An unknown concentration of formic acid (HCOOH, Ka = 1.8 x 10^-4 M) is titrated with NaOH. If a 0.150 M solution of NaOH requires 35 mL of NaOH to neutralize 15.0 mL of the formic acid, calculate the concentration of the acid. Calculate the pH of the solution at the titration’s end point.
An unknown concentration of formic acid (HCOOH, Ka = 1.8 x 10^-4 M) is titrated with NaOH. If a 0.150 M solution of NaOH requires 35 mL of NaOH to neutralize 15.0 mL of the formic acid, calculate the concentration of the acid. Calculate the pH of the solution at the titration’s end point.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 124QRT
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An unknown concentration of formic acid (HCOOH, Ka = 1.8 x 10^-4 M) is titrated with NaOH.
If a 0.150 M solution of NaOH requires 35 mL of NaOH to neutralize 15.0 mL of the formic acid,
calculate the concentration of the acid.
Calculate the pH of the solution at the titration’s end point.
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