Please explain in detail the steps to solve this **Title: Balancing Redox Reactions in Basic Solutions****Objective:**Learn how to complete and balance redox reactions in basic solutions.**Example Problem:****Given Reaction:**\[ \text{Zn(OH)}_4^{2-} (aq) + \text{As} (s) \rightarrow \text{Zn} (s) + \text{H}_2\text{AsO}_4^- (aq) \]**Steps to Balance:**1. **Identify Oxidation and Reduction Half-Reactions:** - **Oxidation:** As(s) is oxidized to $\text{H}_2\text{AsO}_4^-$. - **Reduction:** $\text{Zn(OH)}_4^{2-}$ is reduced to Zn(s).2. **Balance Atoms Other Than O and H:** - Ensure all atoms except oxygen and hydrogen are balanced in each half-reaction.3. **Balance Oxygen Atoms:** - Add water molecules ($\text{H}_2\text{O}$) to balance oxygen atoms.4. **Balance Hydrogen Atoms:** - Add hydrogen ions ($\text{H}^+$) to balance hydrogen atoms.5. **Balance Charge:** - Add electrons ($e^-$) to one side of each half-reaction to balance the charge.6. **Combine Half-Reactions:** - Multiply the half-reactions by appropriate factors so the electrons cancel out when added together.7. **Ensure the Reaction Occurs in Basic Solution:** - Add $\text{OH}^-$ ions to each side of the reaction to neutralize $\text{H}^+$ and form water, reflecting that the reaction occurs in a basic solution. Simplify water and hydroxide ions if necessary.**Final Reaction:**\[ \text{Balanced form of the initial equation.} \]In this tutorial, you will practice these steps to successfully balance any redox reaction in a basic solution.

Answered: Complete and balance the fallauing…

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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Please explain in detail the steps to solve this

**Title: Balancing Redox Reactions in Basic Solutions**

**Objective:**
Learn how to complete and balance redox reactions in basic solutions.

**Example Problem:**

**Given Reaction:**
\[ \text{Zn(OH)}_4^{2-} (aq) + \text{As} (s) \rightarrow \text{Zn} (s) + \text{H}_2\text{AsO}_4^- (aq) \]

**Steps to Balance:**

1. **Identify Oxidation and Reduction Half-Reactions:**
- **Oxidation:** As(s) is oxidized to $\text{H}_2\text{AsO}_4^-$.
- **Reduction:** $\text{Zn(OH)}_4^{2-}$ is reduced to Zn(s).

2. **Balance Atoms Other Than O and H:**
- Ensure all atoms except oxygen and hydrogen are balanced in each half-reaction.

3. **Balance Oxygen Atoms:**
- Add water molecules ($\text{H}_2\text{O}$) to balance oxygen atoms.

4. **Balance Hydrogen Atoms:**
- Add hydrogen ions ($\text{H}^+$) to balance hydrogen atoms.

5. **Balance Charge:**
- Add electrons ($e^-$) to one side of each half-reaction to balance the charge.

6. **Combine Half-Reactions:**
- Multiply the half-reactions by appropriate factors so the electrons cancel out when added together.

7. **Ensure the Reaction Occurs in Basic Solution:**
- Add $\text{OH}^-$ ions to each side of the reaction to neutralize $\text{H}^+$ and form water, reflecting that the reaction occurs in a basic solution. Simplify water and hydroxide ions if necessary.

**Final Reaction:**
\[ \text{Balanced form of the initial equation.} \]

In this tutorial, you will practice these steps to successfully balance any redox reaction in a basic solution.

Expert Solution

Step 1

The redox reactions are the oxidation-reduction reactions, which involves simultaneous oxidation and reduction takes place. In the redox reactions, the transfer of electrons between two reactants produce two different products. The oxidation state of species changes due to electron transfer.

Step 2

The given reaction is as follows,

$Zn {(OH)}_{4}^{2 -} (aq) + As (s) \overset{}{\to} Zn (s) + H_{2} {AsO}_{4}^{-} (aq)$

The oxidation half-reaction is as follows,

$As (s) \overset{}{\to} H_{2} {AsO}_{4}^{-} (aq)$

The reduction half-reaction is as follows,

$Zn {(OH)}_{4}^{2 -} (aq) \overset{}{\to} Zn (s)$

Step 3

Balancing hydrogen atoms by adding H₂O molecules on deficient side in both the half reactions,

$As (s) + H_{2} O (l) \overset{}{\to} H_{2} {AsO}_{4}^{-} (aq)$

$Zn {(OH)}_{4}^{2 -} (aq) \overset{}{\to} Zn (s) + 2 H_{2} O (l)$

Balancing oxygen atoms by adding same number of H₂O molecules on the excess side and double the number of OH^- ions (since the medium is basic) on deficient side,

$As (s) + H_{2} O (l) + 6 {OH}^{-} (aq) \overset{}{\to} H_{2} {AsO}_{4}^{-} (aq) + 3 H_{2} O (l)$

$Zn {(OH)}_{4}^{2 -} (aq) + 2 H_{2} O (l) \overset{}{\to} Zn (s) + 2 H_{2} O (l) + 4 {OH}^{-} (aq)$

Step 4

After cancelling the water molecules,

$As (s) + 6 {OH}^{-} (aq) \overset{}{\to} H_{2} {AsO}_{4}^{-} (aq) + 2 H_{2} O (l)$

$Zn {(OH)}_{4}^{2 -} (aq) \overset{}{\to} Zn (s) + 4 {OH}^{-} (aq)$

Balancing the electrons on both sides,

$As (s) + 6 {OH}^{-} (aq) \overset{}{\to} H_{2} {AsO}_{4}^{-} (aq) + 2 H_{2} O (l) + 5 e^{-}$

$Zn {(OH)}_{4}^{2 -} (aq) + 2 e^{-} \overset{}{\to} Zn (s) + 4 {OH}^{-} (aq)$

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