Ammonium chloride, nh4cl, is a salt formed from the neutralization of the weak base ammonia, nh3, with the strong acid hydrochloric acid. given that the value of kb for ammonia is 1.8×10−5, what is the ph of a 0.176 m solution of ammonium chloride at 25∘c?

The pH of a 0.176 M solution of ammonium chloride is 4.9902.

Explanation:

Given:

Kb for ammonia = 1.8×10⁻⁵

Since ammonium ions are the conjugate acid of ammonia.

Thus, Ka for ammonium ions;

Ka = Kw/Kb = 10⁻¹⁴ / 1.8×10⁻⁵ = 5.5556×10⁻¹⁰

Given concentration of Ammonium chloride (C) = 0.176 M

Thus, for weak acids,

pH is:

pH = 4.9902

Thus,

The pH of a 0.176 M solution of ammonium chloride is 4.9902.

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be