An acidic solution is prepared by mixing 100.0 mL of 0.0200 M potassium permanganate…
CHEMISTRY · Multi-part · A Level · Chemistry · Oxidation, reduction and redox reactions · Oxidation, reduction and redox reactions
Problem
An acidic solution is prepared by mixing 100.0 mL of 0.0200 M potassium permanganate with excess 1.00 M sulfuric acid. This purple solution is titrated with 0.0800 M sodium oxalate solution that also contains 0.100 M calcium nitrate. During the titration, a colorless solution results, gaseous carbon dioxide is evolved, and an insoluble white solid is observed at the bottom of the flask.
Assume all reactions proceed to completion and that volumes are additive.
(a) Write the overall balanced molecular equation that accounts for all observable changes in the system, including the formation of any gases or solids.
(b) Write the balanced net ionic equation for the reaction occurring in the titration, using acidic conditions.
(c) Identify the spectator ions present in the titration mixture.
(d) Determine the number of moles of electrons transferred per mole of permanganate ion reacted, based on the balanced net ionic equation from part (b).
(e) Calculate the volume, in milliliters, of the sodium oxalate solution required to reach the equivalence point with the given volume of permanganate solution.