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NISA [10]
3 years ago
15

What is the ph of a 4.8 m pyridine solution that has kb = 1.9 × 10-9? the equation for the dissociation of pyridine is?

Chemistry
2 answers:
Arte-miy333 [17]3 years ago
7 0
C5H5N(aq)+H2)⇄C5H5NH+(aq)+OH-(aq) 
Eddi Din [679]3 years ago
4 0

Answer: 9.98


Explanation:


1) The equation for the dissociation of pyridine is:


C₅H₅N₅(aq )+ H₂O(l) ⇄ C₅H₅NH⁺(aq) + OH⁻(aq)


2) Kb equation:


Kb = [C₅H₅NH⁺(aq)] [OH⁻(aq)] / [C₅H₅N₅(aq )]


Where:


[C₅H₅NH⁺(aq)] = [OH⁻(aq)] ← from the equilibrium reaction


[C₅H₅N₅(aq )] = 4.8 M ← from the statement


⇒ 1.9 × 10 ⁻⁹ = x² / 4.8 ⇒ x² = 9.12 × 10⁻⁹


⇒ x = 9.55 × 10⁻⁵ = [OH⁻(aq)]


3) pOH


pOH = - log [OH⁻(aq)] = 4.02


4) pOH + pH = 14


⇒ pH = 14 - 4.02 = 9.98

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