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Minor Versionm

by Procheta Mallik

Introduction

Different metals have different reactivity. Here, we perform a simple experiment with 3 metals to see how their reactivities compare.

    • Avoid skin contact with the chemicals

    • Do not ingest any of the materials

    • Care should be taken while doing the experiment

    • Use the scissor/cutter with care

  1. Take out given bottle containing copper sulphate (CuSO4) crystals. Fill the container with water Tightly seal the cap and shake well till the CuSO4 crystals dissolve
    • Take out given bottle containing copper sulphate (CuSO4) crystals.

    • Fill the container with water

    • Tightly seal the cap and shake well till the CuSO4 crystals dissolve

  2. In a test tube, add 10 ml of copper sulphate solution. Add the given iron filings to it. Leave it for some time and observe the colour change .
    • In a test tube, add 10 ml of copper sulphate solution.

    • Add the given iron filings to it.

    • Leave it for some time and observe the colour change .

  3. Take a plastic bottle , cut it in half using a cutter/scissor . Place the upper half of the bottle inverted onto the lower part without the cap. Place a filter paper on the upper part of bottle.
    • Take a plastic bottle , cut it in half using a cutter/scissor .

    • Place the upper half of the bottle inverted onto the lower part without the cap.

    • Place a filter paper on the upper part of bottle.

  4. Transfer the solution containing iron filings and copper sulphate solution through the filter paper. Observe what is left as residue on the filter paper . Re-collect the filtrate in the test tube and observe its colour. Make a note/photo of it.
    • Transfer the solution containing iron filings and copper sulphate solution through the filter paper.

    • Observe what is left as residue on the filter paper .

    • Re-collect the filtrate in the test tube and observe its colour. Make a note/photo of it.

  5. Clean out the test tube with water and once again, pour 10 ml of copper sulphate in it. Cut the given magnesium ribbon into very small pieces using scissors. Add these Mg pieces to the CuSO4 solution in the test tube
    • Clean out the test tube with water and once again, pour 10 ml of copper sulphate in it.

    • Cut the given magnesium ribbon into very small pieces using scissors.

    • Add these Mg pieces to the CuSO4 solution in the test tube

  6. Observe what happens. Leave it for some time, even an hour if you can. You should clearly be able to see brown-ish particles depositing on the bottom of the test tube Filter the solution through a new filter paper, as shown in image .
    • Observe what happens. Leave it for some time, even an hour if you can.

    • You should clearly be able to see brown-ish particles depositing on the bottom of the test tube

    • Filter the solution through a new filter paper, as shown in image .

    • Observe what is left as a residue on the filter paper.

  7. Observe the filtrate in the test tube. Take a note/photo of the colour Compare the colour of all three solutions.
    • Observe the filtrate in the test tube. Take a note/photo of the colour

    • Compare the colour of all three solutions.

    • Cut the magnesium into as small pieces as possible for maximum effect

    • CuSO4 solution is too concentrated to see a noticeable colour change

    • Experiment not undertaken over sufficient time; let the Fe/Mg be in the blue solution for at least 15-20 min.

    • What colour does the CuSO4 solution change to when you add iron filings? Can you think why?

    • What colour change do you observe in the case of Mg? What do you think is happening?

    • What is the brownish powder that seems to deposit on the iron filings and magnesium ribbon after filtration?

    • Write down all the chemical reactions, even in words, involved.

Finish Line

Vishal Bhatt

Member since: 04/26/2017

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