Molarity = moles / volume in L Molarity = 0.0342/8.39 Molarity = 0.004076 M solution Now use the Ka equation to calculate the [H+] of the solution: Ka for CH3COOH = 1.8*10^-5 Ka = [H+] / [CH3COOH] 1.8*10^-5 = [H+]²/ 0.004076 [H+]² = (1.8910^-5) * ( 0.004076 [H+]² = 7.34*10^-8 [H+] = 2.71*10^-4 pH = -log [H+] pH = -log 2.71*10^-4 pH = 3.57 Solution Molarity = moles / volume in L Molarity = 0.0342/8.39 Molarity = 0.004076 M solution Now use the Ka equation to calculate the [H+] of the solution: Ka for CH3COOH = 1.8*10^-5 Ka = [H+] / [CH3COOH] 1.8*10^-5 = [H+]²/ 0.004076 [H+]² = (1.8910^-5) * ( 0.004076 [H+]² = 7.34*10^-8 [H+] = 2.71*10^-4 pH = -log [H+] pH = -log 2.71*10^-4 pH = 3.57.