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)

0.0750 mol C5H5N1 L×2.65 L

= 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


0.19875 mol HNO3 × 1 L0.447 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+


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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 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.