If 36.44 ml of a 0.01652 M KMnO4 solution are required to completely oxidize 25.000 ml of a H2O2 solution, calculate the molarity of the H2O2 solution. The equation of the reaction is as follows:
2MnO4- + 5H2O2 + 6H+ à5O2 + 2Mn2+ + 8H2O
Originally posted by felirox:
If 36.44 ml of a 0.01652 M KMnO4 solution are required to completely oxidize 25.000 ml of a H2O2 solution, calculate the molarity of the H2O2 solution. The equation of the reaction is as follows:
2MnO4- + 5H2O2 + 6H+ à5O2 + 2Mn2+ + 8H2O
1) Calculate no. of moles of MnO4- used.
2) Apply stoichiometry from the balanced redox equation to determine no. of moles of H2O2 oxidized.
3) Calculate molarity using the formula :
Molarity (mol/dm3) = No of Moles (mol) / Volume of Solution (dm3).