Problem: The half-equivalence point of a titration occurs halfway to the endpoint, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.300 moles of a weak acid Ka = 4.7X 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?

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At the half equivalence point, the concentration of weak acid and its conjugate base is equal

Using the Henderson-Hasselbalch equation:

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Problem Details

The half-equivalence point of a titration occurs halfway to the endpoint, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.300 moles of a weak acid Ka = 4.7X 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?

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