Stoichiometric Question! Urgent!

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I am confused about iodometric titrations using a standard:

An iodimetric titration is a redox titration beginning with an analyte in its reduced state.
An iodometric titration is a redox titration beginning with an analyte in its oxidized state.

Mcat-review.org says the following:

S=standard
X=intermediate
A=analyte
T=titrane
(ox) or (red) = in its oxidized state (oxidizing agent) or in its reduced state (reducing agent)

"Iodometric titration with standard:

• 1) Sox + Xred → Sred + Xox
• 2) Xox + Ared(limiting reagent) → Xred + Aox
• 3) Xox(left over) + 2I- → Xred + I2
• 4) I2 + Tred → 2I- + Tox
• notes:
  • step 1 makes an intermediate of accurately known amount.
  • step 2: the analyte eating up an unknown, but calculatable, amount of the intermediate.
  • step 3: the remaining intermediate going on to make I2
  • step 4: Here, you will find out how much T is needed to eat up all the I2 produced from step 3. From this, you'll know the amount of Xox(left over). You also can calculate the amount of Xox originally produced by the standard. Thus Xox - Xox(left over) = the amount of analyte. Important note: this is usually not a simple subtraction because you need to take stochiometric ratios into consideration."

I don't understand step #2, or specifically, where A(ox) comes in. A(0x) should be the analyte in its oxidized state, the one we are attempting to titrate. Therefore it should be in the start of the reaction. Why is step 2 listening A(red) as the starting analyte? Where does this analyte come from? If we have an A(red) analyte, we might as well just complete and iodimetric titration instead of an iodometric one.