Question

An impure sample of oxalic acid (H2C2O4) wasoxidized by potassium permanganate. A 0.261-g sample of oxalic acidwas dissolved, and the solution was diluted to 100.0 mL. A 25.0-mLportion of the oxalic acid solution was titrated with 26.2 mL of0.0107 M potassiumpermanganate.

a) write a balanced equationfor the titration reaction.

b)how many moles of potassiumwere used? (ans: 2.8 x10^-4 mol)

c)How many moles of oxalicacid were titrated? (ans: 7.01X10^-4 mol)

d)Calculate the percent purityof the oxalic sample. (ans: 96.7%)

please shows steps, thankyou