Question

What is the pH at the half-equivalence point in the titration of a weak base with a strong acid? The pKb of the weak base is 7.95. What is the pH at the half-equivalence point in the titration of a weak base with a strong acid? The of the weak base is 7.95. 8.75 6.05 7.95 5.25

Answer 1

Hey there!

Given the reaction:

B + H⁺   => HB⁺

At half-equivalence point :  [B] = [HB⁺]

=> [B] / [HB⁺] = 1

Henderson-Hasselbalch equation :

pH = pKa + log ( [B] ) / ( HB⁺)]

pH = 14 - pKb + log ( 1 )

pH = 14 -  7.95 + 0

pH = 6.05

Answer C

Hope that helps!