Problem: 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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We are being asked to determine the pH at half-equivalence point.


We will use the Henderson-Hasselbach equation

pH = pKa + log[A-][HA]


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Problem Details

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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Our tutors have indicated that to solve this problem you will need to apply the Weak Acid Strong Base Titrations concept. You can view video lessons to learn Weak Acid Strong Base Titrations. Or if you need more Weak Acid Strong Base Titrations practice, you can also practice Weak Acid Strong Base Titrations practice problems.