# Problem: A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl.Calculate the pH at 40 mL of added acid.

###### FREE Expert Solution

We’re being asked to calculate the pH of a solution after the addition of 40 mL 0.100 M HCl solution. The solution is made up of 25.00 mL of 0.125 M pyridine (C5H5N).

HCl (strong acid) will react with C5H5N (base).

▪ C5H5N is a weak base and based on Bronsted-Lowry definition it is a proton acceptor.
▪ HCl is a strong acid and based on Bronsted-Lowry definition it is a proton donor.

Reaction:

C5H5N(aq) + HCl(aq)C5H5NH+(aq) + Cl-(aq)

We will calculate the pH of the solution using the following steps:

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###### Problem Details

A 25.0-mL sample of 0.125 M pyridine is titrated with 0.100 M HCl.

Calculate the pH at 40 mL of added acid.

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.