NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0....

Question

Question

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.048 M in NH4Cl at 25 °C?

pH=_______?

Answer 1

Answer #1

The following reaction takes place in the solution :

NH₄⁺ + H₂O ----> NH₃ + H₃O⁺

Initial 0.048 0 0

Eqb. 0.048-x x x

Hydrolysis constant, Kh = [NH₃] [H₃O+] / [NH₄+]

Also, Kh = Kw / Kb

Putting values we get :

Kh = 10^-14 / 1.8*10^-5 = 5.5*10^-9

Putting this in above equation we get :

x²/0.048-x = Kh

Since Kh is small and x is also supposed to be small, we can safely ignore the term x*Kh.

Solving further we get :

x = 5.164*10^-6

pH = -log₁₀[H₃O+] = -log x = 5.29

Answer 2

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