**Balancing Chemical Equations and Writing Ionic Equations**4. (cont.)(e) ___ CO₂ (g) + ___ H₂O (l) → 5. Balance the following equations; write the ionic equations and the corresponding balanced net ionic equation with the proper phase symbols (if different from the ionic equation).(a) ___ H₂SO₄ (aq) + ___ NaOH (aq) → ___ Na₂SO₄ (aq) + ___ H₂O (l)(b) ___ Al₂O₃ (s) + ___ HCl (aq) → ___ AlCl₃ (aq) + ___ H₂O (l)(c) ___ H₂SO₃ (aq) + ___ KOH (aq) → ___ K₂SO₃ (aq) + ___ H₂O (l)(d) ___ HC₂H₃O₂ (aq) + ___ Ca(OH)₂ (aq) → ___ Ca(C₂H₃O₂)₂ (aq) + ___ H₂O (l)Page 55---**Explanations of Tasks:**- *Balancing Equations*: Ensure the same number of each type of atom appears on both the reactant and the product sides.- *Ionic Equations*: Display all strong electrolytes as ions.- *Net Ionic Equations*: Eliminate ions not directly involved in the reaction (spectator ions) from the ionic equations, providing a simplified version highlighting the actual chemical change. This exercise is an essential practice in understanding stoichiometry and the conservation of mass in chemical reactions. **Problems***You must show your method of solution!*1. Calculate the molarity of a solution prepared by dissolving 0.600 g of KHC₈H₄O₄ in enough water to make 50.0 mL of solution. ______ M2. Calculate the molarity of a solution prepared by dissolving 0.600 g of H₂C₂O₄・2H₂O in enough water to make 50.0 mL of solution. ______ M**[No graphs or diagrams present on this page.]**

Since you have asked multiple questions, we will solve first question for you. If you want any…

Answered: You must show your method of solution!…

You must show your method of solution! 1. Calculate the molarity of a solution prepared by dissolving 0.600 g of KHC,H O4 in enough water to make 50.0 mL of solution.

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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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

**Balancing Chemical Equations and Writing Ionic Equations**

4. (cont.)
(e) ___ CO₂ (g) + ___ H₂O (l) →

5. Balance the following equations; write the ionic equations and the corresponding balanced net ionic equation with the proper phase symbols (if different from the ionic equation).

(a) ___ H₂SO₄ (aq) + ___ NaOH (aq) → ___ Na₂SO₄ (aq) + ___ H₂O (l)

(b) ___ Al₂O₃ (s) + ___ HCl (aq) → ___ AlCl₃ (aq) + ___ H₂O (l)

(c) ___ H₂SO₃ (aq) + ___ KOH (aq) → ___ K₂SO₃ (aq) + ___ H₂O (l)

(d) ___ HC₂H₃O₂ (aq) + ___ Ca(OH)₂ (aq) → ___ Ca(C₂H₃O₂)₂ (aq) + ___ H₂O (l)

Page 55

---

**Explanations of Tasks:**

- *Balancing Equations*: Ensure the same number of each type of atom appears on both the reactant and the product sides.
- *Ionic Equations*: Display all strong electrolytes as ions.
- *Net Ionic Equations*: Eliminate ions not directly involved in the reaction (spectator ions) from the ionic equations, providing a simplified version highlighting the actual chemical change.

This exercise is an essential practice in understanding stoichiometry and the conservation of mass in chemical reactions.

**Problems**

*You must show your method of solution!*

1. Calculate the molarity of a solution prepared by dissolving 0.600 g of KHC₈H₄O₄ in enough water to make 50.0 mL of solution.

______ M

2. Calculate the molarity of a solution prepared by dissolving 0.600 g of H₂C₂O₄・2H₂O in enough water to make 50.0 mL of solution.

______ M

**[No graphs or diagrams present on this page.]**

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