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A 16.42 mL volume of 0.1327 M KMnO4 solution is needed to oxidize 25.00 mL of a FeSO4 solution in acidic medium. What is the concentration of the FeSO4 solution in molarity?

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The concentration of the FeSO4 solution in molarity would be 0.4356

The concentration can be derived first by writing out the balanced equation of the reaction:

  • [tex]5Fe^2^++MnO^4^-+8H^+--->5Fe^3^++Mn^2^++4H_2O[/tex]

From the balanced equation: for every 1 mole of KMnO4, 5 moles of FeSO4 is needed for complete oxidation.

Recall that: mole = molarity x volume

Mole of KMnO4 needed = 0.1327 x 0.01642

                  = 0.002179 mole

1 mole KMnO4 = 5 mole FeSO4

0.002178 mole = 5 x 0.002178/1

                             = 0.01089 moles of FeSO4

Molarity of FeSO4 = mole/volume

                                 = 0.01089/0.025

                               = 0.4356 M

More on the calculation of molarity of solutions can be found here: https://brainly.com/question/16587536

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