An equilibrium involving chromate(VI) and dichromate(VI) ions
sulfuric acid is added to an aqueous solution of . Colour changes are observed. The reaction is then reversed using aqueous potassium chromate(VI) sodium hydroxide.
This experiment is most appropriate with A-level students, given the potential hazards with solutions containing chromate(VI) and dichromate(VI) ions. Otherwise it could be carried out as a teacher demonstration. This experiment can be carried out individually by students, but the
potassium chromate(VI) solution used should be prepared beforehand by the teacher or technician, given the hazards presented by the solid. It should take no more than 5 min.
For one demonstration:
Eye protection: goggles
Potassium chromate(VI) solution, 0.2 M (TOXIC, OXIDISING, DANGEROUS FOR THE ENVIRONMENT), about 1 cm 3
Sodium hydroxide solution, 1.0 M (CORROSIVE), about 10 cm 3
sulfuric acid, 1.0 M (IRRITANT), about 5 cm 3
Refer to Health & Safety and Technical notes section below for additional information.
Health & Safety and Technical notes
Read our standard health & safety guidance
Potassium chromate(VI) solution, K 2CrO 4(aq) (TOXIC, OXIDISING, DANGEROUS FOR THE ENVIRONMENT) - see CLEAPSS Hazcard and CLEAPSS Recipe Book.
Sodium hydroxide solution, NaOH(aq) (CORROSIVE) - see CLEAPSS Hazcard and CLEAPSS Recipe Book.
sulfuric acid, H 2SO 4(aq), (IRRITANT) - see CLEAPSS Hazcard and CLEAPSS Recipe Book.
a Put 10 drops of potassium chromate(VI) solution in a test-tube.
b Add about 5 cm 3 of sulfuric acid and shake to mix thoroughly. What do you observe?
c Now add about 10 cm 3 of sodium hydroxide solution and shake the mixture. Do you get back to where you started?
d Can you repeat the whole process by adding sulfuric acid and sodium hydroxide alternately all over again?
The process occurring involves the equilibrium between chromate(VI), dichromate(VI) and hydrogen ions:
4 2-(aq) (yellow) + 2H +(aq) ⇌ Cr 2O 7 2-(aq) (orange) + H 2O(l)
The addition of acid encourages the equilibrium towards the right, producing more orange-coloured dichromate(VI) ions. The addition of hydroxide ions causes the concentration of hydrogen ions to decrease, and this brings the equilibrium back to the left-hand side, regenerating yellow chromate(VI) ions.
It is important that students realize that both ions are always present and exist in equilibrium with one another, but that the yellow chromate(VI) ions predominate under alkaline conditions and the orange dichromate(VI) ions predominate in acidic solutions.
Students may be asked if this is a redox reaction. Their answer is often ‘yes’, but examination of oxidation numbers will show that chromium remains in the +6 oxidation state throughout.
Health & Safety checked, 2016
This Practical Chemistry resource was developed by the Nuffield Foundation and the Royal Society of Chemistry.
© Nuffield Foundation and the Royal Society of Chemistry
Page last updated October 2015