Lab 8 Le Chatlier’s Principle

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Results Sheet, Experiment 9 Part 1 Mg(OH)2(s)  Mg2+(aq) + 2 OH-(aq) Observations: Well Initial Observation (Step 5) Step 6, 7, 9 or 10 (depending on the well) Step 12 C1 Turned pink 1 drop, removed most pink. 2 drops, pink gone C2 Turned pink 4 drops started lightening. 10 drops pink nearly gone C3 Turned pink Became thinner Became thicker C4 Turned pink Became thicker Became thinner Part 1. Questions: When asked about a shift to an equilibrium, the reaction either shifts toward reactants or toward products (the reaction starts at equilibrium, something is done to the reaction; after the disturbance, the reaction proceeds in the reverse direction as written forming more reactants to relieve the stress or the reaction proceeds in the forward direction to form more product). In Part I the reaction you observed was Mg(OH)2 (s) ↔ Mg2+ (aq) + 2 OH- (aq). Compare the colors you observed in the experiment and answer these questions: Which way should the equilibrium shift when HCl is added? How do your results support your answer? It should shift toward the reactants. It is shown by removing the pink color from the product. B. Which way should the equilibrium shift when Na2 EDTA is added? How do your results support your answer? It should shift toward the reactants. It is shown by removing the pink color from the product. Is this reaction endothermic or exothermic? How do you know? Endothermic. The reaction shifts to the left and it consumes heat. Part 2. HSO4-(aq) + H2O(l)  H3O+(aq) + SO42-(aq) Observations: Well Step 3, 5, or 12 (depending on the well) Step 14 A1 Turns more of an orange color than pink A2 (Control) None None A3 Color turns darker A4 Initial Temperature: 43 degrees C. No noticeable change A5 Initial Temperature: 14 degrees C No noticeable change Questions: In Part II the
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