Chemical Equilibrium: Observing Changes in Cr2O7- & CrO4- Mixture

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SUMMARY

The discussion focuses on the chemical equilibrium between chromate ions (CrO4^2-) and dichromate ions (Cr2O7^2-) when potassium chromate is dissolved in acid. The net ionic equation for this equilibrium is 2 CrO4^2- (aq) + 2 H3O^+ ⇌ Cr2O7^2- (aq) + 3 H2O (l). When sulfuric acid (H2SO4) is added, the equilibrium shifts towards the formation of dichromate ions, resulting in a color change from light orange to a deeper orange. Conversely, the addition of sodium hydroxide (NaOH) shifts the equilibrium back towards chromate ions, leading to a color change towards yellow.

PREREQUISITES
  • Understanding of chemical equilibrium principles
  • Familiarity with net ionic equations
  • Knowledge of acid-base reactions
  • Basic concepts of colorimetry in chemical solutions
NEXT STEPS
  • Study Le Chatelier's Principle in detail
  • Explore the effects of pH on chromate and dichromate equilibria
  • Learn about the applications of chromate and dichromate in analytical chemistry
  • Investigate colorimetric analysis techniques for solution concentration
USEFUL FOR

Chemistry students, educators, and laboratory technicians interested in chemical equilibria, acid-base reactions, and colorimetric analysis in solutions.

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an equilibrium exists between chromate ion and the dichromate ion when potassium chromate is dissolved acid. the net ionic equation describing this reaction is given in the follwering equation:

2 CrO4^2- (aq) + 2 H3O^+ (equilibrium symbol) Cr2O7^2- (aq) + 3 H2O (l)

a student studying this equilibrium begins w/ an equilibrium mixture that is light orage in color.

a. what change will the student observe when a solution of H2SO4 is added to this mixture at equilibrium?

b. briefly explain the above answer

c. what change will the student observe when a solution of NaOH is added to another example of this solution at equilibrum. why?
 
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