Question

Asked Oct 15, 2019

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Step 1

The steps involved in the balancing of a redox equation are:

- First, balance the number of electrons present on both the sides of the half-cell equation.
- Add the appropriate number of water molecules to the opposite side of the chemical equation in order to balance the number of oxygen atoms.
- Add the appropriate number of hydrogen ions to the opposite side of the chemical equation in order to balance the number of hydrogen atoms.
- Add the balanced half-cell reactions in order to obtain a complete redox reaction.
- The last step is to balance the charges on both sides of the half-cell reaction.

The molarity of an unknown solution can be determined by titrating it with a known solution by using the equation (1), in which, M_{1} is the molarity of the unknown solution, V_{1} is the volume of the unknown solution, M_{2} is the molarity of the known solution and V_{2} is the volume of the known solution.

Step 2

The given half-cell reactions are,

- I) MnO
_{4}^{-}→ MnO_{2} - II) Mn
^{2+}→ MnO_{2}

Balance the (I) reaction as follows:

The oxidation state of manganese is changed from +7 to +4 on going from the reactant to the product side. Therefore, the number of electrons will be balanced on both sides by adding 3 electrons to the reactant side.

MnO_{4}^{-} + 3e^{-} → MnO_{2}

Add 2 water molecules on the product side in order to balance the number of oxygen atoms.

MnO_{4}^{-} + 3e^{-} → MnO_{2} + 2H_{2}O

Add 4 hydrogen ions on the reactant side in order to balance the number of hydrogen atoms.

MnO_{4}^{-} + 4H^{+} + 3e^{-} → MnO_{2} + 2H_{2}O …… (III)

Step 3

Balance the (II) reaction as follows:

The oxidation state of manganese is changed from +2 to +4 on going from the reactant to the product side. Therefore, the number of electrons will be balanced on both sides by adding 2 electrons to the product side.

Mn2+ → MnO2 + 2e-

Add 2 water molecules on the reactant side in order to balance the number of oxygen atoms.

Mn2+ + 2H2O →...

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