Chemistry lab worksheet focusing on writing balanced molecular, ionic, and net ionic equations for aqueous reactions.

Let's go through each of the five reactions step by step, writing the balanced molecular, ionic, and net ionic equations. We'll determine if a reaction occurs (and if not, write "NR"). For aqueous solutions, we assume all soluble compounds dissociate into ions unless they are precipitates, gases, or weak electrolytes.

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1.

Molecular Equation:
$$
2\text{NaCl}(aq) + \text{Pb(NO}_3)_2(aq) \rightarrow \text{PbCl}_2(s) + 2\text{NaNO}_3(aq)
$$

- PbCl₂ is insoluble (precipitate), so reaction occurs.

Ionic Equation:
Break all soluble strong electrolytes into ions:
$$
2\text{Na}^+(aq) + 2\text{Cl}^-(aq) + \text{Pb}^{2+}(aq) + 2\text{NO}_3^-(aq) \rightarrow \text{PbCl}_2(s) + 2\text{Na}^+(aq) + 2\text{NO}_3^-(aq)
$$

Net Ionic Equation:
Cancel spectator ions (Na⁺ and NO₃⁻):
$$
\text{Pb}^{2+}(aq) + 2\text{Cl}^-(aq) \rightarrow \text{PbCl}_2(s)
$$

✔ Reaction occurs.

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2.

Molecular Equation:
$$
\text{Mg(OH)}_2(s) + 2\text{HCl}(aq) \rightarrow \text{MgCl}_2(aq) + 2\text{H}_2\text{O}(l)
$$

- Mg(OH)₂ is insoluble (a base), but it reacts with acid (HCl) in a neutralization.
- H₂O is a liquid (not ionized).

Ionic Equation:
Mg(OH)₂ is solid → remains as is; HCl and MgCl₂ are aqueous and dissociated:
$$
\text{Mg(OH)}_2(s) + 2\text{H}^+(aq) + 2\text{Cl}^-(aq) \rightarrow \text{Mg}^{2+}(aq) + 2\text{Cl}^-(aq) + 2\text{H}_2\text{O}(l)
$$

Net Ionic Equation:
Cancel Cl⁻:
$$
\text{Mg(OH)}_2(s) + 2\text{H}^+(aq) \rightarrow \text{Mg}^{2+}(aq) + 2\text{H}_2\text{O}(l)
$$

✔ Reaction occurs.

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3.

Molecular Equation:
$$
\text{Na}_2\text{CO}_3(aq) + 2\text{HCl}(aq) \rightarrow 2\text{NaCl}(aq) + \text{CO}_2(g) + \text{H}_2\text{O}(l)
$$

- Carbonate reacts with acid to produce CO₂ gas and water.

Ionic Equation:
All soluble compounds dissociate:
$$
2\text{Na}^+(aq) + \text{CO}_3^{2-}(aq) + 2\text{H}^+(aq) + 2\text{Cl}^-(aq) \rightarrow 2\text{Na}^+(aq) + 2\text{Cl}^-(aq) + \text{CO}_2(g) + \text{H}_2\text{O}(l)
$$

Net Ionic Equation:
Cancel spectator ions (Na⁺, Cl⁻):
$$
\text{CO}_3^{2-}(aq) + 2\text{H}^+(aq) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(l)
$$

✔ Reaction occurs.

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4.

Molecular Equation:
$$
2\text{FeCl}_3(aq) + 3\text{Mg}(s) \rightarrow 3\text{MgCl}_2(aq) + 2\text{Fe}(s)
$$

- This is a single displacement reaction.
- Mg is more reactive than Fe (Mg above Fe in activity series), so Mg displaces Fe.

Ionic Equation:
FeCl₃ and MgCl₂ are aqueous and dissociate; Mg(s) and Fe(s) are solids:
$$
2\text{Fe}^{3+}(aq) + 6\text{Cl}^-(aq) + 3\text{Mg}(s) \rightarrow 3\text{Mg}^{2+}(aq) + 6\text{Cl}^-(aq) + 2\text{Fe}(s)
$$

Net Ionic Equation:
Cancel Cl⁻:
$$
2\text{Fe}^{3+}(aq) + 3\text{Mg}(s) \rightarrow 3\text{Mg}^{2+}(aq) + 2\text{Fe}(s)
$$

✔ Reaction occurs.

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5.

Molecular Equation:
$$
3(\text{NH}_4)_2\text{C}_2\text{O}_4(aq) + 2\text{Al(ClO}_4)_3(aq) \rightarrow 6\text{NH}_4\text{ClO}_4(aq) + \text{Al}_2(\text{C}_2\text{O}_4)_3(s)
$$

- Check solubility:
- All ammonium salts are soluble.
- Most perchlorates are soluble.
- Aluminum oxalate (Al₂(C₂O₄)₃) is insoluble → precipitate forms.

So, reaction occurs.

Ionic Equation:
Break all soluble compounds into ions:
$$
6\text{NH}_4^+(aq) + 3\text{C}_2\text{O}_4^{2-}(aq) + 2\text{Al}^{3+}(aq) + 6\text{ClO}_4^-(aq) \rightarrow 6\text{NH}_4^+(aq) + 6\text{ClO}_4^-(aq) + \text{Al}_2(\text{C}_2\text{O}_4)_3(s)
$$

Net Ionic Equation:
Cancel spectator ions (NH₄⁺, ClO₄⁻):
$$
2\text{Al}^{3+}(aq) + 3\text{C}_2\text{O}_4^{2-}(aq) \rightarrow \text{Al}_2(\text{C}_2\text{O}_4)_3(s)
$$

✔ Reaction occurs.

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✔ Final Answers:

#### 1.
- Molecular: $2\text{NaCl}(aq) + \text{Pb(NO}_3)_2(aq) \rightarrow \text{PbCl}_2(s) + 2\text{NaNO}_3(aq)$
- Ionic: $2\text{Na}^+(aq) + 2\text{Cl}^-(aq) + \text{Pb}^{2+}(aq) + 2\text{NO}_3^-(aq) \rightarrow \text{PbCl}_2(s) + 2\text{Na}^+(aq) + 2\text{NO}_3^-(aq)$
- Net Ionic: $\text{Pb}^{2+}(aq) + 2\text{Cl}^-(aq) \rightarrow \text{PbCl}_2(s)$

#### 2.
- Molecular: $\text{Mg(OH)}_2(s) + 2\text{HCl}(aq) \rightarrow \text{MgCl}_2(aq) + 2\text{H}_2\text{O}(l)$
- Ionic: $\text{Mg(OH)}_2(s) + 2\text{H}^+(aq) + 2\text{Cl}^-(aq) \rightarrow \text{Mg}^{2+}(aq) + 2\text{Cl}^-(aq) + 2\text{H}_2\text{O}(l)$
- Net Ionic: $\text{Mg(OH)}_2(s) + 2\text{H}^+(aq) \rightarrow \text{Mg}^{2+}(aq) + 2\text{H}_2\text{O}(l)$

#### 3.
- Molecular: $\text{Na}_2\text{CO}_3(aq) + 2\text{HCl}(aq) \rightarrow 2\text{NaCl}(aq) + \text{CO}_2(g) + \text{H}_2\text{O}(l)$
- Ionic: $2\text{Na}^+(aq) + \text{CO}_3^{2-}(aq) + 2\text{H}^+(aq) + 2\text{Cl}^-(aq) \rightarrow 2\text{Na}^+(aq) + 2\text{Cl}^-(aq) + \text{CO}_2(g) + \text{H}_2\text{O}(l)$
- Net Ionic: $\text{CO}_3^{2-}(aq) + 2\text{H}^+(aq) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(l)$

#### 4.
- Molecular: $2\text{FeCl}_3(aq) + 3\text{Mg}(s) \rightarrow 3\text{MgCl}_2(aq) + 2\text{Fe}(s)$
- Ionic: $2\text{Fe}^{3+}(aq) + 6\text{Cl}^-(aq) + 3\text{Mg}(s) \rightarrow 3\text{Mg}^{2+}(aq) + 6\text{Cl}^-(aq) + 2\text{Fe}(s)$
- Net Ionic: $2\text{Fe}^{3+}(aq) + 3\text{Mg}(s) \rightarrow 3\text{Mg}^{2+}(aq) + 2\text{Fe}(s)$

#### 5.
- Molecular: $3(\text{NH}_4)_2\text{C}_2\text{O}_4(aq) + 2\text{Al(ClO}_4)_3(aq) \rightarrow 6\text{NH}_4\text{ClO}_4(aq) + \text{Al}_2(\text{C}_2\text{O}_4)_3(s)$
- Ionic: $6\text{NH}_4^+(aq) + 3\text{C}_2\text{O}_4^{2-}(aq) + 2\text{Al}^{3+}(aq) + 6\text{ClO}_4^-(aq) \rightarrow 6\text{NH}_4^+(aq) + 6\text{ClO}_4^-(aq) + \text{Al}_2(\text{C}_2\text{O}_4)_3(s)$
- Net Ionic: $2\text{Al}^{3+}(aq) + 3\text{C}_2\text{O}_4^{2-}(aq) \rightarrow \text{Al}_2(\text{C}_2\text{O}_4)_3(s)$

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✔ All reactions occur — no "NR" cases.

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