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Hi-Ho Silver Lab.docx - Chapman _ Norquay School

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					Mr. Chapman                                                                   Chemistry 20
Hi-Ho Silver Lab

Hi-Ho Silver Lab
Purpose: To begin to understand the relationship between balanced chemical
equations and mole ratios. In this chemical reaction we will use mole ratios to
determine which copper ion is formed when solid copper reacts with aqueous
silver acetate.

Hypothesis: Record your prediction. Will copper (I) or copper (II) ions be
formed?

Procedure:

Day 1

    □ Write out and balance the two possible chemical reactions that could occur
      when silver acetate reacts with copper metal.
    □ Determine the mass of a clean, dry labelled beaker.
    □ Obtain a sample of 1.0 g of silver acetate.
    □ Dissolve the silver acetate in about 75 mL of distilled water. We will assume
      that all of the silver nitrate reacts. It is important you use distilled water
      because the silver ions will react with the fluorine in ordinary tap water forming a
      fine white precipitate which would introduce considerable error to your lab.
    □ Obtain a piece of copper wire about 30 cm long.
    □ Coil one end of the copper wire around a pencil or your finger. Bend the other
      end to form a hook so that the wire
      can be hung on the lip of the beaker.
      Carefully determine the mass of the
      copper and record it.
    □ Place the copper coil in the beaker of
      silver acetate solution. Leave it sit
      perfectly still for a period of 15
      minutes. Record your observations of
      the reaction during this time.
    □ Set your beaker aside and allow the
      reaction to proceed until tomorrow.
Mr. Chapman                                                             Chemistry 20
Hi-Ho Silver Lab

Day 2

    □ Set up a filtration apparatus (see the previous page)
    □ Obtain a beaker to be used to catch the filtrate (the fluid that is currently
      in your beaker)
    □ Determine the mass of a sheet of filter paper. Fold it into a cone and set
      it into a funnel. Wet the filter paper with tap water to hold it in place.
    □ CAREFULLY transfer the contents of the beaker into the filter funnel. You
      want to have all the silver metal inside the filter paper. Rinse the insides
      of the beaker with distilled water, pouring the water over the silver in the
      filter funnel. Use the distilled water bottle to clean off the copper wire,
      again allowing the water to run through the filter paper.
    □ Wash the silver in the filter funnel thoroughly with distilled water.
    □ Discard the filtrate (blue copper acetate solution) down the sink.
    □ Place the filter paper with the silver in the beaker with your piece of
      copper and place it in the oven to dry overnight.

Day 3

    □ Determine the mass of copper wire after the reaction
    □ Determine the mass of the dry silver and filter paper
    □ Perform the analysis calculations and complete the conclusion section

Analysis: – Show all of your work!

    1. Copper
       a. Determine the mass of copper that reacted
       b. Determine the number of moles of copper that reacted

    2. Silver acetate
       a. Determine the mass of silver acetate that reacted
       b. Determine the number of moles of silver acetate that reacted
Mr. Chapman                                                           Chemistry 20
Hi-Ho Silver Lab

    3. Silver
       a. Determine the mass of solid silver that is produced
       b. Determine the number of moles of silver produced

    4. Ratios
       a. Determine the ratio of moles of Ag produced to moles of Cu reacted.
          Round off this ratio to the nearest whole number
       b. Determine the ratio of moles of Ag produced to moles of AgCH3COO.
          Round this ratio to the nearest whole number

    5. Using the ratios calculated in #4, determine which of the two possible
       reactions occurred. Explain your answer.

Conclusion:

    1. Write the balanced chemical equation determined in this experiment (be
       sure to include the state of all substances)
    2. Stoichiometry calculations: Use the balanced equation to solve the
       following problems.
       a. What mass of copper would need to be used to produce a 25 g silver
           bar?
       b. What mass of silver nitrate would be needed to produce the same 25
           g silver bar?

				
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