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PH at the equivalence point?

Calculate the pH at equivalence point?

  • Ok, I am doing a lab where we are doing a titration of ASA (aspirin) with NaOH. I calculate the moles of ASA to be .0030. We used 31.12ml of NaOH to do the titration. It was a 40l solution of ASA that was .098M. We are supposed to "calculate the pH at the equivalence point using stoich and an equilibrium expression. Apparently, the conjugate base formed from this reaction also has an effect on pH. So we are supposed to determine the molarity of the conjugate base produced through stoich, and then work the equilibrium problem. I have no idea what this means, and I have no idea how to answer this question. It would be great if you could show your work.

  • Answer:

    aspirin = HC9H7O4 what is the mass of the aspirin used? what is the molarity of the NaOH? what is the Ka of aspirin? you are missing a lot of info here

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