Chemistry Practice Problems Weak Base Strong Acid Titrations Practice Problems Solution: Calculate the pH during the titration of 20.00 mL ...

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Solution: 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.

Problem

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.

Solution

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.

Reaction:

NH3(aq) + HCl(aq) → NH4+(aq) + Cl-(aq)


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

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