Complete and balance the following redox reaction in acidic solution 2+ MnO4 (aq) + S₂O3(aq) → S4062- (aq) + Mn²+ (aq) 3C22 1 + (s) O 2 3 4 D₁ H Reset e (1) LO 5 H₂O OH 6 (g) Mn S 7 8 H₂O+ 9 (aq) xH₂O H* X 0

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### Balancing Redox Reactions in Acidic Solutions

**Objective:**
Complete and balance the following redox reaction in acidic solution:

\[ \text{MnO}_4^- \, (\text{aq}) + \text{S}_2\text{O}_3^{2-} \, (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} \, (\text{aq}) + \text{Mn}^{2+} \, (\text{aq}) \]

**Steps to Balance the Reaction:**

#### Step 1: Write the Unbalanced Reaction
\[ \text{MnO}_4^- + \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} + \text{Mn}^{2+} \]

#### Step 2: Split into Half-Reactions
Identify the oxidation and reduction half-reactions.

Oxidation half-reaction:
\[ \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} \]

Reduction half-reaction:
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]

#### Step 3: Balance Elements in Each Half-Reaction
For the reduction half-reaction:
\[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]

1. Balance the manganese (Mn) atoms.
   \[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \]

2. Balance oxygen atoms by adding H₂O.
   \[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]

3. Balance hydrogen atoms by adding H⁺.
   \[ \text{MnO}_4^- + 8 \text{H}^+ \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \]

4. Balance the charges by adding electrons.
   \[ \text{MnO}_4^- + 8 \text{H}^+ + 5 \text{e}^- \rightarrow \text{Mn
Transcribed Image Text:### Balancing Redox Reactions in Acidic Solutions **Objective:** Complete and balance the following redox reaction in acidic solution: \[ \text{MnO}_4^- \, (\text{aq}) + \text{S}_2\text{O}_3^{2-} \, (\text{aq}) \rightarrow \text{S}_4\text{O}_6^{2-} \, (\text{aq}) + \text{Mn}^{2+} \, (\text{aq}) \] **Steps to Balance the Reaction:** #### Step 1: Write the Unbalanced Reaction \[ \text{MnO}_4^- + \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} + \text{Mn}^{2+} \] #### Step 2: Split into Half-Reactions Identify the oxidation and reduction half-reactions. Oxidation half-reaction: \[ \text{S}_2\text{O}_3^{2-} \rightarrow \text{S}_4\text{O}_6^{2-} \] Reduction half-reaction: \[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \] #### Step 3: Balance Elements in Each Half-Reaction For the reduction half-reaction: \[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \] 1. Balance the manganese (Mn) atoms. \[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} \] 2. Balance oxygen atoms by adding H₂O. \[ \text{MnO}_4^- \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \] 3. Balance hydrogen atoms by adding H⁺. \[ \text{MnO}_4^- + 8 \text{H}^+ \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} \] 4. Balance the charges by adding electrons. \[ \text{MnO}_4^- + 8 \text{H}^+ + 5 \text{e}^- \rightarrow \text{Mn
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