# Sodium acetate and pH question

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Hi,

This is from a part of solution from the list of problems I have to do for Analytical Chemistry class. This one line perplexes me, and I'm basically :doh:ing myself (smacking myself in the forehead..) because I can't understand it.

The question is to find the fraction of association ($\alpha$) for $1.00 \times 10^{-12}$ M sodium acetate. Now, the solution says, "For $1.00 \times 10^{-12}$ M sodium acetate, pH = 7.00."

When I tried to use the equation for fraction of association, I ended up as x (the variable for [bH+] and [OH-]) as zero. Something isn't right, and I wonder if this is conceptual thing that I am missing out.

Sorry if this sounds like a homework. It's not. It's just one sentence that makes me confused on how you go from molarity to pH like that (and not just any pH, 7.00!).

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• 2 weeks later...

What is the fraction of association?

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