Answer:
pH = 11.05
Explanation:
It is possible to answer this question using Henderson-Hasselbalch formula:
pH = pka + log₁₀ [A] / [HA⁺]
Where A in this case is weak base (dimethylamine) and conjugate acid (HA⁺) is dimethylamine hydrochloride.
As Ka= Kw / Kb = 1x10⁻¹⁴ / 7.4x10⁻⁴ = 1.35x10⁻¹¹ And pKa is -log Ka = 10.87 pH of the solution is:
pH = 10.87 + log₁₀ [0.600] / [0.400]
pH = 11.05
I hope it helps!
The pH of the solution is 11.05
pH = pka + log₁₀ [A] / [HA⁺]
where,
A in this case is weak base (dimethylamine) and conjugate acid (HA⁺) is dimethylamine hydrochloride.
Ka = Kw / Kb
Ka= 1x10⁻¹⁴ / 7.4x10⁻⁴
Ka = 1.35x10⁻¹¹
pKa is -log Ka = 10.87
pH = 10.87 + log₁₀ [0.600] / [0.400]
pH = 11.05
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