An organic monobasic acid has dissociation constant 1.96 10⁻⁸ . What is its percentage dissociation in 0.01 M solution ?

Step-by-step solution

For a weak monobasic acid, the dissociation constant is given by K_a = C ^2 , where is the degree of dissociation and C is the concentration. = K_a C Substituting the given values K_a = 1.96 10⁻⁸ and C = 0.01 M: = 1.96 10⁻⁸ 0.01 = 1.96 10⁻⁶ = 1.4 10⁻³ Percentage dissociation = 100 Percentage dissociation = 1.4 10⁻³ 100 = 0.14 , % Answer: 0.14 , %