A 20.0 mL sample of 1.80 M formic acid, HCHO2, is titrated with a 2.40 M NaOH solution. pK, = 3.74 for formic acid. Calculate the pH at the following points of the titration: a) After adding 5.00 mL of NaOH b) ½ equivalence point c) Equivalence point
A 20.0 mL sample of 1.80 M formic acid, HCHO2, is titrated with a 2.40 M NaOH solution. pK, = 3.74 for formic acid. Calculate the pH at the following points of the titration: a) After adding 5.00 mL of NaOH b) ½ equivalence point c) Equivalence point
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 52QAP: A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of...
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![A 20.0 mL sample of 1.80 M formic acid, HCHO2, is titrated with a 2.40 M NaOH solution.
pK, = 3.74 for formic acid. Calculate the pH at the following points of the titration:
a) After adding 5.00 mL of NaOH
b) ½ equivalence point
c) Equivalence point](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1552ca78-5815-4aaf-a191-7400f3dd2649%2F05aa36ef-963a-4cfc-9d02-209b890e36b4%2Fz03r2vj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 20.0 mL sample of 1.80 M formic acid, HCHO2, is titrated with a 2.40 M NaOH solution.
pK, = 3.74 for formic acid. Calculate the pH at the following points of the titration:
a) After adding 5.00 mL of NaOH
b) ½ equivalence point
c) Equivalence point
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