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1 Name: Chem 9, Section: Lab Partner: Experiment Date: Double Replacement Reactions For each of the reactions performed: -- predict the reaction type (precipitation, neutralization or gaseous) -- record your observations -- predict the names and states of the products formed -- write the balanced equation, including all physical states. 1. Aqueous sodium chloride + aqueous silver nitrate Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 2. Hydrochloric acid + aqueous sodium hydroxide Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 3. Hydrochloric acid + solid sodium bicarbonate Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 4.

Aqueous iron (III) chloride + aqueous ammonium hydroxide Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: . Aqueous barium chloride + sulfuric acid Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 6. Aqueous sodium phosphate + aqueous copper(II) sulfate Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 7. Aqueous sodium carbonate + cobalt(II) nitrate Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 8. Aqueous sodium chloride + aqueous potassium nitrate Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 9.

Aqueous nickel(II) nitrate + aqueous sodium hydroxide Reaction Type: Observations: Product Names & States (if none, why not?): Balanced Equation: 3 Describe each of the following compounds as ionic, covalent, or acid. Use IUPAC nomenclature rules to write the chemical formula or the chemical name. Name Formula Description 1. Aluminum oxide 2. Calcium carbonate 3.

Tin(IV) sulfate 4. Silver sulfite 5. Nitric acid 6. Carbon tetrachloride 7. Hydrosulfuric acid 8.

P2O. NO. CaO. PbCl. AlPO.

H2SO. NBr3

Paper for above instructions

Introduction

Double replacement reactions, a category of chemical reactions in which the ions of two compounds exchange places in an aqueous solution, are pivotal in understanding various chemical principles. They can result in precipitation, gas evolution, or neutralization reactions. This report outlines the expected types of reactions for given combinations, provides observations, predicts product names and states, and presents balanced equations for reactions involving several ionic and covalent compounds.

Experimental Reactions

Reaction 1: Aqueous Sodium Chloride + Aqueous Silver Nitrate

- Reaction Type: Precipitation Reaction
- Observations: Formation of a white precipitate.
- Product Names & States: Silver chloride (AgCl, s) and Sodium Nitrate (NaNO₃, aq).
- Balanced Equation:
\[
\text{NaCl (aq) + AgNO}_3\text{ (aq) } \rightarrow \text{ AgCl (s) + NaNO}_3\text{ (aq)}
\]

Reaction 2: Hydrochloric Acid + Aqueous Sodium Hydroxide

- Reaction Type: Neutralization Reaction
- Observations: No visible change; the solution may become warmer.
- Product Names & States: Sodium chloride (NaCl, aq) and water (H₂O, l).
- Balanced Equation:
\[
\text{HCl (aq) + NaOH (aq) } \rightarrow \text{ NaCl (aq) + H}_2\text{O (l)}
\]

Reaction 3: Hydrochloric Acid + Solid Sodium Bicarbonate

- Reaction Type: Gas Evolution (Neutralization Reaction)
- Observations: Formation of bubbles (carbon dioxide gas).
- Product Names & States: Sodium chloride (NaCl, aq), water (H₂O, l), and carbon dioxide (CO₂, g).
- Balanced Equation:
\[
\text{HCl (aq) + NaHCO}_3\text{ (s) } \rightarrow \text{ NaCl (aq) + H}_2\text{O (l) + CO}_2\text{ (g)}
\]

Reaction 4: Aqueous Iron (III) Chloride + Aqueous Ammonium Hydroxide

- Reaction Type: Precipitation Reaction
- Observations: Formation of a reddish-brown precipitate.
- Product Names & States: Iron(III) hydroxide (Fe(OH)₃, s) and Ammonium chloride (NH₄Cl, aq).
- Balanced Equation:
\[
\text{FeCl}_3\text{ (aq) + 3 NH}_4\text{OH (aq) } \rightarrow \text{ Fe(OH)}_3\text{ (s) + 3 NH}_4\text{Cl (aq)}
\]

Reaction 5: Aqueous Barium Chloride + Sulfuric Acid

- Reaction Type: Precipitation Reaction
- Observations: Formation of a white precipitate.
- Product Names & States: Barium sulfate (BaSO₄, s) and hydrochloric acid (HCl, aq).
- Balanced Equation:
\[
\text{BaCl}_2\text{ (aq) + H}_2\text{SO}_4\text{ (aq) } \rightarrow \text{ BaSO}_4\text{ (s) + 2 HCl (aq)}
\]

Reaction 6: Aqueous Sodium Phosphate + Aqueous Copper(II) Sulfate

- Reaction Type: Precipitation Reaction
- Observations: Formation of a blueish precipitate.
- Product Names & States: Copper(II) phosphate (Cu₃(PO₄)₂, s) and Sodium sulfate (Na₂SO₄, aq).
- Balanced Equation:
\[
2 \text{Na}_3\text{PO}_4\text{ (aq) + 3 CuSO}_4\text{ (aq) } \rightarrow \text{ Cu}_3\text{(PO}_4\text{)}_2\text{ (s) + 3 Na}_2\text{SO}_4\text{ (aq)}
\]

Reaction 7: Aqueous Sodium Carbonate + Cobalt(II) Nitrate

- Reaction Type: Precipitation Reaction
- Observations: Formation of a precipitate with a pink hue.
- Product Names & States: Cobalt(II) carbonate (CoCO₃, s) and Sodium nitrate (NaNO₃, aq).
- Balanced Equation:
\[
\text{Na}_2\text{CO}_3\text{ (aq) + Co(NO}_3\text{)}_2\text{ (aq) } \rightarrow \text{ CoCO}_3\text{ (s) + 2 NaNO}_3\text{ (aq)}
\]

Reaction 8: Aqueous Sodium Chloride + Aqueous Potassium Nitrate

- Reaction Type: No Reaction
- Observations: No visible change.
- Product Names & States: None, as no precipitate forms.
- Balanced Equation:
\[
\text{NaCl (aq) + KNO}_3\text{ (aq) } \rightarrow \text{No Reaction}
\]

Reaction 9: Aqueous Nickel(II) Nitrate + Aqueous Sodium Hydroxide

- Reaction Type: Precipitation Reaction
- Observations: Formation of a green precipitate.
- Product Names & States: Nickel(II) hydroxide (Ni(OH)₂, s) and Sodium nitrate (NaNO₃, aq).
- Balanced Equation:
\[
\text{Ni(NO}_3\text{)}_2\text{ (aq) + 2 NaOH (aq) } \rightarrow \text{ Ni(OH)}_2\text{ (s) + 2 NaNO}_3\text{ (aq)}
\]

Classification of Compounds

| Compound Name | Chemical Formula | Description |
|-------------------------|--------------------|------------------------------------------------------------|
| Aluminum oxide | Al₂O₃ | Ionic compound |
| Calcium carbonate | CaCO₃ | Ionic compound |
| Tin(IV) sulfate | Sn(SO₄)₂ | Ionic compound |
| Silver sulfite | Ag₂SO₃ | Ionic compound |
| Nitric acid | HNO₃ | Acid |
| Carbon tetrachloride | CCl₄ | Covalent compound |
| Hydrosulfuric acid | H₂S | Acid |
| Diphosphorus pentoxide | P₂O₅ | Covalent compound |
| Calcium oxide | CaO | Ionic compound |
| Lead(II) chloride | PbCl₂ | Ionic compound |
| Aluminum phosphate | AlPO₄ | Ionic compound |
| Sulfuric acid | H₂SO₄ | Acid |
| Nitrogen tribromide | NBr₃ | Covalent compound |

Conclusion

This experimental study of double replacement reactions illustrates the diverse forms such reactions can take and provides insight into the nature of ionic and covalent compounds. By predicting the reaction types based on chemical reactivity, observing the outcomes, and systematically balancing equations, we gain a foundational understanding crucial to the study of chemistry.

References

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