Problem: 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.20.0 mL

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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.

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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Problem Details

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.

20.0 mL