2. If 25.00 mL of a 0.09864 M CH3COOH (Ka = 1.8 x 10-5) solution is titrated with a 0.1027 M NaOH solution, what will be the pH in the following conditions? a) at the start before adding the titrant (0.00 mL) b) after adding 5.00 mL of the titrant c) after adding 25.00 mL titrant

2. If 25.00 mL of a 0.09864 M CH3COOH (Ka = 1.8 x 10-5) solution is titrated with a 0.1027 M NaOH solution, what will be the pH in the following conditions? a) at the start before adding the titrant (0.00 mL) b) after adding 5.00 mL of the titrant c) after adding 25.00 mL titrant

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

2. If 25.00 mL of a 0.09864 M CH;COOH (Ka = 1.8 x 10-5) solution is titrated with a 0.1027 M
NaOH solution, what will be the pH in the following conditions?
a) at the start before adding the titrant (0.00 mL)
b) after adding 5.00 mL of the titrant
c) after adding 25.00 mL titrant
d) equivalence point
e) adding 35.00 mL of the titrant

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