Chromate ion equilibrium experiment

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Chromate ion equilibrium experiment. Yellow potassium chromate (VI) solution is added to a beaker. This contains the yellow chromate (CrO4 2-) ion, in equilibrium with the orange dichromate (Cr2O7 2- )ion. The equilibrium is heavily towards the chromate side in alkali conditions. Adding sulphuric acid shifts the equilibrium to the dichromate side, changing the colour of the solution to orange. Adding alkali sodium hydroxide brings the equilibrium back to the chromate side. Adding acid again takes it back the other way, and so on, demonstrating its reversible nature. This change in the equilibrium position occurs because the chromate ion side of the equilibrium also contains two free acidic protons (H+), whose existence is favoured under alkali conditions. This is an example of Le Chatelier's principle. The full equilibrium equation is: Cr04 2- + 2H+ <---> Cr2O7 2- + H2O
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Credit: Science Photo Library / Chillmaid, Martyn F. / University of Nottingham
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