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Solution Equilibrium

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Solution Equilibrium. A pink solution is warmed and becomes blue Upon cooling it becomes pink again, demonstrating a reversible chemical change. Purpose. To shift a chemical equilibrium by temperature alone

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A pink solution is warmed and becomes blue

Upon cooling it becomes pink again,

demonstrating a reversible chemical change

  • To shift a chemical equilibrium by temperature alone
  • To observe the color change which occurs and relate it to the chemical reaction for the demonstration
  • The chemical equation for the reaction was

Co(H2O)62+ + 4Cl-CoCl42- (aq) + 6H2O

Higher temperatures shift the equilibrium to the blue


Lower temperatures favor the pink


Thus, the reaction adjusted to its environment!


1. Reversible Chemical Reactions

2. Chemical Equilibria

3. Hydrated Ions

1 reversible chemical reactions
1. Reversible Chemical Reactions
  • Not all chemical reactions convert reactants completely to products

A + B C + D

  • Many reactions will contain ALL species rather than converting completely

A + B C + D

  • The double arrow indicates the reaction is reversible and both A and B as well as C and D are simultaneously present when the reaction is finished
2 chemical equilibrium
2. Chemical Equilibrium
  • In a reversible chemical reaction
    • A + B C + D
    • reactants are said to be
    • “in equilibrium” with their products
  • Equilibria may lie
    • more toward products
    • A + B C + D
          • or
    • more toward reactants
  • A + B C + D
3 hydrated ions
3. Hydrated Ions
  • Ions in aqueous solution are surrounded by a shell of water
  • Such ions are said to be hydrated
  • Hydrated ions such as sodium ion are written as Na+(aq) where aq is Latin for aqua, meaning ‘water’
  • The equilibrium of a solution at a given temperature shifted when the temperature was changed
  • The change was noted by the color change from the pink, hydrated ion to the blue, anhydrous ion
  • The change was reversible
  • Most chemical reactions of

biochemical systems are at