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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 11
A 0.025 M solution of sodium thiosulfate is used to titrate 25.0 mL of iodine solution. If 30.0 mL of thiosulfate is required, calculate the molarity of the iodine solution.
A 20.0 mL sample of 0.05 M oxalic acid is titrated with 0.02 M KMnO4 in acidic medium. Calculate the volume of KMnO4 required. (Reaction: 2 MnO4- + 5 C2O42- + 16 H+ → 2 Mn2+ + 10 CO2 + 8 H2O)
A 25.0 mL sample of 0.1 M FeSO4 is titrated with 0.02 M KMnO4. What volume of KMnO4 is required? (Reaction: 5 Fe2+ + MnO4- + 8 H+ → 5 Fe3+ + Mn2+ + 4 H2O)
A solution contains both Fe2+ and Fe3+. Which ion can be titrated directly with KMnO4?
Calculate the molarity of a KMnO4 solution if 25.0 mL of it reacts completely with 50.0 mL of 0.100 M FeSO4 solution in acidic medium. (The reaction is: 5 Fe2+ + MnO4- + 8 H+ → 5 Fe3+ + Mn2+ + 4 H2O)
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 role of an indicator in a redox titration.
Explain the term 'back titration' in the context of redox titrations.
Explain why KMnO4 is not used as a primary standard.
Explain why potassium permanganate acts as a self-indicator in redox titrations.
Explain why the titration of oxalic acid with KMnO4 is carried out at about 60°C.
In a titration, 20.0 mL of 0.02 M K2Cr2O7 is required to oxidize Fe2+ in 50.0 mL of solution. Calculate the molarity of Fe2+ in the solution. (Reaction: Cr2O72- + 6 Fe2+ + 14 H+ → 2 Cr3+ + 6 Fe3+ + 7 H2O)
State one precaution to be taken while performing a redox titration involving KMnO4.
State one reason why redox titrations are important in analytical chemistry.
Why is starch added near the endpoint in iodometric titrations?
Write the balanced ionic equation for the reaction between MnO4- and Fe2+ in acidic medium.