moles

Moles = C x V 0.145 x 46.9 mL = 6.80 millimoles

Step 3: use the mole ratio from the equation to find the number of miles of H2O2 you will need to react with 6.80 millimoles of KMnO4. The mole ration is 5 to 2 OR looking at it another way you will need 5/2 times as many moles of H2O2 as you have of KMnO4. So 6.80 x 5/2 = 17.0 millimoles.

Step 4: Use the fact that you have 50 mL of H2O2 and 17 millimoles of H2O2 to find the concentration of H2O2

C = n / V 17.0 mmoles / 50 mL = 0.340 mol/L

OK?

5H2O2 + 2KMnO4 + 3H2SO4 => 5O2 + 2MnSO4 + 8H2O + K2SO4

moles of MnO4- at the eq point = .145 x .0469 = 0.00680 moles

these react with 0.00680 x 5 / 2 moles of H2O2 = 0.0170 moles

these are in 50.0 ml so moles per liter = 0.0170 x 1000 / 50

= 0.3400 M H2O2