Balance each redox reaction occurring in acidic aqueous solution. a. Zn(s) + Sn²⁺(aq) → Zn²⁺(aq) + Sn(s)

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Identify the oxidation and reduction half-reactions. Zn is oxidized from Zn(s) to Zn^{2+}(aq), and Sn^{2+}(aq) is reduced to Sn(s).

Write the oxidation half-reaction: Zn(s) \(\rightarrow\) Zn^{2+}(aq) + 2e^{-}.

Write the reduction half-reaction: Sn^{2+}(aq) + 2e^{-} \(\rightarrow\) Sn(s).

Since the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction, the electrons cancel out when the half-reactions are added together.

Combine the balanced half-reactions to obtain the balanced overall redox reaction: Zn(s) + Sn^{2+}(aq) \(\rightarrow\) Zn^{2+}(aq) + Sn(s).

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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 another 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 essential to account for the presence of H+ ions and water to maintain charge and mass balance.

Balance each redox reaction occurring in acidic aqueous solution. a. Zn(s) + Sn2+(aq) → Zn2+(aq) + Sn(s)