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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

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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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