4 and 5 **Balancing Chemical Equations and Writing Ionic Equations**Below are several reactions for which you need to write complete balanced equations. For reactions occurring in solution, it's important to write the ionic and net ionic equations when appropriate.1. **Reaction:** Mixing solutions of sodium sulfate and barium nitrate to form a precipitate. 2. **Reaction:** Mixing solutions of nitric acid and calcium acetate.3. **Reaction:** Pouring a diluted hydrochloric acid solution on a piece of zinc metal.4. **Reaction:** Adding a manganese(II) nitrate solution to a lithium hydroxide solution, resulting in a precipitate.5. **Reaction:** Adding aluminum metal to a solution of copper(I) chloride.6. **Reaction:** Dropping sodium metal in water.7. **Reaction:** Heating solid iron(III) chlorate.**Guideline for Writing Equations:**- **Complete Balanced Equation:** Shows all reactants and products in their undissociated form.- **Ionic Equation:** Breaks down all soluble ionic compounds into ions.- **Net Ionic Equation:** Shows only the species that actually participate in the reaction, omitting spectator ions.To practice these, remember to check solubility rules, activity series, and the states of matter for each compound involved.

Answered: Image /qna-images/answer/04e8dae9-1bbf-4446-b8d6-54eea4c1e5ff.jpg

Answered: 4. a manganese(II) nitrate solution is…

4. a manganese(II) nitrate solution is added to a lithium hydroxide solution and forms a precipitate 5. aluminum metal is added to a solution of copper(I) chloride

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

4 and 5

**Balancing Chemical Equations and Writing Ionic Equations**

Below are several reactions for which you need to write complete balanced equations. For reactions occurring in solution, it's important to write the ionic and net ionic equations when appropriate.

1. **Reaction:** Mixing solutions of sodium sulfate and barium nitrate to form a precipitate.

2. **Reaction:** Mixing solutions of nitric acid and calcium acetate.

3. **Reaction:** Pouring a diluted hydrochloric acid solution on a piece of zinc metal.

4. **Reaction:** Adding a manganese(II) nitrate solution to a lithium hydroxide solution, resulting in a precipitate.

5. **Reaction:** Adding aluminum metal to a solution of copper(I) chloride.

6. **Reaction:** Dropping sodium metal in water.

7. **Reaction:** Heating solid iron(III) chlorate.

**Guideline for Writing Equations:**
- **Complete Balanced Equation:** Shows all reactants and products in their undissociated form.
- **Ionic Equation:** Breaks down all soluble ionic compounds into ions.
- **Net Ionic Equation:** Shows only the species that actually participate in the reaction, omitting spectator ions.

To practice these, remember to check solubility rules, activity series, and the states of matter for each compound involved.

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