**Titration of a Tribasic Salt**In this experiment, we perform a titration of 35.0 mL of an unknown tribasic salt, Li₃A. The goal is to reach the third equivalence point using 90.00 mL of 0.250 M HCl. Below are the titration data collected during the experiment:| Volume of HCl (mL) | pH ||---------------------|------|| 15.00 | 10.45 || 30.00 | 8.62 || 45.00 | 6.79 || 60.00 | 4.86 || 75.00 | 2.93 || 90.00 | 1.35 |**Objective:**Calculate the value of Kₐ₁ of H₃A.**Data Analysis:**This data represents the pH changes observed as HCl is added to the solution containing the tribasic salt. The pH decreases as the acid neutralizes the base, progressing toward the equivalence points.The task involves finding the acid dissociation constant (Kₐ₁) of the first dissociation of H₃A. This requires analyzing the pH changes corresponding to the initial parts of the titration curve before significant buffering occurs.**Conclusion:**Upon successful calculation, the Kₐ₁ value provides insight into the strength of the first dissociation of the tribasic acid, H₃A.

A titration of 35.0 mL of an unknown tribasic salt, Li¸A, requires 90.00 mL of 0.250 M HCI to reach the 3rd equivalence point. The titration data is shown below: Vol of HCI (mL) 15.00 30.00 45.00 60.00 pH 10.45 8.62 6.79 4.86 What is the value of Ka, of H,A? 1111 75.00 90.00 2.93 1.35

A titration of 35.0 mL of an unknown tribasic salt, Li¸A, requires 90.00 mL of 0.250 M HCI to reach the 3rd equivalence point. The titration data is shown below: Vol of HCI (mL) 15.00 30.00 45.00 60.00 pH 10.45 8.62 6.79 4.86 What is the value of Ka, of H,A? 1111 75.00 90.00 2.93 1.35

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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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

**Titration of a Tribasic Salt**

In this experiment, we perform a titration of 35.0 mL of an unknown tribasic salt, Li₃A. The goal is to reach the third equivalence point using 90.00 mL of 0.250 M HCl. Below are the titration data collected during the experiment:

| Volume of HCl (mL) | pH |
|---------------------|------|
| 15.00 | 10.45 |
| 30.00 | 8.62 |
| 45.00 | 6.79 |
| 60.00 | 4.86 |
| 75.00 | 2.93 |
| 90.00 | 1.35 |

**Objective:**

Calculate the value of Kₐ₁ of H₃A.

**Data Analysis:**

This data represents the pH changes observed as HCl is added to the solution containing the tribasic salt. The pH decreases as the acid neutralizes the base, progressing toward the equivalence points.

The task involves finding the acid dissociation constant (Kₐ₁) of the first dissociation of H₃A. This requires analyzing the pH changes corresponding to the initial parts of the titration curve before significant buffering occurs.

**Conclusion:**

Upon successful calculation, the Kₐ₁ value provides insight into the strength of the first dissociation of the tribasic acid, H₃A.

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A titration of 35.0 mL of an unknown tribasic salt, Li₃A, requires 90.00 mL of 0.250 M HCl to reach the 3rd equivalence point. The titration data is shown below: Vol of HCl (mL) 15.00 30.00 45.00 60.00 75.00 90.00 pH 10.45 8.62 6.79 4.86 2.93 1.35 What is the value of Kb₁ of A³⁻?
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