#
**Problem**: 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 8.75.

###### FREE Expert Solution

Answer:

###### Sign up for free to keep watching this solution

###### Sign up for free

581,500

students enrolled97%

improved grades2,784

minutes of videos###### FREE Expert Solution

We are asked to **calculate the pH at the half equivalence point**.

We can use the **Henderson Hasslebalch equation to calculate the pOH of a titrated base: **

$\overline{){\mathbf{pOH}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{{\mathbf{pK}}}_{{\mathbf{b}}}{\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{log}}{\mathbf{\left(}}\frac{{\mathbf{BH}}^{\mathbf{+}}}{\mathbf{B}}{\mathbf{\right)}}}$

We then can use the equation below to** calculate the pH:**

$\overline{){\mathbf{pH}}{\mathbf{\hspace{0.17em}}}{\mathbf{=}}{\mathbf{}}{\mathbf{14}}{\mathbf{-}}{\mathbf{}}{\mathbf{pOH}}}$

###### Sign up for free to view this solution

###### Sign up for free

581,500

students enrolled97%

improved grades2,784

minutes of videos###### Problem Details

What is the pH at the half-equivalence point in the titration of a weak base with a strong acid? The pK_{b} of the weak base is 8.75.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equivalence Point concept. If you need more Equivalence Point practice, you can also practice Equivalence Point practice problems .

How long does this problem take to solve?

Our expert Chemistry tutor, Dayana took 3 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Dawe's class at Wilfrid Laurier University.