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7.1: Observing Two Major Classes of Chemical Reactions - Experiment

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    547466

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    SAFETY PRECAUTIONS
    • Always wear safety goggles and a lab coat in the laboratory.
    • Hydrochloric acid and sulfuric acid are corrosive. Avoid contact with skin and eyes. In case of contact, flush the affected area immediately with plenty of water and seek medical attention if necessary.
    • Sodium hydroxide is caustic. Avoid contact with skin and eyes. In case of contact, flush immediately with water.
    • Metal solutions are toxic. Avoid ingestion and skin contact. Dispose of all chemical waste in designated containers.

    EQUIPMENT AND CHEMICALS NEEDED

    Table \(\PageIndex{1}\): Materials List
    Equipment Solutions Solutions Metal Samples
    12- or 24-hole well plates & small test tubes 1.0 M Na2CO3 3.0 M H2SO4 Ca metal
    Dropper bottles 6.0 M HCl 0.1 M AgNO3 Cu metal
    Test tube rack 0.1 M Na2CO3 0.1 M KCl Al metal
    Labels 0.1 M Cu(NO3)2 0.1 M NaNO3 Mg metal
      0.1 M Na3PO4 0.1 M CuCl2 Zn metal
      0.1 M Fe(NO3)3 0.1 M Mg(NO3)2  
      0.1 M NaOH 0.1 M Zn(NO3)2  
      1.0 M NaHCO3    

    EXPERIMENTAL PROCEDURE

    Part A: Perform Double Displacement Reactions

    Evidence of a chemical reaction can be observed through the formation of a precipitate, gas evolution, a color change, a pH shift, or temperature changes (exothermic or endothermic).

    1. Label well plates or test tubes with the appropriate reactant combinations.
    2. Using dropper bottles, add approximately 10 drops (or 1 mL in a test tube) of each solution to the corresponding well or test tube as indicated below and record your observations on the report sheet:
      1. 1.0 M Na2CO3 + 6.0 M HCl
      2. 0.1 M Na2CO3 + 0.1 M Cu(NO3)2
      3. 0.1 M Cu(NO3)2 + 0.1 M Na3PO4
      4. 0.1 M Fe(NO3)3 + 0.1 M Na3PO4
      5. 0.1 M Fe(NO3)3 + 0.1 M NaOH
      6. 6.0 M NaOH + 6.0 M HCl
      7. 1.0 M NaHCO3 + 6.0 M HCl
      8. 1.0 M NaHCO3 + 3.0 M H2SO4
      9. 0.1 M AgNO3 + 0.1 M KCl
      10. 0.1 M KCl + 0.1 M NaNO3
    3. Carefully observe each reaction mixture for evidence of a chemical reaction. Record your observations in the data table. Note any precipitate formation, gas evolution, color changes, or temperature changes.
    4. For each reaction, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no reaction occurred, record "NR".

    Part B: Perform Redox Reactions

    B1: React Metals with Acid

    1. Place a small piece of each metal (Ca, Cu, Al, Mg, and Zn) into separate wells or small test tubes.
    2. Add approximately 10 drops (or 1 mL) of 6.0 M HCl to each well or test tube.
    3. Observe the reactions for at least 5 minutes. Record your observations in the data table, noting any gas evolution, color changes, or disappearance of the metal.
    4. Write balanced molecular and net ionic equations for the observed reactions.

    B2: React Metals with Metal Ions

    1. Place a small piece of aluminum in three separate wells or test tubes.
    2. Add approximately 10 drops (or 1 mL) of each of the following solutions: 0.1 M CuCl2, 0.1 M Mg(NO3)2, and 0.1 M Zn(NO3)2.
    3. Observe reactions for at least 5 minutes. Record any color changes, precipitate formation, or changes in the appearance of the metal surface.
    4. Repeat using Cu, Mg, and Zn, adding the corresponding metal ion solutions as listed in the data table.
    5. Write balanced molecular and net ionic equations for the observed reactions.
    CHEMICAL DISPOSAL
    • Place all aqueous waste solutions into the designated INORGANIC LIQUID WASTE container.
    • Place all unreacted metal solids into the designated SOLID METAL WASTE container.

    This page titled 7.1: Observing Two Major Classes of Chemical Reactions - Experiment was last modified on Thu, 01 Oct 2026 18:07:22 GMT and is shared under a CC BY 4.0 license and was authored, remixed, and/or curated by Vincent Hradil and Saadia Khan.