In titration we are interested in the equivalence point. Chemically this is when enough of the base has been added to completely neutralize the acid. Graphically this is when the reaction rate begins to decrease. How do we determine the equivalence point from P? Next, how do we determine the equivalence point from P'? What does the data suggest? Estimate the equivalence point with these two approaches using your data and graph.

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...
icon
Related questions
icon
Concept explainers
Question

In titration we are interested in the equivalence point. Chemically this is when enough of the base has been added to completely neutralize the acid. Graphically this is when the reaction rate begins to decrease. How do we determine the equivalence point from P? Next, how do we determine the equivalence point from P'? What does the data suggest? Estimate the equivalence point with these two approaches using your data and graph.

This dataset shows the pH changes in a solution as sodium hydroxide (NaOH) is added. The table consists of two columns: "mL of NaOH" and "pH."

### Data Table

- **mL of NaOH**
  - 0
  - 5
  - 8
  - 10
  - 13
  - 15
  - 18
  - 20
  - 25
  - 27
  - 28
  - 29
  - 30
  - 31
  - 33
  - 35
  - 40

- **pH**
  - 2.22
  - 2.83
  - 3.09
  - 3.23
  - 3.41
  - 3.53
  - 3.71
  - 3.83
  - 4.24
  - 4.51
  - 4.72
  - 5.1
  - 10.66
  - 11.37
  - 11.77
  - 11.96
  - 12.22

### Analysis

- **Initial Stage (0-20 mL):** The pH gradually increases from 2.22 to 3.83, indicating a weak acidic solution being neutralized.

- **Buffer Region (20-29 mL):** The pH continues to rise slowly, from 3.83 to 5.1, suggesting the presence of a buffering system.

- **Equivalence Point and Beyond (30-40 mL):** A rapid increase in pH occurs, reaching alkalinity with values from 10.66 to 12.22. This suggests the neutralization of acidic components and the dominance of NaOH.

This pattern is typical in titration, where a solution transitions from acidic to basic as a strong base is added. The dramatic rise in pH around 30 mL indicates the point where the acid is fully neutralized.
Transcribed Image Text:This dataset shows the pH changes in a solution as sodium hydroxide (NaOH) is added. The table consists of two columns: "mL of NaOH" and "pH." ### Data Table - **mL of NaOH** - 0 - 5 - 8 - 10 - 13 - 15 - 18 - 20 - 25 - 27 - 28 - 29 - 30 - 31 - 33 - 35 - 40 - **pH** - 2.22 - 2.83 - 3.09 - 3.23 - 3.41 - 3.53 - 3.71 - 3.83 - 4.24 - 4.51 - 4.72 - 5.1 - 10.66 - 11.37 - 11.77 - 11.96 - 12.22 ### Analysis - **Initial Stage (0-20 mL):** The pH gradually increases from 2.22 to 3.83, indicating a weak acidic solution being neutralized. - **Buffer Region (20-29 mL):** The pH continues to rise slowly, from 3.83 to 5.1, suggesting the presence of a buffering system. - **Equivalence Point and Beyond (30-40 mL):** A rapid increase in pH occurs, reaching alkalinity with values from 10.66 to 12.22. This suggests the neutralization of acidic components and the dominance of NaOH. This pattern is typical in titration, where a solution transitions from acidic to basic as a strong base is added. The dramatic rise in pH around 30 mL indicates the point where the acid is fully neutralized.
Titration is a method of chemical analysis in which a reactive substance is slowly added to another substance, and some property of the combined substance is measured. This procedure is taught in CHM 116, General Chemistry II.

We will be looking at an example of acid-base titration. Specifically, 25 mL of an unknown monoprotic weak acid is titrated against 0.105M NaOH (which is a strong base). This means we are adding the base to the acid using a burette in a slow and precisely controlled manner. We measure the pH after each addition. (A pH of less than 7 is an acid, and a pH of more than 7 is a base.)
Transcribed Image Text:Titration is a method of chemical analysis in which a reactive substance is slowly added to another substance, and some property of the combined substance is measured. This procedure is taught in CHM 116, General Chemistry II. We will be looking at an example of acid-base titration. Specifically, 25 mL of an unknown monoprotic weak acid is titrated against 0.105M NaOH (which is a strong base). This means we are adding the base to the acid using a burette in a slow and precisely controlled manner. We measure the pH after each addition. (A pH of less than 7 is an acid, and a pH of more than 7 is a base.)
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 1 images

Blurred answer
Knowledge Booster
Ionic Equilibrium
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
  • SEE MORE 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