Use a balanced net ionic equation to explain.Ģ. Based on your observations on Part I, what could be expected to happen if the solution of 2+ were diluted with water. Part III: Effect of Temperature on EquilibriaĪ.) Is the reaction exothermic or endothermic? Explain your answer.ġ. Include a balanced net ionic equation for the reaction that occurs and explain which way the equilibrium in (h) shifts as KI(aq) is added and why in terms of Le Châtelier’s principle. Include a balanced net ionic equation for the reaction that occurs and explain which way the equilibrium in (e) shifts as HNO3(aq) is added and why in terms of Le Châtelier’s principle.ī.) Which ions and/or solids are present in the test tube after the addition of HNO3(aq)?Ĭolor changes to bright yellow “lemonade” color, with a cloudy precipitateĪ.) Account for your observations when adding KI(aq). Remains clear, and colorless, produces a water vapor and heat.Ī.) Account for your observations when adding HNO3(aq). Include a balanced net ionic equation and explain which way the equilibrium in (d) shifts as NH3 (aq) is added and why in terms of LeChâtelier’s principle. Solution clears out, removing the cloudy precipitateĪ.) Explain your observation when excess NH3(aq) is added to the test tube. Include the balanced net ionic equation and explain which way the equilibrium in (a) shifts and why in terms of Le Châtelier’s principle.ī.) Which ions remain in the test tube after addition of HNO3(aq)?įormed a solid and chunky precipitate, though not cloudyĪ.) Write the balanced net ionic equation for the equilibrium that is established when HCl(aq) is added to the test tube. Why does this equilibrium occur?ġ drop cleared the solution, no color, no precipitateĪ.) Account for your observations when adding HNO3(aq). Part II: Equilibria Involving Sparingly Soluble Saltsīright yellow “lemon-aid” color, with a cloudy precip.Ī.) Write the balanced net ionic equation for the equilibrium that is established upon mixing. Explain which way the equilibrium in (a) shifts as water is added and why in terms of LeChâtelier’s principle. Include a balanced net ionic equation and explain which way the equilibrium shifts as more HCl(aq) is added and why in terms of LeChâtelier’s principle.ī.) Account for your observation when adding water to the 2- complex solution. Explain which way the equilibria in (a) shift and why in terms of LeChatlier’s principle as HCl is added.Ĭ.) What initially forms as pale blue and pale green precipitates when NH3(aq) is added to 2+ and 2+ solutions, respectively? Why do these precipitates form?Ĭleared changes, returned to red, see through.Ī.) Explain your observation upon addition of 12 M HCl(aq) to the original CoCl2 solution. Include the balanced net ionic equation for the reaction that occurs. Include balanced net ionic equations (2) and explain what happens in the reactions in terms of LeChâtelier’s principle as more NH3(aq) is added.ī.) Explain your observations upon addition of HCl(aq) on the solutions. Produced heat, water vapor, cleared the color, and removed the precipitateĪ.) Explain your observations upon addition of NH3(aq) to the CuSO4 and NiCl2 solutions. Part I: Changes in Reactant or Product Concentrations
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |