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In a weak Acid-Strong Base titration, the equivalence point occurs when 12.75 mL of 0.075M NaOH is added to a solution containing 10mL weak unknown acid and 40mL Deionized water.

According to my graph from my experiment I think the half equivalence point is 6.375 mL with a pH of about 5.14 so pKA=5.14 ? Not sure if my calculations are correct but I did (12.75/1000) x 0.075M to get moles of NaOH and therefore moles of unknown Acid. Then divided the moles by (10mL acid/1000). Any help with explanation is appreciated

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