We’re being asked to calculate the pH of a solution after the addition of 20.0 mL 0.0250 M HCl solution. The solution is made up of 30.0 mL of 0.050 M ammonia (NH3).
HCl (strong acid) will react with NH3 (base).
▪ NH3 is a base and based on Bronsted-Lowry definition it is a proton acceptor.
▪ HCl is an acid and based on Bronsted-Lowry definition it is a proton donor.
NH3(aq) + HCl(aq) → NH4+(aq) + Cl-(aq)
We will calculate the pH of the solution using the following steps:
Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added.
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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.
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