a) pH = -log 0.10 M = 1.00
b) So, the equilibrium is CH3COOH + H2O <--> H3O+ + CH3COO-.
Ka = 1.8X10^-5 = [H3O+][CH3COO-]/[CH3COOH]
Let x = [H3O+] = [CH3COO-]. [CH3COOH] = 0.10 M. Then:
1.8X10^-5 = x^2 / 0.10
x = [H3O+] = 1.34X10^-3
pH = -log (1.34X10^-3) = 2.87
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Answers & Comments
a) pH = -log 0.10 M = 1.00
b) So, the equilibrium is CH3COOH + H2O <--> H3O+ + CH3COO-.
Ka = 1.8X10^-5 = [H3O+][CH3COO-]/[CH3COOH]
Let x = [H3O+] = [CH3COO-]. [CH3COOH] = 0.10 M. Then:
1.8X10^-5 = x^2 / 0.10
x = [H3O+] = 1.34X10^-3
pH = -log (1.34X10^-3) = 2.87