A weak acid, HA and a K _a of 1.00 10⁻⁵ . If 0.100 ~mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closer to:

Step-by-step solution

Given K _a=1.00 10⁻⁵, C =0.100 mol for a weak electrolyte, degree of dissociation = K _a C = 1 10⁻⁵ 0.100 =10⁻²=1 % Related Theory In any acid-base reaction, the equilibrium will favour the reaction that moves the proton to the stronger base. This equilibrium constant is referred to as the ion-product constant for water, Kw. In pure water, some molecules act as bases and some as acids.