Macmillan Learning Complete and balance the precipitation reaction. Include physical states. Refer to the solubilities of common salts as needed. precipitation reaction: CuCl₂(aq) + Na₂CO3(aq) →| I
Macmillan Learning Complete and balance the precipitation reaction. Include physical states. Refer to the solubilities of common salts as needed. precipitation reaction: CuCl₂(aq) + Na₂CO3(aq) →| I
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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How can we complete the precipitation reaction?
![**Transcription and Explanation for Educational Website**
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### Precipitation Reaction Exercise
**Task:**
Complete and balance the precipitation reaction. Include physical states. Refer to the solubilities of common salts as needed.
**Precipitation Reaction:**
\[ \text{CuCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \]
**Instructions:**
- Use the provided reference for solubility rules to determine which compounds will precipitate.
- Ensure the reaction is balanced with respect to both mass and charge.
- Indicate the physical states of all reactants and products (aqueous or solid, as appropriate).
**Additional Tools:**
- Special notation buttons are available for symbols such as (s) for solid, (aq) for aqueous, and other common symbols used in chemistry equations.
### Detailed Explanation
When copper(II) chloride \((\text{CuCl}_2)\) and sodium carbonate \((\text{Na}_2\text{CO}_3)\) are mixed in solution, a double displacement reaction occurs, forming copper(II) carbonate \((\text{CuCO}_3)\) and sodium chloride \((\text{NaCl})\).
**Based on Solubility:**
- Copper(II) carbonate \((\text{CuCO}_3)\) is generally insoluble in water and will form a precipitate (solid).
- Sodium chloride \((\text{NaCl})\) is soluble and will remain in aqueous form.
**Balanced Equation:**
\[ \text{CuCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \text{CuCO}_3(s) + 2\text{NaCl}(aq) \]
This equation can be confirmed by considering the charges and atoms:
- **Charges:** The total charge on both reactant and product sides is zero, maintaining charge balance.
- **Atoms:** There are equal numbers of each type of atom on both sides (1 Cu, 2 Na, 3 O, 2 Cl on both sides).
**Conclusion:**
By following the stoichiometry and solubility rules, one can determine the products and their states in this precipitation reaction. Use these guidelines to handle similar chemical equations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9437567b-8da5-455d-a4fe-2bd0f454b63f%2Fd2b4ef77-950c-4f9f-b22a-e1d9c67d200d%2Fdr10pv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription and Explanation for Educational Website**
---
### Precipitation Reaction Exercise
**Task:**
Complete and balance the precipitation reaction. Include physical states. Refer to the solubilities of common salts as needed.
**Precipitation Reaction:**
\[ \text{CuCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \]
**Instructions:**
- Use the provided reference for solubility rules to determine which compounds will precipitate.
- Ensure the reaction is balanced with respect to both mass and charge.
- Indicate the physical states of all reactants and products (aqueous or solid, as appropriate).
**Additional Tools:**
- Special notation buttons are available for symbols such as (s) for solid, (aq) for aqueous, and other common symbols used in chemistry equations.
### Detailed Explanation
When copper(II) chloride \((\text{CuCl}_2)\) and sodium carbonate \((\text{Na}_2\text{CO}_3)\) are mixed in solution, a double displacement reaction occurs, forming copper(II) carbonate \((\text{CuCO}_3)\) and sodium chloride \((\text{NaCl})\).
**Based on Solubility:**
- Copper(II) carbonate \((\text{CuCO}_3)\) is generally insoluble in water and will form a precipitate (solid).
- Sodium chloride \((\text{NaCl})\) is soluble and will remain in aqueous form.
**Balanced Equation:**
\[ \text{CuCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \text{CuCO}_3(s) + 2\text{NaCl}(aq) \]
This equation can be confirmed by considering the charges and atoms:
- **Charges:** The total charge on both reactant and product sides is zero, maintaining charge balance.
- **Atoms:** There are equal numbers of each type of atom on both sides (1 Cu, 2 Na, 3 O, 2 Cl on both sides).
**Conclusion:**
By following the stoichiometry and solubility rules, one can determine the products and their states in this precipitation reaction. Use these guidelines to handle similar chemical equations.
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