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Buffer/pKa/pH?

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Calculate the pH of a butter formed by dissolving 22 g of benzoic acid and 28 g of sodium benzoate in 1 liter of solution.

I know that you have to find the pKa in order to solve the equation pH=pKa+log(acid/base), and I know that you have to find the molarity of the acid and the base.

The molarity of benzoic acid is .180M.

The molarity of sodium benzoate is .194M.

Can anyone help me please??

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  1. The pKa of benzoic acid is 4.2 (see source below). Actually, the Henderson - Hasselbalch equation is:

    pH = pKa + log([A-]/[HA]).

    You can take it from here.

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