We’re being asked to calculate the pH of a solution after the addition of 15 mL 0.1000 M HCl solution. The solution is made up of 20.00 mL of 1.000 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:
Calculate the pH during the titration of 20.00 mL of 0.1000 M ammonia with 0.1000 M HCl(aq) after 15 mL of the acid have been added. Kb of ammonia = 1.8 x 10-5.
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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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