Solid Nal is slowly added to a solution that is 0.0079 M Cu* and 0.0077 M Ag*. Which compound will begin to precipitate first? Nal Cul AgI Calculate [Ag*] when Cul just begins to precipitate. X 10 M Enter your answer in scientific notation. What percent of Ag* remains in solution at this point?
Solid Nal is slowly added to a solution that is 0.0079 M Cu* and 0.0077 M Ag*. Which compound will begin to precipitate first? Nal Cul AgI Calculate [Ag*] when Cul just begins to precipitate. X 10 M Enter your answer in scientific notation. What percent of Ag* remains in solution at this point?
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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![**Problem Statement:**
Be sure to answer all parts.
Solid NaI is slowly added to a solution that is 0.0079 M Cu\(^+\) and 0.0077 M Ag\(^+\).
**Question 1:**
Which compound will begin to precipitate first?
- NaI
- CuI
- AgI
**Question 2:**
Calculate [Ag\(^+\)] when CuI just begins to precipitate.
Enter your answer in scientific notation.
\[ \_\_\_ \times 10^{\_\_\_} \, \text{M} \]
**Question 3:**
What percent of Ag\(^+\) remains in solution at this point?
\[ \_\_\_ \% \]
---
**Graph/Diagram Description:**
The table below lists the solubility products (K\(_{sp}\)) of some slightly soluble ionic compounds at 25°C:
| Compound | K\(_{sp}\) | Compound | K\(_{sp}\) |
|----------|------------|----------|------------|
| Aluminum hydroxide [Al(OH)₃] | 1.8 × 10\(^{-33}\) | Lead(II) chromate (PbCrO₄) | 2.0 × 10\(^{-16}\) |
| Barium carbonate (BaCO₃) | 8.1 × 10\(^{-9}\) | Lead(II) fluoride (PbF₂) | 4.1 × 10\(^{-8}\) |
| Barium fluoride (BaF₂) | 1.0 × 10\(^{-6}\) | Lead(II) iodide (PbI₂) | 7.9 × 10\(^{-9}\) |
| Barium sulfate (BaSO₄) | 1.1 × 10\(^{-10}\) | Lead(II) sulfate (PbS) | 3.4 × 10\(^{-28}\) |
| Bismuth sulfide (Bi₂S₃) | 1.6 × 10\(^{-72}\) | Lead(II) sulfide (PbS) | 3.4 × 10\(^{-28}\) |
| Cadmium sulfide (CdS) | 1.0 × 10\(^{-28}\) |](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F264afef6-5fb8-47a1-a0f2-19efba1e1114%2F6b37330a-8e96-4af5-8d21-918bff8a6a81%2Flpay8j8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Be sure to answer all parts.
Solid NaI is slowly added to a solution that is 0.0079 M Cu\(^+\) and 0.0077 M Ag\(^+\).
**Question 1:**
Which compound will begin to precipitate first?
- NaI
- CuI
- AgI
**Question 2:**
Calculate [Ag\(^+\)] when CuI just begins to precipitate.
Enter your answer in scientific notation.
\[ \_\_\_ \times 10^{\_\_\_} \, \text{M} \]
**Question 3:**
What percent of Ag\(^+\) remains in solution at this point?
\[ \_\_\_ \% \]
---
**Graph/Diagram Description:**
The table below lists the solubility products (K\(_{sp}\)) of some slightly soluble ionic compounds at 25°C:
| Compound | K\(_{sp}\) | Compound | K\(_{sp}\) |
|----------|------------|----------|------------|
| Aluminum hydroxide [Al(OH)₃] | 1.8 × 10\(^{-33}\) | Lead(II) chromate (PbCrO₄) | 2.0 × 10\(^{-16}\) |
| Barium carbonate (BaCO₃) | 8.1 × 10\(^{-9}\) | Lead(II) fluoride (PbF₂) | 4.1 × 10\(^{-8}\) |
| Barium fluoride (BaF₂) | 1.0 × 10\(^{-6}\) | Lead(II) iodide (PbI₂) | 7.9 × 10\(^{-9}\) |
| Barium sulfate (BaSO₄) | 1.1 × 10\(^{-10}\) | Lead(II) sulfate (PbS) | 3.4 × 10\(^{-28}\) |
| Bismuth sulfide (Bi₂S₃) | 1.6 × 10\(^{-72}\) | Lead(II) sulfide (PbS) | 3.4 × 10\(^{-28}\) |
| Cadmium sulfide (CdS) | 1.0 × 10\(^{-28}\) |
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