# 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.

###### FREE Expert Solution
91% (440 ratings)
###### FREE Expert 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:

91% (440 ratings) ###### Problem Details

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.

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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Our expert Chemistry tutor, Dasha took 8 minutes and 44 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Troyer's class at UTSA.