Oxidation Reactions in Titrations
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Questions and Answers

What color change indicates the endpoint in a titration involving KMnO₄?

  • Colorless to yellow
  • Purple to colorless (correct)
  • Green to blue
  • Colorless to purple

Which statement is true regarding potassium dichromate (K₂Cr₂O₇)?

  • It requires external indicators for titration. (correct)
  • It is a stronger oxidizing agent than KMnO₄.
  • It can oxidize I⁻ to I₂ without additional agents.
  • It serves as a self-indicator.

What reaction occurs during iodimetric titrations involving Cu²⁺ ions?

  • 2Cu²⁺(aq) + 4I⁻(aq) → Cu₂I₂(s) + I₂(aq) (correct)
  • I₂(aq) + 4H⁺(aq) + 2e⁻ → 2I⁻(aq) + 2H₂O(l)
  • Cu²⁺(aq) + I₂(aq) → CuI₂(s)
  • I₂(aq) + S₂O₃²⁻(aq) → Na₂S₄O₆(aq) + 2I⁻(aq)

What is the equivalent weight of KMnO₄ when used in acidic medium?

<p>31.6 g (A)</p> Signup and view all the answers

Which oxidizing agent is used specifically for titrating strong reducing agents like sodium thiosulphate?

<p>Iodine (I₂) (D)</p> Signup and view all the answers

What role does freshly prepared starch solution play in iodimetric titrations?

<p>It forms a blue complex with iodine for endpoint detection. (C)</p> Signup and view all the answers

Which oxidizing agent is characterized as a self-indicator?

<p>Potassium permanganate (KMnO₄) (D)</p> Signup and view all the answers

In iodimetric titrations, released iodine (I₂) is titrated against which solution?

<p>Sodium thiosulphate (Na₂S₂O₃) (C)</p> Signup and view all the answers

Flashcards

KMnO₄ in titration

Potassium permanganate (KMnO₄) is a strong oxidizing agent used in titrations. It acts as a self-indicator, changing color from purple to colorless during the reaction.

Acidified K₂Cr₂O₇

Acidified potassium dichromate (K₂Cr₂O₇) is a weaker oxidizing agent used in redox titrations but needs external indicators.

Iodine (I₂) titration

Iodine (I₂) is a mild oxidizing agent used in titrations, especially with strong reducing agents like sodium thiosulfate.

Iodimetric titration

Iodine is directly titrated against the reducing agent.

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Iodometric titration

Iodine is produced and then titrated against a standard solution.

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Equivalent weight (Eq. wt.)

The equivalent weight of an oxidizing/reducing agent is its molar mass divided by the change in oxidation state or number of electrons gained or lost

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Endpoint detection (I₂)

The endpoint in iodimetric titrations is detected using starch that forms an intense blue complex with iodine.

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Redox titration

Redox Titration is a method to determine the concentration of a reducing agent using an oxidizing agent or vice versa.

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Study Notes

Oxidation Reactions as the Basis of Titrations

  • Potassium permanganate (KMnO4) is a strong oxidizing agent
  • In titrations, KMnO4 acts as a self-indicator; its color disappears when it reacts with a reducing agent.
  • The reaction for the titration of MnO4- against Fe2+ ions is: MnO4- + 8H+ + 5e- → Mn2+ + 4H2O
  • Acidified potassium dichromate (K2Cr2O7) is a weaker oxidizing agent than KMnO4
  • It does not act as a self-indicator; indicators like diphenylamine or potassium ferricyanide (K3[Fe(CN)6]) are used
  • The chemical equation for K2Cr2O7 as an oxidizing agent is: Cr2O72- + 14H+ + 6e- → 2Cr3+ + 7H2O

Iodine (I2)

  • Iodine is a mild oxidizing agent
  • The reaction is: I2 + 2e- → 2I-
  • Iodine is used in titrations with strong reducing agents like sodium thiosulfate (Na2S2O3)
  • The reaction is: I2(aq) + 2S2O32-(aq) → 2I-(aq) + S4O62-(aq)

Iodimetric and Iodometric Titrations

  • Iodimetric titrations: Iodine (I2) is directly titrated against a reducing agent
  • Iodometric titrations: Iodine is liberated from KI by an oxidizing agent, and the liberated iodine is then titrated against a standard solution of sodium thiosulfate (Na2S2O3)
  • The end point of iodimetric titrations is detected using a starch solution, which reacts with iodine to form an intensely blue-colored complex

Note

  • Equivalent weight (Eq. wt.) of an oxidizing or reducing agent = Mol. wt / Change in oxidation state or number of electrons gained or lost
  • Example: Eq. wt. of KMnO4 in an acidic medium = 158/5 = 31.6

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Description

Explore the fundamentals of oxidation reactions as they apply to titrations, highlighting the role of strong oxidizing agents such as potassium permanganate and potassium dichromate. Understand the self-indicating properties of KMnO4 and the use of indicators with K2Cr2O7. This quiz will test your knowledge of these important chemical processes.

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