Question

In: Chemistry

Calculate the percent ionization and the expected intial pH for the 0.10 M acetic acid solution

Expert Solution

CH3COOH(aq) + H2O(l) <-----> CH3COO^-(aq) + H3O^+(aq)

initial 0.1 M 0 M 0 M

change x x x

equilibrium 0.1-x M x x

Ka = [CH3COO-][H3O+]/[CH3COOH]

ka of acetic acid = 1.8*10^-5

1.8*10^-5 = X^2/(0.1-X)

X = 0.00133

So that,

at equilibrium

[H3O+] = X = 0.00133 M

pH = -log(H3O+)

= -log0.00133

= 2.876

Ka = CX^2

X = degree of dissociation = ?

C = inital concentration = 0.1 M

(1.8*10^-5) = 0.1*x^2

x = 0.0134

percentage dissociation = x*100

= 0.0134*100

= 1.34%

queen_honey_blossom answered 2 years ago

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