The SO2 present in air is mainly responsible for the phenomenon of acid rain. The

Question

concentration of SO2 can be determined by titration against a permanganate solution of
known concentration as follows:

SO2 + MnO4^-1 -> SO4^-2 + Mn2+
(unbalanced)

Balance the equation showing all your working and calculate the mass of SO2 in asample of
air if 7.37mL of 0.008 M KMnO4 solution are required toreach the endpoint of the titration.

Answer 1

Please

Answer 2

7.37 mL times 1 L/1000 mL times .008800 over 1L times 5 moles of so2 over 2 moles MnO4 times the molar mass of SO2 which is 64.063 g/1 mole SO2 = 0.00944 g SO2

Answer 3

Balanced equation: 5SO2 + 2MnO4 +H2O ———-> 5SO4 +2Mn +4H

7.37 mL times 1 L/1000 mL times .008800 over 1L times 5 moles of so2 over 2 moles MnO4 times the molar mass of SO2 which is 64.063 g/1 mole SO2 = 0.00944 g SO2