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A 0.02 M Solution of Pyridinium Hydrochloride Has Ph = 3.44. Calculate the Ionization Constant of Pyridine - Chemistry

A 0.02 M solution of pyridinium hydrochloride has pH = 3.44. Calculate the ionization constant of pyridine

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Solution

pH = 3.44

We know that,

pH = – log [H+]

`:. [H^+] = 3.63xx 10^(-4)`

Then `K_h = (3.63 xx 10^(-4))^2/0.02`  (∵ concentration = 0.02 M)

`=> K_h = 6.6 xx 10^(-6)`

Now `K_h = K_w/K_a`

`= > K_a = K_w/K_h = 10^(-14)/(6.6 xx 10^(-6))`

`= 1.51 xx 10^(-9)`

Concept: Ionization of Acids and Bases - Ionization of Weak Bases
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APPEARS IN

NCERT Class 11 Chemistry Textbook
Chapter 7 Equilibrium
Q 62 | Page 230
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