The white is my incorrect answers Redox reactions in basic medium

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Follow the steps  for your questions -

Step 1 Assign oxidation states to all atoms and identify the substances being oxidized and reduced.
Step 2 Separate the overall reaction into two half-reactions: one for oxidation and one for reduction.
Step 3
Balance each half-reaction with respect to mass in the following order:
? Balance all elements other than H and O.
? Balance O by adding H2O.
? Balance H by adding H+.
All elements are balanced,
so proceed to the next step.                                                                                                                                        

Step 4 Balance each half-reaction with respect to charge by adding electrons. (Make the sum of the charges on both sides of the equation equal by adding as many electrons as necessary.)
   
Step 5 Make the number of electrons in both half-reactions equal by multiplying one or both half-reactions by a small whole number.
   
Step 6 Add the two half-reactions together, canceling electrons and other species as necessary.
   
Step 7 Verify that the reaction is balanced with respect to both mass and charge.
   

To balance redox reactions occurring in basic solution, follow the half-reaction method outlined above but add an extra step to neutralize the acid with OH- after step 7
Add  OH- equal  to H+ on both sides of the balanced reaction.