The dissociation constant of weak acid HA is 1.5 10⁻⁵ . Find the percent dissociation, containing 0.2 moles per 2 liters of solution.

Step-by-step solution

Concentration of the weak acid C = 0.2 2 = 0.1 M Dissociation constant K_a = 1.5 10⁻⁵ For a weak acid, K_a = C ^2 (assuming 1 ) = K_a C = 1.5 10⁻⁵ 0.1 = 1.5 10⁻⁴ = 1.224 10⁻² Percent dissociation = 100 = 1.224 10⁻² 100 = 1.22 % Answer: 1.22 %