Let's go **step by step** through each reaction based on what’s shown in your image. I’ll walk you through the **balanced equation (ME: Molecular Equation)** and the **CIE: Complete Ionic Equation**, explaining the reasoning for each. --- ## **Reaction 5: Hydrochloric Acid and Sodium Carbonate** **Formula:** HCl + Na₂CO₃ **Observations:** Some bubbles/fizzing, clear → **gas production** ### **Step-by-step Solution** 1. **Write the Molecular Equation (ME):** \[ 2\text{HCl (aq)} + \text{Na}_2\text{CO}_3\text{ (aq)} \rightarrow 2\text{NaCl (aq)} + \text{H}_2\text{O (l)} + \text{CO}_2\text{ (g)} \] - HCl reacts with sodium carbonate to form sodium chloride, water, and carbon dioxide gas (the fizzing observed). 2. **Write the Complete Ionic Equation (CIE):** \[ 2\text{H}^+ (aq) + 2\text{Cl}^- (aq) + 2\text{Na}^+ (aq) + \text{CO}_3^{2-} (aq) \rightarrow 2\text{Na}^+ (aq) + 2\text{Cl}^- (aq) + \text{H}_2\text{O} (l) + \text{CO}_2 (g) \] - Spectator ions: \( \text{Na}^+ \) and \( \text{Cl}^- \) - Net ionic equation: \[ 2\text{H}^+ (aq) + \text{CO}_3^{2-} (aq) \rightarrow \text{H}_2\text{O} (l) + \text{CO}_2 (g) \] --- ## **Reaction 6: Sodium Carbonate and Magnesium Nitrate** **Formula:** Na₂CO₃ + Mg(NO₃)₂ **Observations:** Cloudy, clear at the bottom of the tube → **precipitation** ### **Step-by-step Solution** 1. **Write the Molecular Equation (ME):** \[ \text{Na}_2\text{CO}_3 (aq) + \text{Mg(NO}_3)_2 (aq) \rightarrow 2\text{NaNO}_3 (aq) + \text{MgCO}_3 (s) \] - Magnesium carbonate (\( \text{MgCO}_3 \)) is insoluble and precipitates. 2. **Write the Complete Ionic Equation (CIE):** \[ 2\text{Na}^+ (aq) + \text{CO}_3^{2-} (aq) + \text{Mg}^{2+} (aq) + 2\text{NO}_3^- (aq) \rightarrow 2\text{Na}^+ (aq) + 2\text{NO}_3^- (aq) + \text{MgCO}_3 (s) \] - Spectator ions: \( \text{Na}^+ \), \( \text{NO}_3^- \) - Net ionic equation: \[ \text{Mg}^{2+} (aq) + \text{CO}_3^{2-} (aq) \rightarrow \text{MgCO}_3 (s) \] --- ## **Reaction 7: Sodium Phosphate and Magnesium Nitrate** **Formula:** Na₃PO₄ + Mg(NO₃)₂ **Observations:** Cloudy, solid/liquid, clear at bottom → **precipitation** ### **Step-by-step Solution** 1. **Write the Molecular Equation (ME):** \[ 2\text{Na}_3\text{PO}_4 (aq) + 3\text{Mg(NO}_3)_2 (aq) \rightarrow 6\text{NaNO}_3 (aq) + \text{Mg}_3(\text{PO}_4)_2 (s) \] - Magnesium phosphate (\( \text{Mg}_3(\text{PO}_4)_2 \)) is insoluble and precipitates. 2. **Write the Complete Ionic Equation (CIE):** \[ 6\text{Na}^+ (aq) + 2\text{PO}_4^{3-} (aq) + 3\text{Mg}^{2+} (aq) + 6\text{NO}_3^- (aq) \rightarrow 6\text{Na}^+ (aq) + 6\text{NO}_3^- (aq) + \text{Mg}_3(\text{PO}_4)_2 (s) \] - Spectator ions: \( \text{Na}^+ \), \( \text{NO}_3^- \) - Net ionic equation: \[ 3\text{Mg}^{2+} (aq) + 2\text{PO}_4^{3-} (aq) \rightarrow \text{Mg}_3(\text{PO}_4)_2 (s) \] --- ## **Reaction 8: Sulfuric Acid and Sodium Hydroxide** **Formula:** H₂SO₄ + NaOH **Observations:** Hot tube, clear → **no precipitation** ### **Step-by-step Solution** 1. **Write the Molecular Equation (ME):** \[ \text{H}_2\text{SO}_4 (aq) + 2\text{NaOH} (aq) \rightarrow 2\text{H}_2\text{O} (l) + \text{Na}_2\text{SO}_4 (aq) \] - This is a neutralization; all products are soluble (no precipitate). 2. **Write the Complete Ionic Equation (CIE):** \[ 2\text{H}^+ (aq) + \text{SO}_4^{2-} (aq) + 2\text{Na}^+ (aq) + 2\text{OH}^- (aq) \rightarrow 2\text{Na}^+ (aq) + \text{SO}_4^{2-} (aq) + 2\text{H}_2\text{O} (l) \] - Spectator ions: \( \text{Na}^+ \), \( \text{SO}_4^{2-} \) - Net ionic equation: \[ 2\text{H}^+ (aq) + 2\text{OH}^- (aq) \rightarrow 2\text{H}_2\text{O} (l) \] or simplified: \[ \text{H}^+ (aq) + \text{OH}^- (aq) \rightarrow \text{H}_2\text{O} (l) \] --- ## **Summary Table** | Reaction | Formula | Main Observation | ME | CIE | |----------|---------|------------------|----|-----| | 5 | HCl + Na₂CO₃ | Bubbles/gas | \(2\text{HCl} + \text{Na}_2\text{CO}_3 \rightarrow 2\text{NaCl} + \text{H}_2\text{O} + \text{CO}_2\) | \(2\text{H}^+ + \text{CO}_3^{2-} \rightarrow \text{H}_2\text{O} + \text{CO}_2\) | | 6 | Na₂CO₃ + Mg(NO₃)₂ | Precipitate | \(\text{Na}_2\text{CO}_3 + \text{Mg(NO}_3)_2 \rightarrow 2\text{NaNO}_3 + \text{MgCO}_3\) | \(\text{Mg}^{2+} + \text{CO}_3^{2-} \rightarrow \text{MgCO}_3\) | | 7 | Na₃PO₄ + Mg(NO₃)₂ | Precipitate | \(2\text{Na}_3\text{PO}_4 + 3\text{Mg(NO}_3)_2 \rightarrow 6\text{NaNO}_3 + \text{Mg}_3(\text{PO}_4)_2\) | \(3\text{Mg}^{2+} + 2\text{PO}_4^{3-} \rightarrow \text{Mg}_3(\text{PO}_4)_2\) | | 8 | H₂SO₄ + NaOH | No precipitate | \(\text{H}_2\text{SO}_4 + 2\text{NaOH} \rightarrow 2\text{H}_2\text{O} + \text{Na}_2\text{SO}_4\) | \(2\text{H}^+ + 2\text{OH}^- \rightarrow 2\text{H}_2\text{O}\) | --- **If you have any specific questions or need help with a particular reaction, let me know!**