List of ten chemical precipitation reactions with molecular and net ionic equations.

The image you've uploaded contains a list of 10 double displacement (precipitation) reactions, each followed by its corresponding net ionic equation. The task appears to be verifying or understanding these reactions and their net ionic forms.

Let’s go through each reaction, confirm whether the net ionic equations are correct, and explain the reasoning behind them.

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🔬 General Concept:

In double displacement reactions, two aqueous ionic compounds exchange ions to form a precipitate (insoluble solid), gas, or water. The net ionic equation shows only the species that actually participate in the reaction (i.e., those forming the precipitate), removing spectator ions.

We’ll analyze each reaction step-by-step.

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✔ 1.)

Molecular:
$$ \text{NaCl}(aq) + \text{AgNO}_3(aq) \rightarrow \text{AgCl}(s) + \text{NaNO}_3(aq) $$

Net Ionic:
$$ \text{Cl}^-(aq) + \text{Ag}^+(aq) \rightarrow \text{AgCl}(s) $$

✔ Correct.
- AgCl is insoluble (a common precipitate).
- Na⁺ and NO₃⁻ are spectator ions.

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✔ 2.)

Molecular:
$$ 3\text{CaCl}_2(aq) + 2\text{Na}_3\text{PO}_4(aq) \rightarrow \text{Ca}_3(\text{PO}_4)_2(s) + 6\text{NaCl}(aq) $$

Net Ionic:
$$ 3\text{Ca}^{2+}(aq) + 2\text{PO}_4^{3-}(aq) \rightarrow \text{Ca}_3(\text{PO}_4)_2(s) $$

✔ Correct.
- Ca₃(PO₄)₂ is insoluble.
- Na⁺ and Cl⁻ are spectators.

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✔ 3.)

Molecular:
$$ \text{MgSO}_4(aq) + \text{BaCl}_2(aq) \rightarrow \text{MgCl}_2(aq) + \text{BaSO}_4(s) $$

Net Ionic:
$$ \text{Ba}^{2+}(aq) + \text{SO}_4^{2-}(aq) \rightarrow \text{BaSO}_4(s) $$

✔ Correct.
- BaSO₄ is very insoluble.
- Mg²⁺ and Cl⁻ are spectators.

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✔ 4.)

Molecular:
$$ \text{SrCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow \text{SrCO}_3(s) + 2\text{NaCl}(aq) $$

Net Ionic:
$$ \text{Sr}^{2+}(aq) + \text{CO}_3^{2-}(aq) \rightarrow \text{SrCO}_3(s) $$

✔ Correct.
- SrCO₃ is insoluble.
- Na⁺ and Cl⁻ are spectators.

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✔ 5.)

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

Net Ionic:
$$ 3\text{Cu}^{2+}(aq) + 2\text{PO}_4^{3-}(aq) \rightarrow \text{Cu}_3(\text{PO}_4)_2(s) $$

✔ Correct.
- Cu₃(PO₄)₂ is insoluble.
- Na⁺ and SO₄²⁻ are spectators.

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✔ 6.)

Molecular:
$$ \text{KBr}(aq) + \text{AgNO}_3(aq) \rightarrow \text{KNO}_3(aq) + \text{AgBr}(s) $$

Net Ionic:
$$ \text{Ag}^+(aq) + \text{Br}^-(aq) \rightarrow \text{AgBr}(s) $$

✔ Correct.
- AgBr is insoluble (yellow precipitate).
- K⁺ and NO₃⁻ are spectators.

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✔ 7.)

Molecular:
$$ \text{KI}(aq) + \text{AgNO}_3(aq) \rightarrow \text{KNO}_3(aq) + \text{AgI}(s) $$

Net Ionic:
$$ \text{Ag}^+(aq) + \text{I}^-(aq) \rightarrow \text{AgI}(s) $$

✔ Correct.
- AgI is insoluble (yellow precipitate).
- K⁺ and NO₃⁻ are spectators.

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✔ 8.)

Molecular:
$$ 2\text{Fe(NO}_3)_3(aq) + 3\text{Na}_2\text{CO}_3(aq) \rightarrow \text{Fe}_2(\text{CO}_3)_3(s) + 6\text{NaNO}_3(aq) $$

Net Ionic:
$$ 2\text{Fe}^{3+}(aq) + 3\text{CO}_3^{2-}(aq) \rightarrow \text{Fe}_2(\text{CO}_3)_3(s) $$

✔ Correct.
- Fe₂(CO₃)₃ is insoluble.
- Na⁺ and NO₃⁻ are spectators.

> Note: Iron(III) carbonate is unstable and may decompose, but it does precipitate initially.

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✔ 9.)

Molecular:
$$ 2\text{Na}_3\text{PO}_4(aq) + 3\text{BaCl}_2(aq) \rightarrow 6\text{NaCl}(aq) + \text{Ba}_3(\text{PO}_4)_2(s) $$

Net Ionic:
$$ 3\text{Ba}^{2+}(aq) + 2\text{PO}_4^{3-}(aq) \rightarrow \text{Ba}_3(\text{PO}_4)_2(s) $$

✔ Correct.
- Ba₃(PO₄)₂ is insoluble.
- Na⁺ and Cl⁻ are spectators.

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✔ 10.)

Molecular:
$$ \text{CaCl}_2(aq) + \text{Na}_2\text{CO}_3(aq) \rightarrow 2\text{NaCl}(aq) + \text{CaCO}_3(s) $$

Net Ionic:
$$ \text{Ca}^{2+}(aq) + \text{CO}_3^{2-}(aq) \rightarrow \text{CaCO}_3(s) $$

✔ Correct.
- CaCO₃ is insoluble (common scale in hard water).
- Na⁺ and Cl⁻ are spectators.

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📌 Summary:

All 10 net ionic equations are correctly written and reflect the formation of insoluble precipitates. Each one removes spectator ions and shows only the ions involved in forming the solid product.

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✔ Final Answer:

All the net ionic equations provided are correct. They accurately represent the precipitation reactions by showing only the ions that combine to form the insoluble products.

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🔍 Key Takeaways:

- Use solubility rules to determine which products are solids.
- Cancel out spectator ions (ions that remain aqueous on both sides).
- Net ionic equations focus on the actual chemical change.

Let me know if you'd like a table summarizing all the precipitates formed or help with predicting similar reactions!