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Solution Equilibrium

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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Solution Equilibrium

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  1. SolutionEquilibrium A pink solution is warmed and becomes blue Upon cooling it becomes pink again, demonstrating a reversible chemical change

  2. Purpose • 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

  3. Demonstration • The chemical equation for the reaction was Co(H2O)62+ + 4Cl-CoCl42- (aq) + 6H2O Higher temperatures shift the equilibrium to the blue CoCl42-specie Lower temperatures favor the pink Co(H2O)62+specie Thus, the reaction adjusted to its environment!

  4. Concepts 1. Reversible Chemical Reactions 2. Chemical Equilibria 3. Hydrated Ions

  5. 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

  6. 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

  7. 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’

  8. Conclusions • 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

  9. Comments • Most chemical reactions of biochemical systems are at equilibrium

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