A Bronsted-Lowry base is defined as a substance that
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This question is asking for the pH of a buffer solution between ammonia and nitric acid, with given volumes and concentrations. At the end, the result turns out to be 10.488.
<h3>Buffers</h3>In chemistry, buffers are known as substances attempting to hold a relatively constant pH by mixing and acid and a base (weak and strong). In such a way, for the substances given, the first step will be to calculate the consumed moles as they are mixed:
Now, since ammonia is in a greater proportion, one can calculate how much of it is left after being consumed by the nitric acid:
And its new concentration:
Next, with ammonia's ionization:
We set up the equilibrium expression based on ammonia's Kb:
Which can be solved by introducing x and using ammonia's Kb:
Then, we solve for x which is also equal to the concentration of ammonium and hydroxide ions in the solution:
Ultimately, we calculate the pOH and then turn it into pH with:
Learn more about buffers: brainly.com/question/24188850