Balance the following redox equations by the ionelectron...

Balance the following redox equations by the ionelectron method: (a) $\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{Fe}^{2+} \longrightarrow \mathrm{Fe}^{3+}+\mathrm{H}_{2} \mathrm{O}$ (in acidic solution) (b) $\mathrm{Cu}+\mathrm{HNO}_{3} \longrightarrow \mathrm{Cu}^{2+}+\mathrm{NO}+\mathrm{H}_{2} \mathrm{O}$ (in acidic solution) (c) $\mathrm{CN}^{-}+\mathrm{MnO}_{4}^{-} \longrightarrow \mathrm{CNO}^{-}+\mathrm{MnO}_{2}$ (in basic solution) (d) $\mathrm{Br}_{2} \longrightarrow \mathrm{BrO}_{3}^{-}+\mathrm{Br}^{-}$ (in basic solution) (e) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{I}_{2} \longrightarrow \mathrm{I}^{-}+\mathrm{S}_{4} \mathrm{O}_{6}^{2-}$ (in acidic solution)

Balance the following redox equations by the ionelectron method:
(a) $\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{Fe}^{2+} \longrightarrow \mathrm{Fe}^{3+}+\mathrm{H}_{2} \mathrm{O}$ (in acidic solution)
(b) $\mathrm{Cu}+\mathrm{HNO}_{3} \longrightarrow \mathrm{Cu}^{2+}+\mathrm{NO}+\mathrm{H}_{2} \mathrm{O}$ (in acidic solution)
(c) $\mathrm{CN}^{-}+\mathrm{MnO}_{4}^{-} \longrightarrow \mathrm{CNO}^{-}+\mathrm{MnO}_{2}$ (in
basic solution)
(d) $\mathrm{Br}_{2} \longrightarrow \mathrm{BrO}_{3}^{-}+\mathrm{Br}^{-}$ (in basic solution)
(e) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{I}_{2} \longrightarrow \mathrm{I}^{-}+\mathrm{S}_{4} \mathrm{O}_{6}^{2-}$ (in acidic solution)

Key Concepts

Balancing in Acidic and Basic Solutions

Redox reactions are balanced differently depending on the medium. In acidic solutions, hydrogen ions (H+) and water are used to balance hydrogen and oxygen atoms, while in basic solutions, hydroxide ions (OH-) and water serve this function. Recognizing the reaction medium is critical for correctly balancing the overall equation.

Redox Reactions

Redox reactions are chemical processes in which electrons are transferred between species, leading to changes in their oxidation states. This concept is foundational for understanding many chemical reactions, as it explains how energy is managed and how substances are transformed.

Oxidation and Reduction

These concepts denote the two complementary processes in redox chemistry: oxidation involves the loss of electrons, while reduction involves the gain of electrons. Clearly distinguishing between these processes is essential in identifying which species are oxidized and which are reduced.

Half-Reaction Method

The half-reaction method is a systematic approach to balancing redox equations. It involves splitting the overall reaction into two parts—one for oxidation and one for reduction—balancing each separately for mass and charge, and then recombining them to ensure that electrons cancel out.

Ion-Electron Method

Also known as the electron-transfer method, this technique further refines the half-reaction method by explicitly balancing the number of electrons lost and gained. It is particularly useful in aqueous solutions where ions participate in the reaction, and it requires the careful addition of water, protons, and sometimes hydroxide ions.

Oxidation State Determination

Assigning oxidation states to the elements in a reaction is a key step in identifying the species undergoing oxidation and reduction. This determination helps in setting up the half-reactions and in calculating the number of electrons transferred, ensuring the conservation of charge in the reaction.

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