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\ \mathrm{M} oxalic acid is titrated with 0.02\ \mathrm{M}\ \mathrm{KMnO_4} in acidic medium. Calculate the volume of \mathrm{KMnO_4} required. (Reaction: 2\ \mathrm{MnO_4^-} + 5\ \mathrm{C_2O_4^{2-}} + 16\ \mathrm{H^+} \rightarrow 2\ \mathrm{Mn^{2+}} + 10\ \mathrm{CO_2} + 8\ \mathrm{H_2O})
A 25.0 mL sample of 0.1\ \mathrm{M}\ \mathrm{FeSO_4} is titrated with 0.02\ \mathrm{M}\ \mathrm{KMnO_4}. What volume of \mathrm{KMnO_4} is required? (Reaction: 5\ \mathrm{Fe^{2+}} + \mathrm{MnO_4^-} + 8\ \mathrm{H^+} \rightarrow 5\ \mathrm{Fe^{3+}} + \mathrm{Mn^{2+}} + 4\ \mathrm{H_2O})
A solution contains both \mathrm{Fe^{2+}} and \mathrm{Fe^{3+}}. Which ion can be titrated directly with \mathrm{KMnO_4}?
Calculate the molarity of a \mathrm{KMnO_4} solution if 25.0 mL of it reacts completely with 50.0 mL of 0.100\ \mathrm{M}\ \mathrm{FeSO_4} solution in acidic medium. (The reaction is: 5\ \mathrm{Fe^{2+}} + \mathrm{MnO_4^-} + 8\ \mathrm{H^+} \rightarrow 5\ \mathrm{Fe^{3+}} + \mathrm{Mn^{2+}} + 4\ \mathrm{H_2O})
Calculate the normality of a 0.02\ \mathrm{M}\ \mathrm{KMnO_4} 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 \mathrm{KMnO_4} 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 \mathrm{KMnO_4} is carried out at about 60^\circ\mathrm{C}.
In a titration, 20.0 mL of 0.02\ \mathrm{M}\ \mathrm{K_2Cr_2O_7} is required to oxidize \mathrm{Fe^{2+}} in 50.0 mL of solution. Calculate the molarity of \mathrm{Fe^{2+}} in the solution. (Reaction: \mathrm{Cr_2O_7^{2-}} + 6\mathrm{Fe^{2+}} + 14\mathrm{H^+} \rightarrow 2\mathrm{Cr^{3+}} + 6\mathrm{Fe^{3+}} + 7\mathrm{H_2O})
State one precaution to be taken while performing a redox titration involving \mathrm{KMnO_4}.
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 \mathrm{MnO_4^-} and \mathrm{Fe^{2+}} in acidic medium.
