CHEM 1A Lecture 27: 12-02 Lecture 27
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CHEM 1A Full Course Notes
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Titrating weak acid with a strong base. This is in the middle of the buffer region. Major differences between a strong acid and a weak acid-strong titration curve with a strong base. :: \lled the buffer region, appears before the steep rise to the equivalence point. z,. The ph at the equivalence point is greater than 7. 00. Assume 0. 1 eq base has been added to a fully protonated solution of acetic acid. The henderson-hasselbalch equation can be used to calculate the ph of the solution: Ph = pka + {log [a-] / [ha]} must be between -1 and 1. Ph = pka + log [0. 1] / [0. 9] Both a weak acid, ha, and its conjugate base, a-, in solution. Both a weak base and its conjugate acid in solution. Ph = pka + log [a-] / [ha] The loss of each mole of h+ shows up as separate equivalence point.