For a particular redox reaction, ClO−2 is oxidized to ClO−4 and Cu2+ is reduced to Cu+ . Complete and balance the equation for this reaction in basic solution. The phases are optional.
Did you mean [ClO2]^- and [ClO4]^-?
The balanced equation for the redox reaction described in basic solution is as follows:
2 ClO−2 + 2 OH− → ClO−4 + Cl− + H2O
To balance the equation, you can follow these steps:
Step 1: Separate the reaction into half-reactions for oxidation and reduction:
Oxidation half-reaction: ClO−2 → ClO−4
Reduction half-reaction: Cu2+ → Cu+
Step 2: Balance the atoms other than oxygen and hydrogen in each half-reaction:
For the oxidation half-reaction:
Cl: 2 ClO−2 → ClO−4
For the reduction half-reaction:
Cu: Cu2+ → Cu+
Step 3: Balance the oxygen atoms by adding water molecules (H2O) to the side that is deficient in oxygen:
For the oxidation half-reaction, there are 4 oxygen atoms on the product side (ClO−4 ), but only 2 on the reactant side (ClO−2 ). Adding 2 water molecules to the reactant side balances the oxygen atoms:
2 ClO−2 → ClO−4 + 2 H2O
Step 4: Balance the hydrogen atoms by adding hydrogen ions (H+) to the side that is deficient in hydrogen:
For the oxidation half-reaction, there are 4 hydrogen atoms on the product side (H2O), but none on the reactant side. Adding 4 hydrogen ions to the reactant side balances the hydrogen atoms:
2 ClO−2 + 4 H+ → ClO−4 + 2 H2O
Step 5: Balance the charge by adding electrons (e−) to the side that is deficient in charge:
For the reduction half-reaction:
Cu2+ → Cu+
Since the charge on Cu2+ is 2+ and on Cu+ is 1+, we need to add 1 electron to the product side to balance the charge:
Cu2+ + 1 e− → Cu+
Step 6: Multiply each half-reaction by the appropriate number so that the electrons lost in oxidation are equal to the electrons gained in reduction:
To do this, multiply the oxidation half-reaction by 1 and the reduction half-reaction by 2:
2 ClO−2 + 4 H+ → 2 ClO−4 + 4 H2O
2 Cu2+ + 2 e− → 2 Cu+
Step 7: Add the half-reactions together and cancel out any species that appear on both sides:
2 ClO−2 + 4 H+ + 2 Cu2+ + 2 e− → 2 ClO−4 + 4 H2O + 2 Cu+
Step 8: Simplify the equation by canceling out the electrons and combining like terms:
2 ClO−2 + 4 H+ + 2 Cu2+ → 2 ClO−4 + 4 H2O + 2 Cu+
The balanced equation for the redox reaction in basic solution is:
2 ClO−2 + 4 H+ + 2 Cu2+ → 2 ClO−4 + 4 H2O + 2 Cu+
To balance a redox reaction in basic solution, follow these steps:
1. Write the unbalanced equation:
ClO−2 + Cu2+ → ClO−4 + Cu+
2. Separate the equation into two half-reactions – oxidation and reduction.
Oxidation half-reaction: ClO−2 → ClO−4
Reduction half-reaction: Cu2+ → Cu+
3. Balance the atoms, except for oxygen and hydrogen, in each half-reaction.
Oxidation half-reaction: ClO−2 → ClO−4
As there are no atoms other than Cl in both species, the oxidation half-reaction is already balanced.
Reduction half-reaction: Cu2+ → Cu+
Since there are no atoms except copper in both species, the reduction half-reaction is already balanced.
4. Balance oxygen atoms by adding water (H2O) molecules to the side that needs more oxygen.
Oxidation half-reaction: ClO−2 → ClO−4 + 2H2O
5. Balance hydrogen atoms by adding hydrogen ions (H+) to the side that needs more hydrogen.
Oxidation half-reaction: ClO−2 + 2OH- → ClO−4 + 2H2O
6. Balance charge by adding electrons (e-) to the more positive side of the equation.
Oxidation half-reaction: ClO−2 + 2OH- → ClO−4 + 2H2O + 2e-
7. To balance the electrons in both half-reactions, multiply the oxidation half-reaction by the coefficient of the reduction half-reaction and vice versa.
Oxidation half-reaction: 3ClO−2 + 6OH- → 3ClO−4 + 6H2O + 6e-
Reduction half-reaction: 6Cu2+ → 6Cu+
8. Combine both half-reactions, cancel out common species, and simplify.
Overall balanced equation: 3ClO−2 + 6OH- + 6Cu2+ → 3ClO−4 + 6Cu+ + 6H2O
This is the balanced equation for the given redox reaction in basic solution.