Question

Can a solution be both ammoniacal and strongly basic? If so, how could it be determined experimentally?

Answer 1

By definition: Ammoniacal Solution --> Solution that contains any ammonium related ion (NH4+) Generally formed by NH3 gas.

In solution:

NH3 + H2O <--> NH4+ and OH-

As you can see, this solution contains NH4+ ions (ammonium ions) and OH- ions, which will increase the pH to a basic pH

pKb of Ammonia = 4.75

That is

Kb = -log[Kb]

4.75 = -log[Kb]

[Kb] = 1.77*10^-5

NH₃ + H₂O <-> NH₄⁺ + OH-

NOTE:

In a 1M ammonia solution, about 0.42% of the ammonia is converted to ammonium, equivalent to a pH of 11.63.

This is not considered "Strongly Basic"

This range is considered medium Basic

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In an experiment:

Use a pH-meter to measure the pH

If pH is between 13-14, this will be considered Strongly Basic

For the presence of NH4+ ion

Use gasification technique

Add concentrated + Warm NaOH (strong Base)

NH₄⁺ (aq) + OH- (aq) → NH₃ (g) + H₂O (l)

IF you see a bluish gas with a pungent odor, this is NH3