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Posted by on Monday, April 2, 2012 at 11:44am.

Please help!!

Given this data:
mass of unknown acid 1.4671g
Volume of NaOH used in titration 18.47mL
Concentration of the NaOH used 0.2403M
pH of the original acid solution 2.16
pH of the final acid solution 3.49

Show me how do I calculate the Ka of the unknown acid and the concentration of undissociated acid from pH measurements? and

How do I calculate the total concentration of Unknown acid from pH measurements?

If this helps answer, I have already found the molecular weight to be 165.3 g/mol
the molarity of unknown acid solution from titration is 0.1774 M


Thank you so much to whoever replies...

  • Chemistry, pH, Buffers - , Monday, April 2, 2012 at 1:02pm

    Is the 18.47 mL base used the amount to titrate to the equivalence point. Is the pH at the equivalence point 3.49 or is that some other point on the titration curve? I don't get a molar mass of 165.3 from the data above. Is there more data? I suspect so. Please type the entire question.

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