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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What is the pH of a 0.0200 M Na3PO4 solution, show hydolysis equation and ICE table. If 5% assumption is used, verify x.
![**Acid-Dissociation Constants at 25°C**
The table below lists various acids, their chemical formulas, and their dissociation constants (Ka₁, Ka₂, Ka₃) at 25°C. These constants are a measure of the strength of the acids in water, with lower values indicating weaker acids.
| Acid | Formula | Ka₁ | Ka₂ | Ka₃ |
|--------------------|-----------|-------------|-------------|-------------|
| Acetic | CH₃CO₂H | 1.8 × 10⁻⁵ | | |
| Acetylsalicylic | C₉H₈O₄ | 3.0 × 10⁻⁴ | 1.7 × 10⁻⁷ | 4.0 × 10⁻¹² |
| Arsenic | H₃AsO₄ | 6 × 10⁻³ | 1.1 × 10⁻⁷ | 3 × 10⁻¹² |
| Arsenious | H₃AsO₃ | 5.5 × 10⁻¹⁰ | | |
| Ascorbic | HC₆H₇O₆ | 8 × 10⁻⁵ | 1.6 × 10⁻¹² | |
| Benzoic | C₆H₅CO₂H | 6.5 × 10⁻⁵ | | |
| Boric | H₃BO₃ | 5.9 × 10⁻¹⁰ | | |
| Carbonic | H₂CO₃ | 4.3 × 10⁻⁷ | 5.6 × 10⁻¹¹ | |
| Chloroacetic | CH₂ClCO₂H | 1.4 × 10⁻³ | | |
| Citric | C₆H₈O₇ | 7.1 × 10⁻⁴ | 1.7 × 10⁻⁵ | 4.1 × 10⁻⁷ |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5e0b02f6-f1e5-40a9-9b9d-2488529fd6df%2F9dd57c3b-31ef-4a59-a845-2e72ad420dda%2F5xlg9n_processed.png&w=3840&q=75)
Transcribed Image Text:**Acid-Dissociation Constants at 25°C**
The table below lists various acids, their chemical formulas, and their dissociation constants (Ka₁, Ka₂, Ka₃) at 25°C. These constants are a measure of the strength of the acids in water, with lower values indicating weaker acids.
| Acid | Formula | Ka₁ | Ka₂ | Ka₃ |
|--------------------|-----------|-------------|-------------|-------------|
| Acetic | CH₃CO₂H | 1.8 × 10⁻⁵ | | |
| Acetylsalicylic | C₉H₈O₄ | 3.0 × 10⁻⁴ | 1.7 × 10⁻⁷ | 4.0 × 10⁻¹² |
| Arsenic | H₃AsO₄ | 6 × 10⁻³ | 1.1 × 10⁻⁷ | 3 × 10⁻¹² |
| Arsenious | H₃AsO₃ | 5.5 × 10⁻¹⁰ | | |
| Ascorbic | HC₆H₇O₆ | 8 × 10⁻⁵ | 1.6 × 10⁻¹² | |
| Benzoic | C₆H₅CO₂H | 6.5 × 10⁻⁵ | | |
| Boric | H₃BO₃ | 5.9 × 10⁻¹⁰ | | |
| Carbonic | H₂CO₃ | 4.3 × 10⁻⁷ | 5.6 × 10⁻¹¹ | |
| Chloroacetic | CH₂ClCO₂H | 1.4 × 10⁻³ | | |
| Citric | C₆H₈O₇ | 7.1 × 10⁻⁴ | 1.7 × 10⁻⁵ | 4.1 × 10⁻⁷ |
Expert Solution
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Step 1
Concept based on the finding out the pH of the solution formed by the salt hydrolysis of Na3PO4.
From the given data, we can able to find out the pH of the given solution as it is a salt of strong base and weak acid.
After salt hydrolysis, the solution might be basic because one of the component is a strong base.
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Follow-up Questions
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Follow-up Question
How was x calculated, was quadratic or the 5% assumption used?
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