(Solved): 1. Consider the following molecular equation for the reaction involved in today's experiment: (Plac ...

1. Consider the following molecular equation for the reaction involved in today's experiment: (Place \( a \) and \( b \) at the end the Procedure for Part 2) \[ \mathrm{KMnO}_{4}+\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow \mathrm{MnSO}_{4}+\mathrm{CO}_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{H}_{2} \mathrm{O} \] a. Write a balanced, unmultiplied ionic half-reaction for the oxidation: b. Write a balanced, unmultiplied ionic half-reaction for the reduction: c. Write the balanced net-ionic reaction: d. Write the balanced molecular reaction: 2. How many \( \mathrm{mL} \) of a \( 1.260 \mathrm{~N} \mathrm{KMnO}_{4} \) solution are needed to completely react with (titrate) \( 3.200 \) grams of \( \mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \) in acid solution. Show all work and units.