Ncert Exercises & Solutions

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.

c = 0.1 M

pH = 2.34

$- \log [H^{+}] = pH - \log [H^{+}] = 2.34 [H^{+}] = 4.5 \times 10^{- 3} Also, [H^{+}] = cα 4.5 \times 10^{- 3} = 0.1 \times α \frac{4.5 \times 10^{- 3}}{0.1} = α α = 45 \times 10^{- 3} = . 045 Then, K_{α} = {cα}^{2} = 0.1 \times {(45 \times 10^{- 3})}^{2} = 202.5 \times 10^{- 6} = 2.02 \times 10^{- 4}$

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