DO 10 W 310Huops 3140/ HNO3(aq) +_ Naz (O3(aq) →

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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**Lab Assignment**

**Goals:**
1. Identify which unknown is which.
2. Write balanced chemical equations and net ionic equations.

**Notes:**
- If you see bubbles, that is due to the decomposition of \( \text{H}_2\text{CO}_3 \).
- In other words, \( \text{H}_2\text{CO}_3 \) is a product, but it doesn't exist for long. It breaks down into \( \text{CO}_2(g) \) and \( \text{H}_2\text{O}(l) \).
- For these reactions, you will have a solid, liquid, or gas (not an ionic compound) and an ionic compound as products: \( \text{CO}_2(g) \) and \( \text{H}_2\text{O}(l) \).
- Solids, liquids, and gases do not break apart in solution, so they do not get broken apart in the complete ionic equation or the net ionic equation.
Transcribed Image Text:**Lab Assignment** **Goals:** 1. Identify which unknown is which. 2. Write balanced chemical equations and net ionic equations. **Notes:** - If you see bubbles, that is due to the decomposition of \( \text{H}_2\text{CO}_3 \). - In other words, \( \text{H}_2\text{CO}_3 \) is a product, but it doesn't exist for long. It breaks down into \( \text{CO}_2(g) \) and \( \text{H}_2\text{O}(l) \). - For these reactions, you will have a solid, liquid, or gas (not an ionic compound) and an ionic compound as products: \( \text{CO}_2(g) \) and \( \text{H}_2\text{O}(l) \). - Solids, liquids, and gases do not break apart in solution, so they do not get broken apart in the complete ionic equation or the net ionic equation.
Certainly! The image contains a chemical equation that can be used to illustrate a reaction between two aqueous solutions. Here’s the transcription and explanation:

---

**Chemical Reaction:**

\[\_\_ \, \text{HNO}_3(\text{aq}) + \_\_ \, \text{Na}_2\text{CO}_3(\text{aq}) \rightarrow\]

**Explanation:**

This represents an unbalanced chemical equation involving nitric acid (HNO₃) and sodium carbonate (Na₂CO₃), both in aqueous form. The reaction typically results in the formation of products such as sodium nitrate (NaNO₃), water (H₂O), and carbon dioxide (CO₂). The underscores indicate that stoichiometric coefficients are needed to balance the equation.

**Balancing Tip:**

1. **Identify Products:** When HNO₃ reacts with Na₂CO₃, the products are typically NaNO₃, H₂O, and CO₂.
2. **Balance Elements:** Ensure the number of atoms for each element is equal on both sides of the equation.
3. **Adjust Coefficients:** Use coefficients to balance oxygen and hydrogen atoms last.

Example balanced equation:
\[ 2 \, \text{HNO}_3(\text{aq}) + \text{Na}_2\text{CO}_3(\text{aq}) \rightarrow 2 \, \text{NaNO}_3(\text{aq}) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \]

This equation demonstrates a typical acid-carbonate reaction, resulting in the formation of a salt, water, and carbon dioxide gas. Understanding how to balance such equations is fundamental in chemistry education.

---
Transcribed Image Text:Certainly! The image contains a chemical equation that can be used to illustrate a reaction between two aqueous solutions. Here’s the transcription and explanation: --- **Chemical Reaction:** \[\_\_ \, \text{HNO}_3(\text{aq}) + \_\_ \, \text{Na}_2\text{CO}_3(\text{aq}) \rightarrow\] **Explanation:** This represents an unbalanced chemical equation involving nitric acid (HNO₃) and sodium carbonate (Na₂CO₃), both in aqueous form. The reaction typically results in the formation of products such as sodium nitrate (NaNO₃), water (H₂O), and carbon dioxide (CO₂). The underscores indicate that stoichiometric coefficients are needed to balance the equation. **Balancing Tip:** 1. **Identify Products:** When HNO₃ reacts with Na₂CO₃, the products are typically NaNO₃, H₂O, and CO₂. 2. **Balance Elements:** Ensure the number of atoms for each element is equal on both sides of the equation. 3. **Adjust Coefficients:** Use coefficients to balance oxygen and hydrogen atoms last. Example balanced equation: \[ 2 \, \text{HNO}_3(\text{aq}) + \text{Na}_2\text{CO}_3(\text{aq}) \rightarrow 2 \, \text{NaNO}_3(\text{aq}) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \] This equation demonstrates a typical acid-carbonate reaction, resulting in the formation of a salt, water, and carbon dioxide gas. Understanding how to balance such equations is fundamental in chemistry education. ---
Expert Solution
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Answer:

Complete ionic equation is the representation of chemical reaction in which all the ions and species present in the reaction are shown while in net ionic equation spectator ions and species are not mentioned.

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