**Calculation of degrees of dissociation (α) in solution**

pH = 2.34 or log\(\bigg[\frac{1}{H^+}\bigg]\) = 2.34

\(\bigg[\frac{1}{H^+}\bigg]\) = Antilog 2.34 or [H^{+}]

= Antilog (-2.34)

[H^{+}] = Antilog (3.66) = 4.571 x 10^{-3} M

α = \(\frac{[H^+]}{C}\) = \(\frac{(4.571\times 10^{-3}\,M)}{(0.1\,M)}\)

= 4.571 x 10^{-2} = 0.04571 M

**Calculation of the ionization constant of the acid**

[H^{+}] = (K_{a} x C)^{1/2}

or, [H^{+}]^{2} = (K_{a} x C)