Write the precipitation reaction for ammonium carbonate in aqueous solution: Be sure to specify the state of each reactant and product. Is ammonium carbonate considered soluble or not soluble ? A. Soluble B. Not soluble
Write the precipitation reaction for ammonium carbonate in aqueous solution: Be sure to specify the state of each reactant and product. Is ammonium carbonate considered soluble or not soluble ? A. Soluble B. Not soluble
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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![**Educational Exercise: Precipitation Reaction for Ammonium Carbonate**
**Instructions:**
Write the *precipitation reaction* for ammonium carbonate in an aqueous solution.
Be sure to specify the state of each reactant and product.
**Reaction Equation:**
\[ \_\_\_\_ + \_\_\_\_ \rightarrow \_\_\_\_ \]
**Question:**
Is ammonium carbonate considered soluble or not soluble?
- A. Soluble
- B. Not soluble
**Options for Submission:**
- Submit Answer
- Retry Entire Group
*Note: You have 3 more group attempts remaining.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F756e5f41-24a8-4ad5-bbf6-ede0df93f901%2F62372682-62e4-4b40-b7df-230b462a6a6d%2F8suk5p_processed.png&w=3840&q=75)
Transcribed Image Text:**Educational Exercise: Precipitation Reaction for Ammonium Carbonate**
**Instructions:**
Write the *precipitation reaction* for ammonium carbonate in an aqueous solution.
Be sure to specify the state of each reactant and product.
**Reaction Equation:**
\[ \_\_\_\_ + \_\_\_\_ \rightarrow \_\_\_\_ \]
**Question:**
Is ammonium carbonate considered soluble or not soluble?
- A. Soluble
- B. Not soluble
**Options for Submission:**
- Submit Answer
- Retry Entire Group
*Note: You have 3 more group attempts remaining.*
Transcribed Image Text:**Solubility Rules for Some Ionic Compounds in Water**
**Soluble Ionic Compounds**
1. **All sodium (Na⁺), potassium (K⁺), and ammonium (NH₄⁺) salts are SOLUBLE.**
2. **All nitrate (NO₃⁻), acetate (CH₃CO₂⁻), chlorate (ClO₃⁻), and perchlorate (ClO₄⁻) salts are SOLUBLE.**
3. **All chloride (Cl⁻), bromide (Br⁻), and iodide (I⁻) salts are SOLUBLE, EXCEPT those containing: lead, silver, or mercury (I) (Pb²⁺, Ag⁺, Hg₂²⁺) which are NOT soluble.**
4. **All sulfate (SO₄²⁻) salts are SOLUBLE, EXCEPT those containing: calcium, silver, mercury (I), strontium, barium, or lead (Ca²⁺, Ag⁺, Hg₂²⁺, Sr²⁺, Ba²⁺, Pb²⁺) which are NOT soluble.**
**Not Soluble Ionic Compounds**
5. **Hydroxide (OH⁻) and oxide (O²⁻) compounds are NOT SOLUBLE, EXCEPT those containing: sodium, potassium, or barium (Na⁺, K⁺, Ba²⁺) which are soluble.**
6. **Sulfide (S²⁻) salts are NOT SOLUBLE, EXCEPT those containing: sodium, potassium, ammonium, or barium (Na⁺, K⁺, NH₄⁺, Ba²⁺) which are soluble.**
7. **Carbonate (CO₃²⁻) and phosphate (PO₄³⁻) salts are NOT SOLUBLE, EXCEPT those containing: sodium, potassium, or ammonium (Na⁺, K⁺, NH₄⁺) which are soluble.**
---
**Definitions:**
- **Soluble compounds** are defined as those that dissolve to the extent of 1 g or more per 100 g water.
**NOT soluble compounds** are further classified as:
- *Slightly soluble*, which dissolve to the extent of 0.01 g to 1 g per 100 g water.
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