Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Determine the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H5NH2, Kb = 4.3x10-4) by 0.333 M HCIO4 at the following points. (a) Before the addition of any HCIO4| (b) After the addition of 13.5 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 49.1 mL of HCIO4

Determine the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H5NH2, Kb = 4.3x10-4) by 0.333 M HCIO4 at the following points. (a) Before the addition of any HCIO4| (b) After the addition of 13.5 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 49.1 mL of HCIO4

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
**Titration of Ethylamine with Perchloric Acid: Calculating pH at Key Points** This experiment involves determining the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H₅NH₂), which has a base dissociation constant (Kb) of 4.3×10⁻⁴, using 0.333 M perchloric acid (HClO₄). The pH is to be calculated at the following key points: (a) **Before the Addition of Any HClO₄** - Calculate the initial pH of the ethylamine solution. (b) **After the Addition of 13.5 mL of HClO₄** - Determine the pH after adding the indicated volume of the acid. (c) **At the Titration Midpoint** - Find the pH at the halfway point to the equivalence. (d) **At the Equivalence Point** - Calculate the pH when the moles of acid equal the moles of base. (e) **After Adding 49.1 mL of HClO₄** - Determine the final pH after this amount of acid is added. **Note**: No graphs or diagrams are present. Solutions require calculations based on stoichiometry and equilibrium chemistry principles.
Transcribed Image Text:**Titration of Ethylamine with Perchloric Acid: Calculating pH at Key Points** This experiment involves determining the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H₅NH₂), which has a base dissociation constant (Kb) of 4.3×10⁻⁴, using 0.333 M perchloric acid (HClO₄). The pH is to be calculated at the following key points: (a) **Before the Addition of Any HClO₄** - Calculate the initial pH of the ethylamine solution. (b) **After the Addition of 13.5 mL of HClO₄** - Determine the pH after adding the indicated volume of the acid. (c) **At the Titration Midpoint** - Find the pH at the halfway point to the equivalence. (d) **At the Equivalence Point** - Calculate the pH when the moles of acid equal the moles of base. (e) **After Adding 49.1 mL of HClO₄** - Determine the final pH after this amount of acid is added. **Note**: No graphs or diagrams are present. Solutions require calculations based on stoichiometry and equilibrium chemistry principles.
Expert Solution
Step 1

we need to calculate the pH of solution during the given titration 

steps

Step by step

Solved in 4 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Acid-Base Titrations
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS