Mg(OH)2 (aq) + HC (aq) MgCl, (aq) + H,O() CH,COOH (aq) + KOH (aq)→ CH,COOK (aq) + H,O(1) AgNO, (aq) + NaCI (aq) → AgCl (s). + NaNO, (aq) Pb(NO,), (aq) + KI (aq) Pbl, (s) + KNO, (aq) BaCl, (aq) + Na,SO, (aq) > BaSO, (s), + NaCI (aq) HBr (aq) + NaOH (aq) NaBr (aq) +H,O(1) Neutralization reaction Precipitation reaction

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Classify the following unbalanced chemical reactions as neutralization or precipitation reactions.

 

**Neutralization Reactions and Precipitation Reactions**

**Chemical Reactions:**

1. **Neutralization Reactions:**
   - **\( \text{Mg(OH)}_2 (aq) + \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2\text{O} (l) \)**
   - **\( \text{CH}_3\text{COOH} (aq) + \text{KOH} (aq) \rightarrow \text{CH}_3\text{COOK} (aq) + \text{H}_2\text{O} (l) \)**
   - **\( \text{HBr} (aq) + \text{NaOH} (aq) \rightarrow \text{NaBr} (aq) + \text{H}_2\text{O} (l) \)**

2. **Precipitation Reactions:**
   - **\( \text{AgNO}_3 (aq) + \text{NaCl} (aq) \rightarrow \text{AgCl} (s) + \text{NaNO}_3 (aq) \)**
   - **\( \text{Pb(NO}_3\text{)}_2 (aq) + \text{KI} (aq) \rightarrow \text{PbI}_2 (s) + \text{KNO}_3 (aq) \)**
   - **\( \text{BaCl}_2 (aq) + \text{Na}_2\text{SO}_4 (aq) \rightarrow \text{BaSO}_4 (s) + \text{NaCl} (aq) \)**

**Explanation:**

- **Neutralization Reactions** involve the reaction of an acid and a base to form water and a salt. These reactions are exothermic and usually result in a pH change towards neutrality.

- **Precipitation Reactions** occur when two aqueous solutions are combined and an insoluble solid, called a precipitate, forms. This is due to the solubility rules of the ions in the solution. 

**Diagrams:**

- The image contains boxes labeled "Neutralization reaction" and "Precipitation reaction" to categorize these types of reactions. 
- Each chemical equation represents actual chemical reactions that occur under laboratory
Transcribed Image Text:**Neutralization Reactions and Precipitation Reactions** **Chemical Reactions:** 1. **Neutralization Reactions:** - **\( \text{Mg(OH)}_2 (aq) + \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2\text{O} (l) \)** - **\( \text{CH}_3\text{COOH} (aq) + \text{KOH} (aq) \rightarrow \text{CH}_3\text{COOK} (aq) + \text{H}_2\text{O} (l) \)** - **\( \text{HBr} (aq) + \text{NaOH} (aq) \rightarrow \text{NaBr} (aq) + \text{H}_2\text{O} (l) \)** 2. **Precipitation Reactions:** - **\( \text{AgNO}_3 (aq) + \text{NaCl} (aq) \rightarrow \text{AgCl} (s) + \text{NaNO}_3 (aq) \)** - **\( \text{Pb(NO}_3\text{)}_2 (aq) + \text{KI} (aq) \rightarrow \text{PbI}_2 (s) + \text{KNO}_3 (aq) \)** - **\( \text{BaCl}_2 (aq) + \text{Na}_2\text{SO}_4 (aq) \rightarrow \text{BaSO}_4 (s) + \text{NaCl} (aq) \)** **Explanation:** - **Neutralization Reactions** involve the reaction of an acid and a base to form water and a salt. These reactions are exothermic and usually result in a pH change towards neutrality. - **Precipitation Reactions** occur when two aqueous solutions are combined and an insoluble solid, called a precipitate, forms. This is due to the solubility rules of the ions in the solution. **Diagrams:** - The image contains boxes labeled "Neutralization reaction" and "Precipitation reaction" to categorize these types of reactions. - Each chemical equation represents actual chemical reactions that occur under laboratory
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