Final answer:
The balanced redox reaction in acidic solution for the transformation of NO₂(g) to NO₃⁻(aq) + NO(g) is:
2 NO₂(g) + 2 H₂O(l) + 4 H⁺(aq) → 4 HNO₃(aq) + 2 NO(g)
Step-by-step explanation:
To balance the given redox reaction in an acidic solution, the key is to determine the oxidation states and the number of atoms involved. Here, nitrogen in NO₂(g) undergoes oxidation to form NO₃⁻(aq) and NO(g). Begin by assigning oxidation states: Nitrogen goes from +4 in NO₂(g) to +5 in NO₃⁻(aq) and to +2 in NO(g).
To balance the oxygen atoms, add water molecules on the reactant side as needed (in this case, two water molecules). Then, balance the hydrogen atoms by adding H⁺ ions to the appropriate side of the equation. In this case, four H⁺ ions are added on the left side. The nitrogen atoms are balanced by adding appropriate coefficients in front of the molecules. Finally, balance the charge by adding electrons (not needed in this case).
The balanced redox equation in acidic solution for the conversion of NO₂(g) to NO₃⁻(aq) and NO(g) is 2 NO₂(g) + 2 H₂O(l) + 4 H⁺(aq) → 4 HNO₃(aq) + 2 NO(g). This balanced equation adheres to the conservation of mass and charge, ensuring that the number of atoms and total charge is the same on both sides of the equation.