Balance each redox reaction occurring in acidic aqueous solution. c. BrO₃^–(aq) + N₂H₄(g) → Br^–(aq) + N₂(g)

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Identify the oxidation and reduction half-reactions. BrO_3^- is reduced to Br^- and N_2H_4 is oxidized to N_2.

Balance the atoms in each half-reaction, starting with elements other than O and H. For the reduction half-reaction, balance Br. For the oxidation half-reaction, balance N.

Balance the oxygen atoms by adding H_2O molecules. For the reduction half-reaction, add H_2O to the side lacking oxygen.

Balance the hydrogen atoms by adding H^+ ions. For the reduction half-reaction, add H^+ to the side lacking hydrogen.

Balance the charge by adding electrons. Ensure that the number of electrons lost in the oxidation half-reaction equals the number gained in the reduction half-reaction.

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Redox Reactions

Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between two species. In these reactions, one species is oxidized (loses electrons) while the other is reduced (gains electrons). Understanding the oxidation states of the elements involved is crucial for identifying which species undergo oxidation and reduction.

Balancing Redox Reactions

Balancing redox reactions requires ensuring that both mass and charge are conserved. This is typically done using the half-reaction method, where the oxidation and reduction processes are balanced separately before combining them. In acidic solutions, hydrogen ions (H+) and water (H2O) are often added to balance the equation.

Acidic Aqueous Solution

An acidic aqueous solution contains a higher concentration of hydrogen ions (H+) than hydroxide ions (OH-). This environment affects the behavior of the reactants and products in a redox reaction. When balancing reactions in such solutions, it is important to account for the presence of H+ ions and water molecules to maintain charge and mass balance.

Balance each redox reaction occurring in acidic aqueous solution. c. BrO3–(aq) + N2H4(g) → Br–(aq) + N2(g)