#### 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)`

Is there an error in this question or solution?

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.