We are being asked to determine the pH at half-equivalence point.
We will use the Henderson-Hasselbach equation
The half equivalence point of a titration occurs halfway to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.280 moles of a monoprotic weak acid (Ka = 6.1x10-5) is titrated with NaOH what is the pH of the solution at the half-equivalence point?
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