Redox Titrations

Chemistry ⇒ Redox Reactions and Electrochemistry

Redox Titrations starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Redox Titrations. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

A 25.0 mL sample of 0.100 M Fe²⁺ is titrated with 0.0200 M KMnO₄ in acidic medium. Calculate the volume of KMnO₄ required to reach the endpoint.

A 50.0 mL sample of 0.100 M oxalic acid (H₂C₂O₄) is titrated with 0.0200 M KMnO₄ in acidic medium. Calculate the volume of KMnO₄ required. (Reaction: 5H₂C₂O₄ + 2MnO₄^- + 6H⁺ → 10CO₂ + 2Mn²⁺ + 8H₂O)

A redox titration is performed to determine the concentration of hydrogen peroxide using KMnO₄. Write the balanced equation for the reaction in acidic medium.

A redox titration is performed using 0.0250 M K₂Cr₂O₇ as the titrant. If 30.0 mL of titrant is required to reach the endpoint, how many moles of Cr₂O₇^2- were used?

A solution contains 0.025 mol of Fe²⁺. How many moles of KMnO₄ (in acidic medium) are required to completely react with the Fe²⁺? (The reaction is: 5Fe²⁺ + MnO₄^- + 8H⁺ → 5Fe³⁺ + Mn²⁺ + 4H₂O)

A student titrates 20.0 mL of 0.0500 M Na₂S₂O₃ with iodine solution. How many moles of I₂ are required for complete reaction? (Reaction: 2S₂O₃^2- + I₂ → S₄O₆^2- + 2I^-)

A student titrates 25.0 mL of 0.200 M Fe²⁺ with 0.0200 M KMnO₄. Calculate the volume of KMnO₄ required to reach the endpoint.

Calculate the normality of a 0.02 M KMnO₄ solution used in acidic medium (n-factor = 5).

Describe the difference between iodometric and iodimetric titrations.

Describe the function of a redox indicator.

Explain why potassium dichromate is not used as a self-indicator in redox titrations.

Explain why potassium permanganate acts as its own indicator in redox titrations.

Explain why sodium thiosulfate solutions should be standardized before use in titrations.

Explain why the solution must be acidic during the titration of Fe²⁺ with KMnO₄.

In the titration of oxalic acid with KMnO₄, the reaction mixture must be heated. State the reason.

State the role of starch in iodometric titrations.