A group of students is given the task of determining the iodide ion (I-) content of tablets that contain KI and an inert filler. This inert filler...
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A group of students is given the task of determining the iodide ion (I-) content of tablets that contain KI and an inert filler. This inert filler and the KI will both dissolve in water. A tablet is dissolved in 75.0 mL of distilled water and an excess of 0.20 M Pb(NO3)2 solution is added. A yellow precipitate forms, which is then filtered, washed and dried. The data for the group's experiment is shown above.

For the chemical reaction that occurs when the yellow precipitate forms:

  1. write the balanced, net-ionic equation for the reaction. (1 point)
  2. explain why the reaction is best represented by a net-ionic equation. (2 points)
  3. Explain why the filter paper with the precipitate was dried and weighed three times. (2 points)
  4. In the filtrate solution, is the concentration of NO3- greater than, less than or equal to the concentration of K+. Explain your answer. (3 points)
  5. Calculate the number of moles of precipitate produced in the experiment. (3 points)
  6. Calculate the mass percent of iodide ion (I-) in the tablet. (3 points)
  7. In another trial, the group dissolves a tablet in 85.0 mL of water. Will the mass percent of iodide ion (I-) be greater than, less than, or equal to the amount calculated in part (e). Justify your answer. (3 points)
  8. Consider the solution of Pb(NO3)2 used in the experiment. If viewed on a molecular level, describe the appearance, charge and shape of a single Pb(NO3)2 unit in solution. (3 points)

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