Lesson Worksheet: Reduction–Oxidation Titrations Chemistry • 10th Grade

In this worksheet, we will practice describing iodometry, iodimetry, and other redox titration methods and troubleshooting common errors.

Q1:

Triiodide ions are produced by the reaction of iodine with iodide ions. Why should iodine solutions contain an additional iodide salt if used as a titrant?

  • ATriiodide salts are more soluble in water than iodine.
  • BTriiodide ions undergo a more visible color change during reduction–oxidation reactions.
  • CTriiodide ions are more strongly oxidizing than iodine.
  • DTriiodide ions are more highly colored than iodine in water.
  • ETriiodide ions are more stable than iodine when stored under air.

Q2:

Which of the following is an accurate description of iodometry?

  • AExcess analyte is reacted with iodine, and the remainder is titrated against sodium thiosulfate.
  • BIodine is used as a titrant for an oxidizing analyte.
  • CIodine is used as a titrant for a reducing analyte.
  • DExcess sodium thiosulfate is reacted with an analyte, and the remainder is titrated against iodine.
  • EExcess iodide is reacted with an analyte, and the resulting iodine is titrated against sodium thiosulfate.

Q3:

Which of the following would not improve the accuracy of an iodometric titration?

  • AUsing only fresh thiosulfate solutions
  • BUsing excess iodide in the iodine solution
  • CUsing only fresh iodide solutions
  • DAdding starch indicator to the iodine solution
  • ELowering the pH of an acidic analyte solution

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