What is the pH at the equivalence point from the titration of .145 g of a weak acid with .100 M NaOH?
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The data table is shown as: Volume of NaOH added (mL)...................... pH 0.00....................................… 2.88 5.00 ........................................… 4.15 10.00...................................… 4.58 12.50...................................… 4.76 15.00...................................… 4.93 20.00 ........................................… 5.36 24.00 ........................................… 6.14 24.90...................................… 7.15 25.00...................................… 8.73 26.00 ........................................… 11.29 30.00 ........................................… please help me!!!
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Answer:
Hi pH = pKw / 2 + pKa / 2 + log( [salt] ) / 2
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