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...
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The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl. How would you classify the species being titrated in this titration?
- diprotic weak base
- monoprotic weak base
- triprotic weak acid
- triprotic weak base
- diprotic weak acid
- monoprotic weak acid

Transcribed Image Text:The image displays a titration curve graph that depicts the change in pH as hydrochloric acid (HCl) is added to a solution.
**Graph Description:**
- **Axes:**
- The x-axis represents the volume of HCl added in milliliters (mL), ranging from 0 to 15 mL.
- The y-axis represents the pH level of the solution, ranging from 0 to 14.
- **Curve:**
- Initially, at 0 mL of HCl, the pH is around 11, indicating a basic solution.
- As HCl is gradually added, the pH decreases, showing an initial gradual drop.
- A significant dip occurs around 5 mL of HCl, where the pH rapidly transitions from approximately 10 to 3. This sharp change represents the equivalence point, where the solution changes from basic to acidic.
- Beyond this point, the addition of more HCl continues to lower the pH until it levels off around 2 at 15 mL of HCl.
This graph is commonly used in educational resources to illustrate the process of titration and the concept of pH changes during acid-base reactions.
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