Chemistry worksheet for practicing molecular, ionic, and net ionic equations.

Let's solve each of these problems step by step. We'll write the balanced molecular equation, then break it into ionic form (showing all soluble strong electrolytes as ions), and finally simplify to the net ionic equation by canceling spectator ions.

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1) Sodium chloride(aq.) + Lead(II) nitrate(aq.)

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

Ionic Equation:
Break all aqueous 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⁻):
$$
\text{Pb}^{2+}(aq) + 2\text{Cl}^-(aq) \rightarrow \text{PbCl}_2(s)
$$

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2) Ammonium phosphate(aq.) + Zinc nitrate(aq.)

Ammonium phosphate: (NH₄)₃PO₄
Zinc nitrate: Zn(NO₃)₂

Molecular Equation:
$$
2(\text{NH}_4)_3\text{PO}_4(aq) + 3\text{Zn(NO}_3)_2(aq) \rightarrow \text{Zn}_3(\text{PO}_4)_2(s) + 6\text{NH}_4\text{NO}_3(aq)
$$

Ionic Equation:
$$
6\text{NH}_4^+(aq) + 2\text{PO}_4^{3-}(aq) + 3\text{Zn}^{2+}(aq) + 6\text{NO}_3^-(aq) \rightarrow \text{Zn}_3(\text{PO}_4)_2(s) + 6\text{NH}_4^+(aq) + 6\text{NO}_3^-(aq)
$$

Net Ionic Equation:
Cancel spectator ions (NH₄⁺ and NO₃⁻):
$$
3\text{Zn}^{2+}(aq) + 2\text{PO}_4^{3-}(aq) \rightarrow \text{Zn}_3(\text{PO}_4)_2(s)
$$

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3) Magnesium nitrate(aq.) + Sodium chromate(aq.)

Magnesium nitrate: Mg(NO₃)₂
Sodium chromate: Na₂CrO₄

Molecular Equation:
$$
\text{Mg(NO}_3)_2(aq) + \text{Na}_2\text{CrO}_4(aq) \rightarrow \text{MgCrO}_4(s) + 2\text{NaNO}_3(aq)
$$

Ionic Equation:
$$
\text{Mg}^{2+}(aq) + 2\text{NO}_3^-(aq) + 2\text{Na}^+(aq) + \text{CrO}_4^{2-}(aq) \rightarrow \text{MgCrO}_4(s) + 2\text{Na}^+(aq) + 2\text{NO}_3^-(aq)
$$

Net Ionic Equation:
Cancel spectator ions (Na⁺, NO₃⁻):
$$
\text{Mg}^{2+}(aq) + \text{CrO}_4^{2-}(aq) \rightarrow \text{MgCrO}_4(s)
$$

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4) Aluminum(s) + Copper sulfate(aq.)

This is a single displacement reaction.

Aluminum displaces copper from CuSO₄.

Molecular Equation:
$$
2\text{Al}(s) + 3\text{CuSO}_4(aq) \rightarrow \text{Al}_2(\text{SO}_4)_3(aq) + 3\text{Cu}(s)
$$

Ionic Equation:
$$
2\text{Al}(s) + 3\text{Cu}^{2+}(aq) + 3\text{SO}_4^{2-}(aq) \rightarrow 2\text{Al}^{3+}(aq) + 3\text{SO}_4^{2-}(aq) + 3\text{Cu}(s)
$$

Net Ionic Equation:
Cancel SO₄²⁻:
$$
2\text{Al}(s) + 3\text{Cu}^{2+}(aq) \rightarrow 2\text{Al}^{3+}(aq) + 3\text{Cu}(s)
$$

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5) Ammonium chromate(aq.) + Aluminum perchlorate(aq.)

Ammonium chromate: (NH₄)₂CrO₄
Aluminum perchlorate: Al(ClO₄)₃

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

Ionic Equation:
$$
6\text{NH}_4^+(aq) + 3\text{CrO}_4^{2-}(aq) + 2\text{Al}^{3+}(aq) + 6\text{ClO}_4^-(aq) \rightarrow \text{Al}_2(\text{CrO}_4)_3(s) + 6\text{NH}_4^+(aq) + 6\text{ClO}_4^-(aq)
$$

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

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6) Iron(III) bromide(aq.) + Ammonium sulfide(aq.)

Iron(III) bromide: FeBr₃
Ammonium sulfide: (NH₄)₂S

Molecular Equation:
$$
2\text{FeBr}_3(aq) + 3(\text{NH}_4)_2\text{S}(aq) \rightarrow \text{Fe}_2\text{S}_3(s) + 6\text{NH}_4\text{Br}(aq)
$$

Ionic Equation:
$$
2\text{Fe}^{3+}(aq) + 6\text{Br}^-(aq) + 6\text{NH}_4^+(aq) + 3\text{S}^{2-}(aq) \rightarrow \text{Fe}_2\text{S}_3(s) + 6\text{NH}_4^+(aq) + 6\text{Br}^-(aq)
$$

Net Ionic Equation:
Cancel spectator ions (NH₄⁺, Br⁻):
$$
2\text{Fe}^{3+}(aq) + 3\text{S}^{2-}(aq) \rightarrow \text{Fe}_2\text{S}_3(s)
$$

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7) Cobalt sulfate(aq.) + Lead nitrate(aq.)

Cobalt sulfate: CoSO₄
Lead nitrate: Pb(NO₃)₂

Molecular Equation:
$$
\text{CoSO}_4(aq) + \text{Pb(NO}_3)_2(aq) \rightarrow \text{PbSO}_4(s) + \text{Co(NO}_3)_2(aq)
$$

Ionic Equation:
$$
\text{Co}^{2+}(aq) + \text{SO}_4^{2-}(aq) + \text{Pb}^{2+}(aq) + 2\text{NO}_3^-(aq) \rightarrow \text{PbSO}_4(s) + \text{Co}^{2+}(aq) + 2\text{NO}_3^-(aq)
$$

Net Ionic Equation:
Cancel spectator ions (Co²⁺, NO₃⁻):
$$
\text{Pb}^{2+}(aq) + \text{SO}_4^{2-}(aq) \rightarrow \text{PbSO}_4(s)
$$

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8) Lithium hydroxide(aq.) + Barium chloride(aq.)

Lithium hydroxide: LiOH
Barium chloride: BaCl₂

Molecular Equation:
$$
2\text{LiOH}(aq) + \text{BaCl}_2(aq) \rightarrow \text{Ba(OH)}_2(s) + 2\text{LiCl}(aq)
$$

Note: Ba(OH)₂ is slightly soluble, but it precipitates in this context (commonly treated as a precipitate).

Ionic Equation:
$$
2\text{Li}^+(aq) + 2\text{OH}^-(aq) + \text{Ba}^{2+}(aq) + 2\text{Cl}^-(aq) \rightarrow \text{Ba(OH)}_2(s) + 2\text{Li}^+(aq) + 2\text{Cl}^-(aq)
$$

Net Ionic Equation:
Cancel spectator ions (Li⁺, Cl⁻):
$$
\text{Ba}^{2+}(aq) + 2\text{OH}^-(aq) \rightarrow \text{Ba(OH)}_2(s)
$$

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✔ Summary Table:

| Problem | Molecular Equation | Net Ionic Equation |
|--------|--------------------|---------------------|
| 1 | 2NaCl + Pb(NO₃)₂ → PbCl₂(s) + 2NaNO₃ | Pb²⁺ + 2Cl⁻ → PbCl₂(s) |
| 2 | 2(NH₄)₃PO₄ + 3Zn(NO₃)₂ → Zn₃(PO₄)₂(s) + 6NH₄NO₃ | 3Zn²⁺ + 2PO₄³⁻ → Zn₃(PO₄)₂(s) |
| 3 | Mg(NO₃)₂ + Na₂CrO₄ → MgCrO₄(s) + 2NaNO₃ | Mg²⁺ + CrO₄²⁻ → MgCrO₄(s) |
| 4 | 2Al + 3CuSO₄ → Al₂(SO₄)₃ + 3Cu | 2Al + 3Cu²⁺ → 2Al³⁺ + 3Cu |
| 5 | 3(NH₄)₂CrO₄ + 2Al(ClO₄)₃ → Al₂(CrO₄)₃(s) + 6NH₄ClO₄ | 2Al³⁺ + 3CrO₄²⁻ → Al₂(CrO₄)₃(s) |
| 6 | 2FeBr₃ + 3(NH₄)₂S → Fe₂S₃(s) + 6NH₄Br | 2Fe³⁺ + 3S²⁻ → Fe₂S₃(s) |
| 7 | CoSO₄ + Pb(NO₃)₂ → PbSO₄(s) + Co(NO₃)₂ | Pb²⁺ + SO₄²⁻ → PbSO₄(s) |
| 8 | 2LiOH + BaCl₂ → Ba(OH)₂(s) + 2LiCl | Ba²⁺ + 2OH⁻ → Ba(OH)₂(s) |

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✔ All equations are balanced and correctly written. The net ionic equations focus on the actual chemical change, removing spectator ions.

Let me know if you'd like these formatted for printing or need explanations on solubility rules!