please help this equation is driving my crazy.

balance the following redox reaction in basic solution.
H2O2 + ClO2 --> ClO-2 + O2

Did you follow the instructions I left for you on your problem yesterday? Here is a link to it. Those work EVERY time. Let me know if you have trouble BUT tell me what your problem is so I can diagnose what is wrong.

http://www.jiskha.com/display.cgi?id=1322000859

To balance the given redox reaction in basic solution, you need to follow these steps:

Step 1: Assign oxidation numbers to each element in the equation.
Start by assigning oxidation numbers to the elements on both sides of the equation. The oxidation number represents the charge that an atom would have if electrons were transferred completely.

In this reaction:
H2O2 + ClO2 --> ClO-2 + O2

The oxidation number of H in H2O2 is +1 (since it is a diatomic molecule), and the oxidation number of O is -1.
The oxidation number of Cl in ClO2 is +4, and the oxidation number of O is -2.

Step 2: Identify the atoms that undergo oxidation and reduction.
In the given reaction, the oxidation state of Cl changes from +4 to -2 (reduction), and the oxidation state of H changes from +1 to 0 (oxidation).

Step 3: Balance the atoms that undergo oxidation or reduction.
To balance the Cl atoms, you need to add two ClO-2 to the right-hand side of the equation.

H2O2 + ClO2 --> 2ClO-2 + O2

Now, both sides of the equation have the same number of Cl atoms.

Step 4: Balance the atoms other than oxygen and hydrogen.
Next, balance the oxygen atoms by adding water (H2O) molecules to the side that needs more oxygen. In this case, you need to add three water molecules to the left-hand side.

H2O2 + ClO2 --> 2ClO-2 + O2 + 3H2O

Now, both sides of the equation have the same number of oxygen atoms.

Step 5: Balance the hydrogen atoms.
Finally, balance the hydrogen atoms by adding hydrogen ions (H+) to the side that needs more hydrogen. In this case, you need to add four hydrogen ions to the left-hand side to balance the hydrogen atoms.

H2O2 + ClO2 + 4H+ --> 2ClO-2 + O2 + 3H2O

Step 6: Balance the charges.
To balance the charges, add electrons (e-) to the side that needs more negative charge. In this case, the left-hand side needs a total of 10 electrons to balance the charges.

H2O2 + ClO2 + 4H+ + 10e- --> 2ClO-2 + O2 + 3H2O

Step 7: Check the balancing of mass and charges.
Make sure both sides of the equation have the same number of atoms and the same total charge.

In the given balanced equation:
H2O2 + ClO2 + 4H+ + 10e- --> 2ClO-2 + O2 + 3H2O

Both sides have a total of 2 hydrogen atoms, 5 oxygen atoms, and the same total charge.

Therefore, the balanced equation for the given redox reaction in basic solution is:

H2O2 + ClO2 + 4H+ + 10e- --> 2ClO-2 + O2 + 3H2O