Ice water bath solution became darker pink the

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Ice water bath: solution became darker pink; the product heat was decreased, so equilibrium shifted to the right CoCl 4 + 6H 2 O (l) → Co(H 2 O) 6 + 4Cl - (aq) Addition of HCl: Counteracts the effect of the OH - group in CoCl 4 , causing the solution to turn blue; equilibrium shifts to the left Addition of HCl and AgNO 3 : precipitate forms; equilibrium shifts to the right Addition of acetone: turns blue; equilibrium shifts to the left Hot water bath: solution became light blue; from this it can be determined that the reaction is endothermic; with reactant being added, equilibrium will shift to the right toward the products Ice water bath: solution turned pink; equilibrium will shift to the right Reactions rewritten with heat included: (aq) + 2NaOH(aq) → 2NaCl(aq) + (s) + Heat This reaction is exothermic because when one of the solutions from part I is placed in the hot water bath, the solution turned light pink showing that the reaction is exothermic (heat is a product) because when product is added, equilibrium shifts to the left. CoCl 4 + 6H 2 O (l) + Heat → Co(H 2 O) 6 + 4Cl - (aq) This reaction is endothermic because when one of the solutions from part II is placed in the hot water bath, the solution turned light blue, indicating that equilibrium was moving away from the reactant side. This shows that the reaction is endothermic because when reactant is added, equilibrium shifts to the right.
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Each reactant or indicator added to the two reactions caused a different change in colors of the solutions or a different precipitant to form. The directions of equilibrium shifts can be determined from these changes or precipitate formations. Temperature change also affects the shifting of equilibrium. When the solution was in the hot water bath, it turned light pink. This means the reaction of MgCl 2 and NaOH is exothermic; therefore, when heat was added and the product side of the reaction was increased, equilibrium shifted to the left. The opposite situation occurs when the solution is in the ice water bath. The product side of the reaction is decreased, so equilibrium shifts toward the right. The same thing occurs with the reaction of the hexaaquacobalt (II) complex ion. The equilibrium shift can be determined by looking at the color changes and precipitation formations. Some sources of error that could have occurred in this experiment include:
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