Find the pH of a 0.08744 acetic acid solution Solution VERY GOOD DEDUCTION. Acet

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VERY GOOD DEDUCTION. Acetic acid ionizes partially, so you need the pka or ka value of acetic acid (in data book), this should be given in the question. SO YOU NEED TO CALCULATE THE CONCENTRATION OF H+ (OR H3O+) Calculation CH3COOH(aq) + H2O(l) -----> CH3COO-(aq) + H3O+(aq) Ka IS DISSOCIATION CONSTANT WHICH IS CONCENTRATION OF PRODUCT/CONCENTRATION OF REACTANT. Ka= [CH3COO-] * [H3O+] / [CH3COOH] [H2O] is not included because its change in concentration is negligible. After partial dissociation, [CH3COOH] IS STILL APPROXIMATELY 0.1M. [CH3COO-] = [H3O+] Ka of CH3COOH=1.74 * 10^-5 (from data book) 1.74 * 10^-5 = [H30+]^2 / 0.1 [H30]^2 = 1.74*10^-5 * 0.08744 [H30+]= 0.00123 pH= -log[H30+] pH= -log(0.00123) pH= 2.9089 pH of 0.08744M acetic acid is 2.9

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