Problem: Find the pH of the equivalence point(s) and the volume (mL) of 0.447 M HNO3 needed to reach the point(s) in titrations of(a) 2.65 L of 0.0750 M pyridine (C5H5N)
FREE Expert Solution
We are asked to find the pH of the equivalence point(s) and the volume (mL) of 0.447 M HNO3 needed to reach the point in titration of 2.65 L of 0.0750 M pyridine (C5H5N)
Step 1. Calculate mole pyridine (C5H5N)
= 0.19875 mol C5H5N
Step 2. Calculate the volume of 0.447 M HNO3
at equivalence point:
mol base = mol acid
mol C5H5N = mol HNO3
= 0.445 L
Step 3. Calculate molarity C5H5NH+
C5H5N + H+ → C5H5NH+
This will act as a weak acid in the solution:
C5H5NH+ + H2O → C5H5N + H3O+
Problem Details
Find the pH of the equivalence point(s) and the volume (mL) of 0.447 M HNO3 needed to reach the point(s) in titrations of
(a) 2.65 L of 0.0750 M pyridine (C5H5N)
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 Weak Base Strong Acid Titrations concept. You can view video lessons to learn Weak Base Strong Acid Titrations. Or if you need more Weak Base Strong Acid Titrations practice, you can also practice Weak Base Strong Acid Titrations practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Lewis' class at University of Wisconsin - Eau Claire.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.