Redox Titrations
Chemistry ⇒ Redox Reactions and Electrochemistry
Redox Titrations starts at 11 and continues till grade 12.
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A 25.0 mL sample of 0.100\ \mathrm{M}\ \mathrm{Fe^{2+}} is titrated with 0.0200\ \mathrm{M}\ \mathrm{KMnO_4} in acidic medium. Calculate the volume of \mathrm{KMnO_4} required to reach the endpoint.
A 50.0 mL sample of 0.100\ \mathrm{M} oxalic acid (\mathrm{H_2C_2O_4}) is titrated with 0.0200\ \mathrm{M}\ \mathrm{KMnO_4} in acidic medium. Calculate the volume of \mathrm{KMnO_4} required. (Reaction: 5\mathrm{H_2C_2O_4} + 2\mathrm{MnO_4^-} + 6\mathrm{H^+} \rightarrow 10\mathrm{CO_2} + 2\mathrm{Mn^{2+}} + 8\mathrm{H_2O})
A redox titration is performed to determine the concentration of hydrogen peroxide using \mathrm{KMnO_4}. Write the balanced equation for the reaction in acidic medium.
A redox titration is performed using 0.0250\ \mathrm{M}\ \mathrm{K_2Cr_2O_7} as the titrant. If 30.0 mL of titrant is required to reach the endpoint, how many moles of \mathrm{Cr_2O_7^{2-}} were used?
A solution contains 0.025 mol of \mathrm{Fe^{2+}}. How many moles of \mathrm{KMnO_4} (in acidic medium) are required to completely react with the \mathrm{Fe^{2+}}? (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})
A student titrates 20.0 mL of 0.0500\ \mathrm{M}\ \mathrm{Na_2S_2O_3} with iodine solution. How many moles of \mathrm{I_2} are required for complete reaction? (Reaction: 2\mathrm{S_2O_3^{2-}} + \mathrm{I_2} \rightarrow \mathrm{S_4O_6^{2-}} + 2\mathrm{I^-})
A student titrates 25.0 mL of 0.200\ \mathrm{M}\ \mathrm{Fe^{2+}} with 0.0200\ \mathrm{M}\ \mathrm{KMnO_4}. Calculate the volume of \mathrm{KMnO_4} required to reach the endpoint.
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 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 \mathrm{Fe^{2+}} with \mathrm{KMnO_4}.
In the titration of oxalic acid with \mathrm{KMnO_4}, the reaction mixture must be heated. State the reason.
State the role of starch in iodometric titrations.
