Final answer:
Balancing redox reactions involves writing separate oxidation and reduction half-reactions, balancing the number of atoms and charge, and adding H+ or OH- in acidic or basic solutions respectively.
Step-by-step explanation:
The process of balancing redox reactions depends on the environment in which the reaction occurs - acidic or basic. In acidic solutions, H+ ions are added to balance the charge, while in basic solutions, OH- ions are used. Following the step-by-step procedure for balancing using oxidation states, one would write separate half-reactions for the oxidation and reduction processes. Then, adjust the coefficients to balance the number of atoms of each element and add the equations, canceling out the electrons. Lastly, add enough H+ or OH- ions to both sides to ensure the charges on the reactants and products are equal. For example, given the equation H₂AsO + 4 Zn(s) → AsH₂(g) + 4 Zn²+, adding 8 H+ ions to the left side would balance the charges in an acidic solution, while in basic solution OH- ions would be used instead.