An analytical chemist is titrating of a solution of butanoic acid with a solutio

Question

An analytical chemist is titrating of a solution of butanoic acid with a solution of . The of butanoic acid is . Calculate the pH of the acid solution after the chemist has added of the solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of solution added. Round your answer to decimal places. An analytical chemist is titrating 118.3 mL of a 0.3500 M solution of butanoic acid (HC3H7CO2) with a 0.400 M solution of KOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 115.4 mL of the solution to it. Note for advanced students: you may assume the final volume equals the initial volume of KOH the solution plus the volume of solution added. Round your answer to 2 decimal places.

Explanation / Answer

Butanoic acid + KOH

initial moles butanoic acid = 0.3500 M x 118.3 ml = 41.405 mmol

KOH added = 0.4000 M x 115.4 ml = 46.16 mmol

excess [KOH] = [OH-] = 4.755 mmol/233.7 ml = 0.0203 M

pOH = -log[OH-] = -log(0.0203) = 1.7

pH = 14 - pOH = 14 - 1.7 = 12.3

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