At the half point, pH = pKa. You can work it out if necessary.
pH = pKa + log(base)/(acid)
At the half way point, as you've explained above, (base) formed = (acid) left which makes (base) = (acid)
So base/acid = 1, log 1 = 0 and pH = pKa.
The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.220 moles of a monoprotic weak acid (Ka = 3.7 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?
1 answer
1 answer