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if 16.9 mL of an acetic acid (HC2H3O2) solution are completely neutralized by 22.4 mL of...

if 16.9 mL of an acetic acid (HC2H3O2) solution are completely neutralized by 22.4 mL of 0.464 M Ba(OH)2 .

a. what is the molarity of the HC2H3O2? and

b.what is the molar concentration of barium ion in the resulting solution?

for a I have 0.615 M of HC2H3O2

and for b I havr 20.1 M but I think its off. please help

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Homework Answers

Answer #1

(a) 2CH3COOH (aq.) + Ba(OH)2 (aq.) ---------> (CH3COO)2Ba (aq.) + 2 H2O (l)

Using the neutralisation formula,

M1V1 / n1 = M2V2 / n2

M1 * 16.9 / 2 = 0.464 * 22.4 / 1

M1 = Molarity of acetic acid = 1.23 M

(b)

Ba(OH)2 (aq.) ---------> Ba2+ (aq.) + 2 OH- (OH)2 (aq.)

0.464 M                             0.464 M

Molarity of Ba2+ ions in the resulting solution = 0.464 * 22.4 / (22.4 + 16.9) = 0.264 M

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