I've been using the formula:
Soap ppm (KOH) = ml HCl x Normality x 320,400/g sample.

Here's an example using .01N HCl titrant.
1.5ml HCl needed to reach end point (Bromo Blue).
1.5 x .01N x 320,400/10g (sample size)= 480.6ppm

Checking the math though I get a vastly different answer.
A .01N HCl solution contains .365mols HCl.
.365/1000= .000365mol HCl per ml.
I needed 1.5ml in the example so 1.5 x.000365= .0005475mols HCl used to reach the end point.
This tells me that there are .0005475mols K soap in the 10g sample.
I'm using a molecular weight of 320.4g per mole for Potassium oleate soap.
.000547x320.4= .175419g Potassium Oleate in the 10g sample.

The formula for ppm is:
ppm = weight(g) of solute/ weight(g) of solution x 1,000,000.
weight of the solute (K soap) = .175419g
weight of the solution = 10g
.175419/10=.0175419x1,000,000 = 17,541.9ppm

Help someone, where is my math wrong?

I copied this question to the U.K. forum as well.
Mespilus and Countrypaul pointed out my error.
My error was right in the beginning saying that a .01N solution contained .365mols as opposed to .01 moles and weighs .365g.
So the formula as written at the top is spot on.
My error.

Thanks for the help guys.