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The Ph of 0.1m Solution of Cyanic Acid (Hcno) is 2.34. Calculate the Ionization Constant of the Acid and Its Degree of Ionization in the Solution. - CBSE (Science) Class 11 - Chemistry

ConceptIonization of Acids and Bases The pH Scale

Question

The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

Solution

c = 0.1 M

pH = 2.34

- log[H^+] = pH

-log[H^+]  = 2.34

[H^+] = 4.5 xx 10^(-3)

Also

[H^+ ] =  calpha

4.5 xx 10^(-3) = 0.1 xx alpha

(4.5 xx 10^(-3))/0.1 = alpha

alpha = 45 xx 10^(-3) = .045

Then

K_a = calpha^2

= 0.1 xx  (45 xx 10^(-3))^2

= 202.5 xx 10^(-6)

= 2.02 xx 10^(-4)`

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Solution The Ph of 0.1m Solution of Cyanic Acid (Hcno) is 2.34. Calculate the Ionization Constant of the Acid and Its Degree of Ionization in the Solution. Concept: Ionization of Acids and Bases - The pH Scale.
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