HCN ⇄ H⁺ + CN⁻
Initial 0.14 0 0
Change -x +x +x
Equilibrium (0.14 -x) +x +x
Ka = [tex] \frac{[CN^{-}][ H^{+} ]}{[HCN]} [/tex]
6.2 x 10⁻¹⁰ = [tex] \frac{(x)(x)}{(0.14 - x)} [/tex]
value of x <<<< 0.14
so x² = (6.2 x 10⁻¹⁰) (0.14)
x = 9.32 x 10⁻⁶ = [H⁺] = [CN⁻]
% ionization = Hydrogen ion concentration / total concentration x 100
= [tex] \frac{ [H^{+}]}{[HCN]} x 100 [/tex]
= [tex] \frac{(9.32 x 10^{-6} )}{0.14} x 100 [/tex]
= 6.65 x 10⁻³ %
