1. Tardigrade
  2. Question
  3. Chemistry
  4. When 10 mL of 0.1 M acetic acid (pKa = 5.0) is titrated against 10 mL of 0.1 M ammonia solution (pKb = 5.0), the equivalence point occurs at pH

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. When $10\, mL$ of $0.1\, M$ acetic acid $(pK_{a} = 5.0)$ is titrated against $10\, mL$ of $0.1\, M$ ammonia solution $(pK_{b} = 5.0)$, the equivalence point occurs at $pH$

AIIMSAIIMS 2005Equilibrium

Solution:

$p K_{a} =-\log K_{a} \text { and } p K_{b}=-\log K_{b}$
$pH =-\frac{1}{2}\left[\log K_{a}+\log K_{w}-\log K_{b}\right]$
$=-\frac{1}{2}\left[-5+\log 10^{-14}-(-5)\right]$
$=-\frac{1}{2}[-5-14+5]$
$=7$
Thus, the end point or equivalence point is obtained at $pH =7$ in neutral medium.