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Class 11
Chemistry
Equilibrium
it has been found that the ph of a 0 01m solution...

Question:
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pK_a.

Answer:

Let the organic acid be HA.

⇒ HA ↔ H⁺ + A^-

Concentration of HA = 0.01 M

pH = 4.15

-log[H⁺] = 4.15

[H⁺] = 7.08x10^-5

Now, K_a = [H⁺] [A^-] / [HA]

[H⁺] = [A^-] = 7.08x10^-5

[HA] = 0.01

Then,

K_a = 7.08x10^-5x 7.08x10^-5/ 0.01

K_a = 5.01x10^-7

pK_a= -log K_a

= -log(5.01x10^-7)

pK_a = 6.3001

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Question:
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pK_a.

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Question: It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pKa.

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Question:
It has been found that the pH of a 0.01M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its pK_a.