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You have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water...

You have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water to make 20.00 mL of solution. HA reacts with KOH(aq) according to the following balanced chemical equation:
HA(aq)+KOH(aq)--->KA(aq)+H2O(l)
If 13.40 mL of 0.715 M KOH is required to titrate the unknown acid to the equivalence point, what is the concentration of the unknown acid?

What is the molar mass of HA?

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