Experiment Title:
Study of Chemical Equilibrium – Effect of Concentration on the Position of Equilibrium
Objective:
To observe the effect of changing concentration on the position of equilibrium in a reversible reaction.
Materials Required:
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Iron(III) chloride solution (FeCl₃)
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Potassium thiocyanate solution (KSCN)
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Distilled water
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Test tubes
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Dropper
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Beaker
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Glass rod
Chemical Reaction:
This reaction shows a reddish-brown complex formation, which is reversible.
Procedure:
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Preparation of Equilibrium Mixture:
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Take about 5 mL of 0.002 M FeCl₃ solution in a test tube.
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Add 5 mL of 0.002 M KSCN solution.
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Mix well and observe the reddish-brown colour of FeSCN²⁺ complex indicating equilibrium.
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Effect of Adding Reactant (KSCN):
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Take a small portion of the equilibrium mixture in another test tube.
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Add a few drops of KSCN solution.
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Observe the intensification of the reddish-brown colour (due to shift in equilibrium to the right).
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Effect of Adding Reactant (FeCl₃):
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Take another portion of the original equilibrium mixture.
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Add a few drops of FeCl₃ solution.
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Observe the increase in colour intensity again (shift to the right).
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Effect of Dilution:
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Take a third portion of the equilibrium mixture.
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Add distilled water.
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Observe the fading of the colour indicating a shift in equilibrium (can be interpreted depending on ion concentration changes).
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Observation:
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Addition of either Fe³⁺ or SCN⁻ ions deepens the colour of the complex.
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This confirms that equilibrium shifts to the right (product side) when reactant concentration increases (as per Le Chatelier’s Principle).
Conclusion:
The position of chemical equilibrium is influenced by the concentration of reactants. Increasing the concentration of reactants shifts the equilibrium towards the formation of more product.