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7.60     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.

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We have,
Concentration of cyanic acid = 0.1 M
p^H=-\log [H^+] = 2.34

Therefore, the concentration of [H^+] = antilog (-2.34)
                                                            = 4.5 \times 10^{-3}

It is known that,
[H^+] =C.\alpha  = 4.5 \times 10^{-3}
 \alpha = \frac{4.5\times 10^{-3}}{0.1} = 4.5\times 10^{-2}

Then Ionization constant (K_a) =C.\alpha^2 = 
                                                   =(0.1)(4.5\times10^{-2})^2
                                                     =2.02\times 10^{-4}

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manish

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