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Finding the ionic strength of a buffer?

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AussieKenDoll:
I made a buffer of 0.1M acetic acid-sodium acetate having a pH of 5.0 using 1 M acetic acid solution and a 1M sodium acetate solution.
So the molarity of the buffer is 0.1M and how do I find the ionic strength?
This is my calculation
Molarity of the buffer = 0.1 mol dm^(-3)
CH3COOH- 1M  CH3COONa – 1M

I=1/2 ∑cizi^2
I=1/2 (1(+1)^2+1(-1)^2+1(+1)^2 )
I=0.5×3
I=1.5 mol dm^(-3) 

AWK:
buffer of 0.1M acetic acid-sodium acetate
means that the sum of concentrations of both reagents is 0.1 M. For calculations you need a volume of buffer solution. Otherwise, use 1 L.

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