## Ion Detection Tests### 2. Detection of \( \text{NH}_4^+ \) Ion**Test:** Add NaOH to the sample and heat gently. **Expected Reaction:** Ammonia gas is released, which turns moist red litmus paper blue.### 3. Detection of \( \text{CO}_3^{2-} \) Ion**Test:** Add dilute hydrochloric acid to the sample. **Expected Reaction:** Carbon dioxide gas is produced, causing effervescence. The gas turns limewater milky.### 4. Detection of \( \text{Cl}^- \) Ion**Test:** Add silver nitrate solution to the sample. **Expected Reaction:** A white precipitate of silver chloride is formed, which is soluble in ammonia.### 5. Detection of \( \text{SO}_4^{2-} \) Ion**Test:** Add barium chloride solution to the sample in the presence of dilute HCl. **Expected Reaction:** A white precipitate of barium sulfate is formed, which is insoluble in HCl.### 6. Detection of \( \text{I}^- \) Ion**Test:** Add silver nitrate solution to the sample. **Expected Reaction:** A yellow precipitate of silver iodide is formed, which is insoluble in ammonia.### 7. Detection of \( \text{Ag}^+ \) Ion**Test:** Add hydrochloric acid to the sample. **Expected Reaction:** A white precipitate of silver chloride is formed, which is soluble in ammonia. **Chemicals in Everyday Life**8. **Complete and balance the following equations:** - LiCl(s) + H₂SO₄(aq) → - NH₄⁺(aq) + OH⁻(aq) ⇌ - AgNO₃(aq) + I⁻(aq) → - NaHCO₃(aq) + H⁺(aq) →9. **Why should distilled water be used when making chemical tests?**10. **Assume you had a mixture of solid Na₂CO₃ and NaCl.** a. Could you use only H₂SO₄ to determine whether Na₂CO₃ was present? Explain. b. How could you show the presence of both carbonate and chloride in this mixture?*Note: There are no graphs or diagrams in the image.*

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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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Question

## Ion Detection Tests

### 2. Detection of \( \text{NH}_4^+ \) Ion
**Test:** Add NaOH to the sample and heat gently.
**Expected Reaction:** Ammonia gas is released, which turns moist red litmus paper blue.

### 3. Detection of \( \text{CO}_3^{2-} \) Ion
**Test:** Add dilute hydrochloric acid to the sample.
**Expected Reaction:** Carbon dioxide gas is produced, causing effervescence. The gas turns limewater milky.

### 4. Detection of \( \text{Cl}^- \) Ion
**Test:** Add silver nitrate solution to the sample.
**Expected Reaction:** A white precipitate of silver chloride is formed, which is soluble in ammonia.

### 5. Detection of \( \text{SO}_4^{2-} \) Ion
**Test:** Add barium chloride solution to the sample in the presence of dilute HCl.
**Expected Reaction:** A white precipitate of barium sulfate is formed, which is insoluble in HCl.

### 6. Detection of \( \text{I}^- \) Ion
**Test:** Add silver nitrate solution to the sample.
**Expected Reaction:** A yellow precipitate of silver iodide is formed, which is insoluble in ammonia.

### 7. Detection of \( \text{Ag}^+ \) Ion
**Test:** Add hydrochloric acid to the sample.
**Expected Reaction:** A white precipitate of silver chloride is formed, which is soluble in ammonia.

**Chemicals in Everyday Life**

8. **Complete and balance the following equations:**

- LiCl(s) + H₂SO₄(aq) →
- NH₄⁺(aq) + OH⁻(aq) ⇌
- AgNO₃(aq) + I⁻(aq) →
- NaHCO₃(aq) + H⁺(aq) →

9. **Why should distilled water be used when making chemical tests?**

10. **Assume you had a mixture of solid Na₂CO₃ and NaCl.**

a. Could you use only H₂SO₄ to determine whether Na₂CO₃ was present? Explain.

b. How could you show the presence of both carbonate and chloride in this mixture?

*Note: There are no graphs or diagrams in the image.*

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